Unit 1: Getting Ready for Chemistry

If you can do all the things listed below, you are ready for the Unit 1 test.

Place a checkmark next to each item that you can do! If a sample problem is given, complete it as evidence.

5 important lab safety rules are:

2. _____1. I can list five important lab safety rules. 3.

_____2. I can identify the most Draw and label as many of the common laboratory tools as you can! common laboratory tools such as: beaker, graduated cylinder, Erlenmeyer flask, scoop, beaker tongs, test tube, test tube rack, test tube holder, crucible tongs, Bunsen burner, striker, stirring rod, funnel, dropper pipette (aka eye dropper)

A farmer wants to know what the effect the amount of fertilizer has on the amount of fruit an apple tree produces.

_____3. I can determine the What is the independent variable? independent and dependent variable in a lab experiment. What is the dependent variable?

How many significant figures are there in 30.50 cm? _____4. I can determine the number of significant figures in a How many significant figures are there in 400.0 sec? measurement.

_____5. I can determine the To the correct number of significant figures, what is the answer to answer to a math problem to the 5.93 mL + 4.6 mL? correct number of significant figures. To the correct number of significant figures, what is the answer to 5.93 cm * 4.6 cm? _____6. I can read the meniscus on a graduated cylinder to the correct number of significant figures.

The volume is______mL. To the correct number of significant figures, determine how many meters there are in 15.4 ft.

_____7. I can use dimensional To the correct number of significant figures, determine how many minutes analysis to solve math problems. there are in 2.7 years.

Convert 87,394,000,000,000 to scientific notation.

_____8. I can convert numbers into scientific notation from Convert 0.0000040934 to scientific notation. standard notation.

9 Convert 5.8 x 10 to standard notation.

_____9. I can convert numbers into standard notation from -5 Convert 4.3 x 10 to standard notation. scientific notation.

_____10. I can use my calculator 52 Enter the number 5.67 x 10 on your calculator to input numbers in scientific notation using the “2nd function & EE keys. 9.3 km = ? m _____11. I can convert between different metric units by using “King Henry died by drinking 39,983 mL = ?kL chocolate milk”.

_____12. I can convert between -3 1.5 x 10 km = ? m different metric units by using Reference Table C and dimensional analysis. 13 4.67 x 10 pm = ?dm Which equation would you use to solve the following problem? (Don’t solve it. Just tell me WHICH equation to use.) _____13. I can determine which equation to use from Reference Problem: How many grams of LiBr (gram-formula mass = 87 g/mol) would 3.5 Table T by looking at the given moles of LiBr be? information.

3 3 _____14. I can solve for “x” when What is the volume, in cm , of 54.6 g of beryllium (density = 1.85 g/cm ) it’s in the denominator of a fraction.

o What kelvin temperature is equal to 200 C? o _____15. I can convert C to degrees kelvin and degrees kelvin o What Celsius temperature is equal to 200K? to C.

Al______

Ca______

Ne______16. Given the symbol I can write the name for any element N______in Group 1, Group 2, Group 13, Group 14, Group 15, Group 16, Na______Group 17 or Group 18 S______

Br______

Ge______Al______

Ca______

_____17. Given the symbol or the Ne______name, I can determine the Group N______for any element in Group 1, Group 2, Group 13, Group 14, Na______Group 15, Group 16, Group 17 or Group 18 S______

Br______

Ge______18. I can define gram- Definition: formula mass (AKA molar mass).

How many moles of atoms are in N ? 2

_____19.Given the chemical What is the total # of moles of atoms in Pb(C H O ) ? symbol/formula, I can determine 2 3 2 2 how many atoms are present. How many moles of C atoms are in Pb(C H O ) ? 2 3 2 2

What is the gfm for N ? 2 _____20. I can determine the gram-formula mass for any element or compound. What is the gfm for Pb(C H O ) ? 2 3 2 2

Definition: _____21. I can define a mole as it pertains to chemistry.

_____22. I can find the number of 94.3 g is how many moles of NaCl? moles of substance if I am given the mass and formula for the substance. What is the percent by mass of Mg in Mg(NO ) ? _____23. I can determine the 3 2 percent composition of an element in a compound.

24 _____24. I can convert between How many moles of carbon atoms are there in 4.8 x 10 atoms of C? moles and numbers of particles NOT NEEDED FOR REGENTS using Avogadro’s number? How many L does 4.60 moles of O occupy assuming STP? _____25. I can convert between 2 moles and L (assuming STP). NOT NEEDED FOR REGENTS Unit 2: Introduction to Matter

_____1. I can still do everything from Unit 1. Definitions: atom

element

_____2. I can define the following: atom, element, compound, compound mixture

mixture

2 Atoms of 1 Element 2 Molecule of 1 Compound

Mixture of 2 elements Mixture of 2 compounds

_____3. I can draw particle diagrams to represent an atom, an element, a molecule, a compound, a mixture

Mixture of an element and a compound Put each of the following examples into the correct column.

Examples: C H O , NaCl, Fe, salt water, air, CO , H , Ar, soda 12 22 11 2 2 Element Compound Mixture _____4. I can classify substances as a pure substance (element or compound) or as a mixture.

Definitions: homogeneous mixture

_____5. I can define homogeneous mixture and heterogeneous mixture in terms of particle heterogeneous mixture distribution.

Two examples of homogeneous mixtures: a.

_____6. I can give an example of homogeneous and heterogeneous Two examples of heterogeneous mixtures: mixtures. a.

Write “P” for physical or “C” for chemical on the line provided.

_____copper (II) sulfate is blue.

_____copper reacts with oxygen.

_____copper can be made into wire. _____7. I can classify a property as physical or chemical. 3 _____copper has a density of 8.96 g/cm .

_____ copper melts at 1358K.

_____copper reacts with nitric acid.

_____copper doesn’t dissolve in water. Write “P” for physical or “C” for chemical on the line provided.

_____copper (II) sulfate dissolves in water.

_____copper reacts with oxygen to form solid copper (I) oxide.

_____solid copper is melted. _____8. I can classify a change as physical or chemical. _____a chunk of copper is pounded flat.

_____copper and zinc are mixed to form brass.

_____a large piece of copper is chopped in half.

_____copper reacts with bromine to form copper (II) bromide.

Substance A

_____9. In a particle diagram, I can Circle the particle diagram that best represents Substance A after a physical distinguish between a physical change has occurred. change and a chemical change.

Definitions: solute

solvent

_____10. I can define: solute, solution solvent, solution, and solubility.

solubility

_____11. I can describe the trend As the temperature increases, the solubility of a solid ______. in solubility for solids as the temperature changes.

_____12. I can describe the trend As the temperature increases, the solubility of a gas ______. in solubility for gases as the temperature changes. Write “S” for soluble and “NS” for not soluble. Use Reference Table F to determine the solubility of the following compounds:

_____potassium chlorate _____13. I can use Reference Table F to determine if a substance will _____silver bromide be soluble in water. _____lithium carbonate

_____calcium carbonate _____14. I can use Table G to o How many grams of KClO must be dissolved in 100 grams of water at 20 C determine how much solute to add 3 at a given temperature to make a to make a saturated solution? saturated solution. _____15. I can use Table G to o If 20.0 g of NaNO are dissolved in 100.0 g of water at 25.0 C, will the determine if a solution is 3 saturated, unsaturated, or resulting solution be saturated, unsaturated, or supersaturated? supersatured. Definitions: dilute

concentrated

_____16. I can define: dilute, concentrated, concentration, and electrolyte. concentration

electrolyte

Which solution is most concentrated? o A) 125.0 g of KI dissolved in 100.0 g of water at 10 C _____17. I can interpret Table G to o B) 70.0 g of NH Cl dissolved in 100.0 g of water at 70 C determine which solution is the 4 most concentrated or the most o C) 120.0 g of KNO dissolved in 100.0 g of water at 70 C dilute. 3 o D) 30.0 g of SO dissolved in 100.0 g of water at 90 C 2 _____18. I can use Reference Table What is the concentration, in ppm, of a 2600 g of solution containing 0.015 g of CO ? T to calculate the concentration of 2 a solution in ppm. _____19. I can use Reference Table What is the molarity of 3.5 moles of NaBr dissolved in 500 mL of water? T to calculate the concentration of a solution in molarity. When a mixture of sand, salt, sugar, and water is filtered, what passes through _____20. I can determine how the filter? matter will be separated using filtration. Which physical property makes it possible to separate the components of _____21. I can describe how crude oil by means of distillation? matter can be separated using distillation. To separate a mixture of salt and water, the best method of separation would be______. _____23. I can state which To separate a mixture of ethanol and water, the best method of separation separation process (decanting, would be ______. filtering, distilling, To separate a mixture of food coloring dyes, the best method of separation chromatography, or evaporating) would be ______. is best for a given situation. To separate a mixture of oil and water, the best method of separation would be______. Defintion: allotrope _____24. I can define allotrope.

_____25. I can state the Two allotropes of the same element have different molecular structures and differences between two therefore have different ______and ______allotropes of the same element. properties. Unit 3: Matter & Energy

_____1. I can still do everything from Unit 1. _____2. I can still do everything from Unit 2. Defintions: kinetic energy

potential energy

temperature _____3. I can define kinetic energy, potential energy, temperature, heat, endothermic, and heat exothermic.

endothermic

exothermic

Draw a particle diagram to represent atoms of Li in each phase.

Solid Liquid Gas ____4. I can use particle diagrams to show the arrangement and spacing of atoms/molecules in different phases. Solid Liquid Gas

Relative Kinetic Energy _____5. I can compare solids, liquids, and gases in terms of their relative kinetic energy, ability to Ability to completely fill a container, ability Completely Fill to change shape. a Container Ability to Change Shape

During fusion a substance changes from ______to ______.

During solidification a substance changes from ______to ______.

During condensation a substance changes from ______to ______.

During vaporization a substance changes from ______to _____6. I can state the change of ______. phase occurring in fusion, solidification, condensation, During melting a substance changes from ______to vaporization, melting, boiling, ______. sublimation, deposition, and freezing. During boiling a substance changes from ______to ______.

During sublimation a substance changes from ______to ______.

During deposition a substance changes from ______to ______.

During freezing a substance changes from ______to ______.

_____7. I can indicate if a phase For each phase change listed, indicate whether the change is exothermic or change is exothermic or endothermic. endothermic. fusion/melting______

solidification/freezing______

condensation______

vaporization/boiling______

sublimation______deposition______

_____8. Given a heating/cooling curve, I can determine the temperature at which a substance freezes/melts or condenses/vaporizes. What is the freezing point of this substance?

What is the boiling point of this substance?

_____9. Given a heating/cooling curve, I can determine which sections of the curve show changes in potential energy.

On the graph, circle the sections that show a change in potential energy.

_____10. Given a heating/cooling curve, I can determine which sections of the curve show changes in kinetic energy.

On the graph, circle the sections that show a change in kinetic energy.

_____11. I can state the o What is the freezing point of water in C and K? temperature at which water o freezes in C and K.

_____12. I can state the o What is the melting point of water in C and K? temperature at which water melts o in C and K.

_____13. I can state the o What is the boiling point of water in C and K? temperature at which water o vaporizes/boils in C and K.

_____14. I can state the o What is the condensing point of water in C and K? temperature at which water o condenses in C and K. Which heat equation should be used in each of the following:

o a. How much heat is needed to vaporize 100.0 g of water at 100 C?

_____15. I can use Reference Table T to determine which “heat” b. How much heat is needed to raise the temperature of 100.0 g of water by o equation is needed for a given 35 C? problem. o c. How much heat is needed to melt 100.0 g of ice at 0 C?

Definitions: specific heat capacity

_____16. I can define specific heat heat of fusion capacity, heat of fusion, heat of vaporization. heat of vaporization

o How many grams of water can be heated by 15.0 C using 13,500 J of heat?

_____17. I can use the “heat” equations to solve for any variable, It takes 5210 J of heat to melt 50.0 g of ethanol at its melting point. What is if I am given the other variables. the heat of fusion of ethanol?

_____18. I can state the 5 parts of The five parts of the Kinetic Molecular Theory are: the Kinetic Molecular Theory. a.

e. Definition: ideal gas _____19. I can define an ideal gas.

_____20. I can state the conditions A gas will act most “ideally” under the conditions of ______pressure of pressure and temperature under which a gas will act and ______temperature. “ideally”. _____21. I can state the two The two elements that act ideally most of the time are ______& elements that act ideally most of the time. ______. What causes gas molecules to create pressure? _____22. I can explain how pressure is created by a gas.

_____23. I can state the At constant temperature, as the pressure on a gas increases, the volume relationship between pressure and volume for gases (assuming ______. constant temperature). _____24. I can state the At constant pressure, as the temperature on a gas increases, the volume relationship between temperature and volume for gases (assuming ______. constant pressure). _____25. I can state the In a fixed container (AKA “has constant volume), as the temperature on a gas relationship between temperature and pressure for gases (assuming increases, the pressure______. constant volume). _____26. I can state Avogadro’s Avogadro’s Hypothesis says______Hypothesis. ______o _____27. I can remember to A gas originally occupies 2.3L at 56 C and 101.3 kPa. What will its volume be o o convert C to K when using the at 100 C and 105.7 kPa? Combined Gas Law to determine changes in V, P, or T of a gas. Definition: boiling point

_____28. I can define boiling point and vapor pressure. vapor pressure

_____29. I can state the condition The normal boiling point of a substance occurs at a pressure of of pressure that is used for ______atm/______kPa. “normal” boiling points. _____30. I can state the relationship between atmospheric As the atmospheric pressure increases, the boiling point ______. pressure and boiling point. Unit 4: Atomic Theory

_____1. I can still do everything from Unit 1. _____2. I can still do everything from Unit 2. _____3. I can still do everything from Unit 3. Dalton’s Model:

_____4. I can describe John What it looked like: Dalton’s contribution to our understanding of the atom.

Thomson’s Experiment:

Thomson’s Model: _____5. I can describe JJ Thomson’s contribution to our understanding of the atom. What it looked like:

Rutherford’s Experiment:

Rutherford’s Model: _____6. I can describe Ernest Rutherford’s contribution to our understanding of the atom. What it looked like:

Bohr’s Model:

_____7. I can describe Niels Bohr’s What it looked like: contribution to our understanding of the atom. _____8. I can describe James What subatomic particle did Chadwick discover? NOT NEEDED FOR REGENTS Chadwick’s contribution to our understanding of the atom. What does the modern model of the atom look like?

_____9. I can describe the current model of the atom. Where, in an atom, are electrons likely to be found according to the modern model?

From oldest to newest, list the models that we have used to describe an atom.

_____10. I can state the chronological order of atomic models.

Particle #1 Particle #2 Particle #3 Name

_____11. I can state the three Charge subatomic particles, their location in an atom, their charges, and their Mass masses (in amu). Location in Atom

_____12. I can explain why atoms Atoms are electrically neutral because the number of ______is are electrically neutral. equal to the number of ______. Definitions: mass number

_____13. I can define mass number and atomic number. atomic number

_____14. Given the mass number, 212 In an atom of Po, how many protons are present? I can determine the number of protons, neutron, and electrons in 84 an atom. 212 In an atom of Po, how many electrons are present? 84

212 In an atom of Po, how many neutrons are present? 84 How many protons are in an atom of selenium? _____15. I can use the Periodic Table to determine the atomic How many protons are in an atom of silicon? number of an element.

Definition: isotope _____16. I can define isotope.

Write the four different methods of isotopic notation for an atom of bromine that has 45 neutrons. _____17. I can represent an atom in any of the four methods of Method 1 Method 2 Method 3 Method 4 isotopic notation.

Element Q has two isotopes. If 77% of the element has an isotopic mass of 83.7 amu and 23% of the element has an isotopic mass of 89.3 amu, what is the average atomic mass of the element? _____18. I can calculate average atomic mass given the masses of the naturally occurring isotopes and the percent abundances.

Definitions: ion

cation _____19. I can define ion, cation, and anion.

_____20. Given the mass number 19 1- How many protons are in F ? and the charge, I can determine the number of protons, neutrons, 9 and electrons in an ion. 19 1- How many neutrons are in F ? 9 19 1- How many electrons are in F ? 9 Definitions: principal energy level (PEL)

orbital

ground state _____21. I can define principal energy level, orbital, ground state, excited state, electron excited state configuration, and bright line spectrum.

electron configuration

bright line spectrum

PEL1 holds a maximum of ______electrons.

_____22. I can state the maximum PEL2 holds a maximum of ______electrons. number of electrons that will fit into each of the first four principal PEL3 holds a maximum of ______electrons. energy levels. PEL4 holds a maximum of ______electrons.

_____23. I can state the As the distance between the nucleus and the electron increases, the energy of relationship between distance from the nucleus and energy of an the electron ______. electron. _____24. I can state the As the number of the PEL increases, the distance to the nucleus ______. relationship between the number of the principal energy level and the distance to the atom’s nucleus. A brightline spectrum is created when _____25. I can explain, in terms of subatomic particles and energy states, how a bright line spectrum is created. _____26. I can identify the elements shown in a bright line spectrum.

Which element(s) is/are present in the mixture?

Definition: valence electron _____27. I can define valence electrons.

How many valence electrons does an atom of rubidium have in the ground state? _____28. I can locate and interpret an element’s electron configuration on the Periodic How many principal energy levels contain electrons in an atom of iodine in the Table. ground state?

Which electron configuration represents an atom of potassium in the excited state?

_____29. I can identify an electron configuration that shows an atom A) 2-8-7-1 in the excited state. B) 2-8-8-1 C) 2-8-7-2 D) 2-8-8-2 Draw the Lewis electron dot diagram for the following atoms: _____30. I can draw Lewis electron dot diagrams for a given element. Li Be B C N O F Ne

_____31. I can define and state the Definition: importance of “octet of valence octet of valence electrons electrons.”

The importance of having a complete“octet of valence electrons” is

Unit 5: Nuclear Chemistry

_____1. I can still do everything from Unit 1. _____2. I can still do everything from Unit 2. _____3. I can still do everything from Unit 3. _____4. I can still do everything from Unit 4. Type Symbol Mass # Charge Penetrating Shielding Bio Power Required Hazard alpha

beta _____5. I can compare types of radiation in terms of symbol, mass gamma number, charge, penetrating power, shielding required, and biological hazard. neutron

positron

The three types of nuclear reactions are:

a. _____6. I can identify the three types of nuclear reactions. b.

_____7. I can define Definitions: transmutation, fission, and fusion. transmutation

fission fusion

_____8. I can state two synonyms Two synonyms for spontaneous decay are:______for spontaneous decay. and ______. _____9. I can show how mass Complete the following nuclear equation: number and electrical charge must be conserved in any nuclear reaction. ______10. I can explain what makes The stability of the nucleus is dependent on the ______to a nucleus stable or unstable. ______ratio.

The difference between natural transmutation and artificial transmutation is _____11. I can explain the that in natural transmutation an______breaks apart on difference between natural its own and in artificial transmutation a ______is transmutation and artificial made ______by hitting it with a high energy particle (such as a transmutation. proton, neutron, or gamma radiation).

Which equation represents a natural decay?

_____12. I can identify a natural decay reaction from a list of reactions.

Which equation represents artificial transmutation?

_____13. I can identify an artificial transmutation reaction from a list of reactions.

_____14. I can identify a fission Which equation represents fission? reaction from a list of reactions. Which equation represents fusion?

_____15. I can identify a fusion reaction from a list of reactions. _____16. I can state the conditions The temperature and pressure conditions needed for fusion to happen are: of temperature and pressure that are needed for a fusion reaction to ______temperature and ______pressure happen. Nuclear reactions release LOTS more energy than chemical reactions do _____17. I can explain why all because nuclear reactions release LOTS more energy than chemical reactions do. Which of the following equations represent NUCLEAR reactions?

_____18. Given a list of reactions, I can differentiate a “nuclear” reaction from a “chemical” reaction.

Definition: half-life _____19. I can define half-life.

Based on Reference Table N, what fraction of a radioactive sample of Au-198 will remain unchanged after 10.78 days?

_____20. Given the length of the half-life and the amount of time that has passed, I can determine What was the original mass of a radioactive sample of K-37 if the sample the amount of radioactive sample. decayed to 25.0 g after 4.92 seconds? The half-life of K-37 is 1.23 seconds)

_____21. Given the length of the A 100.0 g sample of Co-60 decays until only 12.5 g of it remains. Given that half-life and the amount of the half-life of Co-60 is 5.271 years, how long did the decay take? radioactive sample, I can determine the amount of time that has passed. _____22. Given the amount of What is the half-life of a radioisotope if 25.0 g of an original 200.0 g sample time that has passed and the remains unchanged after 11.46 days? amount of radioactive sample, I can determine the length of the half-life. Compared to K-37, the isotope K-42 has

A) shorter half-life and the same decay mode _____23. Using Table N, I can B) shorter half-life and a different decay mode determine the length of half-life and/or decay mode for a specific C) longer half-life and the same decay mode radioactive isotope. D) longer half-life and a different decay mode

Five beneficial uses for radioactive isotopes are: a.

_____24. I can state 5 beneficial c. uses for radioactive isotopes. d.

C-14 is used for ______

I-131 is used for______25. I can state the scientific use of 4 specific radioactive U-238 is used for ______isotopes. Co-60 is used for______

Three risks associated with radioactivity and radioactive isotopes are:

_____26. I can state three risks b. associated with radioactivity and radioactive isotopes. c. Unit 6: Periodic Table

_____1. I can still do everything from Unit 1. _____2. I can still do everything from Unit 2. _____3. I can still do everything from Unit 3. _____4. I can still do everything from Unit 4. _____5. I can still do everything from Unit 5. Classify each of the following elements as metals (M), nonmetals (NM), or metalloids (MTLD).

______B ______K ______Li ______C ______Ar _____6. I can classify elements as metals, nonmetals, or metalloids ______Sb ______H ______Fe ______Au ______S based on their placement on the Periodic Table. ______F ______Si ______Fr ______He ______Rn

______Ge ______Al ______As ______Bi ______I

Group 1 is called the ______.

_____7. I can state the group Group 2 is called the ______. names for elements in groups 1, 2, 17, and 18. Group 17 is called the ______.

Group 18 is called the ______. Elements in the same group have similar chemical properties because _____8. I can explain why elements in the same group have similar chemical properties.

Elements in Group 18 don’t usually react with other elements because _____9. I can explain why the elements in Group 18 don’t usually react with other elements. STP stands for ______. _____10. I can state the meaning of “STP” and the Reference Table The values can be found on Reference Table______. on which it can be found. _____11. I can state the The two elements that are liquids at STP are: names/symbols for the two elements on the Periodic Table ______and ______that are liquids at STP. The 11 elements that are gases at STP are:

______, ______,

_____12. I can state the ______, ______, names/symbols of the 11 elements that are gases at STP. ______, ______,

______, ______,

and ______

_____13. I can state how the The elements on the Periodic Table are arranged by increasing elements on the Periodic Table are arranged. ______. The seven diatomic elements are:

_____14. I can list the 7 diatomic elements.

Definitions: electronegativity

first ionization energy

atomic radius _____15. I can define electronegativity, first ionization energy, atomic radius, ionic radius, ionic radius metallic character, and activity/reactivity.

metallic character

activity/reactivity As one reads down a group from top to bottom, electronegativity

______because ______

_____16. I can state the periodic ______. trend for electronegativity and As one reads across a period from left to right, electronegativity explain why it occurs. ______because ______

______.

As one reads down a group from top to bottom, first ionization energy

______because ______

_____17. I can state the periodic ______. trend for first ionization energy As one reads across a period from left to right, , first ionization energy and explain why it occurs. ______because ______

______.

As one reads down a group from top to bottom, atomic radius

______because ______

_____18. I can state the periodic ______. trend for atomic radius and explain As one reads across a period from left to right, atomic radius why it occurs. ______because ______

______.

As one reads down a group from top to bottom, metallic character

______because ______

_____19. I can state the periodic ______. trend for metallic character and As one reads across a period from left to right, metallic character explain why it occurs. ______because ______

______.

_____20. I can state the trend for As one reads down a group from top to bottom, the melting points and boiling melting points and boiling point for METALS as one reads down a points for METALS ______. group. _____21. I can state the trend for As one reads down a group from top to bottom, the melting points and boiling melting points and boiling point for NONMETALS as one reads points for NONMETALS ______. down a group. _____22. I can state the trend for As one reads down a group from top to bottom, the activity/reactivity of activity/reactivity for METALS as METALS ______. one reads down a group. _____23. I can state the trend for As one reads down a group from top to bottom, the activity/reactivity of activity/reactivity for NONMETALS NONMETALS ______. as one reads down a group. Metals tend to lose electrons (get oxidized). This loss of electrons causes

_____24. I can explain how loss or cations to be ______than the original atom. gaining of electrons affects the radius of an element. Nonmetals tend to gain electrons (get reduced). This gain of electrons causes

anions to be ______than the original atom. Ten properties of metals are:

_____25. I can list 10 properties of e. f. metals. g. h.

Eight properties of non metals are:

c. d. _____26. I can list 8 properties of nonmetals. e. f.

g. h. Unit 7: Acids & Bases

_____1. I can still do everything from Unit 1. _____2. I can still do everything from Unit 2. _____3. I can still do everything from Unit 3. _____4. I can still do everything from Unit 4. _____5. I can still do everything from Unit 5. _____6. I can still do everything from Unit 6. “Alternate Method” (AKA Arrhenius Bronsted-Lowry)

_____7. I can use two different systems to define acids and bases.

_____8. I can define pH, [ ], Definitions: hydronium ion, hydroxide ion, and pH electrolyte.

hydronium ion

hydroxide ion

electrolyte

_____9. I can state another name The hydronium ion is also known as the ______. for the hydronium ion. + -8 If the [H O ] is 1 x 10 , the pH of the solution will be______. 3

+ -1 If the [H O ] is 1 x 10 , the pH of the solution will be______. 3 _____10. Given the hydronium ion concentration, I can determine the + -14 pH. If the [H O ] is 1 x 10 , the pH of the solution will be______. 3

+ -7 If the [H O ] is 1 x 10 , the pH of the solution will be______. 3

If the pH of a solution is 4.5, the solution is ______.

_____11. Based on pH, I can determine if a solution is acidic, basic, or neutral. If the pH of a solution is 11, the solution is ______.

+ _____13. I can state the As the H concentration decreases , the pH ______. + relationship between H + concentration and pH. As the H concentration increases, the pH ______. + If the H concentration is increased by a factor of 10,

the pH will decrease by ______.

_____14. I can determine the + If the H concentration is increased by a factor of 100, + change in pH when the H concentration of a solution is the pH will decrease by ______. changed. + If the H concentration is decreased by a factor of 1000,

the pH will increase by ______. List the chemical names of three common acids and three common bases.

Acids Bases _____15. I can give examples of the chemical names of common acids and bases. List the chemical formulas of three common acids and three common bases.

Acids Bases

_____16. I can give examples of chemical formulas of common acids and bases.

Definition: neutralization _____17. I can define neutralization.

Which of the following equations is a neutralization reaction?

A) 6Na + B O -----> 3Na O + 2 B _____18. I can identify a 2 3 2 neutralization reaction from a list B) Mg(OH) + 2HBr -----> MgBr + 2HOH of reactions. 2 2 C) 2H + O -----> 2H O 2 2 2 D) 2KClO -----> 2KCl + 3O 3 2 _____19. I can state the name of Which piece of laboratory equipment is used to carry out a titration? the laboratory equipment that is used to carry out a titration. Why do scientists do titrations? _____20. I can state the purpose of titration.

If it requires 56.95 mL of 0.0043 M HNO to neutralize 34.56 mL of LiOH, 3 what is the concentration of the LiOH? _____21. I can solve for any variable in the titration equation from Reference Table T.

_____22. I can state the three types of substances that are ______, ______, and ______are three electrolytes. classes of compounds that are electrolytes. _____23. Given the pH, I can Which indicator is red in a solution that has a pH of 3.6? determine the color of acid-base indicators. A) bromcresol green

B) bromthymol blue

C)litmus D) thymol blue Unit 8: Redox & Electrochemistry

_____1. I can still do everything from Unit 1. _____2. I can still do everything from Unit 2. _____3. I can still do everything from Unit 3. _____4. I can still do everything from Unit 4. _____5. I can still do everything from Unit 5. _____6. I can still do everything from Unit 6. _____7. I can still do everything from Unit 7. Definitions: oxidation

reduction _____8. I can define oxidation, reduction, oxidation number, and oxidation number redox reaction

redox reaction

Assign oxidation number to each of the elements below. _____9. I can assign oxidation numbers to any element. O ______Li______Si______2 Assign oxidation numbers to each element in the compounds below. _____10. I can assign oxidation MnCl : Mn______Cl______numbers to the elements in a 3 compound. H SO : H______S______O______2 4 Assign oxidation numbers to each element in the polyatomic ions below.

3- _____11. I can assign oxidation PO : P______O______4 numbers to the elements in a polyatomic ion. - ClO : Cl______O______3 Which half-reaction equation represents the reduction of a potassium ion?

+ - A) K + e -----> K - + B) K + e -----> K + - C) K -----> K + e + - D) K -----> K + e

_____12. I can distinguish between an oxidation half-reaction and a reduction half-reaction.

The law of Conservation of Charge states _____13. I can state the Law of Conservation of Charge.

The two half-reactions that come from the following equation are:

Li(s) + Ag+(aq) -----> Li+(aq) + Ag(s)

_____14. I can break a redox oxidation half-reaction reaction into its two half-reactions.

reduction half-reaction Given the reaction:

2+ - _____Cl (g) + _____Fe (aq) -----> _____Fe(s) + _____Cl (aq) 2

When the equation is correctly balanced using smallest whole numbers, the - coefficient of Cl will be

A) 1 B) 2 C) 6 D) 7

_____15. I can balance a redox reaction.

_____16. I can identify a redox reaction from a list of chemical reactions.

_____17. From a list of given list of Which of the following elements is most likely to react? elements, I can determine which element is most active. A) Cu B) Al C) Li D) Mg

The two types of electrochemical cells are: _____18. I can state the two types of electrochemical cells. ______and ______

Voltaic Electrolytic

Components

_____19. I can compare the two Oxidation occurs at the types of electrochemical cells in terms of: components, location of Reduction occurs at oxidation, location of reduction, the direction of electron flow, Electrons flow from conversion between electrical and chemical energy, and spontaneity of reaction. Energy conversion that occurs in this cell

Is this reaction spontaneous or does it require an outside power source to happen?

The purpose of the salt bridge is _____20. I can state the purpose of the salt bridge in a voltaic cell.

_____21. Given an electrochemical cell, I can predict the direction of electron flow.

_____22. I can explain, in terms of Explain, in terms of atoms and ions, why the mass of the cathode increases atoms and ions, the changes in during the operation of an electrochemical cell. mass that take place at the anode and cathode of an electrochemical Explain, in terms of atoms and ions, why the mass of the anode decreases during the operation of an electrochemical cell. cell.

Unit 10: Chemical Reactions

_____1. I can still do everything from Unit 1. _____2. I can still do everything from Unit 2. _____3. I can still do everything from Unit 3. _____4. I can still do everything from Unit 4. _____5. I can still do everything from Unit 5. _____6. I can still do everything from Unit 6. _____7. I can still do everything from Unit 7. _____8. I can still do everything from Unit 8. Write the chemical formula for the following compounds: _____9. Given the IUPAC name, I can write the chemical formula for sodium bromide______lithium selenide______binary compounds. iron (III) fluoride______vanadium (V) oxide______Write the IUPAC name for the following compounds: _____10. Given the chemical formula, I can write the IUPAC CrO______name for binary compounds. MgI ______2 Write the chemical formula for the following compounds: _____11. Given the IUPAC name, I can write the chemical formula for calcium oxalate______ternary compounds. nickel (II) thiosulfate______Write the IUPAC name for the following compounds: _____12. Given the chemical Sn(C H O ) ______formula, I can write the IUPAC 2 3 2 2 name for ternary compounds. (NH ) PO ______4 3 4 _____13. I can state the three The three types of chemical formulas are: types of chemical formulas. ______, ______, & ______Definitions: empirical formula

_____14. I can define empirical molecular formula formula, molecular formula, and hydrate.

hydrate

What is the molecular formula of a compound that has the empirical formula of CH and a molar mass of 78 g/mol. _____15. Given the empirical formula and the molar mass, I can determine the molecular formula of a compound.

Using the symbols shown below, complete the equation below to illustrate conservation of mass.

_____16. I can use particle diagrams to show conservation of 2Al + 3Br -----> 2AlBr mass in a chemical equation. 2 3

Balance the following chemical equation using the lowest whole number _____17. I can balance a chemical coefficients. equation showing conservation of mass using the lowest whole _____Al (SO ) + _____Ca(OH) -----> _____Al(OH) + _____CaSO number coefficients. 2 4 3 2 3 4

_____18. Given a partially Use the law of conservation of mass to predict the missing product. balanced equation, I can predict 2NH Cl + CaO -----> 2NH + ______+ CaCl the missing reactant or product. 4 3 2 Classify the following reactions as synthesis, decomposition, single _____19. Given a list of chemical replacement, or double replacement. reactions, I can classify them as being a synthesis reaction, decomposition reaction, single replacement reaction, or double replacement reaction. Given the following balanced equation, state the mole ratios between the requested substances.

C H (g) + 5O (g) -----> 3CO (g) + 4H O(l) 3 8 2 2 2

The mole ratio between C H and O is ______C H :______O . _____20. Given a balanced 3 8 2 3 8 2 equation, I can state the mole The mole ratio between C H and CO is ______C H :______CO . ratios between any of the 3 8 2 3 8 2 reactants and/or products. The mole ratio between C H and H O is ______C H :______H O. 3 8 2 3 8 2

The mole ratio between CO and O is ______CO :______O . 2 2 2 2

The mole ratio between H O and CO is ______H O:______CO . 2 2 2 2

Definition: stoichiometry _____21. I can define stoichiometry.

Using the equation from question #20, determine how many moles of O are 2 needed to completely react with 7.0 moles of C H . 3 8 _____22. Given the number of moles of one of the reactants or products, I can determine the number of moles of another Using the equation from question #20, determine how many moles of CO are reactant or product that is needed 2 to completely use up the given produced when 7.0 moles of C H completely react. 3 8 reactant/product.

_____23. Given the mass or Using the equation from question #20, determine how many liters of O at STP 2 volume of one of the reactants or are needed to react completely with 88.0 g of C H . products, I can determine the mass 3 8 or volume of another reactant or product that is needed to completely use up the given reactant/product. NOT NEEDED FOR REGENTS

Using the equation from question #20, determine how many grams of H O are 2 produced when 88.0 g of C H completely react. 3 8 Unit 11: Bonding & IMF

_____1. I can still do everything from Unit 1. _____2. I can still do everything from Unit 2. _____3. I can still do everything from Unit 3. _____4. I can still do everything from Unit 4. _____5. I can still do everything from Unit 5. _____6. I can still do everything from Unit 6. _____7. I can still do everything from Unit 7. _____8. I can still do everything from Unit 8. _____9. I can still do everything from Unit 10. The three types of chemical bonds are: _____10. I can state the three ______, ______, and types of chemical bonds. ______. _____11. I can state the number of valence electrons that an atom Atoms are most stable when they have ______valence electrons. attains to be most stable.

_____12. I can state the two types The two types of compounds are ______and of compounds. ______. _____13. I can define ionic bond, Definition: covalent bond, and metallic bond ionic bond in terms of the types of elements (metals, nonmetals) from which they are formed. covalent bond

metallic bond

Definition: In an ionic bond, the valence electrons of the ______are

______to the ______so that each atom _____14. I can define ionic and attains a stable octet (like noble gases). covalent bonds based on what happens to the valence electrons. In a covalent bond, the valence electrons of the two ______

are ______so that each atom attains a stable octet (like noble gases). _____15. I can explain TICS as it TICS stands for ______. relates to chemical bonding. It helps me remember what happens to the electrons in each type of bond. NOT an acronym we used in class Explain, in terms of valence electrons, why the bonding in methane (CH ) is 4 similar to the bonding in water (H O). 2

_____16. In terms of valence electrons, I can find similarities and differences between the Explain, in terms of valence electrons, why the bonding in HCl is different than bonding in several substances. that bonding in NaCl.

Draw Lewis dot diagrams for the following ionic compounds.

LiBr CaCl _____17. I can draw a Lewis dot 2 diagram to represent an ionic compound.

Draw Lewis dot diagrams for the following molecular substances.

H O CO 2 2

_____18. I can draw a Lewis dot diagram to represent a molecular (covalently bonded) compound. I CH 2 4 In a single covalent bond, ______electrons are shared. _____ 19. I can state the number of electrons that are shared in In a double covalent bond, ______electrons are shared. single and multiple covalent bonds. In a triple covalent bond, ______electrons are shared.

Lewis dot diagrams for ionic compounds have brackets because _____20. I can explain why the Lewis dot diagrams of ionic ______. compounds have brackets and the Lewis dot diagrams of molecular Lewis dot diagrams for molecular compounds do NOT have brackets because compounds do not. ______. _____21. I can state the type of bonding that occurs in the Polyatomic ions have ______bonding because polyatomic ions (Reference Table E) and explain why they have that ______. type of bonding. State the type(s) of bonding in the following compounds: _____22. Given the chemical formula for a compound, I can NaCl______CO______determine the type(s) of bonding in the compound. Hg______Na PO ______&______3 4 _____ 23. I can explain and apply the meaning of BARF as is applies BARF stands for ______to chemical bonding. This means that when a bond is FORMED, energy is ______and when a bond is BROKEN, energy is ______.

Given the balanced equation: N + N -----> N 2 Which statement describes the process represented by this equation?

A) A bond is formed as energy is absorbed. B) A bond is formed as energy is released. C) A bond is broken as energy is absorbed. D) A bond is broken as energy is released. _____24. I can explain the difference between a polar Polar covalent bonds are formed when ______covalent bond and a nonpolar nonmetals share electrons unevenly. covalent bond in terms of the types of nonmetals involved. Nonpolar covalent bonds form when ______nonmetals share electrons evenly.

_____25. I can explain how to The degree of polarity of a covalent bond is determined by the determine the degree of polarity of a covalent bond. ______between the elements. .

_____26. I can explain why one Explain, in terms of electronegativity difference, why the bond between carbon covalent bond is more or less polar and oxygen in a carbon dioxide molecule is less polar than the bond between than another covalent bond, based hydrogen and oxygen in a water molecule. on electronegativity difference.

_____27. I can define symmetrical Definition: and asymmetrical. symmetrical

asymmetrical

_____28. I can determine if a When determining if a MOLECULE is polar or non-polar, the question to MOLECULE is polar or nonpolar. ask is______

_____29. I can explain and apply the meaning of SNAP as it applies SNAP means______to determining molecule polarity. NOT an acronym we used in class Why is a molecule of CH nonpolar even though the bonds between the 4 carbon and hydrogen are polar?

A) The shape of the CH molecule is symmetrical. 4 B) The shape of the CH molecule is asymmetrical. 4 C) The CH molecule has an excess of electrons. 4 D) The CH molecule has a deficiency of electrons. 4

Explain, in terms of charge distribution, why a molecule of water (H O) is 2 polar. _____30. I can determine if a Determine which molecules are polar and which are nonpolar. Justify your molecular is polar or nonpolar. answer.

H O CO 2 2

I CH 2 4

_____31. I can explain and apply “Like dissolves like” means the expression “like dissolves like” and give an example.

An example of “like dissolving like” is ______

______

Explain, in terms of molecular polarity, why ammonia is more soluble than o methane in water at 20 C at standard pressure.

_____32. I can define Definition: intramolecular forces and Intramolecular forces intermolecular forces and give examples of each.

Examples:

Intermolecular forces

Examples:

_____33. I can list the intramolecular forces from STRONGEST to WEAKEST. Strongest______bonds>______bonds Weakest _____34. I can list the intermolecular forces from Strongest______> ______> STRONGEST to WEAKEST. ______Weakest

_____35. I can state 8 physical Eight physical properties that are dependent on the type of bonding and the properties of substances that are strength of the IMF are: dependent on the type of bonding in the substance and the strength 1.______2.______of the IMF. 3.______4.______

5.______6.______

7.______8.______

_____36. I can state the relationship between polarity and As the polarity of the molecule ______, the strength IMF strength. of the IMF ______.

_____37. I can state the relationship between size of the As the size of the molecule______, the strength molecule and IMF strength. of the IMF ______.

_____38. Given the physical state At STP, iodine (I ) is a crystal and fluorine (F ) is a gas. Compare the strength 2 2 of some substances, I can compare of the IMF in a sample of I at STP to the strength of the IMF in a sample of F the relative strength of the IMF. 2 2 at STP.

_____39. Given the boiling points o o At STP, CF boils at -127.8 C and NH boils at -33.3 C. Which substance has (or freezing points) of some 4 3 substances, I can compare the stronger IMF? Justify your answer. relative strength of the IMF.

_____40. I can explain and apply the meaning of “Hydrogen bonding “Hydrogen bonding is FON” is FON”. means______

______Which compound has hydrogen bonding between its molecules?

A) CH B) CaH C) KNO D) H O 4 2 3 2 _____41. I can define normal Definition: boiling point, vapor pressure, normal boiling point volatile, and nonvolatile.

vapor pressure

volatile

nonvolatile

_____42. I can determine the o What is the vapor pressure of ethanol at 56 C? vapor pressure of ethanol, ethanoic acid, propane, or water at a given temperature.

_____43. I can state the relationship between the strength As the strength of IMF ______, vapor pressure of IMF and vapor pressure. ______.

_____44. I can explain the how When a nonvolatile solute is added to a solvent, the freezing point of the adding a nonvolatile solute to a pure solvent affects the freezing solvent ______because the solute ______point of the solvent. ______

The more solute that is added, the ______the feeezing point gets.

____45. I can explain the how When a nonvolatile solute is added to a solvent, the boiling point of the adding a nonvolatile solute to a pure solvent affects the boiling solvent ______because the solute ______point of the solvent. ______

The more solute that is added, the ______the boiling point gets. _____46. I can state 5 physical Five physical properties of ionic substances are: properties of ionic substances. 1.______

2.______

3.______

4.______

5.______

_____47. I can identify a substance A solid substance was tested in the laboratory. The results are shown below. as “ionic” based on its properties. *dissolves in water *is an electrolyte * has a high melting point

Based on these results, the solid substance could be

A) Hg B) AuCl C) CH 4 D) C H O 12 22 11

Based on bond type, which compound has the highest melting point?

A) CH B) C H O C)NaCl D) C H 4 12 22 11 5 12 _____48. I can state 5 physical Five physical properties of molecular substances are: properties of molecular substances. 1.______

2.______

3.______

4.______

5.______49. I can identify a substance as “molecular” based on its properties. Unit 12: Reaction Rates & Equilibrium

_____1. I can still do everything from Unit 1. _____2. I can still do everything from Unit 2. _____3. I can still do everything from Unit 3. _____4. I can still do everything from Unit 4. _____5. I can still do everything from Unit 5. _____6. I can still do everything from Unit 6. _____7. I can still do everything from Unit 7. _____8. I can still do everything from Unit 8. _____9. I can still do everything from Unit 10. _____10. I can still do everything from Unit 11. Definition: effective collision

_____11. I can define effective collision and collision theory collision theory

_____12. I can state and apply the relationship between temperature As the temperature ______, the reaction rate for most and reaction rate in terms of collision theory. chemical reactions ______because there are ______

effective collisions between particles.

Given the reaction:

2Mg(s) + O (g) -----> 2MgO(s) 2

At which temperature would the reaction occur at the greatest rate? o o o A) 0 C B) 15 C C) 95 C D) 273K

As the surface area ______, the reaction rate

______because there are ______13. I can state and apply the effective collisions between particles. relationship between surface area and reaction rate in terms of At STP, which 4.0 g sample of Zn(s) will react most quickly with dilute collision theory. hydrochloric acid?

A) lump B) bar C) powdered D) sheet metal

As the concentration ______, the reaction rate

______because there are ______effective _____14. I can state and apply the collisions between particles. relationship between concentration and reaction rate in o terms of collision theory. At 20 C, a reaction between powdered Zn(s) and hydrochloric acid will occur most quickly if the concentration of the HCl is

A) 1.0 M B) 1.5 M C) 2.5 M D) 2.8 M

_____15. I can state the unit used Energy is measured in ______. to measure energy. Given the following balanced equation:

I + I -----> I + 146.3 kJ _____16. Based on the location of 2 the energy term, I can determine if the reaction is exothermic or Is this reaction exothermic or endothermic? Justify your answer. endothermic.

_____17. I can use Table I to determine if a reaction is exothermic or endothermic. _____19. I can define potential Definitions: energy diagram, reaction potential energy diagram coordinate, PE , PE , reactant product heat of reaction (H), activation energy, catalyst. reaction coordinate

PE reactant

PE product

heat of reaction (H)

activation energy

catalyst

entropy

_____20. Given a potential energy Give the potential energy diagram below, determine if the reaction is diagram, I can determine if the exothermic or endothermic. Justify your answer. reaction is exothermic or endothermic.

_____21. Given a potential energy Given the potential energy diagram below, determine the PE , reactant diagram, I can determine the PE , H, and the activation energy. PE , PE , H, and product reactant product activation energy.

PE = PE = reactant product

H = activation energy =

_____22. Given a potential energy Draw a dotted line on the potential energy diagram shown below to indicate diagram for an uncatalyzed how it will change if a catalyst is added. reaction diagram, I can how the diagram will change when a catalyst is been added.

_____23. I can rank the three phases of matter from least Least entropy Most entropy entropy to most entropy. ______<______<______

_____24. I can state the trends in In nature most systems in nature tend to undergo reactions that have a(n) nature for entropy and energy. ______in entropy and a(n) ______in energy. As Mrs. S says, nature is like a teenager ---- lazy and messy! _____25. Given a balanced equation, I can determine if the reaction results in an overall increase or decrease in entropy.

_____26. I can define forward Definitions: reaction, reverse reaction, forward reaction reversible reaction, and closed system

reverse reaction

reversible reaction

closed system

_____27. I can state the three The three types of equilibrium are: types of equilibrium. ______equilibrium

______equilibrium and

______equilibrium

_____28. I can state two conditions that apply to all In a system at equilibrium the ______of the forward and systems at equilibrium. reverse reaction must be ______and the ______of the reactants and products must be ______. _____29. Given a list of reactions, Which balanced equation represents phase equilibrium? I can identify reactions that show A) H (g) + I (s) <-----> 2HI(g) equilibrium (chemical, phase, or 2 2 solution). B) I (s) <-----> I (g) 2 2

C) KCl(s) <-----> KCl(aq) D) 2KCl(s) + 3O (g) -----> 2KClO 2 3

Which balanced equation represents solution equilibrium? A) H (g) + I (s) <-----> 2HI(g) 2 2

B) I (s) <-----> I (g) 2 2

C) KCl(s) <-----> KCl(aq) D) 2KCl(s) + 3O (g) -----> 2KClO 2 3

Which balanced equation represents chemical equilibrium? A) H (g) + I (s) <-----> 2HI(g) 2 2

B) I (s) <-----> I (g) 2 2

C) KCl(s) <-----> KCl(aq) D) 2KCl(s) + 3O (g) -----> 2KClO 2 3 _____30. In terms of saturation, I In terms of saturation, a solution that is at equilibrium must be can describe a solution that is at equilibrium. ______.

_____31. I can state LeChatelier’s LeChatelier’s Principle states Principle.

_____32. Given a balanced Given the reaction at equilibrium: equation at equilibrium, I can predict the direction of shift in the equilibrium when the 2SO (g) + O (g) <-----> 2SO (g) + 392kJ temperature, concentration, or 2 2 3 pressure is changed or if a catalyst is added. Predict the direction of shift in the equilibrium (right, left, no shift) when the following changes are made to the system.

Change Direction of Shift Increase concentration of SO 2 Increase concentration of SO 3 Increase temperature Increase pressure Add a catalyst

Unit 13: Organic Chemistry

_____1. I can still do everything from Unit 1. _____2. I can still do everything from Unit 2. _____3. I can still do everything from Unit 3. _____4. I can still do everything from Unit 4. _____5. I can still do everything from Unit 5. _____6. I can still do everything from Unit 6. _____7. I can still do everything from Unit 7. _____8. I can still do everything from Unit 8. _____9. I can still do everything from Unit 10. _____10. I can still do everything from Unit 11. _____11. I can still do everything from Unit 12. _____12. I can define organic Definitions: compound, saturated organic compound hydrocarbon, unsaturated hydrocarbon, and isomer.

saturated hydrocarbon

unsaturated hydrocarbon isomer Draw the complete structural formula for CH CH CH CH CH . 3 2 2 2 3

_____13. I can expand a condensed structural formula to show the structural formula of an Draw the complete structural formula for CH CHCHCH . organic compound. 3 3

_____14. I can state the name and The element that is capable of forming rings, chains, and networks is symbol of the element that is capable of forming rings, chains, ______. Its symbol is______. and networks. HONC1234 tells me that

_____15. I can explain the meaning of and apply HONC1234.

_____16. Given the formula, I can determine if a compound is a hydrocarbon or not.

Determine how many carbon atoms are in each of the following compounds: _____17. Given the name, I can use Reference Table P to decane______ethene______determine how many carbons atoms are in a compound. 3-nonene______1-pentyne______

Determine the homologous series of hydrocarbons to which each of the _____18. Given the name, I can following belongs: use Reference Table Q to determine to which class of decane______2-decene______hydrocarbons a compound belongs. 3-nonene______1-pentyne______

_____19. Given the name, I can Determine if each of the following is a saturated or unsaturated hydrocarbon. determine if the hydrocarbon is saturated or unsaturated. decane______ethene______3-nonene______1-pentyne______Determine the homologous series of hydrocarbons to which each of the following belongs:

belongs to the ______series.

_____20. Given the formula, I can determine to which homologous series a hydrocarbon belongs. belongs to the ______series.

belongs to the ______series.

Determine if each of the following is a saturated or unsaturated hydrocarbon.

_____21. Given the formula, I can determine if a hydrocarbon is CH CH CH CH ______3 2 2 3 saturated or unsaturated. CH CHCHCH ______3 3 Determine the number of hydrogen atoms in each of the following. _____22.Given the name, I can use Reference Table Q to determine decane______1-butene______how many hydrogen atoms the hydrocarbon contains. 3-nonene______1-pentyne______

_____23. Given a list of compounds, I can determine which ones are isomers.

_____24. Given a structural formula, I can use Reference Table R to identify to which class of organic compounds a substance belongs.

_____25. I can use Reference Name the following hydrocarbons. Tables P & Q and IUPAC nomenclature to name simple hydrocarbons.

Name the following organic compounds.

_____26. I can use Reference Tables P & R and IUPAC nomenclature to name simple compounds in any of the classes of organic compounds.

_____27. I can use F-SCAPES to list and describe the 7 types of organic F stands for______. This type of organic reactions. NOT an acronym we used in class reaction results from a reaction of ______to form

______and ______. It typically requires a catalyst, in the form of an enzyme to occur.

S stands for ______. This type of organic

reaction happens when ______hydrocarbons

replace one of the ______for some other element (often a halide).

C stands for ______. In this type of organic

reaction a ______reacts with

______to form ______and

______. It is an exothermic reaction.

A stands for ______. In this type of organic reaction

an ______becomes a ______when the double bond breaks and two atoms of another element (often a halide) are added.

P stands for ______. In this type of organic

reaction many ______are linked together to form a

______. A generalized form of this reaction looks like this…..

_____27. I can use F-SCAPES to list and describe the 7 types of organic reactions. (continued) E stands for ______. In this type of organic

reaction an ______reacts with a

______to form an ______and

______. The products of this reaction are typically fragrant.

S stands for ______. In this type of organic

reaction a ______reacts with a ______to form

______. You can really “clean up” if you remember this organic reaction. _____28. Given an equation, I can identify the type of organic reaction that is occurring.