A. Calculate Density When Given a Means to Determine a Substance S Mass and Volume

SPS2: Students explore the nature of matter, its classifications, the naming system for types of matter. a. Calculate density when given a means to determine a substance’s mass and volume. . Density=Mass/Volume: remember My Dear Valentine. . Solve the following: o A student determines that a piece of an unknown material has a mass of 5.854 g and a volume of 7.57 cm3. What is the density of the material? o In science lab you are given a rectangular shaped solid made from some synthetic (manmade) substance. Its dimensions are 3.5 cm by 2.4 cm by 14.6 cm. If this substance masses 20 g, what is its density in g/cm3? (DA) b. Predict formulas for stable binary ionic compounds based on balance of charges. 1. Find the charge for each element based on what group it is in. (Group 1= +1 charge) +2 -1 2. Criss-Cross the charges to make the correct formula. Ca + Cl = CaCl2 c. Use IUPAC nomenclature for transition between chemical names and chemical formulas of  Binary ionic compounds (containing representative elements).  Steps for writing Binary Ionic Compounds: 1. Write the symbol for the ions side by side. Write the ______first. 2. Cross over the charges by using the ______as the subscripts for the other ion. 3. Check the subscripts and divide them by their largest common factor to give the smallest possible whole number-ratio of ions.  (2 x +3 = +6 and 3 x-2 = -6 which cancel each other out)  Binary covalent compounds (i.e. carbon dioxide, carbon tetrachloride).  Naming Covalent Compounds-USES ______!!!  1. The less electronegative element is given first. Take the ______of the first element and change it to the correct prefix; do not use the prefix ______ 2. The second element is named by combining (a) a prefix indicating the number of atoms contributed by the element, (b) the root of the name of the second element, and (c) the ending –ide. With few exceptions, the ending –ide indicates that a compound contains only two elements.  3. The “o” or “a” at the end of a prefix is usually dropped when the word following the prefix begins with another vowel. Ex: monoxide or pentoxide  Ex: P4O10

 Numerical Prefixes  1- 4- 7- 10-  2- 5- 8-  3- 6- 9-

 Fill in the missing information for the following compounds.  ELEMENTS TYPE OF NAME FORMULA COMPOUND N2F4 Copper (II) & sulfur

Sulfur dichloride

Magnesium and oxygen Barium & fluorine

d. Demonstrate the Law of Conservation of Matter in a chemical reaction. State the Law of Conservation of Matter______

______. . Steps for balancing an Equations- RAP TABLE! . 1. Divide the equation in half. Reactants on the left and Products on the right. . 2. Count the number of atoms for EACH element on the Reactants side. . 3. Count the number of atoms for EACH element on the Products side. o Hint: if you write them in the same order on each side it is easier to see what needs to be balanced. . IMPORTANT: you can only add/change the coefficient, not the subscript (the little number). . 4. Write the newly balanced equations with the Coefficients. Examples:

Balance the following equations:

____ P4 + ____ O2  ____ P2O3

____ N2 + ____ H2  ____ NH3

____ Al + ____ HCl  ____ H2 + ____ AlCl3

2 e. Apply the Law of Conservation of Matter by balancing the following types of chemical equations:

 Synthesis ______o Ex. Element + ElementCompound or o A +B= AB o 2Na + Cl2= 2NaCl ______Na + ______Br2 → ______NaBr

 Decomposition is______o COMPOUND __Element___ + ___Element__ or o COMPOUND  _Compound_____ + __Compound____ o AB=A + B or 2 H2O= 2H2 + O2

______Al2O3 →______Al + ______O2

 Single Replacement is______o ELEMENT + COMPOUND ELEMENT + COMPOUND o A+BC = B+AC o Cu+2AgNO3=2Ag+Cu(NO3)2 o ______Cl2 + ______NaBr → ______NaCl + ______Br2

 Double Replacement is______o COMPOUND + COMPOUND COMPOUND + COMPOUND o AB+CD=AD+CB o CaCO3+2HCl=CaCl2+H2CO3

______CuCl2 + ______H2S → ______CuS + ______HCl IDENTIFY THE FOLLOWING EQUATIONS:

1. C4H8 + 6O2 ---> 4CO2 + 4H2O 2. HCl + NaOH ---> H2O + NaCl

3. 2KNO3(s) ---> 2KNO2(s) + O2(g) 4. AgNO3 + NaCl ---> NaNO3 + AgCl

5. 2Mg + O2 ---> 2MgO 6. 2Ag + S ---> Ag2S

7. MgCO3(s) ---> MgO(s) + CO2(g) 8. Cl2 + 2KBr ---> 2KCl + Br2

SPS6 SPS6. Students will investigate the properties of solutions. a. Describe solutions in terms of A ______is a special type of mixture. It has a uniform composition throughout and is made up of two parts—a solute and a solvent.  Solute-  Solvent- o Saturated Solution o Unsaturated Solution  Conductivity- The conductivity gives important clues as to the type of solute dissolved. In aqueous (water based) solutions, dissolved ionic compounds yield solutions with high conductivity. Cations and anions readily carry electrical charges through the solution. Strong acids and bases also have a high conductivity for the same reason. All of these solutions are considered ______electrolytes. Weak acids or bases ionize only partially so they form solutions with low conductivity. These compounds are called ______electrolytes. Solutions made from covalent compounds have zero conductivity since they dissolve as molecules, not ions. They cannot carry electrical charges. These substances are known as______.  Concentration-

b. Observe factors affecting the rate a solute dissolves in a specific solvent. There are three factors that affect the rate at which a solution dissolves. They are Agitation Size of Particles Temperature Define: Define: Define:

Affect: Affect: Affect: c. Demonstrate that solubility is related to temperature by constructing a solubility curve. What is a solubility curve?

What is the solubility of Potassium Chloride (KCl) at 45◦ C?

Which compound is a gas?

Look at Calcium chloride. At 10 C, there are 450g of solute dissolved into 100 g of water. Is this solution saturated or unsaturated? How do you know this?

d. Compare and contrast the components and properties of acids and bases. Acids Bases Definition Taste Touch Reacts with Metals Electrical Conductivity Litmus Paper Test Ph Scale e. Determine whether common household substances are acidic, basic, or neutral. List 5 common acids: List 5 common bases:

What is an example of a neutral substance? What is its pH?

What are the products of a neutralization reaction?