Unit 5: Chemical Names & Formulas

Unit 5: Chemical Names & Formulas (Chapter 9)

2 Monatomic Ion Formation & Nomenclature

Monatomic Ions consist of a ______atom with a positive or negative charge resulting from the gain or loss of one or more valence ______.

Cation: any atom or group of atoms with a ______charge. Cations are formed by ______one or more electrons. ______form cations!

Group 1A and Group IIA form cations with positive charges equal to their ______.

Group IA metals are always ______Group IIA metals are always ______

Anion: any atom or group of atoms with a ______charge. Anions are formed by ______one or more electrons. ______form anions!

The charge of any Group A nonmetal is determined by subtracting ____ from the ______.

Group VIA nonmetals are always ______Group VIIA nonmetals are always ______.

Using the periodic table below, label the elements whose ionic charges can be determined from their positions on the table.

3 Symbol Formula Change in Electrons Name of Ion of Ion

Ca ______

F ______

Al ______

O ______

Na ______

P ______

Ar ______

C ______

H ______

______

Many transition metals and representative elements can form more than one cation. Since the metal can form more than one ion, the name of the ion must include the charge in order to distinguish between the two. This charge is indicated by placing a Roman numeral after the name of the metal.

EX: Lead can form both +2 and +4 ions. They are called ______and ______.

It is important to note that when a metal forms only one possible ion, a Roman numeral is NOT needed and NEVER used in the name. We do not call Ca+2 the calcium II ion, because the +2 charge on the calcium ion is understood.

The following metals NEVER have a Roman numeral in their name because they can form only one ion:

Group 1A metals are always ______Group 11A metals are always ______.

Al is always ______Zn & Cd are always ______Ag is always ______

There is a pattern to help you remember these last three:

4 Symbol Formula of Ion Name of Ion

Cr Cr+2 ______

______chromium III

Ga ______gallium I

______Ga+3 ______

Bi ______bismuth III

______Bi+5 ______

The method used above to name the ions of metals that exhibit more than one charge was devised by the International Union of Pure and Applied Chemistry (IUPAC) and is called the Stock System.

There is another method that can be used to name these ions. In classical nomenclature, when a metal forms more than one cation, the name of the metal (usually the Latin name) is modified with the suffixes -ous and -ic to distinguish between the two. The lower charge cation is given the -ous ending and the higher one, the -ic ending.

EX: Pb+2 ~ the lower charge, is called plumbous. Pb+4 ~ the higher charge, is called plumbic.

In addition to lead, you are responsible for naming the metals listed below in both systems:

Stock Classical

Cu+1 ______cuprous Cu+2 ______Children Hg+1 ______mercurous Hg+2 ______Have Fe+2 ______Fe+3 ______ferric Fun Pb+2 ______

+4 Pb ______Practicing Sn+2 ______Sn+4 ______stannic Science

6 Naming Monatomic Ions

1. Metals that form only 1 common ion: element name + ion  found in groups 1A (+1), 2A (+2), Al+3,Zn+2, Cd+2, Ag+1  always a positive charge  EX: Na+ is called the sodium ion

2. Nonmetals (always only form 1 common negative ion): drop end of element’s name and add “ide” + ion  found in groups 5A, 6A, 7A  negative charge equals (8 - group #)  EX: O-2 is called the oxide ion

3. Metals that form more than 1 common ion: Stock system - use Roman numerals or Classical method - change ending to “ous” or “ic”  found in groups 3A (except aluminum), 4A, 5A, and the transition metals (except Ag+1,Zn+2 and Cd+2)  always a positive charge  EX: Stock System — Pb+2 lead (II) ion Pb+4 lead (IV) ion  EX: Classical Method — Pb+2 plumbous ion Pb+4 plumbic ion  always use one of these methods (stock or classical) when naming transition metals (except for the 3 listed above!)

7 1. What is the common charge of the following elements? (For metals with more than one common ionic charge, the number of electrons lost is indicated.)

a. Zn ______b. S ______c. P ______

d. Br ______e. Cd ______f. Se ______

g. Pb (4 electrons lost) ______h. Sn (2 electrons lost) ______

i. Cu (1 electron lost) ______j. Fe (3 electrons lost) ______

2. Name the ions in problem 1. (WRITE BOTH POSSIBLE NAMES FOR G-J.)

a. ______b. ______c. ______

d. ______e. ______f. ______

g. ______h. ______i. ______

______

j. ______

______

3. What are the possible charges on the following metals? Be sure to list all of them.

a. copper ______b. iron ______

c. tin ______d. mercury ______

e. silver ______f. lead ______

4. Write the symbol and charge of each of the following ions.

a. cuprous ion ______b. iodide ion ______

c. plumbic ion ______d. stannic ion ______

e. ferrous ion ______f. sodium ion ______

g. chromium III ______h. nitride ion ______

8 : 1. Examine the data table. 2. Cut out the paper squares of each cation and anion separately. 3. Using the ion models, build the model of the formula. Remember, the total of positive charges must equal the total of negative charges. 4. Write the formula for the compound formed by writing the symbol and indicating the number of ions in your model (if more than one) as a subscript. EXAMPLE: If the model contains one Ca ion and two F ions the formula would be ______5. Write the name of the compound. These compounds are named by writing the name of the first ion, which is the name of the element, followed by the name of the second element with the ending, “-ide.” For the example in #4, the name would be ______.

ELEMENTS FORMULA NAME sodium + chlorine

aluminum + bromine

calcium + iodine

barium + nitrogen

aluminum + fluorine

silver + nitrogen

aluminum + oxygen

potassium + sulfur

magnesium + sulfur

aluminum + phosphorus

1. What is a binary compound? (consult your text)

______

a. What are the components of a binary ionic compound?

______

b. Which of the compounds in the data table are binary ionic compounds?

______

2. What is a cation? An anion? (define below)

______

3. Name ALL of the substances you made which combined in a one-to-one ratio.

______

a. Why did they combine in a one-to-one ratio?

______

4. What does the total charge have to add up to in any correctly written formula for a compound?

______

+3 Na+1 +2 Na +1 Ba Al +2 K+1 Ba +3 +1 Al K Ba+2 +3 +2 Ca Mg+2 Al +2 Ca +2 +3 Mg Al +1 +2 Ag +1 Mg Ag +3 +1 Ag Al

-3 Br-1 -2 Br -1 O N -1 Br -2 -3 O Cl-1 -2 N Cl -1 O Cl -1 -3 -2 N I -1 S I -1 -2 I - 1 S -3 -2 -1 P F S F -1

F-1 -3 P -3 P

14 Writing Formulas and Naming Binary Ionic Compounds

1. What are the components of a binary ionic compound?

2. What is the ending of the name of a binary ionic compound?

3. What condition must be met in writing a “balanced” formula for a compound?

4. Write formulas for compounds formed form the following pairs of ions.

a. Sr+2, Se-2 ______c. Ca+2, N-3 ______

b. K+1, O-2 ______d. Co+3 , I-1 ______

5. Write formulas for the following compounds.

a. rubidium oxide ______e. sodium nitrate ______

b. barium oxide ______f. ferric chloride ______

c. potassium phosphide ______g. aluminum carbide ______

d. calcium fluoride ______h. gallium III selenide______

6. Name the following binary ionic compounds.

a. BaO ______e. Li3N ______

b. Na2S ______f. CuF ______

c. SnSe ______g. GeS2 ______

d. AlBr3 ______h. Fe2O3 ______

15 Writing Formulas and Naming Binary Ionic Compounds

Supply the missing information: either name or the ionic compound or write its formula.

1. Mg3P2 ______2. copper II sulfide ______

3. SrBr2 ______4. iron III chloride ______

5. Na3N ______6. rubidium oxide ______

7. ZnS ______8. calcium chloride ______

9. Pb2C ______10. chromium VI nitride ______

11. FeCl3 ______12. copper I oxide ______

13. AlF3 ______14. calcium bromide ______

15. Ag2O ______16. tin IV iodide ______

17. Cu2S ______18. cobalt II fluoride ______

19. CaSe ______20. mercury II telluride ______

21. CoI2 ______22. plumbic selenide ______

23. Cs2O ______24. stannic fluoride ______

25. SnCl4 ______26. ferrous oxide ______

27. Na3As ______28. mercurous chloride ______

29. Fe2O3 ______30. aluminum arsenide ______

31. NiBr2 ______32. cupric sulfide ______

33. AuCl3 ______34. lithium phosphide ______

35. HgS ______36. silver sulfide ______

37. Cd3N2 ______38. titanium III chloride ______

16 Write formulas for the following compounds:

1. magnesium bromide ______

2. iron II nitride ______

3. aluminum sulfide ______

4. stannic oxide ______

5. zinc phosphide ______

Write the name for each of the following compounds. If two names exist, write both.

6. AgCl ______

7. Li3P ______

8. Hg2S ______

9. BaF2 ______

10. CoO ______

Write the correct symbol and charge for the following ions.

1. ferric ______2. zinc ______3. barium ______

4. sulfide ______5. cupric ______6. phosphide ______

Write the correctly spelled name for the following ions:

7. Sn+4 (classical) ______

8. Ni+2 (stock) ______

9. I- ______

10. Pb+2 (classical) ______

11. O-2 ______

Name each binary ionic compound or write the proper formula.

12. arsenic (III) sulfide ______

13. sodium nitride ______

14. Fe3P2 ______

15. CaF2 ______

16. silver oxide ______

17. cuprous chloride ______

18. SnS ______

18 Common Polyatomic Ions +1 charge -1 charge

+ - ammonium ion NH4 acetate ion C2H3O2 - perchlorate ion ClO4 - chlorate ion ClO3 - chlorite ion ClO2 hypochlorite ion ClO- cyanide ion CN- hydroxide ion OH- - nitrate ion NO3 - nitrite ion NO2 - permanganate ion MnO4 - bicarbonate ion HCO3 (hydrogen carbonate ion)

-2 charge -3 charge

-2 -3 carbonate ion CO3 phosphate ion PO4 -2 -3 chromate ion CrO4 phosphite ion PO3 -2 dichromate ion Cr2O7 -2 peroxide ion O2 -2 sulfate ion SO4 -2 sulfite ion SO3

3A 4A 5A 6A 7A

B C N O F

Al Si P S Cl

Se Br

Te I

The “ate” polyatomic ions contain 3 oxygens

The “ate” polyatomic ions contain 4 oxygens

For the ions that you need to know, this method will work for predicting the charge:

If the root element is located in an column, the charge is .

If the root element is located in an column, the charge is , except for --the only one that is

20 Predicting Polyatomic Ions

The difference between –ate and –ite: The “–ite” form of any polyatomic ion can be determined by subtracting one oxygen from the “–ate” form.

-2 memorize the “-ate” SO4 sulfate ion -2 one less oxygen SO3 sulfite ion

Complete the following. - -3 - Nitrate = NO3 Phosphate = PO4 Chlorate = ClO3

Nitrite = ______Phosphite = ______Chlorite = ______

Follow this pattern for all halogen ions (fluorine, chlorine, bromine, & iodine):

- one more oxygen ClO4 perchlorate ion

- memorize the “-ate” ClO3 chlorate ion

- one less oxygen ClO2 chlorite ion

two less oxygens ClO- hypochlorite ion

no oxygens Cl- chloride ion

Complete the following.

Periodate ______Perbromate ______

- Iodate IO3 Bromate ______

Iodite ______Bromite ______

Hypoiodite ______Hypobromite ______

Iodide ______Bromide ______

22 CHEMICAL NAMES AND FORMULAS

SECTION 9.1 NAMING IONS (pages 253 – 258) This section explains the use of the periodic table to determine the charge of an ion. It also defines polyatomic ion and gives the names and formulas for the most common polyatomic ions.

Monatomic Ions (pages 253–256)

1. What are monatomic ions? ______

2. How is the ionic charge of a Group 1A, 2A, or 3A ion determined? ______

______

3. How is the ionic charge of a Group 5A, 6A, or 7A ion determined? ______

______

4. Circle the letter of the type of element that often has more than one common ionic charge.

a. alkali metal

b. alkaline earth metal

c. transition metal

d. nonmetal

5. The ______of naming transition metal cations uses a Roman numeral in

parentheses to indicate the numeric value of the ionic charge.

6. An older naming system uses the suffix -ous to name the cation with the ______charge,

and the suffix -ic to name the cation with the ______charge.

7. What is a major advantage of the Stock system over the old naming system? ______

______

23 CHAPTER 9, Chemical Names and Formulas (continued)

8. Use the periodic table to write the name and formula (including charge) for each ion in the table below.

Element Name Formula

Fluorine

Calcium

Oxygen

Polyatomic Ions (pages 257–258)

9. What is a polyatomic ion? ______

10. True or false: The names of polyatomic anions always end in -ide. ______

11. What is the difference between the anions sulfite and sulfate? ______

______

12. Look at Table 9.3 on page 257. Circle the letter of a polyatomic ion that is a cation.

a. ammonium

b. acetate

c. oxalate

d. phosphate

13. How many atoms make up the oxalate ion and what is its charge? ______

______

14. What three hydrogen-containing polyatomic anions are essential components of living

systems?

a. ______

b. ______

c. ______

15. Look at Figure 9.5 on page 257. Identify each of the ions shown below. +1 -3 -1 H H O O O N P H N H O O O O

a. ______b. ______c. ______

SECTION 9.2 NAMING AND WRITING FORMULAS FOR IONIC COMPOUNDS (pages 260–266)

This section explains the rules for naming and writing formulas for binary ionic compounds and compounds containing a polyatomic ion.

Binary Ionic Compounds (pages 260–263)

1. Traditionally, common names were based on some ______of a compound or

its ______.

2. What is the general name for compounds composed of two elements? ______

3. When writing the formula for any ionic compound, the charges of the ions must ______.

4. What are two methods for writing a balanced formula?

a. ______

b. ______

5. What are the formulas for the compounds formed by the following pairs of ions?

2+ - a. Fe , Cl ______

3+ 2- b. Cr , O ______

+ 2- c. Na , S ______

6. What are the formulas for these compounds?

a. lithium bromide ______

b. cupric nitride ______

c. magnesium chloride ______

7. The name of a binary ionic compound is written with the name of the ______

first followed by the name of the ______.

CHAPTER 9, Chemical Names and Formulas (continued)

8. How can you tell that cobalt (II) iodide is a binary ionic compound formed by a transition metal

with more than one ionic charge? ______

______

9. Write the names for these binary ionic compounds.

a. PbS ______

b. MgCl2 ______

c. Al2Se3 ______

Compounds with Polyatomic Ions (pages 264–266)

10. What is a polyatomic ion? ______

11. How do you write the formula for a compound containing a polyatomic ion? ______

______

12. Why are parentheses used to write the formula Al(OH)3?______

______

13. Complete the table for these ionic compounds containing polyatomic ions.

Cation Anion Name Formula

+ -2 NH4 S

+3 Fe iron(III) carbonate

- NO3 AgNO3

potassium cyanide KCN

26 Ternary Ionic Compounds

I. Write formulas for the following compounds.

1. sodium hydroxide ______2. mercuric bicarbonate ______

3. calcium hypochlorite ______4. lead II phosphate ______

5. aluminum chlorate ______6. ammonium dichromate ______

7. cuprous perchlorate ______8. mercury I nitrate ______

9. lead II acetate ______10. manganese III sulfite ______

11. stannic carbonate ______12. silver peroxide ______

13. zinc sulfate ______14. chromium III nitrite ______

15. ammonium phosphite ______16. ferrous cyanide ______

17. potassium permanganate ______18. magnesium chromate ______

II. Name the following compounds.

1. Rb2O2 ______2. Li2SO4 ______

3. BeSO4 ______4. MgCO3 ______

5. FePO3 ______6. CdCrO4 ______

7. NaHCO3 ______8. AgClO3 ______

9. Sr(C2H3O2)2 ______10. Al(OH)3 ______

11. HCN ______12. CuMnO4 ______

13. Co(NO3)2 ______14. HgClO2 ______

15. Hg(ClO)2 ______16. Pb(Cr2O7)2 ______

27 Binary & Ternary Ionic Compounds Indicate whether the following compounds are binary ionic (BI) or ternary ionic (TI). Then supply the missing information by either writing the name or the formula of the compound.

1. ______Na2S ______

2. ______(NH4)2CO3 ______

3. ______nickel II chloride ______

4. ______ammonium nitride ______

5. ______Hg(NO3)2 ______

6. ______gold IV sulfite ______

7. ______CuF ______

8. ______cesium selenide ______

9. ______Pb(CN)4 ______

10. ______Ge(ClO4)2 ______

11. ______sodium peroxide ______

12. ______ferrous dichromate ______

13. ______AgC2H3O2 ______

14. ______SnO2 ______

15. ______Ba(HCO3)2 ______

16. ______KMnO4 ______

17. ______calcium hydroxide ______

18. ______cobalt II iodide ______

19. ______chromium II phosphate ______

20. ______Mg(ClO)2 ______

28 The names of twenty polyatomic ions are scrambled below. Unscramble the name and write the formula and charge of each of the ions in the space provided. NAME FORMULA & CHARGE

A. DYCINAE ______

B. TACATEE ______

C. BARONTACE ______

D. ENITTAR ______

E. THSPEIHOP ______

F. DERYDIXOH ______

G. TELUSAF ______

H. YOLPHIRTECHO ______

I. MAROTECH ______

J. TEERMAGNAPAN ______

K. ATIBERCANOB ______

L. INIRETT ______

M. MOMMINUA ______

N. SOPPETHAH ______

O. CHARTELO ______

P. RATCHOMIDE ______

Q. SIFULET ______

R. LEPORRCHATE ______

S. DIEROPEX ______

T. TORCHLIE ______

29 Academic Chemistry “Cheat Sheet”

Types of Chemical Reactions Activity Series of Halogens A. Composition A + B AB 1. two elements a binary compound fluorine 2. metallic oxide + water a base (metallic hydroxide) chlorine 3. nonmetallic oxide + water an acid bromine iodine B. Decomposition AB A + B 1. binary compound two elements 2. base metallic oxide + water 3. acid nonmetallic oxide + water Activity Series 4. metallic carbonate metallic oxide + carbon dioxide of Metals 5. metallic chlorate metallic chloride + oxygen gas 6. hydrated salt salt + water lithium rubidium C. Single Replacement A + BX B + AX ; X + AY Y + AX potassium barium 1. active metal (or H2) + ionic cmpd new metal (or H2) + ionic cmpd 2. active halogen + ionic halide halogen + ionic compound strontium calcium

sodium D. Double Replacement AX + BY AY + BX magnesium 1. two soluble ionic compounds two new compounds, one of which aluminum must be an insoluble ionic compound or a molecular compound manganese zinc Common Polyatomic Ions Solubility Chart chromium Name Formula positive ion negative ion iron + + + - - - cadmium +1 Na , K , NH4 NO3 , C2H3O2 , ClO3 soluble ammonium NH4 cobalt -1 -2 -3 -2 - nickel acetate C2H3O2 silver, mercury, lead CO3 , PO4 , S , OH insoluble bicarbonate HCO -1 tin 3 chlorate ClO -1 Cl-1, Br-1, I-1 soluble lead 3 hydrogen cyanide CN-1 copper cyanate CNO-1 Ba+2, Ca+2, Sr+2 insoluble -1 mercury hydroxide OH -2 silver -1 SO4 soluble nitrate NO3 gold -1 permanganate KMnO4 thiocyanate SCN- -2 carbonate CO3 -2 chromate CrO4 -2 dichromate Cr2O7 -2 peroxide O2 -2 sulfate SO4 -3 phosphate PO4

Steps for Solving a Reaction Stoichiometry Problem

GRAMS of MOLES of MOLES of GRAMS of use use use reactant molar mass reactant mole ratio new reactant molar mass new reactant or of R or P or of R or P or of R or P or product product new product new product

30 Binary & Ternary Ionic Compounds

Directions: In the table below, write the formulas for the following ionic compounds.

zinc sulfide cupric cyanide cobalt II phosphate barium fluoride

ammonium oxide silver bromide magnesium chlorate ferric nitrate

potassium permanganate chromium III sulfate beryllium fluoride mercurous dichromate

sodium bicarbonate aluminum oxide cuprous bromide potassium chlorite

tin II acetate lithium phosphite strontium carbonate stannic nitride

rubidium iodide barium chromate sodium peroxide calcium hydroxide

lead IV phosphate lithium iodide sodium hypochlorite ammonium perchlorate

31 Binary & Ternary Ionic Compounds Pre-Quiz

Directions: Name each ionic compound or write the proper formula. Use either the stock or classical system where necessary.

1. potassium carbonate ______

2. CoSO3 ______

3. strontium nitride ______

4. stannous cyanide ______

5. Fe(ClO)2 ______

6. Ag2O2 ______

7. beryllium sulfide ______

8. Ca3(PO4)2 ______

9. plumbic selenide ______

10. aluminum chromate ______

32 Binary Covalent Compounds

Definition - compound composed of 2 nonmetals joined by a covalent bond (electron sharing)

Unlike metals that form only one or two cations, nonmetals can share electrons in many ways, so there are numerous compounds that can exist between two nonmetals. As a result we must have a method to distinguish among the various compounds.

When a metal exhibits more than one charge, we use a Roman numeral to distinguish between the two ions. With binary molecular compounds, we use prefixes to distinguish among the similar formulas. 1 - ______2 - ______3 - ______4 - ______5 - ______6 - ______7 - ______8 - ______9 - ______10 - ______

To name binary covalent compounds, we use the following rules: 1) ______2) ______

NO2 nitrogen dioxide (notice no prefix before nitrogen since subscript is1) N2O dinitrogen monoxide (notice prefix before oxygen even though subscript is1) NO nitrogen ______oxide N2O3 ______nitrogen trioxide N2O4 ______nitrogen ______oxide

NOTE: DO NOT reduce the subscripts in covalent compounds. N2O4 would reduce to NO2, and they are not the same compounds!

To write formulas, we do NOT need the periodic table because the prefixes in the name indicate the subscript. These are the easiest formulas to write. 1. PCl5 ______

2. SF6 ______

3. CO ______

4. CO2 ______

5. P4Cl10 ______

6. SO3 ______-2 7. SO3 ______8. nitrogen triiodide ______9. disulfur dichloride ______10. octabromine heptoxide ______11. carbon tetrachloride ______12. pentasilicon nonaselenide ______13. nitrogen dioxide ______14. nitrite ion ______

33 Binary Covalent Compounds Supply the missing information: either name the molecular compound or write its formula.

1. CS2 ______15. phosphorous trichloride ______

2. IF7 ______16. sulfur trioxide ______

3. S2Cl2 ______17. nitrogen dioxide ______

4. NCl3 ______18. diphosphorus pentasulfide ______

5. P2O5 ______19. iodine trichloride ______

6. OF2 ______20. carbon tetraiodide ______

7. SF6 ______21. dichlorine heptoxide ______

8. N2H4 ______22. carbon dioxide ______

9. PBr5 ______23. silicon monochloride ______

10. As2O5 ______24. dinitrogen pentoxide ______

11. SCl2 ______25. oxygen difluoride ______

12. SeS6 ______26. carbon disulfide ______

13. CF2 ______27. trisilicon tetranitride ______

14. ICl3 ______28. tetraiodine nonoxide ______

34 Naming Acids Acids are an important group of hydrogen-containing compounds that have been used in chemical reactions since before alchemical times. In the laboratory, acids are typically used in water solutions. When naming them and writing formulas, consider them anions connected to the number of hydrogen ions (H+) needed for electrical neutrality. The two types of common acids are binary acids and oxyacids.

Binary Acids A binary acid is a compound formed between hydrogen and a monatomic anion or a polyatomic ion that does not contain oxygen. They usually form when a gas dissolves in water. Use the following rules to name a binary acid: 1. Begin with the prefix hydro. 2. Add either the root or full name of the nonmetallic anion. 3. Add the suffix ic and the word acid. prefix hydro + anion nonmetal root + suffix ic + word acid Example: HCl — Hydro + chlor + ic + acid

HI ______hydrosulfuric acid ______

**This naming pattern holds for many compounds in which hydrogen combines with an anion that ends in -ide.

Oxyacids An oxyacid is a compound formed between hydrogen and a polyatomic ion that contains oxygen. The names are very similar to the name of the oxoanion except for two suffix changes. Use the following rules to name an oxyacid: 1. Name the polyatomic ion. 2. Change an “-ate” ion’s ending to ic; an “-ite” anion suffix changes to ous. 3. Add the word acid. Example: H2CO3 ______sulfurous acid ______

The Who's Who of Acids The above system of naming can be used to name all inorganic acids. However, although most elements will form acids, only a few acids are commonly used. Below is a list of the 7 common acids that you are responsible for naming and for writing their formulas.

You must memorize these!!!

HCl ______

______acetic acid

HNO3 ______

______carbonic acid

______sulfuric acid

H2SO3 ______

H3PO4 ______

35 Name ______Period ______

NOMENCLATURE – Vocabulary Review

Match the correct vocabulary term to each numbered statement. Write the letter of the correct term on the line. Each answer can only be used once. a. binary ionic compound f. ternary ionic compound k. monatomic ion b. acid g. stock system of naming l. binary compound c. cation h. classical system of naming m. polyatomic ion d. anion i. law of definite proportions e. base j. covalent (molecular) compound

______1. A compound composed of two elements and can be either ionic or covalent. ______2. A compound that contains a polyatomic ion ionically bonded to a metal, nonmetal, or another polyatomic ion. ______3. Consists of a single atom with a positive or negative charge. ______4. A compound that contains one or more hydrogen atoms and produces hydrogen ions in solution. ______5. In samples of any compound, the masses of the elements are always in the same proportions. ______6. The naming method devised by the IUPAC that uses roman numerals to distinguish between metals that exhibit more than one charge. ______7. Any atom or group of atoms with a negative charge. ______8. Compounds comprised of a metal cation and a nonmetal anion. ______9. The naming method that uses Latin names to distinguish between metals that exhibit more than one charge. ______10. An ionic compound that produces hydroxide ions when dissolved in water. ______11. A compound that composed of two nonmetals joined by a covalent bond. ______12. Any atom or group of atoms with a positive charge. ______13. A tightly bound group of atoms that behaves as a unit and carries a charge.

36 Formula Writing & Naming Review

1. Metals with only one common charge include Groups IA, IIA, Al, Zn, Cd, and Ag. You never use a RN when naming compounds that contain these metallic ions.

2. The numerical charge of a nonmetal’s ion can be determined by subtracting the group number from eight.

3. The charge on all transition metals (except Ag, Cd, and Zn) must always be indicated by either a Roman numeral (Stock system) or the classical method.(Never use both in a name.)

4. A Roman numeral shows the ionic charge of the cation.

5. All binary compounds, whether molecular or ionic, end in -ide.

6. An -ite or -ate ending means that the formula has a polyatomic ion (with a few exceptions).

7. Whenever more than a single polyatomic ion is needed to balance a formula, parentheses must be used.

8. Prefixes in the name indicate a molecular compound (two nonmetals). They show the number of atoms of each element in the formula.

9. A binary acid always starts with hydro-.

10. An oxyacid begins with the name of the oxygen-containing polyatomic ion whose ending has been changed: -ate to -ic, -ite to -ous.

Compound Identification

Binary Ionic Compounds: Binary Molecular Compounds: - metal + nonmetal - nonmetal + nonmetal - cation + monatomic anion - all end in -ide - all end in -ide - use prefixes

Ternary Ionic Compounds: Acids: - metal + polyatomic ion - begin with hydrogen - majority end in -ate and -ite - binary (no oxygen, use hydro-) - few end in -ide - oxyacid (polyatomic ion containing oxygen) -ate ion becomes -ic acid; -ite ion becomes -ous acid

37 Naming Compounds

Is the First Element a metal? YES NO

covalent compound of 2 nonmetals binary covalent compound Only 2 elements more than 2 elements binary ionic compound ternary ionic compound

1. Name the first

element. Precede the Is the metal in column IA, Is the metal in column IA, name with the prefix column IIA, or Al, Zn, Cd, Ag? column IIA, or Al, Zn, Cd, Ag? for the subscript, but NEVER mono. 2. Name the second element. ALWAYS YES NO YES NO precede it with a prefix. 1. Name the 1. Name the 1. Name the 1. Name the 3. Change the ending to metal. metal using metal. metal using “-ide.” 2. Name the the stock 2. Name the the stock

nonmetal. (Roman polyatomic (Roman 1 mono 3. Change Numerals) or ion. Numerals) 2 di the ending classical or classical 3 tri to “–ide.” (ic or ous) (ic or ous) 4 tetra system. system. 5 penta 2. Name the 2. Name the 6 hexa nonmetal. polyatomic 7 hepta 3. Change the ion. 8 octa ending to 9 nona “–ide.” 10 deca

38 Naming & Formula Writing Review Write formulas for the following compounds.

1. ferrous sulfate ______13. sulfuric acid ______

2. barium permanganate ______14. sodium bicarbonate ______

3. stannic nitrite ______15. cuprous chlorite ______

4. manganese II peroxide ______16. dichlorine monoxide ______

5. carbonic acid ______17. strontium nitride ______

6. iodine pentafluoride ______18. acetic acid ______

7. potassium chlorate ______19. mercuric hypochlorite ______

8. lead IV carbonate ______20. ferric hydroxide ______

9. nitric acid ______21. platinum II acetate ______

10. lead II chromate ______22. silicon dioxide ______

11. ammonium cyanide ______23. hydrochloric acid ______

12. nitrogen triiodide ______24. tin II phosphate ______

Name the following compounds.

1. CsBr ______12. BrF3 ______

2. Al2O3 ______13. SiF4 ______

3. H3PO4 ______14. CuClO2 ______

4. KC2H3O2 ______15. FeO ______

5. N2O5 ______16. Na2O2 ______

6. FePO3 ______17. Cr(CN)2 ______

7. CuCl2 ______18. PbO ______

8. Mg(OH)2 ______19. Hg(NO3)2 ______

9. Li2CO3 ______20. Sn(OH)2 ______

10. H2SO3 ______22. LiHCO3 ______

11. I2O7 ______23. Ni(ClO4)2 ______

39 FORMULA WRITING AND NAMING COMPOUNDS PRE-TEST

Name ______Period ______

DIRECTIONS: Complete the following chart. Element Possible Ions Name (stock) Name (Latin)

Cu Cu+___ copper ( ) ______+___ Cu copper ( ) ______

Hg Hg+___ mercury ( ) ______+___ Hg mercury ( ) ______

Fe Fe+____ iron ( ) ______+___ Fe iron ( ) ______

Pb Pb+___ lead ( ) ______+___ Pb lead ( ) ______

Sn Sn+___ tin ( ) ______+___ Sn tin ( ) ______

DIRECTIONS: Answer the following questions by filling in the blank.

1. If the first element in a compound is a metal then the compound is (ionic/covalent).______2. If two nonmetals are bonded together, prefixes must be used when naming the compound. (T/F) ______3. When naming ionic compounds, which TWO groups of metals DO NOT need a roman numeral? ______4. Which other FOUR metals do not need a roman numeral? ______5. What are the common charges for the metals in question #4? ______

40 Errors in Chemical Names and Formulas Each of the following formulas or names contains an error. Correct each example; then write the corresponding name or formula. EX: carbon IV oxide ---> carbon dioxide, CO2

1. aluminum III nitrite 1. ______

2. Al2O2 2. ______

3. (NH4)3Cl2 3. ______

4. lead III hydride 4. ______

5. leadic acetate 5. ______

6. stannous II hydroxide 6. ______

7. monocalcium dibromide 7. ______

8. K(ClO2) 8. ______

9. (OH)3Al 9. ______

10. Al4(CN) 10. ______

11. Pb(NO3)3 11. ______

12. copper I chloric 12. ______

13. carbonic disulfide 13. ______

14. NiNO32 14. ______

15. Mg2I 15. ______

16. ironic chlorate 16. ______

17. ClK 17. ______

18. nitrogen V fluoride 18. ______

19. silver I carbonate 19. ______

20. diiron trioxide 20. ______

21. dihydrogen oxide 21. ______

22. zinc dihydride 22. ______

23. cuprous I sulfate 23. ______

24. strontium phosphoride 24. ______

25. disodium dioxide 25. ______

ACROSS DOWN

-2 1. the formula for sodium thiocyanate 2. the name of the SiO3 ion 4. the formula for scandium III nitride 3. the formula for nitrogen monoxide 6. solid, liquid, and gas express a 5. the name for the Cu+2 ion ______of matter 6. the symbol for antimony 8. the formula for the hydroxide ion 7. the element in Period 3 with 3 valence electrons 10. 10. the symbol for lead 9. the name of the ClO-1 ion -1 12. the symbol for the smallest alkali metal 10. the name of the MnO4 ion 13. the symbol for copper 11. another name for the mercuric ion 15. the formula for Einsteinium I iodide 14. K 16. the formula for magnesium oxide 18. formula for bisulfide ion +3 17. Cr 20. charge on cobalt in CoCl2 21. symbol for arsenic 28. formula for uranium III phosphide 22. symbol for the element in Period 5 & Group IIIA 29. formula for neptunium III nitride 24. formula for potassium hydrogen sulfide 30. symbol for atom with 34 electrons 25. formula for stannous oxide 34. number of carbon atoms in a molecule of ammonia 26. formula for uranium III arsenide 35. formula for lithium astitide 27. symbol for element with atomic mass 152 38. symbol for element with Z = 29 30. symbol for element with 62 electrons 40. formula for strontium oxide 31. symbol for element with 70 protons 41. formula for chromium II sulfide -3 32. name of the PO4 ion 42. formula for thallium II sulfide 33. prefix meaning “two” 43. abbreviation of deoxyribonucleic acid 36. the iron ion which has 23 electrons 45. symbol for element in Period 4 and Group IIIB 37. name of the alkaline earth element in period 4

39. If H2StO4 is persecutedic acid, then the name for -2 the StO4 ion is ______. 46. a name for the Fe+2 ion 47. another name for tin IV ion

42 Name ______Period ______Uno! Dos! Tres! DIRECTIONS: Write the correct formula for the following compounds or ions.

1. sodium carbonate ______

2. hydrogen peroxide ______

3. ferrous phosphate ______

4. sodium hypochlorite ______

5. ammonia (nitrogen trihydride) ______

6. chromium II phosphate ______

7. potassium permanganate ______

8. sodium acetate ______

9. potassium cyanide ______

10. potassium sulfide ______

11. calcium hydroxide ______

12. cobalt III sulfate ______

13. strontium oxide ______

14. silver selenide ______

15. dinitrogen monoxide ______

16. potassium chlorate ______

17. ammonium hydroxide ______

18. mercuric chromate ______

19. cupric nitrate ______

20. methane ______

21. barium fluoride ______

22. stannous bromide ______

23. acetic acid ______

24. ferric iodide ______

OVER  Each numbered question on the back asks you to determine the number of cations, anions, or total ions in the formulas you wrote on the top of this paper. Cross out a number 1, 2, or 3 in the box each time you answer the statement. What’s left? Uno, Dos, or Tres?

3 1 1 2 1

Answer: 2 1 3 1 3

3 2 2 1 2 ______

3 2 2 3 3

3 2 3 2 2

______1. Number of sodium ions that bond with a carbonate ion. ______2. Number of oxygen atoms in one molecule of hydrogen peroxide. ______3. Charge of the cation in ferrous phosphate. ______4. Total number of anions in one formula unit of common household bleach, sodium hypochlorite. ______5. Number of hydrogen atoms in one molecule of ammonia. ______6. Number of chromium II ions that bond with two phosphate ions. ______7. Total number of ions in one formula unit of potassium permanganate. ______8. Number of acetate ions in sodium acetate. ______9. Number of cyanide ions that bond with potassium ion. ______10. Number of potassium ions that bond with one sulfide ion. ______11. Total number of ions in one formula unit of calcium hydroxide. ______12. Number of anions in one formula unit of cobalt III sulfate. ______13. Total number of ions in one formula unit of strontium oxide. ______14. Total number of ions in one formula unit of silver selenide. ______15. Total number of atoms in one molecule of dinitrogen monoxide. ______16. Number of anions in one formula unit of potassium chlorate. ______17. Number of cations in one formula unit of ammonium hydroxide. ______18. Charge of the cation in mercuric chromate. ______19. Number of nitrate ions that bond with one cupric ion. ______20. Number of carbon atoms in one molecule of natural gas, methane. ______21. Number of fluoride ions in one formula unit of barium fluoride. ______22. Total number of ions in one formula unit of stannous bromide. ______23. Number of carbon atoms in one molecule of vinegar, acetic acid. ______24. Charge on iron in ferric iodide.

1. Name each of the following ions.

- a.) NO3 ______b.) Fe3+ (stock) ______(Latin)______c.) O-2 ______d.) Mg2+ ______-2 e.) SO4 ______f.) Pb+2 (stock) ______(Latin)______g.) Cu+1 (stock) ______(Latin)______h.) Hg+2 (stock) ______(Latin)______- i.) C2H3O2 ______j.) P-3 ______

2. Write the formula for the ion formed from each of the following.

a.) barium ______b.) iodide ______c.) cobalt (III) ______d.) potassium ______e.) nitride ______f.) chromium (II) ______

3. Provide the name or the formula for each of the following.

a.) Li3As ______

b.) SnO2 (stock) ______(Latin)______c.) strontium nitrate ______d.) cupric fluoride ______

e.) MnCl2 ______f.) Iron (II) chlorite ______

45 4. Provide the name or the formula for each of the following.

a.) diboron octoxide ______

b.) Br2O ______

c.) Mg(HCO3)2 ______

d.) CSe2 ______

e.) calcium acetate ______

f.) BrF5 ______g.) sulfur hexafluoride ______h.) silicon tetrachloride ______

i.) Cl2O7 ______j.) dinitrogen pentasulfide ______

k.) PI3 ______

l.) Cr(NO2)3 ______

m.) P4O6 ______

5. Complete the following chart.

Element Possible Ions Name (stock) Name (Latin)

Cu Cu+___ copper ( ) ______+___ Cu copper ( ) ______

Hg Hg+___ mercury ( ) ______+___ Hg mercury ( ) ______

Fe Fe+____ iron ( ) ______+___ Fe iron ( ) ______

Pb Pb+___ lead ( ) ______+___ Pb lead ( ) ______

Sn Sn+___ tin ( ) ______+___ Sn tin ( ) ______

I. Write the formulas for the following compounds.

a.) lithium oxide ______b.) calcium bromide ______c.) sodium oxide ______d.) copper (I) sulfite ______e.) tin (IV) fluoride ______f.) gold (III) cyanide ______g.) lead (II) sulfide ______h.) carbon tetrachloride ______i.) iodine heptafluoride ______j.) dinitrogen monoxide ______k.) sulfur dioxide ______

II. Name the following compounds. For those compounds with two possible names, WRITE BOTH.

a.) Pb(NO3)2 ______

b.) Fe2O3 ______

c.) Ni(C2H3O2)2 ______

d.) HgF2 ______

e.) Na2SO4 ______

f.) Sn(OH)2 ______

g.) S2Cl2 ______

h.) CS2 ______

i.) SO3 ______

j.) P4O10 ______

III. Write the formulas for the following acids.

a.) carbonic acid ______b.) nitric acid ______c.) sulfuric acid ______d.) hydrochloric acid ______

I Nomenclature

Provide the name or the formula for each of the following:

1. lithium hydroxide ______

2. chromium (III) ion ______

3. CaO ______

4. potassium nitrite ______

5. nickel (II) ion ______

6. potassium bromide ______

7. fluoride ion ______

8. calcium carbonate ______

9. nitrite ______

10. ZnO ______

11. barium sulfate ______

12. lead (II) phosphide ______

13. PbCl2 ______

14. cyanide ______

15. chromate ion ______

16. KMnO4 ______

48 Measuring Densities Making “Cents”

of Pennies

Introduction: 8. Add 5 more pennies to the cylinder; read Pennies were originally made of pure the new water level and record in the copper. In 1837, the U.S. Mint added 5 appropriate data table. percent zinc to the copper. The alloy 9. Repeat step eight, adding 5 more pennies remained 95 percent copper and 5 percent to those already in the graduated cylinder zinc until 1982, Since then, the penny has until you have used all 25 pennies. Record been made with an outside coating of copper all volumes in the appropriate data table. and an inner core of a different metal. 10. Discard the water. Dry the pennies with a These differences in composition of the paper towel and place in the proper older and more recently minted pennies beaker, labeled, “wet,” found on the results in a difference in the penny’s central distribution table. characteristics, including its density, or mass 11. Repeat steps 1-9 with the other set of per unit volume. coins. Record your data in the other data In this experiment, you will determine and table. compare the densities of pennies minted before 1982 and after 1983, and then use these densities to identify the metal used in the core of pennies minted after 1983.

Materials 25 pre-1982 pennies balance 25 post-1982 pennies water 100-mL graduated cylinder eye dropper

Procedure: 1. Obtain 25 pre-1982 pennies and 25 post-1982 pennies. 2. Work with one set of 25 pennies at a time. 3. Find the mass of 5 pennies from one set. Record the mass in the appropriate table. 4. Add five more pennies to the first group and obtain the mass of these 10 pennies. Record the mass. 5. Repeat step 3, adding 5 more pennies to those already on the balance until you have used all 25 pennies. Record all masses. 6. Fill a 100-mL graduated cylinder to the 20.0-mL mark. If necessary, use an eye dropper until the bottom of the meniscus is on the 20.0 mL line. 7. Still working with the same set of 25 pennies, gently drop 5 of the pennies into the graduated cylinder. Record the new water level in the appropriate table.

50 Name: ______Period ______

1. Using the data you collected, calculate the volume and density of the pennies. Make sure you label all data and calculations with units and pay attention to significant figures.

Pre-1982 Pennies

Number of Mass of Total Volume Volume of Density of Pennies Pennies in Cylinder Pennies Pennies

Average Densities of the Pennies

Post-1982 Pennies

Number of Mass of Total Volume Volume of Density of Pennies Pennies in Cylinder Pennies Pennies

Average Densities of the Pennies

51 Conclusion: 1. Construct a graph of your results using Microsoft Excel. a. Plot the pre-1982 data first. Plot the mass of the pennies on the y-axis. Plot the volume of the pennies on the x-axis. Answer question #2. b. Make a separate graph and plot the data for the post-1982 pennies (you can simply replace the data that you already entered). Answer question #2.

2. Determine the equation of both lines on your graph.

Pre-1982 Equation ______Post-1982 Equation ______

Analysis of Data 1. Using the equation from the graph, what is the slope of the line of the pre-1982 pennies? ______2. Using the equation from the graph, what is the slope of the line of the post-1982 pennies? ______3. What do the values of these slopes represent about the pennies? ______

4. How does the slopes of the lines compare to the average densities calculated in your data tables? ______

5. Compare the density of copper (found on page R47 Table 2 in your book) to the density of the pre-1982 pennies that you determined from your graph. ______

6. List the densities of Pb, W, Zn, Au, Ag, and Ti (found on page R47 Table 2 in your book)? Compare those with the density of the post-1982 pennies from your graph. What element has a similar density to your result? ______7. Calculate the percent error in your density of the pre-1982 pennies. Assume the density of pure copper (from #5) to be the actual value and assume the density value from the graph as the experimental value. (Show all work and pay attention to significant figures.)

8. Discuss two possibilities for sources of error in this experiment. ______

Reliability of Measurements Water, Water

Everywhere

Introduction: 4. Pour the water out of the beaker; dry the When scientists make measurements, they beaker. evaluate both the accuracy and precision of the 5. Repeat steps 1 - 4 two more times for a total of measurements. Accuracy refers to how close a three trials. measured value is to the accepted value; precision refers to how close a series of measurements are PART C to each other. 1. Obtain a buret and buret clamp. Secure the In this lab, you will examine the accuracy and buret in the clamp attached to a ring stand. precision of three different tools used for 2. Mass your 250-mL beaker; record in Table C. measuring. A 250-mL beaker, a 100-mL graduated 3. Using a funnel, slowly fill the buret to the 0- cylinder, and a 50-mL buret will be used to make mL line. (To do this, fill slightly past the 0-mL the measurements. mark and drip out the excess until the bottom of the meniscus is on the 0-mL line.) Materials 4. Place the 250-mL beaker under the buret. 250-mL beaker 600-mL beaker Open the stopcock on the buret and slowly 50-mL buret buret clamp drain 50-mL of water into the beaker. ring stand water CAUTION: As you approach the 50-mL line, funnel eye dropper drain the water from the buret drop by drop 100-mL graduated cylinder balance until the bottom of the meniscus is on the 50- mL line. Procedure: 5. Mass the beaker and water; record in Table C. 6. Pour the water out of the beaker; dry the Part A beaker. 1. Obtain a 250-ml beaker and a 600-mL beaker. 7. Repeat steps 2 -5 two more times for a total of Fill the large beaker with water. three trials. 2. Mass the 250-mL beaker; record in Table A. 8. In Table C, record the 50-mL of the water 3. Measuring as accurately as possible, pour 50 mL measured with the buret to the correct number of water into the beaker. Mass the beaker and of significant figures. This will be the same for all water; record in Table A. three trials. 4. Pour the water out of the beaker; dry the beaker. 5. Repeat steps 2 - 4 two more times for a total of three trials. 6. Although the beaker can be read only to the tens column, we are going to assume that the volume of the water is 50 mL for all three trials.

PART B 1. Mass your 250-mL beaker; record in Table B. 2. Measuring as accurately as possible, pour 50 mL of water into a 100-mL graduated cylinder. If necessary, use an eye dropper to make sure that the bottom of the meniscus is “exactly” on the 50-mL line. Record the volume in the data table (remember significant figures). The volume will be the same for all three trials. 3. Pour the water into the dry beaker. Mass the beaker and water; record in Table B.

54 Name ______Period ______

Table A – Beaker Measurements

Mass of Mass of Beaker Mass of Volume of Beaker And Water Water Water

Trial 1

Trial 2

Trial 3

Average

Table B – Graduated Cylinder Measurements

Mass of Mass of Beaker Mass of Volume of Beaker And Water Water Water

Trial 1

Trial 2

Trial 3

Average

Table C – Buret Measurements

Mass of Mass of Beaker Mass of Volume of Beaker And Water Water Water

Trial 1

Trial 2

Trial 3

Average

55 CONCLUSION:

1. The known mass of 1.00 mL of water is 1.00 grams. For this experiment, what mass should you expect for each of your samples?______

2. Using your answer to #1 as the accepted value and the average mass of water as your experimental value, calculate the percent error for Part A, B, and C. SHOW YOUR WORK!

3. Explain how you decided how many significant figures were needed for the volume measurements made with the graduated cylinder and buret. ______

4. Which of the three measurement tools produced the most accurate results? Explain, using the definition of accuracy in your answer. ______

5. Which of the three measurement tools produced the most precise results? Explain, using the definition of precision in your answer. ______

56 Naming compounds and writing formulas for a series of copper reactions “Cu” Later

INTRODUCTION: PROCEDURE: Substances may be created by chemical change PART I and may also undergo chemical change. If a 1. In a 100-mL beaker, make a water bath by substance is produced as a result of a chemical heating until boiling 50 mL of tap water. change or reaction, it is called a product. If a 2. Place approximately 50 mL of tap water in a substance is the subject of a chemical change, it is separate 100 mL beaker and set aside. called a reactant. The same substance can be either 3. While the water bath is heating, make three a reactant or product, depending on the chemical marks that are 2 cm apart on a small test tube. reaction. Use a red lab pencil and make the marks from One way of knowing that a chemical change has the bottom up. occurred is by observing that the properties of the 4. Add the copper II nitrate solution to the first product(s) are different from those of the reactants. The new product(s) can then become the reactants mark on the test tube. in another chemical reaction. In this experiment, 5. Add the 3 M sodium hydroxide solution to the you will observe the sequence of changes that second mark on the test tube. occurs when a solution of copper II nitrate (cupric 6. Observe the contents of the test tube for an nitrate) is treated with a series of different reactants. indication of a chemical reaction. Record the All of the reactions will take place in the same test observations in the Observations Table. tube. Look for evidence that a new substance has 7. Mix with the stirring rod and then rinse off the formed from each chemical change. stirring rod. The chemical conversion of one product into 8. The copper II nitrate has been converted to another useful product is called recycling. The copper II hydroxide. The other product, a copper II nitrate solution used in this experiment is white solid which remains dissolved in the prepared originally from elemental copper and nitric water, is sodium nitrate. acid. After a series of chemical reactions, the copper metal is recovered. PART II Chemical changes are required to make these 1. Place the test tube in the water bath begun in conversions. For example, the metals that are step I. changed into alloys and shaped into soft drink cans 2. Heat the test tube until no more change are themselves converted by chemical changes into occurs. Observe and record in the other products. Recycling enables people to reuse Observations Table. scarce natural resources, such as copper and 3. The products of this reaction are copper II aluminum, usually at a lower cost than mining the oxide and water. ores and refining them.

OBJECTIVES: PART III

 To write formulas of reactants and products 1. Turn off the burner and, using a test tube involved in a chemical reaction. holder, remove the test tube from the hot  To observe the types of evidence that indicates a water bath. chemical change has taken place. 2. Place the test tube into the beaker that you set  To infer from the observation of chemical aside in step 2 of part I. COOL the test tube change that a new substance has been formed. and its contents in this beaker for TWO MINUTES. MATERIALS: 3. Add 6 M hydrochloric acid to the third mark. copper II nitrate solution 6 M HCL 4. Mix with the stirring rod until a clear solution 3 M sodium hydroxide solution test tube is observed. Then rinse the rod. small Pyrex test tube stirring rod 5. Observe any changes and record in your 2 100-mL beakers iron ring Observations Table. ring stand ruler 6. The products of this chemical change are Bunsen burner wire gauze copper II chloride and water. aluminum wire marker

57 PART IV 3. What is the color of solutions of copper 1. Place a 12-cm piece of aluminum wire in the test compounds? tube. LEAVE IT ALONE until the reaction stops. 4. What is the color of copper II oxide? Make sure the reaction goes to completion 5. Is part IV exothermic or endothermic? Explain before recording your observations. your answer. 2. Touch the bottom of the test tube to check for 6. What color is the solution at the end of the any temperature change. experiment (step 2 part IV)? 3. Record in the data table all observed changes. 7. Write a word equation for each of the four 4. Throw the wire away in the trash can and chemical changes. Refer to the procedure to discard the solution down the sink. determine what the reactants and products are 5. The copper compound has finally been in each reaction. Then write the formula converted back into copper metal. The other equation under each word equation. The product is aluminum chloride. equation does not need to be balanced.

CONCLUSIONS: EXAMPLE: Answer the questions on a separate sheet of paper. zinc + hydrochloric acid ---> zinc chloride + hydrogen gas 1. List three observations that indicate that a Zn + HCl ---> ZnCl2 + H2 chemical change has occurred. Be specific. EX: When the zinc reacted with the hydrochloric acid, a gas was produced.

2. In the last step of this experiment, aluminum chloride, which exists as a white solid at room temperature, is produced. This is similar to the product, sodium nitrate, formed in Part 1. Where can the aluminum chloride be found in the test tube? How can one recover it?

Observation Table Observations

Part I

Part II

Part III

Part IV

58 WHAT dO I need to know?? Unit 5: Nomenclature

written part ~ naming o 20 writing formulas o 20 naming multiple choice o common charges o Latin names o definitions: cations vs. anions; ionic vs. covalent bonds o Cumulative Review: Chemistry is a subject that builds upon prior knowledge. You are responsible for general concepts that have been covered on previous tests.