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Chapter 5 You do not need to put the answers on a separate piece of paper. GENERAL QUESTIONS 1. Metals lose or gain electrons to form what type of ions? 2. Hydrogen is unusual because it can form both positive and negative ions. Write the chemical symbol and name for each of these ions. CHEMICAL FORMULAS 3. Determine each type of atom in each formula. a. NH4Cl b. NaCN c. Ba(HCO3)2 d. Ca(NO2)2 e. MgCl2 4. Which of these formulas represent molecules? State how many atoms are in each molecule. a. Fe b. PCl3 c. P4 d. Ar 5. Write the formula for each compound a. magnesium sulfate, which has 1 magnesium atom, 4 oxygen atoms, and 1 sulfur atom b. ethylene glycol (antifreeze), which has 6 hydrogen atoms, 2 carbon atoms, and 2 oxygen atoms c. acetic acid, which has 2 oxygen atoms, 2 carbon atoms, and 4 hydrogen atoms potassium chlorate, which has 1 chlorine atom, 1 potassium atom, and 3 oxygen atoms d. sodium hypochlorite pentahydrate, which has 1 chlorine atom, 1 sodium atom, 6 oxygen atoms, and 10 hydrogen atoms 6. Complete the table. Formula Number of SO42- Units Number of Sulfur Atoms Number of Oxygen atoms Number of metal atoms CaSO4 Al2(SO4)3 K2SO4 7. Write the chemical formula of the compound containing one magnesium atom for every two chlorine atoms? MOLECULAR VIEW OF ELEMENTS AND COMPOUNDS 8. For each of the following compounds, state whether it is ionic or covalent. If it is ionic, write the symbols for the ions involved: a. NF3 b. BaO, c. (NH4)2CO3 d. Sr(H2PO4)2 e. IBr 9. Classify each compound as ionic or molecular. a. PtO2 b. FeN2 c. SiH4 d. BaSO4 10. Which elements have molecules as their basic units? a. iron b. Bromine c. Oxygen d. Helium 11. Classify each element as atomic or molecular. a. b. c. d. Bromine Fluorine Neon Cobalt 12. Provide the classification (i.e. atomic element, molecular element, molecular compound, or ionic compound) of each substance. a. PCl3 b. LiBr c. P4 d. oxygen gas 13. Classify each compound as ionic or molecular. a. CF2Cl2 b. CO c. SO3 d. Al(NO3)2 14. Predict whether the compound formed in each case will be an ionic or a covalent compound. a. Carbon Dioxide b. Potassium Oxide c. Nitrogen Chloride d. Dinitrogen Tetroxide WRITING FORMULA FOR IONIC COMPOUNDS: NAMING IONIC COMPOUNDS 15. In what order do the names of ions appear in the names of ionic compounds? 16. Name the ionic compound formed by each pair of ions. Use both the Stock and common systems, where appropriate. a. Fe3+ and Br− b. Fe2+ and Br− c. Au3+ and S2− d. Au+ and S2− 17. Provide the formula for each ionic compound named below. a. Sodium hypochlorite b. c. d. e. Potassium hydroxide Ammonium nitrate Aluminum sulfite Iron(III) cyanide 18. Complete the table below Cations Anions Zn2+ Br- K+ CO32- Al3+ HCO3- Fe2+ OH- Cu+ NO3- Formula Unit 19. Combine the following pairs of elements (or ions) to express them as an ionic compound. a. Sodium and Sulfur b. Barium and Iodine c. Iron(III) and Oxygen d. Aluminum and Bromine e. Lithium and Nitrogen 20. Name each ionic compound AND give the names of the individual ions that make up the formula. a. Hg2S b. Cr2O3 c. K2SO4 d. Fe2(CO3)3 e. Zn(ClO)2 21. Transition metals tend to have varying charges. Determine the charges on each transition metal in the following ionic compounds. a. b. c. d. e. AuN SnO2 Cu2S PbBr4 FeI2 22. The following chemical formulas are INCORRECT. Rewrite the formulas with the proper number of cations and anions to balance the formulas and name the ionic compounds a. BaC2H3O2 b. NH4SO4 c. ZnClO d. AlOH e. NaCO3 23. Which compounds would you predict to be ionic? a. Li2O b. (NH4)2O c. CO2 d. FeSO3 e. C6H6 f. C2H6O 24. The following ionic compounds are found in common household products. Write the formulas for each compound: a. potassium phosphate b. copper(II) sulfate c. calcium chloride d. titanium dioxide e. ammonium nitrate f. sodium bisulfate (the common name for sodium hydrogen sulfate) 25. Name each ionic compound. a. CaCl2 b. AlF3 c. Co2O3 d. Sc2O3 e. AgCl NAMING MOLECULAR COMPOUNDS 26. Write the formulas of the following molecular and ionic compounds: a. chlorine dioxide b. dinitrogen tetroxide c. potassium phosphide d. silver(I) sulfide e. aluminum nitride 27. Write the formula for each molecular compound. a. dinitrogen monoxide b. silicon tetrafluoride c. boron trichloride d. nitrogen trifluoride e. phosphorus tribromide 28. Determine whether the name shown for each molecular compound is correct. If not, provide the compound’s correct name. a. NCl3 Nitrogen Chloride b. CI4 Carbon(IV)iodide c. CO Carbon Oxide d. SCl4 Sulfur tetrachloride 29. Give the formula for each molecule. a. carbon tetrachloride b. silicon dioxide c. trisilicon tetranitride d. disulfur difluoride e. iodine pentabromide 30. Name the following molecular compounds. a. NBr3 b. O2 c. NH3 d. CH4 31. Write a formula for each molecular compound. a. Hydrogen iodide b. Sulfur tetrachloride c. Chlorine Dioxide d. Selenium hexafluoride 32. What is the formula mass for each compound? a. FeBr3 b. FeBr2 c. Au2S3 d. Au2S Cumulative 33. Complete the table below. Ionic compound Cation Symbol and name Anion symbol and name NaC2H3O2 Cr(NO3)3 PbCl2 Hg3(PO4)2 Ca(HCO3)2 34. Complete the table below. Formula Unit Chemical Name MgS Aluminum Oxide Fe(OH)3 Copper(II) chloride Pb(CO3)2 Zinc bicarbonate CaSO4 Sodium acetate BaBr2 Ammonium nitrate 35. Each of the following compounds contains a metal that can exhibit more than one ionic charge. Name these compounds: a. Cr2O3 b. FeCl2 c. CrO3 d. TiCl4 e. CoO 36. determine whether the name shown for each molecular compound is correct. If not, provide the compound’s correct name. a. SF4 monosulfur hexafluoride b. K2O dipotassium monoxide c. CaI2 Calcium diiodide d. PBr5 Phosphorus (v) pentabromide 37. Classify each as molecular element, molecular compound, or ionic compound d 38. Name each compound and calculate its formula mass. a. NaCl b. AgNO3 c. AlF3 d. IF5 39. Write a molecular formula for each molecular model. (white= hydrogen; red=oxygen; black= carbon; Blue= nitrogen; yellow= sulfur) a) b) 40. c) d) Complete the table. Formula Type of compound Name K3N VCl4 molecular Carbon monoxide NBr3 41. Complete the table below. Formula Type of compound Name tin (IV) selenide Al(CN)3 ionic IBr Carbon Disulfide
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sirname1

Student’s Name
Instructor
Course
Date
Chemistry questions
GENERAL QUESTIONS
1. Metals lose or gain electrons to form what type of ions?
cations

2. Hydrogen is unusual because it can form both positive and negative ions. Write the
chemical symbol and name for each of these ions.

CHEMICAL FORMULAS
3. Determine each type of atom in each formula.
a. NH4Cl
b. NaCN
c. Ba(HCO3)2
d. Ca(NO2)2
e. MgCl2

H+ and H-

sirname2

4. Which of these formulas represent molecules? State how many atoms are in each .
a. Fe
b. PCl3 with 4 atoms
c. P4

with two molecules

d. Ar

5. Write the formula for each compound
a. magnesium sulfate, which has 1 magnesium atom, 4 oxygen atoms, and 1 sulfur
atom MgSO4
b. ethylene glycol (antifreeze), which has 6 hydrogen atoms, 2 carbon atoms, and 2
oxygen atoms(CH2 OH)2
c. acetic acid, which has 2 oxygen atoms, 2 carbon atoms, and 4 hydrogen atoms
CH3COOH
potassium chlorate, which has 1 chlorine atom, 1 potassium atom, and 3 oxygen
atoms KCLO3
d. sodium hypochlorite pentahydrate, which has 1 chlorine atom, 1 sodium atom, 6
oxygen atoms, and 10 hydrogen atoms NaOCL.5 H2 O

sirname3

6. Complete the table.
Formula

Number of

Number of

Number of

Number of

SO42- Units

Sulfur Atoms

Oxygen atoms

metal atoms

CaSO4

1

1

4

1

Al2(SO4)3

3

3

12

2

K2SO4

1

1

4

2

7. Write the chemical formula of the compound containing one magnesium atom for every two
chlorine atoms?
MgCL2

MOLECULAR VIEW OF ELEMENTS AND COMPOUNDS

8. For each of the following compounds, state whether it is ionic or covalent. If it is ionic,
write the symbols for the ions involved:
a.

NF3

covalent compound

b.

BaO,

covalent compound

c. (NH4)2CO3

Covalent compound

sirname4

d.

Sr(H2PO4)2 Ionic compound

e.

IBr

covalent compound

9. Classify each compound as ionic or molecular.
a. PtO2

molecular compounds

b. FeN2

ionic compounds

c. SiH4

molecular compounds

d. BaSO4

ionic compound

10. Which elements have molecules as their basic units?
a. Iron
b. Bromine has molecule as their basic unit
c. Oxygen

has molecules their basic units

d. Helium

11. Classify each element as atomic or molecular.
a. Bromine

molecular

b. Fluorine

molecular

c. Neon

ionic

d. Cobalt

molecular

sirname5

12. Provide the classification (i.e. atomic element, molecular element, molecular compound, or
ionic compound) of each substance.
a. PCl3

molecular compound

b. LiBr

atomic compound

c. P4

Molecular element

d. oxygen gas

molecular compound

13. Classify each compound as ionic or molecular.
a. CF2Cl2

molecular

b. CO

molecular

c.

molecular compound

SO3

d. Al(NO3)2

ionic compound

14. Predict whether the compound formed in each case will be an ionic or a covalent
compound.
a. Carbon Dioxide

covalent compound

b. Potassium Oxide

ionic compound

c. Nitrogen Chloride

covalent compounds

d. Dinitrogen Tetroxide covalent bond

WRITING FORMULA FOR IONIC COMPOUNDS: NAMING IONIC COMPOUNDS

sirname6

15. In what order do the names of ions appear in the names of ionic compounds?

Cations then anions
16. Name the ionic compound formed by each pair of ions. Use both the Stock and common
systems, where appropriate.
a. Fe3+ and Br− and iron(III)Bromide
b. Fe2+ and Br−

iron(II)bromide

c. Au3+ and S2− Gold (III)Sulfide
d. Au+ and S2−

Gold(I)Sulfide

17. Provide the formula for each ionic compound named below.
a. Sodium hypochlorite

NaCLO

b. Potassium hydroxide KOH
c. Ammonium nitrate

NH4N3

d. Aluminum sulfite Al2S3
e. Iron(III) cyanide Fe(CN)3

18. Complete the table below
Cations

Anions

Formula Unit

sirname7

Zn2+

Br-

ZnBr2

K+

CO32-

K2CO

Al3+

HCO3-

Al(HCO)3

Fe2+

OH-

Fe(OH)2

Cu+

NO3-

CuNO3

19. Combine the following pairs of elements (or ions) to express them as an ionic compound.
a. Sodium and Sulfur

Sodium sulfide

b. Barium and Iodine

BaI2

c. Iron(III) and Oxygen

Iron(III) oxide

d. Aluminum and Bromine

Al2 Br3

e. Lithium and Nitrogen

Li3N

20. Name each ionic compound AND give the names of the individual ions that make up the
formula.
a. Hg2S

MERCURY(I)SULFIDE

b. Cr2O3

CHROMIUM (III) OXIDE

(chromium and oxygen)

c. K2SO4

POTASSIUM SULFIDE

(potassium and sulphur)

d. Fe2(CO3)3 IRON(III)CARBONATE
e. Zn(ClO)2

(mercury and sulphur)

(iron and carbonate)

sirname8

21. Transition metals tend to have varying charges. Determine the charges on each transition
metal in the following ionic compounds.
a. AuN

+1

b. SnO2

-1

c. Cu2S
d. PbBr4

+1

e. FeI2

+2

22. The following chemical formulas are INCORRECT. Rewrite the formulas with the proper
number of cations and anions to balance the formulas and name the ionic compounds
a. BaC2H3O2

BaCH23O2

b. NH4SO4

(NH4 )2 SO4

c. ZnClO

ZnCl2

d. AlOH

Al(OH)3

e. NaCO3

NaCO3

23. Which compounds would you predict to be ionic?

sirname9

a. Li2O Ionic compound
b. (NH4)2O
c. CO2
d. FeS...


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