Chapter 6: Ionic and Molecular Compounds

Chapter 6.1: Ions: Transfer of Electrons

100

The tendency of atoms to attain a stable electron configuration is known as:

The octet rule

200

This type of bond occurs when the valence electrons of metal atoms are transferred to atoms of nonmetals

Ionic bonds

300

This type of bond forms when atoms of nonmetals share valence electrons

covalent bonds

400

Write the symbols for the ions with the following number of protons and electrons:
a. 3 protons, 2 electrons
b. 9 protons, 10 electrons
c. 12 protons, 10 electrons
d. 27 protons, 24 electrons

a. Li⁺
b. F^-
c. Mg²⁺
d. Co³⁺

500

State the number of protons and electrons in each of the following ions:
A. O^2-
B. K⁺
C. I^-
D. Ca²⁺

A. P⁺: 8, e^-: 10
B. P⁺: 19, e^-: 18
C. P⁺: 53, e^-: 54
D. P⁺: 20, e^-: 18

Chapter 6.2: Ionic Compounds

100

When one or more electrons are transferred from metals to nonmetals forming positive and negative ions it creates

an ionic compound

200

The charge of an ionic compound is always _____. How do you show this in the chemical formula?

0. Subscripts

300

Which of the following pairs of elements are likely to form an ionic compound?
a. Lithium and Chlorine
b. Oxygen and bromine
c. Potassium and oxygen
d. Sodium and neon
e. Cesium and magnesium
f. Nitrogen and fluorine

a. Lithium and Chlorine
c. Potassium and Oxygen

400

Write the correct ionic formula for the compound formed between each of the following pairs of ions:
a. Na⁺ and O^2-
b. Al³⁺ and Br^-
c. Ba²⁺ and N^3–
d. Mg²⁺ and F^-
e. Al³⁺ and S^2-

a. Na₂O
b. AlBr₃
c. Ba₃N₂
d. MgF₂
e. Al₂S₃

500

Write the symbols for the ions and the correct formula for the ionic compound formed by each of the following:
a. Potassium and sulfur
b. Sodium and nitrogen
c. Aluminum and iodine

a. K⁺, S^2-, K₂S
b. Na⁺, N^3-, Na₃N
c. Al³⁺, I^-, AlI₃

Chapter 6.3: Naming & Writing Ionic F0rmulas

100

Write the name for the ionic compound:
a. AlF₃
b. CaCl₂
c. Na₂O

a. Aluminum Fluoride
b. Calcium Chloride
c. Sodium Oxide

200

Write the name for each of the following ions (include Roman numeral when necessary):
a. Fe²⁺
b. Cu²⁺
c. Zn²⁺

a. Iron(II)
b. Copper(II)
c. Zinc

300

Write the name for each of the following ionic compounds:
a. SnCl₂
b. FeO
c. Cu₂S
d. CdBr₂

a. Tin(II) Chloride
b. Iron(II) oxide
c. Copper(I) sulfide
d. Cadmium bromide

400

Write the symbol for the cation in each of the following ionic compounds:
a. AuCl₃
b. Fe₂O₃
c. PbI₄
d. AlP

a. Au³⁺
b. Fe³⁺
c. Pb⁴⁺
d. Al³⁺

500

Write the formula for each of the following ionic compounds:
a. Magnesium chloride
b. Sodium sulfide
c. Copper(I) oxide
d. Gold(III) nitride

a. MgCl₂
b. Na₂S
c. Cu₂O
d. AuN

Chapter 6.4: Polyatomic Ions

100

Write the formula including the charge for each of the following polyatomic ions:
a. Hydrogen carbonate (bicarbonate)
b. Ammonium
c. Phosphite
d. Chlorate

a. HCO₃^-
b. NH₄⁺
c. PO₃^3-
d. ClO₃⁺

200

Name the following polyatomic ions:
a. SO₄^2-
b. CO₃^2-
c. HSO₃^-
d. NO₃^-

a. Sulfate
b. Carbonate
c. Hydrogen sulfite (bisulfate)
d. Nitrate

300

Write the correct formula for the following ionic compounds:
a. Barium hydroxide
b. Sodium hydrogen sulfate
c. Iron(II) nitrite
d. Zinc phosphate
e. Iron(III) carbonate

a. Ba(OH)₂
b. NaHSO₄
c. Fe(NO₂)₂
d. Zn₃(PO₄)₂
e. Fe(CO₃)₃

400

Write the formula for the polyatomic ions and name each of the following compounds:
a. Na₂CO₃
b. (NH₄)₂S
c. Ca(OH)₂
d. Sn(NO₂)₂

a. CO₃^2-, sodium carbonate
b. NH₄⁺, ammonium sulfide
c. OH₂^-, Calcium hydroxide
d. NO₂^-, tin(II) nitrite

500

Name each of the following compounds:
a. Zn(C₂H₃O₂)₂
b. Mg₃(PO₄)₂
c. NH₄Cl
d. Sr(NO₃)₂
e. NaNO₂

a. Zinc acetate
b. Magnesium phosphate
c. Ammonium chloride
d. Strontium nitrate
e. Sodium nitrite

Chapter 6.5: Molecular Compounds: Sharing Electrons

100

Two or more nonmetals that share one or more valence electrons are called ____________________ and are held together by ________________.

molecular compound, covalent bonds

200

Name each of the following molecular compounds:
a. PBr₃
b. Cl₂O
c. CBr₄
d. HF
e. NF₃

a. Phosphorus tribromide
b. Dichlorine oxide
c. Carbon tetrabromide
d. Hydrogen fluoride
e. Nitrogen trifluoride

300

a. N₂O₃
b. Si₂Br₆
c. P₄S₃
d. PCl₅
e. SeF₆

a. Dinitrogen trioxide
b. Disilicon hexabromide
c. Tetraphosphorus trisulfide
d. Phsphorus pentachloride
e. Selenium hexafluoride

400

Write the formula for each of the following molecular compounds:
a. Carbon tetrachloride
b. Carbon monoxide
c. Phosphorus trifluoride
d. Dinitrogen tetroxide

a. CCl₄
b. CO
c. PF₃
d. N₂O₄

500

Name each of the following ionic or molecular compounds:
a. Al₂(SO₄)₃
b. Zn₃(PO₄)₂
c. N₂O
d. Mg(OH)₂

a. Aluminum sulfate
b. Zinc phosphate
c. Dinitrogen oxide
d. Magnesium hydroxide