Free Printable Chapter 6 Practice

1.

How many valence electrons does Lithium (Li) have?

a)

1

b)

2

c)

3

d)

0

2.

How many valence electrons does Magnesium (Mg) have? (Electron configuration: 3s²)

a)

2

b)

4

c)

6

d)

8

3.

How many valence electrons does Sulfur (S) have? (Electron configuration: 3s²3p⁴)

a)

6

b)

4

c)

2

d)

8

4.

How many valence electrons does Bromine (Br) have?

a)

5

b)

6

c)

7

d)

8

5.

What are chemical bonds formed by?

a)

Atoms losing, gaining, or sharing valence electrons

b)

Atoms splitting into smaller atoms

c)

Atoms changing color

d)

Atoms evaporating

6.

Eight valence electrons is called a _________.

a)

noble gas configuration

b)

octet rule

c)

covalent bond

d)

isotope

7.

In the example given, Argon (Ar) has the electron configuration 3s²3p⁶. Is this a very stable element?

a)

True

b)

False

8.

What type of compound is formed by ionic bonds?

a)

Molecular compound

b)

Ionic compound

c)

Metallic compound

d)

Covalent compound

9.

What type of compound is formed by covalent bonds?

a)

Ionic compound

b)

Molecular compound

c)

Metallic compound

d)

Noble gas

10.

What is a cation?

a)

A) A positively charged ion

b)

B) A negatively charged ion

c)

C) A neutral atom

d)

D) An atom that gains electrons

11.

What is an anion?

a)

A) A positively charged ion

b)

B) A negatively charged ion

c)

C) A neutral atom

d)

D) An atom that loses electrons

12.

Fill in the blank: Atoms form positively charged ions when they ______ electrons and negatively charged ions when they ______ electrons.

a)

lose; gain

b)

gain; lose

c)

share; lose

d)

lose; share

13.

Refer to the diagram showing the transfer of electrons between Na and Cl. Which atom loses an electron and which atom gains an electron?

a)

Na loses an electron; Cl gains an electron.

b)

Cl loses an electron; Na gains an electron.

c)

Both Na and Cl lose electrons.

d)

Both Na and Cl gain electrons.

14.

Ionic bonds are formed by the strong attractive forces between ______ and ______ ions.

a)

positive; negative

b)

neutral; positive

c)

negative; neutral

d)

positive; positive

15.

In ionic bonding, ions form when atoms gain or lose their valence electrons to form a stable electron configuration. Metals in Group 1A (1), Group 2A (2), and Group 3A (13) have low ________ energies.

a)

ionization

b)

electronegativity

c)

atomic

d)

melting

16.

In ionic bonding, ions form when atoms gain or lose their valence electrons to form a stable electron configuration. Metals in Group 1A (1), Group 2A (2), and Group 3A (13) readily lose one or more of their valence electrons to form ions with a ________ charge. Fill in the blank.

a)

positive

b)

negative

c)

neutral

d)

zero

17.

In ionic bonding, ions form when atoms gain or lose their valence electrons to form a stable electron configuration. Metals in Group 1A (1), Group 2A (2), and Group 3A (13) lose electrons until they have the same number of valence electrons as the nearest noble gas, usually ______ valence electrons. What is the correct number of valence electrons?

a)

eight

b)

two

c)

four

d)

six

18.

What is the electron configuration of sodium?

a)

1s² 2s² 2p⁶ 3s¹

b)

1s² 2s² 2p⁶ 3p¹

c)

1s² 2s² 2p⁵ 3s²

d)

1s² 2s² 2p⁶ 3s²

19.

True or False: Metals have high ionization energies.

a)

True

b)

False

20.

Nonmetals in Group 5A (15), Group 6A (16), and Group 7A (17) have high ionization energies.

a)

True

b)

False

21.

Nonmetals gain electrons until they have the same number of valence electrons as the nearest noble gas, usually eight valence electrons.

a)

True

b)

False

22.

Fill in the blank: The electron configuration for chlorine (Cl) is _____

a)

1s2 2s2 2p6 3s2 3p5

b)

1s2 2s2 2p6 3s2 3p6

c)

1s2 2s2 2p6 3s2 3p4

d)

1s2 2s2 2p6 3s2 3p3

23.

Refer to the diagram of the chlorine atom. The orbital that contains 5 electrons in the outermost shell is:

a)

3p orbital

b)

2p orbital

c)

3s orbital

d)

1s orbital

24.

What is the nearest noble gas to the Li+ ion?

a)

He

b)

Ne

c)

Ar

d)

Kr

25.

What is the nearest noble gas to the Na+ ion?

a)

Ne

b)

He

c)

Ar

d)

Kr

26.

What is the nearest noble gas to the K+ ion?

a)

Ar

b)

Ne

c)

He

d)

Kr

27.

What is the nearest noble gas to the Rb+ ion?

a)

Kr

b)

Ne

c)

Ar

d)

Xe

28.

What is the nearest noble gas to the Cs+ ion?

a)

Xe

b)

Ne

c)

Ar

d)

Kr

29.

What is the nearest noble gas to the N3- ion?

a)

Ne

b)

He

c)

Ar

d)

Kr

30.

What is the nearest noble gas to the O2- ion?

a)

Ne

b)

He

c)

Ar

d)

Kr

31.

What is the nearest noble gas to the F- ion?

a)

Ne

b)

He

c)

Ar

d)

Kr

32.

What is the nearest noble gas to the S2- ion?

a)

Ar

b)

Ne

c)

Kr

d)

Xe

33.

What is the nearest noble gas to the Cl- ion?

a)

Ar

b)

Ne

c)

Kr

d)

Xe

34.

What is the nearest noble gas to the Br- ion?

a)

Kr

b)

Ne

c)

Ar

d)

Xe

35.

What is the nearest noble gas to the I- ion?

a)

Xe

b)

Ne

c)

Ar

d)

Kr

36.

Given the atomic symbol, determine the number of protons, neutrons, and electrons in the following ion: 55Co3+.

a)

Protons: 27, Neutrons: 28, Electrons: 24

b)

Protons: 27, Neutrons: 30, Electrons: 27

c)

Protons: 28, Neutrons: 27, Electrons: 24

d)

Protons: 27, Neutrons: 28, Electrons: 27

37.

Write the formula and the symbol of an ion with 16 protons and 18 electrons.

a)

S²⁺

b)

Ar

c)

Ar²⁺

d)

S²⁻

e)

P²⁻

38.

What are ionic compounds?

a)

Compounds made of only positive charges

b)

Compounds made of only negative charges

c)

Compounds consisting of positive and negative charges held together by strong electrical attractions between oppositely charged ions

d)

Compounds that are always liquids at room temperature

39.

Fill in the blank: The strong electrical attractions between oppositely charged ions in ionic compounds are called _________.

a)

ionic bonds

b)

covalent bonds

c)

metallic bonds

d)

hydrogen bonds

40.

Which of the following are properties of ionic compounds? Choose all that apply.

a)

Low melting points

b)

High melting points

c)

Liquids at room temperature

d)

Solids at room temperature

41.

The diagram shows the structure of sodium chloride. Which ions are present in sodium chloride?

a)

Na+ and Cl-

b)

K+ and Br-

c)

Ca2+ and O2-

d)

H+ and OH-

42.

In a chemical formula, the symbols and subscripts are written in the lowest whole-number ratio of the atoms or ions.

a)

True

b)

False

43.

In a chemical formula, the sum of ion charges equals ____.

a)

zero

b)

one

c)

two

d)

ten

44.

What is the lowest whole number combination for a compound called?

a)

Molecule

b)

Formula unit

c)

Isotope

d)

Ion

45.

In the formation of NaCl, which atom loses an electron and which atom gains an electron?

a)

Na loses an electron, Cl gains an electron.

b)

Cl loses an electron, Na gains an electron.

c)

Both Na and Cl lose electrons.

d)

Both Na and Cl gain electrons.

46.

To balance ionic charge in an ionic compound, what must be true?

a)

Total positive charge > total negative charge

b)

Total positive charge < total negative charge

c)

Total positive charge = total negative charge

d)

Total positive charge is ignored

47.

In the formation of MgCl2, how many electrons does magnesium lose?

a)

2 electrons

b)

1 electron

c)

3 electrons

d)

0 electrons

48.

In the formation of MgCl2, each chlorine atom gains ____.

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

0 electrons

49.

What is the chemical formula for magnesium chloride?

a)

MgCl

b)

MgCl2

c)

Mg2Cl

d)

Mg2Cl2

50.

According to the image, what must be true to balance ionic charge in an ionic compound?

a)

Total positive charge must be greater than total negative charge

b)

Total positive charge must be less than total negative charge

c)

Total positive charge must equal total negative charge

d)

Total negative charge must be zero

51.

In the formation of Na2S, how many electrons does each sodium atom lose?

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

0 electrons

52.

Fill in the blank: The formula for sodium sulfide is _____

a)

Na2S

b)

NaS

c)

Na2SO4

d)

NaSO3

53.

What is the name of the compound with the formula Na2S?

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfur

54.

What is the ionic formula of the compound formed between Al³⁺ and Cl⁻ ions?

a)

AlCl₃

b)

AlCl

c)

Al₂Cl₃

d)

Al₃Cl₂

55.

What is the ionic formula of the compound formed between Mg²⁺ and N³⁻ ions?

a)

Mg₃N₂

b)

MgN

c)

Mg₂N₃

d)

MgN₂

56.

What is the ionic formula of the compound formed between calcium and bromine?

a)

Ca₂Br₂

b)

Ca₂Br

c)

CaBr

d)

Ca₇Br₂

e)

CaBr₂

57.

According to the instructions for naming ionic compounds: 1. The name of the metal is written first and is the same as the name of the element. 2. The name of the nonmetal is the first syllable of the nonmetal name + ide ending and is written second. 3. A space is placed between the name of the metal and nonmetal ion. What is the name of the compound KI?

a)

Potassium iodide

b)

Potassium oxide

c)

Potassium chloride

d)

Potassium fluoride

58.

What is the name of the compound MgBr2?

a)

Magnesium bromide

b)

Magnesium bromate

c)

Manganese bromide

d)

Magnesium dibromide

59.

According to the instructions for naming ionic compounds: 1. The name of the metal is written first and is the same as the name of the element. 2. The name of the nonmetal is the first syllable of the nonmetal name + ide ending and is written second. 3. A space is placed between the name of the metal and nonmetal ion. What is the name of the compound Al2O3?

a)

Aluminum oxide

b)

Aluminum trioxide

c)

Aluminum oxygen

d)

Alumina

60.

Identify the cation and anion in the compound K2O. The cation, K+, is from which group?

a)

Group 1A (1)

b)

Group 2A (2)

c)

Group 3A (13)

d)

Group 7A (17)

61.

Identify the cation and anion in the compound K2O. The anion, O2-, is from which group?

a)

Group 6A (16)

b)

Group 1A (1)

c)

Group 2A (2)

d)

Group 7A (17)

62.

STEP 2: Name the cation in K2O by its element name. The cation, K+, is ________.

a)

potassium

b)

sodium

c)

calcium

d)

magnesium

63.

Name the anion in K2O by using the first syllable of its element name followed by 'ide'. The name of the anion O2- is ________.

a)

oxide

b)

oxalate

c)

oxygenide

d)

oxonate

64.

What is the name of K2O?

a)

potassium oxide

b)

potassium peroxide

c)

potassium hydroxide

d)

potassium carbonate

65.

What is the name of the ionic compound Ca3N2?

a)

calcium nitride

b)

calcium nitrate

c)

calcium nitrite

d)

calcium nitride oxide

66.

What is the formula for the ionic compound formed with $Na^+$ and $PO_4^{3-}$ ?

a)

Na2PO4

b)

NaPO4

c)

Na3PO4

d)

Na(PO4)3

e)

Na2(PO4)3

Chapter 6 Practice

Total questions: 66

Worksheet time: 33mins

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