Free Printable Bonding Test Review

1.

An ionic bond is the attraction between:

a)

oppositely charged ions

b)

similarly charged ions

c)

neutral ions

d)

neutral atoms

2.

A(n) _________ is an ion with a positive (+) charge.

a)

anion

b)

cation

c)

ion

d)

solute

3.

Atoms gain or lose electrons to become stable by satisfying this rule.

a)

Lewis Structure rule

b)

Periodic Law

c)

octet rule

d)

Ionic Law

4.

What do you call a bond that forms when electrons are transferred from one atom to another?

a)

a compound bond

b)

an ionic bond

c)

a crystal bond

d)

an atomic bond

5.

What do atoms that form positive ions tend to do?

a)

Tend to lose electrons

b)

Tend to lose protons

c)

Tend to gain electrons

d)

Tend to gain protons

6.

What elements generally make an ionic bond?

a)

metal and nonmetal

b)

2 or more nonmetals

c)

metal

d)

none of the above

7.

What is a valence electron?

a)

an electron that is found in the outermost shell of an atom.

b)

an electron found in the innermost shell of an atom.

c)

an electron found in the middle shell.

8.

What is the number of valence electrons for Oxygen?

a)

8

b)

6

c)

2

d)

1

9.

This type of model shows only the valence electrons of an element?

a)

Bohr diagram

b)

Childers model

c)

Lewis-dot diagram

d)

What is a valence electron again?

10.

Magnesium bromide is an ionic compound with the chemical formula MgBr₂. What does the "2" tell you?

a)

There are 2 bromide ions for every magnesium ion

b)

Bromide has a 2- charge

c)

Bromide has a 2+ charge

d)

There are 2 magnesium ions to every bromide ion

11.

How many electrons does #15 phosphorus need to gain to be stable?

a)

one

b)

two

c)

three

d)

four

12.

A bond between a nonmetal and a nonmetal is called a(n)

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

transfer bond

13.

What can be generalized about covalent bonds?

a)

Electrons will be exchanged.

b)

Electrons will be transferred.

c)

Electrons will be given and taken.

d)

Electrons will be shared.

14.

What is it called if there are three-pairs of electrons being shared?

a)

Triple Bond

b)

Three Single Bonds

c)

Tribond

d)

Double and Single Bond Combo

15.

Carbon is in 4A, so how many bonds can it form based on electrons needed to fill its outer shell?

a)

1

b)

3

c)

4

d)

5

16.

What two types of atoms make a covalent bond?

a)

2 Nonmetals

b)

1 Nonmetal & 1 Metal

c)

2 Metals

d)

2 Noble Gases

17.

What is a diatomic element?

a)

a metal bonded with a nonmetal

b)

2 or more nonmetals bonded together

c)

2 or more metals bonded together

d)

2 atoms of the same element bonded together

18.

How many electrons are shared in a double bond?

a)

2

b)

4

c)

6

d)

8

19.

Which of the following is NOT an ionic compound:

a)

CaO

b)

NaOH

c)

BaCl₂

d)

Br₂

20.

What is the correct formula for this molecule?

a)

CH

b)

C₁H⁴

c)

CH₄

d)

C₄H

21.

What is the correct Lewis Dot Structure for NH₃?

a)

b)

c)

d)

22.

Which is the correct molecular structure for carbon dioxide CO₂?

a)

b)

c)

d)

23.

Is Hydrogen considered a metal or a non-metal?

a)

Metal

b)

Non-metal

24.

In metallic bonds, the force of attraction is between

a)

positive and negative ions

b)

cations and electrons

c)

two different metals

d)

neutrons and electrons

25.

Metals are used to make electric wires because metals (choose all that apply)

a)

are ductile

b)

are shiny

c)

have free moving electrons

d)

form a lattice

26.

How does a metallic lattice differ from an ionic crystal?

a)

A metallic lattice is less flexible

b)

A metallic lattice can change shape without breaking

c)

A metallic lattice shatters when struck

27.

An alloy of iron and carbon is

a)

more likely to rust than pure iron

b)

weaker than pure iron

c)

a mixture of two METALS

d)

known as steel

28.

True or False: A metallic bond may form between a metal and any other element

a)

True

b)

False

29.

True or False: Metals can be shaped into thin sheets

a)

True

b)

False

30.

Metal ions are surrounded by a "sea" of POSITIVE charge

a)

True

b)

False

31.

What are some benefits of alloys? (choose all that apply)

a)

they can be stronger than pure metal

b)

they may not rust/corrode as easily

c)

they don't have electrons

d)

they form covalent bonds

32.

Atoms with greatly differing electronegativity values are expected to form ________.

a)

no bonds

b)

polar covalent bonds

c)

nonpolar covalent bonds

d)

triple bonds

e)

ionic bonds

33.

Metals typically have ________ electronegativity values.

a)

high

b)

low

c)

negative

d)

no

e)

none of these

34.

Nonmetal elements typically have ________ electronegativities.

a)

low

b)

high

c)

neutral

d)

strong

e)

none of these

35.

The electron pair in a C - F bond could be considered

a)

closer to C because carbon has a larger radius and thus exerts greater control over the shared electron pair

b)

closer to F because fluorine has a higher electronegativity than carbon

c)

closer to C because carbon has a lower electronegativity than fluorine

d)

an inadequate model because the bond is ionic

e)

centrally located directly between the C and F

36.

$N_2O$ is a ________ molecule.

a)

ionic

b)

covalent

37.

$Al_2O_3$ is a ________ molecule.

a)

ionic

b)

covalent

38.

$CF_4$ is a ________ molecule.

a)

nonpolar

b)

polar

39.

$H_2S$ is a ________ molecule.

a)

nonpolar

b)

polar

40.

$I_2$ is a ________ molecule.

a)

nonpolar

b)

polar

41.

$CO$ is a ________ molecule.

a)

nonpolar

b)

polar

42.

The electron configuration for $Ca^{2+}$ is identical with

a)

Ne

b)

Kr

c)

Ca

d)

Ar

43.

Magnesium reacts with sulfur to form

a)

$MgS$

b)

$MgS_2$

c)

$Mg_2S$

d)

$Mg_2S_3$

e)

none of these

44.

Calcium reacts with fluorine to form

a)

$CaF$

b)

$CaF_2$

c)

$Ca_2F$

d)

$Ca_2F_3$

e)

none of these

45.

Which of the following is the product of the reaction between $Al$ and $O_2$ ?

a)

$AlO$

b)

$AlO_2$

c)

$AlO_3$

d)

$Al_3O_2$

e)

$Al_2O_3$

46.

When they react chemically, the alkali metals (Group 1)

a)

gain one electron

b)

gain seven electrons

c)

gain or lose seven electrons

d)

lose one electron

47.

How many lone pairs of electrons are in the Lewis structure for ammonia, $NH_3$ ?

a)

0

b)

1

c)

2

d)

3

e)

4

48.

Which of the following has a double bond?

a)

$H_2O$

b)

$NH_3$

c)

$O_2$

d)

$CO$

e)

$H_2S$

49.

Which of the following has a double bond?

a)

$H_2O$

b)

$C_2H_2$

c)

$C_2H_4$

d)

$CN$

e)

none of these

50.

One of the most important characteristics of the water molecule is its ________, which allows it to surround and attract both positive and negative ions.

a)

polarity

b)

strength

c)

magnetism

d)

fluidity

e)

stability

51.

Characteristics of METALS - check all that apply.

a)

Brittle

b)

Ductile

c)

Lose valence electrons

d)

Gain valence electrons

e)

Malleable

52.

Valence electrons - check all that apply

a)

inner most electrons

b)

responsible for an atoms chemical behavior (bonding)

c)

only found in the s orbitals

d)

outer most electrons

53.

When an atom gains electrons it

a)

becomes smaller

b)

becomes larger

c)

collapses

d)

explodes

54.

When a magnesium atom becomes an ion it

a)

loses 2 electrons

b)

gains 2 electrons

c)

gains 2 protons

d)

loses 2 protons

55.

In a single bond between two atoms, the number of shared electrons is

a)

2

b)

4

c)

6

d)

8

56.

Atoms are most stable when their outer shell is complete.

a)

True

b)

False

57.

Why do elements form chemical bonds?

a)

Because they're friendly

b)

To create a new element

c)

To become stable

d)

Because they all need to gain more electrons

58.

Nonmetals (like Cl) typically ____ electrons when they form ionic bonds.

a)

Gain

b)

Lose

c)

Keep the same

59.

Where are the nonmetals typically located on the periodic table?

a)

Left side

b)

Middle

c)

Right side

60.

Fill in the blanks. $C\ell_2$ has a low boiling point because it is a ____ compound. It has ____ intermolecular forces of attraction between molecules. ____ energy is required to overcome them.

a)

ionic, strong, Much

b)

covalent, strong, Much

c)

ionic, weak, Less

d)

covalent, weak, Less

61.

The following properties are all characteristics of ionic compounds EXCEPT

a)

solid at room temperature

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

62.

Which of the following is NOT a property of ionic compounds?

a)

They conduct electricity when molten

b)

They conduct electricity when in solution

c)

They have high boiling points

d)

They are insoluble in water

63.

What force holds together cations and anions in ionic bonds?

a)

The electrical attraction between the positive cation and the negative anion

b)

The electrons shared between the positive cation and the negative anion

c)

The magnetic attraction between the positive cation and the negative anion

d)

The gravitational attraction between two pieces of matter

64.

Hydrogen needs _____ electrons in its valence shell to be stable.

a)

4

b)

6

c)

8

d)

2

65.

Which of the following is an acceptable Lewis structure for CH₃Cl?

a)

Option A

b)

Option B

c)

Option C

d)

Option D

66.

NaCl, otherwise known as table salt, is an Ionic Compound. In an ionic compound

a)

a positively charged group of atoms attract a negatively charged group of atoms

b)

ions are held together by electrostatic force

c)

the net charge on the compound is zero

d)

metals tend to lose electrons while non-metals tend to gain electrons

e)

all of the above

67.

This type of bond can form multiple ones, such as double and triple bonds.

a)

Covalent

b)

ionic

68.

The physical state at room temperature for almost all ionic compounds is:

a)

solid

b)

liquid

c)

gas

d)

different for each ionic compound

69.

Because of it's dissociation into it's component parts in water, high conductivity are generally observed for this species.

a)

anion

b)

cation

c)

ionic compound

d)

Covalent

70.

When writing the Lewis Dot structure of this species, there are typically no dots around the chemical symbol.

a)

anion

b)

cation

c)

ionic compound

d)

monoatomic ion

71.

When writing the Lewis Dot structure of this species,there are typically 8 dots around the chemical symbol

a)

anion

b)

cation

c)

ionic compound

d)

monoatomic compound

72.

In this species it is important that the charges be perfectly balanced

a)

anion

b)

cation

c)

ionic compound

d)

monoatomic ion

73.

This picture shows what type of bond?`

a)

Covalent

b)

Ionic

74.

Would an N---O bond, be polar or nonpolar?

a)

polar

b)

nonpolar

c)

neither

75.

Which is a more electronegative element?
N or O

a)

N

b)

O

Bonding Test Review

Total questions: 75

Worksheet time: 46mins

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