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Bonding Test

Total questions: 90

Worksheet time: 4hrs 42mins

Name
Class
Date
1.

The positive ions tend to _____________ electrons.

a)

lose

b)

gain

2.

The negative ions tend to _____________ electrons.

a)

lose

b)

gain

3.

Why do all bonds form?

a)

so the number of protons equals the number of electrons

b)

so an atom can become unstable

c)

to fill the outermost energy level

4.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
5.

What type of elements form cations?

a)

metals

b)

nonmetals

c)

metalloids?

6.

How does calcium become an calcium ion?

a)

it loses 2 electrons

b)

it gains 2 electrons

7.

How many Aluminum atoms are in Al2O3?

a)

3

b)

5

c)

2

d)

1

8.

An atom with 1 valence electron 'needs' a full shell, so it can either gain 7 electrons or lose 1. Which is more likely to occur?

a)

nothing

b)

gain 7

c)

lose 1

9.

How many valence electrons does Boron have?

a)

1

b)

2

c)

3

d)

4

10.

Group numbers on the periodic table help us determine

a)

number of valence electrons

b)

state of the element (solid, liquid, gas)

11.

Valence electrons are found

a)

in the innermost energy level of an atom

b)

in the middle energy levels of an atom

c)

in the outermost energy levels of an atom

12.

Will a chlorine atom gain or lose electrons?

a)

gain

b)

lose

13.

Which of the following is the correct ionic formula for calcium sulfide?

a)

Ca2S2

b)

CaS

c)

S2Ca2

d)

SCa

14.
Ionic bonds form between two ions that have...
a)
ionic compounds
b)
negative charges
c)
positive charges
d)
opposite charges
15.
Fe +2  and  SO4 -2
a)
FeSO4
b)
Fe4(SO4)2
c)
FeSO2
d)
correct answer is not given
16.
An electron has what kind of charge?
a)
no charge
b)
positive 
c)
negative
d)
it depends
17.
a proton has what charge?
a)
positive
b)
negative
c)
no charge
d)
it depends
18.
An atom that has gained or lost electrons is called ...
a)
a winner
b)
an isotope
c)
an ion
d)
a loser
19.
What is the ionic compound formed between K and F?
a)
KF
b)
K2F
c)
KF2
d)
K2F2
20.
Mg2+ and Cl- create...
a)
Mg2Cl
b)
MgCl2
c)
Mg2Cl2
d)
MgCl
21.
Ca2+ and N3- create...
a)
Ca2N3
b)
Ca3N2
c)
CaN3
d)
Ca2N
22.
What charge does a calcium (Ca) ion have?
a)
+1
b)
+2
c)
+3
d)
+4
23.
A phosphorus atom needs to gain ___ electrons to achieve a full octet.
a)
3
b)
4
c)
6
d)
5
24.
What formula results when Ca+2  and  Br- ions bond?
a)
Ca2Br2
b)
CaBr
c)
Ca(br)2
d)
CaBr2
25.

Match the following element to their number of valence electrons:

a)

lithium

1.

1

b)

magnesium

2.

2

c)

phosphorus

3.

5

d)

fluorine

4.

7

e)

neon

5.

8

26.

This family contains elements that all have two valence electrons

a)

alkali metals

b)

noble gases

c)

alkaline earth metals

d)

halogens

27.
How many Valance electrons does Iodine Have?
a)
6
b)
16
c)
7
d)
17
28.

Boron group has (a)   valence electrons

29.

How do covalent bonds help atoms achieve a full outer shell?

a)

Electrons are transferred between atoms until both have full outer shells

b)

The atoms share electrons in order to get a full outer shell

c)

Covalent bonding turns the atoms into ions

d)

It helps the electrons jump to higher energy levels

30.

What kind of bond is shown in the picture?

a)

A single covalent bond

b)

A double covalent bond

c)

A triple covalent bond

d)

An ionic bond

31.

How many electrons are shared in the bond above?

a)

1

b)

2

c)

3

d)

4

32.

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

33.

Is this correct way to draw the Lewis Dot Structure for Carbon?

a)

Yes

b)

No, too many electrons

c)

No, not enough electrons

d)

No, dots are in wrong places

34.

USE THE PERIODIC TABLE

How many valence electrons does Phosphorus have?

a)

31

b)

5

c)

15

d)

4

35.

This type of bond happens when electrons are shared EQUALLY between the two bonded atoms.

a)

Polar covalent

b)

Nonpolar covalent

c)

Ionic

36.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
37.

This is the displayed formula for what covalent compound?

a)

Water

b)

Hydrogen peroxide

c)

Hydrogen oxide

d)

Ethanol

38.

Chlorine is a diatomic element which means in nature, it is found in two's. (Cl2) Chlorine shares one pair of electrons to make sure each atom complete the octet rule. This creates a...

a)

single bond

b)

double bond

c)

triple bond

39.

Oxygen is a diatomic element which means in nature, it is found in two's. (O2) Oxygen shares two pairs of electrons to make sure each atom completes the octet rule. This creates a...

a)

single bond

b)

double bond

c)

triple bond

40.

Nitrogen is a diatomic element which means in nature, it is found in two's. (N2) Nitrogen shares three pairs of electrons to make sure each atom completes the octet rule. This creates a...

a)

single bond

b)

double bond

c)

triple bond

41.

How many covalent bonds are created in a single water molecule?

a)

0

b)

1

c)

2

d)

3

e)

4

42.

How many pairs of valence electrons are being shared in a single ammonia molecule?

a)

0 pair - 0 valence electrons

b)

1 pair - 2 valence electrons

c)

2 pair - 4 valence electrons

d)

3 pair - 6 valence electrons

43.

When assigning the number of individual atoms in a chemical formula it is written as a...

a)

superscript

b)

subscript

c)

coefficient

d)

script

44.

How many total atoms are in the ionic compound Ca(NO3)2 (Calcium nitrate)?

a)

3

b)

5

c)

6

d)

9

e)

10

45.

How many total atoms are in the covalent compound C4H10 (Butane)?

a)

6

b)

8

c)

10

d)

12

e)

14

46.
Ionic or covalent?
NaBr
a)
Ionic
b)
Covalent
47.
Ionic or covalent?
H2O
a)
Ionic
b)
Covalent
48.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
49.
What molecule could this be? 
a)
H2O
b)
CCl4
c)
PCl5
d)
NaCl
50.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
51.

Single bonds are formed when ____ pair(s) of valence electrons are shared.

a)

one

b)

three

c)

two

d)

four

52.

Anions

a)

Gain electrons, has an overall positive charge

b)

Lose electrons, has an overall positive charge

c)

Lose electrons, has an overall negative charge

d)

Gain electrons, has an overall negative charge

53.
What molecule is this?
a)
CO
b)
CO2
c)
C2O
d)
C2O2
54.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
55.

The chemical bond between a non-metal and another non-metal will be a ________ bond.

a)

metal

b)

ionic

c)

covalent

d)

polar

56.

Which is the correct molecular structure for carbon dioxide CO2?

a)
b)
c)
d)
57.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
58.

Match the following descriptions to the type of bond.

Occurs between two nonmetals - (a)  

Occurs between a metal and a nonmetal - (b)  

Choose from the below words
Covalent bond
Ionic bond
59.
Compared to ionic compounds, molecular compounds generally have...
a)
good conductivity
b)
greater densities
c)
more chemical bonds
d)
a low boiling point
60.

Click on the covalent bond

A
B
61.

How do you represent a covalent bond in a Lewis structure?

a)

By a line or a pair of dots

b)

By a circle

c)

By a dashed line

62.

Why do atoms/ions bond?

a)

Repulsion between positive protons and negative electrons

b)

Attraction between positive protons and positive electrons

c)

Attraction between positive protons and negative electrons

d)

Repulsion between positive protons and positive electrons

63.

What are the properties of metallic bonding?

a)

Good conductors of electricity, ductile, malleable, and arranged in crystal lattice structure

b)

Poor conductors of electricity, not ductile, not malleable, and arranged in random structure

c)

Good conductors of electricity, not ductile, not malleable, and arranged in random structure

d)

Poor conductors of electricity, ductile, malleable, and arranged in crystal lattice structure

64.

Which of the following best describes the electron sea model in metallic bonding?

a)

Electrons are shared between two specific atoms.

b)

Electrons are localized around individual atoms.

c)

Electrons are delocalized and shared among all atoms.

d)

Electrons are transferred from one atom to another.

65.

In an ionic bond, electrons are ​ (a)   from the ​ (b)   to the ​ (c)   . Ionic bonds are ​ (d)   because of the big difference in electronegativity.

Choose from the below words
transferred
metal
nonmetal
strong
weak
semimetal
shared
66.

Match the following to form true statements:

a)

When solid, ionic compounds

1.

cannot conduct electricity

b)

When disolved in water, ionic compounds

2.

can conduct electricity

c)

Ionic compounds have

3.

high melting and high boiling points

d)

There are many strong bonds

4.

between ions in an ionic compound.

e)

Elements in group 1 of the periodic table form ions

5.

with a charge of 1+

67.

If an atom gains an electron, it becomes a(n) ​ (a)   which is ​ (b)   charged. If an atom loses an electron, it becomes a(n) ​ (c)   which is ​ (d)   charged.

Choose from the below words
anion
negatively
cation
positively
neutrally
68.

Covalent bonds are formed by sharing an electron between a nonmetal to a ​ (a)   .

Choose from the below words
metal
metalloid
nonmetal
69.

A substance is composed of a Group 2 element that bonds with an element from Group 4. Which type of bonding does this substance have?

a)
metallic
b)

covalent

c)

ionic

d)

hydrogen

70.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
71.
Name the compound S2F8
a)
sulfur (II) fluoride
b)
disulfur octafluoride
c)
sulfur fluorine
d)
sulfur octafluoride
72.
What is the name of CuCl2? 
a)
copper (II) chloride
b)
copper chloride
c)
copper monochloride
d)
copper (I) chloride
73.
How would you say Ni3P2?
a)
nickel (II) phosphide
b)
nickel phosphide
c)
trinickel diphosphide
d)
nickel phosphorous
74.
Write the name for Mn(CO3)2 
a)
manganese (IV) carbonate
b)
manganese (II) carbonide
c)
manganese dicarbonate
d)
manganese carbonate
75.
Name: PI3
a)
phosphorous (III) iodide
b)
monophosphorous iodide
c)
phosphorous triiodide
d)
phosphide
76.
The substance with the formula HCl is called what?
a)
hydrogen chloride
b)
chloric acid
c)
hydrochloric acid
d)
hydrocarbonic acid
77.

Formula for barium sulfide

a)

B2S3

b)

BaS

c)

Ba2S

d)

BaS2

78.

Name for PBr2

a)

phosphorus bromide

b)

phosphorus dibromide

c)

phosphorus dibromine

d)

phosphorus bromine

79.

Formula for cobalt (II) bromide

a)

CoBr

b)

Co2Br2

c)

Co2Br

d)

CoBr2

80.

Name for CO

a)

carbon monoxide

b)

carbon oxide

c)

monocarbon oxide

d)

carbide monoxide

81.
Name the following ionic compound: BeCl2
a)
beryllium chlorine
b)
beryllium II chloride
c)
beryllium chloride
d)
beryllium dichloride
82.
What is the correct formula for the compound, lithium oxide?
a)
LiO
b)
Li2O
c)
LiO2
d)
Li2O2
83.
What is the formula for manganese(III) oxide?
a)
MgO
b)
Mg2O3
c)
MnO
d)
Mn2O3
84.
The formula of calcium phosphate is 
a)
CaPO4
b)
Ca2(PO4)3
c)
Ca3PO4
d)
Ca3(PO4)2
85.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
86.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
87.
What is the name of C3Cl8 ?
a)
Carbon octachloride
b)
Tricarbon octachloride
c)
Carbon trichloride
d)
Octacarbon trichloride
88.
The correct name of Cu₃N₂ is
a)
copper (III) nitride
b)
copper (II) nitride
c)
copper nitride
d)
tricopper dinitride
89.

This image shows the bonding between Lithium and Fluorine. What does the red arrow show?

a)

electrons being shared

b)

electrons being transferred to Fluorine

c)

electrons being transferred to Lithium

d)

electrons being destroyed

90.

Polar molecules

a)

have even charge density

b)

are symmetric

c)

form hydrogen bonds

d)

have 10 atoms per molecule

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