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Unit 05 Exam Review

Total questions: 68

Worksheet time: 1hrs 8mins

Name
Class
Date
1.

Ionic bonds form between...

a)

nonmetals and nonmetals

b)

metals and nonmetals

c)

metals and metals

d)

noble gases

2.

In an ionic bond, the atom with ___ electronegativity will take an electron from the other atom.

a)

higher

b)

lower

c)

equal

d)

it cannot be predicted

3.

In ionic bonds, electrons tend to be transferred...

a)

from halogens to alkali metals

b)

from nonmetals to metals

c)

from metals to nonmetals

d)

they are shared equally

4.

In a covalent bond...

a)

A metal bonds with a metal

b)

One electron is shared

c)

A pair of electrons are shared

d)

Atoms try to get 6 valence electrons total

5.

A covalent bond that is polar...

a)

Has an uneven share of electrons

b)

Electrons are shared equally

c)

The bond is magnetic

d)

H2 is an example

6.

When two atoms bond, if there is a LARGE difference in electronegativity, they will form...

a)

A covalent bond

b)

An ionic bond

c)

A metallic bond

d)

A double bond

7.

When two atoms bond, if there is a very SMALL difference in electronegativity, they will form...

a)

A nonpolar covalent bond

b)

A polar covalent bond

c)

An ionic bond

8.

In a nonpolar covalent bond...

a)

The electronegativity difference is less than 0.3 between the atoms

b)

H2 (two hydrogens bonded) is an example

c)

There is an equal share of electrons

d)

All of the above

9.
When an atom loses an electron, it becomes a:
a)
positive ion
b)
negative ion
c)
neutral ion
d)
neutral atom
10.
A(n) _________ is an ion with a positive (+) charge.
a)
anion
b)
cation
c)
ion
d)
solute
11.
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
12.
Elements in Group 1 lose one electron to form ions with a _________________ charge.
a)
1+
b)
2+
c)
0
d)
1-
13.
A charged particle that has gained at least one electron is called a(n) _____.
a)
Anion
b)
Cation
c)
Anonion
d)
chemistry cat
14.
When two atoms share electrons, a chemical bond is formed.  This type of bond is called:
a)
covalent bond
b)
ionic bond
c)
crystal bond
d)
polyatomic bond
15.
A covalent compound contains _______.
a)
Alkali metals
b)
Two metals
c)
A metal and a nonmetal
d)
Nonmetals
16.
When two atoms share electrons, a chemical bond is formed.  This type of bond is called:
a)
covalent bond
b)
ionic bond
c)
crystal bond
d)
polyatomic bond
17.
Which group of elements have full outer shells?
a)
The alkali metals
b)
The full gases
c)
The halogens
d)
The noble gases
18.
How many valence electrons do most atoms need to have a complete outer shell and be happy?
a)
1
b)
8
c)
10
d)
5
19.

The element rubidium, Rb, is immediately below potassium in the Periodic Table.

It reacts with bromine to form the compound rubidium bromide.

Which descriptions of this compound are correct?

a)

A

b)

B

c)

C

d)

D

20.

Ionic compounds contain ions. The numbers of electrons, neutrons and protons in four particles, W, X, Y and Z, are shown in the figure.State which particle, W, X, Y or Z, is a negative ion.

a)

W

b)

X

c)

Y

d)

Z

21.
Why do bonds form?
a)
To fill the valence shell of electrons for the elements involved
b)
to release energy stored in the bonds
c)
because whenever you mix two chemicals, there will be a reaction
d)
because of attraction
22.
Atoms with a strong attraction for electrons they share with another atom exhibit
a)
zero electronegativity
b)
low electronegativity
c)
high electronegativity
d)
negative electronegativity
23.

Define ionic bonding.

a)

when atoms share electrons so both atoms have a full outer shell

b)

when atoms lose electrons so both atoms have a full outer shell

c)

when atoms swap electrons so both atoms have a full outer shell

d)

when atoms gain electrons so both atoms have a full outer shell

24.

What type of elements can react using ionic bonding?

a)

metals only

b)

non-metals only

c)

metals and non-metals together

d)

any element can react

25.

The bonds in BaO are best described as

a)

covalent, because valence electrons are shared

b)

covalent, because electrons are transferred

c)

ionic, because valence electrons are shared

d)

ionic because electrons are transferred

26.

In an ionic bond, the ions are held together because...

a)

the positive nucleus of each ion attracts the other ion's negatively charged electrons

b)

the ions have opposite charges

c)

as the electron moved from one atom to another it pulled the atom along with it

d)

electrons are being shared

27.

An example of an ionic compound is Sodium Chloride, which is made from Na+ and Cl- ions. Why do these ions form an ionic bond?

a)

They have like charges

b)

They are from the same group

c)

They are from the same period

d)

They have opposite charges

28.

Lithium is in group 1 of the periodic table, which ion would it form?

a)

Li-

b)

Li2-

c)

Li+

d)

Li2+

29.

Oxygen is in group 6 of the periodic table, which ion would it form?

a)

O-

b)

O+

c)

O2-

d)

O2+

30.

Lead Chloride is an ionic compound, made up from Pb2+ ions and Cl- ions. Which is the correct formula for this compound?

a)

PbCl3

b)

PbCl

c)

PbCl4

d)

PbCl2

31.

Which is the correct formula for aluminum sulfide?

a)

AlS

b)

Al3S2

c)

S3Al2

d)

Al2S3

32.
What is the formula for aluminum fluoride?
a)
AlF
b)
Al2F3
c)
AlF3
d)
Al3F2
33.
What is the correct formula for the compound, lithium oxide?
a)
LiO
b)
Li2O
c)
LiO2
d)
Li2O2
34.
A charged particle that has gained or lost electrons is called a _____.
a)
molecule
b)
ion
c)
isotope
d)
element
35.

Beryllium, Be, will ____ valence electrons when forming an ionic bond.

a)

lose 4

b)

gain 4

c)

lose 2

d)

gain 2

36.

Ionic bonds happen because of the ____ of valence electrons.

a)

sharing

b)

transfer

c)

keeping

d)

covering

37.

Sulfur, S, will ____ valence electrons when forming an ionic bond.

a)

gain 1

b)

lose 1

c)

gain 2

d)

lose 2

38.
How many electrons are needed in the outer energy levels of an atom to be stable?
a)
2
b)
4
c)
6
d)
8
39.

What will be the charge of a bromine ion?

a)

+7

b)

-7

c)

-1

d)

+1

40.
How are covalent bonds explained?
a)
When one atom takes the other atom's electron
b)
When the atom shares an electron with an another atom
c)
When the two nucleus merge
d)
When the neutrons leave the nucleus
41.
In chemical compounds, covalent bonds form when
a)
the electronegativity difference between two atoms is very large.
b)
electrons are completely transferred between two metals.
c)
pairs of electrons are shared between two nonmetal atoms.
d)
two nonmetal atoms are attracted to each other by opposite charges.
42.
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.
43.

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

44.
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
45.
How many electrons are shared in a double bond?
a)
2
b)
4
c)
6
d)
8
46.

When two nonmetals do not share electrons evenly, the resulting covalent bond will be

a)

nonpolar

b)

polar

c)

ionic

d)

metallic

47.
The number of bonds an element will form in a covalent compound will be equal to
a)
the number of valence electrons
b)
eight electrons
c)
the number of electrons needed to reach an octet
d)
the group number
48.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
49.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
50.
How many electrons should Chlorine have around its Lewis dot model?
a)
5
b)
6
c)
7
d)
8
51.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
52.
If electrons are shared equally then the bond is....
a)
Non-polar covalent
b)
Ionic
c)
Non-polar ionic
d)
Polar covalent
53.
How many electrons does each line indicate are shared?
a)
1
b)
2
c)
3
d)
4
54.
When writing Lewis Structures, only __________ electrons are used.
a)
Inner shell
b)
Core 
c)
Valence
d)
Stable
55.
Each line in a Lewis Structure represents __________ electron(s).
a)
3
b)
2
c)
1
d)
4
56.
A molecule of methane has what shape?
a)
Tetrahedral
b)
Triangular
c)
Pyramidal
d)
Octahedral
57.
A molecule of water has what shape?
a)
Linear
b)
Tetrahedral
c)
Bent
d)
Triangular
58.
The theory that is used to predict the arrangement of atoms about a central atom is called?
a)
Valence shell repulsion
b)
Valence shell electron sharing
c)
Valence shell electron pair repulsion
d)
Valence electron shell repulsion pair
59.
Atoms of H only form _________ bonds.
a)
Double
b)
Single
c)
Multiple
d)
Triple
60.

NH3 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

61.

CCl4 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

62.
How do covalent bonds form?
a)
Donating & receiving valence e- between atoms.
b)
Opposite slight charges attract each other between compounds.
c)
Scientists are still not sure how they form.
d)
Sharing valence e- between atoms.
63.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
64.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
65.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
66.
What molecular shape is the structure shown here? (H2O)
a)
tetrahedral
b)
trigonal planar
c)
bent
d)
trigonal pyramidal
67.
Which of the following shapes has an unshared pairs of electrons on the central atom? 
a)
Bipyramidal
b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
68.
VSEPR stands for ________ theory.
a)
Valence Structure of Electron Pyramids and Regression
b)
Varied Structures of Electrons Paired and Replaced
c)
Varied Shell Energy of Protons and Radiation
d)
Valence Shell Electron Pair Repulsion

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