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Unit 4 Review Test

Total questions: 60

Worksheet time: 2hrs 49mins

Name
Class
Date
1.

Ionic bonds are between...

a)

nonmetals and nonmetals

b)

carbon and oxygen

c)

metals and nonmentals

d)

hydrogen and chlorine

2.

Covalent bonds are between...

a)

two or more nonmetals

b)

sodium and chlorine

c)

metals and metals

d)

metals and nonmetals

3.
What kind of bond forms when atoms share electrons?
a)
ionic
b)
covalent
c)
artificial
d)
univalent
4.
What kind of bond forms when atoms exchange electrons?
a)
ionic
b)
covalent
c)
artificial
d)
univalent
5.
What are valence electrons?
a)
sum of the protons and neutrons
b)
protons minus electrons
c)
electrons in the inner shells
d)
electrons in the outer shell
6.
What is the subatomic particle that gives the nucleus its positive charge?
a)
Proton
b)
Neutron
c)
Electron
d)
Galvatron
7.
The properties of a compound is different than the properties of the elements that make it up
a)
True
b)
False
8.
What kind of bond is formed when a hydrogen and a hydrogen shares a electron..
a)
Covalent Bond
b)
Ionic Bond
c)
Metallic Bond
d)
Treasury Bond
9.

Why do the noble gases not react with other elements?

a)

They don't want to

b)

They need many electrons

c)

They have full outer energy levels

d)

Their protons and electrons are balanced

10.

What kind of bond is formed when a sodium and chlorine bond..

a)

Covalent Bond

b)

Ionic Bond

c)

Metallic Bond

d)

Treasury Bond

11.

Chemical bond is ...

a)

the physical mixing of two different atoms.

b)

the force that holds two atoms together

c)

the energy used up when two atoms combined.

d)

the temperature that changes the phase of matter.

12.

What kind of bond is formed when carbon and hydrogen bond..

a)

Covalent Bond

b)

Ionic Bond

c)

Metallic Bond

d)

Treasury Bond

13.

Why do elements bond?

a)

To be friends

b)

To create a new element

c)

To become stable

d)

To get bigger

14.

How many valence electrons does Oxygen (O) have?

a)

6

b)

8

c)

15

d)

16

15.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

16.

When electrons are lost by one atom and gained by another, so that they both get full outer shells.

a)

Covalent bond

b)

Ionic bond

c)

Pairing

d)

Compound

17.
Where are the nonmetals located on the periodic table? 
a)
Blue
b)
Red
c)
Green
18.
If an atom loses two electrons what charge will it have?
a)
-2
b)
-1
c)
+1
d)
+2
19.
If an atom gains two electrons what charge will it have?
a)
-2
b)
-1
c)
+1
d)
+2
20.
If an atom has 7 protons and 7 electrons what charge will it have?
a)
-2
b)
-1
c)
0
d)
+2
21.
Elements that do not have full outer energy levels are more stable in __________________.
a)
bonds
b)
formulas
c)
reactions
d)
compounds
22.
A _______ is a charged particle because it has more or fewer electrons than protons.  When an atom _____ an electron, it becomes a positively charged ion.  When an atom ____an electron, it becomes a negatively charged ion.
a)
isotope, gains, loses
b)
isotope, loses, gains
c)
ion, loses, gains
d)
ion, gains, loses
23.
The sum of the charges on the ions in a unit of the compound is ___________. 
a)
positive
b)
negative
c)
zero
d)
±1
24.

The 3 types of chemical bonds are ________, ________, and ______. (Choose 3)

a)

ionic

b)

valence

c)

covalent

d)

metallic

e)

atomic

25.
What is the name for an ion with a negative charge?
a)
cation
b)
anion
c)
onion
d)
union
26.

Which compound has high melting point?

a)

Ionic

b)

Covalent

27.

The octet rules states that most elements want to have _____ valence electrons.

a)

2

b)

4

c)

6

d)

8

28.

Which of the following is NOT an ionic bond?

a)

NH3

b)

KCl

c)

K3N

d)

NaCl

29.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
30.

Which of the following is the correct Lewis dot between Rb and O?

a)

b)

c)

d)

31.

What is the correct Lewis structure for BF3?

a)
b)
c)
d)

BF3 (The formula is the Lewis Structure)

32.

What category of element usually forms a positive ion?

a)

Metals

b)

Nonmetals

c)

metalloids

d)

Noble gases

33.

Which category of elements usually form negative ions?

a)

metals

b)

nonmetals

c)

metalloids

d)

noble gases

34.
Which of the following has a full valence shell?
a)
Oxygen
b)
Neon
c)
Barium
d)
Carbon
35.
What happens when the sodium atom loses an electron?
a)
It become negatively charged 
b)
It become positively charged
c)
none
36.
In what form can an ionic compound conduct electricity?
a)
when dissolved in water
b)
as a solid
c)
as a crystal
d)
when warmed slightly
37.
What is the chemical name for the compound with the formula Na₂S?
a)
sodium sulfide
b)
sodium fluoride
c)
magnesium sulfide
d)
lithium oxide
38.

Why are metals malleable?

a)

They are shiny

b)

The electrons are held tightly within the lattice structure making it strong

c)

The electrons are delocalized and able to move between the atoms

d)

The electrons are shared between two metal ions and this holds the atoms together

39.

Which of these are considered properties of metals? (choose ALL that apply)

a)

brittleness

b)

low melting point

c)

luster (shininess)

d)

malleability

e)

ductility

40.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
41.
This could be the dot diagram of
a)
Ne
b)
H
c)
C
d)
F
42.
Name this compound:   MgS
a)
Sulfur Magnesium
b)
Magnesium Sulfate
c)
Magnesium Sulfur
d)
Magnesium Sulfide
43.

Mg(NO3)2

a)

magnesium nitrate

b)

magnesium nitrite

c)

magnesium nitride

d)

magnesium nitrogen oxide

44.

magnesium hydroxide

a)

Mg(OH)2

b)

MgOH2

c)

MgOH

d)

MgO

45.

ammonium sulfide

a)

(NH4)2S

b)

NH4S

c)

(NH4)2SO4

d)

NH4(S)2

46.

strontium dichromate

a)

SrCr2O7

b)

Sr2(Cr2O7)2

c)

SrCrO4

d)

Sr2(CrO4)2

47.

What's the correct formula for titanium (II) nitrate?

a)

Ti(NO3)2

b)

Ti(NO3)

c)

(NO3)Ti

d)

none of the above

48.

What's the formula for iron(II) sulfide?

a)

FeS

b)

Fe2S

c)

SFe

d)

S2Fe

49.

What's the name of CdS?

a)

Cadmium Sulfate

b)

Cadmium (II) Sulfide

c)

Cadmium Sulfur

d)

None of the above

50.

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

a)

True

b)

False

51.

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

52.
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.
53.
Which of these is NOT an alloy?
a)
bronze
b)
copper
c)
brass
d)
stainless steel
54.

What is the sea of electrons model related to?

a)

Covalent bonding

b)

Hydrogen bonding

c)

Ionic bonding

d)

Metallic bonding

55.

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

56.

What is an alloy?

a)

A compound with only one type of metal

b)

Composed of two or more elements, at least one of which is a metal

c)

A mixture of non-metallic elements

d)

A pure metal

57.

How many Lewis Dots should Sulfur have?

a)

16

b)

6

c)

7

d)

8

58.

H2O is classified as a(n)

a)

Metallic molecule

b)

Covalent molecule

c)

Ionic molecule

d)

Lewis molecule

59.

Check all element pairs that will form a covalent bond. (Nonmetal + Nonmetal)

a)

S and O

b)

C and F

c)

H and Cl

d)

Na and O

e)

Mg and I

60.

14. Using the image, identify what type of chemical bond would most likely be formed?

a)

An ionic bond because there are positive and negative charges found between the aluminum atoms.

b)

A covalent bond because the electrons are being shared.

c)

A metallic bond because the electrons are being pooled and shared between metal atoms.

d)

An ionic bond because a bond is formed between metal and nonmetal atoms.

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