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Review Module 6-8

Total questions: 86

Worksheet time: 2hrs 0mins

Name
Class
Date
1.

In the formation of an ionic compound, a metal atom typically

a)

Gains electrons to become positively charged

b)

Loses electrons to become positively charged

c)

Gains electrons to become negatively charged

d)

Loses electrons to become negatively charged

2.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
3.
What elements generally make a covalent bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
4.

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.

5.

An ionic bond forms when

a)

Valence electrons are shared

b)

a sea of mobile electrons surround the cations

c)

valence electrons are transferred between atoms

d)

none of the above

6.

What type of bond is expected to form between Oxygen (O) and Hydrogen (H)?

a)

Ionic

b)

Covalent

c)

Metallic

7.

Which of the following best describes a valence electron?

a)

an electron located in the outermost energy level of an atom. 

b)

an electron located in the nucleus of an atom.

c)

an electron located in the second energy level.

8.

Which type of bond is formed between sodium and chlorine atoms?

a)

covalent bond

b)

ionic bond

c)

hydrogen bond

d)

metallic bond

9.

Which compound is formed by a complete transfer of electrons between atoms?

a)

H2O

b)

CH4

c)

NaCl

d)

O2

10.

Which suffix is commonly used for naming simple anions?

a)

-ide

b)

-ous

c)

-ic

d)

-ium

11.

What is the primary reason atoms form chemical bonds?

a)

To increase their energy levels

b)

To decrease their temperature

c)

To attain a stable electron configuration

d)

To increase their size

12.

Which of the following best describes the nature of metallic bonds?

a)

A network of positive metal ions immersed in a sea of free electrons.

b)

The covalent sharing of electrons between metal atoms.

c)

The ionic transfer of electrons from metals to non-metals.

d)

The electrostatic attraction between charged particles.

13.

What is the number of valence electrons in Sulfur and its typical ionic charge?

a)

6, -2

b)

4, +2

c)

6, +4

d)

8, -2

14.

How many valence electrons are present in an oxygen atom?

a)

2

b)

4

c)

6

d)

8

15.

How many electrons does this atom need to gain to complete its valence shell?

a)

1

b)

2

c)

3

d)

4

16.

What is the chemical name for FeCl3?

a)

iron (III) chloride

b)

iron chloride

c)

iron monochloride

d)

iron (II) chloride

17.

True or false: Prefixes are not used when writing the names of ionic compounds.

a)

True

b)

False

18.
Roman numerals tell you the ____ of the metal cation(s) in an ionic compound.
a)
number
b)
mass
c)
type
d)
charge
19.

What is the name for KCl

a)

Potassium Chloride

b)

Potassium monochloride

c)

monopotassium Chloride

d)

Potassium hypochlorite

20.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
21.

How many electrons does hydrogen need to achieve a full valence shell?

a)

1

b)

2

c)

3

d)

4

22.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
23.
When writing Lewis Structures, only __________ electrons are used.
a)
Inner shell
b)
Core 
c)
Valence
d)
Stable
24.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
25.

What is the correct formula for Lead(IV) sulfate?

a)

PbSO4

b)

Pb(SO4)2

c)

Pb2(SO4)4

d)

Pb4(SO4)2

26.

In a polar covalent bond, how are the electrons distributed between the atoms?

a)

Equally

b)

Unequally

c)

Not distributed

d)

None of the Above

27.

In a nonpolar covalent bond, how are the electrons distributed between the atoms?

a)

Equally

b)

Unequally

c)

Not distributed

d)

All of the Above

28.

What is the difference in electronegativity between Nitrogen and Silicon?

a)

1.2

b)

0.7

c)

1.0

d)

0.5

29.

If Chlorine has an electronegativity of 3.0 and Sodium has an electronegativity of 0.9, what type of bond is formed between them?

a)

Nonpolar Covalent

b)

Ionic

c)

Moderately Polar Covalent

d)

Very Polar Covalent

30.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
31.
What molecular shape is the structure shown here? (BCl3)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
32.
What molecular shape is the structure shown here? (H2O)
a)
tetrahedral
b)
trigonal planar
c)
bent
d)
trigonal pyramidal
33.

The VSEPR theory states that electrons will

a)

try to move as far apart as possible

b)

form the fewest bonds possible

c)

have an equal number of bonds on all atoms

d)

have larger bond angles to accommodate larger elements

34.

In a chemical equation, what does the coefficient represent?

a)

The number of atoms in a molecule.

b)

The number of molecules in a substance or compound

c)

The number of electrons in an atom.

d)

The number of protons in a nucleus.

35.

Number of O in Mg(NO3)2

a)
4
b)
2
c)

3

d)

6

36.
What does the Law of Conservation of Mass state?
a)
Matter cannot be gained or lost in a chemical reaction.
b)
Matter can only be lost in a chemical reaction.
c)
Matter can only be gained in a chemical reaction.
d)
Matter can be gained and lost in a chemical reaction. 
37.

Balance this equation:

Na + O2 ---> Na2O

a)

2Na + O2 ---> Na2O

b)

4Na + O2 ---> 2Na2O

c)

Na + 2O2 ---> Na2O

d)

Na + O2 ---> 2Na2O

38.

Balance this chemical reaction:

Al + O2 ---> Al2O3

a)

4Al + 3O2 ---> 2Al2O3

b)

2Al + O2 ---> Al2O3

c)

Al + O2 ---> Al2O3

d)

3Al + 2O2 ---> Al2O3

39.

CuCl2  +  Na2CO3 --> CuCO3 + 2NaCl
What type of reaction is this? 

a)
Synthesis 
b)
Decomposition 
c)
Single Replacement
d)
Double Replacement 
40.
2HI --> H2 + I2
a)
synthesis
b)
decomposition
c)
single replacement
d)
double replacement
41.

CH4 + O2 --> CO2 + H2O + ENERGY

a)
single replacement
b)
double replacement
c)
acid base
d)
combustion
42.
Mg + HCl --> MgCl2 + H2
a)
combustion
b)
synthesis
c)
decomposition
d)
single replacement
43.

What type of reaction?

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

44.

Rank these in order of strength:
covalent bond
London / Dispersion forces
hydrogen bond
dipole-dipole attraction

a)
dipole-dipole>covalent bond>hydrogen bond>London
b)
London>dipole-diple>hydrogen bond>covalent bond
c)

covalent bond>hydrogen bond>dipole-dipole>London/Disp.

d)
hydrogen bond>dipole-dipole>London>covalent bond
45.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
46.

What type of force?

a)

intermolecular

b)

intramolecular

47.

Which of the following elements is most likely to form a cation?

a)

Fluorine

b)

Sodium

c)

Chlorine

d)

Oxygen

48.

What is the name of the compound with the formula N2O5

a)

dinitrogen pentoxide

b)

nitrogen trioxide

c)

nitrogen monoxide

d)

nitrogen dioxide

49.

According to the "Activity Series" Chart, which metals are less reactive, those at the top or those at the bottom?

a)

Top

b)

Bottom

c)

Middle

d)

No Reaction

50.

Will Iron (Fe) react with HCL?

a)

Yes, the reaction will occur

b)

No reaction

c)

Maybe

d)

I have no clue

51.

Which types of bonds are known for their high melting points? (Select all that apply)

a)

Metallic Bonds

b)

Ionic Bonds

c)

Nonpolar Covalent Bonds

d)

Polar Covalent Bonds

52.

In the reaction 2H2 + O2 -> 2H2O, which side contains the reactants?

a)

2H2 + O2

b)

2H2O

c)

2H2

d)

O2

53.

What information does a subscript provide in a chemical formula?

a)

The number of molecules

b)

The number of atoms of an element

c)

The type of chemical bond

d)

The state of matter

54.

Which type of element typically forms an anion and what is its charge?

a)

Metal & positive + charge

b)

Nonmetal & negative - charge

c)

Metalloid & positive + charge

d)

Nonmetal & neutral charge

55.

What molecular geometry would PH3 have?

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Bent

d)

Linear

56.

Which of the following elements would have a complete octet in its Lewis Dot Structure?

a)

Neon

b)

Sodium

c)

Chlorine

d)

Oxygen

57.

What is the main use of Lewis Dot Structures in chemistry?

a)

To predict molecular geometry

b)

To calculate atomic mass

c)

To determine the number of protons

d)

To show valence electrons and bonding.

58.

Which of the following elements would have a Lewis Dot Structure with five dots?

a)

Phosphorus

b)

Sulfur

c)

Chlorine

d)

Argon

59.

What is the significance of a pair of dots in a Lewis Dot Structure?

a)

They represent a pair of protons

b)

They indicate a pair of neutrons

c)

They show a pair of valence electrons

d)

They display a pair of atomic masses.

60.

Which of the following elements would have a Lewis Dot Structure with seven dots?

a)

Fluorine

b)

Neon

c)

Sodium

d)

Magnesium

61.

What are the two things you need to know to draw a Lewis Structure?

a)

A) Element symbol and atomic number

b)

B) Element symbol and number of valence electrons

c)

C) Atomic number and atomic mass

d)

D) Number of valence electrons and atomic mass

62.

Which element is an exception in Group 8 with only 2 valence electrons?

a)

Hydrogen

b)

Helium

c)

Lithium

d)

Neon

63.

What are valence electrons?

a)

Electrons in the innermost ring

b)

Electrons in the outermost ring

c)

Protons in the nucleus

d)

Neutrons in the nucleus

64.

What is the main focus when drawing Lewis Structures?

a)

Atomic mass

b)

Valence electrons

c)

Neutrons

d)

Protons

65.

Which group of elements is likely to have similar Lewis Structures?

a)

Elements in the same period

b)

Elements in the same group

c)

Elements with the same atomic mass

d)

Elements with the same number of protons.

66.

What does a Lewis structure represent?

a)

The atomic mass

b)

The valence electrons

c)

The number of protons

d)

The atomic number.

67.

How many valence electrons are represented in the Lewis structure of Aluminum (Al)?

a)

1

b)

3

c)

5

d)

7

68.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

69.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
70.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
71.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

72.

Is this the correct Lewis Dot Structure for phosphorus?

a)

Yes

b)

No

73.

Which is the correct Lewis dot for C?

a)

D

b)

E

c)

F

d)

G

e)

H

74.
At the end of chemical reactions, what is the total mass of the reactants compared to the total mass of the products?
a)
the product is doubled
b)
the product is half the mass of the reactants
c)
the mass is the same
d)
the mass changes depending on the reaction
75.
In chemical reactions, what does the principle of conservation of mass mean?
a)
Matter is not created or destroyed.
b)
The total mass of the reactants is greater than the total mass of the products.
c)
The total mass of the reactants is less than the total mass of the products.
d)
Matter is not changed.
76.
The red numbers in the image below represent ________
a)
subscripts
b)
coefficients
c)
I don't know, and don't want to try
d)
None of the answers are correct
77.
The blue numbers in the image below represent ________
a)
I don't know, and don't want to try
b)
coefficients
c)
subscripts
d)
none of the answers are correct
78.
The substances at the beginning of a chemical equation are called the ____
a)
product
b)
yield
c)
chemical symbol
d)
reactants
79.

What is the right part of a chemical equation called...

H2 + O2 --> H2O

a)

Reactants

b)

Products

c)

Yields

d)

Chemical Equation

80.

What is the arrow in a chemical equation...

H2 + O2 --> H2O

a)

Reactants

b)

Products

c)

Yields

d)

Chemical Equation

81.
When balancing equations a ____ can be placed to the left of a formula of a substance to make the equations balanced
a)
charge
b)
subscript
c)
random number
d)
coefficient
82.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__Al + __O2--> __Al2O3
a)
4,1 --> 2
b)
4,3 --> 4
c)
3,4 --> 1
d)
4,3 --> 2
83.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__H2SO3 + __KOH--> __H2O+ __K2SO3
a)
2,1 --> 2,1
b)
1,2 --> 1,1
c)
1,2 --> 1,2
d)
1,2 --> 2,1
84.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__H2 + __S --> __H2S
a)
1,1 --> 1
b)
2,2 --> 2
c)
1,2 --> 1
d)
1,2 --> 2
85.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__AgNO3 + __H2S --> __Ag2S+ __HNO3
a)
2,1 --> 1,2
b)
1,2 --> 1,1
c)
1,2 --> 1,2
d)
1,2 --> 2,1
86.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__CH4 + __O2 --> __CO2+ __H2O
a)
2,1 --> 2,1
b)
1,2 --> 1,1
c)
1,2 --> 1,2
d)
1,2 --> 2,1

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