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Chemistry Reviewer for 3rd Quarter

Total questions: 74

Worksheet time: 3hrs 31mins

Name
Class
Date
1.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Linear
2.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
3.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
4.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
5.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
6.

What molecule could this be? (Each purple cloud represents a lone pair of electrons.)

a)

CO2

b)

NH3

c)

H2S

d)

CH4

7.

What is the molecular geometry of CO2?

a)

Bent

b)

Trigonal planar

c)

Trigonal pyramidal

d)

Linear

8.

What determines the polarity of molecules?

a)

Size of the molecule

b)

Geometrical shape of the molecules

c)

Number of atoms in the molecule

d)

Color of the molecule

9.

What is represented by an electric dipole in a molecule?

a)

One positive end and one negative end

b)

Two positive ends

c)

Two negative ends

d)

No charge

10.

Which atom becomes the partial negative pole in a polar covalent bond?

a)

The atom with higher electronegativity value

b)

The atom with lower electronegativity value

c)

The smallest atom

d)

The largest atom

11.

What is the connection between electronegativity and the polarity of bonds?

a)

Electronegativity repels electrons

b)

Electronegativity has no effect on bond polarity

c)

Lower electronegativity attracts electrons more strongly

d)

Higher electronegativity attracts electrons more strongly

12.

It is the ability of an atom in a particular molecule to attract electrons to itself

(a)  

13.

It is a bond formed when there is an equal sharing of electrons between molecules.

a)

Polar bond

b)

Nonpolar bond

c)

Ionic bond

d)

None of the above

14.

A polar compound has

a)

Two positive ends

b)

Two negative ends

c)

One positive and one negative end

d)

No charges between the ends

15.

HBr is an example of a/an _____

a)

Ionic compound

b)

Polar compound

c)

Nonpolar compound

d)

None of the above

16.

Diatomic molecules are considered as

a)

Polar

b)

Nonpolar

c)

Ionic

d)

Metallic

17.

The bigger the electronegativity, the more nonpolar the bond is

a)

TRUE

b)

FALSE

18.

To classify compounds using their electronegativity values, we get the electronegativity ________ between molecules.

a)

Difference

b)

Sum

c)

Quotient

d)

Product

19.

Water

a)

Polar

b)

Nonpolar

20.

δ+ means that an element is partially (a)  

21.

δ− means that the atom is ___

a)

Less electronegative

b)

More electronegative

22.

Ca (1.0) and Br (2.8)

a)

⬅️

b)

➡️

c)

↕️

d)

↗️

23.

What is the electronegativity difference between O2

a)

0

b)

1

c)

2

d)

3

24.

These compounds are soluble in water

a)

Polar

b)

Nonpolar

25.

What must the difference in electronegativity between two atoms be in order for the bond between them to be nonpolar covalent?

a)

less than 0.4

b)

greater than 1.7

c)

between 0.4 and 1.7

d)

exactly 0

26.

The electrons in a polar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

27.

The law of conservation of mass states that matter ___________________.

a)

cannot enter into chemical reactions

b)

cannot be created or destroyed

c)

cannot form different substances

d)

cannot be modeled

28.

Chemical formulas are used to represent _________________.

a)

reactions

b)

substances

c)

processes

d)

none of the above

29.

Chemical equations are used to represent _________________.

a)

reactions

b)

substances

c)

processes

d)

none of the above

30.

The small numbers under and to the right of element symbols in a formula are called _________________.

a)

element symbols

b)

exponents

c)

coefficients

d)

subscripts

31.

The large numbers before a chemical formula that are used as multipliers are known as __________________.

a)

element symbols

b)

exponents

c)

coefficients

d)

subscripts

32.

The materials we start with in a reaction are known as __________________.

a)

chemicals

b)

reactants

c)

products

d)

creations

33.

The materials we end with in a reaction are known as __________________.

a)

chemicals

b)

reactants

c)

products

d)

creations

34.

Reactants are found on the _______________ side of the arrow in a chemical equation.

a)

Right

b)

Left

35.

Products are found on the _______________ side of the arrow in a chemical equation.

a)

Right

b)

Left

36.

What is the correct "inventory" for KClO3

a)

K = 1 Cl = 3 O = 3

b)

K = 3 Cl = 3 O = 3

c)

K = 1 Cl = 1 O = 3

d)

K = 1 C = 1 l = 1 O = 3

37.

What is the coefficient in the formula?

a)

2

b)

N

c)

H

d)

3

38.

What does the arrow in a chemical equation represent?

a)

created

b)

makes

c)

yields

d)

destroys

39.

What is the correct "inventory" for 3Al2O4

a)

Al = 6 O = 4

b)

Al = 6 O = 12

c)

Al = 2 O = 4

d)

Al = 3 O = 4

40.

What is the correct "inventory" for 4Ag(NO3)2

a)

Ag = 4 N = 2 O = 6

b)

Ag = 4 N = 4 O = 6

c)

Ag = 4 N = 8 O = 24

d)

Ag = 1 N = 2 O = 6

41.

Which of the following symbols is NOT a correct indication of the phase of a substance in a reaction?

a)

(s)=solid

b)

(g)=grams

c)

(l)=liquid

d)

(aq)= aqueous

42.

Which is the correct chemical equation for the following: Solid Zn reacts with silver (I) chloride to produce Zinc (II) chloride and silver metal

a)

Zn + AgCl → ZnCl2 + Ag

b)

ZnCl2 + Ag → Zn + AgCl

c)

ZnCl2 + Ag2 → Zn + AgCl

d)

Zn2Cl + Ag → Zn + AgCl

43.

Which of the following is a diatomic molecule?

a)

fluorine

b)

silver

c)

boron

d)

helium

44.

How many carbon atoms are present on the reactant side? C2 + O2 ⇢ CO2

a)

0

b)

1

c)

2

d)

3

45.
What is the part of the chemical equation in green called? 
Fe + S --> FeS
a)
products
b)
reactants
c)
yield
d)
chemical formula
46.

 

Which of the following equations are correctly balanced?

a)

12CO2 + H2O ---> C6H12O6 + O2

b)

CO2 + 9H2O ---> C6H12O6 + O2

c)

CO2 + H2O ---> 3C6H12O6 + O2

d)

6CO2 + 6H2O ---> C6H12O6 + 6O2

47.

Balance this equation:

H2 + Cl2 ---> HCl

a)

It is balanced.

b)

3H2 + Cl2 ---> 6HCl

c)

H2 + Cl2 ---> 2HCl

d)

H2 + 3Cl2 ---> 6HCl

48.

 

What is the right ratio of chemicals for the 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

49.

What is the right ratio of chemicals for the 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

50.

What is the right ratio of chemicals for the balanced chemical equation?

__Na + __H2O --> __NaOH + __H2

a)

4,4 --> 4,1

b)

1,2 --> 2,4

c)

1,2 --> 2,1

d)

2,2 --> 2,1

51.

What is the right ratio of chemicals for the balanced chemical equation?

__Ca + __H2O --> __Ca(OH)2 + __H2

a)

2,1 --> 2,1

b)

1,2 --> 1,1

c)

1,2 --> 2,4

d)

1,2 --> 2,1

52.

 

What is the right ratio of chemicals for the balanced chemical equation?

__CO + __Fe2O3--> __Fe + __CO2

a)

3,2 --> 1,1

b)

3,2 --> 2,4

c)

3,1 --> 2,3

d)

3,2 --> 2,1

53.

What is the right ratio of chemicals for the balanced chemical equation?

__MnO2 + __HCl --> __MnCl2 + __H2O __Cl2

a)

4,1 --> 2,1,2

b)

1,2 --> 1,1,4

c)

1,4 --> 1,2,1

d)

1,4 --> 2,2,1

54.
What is the oxidation number of Fe in FeO?
a)
+1
b)
-1
c)
+2
d)
-2
55.
What is the oxidation number of O in CO2?
a)
+2
b)
-1
c)
+4
d)
-2
56.
What is the oxidation number of N in NO21- ?
a)
-3
b)
+4
c)
-2
d)
+3
57.
A chemical reaction that involves a gain/loss of electrons is called:
a)
Double Replacement
b)
Neutralization
c)
Oxidation-Reduction
d)
Hydrolysis
58.
If in a reaction, copper is reduced; its number of electrons has:
a)
Increased
b)
Decreased
c)
Remained Constant
d)
Varies Randomly
59.
If an atom loses electrons during a chemical reaction, the atom was:
a)
Oxidized
b)
Reduced
c)
Neutralized
d)
Precipitated
60.
The sum of all oxidation numbers in a neutral compound is ___.
a)
0
b)
1
c)
-1
d)
depends on the compound
61.
Which of the following compounds is NOT an ionic compound?
a)
NaCl
b)
NH3
c)
Fe2O3
d)
HCl
62.
What is oxidation number of Mn in MnO2 ?
a)
0
b)
+2
c)
-2
d)
+4
63.
What is the oxidation number of S in SO4 2-  ?
a)
-2
b)
+2
c)
+6
d)
-4
64.

For the equation below, which of the following is the oxidizing agent?

H2 + O2 --> H2O

a)

H2

b)

O2

c)

H2O

d)

O

65.

How many electrons are gained per Cu from the reaction below?

Al  +  Cu+2  -->  Al+3  +  Cu

a)

1

b)

2

c)

3

d)

4

66.

What is the numerical coefficient of H2O in a balanced chemical equation below?

Cr2O3 + H2 --> Cr + H2O

a)

1

b)

2

c)

3

d)

4

67.

What is the oxidation number of chlorine in HClO?

a)

0

b)

-1

c)

+1

d)

+5

68.

Oxidation is the _________ of electrons.

a)

loss

b)

gain

c)

sharing

d)

transfer

69.

Reduction is the ___________ of electrons.

a)

loss

b)

gain

c)

sharing

d)

transfer

70.
Which of the following represents reduction?
a)
C →  CO
b)
N2 →  NH3
c)
Zn  →   Zn2+ 
d)
H2 →  H2O
71.

Which of the following represents oxidation?

a)

C → CH4

b)

Fe3+ → Fe2+

c)

Cl2 → 2Cl-

d)

Zn → ZnO

72.

In the reaction Zn + 2HCl --> ZnCl2 + H2

which element, if any, is oxidized?

a)

Zinc

b)

Hydrogen

c)

Chlorine

d)

None

73.
Which statement is true:
Mg → Mg2+ + 2e–
a)
Mg gains 2 electrons
b)
Mg2+ loses 2 electrons
c)
Mg loses 1 electron
d)
Mg loses 2 electrons
74.
If in a reaction, copper is reduced; its number of electrons has:
a)
Increased
b)
Decreased
c)
Remained Constant
d)
Varies Randomly

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