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Chemistry Review Section 2

Total questions: 87

Worksheet time: 1hrs 29mins

Name
Class
Date
1.

How many atoms of sulfur are in each molecule of H2SO4?

a)

1

b)

4

c)

2

d)

7

2.

Alanine is an amino acid with formula C3H7NO2. How many atoms in all are in each molecule of alanine?

a)

3

b)

7

c)

12

d)

13

3.

Which of the following accurately describes the chemical formula of the molecule shown above?

a)

3CH8O

b)

C3H7O

c)

C4H8O2

d)

C3H8O

4.

A diagram to a molecule is shown above. Based on the diagram, what is the identity of this compound?

a)

Water (H2O)

b)

Hydronium (H3O+)

c)

Hydrogen peroxide (H2O2)

d)

Hydroxide (OH-)

5.

Which elements are in the formula shown above?

a)

Cobalt only

b)

Carbon and Oxygen

c)

Copper only

d)

Carbon and Osmium

6.

How many different elements are in an amino acid with the formula C5H11NO2S?

a)

5

b)

20

c)

18

d)

4

7.
When the number of electrons equals the number of protons the atom has what charge?
a)
sponge bob
b)
positive charge
c)
negative charge
d)
neutral charge
8.
If my charge becomes 2+ what does that say about me?
a)
I am stealing 2 electrons
b)
I am losing 2 electrons
c)
I am in period 2
d)
I have an atomic # of 2
9.

How does oxygen become an oxide ion?

a)

it loses 2 electrons

b)

it gains 2 electrons

10.

Is the following compound ionic or molecular?

A material with a high melting point

a)

Ionic

b)

molecular

11.
Which of the following is NOT an ionic compound:
a)

MgO

b)
NaOH
c)

BeCl2

d)

O2

12.
How are ionic bonds formed?
a)
Transfer of electrons
b)
Sharing of electrons
13.

Ionic bonds could be best described as:

a)

A bond formed when 2 atoms share electrons

b)

A firm handshake

c)

An electrostatic attraction between oppositely charged ions

d)

An electrostatic attraction between anions

14.

Is the following compound ionic or moelcular?

A material that SHARES electrons

a)

Ionic

b)

Molecular

15.

When dissolved in water, the solution is a good conductor of electricity.

a)

ionic compounds

b)

molecular compounds

16.

Why do ionic compounds conduct electricity when dissolved in water, but most covalent compounds do not?

a)

Covalent compounds have lower melting point than ionic compounds.

b)

Covalent compounds are weakly bonded while ionic compounds are strongly bonded.

c)

Covalent compounds do not dissolve in water since they are composed of non- polar molecules.

d)

Covalent compounds dissolve into molecules, while ionic compounds dissolve into ions that conduct charge.

17.

Why are sodium and chlorine ions attracted to each other?

a)

they have opposite charges

b)

they both have negative charges

c)

they both have positive charges

18.

Is the following compound ionic or molecular?

A material that contains a metal and a nonmetal

a)

Ionic

b)

molecular

19.

Which set of elements is most likely to form an ionic compound?

a)

Na and O

b)

C and O

c)

Na and K

20.

Classify ionic or molecular

C2H2

a)

Ionic

b)

Molecular

21.

Classify ionic or molecular

LiOH

a)

Ionic

b)

Molecular

22.
Which of these compounds is ionic? 
a)
Carbon dioxide
b)
Dinitrogen Trioxide
c)
Silicon tetrachloride
d)
Lithium bromide
23.

Classify ionic or molecular

BeO

a)

Ionic

b)

Molecular

24.
Which of the following is NOT an ionic compound:
a)

NaO

b)
NaOH
c)

BeCl2

d)
CH4
25.

Prefixes are used only for naming _______________ compounds

a)
Ionic
b)

covalent (molecular)

26.

What is the chemical formula of Magnesium chloride?

a)

MgCl

b)

MgCl2

c)

MgC

d)

MgC2

27.
What is the formula for aluminum fluoride?
a)
AlF
b)
Al2F3
c)
AlF3
d)
Al3F2
28.

What is the IUPAC name for NaF?

a)

sodium fluoride

b)

sodium fluorine

c)

monosodium monofluoride

d)

sodium monofluorine

29.
Name this compound.
MgF2
a)
magnesium fluoride
b)
manganese Phosphide
c)

magnesium(II) fluoride

d)

magnesium difluoride

30.

Name the following compound: AlF3

a)

aluminum fluoride

b)

monoaluminum trifluoride

c)

aluminum trifluoride

d)

aluminum fluorine

31.

What is the correct formula of phosphorus trichloride?

a)

P2Cl3

b)

P3Cl3

c)

PCl3

d)

PCl5

32.

When sodium and nitrogen combine, this is the formula...

a)

NaN

b)

NA3N

c)

Na3N

d)

S3N

33.

Name the following compound:


Li2S

a)

dilithium sulfide

b)

lithium (II) sulfide

c)

lithium sulfide

d)

lithium sulfate

34.
Which of the following is the correct name for MgCl2....
a)
Magnesium Clorine
b)
Magnesium Dicholorine
c)

Magnesium Chloride

d)
Magnesium Dichloride
35.

Name the following: N2O

a)

nitrogen monoxide

b)

dinitrogen monoxide

c)

nitrogen (II) oxide

d)

nitrogen oxide

36.

Write the formula: beryllium oxide

a)

BO

b)

BeO

c)

BeO2

d)

BO2

37.

what is the correct name of the combination between fluorine and magnesium?

a)

fluorine magnesium

b)

fluoride magnesium

c)

magnesium fluoride

d)

magnesium fluorine

38.

Name for CO

a)

carbon monoxide

b)

carbon oxide

c)

monocarbon oxide

d)

carbide monoxide

39.
The name of SO₃ compound is
a)
sulfate
b)
sulfur oxide
c)
sulfur trioxide
d)
monosulfur trioxide
40.
Which of the following is an example of a chemical reaction?
a)
A marshmallow turning black when heated over a fire
b)
A powder dissolving in water to make lemonade
c)
An ice cube melting into a puddle of water
d)
Salt crystals being crushed into a powder
41.

What are the products of the chemical reaction pictured?

a)

CH4 and CO2

b)

CH4 and O2

c)

CO2 and 2 H2O

d)

O2 and H2O

42.
Consider the chemical equation CH4 + 2 O2 → CO2 + 2 H2O. In this equation, CH4 is a
a)
product
b)
reactant
c)
displacement
43.

What are the REACTANTS :

H2O + CO2 → HCO + HO

a)

H2O + CO2

b)

HCO + HO

c)

H2O ONLY

d)

HCO ONLY

44.
If a chemical reaction is EXOTHERMIC, the temperature would....
a)
Stay the same
b)
Increase
c)
Decrease
45.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
46.
Have you ever eaten sherbet sweets candy? They fizz in your mouth and your tongue feels cold. Why do you think that is?
a)
It is an exothermic reaction
b)
It is an endothermic reaction
c)
It is made of ice
d)
It is dissolving your mouth
47.
Baking bread and cooking an egg are examples of....?
a)
Endothermic processes
b)
Exothermic processess
c)
None of these 
48.

O2(g) + 2 H2 (g) → 2 H2O (g) + EnergyO_2\left(g\right)\ +\ 2\ H_2\ \left(g\right)\ \rightarrow\ 2\ H_2O\ \left(g\right)\ +\ Energy  

a)

endothermic

b)

exothermic

49.
In an endothermic reaction, heat is ...
a)
taken in or absorbed
b)
given out or released 
50.

What type of reaction occurs in a hand warmer?

a)

exothermic

b)

endothermic

51.

When calcium reacts with water, the temperature changes from 18°C to 39°C. Which statement is correct?

a)

The solution at the end is acidic

b)

The reaction is reversible

c)

The reaction is exothermic

d)

The reaction is endothermic

52.

What are the products of combustion?

a)

Hydrogen + oxygen

b)

Carbon dioxide + water

c)

Carbon dioxide + hydrogen

d)

Carbon + water

53.

Which diagram shows the most favourable conditions for rust to appear on the nail?

a)

A

b)

B

c)

C

d)

D

54.

Is this an example of corrosion or combustion?

a)

corrosion

b)

combustion

55.
What are the reactants of cellular respiration?
a)
glucose & carbon dioxide
b)
glucose & oxygen
c)
water & oxygen
d)
water & carbon dioxide
56.

In a chemical reaction, the number of atoms in the products will always equal which amount?

a)

the number of atoms in the reactants

b)

half of the number of atoms in the reactants

c)

twice the number of the atoms in the reactants

d)

thrice the number of the atoms in the reactants

57.
If four hydrogen atoms react with two hydrogen atoms, how many atoms will be in the product?
a)
6
b)
4
c)
8
d)
2
58.

According to the Law of Conservation of Matter, what happens to the wood and oxygen when it is burned?

a)

The wood disappears.

b)

It stays the same chemically.

c)

The atoms in the wood and oxygen rearrange and form smoke and ash.

d)

Nothing.

59.

Why does this picture demonstrate the Law of Conservation of Matter?

a)

the number of atoms of each element are the same on both sides

b)

they start out separate and end up combined

c)

the same elements are used

d)

it doesn't demonstrate the Law of Conservation of Mass

60.
When heated, oxygen reacts with copper to form copper oxide:
If this reaction occurs in a sealed container, will the mass of the container and everything in it increase, decrease, or stay the same and why?
a)
The mass will stay the same because the number of each kind of atom stays the same.
b)
The mass will increase because a new kind of molecule is formed.
c)
The mass will decrease because two substances combine to form one substance.
d)
More information is needed to tell if the mass will change.
61.

Jin bought a heat pack that weighs 15 g. He shook it so it would release heat to warm his hands. The release of heat indicates a chemical reaction took place in a closed system. What would be the mass of the heat pack after the chemical reaction?

a)

5 g

b)

10 g

c)

12 g

d)

15 g

62.
If reaction starts with 20g of reactants it should produce 
a)
a total of 40g of products
b)
a total of 10g of products
c)
a total of 80 g of products
d)
a total of 20g of products
63.
In a reaction A + B ----> C,  reactant A has 5g and product  C has 9g. How many grams does reactant B should have? 
a)
4g
b)
5g
c)
9g
d)
14g
64.
In the reaction AB-----> A + B reactant AB has 12g and product B has 5g. How many grams should product A have?
a)
17g
b)
2g
c)
7g
d)
None of the above
65.

In this reaction, how much O2 is produced?

a)

12 g

b)

22 g

c)

42 g

d)

No grams are produced

66.
12g of Carbon react with 16g of Oxygen, how much carbon monoxide (CO) is formed? 
a)
28 g
b)
4g
c)
30g
d)
12g
67.
A chemical reaction between Hydrogen and Oxygen produces water. If 2g of Hydrogen and 4g of Oxygen react together, how much water is produced?
a)
2g
b)
4g
c)
6g
d)
Not enough information to answer
68.

In a chemical reaction, 4 grams of sodium must combine with how many grams of chlorine to produce 10 grams of table salt?

a)

4 grams

b)

6 grams

c)

8 grams

d)

10 grams

69.
Suppose a reaction were to happen in an open container in a lab.  During the reaction, the scientist observes the chemicals bubble, and produce a gas.   During the analysis the scientist notices that the reactants weighed 20 g when he started, and the product weighed 18 g.  Explain what happened.  
a)
His chemical reaction defied the law of conservation of mass
b)
The product destroyed mass during the reaction
c)
The reactants created matter during the reaction
d)
The gas that was produced was not able to be weighed since the container was open.  
70.

What criteria must be met for reactant collisions to result in a successful product?

a)

The reactants must collide with each other

b)

The reactants must collide with enough energy and be in the right positions

c)

The reactants must have enough energy to form the activated complex

71.
More collisions correspond to a: 
a)
Faster reaction rate  
b)
Slower reaction rate
c)
Constant reaction rate 
d)
None of the above
72.

Which factors increase the rate of a reaction?

a)

increasing temperature

b)

increasing concentration

c)

increasing total surface area

d)

All of these

73.

Which among the following is NOT TRUE about the collision theory and the rate of reaction?

a)

higher temperature ---> faster particle movements ---> more collision

b)

higher concentration ---> more spaces between particles ---> more collision

c)

higher surface area ---> more particle interactions ---> more collision

74.
Products will form faster if____________
a)
the particle size of the reactants are larger.
b)
temperature is decreased.
c)
concentration of the reactants are increased.
d)
the reaction is not stirred.
75.
A ______________ is a substance that increases the rate of a reaction without being used up during the reaction. 
a)
catalyst
b)
product
c)
reactant
d)
solute
76.
Smaller particle size allows for a _________ surface area to be exposed for the reaction.
a)
larger
b)
smaller
77.
Increasing the temperature will increase the kinetic energy of particles, therefore increasing the collisions between particles.
a)
false
b)
true
78.

Why does a higher concentration increase the rate of reaction?

a)

it increases the amount of reactants

b)

it lowers the activation energy

c)

it increases the energy of particle collisions

d)

it increases the frequency of particle collisions

79.

Diagram shows the apparatus set up for an experiment to determine the rate of reaction.

Which of the following techniques is the most suitable to determine the rate of reaction?

a)

Record the time as soon as precipitate is formed

b)

Record the time taken to obtain the maximum temperature

c)

Record the times as soon as the cross mark cannot be seen

d)

Record the times taken for the change of the pH value until a fixed pH value is obtained

80.

How could we make this reaction happen more quickly?

a)

Decrease the concentration of the acid

b)

crush the chalk to increase the surface area

c)

Put the test tube in an ice bath

81.
In which experiment is the rate of reaction between hydrochloric acid and calcium carbonate slowest? 
a)
A
b)
B
c)
C
d)
D
82.

Which graph shows the effect of increasing temperature on the rate of reaction of calcium carbonate with dilute hydrochloric acid?

a)

b)

c)

83.

Table 9 shows the experiments carried out to study the rate of reaction between zinc carbonate and nitric acid.


Which of the following graph represents the two experiments?

a)
b)
c)
d)
84.

Which of the following will lower the rate

of reaction?

a)

adding an enzyme to the reaction

b)

decreasing the temperature from 40°C to

10°C

c)

breaking a chunk of calcium up into

smaller pieces

d)

increasing the amount of solute

dissolved in a solution

85.

Approximately how long did it take for the cross to disappear at 20 Degrees Celsius.

a)

67

b)

54

c)

68

d)

58

86.

To slow down a chemical reaction you will do one of the following:

a)

Place the reactants in hot water

b)

Place the products in ice bath

c)

Place the reactants in an ice bath

d)

Keep stirring the reactants with a stirring rod

87.

What was the manipulated variable in this experiment?

a)

temperature

b)

reaction time

c)

reaction rate

d)

effect of temperature on rate of reaction

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