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T2. Chemistry test Part 2

Total questions: 79

Worksheet time: 1hrs 23mins

Name
Class
Date
1.
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
2.
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.
3.
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
4.
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
5.
The substances at the beginning of a chemical equation are called the ____
a)
product
b)
yield
c)
chemical symbol
d)
reactants
6.

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

H2 + O2 --> H2O

a)

Reactants

b)

Products

c)

Yields

d)

Chemical Equation

7.
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
8.
Number of C's in 2Na₂CO₃
a)
1
b)
2
c)
3
d)
5
9.
How many Elements are in the compound C2H8O ?
a)
2
b)
1
c)
3
d)
0
10.
How many total atoms are in the compound C2H8O ?
a)
11
b)
2
c)
8
d)
1
11.
How many Magnesium are in 10MgCl2?
a)
10
b)
5
c)
20
12.
Balance this equation:
 2Li + Cl2 -> LiCl
a)
2Li + Cl2 -> 4LiCl2
b)
2Li + Cl2 -> LiCl2
c)
2Li + Cl2 -> 2LiCl
13.
Which number should go in the blank?
_ H2 + O2 -> 2 H2O
a)
1
b)
2
c)
3
d)
0
14.
Is the following equation balanced or unbalanced ? 
Al + O2 --> Al2O3
a)
Balanced
b)
Unbalanced
15.

Balance the following equation by filling in the blank:

N2 + 6H2 → _NH3

(a)  

16.

Which type of chemical reaction has the following configuration?


Substance + Substance --> Compound


A + B --> AB

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

17.

Which type of chemical reaction has the following configuration?


Element + Compound --> Element + Compound


A + BC --> B + AC

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

18.

Which type of chemical reaction has the following configuration?


Hydrocarbon + Oxygen --> Carbon Dioxide + Water


CxHy + O2 --> CO2 + H2O

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

19.

What type of chemical reaction has the following configuration?


Ionic Compound(aq) + Ionic Compound(aq) --> Compound + Compound


AB(aq) + CD(aq) --> AD + BC

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

20.

What type of chemical reaction has the following configuration?


Compound --> Substance + Substance


AB --> A + B

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

21.

What type of chemical reaction is Endothermic and needs heat/energy to take place.

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

22.

Select each compound that can be produced by combustion reactions. (more than 1 answer)

a)

Oxygen

b)

Carbon Dioxide

c)

Water

d)

Glucose

e)

Carbon

23.

Classify the following chemical reaction


BaCl2(aq) + K2CrO4(aq) --> BaCrO4(s) + 2KCl(aq)




a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

24.

Classify the following chemical reaction.


Si(s) + 2Cl2(g) --> SiCl4(l)

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

25.

Classify the follow chemical reaction.


2C6H6(l) + 15O2 --> 6H2O(l) + 12CO2(g)

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

26.

What type of chemical reaction is when a single compound is broken down into two or more products?

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

27.

What is a substance that speeds up the rate of a chemical reaction?

a)

Rate

b)

Catalyst

c)

Calorimeter

d)

Hydrocarbon

28.

Identify the type of chemical reaction pictured above

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

29.

Identify the type of chemical reaction pictured above

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

30.

Identify the type of chemical reaction picture above

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

31.

Identify the type of chemical reaction picture above

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

32.

Identify the type of chemical reaction pictured above

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

33.

When does a chemical reaction stop?

a)

When the lab is finished

b)

When the excess reactant is used up

c)

When the limiting reactant is used up

d)

Chemical reactions never stop

34.
Which of the following shows the correct way to balance the chemical equation?
Fe + O2 -> Fe2O3
a)
4Fe + 3O2 -> 2Fe2O3
b)
2 Fe + 3O2 -> Fe2O6
c)
4 Fe + O6 -> 2Fe2O3
d)
None of the options are correctly balanced.
35.
Balance this equation...
HgO --> Hg + O2
a)
It is balanced 
b)
2HgO --> Hg + O2
c)
2HgO --> 2Hg + O2
d)
I don't know...Oh well!
36.
Ice melting
a)
Chemical Change
b)
Physical Change
37.
What happens in ALL chemical changes?
a)
Change in state of matter
b)
A new substance is formed
c)
Bubbles are produced
d)
An explosion
38.
Is the following equation balanced or unbalanced?
Fe + S --> FeS
a)
balanced
b)
unbalanced
39.
Water can dissolve many things so it is called the .....
a)
wonderful water
b)
cohesion
c)
liquid
d)
universal solvent
40.
a solute whose water solution conducts electricity is called a(n)
a)
nonconductor
b)
electrolyte
c)
nonelectrolyte
d)
aqueous solution
41.
The thing that does the dissolving
a)
Solute
b)
Solvent
c)
Colloid
d)
Solution
42.
What is a solute?
a)
The substance that does the dissolving in a solution.
b)
The substance that is dissolved into the solution.
c)
The mixing of different substances.
d)
The process in which neutral molecules lose or gain electrons
43.

According to the law of conservation of mass, how does the amount of each element on the product side compare to each element on the reactant side?

a)

The amount of atoms on each side is equal

b)

The amount of atoms on the product side is greater

c)

The amount of atoms on the reactant side is greater

d)

Depends on the reaction

44.
Which of the following describes a precipitate?
a)
a liquid forms when a block of metal is heated
b)
a solid forms when one liquid is poured into another
c)
a gas forms when a solid is placed in a liquid
d)
bubbles form when an acid is poured on a rock
45.

Balance the following chemical equation:

____KClO3 → ____KCl + ____O2

a)

2KClO3 → 4KCl + O2

b)

4KClO3 → 2KCl + 3O2

c)

2KClO3 → 2KCl + 3O2

46.

The mass of 6.02 x 10^23 atoms of an element is equal to

a)

its atomic number from the periodic table, but in amus.

b)

its atomic mass from the periodic table, but in amus.

c)

its atomic mass from the periodic table, but in grams.

d)

its atomic number from the periodic table, but in grams.

47.

If you're converting between grams and moles you need to use:

a)

1 mole = 6.022x1023 things

b)

the metric prefix chart

c)

molar mass

d)

the atomic number

48.

How many moles of magnesium in a 20g strip?

a)

0.81

b)

0.82

c)

0.83

d)

0.84

49.

How many formula units are in 2.5 moles of NaCl?

a)

1.5 x1024 formula units

b)

1.5 formula units

c)

4.2 formula units

d)

4.2 x10-24 molecules

50.
What is the molar mass of sodium?
a)
11
b)
22.990
c)
45.98
d)
3
51.
What are the units for molar mass?
a)
grams
b)
amu
c)
grams/mole
d)
liters
52.
The molar mass of an element is equal to its...
a)
Atomic mass
b)
Atomic number
c)
Oxidation number
d)
Valence electrons
53.
What is the mass of one mole of aluminum?
a)
27 g
b)
13 g
c)
54 g
d)
14 g
54.
How many particles are in a mole?
a)
602
b)
602 million
c)
602 moles
d)
6.02 x 1023
55.
Calculate the mass of  5 mol of iron atoms.
a)
5
b)
56
c)
130
d)
280
56.
What is the molar mass of NaBr
a)
381.9g/mol
b)
102.9 g/mol
c)
213.6g/mol
d)
93.0g/mol
57.
What is the molar mass of CO2?
a)
12
b)
16
c)
32
d)
44
58.
Which of the following is true about a mole of iron and a mole of zinc?
a)
they have the same mass
b)
the iron sample has more mass
c)
the zinc sample has more mass
59.

What is the molar mass of Ba(OH)2?

a)

153.49 g/mol

b)

171.33 g/mol

c)

56.24 g/mol

60.

Convert 50.0 grams of H2O to moles of H2O.

a)

901 moles

b)

18.02 moles

c)

2.77 moles

61.

What mass of calcium chlorate, Ca(ClO3)2, is equivalent to 0.750 moles of the substance?

a)

155.24 grams

b)

206.98 grams

c)

128.65 grams

62.

What is the molar mass of aluminum carbonate, Al2(CO3)3?

a)

54.99 g/mol

b)

233.99 g/mol

c)

185.99 g/mol

63.

3.0 moles of sodium hydroxide, NaOH, is equal to what mass?

a)

about 40 grams

b)

about 23 grams

c)

about 120 grams

64.

When converting a mass to moles, what unit must be in the denominator of the conversion factor?

a)

grams

b)

moles

c)

grams/mole

65.

When converting a moles to mass, what unit must be in the denominator of the conversion factor?

a)

grams

b)

moles

c)

grams/mole

66.
The Formula to make S'mores is:
2C + 1M + G2 → C2MG2. If you have 5 Marshmallows (M), 9 Chocolate Pieces (C), and 9 Graham Cracker Halves (G), how many S'mores can you make?
a)
5
b)
4
c)
8
d)
42
67.

What are ionic bonds?

a)

weak electrostatic forces of attraction between oppositely charged ions

b)

strong electrostatic forces of attraction between oppositely charged ions

c)

strong electrostatic forces of attraction between metal and non-metal atoms

d)

weak electrostatic forces of attraction between metal and non-metal atoms

68.

What exists between simple covalent molecules?

a)

weak intermolecular forces of attraction between molecules

b)

weak covalent bonds formed by sharing of electrons between atoms

c)

strong intermolecular forces of attraction between molecules

d)

strong covalent bonds formed by sharing of electrons between atoms

69.

Select all the physical properties true for ionic compounds.

a)

high melting and boiling points

b)

low melting and boiling points

c)

can dissolve in water

d)

cannot dissolve in water

e)

can dissolve in organic solvents

70.

Select all the physical properties true for covalent substances.

a)

high melting and boiling points

b)

low melting and boiling points

c)

can dissolve in water

d)

cannot dissolve in water

e)

can dissolve in organic solvents

71.

Select all the states in which ionic compounds can conduct electricity.

a)

solid

b)

liquid / molten

c)

aqueous / dissolved in water

d)

cannot conduct electricity in all states

72.

Select all the states in which covalent substances can conduct electricity.

a)

solid

b)

liquid / molten

c)

aqueous / dissolved in water

d)

cannot conduct electricity in all states

73.

What is NOT a property of ionic compounds?

a)

high melting and boiling points

b)

conduct electricity in all states

c)

soluble in water but insoluble in organic solvents

d)

conduct electricity when molten or in aqueous solutions

74.

Ionic compounds cannot conduct electricity in solid state because

a)

ionic bonds are strong.

b)

electrons are not free to move.

c)

ions are held in fixed positions.

d)

there are no charged particles.

75.

Ionic compounds can conduct electricity in molten and aqueous states because

a)

electrons are free to move.

b)

ions are free to move.

c)

atoms are free to move.

d)

protons are free to move.

76.

Which is a property of simple covalent molecules?

a)

soluble in water

b)

insoluble in organic solvents

c)

conduct electricity when molten

d)

low melting and boiling points

77.

Many covalent substances are volatile liquids or gases at room temperature because

a)

the intermolecular forces of attraction holding the molecules together are weak.

b)

the covalent bonds within the molecules are easily broken.

c)

the electrostatic attraction between ions is a weak force that can be overcome easily.

d)

they consists of simple molecules that do not dissolve in water but dissolve in organic solvents.

78.

Why most covalent substances do not conduct electricity in all states?

a)

no electrons

b)

no free-moving charged particles

c)

too strong covalent bonds

d)

no electron gain or loss between atoms

79.

Polystyrene dissolves in an organic solvent, propanone. What is the bonding in polystyrene?

a)

covalent

b)

ionic

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