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HCS Chemistry sem 2 Final Exam Review

Total questions: 184

Worksheet time: 3hrs 59mins

Name
Class
Date
1.

What is the first thing you must do to solve a stoichiometry problem?

a)

Write a Balanced Equation

b)

Panic

c)

Write an Unbalanced Equation

d)

Ask for help

e)

Look for the same reaction in my notes

2.

What is a Limiting Reagent?

a)

speeds up a reaction

b)

what you run out of first

c)

what you have left over

d)

slows down a reaction

3.

What is a Excess Reagent?

a)

amount you end with

b)

what you run out of first

c)

what you have left over

d)

what you start with

4.

You are driving your car down the road and you have a full tank of gas. You know that your car mixes gasoline with oxygen from the air and ignites it in the engine in a Combustion Reaction. What is the limiting reagent?

a)

Gasoline

b)

Oxygen

c)

Water

d)

Air.

5.

If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the

a)

theoretical yield

b)

mole ratio

c)

actual yield

d)

percentage yield

6.

Fe (s) + S (l) --> FeS (s)  

In a similar experiment, 5.00 g of Fe are allowed to react with 6.00 g of S.
What is the mass of FeS formed?
(Hint: Consider the limiting reactant.)

a)

10.0 g

b)

8.0 g

c)

9.5 g

d)

11.0 g

7.

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

8.

Mole ratios are obtained from the

a)

balanced chemical equation

b)

periodic table

c)

molar mass

9.

Honors:You react iron with excess oxygen. You collect 350 grams of iron (III) oxide, but your calculations show that you should have collected 375g. What is your % yield?

a)

93.33% yield of iron (III) oxide

b)

375 gram of iron (III) oxide

c)

105% yield of iron (III) oxide

d)

6.67 % yield of Iron (III) oxide

10.

2 H2 + O2 → 2 H2O
What is the mass of water formed when 8 grams of hydrogen gas completely reacts with oxygen gas?

a)

72 grams

b)

144 grams

c)

36 grams

d)

18 grams

11.

What is the percent by mass of oxygen in MgO?

a)

20%

b)

40%

c)

50%

d)

60%

12.

How many molecules are in 7.22 moles of NaCl?

Avg number is 6.022x1023)

a)

4.35 molec NaCl

b)

4.35x1024 molec NaCl

c)

1.15 molec NaCl

d)

1.15x1023 molec NaCl

13.

How many moles of magnesium are in 6.02x1022 atoms of magnesium?

(Avg number is 6.022 x 1023)

a)

1.00x1044 moles Mg

b)

0.100 moles Mg

c)

3.02x1046 moles Mg

d)

10 moles Mg

14.

A student conducted an experiment and observed that the percent yield was only 60%. What could be some reasons for the percent yield being less than expected? Select all that apply.

a)

Some of the product might have evaporated during heating.

b)

Some of the product might have been lost during transfer.

c)

Some of the product might have reacted with impurities.

d)

Some of the product might have been converted into light.

15.

3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe

Identify the mole ratios for the following pairs:

​ ​ ​ (a)   Mg : ​ (b)   Fe

​ (c)   Fe2O3 : ​ (d)   Fe

​ 1 Fe2O3 : ​ (e)   MgO

Choose from the below words

3

2

1

16.

When reacting Na with Cl2, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

a)

90.4%

b)

104%

c)

96.15%

d)

1.04%

17.

It refers to the substance(s) that are considered to be "ingredients" of a chemical reaction.

a)

reactants

b)

products

c)

catalysts

d)

enhancers

18.

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

19.

Identify the limiting reagent when 6.00 g HCl combines with 5.00 g Mg to form MgCl2.
 
Mg +  2HCl --> MgCl2  +  H2   
 

a)

Mg

b)

H2

c)

MgCl2

d)

HCl

20.

The amount of moles in CuBr that are in 276.9 g of the compound is (a)   .

21.

Balance this equation:

​ (a)   Fe + ​ (b)   O2 --> ​ (c)   Fe2O3

Choose from the below words

4

3

2

1

0

22.

What is the first thing you must do to solve a stoichiometry problem?

a)

Write a Balanced Equation

b)

Panic

c)

Write an Unbalanced Equation

d)

Ask for help

23.

What is a Limiting Reagent?

a)

speeds up a reaction

b)

what you run out of first

c)

what you have left over

d)

slows down a reaction

24.

What is a Excess Reagent?

a)

amount you end with

b)

what you run out of first

c)

what you have left over

d)

what you start with

25.

For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of Mg to moles Fe?

a)

3mol Mg / 2 mol Fe

b)

2 mol Mg/ 3 mol Fe

c)

1 mol Fe/ 2 mol Fe

d)

3 mol MgO / 2 mol Fe

26.

Use the equation 2 Al + 3 Cl2 ---> 2 AlCl3. If 2 moles of aluminum and 2 moles of chlorine are reacted, identify the limiting reactant.

a)

AlCl3

b)

Cl2

c)

Al

d)

Gary Busey

27.

If you predicted that 1.5 moles of Magnessium are used in a reaction, and you have 2.0 moles of Magnessium, what type of reactant is Magnessium?

a)

Limiting Reactant

b)

Excess Reactant

c)

Fast Reacter

d)

Non-Reactant

28.

If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the

a)

theoretical yield

b)

mole ratio

c)

actual yield

d)

percentage yield

29.

2 KClO3 → 2 KCl + 3 O2
How many moles of oxygen are produced when 6.7 moles of KClO3 decompose completely?

a)

6.7 mol

b)

1.0 mol

c)

10.1 mol

d)

4.5 mol

30.

2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are reacted with excess water?

a)

5.2 g

b)

2.6 g

c)

690 g

d)

45 g

31.

2 CO (g) + O2(g) → 2 CO2 (g)
In the formation of CO2 from CO and oxygen, how many Liters of CO2 are produced by the reaction of 8 mols of O2 with an excess of carbon monoxide?

a)

0.178 L

b)

358.4 Liters

c)

704 grams

d)

0.36 grams

32.

Cl2 + 2 KBr → Br2 + 2 KCl
How many grams of potassium chloride can be produced from 356 g of chlorine and 356 g of potassium bromide?

a)

749 g

b)

223 g

c)

479 g

d)

814 g

33.

CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?

a)

13.7 mol

b)

2.75 mol

c)

6.11 mol

d)

6.85 mol

34.

Fe (s) + S (l) --> FeS (s)  

In the experiment above, 7.62 g of Fe are allowed to react with 8.67 g of S.
How much FeS is formed?

a)

14.8 g

b)

12.2 g

c)

13.7 g

d)

19.9 g

35.

Identify the limiting reagent when 6.00 g HCl combines with 5.00 g Mg to form MgCl2.
 
Mg +  2HCl --> MgCl2  +  H2   
 

a)

Mg

b)

H2

c)

MgCl2

d)

HCl

36.

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

37.

Mole ratios are obtained from the

a)

balanced chemical equation

b)

periodic table

c)

molar mass

38.

How many moles of water could form from 5.00 moles of hydrogen?

a)

5.00 moles

b)

10.00 moles

c)

2.50 moles

d)

No Reaction

39.

How many grams of potassium nitrate would you need to react with 0.901 moles of sulfuric acid?

a)

182 grams of potassium nitrate

b)

901 grams of potassium nitrate

c)

91 grams of potassium nitrate

d)

364 grams of potassium nitrate

40.

How many liters of carbon dioxide at STP are formed from 8.00 liters of oxygen at STP reacting with methane (CH4)?

a)

4.00 liters of carbon dioxide

b)

22.4 liters of carbon dioxide

c)

0.357 liters of carbon dioxide

d)

0.179 liters of carbon dioxide

41.

How many molecules of benzene (C6H6) are combusted if there are 134.4 liters of carbon dioxide produced at STP?

a)

6.02 x 1023 molecules of benzene

b)

1 mole of benzene

c)

78.1 grams of benzene

d)

22.4 liters of benzene

42.

You react 5.00 moles of iron with excess oxygen and collect 385 grams of iron (III) oxide. What is your % yield?

a)

96.5% yield of iron (III) oxide

b)

399 gram of iron (III) oxide

c)

104% yield of iron (III) oxide

d)

82.4% yield of iron (III) oxide

43.

2 H2 + O2 → 2 H2O
How many grams of water are produced from the complete reaction of 4 grams of hydrogen gas?

a)

36 grams

b)

72 grams

c)

18 grams

d)

9 grams

44.

For the reaction: N2 + 3 H2 → 2 NH3, if 5 moles of nitrogen react with 15 moles of hydrogen, what is the limiting reactant?

a)

None

b)

H2

c)

N2

d)

NH3

45.

How many moles of oxygen are required to completely react with 8 moles of propane (C3H8) in the combustion reaction: C3H8 + 5 O2 → 3 CO2 + 4 H2O?

a)

8 moles

b)

40 moles

c)

16 moles

d)

32 moles

46.

the H in pH stands for

a)

helium

b)

henry

c)

hydrogen

d)

hydroxide

47.

An acid has a pH

a)

higher than 7

b)

lower than 7

c)

7

d)

greater than 14

48.

a base has a pH of

a)

lower than 7

b)

higher than 7

c)

7

d)

it only has a pOH

49.

Human blood has a pH between 7.35 and 7.45. Which of the following best describes human blood?

a)

strongly acidic

b)

slightly acidic

c)

strongly basic

d)

slightly basic

50.

What kind of acid does not completely dissociate?

a)

weak

b)

strong

c)

ionic

d)

pH

51.

In a test of pH levels, a baking soda has a pH of 9 and bleach has a pH of 12. What is true about there relationship?

a)

Both of the solution are Bases

b)

Both of the solution are Acids

c)

The Baking soda is an acid and the Bleach is a base

d)

The baking soda is a base and the Bleach is an Acid.

52.

What color is a neutral pH

a)

Green

b)

Red

c)

Orange

d)

Purple

53.

Many cleaning solutions are bases. Which of the following is a property of most bases?

a)

feels slippery

b)

tastes sour

54.

On the pH scale what numbers are bases?

a)

8-14

b)

0-7

c)

7

d)

1

55.

If the pH of a solution is 5.6 the pOH is

a)

6.5

b)

12.4

c)

8.4

d)

5.6

56.

A  pH and a pOH will add up to:

a)

0

b)

7

c)

14

d)

1.0 x 10-14

57.

What is the pH of a solution with a [H+] concentration of 2.5x10-9?

a)

8.6

b)

5.4

c)

9.6

d)

4.4

58.

Which food is the most acidic?

a)

bananas

b)

lemon juice

c)

orange juice

59.

If a solution has a pOH of 3.7, the [OH-] of the solution is

a)

5.0 x 10-11

b)

2.0 x 10-4

c)

10.3

d)

14

60.

Oranges have a [H3O+] of 1.7 x 10-2 M. Their pOH is

a)

1.77

b)

12.23

c)

10.91

d)

3.09

61.

If an acid has a pH of 1.4 will it be strong or weak?

a)

strong

b)

weak

62.

Which is the strongest base?

a)

human blood (8)

b)

broccoli (10)

c)

bleach (12)

d)

sodium hydroxide (14)

63.

What is the pH of a neutral solution at 25°C?

a)

0

b)

7

c)

14

d)

1

64.

Which of the following is a characteristic of a strong acid?

a)

Partially dissociates in water

b)

Feels slippery

c)

Has a high pH

d)

Completely dissociates in water

65.

What is the pH of a solution with a hydrogen ion concentration of 1 x 10-3 M?

a)

3

b)

11

c)

1

d)

7

66.
Question Image

Match the following substances with their acidity level according to the pH range

a)

Hydrochloric acid

1.

Substance with pH less than lemon juice

b)

cabbage

2.

Substance with pH similar to neutral

c)

milk

3.

Substance with pH slightly acidic

67.

When the hydrogen ion concentration goes up, the pH (a)   .

Choose from the below words

gets lower

stays the same

gets higher

goes toward 7

68.

Orange is _______.

a)

acidic (pH < 7)

b)

Basic (pH > 7)

c)

neutral (pH = 0)

d)

Depends on how it is tested.

69.

Many medicines are bitter tasting so are most likely ______

a)

Basic (pH>7)

b)

Acidic (pH<7)

c)

Neutral

d)

Depends on the testing device

70.

Kids often like to simulate a volcano with baking soda and vinegar. Based on our testing in class, what is probably happening?

a)
Heat is generated from the mixture.
b)
The vinegar dissolves the baking soda completely.
c)
A physical change occurs with no gas produced.
d)

The acid and base are reacting, releasing gas.

71.

What is the molarity of 3 mole of hydrochloric acid in 3 L of water. 

a)

3

b)

1

c)

6

d)

9

72.

The ___ is the thing being dissolved

a)

solute

b)

solvent

73.

What is the formula for molarity?

a)

moles/grams

b)

moles/kilograms

c)

moles/milliliters

d)

moles/liters

74.

Calculate the molarity of the following solution:  1.0 mole of KCl in 750.0 mL of solution.

a)

0.750 M

b)

99 M

c)

1.3 M

d)

2.0 M

75.

How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?

a)

1074 mol

b)

0.069 mol

c)

1.07 mol

d)

62.7 mol

76.

How many grams of solute are dissolved in 125.0 mL of 5.00 M NaCl (MM = 58.45)?

a)

0.625 g NaCl

b)

625 g NaCl

c)

36.5 g NaCl

d)

0.04 mol NaCl

77.

How many liters would you need to make a 1 M solution if you have 6 mol of Sodium Hydroxide? 

a)

2

b)

3

c)

4

d)

6 

78.

What is the molarity of a solution made by adding 1.565 moles of PbNO3 to 500 mL?

a)

300. M

b)

31.3 M

c)

3.13 M

d)

1.56 M

79.

When a solvent contains as much of the solute as it can hold, the solution is said to be

a)

supersaturated

b)

diluted

c)

saturated

d)

unsaturated

80.

Solution where more solute can still be dissolved at the given temperature. 

a)

Saturated

b)

Unsaturated

c)

Supersaturated

d)

Homogeneous solution

81.

When 20 grams of potassium chlorate, KClO3, is dissolved in 100 grams of water at 80 ºC, the solution can be correctly described as:

a)

supersaturated

b)

saturated

c)

unsaturated

82.

Which solute is the most soluble at 10 ⁰C?

a)

KI

b)

KClO3

c)

NH4Cl

d)

NH3

83.

How many grams of NaCl are needed to 100 grams of water at 500C? Hover over the graph to see it better.

a)

25

b)

15

c)

38

d)

50

84.

The solute is given in grams. How do you get moles?

a)

Divide by 1,000

b)

Multiply by 1,000

c)

Nothing

d)

Divide by molar mass

85.

What would be the freezing point of a 1 molar solution of NaCl in water? (The Kf = 1.56 oC/mole)

ΔT=i⋅m⋅Kf\Delta T=i\cdot m\cdot K_f

a)

-1.56 oC

b)

-3.12 oC

c)

+1.56 oC

d)

+3.12 oC

86.

What happens to the Molarity if the same number of moles are used, but the volume is reduced by half?

a)

It remains the same

b)

It is reduced by half

c)

It is doubled

d)

It is quadrupled

87.

How many L are required to make 3.5 M hydrochloric acid using 1.1 moles? 

a)

3.18 L

b)

0.31 L

c)

3.85 L

d)

4.6 L

88.

What is the molarity in 650. ml of solution containing 63 grams of sodium chloride?

a)

2.4 M

b)

0.86 M

c)

1.7 M

d)

0.54 M

89.

Which solution is more diluted?

Solution 1:

1000 mL of water

60g of salt


Solution 2:

500 mL of water

60 g of salt

a)

Not enough information to tell

b)

Solution 1

c)

Solution 2

d)

They are equally diluted

90.

What is the concentration of a solution in parts per million (ppm) if 0.02 grams of NaCl is dissolved in 1 Liter of water?

1.000L of water = 1000g of water and 1000g = 1.000Kg

a)

2 ppm

b)

20 ppm

c)

200 pm

d)

0.2 ppm

91.

What is the percent by mass of a solution made by dissolving 10.0 g of NaCl into 180.0 g of water?

a)

5.26 %

b)

5.56 %

c)

180.0 %

d)

20.0 %

92.

What is the percent concentration of sugar in pink lemonade if 28.0 g of sugar is added to 209 g of water?

a)

14.7 %

b)

5.14 %

c)

13.4 %

d)

11.8 %

93.

The amount of solute actually dissolved in a given amount of solvent is called (a)   .

Choose from the below words
dilution
concentration
saturated solution
supersaturated mixture
94.
A solution that has more solute than it can hold is called
a)
saturated
b)
supersaturated
c)
unsaturated 
d)
suspension
95.

During an epic Fortnite battle, Casey needs to determine the parts per million (ppm) of a health potion containing 0.005 grams of a special ingredient in 1 liter of the potion.

a)

5 ppm

b)

50 ppm

c)

500 ppm

d)

0.5 ppm

96.

Why did the chemistry student fail the concentration test? check only the best answer.

a)

Because he couldn’t handle the pressure!

b)

Because his solutions were too diluted!

c)

Because he lost his molarity!

d)

Because he lost his molarity!

97.

What reaction has the following general formula:
CxHy + O2 −>CO2 + H2OC_xH_y\ +\ O_2\ ->CO_{2\ }+\ H_2O  

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

98.

What type of reaction is the following:
BaCl2+2KI −> 2KCl + BaI2BaCl_2+2KI\ ->\ 2KCl\ +\ BaI_2  

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

99.

What type of reaction is the following:
2KI −> 2K + I22KI\ ->\ 2K\ +\ I_2  

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

100.

What type of reaction is the following:
C11H24+17O2−> 11CO2 + 12H2OC_{11}H_{24}+17O_2->\ 11CO_2\ +\ 12H_2O  

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

101.

What type of reaction is the following:
2NaHCO3−> Na2CO3+CO2+H2O2NaHCO_3->\ Na_2CO_3+CO_2+H_2O  

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

102.

What type of reaction is the following:
Zn + 2HCl −> ZnCl2+H2Zn\ +\ 2HCl\ ->\ ZnCl_2+H_2

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

103.
Question Image

Match the type of chemical reaction below.

a)

Synthesis reaction

1.

Na+ Cl2 →\rightarrow NaCl

b)

Decomposition reaction

2.

2KI −> 2K + I2​  

c)

Single displacement reaction

3.

Pb + FeSO4 ----> PbSO4 + Fe

d)

Double displacement reaction

4.

BaCl2​+2KI −> 2KCl + BaI2​

e)

Combustion reaction

5.

CH4​+O2​→CO2​+H2​O

104.
Breaking down a substance into simpler substances
a)
Displacement
b)
Synthesis
c)
Decomposition
d)
Oxidation
105.
Combining substances to form a new substance
a)
Displacement
b)
Synthesis
c)
Decomposition
d)
Oxidation
106.
This pictures simulates what type of reaction?
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
107.
What is the left part of a chemical equation called?
H2 + O → H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
108.
What does (aq) mean in a chemical reaction?
a)
Ag
b)
silver
c)
aqualirious
d)
aqueous
109.
When balancing equations what does
 -->
mean?
a)
subscript
b)
equals
c)
it is just an arrow
d)
yield
110.
What is the right part of a chemical equation called?
H2 + O → H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
111.

Matter and mass can not be

a)

Shaken or stirred

b)

Made

c)

created or destroyed

d)

Transferred

112.

The Law of Conservation of Mass states that the total mass of the reactants should be

a)

More than the mass of the products

b)

Equal to the mass of the products

c)

Ignored during the reaction

d)

Less than the mass of the products

113.
Provides evidence that a chemical reaction has occurred. 
a)
dissolving 
b)
melting
c)
formation of a gas
d)
bending
114.

How many of each type of atom are in Na2SO4?

​ (a)   Na

​ (b)   S

​ (c)   O

​ (d)   atoms total

Choose from the below words
2
1
4
7
3
5
6
115.

Balanced or unbalanced:

2H2 + O2 --> 2H2O

a)

unbalanced

b)

balanced

116.

What the name of the single bond compounds that formed saturated hydrocarbons?

a)

Alkanes

b)

Alkenes

c)

Alkynes

d)

Alkones

117.

Which statement is correct?

a)

All organic compounds contain carbon

b)

All organic compounds contain hydrogen

118.

How many carbon atoms are in propane?

a)

1

b)

2

c)

3

d)

4

119.

____________ groups are atoms, groups of atoms or bond that determine the characteristic of an organic compound.

a)

Aliphatic

b)

Aromatic

c)

Functional

d)

Hydrocarbon

120.

What are Carbohydrates made from?

a)

Carbon

b)

Hydrogen

c)

Oxygen

d)

Nitrogen

e)

Phosphorus

121.

What is the function of a lipid?

a)

store genetic information

b)

long term energy storage

c)

short term energy storage

d)

many many many things...muscle growth, cell transport, lower activation energy...

122.

What is the function of a protein?

a)

store genetic information

b)

long term energy storage

c)

short term energy storage

d)

many many many things...muscle growth, cell transport, lower activation energy...

123.

Which of the following statement(s) is/are true.

a)

The molecules in a gas take up a negligible amount of space in relation to the container they occupy.

b)

Collisions are elastaic, so energy is gained or lost when molecules collide.

c)

The molecules are in constant, linear motion.

d)

All are true

124.

What happens to the Pressure if the Temperature is held constant and the Volume is increased?

a)

Direct, pressure increased

b)

Indirect, pressure decreased

c)

Direct, pressure decreased

d)

Indirect, pressure increased

125.

What happens to the Pressure if the Volume is held constant and the Temperature is decreased?

a)

Indirect, Pressure decreased

b)

Direct, Pressure decreased

c)

Indirect, Pressure increased

d)

Direct, Pressure increased

126.

What happens to the Temperature if the Volume is held constant and the Pressure is increased?

a)

indirect, temperature increased

b)

direct, temperature increased

c)

indirect, temperature decreased

d)

direct, temperature decreased

127.

The volume of a sample of nitrogen is 6.00 L at 35°C and 740. mmHg. What volume will it occupy at STP?

a)

6.59 L

b)

5.46 L

c)

6.95 L

d)

5.18 L

128.

What is the molar mass of NaCl?

a)

50.00 g/mol

b)

55.00 g/mol

c)

60.00 g/mol

d)

58.44 g/mol

129.

What is the atomic number of this atom?

a)

1

b)

3

c)

4

d)

7

130.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

131.
Most of the mass in an atom is made up of _____________________?
a)
protons and electrons
b)
protons and neutrons
c)
neutrons and electrons
d)
electrons and quarks
132.
In order for an atom to be neutral what has to be true?
a)
The atom has more protons than neutrons
b)
The atom has more neutrons than protons
c)
The atom has the same number of protons and neutrons
d)
The atom has the same number of protons and electrons
133.

What does the 6 represent?

a)

Atomic mass

b)

atomic number

c)

chemical symbol

d)

element name

134.

How many electrons does this atom have?

a)

2

b)

4

c)

6

d)

10

135.
The atomic number of an element that has 9 protons, 9 electrons, and 10 neutrons is _____.
a)
9
b)
10
c)
19
d)
28
136.

What is the mass of 0.75 moles of potassium permanganate (KMnO4)?

a)

0.75 g

b)

118.5 g

c)

82.5 g

d)

0.0084 g

137.

What is the family name of this group of elements? 

a)

Alkali metals 

b)

Halogens 

c)

Noble Gases 

d)

Alkali Earth Metals 

138.

Which principle explains the recurring trends in the properties of elements when arranged by increasing atomic number?

a)

periodic law

b)

transition metals

c)

lanthanide series

d)

atomic theory

139.

What is the relationship between electronegativity and atomic radius

a)

Larger radius=Larger electronegativity

b)

Smaller Radius= Smaller electronegativity

c)

These are not related

d)

Smaller Radius= Higher electronegativity

140.

According to the octet rule most elements need _______ valence electrons. (H and He need two)

a)

2

b)

8

c)

6

d)

18

141.

How many of each type of atom are in Ca(OH)2?

​ (a)   Ca

​ (b)   O

2 ​ (c)  

​ (d)   atoms total

Choose from the below words
1
2
H
5
3
OH
Ca
142.

Label the parts of the reaction.

a)

Reactants

b)

Products

1
2
1)
2)
143.

Balance this equation:

​ (a)   Fe + ​ (b)   O2 --> ​ (c)   Fe2O3

Choose from the below words
4
3
2
1
0
144.

In the reaction 2 H2 + O2 → 2 H2O, if you start with 3 moles of H2 and 2 moles of O2, what is the limiting reactant?

a)

H2

b)

O2

c)

None

d)

H2O

145.

What is the percent yield if the theoretical yield is 20 grams and the actual yield is 18 grams?

a)

100%

b)

95%

c)

85%

d)

90%

146.

Read the graduated cylinder to the nearest 0.1 of a milliliter.

a)

76.00 mL

b)

76 mL

c)

76.0 mL

d)

78.0 mL

147.

What is the volume of the ring? In other words, how much water did it displace?

a)

64 mL

b)

68 mL

c)

8 mL

d)

4 mL

148.

How many centimeters are in a meter

a)

1000

b)

10

c)

100

d)

1

149.

kilo is the prefix with a value of

a)

10

b)

100

c)

1000

d)

1

150.

Which is longer one millimeter or one centimeter?

a)

millimeter

b)

centimeter

151.

H2O is an example of a(n):

a)

Element

b)

Compound

c)

Homogeneous Mixture

d)

Heterogeneous Mixture

152.

a substance that cannot be broken down into other substances

a)

matter

b)

mixture

c)

element

d)

solid

e)

solution

153.

a change to a substance that does NOT change the identity of the substance

a)

physical change

b)

physical property

c)

chemical change

d)

chemical property

154.

an example of a chemical change

a)

breaking glass

b)

boiling water

c)

stretching copper into wire

d)

rusting

155.

Anything that has mass and volume.

a)

solid

b)

liquid

c)

gas

d)

matter

e)

mixture

156.
The theory that states that all particles in matter are constantly moving; helps to describe the phases of matter
a)

ideal behavior of gases

b)

kinetic molecular theory (KMT)

c)
matter matters
d)

temperature

157.
When a cold tire is inflated to a certain pressure and then is warmed up due to friction with the road, the pressure increases. This happens because the
a)
air molecules hit the walls of the tire less frequently
b)
rubber in the tires reacts with oxygen in the atmosphere
c)
air molecules speed up and collide with the tire walls more often
d)
air molecules diffuse rapidly through the walls of the tire.
158.

Particles move ____ as the temperature increases.

a)

faster

b)

slower

159.

What is the chemical formula for Nitrogen triiodide?

a)

NI

b)

N3I

c)

NI3

d)

None of these

160.

What is the name of C3Cl8 ?

a)

Carbon octachloride

b)

Tricarbon octachloride

c)

Carbon trichloride

d)

Octacarbon trichloride

161.

A covalent bond results from _________ valence electrons.

a)

exchanging

b)

gaining

c)

sharing

d)

trading

162.

Choose the correct shape for this molecule:

a)

Trigonal planar

b)

Trigonal pyramidal

c)

Tetrahedral

d)

Linear

163.

What is the the shape of this molecule according to VSPER theory?

a)

Linear

b)

Tetrahedral

c)

Trigonal Planar

d)

Trigonal pyramidal

164.
42 L = ___mL
a)
4,200
b)
.0042
c)
4.20
d)
42,000
165.
285 kg = ____ g
a)
285,000
b)
285
c)
2,850
d)
28,500
166.

A sample of sulfur dioxide occupies a volume of 652 mL at 313 K and 150 kPa. What volume will the sulfur dioxide occupy at STP?


STP = 273 K, 101.3 kPa

a)

1682.6 mL

b)

20.7 mL

c)

492.3 mL

d)

842.1 mL

167.

What type of diagram is this?

a)

Lewis Dot Structure

b)

Bohr Model

c)

Alkali Diagram

d)

Chemical Diagram

168.
How many valence electrons in this structure?
a)
6
b)
5
c)
4
d)
7
169.
Predict the bond that will form between Se and Cl.
a)
Ionic
b)
Covalent
170.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
171.
What is the name of C3Cl8 ?
a)
Carbon octachloride
b)
Tricarbon octachloride
c)
Carbon trichloride
d)
Octacarbon trichloride
172.

When naming covalent compounds,

a)

roman numerals are needed but no prefixes required

b)

both roman numerals or prefixes are not required

c)

both roman numerals and prefixes must be included

d)

prefixes are needed but roman numerals are not required

173.

What experiment was Ernest Rutherford famous for?

a)

The oxygen combustion model

b)

The Definite Proportion Experiment

c)

The Cathode Ray-Tube Dixon Theorum

d)

The Gold Foil Experiment

174.

2H2 + O2 → 2H2O

How many moles of water, H2O, can be produced if 8.00 moles of H2 are used? (Show your work and answer)

175.

Balance this equation:

​ (a)   Fe + ​ (b)   O2 --> ​ (c)   Fe2O3

Choose from the below words
4
3
2
1
0
176.

1. Which of the following is a physical change?

a)

A. Burning wood

b)

B. Baking a cake

c)

C. Boiling water

d)

D. Rusting iron

177.

2. Which common item is a mixture, not a pure substance?

a)

A. Distilled water

b)

B. Table salt (NaCl)

c)

C. Aluminum foil

d)

D. Orange juice with pulp

178.

4. What is the main ingredient in table salt?

a)

A. Sodium hydroxide

b)

B. Sodium chloride

c)

C. Potassium nitrate

d)

D. Calcium carbonate

179.

5. Which of the following best describes the atoms in a solid?

a)

A. Moving randomly and far apart

b)

B. Packed closely and vibrating in place

c)

C. Flowing past each other freely

d)

D. Breaking apart into ions

180.

6. Why does salt melt ice on sidewalks in the winter?

a)

A. It generates heat

b)

B. It lowers the freezing point of water

c)

C. It absorbs sunlight

d)

D. It prevents water from sticking to surfaces

181.

What common household product contains acetic acid?

a)

A. Baking soda

b)

B. Vinegar

c)

C. Bleach

d)

D. Soap

182.

What does a chemical reaction always involve?

a)

A. Change in color only

b)

B. A physical change in state

c)

C. Production of new substances

d)

D. Change in size of the material

183.

10. Why does soda fizz when opened?

a)

A. Heat escapes from the can

b)

B. The liquid boils

c)

C. Air gets sucked in

d)

D. Carbon dioxide gas is released

184.

Poll 1:
Why do chemists like nitrates so much?

a)

A. Because they’re cheaper than day rates!

b)

B. Because they’re always bonding!

c)

C. Because they blow up the competition!

d)

D. Because they make salty comments!

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