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Total questions: 121

Worksheet time: 2hrs 1mins

Name
Class
Date
1.

Isomer

a)

Same protons different neutrons

b)

Same name different structure

c)

Same molecular formula different structural formula

d)

Same chemical property different physical property

2.

For the following reaction, determine which species is acting as the Arrhenius acid:

HCl + KOH --> KCl + H2O

a)

HCl

b)

KOH

c)

KCl

d)

H2O

3.

In the following reaction, which substance is classified as an acid according to Arrhenius?

CH3COOH + Al(OH)3 --> CH3COOAl + H2O

a)

CH3COOH

b)

Al(OH)3

c)

CH3COOAl

d)

H2O

4.
If there is excess hydrogen ions, the solution will be...
a)
acidic
b)
basic
5.
In a ____ reaction, an acid and a base produce a salt and a water. 
a)
concentrated
b)
decomposition
c)
dilute
d)
neutralization
6.

Complete the following reaction:

HNO3 + Ca(OH)2 -->

a)

Ca(NO3)2 + H2O

b)

Ca +H2O

c)

Ca(NO3)2 + H2

d)

Ca(NO3)2 + H2O + CO2

7.

30mL of NaOH is neutralized by 12.3mL of 0.2M HCl. What is the concentration of the NaOH.

a)

82 mol/l

b)

0.82 mol/l

c)

0.49 mol/l

d)

0.082 mol/l

8.
What is the molarity of a NaOH solution if 11.6 mL of 3 M HCl was used to neutralize 25 mL of NaOH?
a)
1.392 M
b)
0.155 M
c)
0.718 M
9.

The pH scale is an inverse function. This means the ___________ the concentration of hydrogen ions, the ___________ the pH is. (select all that apply)

a)

higher, lower

b)

lower, higher

c)

higher, higher

d)

lower, lower

10.

Choose the substance that is more acidic using the scale

a)

Milk

b)

Soap

c)

Coffee

d)

Stomach acid

11.
A neutralization reaction will (almost) always produce...
a)
water & salt
b)
water
c)
salt
d)
water & carbon
12.

If element X forms the oxides XO and X2O3, the oxidation numbers of element X are

a)

+1 and +2

b)

+2 and +3

c)

+1 and +3

d)

+2 and +4

13.

Which half-reaction shows both the conservation of mass and conservation of charge?

a)

Cl2 + 2e- →\rightarrow 2Cl-

b)

Cl2 →\rightarrow Cl- + 2e-

c)

2 Br- + 2e- →\rightarrow Br2

d)

Br- →\rightarrow Br2 + 2e-

14.
What reaction occurs at the anode?
a)
Ag+ + e- →Ag
b)
Ag → Ag+ + e-
c)
Ni2+ + 2e- → Ni
d)
Ni → Ni2+ + 2e-
15.
In a voltaic cell the ions flow through the 
a)
wire
b)
salt bridge
16.
What occurs at the cathode in an electrolytic cell?
a)
oxidation
b)
reduction
17.
What element is being Oxidized?
a)
N
b)
H
c)
O
d)
S
18.
What element is being Oxidized?
a)
I
b)
H
c)
S
d)
O
19.
What are the coefficients when the equation is balanced?
a)
1 + 1 + 1 --> 2 + 1 + 3
b)
2 + 2 + 2 --> 4 + 2 + 3
c)
1 + 2 + 1 --> 2 + 2 + 3
d)
1 + 1 + 1 --> 1 + 1 + 1
20.
What is oxidation number of H in H2O?
a)
0
b)
-2
c)
-1
d)
+1
21.
What is oxidation number of H in CaH2?
a)
+1
b)
-1
c)
0
d)
+2
22.

​ (a)   ​ ​ Nuclear waste is toxic and must be stored far away from people, and food and water supplies

Choose from the below words
Disadvantage
Advantage
23.

​ (a)   ​ ​ Nuclear waste must be stored for thousands of years 

Choose from the below words
Disadvantage
Advantage
24.

finish the equation


18173Ta --> ____ + 18174W

a)

42He

b)

0-1e

c)

y

25.

Identify the type of nuclear decay shown here

21483Bi → 0-1e + 21484Po

a)

alpha

b)

beta

c)

gamma

26.

Finish this equation

20983Bi--> _______ + 20581Tl

a)

42He

b)

0-1e

c)

y

27.

What type of nuclear decay is shown here

13756Ba →→ 13756Ba + γ rays

a)

alpha

b)

beta

c)

gamma

28.

Solve this equation for.

614C = ___ + -10e

a)

410Be

b)

714N

c)

210He

d)

613C

29.
What is the missing isotope that will balance the following nuclear equation?
94Be  +  11H →  _____  +  42He
a)
105B
b)
105Ne
c)
63Li
d)
63C
30.

Which of these processes describes a nuclear fusion reaction?

a)

A nucleus absorbs energy to produce lighter nuclei.

b)

A nucleus splits to produce energy and lighter nuclei

c)

Two nuclei bind together to produce energy and heavier nuclei.

d)

Two nuclei bind together to produce energy and a lighter nuclei.

31.
This is an example of...
a)
Fission  reaction
b)
Fusion reaction
c)
Decomposition reaction
d)
Decay
32.

If there are 340 grams of a substance and it's half-life is 23 years how many grams would be left after 46 years?

a)

170 grams

b)

85 grams

c)

340 grams

d)

42.5 grams

33.

If there are 340 grams of a substance and it's half-life is 23 years what percent of the substance would there bve left after 5 half-lives?

a)

50%

b)

25%

c)

12.5%

d)

6.25%

e)

3.125%

34.

What is kinetic energy?

a)

stored energy

b)

energy of motion

c)

elastic energy

d)

gravity

35.

Which of the following is an example of thermal energy?

a)

heat

b)

light

c)

sound

d)

mass

36.

The potential energy stored in chemical bonds in substances is called

a)

chemical energy.

b)

nuclear energy.

c)

electrical energy.

d)

thermal energy.

37.
The _____is the part that gets dissolved. 
a)
solute 
b)
solvent 
c)
solution 
d)
Sacajawea 
38.
The universal solvent is ______. 
a)
sodium 
b)
acid 
c)
water 
d)
wind 
39.

A 2400.-gram sample of an aqueous solution contains 0.012 gram of NH3. What is the concentration of NH3 in the solution, expressed as parts per million?

a)

5.0 ppm

b)

15 ppm

c)

20. ppm

d)

50. ppm

40.

What is the concentration of a solution in parts per million if 0.02 grams of NaCl is dissolved in 1000 grams of solution?

a)

2 ppm

b)

20 ppm

c)

200 pm

d)

0.2 ppm

41.

Helium gas, 3.0 x 10-4 g, is dissolved in 200 g of solution. Express this concentration in parts per million.

(a)  

42.

What is the percent by mass of HYDROGEN in sugar, C12H22O11?

43.

What is the empirical formula for C4H6?

a)

CH

b)

CH3

c)

C2H3

d)

C4H6

44.

Given the following: 42.07% Na, 18.89% P, and 39.04% O, determine the empirical formula.

a)

NaPO2

b)

Na2PO3

c)

Na3PO4

d)

NaPO4

45.
What is the empirical formula if you have 88.80% copper and 11.20% oxygen?
a)
Cu3O8
b)
CuO4
c)
Cu2O
d)
Cu4O10
46.

__ Al + __ FeO → Al2O2 + __ Fe

a)

1, 1, 2

b)

2,1,2

c)

2, 2, 2

d)

2,4,2

47.

PCl5 + ___ H2O → ___ HCl + H3PO4

a)

4, 5

b)

1, 6

c)

3, 8

d)

2,2

48.

Thermo-energy, heat, always flow from ​ (a)   energy area to ​ (b)   enenrgy area.

Choose from the below words
high
low
49.

Which statement correctly describes this reaction?

a)

It is endothermic and energy is absorbed.

b)

It is endothermic and energy is released.

c)

It is exothermic and energy is absorbed.

d)

It is exothermic and energy is released

50.

Which letter in the diagram represents the heat of reaction?

a)

A

b)

B

c)

C

d)

D

51.

For any chemical reaction at equilibrium, the rate of the forward reaction is

a)

less than the rate of the reverse

b)

greater than the rate of the reverse

c)

equal to the rate of the reverse

d)

unrelated to the rate of the reverse

52.

For a chemical reaction, the difference between the potential energy of the products and the potential energy of the reactants is equal to the

a)

heat of fusion

b)

heat of reaction

c)

activation energy of the forward reaction

d)

activation energy of the reverse reaction

53.

As the number of effective collisions between reacting particles increases, the rate of reaction

a)

decreases

b)

increases

c)

remains the same

54.
Entropy increases from solid, liquid to gas. Why?
a)
Molecular disorder increases
b)
Molecular randomness decreases
c)
Molecules are more energetic
d)
Molecules are more reactive
55.

Systems in nature tend to undergo changes toward

a)

lower energy and less disorder

b)

lower energy and more disorder

c)

higher energy and less disorder

d)

higher energy and more disorder

56.

The entropy will usually increase when

a)

a molecule is broken into two or more smaller molecules

b)

a reaction occurs that results in an increase in the number of moles of gas

c)

a solid changes to a liquid

d)

all of these

57.

Potential and Kinetic Energy have a _______________ relationship. When one goes up the other goes down

a)

inverse

b)

direct

58.
A catalyst works by
a)
changing the order of the reaction
b)
increasing the temperature
c)
lowering the activation energy
d)
making the activated complex
59.

How do you calculate Enthalpy of a reaction?

a)

ΔH = ΔHproducts - ΔHreactants

b)

ΔT = q / mC

c)

ΔG = ΔH -TΔS

d)

E = mc2

60.

Calculate the change in enthalpy  ΔH\Delta H  for the following reaction:
2CO + O2 ⟶ 2CO22CO\ +\ O_{2_{\ _{ }}^{ }}\longrightarrow\ 2CO_{2_{ }}  
Use your heats of formation table from your worksheet

a)

-393.5 kJ/mol

b)

-566.0 kJ/mol

c)

566.0 kJ/mol

d)

-369 kJ/mol

61.

What is the difference between calculating ΔH\Delta H   with bond energies versus with heats of formation?

a)

Bond energies are averages based on multiple scenarios of breaking bonds, heats of formation is the energy required to form a specific molecule from its elemental forms.

b)

Heats of formation are averages based on multiple scenarios of breaking bonds, bond energies is the energy required to form a specific molecule from its elemental forms.

c)

Bond energies are calculated using only lewis dot structures, but heats of formation requires a reference table

d)

Heats of formation helps calculate enthalpy, while bond energies helps calculate entropy

62.
You have 20 g of water with specific heat of 4.18 J/gŸ°C.  The temperature changes from 25° C to 20° C.  How much heat energy (Q) moves from the water to the surroundings?
a)
418 Joules
b)
209 J
c)
83 J
d)
4.18 J
63.

A sample of liquid has a mass of 300 g and occupies 50 mL in a graduated cylinder. What is the density?

a)

15,000 g/mL

b)

.16667 g/mL

c)

6 g/mL

d)

Yup, still no clue

64.
Frank has an eraser. It has a mass of 4g, and a volume of 2cm3. What is its density?
a)
8 g/cm3
b)
2 g/cm3
c)
1/2 g/cm3
d)
24 g/cm3
65.
How much water has been displaced in the image shown?
a)
40 mL
b)
65 mL
c)
20 mL
d)
25 mL
66.
Find the density of a 2 cm x 2 cm x 2 cm cube with a mass of 64 g.
a)
6 cm3
b)
12 g/cm3
c)
128 g/cm3
d)
8  g/cm3
67.
What is the density of water?
a)
0 g/ml
b)
1 g/ml
c)
10 g/ml
d)
100 g/ml
68.

An object is is placed into 45 mL of water. The water rises to 48 mL. What is the volume of the object?

a)

3 mL

b)

93mL

c)

8 mL

d)

83 mL

69.

Which of the following will have similar properties?

a)

O, S, Se

b)

O, F, Ne

c)

N, Ne, Na

d)

H, K, P

70.

The blue elements (left side) are called 

a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
71.

The yellow elements (right side) are called 

a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
72.
Which elements have the most similar chemical properties?
a)
K and Na
b)
K and Ca
c)
K and Cl
d)
K and S
73.

When an atom loses a valence electron, it becomes a(n) _____________.

a)

cation

b)

anion

c)

dogion

d)

clingon

74.
If an element has 3 valence electrons, what charge will likely form on its ion ?
a)
+3
b)
+5
c)
-3
d)
-5
75.
Which of the following has a -3 charge?
a)
Boron
b)
Fluorine
c)
Nitrogen
d)
Neon
76.

What is the charge of a sodium ion?

a)

+2

b)

+1

c)

-1

d)

-2

77.
What is the charge of an atom that has lost one electron?
a)
-1
b)
-2
c)
+1
d)
+2
78.
Cations are...
a)
Positive
b)
Negative
c)
Neutral
d)
Purring
79.

An atom with 2 protons, 3 neutrons, and 4 electrons has a charge of ____.

a)

+2

b)

-2

c)

+3

d)

0

80.
Balance the following reaction :
 
CaC₂(s)   +   H₂O(l)   -->   C₂H₂(g)   +   Ca(OH)₂(aq)
a)
1,2,2,2
b)
1,2,1,1
c)
2,1,1,1
d)
2,1,2,1
81.

I use mole ratio (coefficients) from balanced chemical equation?

a)

True

b)

False

82.

Pressure is

a)

defined as the mass that an object exerts when at rest.

b)

not a measurable in gases.

c)

defined as the number of moles of substance divided by the mass of the substance.

d)

created by the force of the gas particles impacting the walls of the container.

83.

Which container will have lower pressure?

a)

First container

b)

second container

84.

As temperature rises ___________.

a)

an atom's kinetic energy decreases

b)

an atom's kinetic energy increases

c)

an atom's kinetic energy stays the same

85.
If a balloon is cooled what will happen to the volume?
a)
Volume will increase
b)
Volume will decrease
c)
Volume will not change
86.

A student measures the pressure and volume of an empty water bottle to be 1.4 atm and 2.3 L. She then decreases the pressure to 0.65 atm. What is the new volume?

a)

2.1 L

b)

5.0 L

c)

8.2 L

d)

3.9 L

87.
Which direction do the electrons flow in wire X and which metal is oxidized?
a)
A
b)
B
c)
C
d)
D
88.
Which species is oxidized in the following reaction?
a)
Ag
b)
Ag+
c)
Cu
d)
Cu2+
89.
Oxidation happens at the
a)
anode
b)
cathode
c)
salt bridge
d)
voltmeter
90.

How is voltaic cell electricity produced?

a)

A chemical reaction

b)

It is pumped into the cell

c)

It injects itself

d)

An injected chemical reaction

91.

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

which element, if any, is oxidized?

a)

Zinc

b)

Hydrogen

c)

Chlorine

d)

None

92.

Given the reaction:

Fe(s) + Cu2+(aq) →\rightarrow Fe2+(aq) + Cu(s)

Which half-reaction correctly shows the oxidation that occurs?

a)

Fe(s) →\rightarrow Fe2+(aq) + 2e-

b)

Fe(s) + 2e- →\rightarrow Fe2+(aq)

c)

Cu2+(aq) →\rightarrow Cu(s) + 2e-

d)

Cu(s) →\rightarrow Cu2+(aq) + 2e-

93.

Given the balanced equation representing the reaction occuring in a voltaic cell:

Zn(s) + Pb2+(aq) →\rightarrow Zn2+(aq) + Pb(s)

In the completed external circuit, the electrons flow from

a)

Pb(s) to Zn(s)

b)

Pb2+(aq) to Zn2+(aq)

c)

Zn(s) to Pb(s)

d)

Zn2+(aq) to Pb2+(aq)

94.

_______ separates mixtures based on differences in boiling point.

a)

filtering

b)

distillation

c)

chromatography

95.

_____ is the average amount of kinetic energy found in an object/system.

a)

Temperature

b)

Kinetic Energy

c)

Heat

d)

Thermal Energy

96.

Adding a solute will ____________ the boiling point and ___________ the freezing point

a)

Decrease, decrease

b)

Decrease, increase

c)

Increase, increase

d)

Increase, decrease

97.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
98.
Compounds made from only nonmetals are _________________ compounds.
a)
ionic
b)
covalent
c)
metallic
d)
chemical
99.
The chemical formula shows one carbon atom bonded to __________ oxygen atoms.
a)
one
b)
two
c)
three
d)
four
100.

What is the formula of this molecule?

a)

CH

b)

HC4

c)

CH4

d)

C4H4

101.

Element with 5 valence electrons

a)

Phosphorus

b)

Oxygen

c)

Hydrogen

d)

Chlorine

102.

In the quantum mechanical model, there is a higher chance of finding electrons when they are _____

a)

far away from the nucleus

b)

close to the nucleus

103.
Sodium has an atomic number of 11, how many protons does this atom have?
a)
22
b)
11
c)
12
d)
2
104.
The following element key shows how many protons?
a)
16
b)
15.999
c)
Oxygen
d)
8
105.
Which subatomic particle causes the nucleus to have a positive charge?
a)
Neutron
b)
Electrons
c)
Protons
d)
Valence electrons
106.
Which subatomic particle along with the protons make up the total mass of an atom.
a)
Neutron
b)
Electrons
c)
Valence electrons
d)
protons make up all the mass
107.
What is an atomic number?
a)
The sum of protons and neutrons in an atom.
b)
The sum of protons and electrons in an atom.
c)
The number of protons in an atom of a specific element.
d)
The number of neutrons in a specific element.
108.
Where are protons located in the atom?
a)
orbitals
b)
nucleus
c)
rings
d)
positive
109.

located in the nucleus

a)

protons and electrons

b)

protons and neutrons

c)

neutrons and electrons

110.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
111.
How many neutrons does the isotope below have?     89 36Kr
a)
53
b)
36
c)
89
d)
125
112.

12 protons and 13 neutrons

a)

Mg-12

b)

Mg-13

c)

Mg-25

d)

Mg-24.305

113.

The atomic mass of an element depends upon the ___.

a)

relative abundance of protons in that element

b)

mass and relative abundance of each isotope of that element

c)

mass of each isotope of that element

d)

mass of each electron in that element

114.

What are the steps for finding the Average Atomic Mass?

a)

1) write given mass, 2) write given %, 3) % to decimal, 4) Mass x abundance decimal 5) Add

b)

1) % to decimal, 2) write given %, 3)write given mass, 4) Mass x abundance decimal 5) Add

c)

1) write given mass, 2) write given %, 3) % to decimal, 4) Mass divided by abundance decimal 5) Add

d)

1) write given mass, 2) write given %, 3) % to decimal, 4) Mass x abundance decimal 5) Subtract

115.

The atomic mass of an element is the ___.

a)

average of the mass number and the atomic number for the element

b)

weighted average of the masses of the isotopes of the element

c)

total mass of the isotopes of the element

d)

total number of subatomic particles in the nucleus

116.

What is the lowest possible energy level that an electron can occupy?

a)

Lower energy level

b)

Ground State

c)

Excited State 

d)

Depressive State

117.

To jump to an excited state the electron must____

a)

emit energy

b)

absorb energy

118.

The electron started in the ____ state

a)

ground state

b)

excited state

119.

When an electron ABSORBS energy:

The electron moves from a ____energy level to a____ energy level

a)

higher / lower

b)

lower / higher

120.

Exothermic reactions release heat into the surroundings, so you observe a...

a)

temperature increase

b)

temperature decrease

c)

no temperature change

121.

Endo means within. Endothermic reactions

a)

Release heat

b)

Absorb heat

c)

Absorb coldness

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