wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Chem 2-24

Total questions: 105

Worksheet time: 3hrs 49mins

Name
Class
Date
1.
What particle completes this reaction?
a)
alpha particle
b)
beta particle
c)
gamma particle
d)
neutron
2.
What particle completes this reaction?
a)
alpha particle
b)
beta particle
c)
gamma particle
d)
neutron
3.
Solve this equation for alpha decay.
22688Ra = ___ + 42He
a)
22286Rn
b)
22689Ac
c)
22484Po
d)
22588Ra
4.

In order of most to least penetrating radiation we have

a)

Alpha , Beta, Gamma

b)

Beta , Gamma , Alpha

c)

Gamma, Beta, Alpha

d)

Gamma, Alpha, Beta

5.
Which type of nuclear radiation is being emitted here?
a)
Alpha
b)
Beta
c)
Gamma 
d)
none
6.
This is an example of...
a)
Fission  reaction
b)
Fusion reaction
c)
Decomposition reaction
d)
Combustion
7.
The nuclear process occurring at a nuclear power plant.
a)
Nuclear fusion
b)
Nuclear fission
c)
Combustion
d)
Multiplication
8.

The energy producing nuclear reaction that takes place between hydrogen atoms in the sun is an example of

a)

gamma decay

b)

alpha decay

c)

fusion

d)

fission

9.
What is Half-life?
a)
The amount of time it takes for some of the nuclei in a sample of the isotope to decay
b)
The amount of time it takes for half the electrons in a sample of the isotope to decay
c)
The amount of time it takes for half the nuclei in a sample of the isotope to decay
d)
the amount of time it takes to double the nuclei in a sample of the isotope to decay
10.
The half-life of strontium-90 is 25 years. How much strontium-90 will remain after 100 years if the initial amount is 4.0 g?
a)
3.0g
b)
0.25mg
c)
0.3g
d)
0.25g
11.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

12.
The Modern Periodic Table of Elements is arranged by
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
13.

Elements that occur in vertical columns on the periodic table.

a)

periods

b)

metalloids (semimetals)

c)

groups

d)

Proton

14.
An element's identity is determined by the number of
a)
electrons.
b)
protons.
c)
neutrons.
d)
valence.
15.

USE THE PERIODIC TABLE

How many valence electrons does sodium have?

a)

1

b)

2

c)

3

d)

4

16.

USE THE PERIODIC TABLE

How many valence electrons does Phosphorus have?

a)

31

b)

5

c)

15

d)

4

17.
Elements in the same column of the periodic table always have the same # of _______ as one another.
a)
Protons
b)
Neutrons
c)
Electrons
d)
Valence Electrons
18.
Families all have similar 
a)
Names
b)
atomic numbers
c)
atomic masses
d)
properties
19.

How does a group 1 metal atom form an ion?

a)

lose 1 electron

b)

lose 2 electrons

c)

gain 1 electron

d)

gain 2 electrons

20.

What is the charge of a group 1 metal ion?

a)

1+

b)

2+

c)

1-

d)

2-

21.
How many valence electrons does a halogen have? 
a)
1
b)
2
c)
7
d)
8
22.
How many valence electrons does an alkaline earth metal have? 
a)
1
b)
2
c)
7
d)
8
23.

If a potassium atom lost one electron, what would be the symbol for that ion?

a)
b)
c)
d)
24.

What is the oxidation number (charge) of Li?

a)

1+

b)

1-

c)

2+

d)

2-

25.

What is the oxidation number (charge) of P?

a)

3+

b)

3-

c)

5+

d)

5-

26.

Magnesium has 12 electrons. In how many energy levels are the electrons of magnesium?

a)

1 energy leve

b)

2 energy levels

c)

3 energy levels

d)

4 energy levels

27.

How many electrons would fluorine need to gain in order to have a stable outer energy level?

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

4 electrons

28.

What is an electron dot diagram?

a)

symbol of element with dots representing the electrons in the outer shell

b)

vertical column of elements on the periodic table

c)

row of elements on periodic table

d)

arrangement of the elements by increasing atomic numbers

29.

The rows or periods on a periodic table represent?

a)

The number of protons

b)

The number of energy levels

c)

The number of atoms in an energy level

d)

The number of electrons and mass number

30.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
31.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
32.

What is the atomic radius?

a)

The distance from the nucleus to outermost electron

b)

The distance from one side of an atom to the other side

c)

The distance around the atom

d)

The distance between atoms in the gas phase

e)

The distance between atoms in the solid phase

33.
What is ionization energy?
a)
Energy needed to destroy an atom
b)
Energy required to remove an electron
c)
Energy needed to split an electron
d)
Energy required to add an electron
34.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
35.
The graph above shows the ionization energy values as the elements are arranged on the periodic table. Which conclusion cannot be drawn from the graph?
a)
The ionization energy drops significantly as you move down a group because the valence electrons are in a shell further from the nucleus.
b)
The ionization energy increases gradually as you move right across a period because the valence electrons are in a shell further from the nucleus.
c)
The ionization energy increases gradually as you move right across a period because you are adding more protons.
d)
The ionization energy increases when the valence electrons are more attracted to the nucleus.
36.

As you look from left to right across a period, electronegativity

a)

increases

b)

decreases

37.

Electronegativity trends are the same as:

a)

Atomic radius trends

b)

Ionization energy trends

c)

Both of these

d)

None of these

38.

What does electronegativity do as you go across a period?

a)

decrease

b)

no pattern

c)

stay the same

d)

increase

39.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
40.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
41.
What is a valence electron?
a)
an electron that is found in the outermost shell of an atom. 
b)
an electron found in the innermost shell of an atom.
c)
an electron found in the middle shell.
42.

Sodium is an element with atoms with 11 protons. For it to be stable, does it lose or gain electrons?

a)

Lose

b)

Gain

43.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
44.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
45.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
46.
What happens when an atom loses an electron?
a)
Neutral (no charge)
b)
Positive charge
c)
Negative charge
47.
What happens when an atom gain an electron?
a)
Neutral(no charge)
b)
Positive charge
c)
Negative charge
48.

Elements tend to react to acquire the stable electron structure of a(n)

a)

ion

b)

halogen

c)

metal

d)

noble gas

49.

How do molecules of gas behave?

a)

They vibrate in place.

b)

They bounce around randomly.

c)

They are locked in place by chemical bonds.

d)

They clump together.

50.

Which diagram represents a gas?

a)

A

b)

B

c)

C

d)

None of the Above

51.

I have a

definite, fixed volume. What could I be?

a)

solid or liquid

b)

liquid only

c)

gas only

d)

solid only

e)

liquid or gas

52.

Which phase of matter is compressible with lots of free space between particles?

a)

Liquid

b)

Gas

c)

Solid

53.

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

54.

What is the pressure of a car tire that had an initial pressure of 1.8 atm but was heated from 38°C to 123°C?

a)

0.9 atm

b)

2 atm

c)

1.6 atm

d)

3.4 atm

55.

You have a gas that has a pressure of 2 ATM and a volume of 10L. What would be the new volume if the pressure was changed to 1 ATM?

P1⋅V1=P2⋅V2P_1\cdot V_1=P_2\cdot V_2  

a)

5 L

b)

20 L

c)

It would stay at 10L

d)

1 L

56.
What is 0.00 degrees Kelvin known as
a)
No such thing
b)
Very cold
c)
Freezing point of Water
d)
Absolute Zero
57.

If 10L of O2 at 273K and 1 atm is compressed to a 7L container at 250K, what is the new pressure?

P2= P1V1T2/V2T1

a)

1.31 atm

b)

9.16 atm

c)

0.76 atm

d)

6.0 atm

58.

PV=nRT what are the units for T?

a)

L

b)

K

c)

mL

d)

Celcius

59.

PV=nRT what is n?

a)

atm or torr

b)

K

c)

mL

d)

mole

60.
What pressure, in atm, is exerted by 2.50 L of gas containing 1.35 mol at 320 K?
PV=nRT
a)
14.19 atm
b)
16.53 atm
c)
18.42 atm
d)
22.54 atm
61.
If the pressure exerted by a gas at 25 degrees C in a volume of 0.044 L is 3.81 atm, how many moles of gas are present?
a)
.002766 mole
b)
.0069 mol
c)
2.766 mol
d)
9.887 mol
62.

A substance moves from a solid to a liquid, what must occur?

a)

the substance must undergo an endothermic reaction and release energy

b)

the substance must undergo an exothermic reaction and release energy

c)

the substance must undergo an endothermic reaction and absorb energy

d)

the substance must undergo an exothermic reaction and absorb energy.

63.

1. Kinetic refers to _______________

a)

Force

b)

Energy

c)

Motion

d)

Acceleration

64.

Gas pressure is caused by ______.

a)

gravity.

b)

gas molecules colliding with each other.

c)

gas molecules colliding with surfaces of the container.

d)

gas molecules reacting with each other.

65.

A mixture of H, Ne, & O has a pressure of 12.4 atm. If Hydrogen measures 5.6 atm and Oxygen measures 2.0 atm, what is the pressure of Neon?

a)

7.6 L

b)

4.8 L

c)

5.4 L

d)

12.0 L

66.
Which of the following has the lowest density?
a)
Gasses
b)
Solids
c)
Liquids
d)
All mater is the same density
67.
Which of the following has the greatest amount of movement at a given temperature?
a)
Gas
b)
Liquid
c)
Solid
d)
They all have the same movement
68.

Which of the following states of matter has the LOWEST level of energy?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

69.

What happens to the average kinetic energy of matter when it is heated?

a)

It increases

b)

It stays the same

c)

It decreases

d)

It cannot be determined

70.
This happens to water at 0 degrees Celsius.
a)
Boils
b)
Freezes
c)
Heats
d)
All of them
71.
Between which points is the temperature of the substance remaining constant?
a)
A-B only. 
b)
A-B, C-D, E-F
c)
B-C only. 
d)
B-C, D-E
72.

Which area represents liquid water temperature rising ?

a)

A-B

b)

B-C

c)

C-D

d)

D-E

73.

Liquid to Gas

a)

deposition

b)

vaporization

c)

condensation

d)

sublimation

74.

Segment D-E represents the...

a)

Melting Point

b)

Boiling Point

75.

Between which two points is Heat of Fusion?

a)

A <----> B

b)

B <----> C

c)

C <----> D

d)

D <----> E

e)

E <----> F

76.

The amount of energy required to raise the temperature 1ºC for every gram is called____?

a)

Thermal Energy

b)

Specific Heat

c)

Temperature

d)

Kinetic Energy

77.

The amount of energy required for a liquid at its boiling point to become a gas is _____________.

a)

heat of fusion

b)

heat of vaporization

c)

transpiration

d)

freezing point

78.

The amount of energy needed to change a substance from the solid phase to the liquid phase is the substance's

a)

heat of vaporization

b)

heat of transformation

c)

melting point

d)

heat of fusion

79.
How would this reaction be classified?
2Na + Cl2 → 2NaCl + 25kJ energy
a)
Exothermic
b)
Endothermic
c)
Isothermic
d)
None of the above
80.
What is true of the reaction described below?
Br2 + Cl2 + 30.0 J of energy  → 2BrCl
a)
It is exothermic because energy was released.
b)
It is endothermic because energy is absorbed.
c)
It is exothermic because energy is absorbed.
d)
It is endothermic because energy is released.
81.

The amount of thermal energy stored in an object depends on:

a)

the mass of the object.

b)

the temperature of the object.

c)

the amount of energy that the particular material stores per degree of temperature.

d)

All of the above

82.
What does the Law of Conservation of Energy state?
a)
Energy cannot be created or destroyed
b)
Nothing can exchange energy
c)
Energy will increase over time.
d)
Energy will decrease over time.
83.

The specific heat of platinum is 0.133 J/g°C. How much heat(Q) is absorbed when a 10 g piece of platinum warms from 100°C to 150°C?

a)

66.5 J

b)

665 J

c)

0.0266 J

d)

0.665 J

84.

A 15.75-g piece of iron absorbs 1086.75 joules of heat energy, and its temperature changes from 25°C to 175°C. Calculate the specific heat capacity of iron.

a)

0.46 J/goC

b)

1.654 J/goC

c)

2,567,446.875 J/goC

85.

What is a compound?

a)

2 or more elements separated

b)

2 or more atoms of the same element

c)

2 or more elements combined in a fixed ratio

d)

A bunch of elements grouped together

86.

The substances in this mixture have been mixed together so well that the different parts will not separate on their own.

a)

Homogeneous mixture

b)

Heterogeneous mixture

c)

Pure substance

d)

Suspension

e)

Solution

87.

Solutions are ___________ mixtures.

a)

Solid

b)

Homogenous

c)

Heterogeneous

d)

Gas

88.
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
89.
What is a solvent?
a)
The substance that does the dissolving in a solution.
b)
The substance that is being dissolved in a solution.
c)
The mixing of different substances.
d)
The process in which neutral molecules lose or gain electrons
90.
Which is an example of a solute?
a)
Egg whites
b)
Sugar
c)
Water
d)
Acetone
91.
Which is not an example of dissolving?
a)
Salt in water
b)
Sugar in water
c)
Water in water
d)
Copper sulfate in water
92.

When you dissolve sugar cubes in tea, the sugar cube is the __________.

a)

solute

b)

solvent

93.

When you dissolve sugar cubes in tea, the tea is the ____________.

a)

solvent

b)

solute

94.

What is the solubility of KNO3 at 50°C?

a)

Approximately 85 g

b)

Approximately 100 g

c)

Approximately 50 g

d)

Approximately 15 g

95.

How does stirring influence the rate of dissolving?

a)

Increases the rate of dissolving

b)

Decreases the rate of dissolving

c)

Does not influence the rate of dissolving

96.

How does temperature generally influence the rate of dissolving?

a)

Increase in temperature generally increases the rate of dissolving

b)

Decrease the temperature generally increases the rate of dissolving

c)

Temperature does not influence the rate of dissolving

97.

These are all ways to make a solution dissolve FASTER. Choose all that apply.

a)

Stirring

b)

Use cold water

c)

Use small particles

d)

Shaking

98.

How many grams of K2Cr2O7, are soluble in 100 g of water at 95 ºC?

a)

83 grams

b)

75 grams

c)

40 grams

d)

12 grams

99.
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
100.
When 50 grams of KCl is dissolved in 100 grams of water at 50 ºC, the solution can be correctly described as:
a)
supersaturated
b)
unsaturated
c)
saturated
101.

When 42 grams of potassium chloride ( KCl), is dissolved in 100 grams of water at 50 ºC, the solution can be correctly described as:

a)

supersaturated

b)

saturated

c)

unsaturated

102.
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
103.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

104.
What is the concentration, in percent by mass, of 0.62 g of solute in 45.0 g of solution?
a)
0.014 %
b)
1.4 %
c)
0.13%
105.

Calorimetry Question:
A piece of metal with a mass of 32.8 g is heated to 100.5°C and dropped into 138.2 g of water at 20.0°C.  The final temperature of the system is 30.2°C.  What is the specific heat capacity of the metal? (Specific heat of water is 4.18 J/g⋅°C)

a)

2.56 J/g⋅°C

b)

0.391 J/g⋅°C

c)

5.29 J/g⋅°C

d)

3.50 J/g⋅°C

Similar Resources on Wayground

Final Exam review2018- 7th science

100 questions

Final Exam review2018- 7th science

quiz

Worksheet

•

7th - 9th Grade

Cell Division (Includes 1st Semester Review)

101 questions

Cell Division (Includes 1st Semester Review)

quiz

Worksheet

•

9th - 12th Grade

Life Science/Biology FINAL Test

100 questions

Life Science/Biology FINAL Test

quiz

Worksheet

•

7th Grade - University

biomolecules

100 questions

biomolecules

quiz

Worksheet

•

9th Grade

photosynthesis and cellular respiration review

102 questions

photosynthesis and cellular respiration review

quiz

Worksheet

•

9th - 11th Grade

OCN: MID-TERM Exam

100 questions

OCN: MID-TERM Exam

quiz

Worksheet

•

9th - 12th Grade

Living Environment Regents DRILL 2

110 questions

Living Environment Regents DRILL 2

quiz

Worksheet

•

9th Grade

GCSE Biology Paper 1

105 questions

GCSE Biology Paper 1

quiz

Worksheet

•

9th - 11th Grade