wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Chemistry Regents Reivew

Total questions: 109

Worksheet time: 2hrs 49mins

Name
Class
Date
1.

Which list of symbols represents nonmetals, only?

a)

B, Al, Ga

b)

Li, Be, B

c)

C, Si, Ge

d)

P, S, Cl

2.

What is the chemical formula for lead(IV) oxide?

a)

PbO2

b)

PbO4

c)

Pb2O

d)

Pb4O

3.
Which statement describes the general trends in electronegativity and atomic radius as the elements in Period 2 are considered in order from left to right? 
a)
Both electronegativity and atomic radius increase.
b)
Both electronegativity and atomic radius decrease. 
c)
Electronegativity increases and atomic radius decreases.
d)
Electronegativity decreases and atomic radius increases.
4.
What is the percent composition by mass of nitrogen in (NH4)2CO3 (gram-formula mass = 96.0 g/mol)? 
a)
14.6% 
b)
29.2%
c)
8.4%
d)
87.5%
5.
Given the balanced equation:
2KI + F2 → 2KF + I2
Which type of chemical reaction does this equation represent? 
a)
synthesis 
b)
decomposition
c)
single replacement 
d)
double replacement 
6.
Which formula represents a nonpolar molecule containing polar covalent bonds?
a)
1
b)
2
c)
3
d)
4
7.
What is the total amount of heat required to completely melt 347 grams of ice at its melting point? 
a)
334 J
b)
1450 J
c)
116000 J
d)
784000 J
8.
What is the charge of the nucleus of an oxygen atom?
a)
0
b)
-2
c)
+8
d)
+16
9.
Which Lewis electron-dot diagram represents a nitrogen atom in the ground state?
a)
1
b)
2
c)
3
d)
4
10.
What is the most likely electronegativity value for a metallic element?
a)
1.3
b)
2.7
c)
3.4
d)
4
11.
Every chlorine atom has
a)
7 electrons
b)
17 neutrons
c)
a mass number of 35
d)
an atomic number of 17
12.
Which substance can not be broken down by a chemical change?
a)
ammonia
b)
methanol
c)
propane
d)
phosphorus
13.

At standard pressure and temperature, what will be the physical state of bromine?

a)

liquid

b)

gas

c)

solid

d)

plasma

14.
Positrons and beta particles have 
a)
the same charge and the same mass
b)
the same charge and different masses
c)
different charges and the same mass 
d)
different charges and different masses
15.
Which term identifies a type of nuclear reaction?
a)
transmutation
b)
neutralization
c)
deposition
d)
reduction
16.
Which property can be defined as the ability of a substance to be hammered into thin sheets?
a)
conductivity
b)
malleability
c)
melting point
d)
solubility
17.
Which list of elements consists of a metal, a metalloid, and a noble gas?
a)
aluminum, sulfur, argon
b)
magnesium, sodium, sulfur
c)
 sodium, silicon, argon
d)
silicon, phosphorus, chlorine
18.
Which substance can not be broken down by a chemical change?
a)
butanal
b)
propene
c)
gold
d)
water
19.
 Which statement describes particles of an ideal gas, based on the kinetic molecular theory? 
a)
Gas particles are separated by distances smaller than the size of the gas particles.
b)
Gas particles do not transfer energy to each other when they collide.
c)
Gas particles have no attractive forces between them. 
d)
Gas particles move in predictable, circular motion.
20.
Which electron configuration represents an excited state for an atom of calcium? 
a)
2-8-7-1
b)
2-8-7-2
c)
2-8-7-3
d)
2-8-8-2
21.
What occurs when potassium reacts with chlorine to form potassium chloride? 
a)
Electrons are shared and the bonding is ionic.
b)
Electrons are shared and the bonding is covalent.
c)
Electrons are transferred and the bonding is ionic.
d)
Electrons are transferred and the bonding is covalent.
22.
Which pair of atoms has the most polar bond? 
a)
H−Br
b)
I−Br
c)
H−Cl
d)
I−Cl
23.
Which two notations represent isotopes of the same element?
a)
1
b)
2
c)
3
d)
4
24.

In an atom, an orbital represents

a)

the most probably location of a proton

b)

the most probable location of an electron

c)

the least probably location of a neutron

d)

photons emitted as electrons move to lower energy levels

25.

Which particle has a mass so small, it is considered to be 0 amu?

a)

proton

b)

hydrogen nucleus

c)

neutron

d)

electron

26.

During a flame test, sodium chloride produces an intense yellow flame. This yellow color is produced when electrons in excited atoms

a)

are gained by the atoms

b)

are lost by the atoms

c)

move to higher energy states within the atoms

d)

move to lower energy states within the atoms

27.

What quantity is the same among atoms of the same element?

a)

mass number

b)

atomic number

c)

number of neutrons

d)

number of nucleons

28.

An atom that has 8 protons and 10 neutrons is an isotope of the element

a)

nitrogen

b)

oxygen

c)

fluorine

d)

neon

29.

Which electron configuration represents the atoms of a bromine atom in the excited state?

a)

2-8-18-7

b)

2-8-18-8

c)

2-8-17-8

d)

2-8-18-7-1

30.

Under which conditions does a gas behave least like an ideal gas?

a)

high temperature and low pressure

b)

high temperature and high pressure

c)

low temperature and low pressure

d)

low temperature and high pressure

31.
The mass of a proton is approximately equal to the mass of
a)
an alpha particle
b)
a beta particle
c)
a neutron
d)
a positron
32.

In an atom, an orbital represents

a)

the most probably location of a proton

b)

the most probable location of an electron

c)

the least probably location of a neutron

d)

photons emitted as electrons move to lower energy levels

33.

During a flame test, sodium chloride produces an intense yellow flame. This yellow color is produced when electrons in excited atoms

a)

are gained by the atoms

b)

are lost by the atoms

c)

move to higher energy states within the atoms

d)

move to lower energy states within the atoms

34.

An atom that has 8 protons and 10 neutrons and 6 electrons is an ion of the what element?

a)

nitrogen

b)

oxygen

c)

fluorine

d)

neon

35.

What part of the atom determines the identity of an atom?

a)

Electrons

b)

Neutrons

c)

Protons

d)

Nucleus

36.

Which scientist discovered the electrons?

a)

Dalton

b)

Thomson

c)

Atristotle

d)

Bohr

37.

Rutherford and his students did experiments that showed

a)

quark

b)

nucleus

c)

proton

d)

electron

38.

Bohr discovered that electrons are located in

a)

the nucleus

b)

inside protons

c)

electron cloud

d)

circular orbits around the nucleus

39.
The most dangerous type of radiation is the ____. 
a)
alpha particle
b)
gamma ray
c)
beta particle
d)
uranium
40.

What is the charge of a neutron?

a)

+1

b)

-1

c)

0

d)

+2

41.

Which scientist is known for the discovery of the nucleus?

a)

Bohr

b)

Rutherford

c)

Thomson

d)

Dalton

42.

An atom that has 7 protons, 7 neutrons and 10 electrons is an ion of what element?

a)

Nitrogen

b)

Oxygen

c)

Fluorine

d)

Neon

43.

The elements on the Periodic Table are arranged in

order of increasing

a)

atomic mass

b)

atomic number

c)

molar mass

d)

oxidation number

44.

Which term represents the strength of the attraction an

atom has for the electrons in a chemical bond?

a)

electrical conductivity

b)

electronegativity

c)

first ionization energy

d)

specific heat capacity

45.

Which term represents the amount of energy required

to remove the most loosely bound electron from an

atom in the gaseous state?

a)

atomic radius

b)

electronegativity

c)

First ionization energy

d)

electrical conductivity

46.

As the elements in Period 2 of the Periodic Table are

considered in order from left to right, which property

generally decreases?

a)

atomic radius

b)

electronegativity

c)

ionization energy

d)

nuclear charge

47.

Which sequence correctly places the elements in order

of increasing ionization energy?

a)

H -> Li -> Na -> K

b)

I -> Br -> Cl -> F

c)

O -> S -> Se -> Te

d)

H -> Be -> Al -> Ga

48.

In a given period of the Periodic Table, the element

with the lowest first ionization energy is always in

a)

Group 1

b)

Group 2

c)

Group 17

d)

Group 18

49.

Which of these elements has physical and chemical

properties most similar to silicon (Si)?

a)

germanium (Ge)

b)

lead (Pb)

c)

phosphorus (P)

d)

chlorine (Cl)

50.

As the atomic number of elements within Group 2

increases, the metallic character of each successive

element

a)

decreases

b)

increases

c)

remains the same

51.

How much energy is required to remove the most

loosely bound electron from a neutral atom of neon

in the gaseous phase?

a)

363 kJ

b)

441 kJ

c)

1086 kJ

d)

2081 kJ

52.

Which atom has the greatest attraction for the

electrons in a chemical bond?

a)

hydrogen

b)

oxygen

c)

silicon

d)

sulfur

53.

Which element is a noble gas?

a)

Argon

b)

chlorine

c)

hydrogen

d)

magnesium

54.

The element helium is classified as a

a)

metal

b)

metalloid

c)

noble gas

55.

An atom of which element has the largest atomic

radius?

a)

Fe

b)

Mg

c)

Si

d)

Zn

56.
A nuclear reaction where a nucleus splits into two smaller nuclei is... 
a)
Fission
b)
Fusion
c)
Gamma decay
d)
Beta decay
57.
What would two different isotopes of an atom have in common?
a)
Number of neutrons 
b)
Number of protons
c)
Atomic weight 
d)
Atomic mass
58.
What happens when the number of protons in an atom changes? 
a)
The number of electrons changes too 
b)
Usually nothing happens, unless the atom is radioactive 
c)
The atomic nucleus explodes
d)
It becomes a completely different atom, with different properties 
59.
What element is the ?
a)
Ag-115
b)
Cd-115
c)
Pd-115
d)
Not Listed
60.
Which type of nuclear radiation is being emitted here?
a)
alpha
b)
beta
c)
gamma
d)
none
61.
Which type of nuclear radiation is being emitted here?
a)
Alpha
b)
beta
c)
gamma 
d)
none
62.
Balance the following equation:
146C --> 0-1e + ________
a)
145B
b)
146C
c)
147N
d)
42He
63.
Negatively charged particles found outside of the nucleus are called
a)
electron
b)
protons
c)
neutrons
d)
nucleons
64.
Positively charged particles found in the nucleus of an atom are called
a)
protons
b)
neutrons
c)
electrons
d)
isotopes
65.
This is an example of...
a)
Fission  reaction
b)
Fusion reaction
c)
Decomposition reaction
d)
Combustion
66.
When nuclei decay, massive amounts of __________ is released.
a)
energy
b)
jello
c)
protons
d)
neutrons
67.
What type of reaction is this?
a)
alpha
b)
beta
c)
gamma
d)
quiet
68.

What is the atomic number?

a)

the number of protons in the nucleus

b)

the number of protons and neutrons in the nucleus

c)

the number of neutrons in the nucleus

d)

the number of protons in the energy levels

69.

What is the mass number?

a)

the number of protons in the nucleus

b)

the number of protons and neutrons in the nucleus

c)

the number of neutrons in the nucleus

d)

the number of protons and electrons in the atom

70.

What is the atomic number of this atom?

a)

1

b)

3

c)

4

d)

7

71.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

72.

Who discovered that the atom had an small, dense, positively charged center?

a)

Ernest Rutherford

b)

J.J Thomson

c)

Robert Millikan

d)

John Dalton

73.

Place the following atomic models in order, from earliest to latest:


A) Rutherford B) Thomson C) Dalton

a)

B, C, A

b)

C, A, B

c)

A, C, B

d)

C, B, A

74.

A hydrogen ion, H+, in aqueous solution may also be written as

a)

OH-

b)

H2O

c)

H3O+

d)

H2O2

75.

Which pH indicates a basic solution?

a)

1

b)

5

c)

7

d)

12

76.

The table shows the molar concentrations of hydronium ions in four different solutions. Which solution has the highest pH?

(Hint: First, decide if the solution is acidic or basic. Then, decide if the solution would have the highest or lowest concentration of H3O+.)

a)

A

b)

B

c)

C

d)

D

77.

Which relationship is present in a solution that has a pH of 6?

a)

[H3O+] = [OH-]

b)

[H3O+] > [OH-]

c)

[H3O+] < [OH-]

d)

[H3O+] + [OH-] = 7

78.

A solution with a pH of 4.0 has a hydronium ion concentration a thousand times greater than a solution with a pH of

a)

1.0

b)

2.0

c)

6.0

d)

7.0

79.

Compared to a solution with a pH value of 8, a solution with a hundred times lower hydronium ion concentration has a pH value of

a)

6

b)

7

c)

9

d)

10

80.

As the pH of a solution changes from 3 to 4, the concentration of hydronium ions

a)

decreases by a factor of 1

b)

decreases by a factor of 10

c)

increases by a factor of 10

d)

increases by a factor of 1

81.

As the pH of a solution is changed from 13 to 11, the concentration of hydronium ions

a)

decreases by a factor of 100

b)

decreases by a factor of 20

c)

increases by a factor of 20

d)

increases by a factor of 100

82.

Which relationship is present in a solution that has a pH of 10?

a)

[H3O+] = [OH-]

b)

[H3O+] > [OH-]

c)

[H3O+] < [OH-]

d)

[H3O+] + [OH-] = 7

83.

Which relationship is present in a solution that has a pH of 7?

a)

[H3O+] = [OH-]

b)

[H3O+] > [OH-]

c)

[H3O+] < [OH-]

d)

[H3O+] + [OH-] = 7

84.

As the pH of a solution is changed from 3 to 1, the concentration of hydronium ions

a)

decreases by a factor of 100

b)

decreases by a factor of 20

c)

increases by a factor of 20

d)

increases by a factor of 100

85.

As the pH of a solution changes from 2 to 5, the concentration of hydronium ions

a)

decreases by a factor of 30

b)

decreases by a factor of 1000

c)

increases by a factor of 1000

d)

increases by a factor of 30

86.

Organic Compound having 3 carbon atoms in a chain has root word as (a)  

87.

Alkene are (a)   compounds

88.

Alkynes are (a)   bonded compounds

89.

CnH2n+2 is the general formula for (a)   series .

90.

How many valency does carbon have

(a)  

91.

Determine whether Al(OH)3 is soluble using Table F

a)

Soluble

b)

Insoluble

92.

Determine whether Na2SO4 is soluble or insoluble using Table F

a)

Soluble

b)

Insoluble

93.
In a gas to liquid mixture, an increase in temperature means...
a)
increase in solubility
b)
decrease in solubility
94.

Which substance is most soluble at 40 degrees Celsius?

a)

KCl

b)

KNO3

c)

NaCl

d)

NH3

95.
The boiling point of a solution is ______ the boiling point of the pure solvent.
a)
higher than
b)
the same as
c)
lower than
d)
higher or lower than
96.
This solution would be considered
a)
Unsaturated
b)
Supersaturated
c)
Saturated
d)
Undefined
97.

Based on Reference Table G, what is the maximum number of grams of KCl(s) that will dissolve in 200 grams of water at 50°C to produce a saturated solution?

a)

38 g

b)

42 g

c)

58 g

d)

84 g

98.

If pressure goes down in a container, what happens to volume when the temperature is held constant.

a)

Increase

b)

Decrease

99.

If temperature goes down in a container, what happens to volume when the pressure is held constant.

a)

Increase

b)

Decrease

100.

What formula would you use to solve the following: A 0.562 L container of Helium has a pressure of 9.5 atm. What volume would be necessary to decrease the pressure to 2.4 atm?

a)
b)
c)
d)
101.

What formula would you use to solve the following: A sample of nitrogen gas was collected over water at a temperature of 23.0°C. What is the partial pressure of nitrogen if the atmospheric pressure (total) was 785 mmHg and the vapor pressure of water was 21.1 mmHg?

a)
b)
c)
d)
102.

What formula would you use to solve the following: A container of carbon monoxide gas is at a temperature of 65.0 °C and occupies a volume of 6.5L. At what temperature would it occupy a volume of 10.2L?

a)
b)
c)
d)
103.

Which of the following is NOT a unit of Pressure?

a)

mmHg

b)

atm

c)

kelvin

d)

psi

104.

In the Question: A cylinder has a volume of 5.4 L of air at a pressure of 140 atm. If the volume is increased to 12.4L, what would the new pressure be? Which answer choice has the data correctly labeled?

a)

P1=5.4L, V1=140atm; P2= 12.4L, V2= ?

b)

P1=140atm, V1=5.4L ; P2= ?, V2=12.4L

c)

T1=140atm, V1=5.4L ; T2= ?, V2=12.4L

d)

There was no important data to label

105.
What is the correct name for C4H6?
a)
Carbon Hexahydride
b)
Pentacarbon Pentahydride
c)
Hexacarbon Tetrahydride
d)
Tetracarbon Hexahydride
106.
What is the correct name for NO?
a)
Mononitrogen Monoxide
b)
Nitrogen Monoxide
c)
Mononitrogen Dioxide
d)
Nitrogen Oxide
107.
BrO3
a)
bromine oxide
b)
monobromine trioxide
c)
bromine trioxide
d)
bromine (III) oxide
108.
What is the OFFICIAL name for H2O
a)
Hydrogen Oxide
b)
Oxygen Dinitride
c)
Agua
d)
Dihydrogen Monoxide
109.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide

Similar Resources on Wayground

Conflict and Cans (CH 4) Test Review

106 questions

Conflict and Cans (CH 4) Test Review

quiz

Worksheet

•

12th Grade

1st 6-weeks test review

114 questions

1st 6-weeks test review

quiz

Worksheet

•

10th - 11th Grade

Chemistry Midterm Review Game

104 questions

Chemistry Midterm Review Game

quiz

Worksheet

•

10th Grade

HC07 Predicting Products - Single Replacement Reactions

107 questions

HC07 Predicting Products - Single Replacement Reactions

quiz

Worksheet

•

9th - 12th Grade

Unit 3 Review

106 questions

Unit 3 Review

quiz

Worksheet

•

10th Grade

Density

104 questions

Density

quiz

Worksheet

•

12th Grade

Covalent Bonding Test Review

108 questions

Covalent Bonding Test Review

quiz

Worksheet

•

10th - 12th Grade