wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Chemistry Regents review

Total questions: 192

Worksheet time: 6hrs 24mins

Name
Class
Date
1.

Using Table F, Al(OH)3 is _____

a)

Insoluble

b)

Soluble

2.

Using Table F, determine if Na2SO4 is _____

a)

Insoluble

b)

Soluble

3.

_____ describes the type of change and the chemical properties of the product and reactants.

a)

The equation represents a chemical change, with the product and reactants having different chemical properties.

b)

The equation represents a physical change, with the product and reactants having identical chemical properties.

c)

The equation represents a physical change, with the product and reactants having different chemical properties.

d)

The equation represents a chemical change, with the product and reactants having identical chemical properties.

4.

The bonds in BaO are best described as _____

a)

ionic because electrons are transferred

b)

covalent, because valence electrons are shared

c)

ionic, because valence electrons are shared

d)

covalent, because electrons are transferred

5.

The chemical name of PbO2 is _____

a)

Lead (IV) Oxide

b)

Lead (II) Oxide

c)

Lead Hydroxide

d)

Lead Oxide

6.

The chemical formula for ammonium sulfide is _____

a)

(NH4)2SO3

b)

(NH4)2S2O3

c)

(NH4)2SO4

d)

(NH4)2S

7.

The number 0.002040 has _____ significant figures.

a)

2

b)

3

c)

4

d)

6

8.

_____ is 78.5 rounded to one significant figure.

a)

80

b)

78.5

c)

70

d)

79

9.

All matter is made of _____

a)

compounds 

b)

electrons 

c)

atoms 

d)

energy 

10.

Rutherford's gold foil experiment demonstrated that _____

a)

alpha particles have a positive charge.

b)

there is a dense positively charged nucleus at the center of an atom.

c)

negative and positive charges are spread evenly throughout the atom.

d)

gold is not as dense as previously thought.

11.

(4G) The statement that is true concerning the reaction N(g) + N(g) --> N2(g) is: _____

a)

A bond is broken and energy is absorbed

b)

A bond is broken and energy is released

c)

A bond is formed and energy is absorbed

d)

A bond is formed and energy is released

12.

When chlorine reacts it wants to _____ electron.

a)

lose 2

b)

gain 1

c)

lose 1

d)

gain 2

13.

Ionization Energy is defined as _____

a)

The amount of energy given off when an electron returns to a ground state

b)

The smallest amount of energy possible to excite an electron to a higher energy level

c)

The energy required to remove one electron from a neutral atom

d)

The amount of energy in one photon

14.

During interval AB, what is happening to the kinetic energy? _____

a)

decreasing

b)

staying constant

c)

increasing

15.

During interval BC, the kinetic energy is _____

a)

staying constant

b)

increasing

c)

decreasing

16.

During interval BC, _____ is happening to the potential energy.

a)

decreasing

b)

staying constant

c)

increasing

17.

Which formula would you use to calculate the heat absorbed when ice is melted at its melting point?

a)
b)
c)
18.

Which formula would you use to calculate the heat absorbed when water is heated from 10°C to 20 °C?

a)
b)
c)
19.

_____ remains constant for atoms of the same element.

a)

number of nucleons

b)

number of neutrons

c)

atomic number

d)

mass number

20.

J.J. Thomson provided evidence that an atom contains _____

a)

has an overall positive charge

b)

contains negatively charged particles

c)

is the smallest particle of matter

d)

has an overall negative charge

21.

_____ are isotopes of the same element based on the information in the table.

a)

A and D

b)

X and Z

c)

X and D

d)

A and Z

22.

The number 0.002040 has _____ significant figures.

a)

4

b)

6

c)

2

d)

3

23.

Determine the number of Significant Figures in _____.

a)

1

b)

4

c)

3

d)

2

24.

If more heat is supplied to the system, the particles would _____

a)

They would stop moving

b)

They would slow down

c)

There would be no effect

d)

They would speed up

25.

Heat will flow from the warmer object to the cooler one UNTIL _____ if two objects have different temperatures when they come in contact.

a)

one runs out of energy

b)

they both have an equal temperature

c)

one reaches a temperature of zero

26.

The SI unit of energy and heat is _____.

a)

watt

b)

joule

c)

calorie

d)

heat

27.

1. The most polar molecule among the following is _____

a)

H − Br

b)

H − F

c)

H − I

d)

H − Cl

28.

_____ is the most ionic compound.

a)

CF4

b)

LiF4

c)

HF

d)

KF

29.

_____ correctly lists the molecule and its type of bond.

a)

NaI Coordinate covalent bond

b)

CH4 Polar covalent bond

c)

CaO Ionic bond

d)

Br2 Polar covalent bond

30.

The type of bond is _____

a)

Nonpolar covalent

b)

Pure covalent

c)

Polar covalent

d)

Ionic

31.

This particle has no charge and is found in the nucleus: _____

a)

Proton

b)

Electron

c)

Neutron

32.

This positively charged particle located in the nucleus is _____

a)

Neutron

b)

Proton

c)

Electron

33.

This is a particle found outside the nucleus that has a _____ charge

a)

Neutron

b)

Proton

c)

Electron

34.

Most of an atom's mass is contained in _____

a)

Electron Cloud

b)

Electron

c)

Nucleus

35.

Rutherford's gold foil experiment provided evidence that _____

a)

gold is not a dense as previously thought.

b)

there is a dense positively charged nucleus at the center of an atom.

c)

negative and positive charges are spread evenly throughout the atom.

d)

alpha particles have a positive charge.

36.

The overall charge of an atom is _____.

a)

neutral 

b)

positive 

c)

negative 

d)

depends

37.

_____ are found in the nucleus of an atom.

a)

Neutrinos and positrons

b)

Protons and neutrons

c)

Electrons and neutrons

d)

DNA and RNA

38.

True or False: Empty space makes up the majority of an atom _____

a)

True

b)

False

39.

_____ contributes almost no mass to an atom.

a)

neutrons

b)

protons and neutrons

c)

electrons

d)

protons

40.

The majority of an atom's mass exists _____

a)

In the electron cloud

b)

In the space between the nucleus and the electrons

c)

In the neutrons

d)

In the nucleus

41.

_____ is responsible for the chemical properties of an atom.

a)

Nucleus

b)

Protons

c)

Neutron

d)

Valence Electrons

42.

Neon has an atomic number of 10 and an atomic mass of 20.180.  It will have _____ protons, _____ electrons, and _____ neutrons.

a)

P=10  E=5  N=5

b)

P=10  E=10  N=10

c)

P=5  E=5  N=10

d)

P=10  E=10  N=11

43.

Given that the atomic number of Oxygen is 8, there are _____ protons in the atom

a)

the atom is decaying

b)

the atomic mass is less than 8

c)

the mass of the atom is 8

d)

there are 8 protons in the atom

44.

-183 oC to Kelvin is _____

a)

183 K

b)

83 K

c)

90 K

d)

-20 K

45.

Convert 100 K to Celsius: _____

a)

-173 o C

b)

273 o C

c)

373 0 C

d)

-273oC

46.

The SI base unit symbol for mass is _____

a)

lb

b)

mg

c)

kg

d)

g

47.

The unit symbol for temperature is _____

a)

F

b)

K

c)

cd

d)

C

48.

Convert 273 K to _____

a)

100oC

b)

50oC

c)

0oC

d)

-273oC

49.

Convert 5900 K to _____

a)

5627 oC

b)

6173 oC

50.

_____ is a property unique to gases.

a)

Expand to fill any container

b)

Assume the shape of their container

c)

Incompressible

d)

All of the above

51.

The method to convert Celsius to Kelvin is _____

a)

Subtract 273

b)

They are the same thing

c)

Add 273

d)

You can't convert those

52.

Endothermic reactions feel _____

a)

cold

b)

warm

53.
Exothermic reactions feel
a)
warm
b)
cold
54.
energy in endothermic reactions are
a)
released
b)
ended
c)
absorbed
55.
energy in exothermic reactions are
a)
released
b)
absorbed
56.
Heat is measured in 
a)
joules
b)
grams
c)
degrees celcius
57.

A covalent bond is formed when two atoms

a)

share an electron with each other.

b)

share one or more pairs of electrons with each other.

c)

gain electrons.

d)

gain and lose electrons.

58.

A single covalent bond involves the sharing of

a)

only one electron.

b)

two electrons.

c)

three electrons.

d)

a variable number of electrons, which depends on the bonding atoms.

59.

Use the table below to choose the pair of elements that will most likely have the least ionic character.

Element = Na

Electronegativity = 0.9

Element = O

Electronegativity = 3.5


Element = Cl

Electronegativity = 3.0


Element = H

Electronegativity = 2.1

a)

Na and Cl

b)

O and Cl

c)

H and O

d)

Na and O

60.
(4B) When sodium and fluorine atoms combine to produce the compound NaF, the ions formed have the same electron configuration as the atom(s) of
a)
Argon, only
b)
Neon, only
c)
Both argon and neon
d)
Neither argon nor neon
61.
(4G) Which statement is true concerning the reaction: 
N(g) + N(g) --> N2(g)
a)
A bond is formed and energy is released
b)
A bond is formed and energy is absorbed
c)
A bond is broken and energy is released
d)
A bond is broken and energy is absorbed
62.
(4G) When a bond is broken in compounds, energy is generally
a)
released, and the reaction is exothermic
b)
released, and the reaction is endothermic
c)
absorbed, and the reaction is exothermic
d)
absorbed, and the reaction is endothermic
63.
(4G) Given the balanced equation representing a reaction:
Cl2(g) + energy --> Cl + Cl
Describe energy change during this reaction
a)
Energy is released as a bond is formed
b)
Energy is absorbed as a bond is formed
c)
Energy is released as a bond is broken
d)
Energy is absorbed as a bond is broken
64.
(4C) In which pair of elements will electrons be transferred from one another?
a)
H to O
b)
Li to Cl
c)
N to F
d)
H to C
65.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

66.

How many valence electrons should Lithium have in its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

67.

This is a correct dot diagram for nitrogen (N)

a)

true

b)

false

68.

Which is the correct Lewis Dot Structure for H2S?

a)
b)
c)
69.

Which is the correct Lewis Dot Structure for NH3?

a)
b)
c)
70.
When chlorine reacts it wants to ______________ electron.
a)
gain 1
b)
lose 1
c)
gain 2
d)
lose 2
71.
When Aluminum forms an ionic compound then it will ________________ electron(s).
a)
gain 1
b)
gain 2 
c)
gain 3
d)
lose 3 
72.
Traveling down a family the atomic radii ______________.
a)
Increases
b)
Decreases
c)
Stays the same
73.
Traveling across a period the atomic radii ______________.
a)
Increases
b)
Decreases
c)
Stays the same
74.
How does ionization energy change as I go across a period ?
a)
It doesn't
b)
It increases
c)
It decreases
75.
How does ionization energy change as I go down a family?
a)
It doesn't
b)
It increases
c)
It decreases
76.
Each element wants to gain or lose electrons so that it can have the same electron configuration as......
a)
a Nobel gas
b)
other elements in its family
c)
other elements in its period
d)
it used to have before reacting
77.
Most elements will gain or lose electrons so that they end up with _______ valence electrons.
a)
2
b)
6
c)
8
d)
10
78.
Ionization Energy is defined as.....
a)
The smallest amount of energy possible to excite an electron to a higher energy level
b)
The amount of energy given off when an electron returns to a ground state
c)
The amount of energy in one photon
d)
The energy required to remove one electron from a neutral atom
79.
How many valence electrons does Helium have?
a)
1
b)
2
c)
8
80.
When Nitrogen reacts with sodium, then _______nitrogen takes _____________.
a)
2 N takes 1 N from each sodium
b)
3 Nitrogen takes 2 electrons from each of 3 sodium
c)
1N takes 1 electron from each of 3 sodium
d)
1 N takes 2 electrons from each sodium
81.
When electrons are swapped or traded then ______________ bonds are formed.
a)
Ionic
b)
Covalent
c)
double
d)
single
82.
When electrons are shared then ____________ bonds / compounds are formed.
a)
Ionic
b)
Covalent
c)
single
d)
double
83.
A anion will be a ____ ion.
a)
negative
b)
positive
84.
A cation is a ____ ion.
a)
negative
b)
positive
85.

In a ___ bond, the atoms share electrons equally because of no difference in electronegativity.

a)

polar covalent

b)

nonpolar covalent

c)

ionic

86.
When writing Lewis Structures, only __________ electrons are used.
a)
Inner shell
b)
Core 
c)
Valence
d)
Stable
87.
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
88.
Is wood burning a physical or chemical change?
a)
Physical 
b)
Chemical
89.

A phase change is a...

a)

physical change

b)

chemical change

90.

During which phase change does a substance absorb energy?

a)

freezing

b)

condensation

c)

evaporation

d)

deposition

91.

During which phase change does a substance release energy?

a)

condensation

b)

evaporation

c)

melting

d)

sublimation

92.

Which phase change is endothermic?

a)

condensation

b)

deposition

c)

melting

d)

freezing

93.

What is happening to the kinetic energy at interval AB?

a)

increasing

b)

decreasing

c)

staying constant

94.

What is happening to the potential energy at interval AB?

a)

increasing

b)

decreasing

c)

staying constant

95.

What is happening to the kinetic energy at interval BC?

a)

increasing

b)

decreasing

c)

staying constant

96.

What is happening to the potential energy at interval BC?

a)

increasing

b)

decreasing

c)

staying constant

97.

Which particle diagram shows a solid?

a)
b)
c)
98.

When particles of a substance move faster, their kinetic energy...

a)

increases

b)

decreases

c)

stays constant

99.

When temperature increases, kinetic energy...

a)

increases

b)

decreases

c)

stays constant

100.

At what time interval is the substance melting?

a)

AB

b)

BC

c)

CD

d)

DE

101.

At what time interval is the substance evaporating?

a)

AB

b)

BC

c)

CD

d)

DE

102.

Which particle diagram shows a liquid?

a)
b)
c)
103.

Which particle diagram shows a gas?

a)
b)
c)
104.

Which formula would you use to calculate the heat absorbed when ice is melted at its melting point?

a)
b)
c)
105.

Which formula would you use to calculate the heat absorbed when water is heated from 10°C to 20 °C?

a)
b)
c)
106.

Which formula would you use to calculate the heat absorbed when water is boiled at 100°C?

a)
b)
c)
107.

Which formula would you use to calculate the heat released when water is frozen at 0°C?

a)
b)
c)
108.

Which formula would you use to calculate the heat released when water vapor condenses to a liquid?

a)
b)
c)
109.

How much heat is released when 20.0 grams of water is cooled from 65°C to 55°C?

a)

300 J

b)

836 J

c)

6,680 J

d)

10,800 J

110.

How much heat is required to completely vaporize a 37 gram sample of water at its boiling point of 100°C?

a)

370 J

b)

3,700 J

c)

12,358 J

d)

83,620 J

111.

The temperature of a sample of water changes from 55°C to 77°C when the sample absorbs 1,103.5 joules of heat. What is the mass of the sample?

a)

7 grams

b)

12 grams

c)

50 grams

d)

72 grams

112.

A 25-gram sample of H2O(l) at 25°C absorbs 731.5 joules of heat. What will be the final temperature of the water?

a)

32°C

b)

21.8°C

c)

-18°C

d)

7°C

113.

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

114.

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

115.

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

a)

proton

b)

hydrogen nucleus

c)

neutron

d)

electron

116.

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

117.

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

a)

nitrogen

b)

oxygen

c)

fluorine

d)

neon

118.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

119.
subatomic particles found on the outermost shell & responsible for the atom's reactivity
a)
neutrons
b)
valence electrons
c)
isotopes
d)
ions
120.

Measure mainly of the nuclear particles: protons + neutrons

a)

Subatomic Particles

b)

Atomic Number

c)

Mass Number

d)

Gluons

121.
Subatomic particles that are neutral in charge
a)
Neutrons
b)
Protons
c)
Nucleus 
d)
Electrons
122.
The smallest particle of an element that shows all the properties of that element.
a)
Subatomic Particles
b)
Atom
c)
Quarks
d)
Gluons
123.
Rutherford's gold foil experiment provided evidence that...
a)
negative and positive charges are spread evenly throughout the atom.
b)
alpha particles have a positive charge.
c)
gold is not a dense as previously thought.
d)
there is a dense positively charged nucleus at the center of an atom.
124.
J.J. Thomson provided evidence that an atom...
a)
is the smallest particle of matter
b)
contains negatively charged particles
c)
has an overall negative charge
d)
has an overall positive charge
125.

According to the wave-mechanical model of the atom, an orbital is a region of the most probable location of

a)

an alpha particle

b)

a gamma ray

c)

an electron

d)

a proton

126.

Which particles have approximately the same mass?

a)

an electron and an alpha particle

b)

an electron and a proton

c)

a neutron and an alpha particle

d)

a neutron and a proton

127.

Compared to the energy and charge of the electrons in the first shell of a Be atom, the electrons in the second shell of this atom have

a)

less energy and the same charge

b)

less energy and a different charge

c)

more energy and the same charge

d)

more energy and a different charge

128.
A tiny but very dense, positively charged portion of the atom that holds most of the atomic mass
a)
Electron Shells
b)
Orbitals
c)
Electron Cloud
d)
Nucleus
129.
Calculation used to find the number of neutrons in an atom
a)
Atomic Mass - Atomic Number
b)
Atomic Number - Atomic Mass
c)
Atomic Mass - Electrons
d)
none of these
130.

Based on the information in the table, which two atoms are isotopes of the same element?

a)

A and D

b)

A and Z

c)

X and D

d)

X and Z

131.

What is the structure of a krypton-85 atom?

a)

49 electrons, 49 protons, and 85 neutrons

b)

49 electrons, 49 protons, and 49 neutrons

c)

36 electrons, 36 protons, and 85 neutrons

d)

36 electrons, 36 protons, and 49 neutrons

132.

The nucleus of an atom of cobalt-58 contains

a)

27 protons and 31 neutrons

b)

27 protons and 32 neutrons

c)

59 protons and 60 neutrons

d)

60 protons and 60 neutrons

133.

Which two notations represent different isotopes of the same element?

a)
b)
c)
d)
134.

Which statement best explains why most atomic masses on the Periodic Table are decimal numbers?

a)

Atomic masses are determined relative to an H–1 standard.

b)

Atomic masses are determined relative to an O–16 standard.

c)

Atomic masses are a weighted average of the naturally occurring isotopes.

d)

Atomic masses are an estimated average of the artificially produced isotopes.

135.

Based on the information in the table, which numerical setup can be used to calculate the atomic mass of the element bromine?

a)

(78.92 u)(50.69) + (80.92 u)(49.31)

b)

(78.92 u)(49.31) + (80.92 u)(50.69)

c)

(78.92 u)(0.5069) + (80.92 u)(0.4931)

d)

(78.92 u)(0.4931) + (80.92 u)(0.5069)

136.

If 75.0% of the isotopes of an element have a mass of 35.0 amu and 25.0% of the isotopes have a mass of 37.0 amu, what is the atomic mass of the element?

a)

37.0 amu

b)

35.5 amu

c)

36.0 amu

d)

35.0 amu

137.

The average isotopic mass of chlorine is 35.5. Which mixture of isotopes (shown as percents) produces this average mass?

a)

50% 12C and 50% 13C

b)

50% 35Cl and 50% 37Cl

c)

75% 12C and 25% 13C

d)

75% 35Cl and 25% 37Cl

138.

Location of an electron

a)

outside the nucleus

b)

inside the nucleus

139.

Charge of an electron

a)

negative charge

b)

positive charge

c)

neutral

140.

Why is an atom neutral?

a)

same number of protons and electron

b)

fewer neutrons than electrons

c)

more protons than electrons

141.
Valence electrons are the...
a)
Innermost electrons
b)
Middle electrons
c)
Outermost electrons
d)
Any electrons
142.

How many valence electrons does carbon have?

a)

4

b)

5

c)

6

d)

7

143.

USE THE PERIODIC TABLE

How many valence electrons does sodium have?

a)

1

b)

2

c)

3

d)

4

144.

USE THE PERIODIC TABLE

How many valence electrons does Phosphorus have?

a)

31

b)

5

c)

15

d)

4

145.

USE THE PERIODIC TABLE

How many valence electrons does Phosphorus have?

a)

31

b)

5

c)

15

d)

4

146.
How many electrons should Beryllium have around its Lewis dot model?
a)
1
b)
2
c)
3
d)
4
147.
How many electrons should Aluminium have around its Lewis dot model?
a)
1
b)
2
c)
3
d)
4
148.

Which of the following is the correct electron-dot diagram for an atom with an electron configuration of 2-8-18-5?

a)
b)
c)
d)
149.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

150.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
151.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Sodium

152.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Helium

153.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Sodium

154.

The diagram represents the bright-line spectra of four elements and a bright-line spectrum produced by a mixture of three of these elements. Which element is not present in the mixture?

a)

A

b)

D

c)

X

d)

Z

155.

Which energy level of Calcium has the most energy?

a)

1st

b)

2nd

c)

3rd

d)

4th

156.
Barium atoms want to form...
a)
an anion
b)
a cation
c)
an onion
d)
a cuddly kitten friend
157.
Cations are...
a)
Positive
b)
Negative
c)
Neutral
d)
Purring
158.
Anions are...
a)
Positive
b)
Negative
c)
Neutral
d)
Crying
159.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
160.
An atom becomes _______ when it loses electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
161.
What is a Rubidium ion's symbol?
a)
Rb-
b)
Rb+
c)
Rb-2
d)
Rb+2
162.

Which pair of atoms will form ionic bonds?

a)

S and F

b)

Mg and O

c)

F and Cl

d)

H and Ne

163.

How would you classify NaCl?

a)

element

b)

compound

c)

heterogeneous mixture

d)

homogeneous mixture

164.

How many electron pairs are shared between the atoms in an N2 molecule?

a)

1

b)

2

c)

3

d)

4

165.

As the elements in Group 2 in the periodic table are considered in order of increasing atomic number, there is a general increase in

a)

stability

b)

atomic radius

c)

electronegativity

d)

first ionization energy

166.

When iron is mixed with sulfur, the iron

a)

becomes a covalent compound

b)

retains its magnetic properties

c)

loses its magnetic properties

d)

transfers its magnetic properties to sulfur

167.

Which compound has both ionic and covalent bonds?

a)

CH4

b)

CO

c)

CaCl2

d)

MgSO4

168.

Which formula represents a polar molecule?

a)

Cl2

b)

CH4

c)

HCl

d)

CO2

169.

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

170.

What is the overall charge of an ion that has 9 protons, 11 neutrons, and 10 electrons?

a)

+1

b)

-1

c)

+2

d)

-2

171.

Which atom has the lowest electronegativity?

a)

Nitrogen

b)

Oxygen

c)

Fluorine

d)

Neon

172.

In a bond between an atom of hydrogen and an atom of chlorine, the hydrogen atom has a

a)

weaker attraction for electrons

b)

stronger attraction for electrons

c)

smaller number of first-shell atoms

d)

larger number of first-shell atoms

173.

Which elements have the most similar chemical properties?

a)

Ge, As, and Sb

b)

Mn, Fe, and Co

c)

S, Se, and Te

d)

P, S, and Cl

174.

Most elements on the periodic table are classified as ____________.

a)

Gases

b)

Metalloids

c)

Metals

d)

Nonmetals

175.

Which accurately describes nonmetals?

a)

Poor conductors of electricity

b)

Often used in computer parts

c)

Both malleable and ductile

d)

Both dull and brittle

176.

Groups on the periodic table are arranged...

a)

Vertically

b)

Horizontally

c)

Diagonally from bottom right corner

d)

Diagonally from top right corner

177.

Which group on the periodic table is the most reactive?

a)

Group 1

b)

Group 2

c)

Group 13

d)

Group 18

178.

How many Valance electrons does Iodine Have?

a)

6

b)

16

c)

7

d)

17

179.
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
180.
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.
181.

Electronegativity is

a)

How much an atom wants an electron

b)

How hard it is to remove an electron

c)

How many electrons an atom has

d)

How negative an electron is

182.

Ionization energy is

a)

The energy required gain an electron

b)

How hard it is to remove an electron

c)

The energy required to combine two elements

d)

None of the above

183.

What is the name of PbO2

a)

Lead Oxide

b)

Lead (II) Oxide

c)

Lead (IV) Oxide

d)

Lead Hydroxide

184.

Which element consists of positive ions immersed in a "sea" of mobile electrons?

a)

Sulfur

b)

Nitrogen

c)

Calcium

d)

Chlorine

185.

What is the chemical formula for sodium oxalate?

a)

NaO

b)

Na2O

c)

NaC2O4

d)

Na2C2O4

186.

What is the number of moles of CO2 in a 220.-gram sample of CO2 (gram-formula mass = 44 g/mol)?

a)

0.20 mol

b)

5.0 mol

c)

15 mol

d)

44 mol

187.

Which formula represents an asymmetrical molecule?

a)

CH4

b)

CO2

c)

N2

d)

NH3

188.

A measured value for the atomic radius of platinum atoms was determined to be 143 picometers. Based on Table S, what is the percent error of this measured value?

a)

0.10%

b)

9.1%

c)

10.%

d)

13%

189.

The results of these tests suggest that

a)

both solids contain only ionic bonds

b)

both solids contain only covalent bonds

c)

Solid A contains only covalent bonds and solid B contains only ionic bonds

d)

Solid A contains only ionic bonds and solid B contains only covalent bonds

190.

Which phrase describes the distribution of charge and the polarity of a CH4 molecule?

a)

symmetrical and polar

b)

symmetrical and nonpolar

c)

asymmetrical and polar

d)

asymmetrical and nonpolar

191.
What is the molar mass of Mg(NO3)2
a)
148.313g/mol
b)
134.306g/mol
c)
54.311g/mol
192.
Molar mass is in units of ________.
a)
grams
b)
grams/mole
c)
mole
d)
moles/gram

Similar Resources on Wayground

Class 10 - chemical reactions

188 questions

Class 10 - chemical reactions

quiz

Worksheet

•

10th Grade

10Chemistry Final Review

190 questions

10Chemistry Final Review

quiz

Worksheet

•

9th - 12th Grade

AP Chemistry Unit 3

193 questions

AP Chemistry Unit 3

quiz

Worksheet

•

10th Grade - University

Ionic and Covalent Bonding Quiz

193 questions

Ionic and Covalent Bonding Quiz

quiz

Worksheet

•

9th - 12th Grade

Element & Symbols (Flash Cards)

195 questions

Element & Symbols (Flash Cards)

quiz

Worksheet

•

9th - 12th Grade

AP Chem The Whole Enchilada Units 1-3

187 questions

AP Chem The Whole Enchilada Units 1-3

quiz

Worksheet

•

11th Grade

Revision Redox aftermidterm M5

192 questions

Revision Redox aftermidterm M5

quiz

Worksheet

•

9th - 12th Grade

chem final

191 questions

chem final

quiz

Worksheet

•

9th - 12th Grade