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Chemistry February Review

Total questions: 103

Worksheet time: 5hrs 7mins

Name
Class
Date
1.

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

2.

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

3.

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

a)

proton

b)

hydrogen nucleus

c)

neutron

d)

electron

4.

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

5.

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

6.

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

a)

nitrogen

b)

oxygen

c)

fluorine

d)

neon

7.

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

8.

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

9.
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
10.

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

11.

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

12.

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

13.

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

a)

Electrons

b)

Neutrons

c)

Protons

d)

Nucleus

14.

Which scientist discovered the electrons?

a)

Dalton

b)

Thomson

c)

Atristotle

d)

Bohr

15.

Rutherford and his students did experiments that showed

a)

quark

b)

nucleus

c)

proton

d)

electron

16.

Bohr discovered that electrons are located in

a)

the nucleus

b)

inside protons

c)

electron cloud

d)

circular orbits around the nucleus

17.
The most dangerous type of radiation is the ____. 
a)
alpha particle
b)
gamma ray
c)
beta particle
d)
uranium
18.

What is the charge of a neutron?

a)

+1

b)

-1

c)

0

d)

+2

19.

Which scientist is known for the discovery of the nucleus?

a)

Bohr

b)

Rutherford

c)

Thomson

d)

Dalton

20.

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

21.

The elements on the Periodic Table are arranged in

order of increasing

a)

atomic mass

b)

atomic number

c)

molar mass

d)

oxidation number

22.

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

23.

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

24.

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

25.

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

26.

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

27.

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)

28.

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

29.

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

30.

Which atom has the greatest attraction for the

electrons in a chemical bond?

a)

hydrogen

b)

oxygen

c)

silicon

d)

sulfur

31.

Which element is a noble gas?

a)

Argon

b)

chlorine

c)

hydrogen

d)

magnesium

32.

The element helium is classified as a

a)

metal

b)

metalloid

c)

noble gas

33.

An atom of which element has the largest atomic

radius?

a)

Fe

b)

Mg

c)

Si

d)

Zn

34.
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
35.
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 
36.
Negatively charged particles found outside of the nucleus are called
a)
electron
b)
protons
c)
neutrons
d)
nucleons
37.
Positively charged particles found in the nucleus of an atom are called
a)
protons
b)
neutrons
c)
electrons
d)
isotopes
38.

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

39.

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

40.

What is the atomic number of this atom?

a)

1

b)

3

c)

4

d)

7

41.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

42.

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

43.

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

44.

The bonds in BaO are best described as

a)

covalent, because valence electrons are shared

b)

covalent, because electrons are transferred

c)

ionic, because valence electrons are shared

d)

ionic because electrons are transferred

45.

Which property best accounts for the conductivity of metals?

a)

the relatively high first ionization energy

b)

the malleability of most metals

c)

the free electrons in the valence energy levels

d)

the filled inner electron energy levels

46.

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

47.

The bond between which two atoms is most polar?

a)

H-O

b)

F-F

c)

C-O

d)

N-H

48.

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

49.

Based on bond type, which compound has the highest melting point?

a)

CH3OH

b)

C6H14

c)

CaCl2

d)

CCl4

50.

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

a)

Sulfur

b)

Nitrogen

c)

Calcium

d)

Chlorine

51.

Which substance contains bonds that involved the transfer of electrons from one atom to another?

a)

KBr

b)

CO2

c)

Cl2

d)

NH3

52.

Which statement best describes the substance that results when electrons are transferred rom a metal to a nonmetal?

a)

It contains covalent bonds and has a high melting point

b)

It contains covalent bonds and has a low melting point

c)

It contains ionic bonds and has a low melting point

d)

It contains ionic bonds and has a high melting point

53.

A substance that does not conduct electricity as a solid but does conduct electricity when melted is most likely classified as

a)

an ionic compound

b)

a nonmetal

c)

a metal

d)

a molecular compound

54.

Which substance is an electrolyte?

a)

C6H12O6

b)

KOH

c)

H2O

d)

CH3OH

55.

A covalent bond forms when atoms

a)

share neutrons

b)

transfer electrons

c)

share electrons

d)

transfer neutrons

56.

How many valence electrons does nitrogen have?

a)

2

b)

3

c)

4

d)

5

57.

Look at the electron dot diagram in the picture. The electron in the bond between hydrogen and fluorine are more strongly attracted to the atom of

a)

hydrogen, which has the higher electronegativity

b)

hydrogen, which has the lower electronegativity

c)

fluorine, which has the higher electronegativity

d)

fluorine, which has the lower electronegativity

58.

The bond between a diatomic nitrogen molecule (N2) is best described as

a)

polar with a triple bond

b)

polar with a double bond

c)

nonpolar with a triple bond

d)

non polar with a double bond

59.
Which statement best describes the energy change as bonds are formed and broken in this reaction?
      H2 + Cl2  ➔  2HCl
a)
The forming of the H-Cl bond releases energy
b)
The forming of the H-Cl bond absorbs energy
c)
The breaking of the H-H bond releases energy
d)
The breaking of the Cl-Cl bond releases energy
60.
Is the molecule H2O polar or non-polar?
a)
polar
b)
non-polar
61.
Which type of bond has an equal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
62.
Which type of bond has an unequal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
63.
If an atom loses two electrons what charge will it have?
a)
+ 2
b)
 - 2
c)
+1
d)
-1
64.
If an atom gains one electron what charge will it have?
a)
-2
b)
-1
c)
+1
65.

As energy is released during the formation of a

bond, the stability of the chemical system generally

will

a)

decrease

b)

increase

c)

stay the same

66.

Which particles may be gained, lost, or shared

by an atom when it forms a chemical bond?

a)

protons

b)

nucleons

c)

electrons

d)

neutrons

67.

When a sodium atom reacts with a chlorine

atom to form a compound, the electron

configurations of the ions forming the compound

are the same as those in which noble gas atoms?

a)

krypton and neon

b)

krypton and argon

c)

neon and argon

d)

neon and helium

68.

Which is the correct electron-dot formula for

a molecule of chlorine?

a)
b)
c)
d)
69.
Blue Color: Chemical or Physical Property
a)
Chemical Property
b)
Physical Property
70.
The gram molecular mass of Ca3(PO4)2 is
a)
246 g
b)
279 g
c)
310 g
d)
342g
71.

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

a)

Soluble

b)

Insoluble

72.
What is the universal solvent?
a)
salt
b)
sugar
c)
water
d)
ice
73.

A mixture with more solute dissolved in the solvent than is usually soluble is called:

a)

concentrated

b)

supersaturated

c)

saturated

d)

unsaturated

74.

When you have added as much solute as can dissolve in the solvent, the solution is called:

a)

concentrated

b)

supersaturated

c)

saturated

d)

unsaturated

75.
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
76.
This is the part of a solution that dissolves
a)
Solute
b)
Solvent
c)
Solution
d)
Mixture 
77.
Kool-Aid - Powder, sugar, and water
Identify the solvent 
a)
water
b)
powder
c)
sugar
d)
powder and sugar
78.
salt water is a 
a)
compound
b)
element
c)
heterogeneous mixture
d)
solution
79.

Solubility refers to the ____ of solute that can dissolve in a certain volume or mass of solvent, at a certain temperature.

a)

Mean

b)

Range

c)

Amount

d)

Mode

80.
What does it mean to dilute a solution?
a)
lower the concentration of solute per solvent
b)
increase the concentration of solute per solvent
81.

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

82.

Which of the following is the correct formula for calculating molarity?

a)

moles/liters of solution

b)

moles/kg of solvent

c)

# particles/Avogadro's #

d)

theoretical yield/actual yield

83.
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
84.
What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?
a)
0.018 M
b)
0.0011 M
c)
1.052 M
d)
0.062 M
85.
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
86.

A dilution is when

a)

solute is added to the volume of solution

b)

water is added to the volume of solution

c)

solute is removed from the volume of solution

d)

water is removed from the volume of solution

87.

What volume, in milliliters, of 10.0 M NaOH is needed to prepare 300.0 mL of 2.00 M NaOH by dilution?

a)

0.067 mL

b)

60.0 mL

c)

100 mL

d)

125 mL

88.
How many mL of 10.8M HCl are required to make 100.0 mL of 3.00M acid?
a)
27.8 mL
b)
27.78 mL
c)
2.8 mL
d)
278 mL
89.

Based on Table S, an atom of which element has the strongest attraction for electrons in a chemical bond?

a)

Aluminum

b)

Chlorine

c)

Magnesium

d)

Sulfur

90.

Which diatomic molecule is formed when two atoms share six electrons?

a)

H2

b)

O2

c)

N2

d)

F2

91.

Which symbol represents an atom in the ground state with the most stable electron configuration?

a)

B

b)

O

c)

Li

d)

Ne

92.

Which compound has the least ionic character?

a)

KBr

b)

HF

c)

MgO

d)

BrCl

93.

The bonds in BaO are best described as

a)

covalent, because valence electrons are shared

b)

covalent, because electrons are transferred

c)

ionic, because valence electrons are shared

d)

ionic because electrons are transferred

94.

Which property best accounts for the conductivity of metals?

a)

the relatively high first ionization energy

b)

the malleability of most metals

c)

the free electrons in the valence energy levels

d)

the filled inner electron energy levels

95.

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

96.

The bond between which two atoms is most polar?

a)

H-O

b)

F-F

c)

C-O

d)

N-H

97.

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

98.

Based on bond type, which compound has the highest melting point?

a)

CH3OH

b)

C6H14

c)

CaCl2

d)

CCl4

99.

The liquids hexane and water are placed in a test tube. The test tube is stoppered, shaken, and placed in a test tube rack. The liquids separate into two distinct layers because hexane and water have different

a)

formula masses

b)

molecular polarities

c)

pH values

d)

specific heats

100.

What is the chemical formula for ammonium sulfide?

a)

(NH4)2S

b)

(NH4)2SO3

c)

(NH4)2SO4

d)

(NH4)2S2O3

101.

What is the name of PbO2

a)

Lead Oxide

b)

Lead (II) Oxide

c)

Lead (IV) Oxide

d)

Lead Hydroxide

102.

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

a)

Sulfur

b)

Nitrogen

c)

Calcium

d)

Chlorine

103.

Which formula represents a tetrahedral molecule?

a)

CH4

b)

CaCl2

c)

HBr

d)

Br2

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