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Quiz 4 - Ionization, Types of Bonds, Naming Compounds

Total questions: 161

Worksheet time: 3hrs 9mins

Name
Class
Date
1.

Valence electrons are those that are

a)

closest to the nucleus.

b)

freely floating between atoms.

c)

in the outermost energy level of the atom.

d)

unable to become involved in chemical bonding.

2.

Which of the following is not a way that ions can form?

a)

gaining electrons

b)

gaining protons

c)

losing electrons

d)

All of the above are ways that ions can form.

3.

Oxygen has six valence electrons. When forming an ion, oxygen will

a)

lose six electrons and have a charge of +6.

b)

lose six electrons and have a charge of -6.

c)

gain two electrons and have a charge is +2.

d)

gain two electrons and have a charge of -2.

4.

Look at the periodic table. What should be the charge on the ion formed by calcium?

a)

+1

b)

+2

c)

-1

d)

-2

5.

Atoms that have gained electrons form

a)

cations.

b)

anions.

c)

negions.

d)

positrons.

6.

Most elements are most stable when their outermost energy levels contain ________ electrons.

a)

2

b)

6

c)

8

d)

18

7.

Look at the Periodic table. Which of the following elements would you expect to form an ion that has the same charge as the oxide ion?

a)

calcium

b)

boron

c)

sulfur

d)

chlorine

8.

Which of the following elements is an exception to the octet rule?

a)

helium

b)

oxygen

c)

chlorine

d)

magnesium

9.

Which of the following tend to gain electrons when forming ions?

a)

metalloids

b)

metals

c)

nonmetals

d)

cations

10.

Anions have

a)

gained electrons.

b)

lost electrons.

c)

gained protons.

d)

lost protons.

11.

Which of the following groups on the Periodic Table will only form ions with positive charges?

a)

Group 2

b)

Group 15

c)

Group 17

d)

Group 18

12.

Atoms are electrically neutral when

a)

They have a minimal charge.

b)

They have a balanced number of protons and neutrons.

c)

They have a balanced number of protons and electrons.

d)

They have no valance electrons.

13.

If an electron is removed, an ion becomes

a)

An atom

b)

Positive

c)

Negative

d)

Neutral

14.

If an ion gains an electron, it becomes

a)

Positive

b)

Stable

c)

Atomic

d)

Negative

15.

Cations have what type of charge?

a)

Positive

b)

Negative

16.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

17.

What is the atomic number of Barium, Ba? (enlarge the periodic table)

a)

20

b)

38

c)

56

d)

88

18.

How many protons are in a sodium atom, Na? (tap to enlarge the periodic table)

a)

Sodium has 1 proton.

b)

Sodium has 3 protons.

c)

Sodium has 11 protons

19.

Atoms of the same element which have a different number of neutrons are called _________________.

a)

ions

b)

isotopes

c)

quarks

d)

molecules

20.

Which subatomic particle has a negative charge in the atom?

a)

proton

b)

neutron

c)

electron

d)

quark

21.

ALL atoms of the same element have:

a)

same number of proton

b)

same number of nucleon

c)

different number of neutron

d)

different number of electron

22.
Which subatomic particles contribute the most to the mass of an atom?
a)
Protons, Neutrons, Electrons
b)
Protons only
c)
Protons and Electrons
d)
Protons and Neutrons
23.
The number of protons is equal to 
a)
the atomic number
b)
the number of neutrons
c)
the energy levels
d)
the periodic table groups
24.
Oxygen has 8 protons. What is oxygen's atomic number?
a)
16
b)
8
c)
15.999
d)
0
25.

What is the charge on a lithium atom that loses 1 electron?

a)

+1

b)

0

c)

-1

d)

-2

26.

What is the atomic number of Fe? (click to see image)

a)

26

b)

55.845

c)

56

d)

30

27.

Valence electrons are in the...

a)

Innermost energy level of the atom.

b)

Middle energy level of the atom.

c)

Outermost energy level of the atom.

d)

energy levels of the atom.

28.

How many valence electrons does Helium have?

a)

1

b)

2

c)

3

d)

4

e)

5

29.
What is an ion?
a)
A Charged Atom
b)
A Large Atom
c)
A Small Atom
d)
A Cute Atom
30.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
31.

What is the charge of a sodium ion?

a)

+2

b)

+1

c)

-1

d)

-2

32.
Group 17 always has ions with a charge of 
a)
+1
b)
+2
c)
-1
d)
-2
33.
What charge will an Oxygen ion have? 
a)
+1
b)
-1
c)
+2
d)
-2
34.
If an element has 3 valence electrons, what charge will likely form on its ion ?
a)
+3
b)
+5
c)
-3
d)
-5
35.
Which of the following has a -3 charge?
a)
Boron
b)
Fluorine
c)
Nitrogen
d)
Neon
36.
charge of lithium ion
a)
-2
b)
-1
c)
+1
d)
+2
37.
charge of beryllium ion
a)
-2
b)
-1
c)
+1
d)
+2
38.
Which of the following has a -1 charge? 
a)
Aluminum
b)
Bromine
c)
Calcium
d)
Potassium
39.
Elements on the LEFT side of the periodic table will most likely form:
a)
Positive ions
b)
Negative ions
c)
Neutral Ions
d)
None of these
40.
Cations are...
a)
Positive
b)
Negative
c)
Neutral
d)
Purring
41.
Anions are...
a)
Positive
b)
Negative
c)
Neutral
d)
Crying
42.
An atom becomes _______ when it loses electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
43.
Which particles change the charge in atoms when ions are formed?
a)
Protons
b)
Electrons
c)
Neutrons
d)
Kittens
44.

How many electrons would a Nitrogen ion gain/lose? If it has 5 valence electrons.

a)

lose 5

b)

gain 5

c)

lose 3

d)

gain 3

45.

What is a negative ion called?

a)

anion

b)

cation

c)

covalent

d)

isotope

46.

What is the ion formed from Sulfur? If it has 6 valence electrons.

a)

S+2

b)

S-2

c)

S+6

d)

S-6

47.

How many electrons would a Calcium ion gain/lose? If it has 2 valence electrons.

a)

lose 1

b)

gain 1

c)

lose 2

d)

gain 2

48.

If an atom loses electrons, the charge will be positive.

a)

true

b)

false

49.

A Bromine ion gains 1 electron, which of the following is the correct symbol for a Bromine ion?

a)

Br-1

b)

Br+1

c)

Br+7

d)

Br-7

50.
What is the charge of an atom that has lost one electron?
a)
-1
b)
-2
c)
+1
d)
+2
51.

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

a)

+2

b)

-2

c)

+3

d)

0

52.

If an element has 3 valence electrons, what charge will likely form on its ion ?

a)

+3

b)

+5

c)

-3

d)

-5

53.
Ions are: 
a)
atoms with a positive or negative charge
b)
atoms with no charge
c)
atoms with ONLY a positive charge
d)
atoms with ONLY a negative charge
54.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 nonmetals
c)
metal
d)
none of the above
55.
What elements generally make a covalent bond?
a)
metal and nonmetal
b)
2 nonmetals
c)
metal
d)
none of the above
56.
In chemical compounds, covalent bonds form when
a)
the electronegativity difference between two atoms is very large.
b)
electrons are completely transferred between two metals.
c)
pairs of electrons are shared between two nonmetal atoms.
d)
two nonmetal atoms are attracted to each other by opposite charges.
57.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
58.
Predict the bond that will form between Se and Cl
a)
Ionic
b)
Covalent
59.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
60.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
61.
What happens when an atom loses an electron?
a)
It becomes Negatively Charged
b)
It remains neutral because the proton also leaves.
c)
It becomes Positively Charged
d)
It stays the same.
62.
The number of _____ is most important in determining how an atoms will bond. 
a)
Neutrons
b)
Protons
c)
Valence Electrons
d)
Electron sin the innermost shell
63.
If an oxygen atom has 8 protons (+) and 10 electrons (-), what is it's charge?
a)
O10-
b)
O8+
c)
O2-
d)
O10+
64.
Soluble in Water
a)
Ionic
b)
Covalent
65.
High Melting & Boiling Points
a)
Ionic
b)
Covalent
66.

Which of the following types of elements can exist in monatomic form?

a)

alkali metals

b)

transition metals

c)

halogens

d)

noble gases

67.
Why do bonds form?
a)
To fill the valence shell of electrons for the elements involved
b)
to release energy stored in the bonds
c)
because whenever you mix two chemicals, there will be a reaction
d)
because of attraction
68.
A substance which has a high melting point, conducts electricity when dissolved in water, and has a crystalline structure probably has what type of bond?
a)
Ionic
b)
Metallic
c)
Covalent
d)
Crystalline
69.

Bonds formed by transferring electrons from one atom to another are

a)

ionic

b)

metallic

c)

non polar covalent

d)

covalent

70.

Bonds formed by sharing electrons between atoms are

a)

ionic

b)

metallic

c)

covalent

d)

dipole-dipole

71.

A compound is made of two nonmetals. It is

a)

ionic

b)

metallic

c)

covalent

72.

A compound forms between a metal and a nonmetal. It is

a)

ionic

b)

metallic

c)

covalent

73.

A compound that is a poor conductor and has low melting and boiling points is most likely

a)

ionic

b)

metallic

c)

covalent

74.

Which compound would have a very low melting point?

a)

sodium chloride

b)

copper (II) sulfate

c)

sulfur dioxide

d)

aluminum

75.

Which solid would be a good conductor?

a)

sodium chloride

b)

copper (II) sulfate

c)

glucose

d)

aluminum

76.

An interaction that holds two atoms together called?

a)

Chemical Bond

b)

Covalent Bond

c)

Ionic Bond

d)

Metallic Bond

77.

Valence electrons are

a)

neutral (no charge)

b)

found in the outer most energy level of the atom

c)

equal to the number of protons

78.
How many valence electrons in this structure?
a)
6
b)
5
c)
4
d)
7
79.
How many more electrons are needed to fill an outermost energy level of a Carbon atom?
a)
its already full, 0 needed
b)
2
c)
4
d)
carbon is a nonmetal, it has no electrons
80.
Which of the following has a full valence shell?
a)
Oxygen
b)
Neon
c)
Barium
d)
Carbon
81.
Which elements are least likely to react with other elements?
a)
metals
b)
nonmetals
c)
noble gases
d)
transition elements
82.

2. Ionic Bonding involves:

a)

The transfer of protons

b)

The transfer of neutrons

c)

The transfer of electrons

d)

None Of the above

83.

Ionic bonding is between a

a)

nonmetal and nonmetal

b)

metal and nonmetal

c)

metal and metal

d)

Depends on the situation

84.

5. What happens when the sodium atom loses an electron?

a)

It become negatively charged

b)

It become positively charged

c)

none

85.

Which bond does this picture best represent?

a)

Metallic bond

b)

ionic bond

c)

covalent bond

d)

James Bond

86.
A bond formed from shared electrons is -
a)
Chemical bond
b)
Ionic bond
c)
Metallic bond
d)
Covalent bond
87.

Which type of bond occurs between non metals?

a)

covalent bonds

b)

ionic bonds

c)

metallic bonds

d)

all types of bonds

88.
Which type of bond has an equal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
89.

The most electronegative element is

a)

Chlorine

b)

Fluorine

c)

Iodine

d)

Sodium

90.

What do atoms that form positive ions tend to do?

a)

tend to lose electrons

b)

tend to lose protons

c)

tend to gain electrons

d)

tend to gain protons

91.

What elements generally compose a covalent bond?

a)

metal and nonmetal

b)

2 or more nonmetals

c)

metal

d)

none of the above

92.

Magnesium Bromide is a (an) ________ compound

a)

metallic

b)

covalent

c)

ionic

d)

organic

93.

How is the bond in F2 different from the bond in KCl ?

a)

F2 is covalent and KCl is ionic

b)

F2 is ionic and KCl is covalent

c)

F2 is ionic and KCl is ionic

d)

F2 is ionic and KCl is ionic

94.

When naming COVALENT/MOLECULAR compounds, you use ______ to indicate the amount of each element in the name.

a)

prefixes

b)

coefficients

c)

subscripts

d)

superscripts

95.

Phosphorous trichloride

a)

PCl3

b)

P3Cl

c)

P3Cl3

d)

PCl

96.

The formula for the ionic compound of magnesium and nitrogen would be

a)

MgN2

b)

MgN

c)

Mg3N2

d)

MgN3

97.

What is the formula for magnesium phosphide?

a)

Mg3P2

b)

Mg2P3

c)

Mg2PO4

d)

Mg3(PO4)2

98.

What is the chemical name for NI3 ?

a)

Nitrogen hydroxide

b)

Nitrogen trinitride

c)

Nitrogen triiodide

d)

Triiodide mononitrogen

99.
The bond between Na & F.   Ionic or covalent?
a)
Ionic
b)
Covalent
100.
What type of bond forms when electrons are transferred from one atom to another?
a)
ionic bond
b)
atomic bond
c)
covalent bond
d)
metallic bond
101.
Which of the following gives the correct chemical formula for the compound Calcium Nitride?
a)
Ca2N3
b)
CaN
c)
Ca3N2
d)
CaN2
102.
Which of the following gives the correct chemical formula for the compound Dinitrogen Monoxide?
a)
NO
b)
N2O
c)
N2O2
d)
O2N2
103.
What is the correct chemical name for the ionic compound:  Na2O
a)
Sodium oxide
b)
Sodium (II) oxide
c)
Disodium monoxide
d)
Disodium oxide
104.
What is the correct chemical name for the ionic compound: Fe3N2
a)
Iron nitride
b)
Iron (III) nitride
c)
Iron (II) nitride
d)
TriIron dinitride
105.
What is the correct chemical name for the ionic compound: CuS
a)
copper sulfide
b)
copper (I) sulfide
c)
copper (II) sulfide
d)
copper monosulfide
106.
What is the correct chemical name for the molecular compound:  CS2
a)
Carbon Sulfide
b)
Carbon diSulfide
c)
diCarbide diSulfide
d)
Carbon (II) Sulfide
107.
What is the correct chemical name for the molecular compound:  SF4
a)
Sulfur Fluoride
b)
Sulfur TetraFluoride
c)
TetraSulfide Fluoride
d)
Sulfur (IV) Fluoride
108.
What type of atoms make a covalent bond?
a)
only Nonmetals
b)
Metal and a Nonmetal
c)
only Metals
d)
only Noble Gases
109.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
110.
What type of compound is CaF2?
a)
covalent
b)
ionic
c)
polar
d)
metallic
111.
Given the picture, what type of bond is  holding the atoms together in this molecule?
a)
polar covalent bond
b)
nonpolar covalent bond
c)
ionic bond
d)
metallic bond
112.

what is the name of CCl4?

a)

carbon tetrachloride

b)

monocarbon tetrachloride

c)

tetracarbon monochloride

d)

carbon chloride

113.

What is the name of the compound SO2

a)

Monosulfate oxide

b)

Sulfur Dioxide

c)

Monosulfur dioxide

114.

What is the name of the compound P2O5

a)

Pentaphosphorus dioxide

b)

Phoshphide dioxide

c)

Diphosphorus pentoxide

115.

What is the name for MgF2 ?

a)

magnesium fluoride

b)

manganese Phosphide

c)

magnesium(III) fluoride

d)

magnesium fluoride(II)

116.

Name Al2S3

a)

Aluminum sulfide

b)

Dialuminum trisulfide

c)

ammonium sulfide

d)

aluminum (II) sulfice

117.

Name the compound CuO

a)

copper (II) oxide

b)

copper oxide

c)

copper (I) oxide

d)

carbon uranium oxide

118.

Ionic or covalent?

CaCl2

a)

ionic

b)

covalent

119.

Ionic or covalent?

CH4

a)

covalent

b)

ionic

120.

Ionic or covalent?

NH4Cl

a)

ionic

b)

covalent

121.

Ionic or covalent?

NH3

a)

ionic

b)

covalent

122.
Name the following compound: SnO2
a)
tin(II) oxide
b)
tin(IV)oxide
c)
tin(II)oxygen 
d)
tin oxide
123.
What kind of bond forms between a cation and an anion?
a)
Chemical bond
b)
Ionic bond
c)
Covalent bond
d)
Electron bond
124.
Name the following ionic compound: FeCl3
a)
iron chloride
b)
iron (III) chloride
c)
iron chlorate
d)
iron (III) chlorate
125.
Name the following ionic compound: Cs2S
a)
cesium sulfide
b)
cesium sulfate
c)
cesium (II) sulfate
d)
cesium (II) sulfide
126.
The name of Mg₃N₂ is
a)
manganese nitride
b)
magnesium nitride
c)
magnesium (III) nitride
d)
trimagnesium dinitride
127.

The correct name for LiCl is _______.

a)

lithium monochloride

b)

lithium(I) chloride

c)

monolithium chloride

d)

lithium chloride

e)

monolithium monochloride

128.

The correct name for FeO is _____.

a)

iron oxide

b)

iron (II) oxide

c)

iron (III) oxide

d)

iron (IV) oxide

e)

iron (I) oxide

129.

The symbol for the rubidium ion is

a)

Rb2+

b)

R+

c)

R2+

d)

Ru

e)

Rb+

130.

Which of the following is not the correct

combination of compound name and its formula?

a)

hydrobromic acid; HBr

b)

calcium sulfate; CaSO4

c)

beryllium oxide; BeO

d)

nickel(II) peroxide; Ni2O

e)

ammonium chromate; (NH4)2CrO4

131.

Titanium(IV) oxide has the formula

a)

Ti4O

b)

TiO4

c)

Ti(IV)O

d)

TiO2

e)

Ti4O2

132.

Which of the following formulas is

incorrect?

a)

CaNO3

b)

MgS

c)

AlBr3

d)

Li2O

e)

NaOH

133.

The correct name for P2O5 is

a)

phosphorus(II) oxide

b)

phosphorus(V) oxide

c)

diphosphorus oxide

d)

diphosphorus pentoxide

e)

phosphorus pentoxide

134.

The carbonate ion has the formula CO32–.

Which of the following is the correct formula

for sodium carbonate?

a)

Na(CO3)2

b)

Na2(CO3)2

c)

Na2CO3

d)

Na3(CO)2

e)

NaCO3

135.

The substance ClO3– is best described as

a)

a molecule

b)

a polyatomic ion

c)

a polyatomic molecule

d)

a mixture

136.

Potassium chlorate has the formula

a)

KCl

b)

KClO

c)

KClO2

d)

KClO3

e)

KClO4

137.

The name for Al(OH)3 is

a)

aluminum(III) hydroxide

b)

aluminum trihydroxide

c)

aluminum hydroxide

d)

monaluminum trihydroxide

e)

aluminum(I) hydroxide

138.
The prefix for 4 is?
a)
quatro
b)
tetra
c)
quarto
d)
tri
139.
What is the prefix for 3?
a)
tre
b)
drei
c)
tetra
d)
tri
140.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
141.
What is the prefix for 6?
a)
hepta
b)
ses
c)
hexa
d)
sieta
142.
7's prefix is
a)
hepta
b)
sieta
c)
hexa
d)
hoho
143.
What is the prefix for nine?
a)
nina
b)
nona
c)
nuevo
d)
nuna
144.
The prefix for 10 is?
a)
deca
b)
diaz
c)
dozen
d)
tena
145.
BrO3
a)
bromine oxide
b)
monobromine trioxide
c)
bromine trioxide
d)
bromine (III) oxide
146.
Phosphorous trichloride
a)
PCl3
b)
P3Cl
c)
P3Cl3
d)
PCL
147.
Disulfur trioxide
a)
S3O2
b)
SO
c)
S2O3
d)
S2O
148.
P2O5
a)
Phosphorus Oxide
b)
Pentaphosphorus Dioxide
c)
Diphosphorous pentoxide
d)
Phosphoric Oxygen
149.
SeF4
a)
Tetraselenium fluoride
b)
Selenium Fluoride
c)
Selenium tetraflouride
d)
Selenium (IV) Fluoride
150.

SiCl6

a)

Monosilicon hexachloride

b)

Silicon hexachloride

c)

Silicon heptachloride

d)

Monosilicon heptachloride

151.

What is the chemical formula for dinitrogen heptachloride?

a)

N2Cl7

b)

2N7Cl

c)

2NCl7

d)

N2Cl5

152.
Octanitrogen tetraoxide
a)
N8O3
b)
N7O3
c)
N8O3
d)
N8O4
153.

CS2

a)

monocarbon disulfide

b)

carbon bisulfide

c)

carbon disulfide

d)

carbon disulfer

e)

monocarbon sulfide

154.

SCl6

a)

sulfur hexachloride

b)

monosulfur hexachloride

c)

sulfide hexachloride

d)

sulfur heptachloride

e)

sulfur chloride

155.

P4H7

a)

tetraphosphorus heptahydrogide

b)

phosphorus heptahydride

c)

tetraphosphorus heptahydride

d)

tetraphosphorus hexahydride

e)

tetraphosphorus heptahydrogen

156.

P3N5

a)

phosphorus pentanitride

b)

triphosphorus pentanitrogen

c)

triphosphide pentanitrogen

d)

triphosphorus pentanitride

e)

phosphorus nitride

157.

Chemical reactions occur around us every day. Combustion of hydrocarbons releases the carbon stored in fossil fuels (e.g. coal, oil, natural gases) into the atmosphere as carbon dioxide gas. Which of the following equations represent this process?

a)

C4H10+ O2→CO2+ H2O

b)

CO2+ H2O → C6H12O6+ O2

c)

CaCO3+ HNO3 →Ca(NO3)2+ H2O + CO2

d)

NaHCO3+ HC2H3O2 → NaC2H3O2+ H2O + CO2

158.

Which type of reaction is represented by the following equation?

2KClO3 → 2KCl + 3O2

a)

synthesis

b)

decomposition

c)

single displacement

d)

double displacement

159.

What is the molecular formula of a compound that has an empirical formula of C2H5 and a molecular mass of 87 grams/mole?
Hint: The molecular formula should have a molar mass = sum(atomic mass for each element x # atoms in the chemical formula), Empirical formulas are the simplest representation of a chemical formula. For example, H2O2 would be the molecular formula of Hydrogen Peroxide, but it would have an Empirical Formula of HO. For H2O2, Its molar mass would be 2(1.01 g/mol) + 2 (15.999 g/mol) ≈ 34.01 g/mol

a)

C2H5

b)

C4H10

c)

C6H15

d)

C8H20

160.

Element X is more reactive than lithium and magnesium but less reactive than potassium. Which element is most likely to be X?

a)

Na

b)

Rb

c)

Ca

d)

Be

161.

Aluminum reacts with a certain nonmetallic element to form a compound with the general formula AlX; where element X is a diatomic gas at room temperature. What is element X?

a)

Oxygen

b)

Fluorine

c)

Nitrogen

d)

Chlorine

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