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Unit 4 Review: Periodic table, Bonding , Nomenclature

Total questions: 142

Worksheet time: 3hrs 21mins

Name
Class
Date
1.

Which type of element typically loses electrons to form a bond?

a)

metal

b)

metalloid

c)

noble gas

d)

nonmetal

2.

Which pair of elements will MOST LIKELY form an ionic bond?

a)

neon and argon

b)

beryllium and lithium

c)

magnesium and sulfur

d)

phosphorus and oxygen

3.

The illustration depicts the formation of an ionic chemical bond between lithium and fluorine atoms. Why is the resulting compound more stable than the individual atoms?

a)

The shared electron from lithium to fluorine provides each atom with an empty electron shell.

b)

The transferred electron from lithium to fluorine provides each atom with a full outer energy level/ electron shell.

c)

The transfer of electrons from lithium to fluorine provides each atom with an empty electron shell.

4.

An atom or element that gains a valence electron(s) to be stable becomes a ________ ion.

(2)

a)

positive

b)

negative

c)

cation

d)

anion

5.
When electrons are shared a ________ bond is formed
a)
Ionic
b)
Covalent
c)
Metallic
6.
If atoms that are sharing electrons have an unequal attraction for the electrons it is a ____
a)
Ionic bond
b)
Nonpolar covalent bond
c)
Polar covalent bond
d)
Metallic bond
7.

Which part of the atom is responsible for chemical bonding?

a)

Core Electrons

b)

Valence Electrons

c)

Protons

d)

Neutrons

8.
A ____________ bond exists between a metal and a nonmetal.
a)
Ionic
b)
Covalent
9.
Metals form ions by _____________ electrons, nonmetals form ions by   ___________ electrons. 
a)
losing, gaining
b)
gaining, losing
c)
 losing, losing
d)
gaining, gaining
10.

What type of bonding is present in dinitrogen pentoxide, N2O5?

a)

ionic

b)

covalent

c)

metallic

d)

bionic

11.

How many valence electrons does an atom of phosphorus have?

a)

3

b)

2

c)

5

d)

8

12.
Electrons that are free to move in metals
a)
delocalized electrons
b)
oxidation number
c)
chemical bond
d)
salts
13.
Metallic bonding is...
a)
a type of covalent bond.
b)
a type of ionic bond.
c)
an attraction between positive ions and electrons.
14.

The following properties are all characteristics of ionic compounds EXCEPT

a)

high melting and boiling points

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

15.

What type of forces hold on an ionic lattice together?

a)

Electrostatic attraction forces

b)

Covalent bond

c)

Metallic bond

d)

Van der Waals forces

16.

What properties does an ionic compound have?

a)

A low boiling point and it conducts electricity when dissolved in water

b)

A high melting and it conducts electricity when liquid

c)

A high boiling point and it conducts electricity when solid

17.

Ionic compounds conduct electricity when dissolved in water. Which statement below best explains the property?

a)

Ions are free to move.

b)

Electrons are free to move.

c)

Bonds are strong.

d)

There are weak intermolecular forces of attraction.

18.

Some are solids, some are liquids, and some are gases at room temperature.

a)

ionic compounds

b)

molecular compounds

19.

When dissolved in water, the solution is a good conductor of electricity.

a)

ionic compounds

b)

molecular compounds

20.

When dissolved in water, the solution does NOT conduct electricity.

a)

ionic compounds

b)

molecular compounds

21.
Which of the following is a molecular compound?
a)
CaO
b)
NaCl
c)
CaCl2
d)
CH4
22.
If an atom becomes an ion with a 2+ charge, what does that mean?
a)
It has lost 2 electrons
b)
It has gained 2 electrons
c)
The atom is in period 2
d)
The atom has an atomic # of 2
23.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
24.
How do the following two elements bond together?
K1+  S2- 
a)
KS
b)
K8S
c)
K6S3
d)
K2S
25.
What is the formula for magnesium chloride?
a)
MgCl
b)
Mg2Cl
c)
MgCl2
d)
Mg(ClO3)2
26.
What is the formula for copper(I) sulfate?
a)
Cu(SO3)
b)
Cu(SO4)
c)
Cu2(SO3)
d)
Cu2(SO4)
27.
What is the element/ion symbol for Iron(III)?
a)
Fe
b)
Fe3+
c)
Fe3-
d)
Fe(III)
28.
What is the name of the compound Li(OH)?
a)
lithium hydrogen oxide
b)
lithium hydroxide
c)
lithium hydride
d)
lithium oxide hydride
29.

Name for NaH

a)

sodium hydrogen

b)

potassium hydride

c)

sodium hydride

d)

potassium hydrogen

30.

Formula for barium sulfide

a)

B2S3

b)

BaS

c)

Ba2S

d)

BaS2

31.

Name for Hg2S

a)

mercury (IV) sulfide

b)

mercury (III) sulfide

c)

mercury (II) sulfide

d)

mercury (I) sulfide

32.

Formula for lead (II) chloride

a)

PbCl2

b)

Pb2Cl

c)

Pb2Cl3

d)

Pb3Cl2

33.

Name for PBr2

a)

phosphorus bromide

b)

phosphorus dibromide

c)

phosphorus dibromine

d)

phosphorus bromine

34.

Formula for Disilicon Heptasulfide

a)

SiS6

b)

SiS7

c)

Si2S6

d)

Si2S7

35.

Name for SrBr2

a)

strontium bromine

b)

strontium bromide

c)

strontium dibromide

d)

strontium dibromine

36.

Formula for Cobalt (II) bromide

a)

CoBr

b)

Co2Br2

c)

Co2Br

d)

CoBr2

37.

What is the formula for diphosphorus pentoxide?

a)

P2O5

b)

PO5

c)

P5O2

d)

Po2O5

38.

What is the name of the compound with the formula Ba3P2?

a)

barium phosphide

b)

barium diphosphide

c)

tribarium diphosphide

d)

barium phosphorous

39.

What is the formula for phosphorous acid?

a)

H3PO4

b)

H2PO4

c)

H3P

d)

H3PO3

40.

What is the formula for nitric acid?

a)

HNO2

b)

HNO3

c)

HNO4

d)

H2NO3

41.

Name this acid with the formula HF

a)

hydrofluoric acid

b)

hypofluoric acid

c)

hydrogen fluorine acid

d)

fluoric acid

42.

What is the formula for hydrochloric acid?

a)

HCl

b)

HClO

c)

H3ClO3

d)

HClO3

43.
What is the formula for perchloric acid?
a)
H3ClO3
b)
H3ClO4
c)
HClO3
d)
HClO4
44.
HBr
a)
hydrogen bromine acid
b)
hydrobromide acid
c)
hydrobromic acid
45.

carbonic acid

a)

H2CO3

b)

H2CrO4

c)

H2C2O4

d)

HCO3

46.

Binary acids start with the prefix "____________"

a)

acid

b)

nitric

c)

hydraulic

d)

hydro

47.

When naming binary acids, the ending always changes to:

a)

-ate

b)

-ite

c)

-ic

d)

-ous

48.

When naming oxyacids, change "-ite" to:

a)

-ate

b)

-ic

c)

-ous

d)

-ite

49.

Name this acid: H2SO4

a)

hydrogen sulfate

b)

hydrosulfuric acid

c)

sulfuric acid

d)

sulfurous acid

50.

Name the acid that uses an acetate ion: HC2H3O2

a)

Acetic acid

b)

Acetous acid

c)

Hydrogen Acetate acid

d)

Hydrogen Acetatic acid

51.
What is the name of NH4Cl?
a)
nitrogen tetrahydrogen chloride
b)
ammonium chlorine
c)
ammonium chloride
d)
ammonium chlorate
52.

Which of the following compounds contains the lead(II) ion?

a)

PbO

b)

PbCl4

c)

Pb2O

d)

Pb2S

53.

The nitrate ion is

a)

N3-

b)

NO3-

c)

NO2-

d)

Ni-

54.
Identify Gallium Sulfate
a)
GaSO4
b)
Ga2(SO4)3
c)
Ga3(SO4)2
d)
Ga2SO4
55.

What is the formula for Calcium Chlorate?

a)

Ca(ClO3)2

b)

CaCl2

c)

CCl

56.

What is the correct formula for Tin(IV) carbonate?

a)

SnCO3

b)

TiCO3

c)

Sn2(CO3)4

d)

Sn(CO3)2

57.

Cyanide

a)

Cn-1

b)

CN-1

c)

Cn2

d)

CN-2

58.

Nitrite

a)

NO3-1

b)

NO3-2

c)

NO2-1

d)

NO2-2

59.

Oxalate

a)

C2O4-2

b)

CO4-1

c)

CO3-2

d)

C2O4-1

60.
Permanganate
a)
NH4+
b)
NO2-
c)
NO3-
d)
MnO4-
61.
Ammonium and oxygen would combine to form:
a)
(NH4)2O
b)
NH4O2
c)
(NH4)O2
d)
NH6O3
62.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
63.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
64.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
65.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
66.
What is the correct structure for BF3?
a)
Option A.
b)
Option B. 
c)
Option C.
d)
Option D.
67.
How many valence electrons are available for bonding in the sulfate ion (SO4-2)?
a)
30 electrons
b)
32 electrons
c)
28 electrons
d)
impossible to tell
68.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
69.
In CO2, how many UNSHARED pairs of electrons does each oxygen have?
a)
2
b)
1
c)
4
d)
6
70.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
71.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
72.

CCl4 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

73.
Each line in a Lewis Structure represents __________ electron(s).
a)
3
b)
2
c)
1
d)
4
74.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
75.

Choose the correct shape for this molecule:

a)

Trigonal planar

b)

Trigonal pyramidal

c)

Bent

d)

Tetrahedral

76.

What geometry will this molecular structure have?: PH3

a)

bent

b)

tetrahedral

c)

trigonal planar

d)

trigonal pyramidal

77.

What is the molecular shape of H2S?

a)

linear

b)

trigonal planar

c)

bent

d)

tetrahedral

78.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
79.
Which of the following shapes has an unshared pairs of electrons on the central atom? 
a)
Bipyramidal
b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
80.

Molecular Shape?

(a)  

81.

Molecular shape?

(a)  

82.

Bond Angles?

(a)  

83.

molecular shape?

(a)  

84.

bond angle?

(a)  

85.

bond angles in a molecule with the following shape: bent (with 1 lone pair)

(a)  

86.

bond angles in a molecule with the following shape: trigonal pyramidal

(a)  

87.

bond angles in a molecule with the following shape: bent (w/ 2 lone pairs)

(a)  

88.

Which of the following molecules does NOT have a linear shape?

a)

CS2

b)

HCN

c)

OF2

d)

BeF2

89.

How many bonding pairs and lone pairs for a pyramidal molecule?

a)

2 bonding pairs 2 lone pairs

b)

2 bonding pairs 0 lone pairs

c)

3 bonding pairs 1 lone pairs

d)

4 bonding pairs 2 lone pairs

90.

Predict the BCl3 bond angle

a)

180

b)

120

c)

90

d)

109.5

91.

What do 2 or more bonded regions in a molecule do?

a)

Attract each other

b)

Nothing

c)

Repel one another as far apart as possible

d)

Cross over

92.

What bond angle does the sulfate ion have?

a)

120 degrees

b)

104.5 degrees

c)

109.5 degrees

d)

180 degrees

93.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

94.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

95.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

96.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

97.
In a polar covalent bond, electrons are shared ___________.
a)
equally
b)
unequally
c)
between non-metals with similar electronegativities
d)
between a metal and a non-metal
98.
This is an example of a __________ bond.
a)
non-polar covalent
b)
polar covalent
c)
ionic
d)
metallic
99.
A bond with a partially negative end and a partially positive end is:
a)
ionic
b)
polar
c)
non-polar
d)
isometric
100.
A diatomic molecule like O2 is always_______ because electrons are shared ________.
a)
nonpolar; equally
b)
polar; equally
c)
nonpolar; unequally
d)
nonpolar; unequally
101.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
102.
Will this molecule be polar or nonpolar? H2S
a)
polar
b)
nonpolar
103.
For carbonate ions, how many resonance structures can be drawn ?
a)
2
b)
3
c)
4
d)
5
104.
How many resonance structures for NO3- ion?
a)
1
b)
2
c)
3
d)
4
105.
How many resonance structure for SO2 ?
a)
1
b)
2
c)
3
d)
4
106.

Elements in the same group or family have _____________.

a)

the same number of valence electrons and different properties.

b)

the same number of valence electrons and similar properties

c)

different number of valence electrons and similar properties.

d)

different number of valence electrons and different properties.

107.

What is the name of Group 1 elements?

a)

Alkali Metals

b)

Alkaline Earth Metals

c)

Transition Metals

d)

Halogens

108.

What is the name of the elements that are unreactive and have a full octet?

a)

Halogens

b)

Noble Gases

c)

Alkali Metals

d)

Transition Metals

109.

The Halogen group has an oxidation number of -1. Why?

a)

The Halogen group will gain one electron, therefore have an oxidation number of -1.

b)

The Halogen group will lose one electron, therefore have an oxidation number of -1.

c)

The Halogen group will lose seven electrons, therefore have an oxidation number of -1.

110.

Where are metalloids located on the Periodic Table?

a)

In the s block.

b)

In the f block.

c)

In the d block.

d)

The elements that touch the staircase except aluminum.

111.

What is the trend for atomic radius (radii)?

a)

It increases left to right on the Periodic Table and decreases down a group.

b)

It decreases left to right on the Periodic Table and increases down a group.

c)

It increases left to right on the Periodic Table and increases down a group.

d)

It decreases right to left on the Periodic Table and decreases down a group.

112.

Why does the atomic radius decrease across a period?

a)

There are more protons in the nucleus that pull electrons closer.

b)

There are more electrons in the nucleus that pull protons closer.

c)

There are more protons in the nucleus that pull neutrons closer.

d)

There are more neutrons in the nucleus that pull protons closer.

113.

What element has the largest atomic radius?

a)

oxygen

b)

neon

c)

carbon

d)

sodium

114.

Which element has the smallest atomic radius?

a)

magnesium

b)

chlorine

c)

bromine

d)

argon

115.

What is the trend for ionization energy?

a)

Across a period (left to right) it increases and down a group it decreases.

b)

Across a period (left to right) it decreases and down a group it increases.

c)

Across a period (left to right) it decreases and down a group it decreases.

d)

Across a period (left to right) it increases and down a group it increases.

116.

What is ionization energy?

a)

The energy required to remove an electron from a neutral atom of an element.

b)

The energy change that occurs when an electron is acquired by a neutral atom.

c)

The measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound.

d)

How close an atom is to its neighboring atom.

117.

Which element has the highest ionization energy?

a)

oxygen

b)

sulfur

c)

silicon

d)

potassium

118.

What is the ability of an atom in a chemical compound to attract electrons from another atom in the compound?

a)

ionization energy

b)

electronegativity

c)

atomic radius

d)

electron affinity

119.

Which element has the largest electronegativity?

a)

barium

b)

oxygen

c)

iron

d)

lithium

120.

Which family is the most reactive Non-Metals

a)

Alkali Metals (Group 1)

b)

Alkaline Earth Metals (Group 2)

c)

Transition Metals (Group 3-12)

d)

Halogens (Group 17)

e)

Noble Gases (Group 18)

121.

As you move down a group on 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

122.

Which atom has the largest atomic radius?

a)

potassium (K)

b)

rubidium (Rb)

c)

francium (Fr)

d)

cesium (Cs)

123.

Electronegativity __________ from left to right within a period and __________ from bottom to top within a group.

a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
124.
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.
125.

What is the name of the family that is highlighted?

a)

Alkali Metal Family

b)

Halogen Family

c)

Alkaline Earth Metals

d)

Transition Metal Family

126.
Is silicon a metal, nonmetal or metalloid?
a)
Metal
b)
NonMetal
c)
Metalloid
127.

How many valence electrons does Beryllium (4Be) have?

a)

5

b)

1

c)

2

d)

8

128.

How many valence electrons does Silicon (14Si) have?

a)

4

b)

8

c)

3

d)

1

129.

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

a)

groups

b)

towers

c)

periods

d)

atomic numbers

130.
The Modern Periodic Table of Elements is arranged by
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
131.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
132.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
133.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
134.
Elements in a ..................have similar chemical properties.  
a)
period
b)
group
c)
row
135.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
136.
The symbols W, X, Y, and Z represent four elements shown on the outline of a periodic table.
Which element has the highest electronegativity?

a)
W
b)
X
c)
Y
d)
Z
137.
Which of the following pairs of elements have similar properties
a)
Barium and Calcium
b)
Sodium and Magnesium
c)
Nickel and Copper
d)
Lithium and Helium 
138.

Which of the following would be the ion formed by sulfur (S)?

a)

S-

b)

S-2

c)

S+

d)

S+2

139.

Which of the following would be the ion formed by Gallium (Ga)?

a)

Ga+

b)

Ga+3

c)

Ga-3

d)

Ga-

140.

Which element in Period 6 has the lowest ionization energy?

a)

Rn

b)

Cs

c)

Os

d)

Tm

141.

How many electrons would a Nitrogen ion gain/lose?

a)

lose 5

b)

gain 5

c)

lose 3

d)

gain 3

142.

USE THE PERIODIC TABLE

How many valence electrons does Phosphorus have?

a)

31

b)

5

c)

15

d)

4

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