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Worksheetsbonding
Total questions: 118
Worksheet time: 2hrs 54mins
Name
Class
Date
1.
A mixture of two or more metals is called:
a)
salt
b)
solution
c)
compound
d)
alloy
2.
Metallic bonding is...
a)
sharing of electrons between 2 nonmetals
b)
transfer of electrons from metal to nonmetal
c)
sharing of electrons between a metal and a nonmetal
d)
an attraction between positive metal ions and mobile electrons.
3.
What does malleable mean?
a)
able to be shaped
b)
will break easily
c)
can be stretched into wire
d)
is shiny
4.
When two atoms share electrons, a chemical bond is formed. This type of bond is called:
a)
covalent bond
b)
ionic bond
c)
metallic bond
d)
polyatomic bond
5.
What is a double bond?
a)
when two atoms share two electrons
b)
when two atoms share four electrons
c)
when two atoms share six electrons
d)
when two atoms lose two electons
6.
Fluorine (F₂) is a(n) _________________ molecule because the valence electrons are shared equally between the two fluorine atoms.
a)
polar
b)
nonpolar
c)
ionic
d)
metallic
7.
What type of compound consists of molecules that are made of atoms that are covalently bonded to each other?
a)
ionic
b)
metallic
c)
alloy
d)
molecular
8.
Molecular compounds that dissolve in water do not conduct electricity because no ___________________ are present.
a)
charged ions (particles)
b)
uncharged ions (particles)
9.
Because the electrons in a molecule of hydrogen iodide(HI) are more strongly pulled toward the fluorine atom, the molecule is:
a)
linear and polar
b)
linear nonpolar
c)
bent and polar
d)
bent and nonpolar
10.
What is the VSEPR theory used to predict?
a)
Bond Type
b)
Bond Polarity
c)
Molecular Shape
d)
Electronegativity
11.
Which molecule has this shape?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
12.
Which chemical formula could be represented by this structure?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
13.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Protons
c)
Neutrons
d)
Nonvalence electrons
14.
A covalent bond is called _______ if the atoms do not equally share electrons.
a)
Polar
b)
Nonpolar
15.
In a triple covalent bond, _____ electrons are shared.
a)
2
b)
4
c)
6
d)
8
16.
A polar covalent bond results in a molecule having regions of slight electrical charge
a)
True
b)
Flase
17.
H2 is a covalently bonded molecule. Since both atoms are the same kind (hydrogen), there is equal sharing of electrons.
a)
True
b)
False
18.
In a covalent bond, the shared electrons are represented by a dash.
a)
True
b)
False
19.
In a covalent bond, the force of attraction results from both atoms wanting to stay close to the shared electron pair.
a)
True
b)
False
20.
Metals usually form covalent bonds with one another.
a)
True
b)
False
21.
Oxygen usually exists as O2 in nature. What kind of bonds are present in this molecule?
a)
Ionic
b)
Nonpolar Covalent
c)
Metallic
d)
Polar Covalent
22.
Hydrogen is classified as a ________.
a)
Metal
b)
Nonmetal
c)
Noble Gas
23.
NaCl
a)
Ionic
b)
Covalent
c)
metallic
24.
Copper (II) oxide
a)
has ionic bonds
b)
has nonpolar covalent bonds
c)
has metallic bonds
d)
has polar covalent bonds
25.
Carbon dioxide
a)
has ionic bonds
b)
has polar covalent bonds
c)
has nonpolar covalent bonds
d)
has metallic bonds
26.
Which elements tend to gain electrons?
a)
metals
b)
nonmetals
27.
Ions that are made of more than one atoms that are covalently boned together are examples of:
a)
polyatomic atoms
b)
negative ions
c)
positive ions
d)
neutral ions
28.
In what form can an ionic compound conduct electricity?
a)
when dissolved in water
b)
as a solid
c)
as a crystal
d)
when warmed slightly
29.
According to the diagram below, how many bonds will this atom need to make to be stable?
a)
1
b)
2
c)
3
d)
4
30.
How many electrons are needed in the outer energy levels of most atoms to be stable?
a)
2
b)
4
c)
6
d)
8
31.
What shape would this have?
a)
Trigonal planar
b)
Trigonal Pyramid
c)
Tetrahedral
d)
Bent
32.
Which group of elements have full outer electron shells?
a)
The alkali metals
b)
The alkaline earth metals
c)
The halogens
d)
The noble gases
33.
Predict the bond that will form between Cu and Zn.
a)
Ionic
b)
Covalent
c)
Metallic
34.
Predict the bond that will form between Mg and Cl.
a)
Ionic
b)
Covalent
c)
Metallic
35.
Predict the bond that will form between H and O
a)
Ionic
b)
Polar Covalent
c)
Metallic
d)
Nonpolar Covalent
36.
Which term means able to be pulled into thin strands or wires?
a)
polar
b)
alloy
c)
ductile
d)
malleable
37.
The molecular geometry of H2O is...
a)
Tetrahedral and polar
b)
Bent and polar
c)
Linear and nonpolar
d)
Trigonal planar and nonpolar
38.
A covalent compound is non-polar when...
a)
the electrons are shared equally.
b)
the electrons are shared unequally.
c)
the electrons are lost to another atom.
d)
the electrons are gained from another atom.
39.
What molecular shape is this?
a)
Tetrahedral
b)
Trigonal Planar
c)
Linear
d)
Bent
40.
Compounds with these kinds of bonds have low melting and boiling points.
a)
Metallic
b)
Ionic
c)
Covalent
41.
Where are metals located on the periodic table?
a)
Orange
b)
Red
c)
Blue
d)
Green
42.
Where are the nonmetals located on the periodic table?
a)
Orange
b)
Red
c)
Blue
d)
Green
43.
What happens to the electrons in a Nonpolar Covalent bond
a)
transferred from one atom to another
b)
shared equally between 2 atoms
c)
shared unequally between 2 atoms
d)
mobile
44.
What kinds of elements are most likely to form an ionic bond?
a)
Nonmetal+Nonmetal
b)
Metalloid+Metalloid
c)
Metal+Nonmetal
d)
Metalloid+Nobel Gas
45.
Flexible
a)
ionic
b)
covalent
c)
metallic
46.
Electrolytes
a)
ionic
b)
covalent
c)
metallic
47.
Of these molecules, which has polar covalent bonding?
a)
O2
b)
NaI2
c)
HBr
d)
MgO
48.
Which of these molecules has nonpolar covalent bonding?
a)
H2O
b)
HCl
c)
I2
d)
NaCl
49.
Which of these molecules is polar?
a)
H2O
b)
BBr3
c)
I2
d)
MgI2
50.
Which of these represents a formula unit?
a)
I2
b)
AlCl3
c)
NH3
d)
CO
51.
Which of these represents a molecule?
a)
NaCl
b)
MgBr2
c)
CaO
d)
NH3
52.
According to VSEPR theory the shape of BBr3 is____
a)
trigonal planar
b)
tetrahedral
c)
trigonal pryamidal
d)
bent
53.
According to VSEPR theory the shape of NH3 is ____
a)
trigonal planar
b)
tetrahedral
c)
trigonal pryamidal
d)
bent
54.
According to VSEPR theory the shape of H2S is ____
a)
trigonal planar
b)
tetrahedral
c)
trigonal pryamidal
d)
bent
55.
The following all contain polar bonds, which one is a polar molecule?
a)
CBr4
b)
PCl3
c)
BCl3
d)
BeCl2
56.
When electrons are transfered from cations to anions a ________ bond is formed
a)
Polar covalent
b)
Nonpolar covalent
c)
Ionic
d)
Metallic
57.
In the HCl molecule which atom would have a slightly negative charge?
a)
H
b)
Both
c)
Cl
d)
Neither
58.
What is a valence electron?
a)
an electron that is found in the outermost shell of an atom.
b)
an electron found in the innermost shell of an atom.
c)
an electron found in the nucleus of an atom.
59.
Predict the bond that will form between Sr and S.
a)
Ionic
b)
Covalent
c)
metallic
60.
Predict the type of bond that will form between S and Cl.
a)
Ionic
b)
Covalent
c)
metallic
61.
Predict the type of bond that will form between Na and F.
a)
Ionic
b)
Covalent
c)
metallic
62.
What elements generally make a covalent bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
2 or more metals
d)
noble gases
63.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
2 or more metals
d)
noble gases
64.
Are atoms more stable when they are bonded together or when they are alone?
a)
Bonded Together
b)
Alone
65.
What is the polarity of BeH2?
a)
polar
b)
nonpolar
66.
What is the shape and polarity of CO2?
a)
linear and polar
b)
linear and nonpolar
c)
bent and polar
d)
bent and nonpolar
67.
Determine the type of bond in a nitrogen molecule (N2)
a)
Double covalent
b)
Single covalent
c)
Ionic
d)
Triple covalent
68.
How strongly an atom attracts electrons is called....................
a)
Ionization energy
b)
Electronegativity
69.
Which of the following contains a polyatomic ion?
a)
Cu2CO3
b)
MnO
c)
CrN
d)
BeCl2
70.
If an atom loses an electron it will be
a)
negatively charged
b)
positively charged
c)
neutral
71.
Which bond would be the least polar?
a)
H-F
b)
H-O
c)
H-H
d)
H-Br
72.
What is a polar molecule?
a)
One that has a partial negatitive on one end and a partial positive on the other
b)
a molecule with little vibration
c)
an ionic compound
d)
the nonpolar bonds are arranged sequentially
73.
Which compound below would be nonpolar?
a)
HF
b)
H2O
c)
Br2
d)
HBr
74.
Why do atoms share electrons?
a)
To attain the electron configuration of a noble gas.
b)
To become ions and take a charge
c)
to increase the mass
d)
it's a nice thing to do.
75.
Choose the list that contains all polar molecules.
a)
CO2, CO, CH4, CH3F
b)
H2O, NH3, CCl4, BH3
c)
H2O, CH3F, HCN, NH3
d)
CO2, CH3F, HCN, NH3
76.
Choose the list that contains all non-polar molecules.
a)
CO2, CO, CH4, CH3F
b)
O2, NH3, CCl4, BH3
c)
H2O, CH3F, HCN, BH3
d)
CO2, CH4, BH3, CCl4
77.
Pick the correct choice and reasoning for the molecule listed.
a)
CO2-nonpolar molecule, non-polar bonds
b)
CO2-nonpolar molecule, symmetry
c)
H2O-nonpolar molecule, non-polar bonds
d)
H2O-nonpolar molecule, symmetry
78.
Pick the correct choice and reasoning for the molecule listed.
a)
BF3-polar molecule, polar bonds and lack of symmetry
b)
BF3-nonpolar molecule, nonpolar bonds
c)
PF3-polar molecule, polar bonds and lack of symmetry
d)
PF3- nonpolar molecule, polar bonds and symmetry
79.
What information do you need to use to decide if a molecule is a polar molecule or not?
a)
its shape
b)
its shape, whether it has polar bonds or not, symmetry
c)
its shape, symmetry
d)
whether it has polar bonds or not
80.
VSEPR stands for ________ theory.
a)
Valence Structure of Electron Pyramids and Regression
b)
Varied Structures of Electrons Paired and Replaced
c)
Varied Shell Energy of Protons and Radiation
d)
Valence Shell Electron Pair Repulsion
81.
Which molecule below is non-polar?
a)
H2O
b)
CH4
c)
NH3
d)
SF4
82.
Which of the following elements has the weakest attraction for electrons in a chemical bond?
a)
S
b)
Cl
c)
O
d)
F
83.
The polarity of a bond between two elements can be best determined by
a)
The difference in electronegativity between the elements
b)
The difference in first ionization energy between the elements
c)
The number of electrons shared in the bond
d)
The difference in atomic radius between the elements
84.
Which substance contains bonds that involve a transfer of electrons from one atom to another?
a)
CO2
b)
NH3
c)
KBr
d)
Cl2
85.
This molecule has______bond and is a _________molecule.
a)
non-polar; non-polar
b)
polar, polar
c)
polar,
non-polar
non-polar
d)
non-polar; polar
86.
This molecule has______bonds and is a _________molecule.
a)
non-polar; non-polar
b)
polar; non-polar
c)
polar; polar
d)
non-polar; polar
polar, pointing straight down
polar, pointing straight down
87.
Which of the following compounds contains both ionic and covalent bonds?
a)
Na3P
b)
Na3PO4
c)
CuCl2
d)
Al2O3
88.
What is the shape of this molecule?
a)
bent
b)
linear
c)
trigonal pyramidal
d)
tetrahedral
89.
What is the shape of this molecule?
a)
Linear
b)
bent
c)
tetrahedral
d)
trigonal planar
90.
What is the shape of this molecule?
a)
Linear
b)
Bent
c)
tetrahedral
d)
Trigonal Pyramidal
91.
What is the shape of this molecule?
a)
Linear
b)
Bent
c)
Tetrahedral
d)
Trigonal Pyramidal
92.
What molecular shape is the structure shown here? (BCl3)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
93.
What intermolecular force present in a sample of pure HCl?
a)
dipole-dipole attraction
b)
London dispersion forces
c)
H-bonds
d)
molecule-ion attraction
94.
What intermolecular force is present in a sample of pure Cl2?
a)
dipole-dipole attraction
b)
H-bonds
c)
London dispersion forces
d)
molecule-ion attraction
95.
Intermolecular forces are the forces that exist
a)
within molecules
b)
between molecules
96.
Which of these is not an intermolecular force?
a)
covalent bonding
b)
hydrogen bonding
c)
London dispersion forces
d)
dipole-dipole forces
97.
What type of intermolecular forces increase with increasing molecular mass?
a)
hydrogen bonding
b)
dipole-dipole forces
c)
London dispersion forces
d)
ion-dipole forces
98.
Which are the strongest intermolecular forces?
a)
hydrogen bonds
b)
dipole-dipole forces
c)
London dispersion forces
d)
molecule-ion attractions
99.
What are the most important intermolecular forces found between water molecules?
a)
hydrogen bonding
b)
dipole-dipole forces
c)
London dispersion forces
d)
ion-dipole forces
100.
Hydrogen bonding is a special type of what force?
a)
London dispersion forces
b)
dipole-dipole forces
c)
ion-dipole forces
d)
covalent force
101.
What type of intermolecular force is present in all substances, regardless of polarity?
a)
London dispersion forces
b)
dipole-dipole forces
c)
ion-dipole forces
d)
hydrogen bonding
102.
Which of these molecules exhibits hydrogen bonding as its major intermolecular force of attraction when dissolved in water?
a)
HBr
b)
HCl
c)
HF
d)
all of these
103.
What explains the very high melting and boiling point of water?
a)
Dipole-dipole forces between water molecules
b)
Hydrogen bonds between water molecules
c)
London dispersion forces between water molecules
d)
Molecule-ion attractions between water molecules
104.
What force explains the ability for water molecules to dissolve ionic compounds?
a)
Dipole-dipole attraction
b)
Hydrogen bonds
c)
Molecule-ion attraction
d)
London Dispersion forces
105.
Which of these typically increases when intermolecular forces increase?
a)
Boiling Point
b)
Melting Point
c)
Viscosity
d)
All of these
106.
In general, substances with stronger intermolecular forces have ________ boiling points than those with weaker forces
a)
Higher
b)
Lower
c)
The same
107.
Which of these has the strongest London dispersion forces?
a)
F2
b)
Br2
c)
Cl2
d)
I2
108.
Hydrogen bonding occurs when hydrogen is bonded to N, O, or F. Which of the following would have hydrogen bonding with water molecules?
a)
CBr4
b)
NO2
c)
H2S
d)
NH3
109.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
110.
Does NH3 have hydrogen bonding?
a)
yes
b)
no
111.
A substance capable of hydrogen bonding has a ___________ boiling point than a similar substance that doesn't hydrogen bond.
a)
higher
b)
lower
112.
What are intermolecular forces?
a)
forces of attraction or repulsion which act between neighboring particles
b)
forces which keep a molecule together.
113.
Is intermolecular bonding generally stronger or weaker than intramolecular bonding?
a)
Stronger
b)
Weaker
114.
Which type of force is this?
a)
Intramolecular
b)
Intermolecular
115.
Which of the following would have the highest boiling point?
a)
H2
b)
HCl
c)
H2S
d)
H2O
116.
What is a dipole?
a)
A polar molecule
b)
A nonpolar molecule
c)
A diatomic element
117.
What type of intermolecular force is the result of temporary uneven distribution of electrons around molecules that result in momentary dipoles?
a)
dipole-dipole
b)
molecule-ion
c)
London dispersion
d)
hydrogen bonds
118.
Which of the following would have molecule-ion attractions?
a)
Cl2(aq)
b)
H2O(s)
c)
NaCl(aq)
d)
CaBr2(s)
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