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Chemical Bonds

Total questions: 136

Worksheet time: 3hrs 7mins

Name
Class
Date
1.

El proceso más favorable es aquel que

a)

Minimize energia

b)

Incremente su energia de enlace

c)

Sea neutro en λ

2.

Escoge la que le corresponde a : Energía de ionización

a)

Na (g) + 496 kJ = Na+(g) + e-

b)

Na (g) + e- = Na-(g) + 53 kJ

c)

Na(s)=Na(l)

3.

Los Procesos endotérmicos son:

a)

AE alta, proceso es fácil.

b)

EI alta, proceso es difícil.

c)

AE alta y EI baja, proceso neutro

4.

Elementos no metales son:

a)

más propenso a aceptar electrones

b)

más propenso a donar electrones

c)

Terminan compartiendo electrones

5.

Elemento no-metal + elemento no-metal tendencia de

a)

pueden atraer o aceptar electrones.

b)

permanecer unidos por la atracción de los núcleos hacia pares de electrones localizados en medio de los núcleos

c)

El enlace ocurre por fuerzas de atracción Coulómbicas.

6.

La energía del enlace iónico se conoce como:

a)

“lattice energy”

b)

Bonding energy

7.

La energía de red es proporcional al producto de las cargas de los iones. Mientras mayor sea la carga de los iones, mayor será la energía de red.

a)

True

b)

False

8.

 Considera todos los pares de electrones alrededor del átomo central

a)

Geometría electrónica

b)

Geometría molecular

c)

Dominios

9.

Indica la geometría molecular y electrónica de CO2

a)

Linear,Linear

b)

Tetrahedral,Linear

c)

Octahedral,Linear

10.

Indica la geometría molecular y electrónica de AsF4^-.

a)

Trigonal Bipiramidal, Seesaw

b)

Tetrahedral,Linear

c)

Linear,Linear

11.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
12.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Linear
13.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Trigonal planar
d)
Linear
14.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
15.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
16.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
17.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Trigonal planar
18.
Choose the correct shape for this molecule:
a)
Tetrahedral
b)
Trigonal pyramidal
c)
Bent
d)
Trigonal planar
19.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Trigonal planar
20.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
21.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
22.
*
a)
linear
b)
trigonal planar
c)
trigonal pyramid
d)
bent of angular
23.
*
a)
trigonal pyramid
b)
linear
c)
bent
d)
angular
24.
*
a)
bent or angular
b)
trigonal pyramid
c)
linear
d)
tetrahedral
25.
*
a)
tetrahedral
b)
trigonal pyramid
c)
angular or bent
d)
trigonal plane
26.
What is this molecule?
a)
CH4
b)
NaCl3
c)
SK4
d)
S4K2
27.

What is the hybridization of a linear molecule?

a)

sp

b)

sp2

c)

sp3

d)

sp3d

28.

Which of the following images represents a Trigonal Planar molecular geometry?

a)
b)
c)
d)
29.

What is the hybridization of this molecule shown above

a)

sp

b)

sp2

c)

sp3

d)

sp4

30.

What is the bond angle for the CH4 molecule?

a)

120°

b)

107°

c)

109.5°

d)

90°

31.

What is the hybridization of the central atom of a bent molecule? (AB2E2)

a)

sp

b)

sp2

c)

sp3

d)

sp3d

32.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
33.
Which of the following elements has the weakest attraction for electrons in a chemical bond?
a)
S
b)
Cl
c)
O
d)
F
34.
The molecule shown in the diagram can best be classified as a
a)
polar covalent molecule
b)
nonpolar covalent molecule
c)
ionic compound
d)
nonpolar ionic compound
35.
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
36.
In the diagram shown, what is the total number of electrons shared in the bond between the two carbon atoms?
a)
2
b)
3
c)
4
d)
6
37.
Which bond is most polar?
a)
H-F
b)
H-Cl
c)
H-Br
d)
H-I
38.
Which formula represents a polar molecule?
a)
H2
b)
H2O
c)
CO2
d)
CCl4
39.
A covalent bond usually forms between
a)
a metal and a nonmetal
b)
either metals or nonmetals
c)
two metals
d)
two nonmetals
40.
A dipole is also known as
a)
polar molecule
b)
nonpolar molecule
c)
bond angles
d)
geometry
41.
The ability of an atom to attract electrons to itself is called
a)
geometry
b)
conductivity
c)
electronegativity
d)
ionization energy
42.
What kind of bond do you have: Li and Cl
a)
Non-polar covalent
b)
Polar covalent
c)
ionic
d)
James Bond
43.
Which has the greater electronegativity: 
H, N, O or F?
a)
H
b)
F
c)
N
d)
O
44.
Which of the following elements has the weakest attraction for electrons in a chemical bond?
a)
S
b)
Cl
c)
O
d)
F
45.
The molecule shown in the diagram can best be classified as a
a)
polar covalent molecule
b)
nonpolar covalent molecule
c)
ionic compound
d)
nonpolar ionic compound
46.
2 bonds, no lone pairs
a)
Linear
b)
Trigonal planar
c)
Tetrahedral
d)
Bent
47.
3 bonds, no lone pairs
a)
Linear
b)
Trigonal planar
c)
Tetrahedral
d)
Bent
48.
3 bonds, one of them a lone pair
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
49.
4 bonds, no lone pairs
a)
Bent
b)
Trigonal planar
c)
Trigonal pyramidal
d)
Tetrahedral
50.
4 bonds, one of them a lone pair
a)
Trigonal pyramidal
b)
Trigonal Planar
c)
Tetrahedral
d)
Bent
51.
4 bonds, two of them lone pairs
a)
Trigonal pyramidal
b)
Bent
c)
Tetrahedral
d)
Trigonal planar
52.
One bond
a)
Bent
b)
Trigonal Planar
c)
Linear
d)
Trigonal pyramidal
53.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
54.
What is the bond angle for this molecule:
a)
120 degrees
b)
90 degrees
c)
180 degrees
d)
109.5 degrees
55.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
56.
What is the hybrid for this molecule:
a)
sp
b)
sp2
c)
sp3
d)
sp4
57.
An ionic bond contains _____________.
a)
Two metals
b)
A metal and nonmetal
c)
Two nonmetals 
58.
Electrons are ______ in covalent bonds.  
a)
Shared
b)
Transferred
c)
Given up
d)
Lost
59.
Hydrogen is classified as a ________.  
a)
Metal
b)
Nonmetal
60.
NaCl
a)
Ionic
b)
Covalent
61.
Which elements tend to lose electrons?
a)
metals
b)
nonmetals
62.
What kind of bond occurs between the carbons in C2H2?
a)
single
b)
double
c)
triple
d)
quadruple
63.
This molecule has______bond and is a _________molecule.
a)
non-polar; non-polar
b)
polar, polar
c)
polar,
non-polar
d)
non-polar; polar
64.
The electron geometry is the same as the molecular shape when there are no lone pairs of electrons on the central atom.
a)
True
b)
False
c)
¯\_(ツ)_/¯
d)
#chem4eva
65.
The basic fact that determines molecular shapes is that
a)
nuclei attract each other.
b)
electron pairs attract each other.
c)
electron pairs repel each other.
d)
nuclei repel each other.
66.
Lone pairs around the oxygen atom of a water molecule play no role in determining its molecular geometry which has what shape?
a)
True;
bent
b)
False;
bent
c)
True;
linear
d)
False;
linear
67.
The bond angle in NH3 is __________ than the bond angle in CH4 because
a)
LARGER; the unshared pair of electrons on nitrogen is LESS repulsive to the bonded electron pairs.
b)
SMALLER; nitrogen has a SMALLER atomic radius than carbon.
c)
LARGER; nitrogen has a LARGER atomic radius than carbon.
d)
SMALLER; the unshared pair of electrons on nitrogen is MORE repulsive to the bonded electron pairs.
68.
Which of the following most likely represents the molecular geometry of water?
a)
A
b)
B
c)
C
d)
D
69.
Which of the following molecules do NOT match their molecular geometry?
I. BeH2: bent
II. NH3: trigonal pyramidal
III. CF4: tetrahedral
IV. NH4+: tetrahedral
a)
I only
b)
I and II only
c)
II, III, and IV only
d)
All are paired correctly.
70.
Water has a bent molecular geometry because
a)
there are unpaired electrons within the bonds.
b)
the two O-H bonds repel each other.
c)
oxygen does not have d-orbitals to allow for an expanded octet.
d)
there are 4 electrons on the oxygen atom which are not in the O-H bonds but which affect molecular shape.
71.
Lewis structures can sometime be deceptive when determining molecular shape because they are drawn in two-dimensions.  Examine the Lewis structures. Which is not linear and why?
a)
CO2 because it has double bonds
b)
BeCl2 because beryllium is an exception to the octet rule
c)
H2S because it has lone pairs on the central atom
d)
All are linear
72.
Use VSEPR theory to predict the molecular shape of the molecule SeF6.
a)
tetrahedral
b)
octahedral
c)
trigonal-planar
d)
trigonal-bipyramidal
73.
What is the name of the molecular geometry shown below? (The dark circle and each white circle represent an atom.)
a)
trigonal pyramidal
b)
bent
c)
tetrahedral
d)
octahedral
74.
What geometry will this molecular structure have?: CH4
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
75.
What geometry will this molecular structure have?: PH3
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
76.
What geometry will this molecular structure have?: CCl4
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
77.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
78.

Which of the following has two bonding pairs and two unshared pairs of electrons around the central atom?

a)

CH4

b)

H2O

c)

NH3

d)

HF

79.
Will this molecule be polar or nonpolar? PH3
a)
polar
b)
nonpolar
80.
Will this molecule be polar or nonpolar? CH4
a)
polar
b)
nonpolar
81.
Will this molecule be polar or nonpolar? CS2
a)
polar
b)
nonpolar
82.
How many valence electrons does a sulfur atom typically have?
a)
3
b)
4
c)
5
d)
6
83.
Which element, that we have talked about, needs less than an octet of valence electrons to be satisfied in a compound?
a)
Carbon
b)
Hydrogen
c)
Fluorine
d)
Nitrogen
84.
Knowing that a compound's molecular geometry is bent, determine the # of electron groups and # of lone pairs that could be around the central atom.
a)
4 electron groups, 0 lone pairs
b)
3 electron groups, 2 lone pairs
c)
2 electron groups, 0 lone pairs
d)
3 electron groups, 1 lone pairs
85.
Looking at the compound provided, determine the hybridization around the central atom and the molecular geometry.
a)
sp2, trigonal pyramid
b)
sp3, trigonal pyramid
c)
sp2, tetrahedral
d)
sp3, tetrahedral
86.
For the following compound, determine the correct hybridization, molecular geometry, and if it is polar or non polar.
a)
sp3d2, trigonal bipyramidal, non polar
b)
sp3d, t-structure, polar
c)
sp3d2, octahedral, non polar
d)
sp3d, octahedral, polar
87.
Which does not fit the "like dissolves like" rule?
a)
Water and oil do not mix.
b)
Polar mixes with polar.
c)
Polar mixes with nonpolar.
d)
Nonpolar mixes with nonpolar.
88.
Water and oil are ____.
a)
Miscible
b)
Polar
c)
Nonpolar
d)
Immiscible
89.
We commonly use sodium chloride (NaCl) to season our food.
a)
Ionic
b)
Covalent
c)
Metallic
90.
Which type of nuclear radiation is being emitted here?
a)
Alpha
b)
beta
c)
gamma 
d)
none
91.
Which of the following gives the correct chemical formula for the compound Magnesium Phosphide?
a)
Mg2P3
b)
MgP
c)
Mg3P2
d)
MgP2
92.
Neutral atoms covalently bonded together form a _________________.
a)
Molecule
b)
Ion
c)

salt

d)
Anion
93.
After drawing in your bonds, what do you do if you don't have enough electrons to get each atom to its octet?
a)
Place dots until everything has eight
b)
Place dots only around the terminal atoms
c)
Add a multiple bond
d)
Have eight only around the central atom
94.
Compounds with these kinds of bonds have low melting and boiling points.
a)
Metallic
b)
Ionic
c)
Covalent
d)
None of the above
95.
Occurs when electrons float in a "sea;" this type of bond can be found in alloys.
a)
Metallic
b)
Ionic
c)
Covalent
d)
None of the above
96.
Occurs when valence electrons are shared between two or more atoms.
a)
Metallic
b)
Ionic
c)
Covalent
d)
None of the above
97.
Carbon tetrachloride has a ______ bond, and its formula is ______.
a)
covalent, CCl
b)
ionic, CCl4
c)
covalent, CCl4
d)
ionic, CCl
98.
Which of the following compounds has a tetrahedral molecular shape?
a)
Br2
b)
CO2
c)
NF3
d)
CH4
99.
The molecular geometry of H2O (a very special molecule) is...
a)
Tetrahedral
b)
Bent
c)
Linear
d)
Trigonal planar
100.
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. 
101.
Warning: Tricky!!
What is the correct name for Cu2O3 ?
a)
Copper (II) Oxide
b)
Copper (III) Oxide
c)
Copper (III) dioxide
d)
dicopper trioxide
102.
What is the correct formula for Beryllium hydroxide?
a)
Be(OH)2
b)
Be(OH)
c)
Be2+(OH)1-
d)
BeOH2
103.
What molecular shape is this?
a)
Tetrahedral
b)
Trigonal Planar
c)
Linear
d)
Bent
104.

What property of this wave is represented by the letter "A"

a)

amplitude

b)

crest

c)

trough

d)

wavelength

105.
solids whose particles are arranged in a crystal structure
a)
crystal
b)
covalent bond
c)
polar covalent bond
d)
chemical formula
106.
Metals tend to _________ electrons to become______ ions
a)
lose,positive
b)
gain, negtive
c)
lose neutral
107.
In a covalent bond, electrons are
a)
lost or gained
b)
shared
c)
none of the above
108.
In an ionic bond electrons are
a)
lost or gained
b)
shared
c)
neutralized
109.

1. Are the atoms more stable when they are bonded together or when they are apart?

a)

Bonded Together

b)

Apart

110.

2. Ionic Bonding involves:

a)

The transfer of protons

b)

The transfer of neutrons

c)

The transfer of electrons

d)

None Of the above

111.

3. 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

112.

4. What usually forms the positive ion?

a)

Metal

b)

Nonmetals

c)

None

113.

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

a)

It become negatively charged

b)

It become positively charged

c)

none

114.

6. What usually forms the negative ion?

a)

Nonmetals

b)

Metal

c)

None

115.

7. Covalent compounds:

a)

Share electrons

b)

Transfer electrons

c)

Neither

116.

10. What charges attract?

a)

Opposite

b)

Same

117.

11. What charges repel?

a)

Same

b)

Opposite

118.

13. What elements generally make a covalent bond?

a)

metal and nonmetal

b)

2 or more nonmetals

c)

metal

d)

none of the above

119.

14. How would I know if an element was a metal or nonmetal?

a)

Periodic Table

b)

Internet

c)

Ask Teacher

d)

all of the above

120.

16. What is the number of valence electrons for Calcium (Group 2)?

a)

1

b)

2

c)

3

d)

4

121.

17. What is the number of valence electrons for Carbon (Group 14)?

a)

1

b)

2

c)

3

d)

4

122.

18. What is the number of valence electrons for Neon and the other Noble Gases?

a)

5

b)

6

c)

7

d)

8

123.

19. If an atom transfers an electron to another atom, those atoms form which bond?

a)

Ionic Bond, which is stronger than a covalent bonds

b)

Covalent Bond, which is stronger than ionic bonds

124.

20. If I was trying to determine if two atoms will bond, what would be helpful to know:

a)

Valence electrons, found by group number

b)

Whether the elements are metals or nonmetals

c)

The electronegativity of the atoms

d)

All of the above, all of which can be found on the Periodic Table

125.
Calculate the reaction enthalpy for the formation of anhydrous aluminum chloride:
2Al(s) + 3Cl2(g) ---> 2AlCl3(s)
from the following data:
2Al(s) + 6HCl(aq) ---> 2AlCl3(aq) + 3H2 (g)ΔH° = -1049 kJ
HCl(g) ---> HCl(aq)ΔH° = -74.8 kJ
H2(g) + Cl2(g) ---> 2HCl (g)ΔH° = -185 kJ
AlCl3(s) ---> AlCl3(aq)ΔH° = -323 kJ
a)
-1406.8 kJ
b)
-1204.5 kJ
c)
-703.4 kJ
d)
-985.8 kJ
126.
Complete combustion of 1.00 mol of acetone (C3H6O) liberates 1790 kJ:
C3H6O(ℓ) + 4O2(g) ---> 3CO2(g) + 3H2O(ℓ); ΔH°comb, acetone = -1790 kJ
Using this information together with the data below (values in kJ/mol), calculate the enthalpy of formation of acetone.
ΔH°f, CO2: -393.5 
ΔH°f, H2O: -285.83
a)
-329.34 kJ/mol
b)
-247.99 kJ/mol
c)
-123.23 kJ/mol
d)
-234.34 kJ/mol
127.
Endothermic reactions feel
a)
warm
b)
cold
128.
Exothermic reactions feel
a)
warm
b)
cold
129.
energy in endothermic reactions are
a)
released
b)
ended
c)
absorbed
130.
energy in exothermic reactions are
a)
released
b)
absorbed
131.
H2 + Cl2 --> 2 HCl + 1845 kJ
Is this reaction endothermic or exothermic?
a)
Endothermic 
b)
Exothermic
132.
6.  The formation ½ A2 + 2 B2 + C --> CAB4 has an enthalpy of formation of -104 kJ and a change in entropy of -60.8 J/K at 30 °C. What is the free energy and spontaneity of the reaction?  
a)
-85.6 kJ, spontaneous
b)
-18.3 kJ, not spontaneous
c)
+18.3 kJ, spontaneous 
d)
+85.6 kJ, not spontaneous 
133.
 For which of these processes is the value of ΔH expected to be positive?
1.  The temperature increases when calcium chloride dissolves in water.
 2.  Steam condenses to liquid water
3.  Water boils
4.  Dry ice sublimates
a)
4 only
b)
1 only
c)
3 and 4 only
d)
2 and 3 only
134.
H2 + 2 C + N2 + 270.3 kJ --> 2 HCN
Is this reaction endothermic or exothermic?
a)
Endothermic 
b)
Exothermic
135.
Given the following data: ΔH○f[FeO(s)] = –270kJmol–1
ΔH○f [Fe2O3(s)] = –820 kJ mol–1
Select the expression which gives the enthalpy change, in kJ mol–1, for the reaction:
2FeO(s) + 1⁄2O2(g) → Fe2O3(s) 
a)
(–820 × 1⁄2) + 270 = –140
b)
(+820 × 1⁄2) – 270 = +140
c)
–820 + (270 × 2) = –280 
d)
+820 – (270 × 2) = +280 
136.

Born-Haber CaCl2

a)
b)

Do not know

c)

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