AnswersCR Chemistry S1 Q3050OXCovalent Bonding

Covalent Bonding Answers

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1
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Which pair of elements will form a covalent bond?

A
hydrogen and chlorine
B
sodium and chlorine
C
copper and bromine
D
zinc and bromine
2
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Which statement describes a property of covalent compounds?

A
They have a high boiling point because of strong intermolecular forces.
B
They have a low boiling point because of weak intermolecular forces.
C
They have a low melting point because of strong intermolecular forces.
D
They have a high melting point because of weak intermolecular forces.
3

How many valence electrons are available for bonding in bromine (Br)?

A
one
B
two
C
five
D
seven
4

Which characteristic best explains the difference in melting behavior of covalent substances and ionic substances?

A
Ionic substances have weaker intermolecular attractions.
B
Ionic substances usually have stronger atomic bonds.
C
Covalent substances have weaker intermolecular attractions.
D
Covalent substances usually have stronger atomic bonds.
5

Some atoms are exceptions to the octet rule by having an expanded octet. Which characteristic is needed for an atom to have an expanded octet?

A
The atom has empty d-orbitals.
B
The atom has more than eight valence electrons before bonding.
C
The atom has empty p-orbitals.
D
The atom has fewer than eight valence electrons after bonding.
6

How many valence electrons are available for bonding in silicon?

A
four
B
five
C
eight
D
fourteen
7

Which compound is an exception to the octet rule?

A
H2O
B
HCl
C
CCl4
D
ClF3
8

Which compound contains only a nonpolar covalent molecule?

A
O2
B
HCl
C
H2O
D
NO3
9

Which element has the greatest number of valence electrons available for bonding?

A
selenium
B
boron
C
calcium
D
chlorine
10

Which statement about covalent compounds is true?

A
They are able to melt at high temperatures.
B
They are poor conductors of heat.
C
They have strong intermolecular attractions.
D
They have atomic bonds that are easy to break.
11

Which type of bond will form between two chlorine atoms?

A
an ionic bond
B
a metallic bond
C
a polar covalent bond
D
a nonpolar covalent bond
12

A solid compound in a sealed container was kept at a very low temperature in a freezer. When placed at room temperature, the substance quickly turned into a liquid. This compound is most likely which of the following?

A
an ionic compound because it has a low boiling point
B
a covalent compound because it has a low boiling point
C
an ionic compound because it has a low melting point
D
a covalent compound because it has a low melting point
13

What is the best reason for the difference in properties of LiCl and C6H14O?

A
LiCl and C6H14O have different atomic masses.
B
Cl and O belong to different groups of the periodic table.
C
One compound is ionic, and the other is metallic.
D
One compound is covalent, and the other is ionic.
14

Which type of bond will most likely be found in HBr given that the electronegativity of hydrogen is 2.20 and the electronegativity of bromine is 2.96?

A
an ionic bond
B
a metallic bond
C
a polar covalent bond
D
a nonpolar covalent bond
15

Which element has the fewest valence electrons available for bonding?

A
iodine
B
aluminum
C
carbon
D
nitrogen
16

Which structure shows the correct electron arrangement in CCl4?

A
A central upper C is single bonded to upper H above, below, and to the left, and single-bonded to upper C l to the right. The C l has three pairs of electron dots, above, right, and below.
Option A
B
A central upper C is single bonded to upper C l to the top, bottom, and left; those upper C l atoms have three pairs of electron dots on the sides away from the bond. The C is also single bonded to an upper H to the right.
Option B
C
A central upper C is single bonded to upper H above and below, and to upper C l to the left and right. The C l have three pairs of dots, above, below, and to the side opposite the bond.
Option C
D
A central upper C is single bonded to upper C l above, right, left, and below. All the C l atoms have 3 pair of electron dots, on the three sides that do not have the bond.
Option D

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