AnswersChemistry 1A - Mr. KaanLab: Ionic and Covalent Bonds

Lab: Ionic and Covalent Bonds — Unit test Answers

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How do ionic bonds affect the properties of ionic compounds?

A
The bonds weakly hold ions together, increasing the melting point.
B
The bonds strongly hold ions together, reducing the boiling point.
C
The bonds prevent ions from moving throughout the crystal, so a solid ionic compound is a poor conductor.
D
The bonds prevent electrons from moving throughout the crystal, so a solid ionic compound is a good conductor.
2
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An element has six valence electrons available for bonding. Which group of the periodic table does this element most likely belong to?

A
group 2
B
group 4
C
group 16
D
group 18
3

The diagram below shows DNA molecules.What do the broken lines connected to hydrogen atoms represent in this diagram?

Question illustration
A
the weakest intermolecular forces
B
the weakest intramolecular forces
C
the strongest intermolecular forces
D
the strongest intramolecular forces
4

Which of the following compounds would be expected to have the strongest ionic bonds?

A
the compound that has the largest ions with the greatest charge
B
the compound that has the largest ions with the least charge
C
the compound that has the smallest ions with the greatest charge
D
the compound that has the smallest ions with the least charge
5

Lewis structures cannot

A
show the number of valence electrons.
B
show the location of bonds.
C
show the strength of bonds.
D
show how many bonds are present in a molecule.
6

When applied to a dish, soap makes grease soluble in water. Which explanation correctly supports the role of intermolecular forces in this common observation?

A
The nonpolar end of a soap molecule attaches itself to grease.
B
The nonpolar end of a soap molecule attaches itself to water.
C
The polar soap molecule attaches itself to the dish.
D
The polar soap molecule attaches itself to a nonpolar soap molecule.
7

Based on its location in the periodic table, what can most likely be predicted about phosphorus?

A
It has three valence electrons.
B
It has four valence electrons.
C
It has five valence electrons.
D
It has six valence electrons.
8

Which statement is true about ionic compounds?

A
Solid ionic compounds are good conductors of electricity.
B
Ionic compounds have varying solubilities in water.
C
Ionic compounds have very low melting points.
D
Ionic compounds are very easy to bend.
9

Which statement best describes London dispersion forces?

A
repulsive intramolecular forces
B
attractive intramolecular forces
C
attractive intermolecular forces
D
repulsive intermolecular forces
10

Among the intermolecular forces, which forces are typically the weakest?

A
dipole-dipole interactions
B
hydrogen bonds
C
dipole-induced dipole interactions
D
London dispersion forces
11

Which compound has the highest melting point?

A
Al2(CO3)3
B
C12H22O11
C
C8H18
D
H2O
12

Which is the Lewis structure for H3PO4?

A
Option
Option A
B
A central upper P is single bonded left, right, above, and below to upper Os. The O above the P is single bonded to upper H on the left and the right, and has two electron dots above it. The O below the P is single bonded to an H below, and has pairs of electron dots to the left and right.
Option B
C
A central upper P is double bonded to an O above, and single-bonded to an upper O single-bonded to an upper H to the left and the right. The O above the P has three pairs of electron dots, to the left, above, and to the right; the O's to the right and left have pairs of dots above and below.
Option C
D
A central upper P is bonded to an upper H above, an upper O below, and upper O's bonded to upper H's to the left and the right. The O below the P has three pairs of electron dots, to the left, right, and below; the other two O's have pairs of dots above and below. A central upper P is double bonded to an O above, and single-bonded to an upper O single-bonded to an upper H to the left and the right. The O above the P has three pairs of electron dots, to the left, above, and to the right; the O's to the right and left have pairs of dots above and below.
Option D
13

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.
14

Which of the following can easily form an ionic bond with a cation?

A
Sr
B
Ne
C
NH4+
D
PO43–
15

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.
16

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

A
one
B
two
C
five
D
seven
17

Which pair of ions can form an ionic bond with each other and why?

A
Cu and Ag; They are both metal ions.
Option A
B
S and O; They have like charges.
Option B
C
Br and At; They are both halogen ions.
Option C
D
Li and Br; They have unlike charges.
Option D
18

How many valence electrons are available for bonding in silicon?

A
four
B
five
C
eight
D
fourteen
19

Which of the following most likely requires intermolecular forces?

A
a spider walking on the bottom of a leaf
B
a rock maintaining its solid shape
C
a koala using claws to hold onto a tree
D
a piece of fruit falling from a branch to the ground
20

What leads to the formation of an ionic bond with Hg2+?

A
the attraction of a noble gas
B
the attraction of an NH4+ ion
C
the attraction of a group 1 element
D
the attraction of an SO42– ion

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