Answers2003350 Chemistry HONORS Sem 1 - MarezIntermolecular Forces

Intermolecular Forces — Unit test Answers

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The table below shows the electronegativity values of various elements on the periodic table.ElectronegativitiesWhich pair of atoms would form a covalent bond ?

Question illustration
A
calcium (Ca) and bromine (Br)
B
rubidium (Rb) and sulfur (S)
C
cesium (Cs) and nitrogen (N)
D
oxygen (O) and chlorine (Cl)
2
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Which statement best describes the effect of low ionization energies and low electronegativities on metallic bonding?

A
The valence electrons are easily delocalized.
B
The valence electrons stay in a single orbital.
C
The valence electrons break free of the crystals.
D
The valence electrons move closer to the nuclei.
3

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.
4

Which element is likely to be the most brittle?

A
selenium
B
cobalt
C
platinum
D
zinc
5

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.
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

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
8

The angle between the hydrogen atoms in water (H2O) is slightly less than expected for a tetrahedral shape. This is because of the

A
extra electron repulsion from the lone pairs.
B
atomic radius of the oxygen atom.
C
additional repulsion of the shared electrons.
D
extra repulsion of the hydrogen atoms.
9

The boron atom of BBr3 has

A
one atomic orbital.
B
two atomic orbitals.
C
three hybrid orbitals.
D
four hybrid orbitals.
10

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.
11

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
12

The incomplete table below shows selected properties of compounds that have ionic, covalent, or metallic bonds.RowSubstanceType of bondLikely property1KCl?Brittle2?CovalentDoes not conduct electricity3??MalleableWhich substance would be most suitable for row 3?

A
sodium chloride (NaCl)
B
silver (Ag)
C
nitrogen (N)
Option C
D
propane (CH)
Option D
13

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.
14

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
15

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
16

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
17

Which compound has the highest melting point?

A
Al2(CO3)3
B
C12H22O11
C
C8H18
D
H2O
18

Which statement describes a molecule that has a trigonal pyramidal molecular shape?

A
The molecule has a trigonal planar electron domain geometry with one lone pair.
B
The molecule has a tetrahedral electron domain geometry with one lone pair.
C
The molecule has a trigonal planar electron domain geometry with two lone pairs.
D
The molecule has a tetrahedral electron domain geometry with two lone pairs.
19

Which of these is a property of a substance that is composed of atoms that are held together by ionic bonds?

A
It can be shaped into wires.
B
It has a low melting point.
C
It conducts electricity when in solid form.
D
It conducts electricity when it is dissolved in water.
20

Which hybrid orbitals would be formed if one s orbital and three p orbitals combined?

A
sp
B
sp2
C
sp3
D
sp4

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