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Honors Chem Unit 3 Liquids

Total questions: 143

Worksheet time: 3hrs 36mins

Name
Class
Date
1.

Define polar covalent bond

a)

transfer of electrons

b)

equal sharing of electrons

c)

unequal sharing of electrons

d)

delocalized sea of valence electrons

2.

Define nonpolar covalent bond

a)

transfer of electrons

b)

equal sharing of electrons

c)

unequal sharing of electrons

d)

delocalized sea of valence electrons

3.

Define ionic bond

a)

transfer of electrons

b)

equal sharing of electrons

c)

unequal sharing of electrons

d)

delocalized sea of valence electrons

4.

What type of bond?

H-H

a)

nonpolar covalent bond

b)

polar covalent bond

c)

ionic bond

d)

metallic bond

5.

What type of bond?

C-H

a)

nonpolar covalent bond

b)

polar covalent bond

c)

ionic bond

d)

metallic bond

6.

What type of bond?

Na-Cl

a)

nonpolar covalent bond

b)

polar covalent bond

c)

ionic bond

d)

metallic bond

7.

Which of the following is not a property of covalent molecules?

a)

non-lustrous, various colors

b)

brittle

c)

poor conductors of heat and electricity

d)

nonmetallic oxides are acidic and covalent

e)

form cations by gaining electrons

8.

Will bonds form between molecules at point A? Why or why not?

a)

no, the nuclei are too close and repel each other

b)

no, the distance between the atoms is too greate

c)

yes, the bonds form when the energy between them is greatest

d)

no, the bond will only form when energy is zero

9.

Will bonds form between molecules at point D? Why or why not?

a)

no, the nuclei are too close and repel each other

b)

no, the distance between the atoms is too greate

c)

yes, the bonds form when the energy between them is greatest

d)

no, the bond will only form when energy is zero

10.

Of C=C, C=C, or C-C, which has the shortest bond length and greatest bond energy?

a)

C-C

b)

C=C

c)

C=C

11.

Bond energy (aka bond enthalpy)

a)

energy required when breaking a bond, or energy released when a bond is formed

b)

number of chemical bonds

c)

distance between two atomic nuclei in angstroms or picometers

12.

Bond order

a)

energy required when breaking a bond, or energy released when a bond is formed

b)

number of chemical bonds

c)

distance between two atomic nuclei in angstroms or picometers

13.

A potential energy diagram for H2, HBr, and Br2 was created but not labeled. Which line corresponds with H2?

a)

A

b)

B

c)

C

14.

Which of the following bonds will be most polar?

a)

Si-O

b)

C-H

c)

O-O

d)

B-F

15.

What hybridization exists for the compound CH2O?

a)

sp3

b)

sp2

c)

sp

d)

there is no hybridization

16.

Which is the correct Lewis structure for the compound CH2O?

a)
b)
c)
d)
17.

A resonance structure for CH2O is shown in the picture. Why is this not the best resonance structure?

a)

because the carbon only has 6 valence electrons

b)

because the oxygen doesn't have a full octet

c)

because the formal charges of oxygen and carbon aren't equal to zero

d)

because the hydrogens don't have a full octet

18.

Which color graph would be the plot for the molecule with the shortest bond length?

a)

purple graph

b)

blue graph

c)

red graph

19.

What is the VSEPR theory used to predict?

a)

Bond Strength

b)

Polarity

c)

Molecular Shape

d)

Electronegativity

20.

Draw the Lewis Dot structure for ICl2- and determine its predicted molecular geometry.

a)

see-saw

b)

trigonal bipyramidal

c)

linear

d)

bent

21.

What is the hybridization of a linear molecule?

a)

sp

b)

sp2

c)

sp3

d)

sp3d

22.

Which of the following is octahedral?

a)

SCl6

b)

XeI4

c)

NBr5

d)

CH4

23.

Which of the following hybrid orbitals is used by the central atom for bonding in CO32-?

a)

sp2

b)

sp3

c)

sp3d

d)

sp3d2

24.

Molecule CO2

a)

undergoes sp2 hybridisation

b)

has 2 σ bond and 2 π bond

c)

undergoes sp3d hybridisation

d)

is trigonal planar molecule

25.

What is the hybridization of the Carbon atom indicated by the arrow?

a)

sp hybridization

b)

sp2 hybridization

c)

sp3 hybridization

d)

dsp3 hybridization

26.

Name the type of bonding in which the electrons are shared.

a)

Ionic bonding

b)

Covalent bonding

c)

Metallic bonding

27.

The energy required to break the bonds between two covalently bonded atoms

a)

bond dissociation energy

b)

activation energy

c)

none of these

28.

Which of the following is the correct Lewis Structure for the molecule fluorine (F2)?

a)

A

b)

B

c)

C

d)

D

29.

what type of bond is the strongest

a)

single

b)

Double

c)

coordination

d)

triple

30.

In covalent bonding, electrons are

a)

shared

b)

transferred

c)

wiped out

31.

What is the correct Lewis Structure for ammonia (NH3)

a)
b)
c)
d)
32.

What are valence electrons?

a)

sum of the protons and neutrons

b)

protons minus electrons

c)

electrons in the inner shells

d)

electrons in the outer shell

33.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

34.

Which of the following best describes why molecules have certain geometries

a)

The unshared pairs of electrons & the bonding pairs of electrons on the central atom are experiencing repulsive forces

b)

The unshared pairs of electrons & the bonding pairs of electrons on the central atom are experiencing attractive forces

c)

The unshared pairs of electrons & the bonding pairs of electrons on the largest atom are experiencing repulsive forces

d)

The bonding pairs of electrons on the atom with the most unshared pairs are experiencing repulsive forces

35.

 A lone pair is defined as

a)

A pair of bonding electrons

b)

One non-bonding electron

c)

A pair of non-bonding electrons

d)

A pair of electrons on the central atom

36.

How many regions of electron density surround the carbon in carbon tetrachloride?

a)

1

b)

2

c)

3

d)

4

37.

Will this molecule be polar or nonpolar? PH3

a)

polar

b)

nonpolar

38.

Which Lewis Dot Model drawing correctly shows an O2 molecule?

a)
b)
c)
d)
39.

When you have Br-Br, what is the polarity?

a)

Polar

b)

nonpolar

c)

Ionic

40.

When you have H-Cl, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

41.

Which of the following molecules, based on the elements present, would be most polar?

a)

HF

b)

H2

c)

HCl

d)

HBr

42.

Which molecule contains bonds with a GREATER polarity?

a)

HCl

b)

CCl4

43.

Partial charges like the ones shown here are called:

a)

dipoles

b)

deltas

c)

ions

d)

magnetic poles

44.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

45.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

46.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

47.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

48.

A difference in electroegativity of 2.1 will result in what type of bond?

a)

ionic

b)

covalent

c)

polar covalent

49.

The type of bond that two elements will form is dependent on

a)

the atomic radius of each atom

b)

the ionization enegry of each atgr

c)

the number of valence electrons of each atom

d)

the electronegativity of each atom

50.

A difference in electronegativity of 0.8 will result in what type of bond?

a)

ionic

b)

covalent

c)

polar covalent

51.

The greater the difference in electronegativity, the

a)

greater the ionic character

b)

the stronger the bond

c)

the longer the bond length

d)

the higher the bond energy

52.

The energy it takes to break a covalent bond is called

a)

bond energy

b)

lattice energy

c)

kinetic energy

d)

electronegativity

53.

The bond length describes the distance between two atoms where the potential energy is

a)

highest

b)

lowest

c)

same

54.

A double bond is longer and less stable than a single bond.

a)

True

b)

False

55.

To draw a Lewis dot model you have to know

a)

the period an element is in

b)

the group an element is in

c)

the number of valence elcctrons an atom has

d)

the number of energy levels an atom has

56.

Which elements do NOT get octets when covalently bonding?

a)

H

b)

B

c)

C

d)

N

57.

Electrons that are not involved in bonding are called (a)   .

58.

The dotted lines in this structure represent

a)

a hybrid bond that is halfway between a double and single bond

b)

equivalent resonance structures

c)

delocalised electrons

59.

When there is more than one possible Lewis structure, (a)   helps you determine the most stable one.

60.

What is the formal charge on the sulfur atom?

(a)  

61.

What is the formal charge on the top oxygen atom?

(a)  

62.

What is the formal charge on the oxygen atom on the right?

(a)  

63.

Draw the net dipole on this molecule.

64.
Calculate the Formal Charge for the Oxygen Labeled 1 
a)
-1
b)
+1
c)
0
d)
-2
65.
Calculate the Formal Charge for the Nitrogen
a)
-1
b)
+1
c)
0
d)
-2
66.
Calculate the Formal Charge for the Oxygen Labeled 2 
a)
-1
b)
+1
c)
0
d)
-2
67.
What is the formal charge for each of the Fluorine atoms
a)
-1
b)
+1
c)
0
d)
+2
68.
What is the formal charge for Xenon
a)
-1
b)
+1
c)
0
d)
+2
69.
What is the formal charge for Selenium
a)
+1
b)
-1
c)
0
d)
-2
70.

How many sigma bonds are found in the molecule shown?

a)

3

b)

9

c)

13

d)

14

71.

How many pi bonds are found in the molecule shown?

a)

2

b)

3

c)

6

d)

9

72.

Describe the hybridization of the carbon on the far right containing a triple bond.

a)

sp

b)

sp2

c)

sp3

73.

Identify the IMF between the two iodine molecules shown.

a)

London Dispersion Force

b)

Hydrogen bonding

c)

dipole-dipole

d)

ion-dipole

74.

Identify the IMF occurring between Na+ and H2O, as shown in the diagram.

a)

London Dispersion Force

b)

Ion-Dipole

c)

Dipole-Dipole

d)

Hydrogen bonding

75.
What is the orbital hybridization for a molecule with a trigonal bipyramidal parent geometry?
a)

sp

b)

sp2

c)

sp3

d)

sp3d

76.
What is the orbital hybridization for a molecule with a linear parent geometry?
a)

sp

b)

sp2

c)

sp3d

d)

sp3d2

77.
What is the orbital hybridization of S in this molecule?
a)

sp2

b)

sp3

c)

sp3d

d)

sp3d2

78.
A triple bond includes 2 sigma bonds and 1 pi bond.
a)
True
b)
False
79.
How many pi bonds does this molecule have?
a)

0

b)

1

c)

2

d)

3

80.
A sigma bond rotates more easily than a pi bond.
a)
True
b)
False
81.

Classify the following molecule.

a)

polar

b)

nonpolar

82.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

83.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

84.

Classify the following molecule.

a)

polar

b)

nonpolar

85.

Does this compound have a dipole moment?

a)

Yes

b)

No

86.

A nonpolar compound can only contain nonpolar bonds.

a)

True

b)

False

87.

What can cause molecules to lack a dipole moment even if they possess polar bonds?

a)

The presence of only nonpolar bonds

b)

The random arrangement of polar bonds

c)

The symmetrical arrangement of polar bonds that cancel each other out

d)

The complete absence of bonds

88.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
89.

This is an example of a(n) (a)   .

90.

Which intermolecular force requires hydrogen and one of the following: nitrogen, oxygen, fluorine?

a)

Dipole-dipole

b)

Hydrogen bonding

c)

London dispersion forces

91.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
92.

What kind of force is the arrow pointing to?

a)

Intramolecular Force

b)

Intermolecular Force

93.
Does NH3 have hydrogen bonding?
a)
yes
b)
no
94.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

95.
London forces are stronger in heavier atoms or molecules, and weaker in lighter atoms or molecules.  Which of these has the strongest London forces?
a)
F2
b)
Br2
c)
I2
d)
Cl2
96.
What information do we look for on the periodic table if we  want to examine intermolecular forces?
a)
atomic mass
b)
atomic number
c)
electronegativity
d)
ionization 
97.
Type of intermolecular force present in I2, Br2, and Cl2.
a)
dipole dipole
b)
H-bond
c)
dispersion
d)
metallic
98.
H2S has what kind of intermolecular force?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
99.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
100.
Intermolecular force present in Cl2?
a)
dipole dipole
b)
H-bond
c)
dispersion
d)
metallic
101.

In a polar covalent bond, the electrons gather around...

a)

Mostly the atom with the greatest electronegativity

b)

The atom with the lowest electronegativity

c)

Each atom equally

d)

Only the atom with the greatest electronegativity

102.

In a nonpolar covalent bond, the electrons gather around...

a)

Mostly the atom with the greatest electronegativity

b)

The atom with the lowest electronegativity

c)

Each atom Equally

d)

Only the atom with the greatest electronegativity

103.
What type of intermolecular force is the strongest?
a)
Hydrogen bonding
b)
Dipole-dipole attractions
c)
London forces
104.
In general, substances with stronger intermolecular forces have ________ boiling points than those with weaker forces
a)
Higher
b)
Lower
c)
Forces and boiling point are not related
105.
Which of the following has the highest boiling point?
a)
H2
b)
NH3
c)
N2
d)
O2
106.

Which of the following properties of substances is NOT determined by IMFs?

a)

Melting/boiling point

b)

Vapor pressure

c)

Density

d)

Shape and color

107.

Match the Following

a)

Hydrogen Bond

1.

Present in Polar involving N, O, F

b)

London Dispersion Forces

2.

Present in both Polar and Non Polar Molecules

c)

Dipole- Dipole

3.

Polar Substances only

108.
Rank these in order of strength:
covalent bond
London forces
hydrogen bond
dipole-dipole attraction
a)

dipole-dipole>covalent bond>hydrogen bond>London

b)

London>dipole-diple>hydrogen bond>covalent bond

c)

covalent bond>hydrogen bond>dipole-dipole>London

d)

hydrogen bond>dipole-dipole>London>covalent bond

109.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

110.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

111.
Which of the following does NOT contain hydrogen bonding?
a)
NH3
b)
H2O
c)
CF4
d)
HOF
112.
Which IMF contains a temporary dipole?
a)
London Dispersion Forces
b)
Dipole Dipole
c)
Hydrogen Bonding
d)
Both London Dispersion Forces and Dipole Dipole
113.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

114.

Chromatography separates solutions on the basis of _____ while distillation separates solutions on the basis of ______.

a)

IMFs; solubility

b)

solubility; conductivity

c)

IMFs; boiling point

d)

boiling point; solubility

115.

In paper chromatography, if water is the mobile phase, what kind of substance will move up the farthest?

a)

polar substance

b)

non polar substance

116.

“More polarizable” refers to which Intermolecular Force?

a)

hydrogen bonding

b)

london dispersion

c)

dipole dipole

117.

List ALL the Intermolecular forces that exist in PCl3

a)

hydrogen bonding, london dispersion

b)

london dispersion, hydrogen bonding, dipole dipole

c)

london dispersion, dipole dipole

d)

london dispersion

118.

Name a property that decreases as Intermolecular Forces increase.

a)

Vapor pressure

b)

Conductivity

c)

Melting point

d)

Solubility

119.

Name a property that increases as Intermolecular Forces increase.

a)

Vapor pressure

b)

Conductivity

c)

Melting point

d)

Solubility

120.

What causes gas pressure?

a)

large space between the molecules

b)

random motion of particles

c)

collisions with the walls of the container

121.

Polar substances will dissolve in what type of substances?

a)

Ionic

b)

Polar

c)

Non-Polar

d)

Metallic

122.

"Like dissolves like" is the easy way to remember the previous question, but what molecular property is causing that to be true?

a)

Boiling Point

b)

IMFs

c)

Melting Point

d)

Vapor Pressure

123.
The physical separation of mixtures into individual components is..
a)
chromatography
b)
opacity 
c)
latent
d)
trace evidence 
124.

Ink can be separated by a method of -----------------------------------------------

a)

distillation

b)

filtration

c)

chromatography

d)

sedimentation

125.
On the chromatogram given -------------- is mixture.
a)
red
b)
orange
c)
green
d)
black
126.
A pure substance shows ------------------ spot on chromat gram
a)
0
b)
1
c)
2
d)
3
127.
A student extracts the colour from some green smarties and uses paper chromatography to separate components colours. She finds blue has a Rf =0.38 and yellow Rf =0.75 this suggests 
a)
the yellow is more strongly adsorbed onto the stationary phase and is less solublein the mobile phase.
b)
the yellow is more strongly adsorbed onto the stationary phase and is more soluble in the mobile phase.
c)
the blue is more strongly adsorbed onto the stationary phase and is less solublein the mobile phase.
d)
the blue is more strongly adsorbed onto the stationary phase and is less solublein the mobile phase.
128.
A high Rf value indicates strong
a)
strong affinity to the stationary phase
b)
strong affinity to the mobile phase
c)
no affinity to the stationary phase
d)
 no affinity to the stationary phase
129.
The Rf value  for the blue component is 
a)
0.3
b)
0.7
c)
10
d)
3
130.
The Rf value  for the red component is 
a)
0.3
b)
0.7
c)
10
d)
7
131.
Which plant species has plant pigments most similar to those in A?
a)
B
b)
C
c)
D
132.
Why must the base line be drawn in pencil and not pen?
a)
a) Pencil is good at keeping substances in place.
b)
b) Pencil is soluble in water
c)
c) Pencil is insoluble in water
d)
d) Pencil is not coloured
133.

In paper chromatography, the LEAST soluble solute ____.

a)

does not move from the start point

b)

stays closest to the start point

c)

travels furthest away from the start point

d)

can be found in the middle of the chromatogram

134.
In chromatography, if a solute does not separate and remains on the start line ....
a)
the solute is insoluble in the solvent
b)
the solute is soluble in the solvent
c)
the solvent is insoluble in the solute
d)
the solvent is soluble in the solute
135.
Whose blood was found at the crime scene?
a)
John
b)
Lisa
c)
Bob
d)
Sure
136.

Octane (C8H18- nonpolar hydrocarbon) and water

a)

Soluble (miscible)

b)

Insoluble (immiscible)

c)

Partially soluble

137.
The diagram below shows a chromatogram obtained when a sample X was analysed together with four other known dyes P, Q, R and S. Dye Q was known to cause cancer. Which of the following dye(s) is/are safe for use?
a)
P only
b)
S only
c)
P and S
d)
P and X
138.
In Chromatography the retardation factor Rf are used for identification of components. A low  Rf and a high Rt (retention time) mean the component has a 
a)
greater affinity to the stationary phase in both TLC and HPLC.
b)
greater affinity to the stationary phase in TLC but a greater affinity for the mobile phase in HPLC
c)
greater affinity to the mobile phase in TLC but a greater affininty for the stationary phase in HPLC
d)
greater affinity to the mobile phase in  both TLC  and HPLC
139.

Which molecule will have hydrogen bonds with other molecules in the sample?

a)

a) CO2

b)

b) HCN

c)

c) C2H2

d)

none of the above

140.
Which of the following compounds has the highest boiling point?
a)
CH3CH2CH3
b)
CH3CH2CH2CH3
c)
CH3CH3
d)
CH4
141.
Which of the following compounds will have the lowest boiling point?
a)
CH4
b)
CHCl3
c)
CH3CH2OH
d)
NH3
142.
What best explains the difference in melting points between Cl2 (-101.5) and F2 (-219)?
a)
Increased mass (polarizability) of chlorine
b)
Increased electronegativity of fluorine
c)
Increased number of electrons in chlorine
d)
Decrease metallic character of fluorine
143.

Which of the following will have the highest heat of vaporization?

a)

CH4

b)

C2H6

c)

C3H8

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