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Timberlake Chemistry Chapter 10 Review Study Deck

Total questions: 112

Worksheet time: 2hrs 3mins

Name
Class
Date
1.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

2.

What is the goal of the Lewis Dot Structure?

a)

To determine the electron position.

b)

To show the element's valence electrons & bonding capabilities.

c)

To find the atomic mass of an element.

d)

To search for the number of electrons in an individual atom.

3.

How many valence electrons should Lithium have in its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

4.

How many valence electrons should Oxygen have in its Lewis dot model?

a)

5

b)

6

c)

7

d)

8

5.

How many valence electrons should Magnesium have in its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

6.

This is a correct dot diagram for nitrogen (N)

a)

true

b)

false

7.

This is a correct dot diagram for carbon (C)

a)

true

b)

false

8.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

9.

Which of these is incorrect?

a)
b)
10.

How many electrons should Boron have around its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

11.
How many valence electrons does chlorine (Cl) have?
a)
2
b)
5
c)
6
d)
7
12.
How many valence electrons does carbon (C) have?
a)
3
b)
4
c)
5
d)
6
13.
Which of these elements has 8 valence electrons?
a)
P
b)
Be
c)
O
d)
Ar
14.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
15.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
16.
Which is the correct structure for ammonia?
(Top picture is A, bottom picture is D.)
a)
Option A
b)
Option B
c)
Option C
d)
Option D
17.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
18.
What is the correct structure for BF3?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
19.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
20.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
21.
 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
22.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
23.
Which of the following shapes has an unshared pairs of electrons on the central atom? 
a)
Bipyramidal
b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
24.
Which molecule would have this molecular geometry?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
25.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
26.
What molecule could this be? 
a)
H2O
b)
CCl4
c)
PCl5
d)
NaCl
27.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
28.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
29.
Who could this be?
a)
H2O
b)
NH3
c)
CO2
d)
CH4
30.

What molecular geometry would PH3 have?

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Bent

d)

Linear

31.
A molecule with a lone pair on the central atom would have the same electron and molecular geometry
a)
True
b)
False
32.
Consider the molecule below.  Determine the molecular geometry at each of the 2 labeled carbons.
a)
C1 = tetrahedral, C2 = linear
b)
C1 = trigonal planar, C2 = bent
c)
C1 = bent, C2 = trigonal planar
d)
C1 = trigonal planar, C2 = tetrahedral
33.
What molecular shape is the structure shown here? (BCl3)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
34.
How many electrons are shared in a triple bond?
a)
6
b)
3
c)
6 pairs
d)
5
35.

What shape would this have?

a)

Trigonal planar

b)

Pyramidal

c)

Tetrahedral

d)

Bent

36.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
37.

The geometry of a molecule with 2 bonded pairs of electrons and 2 lone pairs of electrons, AB2E2

a)

Tetrahedral

b)

Trigonal Planar

c)

Bent

d)

Trigonal Pyramidal

e)

Linear

38.
*
a)
trigonal pyramid
b)
linear
c)
bent
d)
angular
39.

AB3 is a symbol for molecular shape __________________

a)

Tetrahedral

b)

Linear

c)

Trigonal planar

d)

Trigonal pyramidal

40.

The general formula for TETRAHEDRAL shape is __________

a)

AB2

b)

AB3

c)

AB4

d)

AB

41.
Which has the greater EN: 
N or C?
a)
C
b)
N
42.
Which has the greater EN: 
H or F?
a)
H
b)
F
43.
Put these in increasing order:
F, N, B
a)
B < N < F
b)
B < F < N
c)
N < F < B
d)
F < N < B
44.
Put these in increasing order:
C, H, and O
a)
H < C < O
b)
H < O < C
c)
O < C < H
d)
C < H < O
45.
Which has the greater EN: 
Cl or Al?
a)
Cl
b)
Al
46.
Choose the set that goes from lowest to highest electronegativity?
a)
Cu, Mg, Sr, Ca
b)
F, Cl, Br, Si
c)
Cs, Rb, Ca, Mg
d)
Zn, Cd, Ag, Cu
47.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
48.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
49.
The element with the lowest electronegativity in Period 3 is - 
a)
Na
b)
Cl
c)
Ar
d)
Mg
50.
 Which of the following generally applies to the noble gases? 
a)
high ionization energy, low electronegativity, high reactivity
b)
high ionization energy, high electronegativity, high reactivity
c)
low ionization energy, low electronegativity, low reactivity
d)
high ionization energy, low electronegativity, low reactivity 
51.
Elements closer to the noble gases have stronger attraction for electrons.
a)
True
b)
False
52.
Which of the following is the least electronegative element?
a)
oxygen
b)
potassium
c)
fluorine
d)
nitrogen
53.
Which of the following is the most electronegative element?
a)
nitrogen
b)
phosphorus
c)
arsenic
d)
lithium
54.
Put these in order of increasing electronegativity:
Se, S, and O
a)
Se < S < O
b)
Se < O < S
c)
O < S < Se
d)
S < Se < O
55.
Chlorine and Fluorine are both very electronegative, as they are both missing a single electron from their valence energy level.  Why is Fluorine more electronegative than Chlorine? 
a)
Fluorine has less energy levels.
b)
Chlorine has more electrons in its outer shell
c)
Fluorine has more protons.
d)
None of these
56.
What elements have zero electronegativity?
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
57.

Electronegativity (a)   as you go down a group.

58.

What does electronegativity do as you go across a period?

a)

decrease

b)

no pattern

c)

stay the same

d)

increase

59.

As you move across a period, the outer electrons are ________ to the nucleus, so the nucleus of the atom is ________ to attract electrons in a bond.

a)

closer, more able

b)

closer, less able

c)

further, less able

d)

further, more able

60.

The electrons in a POLAR covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

61.

The electrons in a NONPOLAR covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

62.

The electrons in an ionic molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

63.

In a polar covalent bond, the electrons spend more time and localize around the atom...

a)

with the Greatest Electronegativity

b)

with the Lowest Electronegativity

c)

Each atom Equally

64.

In a nonpolar covalent bond, the electrons spend more time and localize around the atom...

a)

with the Greatest Electronegativity

b)

with the Lowest Electronegativity

c)

Each atom Equally

65.

Partial charges are present in which type of bond(s)?

a)

Ionic

b)

Nonpolar Covalent

c)

Polar Covalent

d)

Both Polar Covalent and Ionic

e)

All covalent

66.

Partial charges like the ones shown here are called:

a)

dipoles

b)

deltas

c)

ions

d)

magnetic poles

67.

In this Lewis structure, the symbol above F means...

a)

electrons are being transferred to Fluorine

b)

electrons are less attracted to F than H

c)

electrons are more attracted to F than H

d)

Fluorine has formed an anion

68.
A bond with a partially negative end and a partially positive end is:
a)
ionic
b)
polar
c)
non-polar
d)
isometric
69.

Order the types of bonds based on the charge of their molecules. (lowest amount of charge to greatest)

a)

Polar Covalent --> Ionic --> Nonpolar Covalent

b)

Ionic --> Nonpolar Covalent --> Polar Covalent

c)

Nonpolar Covalent --> Polar Covalent --> Ionic

70.

Look at this covalent molecule as a whole. What type of molecule is it? (Is it symmetrical?)

a)

Polar

b)

Non-polar

c)

Ionic

71.

Look at this covalent molecule as a whole. What type of molecule is it? (Is it symmetrical?)

a)

Polar

b)

Non-polar

c)

Ionic

72.

Look at this covalent molecule as a whole. What type of molecule is it? (Is it symmetrical?)

a)

Polar

b)

Nonpolar

c)

Ionic

73.

Look at this covalent molecule as a whole. What type of molecule is it? (Is it symmetrical?)

a)

Polar

b)

Nonpolar

c)

Ionic

74.

Look at this covalent molecule as a whole. What type of molecule is it? (Is it symmetrical?)

a)

Polar

b)

Nonpolar

c)

Ionic

75.

Will PH3 form a polar or nonpolar bond based on the electronegativity difference ?

a)

polar

b)

nonpolar

c)

ionic

76.

A covalent bond usually forms between:

a)

a metal and a nonmetal

b)

either metals or nonmetals

c)

two metals

d)

two nonmetals

77.

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

a)

Polar

b)

nonpolar

c)

Ionic

78.

When you have Li-O, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

79.

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

a)

nonpolar

b)

polar

c)

ionic

80.
In which region(s) does temperature remain constant?
a)
Region 1, 3, & 5
b)
Region 2 & 4
c)
Region 1 only
d)
Region 1 & 2
81.
In which region(s) does temperature increase?
a)
Region 1, 3, & 5
b)
Region 2 & 4
c)
Region 1 only
d)
Region 1 & 2
82.
In which region(s) of the graph does a phase change occur?
a)
Region 1, 3, & 5
b)
Region 2 & 4
c)
Region 1 only
d)
Region 1 & 2
83.
In which region(s) of the graph would the substance only be in one phase?
a)
Region 1, 3, & 5
b)
Region 2 & 4
c)
Region 1 only
d)
Region 1 & 2
84.
Describe the substance between letters C and D. 
a)
Gas
b)
Liquid
c)
Melting
d)
Evaporating
85.
Between which points is the substance changing its state of matter?
a)
A-B only. 
b)
A-B, C-D, E-F
c)
B-C only. 
d)
B-C, D-E
86.

Thermal energy always moves:

a)

From a high temperature object to a lower temperature object.

b)

From a lower temperature object to a higher temperature object.

c)

From an object with lower kinetic energy to an object with higher kinetic energy.

d)

From an object of higher mass to an object of lower mass.

87.
The freezing and melting points of water are the same.
a)
True
b)
False
88.
What is water's freezing point?
a)
0 F
b)
32 C
c)
50 C
d)
0 C
89.
To determine the freezing and melting points use a 
a)
thermometer
b)
scale
c)
balance
90.
When does condensation happen?
a)
solid to liquid
b)
liquid to gas
c)
gas to liquid
d)
solid to gas
91.

Given the heating curve of a solid being heated at a constant rate, what is the boiling point of this substance?

a)

20°C

b)

50°C

c)

110°C

d)

170°C

92.

The melting point of the sample is

a)

-60 ºC

b)

-100 ºC

c)

60 ºC

d)

100 ºC

93.

NaCl(s) was heated up starting at an initial temperature of 0°C. The heating curve is shown in the picture. What is the melting point of this substance?

a)

0°C

b)

801°C

c)

1000°C

d)

1465°C

94.

Given the heating curve of water, what is happening to potential and kinetic energy during segment CD?

a)

the potential energy and kinetic energy both increase

b)

the potential energy increases while the kinetic energy decreases

c)

the potential energy is constant while the kinetic energy increases

d)

the potential energy increases while the kinetic energy is constant

95.
Energy is transferred as heat between two objects of ___________ temperatures. 
a)
differing
b)
same
96.
As the kinetic energy of the molecules in a substance increases, the temperature of the substance __________.
a)
increases
b)
decreases
97.
The measure of average kinetic energy of all the particles within an object is called ____________. 
a)
temperature
b)
conduction
c)
radiation
d)
heat 
98.
A high specific heat means...
a)
It heats up quickly with energy added
b)
It requires more energy to change temperature
99.
When you measure the temperature of hot soup, you are measuring the:
a)
thermal energy given off by the bowl
b)
specific heat of the bowl
c)
average kinetic energy of the particles in the soup
d)
thermal expansion of the particles in the soup
100.
The symbol for specific heat is .......
a)
c
b)
Q
c)
m
d)
t
101.
What  is the formula to calculate heat energy required to raise the temperature of any substance?
a)
Q=mc∆t
b)
Q=mc
c)
Q= ½mv
d)
m=QC
102.

A 15.75-g piece of iron absorbs 1086.75 joules of heat energy, and its temperature changes from 25°C to 175°C. Calculate the specific heat capacity of iron.

a)

0.46 J/goC

b)

1.654 J/goC

c)

2,567,446.875 J/goC

103.

How many joules of heat are needed to raise the temperature of 10.0 g of aluminum from 22.0°C to 55.0°C, if the specific heat of aluminum is 0.903 J/g°C?

a)

298 Joules

b)

0.003 Joules

c)

297 J/g°C

d)

0.003 J/g°C

104.

A 300.0 g piece of copper is heated and fashioned into a bracelet. The amount of energy transferred by heat to the copper is 66,300 J. If the specific heat of copper is 0.3845 J/g 0C, what is the change of the copper's temperature?

a)

641 °C

b)

7,650,000 Joules

105.
When a  piece of aluminum foil is taken out of the oven and cools from 100° to 50°, What is the change in temperature?
a)
50°
b)
0°
c)
100°
d)
150°
106.

The specific heat of aluminum is 0.9025 J/g°C. How much heat(Q) is released when a 10.0 g piece of aluminum foil is taken out of the oven and cools from 100.0° to 50.0°?

a)

451 J

b)

45.1 J

c)

400 J

107.
For a skillet, used for cooking, do you want a high or low specific heat
a)
High, so that it will need more energy to heat up
b)
Low, so that it will change temperature quickly
108.

20.0 g of water. specific heat of water is 4.184 J/g°C. temperature changes from 25.0° C to 20.0° C, how much heat energy (Q) moves from the water to the surroundings?

a)

418 Joules

b)

209 J

c)

83 J

d)

4.18 J

109.
If 200 grams of water is to be heated from 24.0° C to  100.0° C to make a cup of tea, what is the mass and what is the change in temperature?
a)
m=200g
∆t= 66
b)
m=200g
∆t=124
c)
m=200
∆t=100
d)
m=200g
∆t=76
110.

The specific heat(c) of copper is 0.38 J/g °C. What is the temperature change(∆t) when 100.0 Joules of heat(Q) is added to 20.0 grams?

a)

13 °C

b)

13.2°C

c)

13.16 °C

111.
Which of the following is NOT true about heat? 
a)
Heat moves from hot to cold
b)
Heat is a form of energy
c)
Heat cannot be transferred
d)
Heat makes molecules speed up 
112.
Conversion Factor 1kcal = ___ cal
a)
10
b)
100
c)
1000
d)
1/1000

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