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Chemistry II Final Review

Total questions: 115

Worksheet time: 5hrs 37mins

Name
Class
Date
1.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
2.

If an atom of Sodium has a mass number of 23, it will have...

a)

23 protons

b)

11 neutrons

c)

12 protons

d)

12 neutrons

3.
an element will always have the same number of 
a)
neutrons
b)
protons
c)
isotopes
d)
atoms
4.
Isotopes are elements with a different amount of
a)
protons
b)
neutrons
c)
electrons
d)
atoms
5.

Which scientist developed this model?

a)

Dalton

b)

Thomson

c)

Rutherford

d)

Bohr

6.
4.35% of all X atoms have a mass of 39.946 amu. 83.79% have a mass of 41.941 amu, 9.50% have a mass of 42.941 amu, and 2.36% have a mass of 43.939 amu. What is the average atomic mass of atom X?
a)
41.97 amu
b)
42.19 amu
c)
10.43 amu
d)
40.04 amu
7.

The​ (a)   of a wave is the distance between adjacent crests (or any two analogous points) and is measured in units such as meters, micrometers, or nanometers.

Choose from the below words
wavelength
frequency
8.

Emission spectra (bright line spectra) are created when electrons move from ___.

a)

higher to lower energy levels.

b)

lower to higher energy levels.

c)

s orbitals to p orbitals.

d)

one atom to a different atom.

9.

In which state does an electron have the least amount of energy?

a)

Excited state

b)

Ground state

c)

Orbital

d)

Bohr model

10.

Match the type of orbital with the value of the angular momentum quantum number, l.

a)

s

1.

l = 0

b)

p

2.

l = 1

c)

d

3.

l = 2

d)

f

4.

l = 3

11.

Match the quantum number with what it tells us.

a)

Principal Quantum Number

1.

which shell

b)

Angular momentum quantum number

2.

which shape

c)

Magnetic quantum number

3.

which orbital

d)

Spin quantum number

4.

spin up or spin down

12.

Which of the following sets of quantum numbers (n, l, ml, and ms) describes the valence electron of Na?

a)

2, 1, 0, -½

b)

2, 0, 0, -½

c)

3, 1, 1, +½

d)

3, 0, 0, +½

13.

What is the noble gas configuration for 1s2 2s2 2p6 3s2?

a)

[He] 3s2

b)

[Ne] 3s2

c)

[Ar] 3s2

d)

[Ar] 4s2

14.

In LiH, hydrogen has an oxidation number of

a)

-1

b)

+1

c)

-2

d)

+2

15.

Name the compound.

a)

copper sulfate

b)

copper (I) sulfate

c)

copper (II) sulfate

d)

copper monosulfate

16.

Give the chemical formula. Strontium Bromide

a)

Sr2BrSr_2Br  

b)

SrBr2SrBr_2  

c)

SrBrSrBr  

d)

Sr2Br2Sr_2Br_2  

17.

Give the formula. Lead(IV) Carbonate

a)

PbCO3PbCO_3  

b)

Pb(CO3)2Pb\left(CO_3\right)_2  

c)

Pb(CO3)1Pb\left(CO_3\right)_1  

d)

Pb(CO3)4Pb\left(CO_3\right)_4  

18.

Why do elements form compounds?

a)

to change properties

b)

to lose protons

c)

to become an isotope

d)

to become stable

19.

CO32-

a)
bicarbonate
b)
carbonite
c)
carbonate
d)
chlorite
20.

C2H3O2-

a)
Ammonium
b)
acetite
c)
acetate
d)
arsenate
21.
Cyanide
a)
CrO4-2
b)
Cr2O4-2
c)
CO3-2
d)
CN-
22.

Perchlorate

a)

ClO

b)

ClO4 -2

c)

ClO4 -1

d)

NaCl

23.

Match the following to the correct type of bonding.

a)

HF

1.

Acid

b)

Na2SO4

2.

Ionic

c)

SF6

3.

Molecular Covalent

d)

Diamonds

4.

Network Covalent

e)

Fe3N2

5.

Transition Metal Ionic

24.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
25.
All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces.  Which of these has ONLY London forces?
a)
I2
b)
NH3
c)
OCl2
d)
SH2
26.
You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.
a)
SO
b)
SO2
c)
SO3
d)
SO4
27.
What is the percentage of iron in iron(III)oxide?
a)
30%
b)
70%
c)
40%
d)
60%
28.

Binary acids have the prefix

a)

hydra

b)

hydro

c)

di

d)

hydride

29.

Name this molecule:

a)

methane

b)

ethane

c)

propane

d)

butane

30.

What is the name of this hydrocarbon?

a)

1 - butane

b)

1 - butene

c)

2 - butane

d)

2 - butene

31.

What chemical is this? (C5H10)

a)

Pentene

b)

Pentane

c)

Hexane

d)

Heptene

32.

What is the correct name for the alkyne shown?

a)

butyne

b)

1-butyne

c)

2-butyne

d)

1-methyl-1-propyne

33.

Is the name of doubled bonded, unsaturated hydrocarbons.

a)

Alkanes

b)

Alkenes

c)

Allkynes

d)

Tanins

34.

Is the name of single bonded, saturated hydrocarbons.

a)

Alkanes

b)

Alkenes

c)

Alkynes

d)

Tanins

35.

Is the name of triple bonded, unsaturated hydrocarbons.

a)

Alkanes

b)

Alkenes

c)

Alkynes

d)

Tanins

36.

What functional group is shown?

a)

amide

b)

ketone

c)

organic acid

d)

amine

37.

What is a functional group?

a)

Atoms or group of atoms that give specific characteristics to a molecule

b)

Group of molecules that make up a group of atoms

c)

Group of molecules that give specific characteristics to an atom

d)

Group of atoms that give specific characteristics to an element

38.
Name this structure.
a)
propanal
b)
propanol
c)
propanoic acid
d)
propanone
39.

What is the functional group of alcohols?

a)

–NH2

b)

–COOH

c)

–CHO

d)

–OH

e)

–NO2

40.
What is this functional group?
a)
ketone
b)
amide
c)
ether
d)
amine
41.
a)
amine
b)
ketone
c)
carboxylic acid
d)
ether
42.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
43.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
44.

What molecular geometry would PH3 have?

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Bent

d)

Linear

45.
Define the term resonance structure
a)
Delocalization of electrons in an atom
b)
Delocalization of π electrons within a molecule
c)
Spread of π electrons in an atom
d)
Spread of π electrons within a molecule
46.

This carbon atom went through ....

a)

sp hybridization

b)

sp2 hybridization

c)

sp3 hybridization

d)

dsp3 hybridization

47.

What is the hybridization of a linear molecule?

a)

sp

b)

sp2

c)

sp3

d)

sp3d

48.

For a reaction 2A + B --> 2C, with the rate equation:

Rate = k [A]2 [B]

a)

The order with respect to A is 1 and the order overall is 1

b)

The order with respect to A is 2 and the order overall is 2

c)

The order with respect to A is 2 and the order overall is 3

d)

The order with respect to B is 2 and the order overall is 3

e)

The order with respect to B is 2 and the order overall is 2

49.

Given the following information.

a)

Rate = k[NH4+][NO2-]

b)

Rate = k[NH4+]2[NO2-]2

c)

Rate = k[NH4+]2[NO2-]

d)

Rate = k[NH4+][NO2-]2

e)

none of the above

50.
What is the rate exponent for A?
a)
0
b)
1
c)
2
51.

A substance's heating curve is shown in the graph. What is its boiling point? (Diagram B)

a)

100 C

b)

60 C

c)

80 C

d)

20 C

52.

Moving left to right across the diagram, are the particles moving faster or slower as time goes on? (Diagram F)

a)

Faster

b)

Slower

53.

What letter on the diagram represents a substance only in the liquid?

a)

A

b)

B

c)

C

d)

D

54.

What happens along the AC line?

a)

Melting/Freezing

b)

Boiling/Condensing

c)

Boiling/melting

d)

freezing/condensing

55.
N2 +  3H2 → 2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)
6
b)
2
c)
3
d)
1
56.
CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
a)
13.7 mol
b)
2.75 mol
c)
6.11 mol
d)
6.85 mol
57.

Charles' Law States...

a)

As Volume goes up temperature goes up 

b)

As Pressure goes down volume goes down 

c)

As Pressure goes up volume goes down

d)

As Pressure goes up temperature goes up

58.

Boyle's law : The pressure and volume of a gas show a _____ relationship.

a)

Inverse

b)

Direct

59.

Boyle's PV law : When _______ is held constant, the pressure and volume of a gas are ________ proportional

a)

temperature, equally

b)

temperature, inversely

c)

mass, equally

d)

mass, inversely

60.

What is the Standard for Temperature and Pressure?

a)

273 K and 1 atm

b)

273 C and 1 kPa

c)

273 F and 1 mmHg

d)

273 K and 1 Torr

61.

The pressure on a tank containing 0.3 moles of oxygen is 4.5 atm, and the temperature is 150 K. What is the volume of the gas?

(R = 0.0821)

a)

0.821 L

b)

8.21 L

c)

82.1 L

d)

821 L

62.

If you have 40 L of a gas at 6 atm, and 275K, how many moles will you have?

(R = 0.0821)

a)

10.6 mol

b)

0.1 mol

c)

150.5 mol

d)

81.2

63.

A sealed flask contains 1 mole of hydrogen and 3 moles of nitrogen at 20° C. If the total pressure is 400 torr, the partial pressure of the hydrogen is

a)

100 torr

b)

200 torr

c)

300 torr

d)

400 torr

64.

A rubber tire holds 2.3 moles of CO2 at a temperature of 273 K. The volume of the tire is 8 L. What is the Pressure?

(R = 0.0821)

a)

6.4 atm

b)

412.4 atm

c)

43.5 atm

d)

3.1 atm

65.

Three gases are mixed together in a container with a total pressure of 4.8 atm. If two of the gases have pressures of 1.2 atm and 1.5 atm, what is the pressure of the third gas?

a)

2.5 atm

b)

1.8 atm

c)

2.1 atm

d)

1.3 atm

66.

Which will travel faster: oxygen gas or helium gas?

a)

O2

b)

He

67.

Which of the following correctly describes diffusion?

a)

The movement of gases into an area of higher pressure, always

b)

The movement of gases into a vacuum

c)

a. The mixing of gases

d)

a. Both (a) and (b)

68.

Which of these is a property of acidic solutions?

a)

they taste sour

b)

they feel slippery

c)

they are in many cleaning products

d)

they taste bitter

69.

What are the products of a neutralization reactions

a)

water

b)

salt

c)

acid

d)

base

70.

According to Arrhenius acid-base theory, an acid ___.

a)

is an H+ acceptor

b)

is a H+ donor

c)

is a substance that produces H+ in water

d)

turns litmus paper blue

71.

Which reactant in the following equation is acting as a Brønsted-Lowry acid?

a)

ammonium

b)

ammonia

c)

hydroxide

d)

water

72.

CO32-(aq) + H2O(l) → HCO3-(aq) + OH-(aq)

Using the above reaction, which species is the conjugate base?

a)

CO32-

b)

H2O

c)

HCO3-

d)

OH-

73.

Choose the conjugate base of HNO3

a)

HNO3

b)

H2O

c)

H3O+

d)

NO3-

74.

For this reaction :


HA(aq) + H2O(l) ⇌ H3O+(aq) + A-(aq)


Which one can act as an acid ?

a)

HA(aq) and A-(aq)

b)

H2O(l) and H3O+(aq)

c)

HA(aq) and H3O+(aq)

d)

H2O(l) and A-(aq)

75.

dissociation of weak acid, HA, is represented by following equation :


HA(aq) + H2O(l) ⇌ H3O+(aq) + A-(aq)


The equilibrium constant for this reaction is represented by Ka . Which of the following equation represents expression of equilibrium constant, Ka?

a)
b)
c)
d)
76.

What is the [OH-] if the [H+] is 1.0 x 10-3 M?

a)

1.0 x 10-3 M

b)

6.02 x 10-23 M

c)

1.0 x 10-14 M

d)

1.0 x 10-11 M

77.
Calculate the pH of a 0.47M NH3 (Kb = 1.8 x 10-5) solution.
a)
2.54
b)
8.93
c)
5.07
d)
11.46
78.

Classify this acid.

a)

Arrhenius Acid

b)

Bronsted Lowry Acid

c)

Lewis Acid

79.

What is the definition of solubility?

a)
The ability of a substance to dissolve in another substance
b)
The ability of a substance to react with another substance
c)
The ability of a substance to change its state from solid to liquid
d)
The ability of a substance to change its color when heated
80.

What is a solute?

a)

A type of musical instrument

b)

A substance that is dissolved in a solution

c)
A mathematical solution
d)
A type of physical exercise
81.
How many grams of K2Cr2O7, are soluble in 100 g of water at 95 ºC?
a)
83 grams
b)
75 grams
c)
40 grams
d)
12 grams
82.
When 20 grams of KNO3 is dissolved in 100 grams of water at 80 ºC, the solution can be correctly described as:
a)
supersaturated
b)
saturated
c)
unsaturated
83.
Which is the correct net ionic equation for the reaction of AgNO3 and CaCl2?
a)
Ca2+(aq) +  2Cl- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
84.
Which of the following does NOT form a precipitate?
a)
Pb(NO3)2(aq) + 2KI(aq) →
b)
Sr(NO3)2 (aq) + K2SO4(aq) →
c)
AgNO3(aq) + Na2S(aq) →
d)
 Pb(NO3)2(aq) + AgNO3(aq) →
85.
What are the spectator ions in the reaction of sodium chloride with silver nitrate?
a)
silver and nitrate
b)
sodium and chloride
c)
sodium and nitrate
d)
silver and chloride
86.

The concentration of OH– in a saturated solution of Mg(OH)2 is 3.6 x 10–4 M. The Ksp of Mg(OH)2 is

a)

1.3 x 10–7

b)

4.7 x 10–11

c)

3.6 x 10–4

d)

2.3 x 10–11

87.

The correct mathematical expression for finding the molar solubility (X) of Sn(OH)2 is:

a)

2(X)3 = Ksp

b)

108(X)5 = Ksp

c)

4(X)3 = Ksp

d)

8(X)3 = Ksp

88.

The ______ the acid, the ______ its conjugate base.

a)

stronger, weaker

b)

stronger, stronger

89.

Identify the species reduced in the following reaction.


Fe(s) + 2 Ag+(aq) → Fe2+(aq) + 2 Ag(s)

a)

Fe

b)

Ag

c)

none of these

d)

None of the above

90.
What element is being Oxidized?
a)
N
b)
H
c)
O
d)
S
91.
What are the coefficients when the equation is balanced?
a)
2 + 3 --> 2 + 3 + 4
b)
1 + 3 --> 1 + 3 + 2
c)
2 + 4 --> 2 + 3 + 2
d)
1 + 1 --> 1 + 1 + 1
92.
What are the coefficients when the equation is balanced?
a)
1 + 1 + 1 --> 2 + 1 + 3
b)
2 + 2 + 2 --> 4 + 2 + 3
c)
1 + 2 + 1 --> 2 + 2 + 3
d)
1 + 1 + 1 --> 1 + 1 + 1
93.
What is oxidation number of Fe in FeO ?
a)
+2
b)
-2
c)
0
d)
+1
94.
What is oxidation number of O in O2 ?
a)
0
b)
-2
c)
+1
d)
+2
95.
What is the oxidation number of N in NO2-1?
a)
-3
b)
+4
c)
-2
d)
+3
96.
In the reaction
2Ca(s) + O2(g) --> 2CaO(s), calcium is __________
a)
Reduced
b)
Synthesized
c)
Oxidized
d)
None of the above
97.
Is calcium oxidized or reduced in the following reaction? 
2CaO--> 2Ca + O2
a)
Oxidized
b)
Reduced
98.
What reaction occurs at the anode?
a)
Ag+ + e- →Ag
b)
Ag → Ag+ + e-
c)
Ni2+ + 2e- → Ni
d)
Ni → Ni2+ + 2e-
99.
Which are examples of reduction?
a)
I and II
b)
I and III
c)
II and III
d)
I, II and III
100.

Galvanic cells convert

a)

mechanical energy in to electrical energy

b)

potential energy in to electrical energy

c)

electrical energy in to chemical energy

d)

chemical energy in to electrical energy

101.

In the following reaction

Sn+2 + 2Fe+3 --> Sn+4 + 2Fe+2,

the reducing agent is...

a)

Fe+3

b)

Sn+2

c)

Sn+4

d)

Fe+2

102.

From lowest entropy to highest entropy, the states of matter go in this order:

a)

solid -> liquid -> gas -> plasma

b)

plasma -> gas -> liquid -> solid

c)

gas -> plasma -> liquid -> solid

d)

solid -> liquid -> plasma -> gas

e)

It depends on the temperature of the object

103.

While running your kinetic energy converts to thermal energy. Which law does this refer to?

a)

0th law of thermodynamics

b)

1st law of thermodynamics

c)

2nd law of thermodynamics

d)

3rd law of thermodynamics

104.

Study the reaction below. Is it exothermic or endothermic?

H2 + Cl2 --> 2 HCl + 1845 kJ

a)

Exothermic Reaction

b)

Endothermic Reaction

105.

How do you calculate the Enthalpy of Reaction?

a)

ΔH = ΔHproducts - ΔHreactants

b)

ΔG = ΔH -TΔS

c)

ΔT = q / mC

d)

E = mc2

106.

Given the change of phase:

CO2(g) —> CO2(s)

As CO2(g) changes to CO2(s), the entropy of the system

a)

decreases

b)

increases

c)

remains the same

107.
The first law of thermodynamics states that the change in the internal energy of a system is equal to the difference in energy transferred to or from the system as heat and
a)
mass
b)
work done
c)
force
d)
pressure
108.
A reaction has a positive ΔH and a positive ΔS. Which of the following is true?
a)
It will be spontaneous at all temperatures.
b)
It will be nonspontaneous at all temperatures.
c)
It will be spontaneous at low temperatures.
d)
It will be spontaneous at high temperatures.
109.

Which combination of ΔH and ΔS NEVER has a spontaneous reaction?

a)

+ΔH and +ΔS

b)

+ΔH and -ΔS

c)

-ΔH and -ΔS

d)

-ΔH and +ΔS

110.

6. The formation ½ A2 + 2 B2 + C --> CAB4 has an enthalpy of formation of -104 kJ and a change in entropy of -60.8 J/K at 30 °C. What is the free energy and spontaneity of the reaction?

a)

-85.6 kJ, spontaneous

b)

-18.3 kJ, not spontaneous

c)

+18.3 kJ, spontaneous

d)

+85.6 kJ, not spontaneous

111.

What type of forces hold on an ionic lattice together?

a)

Electrostatic attraction forces

b)

Covalent bond

c)

Metallic bond

d)

Van der Waals forces

112.

The following properties are all characteristics of ionic compounds EXCEPT

a)

high melting and boiling points

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

113.
Electron Orbitals Overlap
a)
Ionic
b)
Covalent
114.
Does not normally conduct Electricity
a)
Ionic
b)
Covalent
115.
Electrically Reactive; Conducts Electricity when Dissolved in Water
a)
Ionic
b)
Covalent

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