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Chem 120 Review Chapts 6,7 & 8

Total questions: 131

Worksheet time: 1hrs 12mins

Name
Class
Date
1.
In the reaction represented by the equation N2 + 3H2 --> 2NH3, what is the mole ratio of nitrogen to ammonia?
a)
1:1
b)
1:2
c)
1:3
d)
2:3
2.
The Haber process for producing ammonia commercially is represented by the equation N2(g) + 3H2(g) --> 2NH3(g). To completely convert 9.0 mol hydrogen gas to ammonia gas, how many moles of nitrogen gas are required?
a)
1.0 mol
b)
2.0 mol
c)
3.0 mol
d)
6.0 mol
3.
For the reaction represented by the equation
2Na + 2H2O --> 2NaOH + H2, how many grams of hydrogen are produced if 120. g of sodium and 80. g of water are available?
a)
4.5 g
b)
45 g
c)
80. g
d)
200. g
4.
In most chemical reactions the amount of product obtained is
a)
equal to the theoretical yield.
b)
less than the theoretical yield.
c)
more than the theoretical yield
d)
more than the percentage yield
5.
For the reaction represented by the equation Cl2 + 2KBr --> 2KCl + Br2, calculate the percentage yield if 200. g of chlorine react with excess potassium bromide to produce 410. g of bromine.
a)
73.4%
b)
82.1%
c)
91.0%
d)
98.9%
6.
Which branch of chemistry deals with the mass relationships of elements in compounds and the mass relationships among reactants and products in chemical reactions?
a)
qualitative analysis
b)
stoichiometry
c)
entropy
d)
chemical kinetics
7.
In a chemical reaction
a)
the mass of the reactants equals the mass of the products.
b)
the mass of the products is greater than the mass of reactants.
c)
the number of atoms in the reactants and products must change.
d)
energy as heat must be added to the reactants.
8.
Which observation does not indicate that a chemical reaction has occurred?
a)
formation of a precipitate
b)
production of a gas
c)
evolution of heat and light
d)
change in total mass of substances
9.
How would oxygen be represented in the formula equation for the reaction of methane and oxygen to yield carbon dioxide and water?
a)
oxygen
b)
O
c)
O2
d)
O3
10.
When the equation Fe3O4 + Al --> Al2O3 + Fe is correctly balanced, what is the coefficient of Fe?
a)
3
b)
4
c)
6
d)
9
11.

In this reaction one substance breaks down into two or more separate substance

(a)  

12.

Present at the start of chemical reaction

(a)  

13.

In a (a)   reaction, one elements knowns another element out of a compound

14.

2Na+2H2O---------->2NaOH+H2O

(a)  

15.

Which of the following is an example of double displacement reaction?

a)

2Na+Cl2h---->2NaCl

b)

HCl+NaOH---->NaCl+H2O

c)

2HCl+Zn------>ZnCl2+H2

16.

Catalyst ________ the rate of chemical reaction.

a)

decreases

b)

increases

c)

normalize

17.

CaCO3------>CaO+CO2

a)

Synthesis

b)

Decomposition

18.

Two or more chemical bond together forming new substance

a)

Synthesis

b)

Decomposition

19.

In this reaction the compound must be a hydrocarbon which is made of hydrogen and carbon

a)

Oxidation

b)

Combustion

20.

Also called as metathesis

a)

Single Displacement

b)

Double Displacement

21.

C5H12+O2------>CO2+H2O

a)

Combustion

b)

Oxidation

c)

Synthesis

d)

Fermentation

22.

Synthesis reaction;

HCl + NaOH ----> (a)   +H2O

23.

Loss of electrons during reaction by a molecule

(a)  

24.

Which of the following is an example of fermentation?

a)

making salt

b)

pickled cucumber

c)

ice making

25.

Substance that is place at the right arrow of chemical reaction

(a)  

26.

Like charges (a)   one another

27.

Opposite charges (a)   one another

28.

The energy possessed by an object due to it's position

a)

Kinetic Energy

b)

Thermal energy

c)

Activation energy

d)

Potential energy

29.

The energy of motion

a)

Potential energy

b)

Activation energy

c)

Kinetic energy

d)

Thermal energy

30.

Possible units of energy(Select all that apply)

a)

Kelvin(K)

b)

Calories(cal)

c)

Nutritional calorie(Cal)

d)

Joules(J)

31.

Shorter Wavelength has a lower energy

a)

True

b)

False

32.

Higher frequency has a higher energy

a)

True

b)

False

33.

Distance between 2 corresponding points of a wave

(a)  

34.

Number of cycles of the wave per second

(a)  

35.

Height of the crest of the wave

(a)  

36.

Efinal-Einitial=n -2.18x10-18 J (1/n2final - 1/n2initial)

(a)  

37.

Each orbital can hold ____ electrons

a)

3

b)

2

c)

4

d)

1

38.

Another name for an energy level(n)

(a)  

39.

An S subshell holds how many orbitals?

a)

3

b)

4

c)

2

d)

1

40.

A P subshell holds how many orbitals?

a)

5

b)

4

c)

3

d)

1

41.

A D subshell holds how many orbitals?

a)

7

b)

5

c)

3

d)

1

42.
a)

D orbital

b)

S orbital

c)

P orbital

43.
a)

P orbital

b)

D orbital

c)

S orbital

44.
a)

P orbital

b)

S orbital

c)

D orbital

45.

How many electrons are in a D subshell?

a)

2

b)

5

c)

7

d)

10

46.

How many electrons are in an S subshell?

a)

5

b)

10

c)

2

d)

7

47.

What atom matches this electron configuration: 1s2 2s2 2p6 3s2

a)

Neon

b)

Magnesium

c)

Aluminum

d)

Potassium

48.

What matches this electron configuration: [Xe] 6s2 4f14 5d9

a)

Thallium

b)

Platinum

c)

Gold

d)

Mercury

49.

The atom with the largest atomic radius in Group 18 is -

a)

Rn

b)

He

c)

Kr

d)

Ar

50.

The atom with the largest atomic radius in Period 4 (row 4) is -

a)

Ca

b)

Kr

c)

Fe

d)

K

51.

The element with the smallest ionization energy in Period 6 is -

a)

Cs

b)

Tm

c)

Rn

d)

Os

52.

The energy required to remove electrons: (a)  

53.

Group B is known as the (a)  

54.

Families all have similar (a)  

55.

The ability of an atom to attract/accept electrons: (a)  

56.

Does C or N have a greater electronegativity?

(a)  

57.

Which sub shell is associated with more energy?

a)

2p

b)

2s

c)

3p

d)

1s

58.

What orbital is shaped like a sphere?

a)

s

b)

p

c)

d

d)

f

59.

What does the 1 in "1s" stand for?

(a)  

60.

How many electrons can a d sublevel hold?

a)

2

b)

5

c)

10

d)

14

61.

For each of the following sub levels, which is lowest in energy?

a)

3d

b)

4s

c)

4p

d)

5s

62.

The region of high probability of finding an electron is called an (a)  

63.

The electronic configuration of an element X is …3s23p5. Thus, element X is a _______ element.

a)

d-block

b)

Group 17

c)

Group 15

d)

Group 13

64.

Element X and Y are in the same short period of the Periodic Table, and have 2 and 5 electrons respectively in the outer shell. What is the most likely formula of the compound they formed?

a)

X2Y5

b)

X3Y2

c)

X2Y3

d)

X5Y2

65.

Which of the following is true about the Bohr Theory?

a)

Lone electron revolves round the nucleus in fixed circular path known as orbitals

b)

Excess energy in transition between ground and excited state is released in the form of heat.

c)

A. Energy of orbits increases with their decreasing distance from the nucleus.

d)

A. Bohr’s theory is applicable to hydrogen atom only.

66.

What is the total number of atomic orbitals in an atom with the principal quantum number n = 4?

a)

30

b)

20

c)

16

d)

23

67.

Which of the following is NOT correct about Pauli Exclusion Principles.

a)

Two electrons occupying the same orbital have same set of four quantum numbers

b)

An orbital holds two electrons with opposite spin direction

c)

An atomic orbital can contains maximum of two electrons

d)

Each electrons have different set of four quantum numbers

68.

What is the total number of unpaired electrons in sulphur atom?

a)

1

b)

2

c)

3

d)

4

69.

What is the valence electronic configuration of P3-?

a)

...3s23p3

b)

...3s2

c)

...3s23p6

d)

...4s24p3

70.

Which of the following quantum numbers describes about orientation of orbitals?

a)

Principal quantum number

b)

Spin quantum number

c)

Angular momentum quantum number

d)

Magnetic quantum number

71.

List the four quantum numbers that describe the fourth electron in 4p subshell.

a)

n =4, l = 1, ml = 0, ms= -1/2

b)

n =4, l = 2, ml = -1, ms= +1/2

c)

n =4, l = 1, ml = 0, ms= +1/2

d)

n =4, l = 1, ml = -1, ms= -1/2

72.

Calculate the frequency of electromagnetic radiation when an electron moves from the third shell to first shell with energy of 52.73 kJ/mol is emitted in the process.

a)

1.32 x 1014 s-1

b)

8.756 x 10-20 s-1

c)

8.756 x 1014 s-1

d)

7.95 x 10-34 s-1

73.

What family on the Periodic Table is non-reactive?

a)

Noble Gases

b)

Halogens

c)

alkali earth metals

d)

Wan Pablo

74.

Metals are on the...

a)

Left side of the Periodic table

b)

Right side of the Periodic Table

c)

Wan Pablo

75.

Zn's atomic number is...

a)

21

b)

30

c)

Wan Pablo

d)

40

76.

Sodium (Na) is on group 15. True or false?

a)

true

b)

False

c)

Wan Pablo

d)

Rick Astley

77.

Bromine (Br) is in which family?

a)

Wan Pablo

b)

Halogens

c)

Alkali metals

d)

Oxygen family

78.

Is Wan Pablo the son of Daddy Jebes? (Graham's suggestion)

a)

Yes, he's Wan Ebes Juilius Caesar Pablo

b)

No, he's adopted

79.

Carbon (C) is in group...

a)

1

b)

Wan Pablo

c)

14

d)

3

80.

Lithium (Li) is is group...

a)

6

b)

1

c)

16

d)

Wan Pablo

81.

Argon (Ar) is in which family?

a)

Wan Pablo

b)

Noble Gases

c)

Transition metals

d)

Bearer of charms

82.

Is Dimitrius Demarcus James John Brown Bartholomere III jr. Daddy Jebes?

a)

Yes, he is daddy Jebes, father of Wan Ebes Juilius Caesar Pablo.

b)

No, he's Graham cracker, right hand man of Wan Ebes Juilius Caesar Pablo.

83.

Electrons have a relative mass of…

a)

1

b)

0

c)

2

d)

very small

84.

What happens to the boiling points and melting points of Group 7 elements as you go down the group?

a)

They decrease

b)

They stay the same

c)

They increase

d)

They decrease and then level off

85.

Atoms are made from…

a)

electrons

b)

protons

c)

neutrons

d)

protons, neutrons and electrons

86.

In the plum pudding model, where were the electrons located?

a)

In the middle

b)

Around the outside

c)

Embedded throughout

d)

In shells

87.

The overall charge of an atom is 0 because…

a)

the number of protons and the number of neutrons are the same

b)

the number of neutrons and the number of electrons are the same

c)

the number of electrons and the number of protons are the same

d)

there is no charge on a proton

88.

When you describe a chemical reaction using a word equation you show the…

a)

reactants

b)

reactants and products

c)

products

d)

symbols

89.

Protons have a relative mass of…

a)

1

b)

0

c)

2

d)

very small

90.

How would you describe the reactivity of Group 1 metals?

a)

Very reactive

b)

Slightly reactive

c)

Not very reactive

d)

Unreactive

91.

How are elements in the modern periodic table arranged?

a)

In order of atomic mass

b)

In order of atomic number

c)

In alphabetical order

d)

By number of neutrons

92.

Later experiments proved that particles in the nucleus had a positive charge. These were named as…

a)

protons

b)

neutrons

c)

electrons

d)

atoms

93.

The nuclear model showed that most of the mass of an atom can be found in the…

a)

centre of the atom

b)

outside of the atom

c)

left-hand side of the atom

d)

right-hand side of the atom

94.

How can the reactivity of the noble gases be described?

a)

Unreactive

b)

Very reactive

c)

More reactive

d)

Less reactive

95.

Which transition metals are commonly used as catalysts?

a)

Iron

b)

Platinum

c)

Palladium

d)

All of the metals listed

96.

Group 1 metals are also known as…

a)

acidic metals

b)

alkali metals

c)

soluble metals

d)

insoluble metals

97.

How did Mendeleev overcome the problems with the early periodic table?

a)

By arranging elements alphabetically

b)

By leaving gaps

c)

By making it up

d)

All of the ways listed

98.

Niels Bohr suggested that ___________ orbited the nucleus.

a)

protons

b)

neutrons

c)

electrons

d)

protons and neutrons

99.

The properties of a compound compared to the properties of the individual elements are…

a)

different

b)

the same

c)

similar

d)

not changed

100.

How does the reactivity of Group 1 metals change as you go down the group?

a)

It decreases

b)

It stays the same

c)

It increases

d)

It decreases and then levels off

101.

How are electrons arranged around the nucleus?

a)

Circles

b)

Shells

c)

Rings

d)

Stacks

102.

Why do equations using formulae need to be balanced?

a)

To make it fair

b)

So it's right

c)

The number of atoms need to be the same for reactants and products

d)

The number of protons need to be the same

103.

Which separation method is used to separate liquids based on their boiling points?

a)

Distillation

b)

Fractional distillation

c)

Filtering

d)

Crystallisation

104.

Protons have an electric charge of…

a)

+1

b)

0

c)

-1

d)

2

105.

A mixture contains two or more elements or compounds that are…

a)

chemically combined

b)

not chemically combined

c)

mixed together

d)

glued together

106.

The overall charge of an atom is…

a)

+1

b)

0

c)

-1

d)

2

107.

How were the elements originally arranged in the early periodic table?

a)

By atomic weights

b)

By number of protons

c)

By number of electrons

d)

By their reactivity

108.

A compound is defined as being…

a)

two or more atoms of different elements chemically combined together

b)

two or more atoms of different elements glued together

c)

an atom of one element chemically bonded to other atoms of the same element

d)

atoms that have reacted

109.

Elements contain…

a)

the same type of element

b)

the same type of atom

c)

the same type of proton

d)

the same type of charge

110.

Later experiments proved that the nucleus also contained __________ as well as protons.

a)

atoms

b)

neutrons

c)

electrons

d)

elements

111.

Isotopes are atoms of an element with a different number of…

a)

neutrons

b)

electrons

c)

protons

d)

protons and electrons

112.

Which separation method is used to separate a soluble solid from a solution?

a)

Crystallisation

b)

Filtering

c)

Distillation

d)

Chromatography

113.

What word or phrase can be used to describe the outer shell of the noble gases?

a)

Half full

b)

Nearly full

c)

Full

d)

Bursting

114.

Relative atomic mass is an average of the amount of…

a)

isotopes

b)

electrons

c)

protons

d)

neutrons

115.

The plum pudding model suggested that atoms were like a ball. What was this ball made of?

a)

Negative charge

b)

Positive charge

c)

Protons

d)

Electrons

116.

What is the maximum number of electrons found in full electron shells?

a)

2,2,8,8

b)

2,2,8

c)

2,8,8,8

d)

2,6,8,2

117.

Where are metals found on the periodic table?

a)

Left

b)

Left and middle

c)

Right

d)

Right and middle

118.

What does the group number in the periodic table tell us about the elements within that group?

a)

The elements all have the same number of neutrons

b)

The elements all have the same number of electrons

c)

The elements all have the same number of electrons in their outer shell

d)

The elements all have the same atomic mass

119.

Electrons have an electric charge of…

a)

+1

b)

0

c)

-1

d)

2

120.

The mass number of an atom is the number of…

a)

protons

b)

neutrons

c)

protons and neutrons

d)

electrons

121.

Atoms of different elements contain a different number of…

a)

electrons

b)

neutrons

c)

protons and neutrons

d)

protons

122.

The number of electrons in an atom is the same as…

a)

the number of protons plus the number of neutrons

b)

the number of neutrons

c)

the number of protons

d)

the number of neutrons minus the number of protons

123.

What happens to the boiling points of noble gases as you go down the group?

a)

They decrease

b)

They stay the same

c)

They become solids

d)

They increase

124.

Where are non-metals found on the periodic table?

a)

Left

b)

Left and middle

c)

Right

d)

Right and middle

125.

Neutrons have an electric charge of…

a)

+1

b)

0

c)

-1

d)

2

126.

Which separation method is used to separate solvents from a solution?

a)

Crystallisation

b)

Distillation

c)

Filtering

d)

Fractional distillation

127.

The number of electrons in an atom can be found by looking at the…

a)

atomic number

b)

atomic mass

c)

symbol

d)

group number

128.

Neutrons have a relative mass of…

a)

1

b)

0

c)

2

d)

very small

129.

How does the reactivity of Group 7 elements change as you go down the group?

a)

It decreases

b)

It stays the same

c)

It increases

d)

It increases and then levels off

130.

How many electrons do Group 1 metals have on their outer shell?

a)

3

b)

2

c)

1

d)

0

131.

Which separation method is used to separate mixtures of soluble substances?

a)

Crystallisation

b)

Filtering

c)

Distillation

d)

Chromatography

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