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Unit 1 review for the final

Total questions: 134

Worksheet time: 4hrs 25mins

Name
Class
Date
1.

Which subatomic particles are responsible for atomic mass?

a)

Electrons

b)

Protons

c)

Neutrons

d)

Positrons

2.

Which subatomic particles are responsible for the charge of an atom?

a)

Electrons

b)

Neutrons

c)

Nucleus

d)

Protons

3.

Which of the follow elements are in the Alkaline Earth metals?

a)

Mg

b)

Ca

c)

K

d)

Li

e)

Fr

4.

Which of the following elements have 4 valence electrons?

a)

Carbon

b)

Bismith

c)

Oxygen

d)

Antimony

e)

Lead

5.

Which element's electron configuration would end in 6d9?

a)

Ag

b)

Cu

c)

Au

d)

Rg

6.

What is the section of the periodic table where elements have electrons in the d orbitals called?

(a)  

7.

Name an element has 6 valence electrons?

(a)  

8.

Which of the following atoms could be represented by the orbital diagram above?

a)

Ar

b)

O2-

c)

F1-

d)

K1+

e)

Ga3+

9.

What is the the electron configuration for Krypton?

(a)  

10.

(a)   has the largest atomic radius?

11.

Fluorine would have the (a)   Atomic radius?

12.

The (a)   group needs only 3 electrons to complete the Octet rule?

13.

The Alkaline earth metals need to lose (a)   electrons to look like the noble gases?

14.

Who discovered the Electron?

a)

Thompson

b)

Rutherford

c)

Dalton

d)

Bohr

15.

Who discovered the nucleus?

a)

Dalton

b)

Bohr

c)

Thompson

d)

Rutherford

16.

Who discovered the Energy levels in the atom?

a)

Schodinger

b)

Bohr

c)

Rutherford

d)

Thompson

17.

Who mathematically predicted the electron clouds?

a)

Bohr

b)

Thompson

c)

Schrodinger

d)

Dalton

18.

How many neutrons would Ca-45 have?

a)

45

b)

5

c)

20

d)

25

19.

How many electrons would Al3+ have?

a)

10

b)

13

c)

16

d)

24

e)

12

20.

How many electrons does Zn1+ have?

a)

30

b)

31

c)

29

d)

65

21.

How many electrons does S2- have?

a)

19

b)

18

c)

16

d)

17

22.

What does the electron configuration of Vandium-53 end with?

a)

3d6

b)

3p6

c)

3d3

d)

3p3

23.

Which of the following was the conclusion of the gold foil experiment by Rutherford

a)

Atom is mostly empty space

b)

Atom has a dense center

c)

The center is positively charged

d)

The center is negatively charged

e)

The atom is a solid sphere

24.

How many electrons does selenium need to complete the octet rule?

a)

1

b)

2

c)

3

d)

4

e)

5

25.

Which ways do the atomic radius decrease on the periodic table?

a)

Down

b)

Up

c)

Left

d)

right

26.

Which way does the electron affinity decrease across the periodic table?

a)

up

b)

down

c)

left

d)

right

27.

Which families would be considered to be the most reactive?

a)

Alkali metals

b)

alkaline earth metals

c)

Oxygen group

d)

Halogens

e)

Noble gases

28.

Which family would be considered the least reactive?

a)

Noble gases

b)

Oxygen group

c)

Lanthanide series

d)

Transition metals

e)

Alkaline earth metals

29.

How many neutrons would Rutherium-105 have?

a)

44

b)

61

c)

105

d)

78

30.

How many neutrons would be in the isotope 9139Y?

a)

52

b)

39

c)

91

d)

55

31.

If Copper-65 naturally occurred 55% of the time and Copper-63 naturally occurred 25% of the time and Copper-61 occurred 20 % of the time, What would Copper's average atomic weight be calculated as?

a)

63 g/mol

b)

63.7 g/mol

c)

63.1 g/mol

d)

63.5 g/mol

32.

If Tin-120 occurred at 73.6% of the time and Tin-116 occurred at 26.4% of the time, What would be Tin's average atomic weight?

a)

120.144 g/mol

b)

118.71 g/mol

c)

118.944 g/mol

d)

115.753 g/mol

33.

What did Bohr base his atomic model on?

a)

Electrons emitting light when they jumped to higher energy levels

b)

Electrons emitting light when they jumped to lower energy levels

c)

The amount, or type, of light produced when electrons jumped multiple energy levels

d)

He concluded that each energy level had an set amount of energy that electrons had absorb and emit to change to that energy level

34.

Aluminum would have to (a)   3 electrons to be stable.

35.

Which subatomic particles are responsible for atomic mass?

a)

Electrons

b)

Protons

c)

Neutrons

d)

Positrons

36.

Which subatomic particles are responsible for the charge of an atom?

a)

Electrons

b)

Neutrons

c)

Nucleus

d)

Protons

37.

Which of the follow elements are in the Alkali metals?

a)

Mg

b)

Ca

c)

K

d)

Li

e)

Fr

38.

Which of the following elements have 5 valence electrons?

a)

C

b)

N

c)

O

d)

Sb

e)

Pb

39.

Which element's electron configuration would end in 3d9?

a)

Ag

b)

Cu

c)

Au

d)

Rg

40.

What is the section of the periodic table where elements have electrons in the d orbitals called?

a)

Transition metals

b)

Translation metals

c)

Transistor metals

d)

Translator metals

41.

Which of the following elements has 8 valence electrons?

a)

He

b)

Ne

c)

Ar

d)

F

e)

Cl

42.

Which of the following atoms could be represented by the orbital diagram above?

a)

P3-

b)

O2-

c)

Cl1-

d)

K1+

e)

Al3+

43.

Which of the following could be the electron configuration for an ion of Oxygen?

a)

1s22s22p6

b)

1s12s22p6

c)

1s22s22p4

d)

1s22s22p5

44.

Which of the following has the smallest atomic radius?

a)

Cl

b)

F

c)

O

d)

Br

e)

Ar

45.

Which of the following would have the biggest Atomic radius?

a)

K

b)

Cu

c)

Mg

d)

Fr

e)

Rb

46.

Which group needs only 2 electrons to complete the Octet rule?

a)

Carbon group

b)

Oxygen group

c)

Noble gases

d)

Lanthanide series

e)

Halogens

47.

How many electrons would the Alkaline earth metals need to lose to look like the noble gases?

a)

1

b)

2

c)

3

d)

4

e)

None, they have to gain electrons

48.

Who discovered the Electron?

a)

Thompson

b)

Rutherford

c)

Dalton

d)

Bohr

49.

Who discovered the nucleus?

a)

Dalton

b)

Bohr

c)

Thompson

d)

Rutherford

50.

Who discovered the Energy levels in the atom?

a)

Schodinger

b)

Bohr

c)

Rutherford

d)

Thompson

51.

Who mathematically predicted the electron clouds?

a)

Bohr

b)

Thompson

c)

Schrodinger

d)

Dalton

52.

How many neutrons would Ca-45 have?

a)

45

b)

5

c)

20

d)

25

53.

How many protons would Al- 27 have?

a)

13

b)

27

c)

14

d)

26

e)

12

54.

How many electrons does O2- have

a)

6

b)

8

c)

10

d)

12

55.

How many electrons does Na1+ have?

a)

9

b)

10

c)

11

d)

12

56.

What does electron configuration of P3- end with?

a)

3d6

b)

3p6

c)

3d3

d)

3p3

57.

Which of the following was the conclusion of the gold foil experiment by Rutherford

a)

Atom is mostly empty space

b)

Atom has a dense center

c)

The center is positively charged

d)

The center is negatively charged

e)

The atom is a solid sphere

58.

How many electrons does C need to complete the octet rule?

a)

1

b)

2

c)

3

d)

4

e)

5

59.

Which ways do the atomic radius increase on the periodic table?

a)

Down

b)

Up

c)

Left

d)

right

60.

Which way does the electron affinity increase across the periodic table?

a)

up

b)

down

c)

left

d)

right

61.

Which families would be considered to be the most reactive?

a)

Alkali metals

b)

alkaline earth metals

c)

Oxygen group

d)

Halogens

e)

Noble gases

62.

Which family would be considered the least reactive?

a)

Noble gases

b)

Carbon group

c)

Halogens

d)

Boron group

e)

Alkali metals

63.

How many neutrons would Carbon-14 have?

a)

14

b)

6

c)

12

d)

8

64.

How many neutrons would be in the isotope 23692U?

a)

92

b)

236

c)

144

d)

146

65.

Which of the follow elements are in the Alkaline Earth metals?

a)

Mg

b)

Ca

c)

K

d)

Li

e)

Fr

66.

Which of the following elements have 4 valence electrons?

a)

Carbon

b)

Bismith

c)

Oxygen

d)

Antimony

e)

Lead

67.

Which of the following elements have 4 valence electrons?

a)

Carbon

b)

Bismith

c)

Oxygen

d)

Antimony

e)

Lead

68.

Which of the following elements have 4 valence electrons?

a)

Carbon

b)

Bismith

c)

Oxygen

d)

Antimony

e)

Lead

69.

Which element's electron configuration would end in 6d9?

a)

Ag

b)

Cu

c)

Au

d)

Rg

70.

What is the section of the periodic table where elements have electrons in the d orbitals called?

(a)  

71.

Name an element has 6 valence electrons?

(a)  

72.

Which of the following atoms could be represented by the orbital diagram above?

a)

Ar

b)

O2-

c)

F1-

d)

K1+

e)

Ga3+

73.

What is the the electron configuration for Krypton?

(a)  

74.

(a)   has the largest atomic radius?

75.

Fluorine would have the (a)   Atomic radius?

76.

The (a)   group needs only 3 electrons to complete the Octet rule?

77.

The Alkaline earth metals need to lose (a)   electrons to look like the noble gases?

78.

How many electrons would Al3+ have?

a)

10

b)

13

c)

16

d)

24

e)

12

79.

How many electrons does Zn1+ have?

a)

30

b)

31

c)

29

d)

65

80.

How many electrons does S2- have?

a)

19

b)

18

c)

16

d)

17

81.

What does the electron configuration of Vandium-53 end with?

a)

3d6

b)

3p6

c)

3d3

d)

3p3

82.

How many electrons does selenium need to complete the octet rule?

a)

1

b)

2

c)

3

d)

4

e)

5

83.

Which ways do the atomic radius decrease on the periodic table?

a)

Down

b)

Up

c)

Left

d)

right

84.

Which way does the electron affinity decrease across the periodic table?

a)

up

b)

down

c)

left

d)

right

85.

Which family would be considered the least reactive?

a)

Noble gases

b)

Oxygen group

c)

Lanthanide series

d)

Transition metals

e)

Alkaline earth metals

86.

How many neutrons would Rutherium-105 have?

a)

44

b)

61

c)

105

d)

78

87.

How many neutrons would be in the isotope 9139Y?

a)

52

b)

39

c)

91

d)

55

88.

If Copper-65 naturally occurred 55% of the time and Copper-63 naturally occurred 25% of the time and Copper-61 occurred 20 % of the time, What would Copper's average atomic weight be calculated as?

a)

63 g/mol

b)

63.7 g/mol

c)

63.1 g/mol

d)

63.5 g/mol

89.

If Tin-120 occurred at 73.6% of the time and Tin-116 occurred at 26.4% of the time, What would be Tin's average atomic weight?

a)

120.144 g/mol

b)

118.71 g/mol

c)

118.944 g/mol

d)

115.753 g/mol

90.

What did Bohr base his atomic model on?

a)

Electrons emitting light when they jumped to higher energy levels

b)

Electrons emitting light when they jumped to lower energy levels

c)

The amount, or type, of light produced when electrons jumped multiple energy levels

d)

He concluded that each energy level had an set amount of energy that electrons had absorb and emit to change to that energy level

91.

Aluminum would have to (a)   3 electrons to be stable.

92.
When filling out an orbital diagram, which of the following is true?
a)
Electrons occupying the same orbital must have the same spin
b)
Each electron is added according to the least amount of energy.
c)
Each electron is added according to the most amount of energy
d)
Electrons will fill orbitals paired before they are individually isolated
93.
How can atoms make light?
a)
After electrons release energy, they get excited to a higher energy level, then fall to the ground state, emitting light.
b)
After electrons absorb energy, they get excited and move to a higher energy level, then fall to the ground state, emitting light.
c)
The electrons absorb energy, fall to the ground state, then get excited to a lower energy level, emitting light.
d)
The electrons release energy, fall to the ground state, then get excited to a higher energy level, emitting light.
94.
How many valence electrons are there in an oxygen atom?
a)
4
b)
5
c)
6
d)
8
95.
Place the following atoms in order of increasing size: He, N, P, Ni, Na. 
a)
He < N < P < Na < Ni
b)
He < N < P < Ni <Na
c)
 N < P < He< Na < Ni
d)
Ni < Na < P < N <He
96.
What does Hund’s rule say about how electrons fill orbitals?
a)
Each electron is added according to least amount of energy
b)
Each electron is added according to the most amount of energy
c)
Electrons will fill orbitals individually before they are paired
d)
Electrons occupying the same orbital must have opposite spins
97.
Which of the following statements is true about atoms?
a)
Electrons are positively charged.
b)
Electrons exist in a cloud surrounding only the neutrons.
c)
Differnt numbers of electrons determine the isotopes of an element.
d)
The number of Protons determines the element.
98.

The electron configuration for an unknown element is 1s22s22p3. Which of the following elements could it be?

a)

B

b)

C

c)

N

d)

F

99.

The particles that are found in the nucleus of an atom are:

1. Proton

2. Neutron

3. Electron

a)

1 only

b)

2 only

c)

3 only

d)

1 & 2

e)

1 & 3

100.

How many arrows would be in the orbital diagram on the 3rd energy level (both s and p) for the Sulfur ion, S2-

a)

2

b)

3

c)

4

d)

5

e)

6

101.
Which of the following has the correct number of orbitals that can be accommodated in each orbital set?
a)
s:2
b)
p:6
c)
d:5
d)
f:14
102.
Which of the following has the correct number of orbitals and the correct number of electrons that can be accommodated in each orbital set?
a)
There is 2 s-orbital that can hold 1 electrons.
b)
There are 5 p-orbitals that hold a total of 10 electrons.
c)
There are 5 d-orbitals that can hold 10 electrons.
d)
There are 9 f-orbitals that can hold 18 electrons.
e)
All are correct
103.
Given the isotope information below with the percent abundance and isotope mass, what is the average atomic mass of this element?<br />48 % Silver-105, 43 % Silver-108, 9 % Silver-109
a)
96.94 amu
b)
106.65 amu
c)
107.33 amu
d)
194.94 amu
104.

Which of the following particles determines the mass of an atom:

1. Proton

2. Electron

3. Neutron

a)

1

b)

2

c)

3

d)

1 & 2

e)

1 & 3

105.

2713Al3\frac{27}{13}Al^3  How many of each subatomic particle is represented here?

a)

Protons -13  Electrons -16 Neutrons - 27

b)

Protons -13 Electrons -13 Neutrons - 27

c)

Protons -13 Electrons -16 Neutrons -14

d)

Protons -13 Electrons -10 Neutrons -14

106.
What is the identy of the element that has a mass of 65 and 29 protons?
a)
Cu
b)
Hf
c)
Zr
d)
Rf
e)
Ge
107.
How many protons are in Mg- 27?
a)
27
b)
24
c)
12
d)
25
108.

Which of the following particles determines the charge of an element:

1. Proton

2. Electron

3. Neutron

a)

1

b)

2

c)

3

d)

1 & 2

e)

1 & 3

109.
Which of the following has the correct number of orbitals and the correct number of electrons that can be accommodated in each orbital set?
a)
There is 1 s-orbital that can hold 4 electrons.
b)
There are 3 p-orbitals that hold a total of 9 electrons.
c)
There are 5 d-orbitals that can hold 15 electrons.
d)
There are 7 f-orbitals that can hold 21 electrons.
e)
None are correct
110.
Rank the following in increasing electron affinity: F, O, Si, Al, Mg
a)
 F < O < Si > Al > Mg 
b)
 F < O < Si < Al < Mg 
c)
 Mg > O > Si > Al > F
d)
Mg  < Al < Si < O <  F
111.

Which ways on the periodic table do the atomic radii increase?

1. Right

2. Left

3. Down

4. Up

a)

1 & 2

b)

1 & 3

c)

1 & 4

d)

2 & 3

e)

3 & 4

112.
Using the gold foil experiment, what did Rutherford conclude about the structure of the atom?
a)
.They are solid spheres. 
b)
An atom is made up of mostly solid material.
c)
The middle of an atom is very dense and made up of positive charges. 
d)
Electrons make up the center of an atom.
113.

 \   42He + 73Li\frac{4}{2}He\ +\ \frac{7}{3}Li  

Which of the following could be the result of these two

 undergoing a fusion reaction?

a)

115C\frac{11}{5}C  

b)

115B\frac{11}{5}B  

c)

115Na\frac{11}{5}Na  

d)

97N\frac{9}{7}N  

114.
Which of the following statements is true about electrons?
a)
Electrons are positively charged
b)
Electrons exist in an electron cloud surrounding the nucleus
c)
Electrons exist within the nucleus
d)
All of the above
115.

Which electron configuration shows the arrangement of electrons in an atom of bromine?

a)

[K]4s23d104p5

b)

[Ar]4s23d104p5

c)

1s22s22p63s23p64s23d104p5

d)

1s22s23s24s22p63p64p54d10

116.

Which are possible reasons for the atomic radii to increase in size?

1. As you go down a group on the periodic table, since there are more energy levels, the different energy levels place the electrons further away from the nucleus.

2. As you go to the right on a period of the periodic table, since there are more electrons and protons, there is more force pulling the electrons towards the nucleus.

3.As you go up a group on the periodic table, since there are fewer energy levels, the radius will be smaller.

4.As you go left on a period of the periodic table, since there are fewer electrons and protons, there is a smaller force pulling the electrons towards the nucleus.

a)

1 & 3

b)

1 & 2

c)

1 & 4

d)

2 & 3

e)

3 & 4

117.

Which ways on the periodic table do electronegativity decrease?

1. Up

2.Right

3. Left

4. Down

a)

1 & 2

b)

1 & 3

c)

1 & 4

d)

2 & 3

e)

3 & 4

118.

Which ways on the periodic table do ionization energy decrease?

1. Down

2. Up

3. Left

4. Right

a)

1 & 2

b)

1 & 3

c)

1 & 4

d)

2 & 3

e)

3 & 4

119.
Which of the following has the correct number of electrons that can be accommodated in each orbital set?
a)
s:1
b)
p:3
c)
d:5
d)
f:14
120.

Which are possible reasons for the atomic radii to increase in size?

1. As you go down a group on the periodic table, since there are more energy levels, the different energy levels place the electrons further away from the nucleus.

2. As you go to the right on a period of the periodic table, since there are more electrons and protons, there is more force pulling the electrons towards the nucleus.

3. As you go up a group on the periodic table, since there are fewer energy levels, the radius will be smaller.

4.As you go left on a period of the periodic table, since there are fewer electrons and protons, there is a smaller force pulling the electrons towards the nucleus.<br />

a)

1 & 2

b)

1 & 3

c)

1 & 4

d)

2 & 3

e)

3 & 4

121.

Which ways on the periodic table do ionization energy increase?

1. Down

2. Up

3. Left

4. Right

a)

1 & 2

b)

1 & 3

c)

1 & 4

d)

2 & 3

e)

2 & 4

122.

Which ways on the periodic table does the electronegativity increase?

1. Up

2. Left

3. Right

4. Down

a)

1 & 2

b)

1 & 3

c)

1 & 4

d)

2 & 3

e)

2 & 4

123.

Which ways on the periodic table do the atomic radii decrease?

1. Right

2. Left

3. Down

4. Up

a)

1 & 2

b)

1 & 3

c)

1 & 4

d)

2 & 3

e)

2 & 4

124.
When filling out an orbital diagram, which of the following is false?
a)
Each electron is added according to the least amount of energy.
b)
Each electron is added according to the most amount of energy first.
c)
Electrons will fill orbitals individually before they are paired
d)
Electrons occupying the same orbital must have opposite spins.
125.

Which element has the following electron configuration? 1s22s2 .... 4s23d10 4p6

a)

Br

b)

Kr

c)

S

d)

Cl

e)

Ge

126.

Which of the following particles determines the charge of an element:

1. Proton

2. Electron

3. Neutron

a)

1

b)

2

c)

3

d)

1 & 2

e)

1 & 3

127.
How do atoms emit light?
a)
After electrons absorb energy, they get excited and move to a higher energy level, then fall to the ground state, emitting light.
b)
After electrons release energy, they get excited to a higher energy level, then fall to the ground state, emitting light.
c)
The electrons absorb energy, fall to the ground state, then get excited to a lower energy level, emitting light.
d)
The electrons release energy, fall to the ground state, then get excited to a higher energy level, emitting light.
128.
Which of the following statements is false about atoms?
a)
Electrons are negatively charged
b)
Electrons exist in an electron cloud surrounding the nucleus
c)
Protons exist within the nucleus
d)
Neutrons exist in orbitals around the nucleus
129.
Which of the following statements is true about atoms?
a)
Electrons are positively charged.
b)
Electrons exist in a cloud surrounding only the neutrons.
c)
Differnt numbers of electrons determine the isotopes of an element.
d)
The number of Protons determines the element.
130.

5826Fe(3+)\frac{58}{26}Fe^{\left(3+\right)}  

How many of each subatomic particle is represented?

a)

Protons -26

Electrons -29

Neutrons - 32

b)

Protons - 23

Electrons -26

Neutrons - 32

c)

Protons -26

Electrons -23

Neutrons -32

d)

Protons - 26

Electrons - 55

Neutrons -23

131.

Which electron configuration shows the arrangement of electrons in an atom of bromine?

a)

[K]4s23d104p5

b)

[Ar]4s23d104p5

c)

1s22s22p63s23p64s24d104p5

d)

1s22s23s24s22p63p64p54d10

132.
The electron configuration for an unknown element is 1s22s22p1. Which of the following elements could it be?
a)
B
b)
C
c)
N
d)
F
133.

261104X\frac{261}{104}X  

What is the identity of the element?

a)

Hf

b)

Zr

c)

Rf

d)

Ge

e)

Cu

134.
What does Hund’s rule say about how electrons fill orbitals?
a)
Each electron is added according to the most amount of energy
b)
Each electron is added according to least amount of energy
c)
Electrons will fill orbitals individually before they are paired
d)
Electrons occupying the same orbital must have opposite spins

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