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CH301 - Unit 1 Exam 2 Review

Total questions: 111

Worksheet time: 2hrs 51mins

Name
Class
Date
1.

Compared to a 280 nm photon, a 320 nm photon has:

a)

1. longer wavelength, lower frequency, lower energy

b)

2. longer wavelength, lower frequency, higher energy 3.

c)

shorter wavelength, lower frequency, higher energy

d)

shorter wavelength, lower frequency, lower energy

e)

longer wavelength, higher frequency, higher energy

2.

We conduct an experiment by shining 500 nm light on potassium metal. This causes electrons to be emitted from the surface via the photoelectric effect. Now we change our source light to 450 nm at the same intensity level. Which of the following is the result from the 450 nm light source compared to the 500 nm source?

a)

No electrons would be emitted from the surface.

b)

The same number of electrons would be emitted, but they would have a higher velocity.

c)

The same number of electrons would be emitted, but they would have a lower velocity.

d)

Fewer electrons would be emitted from the surface.

3.

Consider a filled n = 3 shell. For a given configuration within that shell, how many electrons will be assigned mℓ = 1?

a)

18

b)

8

c)

16

d)

4

4.

How many electrons can possess this set of quantum numbers: principal quantum number n = 4, magnetic quantum number ml = 0?

a)

6

b)

18

c)

8

d)

14

5.

Which of the following valence-shell configurations is/are possible for a neutral atom for an element?

a)

III only

b)

None of the configurations

c)

IV only

d)

I only

6.

Which response includes only species that have the electronic configuration 1s2 2s2 2p6 3s2 3p6 , and no other species?

a)

Cl−, K+, Ar, Mg2+

b)

Na+, Ar, P3−

c)

Na+, K+, Ar

d)

Cl−, K+, Ar, P3−

7.

A comparison of the electron configurations of cobalt (Co) and chromium (Cr) indicates that

a)

Cr has 3 fewer d electrons and the same number of s electrons as Co.

b)

Cr has 3 fewer d electrons and one more s electron than Co.

c)

Cr has 3 fewer d electrons and one less s electron than Co.

d)

Cr has 2 fewer d electrons and one less s electron than Co.

8.

Write the ground-state electron configuration of In+.

a)

[Kr] 4d8 5s1 5p3

b)

[Kr] 4d5 5s1 5p6

c)

[Kr] 4d10 5s2

d)

[Kr] 4d10 5s1 5p1

9.

Fill in the blanks: chlorine is one of the most well-known elements in the halogen . It belongs to 17 which makes it a element. Its valence electrons belong to the n = 3 , and it has a nearly-filled 3p , making it very reactive. Cl− is a very stable anion because it is isoelectronic to a .

a)

family, group, main group, shell, subshell, noble gas

b)

group, column, non-metal, shell, orbital, metal

c)

family, column, common, row, shell, anion

d)

series, family, reactive, row, subshell, noble gas

10.

When dealing with electrons in atoms and molecules, the electrons that are not considered as valence electrons (can, cannot) effectively shield the nucleus and thereby (decrease, increase) the effective nuclear charge.

a)

can; decrease

b)

The non-valence electrons do nothing.

c)

cannot; decrease

d)

can; increase

11.

Which pair of atoms (ions) is listed in order of INCREASING radii?

a)

Mg2+, Na+

b)

Br−, Cl−

c)

Mg, Mg2+

d)

S 2−, Cl−

12.

Given the elements Cl, Ge, and K and the values 418, 1255, and 784 kJ/mol of possible first ionization energies, match the atoms with their first ionization energies.

a)

Cl: 784 kJ/mol; Ge: 1255 kJ/mol; and K: 418 kJ/mol

b)

Cl: 418 kJ/mol, Ge: 1255 kJ/mol; and K: 784 kJ/mol

c)

Cl: 1255 kJ/mol; Ge: 784 kJ/mol; and K: 418 kJ/mol

d)

Cl: 1255 kJ/mol; Ge: 418 kJ/mol; and K: 784 kJ/mol

13.

What is the correct order of decreasing frequency?

a)

radio waves, infrared radiation, visible light, ultraviolet radiation

b)

visible light, ultraviolet radiation, infrared radiation, radio waves

c)

radio waves, visible light, ultraviolet radiation, infrared radiation

d)

ultraviolet radiation, visible light, infrared radiation, radio waves

14.

Which phenomenon provides the best evidence that light can have particle properties?

a)

Electron diffraction

b)

Electromagnetic radiation

c)

X-ray diffraction

d)

Photoelectric effect

15.

Calculate the wavelength of a motorcycle of mass 275 kg traveling at a speed of 125 km/hr.

a)

2.08 × 10−29 m

b)

2.41 × 10−36 m

c)

1.93 × 10−38 m

d)

6.94 × 10−38 m

16.

Can an electron in an atom be in an energy level described by the set of quantum numbers n = 5, l = 3, ml = −2?

a)

No, because n cannot be as large as 5.

b)

No, because ml must be equal to ±1.

c)

No, because ml cannot be negative.

d)

Yes

17.

What is the effective nuclear charge experienced by the 2p electrons of an aluminum atom (Al)?

a)

11

b)

6

c)

4

d)

9

18.

Arrange the following ions in order of increasing radius: K+, Li+, Be2+, Na+.

a)

K+ < Be2+ < Li+ < Na+

b)

Li+ < Na+ < K+ < Be2+

c)

Na+ < K+ < Be2+ < Li+

d)

Be2+ < Li+ < Na+ < K+

19.

Which of the following elements would have a lower ionization energy than nitrogen?

a)

F

b)

O

c)

None of these

d)

Ne

20.

What is the electronic configuration of Sn4+?

a)

[Kr]4d10

b)

[Kr]5s2 4d8

c)

[Kr]5s2 4d10 5p6

d)

[Kr]5s1 4d9

21.

There are seven arrows shown. Which would correspond to the longest wavelength?

a)

the left Lyman arrow

b)

the right Lyman arrow

c)

the left Balmer arrow

d)

the Paschen arrow

22.

For a Bohr atom, which of the following transitions emits the lowest energy photon?

a)

From n = 10 to n = 8

b)

From n = 4 to n = 2

c)

From n = 6

d)

From n = 2 to n = 1

23.

Which two types of electromagnetic radiation affect the nucleus

a)

radio, gamma

b)

micro, gamma

c)

xray, gamma

d)

IR, gamma

24.

Which of the following pairs of quantum numbers does not exist?

a)

2p

b)

3d

c)

2d

d)

5f

e)

4f

25.

How many paired electrons are in an atom of Chlorine?

draw the orbital diagram

a)

10

b)

12

c)

14

d)

16

e)

17

26.

Which of the following statements concerning trends on the periodic table is false?

a)

Atomic radius increases up and to the right

b)

Ionization energy increases up and to the right

c)

Electron affinity increases up and to the right

d)

Electronegativity increases up and to the right

27.

Is chromium paramagnetic or diamagnetic?

a)

paramagnetic

b)

diamagnetic

28.

Which of the following species are isoelectronic?

I. Sn4+

II. Cd

III. Ag+

IV. In3+

a)

I, II, III, IV

b)

I, III, IV

c)

None

d)

II and IV only

29.

Which of the following atoms or ions does not have an s1d5 valence?

a)

Fe+2

b)

Nb-

c)

Tc

d)

W

30.

Which of the following pairs of electrons experiences the same effective nuclear charge?

a)

the 1s of H and the 1s of He

b)

the 1s of He and the 2s of Be

c)

the 2p of C and the 2p of N

d)

the 3s of Al and the 2s of N

31.

The atom having the valence-shell configuration 4s2 4p5 would be in:

a)

Group VIA and Period 5

b)

Group IVB and Period 4

c)

Group VIB and Period 7

d)

Group VIIA and Period 4

e)

Group VIIB and Period 4

32.

Select the term best describing the series of elements: Mn, Fe, Co, Ni, Cu.

a)

d-transition metals

b)

main group elements

c)

metalloids

d)

alkaline earth metals

e)

halogens

33.

Which element has the largest atomic radius?

a)

Li

b)

Na

c)

Rb

d)

F

e)

I

34.

Which of the following terms accurately describes the energy associated with the process:

a)

electron affinity

b)

binding energy

c)

ionization energy

d)

electronegativity

e)

none of these

35.

Which element has the lowest first ionization energy?

a)

He

b)

Ne

c)

Ar

d)

Kr

e)

Xe

36.

Which element has the highest first ionization energy?

a)

Be

b)

B

c)

C

d)

N

e)

O

37.

Which of these isoelectronic species has the smallest radius?

a)

Br-

b)

Sr2+

c)

Rb+

d)

Se2-

e)

They are all the same size because they have the same number of electrons.

38.

Which of the following elements has the greatest attraction for electrons in a covalent bond?

a)

Ge

b)

As

c)

Se

d)

Br

e)

Bi

39.

All of the following properties of the alkaline earth metals increase going down the group except

a)

atomic radius

b)

first ionization energy

c)

ionic radius

d)

atomic mass

40.
Elements closer to the noble gases have stronger attraction for electrons.
a)
True
b)
False
41.
Which of the following is the least electronegative element?
a)
oxygen
b)
potassium
c)
fluorine
d)
nitrogen
42.
Put these in order of increasing electronegativity:
F, N, B
a)
B < N < F
b)
B < F < N
c)
N < F < B
d)
F < N < B
43.
 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 
44.

As you look down a group, ionization energy and electronegativity

a)

increases

b)

decreases

45.

The amount of energy released when an electron is added to a neutral atom to form a negative ion

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

46.

Why do Group 18 elements have such high Ionization Energies?

a)

They have full outer energy levels and therefore do not want to lose electrons from their outer energy level.

b)

They are non metals.

c)

They are metals

47.

Why do Group 1 elements have such low Ionization Energies?

a)

They have full outer energy levels and therefore do not want to lose electrons from their outer energy level.

b)

They are non metals and therefore require more electrons to complete their outer energy level.

c)

They are metals and its easier to give away the electrons in their outer energy level.

48.

Why is there such an increase in 1st to 2nd Ionization energies for Lithium?

a)

The 2nd ionization energy is higher because this energy level is full.

b)

Lithium only has 1 electron in its outer energy level and therefore does not hold on to it very hard.

49.

Why is the Electron Affinity in Group 1 elements so low?

a)

They want to accept electrons

b)

They have opposite charges which repel.

c)

They do not want to accept electrons.

50.

The Electron Affinity decreases from TOP TO BOTTOM in a GROUP.

a)

TRUE

b)

FALSE

51.

Order the following from smallest to largest atomic radius:

Ra, Be, Ca, Rb, H

a)

Ra, Be, Rb, H, Ca

b)

Rb, H, Ca, Be, Ra

c)

Ra, Rb, Ca, Be, H

d)

H, Be, Ca, Rb, Ra

52.

The effective nuclear charge of a valence electron of magnesium is

a)

+1

b)

+2

c)

+12

d)

+24

53.

Effective nuclear charge ________ across a period.

a)

increases

b)

decreases

c)

stays the same

54.

What is effective nuclear charge?

a)

The charge that effects the mass of the atom.

b)

The charge that the protons feel from the rest of the atom.

c)

The charge felt by the valence electrons.

d)

The charge felt by the core electrons.

55.

Down the group , attraction between the nucleus and the valence electrons __________.

a)

Increases due to shielding

b)

Decreases due to shielding

c)

Stays the same

56.
As you go across a period, the amount of shielding...
a)
Increases
b)
decreases
c)
stays the same
57.
Which of the following elements has the most "shielding" electrons?
a)
Neon
b)
flourine
c)
oxygen
d)
They have the same
58.
Which of the following elements has the highest effective nuclear charge?
a)
Indium
b)
Antimony
c)
tellerium
d)
Tin
59.
In the following configuration, which electrons are the shielding electrons? 1s2 2s2 2p6 3s2 3p4
a)
1s2 2s2 2p6
b)
3s2 3p4
c)
1s2 2s2
d)
2s2 2p6 3s2 3p4
60.
What makes a valence electron more attracted to the nucleus?
a)
less distance between the nucleus and having less protons
b)
less distance between the nucleus and having more protons
c)
more distance between the nucleus and having less protons
d)
more distance between the nucleus and having more protons
61.

What is the tendency of an atom to attract electrons towards itself in a bond?

a)

atomic radius

b)

ionization energy

c)

shielding

d)

Electronegativity

62.
The higher the ionization energy...
a)
the more attracted the valence electron is to the nucleus
b)
the less attracted the valence electron is to the nucleus
c)
the more attracted the valence electron is to another electron
d)
the less attracted the valence electron is to another electron
63.
Which is larger... P or P3- ?
a)
P3- because it gains an energy level
b)
P3- due to extra electron repulsion
c)
P because it loses an energy level
d)
P because of extra electron repulsion
64.

Why does ionization energy decrease going down a group?

a)

Adding more energy levels places the valence e- further from the nucleus

b)

There are more valence electrons in the outer shell

c)

There are more protons in the nucleus

d)

There are less protons in the nucleus

65.

Why does electronegativity increase across a period?

a)

Adding more energy levels places the valence e- further from the nucleus

b)

There are more valence electrons in the outer shell

c)

There are more protons in the nucleus

d)

There are less protons in the nucleus

66.

Which is smaller... Mg or Mg2+ ?

a)

Mg because it gains an energy level

b)

Mg due to extra electron repulsion

c)

Mg2+ because of extra electron repulsion

d)

Mg2+ because it loses electrons

67.

List the following in order of smallest to largest ionization energy.

P, Cs, Co, Sr

a)

P, Co, Sr, Cs

b)

Cs, Sr, Co, P

c)

Sr, Cs, Co, P

d)

P, Co, Cs, Sr

68.
List the following from largest to smallest atomic radius.
P, Cs, Co, Sr
a)
P, Co, Sr, Cs
b)
P, Cs, Co, Sr
c)
Cs, Sr, Co, P
d)
Sr, Cs, Co, P
69.

What happens to atomic radius across a period?

a)

the atoms get bigger because the nucleus is bigger as more protons are added

b)

the atoms get bigger because there are more valence electrons

c)

the atoms get smaller because with more attraction to the extra protons, the e- cloud moves closer to the nucleus

70.

Why doesn't having more protons increase the attraction down a column?

a)

there are more valence electrons in the outermost energy level

b)

actually, there aren't more protons in the nucleus down the column

c)

as energy levels are added, non-valence electrons block the extra protons from attracting valence electrons

d)

more neutrons block the extra protons

71.

There may be a maximum of ____ p orbitals at a given energy level.

a)

2

b)

6

c)

3

d)

8

72.

The spin of an electron is represented by this variable:

a)

n

b)

ml

c)

l

d)

ms

73.

The principle quantum number, n, represents the:

a)

spin value

b)

shape

c)

energy level

d)

orientation

74.

Which best describes the angular momentum quantum number?

a)

l, shape of orbital

b)

ml, orientation of orbital

c)

ms, electron spin

d)

n, energy level

75.

The proper pair of the l value with the orbital shape.

a)

0; f

b)

3; p

c)

1; s

d)

2; d

76.

Which of the following pairs of quantum numbers does not exist?

a)

2p

b)

3d

c)

2d

d)

5f

e)

4f

77.

How many paired electrons are in an atom of Chlorine?

draw the orbital diagram

a)

10

b)

12

c)

14

d)

16

e)

17

78.

2. A quantum number determining orbital orientation around the atom’s core is called... .

a)

n

b)

l

c)

m

d)

s

79.

4. Below are the examples on how to fill the atomic quantum number, except... .

a)

n = 2, l =1, m = 0, s = -1/2

b)

n = 1, l =3, m = 0, s = +1/2

c)

n = 3, l =1, m = 0, s = -1/2

d)

n = 3, l = 2, m = +2, l = +1/2

80.

8. A theory stating that electrons have the trend of taking the orbitals from the lowest energy level to the highest is the theory of... .

a)

Pauli exclusion’s principle

b)

Aufbau principle

c)

Hund’s rule

d)

Heissenberg’s probability

81.

13. A theory stating that it is forbidden for 2 electrons having the same value of atomic quantum numbers is explained by... .

a)

Hund

b)

Aufbau

c)

Pauli

d)

Schrodinger

82.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
83.
Identify the following element:
1s22s22p63s23p64s23d10
a)
nickel
b)
copper
c)
zinc
d)
gallium
84.
Identify the element whose electron configurations ends with 5p3
a)
As
b)
Te
c)
Sb
d)
Sn
85.
Which of the following quantum number sets is not allowed?
a)
{ 3, 2, +1, -1/2 }
b)
{ 5, 3, -1, +1/2 }
c)
{ 12, 1, +2, +1/2 }
d)
{ 7, 6, -5, -1/2 }
86.
According to the Aufbau Principle, which sublevel should starting filling with electrons before the 3p sublevel?
a)
3s
b)
2p
c)
4s
d)
4p
87.
I am an element in the 3rd row of the periodic table...I have one unpaired electron in my last sublevel...I have 3 valence electrons...who am I?
a)
Na
b)
Al
c)
Cl
d)
Ar
88.

The electron configuration of an atom is 1s22s22p6. The number of electrons this atom has is

a)

3

b)

6

c)

8

d)

10

89.

Choose the correct noble gas configuration for iodine.

a)

[Ar]4s24d104p5

b)

[Kr]5s24d105p5

c)

[Xe]5s25d105p5

d)

none of the above

90.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
91.
Cations are _______ that form ____________ ions and __________ electrons.
a)
nonmetals, positive, lose
b)
nonmetals, negative, gain
c)
metals, positive, gain
d)
metals, positive, lose
92.
Anions are _______ that form ____________ ions and __________ electrons.
a)
nonmetals, positive, lose
b)
nonmetals, negative, gain
c)
metals, positive, gain
d)
metals, positive, lose
93.

Which element's electron configuration ends 4p4?

a)

sulfur

b)

arsenic

c)

selenium

d)

antimony

94.
Identify the Electron Configuration for Aluminum (Al)
a)
1s2 2s2 2p6 3s2 3p1
b)
1s2 2s2 2p6 3s2 3p3
c)
1s2 2s2 2p6 3s2 4p1
95.

Is the following electron configuration correct? Why or why not?


1s22s22p63s23p64s24d104p65s1

a)

No. 4p6 should be after 5s1.

b)

No. It should be 3d10 not 4d10

c)

Yes. All electrons are represented properly.

d)

Yes.

96.

What is the electron configuration for a Bromine ion, Br-?

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6

d)

1s2 2s2 2p6

97.
What is the noble gas configuration for Sulfur?
a)
[Ar] 3p4
b)
[He] 3s2 3p4
c)
[Ne] 3s2 3p4
d)
[Ne] 3p4
98.

Which of the following shows a proper pair of the l value with the orbital shape.

a)

0=f

b)

3=p

c)

1=s

d)

2=d

99.

As the energy level goes higher, the electrons

a)

have lower in energy

b)

are more stable

c)

are weaker

d)

are farther from the nucleus

100.

What is the correct representation for an orbital which has an "n" value of 4 and an "L" value of 2?

a)

4d

b)

4s

c)

4f

d)

4p

101.

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

a)

energy level

b)

s orbitals

c)

p orbitals

d)

the number of electrons

102.

The subshells s, p, d, and f all have the same energy as long as they are in the same principal shell.

a)

True

b)

False

103.
How do n and l relate?
a)
l is always equal to n
b)
l can be any integer from 0 to n
c)
l can be any integer from 0 to (n-1)
d)
l can be any integer from -n to n
104.
What are all the possible l values for n=2?
a)
0, 1, 2
b)
0, 1
c)
1, 2
d)
2
105.
What are all the possible l values for n=3?
a)
1, 2, 3
b)
0, 1, 2, 3
c)
0, 1, 2
d)
1, 2
106.
Which of the following has an l = 0?
a)
b)

c)

d)

107.

The magnetic quantum number, ml, can be negative.

a)

True

b)

False

108.

If l=1, what are all the possible values for ml?

a)

0, 1

b)

-1, 0, 1

c)

1, 2

d)

-2, -1, 0, 1, 2

109.
How many orbitals with n=1 and l=2 are possible?
a)
5
b)
3
c)
1
d)
0, this combination is impossible.
110.

How many orbitals with n=4 and ml=-2 are possible?

a)

7

b)

2

c)

1

d)

0, this combination is impossible.

111.
Which of these has the highest energy?
a)
1s sublevel
b)
2p sublevel
c)
3p sublevel
d)
4s sublevel

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