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Unit 4 Review Light and Electrons

Total questions: 103

Worksheet time: 2hrs 21mins

Name
Class
Date
1.

Name the element- 1s2 2s2 2p6 3s2 3p6 4s2 3d5

a)

Manganese

b)

Magnesium

c)

Aluminum

d)

Boron

2.

In what family is this element found?

1s22s22p63s23p64s2

a)

alkaline earth metal

b)

alkali metal

c)

noble gas

d)

halogen

3.

Which of these represents a transition element?

a)

1s2 2s2 2p6 3s2 3p3

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1

c)

1s2 2s1

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d1

4.

Which "rule" explains why the two electrons in an orbital have opposite spin?

a)

Pauli Exclusion Principle

b)

Hund's Rule

c)

Heisenberg Uncertainty Principle

d)

Bohr's Rule

5.

How many valence electrons are in an atom of zinc?

a)

2

b)

10

c)

12

d)

8

6.

Which of these has the shortest wavelength?

a)

infrared

b)

yellow light

c)

microwaves

d)

blue light

7.

Which does NOT have the same number of electrons as the others?

a)

S2-

b)

Ar

c)

K+

d)

Mg2+

8.

What is the predicted electron configuration of Fe3+?

a)

[Ar] 4s2 3d3

b)

[Ar] 4s1 3d4

c)

[Ar] 3d6

d)

[Ar] 3d3

9.

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.

10.

Which scientist is credited with the discovery of atomic energy levels?

a)

Bohr

b)

Thomson

c)

Rutherford

d)

Bunsen

11.

All forms of EM radiation travel at the same speed and have the same energy.

a)

False, they travel at the same speed but have different energies

b)

True

c)

False, they travel at different speeds but have the same energy

12.
Which of the following has the least energy
a)
x-rays
b)
gamma rays
c)
radiowaves
13.
The distance between higher energy levels is _________ than the lower energy levels
a)
larger
b)
smaller
14.
Which of the following has the longest wavelength
a)
infrared
b)
UV rays
15.
Which of the following has the lowest frequency
a)
microwaves
b)
x rays
16.
Waves with a high frequency have _________ energy
a)
low
b)
high
17.

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

18.
a)

10

b)

2

c)

8

d)

18

19.

Valence electrons are located...

a)

inside the nucleus

b)

in outer space

c)

on the outermost orbit of an atom

20.

This is a correct dot diagram for fluorine (F)

a)

true

b)

false

21.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
22.
Elements in a ..................have similar chemical properties.  
a)
period
b)
group
c)
row
23.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)
the number of protons increases, so attraction to electrons increases
b)
the number of energy levels increases
c)
the number of electrons increases
d)
the atomic mass increases
24.

Of the halogens, which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

25.

Which element in Period 2 has the greatest atomic radius?

a)

Be

b)

C

c)

Na

d)

Li

26.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
27.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
28.

Which of the following will have a lower ionization energy than Scandium (Sc)?

a)

Helium (He)

b)

Titanium (Ti)

c)

Calcium (Ca)

d)

Magnesium (Mg)

29.

Which of the following will have a higher electronegativity than arsenic (As)?

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

30.
Identify the element that is non-reactive (inert) with 4 energy levels.
a)
Krypton
b)
Argon
c)
Potassium
d)
Calcium
31.

When atom gains an electron, the size will

a)

increase

b)

decrease

c)

have no change

d)

smaller

32.

When atom loses an electron, the size will

a)

be greater

b)

increase

c)

have no change

d)

be smaller

33.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
34.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
35.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
36.
Atoms that have a high electronegativity, _______________.
a)
give up their electrons more easily.
b)
hold on to their electrons more tightly.
c)
have more electron shells.
37.
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. 
38.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
39.
Which of the following pairs of elements have similar properties
a)
Barium and Calcium
b)
Sodium and Magnesium
c)
Nickel and Copper
d)
Lithium and Helium 
40.
Which of the following is true for Calcium
a)
Metal and Low electronegativity value 
b)
Metal and has 2 valence electrons
c)
Metal, Low electronegativity, has 2 valence electrons
d)
Metal and Semi conductor 
41.
Which of the following electron configurations represents the most chemically stable atom?
a)
[Ne] 3s1
b)
[Ne] 3s2 3p3
c)
[Ne] 3s2 3p6
d)
[Ar] 4s2 3d6
42.
The minimum energy required to remove an electron from the ground state of an atom
a)
electron configuration
b)
energy levels
c)
ionization energy
d)
ionic bond
43.
What is the noble gas configuration for beryllium?
a)
[He]1s2
b)
[He]2s2
c)
[Li]2s1
d)
[Li]2s2
44.
What is the noble gas configuration for Sulfur?
a)
[Ar] 3p4
b)
[He] 3s2 3p4
c)
[Ne] 3s2 3p4
d)
[Na] 3s2 3p4
45.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
46.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
47.

What element has this orbital notation?

a)

lithium

b)

beryllium

c)

boron

d)

carbon

48.
All orbitals of equal energy are occupied by one electron before any single orbital is occupied by a second electron.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Core Notation
49.
An electron occupies the lowest energy orbital that can receive it.
a)
Hund’s rule
b)
Pauli exclusion principle
c)
Bohr model of the atom
d)
Aufbau principle
50.
No two electrons in the same atom can have the same four quantum numbers.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Noble gas notation
51.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Hund's
b)
Aufbau's
c)
Pauli's Exclusive
52.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Aufbau's
b)
Hund's
c)
Pauli exclusive
53.
Electrons are paired based on their spin directions, clockwise and counterclockwise, is what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
54.
Which orbital shows a violation of the Aufbau Principle?
a)
A
b)
B
c)
C
d)
D
55.
This is the correct dot diagram for sodium (Na)
a)
true
b)
false
56.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
57.

What is the octet rule?

a)

Elements can only have 8 electrons in its outermost shell

b)

The elements must form an octopus like structure

58.

Electron dot notation is . . . .

a)

A representation of an element in which only valence electrons of an atom are shown

b)

A representation of how compounds are formed.

59.
How many electrons should Helium have around its Lewis dot model?
a)
1
b)
2
c)
7
d)
8
60.

Each element on the periodic table can be identified by its

a)

classification as a solid, liquid or gas.

b)

location on the table.

c)

ability to react to form compounds.

d)

unique spectral "fingerprint."

61.

Emission spectra emitted by an element (or compound) will produce ___ through a spectroscope.

a)

bright lines

b)

a continuous rainbow

c)

dark lines

d)

white light

62.

Look carefully at the picture. It shows an electron in the excited state on the left, and the electron returning to its ground state on the right. When the electron return to the ground state it emits a_______________________.

a)

blast of cold air

b)

electrostatic charge

c)

proton

d)

photon (light)

63.

The picture shows an atom in the ground state absorbing energy and the electron jumps to the excited state. Which state has higher energy?

a)

Ground State

b)

Excited State

64.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
65.

When an electron moves from n=2 (energy level 2) to n=4 (energy level 4)

MULTIPLE ANSWERS: CHECK ALL CORRECT ANSWERS

a)

it must absorb light

b)

it will release light

c)

it will move farther from the nucleus

d)

it will move closer to the nucleus

66.

A ground state electron is

a)

freshly crushed into a fine powder.

b)

in the highest possible energy level.

c)

in the lowest possible energy level.

d)

constantly emitting light.

67.

According to Bohr, the energy absorbed by an electron upon excitation comes in a fixed amount called

a)

exact energy

b)

fixed energy

c)

quantized energy

d)

None of the above

68.
Visible light is the only type of electromagnetic radiation.
a)
True
b)
False
69.
Every element has its own unique atomic spectra.
a)
True
b)
False
70.

In order to go from ground state to an excited state, an electron must

a)

emit energy

b)

absorb energy

c)

rotate

d)

wiggle

71.

When an electron returns to ground state from an excited state, the atom will

a)

emit energy

b)

absorb energy

c)

rotate

d)

wiggle

72.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
73.

How many electrons can a d sublevel hold?

a)

14

b)

10

c)

2

d)

6

74.

How many orbitals does a d sublevel have?

a)

1

b)

3

c)

5

d)

7

75.

How many orbitals does an f sublevel have?

a)

1

b)

3

c)

5

d)

7

76.

How many f orbitals can an f sublevel hold?

a)

1

b)

7

c)

5

d)

14

77.

Electrons fill energy levels and sublevels _____ in energy first.

a)

lower

b)

higher

78.
Which of the following statements is true about the 3s and the 4s sublevels?
a)
These sublevels have the same energy
b)
These sublevels are the same distance from the nucleus
c)
These sublevels hold different amounts of electrons
d)
These sublevels have the same shape
79.

Which of the following units is represented simply by a letter?

a)

orbital

b)

energy level

c)

sublevel

d)

quantum number

80.

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

a)

4s

b)

3d

c)

4p

d)

5s

81.

Of the following sublevels, which is the highest in energy?

a)

4s

b)

3d

c)

4p

d)

5s

82.

Region of high probability of finding an electron

a)

atomic orbital

b)

ground state

c)

Heisenberg uncertainty principle

d)

electron configuration

83.

Each element on the periodic table can be identified by its

a)

classification as a solid, liquid or gas.

b)

location on the table.

c)

ability to react to form compounds.

d)

unique spectral "fingerprint."

84.

Emission spectra emitted by an element (or compound) will produce ___ through a spectroscope.

a)

bright lines

b)

a continuous rainbow

c)

dark lines

d)

white light

85.

The line with the shortest wavelength (in other words the greatest energy) is produced in the hydrogen spectrum when electron moves

a)

from n=2 to n=1

b)

rom n=4 to n=1

c)

from n=3 to n=1

d)

from n=4 to n=3

86.
The parallel lines represents...
a)
energy levels of the atom
b)
energy levels of the electrons
c)
energy levels of the photons
d)
energy levels of the nucleus
87.
Light is emitted when electrons ...
a)
jump from high to low 
b)
jump from low to high 
c)
either of these
d)
none of these
88.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Helium

89.

Look carefully at the picture. It shows an electron in the excited state on the left, and the electron returning to its ground state on the right. When the electron return to the ground state it emits a_______________________.

a)

blast of cold air

b)

electrostatic charge

c)

proton

d)

photon (light)

90.

The picture shows an atom in the ground state absorbing energy and the electron jumps to the excited state. Which state has higher energy?

a)

Ground State

b)

Excited State

91.

Line emission spectra is produced from atoms when

a)

electrons release energy as they move to their excited state.

b)

electrons absorb energy as they move to their excited state.

c)

electrons release energy as they return to the ground state.

d)

electrons absorb energy as they return to the ground state.

92.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
93.

When an electron moves from n=2 (energy level 2) to n=4 (energy level 4)

MULTIPLE ANSWERS: CHECK ALL CORRECT ANSWERS

a)

it must absorb light

b)

it will release light

c)

it will move farther from the nucleus

d)

it will move closer to the nucleus

94.

According to Bohr, the energy absorbed by an electron upon excitation comes in a fixed amount called

a)

exact energy

b)

fixed energy

c)

quantized energy

d)

None of the above

95.
Visible light is the only type of electromagnetic radiation.
a)
True
b)
False
96.
Every element has its own unique atomic spectra.
a)
True
b)
False
97.

Infrared rays have a shorter wavelength than

a)

Ultraviolet ray

b)

X-rays

c)

gamma rays

d)

radio waves

98.

What happens to frequency when the energy increases?

a)

it increases

b)

it stays the same

c)

it decreases

99.

Which wave has a longer wavelength?

a)

wave C

b)

wave D

100.

Which wave has a greater frequency?

a)

wave B

b)

wave C

101.

Which has the LONGEST wavelength and, therefore, the LOWEST frequency/energy

a)

Gamma Rays

b)

Visible Light

c)

Ultraviolet

d)

Infrared rays

102.

High frequency in EM waves equals

a)

high energy and short wavelength

b)

low energy and short wavelength

c)

high energy and long wavelength

d)

low energy and long wavelength

103.

Which section of the spectrum is the ONLY one we can see?

a)

X-rays

b)

Gamma Rays

c)

Visible Light

d)

Ultraviolet Rays

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