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Electrons Review

Total questions: 71

Worksheet time: 2hrs 12mins

Name
Class
Date
1.

What does #1 represent?

a)

Period

b)

Frequency

c)

Wavelength

d)

Amplitude

2.

What does #2 represent?

a)

Period

b)

Frequency

c)

Wavelength

d)

Amplitude

3.
What property of this wave is represented by the letter "A"
a)
amplitude
b)
crest
c)
trough
d)
wavelength
4.
Which wave in the diagram has the greatest frequency?
a)
1
b)
2
c)
3
d)
4
5.
Which wave in the diagram has the greatest wavelength?
a)
1
b)
2
c)
3
d)
4
6.

If a wave has a greater frequency, what happens to the wavelength?

a)

increases

b)

decreases

c)

stays the same

7.

What property does the orange arrow (A) represent?

a)

Crest

b)

Trough

c)

Wavelength

d)

Peak

8.
Which wave has a greater frequency?
a)
A
b)
B
9.

If a wave has a greater frequency, what happens to the wavelength?

a)

increases

b)

decreases

c)

stays the same

10.

If a wave has a greater frequency, what happens to number of waves per second?

a)

increases

b)

decreases

c)

stays the same

11.

Which EM waves have the longest wavelength?

a)

radio

b)

x-rays

c)

ultraviolet

d)

gamma rays

12.

Which EM waves have the shortest wavelength?

a)

radio

b)

x-rays

c)

ultraviolet

d)

gamma rays

13.

Which EM waves are have a SHORTER wavelength than visible?

a)

radio

b)

none

c)

infrared

d)

x-rays

14.

Which EM waves are have the lowest frequency?

a)

radio

b)

none

c)

infrared

d)

x-rays

15.

Which EM waves are have the highest energy & are the most dangerous?

a)

radio

b)

gamma rays

c)

infrared

d)

x-rays

16.

The lower the frequency the ______ the energy.

a)

higher

b)

lower

c)

neither, stays the same

17.
The higher the frequency the ______ the energy. 
a)
higher
b)
lower
c)
neither, stays the same
18.

Which color has the longest wavelength?

a)

Red

b)

Orange

c)

Yellow

d)

Blue

19.

Which color has the shortest wavelength?

a)

Red

b)

Orange

c)

Yellow

d)

Blue

20.

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."

21.

What subatomic particle is responsible for the spectral lines seen in emission spectra diagrams?

a)

electrons

b)

protons

c)

neutrons

22.

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

a)

emit energy

b)

absorb energy

c)

wiggle

23.

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

a)

emit energy

b)

absorb energy

c)

rotate

d)

wiggle

24.

If an electron moves from n=4 to n=2 it ____

a)

absorbs energy

b)

releases energy

25.

Which element(s) is/are found in the star's spectra below?

a)

Hydrogen only

b)

Hydrogen & Helium

c)

Calcium only

d)

Hydrogen & Calcium

26.
Which elements are in the unknown sample?
a)
A and B
b)
B and C
c)
A and D
d)
B and D
27.

True or False: The ground state is the highest energy state of an atom.

a)

True

b)

False

28.

What is the light that you can see called?

a)

observatory light

b)

ultraviolet light

c)

visible light

d)

infrared light

29.
Line emission spectrum shown below happens when
a)
Electron transition from lower to higher energy level.
b)
Electron transition from higher to lower energy level.
c)
Electron exist in fixed energy states
d)
Electron transition between different energy levels.
30.
Emission of light from an atom occurs when an electron
a)
drops from a higher to a lower energy level.
b)
   jumps from a lower to a higher energy level.   
c)
   moves within its atomic orbital.
d)
falls into the nucleus.
31.
Why are line emission spectra of elements called "atomic fingerprints"?
a)
They are all the same
b)
They are all unique
c)
They are all similar
d)
They all contain colored light
32.

All stars are composed of a mixture of elements. When these elements are heated they emit specific amounts of electromagnetic radiation, known as an emission spectrum. Each element emits a unique, identifiable, spectrum.


Using the Bright-line emission spectrum chart below, identify the elements present in this modeled star (found in the line labeled “mixture”).

a)

Lithium and cadmium are in the mixture. Strontium is not in the mixture.

b)

Lithium and strontium are in the mixture. Cadmium is not in the mixture

c)

Cadmium and strontium are in the mixture. Lithium is not in the mixture

d)

All of the shown elements are present in the mixture.

33.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Sodium

34.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Sodium

35.
What gases are in the unknown mixture?
a)
Gas B & Gas D
b)
Gas C & Gas B
c)
Gas A & Gas D
d)
Gas D & Gas C
36.
Which elements are in the unknown sample?
a)
A and B
b)
B and C
c)
A and D
d)
B and D
37.

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)

38.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
39.

The second shell from the center of an atom can hold how many electrons?

a)

2

b)

6

c)

8

d)

18

40.

Valence electrons are located...

a)

inside the nucleus

b)

in outer space

c)

on the outermost orbit of an atom

41.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
42.

How many electrons can the d sublevel hold?

a)
8
b)
10
c)
2
d)
4
43.

How many electrons can the p sublevel hold?

a)
8
b)

6

c)
2
d)
4
44.

What is the maximum number of electrons that an s orbital can have?

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

4 electrons

45.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
46.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
47.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
48.

What do you start all electron configurations with?

a)

1s2

b)

1d10

c)

1f14

d)

1p6

49.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
50.
What atom matches this electron configuration?
[Xe] 6s2 4f14 5d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
51.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

52.

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

53.

Determine the group and periodicity of the following atoms!

a)

IIIA and 2

b)

IIA and 2

c)

VA and 3

d)

IVA and 1

54.

The element Br has mass number 80 and 45 neutron. How many electron valence this atom has?

a)

Seven

b)

Eleven

c)

Sevel

d)

Eight

55.

What element has the electron configuration 

1s22s22p31s^22s^22p^3  

a)

Nitrogen

b)

Oxygen

c)

Magnessium

d)

Carbon

56.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
57.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
58.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
59.
What atom matches this electron configuration?
[Xe] 6s2 4f14 5d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
60.
Which electron configuration belongs to Copper (Cu)?
a)
1s2 2s2 2p6 3s2 3p6 4s2 3d8
b)
1s2 2s2 2p6 3s2 3p6 4s2 3d9
c)
1s2 2s2 2p6 3s2 3p6 4s2 3d10
61.

Electron configuration of beryllium (Be)

a)

1s2 2s1 2p11s^{2^{\ }}2s^1\ 2p^1  

b)

1s2 2p11s^2\ 2p^1  

c)

1s2 2s11s^2\ 2s^1  

d)

1s2 2s2 2p11s^2\ 2s^2\ 2p^1  

62.

Electron configuration of boron (B)

a)

1s2 2s1 2p11s^{2^{\ }}2s^1\ 2p^1  

b)

1s2 2s2 2p11s^2\ 2s^{2\ }2p^1  

c)

1s2 2s11s^2\ 2s^1  

d)

1s1 2s1 2p11s^1\ 2s^1\ 2p^1  

63.

Electron configuration of fluorine (F)

a)

1s1 2s2 2p51s^{1^{\ }}2s^2\ 2p^5  

b)

1s2 2s2 2p71s^2\ 2s^{2\ }2p^7  

c)

1s2 2s2 2p51s^2\ 2s^2\ 2p^{5^{ }}  

d)

1s1 2s1 2p51s^1\ 2s^1\ 2p^5  

64.

Electron configuration of neon (Ne)

a)

1s2 2s2 2p21s^{2^{\ }}2s^2\ 2p^2  

b)

1s1 2s2 2p61s^1\ 2s^{2\ }2p^6  

c)

1s2 2s2 2p101s^2\ 2s^2\ 2p^{10^{ }}  

d)

1s2 2s2 2p61s^2\ 2s^2\ 2p^6  

65.

What is the electron configuration for potassium (K) ?

a)

1s2 2s2 2p2 3s2 3p2 4s2 3d2 4p2 5s2 4d2

b)

1s2 1p6 1d10 1f1

c)

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

d)

1s2 2s2 2p6 3s2 3p6 4s1

66.

What atom matches this electron configuration? 1s2 2s2 2p6 3s2 3p6 4s2 3d6

a)

Sulfur (S)

b)

Magnesium (Mg)

c)

Selenium (Se)

d)

Iron (Fe)

67.

What atom matches this electron configuration? 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3

a)

Phosphorus (P)

b)

Nitrogen (N)

c)

Arsenic (As)

d)

Niobium (Nb)

68.

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

a)

Argon (Ar)

b)

Neon (Ne)

c)

Chlorine (Cl)

d)

Iron (Fe)

69.

What is the noble gas configuration for silicon?

a)

[Ne] 3s2 3p1

b)

[Ar] 4s1

c)

[Kr] 5s1

d)

[Ne] 3s2 3p2

70.

What is the position of an element in the periodic table if its electron configuration is 1s2 2s2 2p6 3s2 3p5?

a)

Group 1A

b)

Group 2A

c)

Group 5A

d)

Group 7A

71.

The electron configuration 1s2 2s22p6 3s23p6 represents which noble gas?

a)

neon

b)

argon

c)

helium

d)

krypton

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