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Electrons in the Atom PRACTICE

Total questions: 50

Worksheet time: 39mins

Name
Class
Date
1.

Maximum number of ELECTRONS that can be placed in an s orbital.

a)

2

b)

6

c)

10

d)

14

2.

The maximum number of ELECTRONS that can be placed in an p orbital.

a)

2

b)

6

c)

10

d)

14

3.

The maximum number of ELECTRONS that can be placed in an d orbital.

a)

2

b)

6

c)

10

d)

14

4.

The maximum number of ELECTRONS that can be placed in an f orbital.

a)

2

b)

6

c)

10

d)

14

5.

Which orbital is spherical and has the lowest energy

a)

s

b)

p

c)

d

d)

f

6.
What is the shape of s orbitals?
a)
Dumbbell shaped
b)
Peanut shaped
c)
Spherical shaped
d)
Hybrid structure
7.

What is the Aufbau principle?

a)

electrons always spin right

b)

electrons always pair up

c)

electrons always enter the HIGHER energy orbitals first

d)

electrons always enter the LOWER energy orbitals first

8.

What is Hund's Rule?

a)

electrons always pair up first

b)

electrons must equally distribute between orbitals before pairing up

c)

electrons always spin right

d)

electrons must go to the nucleus for instructions

9.

Which colored area represent the s orbitals?

a)

blue

b)

red

c)

orange

d)

green

10.

Which colored area represent the f orbitals?

a)

blue

b)

red

c)

orange

d)

green

11.

Electrons in the same orbital ......

a)

must have opposite spins

b)

must have the same spin

c)

one must be negatively charged and the other positively charged

d)

must have lower energy

12.

According to the shell model of the atom, which of the following elements has a full outer energy level of electrons?

a)

krypton

b)

strontium

c)

iodine

d)

sodium

13.
In a stable atom the amount of electrons is electron is equal to
a)
neutrons
b)
protons
c)
atomic mass
d)
neutrons + protons
14.
What is the location of the electron?
a)
the free floating negatively charged electron cloud
b)
the free floating positively charged electron cloud
c)
the very dense positively charged electron orbital
d)
the positively charged very dense nucleus
15.
How many electrons does an atom with 8 protons have?
a)
8
b)
16
c)
15.99
d)
24
16.
Which of the following best describes an electron?
a)
It has no charge and about the same mass as a proton
b)
It has a negative charge and much less mass than a proton
c)
It has a positive charge and much more mass than a neutron
d)
It has a negative charge and about the same mass as a neutron
17.
The higher the frequency the ______ the energy. 
a)
higher
b)
lower
c)
neither, stays the same
18.

What is the name of the element whose electron configuration is 1s22s22p3?

a)

magnesium

b)

nitrogen

c)

carbon

d)

phosphorous

19.
What is the noble gas shorthand electron for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p4
20.
What element's orbital diagram is shown in the figure?
a)
stontium
b)
chromium
c)
antimony
d)
fluorine
21.

The distance between two successive crests of a waves is the

a)

speed

b)

frequency

c)

wavelength

d)

energy

22.
Who discovered the electron?
a)
Dalton
b)
Thomson
c)
Rutherford
d)
Bohr
23.
What is the total number of energy levels used by an atom of aluminum
(Al, atomic #13) in the ground state?
a)
3
b)
7
c)
13
d)
0
24.
Based on the picture, choose the best description of how wavelength and frequency are related
a)
As wavelength increases, frequency increases
b)
As frequency increases, wavelength remains the same
c)
As frequency increases, wavelength decreases
d)
frequency and wavelength mean the same thing
25.
Which element has the following noble gas notation [Ar]4s23d104p5?
a)
bromine
b)
calcium
c)
helium
d)
boron
26.
What is the shape of a p atomic orbital?
a)
an oval
b)
a sphere
c)
an egg
d)
a dumbbell or peanut
27.

Which of the following elements has a full outer energy level of electrons?

a)

krypton

b)

strontium

c)

iodine

d)

sodium

28.

If the wavelength of an electromagnetic wave is longer, what is true about the energy?

a)

Energy is higher.

b)

Energy is lower.

c)

Energy is not dependent on wavelength.

d)

Energy is cancelled out.

29.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
30.
Which portion of the electromagnetic spectrum includes the range of light that can be detected by the human eye? 
a)
ultraviolet light
b)
visible light
c)
infrared light
d)
x-rays
31.

The maximum number of ELECTRONS that can be placed in an f orbital.

a)

2

b)

6

c)

10

d)

14

32.

How many VALENCE ELECTRONS are represented here?

a)

7

b)

5

c)

2

d)

8

33.

What orbital level comes after 6s?

a)

7s

b)

6p

c)

5d

d)

4f

34.

the minimum quantity of energy that can be lost or gained by an atom → frequency

a)

true

b)

false

35.

all the forms of electromagnetic radiation

a)

electromagnetic spectrum

b)

line emission spectrum

c)

electromagnetic radiation

d)

photoelectric effect

36.

The images above, in order, are images of the orbitals:

a)

s, p, d

b)

p, d, s

c)

s, d, p

d)

d, s, p

37.

How many valence electrons are represented here?

a)

2

b)

4

c)

8

d)

12

38.

1. What atom matches this electron configuration?

1s2 2s2 2p6 3s23p4

a)

sodium

b)

sulfur

c)

silicon

d)

potassium

39.

What is the correct electron configuration for oxygen?

a)

1s22s22p63s23p64s2

b)

1s22s22p63s23p4

c)

1s12s22p5

d)

1s22s22p4

40.

What is this element?

1s2 2s2 2p6 3s2 3p6 4s2 3d5

a)

magnesium

b)

iron

c)

manganese

d)

chromium

41.

Which element is show above?

a)

lithium

b)

hydrogen

c)

helium

d)

carbon

42.

Which of the following is correct for germanium (Ge)?

a)

[Ar] 4s2 4d10 4p2

b)

1s2 2s2 2p6 3s2 3p6 4s2 4d10 4p2

c)

[Ar] 4s2 3d10 4p2

d)

4s2 3d10 4p2

43.
If an electron moves from n=5 to n=2 ...
a)
it absorbs energy
b)
it releases energy
44.

The element with electron configuration 1s22s22p63s23p2

a)

Si

b)

Mg

c)

S

d)

C

45.
What element's orbital diagram is shown in the figure?
a)
stontium
b)
chromium
c)
antimony
d)
fluorine
46.

Which change occurs when an atom in an excited state returns to the ground state?

a)

Energy is emitted

b)

Energy is absorbed

c)

The number of electrons decreases

d)

The number of electrons increases

47.

Which electron configuration is correct for oxygen (8O)?

a)

1s22s22p63s2, 3p64s23d104p5

b)

1s22s22p4

c)

1s22s22p6

d)

1s22s22p63s23p64s23d1

48.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
49.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
50.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3

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