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Practice test on Electrons in atoms

Total questions: 49

Worksheet time: 41mins

Name
Class
Date
1.

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

a)

absorbs energy

b)

releases energy

2.

What is the electron configuration of an atom that has eight electrons?

a)

1s22s22p22p2

b)

1s22s22p23s2

c)

1s21p22s22p2

d)

1s22s22p4

3.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
4.
What is the noble gas shorthand electron for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p4
5.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
6.
The electron configuration of an atom is 1s22s22p6.  The number of valence electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
7.
Valence electrons are: 
a)
Electrons farthest away from the nucleus
b)
Electrons closest to the nucleus
c)
Electrons that just come and go - they don't stay with the atom
8.
Which is associated with more energy? 
a)
2p
b)
2s
c)
3p
d)
1s
9.

Chemists can identify the composition of some unknown salts by conducting a flame test. When potassium salts are heated in a flame, a purple color is observed.


This is due to the movement of electrons between energy levels. What is the electron configuration of a potassium atom at ground state?

a)

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

b)

1s2; 2s2; 2p6; 3s2;3p6; 3d1

c)

1s2; 2s2; 2d6; 3s2; 3d6; 4s1

d)

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

10.
What is the Pauli Exclusion Principle?
a)
An atomic orbital can only hold a maximum of 2 electrons, each with opposite spins
b)
An atomic orbital can hold a minimum of 6 electrons, each with opposite spins
c)
An atomic orbital can hold a maximum of 6 electrons, each with the same spin
d)
An atomic orbital can hold a minimum of 2 electrons, each with opposite spins
11.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
12.
What shape are P Orbitals? 
a)
Cloverleaf shaped
b)
Spherical shaped
c)
Hybrid structure
d)
Dumbell shaped
13.
Hund’s rule states…
a)
Atomic orbitals have opposite spins and 2 electrons each
b)
Electrons occupy orbitals of highest energy first and energy level changes as you go up
c)
Electrons occupy orbitals of lowest energy first, starting with 1s
d)
Electrons occupy orbitals of equal energy, one electron enters EACH orbital ONE AT A TIME until orbitals of the entire energy level have one electron with the SAME SPIN.
14.
What is the electron configuration of Ag?
a)
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d9
b)
[Kr] 5s2 4d9
c)
1s2 2s2 2p6 3s2 3p6 4s2 4p6 5s2 4d9
d)
1s2 2s2 2p6 
15.
How many orbitals are there in the "d" sublevel?
a)
1
b)
3
c)
5
d)
7
16.
How many total electrons can the orbitals in the "f" sublevel hold?
a)
2
b)
14
c)
6
d)
10
17.
What shape are D Orbitals?
a)
Hybrid structure
b)
Spherical shaped
c)
Dumbell shaped
d)
Cloverleaf shaped
18.

How many sub-levels are in the 2nd Energy Level

a)

1

b)

2

c)

3

d)

4

19.

How many orbitals are on the 3rd energy level?

a)

1

b)

9

c)

12

d)

3

20.

How many energy levels are on the periodic table

a)

3

b)

18

c)

5

d)

7

21.

How many electrons can you put in the 2nd Energy Level?

a)

2

b)

6

c)

8

d)

18

22.

How many sub-levels are in the 4th Energy Level?

a)

1

b)

2

c)

3

d)

4

23.

How many electrons can fit in the 3rd Energy Level?

a)

18

b)

8

c)

2

d)

32

24.

Write the electron configuration for Beryllium

a)

1S2S2

b)

2S2

c)

1S22s2

d)

1s22S22P2

25.

Write the shorthand electron configuration for Ca

a)

1S22S22P63S23P64S2

b)

[Kr]4S2

c)

[Ar]4S2

d)

[Ar)2P2

26.

What atom matches this electron configuration?

1s22s22p63s23p64s23d10

a)

Zinc

b)

Copper

c)

Nickel

d)

Germanium

27.

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

28.

What electron configuration matches an oxygen atom?

a)

1s22s22p63s2, 3p64s23d104p5

b)

1s22s22p4

c)

1s22s22p6

d)

1s22s22p63s23p64s23d1

29.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
30.

How many valence electrons does Lithium (Li) have?

a)

8

b)

1

c)

5

d)

2

31.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

32.
This could be the dot diagram of 
a)
Ne
b)
Si
c)
Al
d)
Be
33.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

34.

How many VALENCE ELECTRONS does Boron have?

a)

3

b)

5

c)

2

35.

How many VALENCE ELECTRONS does Nitrogen have?

a)

7

b)

5

c)

2

36.
What element's orbital diagram is shown in the figure?
a)
stontium
b)
chromium
c)
antimony
d)
fluorine
37.

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

a)

2

b)

6

c)

3

d)

8

38.

This is the shape of ____ orbital

a)

s

b)

d

c)

p

d)

d

39.

This shape is that of

a)

s-orbital

b)

d-orbital

c)

p-orbital

d)

f-orbital

40.

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

41.

What model is the current model of the atom?

a)

Rutherford's

b)

Bohr's

c)

The Quantum Mechanical Model

d)

Dalton's

42.
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
43.
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
44.
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
45.
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
46.
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
47.
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
48.

If waves can behave like particles, then particles can behave like a wave. This is the idea behind...

a)

Quantization of Energy

b)

Photoelectric Effect

c)

Compton Effect

d)

deBroglie Waves

49.

Determined that electron paths cannot be predicted and exist inside the Electron Cloud. Defined it with mathematics as a probability.

a)

John Dalton

b)

Ernest Rutherford

c)

Schrodinger & Heisenberg

d)

Bohr

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