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Unit 4: Final Review (HONORS) Electrons

Total questions: 30

Worksheet time: 50mins

Name
Class
Date
1.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
2.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
3.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
4.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
5.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
6.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
7.
What do you start electron configuration with?
a)
1s2
b)
1d10
c)
1f14
d)
1p6
8.
What is this element?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
9.
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
10.
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
11.
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
12.
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
13.

What does Pauli exclusion principle state ?

a)

states that each electron occupies the lowest energy orbital available

b)

states that -no two electrons in the same orbital can have the same spin

c)

states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals

14.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
15.

How many electrons can the d sublevel(orbital) hold?

a)

8

b)

10

c)

2

d)

4

16.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
17.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
18.

Which area on the periodic table represents the electrons in the "d" sublevel?

a)

representative elements

b)

columns 3-8

c)

rare earth elements

d)

transition elements

19.
Anions are _______ that form ____________ ions and __________ electrons.
a)
nonmetals, positive, lose
b)
nonmetals, negative, gain
c)
metals, positive, gain
d)
metals, positive, lose
20.
The total number of orbitals that can exist at the second main energy level is
a)
2
b)
3
c)
4
d)
8
21.
If electrons in an atom have the lowest possible energies, the atom is in the
a)
ground state.
b)
inert state.
c)
excited state.
d)
radiation-emitting state.
22.
An orbital that can never exist according to the quantum description of the atom is
a)
6d.
b)
3f.
c)
3d.
d)
8s.
23.
Which orbital shows a violation of the Aufbau Principle?
a)
A
b)
B
c)
C
d)
D
24.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
25.
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.
26.
Which orbital has the least amount of energy? 
a)
p orbital
b)
d orbital
c)
s orbital 
d)
What is an orbital?
27.

How many orbitals does a d sublevel have?

a)

1

b)

3

c)

5

d)

7

28.

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

a)

energy level

b)

s orbitals

c)

p orbitals

d)

the number of electrons

29.

What is the noble gas configuration for Cobalt?

a)

[Kr] 4s2 3d7

b)

[Kr] 4s2 4d7

c)

[Ar] 4s2 3d7

d)

[Ar] 4s2 4d7

30.

What is the noble gas configuration for 1s2 2s2 2p6 3s2?

a)

[He] 3s2

b)

[Ne] 3s2

c)

[Ar] 3s2

d)

[Ar] 4s2

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