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Electron Configuration & Groups on the Periodic table

Total questions: 60

Worksheet time: 6hrs 33mins

Name
Class
Date
1.

Which equation helps you calculate the number of electrons in an energy level?

a)

N2

b)

2N

c)

2N2

2.

How many sublevels are there in the following and what orbitals

a)

N=2

1.

2 sublevels

Orbitals are S& P

b)

N=4

2.

4 sublevels

Orbitals are S, P, D & F

c)

N=1

3.

1 sublevel

orbitals are S

3.

What element has this orbital notation?

a)

lithium

b)

beryllium

c)

boron

d)

carbon

4.

What element has this electron configuration?

a)

helium

b)

lithium

c)

beryllium

d)

boron

5.

What element has this electron configuration?

a)

boron

b)

carbon

c)

nitrogen

d)

oxygen

6.

Which element is represented by this orbital notation?

a)

carbon

b)

nitrogen

c)

oxygen

d)

fluorine

7.

Which element is represented by this electron configuration?

a)

neon

b)

sodium

c)

magnesium

d)

aluminum

8.

Which element is represented by this orbital notation?

a)

neon

b)

sodium

c)

magnesium

d)

aluminum

9.

Which of the following is the electron configuration for Fluorine

a)
b)
c)
d)
10.

Which of the following is the electron configuration for silicon?

a)
b)
c)
d)
11.

Which of the following is the orbital notation for oxygen?

a)
b)
c)
d)
12.
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
13.
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
14.
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
15.
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
16.
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
17.

What is the element?

a)

Neon

b)

Chlorine

c)

Aluminum

d)

Argon

18.

What is the element?

a)

sulfur

b)

chlorine

c)

phosphorus

d)

silicon

19.

Put the orbitals in order from the smallest to largest?

a)

1s

b)

2p

c)

3s

d)

4d

1)
2)
3)
4)
20.

How many electrons can fill the 2nd energy level of an atom?

(a)  

21.

Which of the following is the correct shorthand notation for aluminum?

a)

[Ne] 3s2 3p1

b)

[Ar] 3s2 3p1

c)

[Ne] 4s2 4p1

d)

[He] 3s2 3s1

22.

Which of the following is the proper shorthand notation for nickel?

a)

[Ar] 4s2 3d8

b)

[Kr] 4s2 3d8

c)

[Ar] 4s2 4d8

d)

[Kr] 4s2 4d8

23.

Which element is represented by the following electron configuration?

[Ar] 4s2 3d3

a)

V

b)

Nb

c)

As

d)

P

24.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
25.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
26.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
27.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
28.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
29.
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
30.
What is the noble gas configuration for Sulfur?
a)
[Ar] 3p4
b)
[He] 3s2 3p4
c)
[Ne] 3s2 3p4
d)
[Na] 3s2 3p4
31.
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
32.
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.
33.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
34.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
35.

What are the four energy sublevels?

a)

s, p, d, and f

b)

a, b, c, and d

c)

w, x, y, and z

d)

1, 2, 3, and 4

36.

If the f energy sublevel has a total of seven orbitals, what is the maximum number of electrons that it can hold?

a)

2

b)

10

c)

14

d)

6

37.

Determine the principal energy level in: 4s24s^2  

a)

4

b)

s

c)

2

d)

8

38.

What element has this electron configuration?

a)

boron

b)

carbon

c)

nitrogen

d)

oxygen

39.

Which of the following is the electron configuration for Fluorine

a)
b)
c)
d)
40.
What does Hund's rule states ?
a)
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
b)
states that each electron occupies the lowest energy orbital available
c)
states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins
41.

How many valence electrons are represented here?

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

a)

2

b)

12

c)

4

d)

10

42.

Match the following

a)

lithium (3)

1.

2 energy levels

b)

helium (2)

2.

1 energy level

c)

aluminum(13)

3.

3 energy levels

d)

bromine(35)

4.

4 energy levels

e)

strontium(38)

5.

5 energy levels

43.

How many orbitals are found in 4f​ ​

a)

How many orbitals in 4f

1.

7

b)

How many orbitals in N=3

2.

9

c)

How many orbitals in 2s

3.

1

d)

How many orbitals in 3f

4.

not possible

e)

How many orbitals in N=4

5.

16

44.

Which equation helps you calculate the number of orbitals in an energy level?

a)

N2

b)

2N

c)

2N2

45.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
46.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
47.

Which electron configurations do not exsist?

a)

2s3

b)

2d10

c)

7s25f12

d)

2s2 2p4

e)

4s24d4

48.
What do you start electron configuration with?
a)
1s2
b)
1d10
c)
1f14
d)
1p6
49.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
50.
What atom matches this electron configuration?
[Xe] 6s2 4f14 5d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
51.
What noble gas should be used to write the shorthand configuration for Te?
a)
Ar
b)
Kr
c)
Xe
d)
Sb
52.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
53.
What is the shape of a p orbital?
a)
sphere
b)
it's just too complex to think about it
c)
dumbbell
d)
I don't know this stuff.
54.
What is the shape of an s orbital?
a)
sphere
b)
dumbbell
c)
double dumbbell
d)
TOO COMPLEX TO KNOW IT.
55.
Which is associated with more energy? 
a)
2p
b)
2s
c)
3p
d)
1s
56.
How many total electrons can the f orbitals in a sublevel hold?
a)
2
b)
14
c)
6
d)
10
57.
There are 4 different types of sublevels on the periodic table:
s,p,d,f
a)
True
b)
False
58.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
59.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
60.
Which orbital shows a violation of the Aufbau Principle?
a)
A
b)
B
c)
C
d)
D

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