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ELECTRON CONFIGURATIONS

Total questions: 60

Worksheet time: 30mins

Name
Class
Date
1.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
2.
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

3.

What atom matches this electron configuration? 1s22s22p63s23p64s23d10 4p2

a)

Zinc

b)

Copper

c)

Nickel

d)

Germanium

4.
How many electrons can the s sublevel hold?
a)
14
b)
10
c)
2
d)
6
5.
How many electrons can the p sublevel hold?
a)
14
b)
10
c)
2
d)
6
6.

What atom matches this electron configuration? 1s22s22p63s23p64s23d5

a)

Zinc

b)

Copper

c)

Nickel

d)

Manganese

7.
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

8.
What is the number of valence electrons for Carbon?
a)

12

b)

6

c)

4

9.

How many valence electrons are represented here?

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

a)

2

b)

12

c)

4

d)

10

10.
What is the correct electron configuration for a ground-state atom with 7 electrons? 
a)

 a. 1s2 2s2 2p3

b)

 b. 1s2 2s2 2p2 3s1

c)

c. 1s2 2s3 2p2

d)

 d. 1s2 2s5

11.

What atom matches this electron configuration? 1s2 2s2 2p6 3s2 3p6 4s1

a)

Magnesium

b)

Aluminum

c)

Potassium

d)

Calcium

12.
How many valence electrons does Chlorine have?
a)

5

b)

7

c)

5

13.
What do you start electron configuration with?
a)

1s2

b)

1d10

c)

1f14

d)

1p6

14.
There are 4 different types of subshells s,p,d,f
a)
true
b)
false
15.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)

3

b)

6

c)

8

d)

10

16.

Identify the Electron Configuration for Gallium (Ga).

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3

c)

1s2 2s2 2p6 3s2 4p1

17.

What is this element? [Kr] 5s2 4d10 5p5

a)

Iodine

b)

Tellurium

c)

Bromide

18.

Which of the following is a p block element?

a)

Calcium

b)

Argon

c)

Osmium

d)

Gold

19.

What element has the valence shell configuration

3s2 3p2

a)

Aluminium

b)

Boron

c)

Silicon

d)

Gallium

20.

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

a)

representative elements

b)

rare earth elements

c)

transition elements

21.

Which of the following is not a correct designation for a sublevel?

a)

zz

b)

p

c)

d

d)

f

22.

This could be the dot diagram of

a)

Magnesium

b)

Chlorine

c)

Carbon

d)

Oxygen

23.

What is the noble gas configuration for beryllium (Be)?

a)

[He]1s2

b)

[Li]2s2

c)

[He]2s2

24.

What is the noble gas short configuration for Astatine (At)?

a)

[Kr] 5s2 4d10 5p4

b)

[Xe] 6s2 4f14 5d10 6p5

c)

[Xe] 6s2 5d10 6p5

25.

What is the noble gas short configuration for Strontium (Sr)?

a)

[Ar] 4s2 3d10 4p6 5s2

b)

[Ne] 3s2 3p4

c)

[Kr] 5s2

26.

What is the noble gas short configuration for Tin (Sn)?

a)

[Kr] 5s2 4d10 5p2

b)

[Ar] 4s2 3d10 4p2

c)

[Xe] -5p4

d)

[Rb] 5s2 4d10 5p2

27.
What is the noble gas configuration for Neon?
a)

[Ne]

b)

[He]2s22p6

c)

[F]2p1

d)

[Ne]2s21p6

28.
[Ne]3s1 is the noble gas configuration for which element?
a)

sodium

b)

fluorine

c)

aluminum

29.

[Ne]3s23p1 is the noble gas configuration for which element?

a)

scandium

b)

boron

c)

aluminum

30.

What atom matches the electron configuration below?

1s2 2s2 2p6 3s2 3p6 4s23d10

a)

Zinc

b)

Copper

c)

Nickel

31.

What is the short electron configuration for silver?

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1 4d10

b)

[Kr] 5s1 4d10

c)

[Ar] 4s2 3d9

32.

What is the proper Noble Gas notation for the electron configuration of a neutral atom of Germanium (Ge)?

a)

[Ne] 4s23d104p2

b)

[Ar] 4s23d104p2

c)

[Kr]4s23d104p2

33.

Which neutral atom has the following electron configuration: |Xe| 6s2 4f14 5d4

a)

Hassium (Hs)

b)

Tungsten (W)

c)

Lutetium (Lu)

34.

Which one of the following statements about d orbitals is incorrect?

a)

they are not found in the first two principal energy levels

b)

d orbitals are filled before p orbitals in the same principal energy level

c)

they are associated with transition elements

35.

Which subshell is highlighted in the periodic table below?

a)

5s

b)

5p

c)

4p

36.

Which of the following is the noble gas short for Rubidium (Rb)?

a)

[Ar] 5s1

b)

[Kr] 5s1

c)

[Xe] 4s1

37.

The electron configuration below is for which element? [Xe]5d106s26p4

a)

Lead (Pb)

b)

Bismuth (Bi)

c)

Polonium (Po)

38.

What element am I? [He]2s2 2p5.

a)

Fluorine

b)

Chlorine

c)

Neon

39.

[Ne]3s23p6 What element does this configuration represent?

a)

Calcium(Ca)

b)

Sulfur (S0

c)

Argon (Ar)

40.

Which of the following orbital notations for phosphorus is correct?

a)
b)
c)
d)
41.

The diagram represents two electrons with  

a)

opposite spin states.

b)

the same spin state.

c)

different energies.

d)

the same energy.

42.

What is the correct electron configuration for an atom with 7 electrons?

a)

1s22s32p2

b)

1s22s22p23s1

c)

1s22s22p3

d)

1s22s5

43.

What is the correct noble-gas notation for the electron configuration of an atom of Calcium (Cl)?

a)

[Ar]3s23p5

b)

[Ne]4s2

c)

[Ar]4s2

d)

[Ne]3s23p5

44.

Which element is depicted in this orbital diagram

a)

Neon

b)

Chlorine

c)

Argon

45.
This orbital diagram represents:  
a)

Carbon

b)

Fluorine

c)

Oxygen

46.

How many valence electrons are in this element? AND identify the element.

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d3

a)

11; Hafnium (Hf)

b)

2; Barium (Ba)

c)

3; Lanthanum (La)

d)

2; Tantalum (Ta)

47.

What is the shape of a p orbital?

a)

sphere

b)

it's just too complex to think about it

c)

dumbbell

d)

It has 4 lobes

48.

What is the shape of an s orbital?

a)

sphere

b)

dumbbell

c)

double dumbbell

49.

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

a)

Zinc

b)

Copper

c)

Nickel

d)

Germanium

50.

What atom matches this electron configuration? 1s2 2s2 2p6 3s2 3p6 4s1

a)

Potassium (K)

b)

Magnesium (Mg)

c)

Sodium (Na)

d)

Gallium (Ga)

51.

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)

52.

Which of the following is NOT a valid electron configuration?

a)

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

b)

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

c)

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

d)

1s2 2s2 2p6 3s2 3p6

53.
This is the electron configuration for what element... 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p1
a)

Aluminum

b)

Indium

c)

Gallium

d)

Silicon

54.
Noble gas notation for Radium
a)

[Rn] 7s1

b)

[Rn] 7s2

c)

[Og] 7s1

d)

[Og] 7s2

55.

Which element is represented by this orbital notation?

a)

Neon

b)

Sodium

c)

Magnesium

d)

Aluminum

56.

Choose the correct shortcut configuration for iodine.

a)

[Ar]4s24d104p5

b)

[Kr]5s24d105p5

c)

[Xe]5s25d105p5

57.
Identify the element whose electron configurations ends with 5p3
a)

Arsenic (As)

b)

Tellurium (Te)

c)

Antimony (Sb)

d)

Tin (Sn)

58.

Which of the following groups of atoms have the same outermost electron configurations but with different (principal) energy levels?

a)

N, O, F, Ne

b)

Ca, Ge, Sr, In

c)

O, S, Se, Te

d)

S, Cl, Ar, K

59.

The letter designations for the first four sublevels with the maximum number of electrons that can be accommodated in each sublevel are

a)

s:1, p:3, d:10, and f:14

b)

s:1, p:3, d:5, and f:7.

c)

s:1, p:2, d:3, and f:4

d)

s:2, p:6, d:10, and f:14.

60.

What comes after 5s?

a)

5p

b)

5d

c)

4d

d)

6s

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