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3.3 e- configurations

Total questions: 60

Worksheet time: 2hrs 7mins

Name
Class
Date
1.
What is the electron configuration for Arsenic?
a)
1s2 2s2 2p6 3s2 3p6 4s2 4p3
b)
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6
c)
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3
d)
1s2 2s2 2p6 3s2 3p6 4s2 4d10 4p3
2.
The electron notation for aluminum is-
a)
1s2 2s2 2p6 3s2 2d1.
b)
1s2 2s2 2p9.
c)
1s2 2s2 2p6 3s2 3p1.
d)
1s2 2s2 2p3 3s2 3p3 3d1.
3.
Which element has a noble gas configuration of [Ne] 3s2 3p3?
a)
Magnesium
b)
Phosphorus
c)
Aluminum
d)
Sulfur
4.
What is the electron configuration for nitrogen? 
a)
1s2 2s3 2p2
b)
1s2 2s2 2p3
c)
1s2 2s2 2p2 3s1
d)
1s2 2s3 2p1
5.
The orbitals shown correspond to which elements?
a)
Nitrogen, Argon, Sodium
b)
Phosphorus, Neon, Sodium
c)
Nitrogen, Neon, Sodium
d)
Phosphorus, Argon, Sodium
6.
Which element has the electron configuration, 1s2 2s2 2p6 3s2 3p6 4s23d10?
a)
Phosphorus
b)
Zinc
c)
Potassium
d)
Copper
7.
The orbital notation shown represents an element in which block and period?
a)
Block-s and Period 2
b)
Block-p and Period 3
c)
Block-s and Period 4
d)
Block-d and Period 3
8.
What is the noble gas shorthand electron for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p4
9.
What is the electron configuration for this atom?
a)
1s22s22p6
b)
1s22s22p5
c)
1s22s22p3
d)
2s22p3
10.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
11.
Which is associated with more energy? 
a)
2p
b)
2s
c)
3p
d)
1s
12.
What is the charge of an atom that has lost one electron?
a)
-1
b)
-2
c)
+1
d)
+2
13.
What is the charge of an atom that has gained one electron?
a)
-1
b)
-2
c)
+1
d)
+2
14.
Anions are _______ that form ____________ ions and __________ electrons.
a)
nonmetals, positive, lose
b)
nonmetals, negative, gain
c)
metals, positive, gain
d)
metals, positive, lose
15.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
16.
How many electron can be found in a s orbital?
a)
2
b)
3
c)
4
d)
1
17.
How many electron can be found in a p orbital?
a)
2
b)
3
c)
4
d)
6
18.

What is the electronic configuration of sodium?

a)

1s22s22p63s1

b)

[Ne]3s1

c)

1s22s22p7

d)

1s22s22p63s1 AND [Ne]3s1

19.
What is the electronic configuration of iron?
a)
1s22s22p63s23p64s23d6
b)
1s22s22p63s23p63d8
c)
1s22p63s23p64s23d6
d)
1s22s22p63s23p64s13d6
20.
Which is the electron configuration for an oxygen atom?
a)
1s22s22p63s23p64s2
b)
electronic configuration
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p6
21.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
22.
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
23.
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
24.
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
25.
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
26.
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
27.
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
28.
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
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.
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
31.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
32.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
33.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
34.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
35.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
36.

What do you start all electron configurations with?

a)

1s2

b)

1d10

c)

1f14

d)

1p6

37.
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
38.

The 4 orbitals are

a)

s, p, d, f

b)

a, b, c, d

c)

2, 4, 6, 8

39.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
40.
How many p orbitals are there in a sublevel?
a)
2
b)
1
c)
4
d)
3
41.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
42.
What atom matches this electron configuration?
[Xe] 6s2 4f14 5d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
43.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
44.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
45.
What noble gas should be used to write the shorthand configuration for Te?
a)
Ar
b)
Kr
c)
Xe
d)
Sb
46.
Electron arrangement that uses arrows
a)
Electron configuration
b)
Shorthand configuration
c)
Lewis dot structure
d)
Orbital diagram
47.
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
48.
What does Pauli exclusion principle state ?
a)
states that each electron occupies the lowest energy orbital available
b)
states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins
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
49.
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
50.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

51.

The filling of which orbital is represented by the transition metals in period 4?

a)

3d

b)

3s

c)

2s

d)

2p

52.

What does Hund's rule state?

a)

An orbital can contain two electrons only if the electrons have opposite spins.

b)

An orbital can contain two electrons only if all other orbitals at that sublevel are empty.

c)

An orbital can contain two electrons only if the electrons have different energy levels.

d)

An orbital can contain two electrons only if all other orbitals in that sublevel contain at least one electron.

53.

What is the noble gas configuration for silicon?

a)

[Ne] 3s2 3p1

b)

[Ar] 4s1

c)

[Kr] 5s1

d)

[Ne] 3s2 3p2

54.

Which element has three unpaired electrons in its p orbital?

a)

carbon (atomic number 6)

b)

oxygen (atomic number 8)

c)

nitrogen (atomic number 7)

d)

beryllium (atomic number 4)

55.

The electron configuration 1s2 2s22p6 3s23p6 represents which noble gas?

a)

neon

b)

argon

c)

helium

d)

krypton

56.

What is the position of an element in the periodic table if its electron configuration is 1s2 2s2 2p6 3s2 3p5?

a)

Group 1A

b)

Group 2A

c)

Group 5A

d)

Group 7A

57.

Why do electrons enter the 4s orbital before entering the 3d orbital? 

a)

because the 3d orbital is at a lower energy level

b)

because both the 4s and 3d orbitals are at the same energy level

c)

because the 4s orbital is at a lower energy level

d)

because the 4s orbital is at a higher energy level

58.

Which electron configuration represents the element carbon (atomic number 6)?

a)

1s2 2s2 2p6

b)

1s2 2s2 2p4

c)

1s2 2s2 2p2

d)

1s2 2s2

59.

What does the sign represent with respect to electrons?

a)

opposite spin of two electrons

b)

different principal energy levels of two electrons

c)

distances of two electrons from the nucleus

d)

attraction between two electrons

60.

According to the Pauli exclusion principle, when can two electrons occupy the same orbital?

a)

only if there is no place else to put them

b)

only if they have the same spin

c)

only if they have opposite spins

d)

only if they are alike in all their properties

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