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Test Review: e-config. and the P.T.

Total questions: 80

Worksheet time: 2hrs 32mins

Name
Class
Date
1.

What are the sublevels named?

a)

1, 2, 3, 4

b)

s, p, d, f

c)

+1/2 (CW) and -1/2 (CCW)

d)

x, y, z axis

2.

how many electrons can fit in an orbital of the 4s sublevel?

a)

1

b)

2

c)

14

d)

10

3.

Within an orbital, do electrons have the same or opposite spins?

a)

same

b)

opposite

4.

how many orientations can a p sublevel have around the nucleus?

a)

1

b)

3

c)

5

d)

7

5.

how many sublevels are there in the second energy level

a)

1

b)

2

c)

3

d)

4

6.

where are the metals located on the periodic table?

a)

right of the staircase

b)

on the staircase

c)

left of the staircase

7.

What ion is most likely to form from an atom in the alkali metal family?

a)

+1

b)

+2

c)

+3

d)

-1

8.

What family does fluorine belong to?

a)

alkali metals

b)

halogens

c)

noble gases

d)

alkali earth metals

9.

Elements that behave most similarly are placed in _________.

a)

groups/families

b)

period/series

10.

What are the electron configurations for Calcium?

a)

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

b)

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

c)

[Ar] 4s2

d)

[K] 4s1

11.
What is the noble gas notation for Chlorine?
a)
[Ar] 3s2 3p5
b)
[Ne] 3s2 3p5
c)
[Ne] 3s2 3p6
12.
How many valence electrons does Magnesium have?
a)
2
b)
4
c)
6
d)
7
13.

How many valence electrons does Helium have?

a)

2

b)

4

c)

6

d)

8

14.
This is a Lewis Dot Structure for which element?
a)
Calcium
b)
Fluorine
c)
Neon
d)
Carbon
15.
Lewis Dot Structures only have to do with what?
a)
protons
b)
neutrons
c)
electrons
d)
valence electrons
16.

If an element has a charge of +2, does that mean it has gained or lost 2 electrons?

a)

gained

b)

lost

17.

The electron configuration of an element is 1s2 2s2 2p4. How many more electrons does the element need to gain to be "like" a Noble Gas?

a)

2

b)

3

c)

1

d)

8

18.

Challenge Problem!

Which of the following could have the electron configuration 1s22s22p63s23p6

1.Cl-

2. K+

3. Al3+

a)

1 only

b)

2 only

c)

1 and 2

d)

1, 2, and 3

19.

The electron configuration 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.

20.
Which element has a noble gas configuration of [Ne] 3s2 3p3?
a)
Magnesium
b)
Phosphorus
c)
Aluminum
d)
Sulfur
21.
What is the electron configuration for nitrogen? 
a)
1s2 2s3 2p2
b)
1s2 2s2 2p3
c)
1s2 2s2 2p2 3s1
d)
1s2 2s3 2p1
22.
Which element has a noble gas (core) configuration of [Xe] 6s2?
a)
Tungsten
b)
Mercury
c)
Cesium
d)
Barium
23.
The orbitals shown correspond to which elements?
a)
Nitrogen, Argon, Sodium
b)
Phosphorus, Neon, Sodium
c)
Nitrogen, Neon, Sodium
d)
Phosphorus, Argon, Sodium
24.

For an atom to be electrically neutral, it must contain the same number of _____

a)

protons and neutrons

b)

neutrons and electrons

c)

protons and electrons

d)

nucleons and electrons

25.

A horizontal row of elements (repeating pattern of properties) in the periodic table is a ________.

a)

column

b)

group

c)

period

d)

family

26.

an element will always have the same number of

a)

neutrons

b)

protons

c)

electrons

d)

atoms

27.

What sub-atomic particle is this?

In the Nucleus

No Charge

Mass of 1 amu

a)

proton

b)

electron

c)

neutron

d)

nucleus

28.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
29.

How many electrons does Si contain?

a)

14

b)

28

c)

2

d)

4

30.
What is this element?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
31.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
32.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
33.

What do you start every electron configuration with?

a)

1s2

b)

1d10

c)

1f14

d)

1p6

34.

In 1s2, the 1 means

a)

there is 1 electron

b)

the electrons are in the 1st energy level

c)

the shape is circular

d)

there is a -1 charge

35.

In 1s2, the s means

a)

the shape of the orbital is circular

b)

the shape of the orbital is figure 8

c)

there are six electrons

d)

it is neutral

36.

Which element is not a metal?

a)

Bi

b)

Re

c)

Al

d)

B

37.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
38.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
39.
Calcium is most like which of the following?
a)
Barium
b)
Potassium
c)
Cesium
d)
Nitrogen
40.
The alkali metals have how many valence electrons?
a)
1
b)
2
c)
7
d)
8
41.

The noble gases have how many valence electrons? (except He)

a)

1

b)

2

c)

7

d)

8

42.
Membership in a family is based on the number of 
a)
electrons
b)
valence electrons
c)
protons
d)
neutrons
43.

What does the 1.00794 stand for?

a)

Hydrogen

b)

atomic number

c)

atomic mass

d)

mass #

44.
The blue atoms are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
45.

Which element is not a Alkali metal?

a)

Li

b)

H

c)

Fr

d)

Cs

46.

Beryllium is in family number______.

a)

2

b)

3

c)

4

d)

7

47.

The period for Bromine is ___________.

a)

3

b)

2

c)

4

d)

5

48.

How many Valance electrons does Sulfur have?

a)

6

b)

3

c)

7

d)

17

49.
Most elements on the periodic table are this type.
a)
Gases
b)
Nonmetals
c)
Metals
d)
Metalloids
50.
Which elements have the most similar chemical properties?
a)
K and Na
b)
K and Ca
c)
K and Cl
d)
K and S
51.

What do elements in the same period have in common?

a)

energy levels

b)

valence electrons

c)

protons

d)

neutrons

52.

Which rule is being broken this orbital diagram?

a)

Aufbau Principle

b)

Pauli Exclusion Principle

c)

Hund's Rule

d)

The diagram is correct.

53.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
54.
How many electrons can the s sublevel hold?
a)
14
b)
10
c)
2
d)
6
55.

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

d)

Heisenberg Principle

56.

Each orbital can hold ____ electrons

a)

5

b)

4

c)

8

d)

2

57.

Which rule is being broken with this orbital diagram?

a)

Aufbau Principle

b)

Pauli Exclusion Principle

c)

Hund's Rule

d)

The diagram is correct.

58.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
59.
How many electrons can the p sublevel hold?
a)
14
b)
10
c)
2
d)
6
60.

What is the shape of the s orbital?

a)

dumbbell

b)

spherical

c)

flower

d)

flat

61.

What quantum number describes the energy level and size of an orbital?

a)

l

b)

m

c)

s

d)

n

62.

What quantum number describes the spin of the electron?

a)

s

b)

l

c)

m

d)

n

63.

Name the element. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1

a)

Gallium

b)

Indium

c)

Aluminum

d)

Germanium

64.

How many orbitals are in a "p" sublevel?

a)

1

b)

3

c)

5

d)

7

65.

Which quantum number describes the shape of the orbital?

a)

n

b)

l

c)

m

d)

s

66.

According to the Aufbau Principle, which sublevel should starting filling with electrons before the 3s sublevel?

a)

2p

b)

3p

c)

4s

d)

4p

67.
For a principle quantum number, "n", equal to 2, what is the total electron capacity of that level?  
a)
2
b)
4
c)
8
d)
16
68.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
69.
How many electrons should Beryllium have around its Lewis dot model?
a)
1
b)
2
c)
3
d)
4
70.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
71.
 The diagram above represents two electrons with 
a)
a. opposite spins.
b)
 b. the same spin.
c)
c. different energies.
d)
d. different energy levels.
72.
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
73.
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
74.

What element's orbital notation is pictured here?

a)

Ar

b)

Br

c)

Cu

d)

Cl

75.

This shape is that of a/n:

a)

s orbital

b)

p orbital

c)

d orbital

d)

f orbital

76.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
77.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

78.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
79.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
80.
How many electron can be found in a p orbital?
a)
2
b)
3
c)
4
d)
6

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