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Periodic Trends and Electrons Review

Total questions: 40

Worksheet time: 2hrs 0mins

Name
Class
Date
1.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Nitrogen (N)
b)
Lithium (Li)
c)
Antimony (Sb)
d)
Germanium (Ge)
2.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
3.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
4.

Ionization energy is...

a)

the energy required to add an electron to a specific atom.

b)

how much energy it takes to remove an electron from an atom.

c)

the energy required to shield the outer electrons from the nucleus.

d)

a measure of the ability of an atom to attract electrons.

5.
The vertical columns of the periodic table are called -
a)
groups.
b)
rows.
c)
periods.
d)
transition.
6.

Atomic radius decreases from left to right across a period because from left to right there is an...

a)

increasing number of valence electrons.

b)

increasing shielding.

c)

increasing effective nuclear charge.

d)

increasing number of protons in the nucleus.

7.

As you move down the periodic table atoms get bigger. This is because ____________.

a)

the atoms have more mass.

b)

the atoms have more protons.

c)

the atoms have more energy levels.

d)

the atoms have more neutrons.

8.

The ionization energy of Na is larger than Cs because...

a)

Na has a greater effective nuclear charge.

b)

Na has fewer energy levels and less shielding.

c)

Cs has a greater effective nuclear charge than Na.

d)

Cs has more valence electrons than Na.

9.

Fluorine has a smaller atomic radius than B because...

a)

F has more valence electrons than B.

b)

F has more shielding than B.

c)

F has a larger atomic number than B.

d)

F has a greater effective nuclear charge than B.

10.
An anion is a negatively charged ion.
a)
True
b)
False
11.

A cation is a positively charged ion.

a)

True

b)

False

12.
Which properties are characteristic of the group 1 metals?
a)
high reactivity and the formation of stable compounds
b)
high reactivity and the formation of unstable compounds
c)
low reactivity and the formation of stable compounds
d)
low reactivity and the formation of unstable compounds
13.

Electronegativity is...

a)

how good an atom is at attracting electrons.

b)

the ability of an atom to lose electrons.

c)

the energy required to remove an electron from a specific atom.

d)

how good an atom is at attracting protons.

14.

What is the name of the group of elements that are the least reactive because of their full outermost ring?

a)

noble gases

b)

transition metals

c)

halogens

d)

alkaline earth metals

15.

Elements on the far right side of the periodic table are classified as nonmetals.

a)

True

b)

False

16.

Elements on the far left side of the periodic table are classified as metals.

a)

True

b)

False

17.
Which compound contains an alkaline earth metal and a halogen? 
a)
CaS
b)
Rb2S
c)
RbCl
d)
CaCl2
18.
a)
Periods
b)
Groups
19.
a)
Periods
b)
Groups
20.
a)
energy levels
b)
valence electrons
c)
protons
d)
neutrons
21.
a)
energy levels
b)
valence electrons
c)
protons
d)
neutrons
22.
a)
Same group
b)
Same period
23.

a)

Alkaline Earth Metals

b)

Halogens

c)

Nonmetals

d)

Noble gases

24.
a)
Metals
b)
Nonmetals
c)
Metalloids
25.
a)
2
b)
8
c)
3
d)
13
26.

Valence electrons are the...

a)

innermost electrons.

b)

middle electrons.

c)

outermost electrons.

d)

any electrons.

27.

USE THE PERIODIC TABLE

How many valence electrons does sodium have?

a)

1

b)

2

c)

3

d)

4

28.

USE THE PERIODIC TABLE

How many valence electrons does phosphorus have?

a)

31

b)

5

c)

15

d)

4

29.

How many electrons can a p-orbital hold?

a)

6

b)

3

c)

2

d)

4

30.

How many orbitals are there in the d-sublevel?

a)

1

b)

3

c)

5

d)

7

31.

Which sublevel is associated with having more energy?

a)

2p

b)

2s

c)

3p

d)

1s

32.
How many total electrons can the f orbitals in a sublevel hold?
a)
2
b)
14
c)
6
d)
10
33.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
34.
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
35.
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
36.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
37.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
38.

How many orbitals are there in the p-sublevel?

a)

2

b)

1

c)

4

d)

3

39.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
40.

According to the Octet Rule, atoms of elements react with each other in order to attain ____ electrons in their outermost energy level or shell.

a)

2

b)

4

c)

6

d)

8

e)

10

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