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Unit 3 Review

Total questions: 44

Worksheet time: 52mins

Name
Class
Date
1.
a)
Periods
b)
Groups
2.
a)
Periods
b)
Groups
3.
a)
Same group
b)
Same period
4.
How did Mendeleev arrange the elements?
a)
alphabetical 
b)
density
c)
melting point
d)
atomic mass
5.
The horizontal row on the periodic table is called a
a)
group
b)
family
c)
period
d)
atomic number
6.
A vertical column is called...
a)
group
b)
tower
c)
period
d)
crew
7.
The blue atoms are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
8.
The atomic number tells you what?
a)
number of electrons
b)
number of protons
c)
number of neutrons
d)
both electrons and protons in an atom.
9.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
10.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
11.

What are the three main groups of the periodic table?

a)

groups

b)

metal

c)

nonmetals

d)

metalloids

e)

periods

12.

What does the number of proton tell us?

a)

electrons

b)

atomic number

c)

atomic mass

d)

neutrons

13.

How do you calculate the number of neutrons? *

a)

Mass = Atomic number - Neutrons

b)

Mass - Atomic number = Neutrons

c)

Atomic number = Neutrons

14.

What is the name of the element? (Periodic table will be needed)

a)

sodium

b)

magnesium

c)

vanadium

15.

What group and period does this element belong in? *

a)

period 1 and group 3

b)

period 3 and group 1

c)

period 2 and group 3

d)

period 3 and group 2

16.

How many valence electrons does the element have?

a)

1

b)

2

c)

3

d)

4

17.

How many protons and electrons does nickel have?

a)

28

b)

58.69

18.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
19.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
20.
The atom with the largest atomic radius in Period 4 (row 4) is - 
a)
K
b)
Kr
c)
Fe
d)
Fe
21.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
22.

Who invented the Periodic Table?

a)

Mendeleev

b)

Bohr

c)

Lewis

d)

Democritus

23.
Atoms with similar properties are most likely located...
a)
in the same period.
b)
in the same group.
c)
in different periods.
d)
to the right and left of each other.
24.

The distance between nucleus and outermost shell occupied electron

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

25.

The tendency of an atom to attract a shared pair of electrons

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

26.

Which element has bigger atomic radii?

a)

Beryllium is bigger than Fluorine

b)

Oxygen is bigger than Sulphur

c)

Litihium is bigger than Sodium

d)

Phosphorus is bigger than Bromine

27.
Beryllium is in group number______.
a)
Group 2
b)
Group 3
c)
Group 4
d)
Group 7
28.
Which elements have the most similar chemical properties?
a)
K and Na
b)
K and Ca
c)
K and Cl
d)
K and S
29.

If an element has 117 protons which group will it be in on the periodic table?

a)

1

b)

7

c)

11

d)

17

30.

Which element is most likely to have six electrons in its 4th energy level?

a)

Oxygen (O)

b)

Selenium (Se)

c)

Krypton (Kr)

d)

Potassium (K)

31.

Which color on the image of the periodic table corresponds with the actinides.

a)

red

b)

black

c)

blue

d)

yellow on bottom

32.
Which properties are characteristic of the Group 1 metals?
a)
high reactivity and the formation of unstable compounds
b)
low reactivity and the formation of unstable compounds
c)
high reactivity and the formation of stable compounds
d)
low reactivity and the formation of stable compounds
33.

The elements in this family are soft, silvery, and very reactive with water.

a)

Alkaline Earth Metals

b)

Alkali Metals

c)

Transition Metals

d)

Lanthanides

34.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
35.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
36.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
37.

What do you start all electron configurations with?

a)

1s2

b)

1d10

c)

1f14

d)

1p6

38.
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
39.

The 4 orbitals are

a)

s, p, d, f

b)

a, b, c, d

c)

2, 4, 6, 8

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

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