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Periodic Trends

Total questions: 28

Worksheet time: 45mins

Name
Class
Date
1.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
2.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)

Barium (Ba)

d)
Magnesium (Mg)
3.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
4.
Electronegativity is...
a)

the ability of an atom in a chemical bond to attracting bonded electrons

b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)

the ability of a neutral atom to attract electrons

5.
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
6.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
7.

Atomic radius generally increases as we move __________.  

a)
down a group and from right to left across a period 
b)
up a group and from left to right across a period 
c)
down a group and from left to right across a period 
d)
up a group and from right to left across a period 
8.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
9.

Put in order from biggest to smallest (decreasing size)

a)

Calcium

b)

Iron

c)

Zinc

d)

Bromine

e)

Krypton

1)
2)
3)
4)
5)
10.

Ions are formed when atoms gain or lose ___.

a)

electrons

b)

protons

c)

neutrons

d)

atomic mass

11.

Select the element with the highest ionization energy

a)

Sodium

b)

Aluminum

c)

Phosphorous

d)

Chlorine

12.

Select the element with the highest ionization energy

a)
Lithium
b)
Beryllium
c)
Helium
d)
Neon
13.

Put the following in order of increasing ionization energy:

a)

Lithium

b)

Boron

c)

Carbon

d)

Oxygen

e)

Neon

1)
2)
3)
4)
5)
14.

In group 2, which of these elements has the lowest electronegativity?

a)

Ba

b)

Mg

c)

Ca

d)

La

15.

The element with the lowest electronegativity in Period 3 is -

a)

Na

b)

Cl

c)

Ar

d)

Mg

16.

Order the elements S, Cl, and F in terms of increasing ionization energy.

a)

S, Cl, F

b)

Cl, F, S

c)

F, S, Cl

d)

F, Cl, S

e)

S, F, Cl

17.

All alkaline earth metals have the following number of valence electrons:

a)

1

b)

3

c)

6

d)

2

e)

none of these

18.

Order the elements S, Cl, and F in terms of increasing atomic radii.

a)

S, Cl, F

b)

Cl, F, S

c)

F, S, Cl

d)

F, Cl, S

e)

S, F, Cl

19.

Choose the element with the highest ionization energy.

a)

Na

b)

Mg

c)

Al

d)

P

e)

S

20.

List the following atoms in order of increasing ionization energy: Li, Na, C, O, F.

a)

Li<Na<C<O<F

b)

Na<Li<C<O<F

c)

F<O<C<Li<Na

d)

Na<Li<F<O<C

e)

Na<Li<C<F<O

21.

Rank the following atoms in order of decreasing electronegativity. Cl, Na, Si, P

a)
Si, Cl, Na, P
b)
Na, Cl, P, Si
c)
Cl, Si, Na, P
d)
Cl, P, Si, Na
e)
P, Na, Cl, Si
22.

Select the properties that go with metals.

a)

malleable

b)

brittle

c)

ductile

d)

dull

e)

shiny

23.

List the following elements in order of INCREASING atomic radius:

Cs, S, Co

a)

They are all about the same

b)

Co, Cs, S

c)

S, Co, Cs

d)

Cs, Co, S

24.

Of the halogens, which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

25.

As you move down a group on 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

26.
Which of the following will have a higher electronegativity than arsenic (As)?
a)

Gold (Au)

b)

Chlorine (Cl)

c)
Antimony (Sb)
d)
Germanium (Ge)
27.
Based on their locations in the periodic table, which element has chemical properties most similar to those of calcium, Ca?
a)
beryllium, Be
b)
potassium, K
c)
titanium, Ti
d)
yttrium, Y
28.

As you move down a group, shielding

a)

increases because there are more shells

b)

increases because there are more protons

c)

decreases because the atomic radius increases

d)

stays constant because the number of valence electrons stays the same

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