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Periodic Trends

Total questions: 50

Worksheet time: 1hrs 6mins

Name
Class
Date
1.

What element has the highest electronegativity?

a)

Neon

b)

Fluorine

c)

Argon

d)

Sulfur

2.

Atomic Size

a)

increases across and decreases down

b)

Decreases across and increases down

c)

Decreases down and increases across

d)

increases down and constant across

3.

1 Ionization Energy

a)

Increases on top right but decreases on bottom left

b)

Increases on top left but decreases on bottom left

c)

Increases on top right but decreases and on bottom right

d)

Increases on top left but decreases and on bottom fight

4.

When atoms lose electrons they become.......

a)

Negatively charged

b)

positively charged

5.

Nuclear Charge

a)

Increases across and decreases down

b)

decreases across and increases down

c)

Increases across and increases down

6.

When atoms gain electrons they are becoming.....

a)

Negatively charged

b)

positively charged

7.

Electronegativity

a)

Increases on top right but decreases on bottom right

b)

Increases on top left but decreases on bottom left

c)

Increases on top right but decreases on bottom left

d)

Increases on top left but decreases on bottom right

8.

Element with the highest atomic Size/Radius

a)

Cesium

b)

Boron

c)

Francium

d)

Magnesium

9.

Which elements are usually not assigned electronegativity values?

a)

Noble gases

b)

Halogens

c)

Alkaline Earth Elements

d)

Representative elements

10.

what are Anions

a)

Positively charged

b)

Negatively charged

11.

What are Cations

a)

Positively charged

b)

negatively charged

12.

What element has the highest ionization energy

a)

Helium

b)

Hydrogen

c)

Fluorine

d)

Lithium

13.

How do you find the valance electron

a)

Add the last S and P orbitals together

b)

subtract the last S and P orbitals

c)

Add the last S, D and P orbital together

d)

Subtract the last D orbital from S+P

14.

what is the most valance electrons and element can have ?

a)

3

b)

6

c)

5

d)

8

15.

The ability to attract an electron in a chemical bond

a)

electronegativity

b)

electron affinity

c)

metallic character

d)

ionization energy

16.

The energy it takes to remove an electron from an atom in the gas phase

a)

electron affinity

b)

electronegativity

c)

metallic character

d)

ionization energy

17.

Ionization energy increases

a)

from L to R and from bottom to top

b)

from L to R and from top to bottom

c)

from R to L and from bottom to top

d)

from R to L and from top to bottom

18.

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

a)

increasing number of valence electrons

b)

increasing shielding

c)

increasing effective nuclear charge

d)

increasing number of protons in the nucleus

19.
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)
20.
As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....
a)
decreases
b)
increases
c)
remains the same
d)
none of the above
21.
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 nuetrons
22.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
23.

The element with the highest electronegativity is -

a)

At

b)

F

c)

Cl

d)

Br

24.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
25.

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

26.

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

a)

F has more valence e- 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

27.

Which atom has the largest atomic radius in Period 4 (row 4)?

a)

K

b)

Kr

c)

Fe

d)

Fe

28.

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 one valence electron is very far from the nucleus, so little energy is needed to remove it

29.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
30.

All groups/families have similar 

a)

Names

b)

Atomic numbers

c)

Atomic masses

d)

Properties

31.

The atom with the largest atomic radius in Period 4 (row 4) is -

a)

K

b)

Kr

c)

Fe

32.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
33.

Arrange the following in order of increasing ionization energy: Strontium, Aluminum, Indium.

a)

Strontium, Indium, Aluminum

b)

Strontium, Aluminum, Indium

c)

Indium, Aluminum, Strontium

d)

Aluminum, Indium, Strontium

34.

Which element has greater ionization energy?

a)

Magnesium

b)

Phosphorus

35.

Arrange these in increasing order of atomic radii: F, N, B

a)

B < N < F

b)

B < F < N

c)

N < F < B

d)

F < N < B

36.

Which of the following elements has the smallest atomic radius: Li, O, C, or F?

a)

Li

b)

O

c)

C

d)

F

37.

Which of the elements Ca, Be, Ba, and Sr has the largest atomic radius?

a)

Be

b)

Ba

c)

Ca

d)

Sr

38.

Which of these has a greater need for electrons?

a)

chlorine (Cl)

b)

Francium (Fr)

39.
Which has the greater EN: 
Cl or Al?
a)
Cl
b)
Al
40.
Which has the greater EN: 
N or C?
a)
C
b)
N
41.
Which has the greater EN: 
H or F?
a)
H
b)
F
42.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
43.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
44.
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)
45.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
46.
Atoms that have a high electronegativity, _______________.
a)
give up their electrons more easily.
b)
hold on to their electrons more tightly.
c)
have more electron shells.
47.
Which statement correctly and completely identifies a trend?
a)
Atomic radius decreases across a period and increases down a group.
b)
Electronegativity decreases across a period and decreases down a group.
c)
Ionization energy increases across a period and increases down a group.
d)
Ionic radius increases across a period and increases down a group.
48.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
49.

The element with the lowest electronegativity in Period 3 is -

a)

Na

b)

Cl

c)

Ar

d)

Mg

50.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals

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