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Worksheets

ملك محمد محروس

Total questions: 52

Worksheet time: 42mins

Name
Class
Date
1.
Which of the following elements has the smallest radius?
a)
Mg
b)
Al
c)
Si
d)
K
2.

Which element in Period 2 has the greatest atomic radius?

a)

Be

b)

C

c)

Na

d)

Li

3.

Of the halogens (group 7A), which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

4.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)
the number of protons increases, so attraction to electrons increases
b)
the number of energy levels increases
c)
the number of electrons increases
d)
the atomic mass increases
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.

Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.

a)

decreases, increases

b)

increases, increases

c)

increases, decreases

d)

stays the same, increases

7.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

8.

The atom with the largest atomic radius in Group 8A is -

a)

Ar

b)

He

c)

Kr

d)

Rn

9.
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
10.
Which has the greater EN: 
H or F?
a)
H
b)
F
11.
Which has the greater EN: 
N or C?
a)
C
b)
N
12.

How many valence electrons does Carbon have?

a)

4

b)

5

c)

6

d)

8

13.
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.
14.
Which of the following sequences corresponds to a correct trend in ionization energy?
a)
Cl > S > P > Al
b)
Sr > Ca > Mg > Be
c)
Rb > K > Na > Li
d)
Rb > Sr > I > Xe
15.

The ability of an atom to attract electrons in a bond is called

a)

Ionization energy

b)

electronegativity

c)

atomic radius

d)

proton affinity

16.
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
17.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
18.

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)

19.

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

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

20.

As you move left to right across a period, ionization energy

a)

increases

b)

decreases

c)

says the same

21.

What group is highlighted here on the periodic table (Group 1A)?

a)

Noble Gases

b)

Halogens

c)

Alkali Metals

d)

Alkaline Earth Metals

22.

What group is highlighted here on the periodic table (Group 8A)?

a)

Noble Gases

b)

Halogens

c)

Alkali Metals

d)

Alkaline Earth Metals

23.

What group is highlighted here on the periodic table (Group 2A)?

a)

Noble Gases

b)

Halogens

c)

Alkali Metals

d)

Alkaline Earth Metals

24.

What group is highlighted here on the periodic table (Group 7A)?

a)

Noble Gases

b)

Halogens

c)

Alkali Metals

d)

Alkaline Earth Metals

25.

What group is highlighted here on the periodic table (D-block elements)?

a)

Non-metals

b)

Metalloids

c)

Rare Earth Metals

d)

Transition Metals

26.
Which of the following elements has the smallest radius?
a)
Mg
b)
Al
c)
Si
d)
K
27.

Which element in Period 2 has the greatest atomic radius?

a)

Be

b)

C

c)

Na

d)

Li

28.

Of the halogens (group 7A), which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

29.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)
the number of protons increases, so attraction to electrons increases
b)
the number of energy levels increases
c)
the number of electrons increases
d)
the atomic mass increases
30.
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
31.

Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.

a)

decreases, increases

b)

increases, increases

c)

increases, decreases

d)

stays the same, increases

32.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

33.

The atom with the largest atomic radius in Group 8A is -

a)

Ar

b)

He

c)

Kr

d)

Rn

34.
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
35.
Which has the greater EN: 
H or F?
a)
H
b)
F
36.
Which has the greater EN: 
N or C?
a)
C
b)
N
37.

How many valence electrons does Carbon have?

a)

4

b)

5

c)

6

d)

8

38.
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.
39.
Which of the following sequences corresponds to a correct trend in ionization energy?
a)
Cl > S > P > Al
b)
Sr > Ca > Mg > Be
c)
Rb > K > Na > Li
d)
Rb > Sr > I > Xe
40.

The ability of an atom to attract electrons in a bond is called

a)

Ionization energy

b)

electronegativity

c)

atomic radius

d)

proton affinity

41.
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
42.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
43.

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)

44.

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

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

45.

As you move left to right across a period, ionization energy

a)

increases

b)

decreases

c)

says the same

46.

What group is highlighted here on the periodic table (Group 1A)?

a)

Noble Gases

b)

Halogens

c)

Alkali Metals

d)

Alkaline Earth Metals

47.

What group is highlighted here on the periodic table (Group 8A)?

a)

Noble Gases

b)

Halogens

c)

Alkali Metals

d)

Alkaline Earth Metals

48.

What group is highlighted here on the periodic table (Group 2A)?

a)

Noble Gases

b)

Halogens

c)

Alkali Metals

d)

Alkaline Earth Metals

49.

What group is highlighted here on the periodic table (Group 7A)?

a)

Noble Gases

b)

Halogens

c)

Alkali Metals

d)

Alkaline Earth Metals

50.

What group is highlighted here on the periodic table (D-block elements)?

a)

Non-metals

b)

Metalloids

c)

Rare Earth Metals

d)

Transition Metals

51.

Which element in Period 2 has the greatest atomic radius?

a)

Be

b)

C

c)

Na

d)

Li

52.

Which element in Period 2 has the greatest atomic radius?

a)

Be

b)

C

c)

Na

d)

Li

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