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Ionisation Energy

Total questions: 23

Worksheet time: 23mins

Name
Class
Date
1.
What is ionization energy?
a)
Energy needed to destroy an atom
b)
Energy required to remove an electron
c)
Energy needed to split an electron
d)
Energy required to add an electron
2.

As you look down a group, ionization energy and electronegativity

a)

increases

b)

decreases

3.

Which of the following is true for alkaline earth metals as their atomic number increases?

a)

The atomic radius decreases.

b)

Ionization energy decreases.

c)

The number of valence electrons increases.

d)

Their electronegativity increases.

4.
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
5.
The bar graph above represents four elements and their respective ionization energies. Based on the organization of the modern periodic table, how would these elements be found on the periodic table?
a)
They are in the same period with W being furthest left.
b)
They are in the same period with W being furthest right.
c)
They are in the same group with W being furthest to the bottom.
d)
They are in a diagonal line with W being at the bottom right.
6.
Which of the following is true about a sulfur atom and a chlorine atom?
a)
Sulfur is larger and has higher ionization energy.
b)
Sulfur is larger and has lower ionization energy.
c)
Sulfur is smaller and has higher ionization energy.
d)
Sulfur is smaller and has lower ionization energy.
7.

Which element has the greater ionization energy?

a)

Magnesium (Mg)

b)

Phosphorus (P)

8.
 Which of the following generally applies to the noble gases? 
a)
high ionization energy, low electronegativity, high reactivity
b)
high ionization energy, high electronegativity, high reactivity
c)
low ionization energy, low electronegativity, low reactivity
d)
high ionization energy, low electronegativity, low reactivity 
9.

Which element has the greater ionization energy?

a)

Iodine (I)

b)

Chlorine (Cl)

10.
Which of these elements has the highest ionization energy?
a)
Lithium (Li)
b)
Potassium (K)
c)
Francium (Fr)
d)
Sodium (Na)
11.
Which of these elements has the lowest ionization energy?
a)
Oxygen (O)
b)
Boron (B)
c)
Carbon (C)
d)
Fluorine (F)
12.
 After the atom is ionised, it then requires more energy to remove a second electron because the second electronis nearer the nucleus.
a)
False
b)
True
c)
Not sure
13.
The atom will spontaneously lose an electron to become stable.
a)
True
b)
False
c)
Not sure
14.
Only one electron can be removed from the atom, as it then has a stable electronic configuration.
a)
True
b)
False
c)
Not sure
15.

The graph above shows the ionization energy values as the elements are arranged on the periodic table. Which conclusion cannot be drawn from the graph?

a)

The ionization energy drops significantly as you move down a group because the valence electrons are in a shell further from the nucleus.

b)

The ionization energy increases gradually as you move right across a period because the valence electrons are in a shell further from the nucleus.

c)

The ionization energy increases gradually as you move right across a period because you are adding more protons.

d)

The ionization energy increases when the valence electrons are more attracted to the nucleus.

16.
The nucleus is not attracted to the electrons.
a)
True
b)
False
c)
Not sure
17.

For which of the following elements would you expect a large jump between IE1 and IE2?

a)

Na

b)

Fe

c)

Ca

d)

F

18.

Which equation correctly describes the first ionization energy of X?

a)

X --> X- + e-

b)

X --> X+ + e-

c)

X --> X- + e+

d)

X + e- --> X-

e)

X + e- --> X+

19.

Which of the following would have the smallest ionization energy?

a)

K

b)

P

c)

S

d)

Ca

e)

Mg

20.

Place the following elements in order of increasing ionization energy: Na, O, Mg, Ne, K

a)

Ne, O, Mg, Na, K

b)

Mg, Na, O, K, Ne

c)

K, Mg, Na, O, Ne

d)

K, Na, Mg, O, Ne

21.

Successive ionization energies for an element in Period 4 were determined experimentally and found to be: IE1=600 kJ/mol, IE2=1800 kJ/mol, IE3=2700 kJ/mol, IE4=11,600 kJ/mol and IE5=15,000 kJ/mol. What element is this?

a)

germanium

b)

selenium

c)

gallium

d)

silicon

e)

phosphorous

22.

Using electron configuration and your knowledge of ionization energy, which would you expect to have a higher second ionization energy: Na or Mg?

a)

Na

b)

Mg

c)

Both would be expected to have the same second ionization energy

d)

Cannot be determined

23.

Which of the following elements has the lowest ionization energy?

a)

cesium

b)

sodium

c)

lithium

d)

rubidium

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