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WorksheetsIONIZATION ENERGY
Total questions: 20
Worksheet time: 21mins
Ionization energy is the _____ energy required to _______ one mole of electron from one mole of gaseous atom at ground state.
maximum, remove
minimum, remove
maximum, add
minimum, add
1. The ______the atomic radius, the ________the attraction, the _______the ionisation energy.
smaller, stonger, higher
bigger, weaker, higher
Across a period, Ionization energy ____a____
Down a group, ionisation energy ____b_____
a : increase
b: decrease
a : increase
b: increase
a : decrease
b: decrease
Which element has the greatest ionization energy: Aluminum (Al) or Chlorine (Cl)?
Aluminum (Al)
Chlorine (Cl)
Which of the following factors will affect ionization energy:
Atomic radius
Effective nuclear charge
Shielding effect
All of the above
Select all that explain the ionization energy trend within periods
electrons are closer to the nucleus
their is a weak pull between electrons from the nucleus, making them easily moveable
feel more of a pull from nucleus, making them harder to move
electrons are further from the nucleus
Ionization energy (a) as you go down a group.
As you look from left to right across a period, ionization energy and electronegativity both
increase
decrease
Which has the greater electronegativity:
N or C?
C
N
What is the amount of energy required to remove an electron from an atom?
atomic energy
ionization energy
ionic energy
electron energy
Explain why ionization energy decreases as you go down a group.
Outer electrons are further away from the nucleus you go down a group
Electrons feel less pull from the nucleus as you go down a group
Electrons are easier to remove as you go down a group
All of the above
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?
The ionization energy drops significantly as you move down a group because the valence electrons are in a shell further from the nucleus.
The ionization energy increases gradually as you move right across a period because the valence electrons are in a shell further from the nucleus.
The ionization energy increases gradually as you move right across a period because you are adding more protons.
The ionization energy increases when the valence electrons are more attracted to the nucleus.
