8.2.2 Ionization Energy

Question 1

Ionization Energy

Answer 1

• Ionization energy (IE) is the energy necessary to remove an electron from an atom, molecule or ion.
• Moving down a group, ionization energy decreases because of increased electron shielding.
• Moving across a row from left to right ionization energy increases because of increased effective nuclear charge.

Question 2

note

Answer 2

• Ionization energy (IE) is the energy necessary to remove an electron from an atom, molecule or ion. IE is usually used to mean the first IE: the energy required for the removal of a single electron from a neutral atom or molecule. The second IE is the removal of an electron from a monovalent anion.
• An electron is removed by a photon with a known energy (E = h ), and the kinetic energy (KE) is measured for the released electron.
• Moving down a group, IE decreases because of increased electron shielding. Moving across a row from left to right, IE increases because of increased effective nuclear charge.
• There are exceptions to the general trends.
• Electrons in higher energy orbitals are easier to remove than electrons in lower energy orbitals.
• It is easier to remove an electron from a 2p orbital than it is to remove one from a 2s orbital.
• It is easier to remove an electron if it is paired than if it is unpaired.

Question 3

What is the total number of electrons that can be held in the 2p orbitals?

Answer 3

6

Question 4

Which of the following is not a periodic trend?

Answer 4

Oxidation state

Question 5

In which of the following lists are the elements arranged in order of increasing ionization energies?

Answer 5

Fe, Co, Ni, Cu

Question 6

Which of the follow explains why there is a difference in first ionization energy between nitrogen and oxygen?

Answer 6

Nitrogen has a more stable electron configuration

Question 7

Which of the following is used to describe the ionization energy for hydrogen?

Answer 7

Schrödinger equation

Question 8

Which of the following transitions of electrons between orbitals results in the emission of energy?

Answer 8

3p to 3s

Question 9

Why does the second ionization energy roughly follow the same trend as the first ionization energy but is offset by one element?

Answer 9

The electron configuration is identical to the next lower element when the first electron is removed.

Question 10

What happens to the successive ionization energies as more and more electrons are removed?

Answer 10

The ionization energies continue to increase a relatively steady amount with each electron removed.

Question 11

What happens to the ionization energy as the size of the nucleus increases?

Answer 11

It increases.

Question 12

How does the magnitude of the second ionization energy compare to the first ionization energy for an atom?

Answer 12

After the first electron is removed, the influence exerted by the nucleus increases which increases the second ionization energy