Ionization Energy Quiz

What is ionization energy?

• The energy required to add an electron to an atom

• The energy required to remove an electron from an atom

• The energy released when an atom gains an electron

• The energy required to split an atom into ions

Which of the following best describes the second ionization energy?

• Energy needed to remove an electron from a neutral atom

• Energy needed to remove an electron after the first has been removed

• Energy needed to remove two electrons simultaneously

• Energy needed to add an electron to a cation

What trend is observed in first ionization energy as you move across a period from left to right?

• It fluctuates randomly

• It remains constant

• It decreases

• It increases

Why does first ionization energy generally decrease as you move down a group?

• Electrons are closer to the nucleus

• Electrons are further from the nucleus

• The number of protons decreases

• The atomic mass decreases

Which element has a higher first ionization energy: arsenic or fluorine?

• It cannot be determined

• Arsenic

• Fluorine

• Both have the same ionization energy

What is the effect of increasing effective nuclear charge on ionization energy?

• It increases ionization energy

• It has no effect on ionization energy

• It decreases ionization energy

• It causes ionization energy to fluctuate

What happens to the effective nuclear charge as you move from left to right across a period?

• It increases

• It fluctuates

• It remains the same

• It decreases

Why is the second ionization energy of lithium much higher than the first?

• The second electron is closer to the nucleus

• The first electron is more tightly bound

• The second electron is removed from a stable noble gas configuration

• The first electron is removed from a higher energy level

What is the electron configuration of a lithium ion after the first electron is removed?

• 1s1

• 2s2

• 1s2

• 2s1

Why is there a large gap between the second and third ionization energies of magnesium?

• The third electron is removed from a stable noble gas configuration

• The second electron is more tightly bound

• The first electron is removed from a higher energy level

• The third electron is closer to the nucleus