Ionization Energy/Periodic Table Practice

Which equation correctly describes the first ionization energy of X?

• X --> X^- + e^-

• X --> X⁺ + e^-

• X --> X^- + e⁺

• X + e^- --> X^-

• X + e^- --> X⁺

Tags

NGSS.HS-PS1-2

NGSS.HS-PS1-3

Which of the following would have the largest ionization energy?

• Na

• Al

• Mn

• N

• Pd

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Which of the following would have the smallest ionization energy?

• K

• P

• S

• Ca

• Mg

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

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

• Ne, O, Mg, Na, K

• Mg, Na, O, K, Ne

• K, Mg, Na, O, Ne

• K, Na, Mg, O, Ne

Tags

NGSS.HS-PS1-1

Place the following elements in order of decreasing ionization energy: N, Si, P, Mg, He

• He, N, P, Si, Mg

• Mg, Si, P, N, He

• N, He, Si, P, Mg

• Si, P, N, Mg, He

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

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?

• germanium

• selenium

• gallium

• silicon

• phosphorous

Tags

NGSS.HS-PS1-1

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

• Na

• Mg

• Both would be expected to have the same second ionization energy

• Cannot be determined

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Which statement best describes the relative first ionization energies of Ca and Mg?

• Calcium has a higher first ionization energy than magnesium because its radius is smaller.

• Magnesium has a higher first ionization energy than calcium because its radius is smaller.

• Calcium has a higher first ionization energy than magnesium because its highest occupied energy sub-level is full.

• Magnesium has a higher first ionization energy than calcium because its highest occupied energy sub-level is full.

• Calcium and magnesium will have the same first ionization energy because they have the same number of valence electrons.

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Which statement best describes the relative first ionization energies of Be and B?

• Beryllium has a higher first ionization energy than boron because its radius is smaller because it has fewer valence electrons than boron.

• Boron has a higher first ionization energy than beryllium because its radius is smaller and its valence electrons are closer to the nucleus.

• Beryllium has a higher first ionization energy than boron because its highest occupied energy level is full.

• Boron has a higher first ionization energy than beryllium because its highest occupied energy level is full.

• They will have the same first ionization energy because boron only has one extra valence electron.

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Ionization Energy increases going down a group because the number of protons is increasing.

• True

• False