Ionization Energy and Electron Configurations

The video tutorial covers the concept of ionization energy, focusing on its definition, trends, and discontinuities in the periodic table. It explains sodium's electron configuration and how ionization energy varies across different groups and periods. The tutorial highlights the unexpected trends in ionization energy due to sublevels and electron repulsions, providing examples with elements like beryllium and boron.

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 electron configuration represents sodium?

• 1s2 2s2 2p6 3s2

• 1s2 2s2 2p6 3p1

• 1s2 2s2 2p5 3s2

• 1s2 2s2 2p6 3s1

Why does the first ionization energy increase across a period?

• Because the atomic radius decreases

• Because the number of protons increases

• Because the number of protons decreases

• Because the atomic radius increases

What causes the discontinuity in ionization energy between groups 2 and 13?

• The presence of s sublevels

• The presence of p sublevels

• The presence of d sublevels

• The presence of f sublevels

Which group has a valence electron configuration of ns2 np3?

• Group 13

• Group 14

• Group 15

• Group 16

Why is it easier to remove an electron from a group 16 element compared to a group 15 element?

• Because group 16 elements have unpaired electrons

• Because group 16 elements have more protons

• Because group 16 elements have fewer protons

• Because group 16 elements have paired electrons causing repulsion

What is the electron configuration of boron?

• 1s2 2s2 2p3

• 1s2 2s2 2p2

• 1s2 2s2 2p4

• 1s2 2s2 2p1

Why does boron have a lower first ionization energy than beryllium?

• Because boron's electron is in a higher energy p sublevel

• Because boron has more protons

• Because beryllium's electron is in a higher energy p sublevel

• Because beryllium has more electrons

What is the main factor affecting ionization energy trends across a period?

• Number of neutrons

• Atomic mass

• Number of isotopes

• Nuclear charge

Which of the following best explains the trend in ionization energy between groups 15 and 16?

• Group 16 elements have fewer protons

• Group 15 elements have more protons

• Group 16 elements have paired electrons causing repulsion

• Group 15 elements have paired electrons causing repulsion