Electron Configuration and the Periodic Table

What is the primary goal of learning electron configuration?

• To read and write electron configurations and understand their organization on the periodic table

• To learn about chemical reactions

• To understand atomic mass

• To memorize the periodic table

In electron configuration, what do the superscript numbers represent?

• The atomic mass

• The number of protons

• The number of neutrons

• The number of electrons in the preceding atomic orbital

What is the electron configuration for boron?

• 1s2 2s2 2p1

• 1s2 2s1

• 1s2 2s2 2p2

• 1s2 2p3

How many electrons does silicon have in its 3p subshell?

• 1

• 3

• 2

• 4

What does the row number or period number in the periodic table indicate?

• The number of protons

• The principal quantum number of the outermost atomic orbital

• The number of neutrons

• The atomic mass

Which section of the periodic table is associated with the highest energy level being an s subshell?

• s block

• p block

• f block

• d block

What is the last part of the electron configuration for iodine?

• 5p5

• 4d10

• 6s2

• 5s2

What is the ground state of an atom?

• A state with no electrons

• A state where electrons are missing

• The most stable electron configuration with electrons in the lowest possible energy levels

• The state with the highest energy

What happens when an electron moves to a higher energy level?

• It loses energy and falls to a lower state

• It absorbs energy and enters an excited state

• It emits a photon

• It becomes a proton

What is an excited state of an atom?

• A stable state with all electrons in the lowest energy levels

• A state where one or more electrons have absorbed energy and moved to higher energy levels

• A state with no electrons

• A state with more protons than electrons