Electron Configurations of Germanium

This video tutorial explains how to write the electron configuration for germanium (Ge), which has an atomic number of 32. It covers two methods: using the diagonal rule and the periodic table blocks. The video provides a detailed step-by-step configuration for germanium, including the condensed notation using the noble gas argon. Additionally, it explains how to write the electron configurations for germanium ions Ge4+ and Ge2+ by removing valence electrons from the S and P blocks.

What is the atomic number of Germanium, and how does it relate to its electron count?

• 16, which is half the number of electrons

• 8, which is the number of valence electrons

• 32, which is the number of electrons

• 64, which is double the number of electrons

Which method is NOT mentioned for writing electron configurations?

• Lewis dot structure

• Periodic table blocks

• Molecular orbital theory

• Diagonal rule

How many electrons can the 's' and 'p' blocks hold, respectively?

• 6 and 10

• 2 and 6

• 4 and 8

• 8 and 18

What is the electron configuration for Germanium using periodic table blocks?

• 1s2 2s2 2p6 3s2 3p6 4s2 4p6

• 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6

• 1s2 2s2 2p6 3s2 3p6 3d10 4s2

• 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2

Which noble gas is used to condense the electron configuration of Germanium?

• Neon

• Argon

• Krypton

• Xenon

In condensed notation, which block sometimes appears after the 3d block?

• 4s

• 5s

• 4p

• 3p

How many electrons are removed to form the Ge4+ ion?

• 4 electrons

• 8 electrons

• 2 electrons

• 6 electrons

From which blocks are electrons removed first when forming Ge4+?

• d and f blocks

• s and p blocks

• p and d blocks

• s and d blocks

What is the electron configuration for the Ge2+ ion?

• 1s2 2s2 2p6 3s2 3p6 4s2 3d10

• 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2

• 1s2 2s2 2p6 3s2 3p6 4s2 4p2

• 1s2 2s2 2p6 3s2 3p6 3d10 4s2

What is the main focus of the video tutorial?

• Writing electron configurations for Germanium and its ions

• Understanding the periodic table layout

• Learning about chemical bonding

• Studying the properties of noble gases