Electron Configurations and Orbital Theory

The tutorial covers electron configurations, focusing on the Aufbau principle, energy levels, and orbitals. It explains how to determine electron configurations using the Aufbau chart and introduces noble gas notation for simplification. Special attention is given to transition metals and exceptions in electron configurations, highlighting stability and energy considerations.

What principle is used to determine the order of orbital filling in electron configurations?

• Heisenberg Uncertainty Principle

• Pauli Exclusion Principle

• Hund's Rule

• Aufbau Principle

Which orbital can hold a maximum of 10 electrons?

• f orbital

• d orbital

• s orbital

• p orbital

How many electrons are needed to fill the first energy level?

• 10

• 8

• 6

• 2

What is the noble gas notation for sodium?

• [He] 2s2 2p6 3s1

• [Ne] 3s1

• [Ar] 3s1

• [Kr] 4s1

Which element's electron configuration can be simplified using argon as a core?

• Neon

• Silicon

• Gallium

• Sodium

What are valence electrons responsible for?

• Chemical bonding

• Nuclear stability

• Radioactive decay

• Thermal conductivity

In which period do the d electrons first appear?

• Fourth

• Third

• Fifth

• Second

Why do some transition metals have unexpected electron configurations?

• Because they are radioactive

• Due to their metallic nature

• Because of sub-level splitting

• Due to high atomic mass

Which element is an example of an exception to the predicted electron configuration?

• Oxygen

• Neon

• Chromium

• Helium

What happens to the energy level of d orbitals as they are filled?

• It fluctuates

• It remains constant

• It decreases

• It increases