Electron Configuration Basics

Exploring Sub Orbitals

Labeling

Label the parts of the atom

Drag labels to their correct position on the image

Proton

Ion

Neutron

Orbit

Electron

Hotspot

Where are the group 1 metals found on the periodic table?

Categorize

Options (20)

Helium

Neon

Argon

Krypton

Xenon

Lithium

Sodium

Potassium

Rubidium

Cesium

Beryllium

Magnesium

Calcium

Strontium

Barium

Fluorine

Chlorine

Bromine

Iodine

Astatine

Categorise the following Elements

Alkali Metals

Alkali Earth metals

Halogens

Nobel Gases

Multiple Choice

What are the orbitals for n=4

• s

• s, p

• s, p, d

• s, p, d, f

Multiple Choice

How many f orbitals can an f sublevel hold?

• 1

• 7

• 5

• 14

Multiple Choice

What are the orbitals that make up the n=1 energy level?

• s

• s, p

• s, p, d

• s, p, d, f

Multiple Choice

Which of the following statements is true about the 3s and the 4s sublevels?

• These sublevels have the same energy
• These sublevels are the same distance from the nucleus
• These sublevels hold different amounts of electrons
• These sublevels have the same shape

Multiple Choice

How many atomic orbitals are there in the d sublevel?

• 3
• 4
• 5
• 6

Multiple Choice

What do you start electron configuration with?

• 1s²
• 1d¹⁰
• 1f¹⁴
• 1p⁶

Multiple Choice

Each row on the periodic table represents:

• an energy level

• a sublevel

• an electron

• an orbital

Multiple Choice

An aluminium ion would have which electron configuration?

• 1s² 2s² 2p⁶ 3s²

• 1s² 2s² 2p⁶ 3s² 3p¹

• 1s² 2s² 2p⁶ 3s² 3p⁶

• 1s² 2s² 2p⁶

Multiple Choice

Region of high probability of finding an electron

• atomic orbital

• ground state

• Heisenberg uncertainty principle

• electron configuration

Multiple Choice

What does Pauli exclusion principle state ?

• states that each electron occupies the lowest energy orbital available
• states that a maximum of two electrons can occupy a single atomic orbital, but if only if the electros have opposite spins
• states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals