Electron Configuration

Presentation

•

Chemistry

•

11th - 12th Grade

•

Medium

T Southerden

Used 4+ times

FREE Resource

25 Slides • 13 Questions

Exploring Sub Orbitals

Labelling

Label the parts of the atom

Drag labels to their correct position on the image

Proton

Electron

Neutron

Orbit

Ion

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, p

s, p, d

s, p, d, f

Multiple Choice

How many f orbitals can an f sublevel hold?

Multiple Choice

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

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?

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

Exploring Sub Orbitals

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