Module 1-3

Question 1

The orbitals are arranged in order of increasing energy based on the principal energy levels and the sublevels where they are in. 1s 2s 2p…

Answer 1

Aufbau Principle

Question 2

This means no atomic orbital can contain more than TWO electrons and these electrons must be of opposite spin if they are to form a pair within an orbital. The boxes… ORBITAL DIAGRAM

Answer 2

Pauli’s Exclusion Principle

Question 3

• The most stable arrangement of electrons is one with the maximum number of unpaired electrons.
• This minimized the electron-electron repulsions and stabilizes the atom.

Up arrows first, then Down arrows

Answer 3

Hund’s Rule

Question 4

what is s, p, d, f stands for?

Answer 4

Sharp
Principal
Diffuse
Fundemental

Question 5

What are the noble gases?

Answer 5

Helium, Neon, Argon, Krypton, Xenon, Radon

Question 6

Atomic mass of
Helium
Neon
Argon

Answer 6

Helium = 2
Neon = 10
Argon = 18

Question 7

Atomic mass of
Krypton
Xenon
Radon*

Answer 7

Krypton = 36
Xenon = 54
Radon = 86

Question 8

• These are the electrons that are found on the outermost energy level of an atom.
• These electrons are important because they give us a deep insight about the chemical property of an element.

Answer 8

VALENCE ELECTRONS

Question 9

The use of noble gases

Answer 9

CORE METHOD

Question 10

Paramagnetism and Diamagnetism

Answer 10

MAGNETIC PROPERTY

Question 11

(attracted to magnetic field) refers to the magnetic state of an atom with one or more unpaired electrons.

Answer 11

Paramagnetism

Question 12

(repelled by magnetic field) paired electrons. This causes the magnetic fields of the electrons to cancel out; there is no net magnetic moment, and the atom cannot be attracted into a magnetic field.

Answer 12

Diamagnetism

Question 13

1s² 2s² 2p⁶ 3s² 3p⁴, ? = 6

Answer 13

Valence electron = 6

Question 14

1s² 2s² 2p⁶ 3s² 3p⁴

Answer 14

Valence Shell = 3

Question 15

• Numbers that are used to describe the probable
  location of an electron in an atom.
• These numbers work like addresses for electrons
  in an atom.

Answer 15

Quantum numbers

Question 16

describes the energy level of the electron. The energy of the electron is determined by its average distance from the nucleus. “1s² 2s² 2p⁶”

Answer 16

Principal Quantum Number (n)

Question 17

It describes the “shape” of the orbital. It designates the sublevel which the electron is said to occupy.s = 0, p = 1, d = 2 and f =
3.

Answer 17

Azimuthal or Angular Momentum Quantum Number (l)

Question 18

describes the shape of the orbitals in a SUBSHELL. Orbitals have shapes that are best described as spherical, polar or cloverleaf. THE BOXES

Answer 18

Magnetic Quantum Number (ml)

Question 19

refers to the “spin” of an electron in a given orbital. It can only have two values: +1/2 and -1/2.

DOWN = -1/2 , UP = +1/2

Answer 19

Spin Quantum Number (ms)