Class notes

Class notes CHEM 121 (CHEM)

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Course
CHEM 121 (CHEM)

Institution
University Of British Columbia (UBC )

Detailed notes of UBC’s CHEM121 class for the 2022W term. This course was taught by Dr Stirchak and in these contains tips and notes advised by the instructor.

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Uploaded on December 27, 2022
Number of pages 6
Written in 2022/2023
Type Class notes
Professor(s) Laura stirchak
Contains All classes

chemistry
structure
ions
bonding
covalent
light
energy
matter
waves
longitudinal wave
transverse waves
vspepr
lewis structure
lone pair
valence bond theory
polarity
quantum numbers
electronic structur

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1
Cornell Topic/Objective: Name:
Notes
Chapter 2: Chemical Bonding Class/Period: Chem 121 111
and Lewis
Date: 09/24/2022

Essential Question:

Keywords: Notes:
Resonance Several ways of expressing the structures of a molecule based on their electron
Structures composition

Hypervalence An expanded octet (more than 8 electrons)

A molecule with 2 or more atoms that have diﬀerent electron negativity, where one
Polar Covalent bonds is PULLED towards another

Non-polar bonds A molecule of the same element or similar electronegativity

Ionic bonds Transferring of electrons USUALLY between a metal and non-metal

- Bond order correlates with the number of bonds.
Bond Order (Eg. 1st order = Single bond, 2nd order = Double Bond)

- Energy to break a bond (or more)
Bond Dissociation Usually given in a value kJ/Mol
Order (BDO)

Ionic/polar & non-polar covalent bonds
Ionic compounds undergo redox reactions, unlike polar covalent bonds, were one atom is pulled to the more
electronegative one
(Redox reaction is when one is oxidized (looses electrons) and the other reduced (gains electrons)
Example:
Ionic compounds
.

Polar covalent I na I [ a
]

, 2
It Means partially positive
Polar covalent dt dt
o Means partially negative
H
-

-
+ ◦
d-
¥
Hydrogen is pulled towards oxygen

How to Associate Bond order, Bond Dissociation Energy (BDE) and Bond Length?

Bond Order 1 2 3
Bond Length Furthest Mid Closest
BDE Least Mid Most

• The lower the order the further the length. There is less energy to keep it tight and close.
• The lower the order the lesser energy it takes to break a bond. Their bond is weaker
Bond Dipole
Example:

dt 1 A d-
H -
CI
When one (or more) atoms in a molecule are PULLED towards more
electronegative atom.

Octet Rule
An atom has to satisfy the octet rule of 8 valence electrons (Outer shell
electrons)
Exceptions (some don’t follow the octet rule):
• Group 13 elements can have less than 8
• Elements in the 3rd row and below of the P block can go into
hypervalence
• Free Radicals (unpaired electrons, often seen in uneven number total
valence electrons in a molecule)

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