Structures and Bonding

Electron configurations

Longhand and Shorthand

The previous halogen,
then the remaining EC

The whole EC,
no previous halogen included

Quantum numbers

Principle
Quantum # (n)

Magnetic Field (m⌄l)

Magnetic/Electron Spin (m⌄s)

+1/2 or -1/2

Energy Sublevel (l)

Aufbau Principle

Lower energy orbitals fill
before higher energy orbitals.

Hund's Rule

One electron (arrow) goes into
each orbital before pairing up

Pauli Exclusion Principle

No two electrons can be
identified by the same set
of quantum numbers
(must have different spins).

Orbital Hybridization

Sp, Sp^2, Sp^3 & others

Atoms

Bonds

Single

Double

Triple

Molecules

Polar/Non-Polar

An uneven charge
distribution in a molecule

Structure and types
of atoms

Intermolecular Forces

Forces of attraction that appear
between two or more molecules

Dipole-Dipole

Magnetic attraction between
S^+ and S^-

Hydrogen Bonding

A type of dipole-dipole
specific to hydrogens

London Dispersion Forces/
Van Der Waals Forces

Temporary (short-term) forces
that can occur between any two molecules

Polar or non-polar

Magnetism

Para Magnetism

Atoms that temporarily rearrange
in the presence of a magnetic field.

Ferro Magnetism

Certain materials form to
be permanent magnets.

Iron, Cobalt, Nickel

Organic Chemistry

Organic Molecules

Hydrogen and Carbon

Alkane

Only single bonds

Least amount of tension

Methane

Alkene

At least 1 double
bond

Methene

Alkyne

At least 1 triple
bond

Methyne

Most amount of tension

Markovnikov's Rule

Rich get richer

Geometric Isomers

Cis

Functional groups on the
same side of the C chain

Trans

Functional groups on the
opposite side of the C chain

Functional Groups

Hydro Halogenation

Adding a halogen to
the molecule

Alkyl Halide

Hydrogenation

Adding a Hydrogen (H2)
to the molecule

Alkane

Alcohol

Adding Water (H2O)
to the molecule

Controlled Oxidation

Primary Alcohol

Aldehyde

Carboxylic Acid

Ester

Secondary Alcohol

Ketone

Tertiary Alcohol

Dehydration

Ether

Change of function, due to
the change in structure

Thermodynamics

Calorimetry

A measure of the amount
of heat released or absorbed
in a chemical reaction.

q = mc∆T

Enthalpy

∆H⌄x, The sum of
internal energy

Hess's Law

The total enthalpy
change is the sum of
all changes, regardless
of the # of steps/stages
of a reaction.

Chemical Kinetics

Rate of Reactions

Instantaneous Rate
of Change (IROC)

Change at a
certain point

Catalysts!

Average Rate
of Change (AROC)

Change over an
interval (2 points)

Rate Law

The RoR is related to the
[A] and [B] but not directly
proportional in all ways.

r = k[A]^m[B]^n

Collision Theory

a reaction consists of
particles that are always
randomly moving.

Brow nian Motion

These collisions with other
particles/wall of container can cause
the breaking/forming of bonds

Arrhenius Equation

The relationship between
the rate of reaction and
temperature for chemical reactions.

Gibbs Free Energy

∆G, The available
energy has to do work

Endothermic Reaction

A reaction that absorbs heat

Exothermic Reaction

A reaction that releases
heat

Activation Energy

Energy needed for
a reaction to occur

Electrochemistry

Redox Reactions

Spectator Ions

Positive E, spontaneous
Negative E, non-spontaneous

Reducing Agent

Atom that loses
electrons

Oxidizing Agent

Atom that gains
electrons

Half Reactions

Electrolysis

Galvanic Cells

Spontaneous
reactions

Standard Reduction Reaction

Tendency of something
to be reduced

Cell Notation

Anode | Anode(aq) | Cathode

Anode | Anode(aq) || Cathode(aq) | Cathode

Corrosion

Chemical Weathering

Ion is oxidized

Oxidation States

Equals the charge of the atom
within the molecule

Catalysts

Speed up a reaction

Equilibrium

Reverse reaction

When the reaction goes
backwards (right to left)

Closed Systems

No change in matter,
energy can be exchanged

Solubility Equilibrium

Dynamic equilibrium
between the solute and
solvent

Equilibrium Constant

Concentration at the
given equilibrium

Chemical Reaction
Equilibrium

Dynamic Equilibrium
between the products
and reactants of a chemical
reaction

Le Chatelier's Principle

Any disturbance will be adjusted
by the system, occurs at equilibrum

Collision Theory

Collisions can produce products
or reactants, the amount is equal

Phase Equilibrium

Dynamic Equilibrium between
the physical states of
substances

Ie. Same molecule but change in state

Equilibrium Law

Rule of 100
Perfect Squares
Quadratics

Elimination reaction

Loss of smaller molecule