Chemistry - Grade 12 Concept Map

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Kinematics and Dynamics

Kyle Tseにより

Foundation Chemistry UNIT 1

Hannah Homenukにより

ionic and metallic bonding

Patogamer1237 Patogamer1237により

Magnetism-psg

privut pursonにより

FAVOURITE MEMORY FROM SCH4U

When you did experiments for us to watch, also the balloon things to make us understand the structures. :)

Galvanic Cell Experiment

Elimination reaction

Loss of smaller molecule

Equilibrium

Equilibrium Law

Rule of 100 Perfect Squares Quadratics

Phase Equilibrium

Dynamic Equilibrium between the physical states of substances

Ie. Same molecule but change in state

Collisions can produce products or reactants, the amount is equal

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

Equilibrium Constant

Concentration at the given equilibrium

Solubility Equilibrium

Dynamic equilibrium between the solute and solvent

Closed Systems

No change in matter, energy can be exchanged

Reverse reaction

When the reaction goes backwards (right to left)

Electrochemistry

Catalysts

Speed up a reaction

Oxidation States

Equals the charge of the atom within the molecule

Corrosion

Ion is oxidized

Chemical Weathering

Cell Notation

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

Anode | Anode(aq) | Cathode

Standard Reduction Reaction

Tendency of something to be reduced

Galvanic Cells

Spontaneous reactions

Electrolysis

Redox Reactions

Half Reactions

Oxidizing Agent

Atom that gains electrons

Reducing Agent

Atom that loses electrons

Positive E, spontaneous Negative E, non-spontaneous

Spectator Ions

Thermodynamics

Activation Energy

Energy needed for a reaction to occur

Exothermic Reaction

A reaction that releases heat

Endothermic Reaction

A reaction that absorbs heat

Gibbs Free Energy

∆G, The available energy has to do work

Arrhenius Equation

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

Collision Theory

a reaction consists of particles that are always randomly moving.

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

Brow nian Motion

Chemical Kinetics

Rate of Reactions

Rate Law

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

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

Average Rate of Change (AROC)

Change over an interval (2 points)

Instantaneous Rate of Change (IROC)

Change at a certain point

Catalysts!

Hess's Law

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

Enthalpy

∆H⌄x, The sum of internal energy

Calorimetry

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

q = mc∆T

Organic Chemistry

Functional Groups

Change of function, due to the change in structure

Alcohol

Controlled Oxidation

Dehydration

Ether

Tertiary Alcohol

Secondary Alcohol

Ketone

Primary Alcohol

Aldehyde

Carboxylic Acid

Ester

Adding Water (H2O) to the molecule

Hydrogenation

Adding a Hydrogen (H2) to the molecule

Hydro Halogenation

Alkyl Halide

Adding a halogen to the molecule

Geometric Isomers

Trans

Functional groups on the opposite side of the C chain

Cis

Functional groups on the same side of the C chain

Markovnikov's Rule

Rich get richer

Organic Molecules

Hydrogen and Carbon

Alkyne

At least 1 triple bond

Most amount of tension

Methyne

Alkene

At least 1 double bond

Methene

Alkane

Only single bonds

Methane

Least amount of tension

Structures and Bonding

Magnetism

Ferro Magnetism

Certain materials form to be permanent magnets.

Iron, Cobalt, Nickel

Para Magnetism

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

Intermolecular Forces

London Dispersion Forces/ Van Der Waals Forces

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

Polar or non-polar

Hydrogen Bonding

A type of dipole-dipole specific to hydrogens

Dipole-Dipole

Magnetic attraction between S^+ and S^-

Forces of attraction that appear between two or more molecules

Molecules

Polar/Non-Polar

Structure and types of atoms

An uneven charge distribution in a molecule

Atoms

Bonds

Triple

Double

Single

Orbital Hybridization

Sp, Sp^2, Sp^3 & others

Pauli Exclusion Principle

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

Hund's Rule

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

Aufbau Principle

Lower energy orbitals fill before higher energy orbitals.

Quantum numbers

Energy Sublevel (l)

Magnetic/Electron Spin (m⌄s)

+1/2 or -1/2

Magnetic Field (m⌄l)

Principle Quantum # (n)

Electron configurations

Longhand and Shorthand

The whole EC, no previous halogen included

The previous halogen, then the remaining EC