SCH3U0-D

Honelako gehiago

9th Grade Concept Map

by Lauren Holler

The Modern View of Matter

by Chris Shaw

Multiple Equations

by Jackie Lindquist

Chapter 8 Mind Map

by Kaitlynne Paul

Bond Polarity

Difference in ENs of bonded atoms

Polar covalent bond

dipole

picture

Partially negative end (electron rich)

δ+

Partially positive end (electron deficient)

δ-

Unequal Sharing

Non-polar covalent bond

Equal sharing

Molecular Polairty

Non-polar

Symmetrical

Polar

one positive end

one negative end

lone pairs

Asymmetrical

Intermolecular Forces

Ion Dipole

Induced dipole-dipole

Hydrogen Bonding

London Dispersion Force

Electronegativity (EN)

contain

Shared Electrons

Transfer of Electrons

can be

Intramolecular Forces

Strength

Weak Base

Strong Base

Weak Acid

Strong Acid

Example of Criss Cross

NM + NM

M + NM

Matter

Chemical Properties

Physical Properties

Types of Matter

Pure Substances

Compounds

Molecules

Elements

Atoms

Parts

Shells

Electrons (- charge)

Valence Electrons

Stability

Octet Rule

Boron and Beryllium

Nucleus

Neutrons (no charge)

Protons (+ charge)

Properties

Atomic Mass

Mass Number

Isotopes

Atomic Number

Mixtures

Heterogenous

Homogenous

States of Matter

Bose-Einstien Condensate

NOTE: Connect back to Gase unit

Plasma

Gas

Liquid

Solid

100% dissociated in water

Less than 100% dissociated in water

Less than 100% ionized in water

100% ionized in water

Periodic Table

Groups

Periods

Non-metal (NM)

Metal (M)

Metalloids

include

artificially made

(WIP) NET IONIC AND PERCIPITATION

represented as

Symbols

Aqueous (aq)

Liquid (l)

Solid (s)

Gas (g)

are

if

Logarithmic Equations

[OH⁻] = 10⁻^pOH

[H₃O⁺/H⁺] = 10⁻^pH

pOH = -log[OH⁻]

pH = -log[H₃O⁺/H⁺]

pH + pOH = 14

such as

Ionization/Dissociation

NH₃(aq) + H₂O(l) -> NH₄⁺(aq) + OH⁻(aq)

NaOH(aq) + H₂O(l) -> Na⁺(aq) + OH⁻(aq)

CH₃COOH(aq) + H₂O(l) -> CH₃COOH⁻(aq) + H(aq)

HCl(aq) + H₂O(l) -> H₃O⁺(aq) + Cl⁻(aq)

pH Scale

Picture of ph Scale

Basic/Alkaline

Neutral

Acidic

Hydroxide Ion Concentration [OH-]

Hydronium/Hydrogen Ion Concentration [H30+/H+]

SCH3U0-D

Matter, Chemical Trends and Chemical Bonding

Nomenclature

All Non-metals (NM) have - charge

Anion

All Metals (M) have + charge

Cation

Bonds

Ionic

Ionic Compound

Multivalent Compound

Metal has more than one charge

roman numerals (e.g. I, II, IV, V)

Polyatomic Ion

Covalent

Diatomic

HOFBRNCl

Molecular Compound

Metallic

M + M

Hydrate

*H₂O

Base

Acid

Binary Acid

Oxyacid

Criss Cross

Simplify Formula

Chemical Reactions

Equations

Complete Ionic Equations

Net Ionic Equations

Chemical Equations

Stoichiometry

2KI(aq) + Pb(NO₃)₂(aq) → 2KNO₃(aq) + PbI₂(s)

Balanced (Equal number of atoms on reactant and product side)

Word Equation

Sodium + Chloride -> Sodium Chloride

Types of Reactions

Oxidations

Non-metal Oxide

Metal Oxide

Displacements

Activity Series

Element's reactivity relative to each other

Displacment occurs quicker

Compound's element if it's below

Single Displacement

A(non-metal) + B(metal)C -> AB + C

A(metal) + B(metal)C -> AC + B

Double Displacement

AB + CD -> AD + CB

Precipitate

ionic formed

insouluble (connect to solutions unit)

Combustion

Fuel

Incomplete Combustion

limited oxygen

Carbon Dioxide, Water Vapor, and Energy + Carbon Monoxide and/or Soot (Carbon)

Complete Combustion

extra oxygen gas

"Connect the extra and limited to the concept of excess reagent and limited reagent"

Carbon Dioxide, Water Vapor, and Energy

Neutralization

A salt and water

Decomposition

AB -> A + B

Synthesis

A + B -> AB

Reactants and Products

Observations

An indicator may not necessarily be a chemical change, but physical.

Painting a car (change in color) is a physical change. While a solution changing color is a chemical change

Physical Changes

Chemical Composition

Texture

Change in States of Matter

endothermic

exothermic

Melting Point

Boiling Point

Shape

Chemical Changes

Irreversible

Odor

Color

Bubbles/Gas

New Substance

Heat/Light

Solutions and Stoichemetry

Colloid

Suspension +(precipitate)

Solution

Components

Solubility

Amount of solute per amount of solvent: e.g. 36.0 NaCl/100g of H20 at 20°C

Solubility Curves

Saturated

Supersaturated

Unsaturated

Solubility Factors

Subtopic

Pressure

Temperature

Concentration

C₁V₁ = C₂V₂

Molar Concentrations

M = n/V

Very Small Concentrations

Parts Per Trillion

ppt = solute/solution * 10^12

Parts Per Billion

ppb = solute/solution * 10^9

Parts Per Million

ppm = solute/solution * 10^6

Solution Concentrations

Percentage Mass(g) (%m/m)

Percentage Mass(g) by Volume(L) (%m/V)

Percentage by Volume(L) (%V/V)

% C (m/V) = msolute/Vsolution

Solute

Solvent

Golden Rule "Like Dissolves Like"

Gases and Atmospheric Pressure

Quantities of Chemical Reactions