Basic Atomic Model

Element Notation

Rings = Energy Levels (can be labeled 1, 2, … or K, L, …)

Outermost Electron = Valence Electron

Outermost Ring = Valence Shell

X = C = Element Symbol

A = 12 = Mass Number = # of protons + # of neutrons

Z = 6 = # of protons = # of electrons

Sublevels

Orbitals

Number of Electrons

s

1

2

p

3

6

d

5

10

f

7

14

Description

Rules

Examples

Knowing the oxidation number and the charge of one of the elements in the compound allows us to solve for the charge of the other element,

Charge of H = +1

Charge of O = -2 (except for in hydrogen peroxide)

Isotopes

Ions

Same element but with a different number of neutrons

Same element but with a different number of valence electrons

Ionic Bond

Covalent Bond

Electron donating; between one nonmetal and metal

Electron sharing; between two nonmetals

Description

Rule

Example

Binary Compounds

(Compounds with two elements)

Cation + Anion in ide ending

K⁺ = Potassium (Cation)

O^2- = Oxygen (Anion)

K₂O = Potassium Oxide

Ternary/Tertiary Compounds (Compounds with three elements)

Cation + Anion

Na⁺ = Sodium (Cation)

PO₄^3- = Phosphate (Anion)

Na₃PO₄ = Sodium Phosphate

Binary Acids

(Anion is NOT a compound)

Hydro + Anion in ic ending + Acid

H⁺ = Hydrogen (Cation)

Cl^- = Chlorine (Anion)

HCl = Hydrochloric Acid

Acids with Anion in ate Ending

Anion in ic ending + Acid

H⁺ = Hydrogen (Cation)

SO₄^2- = Sulfate (Anion)

H₂SO₄ = Sulfuric Acid

Acids with Anion in ite Ending

Anion in ous ending + Acid

H⁺ = Hydrogen (Cation)

NO₂^- = Nitrite (Anion)

HNO₂ = Nitrous Acid

Covalent Compounds

(Compounds Composed of Only Nonmetals)

Use mono, di, tri, etc.

C = Carbon

O = Oxygen

CO = Carbon Monoxide

CO₂ = Carbon Dioxide

Elements with Different Ions/Different Oxidation Numbers

Lower Oxidation Number = ous ending

Higher Oxidation Number = ic ending

Fe²⁺ = Ferrous

Fe³⁺ = Ferric

Pb²⁺ = Plumbous

Pb⁴⁺ = Plumbic

Compounds with a Different Number of Oxygen

Lower Oxygen Number = ite ending

Higher Oxygen Number = ate ending

PO₃^3- = Phosphite

PO₄^3- = Phosphate

Type

Description

Example

Single Displacement Reaction

Only one element in the compound is replaced by another

2 Al (s) + 6 HCl (g) → 2 AlCl₃ (aq) + 3 H₂ (g)

Double Displacement Reaction

Reactants and products switch their ions

3 NaOH (aq) + FeCl₃ (aq) → 3 NaCl (aq) + Fe(OH)₃ (s)

Combination Reaction/Synthesis

Two reactants result in one product

Na₂O + H₂ → 2 NaOH

Decomposition Reaction/Analysis

One reactant results in two products

2KClO₃ (s) → 2 KCl (s) + 3 O₂ (g)

Chemical Name

Chemical Formula

Chemical Name

Chemical Formula

Iodine

I₂

Ferric Chloride

FeCl₃

Sodium Thiosulfate

Na₂S₂O₃

Chromic Sulfate

Cr₂(SO₄)₃

Carbon Tetrachloride

CCl₄

Calcium Chloride

CaCl₂

Chloroform

CHCl₃

Zinc Nitrate

Zn(NO₃)₂

Ethyl Alcohol

CH₃CH₂OH

Aluminum Sulfate

Al₂(SO₄)₃

Glycerin

C₃H₈O₃

Ammonium Hydroxide

NH₄OH

Blue Vitriol (or Cupric Sulfate)

CuSO₄

Acetic Acid

CH₃COOH

Sodium Hydroxide

NaOH

Hydrochloric Acid

HCl

Ammonium Chloride

NH₄Cl

Aluminum Shavings

Al

Marble Chips

CaCO₃

Substance

Iodine

Sand

Table Salt

Sugar

Solubility in Water

Slightly Soluble

(Dissolved faster in chloroform)

Insoluble

Soluble

Soluble

Substance

Ethyl Alcohol (CH₃CH₂OH)

Glycerine

Oil

Solubility in Water

Mixes with water meaning it is a miscible liquid

Does not mix with water, sinks to the bottom

Does not mix with water, remains at the top

Unsaturated

Saturated

Supersaturated

Occurred in steps…

1. Take 1 mL H₂O and add a crystal of Na₂S₂O₃

2. Add more crystals of Na₂ S₂O₃

3. Add more crystals of Na₂ S₂O₃ and heat

4. Allow solution to cool, add 1 crystal of Na₂ S₂O₃

Occurred in steps…

1. Take 1 mL H₂O and add a crystal of Na₂S₂O₃

2. Add more crystals of Na₂ S₂O₃

3. Add more crystals of Na₂ S₂O₃ and heat

4. Allow solution to cool, add 1 crystal of Na₂ S₂O₃

Occurred in steps…

1. Take 1 mL H₂O and add a crystal of Na₂S₂O₃

2. Add more crystals of Na₂ S₂O₃

3. Add more crystals of Na₂ S₂O₃ and heat

4. Allow solution to cool, add 1 crystal of Na₂ S₂O₃

Exothermic

Endothermic

Energy RELEASING reaction; solution becomes WARMER

Energy ABSORBING reaction; solution becomes COLDER

Occurred when 10mL H₂O added to NaOH (s)

Occurred when 10mL H₂O added to NH₄Cl (s)

Taste

Litmus Paper

Indicator

Acetic Acid (CH₃COOH)

Sour, vinegar-like

Blue → Red

Methyl Orange (Neon Pink)

Hydrochloric Acid (HCl)

Astringent (dry), less sour

Blue → Red

Methyl Orange (Neon Pink)

Ammonium Hydroxide (NH₄OH)

Bitter, acrid (strong & sharp)

Red → Blue

Phenolphthalein (Dark Pink)

Sodium Hydroxide (NaOH)

Bitter

Red → Blue

Phenolphthalein (Light, Clear Pink)

Reacts faster with Al?

Reacts faster with CaCO₃?

CH₃COOH

NO

HCl

YES

6 HCl (aq) + 2 Al (s) → 2 AlCl₃ (aq) + 3 H₂ (g)