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Honors Chemistry Name ______

Chapter 2 – Atoms, Molecules and a Ions

Introduction

Atoms:

Molecules:

Ions:

2.1 Atoms and the Atomic Theory

Greeks: Empedocles and Democritus

John Dalton:

Atomic Theory

1.)

2.)

3.)

4.)

1 Fundamental Laws of Matter

Law of Conservation of Mass:

Law of Constant Composition:

Law of Multiple Proportions:

2.2 Components of the atom

2 J.J Thomson:

Cathode Ray Tube:

Electrons

J.J. Thomson’s Model

3 Ernest Rutherford:

Gold Foil Experiment:

Nuclear Particles:

Atomic Mass –

Properties of subatomic particles

Particle Location Relative charge Relative Mass Proton Neutron Electron

4 Terminology:

Atomic Number, Z A Mass number, A Z X

Isotopes

Examples:

5 Radioactivity Radioactive isotopes are unstable

1)

2)

Particles emitted

1)

2)

3)

Nuclear Stability

Depends on …

2.3 Introduction to the Periodic Table Dmitri Mendeleev:

Modern Periodic Table

6 Period –

Group –

Blocks –

Families -

Blocks in the Periodic Table

7 2.4 Molecules and Ions molecule:

1.

2.

8 Molecular formulas:

Structural formulas:

Ion :

Cation:

Anion:

Examples:

2.5 Ionic Compounds

Forces –

Solutions –

Conductivity –

9 Formulas for Ionic Compounds

Transition Metals:

Polyatomic ions:  Memorize 24 given on hand out 

Noble Gases:

10 2.6 Naming of compounds

Cations:

Anions:

To name an ionic compound: name the cation first, then, name the anion (with the word 'ion' omitted). It is not necessary to indicate the number of cations and anions in the compound because it is understood that the total positive charges carried by the cations must equal the total negative charges carried by the anions. A few examples are listed below: KI potassium ion + iodide ion = potassium iodide

CoCl2 cobalt(II) ion + two chloride ions = cobalt(II) chloride

CoCl3cobalt(III) ion + three chloride ions = cobalt(III) chloride mercury(I) ion + two chloride ions = mercury(I) chloride or Hg Cl 2 2 mercurous chloride

AgNO3 silver ion + nitrate ion = silver nitrate

11 Oxoanions:

-ate

-ite

-per

-hypo

Practice Examples :

Sodium bromide ______Calcium phosphate ______Magnesium oxide ______Sodium hypochorite ______Potassium nitrite ______Iron (III) sulfate ______

Binary Molecular Compounds

Systematic Naming

12 1-

2-

Examples: diphosphorus pentaoxide sulfur dioxide dinitrogen tetraoxide hydrogen dioxide carbon monoxide phosphorus trichloride

Acids:

Naming: Common

Oxoacids

Acids of chlorine

Examples:

Hydrogen chloride (hydrochloric acid) Nitric acid Sulfuric acid Hypobromous acid Nitrous acid Phosphoric acid

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