2.1 Know the three basic subatomic particles of an atom and their charges: 1. Protons (+) 2. Electrons (-) 3. Neutrons (0)

2.2 Define

Atomic number (Z) Mass number (A) Use the notation, AZX to particular atoms

2.3 – Isotopes & Atomic Weights ▪ Define the word isotope and how it

relates to the number of neutrons of a particular type of atom

▪ Know the two conventions for writing isotopes

▪ Define the atomic weight of the average atom (what’s in the periodic table)

• Isotopes:Isotopes: atoms with the same number of protons but a different number of neutrons.– carbon-12 has 6 protons and 6 neutrons;– carbon-13 has 6 protons and 7 neutrons;– carbon-14 has 6 protons and 8 neutrons;

• Most elements found on Earth are mixtures of isotopes:– chlorine is 75.77% chlorine-35 (18 neutrons) and

24.23% chlorine-37 (20 neutrons).

C136C

136

C126C

126

C146C

146

• Mass number:Mass number: the number of protons and neutrons in the nucleus of an atom.– the mass of the electrons in an atom is so small

compared to that of its protons and neutrons that electrons are not counted in determining mass number.

• Atomic number:Atomic number: the number of protons in the nucleus of an atom.

• a carbon atom of this composition is referred to as carbon-12.

Mass number (number of protons & neutrons)Atomic number (number of protons)6

12C

• Atomic weight:Atomic weight: the weighted average of the masses (in amu) of the naturally occurring isotopes of an element.– example: chlorine is 75.77% chlorine-35 and

24.23% chlorine-37

75.77100

x 34.97 amu + 24.23100

x 36.97 amu = 35.45 amu

chlorine-35 chlorine-37 17Cl

35.4527

atomic weight in the Periodic Tableis given to four

four decimal places

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2.3 Define and apply Atomic Mass Unit Know what is meant by Atomic Weight Know how to calculate percent abundances for elements with two isotopes

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2.4 Know how to determine atomic weights - check

2.5 Be able to identify and locate the following features in the Periodic Table: 1) Metals & Nonmetals 2) Groups (both number systems)

(a) Main Group 1. Alkali Metals 2. Halogens 3. Noble Gasses 4. Alkali Earth Metals

(b) Transition Metals (c) Inner Transition Metals

3) Periods

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2.6 & 2.7 1) Define, apply and distinguish among the terms: i) Element ii) Compound iii)Molecular Compound iv) Ionic Compound v) Formula

2.6 & 2.7 1) Understand the following features of Ionic

Compounds: i) General Composition

(a) Cation & Anion (b) Metal/Nonmetal (some exceptions)

ii) Monatomic Ions & the Periodic Table (a) M. Groups I & II metal cations (b) M. Groups V, VI & VII anions

iii) Polyatomic Ions – mostly anions (1) Memorize the name and formula for the

following (a) Ammonium, Acetate, Carbonate, Hydrogen

Carbonate, Nitrate, Sulfate, Phosphate, Hydroxide iv) Formulas

(1) Naming given formula (2) Writing formula given name

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2.8 1) Learn to recognize, name and write formulas for one class of Molecular (Covalent) Compounds: Binary

a) Learn the guidelines 1. Put atoms in order of increasing group#

2. Prefixes for first atom Prefix Amount Di 2 Tri 3 Tetra 4 Penta 5 Hexa 6 Hepta 7 Octa 8 Nona 9 Deca 10

3. Prefixes for second atom Prefix Amount Mono 1 Di 2 Tri 3 Tetra 4 Penta 5 Hexa 6 Hepta 7 Octa 8 Nona 9 Deca 10

2.9 1. Understand and apply the Mole as a counting unit

2. Understand and apply, molar mass 3. Perform mole to mass and mass to

mole conversions for elements and compounds

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2.10 1. Perform percent composition problems 2. Understand the term, Empirical Formula 3. Use percent composition to derive an

Empirical Formula 4. Use Empirical Formula and Molar Mass

to derive a Molecular Formula.

Empirical Formula

Molecular Formula is…

4.4 Use Combustion Analysis to derive Molecular Formulas

2.11 1. Understand & Recognize Hydrated Compounds

2. Determine the formulas of Hydrated Compounds