© 2003 Mark S. Davis AP Chemistry Chapter 2. © 2006 Mark S. Davis 5.

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Presentation transcript:

© 2003 Mark S. Davis AP Chemistry Chapter 2

© 2006 Mark S. Davis 5

cs/ChemTeamInd ex.html

© 2006 Mark S. Davis A man was out walking in the desert when a voice said to him, "Pick up some pebbles and put them in your pocket, and tomorrow you will be both happy and sad." The man obeyed. He stooped down and picked up a handful of pebbles and put them in his pocket. The next morning he reached into his pocket and found diamonds and rubies and emeralds. And he was both happy and sad. Happy he had taken some - sad that he hadn't taken more. And so it is with education

© 2006 Mark S. Davis Atomic Theory of Matter Dalton’s Postulates 1.Each element is composed of extremely small particles called 2.All atoms of a given element are identical; the atoms of different elements are different and have different properties (including different masses.)

© 2006 Mark S. Davis Dalton 3. Atoms of an element are not changed into different types of atoms by chemical reactions; atoms are neither created nor destroyed 4. Compounds are formed when atoms of more than one element combine; a given compound has the same relative number and kinds of atoms.

© 2006 Mark S. Davis Define Atom:Atom – Element: –

© 2006 Mark S. Davis Define Compounds: –Substance composed Mixtures: –Combination of two or more Law of conservation of Mass:Law of conservation of Mass

© 2006 Mark S. Davis Atomic Structure Protons: – Neutrons: – Electrons: – –Charge is 1.6 x C

© 2006 Mark S. Davis Atomic Numbers Tell you: –Number of

© 2006 Mark S. Davis

Atomic Weights Atomic mass units (amu) 1 amu = x g 1 g = x amu Mass on the table –1 C = 12 amu

© 2006 Mark S. Davis Average Mass Isotopes Ave mass = (mass x %) + (mass x %) C has two isotopes –C-12 at 98.93% –C-13 at 1.07 % –Determine the average atomic mass

© 2006 Mark S. Davis The Periodic Table Family/Group – Period – Isotopes

© 2006 Mark S. Davis Types of elements Alkali Metals Alkaline Earth Metals Transition Metals Metalloids Non-metals Noble Gases Halogens Chalcogens Pnictides F-block Transuranium

© 2006 Mark S. Davis Molecules and Ions Molecule: –Chemically combined elements Diatomic Molecule

© 2006 Mark S. Davis Formulas Molecular – Empirical – Structural –

© 2006 Mark S. Davis IONS Cation: – Anion: – Polyatomic: –

© 2006 Mark S. Davis Predicting Charges Based on the Periodic Table Na Br O Ca Al Si

© 2006 Mark S. Davis Ionic Compounds Contain cations and anions – Use ELECTRONEGATIVITY to determine whether a compound is ionic –

© 2006 Mark S. Davis Ionic Compounds Most ionic compounds can only be represented by empirical formulas – Writing formulas for ionic compounds – – –

© 2006 Mark S. Davis Nomenclature System to ‘easily’ name chemical compounds. Organic, rules, rules, rules… –Ethane, ethanol, dimethyl ether Inorganic – much simpler

© 2006 Mark S. Davis Ionic Naming Look at Periodic Table… Oxidation numberOxidation number Cations with one possible charge keep name – – – –

© 2006 Mark S. Davis Ionic Naming Look at Periodic Table… Oxidation numberOxidation number Cations with more than one possible charge – – – Use the Stock System

© 2006 Mark S. Davis Stock System Use a Roman Number, I, II, III, IV, V, VI to represent the oxidation number Cr +3 Copper (I)

© 2006 Mark S. Davis Anions Monatomic: –Ending is changed to Polyatomic: some have –ide ending –CN - –OH -

© 2006 Mark S. Davis Practice Write the formula for the following: – –

© 2006 Mark S. Davis Oxyanions Oddly enough… contain oxygen! –Ending is changed to: -ate -ite Chlorine series

© 2006 Mark S. Davis Practice Name the following –

© 2006 Mark S. Davis Acids Defined: –Donate a proton Anion needs to be balance by hydrogen KNOW THE SIX STRONG ACIDS

© 2006 Mark S. Davis Binary MOLECULAR Compounds Characterized by covalent bonds, not ionic Use prefixes mono-, di-, tri-, etc… More positive element named first Second element has –ide ending

© 2006 Mark S. Davis Practice Name the following –