CHAP 2 Atoms, Molecules, and ions. History Greeks everything made up of 4 fundamental substances (earth,air,fire,water) “atomos” – later became atom –

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Presentation transcript:

CHAP 2 Atoms, Molecules, and ions

History Greeks everything made up of 4 fundamental substances (earth,air,fire,water) “atomos” – later became atom – small, indivisible particles Dalton’s Atomic Theory – Each element made up of atoms Atoms of same element same; different element different Compounds form from combinations of elements in definite proportions. Chemical reactions involve rearrangements of atoms.

More History Thomson – studied cathode-ray tubes/Plum Pudding Model Negative particle (electron) Determined charge to mass ratio of electron Milikan – Oil Drop Experiment Determined magnitude of electron charge Rutherford – Gold Foil Experiment Found positive center of atom (nucleus) Positive particle – proton Bohr – model of Hydrogen atom Chadwick – discovered neutron

Key Terms Atomic mass – average # of protons & neutrons in an atom Atomic weight – weighted average mass determined by a standard Atomic number – # of protons in an atom Mass number – total # of protons & neutrons Isotope – same # protons, but different # neutrons Ion – gain or lost electrons (no longer equal to # protons) Neutral atom – equal # of protons and electrons Nucleus – positively charged, dense center of the atom

Atomic Structure SymbolMassChargeLocation ProtonP+P+ 1+nucleus Neutronn0n0 1-nucleus Electrone-e- 00Electron cloud Nucleus – contains mass of atom Electron cloud – gives volume to atom

Periodic Table Types of elements Metals – left side; majority of elements; good conductors; lose electrons (+ ions) Nonmetals – right side; poor conductors; gain electrons (- ions) Metalloids – stair-step line Groups – columns; grouped by similar properties 18 – each has a name Periods – rows 7

More on Periodic Table Group 1 – Alkali Metals Group 2 - Alkaline Earth metals Groups 3-12 – transition metals Groups – named after first element and word family (ie. Carbon family – group 14) Group 17 – Halogens Group 18 – Noble Gases Bottom – Lanthanide and Actinide series

Naming Binary Compounds Cation (+ion) named first, anion (-ion) named second First element is named as the element Second element, keep root & change ending to – ide if has more than 1 charge possible, use Roman numeral to indicate charge of metal (systematic) May use latin root of element – higher charge ends in –ic, lower charge in –ous Polyation ions named as is – change nothing If covalent compound (2 nonmetals) – need to use prefixes.

Formula Writing Compound needs to be electrically neutral – balance out charges. Criss-cross the ion charges to become the subscripts in the formula. Polyatomic ions belong in parentheses. Any criss- crossed subscript goes outside parentheses. Remember roman numeral indicates charge of that metal. Prefix value goes with the element it is attached to – no criss-crossing if have prefix.

Acids Always contain hydrogen first in the formula If it does not contain oxygen (just H and another element), named with prefix hydro-, root, and ends in –ic. If does contain oxygen, if polyatomic ion ends in –ite, acid ends in –ous. If polyatomic ion ends in –ate, acid ends in -ic