Chapter 2 Atoms, Molecules & Ions. Atomic Theory Elements composed of atoms Atoms can’t be changed by “normal” chemical reactions Compounds of multiple.

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Atoms, Molecules, and Ions

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Presentation transcript:

Chapter 2 Atoms, Molecules & Ions

Atomic Theory Elements composed of atoms Atoms can’t be changed by “normal” chemical reactions Compounds of multiple atoms John Dalton

Conservation of Mass In ordinary chemical reactions, matter can be neither created nor destroyed

Constant Composition Compounds contain elements that are always in the same proportions

Period 2 stopped here 9/7/06

Multiple Proportions The elements making up a compound will form whole number ratios

Atom The smallest particle an element can be broken down into and still maintain the identity of the element

Nuclear Atom Proved by Rutherford & Bohr in the famous gold foil experimentsgold foil experiments

Subatomic CompositionComposition Proton: in the nucleus Neutron: in the nucleus Electron: outside the nucleus

Proton In Nucleus +1 relative charge About 1 amu in mass

Neutron In nucleus Neutral, zero charge Mass is about 1 amu

Electron Outside the nucleus -1 in relative charge Negligible mass about 1/2000 amu

Electron Charge Determined by Robert Milliken in the famous oil droplet experimentoil droplet experiment

Atomic Number The number of protons in an element Z number

Mass Number = number of protons and neutrons in an atom A - number

Nuclear Symbol A 4 X He Z 2 GeneralSpecific FormulaExample

Isotopes Atoms that contain the same number of protons, but different number of neutrons Z constant, A variable

Isotopes are useful! C 14 - dating Isotopic - tracing – Works like a flag – you can follow an atom or molecule through a reaction

Shorthand for isotopes Instead of full notation: 14 CWrite: C-14 6 So, only the A number (protons + neutrons)

Atomic Mass All elements have >1 isotope. The percentage of one isotope is its relative abundance. Atomic mass = (A # of isotope 1 x % isotope #1) + (A # of isotope 2 x % isotope # 2) + etc…

Periodic Table Hierarchy of all the elements. The order is used to predict size, charge, electronic structure & reactivity of elements

Periods Rows which indicate energy level or shell or size of the atoms

Groups or Families Columns which indicate the number of electrons in the outermost energy level determining charge & reactivity

Metals Left three quarters of the chart Lose electrons Become positive

Nonmetals Upper right portion Gain, lose, or share electrons when they react

Metalloids Along the stair-stepped line from B to At Share properties of metals & nonmetals

Radioactivity The spontaneous breakdown of an unstable nucleus

Compound A grouping of atoms that are chemically combined

Molecule A compound that can exist by itself

Diatomic Molecule Two atoms of the same element that are chemically combined Cl 2, F 2, O 2

Ion Charged Particle Cl -1

Polyatomic Ion A group of atoms chemically combined that together has a charge SO 4 -2

9/7/06 period 1 stopped here

Binary Compound A compound made up of two elements in any ratio NaCl Mg 3 P 2

Chemical Formula A formula that shows the number and kinds of atoms in a compound CaCO 3

Molecular Formula A formula that shows the number and kinds of atoms in a molecule C 6 H 12 O 6

Period 4 stopped here 9/7/06

Atomic Structure List & describe the three subatomic particles

Atomic Structure Fill in the Chart: Isotope protons neutrons electrons U

Calculate the atomic mass of the element made up of the following isotopes: % H % H % H-3

Calculate Pt’s atomic mass : 5.0 % Pu % Pu % Pu % Pu-245

Determine the number of atoms in each compound C 6 H 12 O 6 NaNO 3 H 3 PO 4 Al 2 (SO 4 ) 3