A.P. Ch. 2 Review Work Atoms, Molecules, Ions. Conservation of mass: during a reaction the amount of...
Transcript of A.P. Ch. 2 Review Work Atoms, Molecules, Ions. Conservation of mass: during a reaction the amount of...
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A.P. Ch. 2 Review Work
Atoms, Molecules, Ions
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• Conservation of mass: during a reaction the amount of material you start with equals the amount you end with
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Dalton’s Atomic Theory• 1. Elements made of atoms • 2. Atoms of same elements identical, different
elemental atoms are different • 3. Compounds are atoms combined • 4. Chemical rxns: reorganization of atoms • 5. Cannot change one element into another
through chemical rxn
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Thomson’s Experiment• Electrified gas in a cathode ray tube sends a beam
from anode (- end) to cathode (+ end)
• When a positive charge is presented to the light beam, it is bent towards charge
• Thomson reasoned beam made of negatively charge particles he called “electrons”
• Identified their charge to mass ratioPositive Magnet
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Rutherford’s Experiment• Used radioactive particles shot at a piece of
gold foil to determine the composition of atoms
• Based on “Plum-Pudding Model” of atom, assumed particles go through with few deflections
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• Most particles went through, yet some large deflections, indicating atoms made of mostly space with dense part
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Atomic Particles• Protons: positively charged in nucleus• Neutrons: no charge in nucleus• Electrons: negatively charged around nucleus
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Molecules• Multiple atoms joined together by covalent bonds
• Covalent bond: e- shared by attached atoms
• Ionic bond: electrostatic attraction between oppositely charged ions (when e- lost or gained by an atom), different elements joined form “compounds”
• Lose e- (+ ion “Cation”)
• Gain e- (- ion “Anion”)
Covalent bond
Ionic bond
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Periodic Table• Organized by # of protons
• Vertical columns (“groups”) based on similar properties
• Horizontal rows (“periods”) based on similar electron organizations
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Determining Ionic Charges• Based on periodic table location
• Atoms are more stable with optimum number of electrons in their outer orbits (usually 8)
• They can take in electrons to reach this # or lose some to make their next inner orbit full
Outer e- 1 2 3 4 5 6 7 8
Charge +1 +2 +3 +/-4 -3 -2 -1 0
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Nomenclature (“Naming”)• Binary (type I) Ionic compounds:
Cation keeps name, Anion has –ide endingSodium + Chlorine = (NaCl)
( )
Na + Cl2 NaCl
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• Binary (type II) Ionic compounds:
If cation has more than one positive state (some transition metals, see table 2.4) then must use roman numeral to show actual charge
Iron + oxygen = (FeO)
Iron + oxygen = (Fe2O3) Fe + O2 FeO
Fe + O2 Fe2O3
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If anion has more than one atom in it (polyatomic ion), it has a special ending other than –ide (see table 2.5)
Mg(OH)2 =
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• Binary (Type III) Covalent Compounds:Same rules as type I but need prefixes to indicate how many atoms of each
C2H2 =
CO2 = (“Mono” never precedes first atom)
Mono, Di, Tri, Tetra, Penta, Hexa, Hepta, Octa, Nona, Deca
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• Acid Names:
Acids usually preceded by Hydrogen
Acid names depend on anion ending
1. Ending “-ide” Hydro _anion prefix_ ic Acid
Ex. HCl =
2. Ending “-ate” Anion prefix ic Acid
Ex. H2SO4 =
3. Ending “-ite” Anion prefix ous Acid
Ex. H2SO3 =