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valence electrons
- electrons in the outermost shell
- group # on periodic table
- noble gases have complete octet of 8 (except He - 2)
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Lewis Structure
valence electrons represented as dots around elemental symbol
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Octet Rule
atoms will gain/lose electrons to achieve 8 outer electrons
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simple ion
atom that has acquired a net +/- charge by losing/gaining one or more electrons
- Na -> Na+ + e-
- Sodium (11 e-) = sodium ion (10 e-) + 1 e-
- Cl + e- -> Cl-
- Chlorine (17 e-)+ 1 e- = chloride (18 e-)
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Cation Names
"element" ion
sodium ion, magnesium ion
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Transition Metal Ions
can form more than one positive ion
- Cu -> 1+ 2+
- Fe -> 2+ 3+
- Sn -> 2+ 4+
- Pb -> 2+ 4+
- Ag -> 1+
- Zn -> 2+
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Transition Metal Stock Names
element name with roman numeral charge in parenthesis
- Fe2+: iron (II) ion
- Fe3+: iron (III) ion
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Transition Metals -ic/-ous Names
- -ic for higher charge
- -ous for lower charge
- Fe2+: ferrous
- Fe3+: ferric
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Transition Metal Stems
- copper: cupr
- iron: ferr
- tin: stann
- lead: plumb
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Anion Names
"stem-ide" ion
chloride ion, phosphide ion
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chemical bond
attractive force that holds atoms together in molecules and ions together in crystals
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ionic bond
chemical bond that holds together + charged ion (metal) and - charged ion (non-metal)
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ionic compound
- substance formed when ionic bonds form
- named using metal (cation) then nonmetal (anion)
- neutral - overall charge is zero
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salt
ionic compound containing any cation except H+ and any anion except OH-
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binary ionic compound
ionic compound formed by a cation and an anion
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Binary Ionic Compound Names
name of metal + stem of nonmetal-ide
sodium chloride, aluminum bromide
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polyatomic ions
- cluster of 2 or more atoms with overall chargeonly 1 polyatomic cation - NH4+ (ammonium)
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-ate vs -ite
polyatomic ions that contain oxygen atoms
- -ate: more O atoms (SO42- - sulfate)
- -ite: less O atoms (SO32- - sulfite)
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bi-
prefix for hyrdrogen (does not mean 2)
bicarbonate: HCO3-
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oxyanion
- polyatomic ion that contains oxygen
- can contain a different number of oxygen atoms
- perchlorate: ClO4-
- chlorate: ClO3-
- chlorite: ClO2-
- hypochlorite: ClO-
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covalent bond
- chemical bond where atoms share valence electrons
- 2 nonmetals
- can occur between identical atoms (O2) or different atoms (H2O)
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nonpolar covalent bond
- equal sharing of electrons
- occurs between same kind of atoms
H 2, Cl 2
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polar covalent bond
- unequal sharing of electrons
- occurs between atoms of different elements
HF, SO 3
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single bond
2 shared electrons
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double bond
4 shared electrons
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triple bond
6 shared electrons
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electronegativity
measure of the ability of an atom to attract shared electrons to itself in a covalent bond
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binary covalent compound
atoms of two non-metallic elements sharing valence electron pair(s)
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Binary Covalent Compound Naming
- use prefixes to indicate number of atoms in each element
- omit mono for first atom only
- CCl4 - carbon tetrachloride
- CO2 - carbon dioxide
- N2O3 - dintirogen trioxide
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Prefixes
- 1: mono
- 2: di
- 3: tri
- 4: tetra
- 5: penta
- 6: hexa
- 7: hepta
- 8: octa
- 9: nona
- 10: deca
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diatomic molecules of the same element
HI BrONClF
H, I, Br, O N, Cl, F
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acid
releases H+ ions when dissolved in water
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strong acid
- completely ionizes in water
- conducts electricity
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weak acid
only a small amount ionizes in water
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