Chemistry Unit 2 Study Guide
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Last updated 10:26 PM on 11/14/22
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52 Terms
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Zinc
Zn⁺²
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Silver
Ag⁺
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Cadmium
Cd⁺²
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Nitrate
NO₃⁻
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Carbonate
CO₃⁻²
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Sulfate
SO₄⁻²
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Phosphate
PO₄⁻³
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Ammonium
NH₄⁺
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Cyanide
CN⁻
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Hydroxide
OH⁻
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Chlorate
ClO₃⁻
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Hypochlorite
ClO⁻
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Perchlorate
ClO₄⁻
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Chlorite
ClO₂⁻
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Phosphite
PO₃⁻³
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Sulfite
SO₃⁻²
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Carbonite
CO₂⁻²
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Nitrite
NO₂⁻
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Group 1A
Alkali metals
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Group 2A
Alkaline earth metals
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Group 7A
Halogens
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Group 8A
Noble gases
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valence electrons
outermost electrons that participate in chemical reactions
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ion
atom with a charge
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cation
positive ion
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anion
negative ion
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ionic compounds
transfer of electrons from metal to non-metal
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covalent compounds
sharing of electrons between non-metals
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-ous
"smaller"
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-ic
"larger"
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acids
formula starts with H
no charge
no charge
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binary
two elements
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ternary
three elements
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binary acids
begin with hydro-
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ternary acids/oxyacids
no hydro-, 'ate - 'ous, 'ite - 'ic
must be an O-H bond
must be an O-H bond
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mono
1
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di
2
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tri
3
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tetra
4
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penta
5
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hexa
6
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hepta
7
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octa
8
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nona
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deca
10
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VSB table
valence (add negative charge, subtract positive), shared (subtract negative charge, add positive), bonds (shared/2)
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electronegativity
ability of an atom to attract electrons
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electronegativity increases
as you go right and up
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most electronegative atoms:
1. Fluorine
2. Oxygen
3. nitrogen/chlorine
2. Oxygen
3. nitrogen/chlorine
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pure ionic
ionic bond, electronegativity difference ≥ 2.0
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polar covalent
most covalent bonds, partial charges indicated by δ symbol
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pure covalent
identical electronegativities
Note 
Flashcards (49)