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34 Cards in this Set

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NH4(+), Group 1 Metals, C2H3O2(-), NO3-
Always Soluble
Ag+, Pb2+, Hg(2+), Hg2(2+)
Almost Never Soluble (Unless paired w/"always soluble"
Cl(-), Br(-), I(-), SO4(2-)
Usually Soluble
CO3(2-), PO4(3-), S(2-), OH(-)
Usually Insoluble
Switches Classification when paired with Ca(2+), Ba(2+), and Sr(2+)
OH(-) & SO4(2-)
Breaks Up 100% in Water
Strong Electrolyte
Weak Electrolyte
Breaks up partially in Water
Energy required to break apart and dissolve ions
Lattice Energy
Low Solubility results in a ___________ lattice energy
Higher
High charges usually result in _______ solubility
Low
An arrenius acid...
breaks up into H(+) ions in solution
An Arrenius base...
breaks up into OH(-) in solution
What are the 7 Strong Acids?
HCl, HBr, HI, HNO3, HCLO3, HCLO4, H2SO4
What are the strong bases?
Group 1 Hydroxides (except H); Group 2 Hydroxides (except Be, Mg)
Amphiteric substance can...
Act as an acid or a base (HSO4)
A Bronsted Acid is...
a proton donor H(+)
A Bronsted Base is....
a proton acceptor H(+)
A Lewis acid is...
an electron pair acceptor
A Lewis base is...
an electron pair donor
What is electronegativity?
A measure of how much an atom wants electrons
Metals =
Low Electronegativity
Non-Metals =
High Electronegativity
Rank in order of Electronegativity: O, Cl, F
1= F
2= O
3= Cl
Oxidizing Agent =
Gains electrons
Reducing Agent =
Gives Electrons
>1 Molar ...
Concentrated
< 1 Molar ...
Dilute
q = heat flow = c(s)* m * delta(T)
Delta H = q
Exothermic...
when Delta H < 0
Endothermic...
when Delta H > 0
1 C =
1 k cal = 10^3 cal
Hesse's Law
DH1 + DH2 => DH3
Specific Heat H2O ...
4.184J/g*C
Principle Quantum numbers
n = 1, n = 2, n= 3, etc...