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