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_H (-)
Exothermic, favorable, only spontaneous at LOW t
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_H (+)
Endothermic, unfavorable, NONspontaneous at LOW T
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_S (+)
More disorder, favorable, spontaneous at HIGH T
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_S(-)
Less disorder, unfavorable, NONspontaneous at HIGH T
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_Srxn=
?nSproducts -?nSreactants = J/K
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_S: if more moles of gas are in PRODUCTS
S increases
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_S: if more moles of gas are in REACTANTS
S decreases
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T-ct (crossover temperature)
(_Hrxn)/(_Srxn)
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if T-ct is (-)
there IS NO EQUILIBRIUM TEMPERATURE
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_Grxn = -RTln(K)
R=8.314(J/mol*k)
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Group 1A: O.N.
+1 in all compoiunds
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Group 2A: O.N.
+2 in all compounds
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Group 7A: O.N.
Usually -1 in all compounds, EXCEPT with Oxygen
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Hydrogen O.N.
+1 with nonmetals, -1 with metals and Boron
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Oxygen O.N.
-2 in most compounds, -1 in peroxides X2O2
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Leo the lion goes GER
loss of electrons is oxidation. gain of electrons is reduction
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oxidized then it
lost electrons, reducing agent
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reduced then it
gained electrons, oxidizing agent
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In acidic solutions, you will only be able to add:
H+ or H20
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To balance oxygen:
add 1 h20 to the side that needs the oxygen and 2H+s to the side that has enough oxygen atoms
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To balance hydrogen
add 1 H+ to the side that needs the hydrogen
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In basic solutions
convert remaining H+ to OH- by adding the same ammount of OH- to both sides
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Nonmetals oxides added to water
THEY FORM ACIDS (NO2)
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Metal oxides added to water
THEY FORM BASES (CaO)
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Nonmetal hydrides are
Covalent and act as acids in solution HF
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Accross period table -> nonmetal hydrice acid strength
increases because of an increase in electronegativity H20 < HF
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Down a group, nonmetal acid strength
increases because of an increase in size of anion HF < HCL
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nonmetal hydrides acidiity trend:
acid strength INCREASES from Left - Right & Top - Bottom; strongest nonmetal hydride compounds are bottom right of periodic table H2Se > PH3
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Metal Hydrides are
ionic and act as bases
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for metal cations,
the larger the charge, higher the acidity Al3+ > Mg2+
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if charge is similar
the smaller the cation the higher the acidity
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Oxyacid trends contain:
H, O, and a nonmetal
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Different number of oxygens in oxyacid trends:
the more oxygen, the more acidic
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Same number of oxygens in oxyacid trends:
depends on electronegativity, more electronegative, more acidic.
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Lewis acid
accept pair of electrons
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Lewis base
donate pair of electrons
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cations, multiple bonds, B, Be
can accept electrons, lewis acids
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NH3, H20, anions -
accept pair of electrons, lewis base
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