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ACETATE
C_{2}H_{3}O_{2}^{}









find wavelength when electron jups energy level:
λ=hc/(R(n_{1}^{2}n_{2}^{2})

λ=hc/(R(n_{1}^{2}n_{2}^{2})

wavelength when given speed and mass
E=h/m_{(kg)}*v_{(m/s)}

Quantom numbers:
~n
N= integers 1,2,3...

quantom numbers:
~L
0,1,2,3,...,(n1)






plancks constant
6.626x10^{34}


e=
(with h and v)
h*v=hc/λ

quantom numbers
~m_{l}
l...0...+l

quantom numbers
~m_{s}
+1/2 or 1/2

Bornhaber cycle
ΔH_{f}=ΔH_{1}+ΔH_{2}+ΔH_{3}+ΔH_{4}+ΔH_{5}

elecronegativity trends
 increase:
 ^>
 F has highest elecrtonegativity

formal charge
fc=
valence e^{}lone pair e^{}1/2 bonding e^{}

ΔH_{rxn}
Σ(ΔH _{breaking bonds})+Σ(ΔH _{forming bonds})

Molecular geometry:
2 groups
 Linear
 180^{o}
 Hybrid: 2sp

molecular geometry:
3 groups
 trigonal planer
 120^{o}
 Hybrid: 3sp^{2}

molecular geometry
4 groups
 tetrahedral
 109.5^{o}
 Hybrid: 4sp^{3}
 ^{}

molecular Goemetry
5 groups
 trigonal bipyramidal
 90^{o} and 120^{o}
 Hybrid: 5sp^{3}d
 ^{}

molecular geometry
6 groups
 Octahedral
 90^{o}
 Hybrid: 6sp^{3}d^{2}
 ^{}

CH_{3 }will always have what molecular geometry?
tetrahedral

Molecular geometry:
~effect of lone pairs:
occupy more space, affect polarity and geometry (2 bonded legs and 2 lone pairs will make BENT)

Hybrid orbitals
#legs=2
2sp

Hybrid orbitals
#legs=3
3sp^{2}

Hybrid orbitals
#legs=4
4sp^{3}

Hybrid orbitals
#legs=5
5sp^{3}d

Hybrid orbitals
#legs=6
6sp^{3}d^{2}

all _____ bonds are sigma bonds
single

The first of each multiple bonds are ____ bonds, then the rest are ___ bonds
Sigma, Pi

Sigma bonds DO NOT exist in which type of overlap?
a) ss
b) sd
c) sp
d) pp end
e) shybrid
f) hybridhybrid
B

