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14 Cards in this Set

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Network Covalent Bonds
C

ZnS

SiO2
rank bond strengths by melting point
dispersion
dipoledipole
h-bonding
= weak

metallic
= weak ---> strong

ionic bonds
covalent bonds
= strong
rank solids by melting point
SOLID M.P.
molecular low
metal low ---> high
ionic high
covalent high
Dalton's Atomic Theory - Part III
in a reaction, atoms don't change, they rearrange
First Law of Thermodynamics
ΔEuniv = 0

conservation of energy
To find the change in energy of a system:
ΔEsys = q + w
enthalpy
H

ΔH - change in enthalpy

**the amount of heat energy absorbed by a process that occurs at a constant pressure (-ΔH is the heat given off)
ENdothermic
heat ENters system
heat leaves surroundings (cool down)

**ABSORBES heat energy

(break bond)
EXothermic
heat EXits system
heat enters surroundings (heat up)

**gives off heat energy

(make bond)
ΔH =
H(final) - H(initial)

+ = endothermic
- = exothermic
entropy
*number of ways a system can be arranged

"S"


S(gas) >> S(liquid) > S(solid)
ΔS =
S(final) - S(initial)

look for:
**change of state
**few big molec. <--> many small molec.
**change in temp.
free energy change
ΔG

ΔG = ΔH - TΔS

if: then:
ΔG - spontaneous
ΔG + nonspontaneous

definition: energy available for a spont. process to do work; for a nonspont. process, it is the amount of energy that must be supplied to cause the process to occur.
spontaniety of:
- endothermic reactions
- exothermic reactions
Endothermic: (+)+(+)
- spont at high T
-nonspont at low T

Exothermic:(-)+(-)
-spont. at low T
-nonspont. at high T