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Chem 1B Final Flashcards

1
Q

°F –> °C

A

1.8*°C +32

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2
Q

Molecular solid (ex & properties)

A

ice
discrete, identifiable molecules, non-covalent weak IMF; intraMF> interMF, low MP

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2
Q

Network solid (ex & properties)

A

BN, SiO2 (sand/quartz), diamond
repeated covalent bonds, nonconductors, break not bend, High MP

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2
Q

Metallic solid (ex & properties)

A

copper, gold, silver, iron
conduct elect., sea of e-, bend under stress, reflect light, high MP

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3
Q

Ionic solid (ex & properties)

A

salts eg. NaCl
discrete ions (cations/anions), strong attraction, brittle, highest MP, conduct e- when molten

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4
Q

Lattice Energy

A

larger ionic charge–> more negative (Exothermic)
smaller ionic size–> more negative (exothermic)

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5
Q

Kinetic Theory of Gases

A

1) particles separated by molecular distance (Untrue @ high pressure; P=0)
2) particles move + collide randomly
3) no attractive or repulsive forces *untrue
4) KE: T (w/o outside forces)

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6
Q

Boyle’s Law

A

When you decrease the Pressure, the Volume increases
P decreases, V increases at a constant T (PV=T)

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7
Q

Dalton’s Law

A

Partial Pressure (Ptotal= P1+P2…)

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8
Q

Partial Pressure Equation

A

P1V1/Ptotal

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9
Q

Charle’s Law

A

When you increase the temperature, the volume increases
T:V (area on the graph =)

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10
Q

Avogadro’s Law

A

When you increase the number of moles, the volume increases
n:V

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11
Q

Ideal Gas Law

A

PV=nRT

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12
Q

Combined Gas Law

A

P1V1/n1T1= P2V2/n2T2

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13
Q

Maxwell Distribution of Speed

A

Large/heavier molecules move slower

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14
Q

Diffusion

A

spread to homostasis

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15
Q

Effusion

A

occurs w/in a pinhole, smallest and fastest particles escape first
eg. smaller/faster = higher effusion rate

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16
Q

Raoult’s Law

A

Total Pressure= molespressure+molepressure
*Ideal=1

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17
Q

mole fraction

A

molesx/total moles

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18
Q

molarity

A

moles solute/L solvent

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19
Q

molality

A

moles solute/kg solvent

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20
Q

Colligative Properties

A

change in the properties of a pure solvent based on the number, not the kind

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21
Q

What happens to Vapor Pressure when you add a solute?

A

Decreases because the solute blocks the evaporation of the solvent

22
Q

What happens to Boiling Point when you add a solute?

A

Increases because it requires more energy to evaporate

23
What happens to Freezing Point when you add a solute?
Decreases because solute interferes with the lattice (requires lower temps to freeze)
24
If both enthalpy and entropy are positive what T will make the reaction spontaneous?
Higher temperatures
25
If both enthalpy and entropy are negative what T will make the reaction spontaneous?
Low temperatures
26
Henry's Law
Sgas=KhPgas solubility of gas= Henry's Constant* Pressure
27
Immiscible solutions are..
NOT IDEAL SOLUTIONS
28
simple cubic cell
1 atom/cell touch along the edge l=2r
29
body centered cubic
2 atoms/cell touch across diagonal (inside) l=4r/rad3
30
face centered cubic
4 atoms/cell touch along face l=rad8r
31
How big would a particle inside a scc be?
0.73*r
32
What percent atom is a scc?
52%
33
What percent atom is bcc?
68%
34
Larger charge difference between ions-->
STRONGER BOND
35
Smaller atomic size within an ion
STRONGER IMG/BOND
36
What are Van der Waals forces?
Londen dispersion < dipole dipole< hydrogen bonding
37
Where are Van der Waals forces found?
Noble Gases (group 8) and molecular solids
38
Low to high viscosity...
Increasing IMF
39
exergonic
energy of products < reactants --> evolution of energy
40
exothermic
energy is released into the surroundings
41
endogonic
energy is required to convert reactants to products
42
endothermic
heat energy is absorbed by the system
43
q (+)
endothermic (head added to the system)
44
q (-)
exothermic (heat lost from the system)
45
w (+)
work is done by the system
46
w (-)
work is done on the system
47
When T decreases is the reaction endo/exothermic?
Endothermic (T gets absorbed by the reaction)--> T drops
48
Hproducts> Hreactants
+; endothermic
49
Hproducts
-; exothermic
50
deltaH = +
endothermic
51
deltaH = -
exothermic
52
deltaSurr=
- deltaH/T
53
combustion
oxygen is ALWAYS a reactant
54

Chem (3 decks)

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