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Chem > Chem 1B Final > Flashcards

Chem 1B Final Flashcards

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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
Q

What happens to Freezing Point when you add a solute?

A

Decreases because solute interferes with the lattice (requires lower temps to freeze)

24
Q

If both enthalpy and entropy are positive what T will make the reaction spontaneous?

A

Higher temperatures

25
Q

If both enthalpy and entropy are negative what T will make the reaction spontaneous?

A

Low temperatures

26
Q

Henry’s Law

A

Sgas=KhPgas
solubility of gas= Henry’s Constant* Pressure

27
Q

Immiscible solutions are..

A

NOT IDEAL SOLUTIONS

28
Q

simple cubic cell

A

1 atom/cell
touch along the edge
l=2r

29
Q

body centered cubic

A

2 atoms/cell
touch across diagonal (inside)
l=4r/rad3

30
Q

face centered cubic

A

4 atoms/cell
touch along face
l=rad8r

31
Q

How big would a particle inside a scc be?

A

0.73*r

32
Q

What percent atom is a scc?

A

52%

33
Q

What percent atom is bcc?

A

68%

34
Q

Larger charge difference between ions–>

A

STRONGER BOND

35
Q

Smaller atomic size within an ion

A

STRONGER IMG/BOND

36
Q

What are Van der Waals forces?

A

Londen dispersion < dipole dipole< hydrogen bonding

37
Q

Where are Van der Waals forces found?

A

Noble Gases (group 8) and molecular solids

38
Q

Low to high viscosity…

A

Increasing IMF

39
Q

exergonic

A

energy of products < reactants –> evolution of energy

40
Q

exothermic

A

energy is released into the surroundings

41
Q

endogonic

A

energy is required to convert reactants to products

42
Q

endothermic

A

heat energy is absorbed by the system

43
Q

q (+)

A

endothermic (head added to the system)

44
Q

q (-)

A

exothermic (heat lost from the system)

45
Q

w (+)

A

work is done by the system

46
Q

w (-)

A

work is done on the system

47
Q

When T decreases is the reaction endo/exothermic?

A

Endothermic (T gets absorbed by the reaction)–> T drops

48
Q

Hproducts> Hreactants

A

+; endothermic

49
Q

Hproducts<Hreactants

A

-; exothermic

50
Q

deltaH = +

A

endothermic

51
Q

deltaH = -

A

exothermic

52
Q

deltaSurr=

A
  • deltaH/T
53
Q

combustion

A

oxygen is ALWAYS a reactant

54
Q
A

Chem (2 decks)

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