finals Flashcards
(88 cards)
1
Q
gases tend to have ___
A
low molecular weight
2
Q
pressure is the same no matter the ____
A
element
3
Q
1 atm = ___ mm Hg = ___ torr = ___ Pa = ___psi
A
760 mm Hg, 760 torr, 1.01325 x 10^5 Pa, 14.70 Psi
4
Q
manometer measure the pressure of _____
A
gas
5
Q
open ended manometer = ___ , closed ended =___
A
compare to 1 atm (760 mm Hg), compare to 0 mm Hg
6
Q
boyles law
A
volume is inversely proportional to pressure V= 1/p
7
Q
boyles law math
A
P1V1=P2V2
8
Q
Charles law
A
temp is proportional to volume
9
Q
Charles law math
A
V1/T1 = V2/T2
10
Q
Combined gas law
A
(P1V1)/T1 = (P2T2)/T2
11
Q
Gay-Lussac’s law
A
temp goes down, pressure goes down
12
Q
Gay-Lussac’s math
A
P1/T1 = P2/T1
13
Q
avogandros law
A
volume is proportional to moles at STP
14
Q
ideal gas law
A
Volume is proportional to (moles*temp)/pressure
15
Q
ideal gas law math
A
PV=nRT
16
Q
R in ideal gas law
A
0.08206 (Latm)/(molK)
17
Q
density version of PV=nRT
A
m/V=MP/RT (M=molarity)
18
Q
Daltons law of partial pressures
A
IT DOESNT MATTER THE WEIGHT PRESSURE WILL ALWAYS BE THE SAME FOR EACH PARTICLE Ptotal = P1 + p2 + p3 + p4 +……
19
Q
mole fraction for gases
A
P1/Pt = (N1RT/V)/(ntRT/V) = N1/Nt
20
Q
mole fraction
A
mole of particular gas/total moles of all gas
21
Q
pressure ratio = _______
A
= mole ratio
22
Q
kinetic molecular theory (5)
A
- gases are in continuous motion
- The volume of the molecules is negligible relative to the total volume in which the gas is contained (FALSE)
- there are no attractive and repulsive forces (FALSE)
- energy can be transferred between molecules during collisions, but average energy does not change.
- the average kinetic energy is proportional to the absolute temperature
23
Q
average kinetic energy equation
A
KE=1/2mv^2
24
Q
lighter gases move ____ and have greater _____ of speed and heavier move ____ and haver less ____ of speed
A
faster, distribution, slower, distribution
25
learn about most probable speed, root speed and the other one
on it
26
u(rms) equation (average kinetic energy of gas)
square root of 3RT/M
27
R in average kinetic energy of gas
= 8.314 J/mol*K = (kg*m^2/S^2)/mole*K
28
effusion
escape of gas molecules through a tiny hole into an evactauted space (leaky air tank)
29
diffusion
gas spreads throughout a space (like febreeze)
30
mean free path
average distance a gas travels before a collision (pressure increases, distance decreases)
31
rate of effusion is related to ____
collision rate
32
Grahams law
R1/R2= square root of Mass2/Mass1 (compares the rate that gases effuse)
33
deviations from ideal gas happens when _____ and ____
theres high and low pressure
34
at low temp, you move ____ and have to deal with _____ forces
slower, attractive
35
van der Waal's equation for real gases
(P + (n^2a)/V^2)*(V - nb) = nRT
36
Kinetic molecular theory (KMT) breaks down at ____
high and low pressures
37
large a in van der Waals=
strong intermolecular forces
38
large b in van der waals =
larger particle size
39
b term breaks down _____ in KMT
the second postulate (gas got no volume)
40
a term breaks down ____ in KMT
the third postulate (intermolular forces dont exist nerd)
41
what determines matter's state?
KE (avg) vs Intermolecular forces (IMFs)
42
liquid has equal ___ and ____
KE and intermolecular forces (almost equal)
43
gas has more _____ than ____
KE than IMFS
44
solid has more _____ than ____
IMFs than KE
45
vander waals paremeters
b = size a =attraction
46
intramolecular forces vs intermolecular forces
intra = in the same molecule inter = inbetween many molecules
47
intermolecular forces we care about (4)
1. dispersion forces (london dispersion force)
2. dipole-dipole interactions
3. hydrogen bonding
4. ion-dipole interactions
48
(london) dispersion force (LDFs)
(surface area) instantaneous dipoles lead to attractions between atoms because one electrical imbalance leads to another. MORE surface area MORE LDFs
49
Dipole-dipole interactions
all molecules have to be polar, positives line up with negatives and higher numbers leads to higher boiling point (bp).
50
hydrogen bonding
when hydrogen bonds to N, O, or F, and another N, O, or F bonds to the hydrogen (with a lone pair) since the hydrogen has so much unequal positive charge due to the unequal electronegativity. STRONGEST IMF you gonna get
51
hydrogen bond is ~ _______ of a covalent bond
5-15%
52
in order to h bond, _____
must have a N,O,F bonded directly to a H
53
as molar mass goes up, _____
imf goes up due to LDFs (ignoring hydrogen bonding anomaly)
54
to hydrogen bond, you need a ____
lone pair
55
tendency for the electron cloud to distort
polarizability
56
factors of polarizability
1. number of electrons
2. size of atoms
3. shape of molecules
57
molar mass leads to ____ which leads to ___ which leads to _____ thus ______
more electrons, more LDFs, more IMFs, higher boiling point
58
weaking to strongest forces
LDFs, Dipole-dipole, hydrogen bonding
59
Ion-dipole interactions
basically hydrogen bonding but with ions. requires high polar solvent.
60
low lattice energy leads to _____
easier ion-dipole dissolving
61
every molecule expierences ______
LDFs (dispersion forces)
62
viscosity =
the resistance to flow
63
higher IMF = ______ in fluids
Higher viscosity
64
surface tension
guys near the surface of water are more densely packed than guys at the bottom due to IMFs pulling the surface downward.
65
Cohesion
IMF's that bond a material to itself (water to water)
66
adhesion
IMF's that bond a material to other materials (water to a towel)
67
capillary action
basically using stronger IMF's to move liquids like water. can be done in reverse like in mercury
68
why do we have a menescus in water?
because waters adhesive force to glass is stronger than its cohesive force to itself
69
vapor pressure
the pressure vapor exerts at equilibrium
70
boiling point
temperature at which the vapor pressure becomes more powerful than the surrounding pressure.
71
in order to escape the liquid phase, you need to overcome _____
IMFs
72
normal boiling point
the boiling point at 1 atm for a liquid
73
lower vapor pressure for chemicals with _____
higher IMFs
74
volatile
evaporate easily
75
critical point
the point where you go past the normal graph and become supercritical
75
triple point
where you are all three phases at once
76
supercritical fluids
behaves kinda like a fluid and a gas at the same time
77
memorize and draw phase diagram in slides
oki
78
crystalline
highly ordered
79
amorphous
lack of order
80
metallic solids
held together by a "sea" of electrons, not brittle (metals)
81
Ionic Solids
salts, cations and anions bonded together, brittle DO NOT CONDUCT ELECTRICITY AS A SOLID
82
covalent-network solids
diamond, SUPER strong,
83
molecular solids
held together with IMFs, not very strong, WEAKEST
84
memorize the solids slide
oki doki
85
polymers
long chains of covalent bonds
86
nanomaterials
crystalline compounds the sizer of 1-100 nm
87
