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AP Chem > Unit 3 > Flashcards

Unit 3 Flashcards

1
Q

IMFs

A

forces between two or more different molecules

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2
Q

IMFs vs. bonds (strength)

A

not nearly as strong

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3
Q

IMFs determine

A

boiling points, melting points, viscosity, surface tension, and capillary action

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4
Q

polar vs nonpolar

A

nonpolar molecules have both elemental and geometrical symmetry

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5
Q

dipole

A

a partially positive end of a molecule is attracted to the partially negative end of a different molecule

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6
Q

dipole-dipole

A

polar to polar
more polar, greater attraction
permanent dipole

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7
Q

LDFs

A

occur in all substances
only IMF in nonpolar molecules
temporary dipole
weak
more surface area –> stronger

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8
Q

to compare strength of IMFs

A

must be of comparable size

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9
Q

hydrogen bonding

A

special dipole-dipole
STRONG
polar molecules with H-N, H-O, or H-F

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10
Q

ion-dipole

A

an ion with something polar
stronger

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11
Q

if there is ion-dipole or hydrogen bonding

A

there will not be dipole-dopole

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12
Q

weakest to strongest IMFs

A

LDFs, dipole-dipole, hydrogen bonding, ion-dipole

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13
Q

network covalent

A

SiO2, SiC, C (graphite and diamonds)

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14
Q

dipole-dipole bp

A

~equal mass and size, more polar, higher bp

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15
Q

viscosity

A

resistance of a liquid to flow (honey)
increases with IMF strength
decreases with temp

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16
Q

cohesion

A

IMFs that bond w themselves

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17
Q

adhesion

A

IMFs that bond with a surface

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18
Q

capillary action

A

rise of liquids up narrow tubes
adhesive forces –> wall (water)
cohesive forces –> itself (mercury)
better capillary, stronger IMFs

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19
Q

surface tension

A

stronger IMFs, greater surface tension

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20
Q

ionic solids

A

sets of cations and anions mutually attracted (electrostatic) to one another
metal nonmetal
think salt
lattice composed of alternately charged ions
small ions (ions w higher charges) will have stronger attractions
high bp and mp, crystals, brittle, dissolve in water, strong

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21
Q

metallic solids

A

sea of shared electrons
metal metal
thing mg ribbon
high mp and bp
conductive, ductile, malleable, strong

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22
Q

covalent-network solids

A

joined by extensive network of covalent bonds in pattern
only in nonmetals
high mp and bp
hard
do not dissolve
strong
think diamonds

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23
Q

molecular solids

A

held by week forces
nonmetal nonmetal
think water
low melting point, don’t conduct, weak

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24
Q

solid

A

low ke, little space, fixed volume and shape, cannot be compressed

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25
Q

liquids

A

close together, higher ke, take shape of container, cannot be compressed

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26
Q

gas

A

highest ke, far apart, easily compressed, take shape of container, no regular arrangement of particles

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27
Q

gas law

A

p1v1/t1n1=p2v2/t2n2

28
Q

to find p of gas collected over water

A

subtract pressure of water vapor from total pressure

29
Q

the lower the molar mass

A

the faster the molecule

30
Q

real gasses do not behave ideally when…

A

at high pressures and low temperatures
volume of particles and intermolecular attractions are now significant

31
Q

strength of dispersion forces tends to

A

increase with molecular weight

32
Q

homogeneous mixtures are made up of…

A

a solute and solvent that can be liquids, gases, or solids

33
Q

solute

A

thing dissolved

34
Q

solvent

A

thing that dissolves

35
Q

molarity

A

moles/l = concentration

36
Q

mixing a solution

A

weigh out mass (moles) of solute, add it to volumetric flask, add solvent to line on neck of flask,

37
Q

diluting a solution

A

deliver volume of solution to volumetric flask, add solvent to line

38
Q

molarity of a new solution

A

m1v1=m2v2

39
Q

miscibility

A

ability of two substances to mix without separating
similar materials are miscible in each other

40
Q

polar solvents dissolve

A

polar and some ionic solutes
polar- molecules spread out with broken imfs
ionic- dissociate

41
Q

nonpolar solvents dissolve

A

nonpolar solutes

42
Q

in aqueous solutions

A

water molecules surround ions to dissolve them

43
Q

paper chromatography

A

more similar in polarity sample is to solvent, farther it travells

44
Q

thin layer chromatography

A

more polar, shorter distance
used with samples not colored to naked eye - uv (amino acids)

45
Q

column (method) chromatography

A

steel wool with gel in buret, mixture placed at top, flushed with nonpolar solvent
used more for separation than analysis
more polar, slower

46
Q

higher frequency

A

high energy

47
Q

spectroscopy

A

study how matter interacts with radiation

48
Q

transitional

A

movement of entire molecule (or electrons in molecule) from one place to another)

49
Q

vibrational

A

periodic motion of atoms within a molecule

50
Q

rotational

A

rotation of molecule about an axis

51
Q

microwave spectroscopy

A

rotational
lower in energy than visible light

52
Q

infrared spectroscopy

A

vibrational
higher in energy than microwaves, lower than visible light
lighter and stronger bonds, higher vibrational frequency

53
Q

ultraviolet (visible light) spectroscopy

A

transitions in energy levels
absorbing – high energy
measure light absorbed, determine concentration

54
Q

binding energy

A

energy involved in attraction between atom and electrons

55
Q

photoelectric effect

A

when light shines on surface of a metal, electrons can be ejected from surface

56
Q

best choice for wavelength

A

where absorbance close to 1

57
Q

beer-lambert law

A

absorbance = slope * path length (1) * concentration (M)

58
Q

soluble in water…

A

all sodium (Na), potassium (K), ammonium (NH4), nitrate (NO3) salts

59
Q

if imfs break strength rules

A

due to molar mass, more opporunities

60
Q

in order to dissolve

A

need strong attraction

61
Q

pv

A

indirect

62
Q

pt

A

direct

63
Q

tv

A

direct

64
Q

vn

A

direct

65
Q

do all gas molecules have the same speed?

A

No! Based on kinetic molecular theory, gas particles have a distribution of speeds that is dependent on the temperature, which is represented in diagram 2.

AP Chem (10 decks)

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