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Sophomore- Spring 2024- Mac > CHem 111- Test 4- St. Thomas > Flashcards

CHem 111- Test 4- St. Thomas Flashcards

1
Q

Atm–> torr–>psi

A

1.00 atm=760.0 torr= 14.7 psi

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2
Q

Ideal gas law

A

PV=nRT

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3
Q

what is R

A

0.08206 atm L/mol K

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4
Q

STP

A

298K and 1.00 atm

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5
Q

density (normal)

A

= Mass/volume

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6
Q

mass=

A

= moles x molar mass

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7
Q

density (special)

A

d= n x MM/nRT =P x MM/RT

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8
Q

kinetic energy, constant temp

A

massive objects have lower average velocity

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9
Q

kinetic energy (higher temperature)

A

objects have higher average velocity

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10
Q

larger or more polar (kinetic energy)

A

they are sticker molecules and deviate from normal behavior

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11
Q

another name for bonds

A

intrAmolecular forces,, hold atoms together

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12
Q

inter molecular forces

A

hold molecules together

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13
Q

3 types of intermolecular forces

A

london (dispersion) forces, dipole dipole forces, hydrogen bonding

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14
Q

london (dispersion) forces

A
  • between nonpolar molecules
  • increase in streath with greater mass
  • form temporary dipole
  • weaker for smaller molecules
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15
Q

dipole-dipole forces

A
  • between polar molecules
  • increase in strength with greater polarity
  • form from permanent dipole
  • intermediate strength
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16
Q

hydrogen bonding

A
  • between polar molecules with H bonded to O, N or F
  • More H-bonds make a stronger force
  • Strongest IMF for molecultes of a smililar size
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17
Q

surface tension and viscosity

A

imcrease with increasing IMF strength

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18
Q

boiling point

A

the temperature where the vapor pressure = atmospheric pressure

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19
Q

Lower IMF means that…

A
  • it is easier to separate molecules into gas phase
  • there is a lower boiling point
  • there is a higher vapor pressure
20
Q

Change in Hvap

A

energy required to vaporize given amount of liquid into gas

21
Q

total heat required equation

A

MCsΔT + ΔHfusn + MClΔT + ΔHvapn+M*CgΔT

M= mass, n = moles

22
Q

boiling point is at what pressure

A

1 atm

23
Q

crystalline

A

ordered, ionic and some covalent

24
Q

amorphous

A

not ordered, mostly covalent

25
Q

how are solids held together?

A
  • Ionic solids
  • Metallic solids
  • Molecular solids
  • network solids
26
Q

ionic solid

A

held by ionic bonds

27
Q

metallic solids

A

held by metallic bonds

28
Q

molecular solid

A

held by IMFs- covalent molecultes (this is strong but weaker than covalent or ionic BONDS)

29
Q

network solids

A

held by covalent bonds

30
Q

melting point of a molecular solid is ____ than ionic or network

A

lower

31
Q

properties of metal

A

malleable (bendable) and conduct electricity

32
Q

what type of solid is diamon

A

network solid

33
Q

why do solutions form?

A

when energy of solution < energy of solute and solvent

when energy of forces holding solvent + solute together < energy of forces holding together solute and solvent individually

34
Q

IMFs (this time, 6 of them)

A
  1. london forces
  2. dipole dipole
  3. h bonding
  4. ion dipole
  5. ion induced dipole
  6. dipole induced dipole
35
Q

ion dipole

A

strong force between an ion and a polar molecule

36
Q

ion- induced dipole

A

force between ion and non-polar molecule

37
Q

dipole-induced dipole

A

force between polar molecule and non-polar molecule

38
Q

what does like dissolves like mean

A

solutes will mostly dissolve in solvents that have same IMF acting on them (also salts (ionic) dissolve in H2O)

39
Q

electrolytes

A

solutions containing ions (conduct electricity)

40
Q

stong electrolytes

A

completely breaks apart to form ions when dissolved- forms strongly conductive solutions (ionic compounds + strong acids)

41
Q

weak electrolytes

A

partially breaks apart ti firn uibs wgeb dussikved- frs weakly conductive (weak acids + bases)

42
Q

non-electrolytes

A

does not form ions when dissolved- non conducting solutions (soluable covalent compounds)

43
Q

soluability of gases in water (temp)

A

higher temp= less gas dissolved

44
Q

soluability of gases in water (pressure)

A

higher pressure= more gas dissolved

45
Q

when are molecules stickier?

A

when they are larger or more polar

46
Q

rate of diffusion

A

the square root thing

47
Q

when will a gas behave most like an ideal gas?

A

at HIGH temp and LOW pressure

Sophomore- Spring 2024- Mac (11 decks)

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