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CHEM 14203 > LO 11 - 21 > Flashcards

LO 11 - 21 Flashcards

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1
Q

Equation to calculate energy added to increase heat

A

q = m ⋅ Cs ⋅ Δ T
- m is mass
- Cs is specific heat

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2
Q

Equation to calculate energy added to change state

A

q = n ΔH (state change)
- n is mols
- either ΔH fusion, vaporization

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3
Q

You can tell what state is denser on a phase diagram based on the …

A

lean of the fusion curve; the state the curve leans TOWARDS is less dense

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4
Q

What are the three sub-groups of crystalline solids?

A

Molecular, ionic, and atomic

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5
Q

Solid with molecules as the composite units held together by the associated IMFS?

A

Molecular solids

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6
Q

Molecular solids have ____ melting points

A

low

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7
Q

Solid with ions as the units that are held together by strong coulombic bonds?

A

Ionic solids

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8
Q

Ionic solids have ____ melting points

A

high

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9
Q

Solid composed of individual atoms?

A

Atomic solids

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10
Q

_________ atomic solids are held together by weak LDF and pack tightly to maximize interactions?

A

Nonbonding

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11
Q

________ atomic solids are held together by metallic bonds contributing to the e sea

A

Metallic

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12
Q

_______ _________ atomic solids are held together by covalent bonds in geometric structures

A

Network Covalent

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13
Q

Nonbonding AS have ___ melting points
Metallic AS have ____ melting points
Network Covalent AS have ___ melting points

A

low, variable, high

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14
Q

What are allotropes

A

forms of the same element in different arrangements. i.e. graphite or diamond

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15
Q

Long chains-like molecules composed of repeating monomers

A

Polymers

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16
Q

Monomer A + Monomer B = _______

A

Dimer

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17
Q

Condensation polymers ______ atoms or small groups during polymerization

A

eliminate

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18
Q

Addition polymers _____ _______ without elimination

A

link together

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19
Q

The amount of a substance that will dissolve in a given amount of solvent

A

solubility

20
Q

solvent-solute > = solvent-solvent AND solute-solute interactions

A

solution generally forms

21
Q

solvent-solute < solvent-solvent and solute-solute interactions

A

solution may or may not form

22
Q

When two substances are soluble in each other in all proportions they are _____

A

miscible

23
Q

The energy to separate solute particles (ΔH solute) and solvent particles (ΔH solvent) from each other is always ______

A

endothermic, ΔH > 0

24
Q

Mixing the solute and solvent (ΔH mix) is an _________ process

A

exothermic, ΔH < 0

25
Q

What is Hess’s Law

A

The enthalpy change of solution is the sum of its formation steps:
ΔH solution = ΔH solute + ΔH solvent + ΔH mix

26
Q

For ionic compounds dissolved in water, ΔH solvent and ΔH mix are combined into one term called _______

A

heat of hydration (ΔH hydration)

27
Q

heat of hydration is always ______

A

exothermic

28
Q

For ionic compounds, ΔH solute = ______

A

-ΔH lattice

29
Q

Soulutions reach dynamic equilibrium when ______

A

rates of dissolution = recrystallization

30
Q

_________ solutions have dynamic equilibrium between dissolved and undissolved solute

A

saturated

31
Q

A solution containing less solute than equilibrium is _______

A

unsaturated

32
Q

A highly unstable solution containing more solute than equilibrium is ______

A

supersaturated

33
Q

The solubility of solids in water
______ with increasing temperature

A

↑ increases

34
Q

The solubility of gasses in water
____ with increasing temperature
____ with increasing pressure

A

↓ decreases
↑ increases

35
Q

Henry’s Law

A

Solubility gas = Kh ⋅ P gas
- Kh is a constant
- P gas = P total ⋅ mol fraction gas

36
Q

Properties that depend on the number of particles dissolved in solution

A

colligative properties

37
Q

The VP of a nonvolatile nonelectrolyte + solvent is ____ the VP of pure solvent

A

less than

38
Q

Raoult’s Law for the VP of a solution

A

P solution = X solvent ⋅ P solvent ( ⋅ i)
- X mol fraction
- VP pure solvent
- Van Hoff factor if electrolyte

39
Q

What is Raoult’s Law for two gasses?

A

P total = Pa + Pb
Pa = Xa ⋅ P pure a
Pb = Xb ⋅ P pure b

40
Q

Strong solute-solvent interactions in gasses cause a _______ deviation from Raoult’s Law

A

negative

41
Q

Weak solute-solvent interactions in gasses cause a _______ deviation from Raoult’s Law

A

positive

42
Q

The freezing point of a solution containing a nonvolatile solute is ____ than the freezing point of pure solvent

A

lower

43
Q

Equation for freezing point depression

A

ΔTf = m ⋅ Kf
- ΔTf change in C relative to pure solvent
- m is molality
- Kf constant for solvent

44
Q

The boiling point of a solution containing a nonvolatile solute is _____ than the boiling point of pure solvent

A

higher

45
Q

Equation for boiling point elevation

A

ΔTb = m ⋅ Kb
- ΔTb change in C relative to pure solvent
- m is molality
- Kb constant for solvent

46
Q

The pressure needed to stop osmotic flow

A

osmotic pressure

47
Q

Equation for osmotic pressure

A

Π = M ⋅ R ⋅ T
- Π is osmotic pressure
- M is molarity
- R gas constant = 0.08206
- T in Kelvin

CHEM 14203 (18 decks)

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