CHEM beast mode > Properties > Flashcards

Properties Flashcards

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1
Q

When pressure increases, boiling point _________

A

Increase

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2
Q

When pressure increases, freezing point _________

A

Increase
Exception: Water

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3
Q

When pressure increases, melting point _________

A

Increase
Exception: Ice

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4
Q

What happens to the melting and boiling points when more solute is added to a solvent?

A

• Melting point decreases → Freezing Point Depression
• Boiling point increases → Boiling Point Elevation

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5
Q

Solid → Liquid:

A

Melting

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6
Q

Liquid → Solid:

A

Freezing

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7
Q

Liquid → Gas:

A

Evaporation / Vaporization/ Boiling

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8
Q

Gas → Liquid:

A

Condensation

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9
Q

Solid → Gas:

A

Sublimation

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10
Q

Gas → Solid:

A

Deposition

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11
Q

Gas → Plasma:

A

Ionization

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12
Q

Plasma → Gas:

A

Recombination / Deionization

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13
Q

What shape does water form in a glass (polar) tube, and why?

A

→ Concave meniscus

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14
Q

What shape does water form in a non-polar tube, and why?

A

→ Convex meniscus

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15
Q

What shape does mercury form in a glass (polar) tube, and why?

A

→ Convex meniscus

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16
Q

When does a liquid form a concave meniscus?

A

→ When adhesive forces are stronger than cohesive forces (e.g., water in glass).

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17
Q

When does a liquid form a convex meniscus?

A

→ When cohesive forces are stronger than adhesive forces

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18
Q

What is the relationship between surface tension and intermolecular forces (cohesive force)?

A

Directly proportional

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19
Q

What is viscosity?

A

The resistance to flow

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20
Q

Which is more viscous, honey or water?

A

Honey

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21
Q

How does temperature affect viscosity?

A

Lower temperature increases viscosity

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22
Q

Types of mixture

A

Homogenous
. No distinguishable components.
Heterogeneous
. Distinguishable components

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23
Q

Solution

A

A homogenous mixture of two substances

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24
Q

Colloid

A

A heterogenous mixture where particles do not settle

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25
Suspension
A heterogeneous mixture where particles are suspended in a liquid or gas and settle over time
26
What is solubility?
Solubility is the amount of solute that can be dissolved per volume of solvent
27
Factors affecting solubility
1. Molecular structure 2. Pressure (for gases only) 3. Temperature
28
Q: What happens to the solubility of a gas in a liquid when temperature increases?
A: It decreases.
29
Q: What happens to the solubility of a solid in a liquid when temperature increases?
A: It increases.
30
Q: What happens to the solubility of a liquid in a liquid when temperature increases?
A: It may increase if the liquids are partially miscible; completely miscible liquids are unaffected.
31
Q: What happens to the solubility of a gas in a liquid when pressure increases?
A: It increases.
32
Saturation point
A point where maximum solubility is reached It spends on temperature, chemical structure and pressure.
33
Q: What is the general rule for how solutes affect phase changes involving liquids?
A: If the change is toward liquid, it gets easier. If it’s away from liquid, it gets harder.
34
Q: How does adding solute affect freezing (liquid → solid)?
A: It gets harder (freezing point decreases).
35
Q: How does adding solute affect melting (solid → liquid)?
A: It gets easier (melts at a lower temperature).
36
Q: How does adding solute affect boiling (liquid → gas)?
A: It gets harder (boiling point increases).
37
Q: How does adding solute affect condensation (gas → liquid)?
A: It gets easier (condenses at a higher temperature).
38
Q: What does evaporation separate, and what type of mixture is it used for?
A: It separates a dissolved solid from a liquid in a homogeneous mixture by evaporating the liquid.
39
Q: What does distillation separate, and what is the requirement?
A: It separates liquid from liquid in a homogeneous mixture; the liquids must have different boiling points.
40
Q: What does filtration separate, and what type of mixture is it used for?
A: It separates an insoluble solid from a liquid in a heterogeneous mixture.
41
Q: What does chromatography separate, and what types of mixtures can it be used for?
A: It separates components based on differences in mobility or solubility; used for liquid-liquid, solid-liquid, and solid-solid mixtures
42
Q: What does centrifugation separate, and what type of mixture is it used for?
A: It separates components by density in a heterogeneous mixture.
43
Q: What does crystallization separate, and how is it different from evaporation?
A: It separates a dissolved crystalline solid from a liquid in a homogeneous mixture; unlike evaporation, it doesn’t remove all the solvent, allowing crystals to form slowly.
44
What does Henry’s Law state?
The concentration of a gas dissolved in a liquid is directly proportional to its partial pressure above the liquid.
45
What is the comparative form of Henry’s Law for changing conditions?
Where S = solubility (or concentration) of the gas, and P = partial pressure.
46
What is the formula form of Henry’s Law using concentration and pressure?
C = kP Where: • C = concentration of the gas dissolved in the liquid • k = Henry’s Law constant (depends on gas, solvent, and temperature) • P = partial pressure of the gas
47
Q: In Henry’s Law, what happens to gas concentration if pressure increases?
A: The gas concentration increases proportionally.
48
Henry gas law constant is unique for each
Gas-liquid pair at a constant temperature
49
What is a partial pressure?
The pressure a gas would exert if it were alone in the container at the same temperature and volume.
50
Active recall the entire solubility rule use for determining whether a compound is soluble or not.
SOLUBLE LIST: NAG SAG Nitrates Acetate Group-1 Sulfates, (Exception: red, and white) Ammonium Group-17 (Exception: red) Red: MLS M for Mercury L for Lead S for Silver White: Castro Bear Calcium Strontium Barium
51
Components of a colloid
. Dispersed phase (suspended particles) . Continuous phase (Medium of suspension)
52
Q: What is the Tyndall effect?
A: The Tyndall effect is the scattering of light by particles in a colloid or suspension, but not in a solution. It helps distinguish between a true solution and a colloid.
53
Q: A beam of light is passed through two mixtures. In one, the light path is visible (scattered); in the other, it is not. What is this phenomenon called?
A: Tyndall effect — light scatters in colloids or suspensions, but not in true solutions.
54
What is osmotic pressure?
The pressure needed to stop osmosis (the pressure exerted by osmosis)
55
Osmotic pressure formula
56
Which factors affect osmotic pressure?
Remember: Osmotic pressure = icRT . Number of molecules (directly proportional) . Volume of solvent (inversely proportional) . Ionization constant (directly proportional) . Temperature (directly proportional)
57
What are colligative properties?
Properties that depend solely on the concentration of solute but not on the identity of the solute
58
State every colligative property
1. Vapor pressure reduction 2. Boiling point elevation 3. Freezing point depression 4. Osmotic pressure
59
What is molality?
Expression of concentration in mole of solute per mass of solvent
60
What is the Van Hoff factor?
Ionization constant If NaCl dissociates into one mole of Na ion and one mole of Cl ion, the van hoff factor is 2. If CaCl2 dissociates into one mole of Ca ion and two moles of Cl ion, the van hoff factor is 3.
61
What is the formula for the colligative property: vapor pressure lowering?
📌 Why this works: Adding solute particles reduces the proportion of solvent particles at the surface, so fewer can escape into vapor. This lowers vapor pressure. Mole fraction reflects this.
62
Formula for boiling point elevation?
63
Formula for freezing point depression?
64
Formula for osmotic pressure?
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