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Chemistry > Solubility > Flashcards

Solubility Flashcards

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1
Q

The unequal sharing of electrons which results in partial charges that helps with dissolving

A

Polarity

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2
Q

This is symmetrical and has no opposites

A

Nonpolar

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3
Q

This is not symmetrical and does have opposites

A

Polar

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4
Q

Molecules ability to stick together

A

Cohesion

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5
Q

Molecules ability to stick to surfaces

A

Adhesion

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6
Q

Movement of water through a porous material

A

Capillary action

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7
Q

Meaning ‘within’ a molecule

A

INTRAmolecular forces

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8
Q

Meaning ‘between’ molecules

A

INTERmolecular forces

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9
Q

What forces are within Intramolecular substances and hold it together?

A

Ionic, Covalent, Metallic

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10
Q

T or F: all INTERmolecular forces are weaker than INTRAmolecular forces

A

True

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11
Q

3 types of INTERmolecular forces(IMF’s)
Aka Van der Waals Forces

A

Dispersion, Dipole-Dipole, Hydrogen bonding

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12
Q

Type of IMF that has momentary opposing charges caused by the motion of e-

A

Dispersion forces

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13
Q

Type of IMF that occurs due to uneven distribution of electrons within the molecules, occurs between polar molecules and is stronger than dispersion. Partial positives are attracted to partial negatives.

A

Dipole-Dipole

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14
Q

Type of IMF that has strong dipole-dipole forces due to polar bonds between H NOF

A

Hydrogen Bonding

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15
Q

Rank: Dispersion forces, Dipole-Dipole, and Hydrogen Bonding from strongest to weakest force

A
  1. Hydrogen Bonding
  2. Dipole-Dipole
  3. Dispersion
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16
Q

Molecules at the top are pulled downward, resulting in a ‘skin’ on top of the water

A

Surface Tension

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17
Q

If the solvent is polar, it will dissolve ______ and ________ solutes

A

polar and some ionic solutes

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18
Q

T or F: Polarity rule- like dissolves like

A

True

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19
Q

If the solvent is non-polar, it will dissolve _________

A

Non-polar solutes

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20
Q

Which will dissolve in water(a polar solvent)?

A

Hydrochloric Acid(polar) and Copper(ll) Chloride(Ionic)

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21
Q

Is water Ionic, polar, or non-polar?

A

Water is polar because of its molecules bent shape

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22
Q
  • The ability to be mixed
  • How well two substances can mix together to form a solution
  • like dissolves like
A

Miscibility

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23
Q

The pressure that the molecules of a liquid exert (or push) when they escape and become vapor (like steam)

A

Vapor Pressure

24
Q

A strong IMF will have what type of boiling point and vapor pressure?

A

HIGH boiling point and LOW vapor pressure

25
Q

T or F: Substances with weak IMFs would evaporate more easily and therefore have more vapor pressure

A

True

26
Q

Term describing the quantity of energy(joules) needed to raise the temperature of 1 gram of water by 1 ℃, identified by the constant c

A

Specific heat

27
Q
  1. Has high surface tension
  2. Attractions and repels substances
  3. Can dissolve extra
  4. Is incredibly polar
  5. Unusual density
  6. Has high specific heat
A

Properties of water

28
Q

T or F: Water is a nonpolar molecule that has polar bonds.

A

False - polar molecule with polar covalent bonds

29
Q

T or F: A nonpolar molecule can have polar bonds.

A

True - Example: CO2 - draw VSEPR diagram (non polar) and use EN diff to determine bond polarity (polar)

30
Q

T or F: Methane, CH4, (MM=16 g/mol) has about the same strength of IMF as ammonia, NH3 (MM = 17g/mol)

A

False - Ammonia has hydrogen bond (stongest IMF) which is much stronger than methane (non polar molecule hence dispersion IMF)

31
Q

Solute

A

The thing being dissolved, you have less of it (ex. salt)

32
Q

Solvent

A

Doing the dissolving, you have more of (ex. water)

33
Q

A type of solute that has a metal, ions exist, charges hold compounds together

A

Ionic

34
Q

A type of solute that has 2 NON metals, IMFs that hold molecule together, and covalent bonds hold atom together

A

Molecular (Covalent)

35
Q

How does water dissolve ionic compounds?

A

Polar water molecule interact with positive and negative ions

36
Q

Term for ionic compounds pulled apart to form ions in water

A

Dissociation

37
Q

The process of dissolving is?

A
  1. Solute particles are surrounded by solvent particles
  2. Solute particles are separated and pulled into solution
38
Q

What is considered a universal solvent that dissolves many solutes?

A

Water

39
Q

Term for ionic compounds that dissolve in water, creates ions that can conduct electricity

A

Electrolytes

40
Q

Whole molecules are hydrated, but DO NOT dissociate or ionize in water

A

Solvation of a molecule

41
Q

Does sugar dissociate?

A

No! Water molecules separate one sugar molecule from one another

42
Q

Ionic: this represents NaCl (s) → Na+(aq) + Cl- (aq)

A

Dissociation

43
Q

Term when two liquids are not soluble in each other

A

Immiscible, ex. oil (non-polar) and water (polar)

44
Q

Contains the max solute it can normally hold at that temp and stay in solution

A

Saturated

45
Q

Contains less than the max for the same condition

A

Unsaturated

46
Q

Contains more solute than it can normally hold at that temp but stays in solution

A

Supersaturated

47
Q

3 ways you can increase the rate of solubility of a solid are…

A
  1. Stir it (agitation)
  2. Heat it (increase temp)
  3. Crush it (increase the surface area)
48
Q

This tells you how much solute should be dissolved in 100g of water at a given temperature

A

Solubility Curves

49
Q

In a solubility curve, the x-axis is??

A

Temperature

50
Q

In a solubility curve, the y-axis is??

A

Grams of solute per 100g

51
Q

A positive slope on a solubility curve is a solid or gas?

A

Solid

52
Q

A negative slope on a solubility curve is a solid or gas?

A

Gas

53
Q

Explains everything in a chemical RXN including spectator ions that do not change in the reaction

A

Complete Ionic Equation (CIE)

54
Q

Only shows the substances that react to form new products. We leave out the spectator ions (ions that do not change).

A

Net Ionic Equation (NIE)

55
Q

When stress is applied to a system at equilibrium, the system acts to relieve the stress & restore equilibrium

A

Le Chatelier’s Principle

Chemistry (5 decks)

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