Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chemistry > Solubility > Flashcards

Solubility Flashcards

1
Q

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

A

Polarity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

This is symmetrical and has no opposites

A

Nonpolar

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

This is not symmetrical and does have opposites

A

Polar

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Molecules ability to stick together

A

Cohesion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Molecules ability to stick to surfaces

A

Adhesion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Movement of water through a porous material

A

Capillary action

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Meaning ‘within’ a molecule

A

INTRAmolecular forces

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Meaning ‘between’ molecules

A

INTERmolecular forces

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What forces are within Intramolecular substances and hold it together?

A

Ionic, Covalent, Metallic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

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

A

True

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

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

A

Dispersion, Dipole-Dipole, Hydrogen bonding

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

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

A

Dispersion forces

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

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

A

Hydrogen Bonding

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

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

A
  1. Hydrogen Bonding
  2. Dipole-Dipole
  3. Dispersion
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

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

A

Surface Tension

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

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

A

polar and some ionic solutes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

T or F: Polarity rule- like dissolves like

A

True

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

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

A

Non-polar solutes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Which will dissolve in water(a polar solvent)?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Is water Ionic, polar, or non-polar?

A

Water is polar because of its molecules bent shape

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q
  • The ability to be mixed
  • How well two substances can mix together to form a solution
  • like dissolves like
A

Miscibility

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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
T or F: Substances with weak IMFs would evaporate more easily and therefore have more vapor pressure
True
26
Term describing the quantity of energy(joules) needed to raise the temperature of 1 gram of water by 1 ℃, identified by the constant c
Specific heat
27
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
Properties of water
28
T or F: Water is a nonpolar molecule that has polar bonds.
False - polar molecule with polar covalent bonds
29
T or F: A nonpolar molecule can have polar bonds.
True - Example: CO2 - draw VSEPR diagram (non polar) and use EN diff to determine bond polarity (polar)
30
T or F: Methane, CH4, (MM=16 g/mol) has about the same strength of IMF as ammonia, NH3 (MM = 17g/mol)
False - Ammonia has hydrogen bond (stongest IMF) which is much stronger than methane (non polar molecule hence dispersion IMF)
31
Solute
The thing being dissolved, you have less of it (ex. salt)
32
Solvent
Doing the dissolving, you have more of (ex. water)
33
A type of solute that has a metal, ions exist, charges hold compounds together
Ionic
34
A type of solute that has 2 NON metals, IMFs that hold molecule together, and covalent bonds hold atom together
Molecular (Covalent)
35
How does water dissolve ionic compounds?
Polar water molecule interact with positive and negative ions
36
Term for ionic compounds pulled apart to form ions in water
Dissociation
37
The process of dissolving is?
1. Solute particles are surrounded by solvent particles 2. Solute particles are separated and pulled into solution
38
What is considered a universal solvent that dissolves many solutes?
Water
39
Term for ionic compounds that dissolve in water, creates ions that can conduct electricity
Electrolytes
40
Whole molecules are hydrated, but DO NOT dissociate or ionize in water
Solvation of a molecule
41
Does sugar dissociate?
No! Water molecules separate one sugar molecule from one another
42
Ionic: this represents NaCl (s) → Na+(aq) + Cl- (aq)
Dissociation
43
Term when two liquids are not soluble in each other
Immiscible, ex. oil (non-polar) and water (polar)
44
Contains the max solute it can normally hold at that temp and stay in solution
Saturated
45
Contains less than the max for the same condition
Unsaturated
46
Contains more solute than it can normally hold at that temp but stays in solution
Supersaturated
47
3 ways you can increase the rate of solubility of a solid are...
1. Stir it (agitation) 2. Heat it (increase temp) 3. Crush it (increase the surface area)
48
This tells you how much solute should be dissolved in 100g of water at a given temperature
Solubility Curves
49
In a solubility curve, the x-axis is??
Temperature
50
In a solubility curve, the y-axis is??
Grams of solute per 100g
51
A positive slope on a solubility curve is a solid or gas?
Solid
52
A negative slope on a solubility curve is a solid or gas?
Gas
53
Explains everything in a chemical RXN including spectator ions that do not change in the reaction
Complete Ionic Equation (CIE)
54
Only shows the substances that react to form new products. We leave out the spectator ions (ions that do not change).
Net Ionic Equation (NIE)
55
When stress is applied to a system at equilibrium, the system acts to relieve the stress & restore equilibrium
Le Chatelier's Principle

Chemistry (5 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions