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CHM 109: General Chemistry II > Solubility, Solutions, IMFs, and Colligative Properties > Flashcards

Solubility, Solutions, IMFs, and Colligative Properties Flashcards

1
Q

What occurs during dissociation?

A

An ionic compound separates into anions and cations when placed in water.

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2
Q

Provide an example of dissociation.

A

Na_2S (aq) –> 2Na^+ (aq) + S^2- (aq)
K_2SO_4(aq) –> 2K^+(aq) + SO_4 ^2- (aq)

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3
Q

What occurs during ionization?

A

A compound dissolves into ions when placed in water.

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4
Q

What makes a compound miscible?

A

When a molecular compound dissolves into molecules (NOT ions) when placed in water.

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5
Q

Provide an example of a miscible substance.

A

Sugar.
Sugar (s) + Water (l) –> Sugar water(aq)

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6
Q

What must occur to form strong electrolytes?

A

A chemical substance completely ionizes into its ions.
Can conduct electricity.

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7
Q

Provide examples of strong electrolytes.

A

Soluble salts, Strong acids, and Strong bases.
HCl(aq) –> H^+ + Cl^-.

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8
Q

What must occur to form weak electrolytes?

A

A chemical substance partially ionizes into its ions.
Can conduct electricity, but not as well as strong electrolytes.

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9
Q

Provide examples of weak electrolytes.

A

Weak acids and weak bases.
CH_3COOH (aq) <—-> CH_3COO^- (aq) + H^+ (aq)

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10
Q

What occurs to form non-electrolytes?

A

A chemical substance that dissolves in water but not as ions.
Cannot conduct electricity.

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11
Q

Provide examples of non-electrolytes.

A

Polar substances (ex: sugar and alcohol).
C_6 H_12 O_6 (s) –> C_6 H_12 O_6 (aq)

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12
Q

What makes a compound soluble?

A

If it dissolves in the given solvent.

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13
Q

What makes a compound insoluble?

A

If it does NOT dissolve in the given solvent.

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14
Q

What three factors affect solubility?

A
  1. Temp. Direct.
  2. Volume. Direct.
  3. Pressure (Gas solubility).
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15
Q

True or False: All gases are soluble in one another.

A

True.

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16
Q

What three ions, if present, make a compound soluble?

A
  1. Li^+
  2. Na^+
  3. K^+
    No exceptions.
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17
Q

What three polyatomic ions, if present, makes a compound soluble?

A
  1. C_2 H_3 O_2^-
  2. NO_3^-
  3. NH_4^+
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18
Q

What are the solubility exceptions for substances containing Cl^-, I^-, and Br^-?

A
  1. Ag^+
  2. Pb^2+
  3. Hg_2^2+
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19
Q

What are the solubility exceptions for substances containing SO_4^2-?

A
  1. Ag^+
  2. Pb^2+
  3. Ca^2+
  4. Sr^2+
  5. Ba^2+
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20
Q

What are the insolubility exceptions for substances containing OH^-?

A
  1. Li^+
  2. NH_4^+
  3. Na^+
  4. K^+
  5. All Group 1 metals.
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21
Q

What are the insolubility exceptions for substances containing CO3^2- and PO_4^3-?

A
  1. Li^+
  2. NH_4^+
  3. Na^+
  4. K^+
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22
Q

What are the insolubility exceptions for substances containing S^2-?

A
  1. Li^+
  2. NH_4^+
  3. Na^+
  4. K^+
  5. Ca^2+
  6. Sr^2+
  7. Ba^2+
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23
Q

What occurs during decomposition?

A

The reactant decomposes into two or more products.
A –> B+C

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24
Q

What occurs during synthesis?

A

Two or more reactants combine to make a product(s).
A+B –> C+D

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25
Q

What are the four types of synthesis reactions?

A
  1. Double displacement/precipitation.
  2. Single displacement.
  3. Reduction-Oxidation (Redox).
  4. Neutralization.
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26
Q

What occurs during neutralization?

A

An equal acid is mixed with an equal base.
A type of double displacement.

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27
Q

What occurs during double displacement/precipitation?

A

Two reactants are mixed, resulting in the formation of a solid in/on the product side.

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28
Q

What occurs during a redox reaction?

A

There is a transfer of electrons, resulting in ions being formed.

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29
Q

What is a common type of redox reaction?

A

Combustion reactions.
A substance is burned in the presence of oxygen, resulting in water and carbon dioxide being created.
*Corrosion is another type of redox reaction.

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30
Q

What occurs during a single displacement reaction?

A

Gases are formed.

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31
Q

What occurs on the reactants side of a double displacement reaction?

A

The reactants switch IONS to create the products.
AD + BC –> AC + BD
*Remember to balance the charges of the products.

32
Q

During the ion exchange during double displacement, which ion moves- the anion or the cation?

A

The anion is switched out and the cation is fixed in place.

33
Q

After charge balancing in a double displacement reaction, what must be checked next?

A

Solubility.
If soluble, mark it as aqueous (aq).
If insoluble, mark it as solid (s).

34
Q

What happens if both products in a double displacement reaction are aqueous?

A

No reaction occurs.

35
Q

What are precipitation reactions?

A

A reaction that occurs between aqueous solutions of ionic compounds results in an insoluble ionic compound called a precipitate.
*Solubility rules apply.

36
Q

What are the three types of equations?

A
  1. Complete Molecular Equation
  2. “Complete Ionic Equation”
  3. “Net Ionic Equation”
37
Q

What step must be taken to create a complete ionic equation?

A

The soluble molecules are separated into their ions, and the insoluble species are kept together.

38
Q

What does the net ionic equation show?

A

It shows only the species actually participating in the reaction.
All other ions are called spectator ions.

39
Q

What are intermolecular forces?

A

The forces that bind atoms together within chemical or molecule bonds.

40
Q

What are intramolecular forces?

A

The attractive forces that exist between molecules and atoms.

41
Q

Which is stronger: intermolecular or intramolecular forces?

A

Intramolecular forces.
*However, intermolecular forces are strong enough to influence physical properties (ex: viscosity).

42
Q

What are the types of intermolecular forces?

A
  1. Ion-dipole.
  2. Dipole-dipole.
  3. Hydrogen bonding.
  4. Dipole-induced (Van der Waals, London forces, Dispersion).
43
Q

What are the types of intramolecular forces?

A
  1. Molecular.
  2. Ionic.
  3. Covalent (non-polar/true and polar).
44
Q

How are dispersion/ Van der Waals/ London forces created?

A

Temporary fluctuations in the electron distribution in atoms or molecules create a temporary dipole.

45
Q

What type of force do all molecules possess?

A

dispersion/ London/ Van der Waals.

46
Q

What is the strength of dispersion forces based on?

A

The number of contact points the molecules have with one another. The more, the better.

47
Q

How are dipole-dipole forces created?

A

When polar molecules have a permanent dipole. The more polar, the stronger the dipole-dipole force.

48
Q

What is the relationship between molecule size and boiling point?

A

Direct.

49
Q

What is the relationship between atomic radius and boiling point?

A

Direct.

50
Q

What type of force is a hydrogen bond a specific version of?

A

Dipole-Dipole.

51
Q

How are hydrogen bonds created?

A

When a hydrogen atom bonds with an F, O, or N atom.

52
Q

Why is hydrogen bonding necessary for life on Earth?

A

It holds together DNA and water.

53
Q

How are ion dipoles formed?

A

When ions from an ionic compound are attracted to the dipole of a polar molecule in a mixture.

54
Q

What does the strength of the ion-dipole determine?

A

The solubility of the ionic compound in its solvent.

55
Q

What is the order of intermolecular forces from weakest to strongest?

A
  1. Dispersion/London/Van der Waals.
  2. Dipole-Dipole.
  3. Hydrogen bonding.
  4. Ion-dipole.
56
Q

What does solubility depend on?

A

The attractive forces between the solute molecules and the solvent molecules.

57
Q

True or False: Unlike polarities dissolve with each other.

A

False. Like dissolves like.

58
Q

What happens when a polar compound mixes with a non-polar compound?

A

They do not react and they end up layering (ex: oil and water).

59
Q

What occurs when the solute-to-solvent attraction is weaker than the sum of the solute-to-solute and solvent-to-solvent attractions?

A

The solution will not form unless the energy difference is small enough to be overcome by the increase in entropy from mixing.

60
Q

What is molarity?

A

A unit of concentration that can be prefixed.
(mols solute/L solution).

61
Q

What is molality?

A

The mols of solute per 1 kg. of solvent. Value does not vary with temperature.
(mols solute/Kg solvent).

62
Q

What is mole fraction?

A

Moles of solute over total moles of solution. Unitless.
(mols solute/mols solution).

63
Q

What is mole percent?

A

Mole fraction x 100%.

64
Q

What are percent by mass concentrations?

A

Amount of solute per amount of solution multiplied by 100.
Weight of solute + weight of solvent= Weight of solution.
((Weight of solute/ weight of solution) x 100%).

65
Q

What is parts per million (ppm) by weight?

A

(solute weight/ solution weight) x 10^6). Can be used with volumes.

66
Q

If both the solute and solvent in a two-component Raoult’s Law system are volatile, what does the delta P look like?

A

Delta P (solution) = xsolute x P^0 solvent.
* Both are liquid.

67
Q

What is lowering the vapor pressure in a two-component system equivalent to?

A

The solute’s mole fraction.

68
Q

What equation is used to give the vapor pressure of a volatile solvent over a solution?

A

P(solvent) = x(solvent) x P^0 (solvent).

69
Q

What equation is used to give the vapor pressure of a volatile solute over a solution?

A

P(solute) = x(solute) x P^0 (solute).

70
Q

What kinds of compounds produce multiple solute particles from a single formula unit?

A

Ionic.

71
Q

What is the van’t Hoff factor or i?

A

The ratio of moles of solute particles to moles of formula units dissolved.

72
Q

How does a solution’s freezing point compare to a pure solvent’s?

A

It is lower or depressed.

73
Q

How does a solution’s boiling point compare to a pure solvent’s?

A

It is higher or elevated.

74
Q

What is osmotic pressure?

A

The force that counterbalances the pressure of the solvent molecules moving through a semipermeable membrane.
Produced by extra solution.

75
Q

What is the osmotic pressure equation?

A

pi = iMRT.

76
Q

What is the driving force of osmosis and most energy?

A

Entropy.

CHM 109: General Chemistry II (5 decks)

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