Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chem 1B > Unit 4: Solutions And Colligative Properties > Flashcards

Unit 4: Solutions And Colligative Properties Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

What type of change is the dissociation of NaCl to its constituent ions?

A

Physical Change

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

What are some important things to know about crystalline structures?

A

Repeating structure of atoms/molecules (ordered)

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

What are some important things to know about amorphous solids?

A

More random arrangement of the molecules/atoms.

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

What technique is used to determine the lattice structure of solids?

A

X-Ray Diffraction

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

What are solid state ionic lattices?

A

They are lattice structures that consist of ions; ion-ion forces are present in between the ions.

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

What are molecular solids?

A

They are solids consisted of molecules; for example, H2O has dipole dipole forces present in it.

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

What are covalent network solids?

A

Solids that are made up of a covalent network; bunch of covalent bonding going on.

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

What type of solid is MgCl2?

A

Ionic; Mg2+, 2Cl-

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

What type of solid is CO2?

A

Molecular

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

What type of solid is Si?

A

Covalent network solid

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

What is an example of a gas in liquid solution?

A

Carbonated water (CO2 in water)

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

What is an example of a liquid in liquid solution?

A

Gasoline (mixture of hydrocarbons)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is an example of a solid in liquid solution?

A

Seawater (NaCl and other salts in water).

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

What are ion-dipole forces?

A

A type of attractive force that results from the electrostatic attraction between an ion and a neutral molecule that has a dipole. This force is present in between the water molecules and solvated ions.

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

What happens to the potential energy when the ionic lattice breaks apart?

A

Increases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

When is DeltaH solution positive and when is it negative?

A

It is negative is the solvent-solute reactions are dominant.

It is POSITIVE when the solvent-solute reactions are NOT DOMINANT.

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

What are the soluble compounds? What are the exceptions?

A

Compounds containing the alkali metal ions and the ammonium ion- Nitrates (NO3-)- Bicarbonates (HCO3-), and Chlorate (ClO3-)-Halides-Sulfates NB-CSH

EXCEPTIONS are halides of Ag+, (Hg2)2+, and Pb2+
Sulfates of Ag+,Ca2+,Sr2+,Ba2+,Hg2+, and Pb2+

18
Q

What are the insoluble compounds are what the exceptions?

A

Carbonates (CO3)2-, phosphates (PO4)3-, chromates (CrO4)2-, and Sulfides (S)2-, Hydroxides (OH-) CP-CSH

EXCEPTIONS are the compounds containing the alkali metal ions and the ammonium ion. Compounds containing the alkali metal ions and the Ba2+ ion.

19
Q

What does “like-dissolves-like” mean?

A

Polar dissolves polar/ionic; non-polar dissolves non polar. Hydrophilic solutes dissolve in water and hydrophobic solitudes dissolve in hydrophobic solvents.

20
Q

Do non-polar solvents have strong or weak IMFs?

A

Weak IMFs.

21
Q

In reactions involving non-polar solvents dissolving non-polar solutes, how is the energy being driven?

A

It is driven by entropy, not the IMFs; more entropy is favorable.

22
Q

What do aggregate hydrophobic regions do?

A

They push H2O into the solution (the higher the entropy, the more H-bond formation).

23
Q

What generally happens to solubility when the temperature is increased?

A

When there is an increase in temperature, there is an increase in kinetic energy; the ions and particles interact more readily and we can increase the # of solute particles that reduce lattice energy.

24
Q

What happens to the solubility of gases when the temperature of the solution is increased? T

A

There is a decrease in solubility; increase in temperature leads to an increase in kinetic energy. The expansion of gases makes it harder for IMFs to take place.

25
Q

What is the equation for molarity?

A

Moles of solute/liters of solution.

26
Q

What is the equation for molality?

A

The moles of solute/kg of SOLVENT

27
Q

What is the equation for more fraction?

A

Moles of component/ total moles making up the solution.

28
Q

What is a non-volatile solute?

A

Ionic solid or liquid with dipole-dipole IMFs.

29
Q

What happens to the VP when there is an increase in non-volatile solute?

A

There is a decrease in the VP of solvent.

30
Q

What happens to the BP when there is an increase in the non-volatile solute?

A

Increased BP of the solvent.

31
Q

What happens to the FP of the solvent when there is an increase in non-volatile solute?

A

The FP is lowered.

32
Q

What happens to the osmotic pressure when there is an increase in non-volatile solute?

A

Increase in Osmotic Pressure

33
Q

Why is there a decrease in vapor pressure and an increase in BP when the non-volatile solute is increased?

A

In the presence of solutes, water makes IMFs with the solute; so, it’s harder for the H2O molecules to escape, leading to the decreased VP. In order to get molecules to escape, a greater input of heat is needed. So, the boiling point would have to be increased.

34
Q

Why does the freezing point go down with the increase of a non-volatile solute?

A

To form solid H2O, you must form the crystal lattice. The solute particles disrupt that process. A lower temperature is then needed to make the H2O freeze.

35
Q

What is the equation for the VP Soln?

A

X Solvent . VP Solvent

36
Q

What is the equation for the increase in BP and decrease in FP? What does each variable stand for?

A

Delta T= m. Kb. i
Delta T= m. Kf. i

M=molality.
i= moles of ions produced per mole of substance (NaCl: i=2, MgCl2: i=3; CH3OH: i=1)
Kf/kb= freezing point or boiling point constant

37
Q

What is the “i” for non-electrolyte substances?

A

The “i” for non-electrolyte substances is ALWAYS 1.

38
Q

What is osmosis?

A

Movement of solvent particles from a higher concentration to a lower concentration

39
Q

What do the presence of solute particles do in H2O?

A

They prevent the passage of H2O molecules; IMFs are present in between solute and H2O.

40
Q

What happens to something in a hypertonic state?

A

It loses water.

41
Q

What happens to something in a hypotonic state?

A

It gains water.

42
Q

What is the relationship between hydration energy, the size of ions, and the charge of ions?

A

Hydration energy has a direct relationship with ionic charge and an INVERSE RELATIONSHIP with ionic size.

Chem 1B (6 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions