Lectures 1-4 Flashcards

1
Q

LDF (London Dispersion Forces)

A

The force of attraction that arises as a result of temporary dipoles induced in the atoms of molecules

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

Hydrogen Bonding

A

A type of dipole-dipole interaction between the hydrogen atoms in a polar bond and an unshared electron pair of an element that is very electronegative; must be N, O, or F

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

Dipole-Dipole

A

Forces that occur between polar molecules

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

Ion-Dipole

A

Experienced by ions interacting with polar molecules in solution

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

Dipole-Induced Dipole Forces

A

Exists when a polar molecule induces a dipole on a nonpolar molecule due to proximity

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

Polarizability

A

Measure of ease with which electron charge density is distorted by an external electric field: reflects the ability for which a dipole can be induced

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

Adhesion

A

The ability to “stick” to things (like glass) other than itself

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

Cohesion

A

The ability to “stick” to itself

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

Viscosity

A

Resistance to flow exhibited by all liquids and gases

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

Surface Tension

A

Resistance of a liquid to increase in its surface area

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

Capillary Rise

A

Spontaneous rising of a liquid up a narrow tube

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

Triple point

A

The point on the phase diagram at which all three states of matter exist (and are in equilibrium)

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

Critical Point

A

The point on the phase diagram where the liquid and gaseous states are indistinguishable

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

Supercritical Fluid

A

Any substance at a temperature and pressure above its critical point

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

Molecular Solids

A

Solids (like ice) that are held together by intermolecular forces like LDF, Dipole-Dipole, Ion-Dipole, etc.; low melting point and nonconducting

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

Ionic Solids

A

Ionic bonds (oppositely charged ions) hold the solid in a regular three dimensional arrangement; high melting point, brittle, and hard

16
Q

Covalent Network

A

A solid consists of atoms held together in large networks or chains by covalent bonding (electrons pairs are shared between atoms); high melting point, hard, and nonconducting

17
Q

Metallic Solids

A

Similar to a covalent network, but with metals; variable hardness and melting, and high conductivity

18
Q

Allotrope

A

Some solid substances can exist in more than one form (diamond, coal, graphite)

19
Q

Solubility

A

The maximum amount of a solute (dissolved substance) that is dissolved in a solvent (the substance dissolving dissolved substance) at a given temperature

20
Q

Saturated Solution

A

Contains the maximum amount of dissolved solute for a given amount of solvent at a specific temperature and pressure

21
Q

Supersaturated Solution

A

Contains more dissolved solute than a saturated solution (more than the solvent is able to handle)

22
Q

Dilute Solutions

A

Contains less dissolved solute than a saturated solution (could dissolve more solute if needed)

23
Q

Strong Electrolyte

A

Complete dissociated into ions in a solution

24
Weak Electrolytes
Produce few ions and do not dissociate completely in a solution
25
Nonelectrolyte
Will not produce ions
26
Miscible
Two liquids which share intermolecular forces and are able to mix with one another
27
Immiscible
Two liquids that do not have intermolecular forces in common and will not mix with one another
28
Q = mc∆T
m = mass c = specific heat ∆t = change in temperature Used to solve when temperature is changing
29
Q = n∆H
n = moles ∆H = enthalpy Used to solve when temperature is stable
30
Clausius Clapeyron
ln(P2/P1)=(-∆Hvap/R)(1/T2-1/T1) R = 8.314 J/mol K Pressure is directly related to temperature
31
Unit Cells
Finding out the number of atoms in a unit cell: d = (# atoms / unit cell) (MW/Na)(1/Vc) d = density # atoms / unit cell = number of atoms per unit cell MW = molecular weight Na = Avogadro's number (6.022 X 10^23) 1/Vc = Reciprocal of the volume
32
Unit Cells (continued)
Simple Cubic: One cell on each corner (there is 1 atom total); edge length formula: a = 2r Body Centered Cubic: One cell on each corner and anther right in the middle (there are 2 atoms total); edge length formula: a = 4r/sqrt3 Face Centered Cubic: One cell on each corner and one in the middle of each face (there are 4 atoms total); edge length formula: a = 2r(sqrt2)
33
Henry's Law
C = kp C = gas solubility (M) P = partial pressure K = Henry's law constant Normally asked to find k using this formula