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Chemistry 2 > Chapter 11 - Liquids, Solids, and IMFs > Flashcards

Chapter 11 - Liquids, Solids, and IMFs Flashcards

1
Q

Crystalline

A

solid with atoms or molecules in well-ordered three dimensional arrangements

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2
Q

Amorphous

A

atoms have no long range order

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3
Q

London Dispersion Force

A
  • present in ALL molecules and atoms

Electrons will unevenly distribute as they move around creating + and - spots

  • Instantaneous or temporary dipoles
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4
Q

Dipole-Dipole Force

A
  • in POLAR molecules

molecule with permanent electron rich and electron poor areas creating strong forces

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5
Q

Permanent Dipole

A

an area of either electron rich or electron poor space creating a charge

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6
Q

Miscibility

A

the ability of a substance to mix without separating into two states of liquids.

  • like dissolves like
  • polar into polar
  • nonpolar into nonpolar
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7
Q

Hydrogen Bonding

A

polar molecules with H atoms and small electron negative atoms

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8
Q

Hydrogen Bond

A

FON are the strongest with H

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9
Q

Ion-dipole Force

A

NOT an IMF but still very impoart!

when an ionic compound is mixed with a polar compound.

Aqueous solutions.

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10
Q

Surface Tension

A

the tendency of a liquid to minimize surface area to increase stability

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11
Q

Viscosity

A

the resistance of a liquid to flow.

More resistance = more viscous

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12
Q

Capillary Action

A

the ability of a liquid to flow against gravity up a narrow tube.

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13
Q

Vaporization

A

The transition from a liquid to a gas

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14
Q

Condensation

A

The transition from a gas to a liquid

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15
Q

Volatile

A

Weaker IMFs allow easy vaporization which = less stable and quicker vaporization.

  • acetone
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16
Q

Nonvolatile

A

liquids that due not vaporize easily have stronger IMFs

  • motor oil
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17
Q

Heat of Vaporization(Hvap)

A

the amount of heat required to vaporize one mole of a liquid to a gas.

Endothermic

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18
Q

Dynamic Equilibrium

A

rate of vaporization = rate of condensation.

Systems always respond to minimize disturbances and return to a state of equilibrium.

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19
Q

Vapor pressure

A

the pressure of a gas in dynamic equilibrium with its liquid phase.

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20
Q

Boiling point

A

the temperature at which the liquids vapor pressure equals the external pressure.

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21
Q

Normal Boiling Point

A

the temperature at which its vapor pressure equals 1ATM

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22
Q

Clausius-Clapeyron Equation

A

the relationship between vapor pressure and temperature is exponential.

linear relationship between the natural log of the vapor pressure and the inverse of the temperature.

23
Q

Critical Temperature(Tc)

A

in a sealed containing, the temperature at which the gas and liquid become comingled creating a supercritical fluid.

Not a gas or a liquid

24
Q

Critical Pressure(Pc)

A

the pressure at which a supercritical fluid is created.

25
Q

Sublimation

A

state transition from a solid directly to a gas

26
Q

Deposition

A

going directly from a gas to a solid

27
Q

Melting point

A

molecules have enough thermal energy to overcome the IMFs that hold molecules at their stationary points.

28
Q

Melting(fusion)

A

the transition from solid to liquid.

“fusing” from sever solid crystals into a continuous liquid

29
Q

Freezing

A

transition from a liquid to a solid

30
Q

Heat of Fusion(Hfus)

A

the amount of heat required to melt 1 mol of a solid

endothermic process

31
Q

Phase Diagram

A

a map of the state or phase of a substance as a function of pressure(y axis) and temperature(x axis)

32
Q

Triple point

A

unique set of conditions at which the three states are equally stable and in equilibrium

33
Q

Critical Point

A

in a phase diagram it represents the temperature and pressure above which a supercritical fluid exists

34
Q

Crystalline lattice

A

the regular arrangement of atoms within a crystalline solid

  • minimizes energy
35
Q

Unit Cell

A

Representation of the crystalline lattice with a small collection of atoms, ions, or molecules

36
Q

Simple Cubic

A

Consist of a cube with one atom at each corner

  • edge length = 2r
  • coordination number = 6
  • packing efficiency = 52%
37
Q

Coordination Number

A

the number of atoms with which each atom is in direct contact
o Those an atom can strongly interact with

38
Q

Packing Efficiency

A

the % of the volume of the unit cell occupied by the spheres

o Higher coordination number = greater packing efficiency

39
Q

Body-centered Cubic

A

a cube with one atom at each corner and one atom(of the same type) in the very center of the cube
o Note – atoms do not touch along the edge but instead along the diagonal line that runs from one corner through the middle of the cube to the opposite corner
o L = 4r/sqrt3
o Coordination number = 8
o Packing efficiency is 68%
 Strongly interacts with more atoms than in a simple cubic unit cell

40
Q

Face-Centered Cubic

A

cube with one atom at each corner and one atom(of the same kind) in the center of each cube face
o Do not touch along the end of the cube but instead along the diagonal of the face
o Edge length = 2sqrt(2)r
o Coordination number = 12
o Packing efficiency = 74%
o Any one atom interacts strongly with more atoms than either the simple cubic unit cell or the body centered cubic cell

41
Q

Hexagonal Closest Packing

A

o Layers stacks on top of each other slight off set
 1st and 3rd rows mirror each other
• 3rd row aligns in exactly the same way as the 1st row
• ABAB
o Unit cell is a hexagon instead of a cubic unit

42
Q

Cubic Closest Packing

A

o 3rd layer is offset from the first
o Every 4th row aligns exactly with the first
o ABCABC
o Identical to the face-centered cubic unit cell structure

43
Q

Molecular Solids

A

o Solids whose composite units are molecules
 H2O(s), CO2(s)
o Tend to have low to moderately low melting points
o Strong IMFs can increase MPs

44
Q

Ionic Solids

A

o Solids whose composite units are Ions
 NaCl, CaF2
o Unit cell must be charge neutral
o The more similar the radii of the cation and anion the higher the coordination number
o Ionic solids tend to have much higher melting points than molecular solids
 Must break Ionic bonds which are much stronger than IMFs

45
Q

Atomic Solids

A

o Solids whose composite units are individual atoms

 Xe, Fe, SiO2

46
Q

Nonbonding Atomic Solid

A

 Held together by relatively weak dispersion forces
 Form closest packed structures, maximizing their coordination numbers and minimizing distance between them
• Close so stronger IMFs
o The only ones are noble gases in their solid form

47
Q

Metallic Atomic Solid

A 
	Held together by metallic bonds
•	Cations in a sea of electrons
•	Iron, gold, etc
	Form closest packed crystal structures
•	Cary in bond strength
48
Q

Network Covalent Atomic Solid

A

 Held together by covalent bonds
• Diamond, graphite, silicon dioxide
 Restricted by the geometrical constraints of the covalent bonds

49
Q

Band Theory

A

o From molecular orbital theory
o Applies to metallic solids and covalent solids
o The gap between orbits becomes infinitely small practically making the orbits a band of energy levels
o Conduction band – empty orbitals
o Valence band – occupied orbitals
o Energy flows continuously between conduction and valence bands which is why metals are good conductors

50
Q

Band Gap

A

o Between valence and conduction bands in insulators and semiconductors
 Insulators have a large gap
 Semiconductors have a small gap which can be exploited in various ways with doping

51
Q

N-type semiconductor

A

o The charge carriers are negatively charged electrons in the conduction band
 Forces electrons into conduction band for charge

52
Q

P-type semiconductor

A

o Creates electron “holes” or empty molecular orbitals in the valence band
o Each hole acts as a positive charge

53
Q

P-N junction

A

o Tiny spots of p-type on one side and n-type on the other

o The heart of most modern electronic devices are silicon chips with millions of these

54
Q

Diode

A

o Circuit elements that allow the flow of electrical current in only one direction

Chemistry 2 (1 decks)

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