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Chem Final > Intermolecular Forces, Liquids, Soldis And Materials > Flashcards

Intermolecular Forces, Liquids, Soldis And Materials Flashcards

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1
Q

Describe solids, liquids and gases

A

Solids: ordered, no diffusion, particles are close together and do not change position
Liquids: disorder, particles move and are close, slow diffusion
Gas: total disorder, lots of empty space, rapid diffusion

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2
Q

Condensation polymerization

A

Formation of polymers via eliminating small molecules like HCl or H2O

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3
Q

Is there a point where all phases (solid, liquid, and gas) can coexist at once?

A

Yes, the triple point occurs at a certain temperature and pressure

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4
Q

What is it called when semiconductors that are inorganic compounds have their 4 valence electrons increased or decreased?

A

Doping

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5
Q

When inorganic semiconductors have more than 4 valence electrons due to doping, what type of band is produced?

A

N-type (the extra electrons are added to the conduction band)

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6
Q

When inorganic semiconductors have less than 4 valence electrons due to doping, what type of band is produced?

A

P-type (holes in the valence band)

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7
Q

How are solar cells formed? And what type of energy are they converting?

A

By joining n-type and p-type silicon solar cells. They convert light/optical energy into electrical energy

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8
Q

What type of energy do LEDs convert?

A

LEDs do the opposite of solar cells and convert electrical energy into light/optical energy

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9
Q

Describe molecular solids and give an example of one

A

-low melting points and boiling points due to weak intermolecular forces
-units are molecules
-held together by intermolecular forces
-a type of crystalline solid
-ex: ice or sucrose

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10
Q

Describe molecular solids

A

-low melting points and boiling points due to weak intermolecular forces
-units are molecules
-a type of crystalline solid

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11
Q

Describe insulators and give some examples of them

A

-have a large band gap (the energy difference between a filled band and an empty band)

Examples: wood, air, rubber, glass and most plastics

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12
Q

Describe metallic solids

A

-consist of metal atoms held together by metallic bonding
-conduct electricity
-ex: gold (Au)

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13
Q

Describe ionic solids

A

-consist of positive and negative ions held together by ionic bonds
-have high melting points
-hard and brittle
-poor conductors of electricity due to the strength of ionic bonds
-ex: sodium chloride (NaCl)

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14
Q

Covalent-network solids

A

-high melting points and are much harder than molecular solids
-held together by strong covalent bonds
-ex: diamond (boiling point of 3550 degrees), quartz

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15
Q

Non bonding solids

A

-held together by London dispersion forces
-low melting point
-ex: xenon (Xe)

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16
Q

Describe semi conductors

A

-have a small band gap so heat or radiation can promote electrons from the valence band to the conduction band
-conductivity in inorganic semiconductors can be increased by doping

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17
Q

What is viscosity and how does molecular shape affect it?

A

-Viscosity is measured by a fluids resistance to flow (honey has higher viscosity than water)
-larger, more complex molecules have higher viscosities because they are more likely to interlock or entangle

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18
Q

What is it called when a solid turns into a liquid?

A

Melting

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19
Q

From liquid to solid

A

Freezing

20
Q

Gas to liquid

A

Condensing

21
Q

From liquid to gas

A

Boiling

22
Q

Gas to solid

A

Sublimination

23
Q

Solid to gas

A

Deposition

24
Q

Is vapour pressure higher or lower when intermolecular forces are stronger

A

Lower

25
Q

What happens at the triple and critical point?

A

At the triple point all three phases are in equilibrium and at the critical point a supercritical fluid is formed

26
Q

When does boiling occur in relation to vapour pressure?

A

When vapour pressure=external pressure

27
Q

Give some examples of Intramolecular forces, are they strong or weak?

A

-Covalent bonding, ionic bonding
-They are relatively strong

28
Q

Give examples of intermolecular forces, are they strong or weak?

A

-relatively weak
-London dispersion forces
-Hydrogen bonding
-Dipole dipole

29
Q

The stronger the intermolecular forces the lower/higher the boiling and melting points

A

Higher

30
Q

How to identify if a compound has hydrogen bonding

A

If it contains an O-H, F-H or N-H bond

31
Q

What is the strongest intermolecular force?

A

Hydrogen bonding

32
Q

When do dipole-dipole interactions happen?

A

When the positive end of a polar molecule interacts with the negative end of another polar molecule. In order to be a polar molecule the molecule must have a net dipole.

33
Q

Order the intermolecular forces in order from strongest to weakest

A

Hydrogen bonding > dipole dipole > London dispersion forces

34
Q

When are London dispersion forces present in compounds?

A

They are present in all compounds regardless whether the molecule is polar or nonpolar

35
Q

If a molecule is polar and has hydrogen bonding what does that mean?

A

It means that it has all three intermolecular forces due to the polarity

36
Q

Explain the relationship between viscosity and intermolecular forces

A

Viscosity increases with the strength of intermolecular forces

37
Q

Why does surface tension happen?

A

Because molecules at the surface are more attracted to each other than they are to the air

38
Q

Cohesive forces

A

Attraction of molecules to each other (liquid molecules sticking to each other)

39
Q

Adhesive forces

A

Attraction of molecules for surface (liquid molecules sticking to the surface)

40
Q

Are the adhesive forces between the glass (capillary) and the liquid weaker or stronger than the cohesive forces between the molecules in the liquid?

A

The adhesive forces are weaker than the cohesive forces

41
Q

Liquid crystals

A

Intermediate phases between solid and liquid, rod-shaped, polar molecules

42
Q

Nematic phase of liquid crystals

A

Aligned in one direction

43
Q

Smectic phase of liquid crystals

A

Aligned in one direction and in layers

44
Q

Cholesteric phase of liquid crystals

A

Aligned in one direction and in twisted/rotated layers

45
Q

Addition polymerization

A

Breaks down double bonds into all single bonds to form polymers from monomers

Chem Final (5 decks)

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