lesson 3 Flashcards

1
Q

if we were to order solids, liquids and gas where does liquid exist?

A

somewhere between gas and solid but not midway.

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

why do phase changes happen?

A

because of the change in the force between molecules,

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

when does a matter change from solid to liquid?

A

when energy is added and the particles move faster.

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

when does a matter change from liquid to gas?

A

when more energy is added and the particles move faster.

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

phase changes and how they affect density.

A

matter becomes less dense the more energy it gains so solid is the most dense, liquid is somewhere in the middle and gas is least dense.

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

what are intramolecular forces?

A

the forces within a molecule. (e.g. ionic bond in NaCl)

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

what are intermolecular forces?

A

the forces between molecules.

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

compare intermolecular and intramolecular forces

A

intramolecular forces happen between molecules and are stronger than intermolecular forces.

intermolecular forces happen inside of a molecule.

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

give examples of intramolecular forces.

A

dipole-dipole forces

london dispersion force.

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

what is a dipole-dipole force?

A

forces between molecules that have a dipole moment.

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

what is a dipole moment?

A

molecules with polar bonds behave like an electrical field that has a positive and negative charge side.

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

what is hydrogen bonding?

A

it’s a bond between highly electronegative atom and hydrogen. and it is the strongest force.

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

what is the hydrogen bond affected by?

A

electronegativity and size.

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

why does size affect hydrogen bonds?

A

because it gives it gives the molecules an opportunity for a closer approach.

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

what are London dispersion forces?

A

instantaneous dipole that occur accidentally in a given atom induces a similar dipole in a neighboring atom

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

where do London dispersion forces occur

A

in all molecules but are most significant in larger atoms.

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

what do melting and boiling points depend on?

A

on the strength of intermolecular forces. as the strength of force increase so does the melting and boiling point.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

compare dipole-dipole force to London dispersion force.

A

dipole-dipole: only in polar molecules that can have a dipole moment and smaller the size the stronger the bond.
london dispersion force: happens in all molecules (even non-polar) and is more common in larger molecules.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

properties of liquid state:

A

low compressibility, not rigid, high density.

20
Q

what are some things that are affected by intermolecular forces in liquids?

A

surface tension and capillary reactions and viscosity.

21
Q

what is surface tension?

A

the resistance of a liquid to increase its surface area.

22
Q

how does intermolecular forces affect surface tesion?

A

larger the intermolecular force, then the higher the surface tension.

23
Q

what role does intermolecular forces play in surface tension?

A

the forces between molecules hold the molecule from 3 different sides creating a surface.

24
Q

what is capillary reaction?

A

rising of liquid in a narrow tube.

25
Q

what are cohesive and adhesive forces.

A

cohesive: between the molecules of the liquid leading to the convex meniscus.
adhesive: between the molecules of the liquid and container leading to a concave meniscus.

26
Q

what is viscosity?

A

the resistance of a liquid to flow.

27
Q

types of solids? + example.

A

amorphous: disordered structure such as glass.
crystalline: ordered structure such as rock salt.

28
Q

components of solid structure,

A

lattice: a 3D system that points to how the components make up the substance.
unit cell: makes up the lattice.

29
Q

types of unit cell. and what it is made of.

A

simple cube -> corners only
body-centered cube -> in the corners and the center.
face-centered cube -> in the corner and each face.

30
Q

bragg equation.

A

n * (wave length) = 2 d sin angle

31
Q

types of crystalline solids and what they are made of. + examples

A

ionic solids -> ions are the point of the lattice. NaCl
molecular solids -> molecules at the points of the lattice. ice
atomic solids -> atoms at the point of the lattice. daimond

32
Q

classification of atomic solids.

A

metal -> metal atoms, delocalized non-directional covalent bond
network -> non-metal atoms, directional covalent bond
group 8A -> group 8A atoms -> london dispersion forces.

33
Q

classification of molecular solids and ionic solids.

A

molecular solids: discrete molecules -> dipole-dipole and london dispersion forces.
ionic solids: ions -> ionic.

34
Q

closest packing model

A

the way that uniform metal spheres are packed in a layer.

35
Q

types of closest packing model

A

abab -> hexagonal closet packing.

abc abc -> cubic closet packing.

36
Q

eqaution for radium of metal atom and length of an edge in unit sphere.

A

r * 8^1/2

37
Q

characteristics of bonding models for metals.

A

must conduct electricity and heat.
is non-directional and strong.
which means difficult to separate but easy to move.

38
Q

bonding models for metals.

A

electron sea model, molecular orbital model. band theory.

39
Q

what is an electron sea model. what characteristics does it agree with.

A

group of cations is found in a sea of valance electrons.

conductivity. and the ability to hammer and pull wires.

40
Q

what is the molecular orbital model.

A

valance electrons from molecular orbitals that travel around the metal crystal.

41
Q

what is band theory used for?

A

to explain the properties of metals and other materials.

42
Q

what other theory does band theory follow.

A

molecular orbital model as the number of molecular orbits = the number of overlapping atomic orbitals.

43
Q

what type of bonding is in the band theory.

A

is delocalized mobile electrons that are responsible for the conductivity of heat and electricity.

44
Q

what are band orbitals. how do they work?

A

a bunch of closely spaced orbitals that allow the electrons to move freely between them
electrons partially fill the bands so they are free to travel.

45
Q

what are conducting bonds.

A

molecular orbitals that have conducting electrons.

46
Q

what are metal alloys

A

substances that have a mix of element and metallic properties.

47
Q

types of alloys and example

A

substitutional alloy -> host metal atoms are replaced by another atom that is similar in size. (e.g. brass )
interstitial alloy -> in the closest packed metal structure are occupied by smaller atoms.