Brainscape's Knowledge GenomeTM

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


See full index

General Chemistry 1 > Chapter 11 > Flashcards

Chapter 11 Flashcards

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

what does crystalline mean?

A

a solid in which atoms, molecules, or ions are arranged in patterns with long-range, repeating order

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

what does amorphous mean?

A

a solid in which atoms or molecules do not have any long-range order

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

what is Coulomb’s law?

A

E = q1q2/r

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

what are intermolecular forces?

A

the forces between of attraction and repulsion between different molecules

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

what is ion-induced dipole force?

A

an intermolecular force between ions and a non-polar molecule

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

what are dispersion forces?

A

an intermolecular force (a type of ion-induced dipole force) exhibited by all atoms an molecules that result from fluctuations in the electron distribution

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

what are dipole-dipole forces?

A

an intermolecular force exhibited by polar molecules that result from the uneven charge distribution

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

what is a temporary dipole?

A

a permanent separation of charge; a molecule with permanent dipole always has a slightly negative charge at one end and a slightly positive charge at the other end

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

what is miscibility?

A

the ability to mix without separating into two phases

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

what is hydrogen bonding?

A

a strong type of intermolecular bonding that occurs between polar molecules that contain hydrogen atoms bonded directly to small electronegative atoms (FON)

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

what is a hydrogen bond ?

A

a strong dipole-dipole attractive force between a hydrogen bonded to FON and one of these electronegative atoms on a neighbouring molecule

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

what are dipole-induced dipole forces?

A

an intermolecular force between molecules that have a permanent dipole and an atom or molecule that is non-polar

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

what are ion-dipole forces?

A

an intermolecular force between an ion and the oppositely charged end of a polar molecule

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

what is surface tension?

A

The energy required to increase the surface area of a liquid by a unit amount: responsible for the tendency of liquids to minimize their surface, giving rise to a membrane-like surface

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

what is viscosity?

A

a measure of the resistance of a liquid to flow

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

what is capillary action?

A

the ability of a liquid to flow against gravity up a narrow tube due to adhesive and cohesive forces

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

what does vaporization mean?

A

the phase transition from liquid to gas

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

what is condensation?

A

the phase transition from gas to liquid

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

what does volatile mean?

A

tending to vaporize easily

20
Q

what does nonvolatile mean?

A

not easily vapourized

21
Q

Summarize the process of water vaporization?

A
  1. The rate of vaporization increases with increasing temperature
  2. The rate of vaporization increases with increasing surface area.
  3. The rate of vaporization increases with decreasing strength of intermolecular forces.
22
Q

what is melting point?

A

The temperature at which the molecules of a solid have enough thermal energy to overcome intermolecular forces and become a liquid

23
Q

what is melting (Fusion)?

A

the transition from solid to liquid

24
Q

what is freezing?

A

the transition from liquid to solid

25
Q

what is X-ray diffraction?

A

a powerful laboratory technique that allows for the determination of the powerful arrangement of atoms in a crystal and the measuring of the distance between them

26
Q

what is Bragg’s Law ?

A

nλ =2d sinθ

distance between atomic layers = d = nλ/2d sinθ

27
Q

what is a crystalline lattice?

A

the regular arrangement of atoms in a crystalline solid

28
Q

what is a unit cell?

A

The smallest divisible unit of a crystal, that when repeated in 3D, reproduces the entire crystal lattice

29
Q

what is a simple cubic?

A

a unit cell that consists of a cube with one atom at each corner

30
Q

what is a coordinate number?

A

the number of molecules or ions directly bound to the metal atom in a complex ion

31
Q

what is packing efficiency?

A

The percentage of volume of a unit cell occupied by atoms, assumed to spherical

32
Q

what is the body-centred cubic?

A

a unit cell that consists of a cube with one atom at each corner and one atom at the centre of the cube
coordinate number = 8

33
Q

what is the face-centred cubic?

A

a crystal structure whose unit cell consists of a cube with one atom at each corner and one atom in the centre of every face
coordinate number = 12

34
Q

what is a hexagonal closet packing ?

A

a closet packed arrangement in which the atoms of the third layer align exactly over those in the first layer

35
Q

what is cubic closet packing?

A

a closet packed arrangement in which the third layer of atoms is offset from the first: the same structure as the faced-centred cubic

36
Q

what are molecular solids?

A

solids whose composite units are molecules; they generally have low melting points

37
Q

what are ionic solids?

A

solids whose composite units are ions; generally have high melting points

38
Q

what are atomic solids?

A

solids whose composite units are atoms, they include nonbonding atomic solids, metallic atomic solids, network covalent solids

39
Q

what are nonbonding atomic solids?

A

atomic solids held together by dispersion forces; they have low melting points

40
Q

what are metallic atomic solids?

A

atomic solids held together by metallic bonds; they have variable melting points

41
Q

what are network covalent atomic solids?

A

atomic solids held together by covalent bonds; they have high melting points

42
Q

what is band theory?

A

A model for bonding in atomic solids that comes from molecular orbital theory in which atomic orbitals combine and become delocalized over the entire crystal

43
Q

what is a band gap?

A

an energy gap that exists between the valence band and conduction band of semiconductors and insulators

44
Q

what is n-type semiconductor?

A

a semiconductor that employs negatively charged electrons in the condition band as the charge

45
Q

what is a diode?

A

a device that allows the flow of electrical current in only one direction

46
Q

what is a p-type semiconductor?

A

a semiconductor that employs positively charged “holes” in the valence band as the charge carriers

47
Q

what are p-n junctions?

A

tiny areas in electrical circuits that have a p-type semiconductors on one side and n-type on the other

General Chemistry 1 (11 decks)

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