Brainscape's Knowledge GenomeTM

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


See full index

physics > physical properties > Flashcards

physical properties Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Physics flashcards Physics 101 flashcards
1
Q

intramolecular bond

A

bond which occurs BETWEEN atoms INSIDE molecules

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

intermolecular forces

A

forces of attraction BETWEEN molecules,ions,atoms,noble gases

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

van der Waals forces

A

intermolecular forces of varying strength specifically between molecules

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

london force

A

weakest van der Waals force
due to the attraction of electrons of one molecule between to the nuclei of another
exists between non polar molecules

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

hydrogen bond force

A

force between highly polar molecules which is a special case of van der Waals forces between polar molecules

stronger than forces between other polar molecules

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

interaction

A

bond/force between particles (atoms,molecules, ions,electrons) of substance responsibility for its physical properties

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

melting and boiling points

A

depends on strength and number of interactions betel particles
more,stronger forces= higher MP + BP

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

conductivity

A

ability for current to flow through substance

substance must contain charged particles (ions,electrons) that are free to move

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

malleable

A

bendability

hard materials ability to be hammered/ pressed into shape w/o breaking/cracking

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

brittle

A

hard material that will break/crack when subjected to force.

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

types of solids

A

metallic lattice
ionic lattice
molecular lattice
atomic lattice

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

what are the particles in a metallic lattice

A

positive kernels and delocalised electrons

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

how is a metallic lattice formed

A

it is a result of metallic bonding

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

metallic lattice strength

A

strong, generally hard

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

metallic lattice MP+BP

A

high MP and BP

  • many strong electrostatic forces of attraction between positive kernels and delocalised electrons
  • more energy need to overcome forces of attraction
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

metallic lattice conductivity

A

good conductors of electricity in all phases

- delocalised electrons can move over positive kernels

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

metallic lattice malleability

A

sheets of cations can slide over each other but remain held together by electrostatic forces of attraction between electrons and cations

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

ionic lattice strength

A

strong

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

ionic lattice particles

A

anions and cations

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

MP + BP ionic lattice

A

high
many strong electrostatic forces of attraction between anions and cations
more energy needed to overcome forces

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

why one w greater BP - ionic lattice

A

electrostatic forces between - are stronger than those between - bcus the size of the charges are greater in -
more energy required to overcome forces

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

ionic lattice brittle

A

a shift in the arrangement of ions brings like charges alongside each other which result in a force of repulsion which causes the solid to fracture

23
Q

conductivity ionic lattice

A

in solid state, cations and anions are not free to move to carry charge in ionic lattice
-cannot conduct electricity in solid state

24
Q

when can ionic lattice conduct electricity

A

aqueous state/molten state

-ions are free to move to carry charge

25
Q

molecular lattice particles

A

molecules held together by electrostatic forces

26
Q

van der waals forces from weak to strong

A

london forces of attraction
dipole dipole forces of attraction
hydrogen bond force

27
Q

strength molecular lattice

A

generally weak when compared

28
Q

london force bond

A

electrons randomly move around molecule

at a point in time e-‘s can exist on one side more

29
Q

metallic lattices conduct electricity in solid state

A

The lattice contains delocalised electrons which are free to move to carry charge

30
Q

Explain why metallic lattices have generally high melting points

A

◦There are many, strong electrostatic forces between cations and delocalised electrons in the lattice
◦More energy is required to overcome these forces

31
Q

Explain why aluminium has a higher melting point than magnesium.

A

◦Both substances are metallic
◦Aluminium cations have a 3+ charge and magnesium cations have a 2+ charge ◦The electrostatic forces of attraction between the cations of aluminium and the
delocalised electrons are stronger than those in magnesium
◦More energy is required to overcome the stronger forces in the aluminium lattice ◦Therefore aluminium has a higher boiling point than magnesium

32
Q

Explain why metals are malleable.

A

◦The sheets of positive cations can slide over one another while the electrostatic forces mm
between the cations and delocalised electrons remain intact ◦The lattice can be bent into different shapes

33
Q

why ionic lattices cannot conduct electricity in the solid state.

A

◦The ions (cations and anions) are not free to move to carry charge in the solid state

34
Q

Why are ionic substances brittle?

A

◦When a force is applied to the ionic lattice the arrangement of the ions can change so that like charges are next to each other.
◦Like charges repel each other ◦The lattice shatters

35
Q

Explain why ionic substances generally have a high melting point.

A

◦There are many, strong electrostatic forces between cations and anions in an ionic lattice
◦More energy is required to overcome these forces

36
Q

Which substance would have a higher melting point? Magnesium oxide or lithium bromide.

A

Both substances are ionic
◦In magnesium oxide the cations have a 2+ charge and the anions have a 2- charge
◦In lithium bromide the cations have a 1+ charge and the anions have a 1- charge
◦The electrostatic forces of attraction between ions (cations and anions) are stronger in
the magnesium oxide lattice as a result
◦More energy is required to overcome stronger forces ◦Magnesium oxide has a higher boiling point than lithium bromide

37
Q

) Do atomic lattices have generally high or low melting points. Explain fully.

A

◦High melting point

◦Many strong covalent bonds holding atoms together ◦More energy is required to break these bonds.

38
Q

Which has a higher melting point? Diamond or graphite? Explain fully.

A

◦Diamond
◦Each carbon atom is bonded 4 times with other carbons compared to graphite
where each carbon atom is bonded only 3 times with other carbon atoms ◦More energy is required to break the many strong covalent bonds in diamond

39
Q

) Which atomic lattice can conduct electricity in the sold phase? Explain.

A

Graphite

◦Each carbon atom has a delocalised electron that is not bonded ◦These electrons are free to move to carry charge

40
Q

london force origin

A

Electrons move randomly around particles
By chance one molecule can form a temporary dipole
When this temporary dipole comes close to a neighbouring molecule the
neighbouring molecule forms an induced dipole
The two dipoles electrostatically attract

41
Q

hydrogen bond force origin

A

when a small highly electronegative atom( N,O,F) bonds with hydrogen, hydrogen bonding can occur
THE highly electronegative atom attracts the bonding pair of e- away from hydrogen exposing a naked proton
the naked proton electrostatically attracts the lone pair of e- of a neighbouring molecule

42
Q

molecular lattice MP/BP

A

low
weak van der waals forces between molecules
less energy required to overcome forces

43
Q

molecular lattice conductivity

A

cannot conduct electrical charge
neutral molecules
no charges to move to carry charge

44
Q

molecular lattice phase change

A

intermolecular forces overcome

45
Q

molecular lattice chemical change

A

intramolecular bonds broken

46
Q

atomic lattice types

A

diamond
graphite
silicon dioxide

47
Q

atomic lattice strength

A

extremely strong
many strong covalent bonds between atoms
more energy needed to break the bonds

48
Q

diamond bonds per atom

A

4

49
Q

graphite bonds per atom

A

3

50
Q

silicon dioxide bonds per atom

A

bonds per atom

51
Q

graphite

A

covalent bonds between atoms
sheets of carbon held together by weak electrostatic forces of attraction- london forces
held by delocalised e- - can conduct electricity

52
Q

why silicon dioxide poor conductor

A

atoms are neutral

no particles to move to carry charge

53
Q

what influence strength of intermolecular forces

A

the type of intermolecular force involved e.g.: weak van der Waals forces (such as
London forces) vs stronger hydrogen bonds.
• The number of electrons in the molecule which is indicated by the molar mass of the
molecule (for London forces only).
• The number of intermolecular forces (relates to hydrogen bonds only)

physics (36 decks)

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