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physical properties Flashcards

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1
Q

intramolecular bond

A

bond which occurs BETWEEN atoms INSIDE molecules

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2
Q

intermolecular forces

A

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

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3
Q

van der Waals forces

A

intermolecular forces of varying strength specifically between molecules

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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

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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

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6
Q

interaction

A

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

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7
Q

melting and boiling points

A

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

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8
Q

conductivity

A

ability for current to flow through substance

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

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9
Q

malleable

A

bendability

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

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10
Q

brittle

A

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

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11
Q

types of solids

A

metallic lattice
ionic lattice
molecular lattice
atomic lattice

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12
Q

what are the particles in a metallic lattice

A

positive kernels and delocalised electrons

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13
Q

how is a metallic lattice formed

A

it is a result of metallic bonding

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14
Q

metallic lattice strength

A

strong, generally hard

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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
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16
Q

metallic lattice conductivity

A

good conductors of electricity in all phases

- delocalised electrons can move over positive kernels

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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

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18
Q

ionic lattice strength

A

strong

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19
Q

ionic lattice particles

A

anions and cations

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20
Q

MP + BP ionic lattice

A

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

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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

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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)

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