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physics > typesof solids > Flashcards

typesof solids Flashcards

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1
Q

metallic lattice particles

A

positive kernels and delocalised valance electrons

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2
Q

how do metallic lattices come about

A

result of metallic bonding

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3
Q

metallic lattice strength and strongness

A

strong
generally hard

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4
Q

metallic lattice bp and mp

A

high melting and boiling points as there are many strong electrostatic forces of attraction between positive kernels and delocalised valence electrons

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5
Q

metallic lattice malleability

A

Sheets of cations can slide past over each other but remain held together by electrostatic forces of attraction between positive kernels and delocalised valence electrons

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6
Q

Na vs Mg boiling point

A

more stronger electrostatic forces of attraction between positive kernels + delocalised electrons in Mg
cation of Mg is 2+ and cation of Na is 1+
Mg has higher boiling water

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7
Q

metallic lattice test for conductivity

A

have a system w a power supply, ammeter and apply potential difference across it
insert test substances between clips/ place substance in beaker using electrodes to make contact w substance

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8
Q

how do ionic lattices come about

A

result of ionic bonding

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9
Q

ionic lattice particles

A

anions + cations

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10
Q

strength ionic lattice

A

strong

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11
Q

ionic lattice mp+ bp

A

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

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12
Q

Al2O3 vs NaF BP

A

electrostatic forces between Al3+ and O2- are stronger than those between Na+ and F- because the sizes of the charges are greater in Al2O3
therefore more energy is required to overcome the forces

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13
Q

brittle ionic solids

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

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14
Q

ionic lattice test for conductivity

A

in solid state cations + anions are not free to move to carry charge in an ionic lattice. can melt solid- molten state or dissolve in water- aqueous state

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15
Q

molecular lattice particles

A

molecules held together by electrostatic forces (van der waals forces)

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16
Q

van der waals forces weakest to strongest

A

london forces
dipole-dipole forces of attraction
hydrogen bond forces

17
Q

molecular lattice strength

A

weak

18
Q

molecular lattice bp and mp

A

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

19
Q

molecular lattice conductivity

A

cannot conduct electric charge- neutral molecules

20
Q

intramolecular bond

A

bond inside molecules (covalent bond)

21
Q

intermolecular force

A

force between molecules

22
Q

origin of london force

A

electrons randomly move around a molecule
at a point in times, electrons can exist more on 1 side of molecule forming a temporary dipole
when a temporary dipole comes close to a neighbouring, neutral molecule , this molecule polarises forming an induced dipole
the temporary and induced dipole electrostatically resulting in a london force

23
Q

hydrogen bond force

A

when hydrogen is bonded to a small highly electronegative atom, ( N,O,F) w/ at least 1 lone pair, hydrogen bonding occurs
the highly electronegative atom pulls the pair of electrons towards itself exposing a naked proton
the naked proton electrostatically attracts the lone pair of the neighbouring molecule

24
Q

phase change

A

intermolecular force overcome

25
Q

chemical change

A

intramolecular bond broken

26
Q

atomic lattice particles

A

atoms

27
Q

diamond lattice strength

A

extremely strong , generally hard

28
Q

diamond mp and bp

A

high
many strong,covalent bonds between atoms (4)
more energy required to break bonds

29
Q

diamond conductivity

A

poor electrical conductor
no charges to move to carry charge (neutral atom)

30
Q

graphite strength

A

extremely strong + hard
many strong covalent bonds between atoms (3 + 1unpaired e)

31
Q

graphite mp + bp

A

high
many strong,covalent bonds between atoms (3)
more energy required to break bonds

32
Q

graphite conductivity

A

good electrical conductor due to delocalised e-

33
Q

silicon dioxide mp+ bp

A

high
many strong,covalent bonds between atoms (3)
more energy required to break bonds

34
Q

silicon dioxide conductivity

A

poor conductor
no particles to move to carry charge (neutral atom)

physics (36 decks)

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