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Alevel > topic 2 > Flashcards

topic 2 Flashcards

1
Q

octet rule?

A

tendency for an atom to lose or gain electrons in order to achieve noble gas electron configuration

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2
Q

Ionic bond

A

strong electrostatic attraction between oppositely charged ions

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3
Q

what do ionic compounds form?

A

giant ionic lattices

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4
Q

factors affecting ionic bond strength

A

ionic charge and ionic radius

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5
Q

ionic properties (5)

A

conduct electricity when molten or dissolved, ions free to move
Hard brittle crystalline
doesn’t conduct when solid - ions fixed in place
insoluble in non polar solvent
soluble inn polar solvents

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6
Q

prove ionic solids have charged particles

A

dissolve KMnO4 onto wet filter paper, place on microscope slide and attach a current
purple MnO4- ions are observed to migrate towards positive terminal

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7
Q

Covalent bond

A

strong electrostatic attraction between shared pairs of electrons and the two nuclei

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8
Q

dative bond

A

a dative covalent bond involves one atom providing both the electrons in the shared pair

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9
Q

Mixed bonding

A

compounds contain both ionic and covalent bonds

NH4Cl

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10
Q

Factors affecting covalent bonds length

A

size of atom

number of pairs of e shared

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11
Q

electron deficient atoms

A

Be, Al, B

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12
Q

expanded octets can be….

A

P
S
Cl
Br

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13
Q

biggest repulsion order in shapes of molecules

A

L.P to L.P repulsion greater than
L.P to B.P repulsion which is greater than
B.P to B.P repulsion

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14
Q

polar covalent bond

A

shared e are drawn to atom with stronger pull on e

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15
Q

electronegativity?

A

ability for an atom to attract bonding in the covalent bond

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16
Q

Dipole

A

difference in electronegativity when polarisation occurs

cation attracts e of the anion

17
Q

what increases polarising power

A

high charge density

18
Q

electronegativity increases across group bc

A

increases N.C, constant shielding = increased attraction between valence e and nucleus

19
Q

electronegativity down group decreases bc

A

increased shielding and increased atomic radius = decreased attraction

20
Q

where do London forces exist

A

exist between all molecules

21
Q

how do London forces work

A

random electron movement in molecule to one side of molecule
creates temporary dipole
this temporary dipole created induced dipole for neighbouring molecule
two molecules now attracted

22
Q

what affects L.F

A

more electrons = more random e movement so bigger dipoles so stronger london forces

increased branching weakens london forces as molecules have less contact points and cant get as close to each other

23
Q

P:D to P;D

A

attraction between the partially positive and partially negative ends of a molecule

due to polar bonds

24
Q

Hydrogen bonding

A

attraction between the lone pair of electrons on an O,N or F atom and an electron deficient hydrogen bonded to an O, N or F atom

25
Q

why do alcohols have higher B.P than alkanes

A

alcohols have H.B, PD:PD bonding and London forces

alkanes only london forces

26
Q

boiling point of hydrogen halides

A

HF highest BP as it has H.B

increased BP from HCl to HI due to increased number of electrons creating stronger london forces

27
Q

how many hydrogen bonds does water form

A

4 HB forming a rigid 3d lattice

28
Q

why can ice float

A

ice forms an open lattice structure with molecules being further apart in solid state than in liquid

ice is less dense so it can float

29
Q

metallic bonding

A

electrostatic attraction between metal ion and sea of delocalised electrons creating a lattice

30
Q

properties of metallic bonding

A

good electrical conductor - delocalised e can carry current
good thermal conductor - energy transferred to delocalised e that move around rapidly conducting heat
High MP
Malleable - layers of atoms can slide over each other into different shapes

31
Q

Diamond structure

A

giant covalent structure with each c having 4 hydrogen bonds

32
Q

diamond properties (3)

A

hard - network of atoms
high mp
poor electric conductor as e fixed in place
good thermal conductor atoms pass vibrations rapidly along bonds in rigid structure

33
Q

Graphite structure

A

giant covalent structure each c contains 3 C.B

delocalised e form weak london forces between layers

34
Q

graphite properties

A

soft - weak L.F easily overcome - layers can slide over each other

high MP - alot of eneegry to overcome 3 covalent bonds

good electrical conductor - delcoalsied e can move throughout

35
Q

allotrope

A

different forms of the same element

36
Q

fullerene

A

simple covalent

each c has 3 covalent bonds

Alevel (30 decks)

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