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chemistry a level > 2. bonding and structure (as) > Flashcards

2. bonding and structure (as) Flashcards

1
Q

ionic bonding

A

strong electrostatic attraction between oppositely charged ions

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2
Q

ionic bonding involves

A

the transfer of electrons from a metallic element to a non metallic element

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3
Q

ionic solids

A

ions in a lattice are arranged in a regular repeating pattern

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4
Q

ionic radius

A

measure of the size of an ion

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5
Q

ionic radii increases with
ionic radii decreases with

A

increasing negative charge
increasing positive charge

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6
Q

negative ions formed by

A

atoms gaining electrons

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7
Q

isoelectronic ions

A

ions that have the same electronic configuration

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8
Q

the type of lattice formed depends on

A

the sizes of positive and negative ions which are arranged in alternating fashion

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9
Q

why are most ionic compounds are solids at room temp

A

there isn’t enough energy to overcome the strong electrostatic forces of attraction between oppositely charged ions that make up the lattice

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10
Q

ionic compounds require

A

high temperatures required to make an ionic compound melt or boil

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11
Q

electrical conductivity of ionic compounds

A

in solid they cannot conduct electricity

but molten or aqueous ions they have ions that can move and carry charge

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12
Q

things that affect the strength of an ionic bond

A

ionic charge
ionic radii increases

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13
Q

ionic charges affects ionic bond how

A

greater charge of ion stronger the ionic bond ,, higher mp/bp

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14
Q

ionic radii explain how it affects ionic bond

A

smaller ions can be packed closer together than larger ions electrostatic attraction gets weaker with distance ,, small, closely packed ions have stronger ionic bonding

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15
Q

what happens to ionic radii down a group

A

ionic radii increases

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16
Q

what happens when isoelectronic ions ionic radii as atomic number increases

A

ionic radii decreases

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17
Q

some evidence is provided by physical properties of ionic compounds

A
  • high mps- strong attraction between ions
  • soluble in water but not non polar solvents- tells you that particles are charges ions pulled apart by polar molecules like water
  • don’t conduct electricity when solid- ions not free to move
  • brittle- if layers pulled same charged ions could be above each other ,, repulsion would be strong
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18
Q

migration of ions evidence for charged particles

A
  • copper (II) chromate (VI) solution is green on a piece of filter paper
  • cathode- filter paper is blue because copper ions- pos ions
  • anode- filter paper is yellow because of chromate ions- neg ions
19
Q

covalent bonds

A

strong electrostatic attraction between two positive nuclei and the shared electrons in the bond

20
Q

bond length

A

distance between the attractive and repulsive forces that balance each other between two nuclei

21
Q

relation between bond enthalpy and bond length

A

the greater the bond enthalpy the shorter the bond

22
Q

dative covalent bonding

A

one atom donates both electrons to a bond

23
Q

2 electron pairs around a central atoms name + bond angle

A

linear molecule
180 degrees

24
Q

3 electron pairs around a central atom no lone pair name + angle

A

trigonal planar
120

25
Q

3 electron pairs around a central atom 1 lone pair name + bond

A

non linear/ bent
119

26
Q

4 electron pairs around central atom no lone pair name + angle

A

tetrahedral
109.5

27
Q

4 electron pairs 1 lone pair name + angle

A

trigonal pyramidal
107

28
Q

4 electron pairs 2 lone pair name + angle

A

non linear/ bent
104.5

29
Q

5 electron pair no lone pair name + angle

A

trigonal bipyramidal
90 and 120

30
Q

5 electron pair one lone pair name + angle

A

seesaw
87 and 102

31
Q

5 electron pair two lone pair name + angle

A

distorted t
87.5

32
Q

6 electron pair no lone pair name + angle

A

octahedral
90

33
Q

6 electron pair one lone pair name + angle

A

square pyramidal
81.9 and 90

34
Q

6 electron pair two lone pair name + angle

A

square planar
90

35
Q

structure of diamond and silicon (IV) dioxide

A

each carbon atom bonded to 4 other and silicon is similar but has oxygen atoms between silicon

36
Q

properties of giant structure w covalent bonds + explain

A
  • high mp- require a lot of energy to break bonds
  • hard- strong bonds through lattice
  • good thermal conductors- vibrations travel easily through lattice
  • insoluble- covalent bonds are more attracted to their neighbours in lattice than solvent molecules. don’t have ions bcs insoluble in polar solvents
  • can’t conduct electricity- no charged ions/ free electrons
37
Q

why can graphite conduct electricity

A

3 carbon atoms covalently bonded ,, one free electron ,, carry charge

38
Q

graphene structure

A
  • sheet of graphite
  • joined together hexagonal
  • one atom thick
  • two dimensional
  • conducts electricity
  • strong
  • transparent
  • light
39
Q

metallic bonding

A

positive metal ions electrostatically attracted to the delocalised negative electrons forming a lattice of closely packed ions in a sea of delocalised electrons

40
Q

metals structure

A
  • high melting point- strong metallic bonds
  • malleable/ ductile- metal ions can slide over each other without disrupting attraction between pos ions + e
  • good thermal conductors- delocalised e can pass KE to each other
  • good electrical conductors- delocalised e to carry charge
  • insoluble- strength of metallic bonds
41
Q

what affects metallic bond

A
  • number of electrons
  • size of metal ions
  • charge of metal ions
42
Q

electronegativity def

A

the ability of an atom to attract the bonding electrons in a covalent bond

43
Q

most electronegative element

chemistry a level (20 decks)

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