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a level chemistry - bonding and structure > ionic and metallic bonding > Flashcards

ionic and metallic bonding Flashcards

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1
Q

what is a lattice?

A

regular repeating structure e.g. lattice pie

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2
Q

ion

A

charged particle - atom lost/gained one or more electrons resulting in a acharge and a stable electronic structure

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3
Q

electrostatic attraction

A

attraction between positively charged and negatively charged particles (protons and electrons or positive and negative ions

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4
Q

ionic bond

A

electrostatic attraction between oppositely charged ions

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5
Q

ionic lattice

A

arrangement of ions into a large structure consisting of alternating positive and negative ions

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6
Q

why does the top of group 4 not form ions?

A

Ge, Sn, Pb form ions - positive because they’re metal
C, Si, do not form ions as too much energy is required to lose/gain electrons

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7
Q

why do group 0 not form ions?

A

full outer shells

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8
Q

cation

A

positive ions

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9
Q

anions

A

negative ions

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10
Q

why do non-metals usually get negative chargers

A

require less energy to gain electrons

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11
Q

why do metals usually get positive chargers

A

require less energy to lose electrons

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12
Q

when do complex ions usually form?

A

when groups of atoms which are covalently bonded gain or lose electrons to form full outer shells of all elements within them

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13
Q

examples of complex ions you must know

A

sulfate - SO4 ^2-
nitrate - NO3 -
carbonate - CO3 ^2-
hydroxide - OH-
ammonium - NH4 +

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14
Q

what affects the size of an ion?

A

shielding, nuclear charge, charge of an ion

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15
Q

how does the size of an ion change as you move down a group in the periodic table?

A
  • bigger down the group, more shielding, nuclear charge is outweighed by shielding increase, same charge
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16
Q

how does the size of an ion change as you move across a period in the periodic table?

A

shielding stays the same, increase nuclear charge, ion size decreases (negative ions have more electrons than protons)

17
Q

what affects the strength of ionic bonding?

A
  • ionic radius
  • charge of ions
    higher charge = stronger attraction
    smaller radii = stronger attraction = can get closer
    shielding on + ions reduces attraction
    shielding on - ions increases distance
18
Q

why are the melting points of ionic compounds high?

A

it has very strong electrostatic attractions, requires lots of energy needed to break attractions

19
Q

why is solubility good in ionic compounds

A

water is polar and attracts ions

20
Q

why is conductivity good as liquid/aqueous in ionic bonding?

A

ions are free to move and carry a charge

21
Q

delocalised electrons

A

not tied to a particular atom, but are free to move throughout a structure. in a metal, these came from the outer shell of the metal atoms

22
Q

metallic lattice

A

giant, regular, repeating structure of positive metal ions existing in a sea of delocalised electrons

23
Q

metallic bond

A

electrostatic attraction between positively charged metal ions and their sea of delocalised electrons

24
Q

why is the melting point of metals high?

A

strong electrostatic attractions which require a lot of energy to overcome

25
Q

why is the conductivity good in metals?

A

they have delocalised electrons - can carry a charge as they move

26
Q

how are metals strong

A

strong electrostatic forces holding it together

27
Q

why are metals malleable and ductile?

A

layers slide but stay attracted to delocalised electrons

28
Q

what affects the strength of metallic bonding

A
  • ionic radius - less shielding/smaller ions = stronger attraction to delocalised electrons
  • charge of ions - higher charge = stronger attraction
  • number of delocalised electrons - more delocalised electrons = stronger attraction
29
Q

trend in melting points of group 1 metals

A
  • decrease down group - more shells requires less energy to overcome electrostatic forces of attraction between delocalised electrons and ions
  • ionic radius increases
  • cahrge doesn’t affect - stays the same
  • delocalised electrons don’t affect
30
Q

crystal stucture

A

type of bonding present in the solid state of that substance - e.g. ionic, metallic, molecular, giant covalent

31
Q
A

a level chemistry - bonding and structure (2 decks)

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