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Physical Chemistry > 3.1.3 - bonding > Flashcards

3.1.3 - bonding Flashcards

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1
Q

how are ions formed?

A

when electrons are transferred from one atom to another

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2
Q

equations showing the formation of a cation
(sodium)

A

Na = Na+ + e-

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3
Q

equations showing the formation of an anion
(chlorine)

A

Cl + e- = Cl-

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4
Q

what do elements in the same group have in common?

A

they all have the same number of outer elctrons

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5
Q

what is the trend of charges of ions in the same group?

A

when elements in the same group form ions, they all have the same charge

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6
Q

what charge ions would group one elements form?

A

1+ ions

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7
Q

what charge ions would group seven elements form?

A

1- ions

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8
Q

what are compound ions?

A

ions made up of groups of atoms with an overall charge

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9
Q

examples of compound ions

A

ammonium, carbonate, hydroxide, nitrate, sulfate

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10
Q

ionic formula for an ammonium ion

A

(NH4)+

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11
Q

ionic formula for a carbonate ion

A

(CO3)2-

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12
Q

ionic formula for a hydroxide ion

A

OH-

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13
Q

ionic formula for a nitrate ion

A

(NO3)-

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14
Q

ionic formula for a sulfate ion

A

(SO4)2-

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15
Q

what is ionic bonding?

A

the net electrostatic attraction between oppositely charged ions

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16
Q

general ionic structure

A

-ions arranged in giant lattice
-cations/anions arranged alternately
-3D array
-lattice is very strong (many ionic bonds)

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17
Q

do ionic compounds conduct electricity?

A

ionic compounds conduct electricity when they are molten or dissolved but not when solid

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18
Q

explanation for ionic compounds conductivity

A

ions in a liquid are free to move and they can carry a charge. in a solid they’re fixed in position by the strong ionic bonds

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19
Q

ionic compounds melting point

A

ionic compounds have high melting points

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20
Q

explanation for ionic compounds melting point

A

giant ionic lattices are held together by strong electrostatic forces which takes lots of energy to overcome them

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21
Q

ionic compounds and solubility

A

ionic compounds tend to dissolve in water

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22
Q

explanation for ionic compounds solubility

A

water molecules are polar so the water molecules pull the ions away from the lattice and cause it to dissolve

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23
Q

ionic formula for a sulfite ion

A

(SO3)2-

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24
Q

when does ionic bonding occur?

A

if there is a big difference in electronegativities i.e. metals and non metals

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25
Q

when does covalent bonding occur?

A

electronegativities are identical/similar (and high) i.e. non metals

26
Q

what is covalent bonding?

A

the sharing of pairs of electrons between non metal atoms to form molecules or giant structures so they both have a full outer shell

27
Q

what is a covalent bond defined as?

A

a shared pair of electrons

28
Q

single covalent bonds

A

contains 1 shared pair of electrons. the positive nuclei are attracted electrostatically to the shared electrons

29
Q

double covalent bonds

A

2 shared pairs of electrons

30
Q

triple covalent bonds

A

3 shared pairs of electrons

31
Q

covalent molecular substances melting and boiling points

A

covalent molecular substances have low melting and boiling points

32
Q

explanation for covalent molecular substances melting and boiling points

A

only intermolecular forces are broken during boiling and melting , these forces are weak so require little energy to break

33
Q

do covalent molecular substances conduct electricity?

A

No as there are no mobile charged particles - electrons aren’t free to move

34
Q

what holds covalently bonded atoms together?

A

electrostatic attraction between positive nuclei and the negative electron pairs shared between those nuclei

35
Q

graphite structure

A

carbon atoms arranged in sheets of flat hexagons, covalently bonded with 3 bonds each. 4th outer electron of each carbon atom is delocalised. sheets of hexagons bonded together by weak Van der Waals forces

36
Q

uses of graphite

A
  • dry lubricant
  • pencils
37
Q

why is graphite soft?

A

weak bonds between the layers in graphite are easily broken, so the sheets can slide over each other

38
Q

is graphite a conductor and why?

A

yes, delocalised electrons in graphite are free to move along the sheets so an electric current can flow

39
Q

graphite - density

A

layers far apart compared to the length of the covalent bonds so graphite has a low density = used to make strong/lightweight sports equipment

40
Q

graphite melting point

A

strong covalent bonds in the hexagon sheets so graphite has a high melting point

41
Q

graphite solubility

A

insoluble in any solvent as the covalent bonds in the sheets are too difficult to break

42
Q

diamond structure

A

made up of carbon atoms, each of which is covalently bonded to 4 other carbon atoms. tetrahedral shape

43
Q

diamond melting point

A

has a high melting point as its strong covalent bonds require lots of energy to break

44
Q

diamond - hard or soft?

A

due to its strong covalent bonds it is very hard , used in diamond-tipped drills and saws

45
Q

diamond - thermal conductivity

A

vibrations travel easily through the stiff lattice so is a good THERMAL conductor

46
Q

diamond - does it conduct electricity?

A

doesn’t conduct electricity = all outer electrons held in localised bonds/no delocalised electrons

47
Q

diamond- solubility

A

diamond won’t dissolve in any solvent

48
Q

define metallic bonding

A

net attraction between cations and delocalised electrons

49
Q

metallic bonding structure

A

lattice of closely packed cations in a sea of delocalised electrons

50
Q

metals - melting points

A

high melting points = strong metallic bonds between cations and delocalised electrons, lots of energy to break them

51
Q

metals - melting point as you go down a group

A

melting point decreases as you go down a group

52
Q

metals - melting point as you go down a group explanation

A

as there are the same number of delocalised electrons per atom but cations get heavier/larger so less strongly held in place by attraction of fixed number of delocalised electrons

53
Q

metals - melting point across a period

A

across a period, melting point increases

54
Q

metals - melting point across a period explanation

A

the number of delocalised electrons per atom increases and so does the charge on cations. therefore more strongly held in place by increasing force of attraction

55
Q

metals - conductivity across a period

A

conductivity increases as you go along a period as the number of delocalised electrons increases

56
Q

metals - malleability

A

layers of cations can slide over each other, still bonded by delocalised electrons so metals are malleable and ductile

57
Q

metals - conductivity (thermal)

A

delocalised electrons can pass kinetic energy to each other so they are good thermal conductors

58
Q

metals - electrical conductivity

A

good electrical conductors, delocalised electrons can move and carry a charge

59
Q

metals - solubility

A

insoluble except in liquid metals, because of the strength of the metallic bonds

60
Q

co-ordinate/dative covalent bond

A

covalent bond formed when both shared electrons are provided by only one atom e.g. pair comes from a lone pair on the donor atom. the atom sharing the lone pair must have an incomplete outer energy level

Physical Chemistry (4 decks)

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