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Chemistry Physical > bonding > Flashcards

bonding Flashcards

1
Q

what is a symbol for nitrate ion

A

NO3-

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2
Q

what is the symbol for a ammonium ion

A

NH4+

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3
Q

what is the symbol for a sulfate ion

A

SO4 2-

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4
Q

what is the symbol for a carbonate ion

A

CO3 2-

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5
Q

what are the steps to working out the formula of an ionic compound

A

1- write the 2 ions
2- swap the charges
3- drop the charges
4- simplify to the whole number ratio

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6
Q

workout the formula for this

Ca2- and O2+

A

Ca2+ and O2-
Ca2 and O2
Ca2O2

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7
Q

what is a giant ionic structure like

A

regular cubic shape
giant repeating pattern

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8
Q

why do ionic compounds have high melting points

A

strong electrostatic forces of attraction and requires lots of energy to overcome

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9
Q

where is the electrostatic attraction in a covalent bond

A

between the shared electrons and the nucleus

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10
Q

what is a Dative covalent bond

A

when one atom donates 2 electrons to form a bond

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11
Q

what usually represents a dative covalent bond

A

an arrow

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12
Q

describe the structure of graphite

A

each carbon bonded 3 times with 4th electron delocalised

layers which can slide over each other

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13
Q

why can graphite conduct electricity

A

delocalised electrons between the layers which can carry a charge

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14
Q

describe the properties of graphite

A

can conduct electricity

insoluble as covalent bonds too strong to break

layers are far apart so low density

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15
Q

why can diamond conduct heat well

A

its tightly packed and rigid

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16
Q

why cant diamond conduct electricity

A

no delocalised electrons

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17
Q

what do lone pairs do to bonding pairs

A

push them closer together

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18
Q

how many bond pairs and lone pairs does a linear shape have

whats the bond angle

A

2 bond pairs 0 lone

180

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19
Q

how many bond pairs and lone pairs does a trigonal planar have

whats the bond angle

A

3 bond pairs 0 lone

120

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20
Q

how many bond pairs and lone pairs does a tetrahedral have

whats the bond angle

A

4 bond pairs 0 lone

109.5

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21
Q

how many bond pairs and lone pairs does a
trigonal bipyramidal have

whats the bond angle

A

5 bond pairs 0 lone

90 and 120

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22
Q

how many bond pairs and lone pairs does a octahedral have

whats the bond angle

A

6 bond pairs 0 lone

90

23
Q

how many bond pairs and lone pairs does a pyramidal shape have

whats the bond angle

A

3 bonded 1 lone

107

24
Q

how many bond pairs and lone pairs does a bent molecule have

whats the bond angle

A

2 bonded 2 lone

104.5

25
Q

how many bond pairs and lone pairs does a trigonal planar have

whats the bond angle

A

3 bonded and 2 lone

120

26
Q

how many bond pairs and lone pairs does a square planar have

whats the bond angle

A

4 bonded and 2 lone

90

27
Q

what is electronegativity

A

the ability for an atom to attract electrons toward itself in a covalent bond

28
Q

how does electronegativity change as you go across the periods

A

it increases

29
Q

how does electronegativity change down the groups

A

decreases

30
Q

describe the trend of electronegativity on the periodic table as a whole

what does this exclude

A

the further up and right you go the more electronegative the element is

the noble gases

31
Q

when do covalent bonds become polar

A

when atoms attached to it have a difference in electronegativity

32
Q

the bigger the difference in electronegativity the more what

A

the more polar the bond will be

33
Q

atoms with the same electronegativity are not what

A

polar

34
Q

what are van der waals

A

weak forces that exist between atoms and molecules

35
Q

van der waals are w—-

A

weak

36
Q

when do temporary dipoles form

A

when 2 molecules are near by and electrons are unevenly distributed

37
Q

what determines how many van der waals the atom has

A

how big the molecule or atom is

38
Q

why do long straight chain hydrocarbons have higher boiling points

A

they have more van der waals which need breaking

39
Q

what is a dipole dipole

A

weak electrostatic force within polar molecules

40
Q

why are dipole dipoles strong

A

they are permanent

41
Q

why are dipole dipoles strong

A

they are permanent

42
Q

when is hydrogen bonding strongest

A

when u have very electronegative elements

43
Q

when does hydrogen bonding occur

A

when one molecule of hydrogen forms a bond with a lone pair of nitrogen, oxygen or fluorine

44
Q

describe the structure of metals

A

giant metallic lattice structures

45
Q

the more atoms a metal can donate the what

A

higher the melting point

46
Q

what kind of crystal structure does iodine have

A

molecular

47
Q

what kind of crystal structure does graphite have

A

giant covalent lattice

48
Q

describe the structure and bonds of graphite

A

layers of carbon atoms
van der waals between layers
strong covalent bonds

49
Q

why does something like iodine vaporize when heated

A

van der walls are weak
van der walls between molecules

50
Q

define electronegativity

A

the ability to attract shared electrons to an atom in a covalent bond

51
Q

why does sulfur having a higher melting point then phosphorus

A

sulfur is larger so more energy is needed to break molecules

52
Q

why are argons van der walls weak

A

argon exists as a single atom so cannot be easily broken

53
Q

why is the bonding of nitrogen oxide covalent instead of ionic

A

small difference in electronegativity

Chemistry Physical (5 decks)

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