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chemistry > physical chem; bonding > Flashcards

physical chem; bonding Flashcards

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1
Q

define the term ionic bonding

A

it’s the electrostatic force of attraction between oppositely charged ions formed electron transfer

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2
Q

what charge does group 1 form?

A

1+

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3
Q

what charge does group 2 form?

A

2+

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4
Q

what charge does group 3 form?

A

3+

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5
Q

what charge does group 5 form?

A

3-

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6
Q

what charge does group 6 form?

A

2-

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7
Q

what charge does group 7 form?

A

1-

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8
Q

list the molecular ions

A

OH⁻ = hydroxide
NO₃⁻ = nitrate
NH₄⁺ = ammonium
SO₄²⁻ = sulfate
CO₃²⁻ = carbonate

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9
Q

do ionic compounds dissolve in water & if so why?

A

yes
as water molecules are polar they can attract the +ve & -ve ions & break up the structure

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10
Q

explain the features of ionic structures

A

can conduct electricity when molten or dissolved as e- are free to move around

have high m.p as the structure has many strong electrostatic forces between oppositely charged ions = lots of energy required to overcome the forces

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11
Q

what makes an ionic bond stronger & provide an example

A

when the ions are smaller/have higher charges
e.g. MgO has a higher m.p than NaCl as MgO’s ions are smaller & have higher charges (2+ & 2-) compared to NaCl (1+ & 1-)

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12
Q

explain the trend of ionic radii in groups & why

A

increases down a group as ions have more shells of e- down a group

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13
Q

define the term covalent bonding

A

its an electrostatic attraction between the shared e- & +ve nucleus

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14
Q

what is a dative/coordinate bond?

A

its a bond where 1 atom donates 2 e- to an atom/ion

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15
Q

give examples of compound that have dative bonds

A

NH₄⁺
H₃O⁺
NH₃BF₃

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16
Q

give examples of giant covalent structures

A

graphite
diamond

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17
Q

what is a covalent simple molecular structure & give examples

A

simple molecular - IMF (van der waals, permanent dipoles, H bonds) between molecules

e.g. iodine, ice, CO₂, H₂O & CH₄

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18
Q

what is a covalent macromolecular structure & give examples

A

it’s a giant molecular structure held together by many strong covalent bonds

e.g. diamond, graphite, silicon dioxide & silicon

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19
Q

describe the structure of graphite

A

layers slide easily as there are weak forces between the layers
delocalised e- between layers allow graphite to conduct electricity as they can carry a charge
has low density - as layers are far apart compared to bond length
many strong covalent bonds = high m.p

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20
Q

describe the structure of diamond

A

good heat conductor - has a tightly packed, rigid arrangement
many very strong covalent bonds = high m.p
doesn’t conduct electricity well as doesn’t have any delocalised e-

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21
Q

describe the similarities in the structures of graphite & diamond

A

they both and many strong covalent bonds and are both insoluble due to the strength of their bonds

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22
Q

define the term metallic bonding

A

it’s the electrostatic force of attraction between the metal +ve ions & the delocalised e-

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23
Q

what structures do metals have?

A

giant metallic structures

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24
Q

describe the structure of giant metallic lattices

A

they have +ve metal ions which are formed as metals donate e- to form a sea of delocalised e-

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25
Q

describe the features of metallic structures

A

high m.p - due to strong electrostatic attractions

good electrical conductors - delocalised e- are mobile & can carry electrical currents

good thermal conductors - delocalised e- can transfer KE

are insoluble as metallic bonds too strong to break

26
Q

what makes a metallic bond stronger & provide an example

A

the more e- an atom can donate to the delocalised e- system = higher m.p
e.g. Mg has a higher m.p than Na as Mg can donate 2 e- whereas Na can only donate 1 e-

27
Q

name the structure of a shape & its bond angle with 2 bonding pairs & 0 lone pairs

A

linear
180º

28
Q

name the structure of a shape & its bond angle with 3 bonding pairs & 0 lone pairs

A

trigonal planar
120º

29
Q

name the structure of a shape & its bond angle with 4 bonding pairs & 0 lone pairs

A

tetrahedral
109.5º

30
Q

name the structure of a shape & its bond angle with 5 bonding pairs & 0 lone pairs

A

trigonal bipyramidal
120º & 90º

31
Q

name the structure of a shape & its bond angle with 6 bonding pairs & 0 lone pairs

A

octahedral
90º

32
Q

name the structure of a shape & its bond angle with 3 bonding pairs & 1 lone pair

A

pyramidal
107º

33
Q

name the structure of a shape & its bond angle with 2 bonding pairs & 2 lone pairs

A

bent
104.5º

34
Q

name the structure of a shape & its bond angle with 4 bonding pairs & 2 lone pairs

A

square planar
90º

35
Q

define the term electronegativity

A

it’s the ability of an atom to attract a pair of e- in a covalent bond

36
Q

what is the most electronegative atom?

A

fluorine

37
Q

list the most electronegative atoms

A

F, O, N & Cl

38
Q

state the general trend of electronegativity in the periodic table

A

electronegativity increases the further up & right you in the periodic table

39
Q

state the factors that affect electronegativity

A

nuclear charge:
increase in no.of protons = increased electronegativity

atomic radius:
its the distance between e- & nucleus - increased atomic radius = decreased electronegativity

shielding:
its the no.of shells & subshells - increased shielding = decreased electronegativity

40
Q

how do covalent bonds become polar?

A

when atoms attached have a difference in electronegativity

41
Q

how do we know if a compound is polar?

A

atoms will have either a delta +ve (on least electronegative atom) / delta -ve (on most electronegative atom)

42
Q

how do we know if an atom is non-polar?

A

if the atoms bonded have the same / similar electronegativities

43
Q

what causes a bond to be more polar?

A

the bigger the difference in electronegativity = the more polar a bond will be

44
Q

what is the difference between intramolecular & intermolecular forces?

A

intramolecular = forces within a molecule & are usually covalent bonds

intermolecular forces = forces between molecules

45
Q

give an example of a molecule with intramolecular forces

A

water
O - H bond within the molecule

46
Q

give an example of a molecule with intermolecular forces

A

water
H bond between 2 water molecules

47
Q

name the types of intermolecular forces from strongest to weakest

A

H bonding
permanent dipole-dipole forces
induced dipole-dipole forces (AKA van der waals)

48
Q

how do induced dipole-dipole (van der waals) forces form?

A

any molecule/atom with e- can form induced dipole when it moves near an atom/molecule
more e- in molecule = higher change induced dipole will form

49
Q

explain whether an induced dipole-dipole force is permanent/temporary & why

A

interaction between 2 molecules is temporary & only exists when they are nearby
when they move apart, the interaction is destroyed

50
Q

state which intermolecular forces can be found in hydrocarbons & how they affect its properties

A

van der waals
straight, long hydrocarbons have more van der waals = more energy needed to overcome forces - m.p increases

51
Q

explain how the arrangement of branched hydrocarbons affects its b.p

A

branched hydrocarbons can’t pack together as close which weakens van der waals = lowers b.p

52
Q

what are permanent dipole-dipole interactions?

A

there are weak electrostatic forces that exist in molecules with a polarity

53
Q

what is the difference between van der waals & permanent dipole-dipole interactions?

A

permanent dipoles are stronger - have a higher m.p

54
Q

name the other type of intermolecular forces found in molecules that have permanent dipole-dipole interactions

A

van der waals

55
Q

explain how we can identify polar molecules

A
  1. place a charged rod near a steady stream of a polar liquid
  2. if polar molecules are present the liquid will bend towards the rod as the molecules align to face the oppositely charged rod
56
Q

when does hydrogen bonding occur?

A

between hydrogen & NOF

57
Q

name the other types of intermolecular forces found in molecules that have H bonding

A

van der waals & permanent dipole-dipole interactions

58
Q

how are H bonds shown in diagrams?

A

shown by using dotted lines

59
Q

explain why ice is less dense than water

A

ice forms a regular structure held by H bonds. & the molecules are further apart which makes it less dense than water

60
Q

explain the boiling points trend of hydrogen halides using examples

A

HF has a higher b.p than HCl as it H bonding - more energy is needed to overcome electrostatic forces

there is a slight increase in b.p from HCl to HI due to the increased mass of molecule = bigger e- cloud - more van der waals

chemistry (34 decks)

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