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Chemistry > Bonding And Structure > Flashcards

Bonding And Structure Flashcards

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1
Q

ionic bonding

A

electrostatic forces of attraction between oppositely charged ions

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2
Q

factors effecting strength of ionic bonds

A
  • ion charges
  • ionic radii
  • effects the strength of attraction between oppositely charged ions
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3
Q

formation of ions

A

loss or gain of electrons

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4
Q

isoelectronic ion radii effects

A

Electron configuration remains constant

  • change in nuclear charge
  • change in strength of attraction between nucleus and electrons
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5
Q

isoelectronic

A

ions that have the same number of electrons

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6
Q

trend in atomic radii down a group

A
  • radii increases
  • ions have the same charge
  • atoms get larger as they gain shells
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7
Q

physical properties of ions as evidence for ions

A
  • high melting and boiling points indicate the strong electrostatic forces existing between the oppositely charged ions in ionic compounds
  • ability to conduct electricity when molten or ion solution shows that mobile charge carrying particles exist in these substances
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8
Q

dashed line in a displayed formula

A

going into the page

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9
Q

blocked out triangle in displayed formula

A

coming out of the page

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10
Q

migration of ions as evidence for ions

A

a rectangle of filter paper soaked in water is placed on a slide, electrodes connected and a crystal of ionic material placed between the electrodes

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11
Q

covalent bonding

A

electrostatic force of attraction between nuclei and shared pair of electrons

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12
Q

dative covalent bonding

A

when both electrons that are shared come from one atom

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13
Q

physical properties of simple covalent

A

weak intermolecular forces between the molecules
Little energy is needed to overcome these forces
melting and boiling points are low

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14
Q

physical properties of giant molecular

A

strong covalent bonds
require a large amount of energy to overcome
high melting and boiling point

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15
Q

conductivity of covalent molecules

A

do not have free electrons
non-conductors of electricity
Graphite is exceptional in that it does have free electrons and so is a conductor

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16
Q

Single covalent bond strength

A
  • change in atomic radii
  • change in distance between nuclei and shared electron pair
  • change in the strength of a attraction between nuclei and shared pair of electrons
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17
Q

sigma bond

A

exists directly between the two atoms; it lies symmetrically along an axis joining the two nuclei

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18
Q

pi bond

A

made up of two halves forming a double bond

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19
Q

expanding the octet

A

the process of splitting electron pairs means that an atom in a compound can have more than 8 electrons

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20
Q

electron pair repulsion theory

A

electrons are all negatively charged and so will repel each other each electron region takes up a position to minimise repulsion

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21
Q

electronegativity

A

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

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22
Q

polarisation

A

one atom will have a greater electronegativity than the other
will have a greater pull on the electrons
distorting the electron region

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23
Q

cause of polar bonds

A

one atom has a higher electronegativity
one atom become more negative
electrons are closer to that atom

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24
Q

three types of intermolecular forces

A

London forces
permanent dipole
hydrogen bonds

25
Q

testing polar molecules

A

place a electrostatically charged rod next to jet of liquid and see if the jet attracts or repels

26
Q

dipole

A

The separation of charge which exists in a polar molecule

27
Q

permanent dipole

A

In a polar material there is an attraction between the positive charge in one molecule and the negative charge in the other

28
Q

London forces

A
  • instantaneous dipole in one molecule
  • induces a dipole in the other molecule
  • the delta + of one attracts the delta - of the other
  • more electrons per atom/molecule yields stronger London forces
29
Q

strength of london forces

A

more electrons per atom/molecule

30
Q

order of strength of IMF

A

weakest=london forces
permanent dipole
strongest=hydrogen bonds

31
Q

which elements does H-bonding occur in and why

A

Nitrogen, fluorine and oxygen
high electronegativity
lone pair of electrons
region of negative charge is attracted towards the exposed proton on the hydrogen in another atom

32
Q

where are each IMF found

A

LF in all substances
permanet dipole in polar substances
H-bond in compounds of NOF with H

33
Q

trend of boiling points in alkanes

A

increase with molecular mass
more electrons so stronger london forces
branched alkanes have lower boiling points as less contact points for bonds

34
Q

trend of boiling points of alcohols

A

The –OH group in alcohols causes hydrogen bonding between the molecules. Therefore an alcohol will have a much higher boiling point than an alkane with a similar number of electrons

35
Q

trend of boiling point of hydrogen halides

A

increase down the group with molecular mass
LF stronger
HF forms h-bonds so highest BP

36
Q

high bp means high or low volatility

A

low volatility

37
Q

physical properties of water

A

high mp and bp

can form two hydrogen bonds

38
Q

what happens when water freezes

A

hydrogen bonds form an open lattice
low density
ice is on the surface acting as an insulator
water beneath remains liquid

39
Q

solubility and IMF

A

if solvents and substances have similar IMF they tend to dissolve

40
Q

solubility of ionic compounds in water

A

polar water attracts ions=hydration
water is shaking so as they bond the ions break free from the lattice
sometimes electrostatic forces are to strong to break

41
Q

solubility of organic compounds in water

A

Alcohols are soluble can form hydrogen bonds with water
water will not dissolve substances which are not ionic or able to form hydrogen bonds
the dissolving process involves molecules of the dissolving substance to intersperse themselves between the water
strong hydrogen bonds prevent other molecules from moving between water unless they are able to form equally strong interactions with water

42
Q

solubility in non-polar solvents

A

dissolve non-polar substances

as have similar IMF so can interact

43
Q

metallic bonding

A

electrostatic force of attraction between positive metal ions and delocalised electrons

44
Q

physical properties of metallic bonding

A

delocalised electrons allow for conduction of electricity and heat
absence of fixed bonds allows the ions to move layers slide over each other=malleability and ductility

45
Q

factors affecting strength of covalent bonds

A

number of electrons shared

distance between nuclei

46
Q

factors affecting the strength of metallic bonds

A
  • change in ionic charges
  • change in ionic radii
  • delocalised electrons per ion
  • change in strength of attraction between cations and delocalised electrons
47
Q

type of structure in ionic

A

giant lattice

strong electrostatic attraction

48
Q

types of structure in covalent

A

giant lattice strong covalent bonds

simple molecular strong covalent bonds with weak IMF

49
Q

type of structure in metallic

A

giant lattice

strong electrostatic attraction

50
Q

structures formed by carbon

A

graphite
diamond
graphene

51
Q

physical properties of diamond

A

strong covalent bonds
high mp bp
non-conductor
hardest natural substance

52
Q

physical properties of graphite

A 
strong covalent bonds and LF
high mp bp
one electron free per atom as only three bonds=conductor
layers can slide=lubricant
non-reactive=electrolysis electrode
53
Q

Multiple covalent bond strength

A
  • change in number of shared electron pairs
  • change in distance between nuclei and shared electron pairs
  • change in strength of attraction between nuclei and shared electron pairs
54
Q

Explain shape with all bonds

A
  • minimise repulsion between electron pairs

- number of bonding electron pairs

55
Q

Explain shape with lone pairs

A
  • minimise repulsion between electron pairs
  • number of bonding and lone electron pairs
  • lone electron pairs repel more than bonding electron pairs
56
Q

Electronegativity across a period

A
  • distance and shielding between nucleus and electron pair is constant
  • change in nuclear charge
  • change in attraction between nucleus and electron pair
57
Q

Electronegativity down a group

A
  • change in distance and shielding between nucleus and electron pair
  • change in nuclear charge
  • change in the attraction between nuclei and electron pair
58
Q

Hydrogen bonds

A

O/N/F are very electronegative

  • causing the bond with H very polar
  • H delta + attracts lone pair of ONF from other molecule

Chemistry (19 decks)

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