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Bonding And Structure Flashcards

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
testing polar molecules
place a electrostatically charged rod next to jet of liquid and see if the jet attracts or repels
26
dipole
The separation of charge which exists in a polar molecule
27
permanent dipole
In a polar material there is an attraction between the positive charge in one molecule and the negative charge in the other
28
London forces
- 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
strength of london forces
more electrons per atom/molecule
30
order of strength of IMF
weakest=london forces permanent dipole strongest=hydrogen bonds
31
which elements does H-bonding occur in and why
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
where are each IMF found
LF in all substances permanet dipole in polar substances H-bond in compounds of NOF with H
33
trend of boiling points in alkanes
increase with molecular mass more electrons so stronger london forces branched alkanes have lower boiling points as less contact points for bonds
34
trend of boiling points of alcohols
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
trend of boiling point of hydrogen halides
increase down the group with molecular mass LF stronger HF forms h-bonds so highest BP
36
high bp means high or low volatility
low volatility
37
physical properties of water
high mp and bp | can form two hydrogen bonds
38
what happens when water freezes
hydrogen bonds form an open lattice low density ice is on the surface acting as an insulator water beneath remains liquid
39
solubility and IMF
if solvents and substances have similar IMF they tend to dissolve
40
solubility of ionic compounds in water
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
solubility of organic compounds in water
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
solubility in non-polar solvents
dissolve non-polar substances | as have similar IMF so can interact
43
metallic bonding
electrostatic force of attraction between positive metal ions and delocalised electrons
44
physical properties of metallic bonding
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
factors affecting strength of covalent bonds
number of electrons shared | distance between nuclei
46
factors affecting the strength of metallic bonds
- change in ionic charges - change in ionic radii - delocalised electrons per ion - change in strength of attraction between cations and delocalised electrons
47
type of structure in ionic
giant lattice | strong electrostatic attraction
48
types of structure in covalent
giant lattice strong covalent bonds | simple molecular strong covalent bonds with weak IMF
49
type of structure in metallic
giant lattice | strong electrostatic attraction
50
structures formed by carbon
graphite diamond graphene
51
physical properties of diamond
strong covalent bonds high mp bp non-conductor hardest natural substance
52
physical properties of graphite
``` 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
Multiple covalent bond strength
- 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
Explain shape with all bonds
- minimise repulsion between electron pairs | - number of bonding electron pairs
55
Explain shape with lone pairs
- minimise repulsion between electron pairs - number of bonding and lone electron pairs - lone electron pairs repel more than bonding electron pairs
56
Electronegativity across a period
- distance and shielding between nucleus and electron pair is constant - change in nuclear charge - change in attraction between nucleus and electron pair
57
Electronegativity down a group
- change in distance and shielding between nucleus and electron pair - change in nuclear charge - change in the attraction between nuclei and electron pair
58
Hydrogen bonds
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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