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Chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

Ionice Bonding

A

strong electrostatic forces between oppositely charged ions

loss or gain or electrons

3D giant ionic lattice

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2
Q

Melting and Boiling poitns in ionic

A

very high

very strong electrostatic forces to break

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3
Q

Condutivity of Ionics

A

solids do not conduct but they do when they are molten or in solution as the ions are free to move

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4
Q

Covalent Bonding

A

sharing a pair of electrons

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5
Q

Co ordinate bond

A

formed between lone pairs of electrons and a H+ ion

both electron come from the same atom

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6
Q

2 types of covalent bonds

A

macro molecular

simple molecular

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7
Q

Macro Molecular mp and bp

A

very high as alot of energy is needed to break the string covalent bonds

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8
Q

simple molecular mp and bp

A

very low as you do not break the strong covalent bonds themselves but you break the weak intermolecular forces between them which does not require a lot of energy

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9
Q

Metalic Bonding

A

cations in a sea of delocalised electrons

metal atoms detached from their outer electrons

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10
Q

Conductivity of metals

A

very good conductors on either state as the energy is carried by the delocalised electrons

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11
Q

Malleable

A

can be beaten into shape easily without having to be broken

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12
Q

Sliding

A

layers of cations ‘slide’ over each other while still bonded by the elcetrons
sliding can occur in all dimensions

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13
Q

Down the Metal Group melting point

A

decreases
same number of delocalised electrons but cation gets larger
less attraction to so easily lost

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14
Q

Across a Metal Period melting point

A

increases
number of delocalised electrons increases
charge increases
stroner attraction so harder to remove

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15
Q

Across Metal Period conductivity

A

increases
more delcoalised electrons
more charge to carry energy

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16
Q

Polar Covalent Bond

A

occurs when electron pairs are shared unevenly

due to electronegativity

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17
Q

Electron pull in PCB

A

towards the more electronegativity

away from the less electronegativ atom

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18
Q

Partial Charge

A

Delta Positive

Delta Negative

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19
Q

Dipole

A

molecule which is still neutral but contains partial charge that cancel out each other

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20
Q

Dipole Dipole

A

stronger attrcation between neighboruing molecules which also contain partial charges

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21
Q

Melting and Boiling Point of PCB

A

higher than expected

22
Q

Solubility in Water of PCB

A

Increased solubility

23
Q

Elcetronegativity

A

Ability of an atom to attract a pair of electrons in a covalent bond

24
Q

increases

A

across periods

25
Q

decreases

A

up groups

26
Q

Nuclear Charge

A

more protons

stronger attraction between nucleus and bodning pair of electrons

27
Q

Aromic Radius

A

closer to the nucleus

stronger attraction between nucleus and bonding pair of electrons

28
Q

Shielding

A

less shells of electrons between the nucleus and the electrons
less shielding (less repulsion)
stronger attraction between nucleus and bonding pair of electrons

29
Q

Down a group Electronegativity

A

decreases
atomic radius increases
more shielding
less attraction between nucleus and bonding pair of electrons

30
Q

Across a period Electronegativity

A

increases
atomic radius decreases
more nuclear charge
stronger attraction between nucleus and bonding pair of electrons

31
Q

No Difference in Electronegativity

A

non polar covalent bond

32
Q

<0.5 electronegativity

A

covalent bond

33
Q

0.5<1.7 electronegativity

A

polar covalent bond

34
Q

> 1.7 electronegativity

A

ionic bond

35
Q

both electrongeativites <1.5

A

metalic bonding

36
Q

Intermolecular Forces

A

weak electrostatic forces of attraction between neighbouring molecules

37
Q

3 types of intermolecular forces

A

Hydrogen Bonding
Dipole-Dipole forces
Van de Walls forces

38
Q

Hydrogen Bonding

A

only between
Flourine, Oxygen, Nitrogen
deshielding the Hydrogen
making it slightly positive (delta positive)
attarction betweena lone pair on NOF and a deshielded hydrogen

39
Q

In Liquids Hydrogen Bonds

A

are continuosly breaking and reforming

40
Q

In Solids Hydrogen Bonds

A

are permanent

41
Q

In Gases Hydrogen Bonds

A

are completly broken

42
Q

As Electronegativity decreases Hydrogen Bond Strength

A

decreases

43
Q

Dipole Dipole Forces

A

uneven electron disribution

differences in electronegativity

44
Q

Permanet dipole causes

A

a permenant dipole in a neighbouring molecule

45
Q

Van De Waal Forces

A

weakest intermolecular force
atoms donate elctrons to the cloud
leading to a momentary tempory dipole

46
Q

when do Van De Waals occur

A

only happen when the other 2 intermolecular forces are not present
can occur when there is dipole dipole but they are disregarded

47
Q

VDW get stronger

A

as the number of electrons in the molecule increases

48
Q

Boiling Points of Noble Gases down the group

A

Increase

as electron shells are added

49
Q

starigh chain molecules

A

stronger van de waals forces

molecules can get closer

50
Q

branched chain molecules

A

weaker van de walls forces

molecules are less close

Chemistry (8 decks)

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