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john 2 Flashcards

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1
Q

across period 2 Li Be etc, what is bond strength determined by

A

the bond order of each one determined by MO theory.

0 bo = weakest bond, bond doesn’t exist between the 2

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2
Q

highest and lowest bond strength for period 2 elements

A

highest bond strength = N2 (3)
lowest bond strength = Be2 (0)

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3
Q

what causes the zig zag like bond strength tree in period 2

A

first: bonding orbitals are not filled so low strength

2nd: antibonding orbitals are being filled so lower strength

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4
Q

what state are N O and F at room temp

A

diatomic gases

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5
Q

what are Li Be B and C in room temp

A

solids

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6
Q

diatomic period 2 strongest bond

A

N2
bond order of 3
(use mo diagram)

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7
Q

single molecular period 2 strongest bonding

A

C
(graphite and diamond)
based on enthalpy of atomisation ( s-> g)

period 3 follows the same trend with group 14, Si on top

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8
Q

what period have the greatest enthalpy of atomisation

A

2
3 is lower apart from their group 17 and 16
S (solid) and Cl (larger enthalpy of atomisation than F bc of weak FF bond due to the side of F)

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9
Q

why does carbon have the strongest enthalpy of atomisation

A

group 14
4 valence electrons
4n electrons for 4 bonding Mo
n= number of atoms

more or less e- = fewer bonding or more antibonding filled

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10
Q

group 14
state, bond length, shape, hybrid

A

solids at room temp
bond length increases down the group
tetrahedral 109.5 (tetravalent)
sp3 hybrids

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11
Q

allotrope meaning

A

different physical form of an element
carbon + graphite (most stable)
carbon + diamond (not most stable)

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12
Q

graphite carbon allotrope

A

most stable carbon allotrope
hexagonal layers of sp2
slanted hexagonal layers (ababab)
e- delocalised into pi orbital (double bond character)

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13
Q

all the carbon allotropes

A

diamond
graphite
graphene
fullerenes

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14
Q

diamond allotrope

A

each c is tetravalent
sp3 hybridised
not most stable allotrope
tetrahedral shape of C
109.5 *

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15
Q

graphite allotrope

A

Sp2 hybridised carbon
1e- delocalised into Pi orbital
double bond character
layers of hexagonal planes slanted
ababab shape
hexagonal layers most stable allotrope

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16
Q

graphene C allotrope

A

one single layer of graphite
1 hexagonal layer

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17
Q

fullerene C allotrope

A

a graphene layer but rolled up into a cylinder

closed sheet of graphene
sheet of hexagons and pentagons (allow bending)
sheet is wrapped around and joined up

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18
Q

Sn tin allotrope

A

white tin
beta tin
distorted octagonal array
stable at room temp
metal
more e- are delocalised than graphite

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19
Q

lead allotrope

A

metallic fcc
only forms metallic structures
closed pack structure

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20
Q

group 14 and bond strength

A

4 valence electrons make the bond strength large

can fill the MO

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21
Q

group 15

A

5 valence : 2* 3 bonding
N is gas at room temp, rest are solids
each has rhombohedral allotrope
( fused cyclohexane chairs with lone pair, tetrahedral shape, hexagonal layers) : black P, alpha As, alpha Sb, alpha Bi.
bond length increases down the group
weaker bonds (bonded to 3 not 4)

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22
Q

group 15, white phosphorus structure

A

tetrahedral shape
lone pair on each phosphorus
3 bonds per P.

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23
Q

anything group 15 has how many bonds

A

3 BONDS
1 lone pair!!!
tetrahedral shape

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24
Q

group 16 has how many valence electrons

A

6!!

can only form 2 BONDS
2 LONE PAIRS
per atom.

2 single bonds per atom

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25
group 16 S8 crown
crown shape 2 bonds each daisy crown of 8 S elements
26
group 16 helical element
single helix (like dna) 2 bonds - chain 2 lone pairs each atom with bunny ears chain lower atom as only 2 bonds need to break
27
why do group 14 have highest enthalpy of atomisation
4 bonds must be broken (all bonding e-)
28
why does group 15 have a lower enthalpy of atomisation than group 14
3 bonding 1 lone easier to break 3 bonds than 4
29
why does group 16 have a lower enthalpy of atomisation than 14 and 15
2 bonds 2 lone pairs per atom. easier to break 2 bonds than 4 or 3
30
group 17
dimers!! only 1 bonding electron left single bond 3 lone pairs F2 Cl2 Br2 etc
31
down group 17melting and bp
melting point and boiling point increases increase in VDW as atomic weight increases
32
F2 colour
colourless
33
Cl2 colour
yellow green Clover: yellow (gold) green (leprechauns)
34
Br2 colour
red brown liquid Breens 🫘:red brown liquid
35
I2 colour
purple / black solid Indigo (dark black purple)
36
group 18
noble gases held together via VDW low melting + bp. m + bp increase down the group monoatomic gases 5K liquid range between bp+mp (must keep temp very constant)
37
group 18 weight
heavier down the group atomic radius increases greater VDW attractions
38
group 18 has the
highest ionisation energies but Xe and O have similar ionisation energies u can ionise O2 into O2+ with strong oxidising agent so u can do it with Xe aswell (PtCl6 = oxi agent)
39
homonuclear bonds
bonds between 2 atoms of the same element
40
small elements have stronger bonds, why is this
smaller element = greater effective overlap = stronger bond
41
N-N O-O F-F are weaker than expected bc what
they’re small repulsion causes a weaker bond significant interaction repulsion bc of their small size
42
down the group what happens to bond strength
decreases diffuse orbitals less effective overlap weaker bond
43
are sigma or pi stronger (not for N or O) but generally
sigma overlap point towards eachother (pz are directional) pi = less effective overlap, non directional, weaker than sigma bond (side side interactions)
44
why are pi bonds better for N and O
small atoms, sigma bonds are weak due to inter atomic repulsion’s due to their small size. pi bonds allow side side interactions allowing for pi bonds to be stronger than sigma bonds for N and O. DOUBLE BONDS ARE PREFERED
45
what is the favoured bond
bond with most energy aka strongest bond N = triple bond!! bc x3 single bond is still smaller than a triple bond
46
why is N a gas
it’s energetically favoured by the element forms triple bonds bc the triple bond is the strongest (most favoured)
47
heteronuclear bonds
bonds between two different atoms
48
what is the strength of heteronuclear bonds determined by
difference in electronegativity more polar = more electronegativity difference = more ionic character = stronger bond pauling and his electronegativity
49
oxidation state definition
the charge the atom would have if a more electronegative atom bonded to it and acquired all the electrons NF3 ( N= +3. F= -1)
50
valency definition
max number of univalent (1bond) atoms that can combine with an atom of another element under consideration eg: trivalent, monovalent , connected to 3 or 1 different things.
51
hyper valent
main group elements (period 2 ns2 np6) that have more than 8e- in their valence shell PF5 PCl5 etc etc!! 10e- in their valence shell not 8e- 😮😮😮😮
52
inert pair effect
when the valence S electrons don’t take part in bonding. oxidation state is 2 less than group valency. group 13 = +3 oxi state, TI group 3 = +1 oxi state
53
higher than expected ionisation energy of an atom means it’s bond strength when bonded to smt else is
weaker ??
54
lewis acid
electron pair acceptor accepts electrons in the LUMO acids accept electrophile
55
lewis base
electron pair donor FROM HOMO nucleophile
56
brønsted-lowry acid
donates protons H+
57
brønsted-lowry base
accepts protons H+
58
brønsted-lowry lowry is based on the movement of
protons
59
lewis theory involves the transfer of
electron pairs.
60
if lewis acids accept electron pairs they must have
empty p orbitals LUMO group 13 have an empty p orbital
61
what are frustrated lewis pairs
bulky lewis acids and bases cannot form addicts due to steric hinderance e- can’t get close enough they rip apart lewis acids and bases
62
how do double pairs affect VSEPR theory
they dont effect the shape of the molecule by changing the amount of e- pairs around the central atom. this is bc they have the same direction as a single bond. there is a sigma bond in a pi bond they change the bond angles due to more repulsion, double bond is shorter, closer to nuc, more repulsion
63
in trigonal bipyramidal, how many nmr environents can there be
2, for axial and equitorial bc theyre of different energies + environments
64
molecular shape fluxionality
when the shape of a molecule is not rigid, atoms can move as bonds stretch or vibrate. if the energy is small enough, the molecule can change shapes rapidly (interconvert) trigonal bipyramidal to square planar ( 4 - 1 - 1 )
65
berry pseudorotation
type of vibration that causes a molecule to isomerise by exchanging ligand position (axial --> equitorial,,, equitorial --> axial) the groups move internally, they arent rotated. happens so fast an average of both is seen by nor.

inorganic sem1 (13 decks)

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