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Chem year 1 > inorganic 3- shapes and isomers > Flashcards

inorganic 3- shapes and isomers Flashcards

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1
Q

Why does a chemical bond form

A

if the bond (resulting arrangement of the nuclei and their electrons) has lower energy than the total energy of the separate atoms

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2
Q

Define covalent bond

A

pair of electrons shared between 2 atoms

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3
Q

what is the goal of a covalent bond

A

to get as close to being an octet by sharing electron pairs

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4
Q

a lewis structure shows — electrons

A

valence electrons

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5
Q

What is an element with an unpaired electron considered

A

a radical

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6
Q

How would a lewis structure represent this

A
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7
Q

What is a 2c-2e bond

A

2 centre 2 electrons

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8
Q

calculate the number of valence electrons of [BF4]-

A
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9
Q

what does hyper valence mean

A

molecule that has an element containing more than 8 valence electrons

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10
Q

is a dative bond any different energetically from a normal covalent bond

A

no

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11
Q

what is a dative bond

A

One atom donating a lone pair of electrons in one orbital into a vacant orbital on another atom = dative bond

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12
Q

what hybridisation is nitrogen in ammonia

A

sp3

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13
Q

How many valence electrons, and therefore pairs of electrons in SO4 2-

A
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14
Q

equation for formal charge

A
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15
Q

How do you get to the electrons being hybridised

A

excite 2s electrons to 2p level

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16
Q

Why can elements get a higher co-ordination number as you go down the group

A

radius of the elements gets bigger

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17
Q

How would these sulphur electrons hybridise/arrange to form SF6

A

most energetically stable way to arrange 6 F bonds/ all S-F bonds must be the same energy

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18
Q

how is molecule shape dictated and what assumptions do we make to decide it

A

electron repulsions. assumption= all bonds are covalent

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19
Q

What type of elements do we not use VSEPR theory to predict molecule shape for

A

VSEPR applicable to s- and p-block compounds. d-block compounds (complexes) have shapes dictated by the number of ligands

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20
Q

What is the heirachy of electron repulsion

A
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21
Q

If all sites are equal (octahedral geometry) then where will the lone pairs be paired in relation to one another

A

lone pairs will be trans (opposite)(180° angle)

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22
Q

Bonding pairs to electro—- substituents occupy less space than those to more electro— substituents.

A

Bonding pairs to electronegative substituents occupy less space than those to more electropositive substituents.

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23
Q

Where would a lone pair go on this arrangement

A

will always be equatorial in a trigonal bipyramidal

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24
Q

When deciding a molecule shape, do double bonds or single bonds take up more space

A

double bonds take up more space

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25
Q

What is a pseudostructure

A

arrangement of electron pairs whether they are bonding or lone pairs

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26
Q

Where would you want the least electronegative/biggest element to go in a shape

A

in the middle

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27
Q

Name all the structures and their bond angles

A
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28
Q

Pentagonal bipy is rarely found experimentally. If something had 6 ligands and 1 lone pair, what would the shape more be like

A

Octrahedral. A stereo-chemically inactive lone pair localised in s orbitals is distributed evenly around the shape. S-orbitals lone pairs are spherical and do not influence shape;
only lone pairs housed in p orbitals influence shape

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29
Q

What is the structure of a molecule with 2 lone pairs

A

linear

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30
Q

What pseudostructure vs real structure would BeCl2 be

A

linear, linear

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31
Q

What pseudostructure vs real structure would BF3 be

A

trigonal planar, trigonal planar

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32
Q

What pseudostructure vs real structure would SnCl2 be

A

trigonal planar, v shaped

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33
Q

What pseudostructure vs real structure would NH3 be

A

tetrahedral, trigonal pyramidal

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34
Q

What pseudostructure vs real structure would CH4 be

A

tetrahedral, tetrahedral

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35
Q

What pseudostructure vs real structure would NH4+ be

A

tetrahedral, tetrahedral

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36
Q

What pseudostructure vs real structure would PCl5 be

A

trigonal bipyramidal, trigonal bipyramidal

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37
Q

What pseudostructure vs real structure would I3- be

A

trigonal bipyramidal, linear

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38
Q

What pseudostructure vs real structure would PCl6- be

A

octahedral, octrahedral

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39
Q

What pseudostructure vs real structure would CIF5 be

A

octahedral, square pyramidal

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40
Q

What pseudostructure vs real structure would IF7 be

A

pentagonal, pentagonal

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41
Q

What type of molecule notation would BeCl2 be

A

AX2

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42
Q

What type of molecule notation would H2O be

A

AX2 E2

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43
Q

What type of molecule notation would CIF5 be

A

AX5 E

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44
Q

C, N and O are all in the same period, so why do the angles get smaller

A

Higher space requirements for the lone pairs

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45
Q

This is the predicted shapes for molecules with 5 valence electrons but this changes as to wether one of those valence electrons is a lone pair. What other shapes do these molecules take

A
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46
Q

Of the other structures for AX5. What is the structure for AX4 E

A
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47
Q

Of the other structures for AX5, what is the structure for AX3 E2

A
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48
Q

Of the other structures for AX5, what is the structure for AX2 E3

A
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49
Q

Which structure would be favoured

A

lone pairs go in equatorial positions Structure (c) appears most favourable energetically. But we cannot look at the lp-lp repulsion in isolation; (c) looses out when considering the number of bp-lp repulsions, at 90 deg from each other too.
The large number of 90 deg repulsions in (b) and (c) means that (a) is most stable in relative terms,
with fewer repulsions

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50
Q

lone pairs/ double bonds go in what positions

A

equatorial

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51
Q

What are fluxional molecules

A

molecules that are an intermediate between two geometries

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52
Q

Is triagonal bipyramidal higher or lower in energy than a square based pyramid

A

slightly lower

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53
Q

Which is generally favoured

A

square based; many species show a geometry which is intermediate between the two

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54
Q

7 pair of electrons AX6E predicts pentagonal bipyramid (e.g. BrF6-, SeBr62-, SbCl63-), but what is usually the structure

A

the real experimental structures are Octahedral with a stereochemical inactive active pair/ Lone pair is a cloud over molecule not housed

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55
Q

in SF4O where would the flourines and the oxygen go. S and O = G6 F= G7

A

double bonds go in equatorial position to minimise repulsion

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56
Q

If F is more electronegative than Cl what is the difference in bond angle between the two molecules

A

F-N-F will be smaller. Electron density is closer to F making it easier to have the bonding pairs closer, so there is the furthest distance between the LP and the BP

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57
Q

can atom size and electronegativity effect molecule shape

A

yes

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58
Q

What elements can VSEPR not predict the shape of

A

transition metals and most heavy p block elements

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59
Q

How would you work out what shape BrF5 is

A
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60
Q

How to work out what shape BrF2 + is

A
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61
Q

What is a Lewis acid

A

electron pair acceptor e.g. transition metals

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62
Q

What is a Lewis base

A

electron pair donor e.g. halides

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63
Q

What is a Bronsted acid

A

donates a H+

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64
Q

What is a Bronsted base

A

accepts H+

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65
Q

When only does the Bronsted acid/bases definitions work

A

in aqueous solution

66
Q

Which would be the Lewis acid and which is the Lewis base

A
67
Q

what is gerade symmetry

A

can be inverted and still the same

68
Q

what is ungerade symmetry

A

inverted and shape remains the same but phases are different

69
Q

When is the only time you use g and u symbolisims

A

if something has symmetry as it lets the person know what type of symmetry it has

70
Q

at a nodal plane what is the probability of finding an electron

A

0

71
Q

Define transition metal

A

where the valence electrons are d electrons

72
Q

What is the order of filling the orbitals 3s, 3p, 3d, 4s

A

3s, 3p, 4s, 3d

73
Q

In oxidation or reduction of transition metals where are the electrons lost/gained from

A

d orbital

74
Q

How to work out a d electron count (e.g of FeCl3(H2O)3 )

A

The d-electron count of a metal in a complex is the number of electrons associated with the metal in its formal oxidation state.

75
Q

What are the two transition metal anomalies that have a different electronic configuration

A

Cr and Cu
Cr= 4s1, 3d5
Cu= 4s1, 3d10

76
Q

What would the ion electronic configurations be

A
77
Q

What would the ionic configuration be

A
78
Q

What would the ion electronic configuration be

A
79
Q

If Cr at oxidation= 0 is d6, then what would Cr 3+ be

A

d3

80
Q

What is the d electron count of Ni 2+

A
81
Q

What is a co-ordination complex

A

a central atom or ion (Lewis acid) coordinated to one or more ligands (Lewis base) by a coordinate bond

82
Q

What is the shape of a complex dictated by

A

number of coordinated ligands

83
Q

What is the co-ordination number of cobalt

A

6

84
Q

What is the co-ordination number of cobalt

A

6

85
Q

What is a mononuclear complex

A
86
Q

What is a binuclear complex

A
87
Q

What is a polynuclear complex

A
88
Q

What is the difference between a monodentate, bidentate and tridentate ligand

A
89
Q

Bidentate ligands have two donor atoms, and can bind to one or two other atoms. Other than a complex, what else can this form

A

rings (size dictated by number of atoms separating the donors in the ligand)

90
Q

How does ETDA bind to form a ligand complex

A

It is a hexadentate ligand

91
Q

What are ambidentate Ligands

A
92
Q

What are each of these things

A
93
Q

In name complexes, where is the central atom part of the name located

A

At the end with the oxidation number

94
Q

What does the tetra prefix mean in regards to ligands

A

4 bond sites

95
Q

What are each of the metals these complex names relate to

A
96
Q

What are hard and soft metal centres in complexes

A

soft= more polarizable
hard= less polarisable

97
Q

Define a ligand

A

A group/atom that gives a metal centre a pair of electrons, normally through an available lone pair e.g H2O or NH3

98
Q

How does the electron cloud of the ligand interact with the available orbital on the metal (wether metal is receiving electrons or giving them)

A
99
Q

What are some examples of bidentate ligands

A

They can also function as monodentate ligands

100
Q

Can a carbon chain radical be a ligand

A

yes

101
Q

hard cations are more compatible with hard/soft ligands

A

hard cations= compatible with hard ligands (hard acids and hard bases)
soft cations= compatible with soft ligands (soft acids and soft bases)

102
Q

hard cation- hard ligand interactions are ionic/covalent

A

more ionic than covalent

103
Q

soft cation-soft ligands interactions are ionic/covalent

A

more covalent (greater overlap)

104
Q

would F- form a better complex with Ti or Pd

A

Ti. (hard-hard interaction) Flourine is a hard base and Pd is a soft acid (low charge density) whereas Ti is a harder acid (high charge density)

105
Q

Trend in transition metals as to wether they make hard or soft metal ions/ acids

A

Becomes softer down the group
Early transition metals= hard; are small ions with large charge density
Later transition metals= soft; have all their d electrons

106
Q

If something is highly electronegative will it be hard or soft

A

hard; less polorizable

107
Q

Why is water left out of constant equations

A

its concentration is assumed to be constant in aqueous solutions

108
Q

What does a larger/smaller stability constant mean

A

constant= large; a ligand binds to the metal more tightly than H2O
small= a ligand binds to metal less tightly than H20

109
Q

What are typical values for the stability constant Kf of a metal ion

A

1-13

110
Q

A chelation reaction results in an increase/decrease in the number of molecules in solution

A

increases molecules in solution

111
Q

In a mono dentate ligand reaction, the number of molecules increases/decreases/ stays same

A

stays the same

112
Q

Which side of the reaction does the equilibrium lie is the equilibrium constant is high

A

lies to right

113
Q

if the equilibrium lies to the right there is a large/small △G

A

large negative △G

114
Q

Which reaction will have the greater value for K (equilibrium constant)

A
115
Q

Which complexes are more stable; chelate complexes or mono-dentate metal / ligand complexes.

A

a complex containing one (or more) 5 or 6 membered chelate rings is more stable
{i.e. stability (or formation) constant is larger} than the one without the ring

116
Q

How is the chelate effect effected with ring size

A

The chelate effect decreases with increasing ring size

117
Q

What is square planar shape

A
118
Q

What is Constitutional/ structural isomerism

A

Compounds with the same empirical formulae but with different atom binding sequences. There are several classes in this
-co-ordination isomers
-linkage isomers
-polymerisation isomers

119
Q

What is a co-ordination isomer (constitutional isomerism)

A
120
Q

What is linkage isomerism

A

-two or more coordination compounds in which the donor atom of at least one of the ligands is different
can only exist when the compound contains a ligand that can bond to the metal atom in two (or more) different ways

121
Q

What is ionization isomerism

A

Occurs when isomers produce different ions in solution, often manifest itself by the exchange of a ligated anion with a counterion:

122
Q

What is geometrical isomerism

A
123
Q

Which isomers are cis and trans

A
124
Q

What is the optical isomer for this

A
125
Q

What is an optical isomer

A

A compound that is non-superimposable on its own mirror image is an

126
Q

What are the optical isomers of these

A
127
Q

The trans -isomer has mirror symmetry and is therefore not optically active. What are the optical isomers of these (enantiomers)

A
128
Q

Why are there relatively few complexes with coordination numbers 1 and 2

A

because they are exposed to attack by additional ligands, so increasing their coordination number

129
Q

This is a complex with a co-ordination number of 1. Usually these are readily attacked, but why could this one be stable

A

the ligand ‘protects’ the metal by steric crowding

130
Q

Co-ordinaiton number of 3 is rare amount d-block elements; what Is needed for a stable CN=3 complex

A

large and kinetically stable ligand

131
Q

for CN=4, what d-block elements will take tetrahedral and square planar

A

tetrahedral- centre atom is small/ our ligands are big
square planar- for larger d8 metal ions – Rh+, Ir+, Pd2+, Pt2+

132
Q

What are the two shapes for CN=5

A

trigonal bipyramidal and square pyramidal

133
Q
A
134
Q

What would be the geometric isomer of this compound

A
135
Q

What would be the geometric isomer of this compound

A
136
Q

if something is non super imposable they are chiral/not chiral

A

Chiral isomers are non-superimposable mirror images of each other

137
Q

What is the oxidation state and dn configurations for the metal
Cu=29 electrons/ group 11

A
138
Q

What is the oxidation state and dn configurations for the metal
V =23 electrons/ group 5

A
139
Q

What is the oxidation state and dn configurations for the metal
Au=79 electrons/ group 11

A
140
Q

What is the oxidation state and dn configurations for the metal
Fe=26 electrons

A
141
Q

What charge/ oxidation state is a CN ligand

A

-1

142
Q

What is the d electron count for Ni (group 10)

A
143
Q

What is the d electron count for Co

A
144
Q

What is an en ligand

A

-1 Ethylenediamine

145
Q

What is the bond order of NO3-

A

(1+1+2)/ 3 [1+1+2 is adding the bonds and 3 is dividing by number of bonds with double being counted as 1]

146
Q
A

They are all ligands

147
Q

What structure does [PoF5] have

A

octrahedral and square based pyramidal are in equillibrium

148
Q

What structure does [GeCl3]- have

A
149
Q

What structure does [AlCl2]+ have

A
150
Q

What structure does [BrF6]- have

A
151
Q

What structure does [Sb(O)Cl4]- have

A
152
Q
A

Why is Cl not -1 in first ligand

153
Q
A
154
Q

Which one is cis and which one is trans

A
155
Q

Which one is fac and which one is mer (can only be done on octrahedral complexes for **tridentate chelates/ligands)

A

fac (on one face)

156
Q

Which isomer is fac and which one is mer

A
157
Q

What are delta and lambda isomers

A

optical isomers

158
Q

Just a

A

cis and trans isomers/ with an optical isomer (delta and lambda) possible

159
Q

Just b

A

only mer and fac

160
Q

Just c

A

cis and trans

161
Q

Just d

A

optical isomers

162
Q

Just e

A

Chem year 1 (26 decks)

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