Readings

Question 1

what is sp3 hybridisation?

Answer 1

when the s orbital hybridises with all three p orbitals to form tetrahedral shapes

Question 2

what shape is made through sp2 hybridisation?

Answer 2

trigonal planes are made

Question 3

sigma bond:

Answer 3

sp2 orbitals merging together nicely in-line with the nuclei

Question 4

what is a sp3 orbital a blend of?

Answer 4

sp3 = a blend of one s orbital and three p orbitals

Question 5

what is an sp2 orbital a blend of?

Answer 5

sp2 = a blend of one s orbital and two p orbitals

Question 6

what is an sp orbital a blend of?

Answer 6

sp orbital = blend of one s and one p orbital

Question 7

what shape is an s orbital?

Answer 7

sphere

Question 8

what does an orbital simply tell you?

Answer 8

the most probably location in which you can find an electron

Question 9

how many types of p orbital are there?

Answer 9

3 types: one in the x-axis (px), on the y-axis (py) and one in the z-axis (plz)

Question 10

what are degenerate orbitals?

Answer 10

degenerate orbitals are orbitals with the same energy

Question 11

what governs the energy of hybrid orbitals?

Answer 11

the energy of a hybridised orbital will be dependant upon the proportion of s:p orbitals within the hybrid orbital - for example if it is sp3 it will be 75% closer to the energy of a p orbital than it is to 25% of an s orbital

Question 12

hybrid orbitals are fused to form which type of bond?

Answer 12

sigma bonds (o with a quiff)

Question 13

what are π bonds always made from?

Answer 13

π bonds are always made from unhybrisised p orbitals. (when you’re dealing with carbon atoms)

Question 14

what is the difference between a pie bond and a sigma bond?

Answer 14

sigma bonds are made from hybridised orbitals whilst pie bonds are made from unhybridised orbitals

Question 15

every double bond has at least:

Answer 15

one sigma and one pie bond

Question 16

every carbon single bond has:

Answer 16

at least one sigma bond

Question 17

every carbon triple bond has at least:

Answer 17

one sigma bonds and two pie bonds

Question 18

what bonds is stronger than the other between sigma and pie bonds?

Answer 18

sigma bonds are stronger than pie bonds

Question 19

every single bond in a organic molecule contains at least:

Answer 19

one sigma bond

Question 20

every double bond in a organic molecule contains at least:

Answer 20

one sigma and one pie bond

Question 21

what essentially is hybridisation:

Answer 21

when different atomic orbitals of same or nearly same energy combine together to form new hybrid orbitals

Question 22

all hybrid orbitals have the same energy, they are referred to as being…

Answer 22

degenerate

Question 23

unhybrid orbitals form:

Answer 23

pi bonds

Question 24

hybrid orbitals form:

Answer 24

sigma bonds

Question 25

what essentially is the span of sp-sp3 orbitals describing?

Answer 25

the sp-sp3 orbitals essentially describe how electrons from different sub-orbitals come together in bonds to form differing types of hybrid orbitals (e.g. count all the electrons present in bonds, determine what proportion are in s:p, these ration values allow you to determine what sp-sp3 it is and there for the structure as each sp hybrid has its own structure)

Question 26

word to describe the energy of degenerate orbitals which have energy in between the two set p & s values:

Answer 26

intermediate energies

Question 27

what happens to the spherical s orbitals and two-lobed p orbitals once hybridisation takes place?

Answer 27

once hybridisation takes place, both the original orbitals cease to exist and together the hybrid forms an entirely new orbital pattern

Question 28

what happens to the shape of electron clouds when hybridisation takes place?

Answer 28

they form into their distinct shapes that are characteristic of their hybridisation types (e.g. sp3 = tetrahedral (4 lobes equally apart from one another))

Question 29

pi bond comes from:

Answer 29

the overlap of unhybridised p orbitals

Question 30

WHERE do sigma and pi bonds form in the molecule?

Answer 30

sigma bonds occur along the axis between nuclei whilst the pi bond occurs above and below the π axis, where the p orbital lobes have overlapped

Question 31

how do you determine what sp orbital hybrid variant a given carbon is in a molecule?

Answer 31

you must count how many different electron groups are attached to it, for example if it was CH4, this would mean that its tetrahedral and therefore sp3, whilst if you were dealing with a C=CH2 molecule, the hybridisation state of the right hand carbon would be sp2 because it is only attached to 3 groups, therefore being triagonal planar

Question 32

how many different groups are present in carbons that are either: sp, sp2, sp3?

Answer 32

sp3 = 4 groups = tetrahedral sp2 = 3 groups = triagonal planar sp = 2 groups = planar

Question 33

how do you determine the hybrid orbital identity of a carbon atom?

Answer 33

(1) counting how many groups are attached to (2) deduce the structure from how many groups you’ve counted (3) link the structure to its designated sp variant (e.g. sp3 = tetrahedral and so on)

Question 34

if you are trying to deduce the hybridisation state of a carbon and a lone pair is present, do you count it as a group that goes towards the sp numbering?

Answer 34

yes - each lone pair is its own group

Question 35

sp2 shows us that:

Answer 35

our molecule is planar & the bond angles are 120*

Question 36

when tackling hybridisation states, how do we teat lone pairs of electrons?

Answer 36

we treat electrons as their own individual groups, contributing to the sp identity

Question 37

dumb words, what is a resonance form?

Answer 37

a resonance form is a different form of a given molecule where the atom nuclei are in the identical places as before but the electron configuration has completely changed

Question 38

amide (N attached to carbons - not hydrogens!) nitrogen’s will always have ___ hybridisation

Answer 38

SP2!

Question 39

2 main rules of resonance:

Answer 39

(1) Thou shall not break a single bond (2) Thou shall not violate the octet rule [atoms must have 8 electrons in their outer shell - in all resonance forms]

Question 40

only two things you move when creating resonance structures are:

Answer 40

(1) π bonds [C=C] (2) lone pairs (:)

Question 41

when moving lone pairs when constructing resonance structures, what must you always do in order to confirm that you aren’t breaking the octet rule?

Answer 41

you must draw out the lewis structure to ensure you aren’t kicking off any hydrogens when creating double, triple bonds etc

Question 42

what arrow do we use for resonance forms?

Answer 42

you must use a double headed arrow - NOT an equilibria one however, just a standard double headed arrow

Question 43

note - something can still be minus charged and yet still also fulfill the octet rule, give an example:

Answer 43

.. -: O :— oxygen above has eight electrons in its outer shell therefore octet is satisfied, however because oxygen has only one bond it will always posses a single negative charge

Question 44

two ways in which you can transfer a double [π] bond when creating resonance structures:

Answer 44

(1) moving them to another double bond location (2) moving the double bond onto a species that can hold a lone pair, hence creating a single bond

Question 45

what must be the same in all resonance structures?

Answer 45

the overall charge of all resonance structures must all be identical

Question 46

if a nitrogen atom is noted as neutral, what do we assume?

Answer 46

that a lone pair is present on the nitrogen [nitrogen cannot be neutral without a lone pair]

Question 47

how do you base your judgment on the charge of C/O/N?

Answer 47

you must look at their numbers of bonds and lone pairs to infer their charge where O has two bonds to be neutral, N has 3 bonds to be neutral and C has 4 bonds to be neutral if they are missing a bond or a lone pair this will result in a (+) charge and a ( - ) charge will take place as a result of additional bonds or lone pairs above their usual amounts

Question 48

you can still create negative and positive charges when drawing resonance structures, even if it feel wrong - SO LONG AS the overall charge cancels out at the end to give the overall charge of your starting molecule

Answer 48

you can still create negative and positive charges when drawing resonance structures, even if it feel wrong - SO LONG AS the overall charge cancels out at the end to give the overall charge of your starting molecule

Question 49

less & more bonds on an atom than that of what is needed for neutrality results in:

Answer 49

positive charge = more bonds than usual negative charge = less bonds than usual

Question 50

how many lone pairs does oxygen always want in order to be neutral?

Answer 50

always wants 2 lone pairs and 2 bonds to fulfil the octet rule

Question 51

if oxygen is neutral, what does this imply?

Answer 51

neutral oxygen implies 2 lone pairs present