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the patient > organic chem 1-2 > Flashcards

organic chem 1-2 Flashcards

1
Q

what does n represent when writing the IUPAC name for example n-propyl?

A

n- REPRESENTS that it is non branched and linear

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2
Q

what is it called when a benzene ring has Ph attached to it?

A

it is not benzene it is Phenyl (sometimes Phenyl doesn’t need to be drawn- the ring of it- it can just be represented as Ph)

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3
Q

what are the energy levels in order?

A

1s2 2s2 2p6 3s2 3p6 3d10 4s2

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4
Q

how can different types of orbitals be differentiated?

A

their shape and symmetries

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5
Q

what are the wave properties of electrons?

A

standing wave vibrates in fixed location. a standing wave appears to be vibrating vertically (up and down) without travelling side to side (horizontally)

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6
Q

amplitude can be positive or negative. what is the amplitude of a wave?

A

the height (shows how much energy the wave has)

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7
Q

what is the node of a wave?

A

the point where the amplitude is zero (the line) and the point doesn’t move

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8
Q

what does an s orbital look like ?

A

spherically symmetric around the nucleus, no phase change

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9
Q

when drawing energy levels how do you draw them?

A

fill up each box individually first with one electron then start paring them, without opposite spins, arrows go through the line

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10
Q

what does the second electron shell look like

A

another shell around the spherical node (where there is no electron density)

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11
Q

what is the node in terms of electron shells?

A

region of space around the nucleus where the probability of finding an electron is ZERO

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12
Q

WHAT DO p orbitals look like?

A

2 oval shapes opposite one another

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13
Q

how many p orbitals are there

A

3 p orbitals. (2p6)

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14
Q

what does the distance from the node of the p orbital to the end of the oval mean?

A

the distance it is from the nucleus

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15
Q

what does the height of the p-orbital wave mean

A

the electron density

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16
Q

what are valence electrons?

A

electrons on the outermost shell of the atom

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17
Q

what does aufbau principle state?

A

fill the lowest energy orbitals first

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18
Q

what does Hund’s rule state?

A

when there are 2 or more orbitals of the same energy, electrons will go into different orbitals rather than pairing up in the same orbital.

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19
Q

what holds ionic bonded atoms together?

A

electrostatic attraction

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20
Q

what does non-polar mean in covalent bonds?

A

electrons are shared evenly in the bond

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21
Q

when there a polar covalent bond what does this mean?

A

electrons are not shared evenly between the atoms, where each atom has a different electronegativity. (more of a pull on the electron towards itself)

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22
Q

what is electron density?

A

the relative amount of negative charge that is located at each point

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23
Q

what do lone pairs determine?

A

the reactivity

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24
Q

which c-c bond length is the longest ?

A

single/sigma c-c bond have larger bond length as only 2 electrons pull the atoms together in the bond

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25
Q

which c-c bond length is the shortest?

A

triples bond as there are 6 electrons and a stronger pull towards each other- decreasing the bond length

26
Q

how do you workout dipole moment?

A

amount of electrical charge x bond length

27
Q

what is a EPM?

A

electrostatic potential map is a representation where the electrostatic potential at the molecular surface is indicated by colours so its easy to visualise the distribution of charge in a molecule. (red is negative and blue is positive)

28
Q

what is the trend for electronegativity in the periodic table

A

electronegativity in creases as you go across the table

nitrogen, oxygen, fluorine, sulfur, chlorine, bromine, iodine

29
Q

how can it be predicted whether a bond will be polar?

A

electro negativities can be used to predict this

30
Q

in bond dipole moments what does the arrow represent?

A

arrow: bond dipole created and the direction the electrons pull towards-> delta negative one (more electronegative pull)

31
Q

what are dipole moments due to ?

A

difference in electronegativity and amount of charge and stance of separation (measure in debyes D)

32
Q

NH2 (AMINE), OH (ALCOHOL), Cl, N+-CL-
order these groups attached to alkanes in order of increasing polarity

A

NH2 (AMINE),
OH (ALCOHOL),
Cl,
N+-CL-

33
Q

if two of the same atoms or molecule was joined together in a bond would it be polar or non polar
E.G:
H2
CH3-CH3

A

NON-POLAR SIMILAR ELECTROGNETIVITY

34
Q

TRUE OR FALSE:

Electronegativity differences
of less than ~0.4 result in nonpolar covalent bonds,
Differences up to 1.9 indicate increasingly polar
covalent bonds, and differences of 2 or more
indicate ionic bonds.

A

true

35
Q

what is the polarity of a c-h bond

A

non-polar

36
Q

what does a correct dipole orientation look like?

A

arrow above bonding pointing from left to right unless its a 3d shape

37
Q

how does a molecule with polar covalent bonds have no net polarity?

A

their symmetrical shapes cause individual bond polarities to cancel each other out

38
Q

is bezene rings polar or non polar

A

non polar

39
Q

what happens to toluene in water?

A

toluene floats in water as it is less dense than water

40
Q

what is the equation for working out the formal charge?

A

Formal Charge= number valence electrons - (e- in lone pairs + number of bonds)

41
Q

what does lipophilic mean?

A

the ability of a chemical compound to dissolve in fats, oils, lipids and non polar solvents such as hexane or toluene.

42
Q

what are lipophilic features?

A

like benzene, ch3, c-c
non-polar

43
Q

what are hydrophilic properties?

A

OH, N
polar

44
Q

what are the two linear combination of atomic orbitals?

A

bond formation, hybridisation

45
Q

what is bond formation?

A

bonds between different atoms

46
Q

what is hybridisation?

A

bonding on the same atom

47
Q

what does IN PHASE mean in wave interactions?

A

two waves coincide with peaks and troughs matching

48
Q

what happens to waves that are in phase

A

they add together and aptitude increases

49
Q

what happens to waves that are out of phase?

A

the waves out of phase cancel out and cause a destructive overlap.

50
Q

what happens when 2 1s orbitals of two hydrogen atoms overlap in phase with each other?

A

formation of σ-bonding MO (sigma)

51
Q

what happens when 2 1s orbitals combine out of phase?

A

generates anti bonding molecular orbital.

52
Q

what happens when 2 p-orbitals overlap?

A

forms a bonding orbital and anti bonding orbital

53
Q

what does a bonding orbital look like of p orbitals

A

one bit positive orbital in the centre with one negatively charged on each side, with a nucleus between them

54
Q

what does a sigma anti bonding orbital look like from a destructive overlap?

A

node split in the centre and on each side is a positive and negative orbital with a nucleus in the centre. the node has one side with a positive orbital and other side with a negative

55
Q

what does the overlap of s and p orbitals give?

A

bonding mo and anti bonding mo

56
Q

what does a sigma bonding mo look like between a s and p orbital ?

A

p orbital with negative and positive ovals with nucleus in the middle is bonded to a s orbital with a positive charge

it creates the same p orbital but the positive charged side of the p orbital is doubled due to the positive s orbital side joining to it

57
Q

what does a sigma ANTIbonding mo look like between a s and p orbital ?

A

p orbital with negative and positive ovals with nucleus in the middle is bonded to a s orbital with a negative charge

p orbital with a node in the next to it separating it from a negative s orbital on the other side of the nose

58
Q

what does the sideway overlap of 2 p orbitals lead to?

A

pi bonding mo and a pi anti bonding mo

59
Q

which is strong a pi bond or sigma bond?

A

sigma bond

60
Q

what does a double bond (2 pairs of electrons shared) consist of?

A

sigma bond, pi bond

61
Q

what does a triple bond consist of?

A

1 sigma bond
and
2 pi bond

62
Q

is bonding or anti bonding MO (MOLECULAR ORBITAL) HIGHER in energy compared to the original atomic orbital which wasn’t bonded?

A

anti bonding mo

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