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DRUGS AND MEDICINE > organic them slides 3-4 > Flashcards

organic them slides 3-4 Flashcards

1
Q

why do atoms form bonds?

A

where atoms have the lowest energy

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2
Q

when atoms react and form bonds with one another they become energetically favourable. What does this mean?

A

low energy, no energy needs to be inputted for the reaction to occur, in fact dingy was released from the reaction.

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3
Q

what does it mean when atoms clash with one another and are energetically unfavourable?

A

unfavorable require energy to put the products at a higher energy state than the reactants.

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4
Q

why do atoms form bonds?

A

atoms are trying to reach the most stable (lowest-energy) state that they can.

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5
Q

what do lewis dot structures show?

A

valence electrons around an atoms

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6
Q

what happens in an ionic bond?

A

electrons transfer and the formation of ions

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7
Q

what happens in covalent bonds?

A

sharing a pair of electrons (one from each atom) etc and the formation of molecules.

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8
Q

what type of elements bond in ionic bonds?

A

metal and non-metal

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9
Q

what type of elements bond in covalent bonds?

A

two non-metals

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10
Q

what type of bond is the sharing of one pair of electrons?

A

single bond

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11
Q

what does the capital Q mean?

A

sigma bond

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12
Q

what is a double bond composed of?

A

one sigma and one pi

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13
Q

what is the bond angle for a linear shape?

A

180

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14
Q

what us the bond angle for a trigonal planar ?

A

120

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15
Q

what is the bond angle for tetrahedral?

A

109.5

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16
Q

what is the bond angle for a octahedral?

A

90 and 180

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17
Q

what is the bond angle for trigonal bipyramidal?

A

120 and 90

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18
Q

true or flase: solids have stronger IMF than gases

A

true

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19
Q

what are intramolecular forces?

A

they’re strong bonds between atoms (covalent ionic …)

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20
Q

what are intermolecular forces ?

A

they’re weak forces that hold bonded atoms together to form molecules.

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21
Q

what are the 6 IMF?

A

1.ELECTROSTATIC/ IONIC BOND
2.VDW INTERACTIONS
3.DIPOLE-DIPOLE INTERACTIONS
4.HYDROGEN BONDS
5.INDUCED DIPOLE INTERACTIONS
6.ION-DIPOLE INTERACTIONS

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22
Q

What is induced dipole interactions?

A

weak attraction that results when a polar molecule induces a dipole in an atom or in a non polar molecule by disturbing the arrangement of electrons in the non polar species.

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23
Q

what are ion-dipole interactions?

A

the intermolecular force of attraction between a charge ion (cation or anion) and a molecule.

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24
Q

what are hydrogen bonds?

A

hydrogen bonded to either: hydrogen, oxygen, fluorine, nitrogen

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25
Q

in the hydrogen bonds present in water where hydrogen is hydrogen bonded to oxygen. Which atom is delta positive and which is negative?

A

oxygen is stronger so it is more electronegative and pulls the electron density towards itself. so oxygen is delta negative and hydrogen is delta positive.

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26
Q

what is the comparison between the strength of H bond compared to covalent?

A

H bond is 1/10 to 1/20 of covalent bond

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27
Q

what are substances which readily dissolve in water called?

A

hydrophilic

28
Q

what happens when something dissolve in solvent water?

A

they react and bond with the water

29
Q

what is an example of ion dipole interactions

A

water molecule reacting with NaCl (+ and - charges)

30
Q

what are permanent dipole dipole bonds?

A

partially positive portion of one molecule is attracted to the partially negative portion of another permanently polar molecule.weak interaction but stronger than VDW

31
Q

what are London dispersion forces/ VDW/ temporary dipole dipole?

A

weak interactions caused by temporary change in electron density of a molecule. present in non polar compounds as well as polar. present in all compounds.

32
Q

what determines the strength of the VDW forces between molecules?

A

surface area of a molecule determines the strength of the VDW interactions between molecules.

33
Q

what happens to the IMF strength as the polarity of a molecule increases?

A

as the polarity increases so does the strength of IMF.

34
Q

what happens to boiling point as IMF increases?

A

boiling point increases as IMF increases> more energy required to break bonds

35
Q

which bond is the most important initial interaction as a drug enters the binding site ?

A

ionic bonds

36
Q

what is an inductive effect?

A

the pull of electron density through a sigma bond caused by electronegativity differences between atoms.

37
Q

what does the arrow show in a bond?

A

arrow shows the direction of electron flow by pointing toward the more electronegative atom.

38
Q

what is +I effect?

A

when electron donating group donates e- and atom become +ve charge afterwards

39
Q

what does +I effect look like with arrow?

A

when an electron is being donated it goes from the atoms donating it and the arrow points to where it is being donated to.

40
Q

what is -I effect?

A

when an atom is withdrawing and giving electron to another the other atom acquired a -ve charge.

41
Q

what does a -I effect look like?

A

when an electron is being donated it goes from the atoms donating it and the arrow points to where it is being donated to.

42
Q

what is resonance effect?

A

resonance effect is the polarity formed in a molecule as a result of contact between a lone pair of electrons and a pi bond, or the interaction of two pi bonds between two nearby atoms.

43
Q

what does a resonance arrow look like?

A

double headed arrow

44
Q

what is the functional group of an aldehyde?

A

CHO (C=O) -AL

45
Q

FUNCTIONAL GROUP OF KETONE?

A

C=O -one

46
Q

functional group carboxylic?

A

COOH (-OIC ACID)

47
Q

ACID ANHYDRIDE FUNCTIONAL GROUP

A

C=O -O- C=O

48
Q

WHAT IS C=O CALLED

A

CARBONYL

49
Q

HOW DO YOU NAME ACID ANHYDRIDES?

A

You name it based on the line of symmetry
So its ethanoic anhydride as it had two eth- on both sides if it had two different you name based on alphabetical order ethanoic propanoic anhydride

50
Q

EXAMPLES OF HYDROGEN BONDING

A

H20

51
Q

EXAMPLE OF ION DIPOLE

A

NaCl with water

52
Q

dipole dipole example

A

HCl

53
Q

examples of VDW?

A

CH4

54
Q

ESTERS FUNCTIONAL GROUP.

A

R-C(=O) -O-R

55
Q

how do you name an ester?

A

split it where the carbon double bond is attached to the O and then name backwards

prop-yl methan-oate

using yl and hate suffixes

56
Q

ether functional group

A

R-O-R

no double (pi) bonds

57
Q

how do you name ethers?

A

split at O bond
name alphabetically
so ethyl methyl
use -yl and -yl suffixes

and ether at the end

ethyl methyl ether

58
Q

functional group of amines

A

N: all sigma bonds and lone pair of electron

59
Q

how do you name amines?

A

name what is attached to the amine like DI-ethyl then add amine at the end.

-yl amine

60
Q

functional group amides

A

R-C(=O) - NH2

61
Q

how do you name amides?

A

you add the suffix and remove the -e and add amide
the carbon with the c=o of the amide is also considered when naming

ethanAMIDE

62
Q

WHAT IS THE GENERAL FORMULA OF ALKANES?

A

CnH2n+2

63
Q

WHAT DOES THE BOILING POINT OF SMALL ALKANES LOOK LIKE?

A

very low therefore they are gases

64
Q

what are constitutional isomers?

A

compounds with the same
molecular formula but the carbons are connected differently. like n-butane and iso-butane, neo-butane

65
Q

how do you name alkyl groups regardless of their position in the chain?

A

in alphabetical order

66
Q

how would you name Three methyl groups at positions 2, 5, and 7 in a 10 carbon molecule?

A

2,5,7-trimethyldecane

67
Q

what happens to boiling point as alkane carbons increase?

A

As the number of carbons in an alkane increases, the boiling point will increase due to the larger surface area and the increased van der Waals attractions.

DRUGS AND MEDICINE (7 decks)

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