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MBB 222 > Topic 2 > Flashcards

Topic 2 Flashcards

1
Q

What are organic molecules?

A
  • are the building blocks of living things
  • contain carbon and hydrogen
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2
Q

What is organic chemistry?

A

The study of the chemistry of carbon compounds

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3
Q

What does the synthesis of urea show in 1828?

A
  • demonstrated that organic compounds can be prepared in the laboratory from non-living material
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4
Q

DNA

A

Deoxyribonucleic acid

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5
Q

RNA

A

Ribonucleic acid

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6
Q

Trends for electronegativity

A

Increasing towards the right and going upwards

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7
Q

Electronegativity

A
  • tend to accept electrons
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8
Q

Electropositive

A

Tend to give up electrons

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9
Q

How do ionic bonds form?

A

Elements near the edges of the periodic table give or accept electrons causing them to become charged. Then they form ionic bonds with each other due to their opposite charges

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10
Q

How do covalent bonds form?

A

Elements near the middle that do no give up or accept electrons easily tend to share electrons forming covalent bonds

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11
Q

Polar covalent bond

A

Electrons are shared but not equally

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12
Q

Nonpolar covalent bond

A

Electrons shared equally

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13
Q

What makes carbon the central component of all molecules that form living organisms?

A

Carbon’s ability to form 4 covalent bonds with as many as 4 different atoms

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14
Q

Carbon hybridization

A

-two non bonding electrons fill the 1s orbital
- 4 valence or bonding electrons are distributed in 4 orbitals in second energy level; one in the 2s orbital, one in each 2px, 2py, and 2pz orbital.
- four orbitals can hybridize to generate 4 sp3 orbitals of equal energy

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15
Q

Carbon sp3 hybridization geometry

A
  • adopts a tetrahedral geometry
  • forms 4 single bonds, each with one electron from each of its sp3 orbitals
  • the angle between the C-H bonds are 109.5
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16
Q

What are the simplest organic compounds?

A

Hydrocarbons, compounds of carbon and hydrogen

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17
Q

The simplest organic compound

A
  • methane, the major component of natural gas
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18
Q

What is methane comprised of?

A
  • a single C atom covalently bonded to 4 H atoms in a tetrahedral manner
  • angle is 109.5
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19
Q

How are C-H bonds formed?

A
  • formed by overlap between the sp3 orbitals of C and the s orbitals of the Hs.
  • the single e- in each of these orbitals is shared between the two atoms
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20
Q

What do shared orbitals produce?

A
  • produce a new sigma orbital, the covalent bond formed by the shared electrons
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21
Q

Some simple hydrocarbons - alkanes

A

Methane - 1 group
Ethane - 2 groups
Propane - 3 groups
Butane - 4 groups

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22
Q

Alkanes

A

Only contain single bonds
- both C-H and C-C bonds are sigma bonds
- the C-C bonds are between sp3 orbitals

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23
Q

What are aliphatic compounds?

A

-linear, branched or cyclic hydrocarbons that are not aromatic
- can have double and triple bonds

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24
Q

Sp2 hybridization

A

Carbon—carbon double bonds
- the sp2 orbitals between 2sp2 hybridized carbons overlap to form a sigma bond
- the second bond is formed by overlap between p bonds to to create a pi bond
- the two bonds of this double bond are non equivalent

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25
Q

So hybridization

A

Carbon-carbon triple bonds
- two p orbitals overlap between 2 sp hybridized carbons forming 2 pi bonds
- the sigma bonds between the sp orbitals make a third bond

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26
Q

Where can rotation occur?

A

Only across a single bond, not across a double or triple bond

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27
Q

What does removing a hydrogen from an alkane result in?

A

In alkyl group or substituent which can bond to other atoms/molecules/groups

28
Q

OH

A

Alcohol

29
Q

NH2

A

Amine

30
Q

F, Cl, Br, I

A

Alkyl halide

31
Q

OR

A

Ether

32
Q

Polarity

A

The asymmetric distribution of e- results in polarity
When there is a partial positive charge on one end, and a partial negative charge on the other end

33
Q

Polar molecules

A

Asymmetric charge distribution due to unequal sharing of bonding electrons

34
Q

Polar covalent bond

A

When an electronegative atom will haver a greater share of the bonding electrons than the electropositive atom, a polar covalent bond forms

35
Q

Permanent dipole

A

When electrons on an atom results in having the molecule having a partial negative charge while another part of the molecule has a partial positive charge

36
Q

Non-polar molecules

A
  • symmetric charge distribution for their bonding electrons
  • also when the bounded atoms are identical or of similar electronegativity
37
Q

What do function groups of simple organic compounds have?

A
  • have specific properties and reactivities based on their polarity, electronegativity
  • more reactive than their alkyl substituents
38
Q

Thiol

A

Functional group is sulfhydryl -SH

39
Q

Acids

A

The function groups is a carboxyl, COOH, comprised of a carbonyl group (carbon with double to oxygen) bonded to a hydroxyl group via the carbon

40
Q

Amines

A

A nitrogen
- is basic (can be protonated, becoming positively charged

41
Q

Phosphate

A

Can be pronated
- acidic

42
Q

Amides

A

Hydroxyl group of a carboxyl if acid is replaced by an amino acid

43
Q

Localized electrons

A
  • when the molecules have discrete single and double bonds
  • electrons stay on their atom
44
Q

Delocalized electrons

A
  • molecule does not have discrete single and double C-O bonds
  • electrons do not stay on their atom
45
Q

Resonance

A

The delocalization of electrons across bonds
- results in a more stable molecule

46
Q

What are amino acid in proteins joined by?

A

By peptide bonds with delocalized electrons

47
Q

What is a important property of peptides/proteins?

A

Delocalization

48
Q

How does delocalization of electrons limit rotation?

A
  • it imposes partial double bond character on the bonds and limits rotation about those bonds
49
Q

What does limited for rotation affect?

A
  • influences the folding of that polypeptide
50
Q

Aromatic compounds

A
  • cyclic ring-shaped molecules that have alternating single and double bonds that result in the delocalization of their electrons to form a pi (p) electron cloud
51
Q

What is the simplest aromatic compound?

A

Benzene (C6H6)

52
Q

Compare and contrast an aromatic molecule and an aliphatic molecule

A

Aromatic:
- cyclized 6 carbon ring with sp2 carbons linked by alternating single and double bonds
- each C has one H
- rigid, planar structure,
- electrons are delocalized in a pi bond
- unique properties due to resonance
- very stable (not reactive)

Aliphatic:
- cyclized 6 carbon ring with sp3 carbons linked by single bonds
- each C has two Hs
- flexible, non-planar structure

53
Q

Benzene

A
  • a planar molecule
  • six identical carbon carbond bonds
  • each pi electron is shared by all six carbons
  • pi electrons are delocalized
54
Q

What cyclic molecules are aromatic?

A

Only the ones that form a closed loop of overlapping pi orbitals

55
Q

What physical properties affect aromatic compounds interactions with other molecules?

A
  • flat molecular structures
  • a tendency to stack upon one another, especially in water (Electrostatic attraction)
56
Q

Can 5-membered rings also be aromatic compounds?

A

Yes

57
Q

What 4 of the 20 naturally occurring amino acids in proteins contain aromatic side chains?

A
  • histidine (contains an imidazole group)
  • phenylalanine (contains an phenyl [=benzene] group)
  • tyrosine (contains a phenol [a phenyl ring with a hydroxyl])
  • tryptophan (contains an indol group)
58
Q

What are aromatic bases?

A

Components of nucleotides which form DNA
- the bases get stacked in the DNA which contributes to the stability of the DNA

59
Q

Isomers

A

Non-identical compounds having the same molecular formula

60
Q

constitutional isomers

A

Have the same molecular formula bit their atoms are linked differently

61
Q

Stereoisomers

A
  • have the same molecular formula and the same linkage between the atoms, but differ in the 30 dimensional orientation of the atoms in space
  • cis-trans isomers
  • isomers that contain asymmetric centers
62
Q

Cis-trans stereoisomers in alkenes

A
  • rotation can occur across a single bond
  • cis: R groups on the same side
  • trans: R groups on opposite sides
63
Q

Chiral objects

A
  • chiral objects are not symmetrical.
  • the mirror image of a chiral object can not be superimposed on the object
  • do not have a plane of symmetry
    This is caused by an asymmetric carbon center
64
Q

Achiral objects

A
  • these objects are symmetrical
  • can be superimposed upon their mirror images
65
Q

Enantiomers

A
  • chiral molecules that are mirror images one another
  • distinct compounds with different properties

MBB 222 (5 decks)

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