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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
So hybridization
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
26
Where can rotation occur?
Only across a single bond, not across a double or triple bond
27
What does removing a hydrogen from an alkane result in?
In alkyl group or substituent which can bond to other atoms/molecules/groups
28
OH
Alcohol
29
NH2
Amine
30
F, Cl, Br, I
Alkyl halide
31
OR
Ether
32
Polarity
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
Polar molecules
Asymmetric charge distribution due to unequal sharing of bonding electrons
34
Polar covalent bond
When an electronegative atom will haver a greater share of the bonding electrons than the electropositive atom, a polar covalent bond forms
35
Permanent dipole
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
Non-polar molecules
- symmetric charge distribution for their bonding electrons - also when the bounded atoms are identical or of similar electronegativity
37
What do function groups of simple organic compounds have?
- have specific properties and reactivities based on their polarity, electronegativity - more reactive than their alkyl substituents
38
Thiol
Functional group is sulfhydryl -SH
39
Acids
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
Amines
A nitrogen - is basic (can be protonated, becoming positively charged
41
Phosphate
Can be pronated - acidic
42
Amides
Hydroxyl group of a carboxyl if acid is replaced by an amino acid
43
Localized electrons
- when the molecules have discrete single and double bonds - electrons stay on their atom
44
Delocalized electrons
- molecule does not have discrete single and double C-O bonds - electrons do not stay on their atom
45
Resonance
The delocalization of electrons across bonds - results in a more stable molecule
46
What are amino acid in proteins joined by?
By peptide bonds with delocalized electrons
47
What is a important property of peptides/proteins?
Delocalization
48
How does delocalization of electrons limit rotation?
- it imposes partial double bond character on the bonds and limits rotation about those bonds
49
What does limited for rotation affect?
- influences the folding of that polypeptide
50
Aromatic compounds
- 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
What is the simplest aromatic compound?
Benzene (C6H6)
52
Compare and contrast an aromatic molecule and an aliphatic molecule
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
Benzene
- a planar molecule - six identical carbon carbond bonds - each pi electron is shared by all six carbons - pi electrons are delocalized
54
What cyclic molecules are aromatic?
Only the ones that form a closed loop of overlapping pi orbitals
55
What physical properties affect aromatic compounds interactions with other molecules?
- flat molecular structures - a tendency to stack upon one another, especially in water (Electrostatic attraction)
56
Can 5-membered rings also be aromatic compounds?
Yes
57
What 4 of the 20 naturally occurring amino acids in proteins contain aromatic side chains?
- 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
What are aromatic bases?
Components of nucleotides which form DNA - the bases get stacked in the DNA which contributes to the stability of the DNA
59
Isomers
Non-identical compounds having the same molecular formula
60
constitutional isomers
Have the same molecular formula bit their atoms are linked differently
61
Stereoisomers
- 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
Cis-trans stereoisomers in alkenes
- rotation can occur across a single bond - cis: R groups on the same side - trans: R groups on opposite sides
63
Chiral objects
- 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
Achiral objects
- these objects are symmetrical - can be superimposed upon their mirror images
65
Enantiomers
- chiral molecules that are mirror images one another - distinct compounds with different properties

MBB 222 (5 decks)

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