Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Biomolecules > interactions etc > Flashcards

interactions etc Flashcards

1
Q

What is an element?

A

A substance which cannot be split by chemical means

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is an atom?

A

The smallest unit of an element, which when split open loses its characteristic chemical properties

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is the difference between relative abundance and relative atomic mass

A

Relative abundance refers to the percentage of a specific isotope in a sample

Relative atomic mass is the weighted mass of the entire sample

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Orbitals with the same energy in a subshell are _

A

degenerate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

equivalent orbitals in a shell are

A

subshells

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

hund’s rule

A

electrons will first occupy an empty orbital

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

reactivity of an atom depends on

A

the tendency of the valence electrons to interact with other atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

a full valence shell requires

A

filled s and p orbitals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

how many electrons confer maximum stability to an atom?

A

8

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

two non metals form

A

covalent bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

non metal and metals form

A

ionic bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

metals are generally found on the _ hand side of the periodictable

A

left

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

non metals are generally found on the _ hand side of the periodic table

A

right

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

ionic compounds exist in what structure

A

lattices, repetitive and organised patterns

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

which compounds don’t form discrete molecules

A

ionic compounds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

what kinds of orbitals are formed from the overlap of two orbitals?

A

a low energy bonding orbital

a high energy anti-bonding orbital

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

what is a hypervalent atom?

A

one holding more than 8 electrons in a shell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

give two examples of hypervalent atoms relevant to biological systems

A

sulfur and phosphorous

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

what is a dative covalent bond?

A

a shared pair of electrons coming from only one of the atoms participating in the bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

give an example of a compound with dative bonding

A

the ammonium ion NH4+

a proton shares one of nitrogens fulll orbitals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

what are dative bonding important for in biological systems

A

binding of metals, (binding iron in haem group)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

which compounds have bonds that are in between single and double bonds

A

aromatic conjugated systems

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

what forms from overlap of adjacent p orbitals?

A

a conjugated system

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

where can a conjugated system occur?

A

wherever there are single bonds surrounded by double bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

give an example of a compound with a conjugated system

A

beta carotene, benzene ring

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

a resonance compound is

A

a hybrid of two structures

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

give an example of a resonance compound1

A

O3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

what kind of compounds feature ionic and covalent bonding

A

polyatomic ionic compounds

29
Q

give an example of a polyatomic ionic compound

A

calcium carbonate

30
Q

what is the only prevalent polyatomic cation?

A

NH4+ ammonium ion

31
Q

an atom which cannot form bonds is

A

inert

32
Q

what is electronegativity?

A

the strength of the force of attraction which an atom can exert on an electron

33
Q

what happens to electronegativity values as you move across periods

A

it increases

34
Q

why are non-covalent molecular interactions important for specificity

A

they allow molecules to form a stable shape which is complementary with other molecules so that they may function together

35
Q

what causes dispersion forces?

A

temporary unequal distributions in electrons

36
Q

dipole moment is a vector pointing to

A

region of highest electron density

37
Q

give an example of a nonpolar molecule with polar bonds

A

carbon dioxide

38
Q

a molecule with polar bonds can be nonpolar if

A

symmetric orientation results in dipole effects cancelling out eachother

39
Q

what are induced dipoles

A

when a partial negative charge in one region induces partial positive charges in neighbouring regions

40
Q

what two factors increases the dispersion forces that a molecule experiences

A

size of molecule (greater attraction)

conformation, molecules that can get closer experience greater forces

41
Q

steric repulsion operates at distances _ than dispersion forces

A

shorter

42
Q

hydrogen bonding is dependent on the presence of

A

oxygen, fluorine or nitrogen

43
Q

water molecules can only interact in a stable way with

A

polar molecules

44
Q

what determines a substances physical state

A

the cumulative strength of the forces of molecular interactions

45
Q

what is a salt bridge

A

when a charged amino acid side chain interacts with an oppositely charged one through ionic forces

46
Q

hydrophobic forces associate _

A

through dispersion forces once they have been partitioned

47
Q

polar molecules have _ melting and boiling points

A

higher, due to more interactions

48
Q

sickle cell anemia causes

A

different shape of haemoglobin,

binds oxygen still but causes blockages and oxygen starvation

49
Q

the atomic radius is

A

half of the distance between two atoms of same element in a covalent bond

50
Q

bond length is

A

the sum of the atomic radii of two covalently bonded atoms

51
Q

atoms with larger valence shell numbers have

A

larger atomic radii

52
Q

as more electrons enter a valence shell, the atomic radius

A

goes down

greater forces of attraction between nucleus and electrons

53
Q

double and triple bonds are _ than single bonds

A

shorter

54
Q

VSEPR excludes

A

pi bonds

55
Q

VSEPR is concerned with

A

bonding and non bonding pairs

56
Q

valence pairs arrange themselves geometrically in order to

A

minimize repulsive forces

57
Q

why is carbon dioxide linear?

A

only two bonds considered for VSEPR

the pi bonds are not considered

58
Q

nonbonding pairs exert

A

greater repulsive forces, pushing bond angles tighter

59
Q

what hybridization will occur for 4 sigma bonds?

A

sp3

60
Q

what type of hybridizarion will occur for 2 sigma bonds

A

sp

61
Q

pi bonds are formed from

A

the overlapping of unhybridized orbitals

62
Q

rotation around single bonds can occur when

A

hybridized orbitals are symmetric round rthe bond, no disruption, bond angles conserved, minimal steric repulsion

63
Q

non bonding pairs undergo hybridization, they are treated as

A

sigma bonds

64
Q

why is rotation not possible around pi bonds

A

overlapm of the orbitals would be disrupted

65
Q

when is rotation around a single bond not possible

A

if bond is part of a delocalised system

66
Q

why are some bonds ni peptide bonds prevented form rotatting

A

due to delocalised system

67
Q

the bonds in peptide bonds that can rotate are limited by

A

long side chains, which cause limitations due to steric repulsions

steric hindrance

68
Q

peptide bonds can only rotate through _ angles

A

dihedral

69
Q

what conformations can a cyclic compound adopt

A

chair, boat

Biomolecules (12 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions