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MC Biochem 1 > Chpt 1-chemistry > Flashcards

Chpt 1-chemistry Flashcards

1
Q

micro prefix

A

u=1x10^-6

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2
Q

nano prefix

A

n=1x10^-9

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3
Q

pico prefix

A

p=1x10^-12

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4
Q

Covalent Bonds

  • def
  • energy
  • length
A 
Sharing a pair of electrons
Energy-355 KJ'mol
length
C-C bond 1.54A
C=C bond 1.34A
CtripleC 1.20

STRONG interaction do not break spontaneously under physiological conditions

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5
Q

Hydrogen Bonds

  • def
  • energy
  • length
A

Sharing of H atom, H has to be shared with N, O, or F
Energy- 4-20 KJ/mol
Length- 1.5-2.6A

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6
Q

Ionic Interaction (Electrostatic Interactions)

  • def
  • energy
  • length
A

Attraction of opposite charges (partial positive/negative)
Energy-5.8
Length-Varies

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7
Q

Van der Waals interactions

  • def
  • energy
  • length
A

interaction of electron clouds
Energy- 2-4
Length-N/A

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8
Q

Hydrophobic interactions

  • def
  • energy
  • length
A

interaction of non polar substances
Energy-very weak
length-N/A

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9
Q

When is Hydrogen bonding the strongest?

A

Strongest when atoms are in a straight line:

  • in DNA, h-bonding holds together complementary strands
  • In proteins, H bonds stabilize alpha helixes and beta sheets
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10
Q

Ionic bonds are important where?

A

at active sites of enzymes

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11
Q

Most important compound in biochem?

A

WATER

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12
Q

Facts about H20

A

-70% of cell’s mass
-has unique properties–>matrix of life
1)BP of water is 100 C
2) MP of water is 0 C
3) High Specific Heat
4) High high (enthalpy) of Vaporization (delta H)
5)Universal Solvent
6)High Surface Tension
7) Density of Solid Water (ICE) is less than density of liquid water
8)Water Ionizes
H2O H+ + OH-

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13
Q

Specific Heat

A

measure of the amount of heat required to raise the temp of one g of water 1 degree C

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14
Q

Heat (enthalpy) of vaporization

A

amount of heat required to convert a liquid to a gas (phase change)

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15
Q

Solution

A

uniform molecular mixture of two or more substances

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16
Q

Solvent

A

solvent in the greatest quantity

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17
Q

Solute

A

substance in lesser quantity

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18
Q

substances are categorized depending on there interaction with water; what are the categories?

A

hydrophilic (water loving)
-dissolves in water

Hydrophobic (water fearing)
-poorly soluble in water

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19
Q

Surface tension

A

the measure of how difficult it is to break the surface of the liquid

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20
Q

Describe water and its high surface tension

A

Water is:

  • Cohesive- attractive to self
  • Adhesive- attractive to surfaces
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21
Q

Why is water so important to life?

A
  1. water is a liquid at physiological temperatures
  2. water has an unusually high boiling point for its molecular weight
  3. Water is a good thermal regulator. Large amount of heat is required to change its temperature
  4. water provides very effective heat dissipationf
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22
Q

Why does water have such unusual properties?

A
  • Shape of molecule
  • Hydrogen Bond–> weak intermolecular bond formed between partial positive of the H and partial negative of Oxygen
  • -> millisecond duration
  • -> requires energy to break
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23
Q

Hydrogen bonds in water explains:

A
  • High Boiling Point/Freezing point
  • High heat of vaporization
  • Universal Solvent
  • High surface tension adhesive/cohesive forces
  • Density of solid water (ice) is less than density of solid liquid
24
Q

Four formulas to convert between pH, pOH, [H+], & [Oh-]

A

1x10^-14=[H+][OH-]

14=pH + pOH

pOH= -log [OH-]

pH= -log [H+]

25
Q

Proton

A

H+

26
Q

Hydronium Ion

A

H3O+

27
Q

Hydrogen atom

A

H.

28
Q

Hydride

A

H: or H-

29
Q

Hydrogen gas or molecule

A

H2 or H:H

30
Q

Hydroxide

A

OH-

31
Q

pH scale

A

-measure of [H+]
-continuous logarithmic scale 0-14
pH=7 is neutral
pH=0-6.99 acidic
pH= 7.01-14 basic
-one pH change represents 10 fold change in [H+]

32
Q

pH and [H+] of human blood

A

pH=7.35-7.45

[H+]= 40nM

33
Q

Strong Acids

A

dissociate 100%

-release all possible protons [H+]

34
Q

Weak Acids

A

do not dissociate 100%

35
Q

what are the Strong acids you need to know

A 
HCl.  hydrochloric acid
HBr.  hydrobromic acid
HI.     hydroiodic acid
HNO3 nitric acid
HClO4 perchloric acid
H2SO4 sulfuric acid
36
Q

Strong Bases

A

Dissociate 100% In water

37
Q

Weak Bases

A

dissociates less than 100% in water

38
Q

Weak Bases you need to know

A

Group I:
LiOH. Lithium Hydroxide
NaOH Sodium Hydroxide
KOH Potassium Hydroxide

Group II: 2 OH ions
Ca(OH)2 Calcium Hydroxide
Sr(OH)2 Strontium Hydroxide
Ba(OH)2 Barium Hydroxide

39
Q

Buffer

  • def
  • who?
  • How does a buffer work
A

substance that resists pH changes in a solution thus stabilizing its relative pH

  • weak acids and conjugate bases
  • buffer works one unit either side of pka (buffering range)
40
Q

What is a buffer in our blood?

A

Carbonic acid (weak acid)- H2CO3

H2CO3 H+ + HCO3-

41
Q

Henderson Hasselbalch equation

A

pH=pKa + log [Base/Acid]

42
Q

Thermodynamics def

A

Is the study of the effects of work, heat, and energy on a system

43
Q

Thermodynamics: System and Surroundings Def

A

System- part of the universe you are interested in studying

Surroundings- areas outside of the system

44
Q

Types of systems and def

A

isolated system- system that does not exchange matter or energy with its surroundings

closed system- system that exchanges energy with surroundings but not matter

Open system- system that exchanges energy and matter with surrounds

45
Q

What type of system (from thermo) do humans use?

A

Open system

-ingest food/give off waste

46
Q

Entropy

A

S

-Disorder or randomness

47
Q

Enthalpy

A

H

-Heat content

48
Q

Temperature

A

T

-Kelvin

49
Q

Gibbs Free Energy

A

G

50
Q

Thermodynamics formulas

A

Total Energy= Usable Energy + Unusable Energy
Enthalpy(H)= Free Energy (G)+ Temp(T)Entropy(S)
Or H=G+TS

Solve for G
G=H-TS
**we can not measure G, H, or S directly thus delta or change multiplied through

deltaG=deltaH-TdeltaS

51
Q

Thermodynamics:

Zeroth Law

A

If two systems are in thermal equilibrium with a third System, they must be in thermal equilibrium with each other
-Defines temperature (T) and thermodynamic equilibrium

If A=B and B=C, thus A must equal C

52
Q

Thermodynamics:

First Law

A

Total energy of a system and its surrounds is constant
other ways to state:
-the energy content of the universe is constant
-energy can be neither created nor destroyed. it can only change forms

Defines heat, work, and energy

53
Q

Thermodynamics:

Second Law

A

The entropy of any isolated system never decreases. Such systems spontaneously evolve towards thermodynamic equilibrium– The state of maximum entropy (S) of the system
or in other terms:
-the total ENTROPY (S) of a system plus that of its surrounds always increases
-entropy is a measure of randomness or disorder

54
Q

Thermodynamics:

Third Law

A

As temperature approaches absolute zero, the entropy of a system approaches a constant minimum

or in other terms:
-the entropy of a perfect crystal at absolute zero is zero

55
Q

Gibbs Free Energy (delta G)

  • equation
  • Rxns with Delta G +/-
A

DeltaG=DeltaH- TDeltaS

Rxns with a -DeltaG occur spontaneously
Rxns with a +DeltaG are NONspontaneous

56
Q

Thermodynamics: Living Organism

A

Living organisms exist in a dynamic steady state NEVER AT EQUILIBRIUM with their surrounds

  • maintaining steady state requires an input of E
  • Equilibrium=death

Living organisms are open systems

  • Organisms take up matter/energy
  • change energy into
    1) Useful energy–>cellular work: chemical synthesis, mechanical work, gradients (osmotic and electrical), Light production, Genetic information transfer
    2) Heat
    3) Metabolic Products- CO2, NH3, H2O, HPO42- (increases entropy in surrounds)
    4) synthesize complex polymers (macromolecules)–> decreases entropy in the system

MC Biochem 1 (30 decks)

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