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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
Proton
H+
26
Hydronium Ion
H3O+
27
Hydrogen atom
H.
28
Hydride
H: or H-
29
Hydrogen gas or molecule
H2 or H:H
30
Hydroxide
OH-
31
pH scale
-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
pH and [H+] of human blood
pH=7.35-7.45 | [H+]= 40nM
33
Strong Acids
dissociate 100% | -release all possible protons [H+]
34
Weak Acids
do not dissociate 100%
35
what are the Strong acids you need to know
``` HCl. hydrochloric acid HBr. hydrobromic acid HI. hydroiodic acid HNO3 nitric acid HClO4 perchloric acid H2SO4 sulfuric acid ```
36
Strong Bases
Dissociate 100% In water
37
Weak Bases
dissociates less than 100% in water
38
Weak Bases you need to know
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
Buffer - def - who? - How does a buffer work
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
What is a buffer in our blood?
Carbonic acid (weak acid)- H2CO3 H2CO3 H+ + HCO3-
41
Henderson Hasselbalch equation
pH=pKa + log [Base/Acid]
42
Thermodynamics def
Is the study of the effects of work, heat, and energy on a system
43
Thermodynamics: System and Surroundings Def
System- part of the universe you are interested in studying Surroundings- areas outside of the system
44
Types of systems and def
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
What type of system (from thermo) do humans use?
Open system | -ingest food/give off waste
46
Entropy
S | -Disorder or randomness
47
Enthalpy
H | -Heat content
48
Temperature
T | -Kelvin
49
Gibbs Free Energy
G
50
Thermodynamics formulas
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
Thermodynamics: | Zeroth Law
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
Thermodynamics: | First Law
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
Thermodynamics: | Second Law
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
Thermodynamics: | Third Law
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
Gibbs Free Energy (delta G) - equation - Rxns with Delta G +/-
DeltaG=DeltaH- TDeltaS Rxns with a -DeltaG occur spontaneously Rxns with a +DeltaG are NONspontaneous
56
Thermodynamics: Living Organism
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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