BIOL 2113 QUESTIONS AND ASWERS LATEST UPDATE
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Biochemistry
The study of chemical composition and reactions of living matter
All chemical are either ___ or ___.
Inorganic and organic. Both are essential for life.
Inorganic Compounds
Water, salts and many acidds and bases
Do not contain carbon
Organic Compounds
Carbohydrates, fats protein and nucleic acids
Water
Most abundant inorganic compound. 60-80 % of the volume of living cells. Most
important inorganic compound because of its properties.
Water properties
High heat capacity
High heat of vaporization
Polar Solvent properties
Reactivity
Cushioning
High Heat Capacity
Ability to absorb and release heat with little temperature change.
Prevents Sudden changes in temperature.
High Heat of Vaporization
Evaporation requires large amounts of heat.
Useful cooling mechanism
Polar solvent properties
Dissolve and dissociates ionic substances
Forms hydration (water) layers around large molecules.
Ex: proteins
Body major transport medium
Reactivity
Necessary part of hydrolysis and dehydration synthesis reactions.
Cushioning
Protects certain organs from physical trauma. Ex: cerebrospinal fluid cushions nervous
system organs.
Salts
Ionic compounds that dissociate into separate ions water. Separate into
cations( positively charged molecules) and anions( negatively charged). Not including
H+ znd OH- ions
Acid and Bases
-both electrolytes
-ionize and dissociate in water
, Acids
Proton donors: they release hydrogen ions H+ bare protons (have no electrons) in
solution. Example: HCL H+ +CL-
Important Acids HCI (hydrochloric acid) HC2H3o2 (acetic acid, abbreviated HAc,
H2CO3 (carbonic acid)
Bases
Proton acceptors pick up H+ ions in solution. NaOH
When a base dissolves in solution, it releases a hydroxyl ion. Important bases.
Biocarbonate ion (HCO3) and ammonia(NH3)
ph Acid base concentration
-PH scale is a measurement of concentration of hydrogen ions-H positive - in a solution.
-The more hydrogen ions in a solution, the more acidic that solution is.
-The pH is negative logarithm of -H positive-in moles per liter that ranges from 0 to 14.
-PH scale is logarithmic, so each pH unit represents a 10 fold difference. example: a pH
5 solution is 10 times more acidic than a pH 6 solution.
Acidic
solutions have high H+ but low ph.
range from 0-6.99
Neutral
all neutral solutions are ph7. Pure water is ph neutral.
Alkaline
have low H+ but high ph
range 7.01-14
Neutralization reaction
acids and bases are mixed together
Displacement reactions occur, forming water and a salt
Buffers
Acidity involves only free H+ in solution, not H+ bound to anions. Resist abrupt and
large swings in pH. Can release hydrogen ions if pH rises. Can bind hydrogen ions if ph
falls. Convert strong acids or bases( completely dissociated) into weak ones ( slightly
dissociated)
Carbonic acid bicarbonate system (important buffer system of blood)
Homeostatic Imbalance 2.1
Enzymes in the body work within a very narrow pH range
An arterial ph of 7.0 during cardiopulmonary predicts a poor outcome. Patients
presenting with arterial pH of less than 6.85
Organic molecules contain
carbon. Exceptions CO2 and CO which are inorganic
Carbon
Electroneutral.
Shares electrons; never gain or loses them.
Forms four covalent bonds with other elements.
Carbon is unique to living systems.
Major organic compounds
carbohydrates, lipids, proteins, nucleic acids
Polymers
100% CORRECT A+ GRADED. Buy Quality Materials!
Biochemistry
The study of chemical composition and reactions of living matter
All chemical are either ___ or ___.
Inorganic and organic. Both are essential for life.
Inorganic Compounds
Water, salts and many acidds and bases
Do not contain carbon
Organic Compounds
Carbohydrates, fats protein and nucleic acids
Water
Most abundant inorganic compound. 60-80 % of the volume of living cells. Most
important inorganic compound because of its properties.
Water properties
High heat capacity
High heat of vaporization
Polar Solvent properties
Reactivity
Cushioning
High Heat Capacity
Ability to absorb and release heat with little temperature change.
Prevents Sudden changes in temperature.
High Heat of Vaporization
Evaporation requires large amounts of heat.
Useful cooling mechanism
Polar solvent properties
Dissolve and dissociates ionic substances
Forms hydration (water) layers around large molecules.
Ex: proteins
Body major transport medium
Reactivity
Necessary part of hydrolysis and dehydration synthesis reactions.
Cushioning
Protects certain organs from physical trauma. Ex: cerebrospinal fluid cushions nervous
system organs.
Salts
Ionic compounds that dissociate into separate ions water. Separate into
cations( positively charged molecules) and anions( negatively charged). Not including
H+ znd OH- ions
Acid and Bases
-both electrolytes
-ionize and dissociate in water
, Acids
Proton donors: they release hydrogen ions H+ bare protons (have no electrons) in
solution. Example: HCL H+ +CL-
Important Acids HCI (hydrochloric acid) HC2H3o2 (acetic acid, abbreviated HAc,
H2CO3 (carbonic acid)
Bases
Proton acceptors pick up H+ ions in solution. NaOH
When a base dissolves in solution, it releases a hydroxyl ion. Important bases.
Biocarbonate ion (HCO3) and ammonia(NH3)
ph Acid base concentration
-PH scale is a measurement of concentration of hydrogen ions-H positive - in a solution.
-The more hydrogen ions in a solution, the more acidic that solution is.
-The pH is negative logarithm of -H positive-in moles per liter that ranges from 0 to 14.
-PH scale is logarithmic, so each pH unit represents a 10 fold difference. example: a pH
5 solution is 10 times more acidic than a pH 6 solution.
Acidic
solutions have high H+ but low ph.
range from 0-6.99
Neutral
all neutral solutions are ph7. Pure water is ph neutral.
Alkaline
have low H+ but high ph
range 7.01-14
Neutralization reaction
acids and bases are mixed together
Displacement reactions occur, forming water and a salt
Buffers
Acidity involves only free H+ in solution, not H+ bound to anions. Resist abrupt and
large swings in pH. Can release hydrogen ions if pH rises. Can bind hydrogen ions if ph
falls. Convert strong acids or bases( completely dissociated) into weak ones ( slightly
dissociated)
Carbonic acid bicarbonate system (important buffer system of blood)
Homeostatic Imbalance 2.1
Enzymes in the body work within a very narrow pH range
An arterial ph of 7.0 during cardiopulmonary predicts a poor outcome. Patients
presenting with arterial pH of less than 6.85
Organic molecules contain
carbon. Exceptions CO2 and CO which are inorganic
Carbon
Electroneutral.
Shares electrons; never gain or loses them.
Forms four covalent bonds with other elements.
Carbon is unique to living systems.
Major organic compounds
carbohydrates, lipids, proteins, nucleic acids
Polymers
