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WorksheetsBiochem Exam 1 Practice
Total questions: 57
Worksheet time: 29mins
Subunit of protein
Subunit of carbohydrates
Subunit of nucleic acids
Subunit of lipids
4 types of macromolecules
Polymer of protein
Polymer of carbohydrates
Weakest of the intermolecular forces
Hydrogen Bonds
Hydrophobic Interactions
Ionic Interactions
Van Der Waals Interactions
True or False: Ionic Interactions can also be Hydrogen Bonds
TRUE
FALSE
What do Van Der Waals Interactions depend on?
The size of the atoms/molecules
The distance between the atoms/molecules
The size AND distance between the atoms/molecules
TRUE/FALSE
More polar atoms produce stronger hydrogen bonds
Which of the following atoms produces the strongest hydrogen bond?
Bond between two nucleic acids
Phosphodiester Bond
Peptide Bond
Glycosidic
Esther
Bond between two proteins
Phosphodiester Bond
Peptide Bond
Glycosidic
Esther
Bond between two sugars
Phosphodiester Bond
Peptide Bond
Glycosidic
Esther
TRUE/FALSE
Ionic bonds contribute to the stability of proteins
TRUE
FALSE
Viruses are _____
Genetic material coated in protein
Genetic material coated in lipids
Genetic material coated in sugars
Genetic material coated in nucleic acids
How many hydrogen bonds does water form?
Water has a BLANK dielectric constant.
High
Low
Moderate
Zero
Ions are always BLANK in water and carry around a BLANK
Hydrogenated; Hydrogen Shell
Hydrated; Hydration Shell
Nonpolar solutes being added to water cause BLANK in entropy.
An increase
A decrease
No Change
T/F: Nonpolar solutes "organize" water.
TRUE
FALSE
T/F: Amphiphilic and Amphipathic are synonyms
TRUE
FALSE
A good example of an amphipathic molecule is BLANK
fatty acid
nucleic acid
protein
carbohydrates
The head of a fatty acid is BLANK and the tail is BLANK
Polar ; Non-Polar
Non-polar ; Polar
Hydrated ; Non-Hydrated
Amphipathic ; Amphiphilic
True/False: Hydrogen Bonding is responsible for water's low dielectric constant
True
False
pH is the BLANK of the hydrogen ion concentration
negative logarithm
positive logarithm
neutral logarithm
pH = BLANK
-Log[H+]
+Log[H+]
-Log[OH-]
+Log[OH-]
pKw = BLANK
pH + pOH = 14
pH - pOH = 14
pH - 7 = pOH
pOH - 7 = pH
Henderson-Hasselbalch Equation
pH = BLANK
pKa + log([A-]/[HA])
pKa + ln([A-]/[HA])
pKa + log([HA]/[A-])
pKa + ln([HA]/[A-])
1st law of thermodynamics
•The total energy of the universe must be constant
•Energy may be:
•converted from one form to another
•Used to do work
•Moved within a system or between system and surroundings
•But it cannot be destroyed or created in any ordinary chemical process
•Systems tend to proceed from ordered (low entropy or low-probability) states to disordered (high-entropy or high-probability) states
•The entropy of the system plus surroundings is unchanged by reversible processes
•The entropy of the system increases for irreversible processes
•All naturally occurring processes proceed toward equilibrium – that is, to a state of minimum potential energy
•Energy flows spontaneously so as to become diffused or dispersed or spread out
•The entropy of any crystalline, perfectly ordered substance must approach zero as the temperature approaches 0 K
•At T = 0 K, entropy is exactly zero
2nd law of thermodynamics
•The total energy of the universe must be constant
•Energy may be:
•converted from one form to another
•Used to do work
•Moved within a system or between system and surroundings
•But it cannot be destroyed or created in any ordinary chemical process
•Systems tend to proceed from ordered (low entropy or low-probability) states to disordered (high-entropy or high-probability) states
•The entropy of the system plus surroundings is unchanged by reversible processes
•The entropy of the system increases for irreversible processes
•All naturally occurring processes proceed toward equilibrium – that is, to a state of minimum potential energy
•Energy flows spontaneously so as to become diffused or dispersed or spread out
•The entropy of any crystalline, perfectly ordered substance must approach zero as the temperature approaches 0 K
•At T = 0 K, entropy is exactly zero
3rd law of thermodynamics
•The total energy of the universe must be constant
•Energy may be:
•converted from one form to another
•Used to do work
•Moved within a system or between system and surroundings
•But it cannot be destroyed or created in any ordinary chemical process
•Systems tend to proceed from ordered (low entropy or low-probability) states to disordered (high-entropy or high-probability) states
•The entropy of the system plus surroundings is unchanged by reversible processes
•The entropy of the system increases for irreversible processes
•All naturally occurring processes proceed toward equilibrium – that is, to a state of minimum potential energy
•Energy flows spontaneously so as to become diffused or dispersed or spread out
•The entropy of any crystalline, perfectly ordered substance must approach zero as the temperature approaches 0 K
•At T = 0 K, entropy is exactly zero
An isolated system BLANK
cannot exchange matter or energy
can exchange energy only
can exchange matter and energy
can exchange matter only
A closed system BLANK
cannot exchange matter or energy
can exchange energy only
can exchange matter and energy
can exchange matter only
An open system BLANK
cannot exchange matter or energy
can exchange energy only
can exchange matter and energy
can exchange matter only
Enthalpy is BLANK
the heat content of a system
the measure of disorder in a system
Entropy is BLANK
the heat content of a system
the measure of disorder in a system
The peptide bond is typically bound in BLANK conformation.
Trans
Cis
Peptide bonds have a partial BLANK
Negative Charge
Positive Charge
Double Bond Character
Triple Bond Character
Proteins are BLANK polymers of amino acids.
Unbranched
Branched
Large
Small
The peptide backbone is a repeating sequence of BLANK
N, Alpha Carbon, Carbonyl Carbon
Alpha Carbon, N, Carbonyl Carbon
Carbonyl Carbon, Alpha Carbon, N
Alpha Carbon, Carbonyl Carbon, N
Amino acids join BLANK
Head to tail
Head to head
Tail to tail
Tail to head
The amide plane
The six atoms of the peptide bond
The four atoms of the peptide bond
The three atoms of the peptide bond
The seven atoms of the peptide bond
Reduced = BLANK
Accepts Electrons
Donates Electrons
Oxidized = BLANK
Accepts Electrons
Donates Electrons
Phosphate, Imidazole, and Carbonic acid are BLANK
Important Buffer systems
Non-essential buffer systems
When DELTA H > 0
When DELTA H < 0
When DELTA G = 0
The reaction is exergonic
The reaction is endergonic
The reaction is at equilibrium
When DELTA G > 0 the reaction is BLANK
Exergonic
Endergonic
at equilibrium
When DELTA G > 0 the reaction is BLANK
Endergonic
Exergonic
at equilibrium
TRUE/FALSE: Enthalpy, Gibbs Free Energy, and Entropy are not state functions.
False
True
Phosphoric Anhydrides are the class of what two important molecules?
ADP and ATP
NADH and NAD-
Sugar and Protein
Electrons and Protons
Highly negative DELTA G of hydrolysis of ADP/ATP is driven by BLANK
Electrostatic repulsion, entropy, and resonance
Enthalpy
Entropy Only
Electrostatic Repulsion Only
How many ionizable hydrogen on ATP?
4
3
2
5
ATP contains how many pyrophosphate linkages?
2
1
3
4
