Introduction to Biochemistry
1. DNA, RNA and proteins are
a. Homopolymers b. Linear polymers
c. Monomeres d.
Heteromeres
2. DNA is aptly known as the
a. Information provider
b. Intermediary in the genetic information flow
c. Work-horse of the cell
d. Cellular structural backbone
3. RNA is aptly known as the
a. Information provider
b. Intermediary in the genetic information flow
c. Work horse of the cell
d. Cellular structural backbone
4. Proteins are aptly known as the
a. Information provider
b. Intermediary in the genetic information flow
c. Work horses of the cell
d. 5. The strongest bonds are
a. Non-covalent linkages b. Covalent bonds
c. Van der Waals forces d. Hydrophobic
interactions
6. Most biochemical reactions rely on
a. Non-covalent linkages b. Covalent bonds
c. Van der Waals forces d. Hydrophobic
interactions
7. Non-covalent bonds do not include
a. Hydrogen bond b. Van der
Waals forces
c. Sharing or exchange of electrons d. Electrostatic interactions
8. Electrostatic interaction energy is defined by
a. Coulomb's law b. Coombs
test
c. Contact distance
d.
Hydrogen bonds
9. The energy range of hydrogen bonds is
a. 1 kcal mol-1 b. 3
kcal mol-1
c. 13 kcal mol-1 d. 31
kcal mol-1
10. The energy of a typical carbon-carbon covalent bond
has an energy of
a. 58 kcal mol-1 b. 8
kcal mol-1
c. 5 kcal mol-1 d. 85
kcal mol-1
11. Typically, an atom pair due to Van der Waals
interactions has an energy of
a. 1.0 to 5.0 kcal mol-1 b. 0.5 to 1.0 kcal
mol-1
c. 0.05 to 0.5 kcal mol-1 d. 5.0 to 10.0 kcal
mol-1
12. Water is
a. Planar b.
Linear
c. Polar
d. Non-polar
13. The distribution of electric charges in water is
a. Symmetrical b.
Asymmetrical
c. Central
d. Peripheral
14. The dielectric constant of water is
a. 80
b. 60
c. 40
d. 20
15. The first law of thermodynamics states that
a. The total entropy of a system and its surroundings always
increases for a spontaneous process
b. Energy can be created
c. The total energy of a system and its surroundings is
constant
d. The total energy of a system and its surroundings is
never constant
16. The second law of thermodynamics states that
a. The total entropy of a system and its surroundings always
increases for
a spontaneous process
b. Energy can neither be created nor destroyed
c. The total energy of a system and its surroundings is constant
d. The total energy of a system and its surroundings is
never constant
17. The energy released during a process occurance is
a. Kinetic energy b. Solar
energy
c. Potential energy d. Bonding
energy
18. A disorder in any given system is defined by its
a. Entropy
b. Eutrophy
c. Enthalpy d.
Kinetic energy
19. The heat content in a system is defined by its
a. Entropy
b.
Eutrophy
c. Enthalpy
d. Kinetic energy
20. The tendency of non polar molecules to aggregate in
water is known as
a. Covalant bonding b. Van der
Waals interractions
c. Hydrogen bonding d. Hydrophobic
interactions
21. The property of biomoloecules having polar functional
groups and hydrophobicity is known as
a. Amphoteric b.
Steric
c. Amphipathic d.
Isochromatic
22. The interactions between oppositely charged groups
usually form
a. Salt bridges b. Covalant bonds
c. Hydrophobic interactions d. Precipitates
23. The process of bond cleaving in biomolecules by
nucleophilic activity of water is known as
a. Oxidation
b. Hydrolysis
c. Reduction
d. Catalysis
24. Acids are
a. Proton acceptors b. Electron
acceptors
c. Proton donors d.
Electron donors
25. Bases are
a. Proton acceptors b. Electron acceptors
c. Proton donors d.
Electron donors
26. High pH dissociates
a. Weak bases b.
Strong bases
c. Strong acids d. Weak
acids
27. Low pH dissociates
a. Weak bases b.
Strong bases
c. Strong acids d. Weak
acids
28. The negative log of acid dissociation constant is
denoted by
a. pH
b. pKa
c. K
d. Dl
29. The negative log of [H+] is denoted by
a. pH
b. pKa
c. K
d. Dl
30. The life forms that obtain energy from inorganic
compounds are
a. Organotrophs b.
Anaerobes
c. Aerobes d. Lithotrophs
31. The life forms that obtain energy from organic
compounds are
a. Organotrophs b.
Anaerobes
c. Aerobes d.
Lithotrophs
32. The term ‘Metabolome’ refers to the
a. Total genetic content b. Total protein content
c. Total small molecule content d. Total enzyme content
33. The mass of a molecule is denoted by
a. pH
b. Da
c. mm
d. Pka
34. Carbon containing molecules with different
configuration, but similar chemical bonds are
a. Isomeres b.
Aptameres
c. Oligomeres d.
Stereoisomers
35. Geometric isomeres are also known as
a. Chirals
b. Enantiomeres
c. cis-trans isomers d.
Diastereomeres
36. Chiral centers are
a. Enantiomeres b.
cis-isomeres
c. trans-isomeres d. Asymmetric
carbons
37. Mirror imaged sterioisomer pairs are known as
a. Enantiomeres
b.
cis-isomeres
c. trans-isomeres d. Chiral
centers
38. Non-mirror imaged sterioisomere pairs are known as
a. Enantiomeres b.
Diastereomers
c. trans-isomeres d. Chiral
centers
39. The spatial arrangement of groups in a molecule
denotes its
a. Configuration b.
Molecular mass
c. Molecular weight d. Conformation
40. Reactions that require energy are
a. Anergic
b. Endergonic
c. Exergonic d.
Entropic
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