Biochemistry 2nd Edition
ST
SOLUTIONS
UV
IA
MANUAL
_A
PP
Raymond S. Ochs
RO
Comprehensive Solutions Manual for Instructors
VE
and Students
© Raymond S. Ochs
D?
All rights reserved. Reproduction or distribution without permission is prohibited.
?
© DREAMSHUB
, Solutions Manual for Biochemistry (2nd Edition)
Raymond S. Ochs
ISBN: 9780367465537
ST
UNIT 1: CHEMICAL FOUNDATIONS OF BIOCHEMISTRY
2. Water
3. Lipids
4. Carbohydrates
UV
5. Amino Acids and Proteins
UNIT 2: ENZYMES, COENZYMES, AND BIOENERGETICS
6. Enzymes
7. Coenzymes
IA
8. Metabolism and Energy
UNIT 3: CENTRAL METABOLIC PATHWAYS
_A
9. Glycolysis
10. The Krebs Cycle
11. Oxidative Phosphorylation
12. Photosynthesis
PP
UNIT 4: INTEGRATED METABOLISM
13. Carbohydrate Pathways Related to Glycolysis
14. Lipid Metabolism
15. Nitrogen Metabolism
RO
UNIT 5: MOLECULAR BIOCHEMISTRY AND GENE EXPRESSION
16. Nucleic Acids
17. Protein Synthesis and Degradation
VE
D?
?
© DREAMSHUB
, Solutions Manual for Biochemistry, 2e by
Raymond S. Ochs (All Chapters)
End of chapter answers
Chapter 2
ST
1. a) The properties are similar because both gas and liquid are fluids.
b) All phase transitions of water are unusual. The liquid to gas because it occurs at a high
temperature, due to hydrogen bonding. The liquid-solid transition is unusual because the
maximal density of water occurs at 4oC, due to closer approach of water molecules in the liquid.
UV
c) Most of the unusual properties are due to the extensive hydrogen bonding possible
because of the OH bond and the geometry of the molecule, forming extensive three dimensional
lattices.
2. It is possible. Using the density (1 g/ml) and molecular weight (18 g/mol) of water, the
concentration is 1/18 mol/l or 55.5 M.
IA
3. Electronegativities are calculated from molecules in which the bonds occur. They are
different in different molecules due to other forces (through bond and through space electrical
effects), so the values are averaged. The scale for each atom is thus a relative one; the difference
_A
between atoms can be easily estimated by subtracting the electronegativity values of each. The
1-4 scale was arbitrarily chosen.
4. Sulfur is larger, the electrons more diffuse, and as a result is unable to form a hydrogen bond.
PP
5. They are in adjacent columns in the periodic table, so we can expect some properties to be
shared, but have distinct valences. The nitrogen atom has five electrons, 1s22p3. The p orbital
has 6 potential electrons; the 3 in nitrogen atom are thus half-filled. Once bound to other atoms,
the electrons are hybrids, such as the common hydride, NH3. The extra electron pair in this
molecule makes it a Lewis base (electron pair donor). However, N can occur in acids too, such
RO
as in nitric acid. As amines, the reason for the tendency to positive charge is that when amines
accept a proton (Bronstead base) they become positively charged.
The oxygen atom as six electrons, 1s22p4. It also hybridizes in forming compounds; in
this case many of its compounds become acids such as R-COOH. When this loses a proton, it
becomes negatively charged. However, the oxygen hydride analogous to NH3 – H2O – can be
considered both basic and acidic.
VE
6. CO2 has polar bonds, but is not a polar molecule because the polarity vectors cancel out. The
geometry of the molecule is linear.
7. NH4+ dissolves in water because it has a full charge, which attracts the partial negative
D?
charges of water even more powerfully than another polar molecule does.
1
?
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ST
SOLUTIONS
UV
IA
MANUAL
_A
PP
Raymond S. Ochs
RO
Comprehensive Solutions Manual for Instructors
VE
and Students
© Raymond S. Ochs
D?
All rights reserved. Reproduction or distribution without permission is prohibited.
?
© DREAMSHUB
, Solutions Manual for Biochemistry (2nd Edition)
Raymond S. Ochs
ISBN: 9780367465537
ST
UNIT 1: CHEMICAL FOUNDATIONS OF BIOCHEMISTRY
2. Water
3. Lipids
4. Carbohydrates
UV
5. Amino Acids and Proteins
UNIT 2: ENZYMES, COENZYMES, AND BIOENERGETICS
6. Enzymes
7. Coenzymes
IA
8. Metabolism and Energy
UNIT 3: CENTRAL METABOLIC PATHWAYS
_A
9. Glycolysis
10. The Krebs Cycle
11. Oxidative Phosphorylation
12. Photosynthesis
PP
UNIT 4: INTEGRATED METABOLISM
13. Carbohydrate Pathways Related to Glycolysis
14. Lipid Metabolism
15. Nitrogen Metabolism
RO
UNIT 5: MOLECULAR BIOCHEMISTRY AND GENE EXPRESSION
16. Nucleic Acids
17. Protein Synthesis and Degradation
VE
D?
?
© DREAMSHUB
, Solutions Manual for Biochemistry, 2e by
Raymond S. Ochs (All Chapters)
End of chapter answers
Chapter 2
ST
1. a) The properties are similar because both gas and liquid are fluids.
b) All phase transitions of water are unusual. The liquid to gas because it occurs at a high
temperature, due to hydrogen bonding. The liquid-solid transition is unusual because the
maximal density of water occurs at 4oC, due to closer approach of water molecules in the liquid.
UV
c) Most of the unusual properties are due to the extensive hydrogen bonding possible
because of the OH bond and the geometry of the molecule, forming extensive three dimensional
lattices.
2. It is possible. Using the density (1 g/ml) and molecular weight (18 g/mol) of water, the
concentration is 1/18 mol/l or 55.5 M.
IA
3. Electronegativities are calculated from molecules in which the bonds occur. They are
different in different molecules due to other forces (through bond and through space electrical
effects), so the values are averaged. The scale for each atom is thus a relative one; the difference
_A
between atoms can be easily estimated by subtracting the electronegativity values of each. The
1-4 scale was arbitrarily chosen.
4. Sulfur is larger, the electrons more diffuse, and as a result is unable to form a hydrogen bond.
PP
5. They are in adjacent columns in the periodic table, so we can expect some properties to be
shared, but have distinct valences. The nitrogen atom has five electrons, 1s22p3. The p orbital
has 6 potential electrons; the 3 in nitrogen atom are thus half-filled. Once bound to other atoms,
the electrons are hybrids, such as the common hydride, NH3. The extra electron pair in this
molecule makes it a Lewis base (electron pair donor). However, N can occur in acids too, such
RO
as in nitric acid. As amines, the reason for the tendency to positive charge is that when amines
accept a proton (Bronstead base) they become positively charged.
The oxygen atom as six electrons, 1s22p4. It also hybridizes in forming compounds; in
this case many of its compounds become acids such as R-COOH. When this loses a proton, it
becomes negatively charged. However, the oxygen hydride analogous to NH3 – H2O – can be
considered both basic and acidic.
VE
6. CO2 has polar bonds, but is not a polar molecule because the polarity vectors cancel out. The
geometry of the molecule is linear.
7. NH4+ dissolves in water because it has a full charge, which attracts the partial negative
D?
charges of water even more powerfully than another polar molecule does.
1
?
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Distribution of this document is illegal extra per year?
