BIOL 1010
Biochemistry and Biophysics
Complete Study Guide
2026-2027 Academic Year
Molecular structure, energy, biomolecules, genetics, and the physical ideas that
explain life
Independent study resource
This guide is independently written for study and review. It is aligned broadly with the publicly described
themes of Yale BIOL 1010, but it is not an official Yale University publication and is not endorsed by Yale
University.
1
,How to Use This Guide
This guide is built for active study. Read a short section, close the page, and explain the idea in your own words.
Then use the practice questions to check whether you can apply the concept rather than simply recognize it.
• Learn the basic language first. Terms such as polarity, free energy, hydrogen bond, and allosteric regulation appear
repeatedly.
• Draw structures and pathways. In biochemistry, a quick sketch often reveals a relationship that is hard to see in
prose.
• Compare similar ideas. A large share of exam errors come from mixing up two concepts that are individually familiar.
• Use the final review after you have worked through the chapters. It is meant to compress the material into a
repeatable exam routine.
Contents
1. Chemistry of Life
2. Water, pH, and Buffering
3. Amino Acids and Proteins
4. Protein Structure and Function
5. Carbohydrates, Lipids, and Membranes
6. Nucleotides, DNA, and RNA
7. Thermodynamics and Free Energy
8. Enzymes and Catalysis
9. Binding, Regulation, and Cooperativity
10. Bioenergetics and ATP
11. Genome Organization and Information Flow
12. Molecular Techniques and Experimental Thinking
13. Human Genome and Medical Innovation
14. Final Review and Practice Exam
2
, Chapter 1 - Chemistry of Life
1.1 Matter at the Molecular Level
Biochemistry starts with matter: atoms, ions, and molecules. The elements most important in living systems include
carbon, hydrogen, oxygen, nitrogen, phosphorus, and sulfur. Carbon is especially useful because it forms four
covalent bonds and can make chains, rings, branches, and complex three-dimensional shapes.
1.2 Covalent and Noncovalent Forces
A covalent bond involves shared electrons. Polar covalent bonds share electrons unevenly, creating partial
charges. Ionic interactions involve attraction between charged groups. Hydrogen bonds are weaker than covalent
bonds but become powerful when many occur together. Van der Waals forces arise from temporary changes in
electron distribution. Hydrophobic effects are not a conventional bond; they reflect how nonpolar groups behave in
water.
1.3 Functional Groups
Functional groups give molecules recognizable chemical behavior. Hydroxyl groups often increase polarity.
Carboxyl groups can donate a proton. Amino groups can accept a proton. Phosphate groups are strongly polar and
often carry negative charge. Methyl groups are comparatively nonpolar and can alter shape and recognition without
adding much polarity.
1.4 Why Shape Matters
A molecule does not work because of its formula alone. Shape, charge, flexibility, and chemical environment
determine what it can bind and how it behaves. This idea connects almost every later topic in the course.
Practice Check
Which interaction is generally strongest?
• A. Hydrogen bond
• B. Covalent bond
• C. Van der Waals interaction
• D. Hydrophobic effect
Answer: B. Covalent bond
Why is carbon central to biochemistry?
• A. It always carries a positive charge
• B. It forms four covalent bonds and supports diverse structures
• C. It cannot bond to hydrogen
• D. It dissolves all lipids
Answer: B. It forms four covalent bonds and supports diverse structures
Chapter Checklist
• Explain why carbon supports molecular diversity
• Distinguish major covalent and noncovalent interactions
• Recognize common functional groups
3
Biochemistry and Biophysics
Complete Study Guide
2026-2027 Academic Year
Molecular structure, energy, biomolecules, genetics, and the physical ideas that
explain life
Independent study resource
This guide is independently written for study and review. It is aligned broadly with the publicly described
themes of Yale BIOL 1010, but it is not an official Yale University publication and is not endorsed by Yale
University.
1
,How to Use This Guide
This guide is built for active study. Read a short section, close the page, and explain the idea in your own words.
Then use the practice questions to check whether you can apply the concept rather than simply recognize it.
• Learn the basic language first. Terms such as polarity, free energy, hydrogen bond, and allosteric regulation appear
repeatedly.
• Draw structures and pathways. In biochemistry, a quick sketch often reveals a relationship that is hard to see in
prose.
• Compare similar ideas. A large share of exam errors come from mixing up two concepts that are individually familiar.
• Use the final review after you have worked through the chapters. It is meant to compress the material into a
repeatable exam routine.
Contents
1. Chemistry of Life
2. Water, pH, and Buffering
3. Amino Acids and Proteins
4. Protein Structure and Function
5. Carbohydrates, Lipids, and Membranes
6. Nucleotides, DNA, and RNA
7. Thermodynamics and Free Energy
8. Enzymes and Catalysis
9. Binding, Regulation, and Cooperativity
10. Bioenergetics and ATP
11. Genome Organization and Information Flow
12. Molecular Techniques and Experimental Thinking
13. Human Genome and Medical Innovation
14. Final Review and Practice Exam
2
, Chapter 1 - Chemistry of Life
1.1 Matter at the Molecular Level
Biochemistry starts with matter: atoms, ions, and molecules. The elements most important in living systems include
carbon, hydrogen, oxygen, nitrogen, phosphorus, and sulfur. Carbon is especially useful because it forms four
covalent bonds and can make chains, rings, branches, and complex three-dimensional shapes.
1.2 Covalent and Noncovalent Forces
A covalent bond involves shared electrons. Polar covalent bonds share electrons unevenly, creating partial
charges. Ionic interactions involve attraction between charged groups. Hydrogen bonds are weaker than covalent
bonds but become powerful when many occur together. Van der Waals forces arise from temporary changes in
electron distribution. Hydrophobic effects are not a conventional bond; they reflect how nonpolar groups behave in
water.
1.3 Functional Groups
Functional groups give molecules recognizable chemical behavior. Hydroxyl groups often increase polarity.
Carboxyl groups can donate a proton. Amino groups can accept a proton. Phosphate groups are strongly polar and
often carry negative charge. Methyl groups are comparatively nonpolar and can alter shape and recognition without
adding much polarity.
1.4 Why Shape Matters
A molecule does not work because of its formula alone. Shape, charge, flexibility, and chemical environment
determine what it can bind and how it behaves. This idea connects almost every later topic in the course.
Practice Check
Which interaction is generally strongest?
• A. Hydrogen bond
• B. Covalent bond
• C. Van der Waals interaction
• D. Hydrophobic effect
Answer: B. Covalent bond
Why is carbon central to biochemistry?
• A. It always carries a positive charge
• B. It forms four covalent bonds and supports diverse structures
• C. It cannot bond to hydrogen
• D. It dissolves all lipids
Answer: B. It forms four covalent bonds and supports diverse structures
Chapter Checklist
• Explain why carbon supports molecular diversity
• Distinguish major covalent and noncovalent interactions
• Recognize common functional groups
3
