MDC (Multi Disciplinary Course): Biophysics

Notes on Biophysics (MDC)

Macromolecules:

Biomacromolecules are large biological molecules that are essential for life. They are typically composed of smaller molecular subunits and play crucial roles in the structure and function of cells.

The four major types of biomacromolecules are:

1.Carbohydrates – Made up of monosaccharides (simple sugars), these molecules provide energy and structural support. Example: Starch, glycogen, and cellulose.

2.Proteins – Composed of amino acids, proteins serve various functions including enzymatic activity, structural support, and signaling. Example: Hemoglobin, enzymes, and collagen.

3.Nucleic Acids – Made up of nucleotides, these molecules store and transmit genetic information. Example: DNA and RNA.

4.Lipids – Although not always considered macromolecules due to their non-polymeric nature, lipids are crucial for cell membranes, energy storage, and signaling. Example: Fats, phospholipids, and steroids.

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Carbohydrates:

Carbohydrates are biological macromolecules made up of carbon (C), hydrogen (H), and oxygen (O), typically in a 1:2:1 ratio. They are one of the primary sources of energy for living organisms and also play structural and functional roles.

Types of Carbohydrates

Carbohydrates are classified into three main types based on their complexity:

Monosaccharides (Simple Sugars)

The basic building blocks of carbohydrates.

Examples:

Glucose (C₆H₁₂O₆) – Primary energy source.

Fructose – Found in fruits.

Galactose – Found in milk.

Disaccharides (Double Sugars)

Formed by the combination of two monosaccharides through a glycosidic bond.

Examples:

Sucrose (Glucose + Fructose) – Table sugar.

Lactose (Glucose + Galactose) – Milk sugar.

Maltose (Glucose + Glucose) – Found in germinating grains.

Polysaccharides (Complex Carbohydrates)

Long chains of monosaccharides used for energy storage or structural functions.

Examples:

Starch – Energy storage in plants.

Glycogen – Energy storage in animals (stored in liver and muscles).

Cellulose – Provides structural support in plant cell walls.

Chitin – Found in fungal cell walls and the exoskeleton of arthropods.

Functions of Carbohydrates

Energy Source: Glucose is the primary fuel for cellular respiration.

Energy Storage: Starch (plants) and glycogen (animals) store energy for later use.

Structural Role: Cellulose in plants and chitin in fungi and arthropods provide support.

Cell Communication: Some carbohydrates (glycoproteins, glycolipids) are involved in cell signaling and immune responses.

Configuration of Carbohydrates

Carbohydrates have specific structural configurations that determine their chemical properties and biological functions. These configurations are based on the arrangement of atoms and the orientation of functional groups in the molecule. The key aspects of carbohydrate configuration include isomerism, stereochemistry, and ring structures.

D annd L - Glucose:

In the open chain structure of glucose, when the -OH group at carbon number 5 or C5 (the chiral carbon with highest locant number) is towards right, that is refered to D-Glucose and when the same -OH group is towards left it is called L-glucose.

Note that the capital and small D and d or L and l represent different stereo isomers of glucose

The d and l isomers of glucose are simply the optical isomers which rotate the plane of polarised light in opposite direction.

Anomers in Carbohydrates

Anomers are a specific type of stereoisomer found in cyclic carbohydrates. They differ in the configuration of the anomeric carbon (C-1 for aldoses, C-2 for ketoses) when a sugar forms a ring structure.

Below are the different repersentations of alpha-D-Glucopyranose as suggested by different chemists:

By Yikrazuul - Own work, Public Domain, https://commons.wikimedia.org/w/index.php?curid=6689685

1.Tollen's representation; 2.Howorth Projection; 3.Chair conformation; 4.Absolute stereo

Mutarotation:

Mutarotation is the change in the optical rotation of a solution due to the interconversion between different anomers (α and β forms) of a sugar until equilibrium is reached. This phenomenon occurs in carbohydrates, especially in cyclic hemiacetals and hemiketals, such as glucose.

Example: Mutarotation of D-Glucose

Pure α-D-Glucose has an optical rotation of +112°. Pure β-D-Glucose has an optical rotation of +18.7°. When dissolved in water, the optical rotation changes until it stabilizes at +52.7°, representing the equilibrium mixture (about 36% α and 64% β).

Factors Affecting Mutarotation

1.Solvent: Water and polar solvents facilitate mutarotation.

2.pH: Acid or base catalysts speed up the interconversion.

3.Temperature: Higher temperatures increase the rate of mutarotation.

Importance of Mutarotation

1.Biological Systems: Enzymes recognize specific anomers, affecting digestion and metabolism.

2.Food Industry: Mutarotation influences sugar sweetness and crystallization.

3.Pharmaceuticals: Drug formulations involving sugars need to account for mutarotation effects.

Proteins: Definition & Structure

Proteins are biological macromolecules made up of long chains of amino acids linked by peptide bonds. They are essential for nearly all biological processes, playing structural, enzymatic, and regulatory roles in cells.

Chemical Structure of Amino Acids

Amino acids are the building blocks of proteins. They have a general structure consisting of a central α-carbon bonded to four groups:

1.Amino group (-NH₂) → Basic in nature

2.Carboxyl group (-COOH) → Acidic in nature

3.Hydrogen atom (H)

4.R-group (Side Chain) → Unique for each amino acid

General Structure:

H2N−CH(R)−COOH

The R-group determines the chemical properties and classification of the amino acid.

Classification of Amino Acids Based on R-Groups

1.Nonpolar (Hydrophobic) Amino Acids

Contain alkyl or aromatic R-groups

Examples: Glycine, Alanine, Valine, Leucine, Isoleucine, Phenylalanine

2.Polar (Uncharged) Amino Acids

Contain hydroxyl (-OH), amide (-CONH₂), or thiol (-SH) groups

Examples: Serine, Threonine, Tyrosine, Asparagine, Glutamine

3.Acidic (Negatively Charged) Amino Acids

Contain extra carboxyl (-COOH) group

Examples: Aspartic acid, Glutamic acid

4.Basic (Positively Charged) Amino Acids

Contain extra amino (-NH₂) group

Examples: Lysine, Arginine, Histidine

Zwitterion Form

Amino acids exist as zwitterions, meaning they have both a positive (-NH₃⁺) and negative (-COO⁻) charge.

Example: H3N⁺−CH(R)−COO⁻

 This property affects solubility and reactivity.

Ionization States of Amino Acids

The ionization state of an amino acid depends on the pH of the solution and its pKa values.

a) At Low pH (Acidic Environment)

• The carboxyl group remains protonated (-COOH).
• The amino group is protonated (-NH₃⁺).
• The overall charge is positive.

b) At Neutral pH (Zwitterion Form, pH ≈ 7)

• The carboxyl group loses a proton (-COO⁻).
• The amino group remains protonated (-NH₃⁺).
• The molecule has no net charge (Zwitterion: a species with both positive and negative charges).

c) At High pH (Basic Environment)

• The carboxyl group remains deprotonated (-COO⁻).
• The amino group loses a proton (-NH₂).
• The overall charge is negative.

3. Isoelectric Point (pI)

The isoelectric point (pI) is the pH at which the amino acid has no net charge (exists primarily in the zwitterionic form). It is calculated as:

$$\mathrm{<b>p</b>}\mathrm{<b>I</b>}<b>=</b>\frac{\mathrm{<b>p</b>}\mathrm{<b>K</b>}{\mathrm{<b>a</b>}}_{\mathrm{<b>1</b>}}<b>+</b>\mathrm{<b>p</b>}\mathrm{<b>K</b>}{\mathrm{<b>a</b>}}_{\mathrm{<b>2</b>}}}{\mathrm{<b>2<span\; style="font-size:\; 14pt;"></span></b>}}$$

• For non-polar and uncharged polar amino acids:
• 
  
• $$\mathrm{<b>p</b>}\mathrm{<b>I</b>}<b>=</b>\frac{\mathrm{<b>p</b>}\mathrm{<b>K</b>}{\mathrm{<b>a</b>}}_{\text{<b>COOH</b>}}<b>+</b>\mathrm{<b>p</b>}\mathrm{<b>K</b>}{\mathrm{<b>a</b>}}_{\text{<b>NH₃⁺</b>}}}{\mathrm{<b>2</b><span\; class="vlist-s"></span>}}$$
• For acidic amino acids (Aspartic acid, Glutamic acid):
• 
    $$pI = \frac{pKa_{\text{COOH}} + pKa_{\text{R-group}}}{2}$$
• ​
• For basic amino acids (Lysine, Arginine, Histidine):
• 
    $$pI = \frac{pKa_{\text{NH₃⁺}} + pKa_{\text{R-group}}}{2}$$​​

Polypeptide

A polypeptide is a long, continuous chain of amino acids linked together by peptide bonds. It serves as the building block of proteins, which perform various biological functions in cells.

Formation of Polypeptides

Peptide Bond Formation:

A peptide bond forms between the carboxyl (-COOH) group of one amino acid and the amino (-NH₂) group of another.

OpenStax College, CC BY 3.0 <https://creativecommons.org/licenses/by/3.0>, via Wikimedia Commons

This reaction is a condensation reaction (removes a molecule of water, H₂O).

The resulting structure consists of repeating amide (-CONH-) linkages.

Directionality:

N-Terminus (Amino End): The start of the polypeptide, containing a free amino (-NH₂) group.

I, Danielle dk, CC BY-SA 3.0 <http://creativecommons.org/licenses/by-sa/3.0/>, via Wikimedia Commons

C-Terminus (Carboxyl End): The end of the polypeptide, containing a free carboxyl (-COOH) group.

CNX OpenStax, CC BY 4.0 <https://creativecommons.org/licenses/by/4.0>, via Wikimedia Commons

Polypeptide vs. Protein

Polypeptide: A simple chain of amino acids, may not be functional.

Protein: A functional molecule that may consist of one or more polypeptide chains folded into a specific 3D structure.

Functions of Polypeptides

Enzymes (e.g., DNA polymerase)

Structural proteins (e.g., collagen, keratin)

Hormones (e.g., insulin)

Transport proteins (e.g., hemoglobin)

Structure of Proteins

Proteins are made from 20 different amino acids, each with a unique side chain (R-group) that determines its properties. The structure of a protein can be described in four levels starting from the complex protein molecule to the unfolding of polypeptide chains and then to the detachment of different amino acids:

1.Quaternary Structure – The arrangement of multiple polypeptide chains (subunits) in a functional protein (e.g., hemoglobin has four subunits).

2.Tertiary Structure – The overall 3D shape of a single polypeptide, stabilized by interactions like hydrogen bonds, ionic bonds, disulfide bridges, and hydrophobic interactions.

3.Secondary Structure – Local folding patterns such as:

α-Helix (coiled structure)

β-Sheet (pleated sheet structure) These are stabilized by hydrogen bonds.

4.Primary Structure – The linear sequence of amino acids in a polypeptide chain.

Functions of Proteins

Proteins serve diverse roles in biological systems:

1. As Structural Proteins – Provide support (e.g., collagen in connective tissue, keratin in hair and nails).

2. As Enzymes – Speed up chemical reactions (e.g., amylase, DNA polymerase).

3. As Transport Proteins – Carry molecules (e.g., hemoglobin transports oxygen, membrane transporters).

4. Hormonal Proteins – Regulate biological processes (e.g., insulin controls blood sugar).

5.Defensive Proteins – Protect against diseases (e.g., antibodies in the immune system).

6.Contractile Proteins – Enable movement (e.g., actin and myosin in muscles).

7.Storage Proteins – Store essential substances (e.g., ferritin stores iron).

Sources of Proteins

Animal Sources: Meat, fish, eggs, dairy.

Plant Sources: Beans, lentils, nuts, soy.

Nucleic acids

Nucleic acids are biomolecules essential for the storage, transmission, and expression of genetic information. They are composed of nucleotide monomers, which consist of a sugar, a phosphate group, and a nitrogenous base. The two main types of nucleic acids are:

Deoxyribonucleic Acid (DNA)

1. It Stores genetic information in cells and has a double-helix structure.

2. It is considered to be a polynucleotides. One nucleotide unit consists of a deoxyribose sugar, four nitrogenous bases [adenine (A), thymine (T), cytosine (C), and guanine (G)] and a phosphate group.

https://commons.wikimedia.org/wiki/File:Deoxyribose.png#filelinks

The nitrogenous bases are classified into two types. They are purine (bicyclic ring names as adenine and guanine) and pyrimidine (monocyclic rings named as cytosine, thymine, and uracil * Uracl present in RNA)

Blausen, CC BY-SA 4.0 <https://creativecommons.org/licenses/by-sa/4.0>, via Wikimedia Commons

A phosphate group is derived from phosphoric acid, with two of the hydrogen atoms from the phosphoric acid being replaced by bonds with the sugar molecules of the nucleotides.

Now that we have the idea of individual component of a DNA, lets discuss further. When a nitrogenous base combines with a ribose sugar it is called a nucleoside.

https://commons.wikimedia.org/wiki/File:DC_chemical_structure.png

When a phosphate unit is added with the Nucleoside it becomes the nucleotide. This nucleotide repeats itself to form a complete chain of a DNA molecule.

DrTOsborne, CC BY 4.0 <https://creativecommons.org/licenses/by/4.0>, via Wikimedia Commons

Now to chains (called strands) are spirally bound which is termed as alpha helix in which A pairs with T, and C pairs with G through hydrogen bonds (See Figure).

Ribonucleic Acid (RNA)

1. Involved in protein synthesis and gene expression and is usually single-stranded.

2. It is composed of nucleotides with ribose sugar and four nitrogenous bases [adenine (A), uracil (U), cytosine (C), and guanine (G)].

A pairs with U, and C pairs with G.

Types of RNA: messenger RNA (mRNA), transfer RNA (tRNA), and ribosomal RNA (rRNA).

Functions of Nucleic Acids:

DNA: Stores and transmits genetic instructions.

RNA: Helps in protein synthesis and gene regulation.

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