DS

Introduction to Biochemistry – Lecture Review

Matter: Elements and Compounds

  • Matter: Anything that occupies space and has mass.

    • Makes up the physical component of the universe.

    • Matter is composed of elements.

Elements and the Periodic Table

  • Elements: Cannot be broken down into other substances by chemical means.

  • Elements are organized into the Periodic Table

Elements: Atoms

  • Elements are made of atoms.

  • All atoms of a given element are identical.

  • Atoms are the smallest particle of an element which retain the chemical properties of that element.

  • The atoms of different elements have different properties.

Atoms & Bonding

  • Chemical Bond: An attraction between atoms that enables them to stay close together.

  • Types of Chemical Bonds:

    • Ionic Bonds: Sodium (Na) + Chlorine (Cl) = Sodium Chloride (NaCl)

    • Covalent Bonds: Water (H2O)

Atoms & Ionic Bonding

  • Ion: An atom that has acquired an electrical charge by either losing or gaining an electron.

  • By definition, an atom is neutral (number of protons = number of electrons), (p+ = e-).

Ionic Bonds

  • Ionic Bonds: The attraction between oppositely charged ions.

  • Electrons are transferred (not shared).

  • Ions: Atoms that are electrically charged as a result of gaining or losing electrons.

Covalent Bonds

  • Covalent Bonds: Two atoms share one or more pairs of outer shell electrons.

  • Molecule: Atoms held together by covalent bonds.

Electron Dot Formula = Lewis Dot Structure (Valence shell diagram)

  • Carbon (C) tends to share electrons to form covalent bonds.

  • Sodium (Na) and Chlorine (Cl) tend to lose or gain electrons, respectively, to form ionic bonds.

Covalent or Ionic Bonding Checkpoint

  • C-H bonds indicate covalent bonding.

  • H + Cl à H+ + Cl- indicates ionic bonding.

Checkpoint: Ions

  • When a neutral atom loses an electron, it becomes a positively charged ion.

  • Example: K + Cl à K+ + Cl-: Potassium loses its electron to chlorine to become a positively charged potassium ion.

Reaction Types

  • Endergonic: Energy in.

  • Exergonic: Energy out.

  • Reduction: Gain of electrons.

  • Oxidation: Loss of electrons.

  • Anabolic: Build-up.

  • Catabolic: Break down.

Enzymes

  • Enzymes are proteins.

  • Function: To allow for chemical reactions to happen that would otherwise take too long (a catalyst).

  • Enzymes lower a reaction’s activation energy.

  • Example: Sucrase breaks down sucrose into glucose and fructose: Sucrose à glucose + fructose.

Enzymes & Chemical Reactions

  • Catalyst: A substance that lowers the activation energy, but is not used up itself.

  • Activation Energy: The amount of energy the reactants in the reaction must absorb to start the reaction.

Enzymes & Chemical Reactions: Types of Reactions

  • Catabolic reaction: Break down substances.

  • Anabolic reaction: Put two substances together.

Enzyme Examples

  • Luciferase: Breaks down luciferin molecules (catabolic enzyme).

  • Sucrase: Breaks down sucrose into glucose and fructose (catabolic enzyme).

  • Carboxypeptidases: Help put together molecules to create insulin, help in blood clotting, growth hormones, and others (anabolic enzyme).

How do Enzymes Work?

  • Active Site: The region of an enzyme where the substrate fits for the reaction to occur.

  • Substrate: The reactant specific to that enzyme.

  • Example: Enzyme for Cellular Respiration = Dehydrogenase.

Acids, Bases and pH

  • Acid: A chemical that donates H^+ (hydrogen ions) to solutions.

  • Base: A chemical that donates OH^- (hydroxyl ions) to solutions.

Checkpoint: pH

  • Which has a higher [H^+]? A solution with pH 5.

  • Which is more acidic? A solution with pH 5.

  • ↑ [H^+] ↓pH

  • ↑ acidic

Biological Molecules

  • Carbohydrates

  • Lipids

  • Proteins

  • Nucleic Acids

Building and Breaking Down Biomolecules Processes or Reaction

  • Dehydration synthesis: Links monomers together to form polymers.

  • Hydrolysis: Breakdown of polymers with water into monomers.

Carbohydrates

  • Function: Energy source.

  • Types:

    • Monosaccharides

    • Disaccharides

    • Polysaccharides

Carbohydrate Structure: Monosaccharides (a.k.a. simple sugars)

  • Monomers of other carbohydrates

  • Examples: glucose, fructose, galactose

Carbohydrate Structure: Monosaccharides

  • Glucose, fructose, and galactose have the same number of each type of atom, but arranged differently

  • Type # C; # H; # O

  • glucose 6; 12; 6

  • fructose 6; 12; 6

  • galactose 6; 12; 6

Carbohydrate Structure: Disaccharides

  • Constructed from two monosaccharides

  • Examples:

    • Maltose (Glucose + Glucose)

    • Lactose (Glucose + Galactose)

    • Sucrose (Glucose + Fructose)

  • Dehydration synthesis forms a disaccharide.

Carbohydrate Structure: Polysaccharides

  • Complex carbohydrates: Long chains of monosaccharides

Lipids

  • Function

    • Store energy

    • Insulation

    • Protect and cushion vital organs

    • Building blocks for cell membranes

    • Steroid function?

  • Types of Lipids

    • Fats

    • Phospholipids

    • Steroids

Lipids: Fats (a.k.a. Triglycerides)

  • Made up of 1 glycerol molecule and 3 fatty acid molecules.

  • Making fats: Dehydration synthesis

  • Saturated and Unsaturated fats

Lipids: Phospholipids

  • Made up of phosphate group and 2 fatty acid molecules

  • Found in cell membranes.

  • Hydrophilic = Water “loving”

  • Hydrophobic = water “fearing”

Lipids: Steroids

  • Structure: Skeleton is bent to form 4 fused rings

  • Examples of steroids:

    • Cholesterol LDL/HDL

    • Sex hormones

Lipids: Steroids (cont.)

  • Cholesterol – Important for cell membranes, hormones, etc.

    • LDL = low-density lipoprotein

      • Too much = build up on artery wall, can cause heart attack

    • HDL = high-density lipoprotein

      • Carries excess cholesterol away

Lipids: Steroids (cont.)

  • Sex hormones: Estrogen and Testosterone

Lipids: Steroids (cont.)

  • Steroids - Anabolic steroids: Made from testosterone

Proteins

  • Structure depends on Function

  • Function

    • Transport

    • Structural (collagen)

    • Storage

    • Contractile

    • Enzymes

    • Defensive

    • Signaling (hormones)

    • (Energy) only during starvation

Proteins (cont.)

  • Generally huge polymers

  • Constructed from amino acid monomers.

Proteins (cont.) Monomer Structure

  • Monomers = amino acids

  • All amino acids have a central carbon atom + a hydrogen atom

    • Amino group

    • Carboxyl group

    • Side group (a.k.a. “R” or functional group)

      • 20 different R groups

      • Hydrophobic or hydrophilic

      • Positively or negatively charged

Proteins (cont.)

  • Peptide Bond: The covalent bond between adjacent amino acids

  • Polypeptide: A chain formed by 3 or more amino acids

Protein Structure

  • Primary (1°): polypeptide (amino acid) chains in sequences unique to a given protein

  • Secondary (2°): coiling or folded sheets held together by hydrogen bonds between neighboring amino acids

  • Tertiary (3°): three-dimensional structure of coils or sheets, held together by amino acid side groups

  • Quaternary (4°): some proteins may be formed by including 2 -4 tertiary structures (subunits)

Checkpoint: Protein Monomers

  • What are the monomers of proteins?

    • Amino acids

Checkpoint: Protein Bonds

  • What type of bond holds the secondary structure of a protein together?

    • Hydrogen bonds

Checkpoint: Overall Shape

  • Which structural level ultimately dictates the overall shape of a protein?

    • Tertiary (3º)

Checkpoint: Protein Structure

  • What level of protein structure is exhibited in Green Fluorescent Protein (GFP)?

    • Tertiary (3º)

Checkpoint: Hemoglobin

  • What level of protein structure is exhibited in hemoglobin?

    • Quaternary (4º)

Nucleic Acids

  • Two types of nucleic acids

    • DNA(Deoxyribonucleic acid)

    • RNA (Ribonucleic acid)

  • Function: Information storage molecules that provide the information for building proteins

Nucleic Acids (cont.)

  • Structure: Monomer = nucleotide

  • Nucleotide consists of 3 parts:

    • 5 Carbon Sugar

    • Phosphate group

    • Nitrogenous base (varies)

Nucleic Acids (cont.)

  • Each DNA nucleotide has 1 of the following Nitrogenous bases:

    • Adenine (A)

    • Guanine (G)

    • Cytosine (C)

    • Thymine (T)

  • RNA has Uracil (U), instead of Thymine (T)

Nucleic Acids (cont.)

  • A single DNA strand -- polymer of nucleotides linked to a sugar-phosphate backbone

  • DNA – 2 strands held together by H-bonds between N-bases

DNA vs. RNA

  • Similarities : Both have nucleotides made of phosphate, sugar, nitrogenous bases

  • Differences:

    • DNA

      • Double-stranded

      • Nitrogenous bases include: A, G, C, (T) Thymine

      • Sugar = deoxyribose

    • RNA

      • Single-stranded

      • Nitrogenous bases include: A, G, C, (U) Uracil

      • Sugar = ribose

Checkpoint: DNA Bonds

  • What type of bond links nucleotides along the sugar-phosphate backbone of DNA?

    • Covalent bonds

Checkpoint: DNA Bonds

  • What type of bond links nucleotides between the nitrogenous bases of the double strand of DNA?

    • Hydrogen bonds

Checkpoint: DNA Structure

  • What type of bond links nucleotides along the sugar-phosphate backbone of DNA?

    • Covalent bonds