Upload
ccdscott
View
156
Download
3
Tags:
Embed Size (px)
Citation preview
CHAPTER 1
The Chemical Nature of Cells
the nature and importance of biomacromolecules in the chemistry of the cell:
– synthesis of biomacromolecules through the condensation reaction
– lipids and their sub-units; the role of lipids in the plasma membrane
– examples of polysaccharides and their glucose monomer
– structure and function of DNA and RNA, their monomers, and complementary base pairing
– the nature of the proteome; the functional diversity of proteins; the structure of proteins in terms of primary, secondary, tertiary and quaternary levels of organisation
Study Design
Internal Environment
• Inside a cell is a chemical world.
• Energy is constantly being used or produced in chemical reactions
• Molecules are constantly being created or broken down.
Biochemical Processes
Anabolic Reactions
• Building materials
• Requires energy
• Eg. Photosynthesis
Catabolic Reactions
• Breaking down materials
• Releases energy
• Eg. Cellular respiration
Metabolism
The sum total of all chemical reactions occurring in the body.
• Takes into account all catabolic and anabolic reactions
Chemicals in a Cell
Who are the key players in the chemistry of a cell ?
• Water
• Carbohydrates
• Proteins
• Lipids
• Nucleic Acids
Water H2O• Oxygen and Hydrogen joined by a strong
covalent bond
• Oxygen has a slightly
negative charge while
hydrogen has a slightly
positive charge. • Water molecules are
attracted to each other –
highly cohesive (Remember transpiration)
Definition
Hydrogen bond
A weak bond between two molecules or parts of the same molecule; the hydrogen atom is slightly positive and is attracted weakly towards an atom of N, O or F
Hydrogen Bonds
Water H2O
• Water molecules tend to stick together by H bonds
• Exists in 3 states
• Solid - as temperature drops, molecular movement drops. Below 4°C movement not sufficient to break H bonds, making a lattice structure which is less dense than water as molecules are further apart than when a liquid
• Liquid – H bonds between water molecules constantly breaking and reforming, but the time apart is so brief, it maintains it cohesive nature
• Gas – movement of molecules increases to a point that H bonds no longer hold them together
http://mrtremblaycambridge.weebly.com/p4-simple-kinetic-molecular-model-
of-matter.html
5/11/14
Water H2O - Universal Solvent
• Hydrophilic or Polar substances
• dissolve easily in water
• eg salt
• Hydrophobic or Non-Polar substances
• will not dissolve easily in water
• eg fats
Water H2O - Universal Solvent
Dissolving
• H2O + NaCl H2O + Na+ + Cl-
• Attraction between Na+ and oxygen and Cl- and hydrogen splits the NaCl molecule
pHA measure of hydrogen H+ ions in a solution.
Below 7 – increasing H+ ions
Above 7 – increasing OH- ions
pH 7 Equal H+ & OH- ions
Cells must regulate their pH
pH• pH of body fluids is kept relatively constant because H+ ions are
continually being used and produced in cells
• Cells contain buffer substances that combine with or release H+ ions in a cell to prevent severe shifts in pH of a cell or fluid
Some fluids – eg urine, blood – have a
range for their pH, as the kidneys assist in
maintaining the pH of the blood and body tissues by excreting more or less of
a particular ion
Terms
• Monomer – a molecule or compound that can join together to form a dimer(2), trimer(3) or polymer (many)
• Polymer – a large molecule made of manyrepeated units (monomers)
Monomer Polymer
Glucose Polysaccharide
Amino Acid Protein
Fatty Acid Lipids
Nucleotides Nucleic acids
Condensation Reaction
• the joining of monomers involves the release of water molecules
2 Hydrogen molecules and 1 Oxygen
molecule are released, joining together to
make H2O
• Occurs when a polymer is broken down and a water molecule is used
• The opposite of a condensation reaction.
Hydrolysis Reaction
Definition
Biomacromolecule
• A naturally occurring substance of large molecular weight
http://maxeybio.blogspot.com.au/2013/10/the-building-blocks-of-life.html 5/11/14
Carbohydrates
• Energy rich molecules
• Consist of C (5 or 6 C ring), H and O in a 1:2:1 ratio (C:H:O).
• The basic unit is a sugar molecule
• Can be simple or complex carbohydrates
http://jennifer.nutritiontransition.co.uk/carbohydrates.htm
5/11/14
• Monosaccharides• one subunit (saccharide)
• Examples
• Glucose C6H12O6
• Fructose C6H12O6
Simple Carbohydrates
Glucose and
Fructose are
structural
isomers
http://www.nutriology.com/carbfunctions.php 5/11/14
Simple Carbohydrates
Glucose C6H12O6 Galactose C6H12O6
Fructose C6H12O6
Simple CarbohydratesDisaccharides
• two subunits (saccharides)
• Examples
• Sucrose, Lactose, Maltose …… all C12H22O11
Glucose + Fructose Sucrose + water
C6H12O6 + C6H12O6 C12H22O11 + H2O
Condensation reaction –
water released
Simple Carbohydrates
• Lactose (C12H22O11)
Glucose + Galactose
• Maltose (C12H22O11)
Glucose + Glucose
• Cellobiose (C12H22O11)
Glucose + Glucose
Trivia
Glucose Glucosamine
Galactose Galactosamine
(Building block for
chitin)
(Building block
for cartilage)
Complex Carbohydrates
Polysaccharides
• Eg. Starch, cellulose, glycogen
• All made with glucose monomers (saccharides)
• Glycogen
• Used for energy in animals
• Stored in liver and muscles
• Starch
• Storage of excess glucose in plants
• Insoluble, no effect on diffusion
• Cellulose (C6H10O5) n• Structural polysaccharide in plants
Proteins
• All have C,H,O,N
• Some have S and P
• Makes up 18% of cell contents
• Monomer
• Amino acids (RCH(NH2)COOH)
• R group varies - different A/A
• 20 naturally occurring A/A
• We can make 11 A/A,
• Other 9 from our food
Amino Acids
http://en.wikipedia.org/wiki/Prot
ein_structure 5/11/14
Bonding together• peptide bond forms between the amino group of
one amino acid and the carboxyl group of another
• Water molecule is released – condensation reaction
• A number of amino acids joined together –polypeptide
• Polypeptide chains fold different ways depending on their function
http://www.ib.bioninja.com.au/higher-level/topic-
7-nucleic-acids-and/75-proteins.html 5/11/14
Proteins - Structure
Four steps to structure
Primary Structure
• Linear sequence of amino acids
Secondary Structure
• Folding of chain into
• Alpha Helix (coil)
• Beta Sheet (Pleated)
• Random coil (not alpha or beta)
• Held by hydrogen bonds
Secondary StructureSome examples:
• The major protein of wool is alpha-keratin, a spiral molecule. If the fibre is stretched and the H bonds are broken the fibre becomes extended. If the fibre is then ‘let go’, the H bonds reform and the fibre returns to its original length.
• The major protein of silk is fibroin that is fully extended and lacks the coiling found in the structure of wool. The silk molecules from a beta-pleated sheet. The polypeptide chains of silk are already extended and cannot be extended further.
• Any major protein or portion is called random coiling if it does not fit into alpha- or beta-coiling. The O2 binding protein of muscle, myoglobin, has random sharp turns in its coil. The place of the random coil is often the most active site of a molecule.
Alpha Helix
Beta pleated
Random Coil
http://en.wikipedia.org/wiki/Pancreatic_lip
ase 5/11/14
Proteins - Structure
Tertiary Structure
• Complex shape
• Irregular folding held in place by ionic or hydrogen bonds
• The 3-D shape of a protein is critical for its function – if changed, esp. at its active site, the protein can no longer function
Quaternary Structure
• Two or more tertiary structures join to form a protein
http://biology.tutorvista.com
/biomolecules/proteins.html
5/11/14
Proteins – Quaternary structure
Fibrous Proteins
• Stringy and physically tough
• Actin, Collagen, Elastin, Fibronectin, Keratin, Myosin, Tropomyosin, Tubulin,
Globular Proteins
• Generally spherical or globular
• most hormones, enzymes, antibodies
• Albumins, Alpha globulin, Beta globulin, Cadherin, Fibrin, Gamma globulin, Haemoglobin, Immunoglobins, Myoglobin, Selectin, Serum albumin, Thrombin
http://www.differencebetween.net/scienc
e/health/difference-between-globular-
protein-and-fibrous-proteins/ 5/11/14
Conjugated Proteins
These are proteins which are joined to other molecules
Examples
• Glycoproteins Protein + sugar
• Nucleoproteins protein + nucleic acid
• Haemoglobin Tertiary structure + heme group
http://www.rottentomatoes.com/q
uiz/higher-biology-quiz 5/11/14
Types of Proteins
• Structural – Collagen, Keratin
• Enzyme – Amylase, ATP synthase
• Contractile – Actin, Myosin
• Immunoglobulin – Antibodies
• Hormone – Insulin
• Receptor – Insulin receptors
• Transport - Haemoglobin
Activating Proteins
• Not all enzymes are made ready to work
• They must be activated. Why?
Example
• Pepsinogen Pepsin
• Pepsinogen is inactive
• Pepsinogen + HCl Pepsin
• Pepsin breaks down polypeptides
What is the Proteome ?
Proteome
• The complete array of proteins produced by a cell or organism in a particular environment
Proteomics
• The study of the proteome
http://pharmaceuticalintelligence.com/tag/clinical-omics/
5/11/14
Lipids
• These are : Fats, Oils, Waxes
• All contain Carbon, Hydrogen, Oxygen
• They have little H2O so they carry more energy per molecule than other compounds
• Animals store excess glucose as fat
Lipids - Fats
Insoluble in water (hydrophobic)
• Each molecule comprises
• Fatty acid(s) and
• Glycerol C3H5(OH)3
• Minimum of one fatty acid
and one glycerol (mono, di & tri)
Eg Triglycerides
- Solid Vs Liquid Fats
Triglyceride
Note the lack of oxygen in the triglyceride molecule
Saturated Vs Unsaturated Fats• Saturated Fats:
• All single bonds between C, so it is saturated with H.
• Can be packed close
together – solid at room
temperature.
• Unsaturated Fats:
• Not all C have a H attached due to double bond, so are unsaturated (more than one C double bond = polyunsaturated), creating kinks in the tail.
• Due to the kinks they are not so tightly packed –liquid at room temperature.
Lipids - Phospholipids
Phospholipid molecules have:
• Two fatty acids
• Glycerol molecule and
• Phosphate group
• Includes a variable
group which makes
each molecule different
- Phospholipids are
a major component
of cell membranes
Cholesterol
• A steroid / lipid molecule
• Maintains the fluidity of a membrane
Fats and Energy
• Fats are energy rich molecules
• Per gram, fats store twice the energy as polysaccharides
• Animals store energy as fat
• Plants store energy as polysaccharides
Why the difference?
Hint:
Nucleotides
There are two types
1. Deoxyribonucleic Acid – DNA
2. Ribonucleic Acid – RNA
DNA
• A molecule made of nucleotides
• Each nucleotide is made of three things
• Sugar
• Phosphate group
• Nitrogen base
These are the same
for all nucleotides
http://scienceaid.co.uk/biology/gene
tics/images/nucleotide.jpg
5/11/14
DNA
There are four different nitrogen bases which create four nucleotides
• Adenine
• Thymine
• Cytosine
• Guanine
DNA• Nucleotides are joined into chains
Complementary Bases
• Adenine bonds with Thymine
• Guanine bonds with Cytosine
• This creates a double stranded molecule
To summarise…
How much DNA ?
• The average length of a chromosome is around 5cm.
• That is about 2m of DNA per cell.
• How do you fit it all into such a small space?
Histone Proteins
The DNA strand is wrapped around special proteins called histones to makechromosomes
Why have DNA ?
• DNA controls the functioning of cells by controlling the proteins a cell makes.
• DNA carries the information required to create polypeptide chains.
• Sets of three nucleotides act as a code for one amino acids
http://www.chemicalconnection.org.uk/chemistry
/topics/view.php?topic=5&headingno=13 5/11/14
RNA – Ribonucleic Acid
Like DNA it:
• Is a polymer of nucleotides
• Has the nucleotides G, C, A ,U (Uracil)
Unlike DNA
• RNA is a single strand of nucleotides
• Ribose replaces deoxyribose as the sugar in the nucleotide
• Thymine is replaced with Uracil
• Uracil bonds with Adenine
RNA
Three main types of RNA
• Messenger RNA (mRNA)
• Carries genetic messages to the ribosome for protein synthesis
• Ribosomal RNA (rRNA)
• A structural unit of the ribosome
• Transfer RNA (tRNA)
• Carries amino acids to the ribosome for assembly into a polypeptide