welcome to bi 212, summer 2010. lecture 1 outline (ch. 3, 4, 5) i.chemical bonds and shape ii.water...
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Welcome to BI 212, Summer 2010
Lecture 1 Outline (Ch. 3, 4, 5)
I. Chemical Bonds and Shape
II. Water Molecules
III. Chemical Reactions
IV. Organic Chemistry – Carbon-based molecules
V. Macromolecules
A. Carbohydrates
B. Lipids (NOT TRUE POLYMERS)
C. Proteins
D. Nucleic Acids
VI. Lecture Concepts
Chemical properties – all about shape
• water • methane
• electronegativity: attraction of e- by atom
• non-polar = e- shared equally
• polar = e- unequal
• bonds can differ in polarity
Chemical Bonds - Covalent
• electronegativity so unequal, e- stripped
• Example: sodium chloride
Chemical Bonds - Ionic
• H atom (covalent bond), attracted to electronegative atom
• between like or unlike molecules
Chemical Bonds - Hydrogen
75% water
70-95% water
Water – chemical properties
• Cohesion – tendency of molecules to stick to each other
• Adhesion – “ ” to stick to surrounding
H2O Hg
Water – chemical properties
• Surface tension
• Capillary action
δ-
δ+δ+
- dissolve anything polar or ionic (salt, proteins)
Water – chemical properties
- poor solvent for non-polar substances (butter, cell membranes)
• hydrophilic – attracted to water
• hydrophobic – repelled by water
Water – chemical properties
• less dense when solid (ice)
• high specific heat - insulating
Water – chemical reactions
Other chemical reactions
CO2 + H2O + light C6H12O6 + O2
Carbon – history of organic compounds
• historically - compounds divided by burn/won’t burn
• early 18th century -
living – wood, fat, oil
non-living – water, rocks
living - organic
non-living - inorganic
• “vital force” – needed to make inorganic organic
Carbon – history of organic compounds
• Friedrich Wölher - 1820s
- heated ammonium cyanate
-made urea(organic compound in urine)
• 19th century - chemists – increasingly complex molecules
• Stanley Miller - 1953
- amino acids from inorganic gasses
Carbon isomers
• Isomers = same molecular formula, different shape
C4H10 C4H10
butane isobutane
• Organic compounds all contain carbon- vary atoms with which carbon bonds- vary shape/structure of molecules
Carbon isomers
Carbon – functional groups
1. Hydroxyl (-OH)
2. Carboxyl (-COOH)
4. Amino (-NH2)
5. Sulfhydryl (-SH)
-
-
3. Phosphate (-PO42-)
• functional groups – common atom combinations, reactions
6. Methyl (-CH3)
Self-Check
Which functional groups are present in the following molecule?
HO
C
O
C
C C
N
H
H
OHH
HH
Which are not present ?
1. Hydroxyl (-OH)
2. Carboxyl (-COOH)
4. Amino (-NH2)
5. Sulfhydryl (-SH)
-
-
3. Phosphate (-PO4
2-)6. Methyl (-CH3)
Macromolecules
Macromolecules = giant molecules
Four biological classes:
Synthesis –
Monomers (single units) joined into polymers (multi-unit)
1. Carbohydrates
2. Lipids
3. Proteins
4. Nucleic acids
Dehydration synthesis = remove H2O, new bond
Hydrolysis = add H2O, break bond
Macromolecules
Carbohydrates
1. Carbohydrates – sugars and sugar polymers
Carbohydrates1. Carbohydrates
• Monosaccharide – simplest sugar molecule
- multiple of CH2O
-hexose – 6 C
-Glucose
-pentose – 5
-Ribose
• In water, sugars = rings
• C @ each cornerglucose
Carbohydrates
• joined by dehydration synthesis
glycosidic bond
Carbohydrates
• Polysaccharide – 100s – 1000s of monosaccharides
Carbohydrates
Two purposes:
Storage:
- plants – starch
- animals – glycogen
Structure:
- plants – cellulose
- (animals – chitin)
Carbohydrates - storage
Animal storage - glycogen
Plant storage - starch
Carbohydrates - structure
α glucose β glucose
starch celluose
digestible (humans) indigestible (humans)
Carbohydrates
2. lipids – fats, phospholipids, steroids
• hydrophobic
• not made of monomers
i. fats – glycerol + fatty acid by dehydration – ester bond
fat molecule:
-one glycerol, 3 f.a. aka triglyceride
Lipids
• saturated fats – all C bonded to as many H as possible
• unsaturated fats – at least one C with fewer H
Lipids
ii. phospholipids – glycerol + 2 f.a. + phosphate + choline
• lipid bilayer
Lipids
iii. steroids (some) – C skeleton 4 fused rings
cholesterol
estradiol
testosterone
Lipids
cortisol
3. proteins – string of amino acids
• very diverse group of macromolecules
Proteins
1) Catalyze Chemical Reactions (e.g. amylase) 2) Structure
(e.g. keratin)
3) Energy Storage (e.g. albumin)
4) Transport (e.g. hemoglobin)
5) Hormones (e.g. insulin)
7) Movement (e.g. muscle fibers)
6) Poisons (e.g. venom)
• monomer – amino acid
• polymer – polypeptide
• joined by dehydration
• peptide bond
Proteins
Proteins – amino acids (a.a.)
Carboxyl (-COOH)Amino (-NH2)
amino terminus (N)
carboxy terminus (C)
Structure of an amino acid
Alpha C
Amino group
Carboxyl group
“R” group – changes
Proteins
Carboxyl (-COOH)
Amino (-NH2)?
Proteins – amino acids (a.a.)
20 different a.a.
• non-polar
• polar
• charged
“R” group different
Classes:
mature proteins - processed, folded
Proteins
ii. Secondary – coiled and folded (sheet or helix)
*determined by amino-carboxyl H-bonds
N
C
Proteins
Four levels of protein structure:
i. Primary – unique sequence of a.a.
*determined by peptide bonds
Four levels of protein structure:
iii. Tertiary – regions linked
*determined by R-group H-bonds
iv. Quaternary – >1 protein
*determined by protein-protein interaction
Proteins
sickle cell normal cell
Proteins
Alterations to protein structure:
• mutations – Ex. sickle cell anemia
• environment – pH, temp, chemicalsEx. hair perm
• denatured – unfolded proteins- Sometimes reversible, usually not
Biomolecules
Self-CheckSpecific Molecule
Which Biomolecule Group?
Building blocks/ Monomers?
Joining Bond?
Biological Function?
CELLULOSE
FAT
STARCH
STEROID -----
GLYCOGEN
PHOSPHO-LIPID
PROTEIN
DNA
RNA
Which term includes all others in the list?
a. Monosaccharide
b. Glycogen
c. Starch
d. Carbohydrate
e. Polysaccharide
Which of the following is NOT a protein?
a. Hemoglobin
b. Cholesterol
c. A keratin molecule
d. An enzyme
e. Insulin
Self-Check
Relationship of DNA to RNA, Proteins
DNA
RNA
Proteins
Relationship of DNA to RNA, Proteins
DNA – macromolecule; 4. Nucleic Acids
• Two types:
i. DNA – deoxyribonucleic acid
ii. RNA – ribonucleic acid
· RNA – copy of gene, directions for protein synthesis
· DNA – nucleus, contains genes
Nucleic acids
• Monomer – nucleotide • Polymer – nucleic acid
• Ends different,
5’ end –
PO42- on C#5
3’ end –
OH group on C#3
Nucleic acid - structure
a. pentose sugarb. nitrogenous base
c. phosphate group
Nucleic acids
OH
• Monomers - dehydration
• Bond formed – phosphodiester bond
Nucleic acid - formation
H
Nitrogenous bases:
- two types – pyrimidines & purines
- cytosine (C)
- thymine (T)
- uracil (U)
UU- adenine (A)
- guanine (G)
Pentose sugars:
- deoxyribose & ribose
DNA
RNA
(DNA) (RNA)
Nucleic acid - components
* *
*
*
*
*
*
*
* *
• “backbone” - PO4 and sugars
• nitrogenous bases - on sugar
• polymer = nucleic acid strand
DNA – two strands
RNA – one strand
Nucleic acid - comparisons
5’
3’5’
3’
• DNA - antiparallel
Nucleic acids
• double helix
• Hydrogen bonds
– base to paired base
• Covalent bonds
- sugars to phosphates
- bases to sugars
Self-Check
DNA RNA
• double stranded • single strand
• •
• •
• •
• •
• •
• •
# strands
Sugar name
Bases used
Function
Backbone
H-bonds?
Covalent bond locations?
Nucleic acid – Comparisons
Lecture 1 Concepts- Discuss properties of water and explain using its structure
- Define the term ‘organic’ according to biochemistry
- Name the six functional groups and draw each one
- Recognize and explain dehydration synthesis and hydrolysis
- Compare and contrast glycogen, starch, and cellulose
- Explain how fats/oils, phospholipids, & steroids are different
- List and recognize the four levels of protein structure – explain what determines each level
- Draw a generalized amino acid (example p.78) & explain how protein primary structure is determined
- Draw a generalized nucleotide – this makes up what molecule(s)?- Discuss how the two ends of a DNA strand are different and what is
meant by ‘antiparallel’
- List four types of macromolecules, including monomer, polymer, examples, bond type
- Write out a list of new terminology and provide descriptions