Announcements 8/29
• Lab starts this week!– Proper Dress required– There are no assignments due this week at the
beginning of lab• Good idea to look over Ex. 1 and 2
• No labs Labor Day week due to short week (that is next week)
• All connect assignments are up for Module 1• Tegrity- explanation
The Chemistry of Life I
Chapter 2
Outline for Today
I. Matter and the Elements
II. Inorganic MatterA. Water
B. Minerals
C. Gases
III. Organic CompoundsA. Overview
B. Classes of Biomolecules1. Carbohydrates
2. Continued in The Chemistry of Life_2
I. Matter and the Elements
http://www.microwaves101.com/encyclopedia/periodicchart.cfm
CpRgDs
• Hopefully, you remember much of your basic chemistry from last year
• Electrons important in bonding– Covalent vs. ionic bonding– Hydrogen bonding (discuss shortly)
COMPOSITION OF LIVING MATTER
I. The Elements
>95%
electrolytes
Co-factors forEssential proteins
Essential elementof thyroid hormone
II. Inorganic Matter: Water
COMPOSITION OF LIVING MATTER
II. Inorganic Compounds
1. WATER
a. Properties that make it the IDEAL solvent for the human body
i. Solvency
ii. Polarity
iii. Adhesion/cohesion
iv. Neutral pH
v. Thermal properties
vi. Reactivity
Fig. 2.8
Solvency/Polarity
Fig. 2.9
δ means a small chargePolar – slightly charged at opposite ends
http://library.thinkquest.org/10429/low/matter/matter.htm
δ-
δ+δ+
http://www.emc.maricopa.edu/faculty/farabee/BIOBK/BioBookCHEM2.html
Solvency/Polarity
• Adhesion means to stick to other things while cohesion means to stick to itself
• Hydrogen bonds cause cohesiveness– Get a surface tension
• Forms a lubrication– What does this do?
• Cuts down on friction
Adhesion/Cohesion
Adhesion/Cohesion
Fig. 2.8
Notice the positive and negative interactions
H bonds are due to H bonding with F, O, or N (F not seen in biological systems)
• Acids or bases affect protein structure– Can render the protein non-functional
Neutral pH
Fig. 2.12
• High Heat Capacity– Amount of energy it
takes to raise 1g of water 1 oC.
– Takes a lot of energy to change the temperature of water
– Stabilization of body temperature
Thermal Stability
• High heat of vaporization– Liquid gas– Heat goes with it– Cools the body
– 1 ml of perspiration evaporating from the body removes 500 cals of heat
Thermal Stability
SWEATING is our main mechanism of heat release
Reactivity
• water is essential in many chemical reactions
universal solvent• water is added to break
covalent bonds
• is crucial in metabolism
• (will discuss more in organic cmpds)
Fig. 2.15
Anabolic reaction
Catabolic reaction
II. Inorganic Matter: Minerals
II. Inorganic Compounds
2. MINERALS
a. elements extracted from the soil; consumed in our diet
b. main minerals are calcium, phosphorus, potassium, sodium, chloride, magnesium, zinc, copper
c. are crucial for synthesis and maintenance of:
Bones
Muscles
Neurons
Calcium, phosphorus
Calcium, sodium, phosphorus
Calcium, sodium, potassium,phosphorus
II. Inorganic Matter: Gases
Gases: Important ones
• Oxygen (O2)– Cellular respiration
• Carbon Dioxide (CO2)– Waste product
• Nitrous Oxide– neurotransmitter
• Methane (CH4)
• Carbon monoxide (CO) is a problem
III. Organic Compounds
Fig. 2.14
• Valence of 4– Can form maximum of 4
bonds– Single, double, triple bonds
• Gives a lot of variety due to the functional groups– Clusters of atoms that
determine the chemical properties/reactivity
Fig. 2.23a
Overview - Carbon
http://www.elmhurst.edu/~chm/vchembook/202linear.html
Functional Groups in Organic Compounds
O-
COO-
PO4-
NH3+
Fig. 2.14
• Macromolecules are large molecules– Usually composed of repeating units
• monomers polymers ( a dimer in the above fig.)• Put together via dehydration synthesis (condensation
reaction)• Notice the loss of water from the molecule
Organic Compounds : Synthesis and Degradation Reactions
Fig. 2.15
• Polymer (dimer) smaller units (e.g. monomers)• Larger molecules broken apart via hydrolysis
reaction (“splitting with water”)• Water is used up in the reaction
Organic Compounds : Synthesis and Degradation Reactions
Fig. 2.15
• Notice that both involve water– Loss from or addition to the molecule(s)
• Both also involve enzymes (get to later with proteins)
Fig. 2.15
Organic Compounds : Synthesis and Degradation Reactions
You join 11 organic molecules together. How many water molecules are formed?
1. 9
2. 10
3. 11
4. 12
5. 13
6. No way to tell
III. Major classes of compounds
http://www.steve.gb.com/images/molecules/cofactors/NADH.jpg
• “Carbon Water” – C, H, and O
• Basic unit is the monosaccharide– Can have
disaccharides and polysaccharides
• Functions are energy and structure
Carbohydrates
• Simple sugars• Most important are 6
carbon hexoses and 5 carbon pentoses– Pentose examples are
ribose and deoxyribose
– Hexose examples are shown on the right
Fig. 2.16
Monosaccharides
Tab 2.6
• Two monosaccharides joined by a dehydration synthesis
• Degraded to monosaccharides for nutritional purposes
Fig. 2.17
Disaccharides
fructoseglucose
glucose
glucose glucose
galactose
Tab 2.6
• What is a polymer?– Link similar small molecules together– Polysaccharides can have a mw of 500,000 or more
while glucose is 180• Glycogen, starch, and cellulose are important
polysaccharides
Fig. 2.18
Polysaccharides
• Glycogen– Energy storing molecule– Only polysaccharide found in human tissues– Made by cells of liver, muscle, uterus, and vagina– Can be broken down to maintain blood glucose – Branching allows for more storage
Fig. 2.18
Polysaccharides
• Starch– Energy storing
molecule in plants– Plants rely on it when
photosynthesis is not occurring
Polysaccharides
• Cellulose– Structural molecule for plant support– Major component of wood– Most common organic compound on earth– Common component of our diets but we have no enzymes to
digest it• Roughage
http://www.steve.gb.com/images/molecules/sugars/cellulose.png
Polysaccharides
Tab 2.6
• Means the carbs are covalently bonded to proteins or lipids
• Glycolipids and glycoproteins – Many of the lipids and
proteins on the cell surface have up to 12 sugars attached
• Proteoglycans– Carb is the major portion
Conjugated Carbohydrates
Notice a pattern?
• Glucose• Fructose• Ribose• Sucrose• Maltose• Cellulose
• If a chemical ends in “ose” it is a carbohydrate
• Note: That does not mean that all carbohydrates end in “ose” (glycogen)