1. Chemistry of life
Chapter 2

2. Lesson 1
Basic Chemistry

3. DO NOW
Define, in your own words:
Atom
Element
Proton
Neutron
Electron

4. Elements and Atoms
All matter is made up of substances called elements.
Only 92 naturally occurring elements
Body is composed of only a few elements
Carbon
Nitrogen
Oxygen
Hydrogen
Phosphorous
Calcium
Atoms – smallest unit of an element
Made up of:
Protons – + charge, nucleus of atom
Neutrons – 0 charge, nucleus of atom
Electrons – ( - ) charge, orbit around nucleus

5. Isotopes
Same element differs in the number of neutrons in the nucleus and weight.
Carbon has 2 common isotopes
Carbon-13 and Carbon-14

6. Radioactive Isotopes
As isotopes break down they release energy in the form of rays and subatomic particles
Carbon-14 is a common Radioactive isotope
Unstable and breaks down over time

7. Molecules and Compounds
Molecule – 2 or more of the same atoms bonded together to form a chemical unit
Compound – 2 or more different atoms bonded together to form a chemical unit.
Types of Bonds:
Ionic – created by an electrical attraction
Covalent – sharing of electrons

8. Bonds

9. Bonds Chemical Bonds Double Bond – 2 pairs of electrons are shared
Triple Bond – 3 pairs of electrons are shared
Polar Covalent – electrons spend more time with the more electronegative element
Non-polar Covalent – equally shared electrons

10. In class assignment
Elements in Living Things Coloring Handout

11. Homework
Study Questions pg 39 # 1-4

12. Lesson 2
Water, Acids and Bases

13. Do Now
Have your homework from last night out on your desk for me to check!
What is the difference between ionic and covalent bonds?
What elements make up the human body?

14. Organic vs Inorganic Organic Molecules – contain carbon
Carbohydrates, proteins, lipids
Inorganic Molecules – do not contain carbon
Most important molecule is WATER

15. Water
Polarity and Hydrogen bonding gives water all of it’s unique and beneficial properties.
Solvent for polar molecules
Cohesive – water molecules stick together
Adhesive – water molecules stick to other surfaces
High Specific Heat Capacity/Heat of vaporization
Video

16. Acids and Bases Acids – substance that separates in water
Bases – takes up hydrogen ions or releases hydroxide ions
pH scale – ranges from 0-14, indicates the acidity and basicity of solutions
pH scale
Acids and bases

17. Acids and Bases
It’s important to maintain body fluid in a narrow pH range. (about 7.4)
Acidosis – pH value drops below 7.35
Occurs when kidneys and lungs can’t keep your pH balanced
Alkalosis – pH value rises above 7.45
Occurs when there is high levels of bicarbonate in your blood
Excessive loss of acid
Low carbon dioxide level
Buffers – help to keep pH in a normal range
they are chemicals or pairs of chemicals that take up excess hydrogen ions or hydroxide ions

18. Content Check
Depending on what you’ve eaten recently, the pH of your urine can vary from 5 to 8.
Which is more acidic – urine at pH 5 of pH 8

19. Electrolytes A substance that releases ions when put into water
These ions can conduct an electrical current
Electrolyte balance is important for good health because it effects the functioning of vital organs.

20. Homework
Study Guide Questions pg 39 # 6-7

21. Lesson 3
Molecules of Life

22. Do Now Macromolecules Handout Hand in Properties of Water Lab

23. Molecules of Life

24. Molecules of Life ^ Dehydration Synthesis
remove water, make bigger molecules
< Hydrolysis – add water, break down molecules

25. Carbohydrates quick, short-term cellular energy
Monosaccharide – one carbon ring. Ex: Glucose, Fructose
Dissaccharide – two carbon rings. Ex: sucrose
Polysaccharide – three or more carbon rings. Ex: starch, cellulose

26. Do Now September 30, 2014 Hand in your homework!
Take out your notes & be ready to work!

27. Carbohydrates Made up of C, H, O in a 1:2:1 ratio
Glucose – used as an immediate source of energy
Maltose is 2 glucose molecules, found in alcoholic beverages
Sucrose – glucose & fructose together, this is table sugar
Lactose – glucose and galactose, this is found in milk

28. Polysaccharides Means many sugars, LONG chains of sugar molecules
Starch – energy storage in plants
Glycogen – energy storage in animals
Cellulose – what cell walls are made up of
We cannot digest this, this helps to scrape the walls of our intestines

29. Common Polysaccharides

30. Lipids long-term energy storage, part of membranes
Saturated Fats - have only single covalent bonds, solid at room temperature. Ex: Butter (usually of animal origin)
Unsaturated Fats – have double/triple bonds, liquid at room temperature. Ex: Oils (usually of plant origin)

31. Lipids
Made of a glycerol molecule and a triglyceride, or three fatty acids.
Can be emulsified – mixed with water, molecules position themselves around a droplet so that their nonpolar ends stick out and the droplet disperse in water
Phospholipids – contain phosphate group, important for cell membranes
Steroids – different structure than fats, back bone of 4 carbon rings, with differing side chains
cholesterol is an example of a steroid

32. Proteins wide range of functions
Macromolecules made up of 20 different Amino Acids
Amino acids are arranged as follows
Central carbon atom
An amino group
An R Group

33. Structure of Proteins Composed of amino acids Primary Structure
When two amino acids join, called a dipeptide
Polypeptide contains 3 or more amino acids
Primary Structure
Sequence of Amino acids in a polypeptide
Secondary Structure
Coiling or folding of the protein
Tertiary Structure
Hydrogen, ionic, covalent bonding all occur in polypeptides
Quaternary Structure
Protein that has more than 1 polypeptide, arrangement of individual polypeptides
When proteins are exposed to extreme heat and pH they denature, and this is irreversible

34. Protein Structure

35. Content Check
The sequence of amino acids found in a protein is that protein’s __________ structure
a. primary b. secondary
c. tertiary d. quaternary
Why is it possible for humans to digest starch but not cellulose?
a. starch is made of glucose molecules but cellulose isn’t
b. Starch comes from plants but cellulose doesn’t
c. The glucose units found in cellulose are linked differently than those in starch

36. Enzymes Protein catalysts
Enable particular metabolic reaction to occur at the body’s normal temperature
Energy activation – energy needed to start a reaction
Substrates – reactants in an enzymatic reaction
Enzymes are very specific this is caused by the shape and chemical composition of it’s active site.

37. Enzyme Substrate Complex

38. Nucleic Acids contain hereditary information
Two Classes:
RNA – ribonucleic acid, bases are AUGC (codes for proteins)
DNA – deoxyribonucleic acid, bases are ATGC (makes up genes)

39. Nucleic Acids

40. DNA v RNA

41. ATP Adenosine plus 3 phosphate groups PRIMARY ENERGY CARRIER IN CELLS
Cells require a constant supply  continually break down glucose
Some uses:
Synthesizing macromolecules
Muscle contraction
Conduction of nerve signals

42. In Class Assignment/Homework
Macromolecules Worksheet #2