1. Chapter 2
The Chemistry of Life

2. What We are Learning Today
Section 1: The Nature of Matter
Review atoms and element structure
Identify the different ways chemicals bond
Define Key Terms

3. Atoms
The smallest unit of matter that cannot be broken down by chemical means
Very small and always changing
3 particles make up an atom
Electrons (-)
Protons (+)
Neutrons (neutral)
Attract each other…
*Therefore atom itself has no charge (negative electron cancels out positive proton)

4. Atomic Structure
Electron Cloud made of electrons, which have (-) charge so Electron Cloud = (-)
Nucleus made up of protons and neutrons, protons have (+) charge and neutrons have neutral (no) charge so nucleus has a (+) charge

5. Elements An element is a pure substance made of only one kind of atom
Represented by chemical symbols (C, N, H)
Elements differ in the # of protons (C=6, O=8)
Equal to the atomic number
Number of protons usually = number neutrons
Are exceptions…

6. Differences in Elements
Atomic Number all atoms of a particular element have the same number of protons which is called the atomic number.
Ex: Helium = b/c it has 2 protons

7. Chemical Bonding 3 Types
Atoms can join together to form a stable substance
The force that joins atoms together is called a chemical bond
A compound is a mixture of the atoms of 2+ different elements joined together in a chemical bond
3 Types
Covalent
Hydrogen
Ionic

8. Covalent bond When 2+ atoms share electrons to form a molecule.
Arrangement of electrons determine how atoms bond together
Electron levels
Closest to nucleus = 2 electrons
Second level = 8 electrons…
Atom becomes stable when the outer electron level is full
If it is not full it will react with atoms that can provide the electrons needed.

9. Atomic # = number of protons = # electrons
Energy Levels
Carbon Energy Levels Carbon = 6 electrons
Atomic # = number of protons = # electrons 3 4 2 1 6 5

10. A Water Molecule has a POLAR Covalent Bond
Water is made of Hydrogen and Oxygen
Hydrogen =H
1 electron in its outer most level
Oxygen =O
6 electrons in its outer most level
They react to fill each ones outer most level 2 2 2 3 1 6 4 5

11. Hydrogen bonds
Electrons in a water molecule are shared by oxygen and hydrogen atoms
Electrons more strongly attracted to the oxygen nucleus than by the hydrogen’s
This unequal distribution of electrical charge are called polar molecules

12. Polar Molecule (Water)
Which pole attracts which pole?

13. Ionic Bonding Sometimes atoms or molecules gain or loose and electron
Electric charge b/c they contain an unequal number of electrons and protons

14. Gaining/Losing an Electron
Gaining Makes the atom more negative
Adds a (-) charge onto the atom… electrons are (-)
Losing Makes the atom more positive
Adds a (+) charge onto the atom… negative charges were lost

15. Ionic Bond Example Na LOST an e- so it became more positive
Cl GAINED an e- so it became more negative

16. Closure Carbon Do you remember anything about atoms?
Make an atom of carbon using playdough
Include the #
protons,
neutrons
and electrons!
Carbon 6

17. What did we learn today? Word Association
Come to the board and write down any word you remember from today’s lesson!

18. QUIZ
FRIDAY 
quiz on Chapter 2 section 1 & 2
Period 12 Quiz THURSDAY

19. Exit Ticket Draw a carbon atom (Atomic number = 6)
Label all the parts and correctly show the number of electrons in the right levels
Write 3 things you learned today

20. Begin 2.1 Section Review
Page 30
Questions 1-4
Finish for HW

21. Chapter 2 Section 2: Water & Solutions
Water in Living Things
Storage of heat
Cohesion/ adhesion
Aqueous Solutions
Polarity
Acids and Bases

22. Water and Solutions Notes
Chapter 2 Section 2
Water and Solutions
Notes

23. Water in Living Things 70% of your body is made of water
Water helps move nutrients into and out of your cells
Certain properties of water make it such an important substance for life
Storage of heat
Cohesion & Adhesion

24. Storage of Heat
Water heats more slowly and retains heat longer than many other substances
Many organisms release heat through water evaporation
Sweating
Helps maintain homeostasis

25. Cohesion & Adhesion Cohesion Adhesion
Attraction between substances of the same kind
Surface tension prevents water from breaking easily
The hydrogen bonds between water molecules cause the cohesion of liquid water
Adhesion
Attraction between substances of a different kind
Substances get wet
Capillary action water molecules move up through a narrow tube (stem of plant)
Because of these water can move up the stems of leaves

26. Aqueous Solutions Many substances dissolve in water
Solution: a mixture in which one or more substances are evenly distributed in another substance
Salt water
Gatorade
Because certain substances can dissolve in water they can more easily move throughout the body

27. Polarity Enables many substances to dissolve in water
When ionic compounds are dissolved in water,
ions become surrounded by polar water molecules
Ions and molecules become evenly distributed in the water
Non polar molecules do not dissolve in water well (oils)

28. Acids and Bases (H+) + (OH-)  WATER
Pure water always has a low concentration of hydrogen ions (H+) and hydroxide ions (OH-)
Compounds that form hydrogen ions when dissolved in water are acids
Compounds that reduce the concentration of hydrogen ions in water are called bases
lower the concentration of hydrogen ions because hydroxide ions react with hydrogen ions to form water
(H+) + (OH-)  WATER

29. pH Scale

30. SECTION REVIEW QUESTIONS
Chapter 2.2 Section Review Questions!

31. On your note sheets… Write at least 1 example of a Carbohydrate
Lipid (fats)
Protein
Nucleic acid
What do you think they all have in common?

32. Question #1 Which of the following is NOT an organic molecule?
Carbohydrate
Ice
Lipid
Nucleic Acid

33. Question #2 Write down 3 types of carbohydrates AND
give examples of each
(how many sugars in each)
Monosaccharide- 1 sugar
Disaccharide – 2 sugar
Polysaccharide- 3 sugar (starch, cellulose, glycogen)

34. Index Card #3 Are lipids polar or non polar?
Do they dissolve in water? no
Give 3 examples of Lipids
Steroids, fats, waxes

35. Card#4 What are the building blocks of proteins?
Amino Acids
Give 2 examples of proteins and where they are located in the body.
Keratin- hair
Hemoglobin- blood

36. Card 5 What is a fatty acid and which bio-molecule does it belong to?
it is a lipid attached to a glycerol backbone
It is a lipid

37. Card 6 Give 2 examples of carbohydrates produced by plants
starch, cellulose
Give 1 example of carbohydrates produced by animals.
glycogen

38. Card 7 What are three characteristics of saturated fats?
Solid at room temp
Made from animal fats
Straight chain

39. Card 8 What are 3 characteristics of unsaturated fats
liquids at room temperature
from plants
structure is kinked because of the
double carbon bond

40. Card 9
What are 2 examples of nucleic acids?
DNA and RNA

41. 10
What is the function of nucleic acids?

42. 11
What is the function of lipids?

43. 12
Which type of fat has a kink in the structure?

44. 13
All organic compounds contain what element?

55. 2.3 Chemistry of Cells Most matter in your body that isn’t water
IS an organic molecule
Organic = Carbon based
4 classes of organic molecules in your body (can’t function w/o them)
Carbohydrates
Lipids
Proteins
Nucleic Acids
Structure
Where its found
Examples
Function
Other

56. Carbohydrates Organic molecules made of carbon, hydrogen and oxygen
Structure
Where its found
Examples
Function
Other
Organic molecules made of carbon, hydrogen and oxygen
Major source of energy for the body
Found in most foods (fruits, veggies, grain) in the form of sugars
3 types of sugars
Monosaccharide (simple sugars; glucose & fructose)
Disaccharide (double sugars; sucrose)
Polysaccharide (3+monosaccharides; starch, glycogen)

57. Examples of Sugars (Carbs)
Polysaccharides storehouses for energy
starch, glycogen, cellulose
Starch – made by plants
Glycogen- made by animals
Both made from linked glucose molecules (pg 34)
Cellulose- made by plants (for structure)
Structure
Where its found
Examples
Function
Other

58. Lipids Non-polar molecules… soluble or non-soluble?
Fats, phospholipids, steroids and waxes
Steroids (cholesterol, estrogen, testosterone)
Important for structure and function of cell membranes
Found in animal cell membranes & pigments
Lipids store energy
Structure
Where its found
Examples
Function
Other

59. Write this in OTHER!
Structure
Where its found
Examples
Function
Other

60. Structure of Lipids
3 fatty acids bonded to a glycerol molecule backbone
Fatty acid is long chain of carbon atoms with hydrogen bonded to them
Strong bonds between carbon and hydrogen  can store lots of energy
Structure
Where its found
Examples
Function
Other

61. Saturated and Unsaturated
All carbons have single bonds to hydrogen
Most animal fats
Butter, lard, grease
Usually solids at room temperature
Unsaturated
Some carbons linked by a double covalent bond
Causes kinks in chain
Plant oils, olive oil, fish oils
Liquids at room temperature
Structure
Where its found
Examples
Function
Other

62. Unsaturated Fats

63. Vocabulary!
Complete Chapter 2.3 Vocabulary!
HW if not finished!

64. What did we talk about yesterday?
What is the name of compounds that contain carbon?
What are the 3 types of carbohydrate “sugars?”
What organism makes cellulose?
What organism makes glycogen?
Are lipids polar or non-polar?
What are some examples of lipids?
What is the difference between saturated and unsaturated fats?

65. Proteins Structure: Function:
Where its found
Examples
Function
Other
Structure:
Large molecules formed by linked smaller molecules called amino acids (AA)
Function:
AA are building blocks of proteins
Only 20 AA
Cause various shapes of proteins
Some proteins are enzymes (help chemical reactions)
Others used for structure
Skin, ligaments, bone (Collagen)
Hair & nails (keratin)
Blood (hemoglobin)

66. Nucleic Acids Where Found Structure Function: Examples:
All cells contain nucleic acids
Structure
Long chain of smaller molecules ( called nucleotides)
3 parts
Sugar
Base
Phosphate group (P& O)
Function:
Store genetic info
Examples:
2 types of nuclei acids
DNA- deoxyribonucleic acid
RNA- ribonucleic acid
Structure
Where its found
Examples
Function
Other

67. Chapter 2.4 Energy & Chemical Reactions
ability to move or change matter
Many forms
light, heat, chemical energy, mechanical energy, electrical energy
Can be stored or released
by chemical reactions (build/break bonds)
Metabolism all of the chemical reactions that occur within an organism

68. Enzymes and Activation Energy
amount of energy needed to start a reaction
Can take a long time for reaction to occur
Heat the substance? NO!
Add a catalyst!! YES
ENZYMES!
Lower the amount of energy needed to start the reaction without changing the original reactants

69. Enzymes Shape specific Enzyme holds the reactant
Fits like puzzle piece
Active site
Each enzyme has its own specific substrate (reactant)
pH, Temperature, environment can affect

71. Section Review Questions
2.4 pg42
#1-4 Write the Questions & Answer

72. Complete 2.3 Directed Reading Worksheet
Finish 2.4 Vocabulary Terms
Complete 2.4 Directed Reading Sheet