1. SB1 Students will analyze the nature of the relationship between structures and functions in living cells b. Explain how enzymes function as catalysts c. Identify the function of the four major macromolecules
GPS

2. Chemistry In Biology

3. Atoms, Elements, and Compounds

4. Matter All living things are made of matter
Matter has mass and takes up space
Atoms are the building blocks of matter

5. What do we call different types of atoms?
Elements
A substance that can’t be broken down into simpler chemical substances

6. The Structure of the Atom
Nucleus
Protons and Neutrons
Electron Clouds
Electrons

7. The Nucleus The Atomic Number of an atom = the number of protons
In a neutral atom, also the number of electrons.
Why do electrons and protons equal each other in a neutral atom?
The Atomic Mass (Mass Number) =The number of protons + the number of neutrons

8. The Periodic Table Organizes all of the known elements Atomic Number
Oxygen 8
*Average Atomic Mass
15.999

9. The major element’s of living organisms
Page 146 in your book
C, H, O, N make up 90% of the human body.

10. How are atoms structured?
Nucleus = protons and neutrons.
electron cloud = electrons
The number of protons = the atomic number
The number or electrons = the atomic number. But only when?

11. Compounds vs. Molecules
Atoms can combine to form molecules
A molecule made of 2 or more atoms combined
Examples:
Oxygen gas = O2
Carbon dioxide = CO2
Glucose = C6H12O6
Elements can combine to form compounds
A compound made of 2 or more different elements combined
Examples:
Water = H2O
Methane = CH4
Sucrose = C12H22O11
Which of these examples is a molecule but not a compound? Why?

12. Chemical Reactions
The process by which atoms or groups of atoms in a substance are reorganized into different substances

13. Chemical Equations 6CO2 + 6 H2O  C6H12O6 + 6 O2 Reactants  Products
Carbon dioxide and water
yield glucose and oxygen
6CO2 + 6 H2O  C6H12O6 + 6 O2
Reactants
Products
Coeffecient
Subscript

14. 5.2 Reaction Types synthesis decomposition single displacement
double displacement

15. Synthesis
a reaction of at least two substances that forms a new, more complex compound
general formula: A + B  AB
2Na + Cl2  2NaCl

16. Decomposition
a reaction in which one compound breaks into at least two products
General formula: AB  A + B
2H2O  2H O2

17. Single displacement
a rxn in which atoms of one element take the place of another element in a compound
general formula: XA + B  BA + X
3 CuCl2 + 2Al  2AlCl Cu

18. Double displacement
a rxn in which the positive and negative parts of two compounds change partners.
General formula: AX + BY  AY + BX
Pb(NO3)2 + K2CrO4  PbCrO4 + 2KNO3

19. Energy of Reactions
Activation Energy – the minimum amount of energy needed to cause a reaction to happen
Chemical reaction can be
Endothermic – absorbs energy – feels cold
Exothermic – gives off energy – feels hot

20. Mixtures
Two or more substances that keep their individual characteristics and properties

21. Two types of Mixtures Homogeneous same through out
Also called a Solution =
Solute + Solvent
Examples =
tea, air, Kool-Aid
Heterogeneous
different through out
Examples =
tossed salad, dirty water, blood, milk

23. Acids, Bases, and pH
acid—a substance that donates hydrogen ions, H+, to form hydronium ions, H3O+, when dissolved in water.
-taste sour
-turn blue litmus paper red
-corrode metal
-conduct electricity when dissolved in water

24. indicator
a compound that can reversibly change color in a solution, depending on the concentration of H3O+ ions

25. Strong acids -fully ionize in water….form the maximum
amount of hydronium ions in water
-conduct electricity very well
Example: Sulfuric acid. Used in car batteries.

26. Weak acids do not conduct electricity as well as strong acids
do not ionize fully
Table 6-1 in book

27. Bases a substance that either contains hydroxide
ions, OH-, or reacts with water to form
hydroxide ions.
-bitter taste
-slippery
-conduct electricity
-turns red litmus paper blue
-very dangerous if not dilute

28. Strong Base
dissociates completely to form ions
Examples: KOH

29. Weak Base reacts with water to form hydroxide ions
does not completely dissociate
Table 6-2 in book

30. Measuring acids and bases
pH—a measure of the hydronium ion concentration in a solution
enzymes in your body work in a narrow pH range
an abnormal pH is a sign of health problems

31. pH Values range from 0-14 -neutral solutions are 7 -acids 0-7
-bases 7-14

32. The Building Blocks of Life
Macromolecules

33. The Four Macromolecules
Carbohydrates
Lipids
Nucleic Acids
Proteins

34. Carbohydrates Carbon, hydrogen, and oxygen
1:2:1 ratio of elements
Carbohydrates are sugars
Used for Energy
Cellulose – Plant walls
Chitin – Insect shells, fungus bodies
1. Monosaccharide – fructose & glucose
2. Disaccharide – two monosaccahrides bonded – sucrose
3. Polysaccharide – many monosaccahrides bonded – starch, glycogen, cellulose

35. Lipids Composed of Carbon and hydrogen Waxes, Fats and oils
Nonpolar - Insoluble in water
Used for energy storage, insulation, and protective coverings
Major component of membranes surrounding cells called a phospholipid
Steroids – cholesterol and hormones

36. Nucleic Acids
Complex macromolecule that stores cellular information in the form of a code.
Composed of carbon, nitrogen, oxygen, phosphorus, and hydrogen
Polymer made of smaller units called nucleotides
Nucleotides contain a nitrogen base, a sugar, and a phosphate group
2 types
DNA – Deoxyribonucleic Acid
RNA – Ribonucleic Acid

37. Proteins Essential to all life – the primary building block of life
Large complex polymer composed of carbon, hydrogen, oxygen, nitrogen, and usually sulfur
Amino Acids are the building blocks
20 common amino acids
2nd major component of cell membranes

38. Enzymes – Special Proteins
Chemical reactions require specific temperature and environmental requirements that are often not found in the human body
An enzyme enables molecules called substrates, to undergo a chemical change to form a new substance

39. Enzymes Features
Enzymes speed up chemical reactions but do not take place in the reaction and are not changed by the reaction.
Do not make a reaction occur that would not occur on its own
Enzymes are reusable
Enzymes are specific to their substrate

40. Energy of Reactions
Activation Energy – the minimum amount of energy needed to cause a reaction to happen
Enzymes lower the activation energy of many reactions that take place in the body

41. Types of Enzymes Amylase – Breaks down sugars
Catalase – breaks down hydrogen peroxide in the blood and in cells
DNA polymerase – helps to make copies of DNA
Lactase – Breaks down lactose (milk sugars) in the digestive tract

42. The Lock and Key Mechanism of Enzymes

43. Factors such as pH, temperature, and other substances affect enzyme activity

46. Carbohydrates What: Sugars Elements: C, H, O
3 classes: Monosaccharides
Ex.) Glucose, fructose
Disaccharides
Ex.) Sucrose
Polysaccharides
Ex.) Cellulose, starch
Function: Energy

47. Nucleic Acids What they do: Store and transmit genetic information.
Elements: C, N, O, P, H
Subunit: Nucleotide
Nitrogen base
Sugar
Phosphate group
Ex.) DNA & RNA

48. Lipids What: Waxes, Fats, Oils Elements: C, H
Function: Stores energy, protective layers, insulation
1st major component of cell membranes
Examples: Hormones, cholesterol.

49. Proteins Essential to all life. Made up of amino acids.
Elements: C, H, O, N and sometimes S
Function: Building block of life
2nd major component of cell membranes
Example: enzymes