frank visco - biology

1

Frank Visco - BiologyEmail: OCCBiology@aol.com

(preferred over phone messages)

Phone: 714-432-0202 ext. 22740

Office hours: by appointment only

Web site: http://occonline.occ.cccd.edu/online/fvisco or through OCC web site – www.occ.cccd.edu

Includes all images used in lecture~ PowerPoint (PPT) Version ~ & pdf. Version (no movement)

Includes all reviews for exams

Copy this page

1

2

Attendance really does count for borderline grades

2

This signifies item important for test purposes

3

Instructor Frank Visco

N.S. 100 Fall 2008

    Tues. Thurs Tues Thurs Tues Thurs Tue Thurs Tues

LAST NAME FIRST NAME Oct. 7 Oct. 9 Oct. 14 Oct. 16 Oct. 21 Oct. 23 Oct. 28 Oct. 30 Nov. 4

Aceves Salvador                

Alonzo Sarah                

Anari Shiva                

Atkins Celeste                

Aytekin Selcuk                

Barnes Chase                  

Bell Tiffany                  

Benjamin Royale                  

Bowlin Bradley                  

Brittell Elizabeth                  

Burgos Gabriel                  

Chadwick Kaylee                  

Conroy Brian                  

Davis Julian                  

Dilly Matthew                  

2b

    Tues.

LAST NAME FIRST NAME Oct. 7

Aceves Salvador SA

Alonzo Sarah SA

Anari Shiva SA

Atkins Celeste  

Aytekin Selcuk SA

4

In this section (biology):Characteristics of Life Cell Theory

Chemistry of Life Midterm 3 (30 points; each question worth ¾ points)

Cell structure and function DNA structure and function

Viruses Biotechnology

Bioenergetics Midterm 4 (30 points; each question worth ¾ points)

Cell Division Gametogenesis Mendelian Genetics

Evolution Origin of Life Kingdoms of Life Ecological Concepts and concerns (tested on course Final)

Midterm 5 (30 points; each question worth ¾ points - including Final)

3

5

Life – A complex physical state and complex series of chemical reactions with these characteristics

-Acquisition and use of energy

-Reproduction

-Growth and development

-Response to stimuli

-Adapt to changing environment

-Highly organized

-homeostasis

6

-Acquisition and use of energy

-Reproduction

-Growth and development

-Ability to respond to stimuli

-Adapt to changing environment

-High degree of organization

-homeostasis

Morphogenesis of the caterpillar into a pupa and then into the butterfly is an example of growth and development.

-Acquisition and use of energy

-Reproduction

-Growth and development

-Ability to respond to stimuli

-Adapt to changing environment

-High degree of organization

-homeostasis

Caterpillar

Pupa

Butterfly

5

7

Brain

Kidney

Liver

Heart

Lung

Stem cell can become any of 220 cell types

Stem cells - building blocks of all tissues

8

8

-Acquisition and use of energy

-Reproduction

-Growth and development

-Ability to respond to stimuli

-Adapt to changing environment

-High degree of organization

-homeostasis

7

Brain Neurons can be derived from human embryonic stem cells.

Embryonic Stem Cells are an example of growth and development

9

Cell Theory - 4 components:

1. Cell is smallest unit of life

2. All cells derived from previously existing cells

3. All cells show basic similarities in their chemical make-up and metabolic

activities

4. An organism (like a rabbit) is sum of all of the individual cells composing

organism

8

109

1. Red Blood cells are an example of the smallest unit of life

11

2. All cells are derived from previously existing cells – that is cells do not arise spontaneously from non-cells, instead cells come only from other cells by cell division.

10

No

12

Experiments to create life (cells) from non-life have not been successful

11

13

Blue Print #1

Blue Print #2

3. All cells have same basic chemical structure and chemical reactions.

12

14

Nutrients same for all life

Human DNA

Human DNA make human products

Dog DNA make dog products

Dog DNA

13

15

Nutrients or Raw Materials

Blueprint

Blueprint

14

16

4. Activity of an organism (such as a human) is the sum of each cell’s individual activities

15

17

Brain activity

Cell structure and function

Cell movements

Heartbeat

Smell, taste

Sperm and egg

Why is chemistry so important to LIFE?

photosynthesisThe human body has thousands of

chemical reactions making thousands of chemical products

16

18

Some chemicals of LIFEOxygen carrying

Photosynthesis

Energy

water

neurotransmitters

Humans make about 35,000 different chemical products

Insects make about 10,000 chemical products

Bacteria make about 1000 chemical products

Viruses make about 10 chemical products

17

19

Matter and energy – compose everything in NATURE

Matter – anything that takes up space and has mass (weight)

Energy – capacity to bring about movement against an opposing force

18

20

Three states of matter (for water)

Gas (Fog)

Solid (Ice)

Liquid

19

21

Chemical Elements are pure forms of matter

Examples include:

Elemental gold

Elemental bromine

Elemental mercury

Elemental silver

Elemental iron

20

22

Periodic Table of Elements;

Includes all natural elements and experimentally made elements.

21

23

Everything in nature is made of

the elements on the periodic table.

22

24

The Periodic Table of

Chemical Elements

Hydrogen (H) is simplest element 23

25

Each element is composed of specific atoms:

Atoms are usually composed of 3 subcomponents:

Protons – positive (+) charge (red)

Electrons – negative (-) charge

Neutrons – no charge or neutral (+/-) charge (white)

24

26

Electron shell (or energy level) has

only 1 electron (-)

Nucleus of Atom has only 1 proton (+)

+

Hydrogen Atom

25

27

0.00000000005 meters = distance between the nucleus (+) and the electron orbital (-)

or

5/10,000,000,000 of a meter

or

5 ten billionths of a meter

26

28

Two electrons (-) are in an shell around the nucleus; nucleus has two protons (+) and two

neutrons (+/-)

Helium Atom27

29

28

30

Protium

There are three forms of Hydrogen.

- one proton, one electron

- one proton, one electron, one neutron

- one proton, one electron, two neutrons

Isotopes - alternate forms of same element; different numbers of neutrons.

Deuterium

Tritium

129

31

Radioactive isotope greater number of neutrons than protons

Radioactive Tritium is unstable and becomes more stable by giving off energy or radiation = radioactivity

Protium Deuterium Tritium

30

32

From water and soil under houses

May cause up to 50% lung cancer if inhaled

Produces alpha radiation

31

33

Radon radiation tracks in lung tissue

Cells hit by tracks can become cancer cells

132

34

=5 kilograms (11 pounds) of weapons grade

plutonium (or uranium)

Nuclear Weapons August 9, 1945 - Nagasaki

100,000 tons of chemical

explosive, such as dynamite

133

35

Atomic Weight vs. Atomic Number

Atomic Weight of an Atom = number of protons and neutrons

Atomic Number of an Atom = number of protons

34

36

Hydrogen (Protium)

Atomic number = 1

Atomic weight = 1

Deuterium

Atomic number = 1

Atomic weight = 2

35

37

Carbon Atom

Atomic number = 6 (protons)

Atomic weight = 12 (6 protons and 6 neutrons)

136

38

Atomic number = ??

Atomic weight = ??

Protons neutrons electrons (8) (8) (8)

816

+

37

39

A human body contains 6.27 x 1027 atoms, or

6,270,000,000,000,000,000,000,000,000 atoms

Hydrogen atoms = 4.22 x 1027

Oxygen atoms = 1.61 x 1027

Carbon atoms = 8.03 x 1026

38

40

See page 1-7B

Calculation of the total number of each atom found in the human body

Oxygen 1.61 x 1027 atoms

Gold 2 x 1019 atoms

39

41

Holds 8 electrons

Has 1 Has 2

Has 4 Has 8

Has 1 Has 8

Holds 2 electrons

Holds 8 electrons

40

42

Hydrogen has room for 2 electrons in the first shell, but only has 1 electron.

Carbon has 2 electrons in the first shell and only 4 electrons in the second shell,

but Carbon can hold 8 electrons in the second shell,

HC

so Carbon can pick up 4 more electrons in the second shell.

41

43

4 hydrogen (H) share their electrons with the 4 electrons in the outer shell of one Carbon (C)

H

H

H

H

C

Sharing of electrons is called a covalent bond

CH4 = molecule 42

44

Each H atom

shares an electron with the other H

Chemical bond

Covalent bond –sharing electrons

143

45

Covalent bond – sharing electrons

Each H needs 2 electrons

O needs 8 electrons144

46

Holds 2 electrons

Holds 8 electrons

Holds 8 electrons

Has 1 Has 2

Has 4 Has 8

Has 1 Has 8

45

47

Polar molecule (+) and (-)

Non polar molecule (+) or (-)

(+)

(+)

(+)

(+)

(+)

(-)

(+)

(+)

46

48

Hydrogen Bond = slight attraction of positive end of one water molecule to slight negative end of another water molecule.

Hydrogen bond

47

49

Hydrogen bonds at surface of water create “surface tension.”

Water strider (insect) can literally walk on water because the tension on the surface of water is firm

148

50

Molecules inside a water drop are attracted in all directions. Drops on the surface are attracted to the sides and inward.

Leaf Surface

Water drop

49

51

Adhesion

Cohesion

Surface Tension – bonds between molecules at the surface of a liquid are stronger than bonds within the liquid

50

52

Adhesion – water sticking to other material

Cohesion – water sticking to itself

151

53

Transpiration – evaporation of water through leaves

Water moves from roots to

leaves

xylem

adhesion

cohesion

52

54

11+

Na (sodium) has 11 (+) and 11 (-)

Cl (chlorine) has 17 (+) and 17 (-)

17+

Na+ (sodium ion) has 11 (+) and 10 (-)

Cl- (chloride ion) has 17 (+) and 18 (-)

Ion = has net (+) or (-) charge

53

55

Positively charged Na+is attracted to negatively

charged Cl-; when they

combine they form an ionic compound NaCl or table salt.

Table salt

54

56

(-) end

(+) end

Water molecule

55

57

Ions and water play an important role in the metabolism (chemical reactions) of plants and all other forms of life. Many ions enter through the roots.

156

58

Diagram from Biology by Solomon et al, 5th ed.

Ions attached to soil particles make their way into root cell.

57

59

Why is water so important to life?

1. It is the solvent in which all life’s molecules are dissolved

2. It is the medium in which all life’s processes occur

158

60

Why does ice float? Why is this important?

59

61

Ice floats because ice is less dense than is liquid water. 160

62

Hydrophilic (water loving) compounds attracted to water (sugar, salt)

Hydrophobic (water hating) compounds not attracted to water (oil, fat)

Hydrophilic and Hydrophobic compounds

61

63

Water has a high specific heat which allows it to buffer temperature extremes

Moderate temperature changes Extreme temperature changes

62

64

Specific Heat

Defined: The specific heat of a substance is defined as the amount of heat that must be absorbed or lost for 1 g of that substance to change its temperature by 1º C.

The specific heat of water is 1.00 cal/g/ºC. Specific heat for ethanol is 0.6 cal/g/ºC.

63

65

Acids and Bases

164

66

pH Scale

(measures amount of H+)

0 1 2 3 4 5 6 7 8 9 10 11 12 13 14

Acid increases Neutrality base increases

Acid Base

65

67

pH Scale

(measures amount of H+)

0 1 2 3 4 5 6 7 8 9 10 11 12 13 14

Increasing H+ (Hydrogen ion concentration) = increasing acid

66

68

What is an acid? pH?

Acid – gives up Hydrogen (H+) ions.

pH - scale used to measure H+ (acid).

pH scale = 0 – 14, lower numbers = more H+.

pH of 0 is considered most acidic

pH of 14 - least acidic

HCl (acid) + H2O H+ (acid) + Cl- + H2O

67

69

pH 0

pH 1

pH 3

pH 4 pH 7

pH 10

pH 11pH 13

pH 5

168

70

Stomach acid

Body Fluids

69

71

Buffer1000 H+ (acid) ions

100 H+ acid ions

900 H+ ions held by buffer

Hydrochloric acid

Buffer – solution that maintains pH

pH before acid = 7

pH after acid = 7

70

72Reproduced by permission of JLM Visuals

Dead trees caused by acid rain in Great Smokey Mountains

Below pH 5.6?

171

7372

74

173

75

Sulfuric acid Nitric Acid

Sulfur dioxide

Nitrogen dioxide

Acid Rain

74