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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

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Attendance really does count for borderline grades

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This signifies item important for test purposes

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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

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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)

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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

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-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

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Brain

Kidney

Liver

Heart

Lung

Stem cell can become any of 220 cell types

Stem cells - building blocks of all tissues

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-Acquisition and use of energy

-Reproduction

-Growth and development

-Ability to respond to stimuli

-Adapt to changing environment

-High degree of organization

-homeostasis

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Brain Neurons can be derived from human embryonic stem cells.

Embryonic Stem Cells are an example of growth and development

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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

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

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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.

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No

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

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Blue Print #1

Blue Print #2

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

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Nutrients same for all life

Human DNA

Human DNA make human products

Dog DNA make dog products

Dog DNA

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Nutrients or Raw Materials

Blueprint

Blueprint

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

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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

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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

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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

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Three states of matter (for water)

Gas (Fog)

Solid (Ice)

Liquid

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Chemical Elements are pure forms of matter

Examples include:

Elemental gold

Elemental bromine

Elemental mercury

Elemental silver

Elemental iron

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Periodic Table of Elements;

Includes all natural elements and experimentally made elements.

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Everything in nature is made of

the elements on the periodic table.

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The Periodic Table of

Chemical Elements

Hydrogen (H) is simplest element 23

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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)

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Electron shell (or energy level) has

only 1 electron (-)

Nucleus of Atom has only 1 proton (+)

+

Hydrogen Atom

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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

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

neutrons (+/-)

Helium Atom27

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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

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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

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From water and soil under houses

May cause up to 50% lung cancer if inhaled

Produces alpha radiation

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Radon radiation tracks in lung tissue

Cells hit by tracks can become cancer cells

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=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

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Atomic Weight vs. Atomic Number

Atomic Weight of an Atom = number of protons and neutrons

Atomic Number of an Atom = number of protons

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Hydrogen (Protium)

Atomic number = 1

Atomic weight = 1

Deuterium

Atomic number = 1

Atomic weight = 2

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Carbon Atom

Atomic number = 6 (protons)

Atomic weight = 12 (6 protons and 6 neutrons)

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Atomic number = ??

Atomic weight = ??

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

816

+

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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

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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

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Holds 8 electrons

Has 1 Has 2

Has 4 Has 8

Has 1 Has 8

Holds 2 electrons

Holds 8 electrons

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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.

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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

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Each H atom

shares an electron with the other H

Chemical bond

Covalent bond –sharing electrons

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Covalent bond – sharing electrons

Each H needs 2 electrons

O needs 8 electrons144

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Holds 2 electrons

Holds 8 electrons

Holds 8 electrons

Has 1 Has 2

Has 4 Has 8

Has 1 Has 8

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Polar molecule (+) and (-)

Non polar molecule (+) or (-)

(+)

(+)

(+)

(+)

(+)

(-)

(+)

(+)

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

Hydrogen bond

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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

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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

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Adhesion

Cohesion

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

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Adhesion – water sticking to other material

Cohesion – water sticking to itself

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Transpiration – evaporation of water through leaves

Water moves from roots to

leaves

xylem

adhesion

cohesion

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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

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Positively charged Na+is attracted to negatively

charged Cl-; when they

combine they form an ionic compound NaCl or table salt.

Table salt

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(-) end

(+) end

Water molecule

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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.

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

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

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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

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Why does ice float? Why is this important?

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

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

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

Hydrophilic and Hydrophobic compounds

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

Moderate temperature changes Extreme temperature changes

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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.

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Acids and Bases

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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

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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

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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

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pH 0

pH 1

pH 3

pH 4 pH 7

pH 10

pH 11pH 13

pH 5

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Stomach acid

Body Fluids

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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

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72Reproduced by permission of JLM Visuals

Dead trees caused by acid rain in Great Smokey Mountains

Below pH 5.6?

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7372

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Sulfuric acid Nitric Acid

Sulfur dioxide

Nitrogen dioxide

Acid Rain

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