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Where does the energy we use come from?

• Electricity • Biomass Energy - energy from plants • Geothermal Energy • Fossil Fuels - Coal, Oil and Natural Gas • Hydro Power and Ocean Energy • Nuclear Energy • Solar Energy • Wind Energy • Transportation Energy

Source: U.S. Energy Information Administration, Office of Coal, Nuclear, Electric and Alternate Fuels 

Courtesy of World Resources Institute, 10 G Street, NE (Suite 800), Washington, DC 20002

Courtesy of Uranium Information Center Ltd Energy for the World - Why Uranium?

http://www.eia.doe.gov/oiaf/ieo/highlights.html

http://www.eia.doe.gov/oiaf/ieo/highlights.html

Courtesy of Economic Energy Report by Michael Hodges

PENNSYLVANIA FACTS

• Pennsylvania ranks second in the nation in nuclear power generating capacity– 5 operating power plants that provide 1/3 of the electricity needs of the

state• PA is a major coal producing state, selling ½ of its coal output to other

states• PA is the leading petroleum refining state in the Northeast• PA’s electricity production exceeds state demands• PA is among the largest users of municipal solid waste and landfill gas

for electricity generation• PA produces substantial hydroelectric power • In December 2004, PA adopted an alternative energy portfolio

standard that requires electricity companies and generators to supply 18.5% of PA’s electricity from alternative energy sources by 2020.

With your assigned group members discuss solutions to the following problem. Come to agreement as a group on a solution, and choose one member that will present your solution at the end of class.

Problem: What can be done to meet the United States’ ever-growing energy demands while

improving the quality of life of today’s society without sacrificing the quality of life of future

generations?

Law of Conservation

of EnergyEnergy cannot be created nor

destroyed!

Type of Energy Examples

Kinetic Sound, Wind, Spinning Wheel

Potential Ball held above ground, water before a dam

Radiant Light, Microwaves, X-rays, Gamma waves

Electrical Electricity, static cling, lightning

Magnetic Magnets, compasses

Mechanical Pistons in a car engine

Thermal Heat

Nuclear Nuclear fission, nuclear fusion, heavy water

Chemical Gasoline, oil, batteries, food

Spring Stretched rubber band, bungee cord, spring scale

Law of Conservation of EnergyEnergy cannot be created nor destroyed!

Any situation

where energy

is transferred

from one object

to another…

…or from one kind

of energy into another kind.

Webster's Dictionary definition of "rube goldberg”: Accomplishing by extremely complex, roundabout

means what seemingly could be done simply.

Draw your final sketch today. Label all 10 forms of energy associated with your machine.

Objective: Make a drawing of a Rube Goldberg device of your own creation which includes examples of each of the 10 basic types of energy and 10 different energy changes.  

10 energies - these should be clearly labeled and numbered in blue next to where the energy occurs in the drawing.

10 different energy changes - arrows should be drawn connecting each energy in the drawing to the next in red to show how one type of energy is changing into another.

Calorie

• Always refers to the energy in food

• A measure of how much potential energy that food possesses

• 1 Calorie = 1 kilocalorie = 1000 calories

• Body burns calories through metabolic processes• Enzymes break carbohydrates into glucose and

other sugars, fats into glycerol and fatty acids and proteins into amino acids

Caloric Breakdown

• 1 gram carbohydrates = 4 Calories

• 1 gram protein = 4 Calories

• 1 gram fat = 9 Calories

Underweight <5%, Healthy 5-85%, Risk of Overweight 85-95%, Overweight >95%

The Body’s Caloric Needs

• 2,000 Calories is an average body’s need

• Height, weight, gender, age and activity level all affect a person’s caloric needs

• To calculate your body’s needs add together– basal metabolic rate– physical activity– thermic effect of food

BMR--Basal Metabolic Rate• Accounts for about 60 to 70 percent of calories burned in a

day

• Includes the energy required to keep the heart beating, the lungs breathing, the kidneys functioning and the body temperature stabilized

Adult male: 66 + (6.3 x body weight in lbs.) + (12.9 x height in inches) - (6.8 x age in years)

Adult female: 655 + (4.3 x weight in lbs.) + (4.7 x height in inches) - (4.7 x age in years)

Ms. Wack’s BMR = 1366.4

Physical Activity

Sedentary Activities Energy Costs in Cals/Hour

Lying down or sleeping - 90Sitting quietly - 84Sitting and writing, card playing, etc. - 114

Moderate Activities (150-350 cal/hr)

Bicycling (5 mph) - 174 Light housework, cleaning, etc - 246

Bicycling (6 mph) - 240 Swimming (crawl, 20 yards/min) - 288Dancing (Ballroom) - 210 Gardening - 323

Golf (twosome, carrying clubs) - 324

Walking (2 mph) - 198 to 240 Walking (3 mph) - 320 Walking (4 1/2 mph) - 440

Thermic Effect of Food

• The amount of energy your body uses to digest the food you eat

• Multiply the number of calories you eat in a day by 10% (0.10)

Food Serving Size CaloriesAmerican Cheese 1 slice 70Apple 1 medium 80Apple Juice 8 fluid ounces 120Bacon 2 slices 80Bologna 1 ounce 90Caesar Salad 10 oz. w/ dressing 520Carrot, fresh 1 medium 35Cheesecake, Plain 1/4 of 19 oz cake 330Cola 8 oz 100French Fries 10 strips 160Frozen Waffles 2 waffles 220Hamburger 4 oz. Patty 445Hamburger roll 1 roll 130Macaroni and Cheese 7.5 ounces 260Milk 8 ounces 160 Pizza, Cheese 1 slice 290Potato Chips 1 ounce 150 Pretzels 1 ounce 110

Effects of Calorie Intake• An accumulation of 3500 extra Calories is stored by your

body as 1 pound of fat

• Lose 1 pound of fat when you burn 3500 more calories than you eat

• Burn what you eat to maintain your weight

• Body burns an increased # of calories for 2 hours after exercise

Use the handouts on your table to determine the # of calories you eat in an average day (estimate it). Then use the calculations from yesterday and the information below to determine whether you should be losing, gaining or maintaining weight. Write your answers on your handout from yesterday.

What happens when you don’t get the Calories you need?

• Body initially responds with weight loss by breaking down fat

• After a few weeks body senses starvation and your metabolism will decrease so less overall energy is needed– Body will look for other sources of fuel & will begin

breaking down muscle resulting in loss of lean muscle mass (if already underweight can result in loss of tissue surrounding internal organs, including the heart).

• Symptoms: Fatigue, diarrhea, inability to stay warm, irritability, weakened immune system,

calories

• A unit of energy

• The quantity of heat needed to raise the temperature of 1 g of pure water 1°C

Calorie

• Always refers to the energy in food

• A measure of how much potential energy that food possesses

• 1 Calorie = 1 kilocalorie = 1000 calories

• Body burns calories through metabolic processes• Enzymes break carbohydrates into glucose and

other sugars, fats into glycerol and fatty acids and proteins into amino acids

Joule

• The SI unit of energy

• the symbol for Joule is J

• 1 J = 0.2390 cal

• 4.184 J = 1 cal

Energy Conversions

1 Calorie = 1000 calories

4.184 J = 1 calorie

Temperature

• Measured with: Fahrenheit Scale: An arbitrary scale created by Gabriel Fahrenheit.

F = (C 9/5) + 32

Celsius Scale: Based on the freezing and boiling points of water.

C = (F – 32) 5/9

C = K – 273

Kelvin Scale: The S.I. Scale

•Based on absolute zero.

Absolute Zero: The point at which the motion of particles of matter (their kinetic energy) ceases.

K = C + 273

Properties & Changes of Matter

Anything that takes up space and has mass

Can be classified as solid, liquid, gas or plasma

Matter

Is it matter?

What is not matter?

ENERGY, HEAT, LIGHT, ELECTROMAGNETIC WAVES, MAGNETIC FIELDS, IDEAS, ETC.

Properties of MatterDescribe the characteristics and behavior

of matter, including the changes that matter undergoes

Observing Matter Macroscopic Observations: Observations made with the

5 senses

Microscopic Observations: Observations made with a microscope

Submicroscopic Observations: Observations of substances so small they cannot even be seen with a microscope

Macroscopic Microscopic Submicroscopic

Qualitative Observation: Describes the properties of a substance

Quantitative Observation: An observation that involves a numerical value.

Physical Properties

What are the physical properties represented in the image above?

chara

cteris

tic

s

quantitative

qualitative

Mass

Units: grams or kilogramsMeasured with: Triple Beam Balance

VOLUME

If the same amount of liquid is found in both of the above containers—which has more volume?

SI Unit: cm3 or m3

Measured with: a meterstick or a metric ruler

Common Unit: mL or L Measured with: a

graduated cylinder

States of Matter

• Depends on:

• Solid:

• Liquid:

• Gas:

PLASMA

Free electrons and ions of an element.

The most common form of matter

Energy is needed to strip atoms of their electrons.

Plasmas can be steered and controlled by magnetic and electric fields.

PLASMA TV’S•Xenon and Neon in each cell

•Intersecting electrodes charged causing electric current through the gas in that cell

•Electric current = rapidly flowing charged particles causing the release of UV photons

•Photons interact with the phosphor coating giving off colored light

Because each cell is lit individually, the image is bright and looks good from almost any angle.

Chemical Properties

Chemical Reaction: A Chemical Change

• After a chemical reaction: The original substance no longer has the same identity

• Chemical reactions can be used to:

Is it a chemical reaction?

Law of Conservation of Matter

•Matter cannot be created nor destroyed in a chemical reaction.

•Developed by: Antoine Lavoisier

•Mathematically:Mass of the reactants = Mass of the products

(starting materials) (ending materials)

PURE SUBSTANCEPURE SUBSTANCE Matter with the same fixed Matter with the same fixed

composition and propertiescomposition and properties– First Type of Pure SubstanceFirst Type of Pure Substance

ElementElement– The Periodic Table:The Periodic Table: A chart that lists the chemical A chart that lists the chemical

name and chemical symbol for each elementname and chemical symbol for each element– Chemical Symbol:Chemical Symbol: A shorthand abbreviation for A shorthand abbreviation for

the name of an elementthe name of an element– You can tell a substance is an element because it You can tell a substance is an element because it

is on the periodic tableis on the periodic table

-Can you separate an element? No-Can you separate an element? No

Aluminum = ___ Aluminum = ___ Gold = ____ Gold = ____ Tin = ____ Tin = ____

PURE SUBSTANCEPURE SUBSTANCE Matter with the same fixed composition and propertiesMatter with the same fixed composition and properties

– Second Type of Pure SubstanceSecond Type of Pure Substance CompoundCompound

– Chemical Formula:Chemical Formula: A combination of chemical A combination of chemical symbols that show what elements make up a symbols that show what elements make up a compound and the number of atoms of each elementcompound and the number of atoms of each element Subscript:Subscript: A number written to the lower right of A number written to the lower right of

an element symbol to indicate the number of an element symbol to indicate the number of atoms of thatatoms of that

– How do you know if a substance is a compound? If it How do you know if a substance is a compound? If it is 1 thing only—and it is not on the periodic table.is 1 thing only—and it is not on the periodic table.

– Can you separate a compound? Yes—by chemically Can you separate a compound? Yes—by chemically decomposing it.decomposing it.

NaHNaH22COCO33 Mg(OH)Mg(OH)22

Decomposing a CompoundDecomposing a Compound

ElectrolysisElectrolysis– ““To tear apart with electricity”To tear apart with electricity”– The process in which electrical energy The process in which electrical energy

causes a non-spontaneous chemical causes a non-spontaneous chemical reaction to occur reaction to occur May break a compound apart into its May break a compound apart into its

elementselements Electrolysis of PbBrElectrolysis of PbBr22 & ZnCl & ZnCl22

Electrolysis of WaterElectrolysis of Water

MIXTURESTwo or more elements physically combined.

How can you tell something is a mixture?It can be physically separated into its parts.

Heterogeneous Mixtures

• The prefix “hetero” means “different”• A mixture with different compositions throughout• You can see each phase (part) of the mixture

Homogeneous Mixtures

• The prefix “homo-” means “the same”

• A mixture that is the same throughout

• You cannot see the phases (parts) of the mixture.

ALLOY

NAME OF ALLOY % MAKE UP EXAMPLE

Stainless Steel 73-79% Fe14-18% Cr7-9% Ni

Sterling Silver 92.5% Ag7.5% Cu

18-karat white gold 75% Au12.5% Ag12.5% Cu

14 karat gold 58% Au14-28% Ag14-28% Cu

Solutions• Solute: The substance being dissolved in a

solution• Solvent: The substance that dissolves the solute• Aqueous Solution: A solution in which water is

the solvent

HETEROGENEOUS OR

HOMOGENEOUS?

What is the solute?What is the solvent?

82% Fe

18% Cr

Methods to Separate Mixtures

• Filtration: Separates a solid from a liquid

Separating…

• Magnet: Separates Fe, Co, or Ni

Separating…• Distillation: Separates two or more liquids

with different boiling points.

Separating…• Crystallization: Separates crystalline solids

from a saturated liquid

Separating…

• Chromatography: Separates different types of liquids