Matter and Energy

1
Matter and Energy
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds D. Energy

• Principles of chemistry
• Water
• Organic compounds
• Energy

2
Principles of Chemistry
II. Matter Energy A. Principles of
Chemistry 1. Atomic structure
2. The periodic table 3. Chemical
bonding 4. Important elements B.
Water C. Organic Compounds D. Energy

• Atomic structure
• The periodic table
• Chemical bonding
• Important elements in environmental processes

3
A.1. Atomic Structure
II. Matter Energy A. Principles of
Chemistry 1. Atomic structure
2. The periodic table 3. Chemical
bonding 4. Important elements B.
Water C. Organic Compounds D. Energy

• Matter
• Anything that takes up space and has mass
• Atom
• The smallest stable particle of matter
• Composed of protons, neutrons, and electrons
• Overall structure textbook figure 2.3

4
A.1. Atomic Structure
II. Matter Energy A. Principles of
Chemistry 1. Atomic structure
2. The periodic table 3. Chemical
bonding 4. Important elements B.
Water C. Organic Compounds D. Energy

• Protons
• Positively charged
• Atomic mass ? 1 atomic mass unit
• Located in the nucleus of an atom
• Neutrons
• Electrically neutral
• Atomic mass ? 1 atomic mass unit
• Located in the nucleus of an atom

5
A.1. Atomic Structure
II. Matter Energy A. Principles of
Chemistry 1. Atomic structure
2. The periodic table 3. Chemical
bonding 4. Important elements B.
Water C. Organic Compounds D. Energy

• Electrons
• Negatively charged
• Atomic mass very small, almost negligible
• Located in electron shells (orbitals) around the
  nucleus
• In a neutral atom, the number of electrons and
  protons is the same
• Atoms can lose or gain electrons during chemical
  bonding

6
A.1. Atomic Structure
II. Matter Energy A. Principles of
Chemistry 1. Atomic structure
2. The periodic table 3. Chemical
bonding 4. Important elements B.
Water C. Organic Compounds D. Energy

• Element
• A substance composed of only a single type of
  atom
• Atomic number of an element
• The number of protons in its atoms
• The atomic number is the same for all atoms of an
  element
• Mass number of an element
• The number of protons plus the number of neutrons
  in its atoms
• The atoms of an element may have a variable
  number of neutrons

7
A.1. Atomic Structure
II. Matter Energy A. Principles of
Chemistry 1. Atomic structure
2. The periodic table 3. Chemical
bonding 4. Important elements B.
Water C. Organic Compounds D. Energy

• Isotopes of an element
• Different forms of an element with the same
  atomic number but with different mass numbers
• The atoms of some isotopes are stable
• Other isotopes are radioactive, having unstable
  atoms that spontaneously break apart (decay) to
  form other atoms
• When radioactive atoms decay, energy is released

8
A.1. Atomic Structure
II. Matter Energy A. Principles of
Chemistry 1. Atomic structure
2. The periodic table 3. Chemical
bonding 4. Important elements B.
Water C. Organic Compounds D. Energy

• For example, carbon has three isotopes
• Carbon-12, with 6 protons and 6 neutrons, is the
  most common form of carbon
• Carbon-13, with 6 protons and 7 neutrons, is
  stable (non-radioactive) and rare
• Carbon-14, with 6 protons and 8 neutrons, is
  unstable (radioactive) and rare

9
A.2. The Periodic Table
II. Matter Energy A. Principles of
Chemistry 1. Atomic structure
2. The periodic table 3. Chemical
bonding 4. Important elements B.
Water C. Organic Compounds D. Energy

• Textbook figure 2.2
• In the periodic table
• Elements are listed in order of their atomic
  numbers
• Elements are designated by standard one or
  two-letter abbreviations
• Elements in the same vertical column often have
  very similar chemical bonding properties

10
A.2. The Periodic Table
II. Matter Energy A. Principles of
Chemistry 1. Atomic structure
2. The periodic table 3. Chemical
bonding 4. Important elements B.
Water C. Organic Compounds D. Energy

• Notable groups in the periodic table
• Metals, nonmetals, and metalloids
• Halogens
• Nobel gases
• Heavy metals
• Synthetic elements (larger than uranium)

11
A.3. Chemical Bonding
II. Matter Energy A. Principles of
Chemistry 1. Atomic structure
2. The periodic table 3. Chemical
bonding 4. Important elements B.
Water C. Organic Compounds D. Energy

• Chemical bonding occurs when two or more atoms
  combine
• Atoms combine by exchanging or sharing electrons
  in their outermost electron shell
• Chemical compound
• Formed when the atoms of two or more different
  elements combine by chemical bonding
• Properties of a compound are usually very
  different than those of its elements

12
A.3. Chemical Bonding
II. Matter Energy A. Principles of
Chemistry 1. Atomic structure
2. The periodic table 3. Chemical
bonding 4. Important elements B.
Water C. Organic Compounds D. Energy

• Ionic bonds
• Formed when electrons are completely transferred
  from one atom to another
• The atom that gains electrons becomes a negative
  ion (anion)
• The atom that loses electrons becomes a positive
  ion (cation)
• Example Sodium chloride Na Cl ? Na Cl

13
A.3. Chemical Bonding
II. Matter Energy A. Principles of
Chemistry 1. Atomic structure
2. The periodic table 3. Chemical
bonding 4. Important elements B.
Water C. Organic Compounds D. Energy

• Covalent bonds
• Form when two atoms share one or more pairs of
  electrons
• Molecule consists of two or more atoms that are
  joined by covalent bonding
• Covalent bonds are generally more stable than
  ionic bonds in aqueous (water) solution
• Examples textbook, figures 2.4 2.6

14
A.4. Important Elements
II. Matter Energy A. Principles of
Chemistry 1. Atomic structure
2. The periodic table 3. Chemical
bonding 4. Important elements B.
Water C. Organic Compounds D. Energy

• Textbook, table 2.1

15
Water
II. Matter Energy A. Principles of
Chemistry B. Water 1. Structure of
Water 2. Ionization of Water
3. Solvent Properties 4. Thermal
Properties C. Organic Compounds D.
Energy

1. Structure of water
2. Ionization of water
3. Solvent properties of water
4. Thermal properties of water

16
B.1. Structure of Water
II. Matter Energy A. Principles of
Chemistry B. Water 1. Structure of
Water 2. Ionization of Water
3. Solvent Properties 4. Thermal
Properties C. Organic Compounds D.
Energy

• A water molecule is composed of two hydrogen
  atoms covalently bonded to an oxygen atom
• The hydrogen atoms form an angle of about 110,
  so the molecule is bent

17
B.1. Structure of Water
II. Matter Energy A. Principles of
Chemistry B. Water 1. Structure of
Water 2. Ionization of Water
3. Solvent Properties 4. Thermal
Properties C. Organic Compounds D.
Energy

• The oxygen nucleus exerts a greater pull on the
  electrons in the covalent bonds
• Therefore, the oxygen atom has a partial negative
  charge
• And the hydrogen atoms have partial positive
  charges

18
B.1. Structure of Water
II. Matter Energy A. Principles of
Chemistry B. Water 1. Structure of
Water 2. Ionization of Water
3. Solvent Properties 4. Thermal
Properties C. Organic Compounds D.
Energy

• Because opposite charges attract each other,
  water molecules are attracted to each other and
  to other charged molecules or ions

19
B.1. Structure of Water
II. Matter Energy A. Principles of
Chemistry B. Water 1. Structure of
Water 2. Ionization of Water
3. Solvent Properties 4. Thermal
Properties C. Organic Compounds D.
Energy

• The bent geometry of water and the attraction
  between water molecules gives rise to unique
  properties that are essential for its role in
  living organisms and the environment

20
B.2. Ionization of Water
II. Matter Energy A. Principles of
Chemistry B. Water 1. Structure of
Water 2. Ionization of Water
3. Solvent Properties 4. Thermal
Properties C. Organic Compounds D.
Energy

• Consider a glass of pure water
• In a tiny fraction of the water molecules (1 out
  of 10 million), one of the hydrogen nuclei is
  completely pulled off the molecule
• This forms two ions
• A hydrogen ion (H)
• And a hydroxyl ion (OH)
• This is caused by the attraction of the water
  molecules for each other

21
B.2. Ionization of Water
II. Matter Energy A. Principles of
Chemistry B. Water 1. Structure of
Water 2. Ionization of Water
3. Solvent Properties 4. Thermal
Properties C. Organic Compounds D.
Energy

• Water molecules are continuously splitting into
  ions and rejoining to form water molecules

22
B.2. Ionization of Water
II. Matter Energy A. Principles of
Chemistry B. Water 1. Structure of
Water 2. Ionization of Water
3. Solvent Properties 4. Thermal
Properties C. Organic Compounds D.
Energy

• In chemically pure water, the number of H and
  OH ions are the same
• Certain chemical substances, when dissolved in
  water, can change the amounts of H or OH

23
B.2. Ionization of Water
II. Matter Energy A. Principles of
Chemistry B. Water 1. Structure of
Water 2. Ionization of Water
3. Solvent Properties 4. Thermal
Properties C. Organic Compounds D.
Energy

• Acid
• A substance that increases the amount of H (and
  decreases the amount of OH)
• Base (Alkaline)
• A substance that increases the amount of OH
  (and decreases the amount of H)
• Neutral substance
• A substance that does not change the amounts of
  H and OH (so H remains equal to OH)

24
B.2. Ionization of Water
II. Matter Energy A. Principles of
Chemistry B. Water 1. Structure of
Water 2. Ionization of Water
3. Solvent Properties 4. Thermal
Properties C. Organic Compounds D.
Energy

• Acidity and alkalinity are represented by a value
  called pH
• Acids pH value is less than 7
• Bases pH value is greater than 7
• Neutral substances pH value is equal to 7
• Each pH value represents a 10-fold change in the
  amount of H in the solution
• So a substance with pH 5 has a 10 times greater
  amount of H than a substance with pH 6
• Textbook, figure 2.5

25
B.3. Solvent Properties of Water
II. Matter Energy A. Principles of
Chemistry B. Water 1. Structure of
Water 2. Ionization of Water
3. Solvent Properties 4. Thermal
Properties C. Organic Compounds D.
Energy

• Solution
• A mixture of two (or more) different substances
  in which the particles of one substance are
  completely interspersed with the particles of the
  other substance(s)
• Solvent The substance that is present in the
  largest amount
• Solute The substance(s) that are present in
  smaller amounts

26
B.3. Solvent Properties of Water
II. Matter Energy A. Principles of
Chemistry B. Water 1. Structure of
Water 2. Ionization of Water
3. Solvent Properties 4. Thermal
Properties C. Organic Compounds D.
Energy

• Hydrophilic substances
• Substances that can be dissolved in water
• Water molecules are attracted to ions or to other
  molecules that have partial positive and negative
  charges
• Examples of hydrophilic substances
• Sodium chloride (table salt) This substance
  consists of sodium ions and chloride ions
• Sucrose (table sugar) This substance is a
  compound with many -OH groups in its structure,
  with many partial positive and negative charges

27
B.3. Solvent Properties of Water
II. Matter Energy A. Principles of
Chemistry B. Water 1. Structure of
Water 2. Ionization of Water
3. Solvent Properties 4. Thermal
Properties C. Organic Compounds D.
Energy

• Hydrophobic substances
• Substances that cannot be dissolved in water
• Water molecules have difficulty interacting with
  uncharged molecules. These substances tend to
  separate from water.
• Example of a hydrophobic substance
• Cooking oil The molecules of cooking oil have
  long chains of carbon atoms bonded to hydrogen.
  The atoms do not have the bent geometry of
  water, so there are no partial charges to attract
  the water.Therefore, oil and water dont mix!

28
B.3. Solvent Properties of Water
II. Matter Energy A. Principles of
Chemistry B. Water 1. Structure of
Water 2. Ionization of Water
3. Solvent Properties 4. Thermal
Properties C. Organic Compounds D.
Energy

• Amphipathic substances
• Substances in which part of the molecule is
  hydrophobic, and part of the molecule is
  hydrophilic
• When amphipathic substances are mixed in water,
  its molecules form into clusters called
  micelles
• with the hydrophilic part on the outside of the
  micelle in contact with water
• and the hydrophobic part on the inside of the
  micelle, away from the water .

29
B.3. Solvent Properties of Water
II. Matter Energy A. Principles of
Chemistry B. Water 1. Structure of
Water 2. Ionization of Water
3. Solvent Properties 4. Thermal
Properties C. Organic Compounds D.
Energy

• Amphipathic substances (cont.)
• Example of an amphipathic substance
• Soap Soap molecules have an ionic group attached
  to one end, and an oily hydrocarbon chain
  attached to the other end. When soap is mixed
  with water, it forms micelles that trap oily dirt
  molecules.

30
B.4. Thermal Properties of Water
II. Matter Energy A. Principles of
Chemistry B. Water 1. Structure of
Water 2. Ionization of Water
3. Solvent Properties 4. Thermal
Properties C. Organic Compounds D.
Energy

• Molecules are in constant motion due to the heat
  energy (kinetic energy) they contain
• Phases of matter
• Solid
• Limited movement of molecules non-fluid
• Liquid
• Molecules can move freely around each other
  fluid
• Gas
• Molecules have greatest freedom of movement
  substance can expand to fill the available space

31
B.4. Thermal Properties of Water
II. Matter Energy A. Principles of
Chemistry B. Water 1. Structure of
Water 2. Ionization of Water
3. Solvent Properties 4. Thermal
Properties C. Organic Compounds D.
Energy

• Water has unusual thermal properties because of
  the attraction of water molecules for each other
• Water has relatively high melting and boiling
  points
• Water remains in a liquid state over a wide
  temperature range
• Water has a high heat capacity it can absorb a
  large amount of heat with a small change in
  temperature
• The solid form of water (ice) is less dense than
  the liquid, so ice floats on water

32
Organic Compounds
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds 1. Bonding of Carbon
2. Monomers Polymers 3. Bioorganic
compounds D. Energy

1. Bonding of carbon
2. Monomers and polymers
3. Bioorganic compounds

33
C. 1. Bonding of Carbon
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds 1. Bonding of Carbon
2. Monomers Polymers 3. Bioorganic
compounds D. Energy

• Carbon can form four covalent bonds with other
  atoms, such as nitrogen, oxygen, phosphorus,
  sulfur, halogens, and other carbons
• Compounds formed from the covalent bonding of
  carbon are called organic compounds
• Carbon-carbon bonds are very stable, allowing the
  formation of very large organic molecules

34
C. 1. Bonding of Carbon
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds 1. Bonding of Carbon
2. Monomers Polymers 3. Bioorganic
compounds D. Energy

• Hydrocarbons
• Consist of carbon and hydrogen
• Usually hydrophobic
• Aromatic hydrocarbons contain one or more benzene
  rings (phenyl groups)

35
C. 2. Monomers and Polymers
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds 1. Bonding of Carbon
2. Monomers Polymers 3. Bioorganic
compounds D. Energy

• Monomer
• An organic molecule that serves as a building
  block to build larger organic molecules
• Polymer
• An organic molecule composed of two or more
  monomer units linked together by covalent bonds

36
C. 2. Monomers and Polymers
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds 1. Bonding of Carbon
2. Monomers Polymers 3. Bioorganic
compounds D. Energy

• Condensation reaction
• Polymers are often formed by the process of
  condensation
• In this process, two hydrogen atoms and an oxygen
  atom are removed from two monomer units
• And a covalent bond forms between the monomers

37
C. 2. Monomers and Polymers
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds 1. Bonding of Carbon
2. Monomers Polymers 3. Bioorganic
compounds D. Energy
38
C. 2. Monomers and Polymers
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds 1. Bonding of Carbon
2. Monomers Polymers 3. Bioorganic
compounds D. Energy

• Hydrolysis reaction
• Polymers are often broken down by the process of
  hydrolysis
• In this process, a water molecule is inserted
  between the monomer units of a polymer
• To split the polymer into its monomer units

39
C. 2. Monomers and Polymers
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds 1. Bonding of Carbon
2. Monomers Polymers 3. Bioorganic
compounds D. Energy
40
C. 3. Bioorganic Compounds
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds 1. Bonding of Carbon
2. Monomers Polymers 3. Bioorganic
compounds D. Energy

• Textbook, figure 2.6 table 2.2
• Carbohydrates
• Composed mostly of carbon, hydrogen, and oxygen
• Large number of OH groups attached to the
  carbons
• Functions
• Energy source for living cells
• Certain structural components of cells

41
C. 3. Bioorganic Compounds
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds 1. Bonding of Carbon
2. Monomers Polymers 3. Bioorganic
compounds D. Energy

• Carbohydrates (cont.)
• Monosaccharides
• Simple sugars
• Monomer unit of carbohydrate group
• Examples Glucose, fructose
• Disaccharides
• Composed of two monosaccharide units joined
  together
• Examples Sucrose, lactose
• Polysaccharides
• Composed of multiple monosaccharide units (100s
  1000s)
• Examples Starch, glycogen, cellulose

42
C. 3. Bioorganic Compounds
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds 1. Bonding of Carbon
2. Monomers Polymers 3. Bioorganic
compounds D. Energy

• Lipids
• Biological compounds with hydrophobic components
  in their molecular structures
• Functions
• Energy storage
• Structural components
• Glycerides
• A major class of lipid
• Composed of a glycerol molecule attached to one,
  two, or three fatty acid molecules

43
C. 3. Bioorganic Compounds
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds 1. Bonding of Carbon
2. Monomers Polymers 3. Bioorganic
compounds D. Energy

• Lipids (cont.)
• Generalized structure of a triglyceride

44
C. 3. Bioorganic Compounds
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds 1. Bonding of Carbon
2. Monomers Polymers 3. Bioorganic
compounds D. Energy

• Proteins
• Composed of chains of amino acids
• There are 20 different amino acids, each with
  distinctive chemical properties
• A protein molecule may contain several hundred
  amino acids
• Each different protein has its own order, or
  sequence, of amino acids
• The correct sequence of amino acids is essential
  for the proteins function

45
C. 3. Bioorganic Compounds
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds 1. Bonding of Carbon
2. Monomers Polymers 3. Bioorganic
compounds D. Energy

• Proteins (cont.)
• Functions
• Enzymes Enzymes are biological catalysts that
  control almost every reaction in living systems
• Cellular recognition and communication
• Structural components of living cells

46
C. 3. Bioorganic Compounds
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds 1. Bonding of Carbon
2. Monomers Polymers 3. Bioorganic
compounds D. Energy

• Nucleic acids
• Composed of chains of nucleotides
• There are 4 different nucleotides
• A nucleic acid molecule may contain several
  thousands or millions of nucleotides
• Each nucleic acid molecule has its own order, or
  sequence, of nucleotides
• The correct sequence of nucleotides is essential
  for the nucleic acids function

47
C. 3. Bioorganic Compounds
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds 1. Bonding of Carbon
2. Monomers Polymers 3. Bioorganic
compounds D. Energy

• Nucleic acids (cont.)
• Overall function
• The sequence of nucleotides in a nucleic acid
  molecule serves as a blueprint to encode the
  correct sequence of amino acids for a protein.
  The code for a specific protein is called a
  gene.
• Deoxyribonucleic acid (DNA) DNA molecules
  (chromosomes) serve as the master blueprint for
  all of the cells proteins. The DNA molecules are
  transmitted to offspring during reproduction.
• Ribonucleic acid (RNA) RNA molecules serve as
  working copies of the genes for the proteins
  that the cell is making at any given time.

48
Energy
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds D. Energy 1. Types of
energy 2. Oxidation and reduction
3. Electrical generation

1. Types of energy
2. Oxidation and reduction
3. Electrical generation

49
D. 1. Types of Energy
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds D. Energy 1. Types of
energy 2. Oxidation and reduction
3. Electrical generation

• Energy
• The ability to do work
• The capacity to change matter
• Kinetic energy and potential energy
• Kinetic energy
• Energy associated with movement
• Energy released as a process occurs
• Potential energy
• Stored energy that is contained in matter
• The potential of matter for undergoing change

50
D. 1. Types of Energy
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds D. Energy 1. Types of
energy 2. Oxidation and reduction
3. Electrical generation

• Heat
• Energy associated with the movement of molecules
• Electromagnetism
• Energy associated with electrical charges and
  magnetic fields
• Electric current is produced by electrons flowing
  through a conductor (such as a copper wire)

51
D. 1. Types of Energy
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds D. Energy 1. Types of
energy 2. Oxidation and reduction
3. Electrical generation

• Electromagnetic radiation
• Energy that travels through space in the form of
  packets of energy waves called photons
• The amount of energy in a photon is related to
  its wavelength the shorter the wavelength, the
  more energy the photon has
• Photons can interact with matter to cause
  different affects, depending on the energy of the
  photons
• Textbook, figure 2.9

52
D. 1. Types of Energy
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds D. Energy 1. Types of
energy 2. Oxidation and reduction
3. Electrical generation

• Chemical energy
• Energy associated with the making or breaking of
  chemical bonds
• Exothermic reaction
• A chemical reaction in which energy is released
• Endothermic reaction
• A chemical reaction in which energy is absorbed
• Atomic energy
• Energy released when radioactive isotopes split
  apart (atomic fission) or fuse together (atomic
  fusion)
• Textbook, figure 12.9

53
D. 2. Oxidation and Reduction
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds D. Energy 1. Types of
energy 2. Oxidation and reduction
3. Electrical generation

• Energy is associated with the gain or loss of
  electrons by atoms in chemical reactions
• Reduction reaction
• A reaction in which an atom gains electrons
• By becoming bonded to a less electronegative atom
  (such as hydrogen)
• Compounds with more reduced atoms often have a
  larger amount of potential chemical energy (in an
  oxygen atmosphere)

54
D. 2. Oxidation and Reduction
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds D. Energy 1. Types of
energy 2. Oxidation and reduction
3. Electrical generation

• Oxidation reaction
• A reaction in which an atom loses electrons
• By becoming bonded to a more electronegative atom
  (such as oxygen)
• Compounds with more oxidized atoms often have a
  smaller amount of potential chemical energy (in
  an oxygen atmosphere)
• Oxidation and reduction reactions always occur
  together one substance is oxidized, and another
  substance is reduced.

55
D. 2. Oxidation and Reduction
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds D. Energy 1. Types of
energy 2. Oxidation and reduction
3. Electrical generation

• Examples
• Oxidation of methane (natural gas)
• 2 CH4 4 O2 2 CO2 4 H2O Energy (Heat
  Light)
• Reduction of CO2 to form glucose in
  photosynthesis
• 6 CO2 6 H2O Energy (Light) C6H12O6 6 O2

56
D. 3. Electrical Generation
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds D. Energy 1. Types of
energy 2. Oxidation and reduction
3. Electrical generation

• Electric current
• The movement of electrons through a conductor
  (such as a copper wire)
• Electrical generator
• When a conductor (such as a copper wire) is moved
  in a magnetic field, a current is generated in
  the wire
• By moving a coil of wire within a strong magnetic
  field, large electrical currents can be generated

57
D. 3. Electrical Generation
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds D. Energy 1. Types of
energy 2. Oxidation and reduction
3. Electrical generation
58
D. 3. Electrical Generation
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds D. Energy 1. Types of
energy 2. Oxidation and reduction
3. Electrical generation

• Types of generators
• Coal, oil, and natural gas generators
• Pressurized steam is generated by boiling water,
  using fossil fuels as an energy source
• The steam pressure is used to run turbines that
  are attached to the generator coils
• Hydroelectric generators
• The energy from falling water (from waterfalls or
  dams) is used to run turbines that are attached
  to generator coils

59
D. 3. Electrical Generation
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds D. Energy 1. Types of
energy 2. Oxidation and reduction
3. Electrical generation

• Types of generators (cont.)
• Nuclear generators
• The tremendous heat from a nuclear chain reaction
  is used to generate pressurized steam
• The steam pressure is used to run a turbine that
  is attached to the generator coils
• Textbook, figures 12.9 12.11
• Other methods
• Windmill generators
• Tidal power generators (Figure 12.30)

60
D. 3. Electrical Generation
II. Matter Energy A. Principles of
Chemistry B. Water C. Organic
Compounds D. Energy 1. Types of
energy 2. Oxidation and reduction
3. Electrical generation

• Other methods of generating electricity
• Chemical cells (batteries)
• Uses chemical oxidation and reduction
• Often, the cells contain substance (such as heavy
  metals) that are difficult to dispose
• Figure 12.23
• Photovoltaic cells
• Crystals of certain substances produce an
  electrical current when exposed to light
• Figure 12.20