02 lecture ppt
TRANSCRIPT
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Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Chapter 2Basic
Chemistry and Cells
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All Matter Is Composed of Chemical Elements
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2.1 Six elements are basic to life Six Elements of Life
Carbon – C Hydrogen – H Nitrogen – N Oxygen – O Phosphorus – P Sulfur – S
Element: substance that cannot be degraded by chemical means into a substance having different properties
Every element has a name and an atomic symbol Atoms: the smallest particles that retain the
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Figure 2.1 Elements that make up the Earth’s crust and its organisms
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2.2 Atoms contain subatomic particles
Two main parts of an atom Nucleus
Center of the atom where almost all the mass is located
Electron Shells Area surrounding the nucleus where the
electrons are located
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Subatomic Particles
Protons Positively charged particles located in the nucleus Protons have mass
Electrons Negatively charged particles located in the electron
cloud Electrons have so little mass that they are not
considered when determining the mass of an atom Neutrons
Neutrally charged (no charge) particles located in the nucleus
The mass of a neutron is equal to that of a proton
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Figure 2.2A The stippled area shows the probable location of electrons
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Figure 2.2B The shells in this atomic model represent the average location of electrons
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Figure 2.2C Atomic model of a carbon atom
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Isotopes
Atoms of a single element that differ in their number of neutrons Isotopes have the same number of protons,
but different atomic masses
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APPLYING THE CONCEPTS—HOW BIOLOGY IMPACTS OUR LIVES
2.3 Radioactive isotopes have many medical uses
Low Levels Small amounts of radiation can be used as a
tracer allowing doctors to ‘see’ inside of the body
High Levels Lots of radiation will damage DNA and kill
cells Can also be used to kill pathogens and treat
disease, like cancer
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Atoms React with One Another to Form Molecules
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2.4 After atoms react, they have a completed outer shell
Atoms are most stable when the outer shell has eight electrons Atoms exchange electrons in order to have a
complete outer shell or valence shell
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Figure 2.4A A portion of the periodic table of the elements
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Figure 2.4B Models of the six elements that are predominant in living things
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Compounds and Molecules
Compound – two or more different elements bonded together
Molecule – the smallest part of a compound that still has the properties of that compound
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2.5 An ionic bond occurs when electrons are transferred
Ion - an atom or molecule that has either lost or gained electrons
Losing an electron results in a net positive Gaining an electron results in a net negative
charge
Ions with opposite charges attract and form bonds known as ionic bonds
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Figure 2.5 Formation of sodium chloride (table salt)
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2.6 A covalent bond occurs when electrons are shared
When two atoms do not have completely full outer shells, they may share electrons so that each has a full outer shell
Example: Hydrogen (H2)
Bond Notation Single covalent bonds are written as H-H Double covalent bonds are written as O=O Triple covalent bonds are written as N≡N
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Figure 2.6A Electron models and formulas representing covalently bonded molecules
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Figure 2.6B Other types of molecular molecules—in this case, for methane (CH4)
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Chemical Reactions
The exchange of electrons between atoms create chemical reactions
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2.7 A covalent bond can be nonpolar or polar
Nonpolar covalent bond – when the sharing of electrons between atoms is fairly equal Electronegativity – the attraction of an atom for the
electrons in a covalent bond
Polar covalent bond – unequal sharing of electrons
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Figure 2.7 Three models of water
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2.8 A hydrogen bond can occur between polar molecules
Polar bonds have charges on either end and often attract to each other
When a hydrogen is bonded to an electronegative atom, it becomes electropositive
This causes it to be attracted to electronegative parts of the same or other molecules
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Figure 2.8 Hydrogen bonding between water molecules
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The Properties of Water Benefit Life
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2.9 Water molecules stick together: Cohesion
The tendency of water molecules to cling together Due to the four hydrogen bonds water has
Cohesion contributes to water transport in plants Adhesion of water to the walls of the vessels also
helps prevent the water column from breaking apart
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Figure 2.9 Water as a transport medium in trees
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2.10 Water warms up and cools down slowly
Calorie – the amount of heat energy needed to raise the temperature of 1 g of water 1°C
Water has a high heat of vaporization because so many hydrogen bonds must be broken
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2.11 Water dissolves other polar substances
A solution contains dissolved substances called solutes that which is dissolved
Water’s hydrogen bonds help it dissolve other polar molecules
Hydrophilic (water-loving) molecules form hydrogen bonds with water
Hydrophobic (water-fearing) molecules do not form hydrogen bonds with water
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Figure 2.11 An ionic salt dissolves in water
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2.12 Frozen water is less dense than liquid water
When water freezes, the crystal lattice expands With a greater volume and the same mass, the
density decreases and the solid, ice, floats in the denser liquid, water
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Figure 2.12A Ice is less dense than liquid water
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Living Things Require a Narrow pH Range
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2.13 Acids and bases affect living things
When water ionizes it releases equal amounts of hydrogen ions (H+) and hydroxide ions (OH-)
Some substances release more or fewer or each Acids - Excess hydrogen ions Bases - Excess hydroxide ions
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Figure 2.13A Dissociation of water molecules
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Figure 2.13B Acids cause H+ to increase
Figure 2.13C Bases cause OH- to increase
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2.14 The pH scale measures acidity and basicity
The pH scale goes from 0 to 14, 7 is neutral
The greater the H+ concentration, the lower the pH and the lower the hydrogen ion concentration, the higher the pH
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Figure 2.14 The pH scale
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2.15 Buffers help keep the pH of body fluids relatively constant
Buffer system: the combination of a weak acid and the base that forms when the acid dissolves in water
By binding or releasing H+’s, it maintains a constant concentration of free H+’s in the solution
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APPLYING THE CONCEPTS—HOW BIOLOGY IMPACTS OUR LIVES
2.16 Acid deposition has many harmful effects
Air pollution, particularly from burning fossil fuels, acidifies rainwater Leaches toxic aluminum and creates methyl mercury
in lakes Destroys leaves, stopping photosynthesis and making
trees susceptible to disease Increases respiratory disease and erodes buildings
and monuments
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Connecting the Concepts: Chapter 2
Cells are made up of chemicals and therefore we must understand chemistry Cells are composed of carbon, hydrogen, nitrogen,
oxygen, phosphorus, and sulfur Carbon forms long chains of carbon atoms
Water is a polar molecules and can dissolve other polar substances Water’s cohesiveness, tendency to change
temperature slowly, ability to expand as it freezes are due to hydrogen bonding
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