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PowerPoint ® Lecture Slide Presentation by Patty Bostwick-Taylor, Florence-Darlington Technical College Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings PART A 2 Basic Chemistry
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Matter and Energy Matter—anything that occupies space and has mass (weight) - solids, liquids, gases - physical changes- __________________ -chemical changes -__________________ Energy—the ability to do work Chemical Electrical Mechanical Radiant
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Composition of Matter __________—fundamental units of matter 96% of the body is made from four elements Carbon (C) Oxygen (O) Hydrogen (H) Nitrogen (N) ________—building blocks of elements
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Atomic Structure Nucleus Protons (p + ) Neutrons (n 0 ) Outside of nucleus Electrons (e - ) – an atom that gains or loses an e- is called an _________ Figure 2.1
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Atomic Structure of Smallest Atoms Figure 2.2
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Identifying Elements Atomic number—equal to the number of protons that the atom contains Atomic mass number—sum of the protons and neutrons
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Isotopes and Atomic Weight Isotopes Have the same number of_________ Vary in number of_________ Figure 2.3
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Isotopes and Atomic Weight Atomic weight average average masses of naturally occurring isotopes Atomic weight reflects natural isotope variation
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Radioactivity Radioisotope Heavy isotope Tends to be unstable Decomposes to more stable isotope Radioactivity—process of spontaneous atomic decay
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Molecules and Compounds Molecule—two or more ______atoms combined chemically Compound—two or more ______atoms combined chemically Figure 2.4
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Chemical Reactions Atoms are united by chemical bonds Atoms dissociate from other atoms when chemical bonds are broken
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Electrons and Bonding Electrons occupy energy levels called electron shells Electrons closest to the nucleus are most strongly attracted Each shell has distinct properties The number of electrons has an upper limit Shells closest to the nucleus fill first
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Electrons and Bonding Bonding involves interactions between electrons in the outer shell (______shell) Full valence shells do not form bonds
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Inert Elements Atoms are stable (_____) when the outermost shell is complete How to fill the atom’s shells Shell 1 can hold a maximum of 2 electrons Shell 2 can hold a maximum of 8 electrons Shell 3 can hold a maximum of 18 electrons
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Inert Elements Atoms will gain, lose, or share electrons to complete their outermost orbitals and reach a stable state Rule of eights Atoms are considered stable when their outermost orbital has 8 electrons The exception to this rule of eights is_____, which can only hold __ electrons
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Inert Elements Figure 2.5a
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Figure 2.5b Reactive Elements Valence shells are not full and are unstable Tend to gain, lose, or share electrons Allow for bond formation, which produces stable valence
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Chemical Bonds (4 types - 1 of 4) Ionic bonds Form when electrons are completely transferred from one atom to another Ions Charged particles _______are negative _______are positive Either donate or accept electrons
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Chemical Bonds (4 types - 2 and 3 of 4) Covalent bonds (polar and nonpolar) Atoms become stable through shared electrons Single covalent bonds share one pair of electrons Double covalent bonds share two pairs of electrons
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Polarity (covalent bonds con’t) Covalently bonded molecules Some are non-polar Electrically neutral as a molecule Some are polar Have a positive and negative side Figure 2.8
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Chemical Bonds (4 types – 4 of 4) Hydrogen bonds ________ chemical bonds Hydrogen is attracted to the negative portion of polar molecule O or N ----H----e- hungry atom Surface tension in water __________ bonds
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Hydrogen Bonds Figure 2.9
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Patterns of Chemical Reactions Synthesis reaction (A + B AB) Atoms or molecules combine Energy is absorbed for bond formation ______ reaction Decomposition reaction (AB A + B) Molecule is broken down Chemical energy is released _______reaction
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Synthesis and Decomposition Reactions Figure 2.10a
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Synthesis and Decomposition Reactions Figure 2.10b
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Patterns of Chemical Reactions Exchange reaction (AB + C AC + B) Involves both synthesis and decomposition reactions Switch is made between molecule parts and different molecules are made
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Patterns of Chemical Reactions Figure 2.10c
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Biochemistry: Essentials for Life Organic compounds Contain carbon Larger – lipids, proteins, carbohydrates, ___________ EXCEPTIONS: CO, CO2, HCO3 Inorganic compounds Lack carbon Tend to be simpler compounds Example: H 2 O (water), salt
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Important Inorganic Compounds Water Most abundant inorganic compound Vital properties High heat capacity Polarity/solvent properties Chemical reactivity ____________
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Important Inorganic Compounds Salts Easily dissociate into ions in the presence of water Vital to many body functions Include electrolytes which conduct electrical currents
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Dissociation of a Salt in Water Figure 2.11
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Important Inorganic Compounds Acids Release hydrogen ions (H + ) Are proton_______ Bases Release hydroxyl ions (OH – ) Are proton_______ Neutralization reaction Acids and bases react to form water and a salt
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Figure 2.12 pH Measures relative concentration of _____ions pH 7 = neutral pH below 7 = acidic pH above 7 = basic Buffers—chemicals that can regulate pH change
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Important Organic Compounds Carbohydrates Contain carbon, hydrogen, and oxygen Include sugars and starches Classified according to size ____________—simple sugars Disaccharides—two simple sugars joined by dehydration synthesis Polysaccharides—long-branching chains of linked simple sugars
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Carbohydrates Figure 2.13a–b
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Carbohydrates Figure 2.13c
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Carbohydrates Figure 2.14
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Important Organic Compounds Lipids Contain carbon, hydrogen, and oxygen Carbon and hydrogen outnumber oxygen Insoluble in water
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Lipids Common lipids in the human body Neutral fats (_________) Found in fat deposits Composed of fatty acids and glycerol Source of stored energy Saturated v. unsaturated Transfats- H added to C at double bond sites
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Lipids Figure 2.15a
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Lipids Common lipids in the human body (continued) Phospholipids Form cell membranes Steroids Include cholesterol, bile salts, vitamin D, and some hormones
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Lipids Figure 2.15b
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Figure 2.15c Lipids Cholesterol The basis for all steroids made in the body
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Important Organic Compounds Proteins Made of amino acids Contain carbon, oxygen, hydrogen, nitrogen, and sometimes sulfur Figure 2.16
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Proteins Account for over half of the body’s organic matter Provide for construction materials for body tissues Act as enzymes, hormones, and antibodies
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Proteins Amino acid structure Contain an amine group (NH 2 ) Contain an acid group (COOH) Vary only by R groups
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Figure 2.17a Proteins Fibrous proteins Also known as _____proteins Appear in body structures Examples include collagen and keratin Stable
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Figure 2.17b Proteins Globular proteins Also known as ______proteins Function as antibodies or enzymes Can be denatured
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Figure 2.18a Enzymes Act as biological catalysts Increase the rate of chemical reactions
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Enzymes Figure 2.18b
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Important Organic Compounds Nucleic Acids Provide blueprint of life 3 Basic parts: 1. Base 2. Phosphate group 3. 5 C sugar Make ____and RNA Figure 2.19a
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Nucleic Acids Deoxyribonucleic acid (DNA) Organized by complimentary bases to form double helix Replicates before cell division Provides instructions for every protein in the body Figure 2.19c
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Important Organic Compounds Adenosine triphosphate (ATP) Chemical energy used by all cells Energy is released by breaking high energy ______bond ATP is replenished by oxidation of food fuels
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Adenosine Triphosphate (ATP) Figure 2.20a
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Copyright © 2009 Pearson Education, Inc., publishing as Benjamin Cummings Figure 2.21 + ADP Solute Contracted muscle cell Product made Relaxed muscle cell Reactants Transport work Mechanical work Chemical work Membrane protein Solute transported Energy liberated during oxidation of food fuels used to regenerate ATP ATP P P P X Y (a) (b) (c) YX P P +
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