Chemistry Comes Alive
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Transcript of Chemistry Comes Alive
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Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings
Human Anatomy & PhysiologySEVENTH EDITION
Elaine N. MariebKatja Hoehn
PowerPoint® Lecture Slides prepared by Vince Austin, Bluegrass Technical and Community College
C H
A P
T E
R
2Chemistry Comes Alive
P A R T A
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Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings
Blood is collected from your patient and treated so it will not clot. This blood is placed in a long narrow tube that is placed vertically on a laboratory bench. In an hour, all the blood cells have settled to the bottom of the tube, leaving the rest of the tube filled with a clear, yellowish liquid called plasma. Why did the blood cells settle out of the blood?
A. blood is an acidic solution of cells and plasma that sticks to the tube
B. blood is a mixture of solids and gases that react with the air C. blood is a solution of Na+ and CL– ions that react to form a
precipitate D. blood is a suspension of cells in plasma that settles by gravity
Human Blood Collection Bellringer – NOT to turn in
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Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings
Human Blood Collection Bellringer – NOT to turn in Blood is collected from your patient and treated so it will not clot.
This blood is placed in a long narrow tube that is placed vertically on a laboratory bench. In an hour, all the blood cells have settled to the bottom of the tube, leaving the rest of the tube filled with a clear, yellowish liquid called plasma. Why did the blood cells settle out of the blood?
A. blood is an acidic solution of cells and plasma that sticks to the tube
B. blood is a mixture of solids and gases that react with the air C. blood is a solution of Na+ and CL– ions that react to form a
precipitate D. blood is a suspension of cells in plasma that settles by gravity
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Copyright © 2006 Pearson Education, Inc., publishing as Benjamin Cummings
Matter Anything that has mass and takes up space States of matter
Solid – has definite shape and volume Liquid – has definite volume, changeable shape Gas – has changeable shape and volume
All are important in Anatomy & Physiology
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Composition of Matter Elements – unique substances that cannot be
broken down by ordinary chemical means Atoms –building blocks for each element
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Major Elements of the Human Body Oxygen (O) Carbon (C) Hydrogen (H) Nitrogen (N)
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Lesser and Trace Elements of the Human Body Lesser elements make up 3.9% of the body and
include: Calcium (Ca), phosphorus (P), potassium (K), sulfur (S), sodium (Na), chlorine (Cl), magnesium (Mg), iodine (I), and iron (Fe)
Trace elements make up less than 0.01% of the body
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If given an element, identify if it is…
A major element of the body A lesser element of the body A trace element of the body
Vitamin Labels
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Molecules and Compounds Molecule – two or more atoms held together by
chemical bonds Compound – two or more different kinds of atoms
chemically bonded together (water or H2O is an example)
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Mixtures and Solutions Mixtures – two or more components physically
intermixed (not chemically bonded) Example: blood cells in blood
Most mixtures can be separated by physical means Solutions – homogeneous mixtures of components
Example: electrolytes such as Na+Cl-, K+CL-, etc. Solvent – substance present in greatest amount Solute – substance(s) present in smaller amounts
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Types of Chemical Bonds
Ionic Covalent Hydrogen Importance of polar and nonpolar molecules
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Factors Influencing Rate of Chemical Reactions
Catalysts – increase the rate of a reaction without being chemically changed
Enzymes = biological catalysts
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Biochemistry
Organic compounds Contain carbon, are covalently bonded, and are
often large Inorganic compounds
Do not contain carbon Water, salts, and many acids and bases
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Salts (NaCL, KCL, Na2SO4, etc.)
Inorganic compounds Contain cations other than H+ and anions other
than OH–
Are electrolytes; they conduct electrical currents
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Acids and Bases
Acids release H+ and are therefore proton donors
HCl H+ + Cl –
Bases release OH– and are proton acceptors
NaOH Na+ + OH–
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Acid-Base Concentration (pH)
Acidic solutions have higher H+ concentration and therefore a lower pH
Alkaline solutions have lower H+ concentration and therefore a higher pH
Neutral solutions have equal H+ and OH– concentrations
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Acid-Base Concentration (pH)
Acidic: pH 0–6.99 Basic: pH 7.01–14 Neutral: pH 7.00
Blood has pH ~ 7.4 Most body fluids pH 7.2 – 7.6
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Buffers
Chemical systems that resist abrupt and large swings in the pH of body fluids
Example: Carbonic acid-bicarbonate system in blood
Carbonic acid dissociates, reversibly releasing bicarbonate ions and protons
The chemical equilibrium between carbonic acid and bicarbonate resists pH changes in the blood
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Bicarbonate Buffer System Removes Acid If blood is too acidic: HLac(aq) + HCO3
-(aq) ↔ Lac-(aq) + H2CO3(aq) Lactic Acid + Bicarbonate Lactate + Carbonic Acid
If blood is too basic (alkaline): H2CO3(aq) ↔ H+(aq) + HCO3
-(aq)Carbonic Acid Protons + Bicarbonate
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Organic Compounds
Molecules unique to living systems contain carbon and hence are organic compounds
They include 4 important macromolecular biochemical polymers:
Carbohydrates Lipids Be able to identify from Proteins descriptions or pictures Nucleic Acids}
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Carbohydrates Contain carbon, hydrogen, and oxygen Their major function is to supply a source of
cellular food Examples:
Monosaccharides or simple sugars
Figure 2.14a
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Carbohydrates Polysaccharides or polymers of simple sugars
Figure 2.14c
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Lipids Contain C, H, and O, but the proportion of oxygen
in lipids is less than in carbohydrates Examples:
Neutral fats or triglycerides Phospholipids Steroids Eicosanoids
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Neutral Fats (Triglycerides)
Composed of three fatty acids bonded to a glycerol molecule
Figure 2.15a
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Other Lipids Steroids – flat molecules with four interlocking
hydrocarbon rings
Figure 2.15c
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Representative Lipids Found in the Body
Neutral fats – found in subcutaneous tissue and around organs
Phospholipids – chief component of cell membranes
Steroids – cholesterol, bile salts, vitamin D, sex hormones, and adrenal cortical hormones
Fat-soluble vitamins – vitamins A, E, and K
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Amino Acids
Building blocks of protein, containing an amino group and a carboxyl group
Amino group NH2
Carboxyl groups COOH
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Amino Acids
Figure 2.16a–c
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Examples of proteins
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Protein Macromolecules composed of combinations of 20
types of amino acids bound together with peptide bonds
Figure 2.17
Amino acid Amino acid
Dehydrationsynthesis
HydrolysisDipeptide
Peptide bond
+N
H
H
C
R
H
O
N
H
H
C
R
CC
H
O H2O
H2O
N
H
H
C
R
C
H
O
N
H
C
R
C
H
O
OH OH OH
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Fibrous and Globular Proteins Fibrous proteins
Extended and strand-like proteins Examples: keratin, elastin, collagen, and certain
contractile fibers
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Fibrous and Globular Proteins Globular proteins
Compact, spherical proteins with tertiary and quaternary structures
Examples: antibodies, hormones, and enzymes
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Characteristics of Enzymes Frequently named for the type of reaction they
catalyze Enzyme names usually end in -ase Lower activation energy of a reaction
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Nucleic Acids Composed of carbon, oxygen, hydrogen, nitrogen,
and phosphorus Their structural unit, the nucleotide, is composed
of N-containing base, a pentose sugar, and a phosphate group
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Nucleic Acids Five nitrogen bases contribute to nucleotide
structure – adenine (A), guanine (G), cytosine (C), thymine (T), and uracil (U)
Two major classes – DNA and RNA
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Deoxyribonucleic Acid (DNA) Double-stranded helical molecule found in the
nucleus of the cell Replicates itself before the cell divides, ensuring
genetic continuity Provides instructions for protein synthesis
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Structure of DNA
Figure 2.22b
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Adenosine Triphosphate (ATP) Source of immediately usable energy for the cell Adenine-containing RNA nucleotide with three
phosphate groups
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Adenosine Triphosphate (ATP)