Chapter 002
-
Upload
laura-gosnell -
Category
Technology
-
view
422 -
download
0
Transcript of Chapter 002
![Page 1: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/1.jpg)
The Human Body in Health and Illness, 4th edition
Barbara Herlihy
Chapter 2:Basic Chemistry
1
![Page 2: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/2.jpg)
Lesson 2-1 Objectives• Define the terms matter and element.• List the four elements that compose 96% of
body weight.• Describe the three components of an atom.• Describe the role of electrons in the formation
of chemical bonds.• Differentiate among ionic, covalent, and
hydrogen bonds.• Explain the differences among electrolytes,
ions, cations, and anions.
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.2
![Page 3: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/3.jpg)
Matter
• Matter: Anything that occupies space and has weight
• Matter exists in three states.– Solid– Liquid– Gas
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.3
![Page 4: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/4.jpg)
Matter: Two Types of Changes
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.4
![Page 5: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/5.jpg)
Elements
• Element: Matter composed of atoms that have the same number of positive charges in their nuclei
• Trace elements: Present in tiny amounts; essential for life
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.5
![Page 6: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/6.jpg)
Elements (cont’d)
• Four elements make up about 96% of human body weight.
Oxygen 65.0%Carbon 18.5%Hydrogen 9.5%Nitrogen 3.2%
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.6
![Page 7: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/7.jpg)
Atoms
• Atom: Smallest unit of an element with that element’s chemical characteristics
• Three subatomic particles Protons Neutrons Electrons
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.7
![Page 8: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/8.jpg)
Atoms (cont’d.)
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.8
![Page 9: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/9.jpg)
Atoms (cont’d.)
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.9
![Page 10: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/10.jpg)
Atoms (cont’d.)
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.10
![Page 11: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/11.jpg)
Atoms (cont’d.)
• Atomic number: The number of protons in the nucleus
• Atomic mass: Sum of the numbers of protons and neutrons in the nucleus of an atom
• Isotope: A different form of the same atom; same atomic number, different atomic mass
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.11
![Page 12: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/12.jpg)
Chemical Bonds
• Chemical bond: The electrical attraction between atoms
• Three types of chemical bonds– Covalent– Hydrogen– Ionic
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.12
![Page 13: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/13.jpg)
Chemical Bonds (cont’d.)
• Ionic bond: Caused by a transfer of electrons between atoms
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.13
![Page 14: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/14.jpg)
Chemical Bonds (cont’d.)
• Covalent bond: Involves a sharing of electrons by the outer shells of the atoms
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.14
![Page 15: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/15.jpg)
Chemical Bonds (cont’d.)
• Hydrogen bond: An intermolecular attraction, not caused by transfer of electrons or sharing of electrons by outer shells of the atoms
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.15
![Page 16: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/16.jpg)
Ions
• Ions: Atoms or groups of atoms that carry an electrical charge
• Two types of ions– Cations: Positively charged– Anions: Negatively charged
• Electrolytes: Form ions when dissolved in water
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.16
![Page 17: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/17.jpg)
Common Ions: Cations
Name Symbol Function
CationsSodium
Calcium
Iron
Na+
Ca2+
Fe2+
Fluid balance; nerve-muscle function
Component of bones and teeth; blood clotting; muscle contraction
Component of hemoglobin
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.17
![Page 18: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/18.jpg)
Common Ions: Cations (cont’d.)
Name Symbol Function
Cations (cont’d.)Hydrogen
Potassium
Ammonium
H+
K+
NH4+
Important in acid-base balance
Nerve and muscle function
Important in acid-base regulation
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.18
![Page 19: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/19.jpg)
Common Ions: Anions
Name Symbol Function
AnionsChloride
Bicarbonate
Phosphate
Cl−
HCO3−
PO43−
Primary extracellular anion
Important in acid-base regulationComponent of bones and teeth; component of ATP
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.19
![Page 20: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/20.jpg)
Electrolytes and Ionization
• When an electrolyte breaks apart in solution, the electrolyte is said to dissociate or ionize.
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.20
![Page 21: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/21.jpg)
Lesson 2-2 Objectives• Explain the difference between a molecule
and a compound.• List five reasons why water is essential to life.• Explain the role of catalysts and enzymes.
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.21
![Page 22: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/22.jpg)
Lesson 2-2 Objectives (cont’d.)
• Differentiate between an acid and a base.• Define pH.• Define energy and describe the role of
adenosine triphosphate (ATP) in energy transfer.
• Differentiate among mixtures, solutions, suspensions, colloidal suspensions, and precipitates.
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.22
![Page 23: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/23.jpg)
Molecules and Compounds• Molecule: Two
or more atoms bonded together
• Compound: Molecules formed bytwo or more different atoms
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.23
![Page 24: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/24.jpg)
Water: A Vital Substance
• Universal solvent• Temperature regulator• Ideal lubricant• Crucial part of most chemical reactions• Protective mechanism
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.24
![Page 25: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/25.jpg)
Chemical Reactions
• Chemical reaction: The interaction of atoms of molecules or compounds to form new chemical combinations
• Catalysts: Chemical substances that speed up the rate of a chemical reaction
• Enzymes: Proteins that serve as catalysts
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.25
![Page 26: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/26.jpg)
Acids and Bases
• Acid: An electrolyte that dissociates into H+ (hydrogen ion) and an anion
• Base: Substance, often OH- (hydroxyl ion), that combines with H+ to make a solution less acidic
• Acids and bases can be strong or weak
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.26
![Page 27: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/27.jpg)
pH Scale
• pH: Unit of measurement indicating how many hydrogen ions are in a solution
• pH scale: Ranges from 0 to 14
• Midpoint of scale: pH 7, or neutral
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.27
![Page 28: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/28.jpg)
Normal blood pH: 7.35 to 7.45
• Acidosis– Too many H+ ions– pH less than 7.35
• Alkalosis– Too few H+ ions– pH greater than 7.45
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.28
![Page 29: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/29.jpg)
Energy: Ability to Perform Work• Six forms of energy– Mechanical – Chemical – Electrical – Radiant – Thermal – Nuclear
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.29
![Page 30: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/30.jpg)
Energy Transfer
• Adenosine triphosphate (ATP): Energy transfer molecule
• Three parts of ATP– Base– Sugar– Three phosphate groups
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.30
![Page 31: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/31.jpg)
Energy Transfer (cont’d.)
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.31
![Page 32: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/32.jpg)
Energy Transfer (cont’d.)
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.32
![Page 33: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/33.jpg)
Energy Transfer (cont’d.)
• After the food we eat is broken down, energy is released. This energy is transferred to ATP so it can be used by the cells of the body.
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.33
![Page 34: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/34.jpg)
Mixtures
• Mixtures: Combinations of two or more substances that can be separated by ordinary physical means.
• Example: A sugar-iron mixture can be separated by a magnet.
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.34
![Page 35: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/35.jpg)
Solutions
• Solutions have two parts that remain evenly distributed (e.g., normal saline).– Solute: Substance present in smaller amount; is
the substance being dissolved– Solvent: Part of solution present in greater
amount; does the dissolving
• Two types of solutions– Aqueous solutions– Tinctures
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.35
![Page 36: Chapter 002](https://reader036.fdocuments.in/reader036/viewer/2022062312/556ba170d8b42a207e8b4712/html5/thumbnails/36.jpg)
Suspensions and Precipitates
• Suspensions: Mixtures with relatively large particles
• Colloidal suspension: Particles remain suspended within the liquid.
• Precipitates: Solids are formed and fall out of solution during a chemical reaction.
Copyright © 2011, 2007 by Saunders, an imprint of Elsevier Inc. All rights
reserved.36