1. Copyright 2010, John Wiley & Sons, Inc. Chapter 2 Introductory Chemistry

2. Copyright 2010, John Wiley & Sons, Inc. Chemical Elements Fundamental unit in chemistry 112 elements total Use 1-2 letter symbols for each  Examples: C= carbon, Na = sodium, Cl = chorine. 26 elements present in human body  4 major ones (O, C, H, and N) make up 96%  8 others significant also. See Table 2.1.

3. Copyright 2010, John Wiley & Sons, Inc. Atoms Smallest unit of an element that retains characteristics of an element Atom contains  Nucleus that has protons (+), neutrons (0)  Electrons (–) surrounding nucleus Total charge is neutral:  Protons # = electron # Atomic number = number of protons = number of electrons Mass number = number of protons + number of neutrons

4. Copyright 2010, John Wiley & Sons, Inc. Ions, Molecules and Compounds When an atom gives up of gains an electron, it becomes an ion When atoms share electrons, they form a molecule Two or more different atoms held together with chemical bonds = a compound Described by the molecular formula

5. Copyright 2010, John Wiley & Sons, Inc. Molecular Formula O 2 = oxygen  Molecule: has 2 atoms bound together H 2 O = water  Molecule has 2 atoms bound together  Compound has 2 different atoms: H (hydrogen): 2 atoms O (oxygen): 1 atom Subscript indicates # of atoms of element

6. Copyright 2010, John Wiley & Sons, Inc. Molecules

7. Copyright 2010, John Wiley & Sons, Inc. Chemical Bonding Attraction between atoms to form attachments Electrons are grouped into shells  Number of electrons in outer shell determines type of bonding Types of bonds:  Ionic  Covalent  Hydrogen

8. Copyright 2010, John Wiley & Sons, Inc. Ionic Bonds Electron is donated or accepted from another atom  ion Typically occurs between atoms in which:  One has just 1 or 2 electrons in outer shells  Other has almost full outer shell (6 or 7 electrons) Electrons are negative (–) so:  If electron is accepted, atom  negative ion: anion  If electron is donated, atom  positive ion: cation Opposite charges attract  ionic bonding

9. Copyright 2010, John Wiley & Sons, Inc. Ionic Bonds

10. Copyright 2010, John Wiley & Sons, Inc. Covalent Bonds Sharing of electrons in outer shell  covalent bonds Typically occurs between atoms in which outer shells are about half full.  Example: bonds involving carbon (C) atoms (with 4 electrons in outer shell). These are organic compounds.  Example: water

11. Copyright 2010, John Wiley & Sons, Inc. Covalent Bonds

12. Copyright 2010, John Wiley & Sons, Inc. Covalent Bonds

13. Copyright 2010, John Wiley & Sons, Inc. Covalent Bonds

14. Copyright 2010, John Wiley & Sons, Inc. Covalent Bonds

15. Copyright 2010, John Wiley & Sons, Inc. Covalent Bonds

16. Copyright 2010, John Wiley & Sons, Inc. Hydrogen Bonds Form when a hydrogen atom (with a partial positive charge) attracts the partial negative charge of neighboring atoms, such as oxygen or nitrogen. Contribute strength and stability within large complex molecules such as  DNA  Proteins

17. Copyright 2010, John Wiley & Sons, Inc. Chemical Reactions Occur when old bonds break and new bonds form Types:  Synthesis  Decomposition  Exchange  Reversible

18. Copyright 2010, John Wiley & Sons, Inc. Chemical Reactions: Synthesis Putting atoms together to form larger molecules A + B  AB Example: 2H 2 + O 2  2 H 2 O Synthesis in the body = anabolism

19. Copyright 2010, John Wiley & Sons, Inc. Chemical Reactions: Decomposition Splitting molecules apart AB  A + B Example: CH 4  C + 2H 2 Decomposition in the body = catabolism

20. Copyright 2010, John Wiley & Sons, Inc. Chemical Reactions: Exchange Involve both synthesis and decomposition AB + CD  AD + BC

21. Copyright 2010, John Wiley & Sons, Inc. Chemical Reactions: Reversible Can go in either direction: synthesis or decomposition or exchange Examples:  A + B ↔ AB  AB ↔ A + B  AB + CD ↔ AD + BC

22. Copyright 2010, John Wiley & Sons, Inc. Classes of Chemicals Inorganic  Structure: lack C-H bonds; structurally simple  Examples Water, carbon dioxide, bicarbonate, acids, bases, and salts Organic  Structure: All contain C-H bonds Structurally complex (include polymers composed of many units = monomers)  Classes: carbohydrates, lipids, proteins, nucleic acids

23. Copyright 2010, John Wiley & Sons, Inc. Inorganic Compounds: Water Characteristics of water  Most abundant chemical in human body  Good solvent and lubricant  Takes part in chemical reactions  Absorbs and releases heat slowly; regulates body temperature  Involved in digestion, circulation, and elimination of wastes

24. Copyright 2010, John Wiley & Sons, Inc. Acids, Bases and Salts Acid dissolves  H + (1 or more) Base dissolves  OH - (1 or more) Acid + base  salt  Example: HCl + NaOH  NaCl + H 2 O acid + base  salt + H 2 O

25. Copyright 2010, John Wiley & Sons, Inc. pH Concept The concentration of H + or OH – expressed on the pH scale pH scale: 0–14 pH 7.0: H + concentration = OH – concentration pH < 7.0 = more H + (acid)  The smaller the number, the more H + pH > 7.0 = more OH – (alkaline)  The larger the number, the more OH –

26. Copyright 2010, John Wiley & Sons, Inc. Organic Compounds Structure  All contain C-H bonds  Structurally complex (include polymers composed of many units = monomers) Classes  Carbohydrates  Lipids  Proteins  Nucleic acids

27. Copyright 2010, John Wiley & Sons, Inc. Carbohydrates Most common sources of energy for humans Three major classes: mono-, di-, poly-  Monosaccharide: simple sugar. Common examples: Glucose (blood sugar) and fructose (fruit sugar)  Disaccharides: two bonded monosaccharides Larger carbohydrates formed by dehydration synthesis and broken down by hydrolysis  Glucose + fructose ↔ sucrose (table sugar)  Glucose + galactose ↔ lactose (milk sugar)  Glucose + glucose ↔ maltose

28. Copyright 2010, John Wiley & Sons, Inc. Carbohydrates

29. Copyright 2010, John Wiley & Sons, Inc. Polysaccharides Monosaccharides (monomers) in long chains  Complex branching structures not usually soluble in water Examples  Glycogen: carbohydrate stored in animals (liver, muscles)  Starch: carbohydrate stored in plants (potatoes, rice, grains)  Cellulose: plant polymer ( indigestible fibers)

30. Copyright 2010, John Wiley & Sons, Inc. Polysaccharides

31. Copyright 2010, John Wiley & Sons, Inc. Lipids Characteristics  Insoluble in water = hydrophobic  Functions: protect, insulate, provide energy Classes  Triglycerides Most plentiful in diet and body Each composed of 3 fatty acids + 1 glycerol May be saturated, monounsaturated, or polyunsaturated  Phospholipids: form lipid bilayer in membranes  Steroids based on ring-structure of cholesterol  Fat-soluble vitamins: A, D, E, and K

32. Copyright 2010, John Wiley & Sons, Inc. Lipids: Triglycerides

33. Copyright 2010, John Wiley & Sons, Inc. Lipids: Phospholipids

34. Copyright 2010, John Wiley & Sons, Inc. Lipids: Steroids

35. Copyright 2010, John Wiley & Sons, Inc. Cholesterol Ring structures similar to cholesterol Used to make steroid hormones  Estrogen, testosterone, cortisone Help make plasma membranes stiff Made in liver

36. Copyright 2010, John Wiley & Sons, Inc. Proteins Structure: composed of amino acids (monomers)  20 different amino acids (like alphabet) Amino acid structure: central carbon with  Acid (carboxyl) group (COOH)  Amino group (NH 2 )  Side chain (varies among the 20 amino acids) Amino acids joined in long chains  By dehydration synthesis to form peptide bonds  dipeptide  tripeptide  polypeptide  Ultimately, form large, complex structures

37. Copyright 2010, John Wiley & Sons, Inc. Amino Acids

38. Copyright 2010, John Wiley & Sons, Inc. Proteins Functions (many)  Much of cell structure  Contraction: muscle fibers  Regulate body: hormones  Transport of O 2 in blood: hemoglobin  Defense: antibodies  Chemical catalysts: enzymes

39. Copyright 2010, John Wiley & Sons, Inc. Enzymes Proteins that serve as chemical catalysts Highly specific: one enzyme works on a specific substrate  product Efficient: one enzyme used over and over Names  Most end in “-ase”  Many give clues to functions: sucrase, lipase, protease, dehydrogenase

40. Copyright 2010, John Wiley & Sons, Inc. Enzymes

41. Copyright 2010, John Wiley & Sons, Inc. Nucleic Acids DNA or RNA Huge polymers composed of nucleotides Each nucleotide (monomer) consists of  Sugar (5-C monosaccharide: ribose or deoxyribose)  Phosphate  Nitrogen-containing (nitrogeneous) base In DNA: adenine (A), guanine (G), cytosine (C), or thymine (T) In RNA: adenine (A), guanine (G), cytosine (C), or uracil (U) (which replaces T of DNA)

42. Copyright 2010, John Wiley & Sons, Inc. DNA Molecule

43. Copyright 2010, John Wiley & Sons, Inc. Nucleic Acids: DNA Nucleotides are connected into long chains that are bonded by bases:  C – G, G – C, T – A, or A – T Two chains form double helix (spiral ladder) Function: stores DNA (genetic information) in genes (found in chromosomes) that:  Direct protein synthesis and therefore regulate everyday activities of cells  Carry this genetic information to the next generation of cells

44. Copyright 2010, John Wiley & Sons, Inc. Nucleic Acid: RNA Nucleotides are connected into a long, single chain (one side of a ladder)  In transcription, RNA (italics) positions next to DNA: C – G, G – C, A - T, or U – A  In translation, t-RNA (italics) positions next to m- RNA (italics): C – G, G – C, A - U, or U - A Function:  Carries out protein synthesis by correctly sequencing amino acids, so helps to regulate everyday activities of cells

45. Copyright 2010, John Wiley & Sons, Inc. ATP Structure: composed of chemicals similar to those in RNA: base (adenine), ribose, and phosphates Function: the main energy-storing molecule in the body  ATP contains 3 phosphates  Carries energy in high-energy chemical bonds between terminal phosphate groups  Energy released from those bonds when they break: ATP  ADP + phosphate + energy

46. Copyright 2010, John Wiley & Sons, Inc. Structure of ATP and ADP

47. Copyright 2010, John Wiley & Sons, Inc. End of Chapter 2 Copyright 2010 John Wiley & Sons, Inc. All rights reserved. Reproduction or translation of this work beyond that permitted in section 117 of the 1976 United States Copyright Act without express permission of the copyright owner is unlawful. Request for further information should be addressed to the Permission Department, John Wiley & Sons, Inc. The purchaser may make back-up copies for his/her own use only and not for distribution or resale. The Publishers assumes no responsibility for errors, omissions, or damages caused by the use of theses programs or from the use of the information herein.