1. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings PowerPoint Lectures for Biology, Seventh Edition Neil Campbell and Jane Reece Lectures by Chris Romero Chapter 2 The Chemical Context of Life

2. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings Overview: Chemical Foundations of Biology Biology is a multidisciplinary science Living organisms are subject to basic laws of physics and chemistry One example is the bombardier beetle, which uses chemistry to defend itself

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4. 1. Concept 2.1: Matter consists of chemical elements in pure form and in combinations called compounds Organisms are composed of matter Matter is anything that takes up space and has mass Matter is made up of elements

5. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings 1. Elements and Compounds An element is a substance that cannot be broken down to other substances by chemical reactions A compound is a substance consisting of two or more elements in a fixed ratio

6. LE 2-2 SodiumChlorineSodium chloride

7. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings 2.-3. Essential Elements of Life About 25 of the 92 elements are essential to life Carbon, hydrogen, oxygen, and nitrogen make up 96% of living matter Most of the remaining 4% consists of calcium, phosphorus, potassium, and sulfur Trace elements are those required by an organism in minute quantities

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9. LE 2-3 Nitrogen deficiencyIodine deficiency

10. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings Concept 2.2: An element ’ s properties depend on the structure of its atoms Each element consists of unique atoms An atom is the smallest unit of matter that still retains the properties of an element

11. LE 2-4 Nucleus Electrons Cloud of negative charge (2 electrons) 4.

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13. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings 6. Subatomic Particles Atoms are composed of subatomic particles Relevant subatomic particles include: – Neutrons (no electrical charge) – Protons (positive charge) – Electrons (negative charge) Neutrons and protons form the atomic nucleus Electrons form a cloud around the nucleus

14. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings 6. Number and Atomic Mass Atoms of the various elements differ in number of subatomic particles An element’s atomic number is the number of protons An element’s mass number is the sum of protons plus neutrons in the nucleus Atomic mass, the atom’s total mass, can be approximated by the mass number

15. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings 6. Isotopes Atoms of an element have the same number of protons but may differ in number of neutrons Isotopes are two atoms of an element that differ in number of neutrons Most isotopes are stable, but some are radioactive, giving off particles and energy

16. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings Some applications of radioactive isotopes in biological research: – Dating fossils – Tracing atoms through metabolic processes – Diagnosing medical disorders

17. LE 2-6 Cancerous throat tissue

18. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings 6. The Energy Levels of Electrons Energy is the capacity to cause change The electron shell is the electron’s energy level represented as the distance from the nucleus of an atom Electrons are directly involved in chemical reactions

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20. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings 8. – 9. Potential energy is the energy that matter has because of its location or structure The electrons of an atom differ in their amounts of potential energy An electron’s state of potential energy is called its energy level, or electron shell

21. LE 2-7a A ball bouncing down a flight of stairs provides an analogy for energy levels of electrons because the ball can come to rest only on each step, not between steps.

22. LE 2-7b Third energy level (shell) Second energy level (shell) First energy level (shell) Atomic nucleus Energy absorbed Energy lost

23. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings 11. Electron Configuration and Chemical Properties The chemical behavior of an atom is determined by the distribution of electrons in electron shells The periodic table of the elements shows the electron distribution for each element

24. LE 2-8 First shell Hydrogen 1 H Lithium 3 Li Second shell Third shell Sodium 11 Na Beryllium 4 Be Magnesium 12 Mg Boron 5 B Aluminum 12 Al Silicon 14 Si Carbon 6 C Nitrogen 7 N Phosphorus 15 P Oxygen 8 O Sulfur 16 S Chlorine 17 Cl Fluorine 9 F Neon 10 Ne Argon 18 Ar Helium 2 He Atomic number Element symbol Electron-shell diagram Atomic mass 2 He 4.00

25. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings Valence electrons are those in the outermost shell, or valence shell The chemical behavior of an atom is mostly determined by the valence electrons 11-12

26. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings Concept 2.3: The formation and function of molecules depend on chemical bonding between atoms Atoms with incomplete valence shells can share or transfer valence electrons with certain other atoms These interactions usually result in atoms staying close together, held by attractions called chemical bonds

27. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings A molecule consists of two or more atoms held together by covalent bonds A single covalent bond, or single bond, is the sharing of one pair of valence electrons A double covalent bond, or double bond, is the sharing of two pairs of valence electrons Covalent bonds can form between atoms of the same element or atoms of different elements Animation: Covalent Bonds Animation: Covalent Bonds 13.

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29. LE 2-11d Methane (CH 4 ) Name (molecular formula) Electron- shell diagram Structural formula Space- filling model

30. LE 2-11c Water (H 2 O) Name (molecular formula) Electron- shell diagram Structural formula Space- filling model 14.

31. LE 2-11b Oxygen (O 2 ) Name (molecular formula) Electron- shell diagram Structural formula Space- filling model.

32. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings 15. Covalent Bonds A covalent bond is the sharing of a pair of valence electrons by two atoms In a covalent bond, the shared electrons count as part of each atom’s valence shell

33. LE 2-10 Hydrogen atoms (2 H) Hydrogen molecule (H 2 )

34. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings Electronegativity is an atom’s attraction for the electrons in a covalent bond The more electronegative an atom, the more strongly it pulls shared electrons toward itself 16.

35. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings In a nonpolar covalent bond, the atoms share the electron equally In a polar covalent bond, one atom is more electronegative, and the atoms do not share the electron equally 17.

36. LE 2-12 H O H H2OH2O ++ ++ –– 18.

37. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings 19. Ionic Bonds Atoms sometimes strip electrons from their bonding partners An example is the transfer of an electron from sodium to chlorine After the transfer of an electron, both atoms have charges A charged atom (or molecule) is called an ion

38. LE 2-13 Na Sodium atom (an uncharged atom) Cl Chlorine atom (an uncharged atom) Na + Sodium ion (a cation) Cl – Chlorine ion (an anion) Sodium chloride (NaCl) 19.

39. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings Compounds formed by ionic bonds are called ionic compounds, or salts Salts, such as sodium chloride (table salt), are often found in nature as crystals 20.

40. LE 2-14 Na + Cl –

41. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings An anion is a negatively charged ion A cation is a positively charged ion An ionic bond is an attraction between an anion and a cation Animation: Ionic Bonds Animation: Ionic Bonds 21.

42. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings Weak Chemical Bonds Most of the strongest bonds in organisms are covalent bonds that form a cell’s molecules Weak chemical bonds, such as ionic bonds and hydrogen bonds, are also important Weak chemical bonds reinforce shapes of large molecules and help molecules adhere to each other

43. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings 22. Hydrogen Bonds A hydrogen bond forms when a hydrogen atom covalently bonded to one electronegative atom is also attracted to another electronegative atom In living cells, the electronegative partners are usually oxygen or nitrogen atoms

44. LE 2-15 –– Water (H 2 O) Ammonia (NH 3 ) Hydrogen bond ++ ++ –– ++ ++ ++

45. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings 23. Van der Waals Interactions Molecules or atoms that are very close together can be attracted by fleeting charge differences These weak attractions are called van der Waals interactions Collectively, such interactions can be strong, as between molecules of a gecko’s toe hairs and a wall surface

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47. Biological molecules recognize and interact with each other with a specificity based on molecular shape Molecules with similar shapes can have similar biological effects 25.

48. LE 2-17a Natural endorphin Morphine Carbon Hydrogen Nitrogen Sulfur Oxygen Structures of endorphin and morphine

49. LE 2-17b Natural endorphin Morphine Brain cell Endorphin receptors Binding to endorphin receptors

50. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings Concept 2.4: Chemical reactions make and break chemical bonds Chemical reactions lead to new arrangements of atoms The starting molecules of a chemical reaction are called reactants The final molecules of a chemical reaction are called products

51. LE 2-UN44 ReactantsReactionProducts 2 H 2 OO2O2 2 H 2

52. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings Photosynthesis is an important chemical reaction In photosynthesis, sunlight powers the conversion of CO 2 and H 2 0 to glucose (C 6 H 12 O 6 ) and O 2 26.

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54. Some chemical reactions go to completion: All reactants are converted to products Most chemical reactions are reversible: Products of the forward reaction become reactants for the reverse reaction Chemical equilibrium is reached when the forward and reverse reaction rates are equal which is also considered dynamic equilibrium.

55. Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings 28. Dynamic Equilibrium Dynamic equilibrium- reactions are still going on, but with no net effect on concentrations Reactant and products are not equal in concentration Their concentrations have stabilized at a particular ratio Example: Ammonia 3H 2 + N 2 = 2NH 3 Reaches equilibrium when decomposition happens at same rate it forms