1. Basic Chemistry 1 Ch. 2 Outline Ch. 2 Outline Basic Chemistry

2. 2 Chemical Elements Matter:  Anything that has mass and occupies space  Only 92 naturally occurring elements Organisms composed primarily (95%) of only six elements  Carbon, Hydrogen, Nitrogen, Oxygen, Phosphorus, Sulfur  CHNOPS

3. 3 Composition of Earth’s Crust versus Organisms

4. Basic Chemistry 4 Atomic Structure Atoms - Smallest particles of elements Atoms composed of three types of subatomic particles  Protons ­Positive charge ­In nucleus  Neutrons ­Neutral charge ­Also found in nucleus  Electrons ­Negative charge ­Orbit nucleus

5. Basic Chemistry 5 Atomic Symbols Each element represented by unique atomic symbol FFFFirst letter capitalized SSSSuperscripted number: ­R­R­R­Represents mass number ­C­C­C­Count of protons plus count of neutrons SSSSubscripted number: ­R­R­R­Represents atomic number ­N­N­N­Number of protons in nucleus Mass Number Atomic Number Atomic Symbol 12 6 Carbon C

6. Basic Chemistry 6 Periodic Table Elements grouped in periodic table based on characteristics VVVVertical columns = groups; chemically similar 1 H 1.008 3 Li 6.941 11 Na 22.99 19 K 39.10 4 Be 9.012 12 Mg 24.31 20 Ca 40.08 5 B 10.81 13 Al 26.98 21 Ga 69.72 6 C 12.01 14 Si 28.09 22 Ge 72.59 7 N 14.01 15 P 30.97 23 As 74.92 8 O 16.00 16 S 32.07 24 Se 78.96 9 F 19.00 17 Cl 35.45 25 Br 79.90 10 Ne 20.18 18 Ar 39.95 26 Kr 83.60 2 He 4.003 I IIIIIIV VVIVII VIII 1 2 3 4 Groups Periods

7. Basic Chemistry 7IsotopesIsotopes: AAAAtoms of the same element with a differing numbers of neutrons SSSSome isotopes spontaneously decay ­R­R­R­Radioactive ­G­G­G­Give off energy in the form of rays and subatomic particles ­C­C­C­Can be used as tracers ­M­M­M­Mutagenic – Can cause cancer 12 6 Carbon 12 C 13 6 Carbon 13 C 14 6 Carbon 14 C

8. 8 Some Medical Uses for Low Level Radiation

9. 9 Some Medical Uses for High Level Radiation

10. Basic Chemistry 10 Electron Shells, Orbitals and Energy Levels Atoms normally have as many electrons as protons Opposite charges balance leaving atom neutral Electrons are attracted to the positive nucleus  Revolve around nucleus in orbitals  Can be pushed into higher orbitals with energy  Release that energy when they fall back to lower orbital  Different energy levels referred to as electron shells

11. Basic Chemistry 11 The Octet Rule for Distribution of Electrons Bohr models show electron shells as concentric circles around nucleus  Each shell has two or more electron orbitals ­Innermost shell has two orbitals ­Others have 8 or multiples thereof Atoms with fewer than 8 electrons in outermost shell are chemically reactive  If 3 or less – Tendency to donate electrons  If 5 or more – Tendency to receive electrons

12. 12 Bohr Models of Atoms

13. 13 Periodic Table (Revisited) Vertical columns indicate number of electrons in outermost shell 1 H 1.008 3 Li 6.941 11 Na 22.99 19 K 39.10 4 Be 9.012 12 Mg 24.31 20 Ca 40.08 5 B 10.81 13 Al 26.98 21 Ga 69.72 6 C 12.01 14 Si 28.09 22 Ge 72.59 7 N 14.01 15 P 30.97 23 As 74.92 8 O 16.00 16 S 32.07 24 Se 78.96 9 F 19.00 17 Cl 35.45 25 Br 79.90 10 Ne 20.18 18 Ar 39.95 26 Kr 83.60 2 He 4.003 1 2 3 4 Horizontal periods indicate total number of electron shells I II IIIIV V VI VII VIII

14. Basic Chemistry 14 Elements and Compounds Molecule - Two or more atoms bonded together by covalent bonds  If all atoms in molecule are of the same element ­Material is still an element ­O 2, H 2, N 2, etc.  If at least one atom is from a different element ­Material formed is a compound ­CO 2, H 2 O, C 6 H 12 O 6, etc. ­Characteristics dramatically different from constituent elements

15. Basic Chemistry 15 Chemical Bonding Bonds between atoms are caused by electrons in outermost shells The process of bond formation is called a chemical reaction Atoms “want” 8 electrons in outer shell  If have < 4 outers, desire to donate them  If have > 4 outers, desire to receive more

16. Basic Chemistry 16 Types of Bonds: Ionic Bonding Sodium:  Has 1 outer electron Chlorine:  Has 7 outer electrons In reaction, Na completely gives up its outer electron to Cl  Na now a positive ion and Cl a negative ion  Dissimilar charges now bind ions together  Forms sodium chloride ­An ionic compound ­NaCl table salt)

17. 17 Formation of Sodium Chloride

18. Basic Chemistry 18 Types of Bonds: Covalent Bonds When atoms are horizontally closer together in the periodic table  The electrons are not permanently transferred from one atom to the other like in NaCl  A pair of electrons from the outer shell will “time share” with one atom and then the other  This also causes the atoms to remain together  Known as covalent bonding Sometimes two pairs of electrons are shared between atoms – a double covalent bond

19. 19 Covalently Bonded Molecules

20. Basic Chemistry 20 Nonpolar Covalent Bonds Consider two elements that are equidistant from the edges of the periodic table  Atoms will have about equal affinity for electrons  When bonded covalently: ­The bond electrons will spend about equal time with both atoms ­Such covalent bonds are said to be nonpolar

21. Basic Chemistry 21 Polar Covalent Bonds Consider two elements with one much closer to the edge of the table than the other  Atoms will have unequal affinity for electrons  The bond electrons will spend more time with one atom than the other ­The atom that gets the most time with the electrons will be slightly negative ­The other will be slightly positive  Such covalent bonds are said to be polar

22. Basic Chemistry 22 Types of Bonds: Hydrogen Bonds Water (H 2 O or H–O–H) is a polar molecule  Electrons spend more time with O than H’s  H’s become slightly +, O slightly – When polar molecules are dissolved in water  The H’s of water molecules are attracted to the negative parts of the solute molecules  Results in a weak bond – the hydrogen bond  Easily broken, but many together can be quite strong

23. 23 Water Molecule

24. 24 Hydrogen Bonding

25. Basic Chemistry 25 The Chemistry of Water: Heat Capacity Water has a high heat capacity  Temperature = rate of vibration of molecules  Apply heat to liquid ­Molecules bounce faster ­Increases temperature  But, when heat applied to water ­Hydrogen bonds restrain bouncing ­Temperature rises more slowly per unit heat ­Water at a given temp. has more heat than most liquids Thermal inertia – resistance to temperature change  More heat required to raise water one degree than most other liquids (1 calorie per gram)  Also, more heat is extracted/released when lowering water one degree than most other liquids

26. Basic Chemistry 26 Properties of Water: Heat of Vaporization High heat of vaporization  To raise water from 98 to 99 ºC; ~1 calorie  To raise water from 99 to 100 ºC; ~1 calorie  However, large numbers of hydrogen bonds must be broken to evaporate water  To raise water from 100 to 101 ºC; ~540 calories! This is why sweating (and panting) cools  Evaporative cooling is best when humidity is low because evaporation occurs rapidly  Evaporative cooling works poorest when humidity is high because evaporation occurs slowly

27. 27 Evaporative Cooling of Animals

28. Basic Chemistry 28 Properties of Water: Heat of Fusion Heat of fusion (melting)  To raise ice from -2 to -1 ºC; ~1 calorie  To raise water from -1 to 0 ºC; ~1 calorie  To raise water from 0 to 1 ºC; ~80 calories! This is why ice at 0 ºC keeps stuff cold MUCH longer than water at 1 ºC This is why ice is used for cooling  NOT because ice is cold  But because it absorbs so much heat before it will warm by one degree

29. 29 Heat Content of Water at Various Temperatures

30. Basic Chemistry 30 Properties of Water: Water as a Solvent Solutions consist of:  A solvent (the most abundant part) and  A solute (less abundant part) that is dissolved in the solvent Polar compounds readily dissolve; hydrophilic Nonpolar compounds dissolve only slightly; hydrophobic Ionic compounds dissociate in water  Na + ­Attracted to negative (O) end of H 2 O ­Each Na + completely surrounded by H 2 O  Cl - ­Attracted to positive (H 2 ) end of H 2 O ­Each Cl - completely surrounded by H 2 O

31. Basic Chemistry 31 Properties of Water: Uniqueness of Ice Frozen water less dense than liquid water  Otherwise, oceans and deep lakes would fill with ice from the bottom up  Ice acts as an insulator on top of a frozen body of water  Melting ice draws heat from the environment

32. 32 Density of Water at Various Temperatures

33. 33 A Pond in Winter

34. Basic Chemistry 34 Properties of Water: Cohesion & Adhesion  Cohesion – Hydrogen bonds hold water molecules tightly together  Adhesion – Hydrogen bonds for between water and other polar materials  Allows water be drawn many meters up a tree in a tubular vessel High Surface Tension  Water molecules at surface hold more tightly than below surface  Amounts to an invisible “skin” on water surface  Allows small nonpolar objects (like water strider) to sit on top of water

35. 35 Water as a Transport Medium

36. Basic Chemistry 36 pH of Water: Acids Acids  Dissociate in water and release hydrogen ions (H + )  Sour to taste  Hydrochloric acid (stomach acid) is a gas with symbol HCl ­In water, it dissociates into H + and Cl - ­Dissociation of HCl is almost total, therefore it is a strong acid

37. Basic Chemistry 37 pH of Water: Bases Bases:  Either take up hydrogen ions (H + ) or release hydroxide ions (OH - )  Bitter to taste  Sodium hydroxide (drain cleaner) is a solid with symbol NaOH ­In water, it dissociates into Na + and OH - ­Dissociation of NaOH is almost total, therefore it is a strong base

38. Basic Chemistry 38 pH Scale pH scale used to indicate acidity and alkalinity of a solution.  Values range from 0-14 ­0 to <7 = Acidic ­7 = Neutral ­>7 to 14 = Basic (or alkaline)  Logarithmic Scale ­Each unit change in pH represents a change of 10X ­pH of 4 is 10X as acidic as pH of 5 ­pH of 10 is 100X more basic than pH of 8

39. 39 The pH Scale

40. Basic Chemistry 40 Buffers and pH When H + is added to pure water at pH 7, pH goes down and water becomes acidic When OH - is added to pure water at pH 7, pH goes up and water becomes alkaline Buffers are solutes in water that resist change in pH  When H + is added, buffer may absorb, or counter by adding OH -  When OH - is added, buffer may absorb, or counter by adding H +

41. Basic Chemistry 41 Buffers in Biology Health of organisms requires maintaining pH of body fluids within narrow limits  Human blood normally 7.4 (slightly alkaline)  Many foods and metabolic processes add or subtract H + or OH - ions ­Reducing blood pH to 7.0 results in acidosis ­Increasing blood pH to 7.8 results in alkalosis ­Both life threatening situations  Bicarbonate ion ( - HCO 3 ) in blood buffers pH to 7.4