1. How to access School Files 1)Google “ocdsb” 2)Go to the students drop down menu and select “My Docs-Active Directory” 3) Enter student number and password 4)Then choose: Data 1 on “ADLTFS1.ad.osdsb.ca”(X:) 5)Click on “Handout” 6)Scroll down and click “SBI4U”

2. The Chemical Basis of Life Atoms, elements, compounds, & molecules How molecules interact Water is essential for life pH and buffers

3. ELEMENTS, ATOMS, AND MOLECULES Living organisms are composed of matter Matter has mass and occupies space Atom: A unit of matter, the smallest unit of an element.

4. Living organisms are composed of about 25 chemical elements Trace elements – Are essential to life, but occur in minute amounts Element: A substance composed of atoms having an identical number of protons in each nucleus. Elements cannot be reduced to simpler substances by normal chemical means.

5. Carbon, hydrogen, oxygen, and nitrogen Make up the bulk of living matter

6. Trace elements are common additives to food and water Dietary deficiencies in trace elements can cause various physiological conditions

7. Elements can combine to form compounds Chemical elements – Combine in fixed ratios to form compounds Sodium Chlorine Sodium Chloride

8. Subatomic Particles An atom is made up of protons, neutrons and electrons The nucleus contains neutrons and protons and is surrounded by electrons + + –– + – 2 2 2 Protons Neutrons Electrons Mass number = 4 + + 2e – Electron cloud Nucleus Atoms consist of protons, neutrons, and electrons Atom: The smallest particle of matter that still retains the properties of an element

9. Differences in Elements Atoms of each element are distinguished by a specific number of protons + 6 6 6 Protons Neutrons Electrons Mass number = 12 + + 6e – Nucleus Electron cloud 6

10. Isotopes The number of neutrons in an atom may vary Variant forms of an element are called isotopes Some isotopes are radioactive Table 2.4 Radioactive isotopes are useful as tracers for monitoring the fate of atoms in living organisms The half-life of a radioisotope is the time required for half of the atoms in a sample to decay

11. During beta-minus decay, a neutron in an atom's nucleus turns into a proton, an electron and an antineutrino.

12. Medical Diagnosis Radioactive tracers are often used for diagnosis - In combination with sophisticated imaging instruments Research Biologists often use radioactive tracers to follow molecules as they undergo chemical changes in an organism

13. How brain function is studied PET, CAT, MRI, etc. Music Appreciation Hearing, speaking, seeing, thinking about words

14. PET Positron emission tomography (PET) is a nuclear medicine imaging technique which produces a three-dimensional image or picture of functional processes in the body. The system detects pairs of gamma rays emitted indirectly by a positron-emitting radionuclide (tracer), which is introduced into the body on a biologically active molecule

15. PET Scan

16. CT Computed tomography (CT) is a medical imaging method employing tomography created by computer processing. Digital geometry processing is used to generate a three- dimensional image of the inside of an object from a large series of two- dimensional X-ray images taken around a single axis of rotation

17. MRI Magnetic resonance imaging (MRI), or nuclear magnetic resonance imaging (NMRI), is primarily a noninvasive medical imaging technique used in radiology to visualize detailed internal structure and limited function of the body Unlike CT, MRI uses no ionizing radiation. Rather, it uses a powerful magnetic field to align the nuclear magnetization of (usually) hydrogen atoms in water in the body

18. MRI

19. Electron arrangement determines the chemical properties of an atom Electrons in an atom are arranged in shells, which may contain different numbers of electrons Hydrogen (H) Atomic number = 1 Electron Carbon (C) Atomic number = 6 Nitrogen (N) Atomic number = 7 Oxygen (O) Atomic number = 8 Outermost electron shell (can hold 8 electrons) First electron shell (can hold 2 electrons )

20. Atoms whose shells are not full, tend to interact with other atoms Atoms gain, lose, or share electrons These interactions form chemical bonds Electron arrangement

21. Chemical Bonds

22. Types of Bonds 1) Ionic bonds are attractions between ions of opposite charge When atoms gain or lose electrons – Charged atoms called ions are created Transfer of electron Na Sodium atom Cl Chlorine atom Na + Sodium ion Cl – Chloride ion Sodium chloride (NaCl) Na Cl Na + – – –

23. Sodium and chloride ions – Bond to form sodium chloride, common table salt Na + Cl – An electrical attraction between ions with opposite charges – Results in an ionic bond

24. 2) Covalent bonds join atoms into molecules through electron sharing In covalent bonds, two atoms share one or more pairs of outer shell electrons, forming molecules

25. Electronegativity Electronegativity refers to the tendency of an atom to attract electrons in a covalent bond Oxygen (3.5) has a high electronegativity Hydrogen (2.1) and Carbon (2.5) have lower affinities A bond between carbon and hydrogen will have nearly equal sharing of electrons (non polar) A bond between oxygen and hydrogen will be highly polar If the atoms have a large difference in electronegativity (>1.8) then the electron is shared so unevenly that it produces an ionic bond.

26. Electronegativity

27. In a polar covalent bond electrons are shared unequally between atoms, creating a polar molecule (–) (+) O H H

28. 3) Hydrogen Bonds Hydrogen bonds are weak bonds important in the chemistry of life The charged regions on water molecules are attracted to the oppositely charged regions on nearby molecules This attraction forms weak bonds called hydrogen bonds Hydrogen bonding occurs in other biologically important compounds such as proteins and DNA. Hydrogen bond (+) H H (–) O

29. Molecular Shape

30. Shapes of Molecules

31. Water is the solvent of life Polar or charged solutes dissolve when water molecules surround them, forming aqueous solutions + – – – – – – – – – – + + + + + Na + + Cl – Ion in solution Salt crystal Cl – WATER’S LIFE-SUPPORTING PROPERTIES

32. Hydrophobic and Hydrophilic molecules Nonploar molecules do not form hydrogen bonds with water and are ‘excluded’ from associating with water These molecules are said to be hydrophobic Hydrophobic molecules such as oxygen require carrier proteins for transportation in the body Polar molecules can form hydrogen bonds with water and are said to be hydrophilic

33. Cell Membrane

34. WATER’S LIFE-SUPPORTING PROPERTIES Hydrogen bonds make liquid water cohesive Due to hydrogen bonding – Water molecules can move from a plant’s roots to its leaves by adhesion Insects can walk on water due to surface tension Created by cohesive water molecules

35. Water’s hydrogen bonds moderate temperature Water’s ability to store heat – Moderates body temperature and climate It takes a lot of energy to disrupt hydrogen bonds - So water is able to absorb a great deal of heat energy without a large increase in temperature As water cools - A slight drop in temperature releases a large amount of heat WATER’S LIFE-SUPPORTING PROPERTIES

36. Liquid water Hydrogen bonds constantly break and re-form Ice Hydrogen bonds are stable Hydrogen bond Figure 2.13 Ice is less dense than liquid water Hydrogen bonds hold molecules in ice farther apart than in liquid water Ice is therefore less dense than liquid water which causes it to float Floating ice protects lakes and oceans from freezing solid

37. The chemistry of life is sensitive to acidic and basic conditions A compound that releases H + ions in solution is an acid And one that accepts H + ions in solution is a base Acidity is measured on the pH scale from 0 (most acidic) to 14 (most basic or alkaline)

38. The pH scale Basic solution Oven cleaner Acidic solution Neutral solution pH scale 0 1 2 3 4 5 6 7 8 9 10 11 12 Lemon juice, gastric juice Grapefruit juice, soft drink Tomato juice Human urine Pure water Human blood Seawater Milk of magnesia Household ammonia Household bleach Increasingly ACIDIC (Higher concentration of H + ) NEUTRAL [H + ]=[OH – ] H+H+ H+H+ H+H+ OH – H+H+ H+H+ H+H+ H+H+ H+H+ H+H+ H+H+ H+H+ H+H+ H+H+ H+H+ Increasingly BASIC (Lower concentration of H + ) OH – H+H+ 14 13 Figure 2.15 The pH of most cells Is kept close to 7 (neutral) by buffers Buffers are substances that resist pH change

39. Acid precipitation threatens the environment Some ecosystems are threatened by acid precipitation Acid precipitation is formed when air pollutants from burning fossil fuels combine with water vapor in the air to form sulfuric and nitric acids Can kill trees and damage buildings

40. Acid, Bases and Buffers Ionization of Water in pure water the concentration of the hydronium ion is 1.0x10 -7 mol/L the pH is defined as the negative logarithm of the hydronium ion concentration In pure water the pH=-log1.0x10-7 = 7

41. Strong Acids and Bases Strong acids and bases completely ionize in water

42. Weak Acids and Bases Ionize partially in water

43. Weak Base 10% ionization

44. Buffers a chemical system containing a substance that can donate H + ions when required or remove H + when too many are in solution therefore resist changes in pH