Essential Chemistry for Biology

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Chapter 2 Essential Chemistry for Biology Lectures

and Jean Dickey Campbell Essential Biology with

1 Chapter 2 Essential Chemistry for Biology Lectures by Chris C. Romero, updated by Edward J. Zalisko PowerPoint Lectures for Campbell Essential Biology, Fourth Edition Eric Simon, Jane Reece, and Jean Dickey Campbell Essential Biology with Physiology, Third Edition Eric Simon, Jane Reece, and Jean Dickey

2 Biology and Society: Fluoride in the Water Fluoride Is a common ingredient in Earth s crust Helps maintain healthy teeth Fluoride prevents cavities by Affecting the metabolism of oral bacteria Promoting the replacement of lost minerals on the tooth surface

3 SOME BASIC CHEMISTRY Take any biological system apart, and you eventually end up at the chemical level.

4 Matter: Elements and Compounds Matter is anything that occupies space and has mass. Matter is found on the Earth in three physical states: Solid Liquid Gas

substances. There are 92 naturally occurring elements on Earth.

5 Matter is composed of chemical elements. Elements are substances that cannot be broken down into other substances. There are 92 naturally occurring elements on Earth. All of the elements are listed in the periodic table. Mercury Hg Copper Cu Lead Pb

H Rb K Na Li Fr Cs Sr Ca Mg Be Ra Ba Y Sc Ac La Zr Ti Rf Hf Nb V Db Ta Mo Cr Sg W Tc Mn Bh Re Ru Fe Hs Os Rh Co Mt Ir Pd Ni Uun Pt Xe Kr Uuo Rn Ag Cu Uuu Au Cd Zn Uub Hg Ar Ne In Ga Tl Al B Sn Ge Uuq

6 H Rb K Na Li Fr Cs Sr Ca Mg Be Ra Ba Y Sc Ac La Zr Ti Rf Hf Nb V Db Ta Mo Cr Sg W Tc Mn Bh Re Ru Fe Hs Os Rh Co Mt Ir Pd Ni Uun Pt Xe Kr Uuo Rn Ag Cu Uuu Au Cd Zn Uub Hg Ar Ne In Ga Tl Al B Sn Ge Uuq Pb Si C Sb As Bi P N Te Se Uuh Po S O I Br At Cl F He Th Ce Pa Pr U Nd Np Pm Pu Sm Am Eu Lr Lu Cm Gd Bk Tb Cf Dy Es Ho Fm Er Md Tm No Yb 6 C 12 Figure 2.1 Atomic number (number of protons) Atomic mass (number of protons + neutrons)

7 Twenty-five elements are essential to life. Four elements make up about 96% of the weight of the human body: Oxygen Carbon Hydrogen Nitrogen

8 Carbon C : 18.5% Hydrogen H : 9.5% Nitrogen N : 3.3% Oxygen O : 65.0% Calcium Ca : 1.5% Phosphorus P : 1.0% Potassium K : 0.4% Sulfur S : 0.3% Sodium Na : 0.2% Chlorine Cl : 0.2% Magnesium Mg : 0.1% Trace elements: less than 0.01% Boron B Manganese Mn Chromium Cr Molybdenum Mo Cobalt Co Selenium Se Copper Cu Silicon Si Fluorine F Tin Sn Iodine I Vanadium V Iron Fe Zinc Zn Figure 2.2

9 Trace elements Required in smaller amounts Are essential for life An iodine deficiency causes goiter.

10 Elements can combine to form compounds. Compounds are substances that contain two or more elements in a fixed ratio. Common compounds include NaCl (table salt) H 2 O (water)

11 Atoms Each element consists of one kind of atom. An atom is the smallest unit of matter that still retains the properties of an element.

12 The Structure of Atoms Atoms are composed of subatomic particles. A proton is positively charged. An electron is negatively charged. A neutron is electrically neutral. Atoms do not have any charge

13 2 2 2 Protons Neutrons Electrons Nucleus Nucleus Cloud of negative charge 2 electrons Figure 2.4

14 Most atoms have protons and neutrons packed tightly into the nucleus. The nucleus is the atom s central core. Electrons orbit the nucleus.

15 Elements differ in the number of subatomic particles in their atoms. The number of protons, the atomic number, determines which element it is. An atom s mass number is the sum of the number of protons and neutrons. Mass is a measure of the amount of matter in an object.

16 Isotopes Isotopes are alternate mass forms of an element. Isotopes have the same number of protons and electrons, but they have a different number of neutrons.

17 Table 2.1

18 The nucleus of a radioactive isotope decays, giving off particles and energy. Radioactive isotopes have many uses in research and medicine. They can be used to determine the fate of atoms in living organisms. They are used in PET scans to diagnose heart disorders and some cancers.

19 Uncontrolled exposure to radioactive isotopes can harm living organisms by damaging DNA. The 1986 Chernobyl nuclear accident released large amounts of radioactive isotopes. Naturally occurring radon gas may cause lung cancer.

20 Electron Arrangement and the Chemical Properties of Atoms Electrons determine how an atom behaves when it encounters other atoms. Electrons orbit the nucleus of an atom in specific electron shells. The farther an electron is from the nucleus, the greater its energy. The number of electrons in the outermost shell determines the chemical properties of an atom.

21 Electron First electron shell can hold 2 electrons Outer electron shell can hold 8 electrons Hydrogen H Atomic number = 1 Carbon C Atomic number = 6 Nitrogen N Atomic number = 7 Oxygen O Atomic number = 8 Figure 2.5

22 Chemical Bonding and Molecules Chemical reactions enable atoms to give up or acquire electrons to complete their outer shells. Chemical reactions usually result in atoms Staying close together Being held together by chemical bonds

23 Ionic Bonds When an atom loses or gains electrons, it becomes electrically charged. Charged atoms are called ions. Ionic bonds are formed between oppositely charged ions. Animation: Ionic Bonds

24 Electron transfer and ionic bonding Outer shell has 1 electron The outer electron is stripped from sodium and completes the chlorine atom s outer shell Outer shell has 7 electrons Na Sodium atom Cl Chlorine atom Figure 2.6-1

25 Electron transfer and ionic bonding Outer shell has 1 electron The outer electron is stripped from sodium and completes the chlorine atom s outer shell Outer shell has 7 electrons Complete outer shells Na Sodium atom Cl Chlorine atom Na Sodium ion Cl Chlorine ion Sodium chloride (NaCl) The attraction between the ions an ionic bond holds them together Figure 2.6-2

26 Covalent Bonds A covalent bond forms when two atoms share one or more pairs of outer-shell electrons. Atoms held together by covalent bonds form a molecule. The number of covalent bonds an atom can form is equal to the number of additional electrons needed to fill its outer shell. Blast Animation: Covalent Bonds Animation: Covalent Bonds

27 Name molecular formula Hydrogen gas H 2 Electron configuration Structural formula Space-filling model Ball-and-stick model Single bond a pair of shared electrons Oxygen gas O 2 Double bond two pairs of shared electrons Methane CH 4 Figure 2.7

28 Concept Check The reactive properties (chemical behavior) of an atom mostly depend on the number of a) electrons in each electron shell of the atom. b) neutrons found in the nucleus. c) filled electron shells. d) electrons in the outer electron shell of the atom.

29 Hydrogen Bonds Water is a compound in which the electrons in its covalent bonds are shared unequally. This causes water to be a polar molecule, one with opposite charges on opposite ends. Blast Animation: Hydrogen Bonds in Water Animation: Water Structure

30 slightly slightly H H O slightly Figure UN2-2

31 The polarity of water results in weak electrical attractions between neighboring water molecules. These interactions are called hydrogen bonds.

32 Hydrogen bond Figure 2.8

33 Concept Check Water molecules form hydrogen bonds because a) the water molecule is polar. b) the oxygen molecule is positively charged. c) the water molecule forms a tetrahedron. d) the hydrogen atoms are negatively charged.

34 Chemical Reactions Cells constantly rearrange molecules by breaking existing chemical bonds and forming new ones. Such changes in the chemical composition of matter are called chemical reactions.

35 Chemical reactions include Reactants, the starting materials Products, the end materials

36 2 H 2 H 2 O 2 O 2 Hydrogen gas Oxygen gas Water Reactants Products Figure UN2-3

37 Chemical reactions can rearrange matter but cannot create or destroy matter.

38 Interpreting Data This is the general equation for photosynthesis the process of capturing sunlight energy and converting it to chemical energy. Which of the following are the reactants of this reaction? a) C 6 H 12 O 6 and O 2 b) CO 2 and H 2 O

39 WATER AND LIFE Life on Earth began in water and evolved there for 3 billion years. Modern life remains tied to water. Your cells are composed of 70% 95% water. The abundance of water is a major reason Earth is habitable.

40 Water s Life-Supporting Properties The polarity of water molecules and the hydrogen bonding that results explain most of water s life-supporting properties. Water molecules stick together. Water has a strong resistance to change in temperature. Frozen water floats. Water is a common solvent for life.

41 The Cohesion of Water Water molecules stick together as a result of hydrogen bonding. This is called cohesion. Cohesion is vital for water transport in plants. Animation: Water Transport

42 SEM Evaporation from the leaves Microscopic tubes Cohesion due to hydrogen bonds between water molecules Figure 2.10

43 Surface tension is the measure of how difficult it is to stretch or break the surface of a liquid. Hydrogen bonds give water an unusually high surface tension.

44 How Water Moderates Temperature Because of hydrogen bonding, water has a strong resistance to temperature change. Heat and temperature are related, but different. Heat is the amount of energy associated with the movement of the atoms and molecules in a body of matter. Temperature measures the intensity of heat. Water can absorb and store large amounts of heat while only changing a few degrees in temperature.

45 Water can moderate temperatures. Earth s giant water supply causes temperatures to stay within limits that permit life. Evaporative cooling removes heat from the Earth and from organisms.

46 The Biological Significance of Ice Floating When water molecules get cold enough, they move apart, forming ice. A chunk of ice has fewer molecules than an equal volume of liquid water. Ice floats because it is less dense than the liquid water around it.

47 Hydrogen bond Liquid water Ice Figure 2.13

48 If ice did not float, ponds, lakes, and even the oceans would freeze solid. Life in water could not survive if bodies of water froze solid.

49 Water as the Solvent of Life A solution is a liquid consisting of a homogeneous mixture of two or more substances. The dissolving agent is the solvent. The dissolved substance is the solute. When water is the solvent, the result is an aqueous solution.

50 Sodium ion in solution Salt crystal Cl Na Na Cl Chloride ion in solution Figure 2.14

51 Acids, Bases, and ph A chemical compound that releases H + to solution is an acid. A compound that accepts H + and removes it from solution is a base. To describe the acidity of a solution, chemists use the ph scale.

52 Increasingly acidic greater H concentration Increasingly basic lower H concentration Each ph unit represents a tenfold change in the concentration of H +. Lemon juice, ph 2 has 100 times more of H + than tomato juice at ph 4 Basic solution Neutral [H + ] [OH ] 14 Oven cleaner 13 Household bleach 12 Household ammonia 11 Milk of magnesia Seawater Human blood Pure water Neutral solution 6 5 Urine 4 Tomato juice Acidic solution ph scale Grapefruit juice, soft drink Lemon juice, gastric juice Figure 2.16

53 Basic solution Neutral solution Acidic solution Figure 2.16a

54 Buffers are substances that resist ph change. Buffers Accept H + ions when they are in excess Donate H + ions when they are depleted Increases in global CO 2 concentrations may lead to the acidification of the oceans.

55 Evolution Connection: The Search for Extraterrestrial Life If life similar to ours has evolved elsewhere in the universe, then it too would depend upon water. Recent NASA missions to Mars have detected evidence that liquid water flowed over the planet s surface.

Essential Chemistry for Biology

1 Chapter 2 Essential Chemistry for Biology Biology and Society: More Precious than Gold A drought is a period of abnormally dry weather that changes the environment and one of the most devastating disasters.