Life is a chemical process

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1 CHEMISTRY FOR LIFE

2 WHY STUDY CHEMISTRY? Chemistry is the ultimate (basic) cause of all physiological processes Interactions of atoms produce chemical changes Chemical reactions involve a transfer of energy between the compounds Life is a chemical process We are made of many non-living substances reacting with each other to give us all of our characteristics of life Metabolism, growth, reproduction, development, energy use, homeostasis, etc.

3 Understanding the basic principles of chemistry will help you better understand the physical structure of the body as well as the physiological processes that keep us alive 3

4 MATTER Anything that has mass and takes up space.

5 3 states of matter Determined by the amount of Energy in the system

6 LEVELS OF ORGANIZATION IN THE HUMAN BODY The simplest level of organization within the body is the chemical level, which is composed of atoms and molecules. (*Atoms are the smallest units of matter.) 1-6

7 LEVELS OF ORGANIZATION IN THE HUMAN BODY Molecules Two or more atoms combine to form a molecule, such as a protein, a water molecule, or a vitamin. Macromolecules Larger and more complex molecules. 4 main macromolecules: carbohydrates, lipids, proteins and nucleic acids (DNA and RNA). 1-7

8 BUT LET S START FROM THE BEGINNING All matter is made of atoms*. *the simplest particle of an element that retains all the properties of that element.

9 ATOMS OF AN ELEMENT ARE IDENTICAL.

10 THERE ARE DIFFERENT ELEMENTS AND THEIR ATOMS ARE DIFFERENT.

11 Some 60 elements are found in the body, but what all of them are doing is still unknown.

12 Roughly 96% of the mass of the human body is made up of just four elements: oxygen, carbon, hydrogen and nitrogen, with a lot of that in the form of water. (The remaining 4% is a sparse sampling of other elements)

13 MAJOR ELEMENTS OF HUMAN BODY Macroelements Big Four: (by weight) Oxygen 65% Carbon 18.5% Hydrogen 9.5% Nitrogen 3.2% 96% Total of Four Other Elements Ca, P, K, S, Cl, Na, Mg Trace elements: Elements needed in extremely small amounts but still very important Co, Cu, F, I, Fe, Mn, Zn Too much copper (Cu) Wilson Disease Too little copper Menke s Disease Kinky Hair syndrome Too much iron (Fe) hemochromatosis Too little iron anemia

14 Atoms of different elements combine to form molecules. With all these elements floating around, it s important to know a little about the chemistry of our bodies!

15 Property of almost all elements the ability to combine with other elements and form molecules* Hydrogen peroxide H 2 O 2 Glucose C 6 H 12 O 6 *the combination of two or more different kinds of atoms.

16 LAW OF DEFINITE PROPORTIONS A specific molecule always contains the same elements in exactly the same proportions, by mass

17 In a molecule (compound), the different elements lose their individual chemical properties. For example, sodium is an explosive, dangerous substance. Chlorine is a highly poisonous gas. When the two are combined chemically they form sodium chloride, a nonpoisonous substance we commonly sprinkle on our food.

18 Atoms are rearranged in reactions

19 LAW OF CONSERVATION OF MASS Mass is not created or destroyed during a chemical reaction or physical change but it can change form.

20 Compounds and Chemical Formula Compounds often have common names such as water or salt - but are also named by their formula which tell what elements make up the compound and in what proportion. For example, a molecule of water is made up of two hydrogen atoms for every one oxygen atom. H 2 O

21 Compounds are represented by chemical (molecular) formulas 2 Cl Cl 2 2Cl 2 Molecules may also have brackets to indicate numbers of atoms. E.g. Ca(OH) 2 Notice that the OH is a group The 2 refers to both H and O H O Ca O H

22 How many of each atom are in the following? a) NaOH b) Ca(OH) 2 c) 3Ca(OH) 2 Na = 1, O = 1, H = 1 Ca = 1, O = 2, H = 2 Ca = 3, O = 6, H = 6

23 Equations specifically show how the atoms of the compounds rearrange. Remember: Compounds can be written with chemical symbols and subscripts to represent what elements are present, and the number of atoms

24 To write a chemical equation for a reaction, replace the words with the correct molecular formulas and symbols Iron Fe + water H 2 O reacts to form Fe rust 2 O 3 reactants products

25

26 BONDING PREDICTING CHEMICAL INTERACTIONS

27 Atom: A unit of matter, the smallest unit of an element. Element: A substance composed of atoms having an identical number of protons in the nucleus.

28 THE ATOM the smallest particle of an element that still retains the chemical properties of that element

29 ATOMIC STRUCTURE Each atom is made up of smaller parts called protons, electrons and neutrons. Protons and neutrons are found in the central portion of the atom called the nucleus. Electrons are found in orbits or shells at different distances around the nucleus. Protons have a positive (+) electrical charge. Neutrons have no charge (are neutral). Electrons have a (-) negative electric charge.

30 ATOMS ARE NEUTRAL IN CHARGE Atoms are electrically neutral # of protons = # of electrons Proton has total + charge equal in magnitude to the total charge of the electrons.

31 THE NUMBER OF PROTONS DETERMINES AN ATOM S IDENTITY boron carbon nitrogen 5 protons 6 protons 7 protons

32

33 Elements are arranged in the Periodic table based on their atomic number (# of protons) the atomic number identifies the element

34 ELEMENTS, ATOMS, AND MOLECULES Living organisms are composed of about 25 main chemical elements. Trace elements are essential to life, but occur in minute amounts

35 CHNOPS carbon, hydrogen, nitrogen, oxygen, phosphorus and sulfur play the biggest role in living organisms

36 THE REACTIONS/ACTIONS OF ELEMENTS

37 HOW COMPOUNDS FORM -

38 BONDING When an atom shares, gains or loses electrons to achieve an octet by partnering with another atom There are 3 main bond types that are important in the human system: ionic, covalent and hydrogen In ionic bonding one atom steals an electron from a second atom creating oppositely charged atoms In covalent bonding atoms share their electrons to obtain an octet. In hydrogen bonding, molecules form because of polar attractions.

39 Electron arrangement determines the chemical properties of an atom.

40 e - move around the nucleus in specific energy levels There is a max. # of electrons that each energy level can hold.

41 When you look at the Periodic Table, the energy levels of the atoms correspond to the groups (rows) of the table. The two elements in group 1, hydrogen and helium, are filling their first energy level. The eight elements of the second row are filling their second energy level.

42 It is the outermost electrons that determine the chemical properties of the element. (very important)

43

44 *The electrons in the outermost (highest) E level.

45 These outermost electrons are the one s that detect the presence of other atoms and hence the one s involved in bonding. Chemistry of an element depends almost entirely on the number of its valence electrons. (very important)

46

47 Atoms will gain or loose share valence electrons to make a filled (or empty) outer most energy level.

48 Atoms bond to achieve stability reach a stable OCTET Atoms are the most stable when they fill their outermost energy level with 8 electrons*. * Special exception is H and He with only 2 electrons for a full 1 st energy level.

49 Electron affinity as move across the periodic table

50 Gaining or Losing an electron is called ionization An ion is an atom that has either a net positive or net negative charge.

51 Electrons can be pulled out of the valence shell if an element with a larger attractive force* is near. *electron affinity

52 cation

53 ionization When an atom gains or looses an electron, the atom becomes charged what would the charge be on an atom that lost an electron? +1 (because your losing an electron) Gained two electrons? -2 (because you gain 2 electrons)

54 cation An ion is an atom that has either a net positive or net negative charge. anion

55 IONIC BONDING Ionic bonding involves 3 steps (3 energies) 1) loss of an electron(s) by one element, 2) gain of electron(s) by a second element, 3) attraction between positive and negative e 1) 2) Na 3) Cl Na + Na Cl +

56

57

58 The ratio of combining atoms results in a neutral compound Example: sodium and chlorine Na can loose 1 e-, sodium can gain 1 e- and they will both have achieved an octet in their valence shells SO.. They combine in a 1:1 ration and the resulting compound is [Na] + [Cl] - or NaCl What about calcium and fluorine? Calcium looses 2 e-, fluorine only gains 1 e- SO the ratio to get a neutral molecule must be 1 calcium atom: 2 fluorine atoms or CaF 2

59 IONS AND THE OCTET RULE Br I Ne K Ca gain or lose? how many? gain 1 gain 1 none lose lose 1 2 Ion Br P 3 none K 1+ Ca 2+ Elements will ionize (and bond) in order to achieve an octet in their valence shell.

60 3 BIOLOGICALLY IMPORTANT PROPERTIES OF IONIC COMPOUNDS 1. Ionic compounds are soluble in water.

61 In aqueous solution, an ionic compound dissociates into its ions. (eg. when NaCl dissolves in water, the solution contains Na + ions and Cl ions.

62 The dissociated ions in aqueous solution give the solution the ability to conduct electricity.

63 COVALENT BONDS A chemical bond that involves sharing a pair of electrons between neutral atoms in a molecule in order to achieve an octet in the valence shell.

64

65 COVALENT bonds result from a strong interaction between atoms of similar electron affinity. Each atom donates an electron resulting in a pair of electrons that are SHARED between the two atoms

66 Generally, elements with similar electronegativity form covalent bonds

67 Many diatomic molecules are covalently bonded.

68 Atoms can bond forming single, double, triple and even quadruple covalent bonds. ethyne

69 The angles formed between covalently bonded atoms are specific and defined. This means that biological molecules formed with covalent bonds have definite and predicable shapes. (very important) glucose

70 In biological systems, covalent bonds are called strong bonds. This means that they are not normally broken under biological conditions. This is in opposition to weak bonds like ionic bonds which are easily broken under normal biological conditions of temperature and pressure. (very important)

71 Try predicting bonds BONDING WITH YOUR CLASSMATES

72 PREDICTING TYPES OF BONDS How do you predict whether atoms will form ionic or covalent bonds? Notice the location of the elements in the Periodic Table. As a rule, elements on the right (non-metals) share electrons with each other (covalent bonds) and elements on the left tend to donate electrons to elements on the right (ionic bonds).

73 Don t forget when forming compounds, that ions combine in whole number ratios to achieve a neutrally charged compound.

74 One word of warning: hydrogen behaves with a divided personality. While it is traditionally placed in the periodic table above lithium, there are good reasons to put it above fluorine instead (or as well). And remember: As with all generalizations, there are exceptions.

75 Bond with a Classmate

76 POLAR COVALENT BONDS Consider, carbon (C) and chlorine (Cl). Chlorine is clearly to the right of carbon. Carbon is however fairly central. Electrons in a bond between these two elements are shared (covalent), but they are not shared equally. The shared electrons (one from Cl, one from C) would spend more of their time under the influence of chlorine, being farther right, but are not completely lost to carbon (as they would be to sodium).

77 The electrons being shared are held closer to the Cl than to the C giving the molecules slightly charged areas.

78 POLAR AND NON-POLAR COVALENT BONDS There is a type of covalent bond called a polar covalent bond. In human body systems, polar covalent bonds are important because of the unique properties exhibited by molecules with these kinds of bonds.

79 The result of this pattern of unequal electron association is a charge separation in the molecule, where one part of the molecule has a partial negative charge and the other has a partial positive charge. (You should note this molecule is not an ion because there is no exchange of electrons, but there is a simple charge separation in this electrically neutral molecule.)

80 In addition to polar covalent bonds, there are nonpolar covalent bonds. In biological systems, if a molecules has a predominance of nonpolar covalent bonds, that substance is hydrophobic. (very important)

81 The interaction between polar and nonpolar molecules is very important in biological systems.

82 WATER Water is the most abundant molecule in the body. Water forms the internal ocean that baths every cell of the human body. It makes up around 65% of the body weight. The water molecule is composed of one atom of oxygen and two atoms of hydrogen held together by covalent bonds.

83 The shape of the water molecule and the atoms in it give water a special property called polarity. This means that one end of the molecule is slightly positive while the other end is slightly negative.

84 UNIVERSAL SOLVENT The water of the body contains many substances in solution. In a solution one or more substances are dissolved. The dissolved substances are called solutes. The water which dissolves the solutes is called the solvent. Water is so effective at dissolving substances that it is referred to as the universal solvent. Notice how the negative ends of water attract sodium and the positive ends attract chloride.

85 ELECTROLYTES Substances that form ions in solutions are called electrolytes. When electrolytes such as sodium chloride dissolve in water, their ions will conduct electricity through the solution. (A substance such as table sugar will not form ions in solution and will not conduct electricity.) A demonstration in class will allow you to see if a substance is an electrolyte or not.

86 HYDROGEN BONDS

87 Hydrophilic: Hydrophobic: Example: mix salad oil with water shake to break H bonds but as these bonds reform between water molecules, they push the oil molecules out of the way-the oil tends to cluster together in drops or as a layer on the water s surface-thereby exposing less surface area to the water

88 Molecules with a polar/ionized region and one end and a non-polar region at the other end are called amphipathic, as the molecule has both hydrophilic and hydrophobic characteristics. If amphipathic molecules are mixed with water, the molecules form clusters with the polar (hydrophilic) regions at the surface, where they will come into contact with water, and the non-polar (hydrophobic) regions nestled in the center of the cluster away from contact with water. The arrangement will increase the overall solubility in water.

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