W2. Chemical structures of protein and DNA

Transcription

1 W2. Chemical structures of protein and DNA Copyright Kang, Lin-Woo, Ph.D. Professor Department of Biological Sciences Konkuk University Seoul, Korea Lectures prepared by Christine L. Case

2 The Structure of Atoms Chemistry is the study of interactions between atoms and molecules The atom is the smallest unit of matter that enters into chemical reactions Atoms interact to form molecules

3 The Structure of Atoms Atoms are composed of Electrons: negatively charged particles Protons: positively charged particles Neutrons: uncharged particles

4 The Structure of Atoms Protons and neutrons are in the nucleus Electrons move around the nucleus

5 Figure 2.1 The structure of an atom. Electron shells Nucleus Proton (p + ) Neutron (n 0 ) Insert Fig 2.1 Electron (e ).

6 Chemical Elements Each chemical element has a different number of protons Isotopes of an element are atoms with different numbers of neutrons. Isotopes of oxygen: 16 O O O 8 8 8

7 Electronic Configurations Electrons are arranged in electron shells corresponding to different energy levels

8 Table 2.1 The Elements of Life Insert Table 2.1

9 How Atoms Form Molecules Atoms combine to complete the outermost shell The number of missing or extra electrons in this shell is known as the valence Molecules hold together because the valence electrons of the combining atoms form attractive forces, called chemical bonds, between the atomic nuclei

10 Chemical Bonds A compound contains different kinds of atoms H 2 O

11 Ionic Bonds The number of protons and electrons is equal in an atom Ions are charged atoms that have gained or lost electrons

12 Figure 2.2a Ionic bond formation. Loss of electron Gain of electron Sodium atom (electron donor) Sodium ion (Na + ) Chlorine atom (electron acceptor) Chloride ion (Cl ) A sodium atom (Na) loses one electron to an electron acceptor and forms a sodium ion (Na + ). A chlorine atom (Cl) accepts one electron from an electron donor to become a chloride ion (Cl ).

13 Ionic Bonds Ionic bonds are attractions between ions of opposite charge One atom loses electrons, and another gains electrons

14 Figure 2.2b Ionic bond formation. Sodium ion (Na + ) Chloride ion (Cl ) Insert Fig 2.2b Sodium chloride molecule Na + Cl NaCl The sodium and chloride ions are attracted because of their opposite charges and are held together by an ionic bond to form a molecule of sodium chloride.

15 Covalent Bonds Covalent bonds form when two atoms share one or more pairs of electrons

16 Figure 2.3a Covalent bond formation. Diagram of Atomic Structure Structural Formula Molecular Formula Insert Fig 2.3a or Hydrogen atom Hydrogen atom Hydrogen molecule A single covalent bond between two hydrogen atoms.

17 Figure 2.3b Covalent bond formation. Diagram of Atomic Structure Structural Formula Molecular Formula or Carbon atom Hydrogen atoms Insert Fig 2.3b Methane molecule Single covalent bonds between four hydrogen atoms and a carbon atom, forming a methane molecule.

18 Hydrogen Bonds Hydrogen bonds form when a hydrogen atom that is covalently bonded to an O or N atom is attracted to another N or O atom in another molecule

19 Figure 2.4b Hydrogen bond formation in water. Hydrogen bond Insert Fig 2.4b

20 Molecular Weight and Moles The sum of the atomic weights in a molecule is the molecular weight One mole of a substance is its molecular weight in grams H 2 O 2H = 2 1 = 2 O = 16 MW = 18 1 mole weighs 18 g

21 Chemical Reactions Chemical reactions involve the making or breaking of bonds between atoms A change in chemical energy occurs during a chemical reaction Endergonic reactions absorb energy Exergonic reactions release energy

22 Synthesis Reactions Occur when atoms, ions, or molecules combine to form new, larger molecules A + B AB Atom, ion, or molecule A Atom, ion, or molecule B Combines to form New molecule AB Anabolism is the synthesis of molecules in a cell

23 Decomposition Reactions Occur when a molecule is split into smaller molecules, ions, or atoms AB New molecule AB Breaks down into A + B Atom, ion, or molecule A Atom, ion, or molecule B Catabolism is the decomposition reactions in a cell

24 Exchange Reactions Are part synthesis and part decomposition NaOH + HCl NaCl + H 2 O

25 Reversible Reactions Can readily go in either direction Each direction may need special conditions Heat A + B AB Water

26 Important Biological Molecules Organic compounds always contain carbon and hydrogen Inorganic compounds typically lack carbon

27 Water Inorganic Polar molecule Solvent Polar substances dissociate, forming solutes

28 Figure 2.4a Hydrogen bond formation in water. Insert Fig 2.4a

29 Figure 2.5 How water acts as a solvent for sodium chloride (NaCl). Sodium ion Insert dissolved Fig 2.5 in water Sodium chloride crystal Chloride ion dissolved in water

30 Water H + and OH participate in chemical reactions R R + H 2 O R OH + H R Maltose + H 2 O Glucose + Glucose

31 Water Maltose + H 2 O Glucose + Glucose Glucose C 6 H 12 O 6 Glucose +C 6 H 12 O 6 Total C 12 H 24 O 12 Maltose C 12 H 22 O 11 The difference is:

32 Water H bonds absorb heat Makes water a temperature buffer

33 Figure 2.4b Hydrogen bond formation in water. Hydrogen bond Insert Fig 2.4b

34 Figure 2.6 Acids, bases, and salts. HCl NaOH NaCl Insert Fig 2.6 Acid Base Salt

35 Acids Substances that dissociate into one or more H + HCl H + + Cl

36 Figure 2.6a Acids, bases, and salts. HCl Insert Fig 2.6a Acid

37 Bases Substances that dissociate into one or more OH NaOH Na + + OH

38 Figure 2.6b Acids, bases, and salts. NaOH Insert Fig 2.6b Base

39 Salts Substances that dissociate into cations and anions, neither of which is H + or OH NaCl Na + + Cl

40 Figure 2.6c Acids, bases, and salts. NaCl Insert Fig 2.6c Salt

41 Acid-Base Balance The amount of H + in a solution is expressed as ph ph = log[h + ] Increasing [H + ] increases acidity Increasing [OH ] increases alkalinity Most organisms grow best between ph 6.5 and 8.5

42 Figure 2.7 The ph scale. ph scale Stomach acid Lemon juice Acidic solution Grapefruit juice Wine Tomato juice Neutral solution Insert Fig 2.7 Urine Milk Pure water Human blood Seawater Basic solution Milk of magnesia Household ammonia Household bleach Oven cleaner Limewater

43 Structure and Chemistry The chain of carbon atoms in an organic molecule is the carbon skeleton

44 Structure and Chemistry Functional groups are responsible for most of the chemical properties of a particular organic compound

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46 Table 2.4 Representative Functional Groups and the Compounds in Which They Are Found (Part 1 of 2) Insert Table 2.4 (two slides if possible)

47 Table 2.4 Representative Functional Groups and the Compounds in Which They Are Found (Part 2 of 2) Insert Table 2.4 (two slides if possible)

48 Functional Groups Identify the functional groups in an amino acid

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50 Organic Compounds Small organic molecules can combine into large macromolecules Macromolecules are polymers consisting of many small repeating molecules The smaller molecules are called monomers

51 Polymers Monomers join by dehydration synthesis or condensation reactions

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53 Carbohydrates Cell structures and energy sources Consist of C, H, and O with the formula (CH 2 O) n Monosaccharides are simple sugars with three to seven carbon atoms

54 Carbohydrates Disaccharides are formed when two monosaccharides are joined in a dehydration synthesis Disaccharides can be broken down by hydrolysis

55 Figure 2.8 Dehydration synthesis and hydrolysis. Dehydration synthesis Insert Fig 2.8 Glucose C 6 H 12 O 6 Fructose C 6 H 12 O 6 Hydrolysis Sucrose C 12 H 22 O 11 Water

56 Carbohydrates Oligosaccharides consist of 2 to 20 monosaccharides Polysaccharides consist of tens or hundreds of monosaccharides joined through dehydration synthesis Starch, glycogen, dextran, and cellulose are polymers of glucose that are covalently bonded differently Chitin is a polymer of two sugars repeating many times

57 Lipids Primary components of cell membranes Consist of C, H, and O Are nonpolar and insoluble in water

58 Simple Lipids Fats or triglycerides Contain glycerol and fatty acids; formed by dehydration synthesis

59 Simple Lipids Saturated fat: no double bonds Unsaturated fat: one or more double bonds in the fatty acids Cis: H atoms on the same side of the double bond Trans: H atoms on opposite sides of the double bond

60 Figure 2.9c Structural formulas of simple lipids. Ester linkage Palmitic acid (C 15 H 31 COOH) + (saturated) H 2 O Stearic acid (C 17 H 35 COOH) + (saturated) H 2 O cis configuration Molecule of fat (triglyceride) (triglyceride) Oleic acid (C 17 H 33 COOH) + (unsaturated) H 2 O

61 Complex Lipids Contain C, H, and O + P, N, or S Membranes are made of phospholipids

62 Figure 2.9ab Structural formulas of simple lipids. Carboxyl group Hydrocarbon chain Insert Fig 2.9a Fatty acid (palmitic acid), C 15 H 31 COOH Glycerol

63 Steroids Four carbon rings with an OH group attached to one ring Part of membranes

64 Figure 2.11 Cholesterol, a steroid. Insert Fig 2.11

65 Proteins Are essential in cell structure and function Enzymes are proteins that speed chemical reactions Transporter proteins move chemicals across membranes Flagella are made of proteins Some bacterial toxins are proteins

66 Amino Acids Proteins consist of subunits called amino acids

67 Figure 2.12 Amino acid structure. Amino group Side group Cyclic side group Insert Fig 2.12 Carboxyl group Generalized amino acid Tyrosine

68 Amino Acids Exist in either of two stereoisomers: D or L L-forms are most often found in nature

69 Figure 2.13 The L- and D-isomers of an amino acid, shown with ball-and-stick models. Mirror L-amino acid D-amino acid Insert Fig 2.13 Left hand Right hand

70 Peptide Bonds Peptide bonds between amino acids are formed by dehydration synthesis

71 Figure 2.14 Peptide bond formation by dehydration synthesis. Peptide bond Dehydration synthesis Insert Fig 2.14 Glycine Alanine Glycylalanine (a dipeptide) Water

72 Levels of Protein Structure The primary structure is a polypeptide chain

73 Figure 2.15a Protein structure. Peptide bonds (a) Primary structure: polypeptide strand

74 Levels of Protein Structure The secondary structure occurs when the amino acid chain folds and coils in a regular helix or pleats

75 Figure 2.15b Protein structure. (b) Secondary structure: helix and pleated sheets (with three polypeptide strands) Helix Insert Fig 2.15b Hydrogen bond Pleated sheet Disulfide bridge

76 Levels of Protein Structure The tertiary structure occurs when the helix folds irregularly, forming disulfide bridges, hydrogen bonds, and ionic bonds between amino acids in the chain

77 Figure 2.15c Protein structure. Hydrophobic interaction Hydrogen bond (c) Tertiary structure: folded helix and pleated sheet Insert Fig 2.15c Disulfide bridge (between cysteine molecules) Ionic bond Polypeptide strand Details of bonds associated with tertiary structure

78 Levels of Protein Structure The quaternary structure consists of two or more polypeptides

79 Figure 2.15d Protein structure. Insert Fig 2.15d (d) Quaternary structure: two or more polypeptides in their folded states

80 Figure 2.15 Protein structure. Peptide bonds (a) Primary structure: polypeptide strand Hydrogen bond (b) Secondary structure: helix and pleated sheets (with three polypeptide strands) Helix Pleated sheet Insert Fig 2.15a Hydrophobic interaction (c) Tertiary structure: folded helix and pleated sheet Disulfide bridge Hydrogen bond Disulfide bridge (between cysteine molecules) Polypeptide strand (d) Quaternary structure: two or more polypeptides in their folded states Ionic bond Details of bonds associated with tertiary structure

81 Levels of Protein Structure Conjugated proteins consist of amino acids and other organic molecules Glycoproteins Nucleoproteins Lipoproteins

82 Nucleic Acids Consist of nucleotides Nucleotides consist of Pentose Phosphate group Nitrogen-containing (purine or pyrimidine) base Nucleosides consist of Pentose Nitrogen-containing base

83 DNA Deoxyribonucleic acid Has deoxyribose Exists as a double helix A hydrogen bonds with T C hydrogen bonds with G

84 Figure 2.16 The Structure of DNA. Adenine and Thymine (as well as Cytosine and Guanine, not shown here) are nitrogenous bases or nucleobases. Phosphate Sugar Adenine (A) Thymine (T) Sugar Phosphate Adenine nucleotide Hydrogen bonds Thymine nucleotide Individual DNA nucleotides are composed of a deoxyribose sugar molecule covalently bonded to a phosphate group at the 5 carbon, and to a nitrogen-containing base at the 3 carbon. The two nucleotides shown here are held together by hydrogen bonds. Sugar-phosphate backbone The sugar-phosphate backbone of one strand is upside down, or antiparallel, relative to the backbone of the other strand. Insert Fig 2.16 Sugars Phosphates The carbon atoms in the sugars are identified by adding a marker, (for example, 5, pronounced 5-prime ). This differentiates them from the carbon atoms in the nucleobases, such as Thymine. DNA double helix DNA s double-helical, ladderlike form is made up of many nucleotides base pairs forming the rungs, and the repeating sugar-phosphate combination, forming the backbone.

85 RNA Ribonucleic acid Has ribose Is single-stranded A hydrogen bonds with U C hydrogen bonds with G

86 Figure 2.17 A uracil nucleotide of RNA. Uracil (U) Phosphate Insert Fig 2.17 Ribose

87 ATP Adenosine triphosphate Has ribose, adenine, and three phosphate groups

88 Figure 2.18 The structure of ATP. Adenosine Adenine Phosphates Insert Fig 2.18 Ribose

89 ATP Is made by dehydration synthesis Is broken by hydrolysis to liberate useful energy for the cell

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