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Life and Chemistry: Small Molecules

Life and Chemistry: Small Molecules. Life and Chemistry: Small Molecules. The Mechanistic View of Life Atoms: The Constituents of Matter Chemical Bonds: Linking Atoms Together -------------------------------------------------------- Chemical Reactions: Atoms Change Partners

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Life and Chemistry: Small Molecules

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  1. Life and Chemistry:Small Molecules

  2. Life and Chemistry: Small Molecules • The Mechanistic View of Life • Atoms: The Constituents of Matter • Chemical Bonds: Linking Atoms Together -------------------------------------------------------- • Chemical Reactions: Atoms Change Partners • Water: Structure and Properties • Acids, Bases, and the pH Scale • Properties of Molecules

  3. Mechanistic View of Life The mechanistic view of life: Life is chemically based, and it obeys universal laws of chemistry & physics.

  4. Atoms: The Constituents of Matter • All matter is composed of atoms. • Each atom consists of at least one proton and one electron. • Atoms have mass. The mass comes mostly from the proton and a neutrally charged body called a neutron.

  5. Figure 2.2 The Helium Atom

  6. Atoms: The Constituents of Matter • Each element contains only one type of atom. • Information on elements is arranged in logical order in a table called the periodic table. • The periodic table arranges elements left to right based on their atomic number, and in columns based on similarities in their properties.

  7. Figure 2.3 The Periodic Table (Part 1)

  8. Figure 2.3 The Periodic Table (Part 2)

  9. Atoms: The Constituents of Matter • Each element has a unique atomic number which is the number of protons found in an atom of the element. • The mass number is the number of protons plus the number of neutrons. • The mass number is used as the weight of the atom, in units called daltons. • Each element has a unique symbol: H is hydrogen, C is carbon, Na is sodium, and Fe is iron.

  10. Figure 2.3 The Periodic Table (Part 1)

  11. Atoms: The Constituents of Matter • All atoms of an element have the same number of protons, but not necessarily the same number of neutrons. • Atoms of the same element that have different atomic weights are called isotopes.

  12. Figure 2.4 Isotopes Have Different Numbers of Neutrons

  13. Atoms: The Constituents of Matter • Some isotopes are radioisotopes, which emit energy as alpha, beta, and gamma radiation from their nuclei. • Radioactive decay transforms the original atom into another atom, usually of another element.

  14. Atoms: The Constituents of Matter • The region in which an electron travels is called the electron’s orbital. • The orbitals constitute a series of electron shells, or energy levels, around the nucleus. • Two electrons at most can occupy each orbital.

  15. Atoms: The Constituents of Matter • The first shell is the innermost shell and has just one orbital, called the s orbital. • The s orbital fills first and its electrons have the lowest energy. • The second shell is next closest to the nucleus and has one s and three p orbitals. • The second shell can accommodate eight electrons, two per orbital.

  16. Figure 2.6 Electron Orbitals

  17. Atoms: The Constituents of Matter • The outermost shell of an atom determines how it reacts with other atoms. • Generally, if eight electrons are in the outer shell, the atom is stable and does not tend to react. • Atoms which do not have eight electrons in the outermost shell will share, gain, or lose electrons to arrive at a stable state.

  18. Atoms: The Constituents of Matter • The tendency of atoms to be stable when they have eight electrons in their outermost shells is called the rule of eight, or the octet rule. • Hydrogen and phosphorus are exceptions to the octet rule.

  19. Figure 2.3 The Periodic Table (Part 1)

  20. Chemical Bonds: Linking Atoms Together • A molecule is two or more atoms bonded together. • A chemical bond is an attractive force that links two atoms together.

  21. Chemical Bonds: Linking Atoms Together • A covalent bond is formed by sharing of a pair of electrons between two atoms. • In hydrogen molecules (H2), a pair of electrons share a common orbital and spend equal amounts of time around each of the two nuclei. • The nuclei stay some distance from each other due to mutually repelling positive charges.

  22. Figure 2.8 Electrons Are Shared in Covalent Bonds Properties of Molecules

  23. Chemical Bonds: Linking Atoms Together • Molecules made up of more than one type of atoms are called compounds. • Every compound has a molecular weight that is the sum of all atoms in the molecule.

  24. Chemical Bonds: Linking Atoms Together • Covalent bonds are very strong. • Each covalent bond has a predictable length, angle, and direction, which makes it possible to predict the three-dimensional structures of molecules. • A double covalent bond occurs when atoms share two pairs of electrons; in triple covalent bonds atoms share three electron pairs.

  25. Figure 2.10 Covalent Bonding With Carbon Properties of Molecules

  26. Chemical Bonds: Linking Atoms Together • Electrons are not always shared equally between covalently bonded atoms. • The attractive force that an atom exerts on electrons is called electronegativity. • When a molecule has nuclei with different electronegativities, an electron spends most of its time around the nucleus with the greater electronegativity.

  27. Chemical Bonds: Linking Atoms Together • Unequal sharing of electrons causes a partial negative charge around the more electronegative atom, and a partial positive charge around the less electronegative atom, resulting in a polar covalent bond. • Molecules that have polar covalent bonds are called polar molecules.

  28. Figure 2.11 The Polar Covalent Bond in the Water Molecule Properties of Molecules

  29. Chemical Bonds: Linking Atoms Together • Hydrogen bonds may form within or between atoms with polar covalent bonds. • The d– portion of one molecule has a weak attraction to the d+ portion of another molecule. Each of these attractions is called a hydrogen bond. • Hydrogen bonds do not share electrons. • Although hydrogen bonds are weak, they tend to be additive, and they are of profound biological importance.

  30. Figure 2.12 Hydrogen Bonds Can Form between or within Molecules Properties of Molecules

  31. Chemical Bonds: Linking Atoms Together • Ionic bonds involve a complete transfer of one or more electrons. • Ions are formed when an atom loses or gains electrons. • Positively charged ions are called cations. • Negatively charged ions are called anions.

  32. Figure 2.13 Formation of Sodium and Chloride Ions Properties of Molecules

  33. Chemical Bonds: Linking Atoms Together • Ionic bonds are formed by the electrical attraction between ions with opposite charges. • Table salt has chloride and sodium ions, held together by ionic bonds. • When salt is introduced into water, the partial charges of the water molecules can easily interfere with the ionic bonds.

  34. Figure 2.14 Water Molecules Surround Ions Properties of Molecules

  35. Chemical Bonds: Linking Atoms Together • Polar molecules tend to be hydrophilic. Substances that are ionic or polar often dissolve in water due to hydrogen bonds. • Nonpolar molecules are called hydrophobic because they tend to aggregate with other nonpolar molecules. • Nonpolar molecules are also attracted to each other via relatively weak attractions called van der Waals forces.

  36. End of Part A

  37. Announcements • Survey Form Due Today • Deadline for Online Quiz #1 (Chapter 2) is midnight, September 6 (next Wednesday); handout & demo

  38. Life and Chemistry: Small Molecules • The Mechanistic View of Life • Atoms: The Constituents of Matter • Chemical Bonds: Linking Atoms Together -------------------------------------------------------- • Review: Animation – Electron Shells & Reactivity • Chemical Reactions: Atoms Change Partners • Water: Structure and Properties • Acids, Bases, and the pH Scale • Properties of Molecules

  39. Chemical Reactions: Atoms Change Partners • Chemical reactions occur when atoms combine or change partners. • In a chemical reaction, reactants are converted to products. • A chemical reaction can be written as an equation. The equation must balance because matter is neither created nor destroyed.

  40. Structure of Propane Source: http://kjd.edu-ctr.pref.kanagawa.jp/edb2/chem/models/3d/Propane.jpg

  41. Figure 2.15 Bonding Partners and Energy May Change in a Chemical Reaction Properties of Molecules

  42. What’s to Come? Metabolic Pathways Source: http://www.humboldt.edu/~rap1/BiochSupp/PathwayDiagrams/FolMetPath.gif

  43. Chemical Reactions: Atoms Change Partners • Changes in energy usually accompany chemical reactions. For example, heat and light are released in the propane reaction. • In living cells, it is unusual to have reactions that release light (exceptions: e.g., firefly) • However, heat is a common product in cellular reactions. Why does a corpse have a much lower body temperature than someone who is living? • Also common are changes in potential energy!

  44. Potential Energy • Stored energy, such as that in chemical bonds, is called potential energy and is available for future use. For example, the potential energy in glucose can be used to make ATP. • We can measure the potential energy of molecules and express it in units of heat called calories. • A calorie is the amount of heat required to raise the temperature of one gram of pure water from 14.5°C to 15.5°C.

  45. Figure 2.16 Hydrogen Bonds Hold Water Molecules Together (Part 2) Properties of Molecules

  46. Water: Structure and Properties Due to its shape, polarity, and ability to form hydrogen bonds, water has some unusual properties. • Ice floats in liquid water; normally the solid form of a substance is more dense than the liquid form. • Water has a high specific heat. • Water has a high heat of vaporization.

  47. Figure 2.16 Hydrogen Bonds Hold Water Molecules Together (Part 1) Properties of Molecules

  48. Water: Specific Heat • A great deal of heat energy is required to change the temperature of liquid water because the hydrogen bonds must be broken. • Specific heat is the number of calories needed to raise one gram of a substance 1oC. The specific heat of liquid water is 1. • Liquid water has a higher specific heat than most other small molecules in liquid form.

  49. Water: Structure and Properties • The heat of vaporization is the amount of heat needed to change a substance from its liquid state to its gaseous state. • A lot of heat is required to change water to a gaseous state because the hydrogen bonds of the liquid water must be broken. • Evaporation has a cooling effect by absorbing calories. (Role of sweating and panting.) • Condensing has the opposite effect, releasing heat.

  50. Cohesion and Surface Tension • Source: http://www.npl.co.uk/acoustics/techguides/wetting/images/insect.jpg

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