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STRENGTH

STRENGTH. “Do not pray for easy lives. Pray to be stronger men! Do not pray for tasks equal to your powers. Pray for power equal to your tasks." -Phillips Brooks. CHAPTER 2. The Chemical basis of Life. Matter. Anything that occupies space and has mass. Can exist as: ____________

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STRENGTH

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  1. STRENGTH “Do not pray for easy lives. Pray to be stronger men! Do not pray for tasks equal to your powers. Pray for power equal to your tasks." -Phillips Brooks

  2. CHAPTER 2 The Chemical basis of Life

  3. Matter • Anything that occupies space and has mass. • Can exist as: • ____________ • ____________ • ____________ • composed of elements • What are examples of each type of matter?

  4. What is an element? • Element- substances that can not be separated into smaller substances by natural means. • 92 of the 112 occur in nature • 2 additional elements are hypothetical (114, 116) • And 2 more are not known to exist (113, 115) • Are referred to by a chemical symbol and are organized in the Periodic Table of Elements.

  5. Elements in Animal Body • Major Elements- make up 96% of the body • ___________(O) • ___________(C) • ___________ (H) • ___________ (N)

  6. Minor Elements • _______________ (Ca) • _______________(P) • _______________ (K) • _______________(S) • _______________(Na) • _______________ (Cl) • ________________ (Mg)

  7. Trace Elements • Silicone (Si) • Aluminum (Al) • Iron (Fe) • Manganese (Mn) • Fluorine (F) • Vanadium (V) • Chromium (Cr) • Copper (Cu) • Boron (B) • Cobalt (Co) • Zinc (Zn) • Selenium (Se) • Molybdenum (Mo) • Tin (Sn) • Iodine (I)

  8. Atoms • The smallest unit of an element that retains the unique properties of that element. • Composed of 3 subatomic particles: • ___________ • ___________ • ___________

  9. Protons, Neutrons, & Electrons • Protons and Neutrons are found in the _____________________. • Each proton and neutron has an atomic mass of ~1. • Together protons and neutrons determine the __________________of the atom. • Protons have a _______________ charge. • Neutrons have ______________charge and are considered neutral. • Electrons have a _____________ charge. • Net charge of atoms are neutral because have equal numbers of protons and electrons.

  10. Electrons • Tiny particles that remain in constant motion around the nucleus. • So tiny that their mass does not contribute to the atomic weight of the atom. • Electrons have a ________________ charge. • Orbit around nucleus

  11. Electron Shells and how they work • “Pathways” around the nucleus where electrons orbit • Only a certain number of electrons can be on each path at one time • If the outermost shell is not full, then an atom will be more active in an attempt to fill its outermost shell. • Helium and Neon have full electron shells so are considered chemically ___________.

  12. How the Shells work • First shell can contain ________ electrons. • Second shell on can contain _________ electrons.

  13. Atoms continued • The atomic number of an atom tells us how many ____________ and ____________ it has. • If an atom loses or gains an electron in an attempt to fill its outermost electron shell then it becomes positively or negatively charged, thereby becoming an _______________. • If an atom has a different number of neutrons, they are called ______________________ of the element

  14. Atomic Number

  15. Isotopes

  16. Ions e- Na atom 11electrons, 11protons Na+ ion 10electrons, 11protons

  17. Molecules and Compounds • ___________________- when atoms are joined together by chemical bonds. These are the smallest particle of a substance that retains the properties of the substance. • _____________________when two or more atoms of the same element are joined together. • _______________- how atoms are attached to one another. • ________________ A substance made up of two or more elements.

  18. Chemical Bonds • Means that the atoms are sharing or transferring electrons between them. • By sharing or giving away electron, each atom can be sure that its outermost shell is full. • Remember that atoms are constantly trying to become more stable. • Types of chemical bonds: • _________________ • _________________ • _________________

  19. Covalent Bonds • Bonds formed when atoms share electrons. • Classified depending on how many electrons are being shared. • single covalent bond—______ electron is shared • double covalent bond —_____ electrons are shared • triple covalent bond—______ electrons are shared • May be shared equally (nonpolar) or unequally (polar).

  20. Polar Water Molecule • Shared electrons in a covalently bonded molecule may spend more time near one atom than the other • Shared electrons in water molecule spend more time near __________atom than __________ atoms • Created ‘poles’ • Gives molecule a slight _________ charge on H side of molecule and slight _________charge on O side of molecule

  21. http://www.youtube.com/watch?v=qmgE0w6E6ZI

  22. Ionic Bonds • Formed when electrons are transferred from one atom to another. • Transfer causes a ______ charge on the atom that gave up the electron and a ____________ charge on the atom that receives the electron. • Since opposites attract, the two atoms stick together through electrostatic attraction.

  23. Electron transferred Attraction betweenopposite charges

  24. Types of Ions • ______________- Ions with a net positive charge. • _______________Ions with a net negative charge. • Ions are important in contraction of muscle fibers, transmission of nerve impulses, and maintenance of water balance.

  25. Hydrogen Bonds • Bond between hydrogen atoms already covalently bonded in a molecule to oppositely charged particles. • Found between water molecules and DNA to stabilize shape.

  26. Chemical Reactions • The formation and breaking of chemical bonds. • Require energy input or release of energy. • Chemical Equation- reaction is described in written form. • X + Y → Z • (reactants) (products) • Arrow indicates direction of the reaction

  27. Types of Chemical Reactions • 1. Synthesis Reaction- new and more complex molecule is made from simpler chemicals. Example: • 2. Decomposition Reaction- single complex chemical is broken down into multiple, simpler, chemicals. Example: • 3. Exchange Reaction- certain atoms are exchanged between molecules. Combination of synthesis and decomposition reaction. Example:

  28. Chemical Reactions Continued • _____________ reactions require energy. • ______________ reactions expend or release energy. • _______________have no net energy requirements. Energy released from decomposition portion, helps with synthesis portion.

  29. Chemical Reactions Continued • Factors that influence reaction rates • ________________________ • ________________________ • __________________-the energy required for the reaction to happen. • Some reactions require presence of a catalyst or enzyme • Reaction speed is increased when catalyst is present • Protein (enzyme)

  30. Chemical Components of Living Organisms: Organic and Inorganic Compounds • Inorganic compounds- do not contain hydrocarbon groups (H and C bonded together) and often have ionic bonding. • Water • Salts • Acids and Bases • Organic compounds- contain hydrocarbon groups and are usually covalently bonded

  31. Why is water so Important? • Water is the universal _______________ • ______________- chemicals added to water • _______________- resulting chemical and water mixture • ________________ (water loving)- chemicals that dissolve well or mix with water. • _________________(water hating)- chemicals or molecules that do not mix well with water. • Water is an ideal ______________________ • Blanketing power allows molecules in water to move around and be cushioned from one another. • Blood • Urine • Water has a _______________and a high _______________________________ • Easily able to absorb heat. • Won’t evaporate easily. • Water is used for ________________.

  32. Salts • Mineral compounds that have ionic bonds • In ionic form are called electrolytes-substances that have ability to transmit an electrical charge.

  33. Acids and Bases • ___________- substances that when added to water freely release hydrogen ions. • Called H donors or proton donors • ___________- alkaline in nature release a hydroxyl ion (OH-) when added to water. • Called proton acceptors • Acids and Bases are also electrolytes as they can transmit electricity when ionized in water.

  34. The pH Scale • Ranges from 1-14. • Lower numbers are the most acidic, higher numbers are more alkaline.

  35. Buffers • A substance that minimizes the change of the acidity of a solution when an acid or base is added to the solution. • By not allowing excessive hydrogen or hydroxyl ions to accumulate, buffers help cell maintain _______________.

  36. Organic Molecules • Molecules that contain carbon. • Why carbon?-4 outer electrons in outer shell, trying to share this to complete outer shell. • Divided into 4 groups: • _____________________ • Glycogen • Ribose • ____________________ • Triglycerides • Phospholipids • Steroids • Prostaglandins • _____________________ • Globular • Fibrous • _____________________ • DNA • RNA • Adenosine triphosphate (ATP)

  37. Carbohydrates • Used for energy, storage of energy, and cellular structures. • Simple Sugars-________________. • Glucose and Fructose • ________________- when two monosaccharides are joined together in synthesis reaction. • _________________- combinations of many monosaccharides. • Glycogen and cellulose

  38. Some terminology • _________________- when a macromolecule is formed out of a carbohydrate attached to a protein. • __________________- process of building molecules needed for cellular functioning. • _____________________- Decomposition of nutrients.

  39. Lipids • Used for energy and stored in fat. • 4 classes of Lipids: • _________________ • _________________ • _________________ • _________________

  40. Lipids continued.. • Neutral Fats • Also called triglycerides or fats. • Contains three fatty acids and a glycerol molecule. • _________________________- all bonds in the hydrocarbon chain are single bonds. • _________________________- when there are some double bonds between the carbon and hydrogen atoms. • __________________________- macromolecule composed of proteins and lipids • __________________________- when triglycerides are decomposed.

  41. Phospholipids • Have a glycerol backbone • Have a lipid bilayer when placed in water. • ________________ heads are facing water, while _______________ tails line up with one another.

  42. Steroids • Take form of four interlocking hydrocarbon rings. • Are hydrophobic. • Examples include: • Cholesterol • Cortisol

  43. Eicosanoids • Lipids formed from a 20 carbon fatty acid and ring structure. (hairpin structure) • Include: • _______________- in inflammation • _______________- platelet function • _______________- bronchoconstriction and increased mucus production.

  44. Proteins • Most abundant organic molecules in the body. • Have widest variety of functions. • Catalyze- speed up reactions occurring in the body. • Composed of ___________________

  45. Amino Acids • 20 different amino acids used by the body. • Central carbon is attached to hydrogen atom, an amino group (NH2), a carboxyl group (COOH), and a side chain. • Include: AlanineArginineAsparagineAspartic acidCysteineGlutamic acidGlutamineGlycineHistidineIsoleucineLeucineLysineMethioninePhenylalanineProlineSerineThreonineTryptophanTyrosineValine

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