Basic Chemistry Review 1. Define and explain the relationship between kinetic and potential energy. 2. Identify the energy form in use in each of the following examples: a. Chewing food: b. Vision (two types, please think!) & c. Bending the fingers to make a fist: d. Breaking the bonds of ATP molecules to energize your muscle cells: 3. An is the smallest unit of an element that can combine chemically with other elements. 4. Why is a study of basic chemistry essential to understanding human physiology? 5. Structure Particle Location in Atom Charge Mass Proton Neutron Electron Protons and neutrons have the same and make up the nucleus. Identification : number of protons Atomic mass number: number of + neutrons 6. How is an atom related to an element? 7. Which is true concerning the atomic nucleus? a. contains the mass of the atom b. the negatively charged particles are there c. particles can be ejected d. contain particle that determine atomic number e. contain particles that interact with other atoms
8. Complete the table. Element Symbol Atomic Number C 27 Argon 17 Atomic Mass 58.845 # protons 8 # electons 19 # neutrons Electron Configurations: Example of Lithium atom atomic configuration. 9. Draw the electronic configurations for the following elements: K Cl O Ne 10. Name and provide the atomic symbols of the four elements that make up the bulk of living matter. 11. Why do we use the orbital model of the atom? 12. Isotopes are two atoms with the same number but different atomic mass numbers. Isotopes differ only in the number of. Heavier isotopes of some elements are called
because their nucleus s break down in a spontaneous decay called. 13. If an element has three isotopes which of them (the lightest, the one with an intermediate mass, or the heaviest) is most likely to be a radioisotope, and why? 14. An atom has 5 neutrons, 4 protons, and 4 electrons. What is its atomic number? What is its atomic mass? 15. What name is given to an unstable atom that has either more or fewer neutrons than its typical number? 16. A is a combination of two or more that are chemically joined. 17. Define molecule. 18. Chemical bonding Ionic: when an atom will either give or take an from another atom. A charged atom: : positive ion Anion: ion Only electrons in the are involved in the chemical behavior or bonding of an atom. 19. Explain the basis for ionic bonding. 20. Draw the formation of an ionic bond between Na and Cl. (Use electron configuration)
21. Covalent: when atoms electrons Forms single,, or triple bonds 22. How do ionic bonds differ from covalent bonds? 23. What kind of bond forms between water molecules? Why are those bonds important in the human body? 24. A is a weak bond that links the charged hydrogen end of one polar molecule and the negative end of another polar molecule. 25. Why is water polar? 26. Draw hydrogen bonding between six water molecules. 27. Life on earth is possible because water molecules form hydrogen bonds. Water is the most abundant inorganic compound in the human body. Explain how the following properties of water make it essential to human life: High heat capacity: polarity: cushioning: chemical reactivity: 28. What property of water prevents rapid changes in body temperature?
29. Identify the four types of chemical reactions: : two or more atoms or molecules are combined : molecules are broken down into simpler forms : involve both synthesis and decomposition reactions 30. Identify each of the following reactions as a synthesis, decomposition, or exchange reaction. a. HNO3 H + NO3 b. HCl + NaOH NaCl + H2O c. Fe + CuSO4 FeSO4 + Cu d. 2Hg + O2 2HgO 31. How can you indicate that a chemical reaction is reversible? 32. Distinguish between organic and inorganic compounds. List the major categories of each in the body. Organic Inorganic 33. A is a substance that releases a H + ion in water. 34. A is a substance that releases OH - ion in water. 35. Which is a proton donor - - - an acid or a base? 36. Is a ph of 11 acidic or basic? 37. Define ph. 38. The ph range of blood is from 7.35 to 7.45. This means blood is slightly acidic or basic? 39. A ph of 3.5 is (1, 10, 100, or 1000) time more acidic that a ph of 4.3. 40. Salts, acids, and bases are electrolytes. What is an electrolyte? 41. Define buffer. What is the function of a buffer in the human body? 42. A neutral solution will have a ph of.
43. A buffer will release ions if the surrounding environment becomes to acidic and will release ions if the surrounding environment becomes to basic. 44. are proton donors and have a sour taste while are bitter tasting, slippery, and are. 45. Balance the following equations: H 2 O H 2 + O 2 C 6 H 12 O 6 + O 2 CO 2 + H 2 O HCl + NaOH H 2 O + NaCl