-AP Biology Biochemistry/Chemistry Review Name Chapter 2 - The Nature of Molecules Sections 2.1-2.3 Chapter 3 The Chemical building blocks of life 1. What occurrence 12.5 billion years ago is proposed to have begun the process that lead to the formation of the earth? When did the earth form? When did life form and begin to diversify? 2. Define matter: 3. All matter is composed of extremely small particles called, the smallest particles of an element. 4. Identify and compare the three subatomic particles: Particle Location Mass (daltons or amu s) Charge a. b. c. 5. Define: a. atomic number b. atomic mass 6. What determines the chemical behavior of an atom? 7. What characteristic do all the atoms of the same element have in common? 8. Give the atomic number and average atomic mass (round to 3 sig.figs) for K. What is the mass number for the most common isotope of potassium? 9. Atoms have the same number of protons and electrons and are thus electrically. 10. An atom which has gained one or more electrons is called an and has a net charge. An atom which has lost one or more electrons is called an and has a net charge. 11. Compare and contrast carbon-12 with its isotope carbon-14 as to abundance, number of p, e, and n and stability.
12. Give two uses of radioactivity related to biology: a. b. 13. Complete the following chart for the most common isotope of each atom/ion. Symbol O Protons Electrons Neutrons Outermost or Valence e- s Predicted oxidation State(s)/# of electrons it tends to gain, lose, or share P Li F -1 Na +1 14. The key to the chemical behavior of an atom lies in the arrangement of its. The area around the nucleus where an electron is most likely to be found is called an, which represents a distribution for an electron. The first energy level, K, is occupied by a single spherical shaped orbital. The second energy level, L, is occupied by one spherical orbital and 3 dumbbell shaped orbitals. Regardless of its shape, no orbital can contain more than electrons. 15. Circle the two correct terms: Electrons that are found in more distant orbitals have (more or less) (kinetic or potential) energy. 16. Electrons within an atom have discrete due to their position or distance from the nucleus. 17. The loss of electrons from an atom in a chemical reaction is called. The gain of electrons is called. 18. Write the complete electron configuration for the following atoms: (Do not use noble gas shorthand.) Atom Electron Configuration Valence e- 19K 26Fe 92U 19. The interactions of outermost or electrons is the basis for differing chemical properties.
20. The noble gases are nonreactive or. Group VII elements, the halogens such as F, Cl, and Br tend to an electron. Group I elements, the alkali metals such as Li, Na, and K tend to an electron. 21. State the octet rule. 22. Explain why iron atoms tend to form +2 Ferrous as well as +3 Ferric ions. 23. Identify the 6 major elements found in living things. 24. Describe the role of carbon in molecular diversity, its characteristics, and its forms of organization structures. 25. Two or more different elements chemically combined in definite proportions make up a. A group of covalently bound atoms with an overall neutral charge is called a. 26. Recognize the importance of molecular bonding and distinguish among strong and weak bonds, giving biological examples of each. (polar covalent, nonpolar covalent, ionic and hydrogen bonds) 27. Which molecule has a stronger covalent bond, O 2 or H 2? Explain. 28. How many covalent bonds does a C atom form? Explain. 29. Distinguish among the three types of isomers: structural, geometric, and enantiomers. 30. Recognize the major functional groups and describe the traits they give their macromolecule.
31. Define monomer, polymer, hydrolysis, and dehydration synthesis and be able to give specific examples from each of 4 macromolecule groups. 32. Complete the chart in order to compare the four groups of macromolecules: carbohydrates monomers Bond types structures functions lipids proteins nucleic acids 33. The affinity of an atom for electrons in a bond is called. Where are the elements located with highest electonegativity? Which element has the highest electronegativity? 34. What type of bonds result when atoms share electrons unequally? 35. Is the bond between 2 oxygen atoms polar or nonpolar? 36. Is the bond between a C and a H atom, polar or nonpolar? 37. Is the bond between an O and a H atom, considered polar or nonpolar? 38. The formation and breaking of chemical bonds is termed a chemical which is represented by a chemical. 39. Why must chemical equations be balanced? 40. State three factors that influence the extent to which a chemical reaction occurs/influence rates of reactions a. b. c.
41. What information can be communicated around the four corners of an element s symbol? upper left? lower left? upper right? lower right? 42. Name the following compounds: a. C 55 H 98 O 6 b. C 6 H 12 O 6 c. C 55 H 72 O 5 N 4 Mg 43. Give the formulas for the following elements/compounds. a. nitrogen gas b. sodium chloride c. magnesium sulfate d. calcium hydroxide e. iron(iii) oxide f. hydrochloric acid g. carbon dioxide h. sodium thiosulfate i. carbonic acid 44. Give the: molecular formula, structural formula and Lewis dot diagram for water. 45. Calculate the molecular mass of 1 molecule of glucose, C 6 H 12 O 6. (Give proper units.) 46. What many molecules are in a mole of glucose molecules?
47. What is the mass of one mole of glucose molecules? 48. Balance the following equation for photosynthesis. b. Circle the reactants and underline the products. CO 2 + H 2 O C 6 H 12 O 6 + O 2 49. How many moles of CO 2 are required to produce 24.0 grams of glucose? (Show work with appropriate conversion factors and units, i.e. use dimensional analysis to solve.)