Chemistry - Chapter 5 Study Guide

Transcription

1 Chemistry Chapter 5 and Special Ionic Nomenclature Checklist I can: List the three properties of a wave Define a wavelength Define a photon Describe Bohr s model Describe the quantum theory of matter Define and locate a valence electron Explain Pauli s Exclusion Principle Explain Aufbau s principle Explain the Heisenberg Uncertainty principle Explain the difference between a ground state and an excited state Explain the change in energy (absorbed or given off) when electrons move from the ground state to the excited state and back. List the filling order of orbitals Determine the number of sublevels (orbital types) in a energy level List the number of orbitals in a sublevel Write an electron configuration for any element in the periodic table Draw an orbital representation for any element in the periodic table Use electron configuration shorthand to write configurations for large atoms Write an electron dot structure for an element in the s or p block Write a chemical formula given the name of a binary special ionic compound Write a chemical formula given the name of a ternary binary special ionic compound Write the name of an binary special ionic compound if given its chemical formula Not Yet Almost Got it! I can identify: The number of unpaired electrons in an elements atom an element from its electron configuration Not Yet Almost Got it!

2 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. CONTENT REVIEW 1. Light has the properties of a. particles only. c. both particles and waves. b. waves only. d. neither particles nor waves. 2. Wavelength is defined as the distance between a. the trough and crest of a wave. b. the beginning and ends of two successive waves. c. the crest of one wave and the trough of another. d. successive crests of a wave. 5. Quanta are fundamental "pieces" of a. energy. c. nuclei. b. matter. d. electrons. 6. The photoelectric effect supported what theory of light a. particle. c. wave. b. dual nature d. quantum 7. When a sample of an element is vaporized in a flame, it releases energy in the form of a. a continuous spectrum. c. light of all wavelengths. b. gamma rays. d. light of only certain wavelengths. 8. The quantum-mechanical model explains the atom by treating the a. atom as a point. b. electron as a particle. c. electron as a wave of quantized energy. d. electron as a wave of unquantized energy. 9. The probability of finding electrons in certain regions of an atom is described by a. orbits. c. quanta. b. orbitals. d. photons. 10. How is an electron's principal quantum number symbolized? a. s c. n b. p d. d 11. The number of sublevels found in each principal energy level of an atom equals a. the principal quantum number. c. three. b. twice the principal quantum number. d. five. 12. Under what conditions can two electrons occupy the same orbital? a. Never b. if they have opposite spins c. if they have parallel spins d. if they have different principal quantum numbers 13. When electrons are in the lowest-energy orbitals available, the atom is a. unstable. c. in the ground state. b. in an excited state. d. chemically unreactive. 14. The principle that states that electrons are added one at a time to the lowest-energy orbitals available in an atom until all electrons have been accounted for is a. the Aufbau principle. c. the uncertainty principle. b. the Pauli exclusion principle. d. Hund's rule. 15. Which principle states that electrons will occupy equal-energy orbitals so that a maximum number of unpaired electrons results? a. the Aufbau principle c. the uncertainty principle b. the Pauli exclusion principle d. Hund s rule

3 16. Because c, the speed of electromagnetic radiation, is a constant, the wavelength of the radiation is a. proportional to its frequency. c. inversely proportional to its frequency. b. equal to its frequency. d. double its frequency. 17. Electromagnetic radiation behaves like a particle when it a. travels through space. c. interacts with photons. b. is absorbed by matter. d. interacts with other radiation. 18. As it travels through space, electromagnetic radiation a. exhibits wavelike behavior. c. varies in speed. b. loses energy. d. releases photons. 19. If electromagnetic radiation A has a lower frequency than electromagnetic radiation B, then compared to B the wavelength of A is a. longer. b. shorter. c. equal. d. exactly half the length of B's wavelength. 20. The distance between two successive peaks on a wave is its a. frequency. c. quantum number. b. wavelength. d. velocity. 21. A quantum of electromagnetic energy is called a(n) a. photon. c. excited atom. b. electron. d. orbital. 22. The wave model of light did not explain a. the frequency of light. c. interference. b. the continuous spectrum. d. the photoelectric effect. 23. The energy of a photon, or quantum, is related to its a. mass. c. frequency. b. speed. d. size. 24. The emission of electrons from metals that have absorbed photons is called the a. interference effect. c. quantum effect. b. photoelectric effect. d. dual effect. 25. A line spectrum is produced when an electron moves from one energy level a. to a higher energy level. b. to a lower energy level. c. into the nucleus. d. to another position in the same sublevel. 26. A bright-line spectrum of an atom is caused by the energy released when electrons a. jump to a higher energy level. b. fall to a lower energy level. c. absorb energy and jump to a higher energy level. d. absorb energy and fall to a lower energy level. 27. The Bohr model of the atom was an attempt to explain hydrogen's a. density. c. mass. b. flammability. d. line-emission spectrum. 28. For an electron in an atom to change from the ground state to an excited state, a. energy must be released. b. energy must be absorbed. c. radiation must be emitted. d. the electron must make a transition from a higher to a lower energy level. 29. If electrons in an atom have the lowest possible energies, the atom is in the a. ground state. c. excited state. b. inert state. d. radiation-emitting state.

4 30. Bohr's model of the atom works best in explaining a. the spectra of the first ten elements. b. only the spectrum of hydrogen. c. only the spectra of atoms with electrons in an s orbital. d. the entire visible spectra of atoms. 31. According to Bohr's theory, an excited atom would a. collapse. c. remain stable. b. absorb photons. d. radiate energy. 32. According to the Bohr model of the atom, the single electron of a hydrogen atom circles the nucleus a. in specific, allowed orbits. b. in one fixed orbit at all times. c. at any of an infinite number of distances, depending on its energy. d. counterclockwise. 33. The drop of an electron from a high energy level to the ground state in a hydrogen atom would be most closely associated with a. long-wavelength radiation. c. infrared radiation. b. low-frequency radiation. d. high-frequency radiation. 34. The French scientist Louis de Broglie believed a. electrons could have a dual wave-particle nature. b. light waves did not have a dual wave-particle nature. c. the natures of light and quantized electron orbits were not similar. d. Bohr's model of the hydrogen atom was completely correct. 36. Which model of the atom explains the orbitals of electrons as waves? a. the Bohr model c. Rutherford's model b. the quantum mechanical model d. Planck's theory 37. The region outside the nucleus where an electron can most probably be found is the a. electron configuration. c. s sublevel. b. quantum. d. orbital. 38. All of the following describe the Heisenberg uncertainly principle EXCEPT a. it states that it is impossible to determine simultaneously both the position and velocity of an electron or any other particle. b. it is one of the fundamental principles of our present understanding of light and matter. c. it helped lay the foundation for the modern quantum theory. d. it helps to locate an electron in an atom. 39. All of the following describe the Schrödinger wave equation EXCEPT a. it is an equation that treats electrons in atoms as waves. b. only waves of specific energies and frequencies provide solutions to the equation. c. it helped lay the foundation for the modern quantum theory. d. it is similar to Bohr's theory. 40. Unlike in an orbit, in an orbital a. an electron's position cannot be known precisely. b. an electron has no energy. c. electrons cannot be found. d. protons cannot be found. 41. A spherical electron cloud surrounding an atomic nucleus would best represent a. an s orbital. c. a combination of p x and p y orbitals. b. a p x orbital. d. a combination of an s and a p x orbital. 42. The major difference between a 1s orbital and a 2s orbital is that a. the 2s orbital can hold more electrons. b. the 2s orbital has a slightly different shape. c. the 2s orbital is at a higher energy level. d. the 1s orbital can have only one electron.

5 43. The p orbitals are shaped like a. electrons. c. dumbbells. b. circles. d. spheres. 44. An orbital that could never exist according to the quantum description of the atom is a. 3d. c. 6d. b. 8s. d. 3f. 45. The number of possible orbital shapes for the third energy level is a. 1. c. 3. b. 2. d The number of orbitals for the d sublevel is a. 1. c. 5. b. 3. d How many electrons can occupy the s orbitals at each energy level? a. two, if they have opposite spins c. one b. two, if they have the same spin d. no more than eight 48. How many electrons are needed to completely fill the fourth energy level? a. 8 c. 32 b. 18 d Which of the following rules requires that each of the p orbitals at a particular energy level receive one electron before any of them can have two electrons? a. Hund's rule c. the Aufbau principle b. the Pauli exclusion principle d. the quantum rule 50. The sequence in which energy sublevels are filled is specified by a. the Pauli exclusion principle. c. Lyman's series. b. the orbital rule. d. the Aufbau principle. 51. The Pauli exclusion principle states that no two electrons in the same atom can a. occupy the same orbital. c. occupy the same sublevel. b. have the same spin. d. be at the same main energy level. Part II A.Draw electron configurations and orbital diagrams for 16. Nitrogen 17. Barium 18. Bromine 19. Palladium (Pd) 20. Polonium (Po) (give short hand, or noble gas notation)

6 Draw the electron dot structures for: Chemistry - Chapter 5 Study Guide 21. P 23. Kr 22. Al 24. K I. Provide the correct name or formula for each of the following: 1. Cu(ClO 2) copper (II) nitride 2. silver oxide 3. zinc nitrate 4. Pb(NO 2) 4 5. Cr(OH) 2 6. tin (II) hydroxide 7. FeI 3 8. zinc phosphide 9. Mn(NO 3) CuF 11. lead (II) phosphate 12. lead (IV) phosphate 13. chromium (III) oxide 15. cobalt (II) acetate 16. silver carbonate 17. Fe(ClO 3) PbBr Sn 3N Hg(OH) Pb(OH) Mercury (I) carbonate 23. Cu(NO 3) Iron (II) oxide 25. ZnS 26. Tin (IV) sulfide

7 Answers to MC 1. c 7. d 13. c 19. a 25. b 31. d 37. d 43. c 49. a 2. d 8. c 14. a 20. b 26. b 32. a 38. d 44. d 50. d 9. b 15. d 21. a 27. d 33. d 39. d 45. c 51. b 10. c 16. c 22. d 28. b 34. a 40. a 46. c 5. a 11. a 17. b 23. c 29. a 41. a 47. a 6. a 12. b 18. a 24. b 30. b 36. b 42. c 48. c I. Answers to nomenclature 1. copper (II) chlorite 2. Ag 2O 3. Zn(NO 3) 2 4. lead (IV) nitrite 5. Chromium (II) hydroxide 6. Sn(OH) 2 7. Iron (III) iodide 8. Zn 3P 2 9. Manganese nitrate 10. Copper(I) fluoride 11. Pb 3(PO 4) Pb 3(PO) Cr 2O Cu 3N Co(C 2H 3O 2) Ag 2CO Iron (II) chlorate 18. Lead (IV) bromide 19. Tin(IV) nitride 20. Mercury(II) hydroxide 21. Lead(II) hydroxide 22. Hg 2CO Copper (II) nitrate 24. FeO 25. zinc sulfide 26. SnS 2