Chemistry Common Assessment Quarter One

Multiple Choice Identify the letter of the choice that best completes the statement or answers the question.

____ 1. The smallest particle of an element that retains the properties of that element is a(n) ____. a. atom c. proton b. electron d. neutron ____ 2. Dalton's atomic theory included which idea? a. All atoms of all elements are the same size. b. Atoms of different elements always combine in one-to-one ratios. c. Atoms of the same element are always identical. d. Individual atoms can be seen with a microscope. ____ 3. Why did J. J. Thomson reason that electrons must be a part of the atoms of all elements? a. Cathode rays are negatively-charged particles. b. Cathode rays can be deflected by magnets. c. An electron is 2000 times lighter than a hydrogen atom. d. Charge-to-mass ratio of electrons was the same, regardless of the gas used. ____ 4. Which of the following is true about subatomic particles? a. Electrons are negatively charged and are the heaviest subatomic particle. b. Protons are positively charged and the lightest subatomic particle. c. Neutrons have no charge and are the lightest subatomic particle. d. The mass of a neutron nearly equals the mass of a proton. ____ 5. Who conducted experiments to determine the quantity of charge carried by an electron? a. Rutherford c. Dalton b. Millikan d. Thomson ____ 6. The particles that are found in the nucleus of an atom are ____. a. neutrons and electrons c. protons and neutrons b. electrons only d. protons and electrons ____ 7. The atomic number of an element is the total number of which particles in the nucleus? a. neutrons c. electrons b. protons d. protons and electrons ____ 8. An element has an atomic number of 76. The number of protons and electrons in a neutral atom of the element are ____. a. 152 protons and 76 electrons c. 38 protons and 38 electrons b. 76 protons and 0 electrons d. 76 protons and 76 electrons ____ 9. The sum of the protons and neutrons in an atom equals the ____. a. atomic number c. atomic mass b. nucleus number d. mass number ____ 10. What does the number 84 in the name krypton-84 represent? a. the atomic number c. the sum of the protons and electrons b. the mass number d. twice the number of protons ____ 11. All atoms of the same element have the same ____. a. number of neutrons c. mass numbers b. number of protons d. mass ____ 12. Isotopes of the same element have different ____. a. numbers of neutrons c. numbers of electrons b. numbers of protons d. atomic numbers ____ 13. How many protons, electrons, and neutrons does an atom with atomic number 50 and mass number 125 contain? a. 50 protons, 50 electrons, 75 neutrons c. 120 neutrons, 50 protons, 75 electrons b. 75 electrons, 50 protons, 50 neutrons d. 70 neutrons, 75 protons, 50 electrons ____ 14. If E is the symbol for an element, which two of the following symbols represent isotopes of the same element? 1. E 2. E 3. E 4. E

a. 1 and 2 c. 1 and 4 b. 3 and 4 d. 2 and 3 ____ 15. What unit is used to measure weighted average atomic mass? a. amu c. angstrom b. gram d. nanogram ____ 16. How does the energy of an electron change when the electron moves closer to the nucleus? a. It decreases. c. It stays the same. b. It increases. d. It doubles. ____ 17. The principal quantum number indicates what property of an electron? a. position c. energy level b. speed d. electron cloud shape ____ 18. How many energy sublevels are in the second principal energy level? a. 1 c. 3 b. 2 d. 4 ____ 19. What is the maximum number of orbitals in the p sublevel? a. 2 c. 4 b. 3 d. 5 ____ 20. If the spin of one electron in an orbital is clockwise, what is the spin of the other electron in that orbital? a. zero c. counterclockwise b. clockwise d. both clockwise and counterclockwise ____ 21. What is the next atomic orbital in the series 1s, 2s, 2p, 3s, 3p? a. 2d c. 3f b. 3d d. 4s ____ 22. What is the number of electrons in the outermost energy level of an oxygen atom? a. 2 c. 6 b. 4 d. 8 ____ 23. What is the electron configuration of potassium? a. 1s 2s 2p 3s 3p 4s c. 1s 2s 3s 3p 3d b. 1s 2s 2p 3s 3p d. 1s 2s 2p 3s 3p 4s ____ 24. How many unpaired electrons are in a sulfur atom (atomic number 16)? a. 0 c. 2 b. 1 d. 3 ____ 25. Which of the following electromagnetic waves have the highest frequencies? a. ultraviolet light waves c. microwaves b. X-rays d. gamma rays ____ 26. How are the frequency and wavelength of light related? a. They are inversely proportional to each other. b. Frequency equals wavelength divided by the speed of light. c. Wavelength is determined by dividing frequency by the speed of light. d. They are directly proportional to each other. ____ 27. Emission of light from an atom occurs when an electron ____. a. drops from a higher to a lower energy level b. jumps from a lower to a higher energy level c. moves within its atomic orbital d. falls into the nucleus ____ 28. Which of the following quantum leaps would be associated with the greatest energy of emitted light? a. n = 5 to n = 1 c. n = 2 to n = 5 b. n = 4 to n = 5 d. n = 5 to n = 4 ____ 29. What are quanta of light called? a. charms c. muons b. excitons d. photons ____ 30. Which scientist developed the quantum mechanical model of the atom? a. Albert Einstein c. Niels Bohr b. Erwin Schrodinger d. Ernest Rutherford ____ 31. Who predicted that all matter can behave as waves as well as particles? a. Albert Einstein c. Max Planck b. Erwin Schrodinger d. Louis de Broglie ____ 32. According to the Heisenberg uncertainty principle, if the position of a moving particle is known, what other quantity CANNOT be known? a. mass c. spin b. charge d. velocity ____ 33. What is another name for the representative elements? a. Group A elements c. Group C elements b. Group B elements d. transition elements ____ 34. What is another name for the transition metals? a. noble gases c. Group B elements b. Group A elements d. Group C elements ____ 35. Which of the following elements is in the same period as phosphorus? a. carbon c. nitrogen b. magnesium d. oxygen ____ 36. Each period in the periodic table corresponds to ____. a. a principal energy level c. an orbital b. an energy sublevel d. a suborbital ____ 37. The modern periodic table is arranged in order of increasing atomic ____. a. mass c. number b. charge d. radius ____ 38. Which of the following categories includes the majority of the elements? a. metalloids c. metals b. liquids d. nonmetals ____ 39. Of the elements Pt, V, Li, and Kr, which is a nonmetal? a. Pt c. Li b. V d. Kr ____ 40. To what category of elements does an element belong if it is a poor conductor of electricity? a. transition elements c. nonmetals b. metalloids d. metals ____ 41. Which of the following is true about the electron configurations of the noble gases? a. The highest occupied s and p sublevels are completely filled. b. The highest occupied s and p sublevels are partially filled. c. The electrons with the highest energy are in a d sublevel. d. The electrons with the highest energy are in an f sublevel. ____ 42. Which subatomic particle plays the greatest part in determining the properties of an element? a. proton c. neutron b. electron d. none of the above ____ 43. What causes the shielding effect to remain constant across a period? a. Electrons are added to the same principal energy level. b. Electrons are added to different principal energy levels. c. The charge on the nucleus is constant. d. The atomic radius increases. ____ 44. What is the charge of a cation? a. a positive charge b. no charge c. a negative charge d. The charge depends on the size of the nucleus. ____ 45. The metals in Groups 1A, 2A, and 3A ____. a. gain electrons when they form ions c. all have ions with a 1 charge b. all form ions with a negative charge d. lose electrons when they form ions ____ 46. Why is the second ionization energy greater than the first ionization energy? a. It is more difficult to remove a second electron from an atom. b. The size of atoms increases down a group. c. The size of anions decreases across a period. d. The nuclear attraction from protons in the nucleus decreases. ____ 47. What is the element with the lowest electronegativity value? a. cesium c. calcium b. helium d. fluorine ____ 48. Which of the following elements has the smallest ionic radius? a. Li c. O b. K d. S ____ 49. What is the energy required to remove an electron from an atom in the gaseous state called? a. nuclear energy c. shielding energy b. ionization energy d. electronegative energy ____ 50. Of the following elements, which one has the smallest first ionization energy? a. boron c. aluminum b. carbon d. silicon

Short Answer: 1 point answer only 2 points answer and work 3 points answer, work and units 4 points answer, work, units and significant figures

51. A fictitious element X is composed of 10.0 percent of the isotope , 20.0 percent of the isotope , and 70.0 percent of the isotope . Estimate the atomic mass of element X. 52. What is the frequency of ultraviolet light with wavelength 2.94 10 m? (c = 3.00 10 m/s) 53. What is the frequency of a radar photon with energy 6.80 10 J? (h = 6.63 10 J s)

Essay: Construct a responce to the essay questions according to the following scoring guide. 1 point basic explanation 2 points well developed explantion 3 points well developed explantion with examples 4 points well developed explanation, examples, and critical connections

54. Explain how the atoms of one element differ from those of another element. 55. Explain why the 4s sublevel fills before the 3d sublevel begins to fill as electrons are added. 56. Describe the three different principles that govern the building of an electron configuration. 57. What is the explanation for the discrete lines in atomic emission spectra? 58. Describe the trends in the atomic size of elements within groups and across periods in the periodic table. Provide examples. 59. Positive ions are smaller than the atoms from which they are formed, but negative ions are larger than the atoms from which they are formed. Explain why this is so.