66. How many protons and electrons are contained in an atom of element 44? element 44 = atomic # 44 44 protons 44 electrons.

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66. How many protons and electrons are contained in an atom of element 44? element 44 = atomic # 44 44 protons 44 electrons

67. A carbon atom has a mass number of 12 and an atomic number of 6 67. A carbon atom has a mass number of 12 and an atomic number of 6. How many neutrons does it have? mass number (p + n) 12 atomic number (p) - 6 = # of neutrons 6 n

68. An isotope of mercury has 80 protons and 120 neutrons 68. An isotope of mercury has 80 protons and 120 neutrons. What is the mass number of the isotope? protons 80 + neutrons + 120 = Mass number 200

69. An isotope of xenon has an atomic number of 54 and contains 77 neutrons. What is the xenon isotope’s mass number? protons 54 + neutrons + 77 = Mass number 131

70. Is an atom has 18 electrons, how many protons does it have?

72. Fill in the blank Cl Zr 17 40 35 37 90 92 18 20 50 52 Element Atomic Number 17 40 Mass Number 35 37 90 92 Protons Neutrons 18 20 50 52 Electrons

73. How many electrons, protons, and neutrons are contained in each? electrons protons neutrons 132 55 Cs 55 55 77 b) 59 27 Co 27 27 32 c) 163 69 Tm 69 69 94 d) 70 30 Zn 30 30 40

74. How many electrons, protons, and neutrons are contained in each? electrons protons neutrons Gallium -69 31 31 38 b) fluorine-23 9 9 14 c) titanium-48 22 22 26 d) tantalum-181 73 73 108

76. Ga, which has atomic mass of 69 76. Ga, which has atomic mass of 69.723 amu, has two naturally occurring isotopes, Ga-69 and Ga-71. Which isotope occurs in greater abundance? Explain. Ga- 69 must be more abundant because the atomic mass of gallium is closer to the mass of Ga-69 than the mass of Ga-71

77. Silver has two isotopes 107 47 Ag, which has a mass of 106 77. Silver has two isotopes 107 47 Ag, which has a mass of 106.905 amu and a percent abundance of 52.00% and 109 47 Ag , which has a mass of 108.905 amu and a percent abundance of 48.00%. What is the atomic mass of silver? 106.905 x .5200 = 55.59 108.905 x .4800 = 52.27 107.86 amu

78. Data for chromium’s four naturally occurring isotopes are provided in the table. Calculate the atomic mass (amu). Isotope Percent Abundance Mass (amu) Cr- 50 4.35 49.946 Cr- 52 83.79 51.941 Cr- 53 9.50 52.941 Cr- 54 2.36 53.939 = 2.17 = 43.52 = 5.03 = 1.27 51.99 amu