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	6.16 \| Why is the electron in a Bohr hydrogen atom bound less tightly when it has a quantum number (The Glaser Tutoring Company) View
	6.31 \| How are the Bohr model and the quantum mechanical model of the hydrogen atom similar How are (The Glaser Tutoring Company) View
	6.18 \| Using the Bohr model, determine the energy, in joules, necessary to ionize a ground-state (The Glaser Tutoring Company) View
	6.28 \| Consider a large number of hydrogen atoms with electrons randomly distributed in the n = 1, 2 (The Glaser Tutoring Company) View
	6.20 \| Using the Bohr model, determine the lowest possible energy, in joules, for the electron in (The Glaser Tutoring Company) View
	6.6 \| Heated lithium atoms emit photons of light with an energy of 2.961 × 10^−19 J. Calculate the (The Glaser Tutoring Company) View
	6.30 \| The spectra of hydrogen and of calcium are shown here. What causes the lines in these spectra (The Glaser Tutoring Company) View
	6.22 \| Using the Bohr model, determine the energy of an electron with n = 6 in a hydrogen atom. (The Glaser Tutoring Company) View
	6.43 \| How many electrons could be held in the second shell of an atom if the spin quantum number ms (The Glaser Tutoring Company) View
	6.24 \| How far from the nucleus in angstroms (1 angstrom = 1 × 10^–10 m) is the electron in a (The Glaser Tutoring Company) View

	6.16 \| Why is the electron in a Bohr hydrogen atom bound less tightly when it has a quantum number (The Glaser Tutoring Company) View
	6.31 \| How are the Bohr model and the quantum mechanical model of the hydrogen atom similar How are (The Glaser Tutoring Company) View
	6.18 \| Using the Bohr model, determine the energy, in joules, necessary to ionize a ground-state (The Glaser Tutoring Company) View
	6.28 \| Consider a large number of hydrogen atoms with electrons randomly distributed in the n = 1, 2 (The Glaser Tutoring Company) View
	6.20 \| Using the Bohr model, determine the lowest possible energy, in joules, for the electron in (The Glaser Tutoring Company) View
	6.6 \| Heated lithium atoms emit photons of light with an energy of 2.961 × 10^−19 J. Calculate the (The Glaser Tutoring Company) View
	6.30 \| The spectra of hydrogen and of calcium are shown here. What causes the lines in these spectra (The Glaser Tutoring Company) View
	6.22 \| Using the Bohr model, determine the energy of an electron with n = 6 in a hydrogen atom. (The Glaser Tutoring Company) View
	6.43 \| How many electrons could be held in the second shell of an atom if the spin quantum number ms (The Glaser Tutoring Company) View
	6.24 \| How far from the nucleus in angstroms (1 angstrom = 1 × 10^–10 m) is the electron in a (The Glaser Tutoring Company) View