Write the condensed electron configurations for the following atoms and indicate how many unpaired electrons each has: (f) Lu.

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Write the condensed electron configurations for the following atoms and indicate how many unpaired electrons each has: (e) Y

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Write the condensed electron configurations for the following atoms and indicate how many unpaired electrons each has: (d) V

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Write the condensed electron configurations for the following atoms, using the appropriate noble-gas core abbreviations: (d) Cd

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Write the condensed electron configurations for the following atoms, using the appropriate noble-gas core abbreviations: (c) Se

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Write the condensed electron configurations for the following atoms, using the appropriate noble-gas core abbreviations: (b) Ni

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Write the condensed electron configurations for the following atoms, using the appropriate noble-gas core abbreviations: (a) Cs

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For each element, indicate the number of valence electrons, core electrons, and unpaired electrons in the ground state: (c) neon

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For each element, indicate the number of valence electrons, core electrons, and unpaired electrons in the ground state: (b) phosphorus

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For each element, indicate the number of valence electrons, core electrons, and unpaired electrons in the ground state: (a) carbon

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What is the maximum number of electrons in an atom that can have the following quantum numbers: (c) n = 4, l = 3

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What is the maximum number of electrons in an atom that can have the following quantum numbers: (b) n = 5, l = 3

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What is the maximum number of electrons in an atom that can have the following quantum numbers: (a) n = 2, m_{s} = -1/2

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What is the maximum number of electrons that can occupy each of the following subshells: (a) 3p

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Sketch the shape and orientation of the following types of orbitals: (c) d _{x2-y2}

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Sketch the shape and orientation of the following types of orbitals: (b) d _{z2}

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Sketch the shape and orientation of the following types of orbitals: (a) p _{x}

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Sketch the shape and orientation of the following types of orbitals: (c) d _{xy}

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Sketch the shape and orientation of the following types of orbitals: (a) s

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For the table that follows, write which orbital goes with the quantum numbers. Don’t worry about x, y, z subscripts. If the quantum numbers are not allowed, write “not allowed.”

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Which of the following represent impossible combinations of n and l: (a) 1p, (b) 4s, (c) 5f, (d) 2d?

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Give the values for n, l, and m _{l} for (a) each orbital in the 2p subshell

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Give the numerical values of n and l corresponding to each of the following orbital designations: (a) 3p

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How many possible values for l and m _{l} are there when (a) n = 5?

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How many possible values for l and m _{l} are there when (a) n = 3?

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