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Chapter 7: Problem 89

Write the ground-state electron configurations for the following elements: \(\mathrm{B}, \mathrm{V}, \mathrm{Ni}, \mathrm{As}, \mathrm{I},\) Au.

Short Answer

Expert verified
Electron Configurations: Boron (B): \(1s^22s^22p^1\), Vanadium (V): \(1s^22s^22p^63s^23p^64s^23d^3\), Nickel (Ni): \(1s^22s^22p^63s^23p^64s^23d^8\), Arsenic (As): \(1s^22s^22p^63s^23p^64s^23d^{10}4p^3\), Iodine (I): \(1s^22s^22p^63s^23p^64s^23d^{10}4p^65s^24d^{10}5p^5\), Gold (Au): \(1s^22s^22p^63s^23p^64s^23d^{10}4p^65s^24d^{10}5p^66s^24f^{14}5d^{10}\).

Step by step solution

01

Identifying Atomic Number

The first step is to identify the atomic number for each element. We can find these in the periodic table: B (Boron) - 5, V (Vanadium) - 23, Ni (Nickel) - 28, As (Arsenic) - 33, I (Iodine) - 53, Au (Gold) - 79.
02

Writing Electron Configuration for Boron (B)

Boron has an atomic number of 5, so it has five electrons in its neutral state. The electron configuration is \(1s^22s^22p^1\).
03

Writing Electron Configuration for Vanadium (V)

Vanadium has 23 electrons. The electron configuration is \(1s^22s^22p^63s^23p^64s^23d^3\).
04

Writing Electron Configuration for Nickel (Ni)

Nickel has 28 electrons. The electron configuration is \(1s^22s^22p^63s^23p^64s^23d^8\).
05

Writing Electron Configuration for Arsenic (As)

Arsenic has 33 electrons. The electron configuration is \(1s^22s^22p^63s^23p^64s^23d^{10}4p^3\).
06

Writing Electron Configuration for Iodine (I)

Iodine has 53 electrons. The electron configuration is \(1s^22s^22p^63s^23p^64s^23d^{10}4p^65s^24d^{10}5p^5\).
07

Writing Electron Configuration for Gold (Au)

Gold has 79 electrons. The electron configuration is \(1s^22s^22p^63s^23p^64s^23d^{10}4p^65s^24d^{10}5p^66s^24f^{14}5d^{10}\).

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Most popular questions from this chapter

In the beginning of the twentieth century, some scientists thought that a nucleus may contain both electrons and protons. Use the Heisenberg uncertainty principle to show that an electron cannot be confined within a nucleus. Repeat the calculation for a proton. Comment on your results. Assume the radius of a nucleus to be \(1.0 \times 10^{-15} \mathrm{~m} .\) The masses of an electron and a proton are \(9.109 \times 10^{-31} \mathrm{~kg}\) and \(1.673 \times 10^{-27} \mathrm{~kg},\) respectively. (Hint: Treat the diameter of the nucleus as the uncertainty in position.)

$$ \begin{array}{lccccc} \lambda(\mathrm{nm}) & 405 & 435.8 & 480 & 520 & 577.7 \\ \hline \mathrm{KE}(\mathrm{J}) & 2.360 \times & 2.029 \times & 1.643 \times & 1.417 \times & 1.067 \times \\ & 10^{-19} & 10^{-19} & 10^{-19} & 10^{-19} & 10^{-19} \end{array} $$ A ruby laser produces radiation of wavelength \(633 \mathrm{nm}\) in pulses whose duration is \(1.00 \times 10^{-9} \mathrm{~s}\). (a) If the laser produces \(0.376 \mathrm{~J}\) of energy per pulse, how many photons are produced in each pulse? (b) Calculate the power (in watts) delivered by the laser per pulse. \((1 \mathrm{~W}=1 \mathrm{~J} / \mathrm{s})\)

State the Aufbau principle and explain the role it plays in classifying the elements in the periodic table.

List all the possible subshells and orbitals associated with the principal guantum number \(n\), if \(n=6\).

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