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Chapter 4: Problem 170

What is the valence shell in \(\mathrm{Mg}\), Ge, \(\mathrm{W}\), \(C \mathrm{~s} ?\)

Short Answer

Expert verified
The valence shells for the four elements are: Magnesium (Mg) - 3rd shell, Germanium (Ge) - 4th shell, Tungsten (W) - 6th shell, and Cesium (Cs) - 6th shell.

Step by step solution

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1. Valence shell of Magnesium (Mg)

Magnesium (Mg) has an atomic number of 12. Based on its location in the periodic table, the electronic configuration can be written as: \(1s^2 2s^2 2p^6 3s^2\). The valence shell is the outermost shell with electrons, which is the 3rd shell in the case of Mg.
02

2. Valence shell of Germanium (Ge)

Germanium (Ge) has an atomic number of 32. Based on its location in the periodic table, its electronic configuration can be written as: \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^{10} 4s^2 4p^2\). The valence shell is the outermost shell with electrons, which is the 4th shell in the case of Ge.
03

3. Valence shell of Tungsten (W)

Tungsten (W) has an atomic number of 74. Its electronic configuration can be written as: \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^{10} 4s^2 4p^6 4d^{10} 5s^2 5p^6 4f^{14} 5d^4 6s^2\). The valence shell is the outermost shell with electrons, which is the 6th shell in the case of W.
04

4. Valence shell of Cesium (Cs)

Cesium (Cs) has an atomic number of 55. Based on its location in the periodic table, its electronic configuration can be written as: \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^{10} 4s^2 4p^6 4d^{10} 5s^2 5p^6 4f^{14} 5d^{10} 6s^1\). The valence shell is the outermost shell with electrons, which is the 6th shell in the case of Cs.

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Most popular questions from this chapter

Predict the formula of the compound that forms when sodium atoms react with sulfur atoms. Completely explain your reasoning.

Consider the anion whose charge is \(2^{-}\) and whose electron configuration is identical to that of argon, Ar. What is the symbol for this anion?

Halogens are very reactive because (choose the correct answer): (a) They need to gain only one electron to satisfy the octet rule. (b) They have seven electrons in their valence shell, and the more electrons an atom has, the more reactive it is. (c) They are nonmetals, and all nonmetals are reactive. (d) They can easily lose their seven valence electrons to satisfy the octet rule.

Arrange the following sets of atoms in order of increasing atomic size: (a) \(\mathrm{F}, \mathrm{Cl}, \mathrm{Br}, \mathrm{I}\) (b) \(\mathrm{Mg}\), \(\mathrm{Na}, \mathrm{S}, \mathrm{Al}\) (c) \(\mathrm{Al}, \mathrm{Si}, \mathrm{Ge}, \mathrm{Te}\)

Below are data on the first four ionization energies for a fictitious element \(X\). First ionization energy \(=500 \mathrm{~kJ} / \mathrm{mol}\) Second ionization energy \(=2000 \mathrm{~kJ} / \mathrm{mol}\) Third ionization energy \(=3500 \mathrm{~kJ} / \mathrm{mol}\) Fourth ionization energy \(=25,000 \mathrm{~kJ} / \mathrm{mol}\) From the data, which of the following statements is(are) incorrect? (a) \(\mathrm{X}\) could belong to group IIIA. (b) The fourth ionization energy is so much greater than the third ionization energy because \(\mathrm{X}^{3+}\) consists of a noble-gas core or a pseudo- noble-gas core. (c) The third ionization energy is greater than the second ionization energy because \(\mathrm{X}^{2+}\) has a bigger charge than \(\mathrm{X}^{+}\). (d) \(\mathrm{X}\) could belong to group IIIB. (e) \(X\) could belong to group VA.
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