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Chapter 8: Problem 11

Consider the element silicon, Si. (a) Write its electron configuration. (b) How many valence electrons does a silicon atom have? (c) Which subshells hold the valence electrons?

Short Answer

Expert verified
(a) The electron configuration of silicon (Si) is 1s² 2s² 2p⁶ 3s² 3p². (b) Silicon has 4 valence electrons. (c) The subshells holding the valence electrons are 3s and 3p.

Step by step solution

01

(a) Electron Configuration of Silicon (Si)

To write the electron configuration of silicon, we should know its atomic number, which is 14 (it has 14 protons and 14 electrons). Using the periodic table, we follow the order of the subshells (s, p, d, f) as we fill the electrons to reach the atomic number 14. The electron configuration is as follows: 1s² 2s² 2p⁶ 3s² 3p²
02

(b) Number of Valence Electrons

Valence electrons are the electrons present in the outermost energy level of an atom. For silicon, if we look at its electron configuration (1s² 2s² 2p⁶ 3s² 3p²), we observe that the outermost energy level is 3, and it has 2 electrons in the 3s subshell and 2 electrons in the 3p subshell. So, the total number of valence electrons for silicon is: 2 + 2 = 4 valence electrons
03

(c) Subshells Holding Valence Electrons

As we determined in part (b), the valence electrons are in the outermost energy level, which for silicon is energy level 3 (n=3). Looking at the electron configuration, we can identify the subshells holding valence electrons in this energy level: 3s² 3p² So, the subshells holding the valence electrons for silicon are 3s and 3p.

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Most popular questions from this chapter

Write Lewis structures for the following: (a) \(\mathrm{H}_{2} \mathrm{CO}\) (both \(\mathrm{H}\) atoms are bonded to \(\mathrm{C} ),(\mathbf{b}) \mathrm{H}_{2} \mathrm{O}_{2},(\mathbf{c}) \mathrm{C}_{2} \mathrm{F}_{6}\) (contains \(\mathrm{a} \mathrm{C}-\mathrm{C}\) bond), \((\mathbf{d}) \mathrm{AsO}_{3}^{3-},\) (e) \(\mathrm{H}_{2} \mathrm{SO}_{3}(\mathrm{H}\) is bonded to \(\mathrm{O})\) \((\mathbf{f}) \mathrm{NH}_{2} \mathrm{Cl}\)

By referring only to the periodic table, select (a) the most electronegative element in group \(6 \mathrm{A} ;(\mathbf{b})\) the least electronegative element in the group Al, Si, P; (c) the most electronegative element in the group \(\mathrm{Ga}, \mathrm{P}, \mathrm{Cl}, \mathrm{Na} ;(\mathbf{d})\) the element in the group \(\mathrm{K}\) \(\mathrm{C}, \mathrm{Zn}, \mathrm{F}\) that is most likely to form an ionic compound with Ba.

In the following pairs of binary compounds, determine which one is a molecular substance and which one is an ionic substance. Use the appropriate naming convention (for ionic or molecular substances) to assign a name to each compound: (a) \(\mathrm{TiCl}_{4}\) and \(\mathrm{CaF}_{2},(\mathbf{b}) \mathrm{ClF}_{3}\) and \(\mathrm{VF}_{3},(\mathbf{c}) \mathrm{SbCl}_{5}\) and \(\mathrm{AlF}_{3} .\)

Consider the ionic compounds KF, NaCl, NaBr, and LiCl. (a) Use ionic radil (Figure 7.8) to estimate the cation-anion distance for each compound. (b) Based on your answer to part (a), arrange these four compounds in order of decreasing lattice energy. (c) Check your predictions in part (b) with the experimental values of lattice energy from Table \(8.1 .\) Are the predictions from ionic radii correct?

Construct a Born-Haber cycle for the formation of the hypothetical compound NaCl , where the sodium ion has a \(2+\) charge (the second ionization energy for sodium is given in Table 7.2 . (a) How large would the lattice energy need to be for the formation of \(\mathrm{NaCl}_{2}\) to be exothermic? (b) If we were to estimate the lattice energy of \(\mathrm{NaCl}_{2}\) to be roughly equal to that of \(\mathrm{MgCl}_{2}(2326 \mathrm{kJ} / \mathrm{mol}\) from Table 8.1\(),\) what value would you obtain for the standard enthalpy of formation, \(\Delta H_{f}^{\circ},\) of \(\mathrm{NaCl}_{2} ?\)
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