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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 1s虏 2s虏 2p鈦� 3s虏 3p虏. (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: 1s虏 2s虏 2p鈦� 3s虏 3p虏
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 (1s虏 2s虏 2p鈦� 3s虏 3p虏), 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: 3s虏 3p虏 So, the subshells holding the valence electrons for silicon are 3s and 3p.

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Most popular questions from this chapter

(a) True or false: The hydrogen atom is most stable when it has a full octet of electrons. (b) How many electrons must a sulfur atom gain to achieve an octet in its valence shell? (c) If an atom has the electron configuration \(1 s^{2} 2 s^{2} 2 p^{3},\) how many electrons must it gain to achieve an octet?

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 \(\mathrm{NaCl}_{2} ?\)

Arrange the bonds in each of the following sets in order of increasing polarity: (a) \(\mathrm{C}-\mathrm{F}, \mathrm{O}-\mathrm{F}, \mathrm{Be}-\mathrm{F}\) ; (b) \(\mathrm{O}-\mathrm{Cl}, \mathrm{S}-\mathrm{Br}, \mathrm{C}-\mathrm{P} ;(\mathbf{c}) \mathrm{C}-\mathrm{S}, \mathrm{B}-\mathrm{F}, \mathrm{N}-\mathrm{O}\)

In the vapor phase, \(\mathrm{BeCl}_{2}\) exists as a discrete molecule. (a) Draw the Lewis structure of this molecule, using only single bonds. Does this Lewis structure satisfy the octet rule? (b) What other resonance structures are possible that satisfy the octet rule? (c) On the basis of the formal charges, which Lewis structure is expected to be dominant for BeCl_ \(_{2} ?\)

State whether each of these statements is true or false. (a) The longer the bond, the larger the bond enthalpy. (b) \(C-C\) bonds are stronger than \(C-H\) bonds. (c) A typical single bond length is in the \(5-10\) 脛 range. (d) If you break a chemical bond, energy is released.(e) Energy is stored in chemical bonds.
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