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Chapter 8: Problem 31

Using Lewis symbols and Lewis structures, diagram the formation of \(\mathrm{SiCl}_{4}\) from \(\mathrm{Si}\) and \(\mathrm{Cl}\) atoms.

Short Answer

Expert verified
In the formation of SiCl4, Silicon (Si) has 4 valence electrons, and Chlorine (Cl) has 7 valence electrons. The Lewis symbols are represented as 鈰�:Si:鈰� and 鈰�:Cl:. In the Lewis structure, Si forms 4 bonds with 4 chlorine atoms, creating a single bond by sharing one valence electron from each Cl atom. The resulting Lewis structure is: :Cl: | :Cl: 鈥� Si 鈥� :Cl: | :Cl: Si is the central atom, and there are 4 single bonds in the SiCl4 molecule.

Step by step solution

01

Determine the Valence Electrons of Si and Cl atoms

First, we need to figure out the number of valence electrons for Si and Cl atoms. Silicon (Si) belongs to Group 14, which means it has 4 valence electrons. Chlorine (Cl) belongs to Group 17, with 7 valence electrons for each atom.
02

Draw the Lewis Symbols for Si and Cl atoms

Now we'll draw the Lewis symbols for Si and Cl atoms using dots to represent their valence electrons: Si:鈰�:Si:鈰� Cl:鈰�:Cl: In Lewis symbols, we place dots around the elements that represent their valence electrons.
03

Draw the Lewis Structure for the Formation of SiCl4

Now, we will draw the Lewis structure for the formation of SiCl4. Since Si has 4 valence electrons, it can form 4 bonds with 4 chlorine atoms. Each Cl atom will share one of its valence electrons with Si to form a single bond. To do this, move one electron from each Cl atom towards the Si atom to create a bond between them: :Cl: | :Cl: 鈥� Si 鈥� :Cl: | :Cl: Great! Now we've got the Lewis structure for the formation of SiCl4, where the Si atom is the central atom bonded to four Cl atoms, making a total of 4 single bonds.

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Most popular questions from this chapter

Barium azide is \(62.04 \%\) Ba and \(37.96 \%\) N. Each azide ion has a net charge of 1 -. (a) Determine the chemical formula of the azide ion. (b) Write three resonance structures for the azide ion. (c) Which structure is most important? (d) Predict the bond lengths in the ion.

(a) What is the octet rule? (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?

Consider the nitryl cation, \(\mathrm{NO}_{2}^{+}\). (a) Write one or more appropriate Lewis structures for this ion. (b) Are resonance structures needed to describe the structure? (c) With what familiar molecule is it isoelectronic?

(a) Based on the lattice cncrgics of \(\mathrm{MgCl}_{2}\) and \(\mathrm{SrCl}_{2}\) given in Table 8.2, what is the range of values that you would expect for the lattice energy of \(\mathrm{CaCl}_{2}\) ? (b) Using data from Appendix C, Figure 7.12, and Figure \(7.14\) and the value of the second ionization energy for \(\mathrm{Ca}\), \(1145 \mathrm{~kJ} / \mathrm{mol}\), calculate the lattice energy of \(\mathrm{CaCl}_{2}\).

Under special conditions, sulfur reacts with anhydrous liquid ammonia to form a binary compound of sulfur and nitrogen. The compound is found to consist of \(69.6 \% \mathrm{~S}\) and \(30.4 \%\) N. Measurements of its molecular mass yield a value of \(184.3 \mathrm{~g} \mathrm{~mol}^{-1} .\) The compound occasionally detonates on being struck or when heated rapidly. The sulfur and nitrogen atoms of the molecule are joined in a ring. All the bonds in the ring are of the same length. (a) Calculate the empirical and molecular formulas for the substance. (b) Write Lewis structures for the molecule, based on the information you are given. (Hint: You should find a relatively small number of dominant Lewis structures.) (c) Predict the bond distances between the atoms in the ring. (Note: The \(\mathrm{S}-\mathrm{S}\) distance in the \(S_{8}\) ring is \(2.05 \AA\).) (d) The enthalpy of formation of the compound is estimated to be \(480 \mathrm{~kJ} \mathrm{~mol}^{-1}\). \(\Delta H_{f}^{\circ}\) of \(S(g)\) is \(222.8 \mathrm{~kJ} \mathrm{~mol}^{-1}\). Estimate the average bond enthalpy in the compound.
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