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Chapter 8: Problem 13

Write the Lewis symbol for atoms of each of the following elements: (a) \(\mathrm{Al}\), (b) \(\mathrm{Br}\), (c) \(\mathrm{Ar}\), (d) \(\mathrm{Sr}\).

Short Answer

Expert verified
The Lewis symbols for the given elements are: (a) Al: \[\chemfig{Al(-[:0,.5]-[,0.5]H)(-[:90,.5]-[,0.5]H)(-[:180,.5]-[,0.5]H)}\] (b) Br: \[\chemfig{Br(-[:0,.5]-[,0.5]H)(-[:90,.5]-[,0.5]H)(-[:180,.5]-[,0.5]H)(-[:225,.5]-[,0.5]H)(-[:270,.5]-[,0.5]H)(-[:315,.5]-[,0.5]H)}\] (c) Ar: \[\chemfig{Ar(-[:0,.5]-[,0.5]H)(-[:45,.5]-[,0.5]H)(-[:90,.5]-[,0.5]H)(-[:135,.5]-[,0.5]H)(-[:180,.5]-[,0.5]H)(-[:225,.5]-[,0.5]H)(-[:270,.5]-[,0.5]H)(-[:315,.5]-[,0.5]H)}\] (d) Sr: \[\chemfig{Sr(-[:0,.5]-[,0.5]H)(-[:45,.5]-[,0.5]H)}\]

Step by step solution

01

Determine the number of valence electrons

Aluminium is in group 13 of the periodic table, which means it has 3 valence electrons.
02

Write the Lewis symbol

To write the Lewis symbol, place the chemical symbol in the center and arrange the three valence electrons around it, with two on one side and one on the other side. Lewis symbol for Aluminium (Al) is: \[ \chemfig{Al(-[:0,.5]-[,0.5]H)(-[:90,.5]-[,0.5]H)(-[:180,.5]-[,0.5]H)} \] (b) Bromine (Br)
03

Determine the number of valence electrons

Bromine is in group 17 of the periodic table, which means it has 7 valence electrons.
04

Write the Lewis symbol

To write the Lewis symbol, place the chemical symbol in the center and arrange the seven valence electrons around it, with four placed on one side and three on the other side. Lewis symbol for Bromine (Br) is: \[ \chemfig{Br(-[:0,.5]-[,0.5]H)(-[:90,.5]-[,0.5]H)(-[:180,.5]-[,0.5]H)(-[:225,.5]-[,0.5]H)(-[:270,.5]-[,0.5]H)(-[:315,.5]-[,0.5]H)} \] (c) Argon (Ar)
05

Determine the number of valence electrons

Argon is in group 18 of the periodic table, which means it has 8 valence electrons.
06

Write the Lewis symbol

To write the Lewis symbol, place the chemical symbol in the center and arrange the eight valence electrons around it. As Argon is a noble gas, it has a full octet and doesn't usually form bonds with other elements. Lewis symbol for Argon (Ar) is: \[ \chemfig{Ar(-[:0,.5]-[,0.5]H)(-[:45,.5]-[,0.5]H)(-[:90,.5]-[,0.5]H)(-[:135,.5]-[,0.5]H)(-[:180,.5]-[,0.5]H)(-[:225,.5]-[,0.5]H)(-[:270,.5]-[,0.5]H)(-[:315,.5]-[,0.5]H)} \] (d) Strontium (Sr)
07

Determine the number of valence electrons

Strontium is in group 2 of the periodic table, which means it has 2 valence electrons.
08

Write the Lewis symbol

To write the Lewis symbol, place the chemical symbol in the center and arrange the two valence electrons on one side. Lewis symbol for Strontium (Sr) is: \[ \chemfig{Sr(-[:0,.5]-[,0.5]H)(-[:45,.5]-[,0.5]H)} \]

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Most popular questions from this chapter

(a) Write the electron configuration for the element titanium, Ti. How many valence electrons does this atom possess? (b) Hafnium, Hf, is also found in group 4B. Write the electron configuration for Hf. (c) Ti and Hf behave as though they possess the same number of valence electrons. Which of the subshells in the electron configuration of Hf behave as valence orbitals? Which behave as core orbitals?

Write the electron configuration for each of the following ions, and determine which ones possess noble-gas configurations: (a) \(\mathrm{Sr}^{2+}\), (b) \(\mathrm{Ti}^{2+}\), (c) \(\mathrm{Se}^{2-}\), (d) \(\mathrm{Ni}^{2+}\), (e) \(\mathrm{Br}^{-}\), (f) \(\mathrm{Mn}^{3+}\).

(a) True or false: An element's number of valence electrons is the same as its atomic number. (b) How many valence electrons does a nitrogen atom possess? (c) An atom has the electron configuration \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{2}\). How many valence electrons does the atom have?

Predict the chemical formula of the ionic compound formed between the following pairs of elements: (a) \(\mathrm{Al}\) and \(\mathrm{F}\), (b) \(\mathrm{K}\) and \(\mathrm{S}\), (c) \(\mathrm{Y}\) and \(\mathrm{O}\), (d) \(\mathrm{Mg}\) and \(\mathrm{N}\).

The compound chloral hydrate, known in detective stories as knockout drops, is composed of \(14.52 \% \mathrm{C}, 1.83 \% \mathrm{H}\), \(64.30 \% \mathrm{Cl}\), and \(13.35 \% \mathrm{O}\) by mass, and has a molar mass of \(165.4 \mathrm{~g} / \mathrm{mol}\). (a) What is the empirical formula of this substance? (b) What is the molecular formula of this substance? (c) Draw the Lewis structure of the molecule, assuming that the \(\mathrm{Cl}\) atoms bond to a single \(\mathrm{C}\) atom and that there are \(\mathrm{C}-\mathrm{C}\) bond and two \(\mathrm{C}-\mathrm{O}\) bonds in the compound.
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