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Chapter 8: Problem 73

How many elements in the periodic table are represented by a Lewis symbol with a single dot? Are all these elements in the same group? Explain.

Short Answer

Expert verified
There are 7 elements in the periodic table represented by a Lewis symbol with a single dot: Hydrogen (H), Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb), Cesium (Cs), and Francium (Fr). These elements are all in the same group, Group 1, also known as alkali metals. They share similar chemical properties, being highly reactive and forming +1 ions, due to having one valence electron.

Step by step solution

01

Understanding Lewis Symbols

A Lewis symbol represents an atom, and specifically, its valence electrons (the electrons in the outermost shell). Lewis symbols consist of the chemical symbol of the element surrounded by dots representing valence electrons. The number of dots around the symbol is equal to the number of valence electrons an element has.
02

Identifying elements with a single dot in their Lewis symbols

Since we are looking for Lewis symbols with a single dot, this means that these elements have only one valence electron. Elements have increasing numbers of valence electrons as we move from left to right across a period. In the first and second periods (rows) of the periodic table, we can find elements in the first group (column), also known as alkali metals, which have one valence electron. These elements are: 1. Hydrogen (H) 2. Lithium (Li) 3. Sodium (Na) 4. Potassium (K) 5. Rubidium (Rb) 6. Cesium (Cs) 7. Francium (Fr)
03

Determining if these elements are in the same group and explain

All these elements with a single dot in their Lewis symbols are found in Group 1 of the periodic table, also known as alkali metals. This group is defined by elements having one valence electron. Elements in the same group share similar chemical properties, and in the case of alkali metals, they are highly reactive and form +1 ions. Hence, the elements represented by a Lewis symbol with a single dot are indeed in the same group, called the alkali metals.

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Most popular questions from this chapter

Draw Lewis structures for the following: (a) \(\mathrm{SiH}_{4}\), (b) \(\mathrm{CO}\), (c) \(\mathrm{SF}_{2}\), (d) \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{H}\) is bonded to \(\mathrm{O})\), (e) \(\mathrm{ClO}_{2}^{-}\) (f) \(\mathrm{NH}_{2} \mathrm{OH}\).

You and a partner are asked to complete a lab entitled "Oxides of Ruthenium" that is scheduled to extend over two lab periods. The first lab, which is to be completed by your partner, is devoted to carrying out compositional analysis. In the second lab, you are to determine melting points. Upon going to lab you find two unlabeled vials, one containing a soft yellow substance and the other a black powder. You also find the following notes in your partner's notebook-Compound 1: \(76.0 \%\) Ru and \(24.0 \%\) O (by mass), Compound 2: \(61.2 \%\) Ru and \(38.8 \% \mathrm{O}\) (by mass). (a) What is the empirical formula for Compound \(1 ?\) (b) What is the empirical formula for Compound 2? (c) Upon determining the melting points of these two compounds, you find that the yellow compound melts at \(25^{\circ} \mathrm{C}\), while the black powder does not melt up to the maximum temperature of your apparatus, \(1200^{\circ} \mathrm{C}\). What is the identity of the yellow compound? What is the identity of the black compound? Be sure to use the appropriate naming convention depending upon whether the compound is better described as a molecular or ionic compound.

Draw the Lewis structures for each of the following ions or molecules. Identify those that do not obey the octet rule, and explain why they do not. (a) \(\mathrm{SO}_{3}{ }^{2-}\), (b) \(\mathrm{AlH}_{3}\), (c) \(\mathrm{N}_{3}^{-}\), (d) \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\), (e) \(\mathrm{SbF}_{5}\).

(a) State the octet rule. (b) Does the octet rule apply to ionic as well as to covalent compounds? Explain, using examples as appropriate.

The iodine monobromide molecule, IBr, has a bond length of \(2.49 \AA\) and a dipole moment of \(1.21 \mathrm{D}\). (a) Which atom of the molecule is expected to have a negative charge? Explain. (b) Calculate the effective charges on the I and Br atoms in IBr, in units of the electronic charge \(e\).
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