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Chapter 8: Problem 15

(a) Using Lewis symbols, make a sketch of the reaction between potassium and bromine atoms to give the ionic substance KBr. (b) How many electrons are transferred? (c) Which atom loses electrons in the reaction?

Short Answer

Expert verified
a) The reaction between potassium and bromine atoms using Lewis symbols is represented as: \(K \cdot + :Br: \rightarrow K^+ + :Br^- \rightarrow K^+Br^-\), forming the ionic substance KBr. b) The number of electrons transferred in the reaction is 1. c) Potassium (K) loses electrons in the reaction.

Step by step solution

01

Determine the electron configurations of potassium and bromine atoms

We can find the electron configurations by referring to the periodic table. Potassium has an atomic number of 19 (19 protons and 19 electrons), while Bromine has an atomic number of 35 (35 protons and 35 electrons). Thus, the electron configurations for potassium and bromine are: Potassium (K): 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ Bromine (Br): 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁵
02

Draw the Lewis symbols for potassium and bromine atoms

Lewis symbols show the valence electrons of an atom as dots arranged around the element symbol. For potassium, there is 1 valence electron in the 4s orbital, and for bromine, there are 5 valence electrons in the 4p orbitals. Their respective Lewis symbols are: Potassium (K): K• Bromine (Br): : Br :
03

Sketch the reaction between potassium and bromine using Lewis symbols and identify the ionic substance KBr

Potassium needs to lose 1 electron to attain a stable noble gas configuration, while bromine needs to gain 1 electron to achieve a stable noble gas configuration. Therefore, in the reaction, potassium will transfer its valence electron to bromine, resulting in the formation of the ionic compound KBr. The Lewis symbols for this reaction can be represented as: K• + :Br: → K⁺ + :Br⁻ → K⁺Br⁻
04

Determine the number of electrons transferred in the reaction

During the formation of the ionic bond between potassium and bromine, 1 electron is transferred from potassium to bromine as represented by the Lewis symbols. Therefore, the number of electrons transferred is 1.
05

Identify which atom loses electrons in the reaction

In the reaction, potassium (K) loses 1 electron to attain a stable noble gas configuration. Thus, potassium is the atom that loses electrons in the reaction. To summarize: a) The reaction between potassium and bromine atoms can be represented using Lewis symbols as K• + :Br: → K⁺ + :Br⁻ → K⁺Br⁻, forming the ionic substance KBr. b) The number of electrons transferred in the reaction is 1. c) Potassium (K) is the atom that loses electrons in the reaction.

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Most popular questions from this chapter

True or false: \((\mathbf{a})\) The \(\mathrm{C}-\mathrm{C}\) bonds in benzene are all the same length and correspond to typical single \(\mathrm{C}-\mathrm{C}\) bond lengths. (b) The \(\mathrm{C}-\mathrm{C}\) bond in acetylene, \(\mathrm{HCCH}\), is longer than the average \(\mathrm{C}-\mathrm{C}\) bond length in benzene.

Which ionic compound is expected to form from combining the following pairs of elements? (a) calcium and nitrogen, (b) cesium and bromine, (c) strontium and sulfur, (d) aluminum and selenium.

By referring only to the periodic table, select (a) the most electronegative element in group \(13 ;(\mathbf{b})\) the least electronegative element in the group As, Se and Br; (c) the most electronegative element in the group \(\mathrm{K}, \mathrm{Mg}, \mathrm{Al}\) and \(\mathrm{In} ;(\mathbf{d})\) the element in the group \(\mathrm{Na}, \mathrm{Be}, \mathrm{Si}\), Ar, that is most likely to form an ionic compound with \(\mathrm{Br}\).

(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 4. 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?

What is the Lewis symbol for each of the following atoms or ions? $(\mathbf{a}) \mathrm{Be},(\mathbf{b}) \mathrm{Rb},(\mathbf{c}) \mathrm{I}^{-},(\mathbf{d}) \mathrm{Se}^{2-} .$
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