Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory

Problem 10

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Chapter 6, Problem 10

Predict the formula of the ionic compound that forms between potassium and sulfur. (LO 6.11) (a) KS (b) KS₂ (c) K₂S₂ (d) K₂S

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Ionic Compounds

Ionic compounds are formed when atoms transfer electrons, resulting in the formation of positively charged cations and negatively charged anions. The electrostatic attraction between these oppositely charged ions leads to the creation of a stable compound. Understanding the charges of the involved ions is crucial for predicting the correct formula of the ionic compound.

Valency and Charge of Ions

The valency of an element indicates its ability to combine with other elements, often determined by the number of electrons in its outer shell. Potassium (K) has a valency of +1, while sulfur (S) has a valency of -2. This difference in valency is essential for determining the ratio of ions in the resulting ionic compound.

Chemical Formula Representation

The chemical formula of an ionic compound reflects the ratio of the constituent ions. For potassium and sulfur, the correct formula must balance the total positive and negative charges. This involves using subscripts to indicate the number of each type of ion, ensuring that the overall charge of the compound is neutral.

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Molecular Formula

Related Practice

The successive ionization energies for a second-period element are given. What is the identity of the element? (LO 6.8) Ea1 = 1402 kJ/mol Ea2 = 2856 kJ/mol Ea3 = 4578 kJ/mol Ea4 = 7475 kJ/mol Ea5 = 9445 kJ/mol Ea6 = 53,266 kJ/mol Ea7 = 64,630 kJ/mol (a) Be (b) C (c) N (d) F

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Textbook Question

Which of the following processes will release the most energy? (LO 6.9) (a) (b) (c) (d)

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Textbook Question

Elements that have large negative electron affinities generally have (LO 6.10) (a) high values for Zeff and a vacancy in a valence orbital. (b) low values for Zeff and a vacancy in a valence orbital. (c) high values for Zeff and filled valence orbitals. (d) low values for Zeff and filled valence orbitals.

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Textbook Question

Which molecular scale image best represents the ionic com-pound that forms between cesium and chlorine? (Cesium is represented by red circles, and chlorine is represented by blue circles.) (LO 6.12) (a)

(b)

(c)

(d)

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Textbook Question

For a multielectron atom, a 3s orbital lies lower in energy than a 3p orbital because (LO 5.16) (a) a 3p orbital has more nodal surfaces than a 3s orbital. (b) an electron in a 3p orbital has a higher probability of being closer to the nucleus than an electron in a 3s orbital. (c) inner electrons shield electrons in a 3p orbital more effec-tively than electrons in a 3s orbital. (d) the energy of the electron can be spread between three 3p orbitals instead of only one 3s orbital.

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Textbook Question

Given the following information, construct a Born–Haber cycle to calculate the lattice energy of CaCl₂(s). (LO 6.13)

Net energy change for the formation of CaCl₂(s) form Ca(s) and Cl₂(g) = -795.4 kJ/mol