Textbook Question
The Ti2+ ion is isoelectronic with the Ca atom. (c) What charge would Ti have to be isoelectronic with Ca2+ ?
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Ch.8 - Basic Concepts of Chemical Bonding
Chapter 8, Problem 101
You and a partner are asked to complete a lab entitled “Carbonates of Group 2 metal” 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 and determining the identity of the Group 2 metal (M). In the second lab, you are to determine the melting point of this compound. Upon going to the lab, you find two unlabeled vials containing white powder. You also find the following notes in your partner’s notebook—Compound 1: 40.04% M, 12.00% C, and 47.96% O (by mass); Compound 2: 69.59% M, 6.09% C, and 24.32% O (by mass). (a) What is the empirical formula for Compound 1 and the identity of M? (b) What is the empirical formula for Compound 2 and the identity of M? Upon determining the melting points of these two compounds, you find that both compounds do not melt up to the maximum temperature of your apparatus; instead, the compounds decompose and liberate a colorless gas. (c) What is the identity of the colorless gas?
Verified step by step guidance1
Step 1: To find the empirical formula for Compound 1, start by assuming you have 100 grams of the compound. This means you have 40.04 grams of M, 12.00 grams of C, and 47.96 grams of O.
Step 2: Convert the masses of each element in Compound 1 to moles by dividing by their respective atomic masses (M: unknown, C: 12.01 g/mol, O: 16.00 g/mol).
Step 3: Determine the mole ratio of the elements in Compound 1 by dividing each element's mole value by the smallest number of moles calculated in Step 2. This will give you the subscripts for the empirical formula.
Step 4: Repeat Steps 1-3 for Compound 2 using its composition: 69.59% M, 6.09% C, and 24.32% O. Convert these percentages to grams, then to moles, and find the mole ratio to determine the empirical formula.
Step 5: The colorless gas released upon decomposition of both compounds is likely carbon dioxide (CO₂), as carbonates typically decompose to release CO₂ gas.
Related Practice
Textbook Question
Consider the molecule C4H5N, which has the connectivity shown below. (a) After the Lewis structure for the molecule is completed, how many s and how many p bonds are there in this molecule?
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Textbook Question
The electron affinity of oxygen is -141 kJ/mol, corresponding to the reaction O(g) + e- → O-(g). The lattice energy of K2O(s) is 2238 kJ/mol. Use these data along with data in Appendix C and Figure 7.10 to calculate the 'second electron affinity' of oxygen, corresponding to the reaction O-(g) + e- → O2-(g)
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Textbook Question
One scale for electronegativity is based on the concept that the electronegativity of any atom is proportional to the ionization energy of the atom minus its electron affinity: electronegativity = k1I - EA2, where k is a proportionality constant. (b) Why are both ionization energy and electron affinity relevant to the notion of electronegativity?
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Textbook Question
One scale for electronegativity is based on the concept that the electronegativity of any atom is proportional to the ionization energy of the atom minus its electron affinity: electronegativity = k1I - EA2, where k is a proportionality constant. (c) By using data in Chapter 7, determine the value of k that would lead to an electronegativity of 4.0 for F under this definition.
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Textbook Question
One scale for electronegativity is based on the concept that the electronegativity of any atom is proportional to the ionization energy of the atom minus its electron affinity: electronegativity = k1I - EA2, where k is a proportionality constant. (d) Use your result from part (c) to determine the electronegativities of Cl and O using this scale. Use your result to determine the electronegativity of Cl using this scale.
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