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 determine 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 lab you find two unlabeled vials containing white powder. You also find the following notes in your partner's notebook-Compound 1: \(40.04 \% \mathrm{M}\) and \(12.00 \%\) C, \(47.96 \%\) O (by mass), Compound \(2: 69.59 \% \mathrm{M}\), \(6.09 \% \mathrm{C},\) and \(24.32 \% \mathrm{O}\) (by mass). (a) What is the empirical formula for Compound 1 and the identity of $\mathrm{M} ?(\mathbf{b})$ What is the empirical formula for Compound 2 and the identity of \(\mathrm{M}\) ? 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 colorless gas. (c) What is the identity of the colorless gas? (d) Write the chemical equation for the decomposition reactions of compound 1 and 2. (e) Are compounds 1 and 2 ionic or molecular?

Step by step solution

01

Calculate the mole ratio of each element in Compound 1

To determine the empirical formula of Compound 1, first, we must find the moles of each element (M, C, and O) based on their mass percentages. Assume we have 100 g of the compound, we can calculate the number of moles as follows: For M: \( \frac{40.04 g}{molar \: mass \: of \: M} \) For C: \( \frac{12.00 g}{12.01\: g/mol} \) For O: \( \frac{47.96 g}{16.00\: g/mol} \) Next, we need to divide each mole value by the smallest mole value of the elements.

02

Determine the empirical formula of Compound 1

Divide all the mole values of Step 1 by the smallest mole value to get the mole ratio, and round them to the nearest whole number to get the empirical formula of Compound 1.

03

Identity of the Group 2 metal M for Compound 1

To find the identity of M, compare the mole ratio calculated in step 2 with the mole ratio of elements in known group 2= metal carbonates, then find the match.

04

Calculate the mole ratio of each element in Compound 2

Use the mass percentages given for Compound 2 to calculate the moles for M, C, and O in the same way as in Step 1.

05

Determine the empirical formula of Compound 2

Divide all the mole values of Step 4 by the smallest mole value to get the mole ratio, and round them to the nearest whole number to get the empirical formula of Compound 2.

06

Identity of the Group 2 metal M for Compound 2

To find the identity of M, compare the mole ratio calculated in step 5 with the mole ratio of elements in known group 2 metal carbonates, then find the match.

07

Identify the colorless gas produced during decomposition

The colorless gas produced during the decomposition of both compounds is a common byproduct of the decomposition of carbonates. In this case, the colorless gas is CO2.

08

Write the chemical equations for the decomposition of compound 1 and 2

Based on the empirical formulas and the gas produced, write the balanced chemical equations for the decomposition of the two compounds.

09

Determine if the compounds are ionic or molecular

Based on the nature of group 2 metal carbonates and the empirical formulas found, determine whether compounds 1 and 2 are ionic or molecular.

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