Give the name, empirical formula, and molar mass of the compound depicted in Figure P 3.38.

Name: Problem 38, Chapter 3: CHEMISTRY: The Molecular Nature of Matter and Change
Uploaded: 2021-05-08T19:43:14-08:00
Duration: 3 min 39 s
Channel: Shaelyn Deal
Description: Give the name, empirical formula, and molar mass of the compound depicted in Figure P 3.38.

Give the name, empirical formula, and molar mass of the...

Key Concepts

Empirical Formula

The empirical formula represents the simplest whole-number ratio of the elements within a compound, rather than the actual number of atoms in the molecule. It is derived from the percent composition of the compound by mass and provides insight into the basic stoichiometry without necessarily reflecting the exact molecular structure.

Molar Mass Calculation

Molar mass is the mass of one mole of a given substance, calculated by adding together the standard atomic masses of each element present in the compound multiplied by its respective number of atoms. This concept is crucial for converting between the mass of a substance and the number of moles, which is a fundamental aspect of quantitative chemical analysis.

Chemical Compound Nomenclature

This concept involves assigning a systematic name to a compound based on its composition and structure according to established rules, such as those set by IUPAC. It ensures that chemical names are standardized and unambiguous, which is essential for clear communication in chemistry. The nomenclature conveys information about the constituent elements and, sometimes, the arrangement of atoms within the molecule.

Transcript

00:01 In this video, we're going to be learning how to name a compound, how to find its empirical formula, and how to find its molar mass based on this diagram that we were given.

00:10 So the first thing we're going to do is we're going to name this.

00:14 And the first thing that we have to do is identify what elements make up this compound.

00:19 So we're given that we have sulfur here, chlorine here, another sulfur here, and another chlorine here.

00:27 So we have two sulfurs and two chlorines.

00:32 The next thing we need to do is determine whether this is an ionic or a molecular compound.

00:37 An ionic compound is going to have a metal in it, which are all on the left side of the periodic table, whereas a molecular compound is going to have two non -metals.

00:49 So we can see that sulfur is here, chlorine is here, it's on the right.

00:55 They're both on the right, sorry.

00:57 So they are both non -metals.

00:59 That means it's going to be molecular.

01:01 They have slightly different naming convention.

01:05 The next thing we're going to do is determine prefixes because we have multiple atoms that make up this compound.

01:12 So we have two sulfers, two chlorines, and the prefix for two is dye.

01:19 We want to make sure that we also don't forget to add the i'd suffix to the last element in our compound here.

01:28 So that's going to complete our name.

01:30 So we have our prefix, our suffix, and our elements.

01:35 So we have disulfur, dichloride, and that's its name.

01:50 The next thing we're going to do is find the empirical formula.