Predict the empirical formulas of the ionic compounds formed...

Key Concepts

Naming Ionic Compounds

Naming ionic compounds involves a systematic approach wherein the name of the metal (or cation) is stated first, followed by the name of the non-metal (or anion) with an -ide suffix for simple ions. This nomenclature reflects the composition and arrangement of ions in the compound while making the identity and stoichiometry clear.

Charge Balance and Ionic Charges

Accurate prediction of the stoichiometry of ionic compounds requires balancing the total positive and negative charges. This involves determining the typical ionic charges of the constituent elements, usually based on their group in the periodic table or their common oxidation states, to ensure that the overall charge of the compound is neutral.

Ionic Bonding

Ionic bonding is the physical process through which atoms transfer electrons to form cations and anions, resulting in an electrostatic attraction between oppositely charged ions that holds the compound together. This concept is fundamental to understanding how ionic compounds are formed and the nature of their properties.

Empirical Formula

An empirical formula represents the simplest whole-number ratio of the ions present in an ionic compound. It provides a concise way to express the composition of the compound by indicating the proportions of the different ions.

Transcript

00:01 So in this video we're going to talk about question 48 from chapter 8, which says, predict the empirical formulas of the ionic compounds formed from the following pairs of elements.

00:11 So in a, we have aluminum and chlorine.

00:15 So first let's look at the periodic table to figure out what ions aluminum and chlorine are going to form.

00:22 So remember that elements like to gain or lose electrons in order to have the same electron configuration as the no -es.

00:31 Gases because that's a very stable electron configuration.

00:35 So chlorine is right here.

00:37 That's just one electron away from argon.

00:41 So chlorine is going to react to gain one electron.

00:46 So aluminum is right here and you might think that it's close to argon, but it's actually closer to neon.

00:53 If it were going to be argon, we'd actually have to gain five electrons in order to get to the electronic configuration of argon.

01:00 Or we can lose three electrons to get to the electronic configuration of neon.

01:06 So we're going to lose three electrons.

01:09 So we have al plus three and cl minus.

01:20 So in order to have our minus one charges balancing our plus three charges, we're going to need three of them.

01:27 So this is going to be al, cl3.

01:32 Next we have sodium and oxygen.

01:34 So let's figure out what ions those elements are going to form.

01:39 So sodium is here.

01:40 That's just one electron away from neon.

01:43 So we're going to lose one electron to have the same electronic configuration as neon.

01:47 So sodium forms plus one.

01:49 And then we have oxygen right here, which is also closest to neon.

01:54 So oxygen needs to gain two electrons in order to get to the electronic configuration of neon.

01:59 So oxygen is going to have a minus two charge.

02:01 So we have n -a plus and o minus 2...

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