Write a general equation for the reaction of an alkali metal with each substance. a. a halo

Write a general equation for the reaction of an alkali metal...

Key Concepts

Redox Reactions

Redox reactions involve the transfer of electrons between reactants. In the context of alkali metals, these reactions illustrate the loss of electrons (oxidation) by the metal and the gain of electrons (reduction) by compounds such as halogens and water, leading to the formation of various ionic compounds.

Reaction with Water

The reaction of an alkali metal with water is an exothermic process that produces a metal hydroxide and hydrogen gas. Here, the alkali metal is oxidized, and water acts as an oxidizing agent, leading to a double displacement reaction that also demonstrates redox chemistry.

Reaction with Halogens

When alkali metals react with halogens, the metals donate their valence electron to the halogen atoms, resulting in the formation of ionic metal halides. This type of reaction exemplifies a redox process, where the alkali metal is oxidized and the halogen is reduced.

Alkali Metals

Alkali metals are highly reactive elements found in group 1 of the periodic table. They readily lose one electron to form cations, which is why they react vigorously with other substances. Their reactivity underpins many of their characteristic reactions, including those with halogens and water.

Transcript

00:01 So this video will take a look at the reactions between an alkali metal plus a halogen and an alkaline metal plus water.

00:07 But before we can do that, we need to understand the general characteristics of an alkali metal.

00:15 So keep in mind that alkaline metals are group one metals.

00:18 They're on that first column on that periodic table.

00:22 And as such, they have a very low ionization energy, low ionization energy.

00:32 Right and that makes sense if you think about it because if you think about you know an atom with its nucleus surrounded by electron clouds right on its outermost electron cloud its valence shell it has exactly one electron and it really really wants to give up that electron so that it can achieve its stable octet state so just know that alkali metals are willing to give up electrons they want to get rid of them so that in mind let's look at this reaction right here alkali metal plus a halogen so i'm going to abbreviate alkali metal.

01:05 I'm going to use the symbol m for metal, and i'll use x for halogen.

01:12 So before you can write out this reaction, we need to note one thing about halogens, right? and the one thing is that they exist as diatonic particles, which means that in nature, they exist bonding to each other.

01:23 You're never going to see a fluorine molecule floating around by itself.

01:26 So it's always going to exist as f2.

01:28 You're ever going to see oxygen floating around by itself.

01:30 It's going to be, or oxygen is not a halogen, so it's a bad example.

01:35 You're never going to see chlorine floating around by itself.

01:37 It's always going to be cl2.

01:40 So keeping that in mind, let's draw our reactants.

01:43 So we have our alkali metal, which is x, and we have our halogen, which is going to be, or sorry, i messed that up.

01:51 We have our alkaline metal, which is m, and we have our halogen, which is x.

01:59 And since the diatomic, it's 2x.

02:02 So each of these halogen molecules is going to accept one electron, and each of these metal atoms are going to donate one electron because they want to get rid of it.

02:12 The problem is since we have two halogens, we need two electrons to be transferred from metal to halogens.

02:20 So in that case, we know that we need two metal atoms so that they can each donate one electron to each of the two halogens right here.

02:28 The net product of this reaction is going to be 2mx, 2 molecules where the metal is ionically bound to the halogen.

02:39 Let's move on to water.

02:41 So we're going to use the same naming conventions.

02:43 I'm going to use m to represent metal, and i'm going to be using h2o to represent water.

02:50 So let's draw it out...

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