Tin forms compounds in the +2 and +4 oxidation states....

Key Concepts

Oxidation States

Oxidation states indicate the hypothetical charges an atom would have if all bonds were completely ionic. This concept is crucial when an element like a metal can exist in multiple oxidation states, leading to the formation of different compounds with varying properties.

Balancing Chemical Equations

This concept focuses on ensuring that the number of atoms for each element is conserved during a chemical reaction. It involves adjusting the coefficients in a chemical equation so that the mass and charge remain balanced on both sides, reflecting the law of conservation of mass.

Inorganic Compound Nomenclature

Inorganic nomenclature uses systematic naming conventions to clearly communicate the composition and oxidation states of compounds. For example, when a metal forms compounds in different oxidation states, its name is modified with a Roman numeral to indicate its oxidation state, which is essential for distinguishing between the compounds.

Fluorine Reactivity

Fluorine is the most electronegative element and acts as a strong oxidizing agent. Its reactivity allows it to form compounds by oxidizing other elements, illustrating how an element’s high reactivity can lead to multiple possible products depending on the oxidation state of the reacting element.

Transcript

00:01 So tins two oxidation states means that it has two different reactions with fluoride ions.

00:07 So the two oxidation states of tin we want to look at our sn2 plus and 4 plus.

00:18 So if we want to look at their reactions with fluoride, well, that's as simple as let's try it out sn.

00:26 Let's do 2 plus first.

00:30 And then we're going to have plus fluoride, which is one minus.

00:36 Right and if we have as n2 plus and f1 minus well how are these going to react we're going to get s n f however we have one minus on the f and we have two plus on s n so that means that we need two fluorides to balance out the charges because we have one minus here and we have two plus so if we have two of these then we have two one minuses and that balances out that charge.

01:16 So then the last thing we want to do for this first equation, the best on 2 plus is look at is to make sure it's balanced.

01:28 So we have one tin on this side and we have one 10 on this side.

01:33 So that's balanced.

01:34 But we have one fluoride on this side and we have two on this side.

01:40 So all we're going to do is rate two.

01:43 Right here and now we have a balanced equation there so it asks us to name this compound but let's let's look at the other oxidation state first and then we'll name both so now for the other one we have tin 4 plus plus our fluoride ion which is still one minus and in this case again we're gonna have asset f however in this case we have four plus on this, we have one minus on the f.

02:27 So we're going to need four of the fs in order to balance out.

02:33 With this four plus charge, we want that four minus charge to balance it out.

02:38 So now here again, we want to track of the equation as balanced, but we have one 10 over here and one to know here.

02:48 Again, we have four fluorid ions over here.

02:53 And only one over here.

02:55 So let's balance this out by just writing in a four.

03:01 So here are our two reactions with the two oxidation states of tin...