Math  /  Numbers & Operations

Question(1) Oxygen atoms don't take positive oxidation number except on binding with \qquad (a) Fluorine 2F{ }^{2} F (b) Chlorine 17Cl{ }_{17} \mathrm{Cl} (c) Hydrogen 1H{ }_{1} H (c) Sulphur 16SS{ }_{16 S} S

Studdy Solution

STEP 1

What is this asking? Which element makes oxygen have a positive oxidation number? Watch out! Oxygen usually has a negative oxidation state, so this is a special case!

STEP 2

1. Oxidation Number Rules
2. Analyze Options

STEP 3

Hey everyone!
Let's talk about *oxidation numbers*!
They're like little tags we put on elements in a compound to keep track of the electrons.
Remember, oxygen *loves* electrons.
It's super electronegative, which means it usually hogs them and gets a **negative oxidation number**, typically 2-2.

STEP 4

But, there's a twist!
Sometimes, oxygen meets an element that's *even more* electronegative than it is, and that element steals oxygen's electrons!
This leaves oxygen with a **positive oxidation number**.
So, we're looking for that super electron-hungry element.

STEP 5

Let's check out our options.
We've got **fluorine**, **chlorine**, **hydrogen**, and **sulfur**.

STEP 6

**Fluorine (F)** is the *most* electronegative element on the periodic table.
It's like the ultimate electron ninja!
So, when oxygen bonds with fluorine, fluorine wins the electron tug-of-war, and oxygen ends up with a **positive oxidation number**.
For example, in OF2OF_2, oxygen has an oxidation number of +2+2.

STEP 7

**Chlorine (Cl)** is also pretty electronegative, but not as much as fluorine.
While chlorine *can* sometimes wrestle electrons away from oxygen, it's not as common.

STEP 8

**Hydrogen (H)** is much less electronegative than oxygen.
In water (H2OH_2O), oxygen pulls electrons away from hydrogen, giving oxygen its usual 2-2 oxidation state.

STEP 9

**Sulfur (S)** is also less electronegative than oxygen.
So, oxygen will typically have a negative oxidation state when bonded with sulfur.

STEP 10

The element that makes oxygen take a positive oxidation number is **(a) Fluorine**.

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