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PROBLEM

(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

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.

SOLUTION

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

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