chapter 7 section 2

Oxidation number, oxidation numbers are usefull in?

In order to indicate the general distribution of electrons among the bonded atoms in a molecular compound or polyatomic ion oxidation numbers are assigned to the atoms composing the compound or ion , naming compounds writing formulas and balancing chemical equations

Assigning oxidation numbers, shared electrons are assumed to belong to the?

More electronegative atom

1 the atoms in pure elements have an oxidation numbers of zero

2 the more electronegative atom will be assigned a number equal to the negative charge and the less electronegtive will be assigned a number equal to the positeve charge

3 flourine is allways -1

4 oxygen is allways -2 only not with peroxide when its -1 and not with flourine which its +2

5 hydrogen is +1 when elements are more electronegative than ut but its -1 with metals

6the algebraic sum of the xoidation numbers is equal to zero

7 the algebraic sum of polyatomic ions is equal to the charge of the ion

8 covalent and ionec compounds both can use oxidation numbers

9 a monatomic ions has an oxidation number equal to its charge can be negative positeve etc

What are the values we allways know?

C=4 o and h and flourine

For the stock system we use its own first oxidation ?

At first without change