Answer:
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Explanation:
PLEASE NOTE; I HAVE WRITTEN THE ATOMIC NUMBER IN BRACKETS, NEXT TO THE SYMBOL OF THE ELEMENT
Which rule for assigning oxidation numbers is correct?
2 answers:
<em>Oxygen with an oxidation number -2 is the correct oxidation number</em>
<h3><em>Further explanation</em></h3>The formula for determining Oxidation Numbers in general:
- 1. The number of oxidation of single element atoms = 0. Examples of Ar, Mg, Cu, Fe, N₂, O₂, etc. = 0
Group IA (Li, Na, K, Rb, Cs, and Fr): +1
Group IIA (Be, Mg, Ca, Sr and Ba): +2
H in compound = +1, except metal hydride compounds (Hydrogen which binds IA or IIA groups) oxidation number H = -1, for example, LiH, MgH₂, etc.
- 2. Oxidation number O in compound = -2, except OF2 = + 2 and in peroxide (Na₂O₂, BaO₂) = -1 and superoxide, for example KO₂ = -1/2.
- 3 The oxidation number in a non-filled compound = 0,
The total amount of oxidation in ion = ion charge, Example NO₃⁻ = -1
If we see the choice of answers
- 1. Hydrogen is usually –1.
This statement is wrong because generally the value of H is +1 except for the Hydride metal
- 2. Oxygen is usually –2
This statement is true, except the oxygen content of OF2, peroxide and superoxide compounds
- 3. A pure group 1 element is +1
In the form of a single or pure element, all the classes of oxidation are 0, so this statement is wrong
- 4. A monatomic ion is 0
Monoatomic ions consist of one ion atom is composed of several atoms called polyatomic ions
Monoatomic ion is dependent on the ion, such as H + oxidation +1, Ca2 + oxidation +2 etc. So this statement is wrong
<h3><em>Learn more</em></h3>Assign an oxidation number to each element
the reduction process
an element's oxidation
an element's oxidation number increase
Keywords: monoatomic ion, element, The oxidation number
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