What is the oxidation number of chlorine in naclo4?

What is the oxidation number of chlorine in naclo4?

Answers

The oxidation number of chlorine can be determined by identifying first the oxidation numbers of oxygen and Na. Oxygen has a charge of -2 and has a total of -8. Na has +1. To make the total zero, Cl has to have a charge of +7. 
2KCl⁺⁵O₃ → 2KCl + 3O₂⁰

reagents
Cl +5
O  -2
K  +1

products
Cl  0
O  -2
K  +1

B, D,E

Explanation:

1) +5

2) -2

3) +1

4) -1

5) 0

6) +1

Explanation:

The rules to determine oxidation number are

a) The oxidation number of alkali metals is +1 (except in super oxides or peroxides).

b) the oxidation number of oxygen is -2 (except in super and peroxide or compounds with fluorine or with itself)

1) the oxidation number of chlorine in the reactant state: KClO₃:

+1 + x + 3(-2) = 0

x = oxidation number of chlorine =+5

2) The oxidation number of oxygen in the reactant state: -2 as it is a normal oxide.

3) The oxidation number of potassium in the reactant state: +1

4) The oxidation number of chlorine in the product state: -1

5 The oxidation number of oxygen in the product state: 0

The compound with itself.

6) The oxidation number of potassium in the product state+ +1 (alkali metal)

Answer- The correct choice of answer out of all would be option C.

Explanation

The given substance magnesium chloride made out of combination of chlorine and magnesium is a compound. Where magnesium has two positive ions and chlorine has two negative ions which trigger the reaction.

Hence the oxidation of the 2 positive ions of Magnesium takes place  and reduction of the Negative Ion chlorine has to offer attract and stabilize each other by forming the compound .

second, fourth, and fifth one

Explanation:

edge told me the answer

This is a three-part question

Answers:

a) The oxidation number of chlorine in bleach (NaOCl) is +1.b) Yes, this is a redox reactionc) The percen yield is 56.8%

Explanation:

1) Part (a) What is the oxidation number of chlorine in bleach (NaOCl)?

a) Rule one: In a neutral compound the sum of the oxidation states is zero.

Since NaOCl is a neutral compound the sum of the oxidation states of Na, O and Cl is 0.

b) Rule two: since Na is an alkaline metal, its oxidation state is +1

c) Rule three: the most common state of oxygen, except in peroxides, is -2.

Then,

Na: +1O:   -2Cl:    x

      Sum = +1 - 2 + x = 0 ⇒ x = 2 - 1 = 1

Conclusion: the oxidation state of NaOCl is +1.

2) Part (b) Is this reaction above redox?  

In a redox reaction the oxidation states of some substances increase (get oxidized) and the oxidation states of some substances decrease (get reduced).

The reaction is represented by the chemical equation given:

NaOH (aq) + Cl₂ (g) → NaOCl (aq) + NaCl (aq) + H₂O (l)

Since the chlorine gas (Cl₂) is a molecule of only chlorine atoms, its oxidation state is zero, and since chlorine is forming compounds on the right side (NaOCl and NaCl) you can immediately conclude that the oxidation state of chlorine changed, and this is a redox reaction.

In fact:

Oxidation state of Cl in Cl₂: 0Oxidation state of Cl in NaOCl: +1 (previously determined)Oxidation state of Cl in NaCl: -1 (becasue Na has oxidation state +1 and so +1 - 1 = 0).

Therefore, chlorine is being oxidized (its oxidation state increases from 0 to +1) and is also being reduced (its oxidation state is reduced from 0 to -1), and this is a redox reaction.

3) Part (c) What is the percent yield of this reaction?

a) Chemical equation (given)

NaOH (aq) + Cl₂ (g) → NaOCl (aq) + NaCl (aq) + H₂O (l)

b) Theoretical mole ratio:

2 mol Cl₂ (g) : 1 mol  NaOCl (aq)

c)  Convert 83.0 g of chlorine gas to moles:

moles = mass in grams / molar massmolar mass of Cl₂(g) = 79.906 g/molmoles = 83.0 g / 79.906 g/mol = 1.039 mol Cl₂(g)

d) Determine the theoretical yiedl using proportions:

x / 1.039 mol Cl₂ (g) = 1 mol NaOCl / 2 mol Cl₂ (g)⇒ x = 0.5195 mol NaOCl

e) Convert 0.5195 mol NaOCl to grams:

molar mass NaOCl = 22.99 g/mol + 16.00 g/mol + 35.453 g/mol = 74.443 g/molmass = number of mol × molar mass = 0.5195 mol × 74.443 g/mol = 38.67 g

         That must be rounded to 3 significant figures (such as the mass of belach is given: 22.0 g)

Theoretical yiedl of NaOCl = 38.7 g

f) Calculate the percent yiled:

Percent yield = (actual yield / theoretical yield) × 100Percent yield = (22.0 g / 38.7 g) × 100 = 56.8%

Zinc is reduced.

The oxidation number of chlorine does not change.

Aluminum is oxidized.

Explanation:

For the reaction:

2AI(s) + 3ZnCI₂(g) → 3Zn(s) + 2AICI₃(aq).

For the elements in the reactants side:

Al has (0) oxidation state and converted to (+3) oxidation state in the products (AlCl₃), which means Al is oxidized and it is the reducing agent.

So, we can check that: Aluminum is oxidized.

Zn has the oxidation state (+2) in the reactants side (ZnCl₂) and converted to (0) in the products side (Zn), which means that Zn is reduced and it is the oxidizing agent.

So, we can check that: Zinc is reduced.

and can not check: Zinc is the reducing agent.  

The oxidation state of Cl does not change, it is the same in both sides (-1).

So, we can check: The oxidation number of chlorine does not change.

and can not check: Aluminum atoms transfer electrons to chlorine atoms.

So, the choices will be:

Zinc is reduced.

The oxidation number of chlorine does not change.

Aluminum is oxidized.

Answer is: A. Magnesium has a 2+ oxidation number and chlorine has a 1- oxidation number. 
Magnesium is metal from second group of Periodic table of elements and it lost two electrons to have electron configuration as closest noble gas neon (₁₀Ne), chlorine is nonmetal from 17. group of Periodic table and it gains one electron to have electron configuration as argon (₁₈Ar).
B. is the correct answer of your question

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