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Leya [2.2K]
2 years ago
13

Determine The Oxidation Number for

Chemistry
1 answer:
bixtya [17]2 years ago
7 0

Answer:

A is +4

B is +4

C is +6

D is +3

E is +4

Explanation:

In order to learn how to find the oxidation number of an atom in a given compound, it is important to learn what oxidation numbers are. The oxidation number of an atom is a number that represents the total number of electrons lost or gained by it.

Calculating Oxidation Numbers

An oxidation number can be assigned to a given element or compound by following the following rules.

Any free element has an oxidation number equal to zero.

For monoatomic ions, the oxidation number always has the same value as the net charge corresponding to the ion.

The hydrogen atom (H) exhibits an oxidation state of +1. However, when bonded with an element with less electronegativity than it, it exhibits an oxidation number of -1.

Oxygen has an oxidation of -2 in most of its compounds. However, in the case of peroxides, the oxidation number corresponding to oxygen is -1.

All alkali metals (group 1 elements) have an oxidation state of +1 in their compounds.

All alkaline earth metals (group 2 elements) exhibit an oxidation state of +2 in their compounds.

In the compounds made up of two elements, a halogen (group 17 elements) have an oxidation number of -1 assigned to them.

In the case of neutral compounds, the sum of all the oxidation numbers of the constituent atoms totals to zero.

When polyatomic ions are considered, the sum of all the oxidation numbers of the atoms that constitute them equals the net charge of the polyatomic ion.

Thus, the oxidation number of an atom in a given compound can be calculated with the steps mentioned above.

How to Calculate Oxidation Number

.

Hydrochloric Acid (HCl)

As per the rules discussed above, the oxidation state of a group 17 element (halogen) in a diatomic molecule is -1. It is also discussed that hydrogen always exhibits an oxidation number of +1 unless it is paired with a less electronegative element.

Since chlorine is more electronegative than hydrogen, an oxidation number of +1 can be assigned to the hydrogen atom in HCl.

Therefore, the oxidation number of hydrogen is +1 and the oxidation of chlorine is -1 in HCl. These values can be verified by adding these oxidation numbers. Since the total is zero, which is the value of the oxidation number corresponding to a neutral molecule, the values are verified.

Carbon Dioxide (CO2)

According to the rules to calculate oxidation number, which can be found in the previous subsection, the oxidation number of oxygen in its compounds (excluding peroxides) is -2.

Since there are two oxygen atoms in carbon dioxide, the total of the oxidation numbers corresponding to each oxygen is -4.

Since the CO2 molecule is neutral, the carbon atom must exhibit an oxidation state of +4 (the sum of all the oxidation numbers in a neutral molecule is zero).

Therefore, the oxidation state of oxygen was found to be -2 and the oxidation number of carbon is +4 in a carbon dioxide molecule.

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the correct ans is 2....

5 0
3 years ago
What is the mass in grams of 14.2 liters of sulfur dioxide gas at STP?
ICE Princess25 [194]

Answer:

Mass = 40.4 g

Explanation:

Given data:

Mass in gram = ?

Volume of SO₂ = 14.2 L

Temperature = standard = 273 K

Pressure =  standard = 1 atm

Solution:

The given problem will be solve by using general gas equation,

PV = nRT

P= Pressure

V = volume

n = number of moles

R = general gas constant = 0.0821 atm.L/ mol.K  

T = temperature in kelvin

1 atm × 14.2 L = n × 0.0821 atm.L/ mol.K   × 273 K

14.2 atm.L = n ×  22.41 atm.L/ mol

n = 14.2 atm.L/22.41 atm.L/ mol

n = 0.63 mol

Mass of sulfur dioxide:

Mass = number of moles × molar mass

Mass = 0.63 mol × 64.1 g/mol

Mass = 40.4 g

7 0
2 years ago
BRAINLIESTTT ASAP!! PLEASE HELP ME :)
Ratling [72]

Jot down the formula of the ionic compound. Let's say the ionic compound you're working with is NaCl.  

Write the name of the metal.

Add the name of the non-metal with an –ide ending.

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7 0
3 years ago
Which property of gases allows them to be stored at high concentrations in a bottle of air freshener?
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7 0
2 years ago
Read 2 more answers
When 18.5 g of HgO(s) is decomposed to form Hg(l) and O2(g), 7.75 kJ of heat is absorbed at standard-state conditions. What is t
taurus [48]

Answer:

The standard enthalpy of formation of HgO is -90.7 kJ/mol.

Explanation:

The reaction between Hg and oxygen is as follows.

\text{Hg(l)}+\frac{1}{2}{O_{2}\rightarrow \text{HgO(s)}

From the given,

Molar mass of HgO = 216.59 g/mol

Mass of HgO decomposed = 18.5 g

Amount of heat absorbed = 7.75 kJ

From the reaction,

The standard  enthalpy of formation = +7.75\times\frac{kJ}{18.5 g}\frac{216.59}{1mol} \,\,= +90.7 kJ/mol

During the decomposition of 1 mol of HgO , 90.7 kJ of energy absorbed.

For the formation of 1 mol of HgO , 90.7 kJ of energy is release

Therefore, the enthalpy of formation of mercury(II)Oxide is -90.7 kJ/mol

5 0
3 years ago
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