Sodium Peroxide Formula: Chemical Formula, Structure and Uses

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The sodium peroxide formula is also referred to as the sodium dioxide formula or the Solozone formula. Sodium peroxide has a molecular formula of Na₂O₂ and is an inorganic peroxide salt. The octahydrate can be obtained by treating hydrogen peroxide and sodium hydroxide together. Sodium peroxide absorbs water and carbon dioxide from the air and is soluble in cold water. It may be an effective oxidizing agent and an effective lowering agent, depending on conditions; It is used as a bleaching agent in wool and yarn processing, and in the refining of oils and fats, and in the manufacturing of timber pulp. Sodium peroxide is likewise used as bleach, in medicine soap, and in the decomposition of minerals. Here, we will learn more about sodium peroxide, its structure, properties, uses and will discuss some important questions.

Other Names: Sodium Dioxide formula, Solozone Formula

Table of Content

What is the Sodium Peroxide formula?
Sodium Peroxide Formula Structure
Sodium Peroxide Formula Properties
Sodium Peroxide preparation
Sodium Peroxide Uses
Sodium peroxide Safety Profile
Things to Remember
Sample Questions

Key Takeaways: Sodium Peroxide, Structure, Properties, Preparation, Uses, Safety Profile

What is Sodium Peroxide Formula?

Sodium peroxide is a granular solid which is a yellowish-white powder that turns yellow in color when heated. When this compound is mixed with combustible materials, it is highly flammable by heat, contact with moisture, or friction. It decomposes rapidly when exposes to heat for a long duration the period. The chemical formula or molecular formula of sodium peroxide is called Na2O2. Sodium dioxide can be produced by reacting metallic sodium with oxygen on a larger scale at temperatures between 130 and 200°C.

Sodium Peroxide

Also check:

Phosphine	Oxides of Nitrogen	Aqua Regia

Sodium Peroxide Structure

The structural formula of sodium peroxide or the structure of Na₂O₂ is given as follows:

Sodium Peroxide Structure

Properties of Sodium Peroxide

The symbol of sodium peroxide is Na₂O₂. Sodium peroxide is stable at ambient temperature and hygroscopic. On heating, it begins to liberate oxygen at around 300 °C and decomposes rapidly above 460 °C. Sodium peroxide is a flammable white powder that turns yellow when heated and ignites when in contact with water. It is stable in dry air; however, it decomposes easily when exposed to moist air or water.

Chemical formula	Na₂O₂
Molecular weight	77.98 g/mol
Density	2.805 g/cm³
Boiling point	657 °C
Melting point	460 °C

Preparation of Sodium Peroxide

The Octahydrate can be made by treating sodium hydroxide with hydrogen peroxide. Sodium peroxide is produced on a large scale by reacting metallic sodium with oxygen at temperatures between 130 and 200 ° C. This is the process of producing sodium oxide, which is a separate step that absorbs oxygen.

It can also be created by placing ozone gas on the solid sodium iodide inside through either Palladium or platinum tube. The Ozone will oxidize sodium to produce sodium peroxide. Iodine can be sublimated with moderate heating. The Palladium or platinum catalyzes the reaction and it is not attacked by sodium peroxide.

Also check:

Noble Gases	Dinitrogen	Oxoacids of Phosphorous

Uses of Sodium Peroxide

Sodium peroxide is hydrolyzed to form hydrogen peroxide and sodium hydroxide according to the following reaction:

Na₂O₂ + 2H₂O → 2NaOH + H₂O₂

Sodium peroxide has historically been used to bleach wood pulp in paper and textile manufacturing. Currently, it is mainly used for special laboratory work. For example, extracting minerals from multiple ores. Sodium peroxide may be sold under the trade names Flocool and Solozone. Sodium peroxide can be used as an oxidizing agent in chemicals. It also reacts with carbon dioxide to form sodium carbonate and oxygen, which serve as a source of oxygen. Therefore, it is especially useful for scuba equipment, submarines, etc.

2Na₂O₂ + 2CO₂ → 2Na₂CO₃ + O₂

Sodium Peroxide Safety Profile

Sodium Peroxide is a strong corrosive oxidizing agent and can cause burns to the eyes and skin, and is also toxic by ingestion and inhalation. Sodium peroxide is water-reactive and possess a dangerous fire and explosion risk when in contact with water, alcohol, or acids. Sodium peroxide forms self-igniting mixtures with powdered metals and organic materials.

Things to Remember

The sodium peroxide formula is also known as the sodium dioxide formula or the Solozone formula.
The chemical formula or molecular formula of sodium peroxide is called Na₂O₂.
Sodium peroxide is a granular solid which is yellow-white in color and highly flammable by heat.
Sodium peroxide is used mostly to bleach wood pulp in textile and paper production. Now, it’s also used for specialized laboratory operations such as extracting minerals from multiple ores. The commercial name of sodium peroxide is Flocool and Solozone. Also, sodium peroxide is used as bleach and as an oxygen-generating material for diving bells and submarines.
When sodium peroxides are dissolved in water, hydrogen peroxides are formed along with sodium hydroxide.
It is incompatible with ethyl or methyl alcohol, glacial acetic acid, carbon disulfide, glycerin, ethylene glycol, and ethyl acetate

Sample Questions

Ques. What is sodium peroxide? (2 Marks)

Ans: Sodium peroxide, or Na₂O₂, is an inorganic compound with the formula Na₂O₂. This yellow solid is produced when sodium is burned in an environment with too much oxygen. It is also a solid foundation. This metal peroxide exists in many peroxyhydrates and hydrates, especially Na₂O₂ · 2H₂O, Na₂O₂ · 2H₂O₂, Na₂O₂ · 2H₂O₂ · 4H₂O, and Na₂O₂ · 8H₂O. Octahydrate, which is very easy to prepare, is a white compound, unlike the anhydrous material.

Ques. What happens when sodium peroxide dissolves in water? (2 Marks)

Ans: On contact with water, sodium peroxide can be hydrolyzed to give hydrogen peroxide and sodium hydroxide.

While sodium peroxide can be used to bleach wood pulp for the production of textiles and paper

Na2O2 + 2H2O –> 2NaOH + H2O2

Ques. Do you distinguish between hydrogen peroxide and sodium hydroxide? (3 marks)

Ans: Hydrogen peroxide is defined as an oxidizing agent. 3% of this solution is used as a topical disinfectant. A higher concentration of about 12% is used to lighten the hair.

Sodium hydroxide is alkaline (or basic). It can be used as a chemical relaxant at a concentration of less than 2%. At the same time, higher concentrations can be used with some chemical depilatory agents. Higher concentrations are used in Drano's commercial drain cleaners.

Ques. What can we get if sodium peroxide is treated with dilute sulphuric acid? (2 Marks)

Ans. When sodium peroxide is treated with dilute sulphuric acid, we get sodium sulfate and hydrogen peroxide.

Na₂O₂+dil.H₂SO₄→ Na₂SO₄+H₂O₂

Ques. What is the safety profile of Sodium Peroxide? (2 Marks)

Ans. The sodium peroxide reacts dangerously with reducing agents, combustible materials, water, alcohol, or any acid. It can cause severe burns to the skin, eyes, and mucous membranes. It is also toxic by ingestion and inhalation and may result in severe injury or death.

Ques. What are the uses of Sodium Peroxide? (3 marks)

Ans. Sodium peroxide has been traditionally used to bleach wood pulp in textile and paper production while it can also use for specialized laboratory operations like extracting minerals from multiple ores. Sodium peroxide is particularly useful in scuba gear, submarines, and so on. In chemistry, sodium peroxide can be used as an oxidizing agent. Moreover, sodium peroxide can be also used with carbon dioxide to form sodium carbonate and oxygen.

Ques. What is the preparation methodology of Sodium Chlorate? (2 marks)

Ans. Sodium peroxide is produced from treating sodium hydroxide with hydrogen peroxide. In this process, the temperature is kept at 130° to 200° C while the sodium peroxide is produced with a reaction of metallic sodium with oxygen.

CBSE CLASS XII Related Questions

1.
How would you account for the following:
Of the d⁴ species, Cr²⁺ is strongly reducing while manganese(III) is strongly oxidising.
Cobalt(II) is stable in aqueous solution but in the presence of complexing reagents it is easily oxidised.
The d¹ configuration is very unstable in ions.

View Solution

2.
Draw the structures of optical isomers of:
(i) \([Cr(C_2O_4)_3]^{3–}\)
(ii) \([PtCl_2(en)_2]^{2+}\)
(iii) \([Cr(NH_3)2Cl_2(en)]^{+}\)

View Solution

3.
Which of the following compounds would undergo aldol condensation, which the Cannizzaro reaction and which neither? Write the structures of the expected products of aldol condensation and Cannizzaro reaction.
\((i) Methanal \)
\((ii) 2-Methylpentanal \)
\((iii) Benzaldehyde \)
\((iv) Benzophenone \)
\((v) Cyclohexanone \)
\((vi) 1-Phenylpropanone \)
\((vii) Phenylacetaldehyde \)
\((viii) Butan-1-ol \)
\((ix) 2, 2-Dimethylbutanal\)

View Solution

4.
Using the standard electrode potentials given in Table 3.1, predict if the reaction between the following is feasible:
(i) Fe³⁺ (aq) and I^- (aq)
(ii) Ag⁺ (aq) and Cu(s)
(iii) Fe³⁺(aq) and Br^-(aq)
(iv) Ag(s) and Fe³⁺(aq)
(v) Br₂ (aq) and Fe²⁺(aq).

View Solution

5.
Discuss briefly giving an example in each case the role of coordination compounds in:
biological systems
medicinal chemistry
analytical chemistry
extraction/ metallurgy of metals

View Solution

6.
Depict the galvanic cell in which the reaction Zn(s) + 2Ag⁺(aq) → Zn²⁺(aq) + 2Ag(s) takes place. Further show:
(i) Which of the electrode is negatively charged?
(ii) The carriers of the current in the cell.
(iii) Individual reaction at each electrode.

View Solution

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Sodium Peroxide Formula: Chemical Formula, Structure and Uses

What is Sodium Peroxide Formula?

Sodium Peroxide Structure

Properties of Sodium Peroxide

Preparation of Sodium Peroxide

Uses of Sodium Peroxide

Sodium Peroxide Safety Profile

Things to Remember

Sample Questions

CBSE CLASS XII Related Questions

1.
How would you account for the following:
Of the d⁴ species, Cr²⁺ is strongly reducing while manganese(III) is strongly oxidising.
Cobalt(II) is stable in aqueous solution but in the presence of complexing reagents it is easily oxidised.
The d¹ configuration is very unstable in ions.

2.
Draw the structures of optical isomers of:
(i) \([Cr(C_2O_4)_3]^{3–}\)
(ii) \([PtCl_2(en)_2]^{2+}\)
(iii) \([Cr(NH_3)2Cl_2(en)]^{+}\)

4.
Using the standard electrode potentials given in Table 3.1, predict if the reaction between the following is feasible:
(i) Fe³⁺ (aq) and I^- (aq)
(ii) Ag⁺ (aq) and Cu(s)
(iii) Fe³⁺(aq) and Br^-(aq)
(iv) Ag(s) and Fe³⁺(aq)
(v) Br₂ (aq) and Fe²⁺(aq).

5.
Discuss briefly giving an example in each case the role of coordination compounds in:
biological systems
medicinal chemistry
analytical chemistry
extraction/ metallurgy of metals

6.
Depict the galvanic cell in which the reaction Zn(s) + 2Ag⁺(aq) → Zn²⁺(aq) + 2Ag(s) takes place. Further show:
(i) Which of the electrode is negatively charged?
(ii) The carriers of the current in the cell.
(iii) Individual reaction at each electrode.

Comments

SUBSCRIBE TO OUR NEWS LETTER

Sodium Peroxide Formula: Chemical Formula, Structure and Uses

What is Sodium Peroxide Formula?

Sodium Peroxide Structure

Properties of Sodium Peroxide

Preparation of Sodium Peroxide

Uses of Sodium Peroxide

Sodium Peroxide Safety Profile

Things to Remember

Sample Questions

CBSE CLASS XII Related Questions

1. How would you account for the following: Of the d4 species, Cr2+ is strongly reducing while manganese(III) is strongly oxidising. Cobalt(II) is stable in aqueous solution but in the presence of complexing reagents it is easily oxidised. The d1 configuration is very unstable in ions.

2. Draw the structures of optical isomers of: (i) \([Cr(C_2O_4)_3]^{3–}\)(ii) \([PtCl_2(en)_2]^{2+}\)(iii) \([Cr(NH_3)2Cl_2(en)]^{+}\)

4. Using the standard electrode potentials given in Table 3.1, predict if the reaction between the following is feasible: (i) Fe3+ (aq) and I- (aq) (ii) Ag+ (aq) and Cu(s) (iii) Fe3+(aq) and Br-(aq) (iv) Ag(s) and Fe3+(aq) (v) Br2 (aq) and Fe2+(aq).

5. Discuss briefly giving an example in each case the role of coordination compounds in:biological systemsmedicinal chemistryanalytical chemistryextraction/ metallurgy of metals

6. Depict the galvanic cell in which the reaction Zn(s) + 2Ag+(aq) → Zn2+(aq) + 2Ag(s) takes place. Further show: (i) Which of the electrode is negatively charged? (ii) The carriers of the current in the cell. (iii) Individual reaction at each electrode.

Comments

SUBSCRIBE TO OUR NEWS LETTER

1.
How would you account for the following:
Of the d⁴ species, Cr²⁺ is strongly reducing while manganese(III) is strongly oxidising.
Cobalt(II) is stable in aqueous solution but in the presence of complexing reagents it is easily oxidised.
The d¹ configuration is very unstable in ions.

2.
Draw the structures of optical isomers of:
(i) \([Cr(C_2O_4)_3]^{3–}\)
(ii) \([PtCl_2(en)_2]^{2+}\)
(iii) \([Cr(NH_3)2Cl_2(en)]^{+}\)

4.
Using the standard electrode potentials given in Table 3.1, predict if the reaction between the following is feasible:
(i) Fe³⁺ (aq) and I^- (aq)
(ii) Ag⁺ (aq) and Cu(s)
(iii) Fe³⁺(aq) and Br^-(aq)
(iv) Ag(s) and Fe³⁺(aq)
(v) Br₂ (aq) and Fe²⁺(aq).

5.
Discuss briefly giving an example in each case the role of coordination compounds in:
biological systems
medicinal chemistry
analytical chemistry
extraction/ metallurgy of metals

6.
Depict the galvanic cell in which the reaction Zn(s) + 2Ag⁺(aq) → Zn²⁺(aq) + 2Ag(s) takes place. Further show:
(i) Which of the electrode is negatively charged?
(ii) The carriers of the current in the cell.
(iii) Individual reaction at each electrode.