Barium Oxide Formula

Barium oxide is a chemical compound that is also known as barium monoxide or calcined baryta is a non-flammable hygroscopic compound. This means that it has the power to attract and hold the water molecules either by a method of adsorption or absorption at a normal room temperature. It is cubic in structure (structural barium formula) that has an octahedral geometry with six coordinates. Due to the strong electronegativity of oxygen atoms and highly electropositive barium atoms, as they form strong ionic bonds, they arrange themselves in a crystal lattice structure that is tightly packed. Thus the hill barium formula is expressed as Ba1O1 and the normal barium formula is BaO which forms an ionic bond. Thus there is no hybridization of the barium oxide molecule as these bonds are formed from simple electrostatic force and donation of lone pairs of electrons from the barium atom to oxygen to attain a stable octane. Hybridization is used only to explain the nature of overlapping of bonds in covalent compounds and they are not isolated in nature. Barium oxide is used as a drying agent in gasoline and solvents. The 3D structural formula of barium oxide is given below. 

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Formula of Barium Oxide

The chemical formula of its oxide is BaO, where the monoisotopic mass of the barium oxide comes around 153.9 g/mol and its actual molar mass is 153.33 g/mol. The one barium ion neutralizes one oxygen ion to form a stable barium oxide ion. Thus, the linear bond structure of barium is as follows.

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The balanced barium chemical formula can be expressed as follows:

2Ba + O2 → 2BaO

Where the standard molecular enthalpy of formation is -582 J/mol/K at 298 K and the standard molar entropy is 70 J/mol/K at 298 K temperature.

Barium Oxide Ion Formula

Barium oxide formula can be explained with the help of the lewis structure for barium and oxygen ions and the electronic configurations of the two atoms. Now the barium oxide formula according to the electron distribution in different energy levels or shells in two atoms (barium and oxygen) is defined as follows. As from the modern periodic table, the molar charge of barium is taken to be 56. Thus its electrons in shell distribution are given as 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2. Now as the 5p subshell is more stable than the 6s subshell thus one pair of electrons can easily be donated to a much electronegative ion and thus barium form Ba2+ ion. Thus barium is a highly electropositive atom with its electropositivity ( χ = 0.9) Again from the periodic table the atomic number of the oxygen is taken as 8. Thus the electronic configuration of the energy shell is 1s2 2s2 2px2 2py1 2pz1. Now as the 2py1 2pz1 both can accommodate one electron each to make a stable 2p subshell thus oxygen is known to be a high electronegative atom with electronegativity (χ = 3.5). So the difference between the electronegative variant is ( χ = 2.6) which is greater than (χ = 2.0) which indicates that these two atoms form ionic bonds. Now the valence electron in barium is 2 and in the case of oxygen atom is 6. Thus as the oxygen gains two electrons for barium its outer valence shell consists of eight electrons and the octane becomes stable in nature. Thus with the lewis structure, the barium oxide formula of formation becomes more clear.

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Thus the two ions each have octet as their valence electron with stable electronic shells as well as two oppositely charged ions making an ionic bond and thus giving a proper barium oxide formula structurally.

[Ba]2+ + \[\ddot{[:O:]}^{2-}\] gives Ba2+O2- or BaO.

Synthesis of Barium Oxide

The synthesis of the barium chemical formula of its common oxide BaO is done by heating barium carbonate. Barium oxide (barium chemical formula of oxide) can also be synthesised by the thermal decomposition of barium nitrate. Alternatively, it is also produced by the thermal decomposition of various barium salts. The reactions for the generation of the compound is mentioned below.

2Ba + O2 → 2BaO which is a balanced barium chemical formula.

BaCO3 → BaO + CO2

In this particular reaction thermal decomposition of the barium carbonate takes place that results in the formation of Barium oxide with the release of carbon dioxide. All products are in molar ratio 1:1:1. A numeric example related to the above decomposition reaction of BaCO2 is given below.

For example, if a student heats 10gm of a sample of barium carbonate until it is fully thermally decomposed. What will be the volume of carbon dioxide released at the room temperature pressure in the dm3 unit?

Solved example, in order to first find out the no. of moles of BaCO3 we need the molar mass of BaCO3 as we already know the given mass.

Now, no. of moles of BaCO3 = given weight of BaCO3/ molar mass of BaCO3

                                                  = 10 / 197.34

                                                  = 0. 0508

The molar ratio of all the components in the reaction is 1:1:1. Therefore the no. of moles of CO2 will also be 0.0508. 

Now, in room temperature and pressure volume of one mole of CO2 = 24 dm3

Therefore, volume of 0.0508 moles of CO2 = (24 X 0.0508) / 1

                                                                            = 1.22 dm3

The physical properties of barium oxide (BaO) is as follows:-

Physical Properties of Barium Oxide

Chemical Properties of BaO as Follows:-

Uses 

The uses of Barium oxide is as follows:

1. For cathode ray tubes, barium oxide is used as a coating for hot cathode tubes.

2. Barium oxide is used to make crown glass nowadays. Before barium oxide, it was lead oxide that was used for the same but it eventually increases the dispersive power of the crown glass thus its refractive property declines and becomes difficult to shine. But barium oxide is observed to raise the refractive index of the crown glass.

3. Barium oxide is used as a common catalyst in the reaction of ethylene oxide with alcohol as an ethoxylation catalyst and the reaction generally takes place at 150 to 200oC.

4. It is applied in the isomer isolation process

5. It is used as a reducing agent in many fuel productions.

6. It works as one of the best oxidizing agents.

7. By heat fluctuation process, it can be used as a source of pure oxygen. It can be readily reduced to BaO2 through the formation of peroxide ions. 

Safety Issues

Barium oxide is an irritant. Thus if it comes in contact with eyes or with skin or if it is inhaled mistakenly then it causes redness and irritation. But it becomes more dangerous if it is ingested and can cause muscle paralysis, diarrhoea, cardiac arrest and even can be a cause of death. Thus in case of ingestion of barium oxide immediate medical attention is a must.  As it is also harmful to aquatic life, it shouldn't be released into the environment directly.