The formulas for the two stable oxides of carbon except carbon dioxide are to be stated. The bonding in each of these forms is to be explained using localized electron model. Concept introduction: When the atomic orbitals overlap with each other in the region where density of electrons is high, then molecular orbitals are formed. Overlap of the atomic orbitals determines the efficiency of the interaction between the atomic orbitals. To determine: The formulas for the two stable oxides of carbon except carbon dioxide and an explanation for bonding in each of these forms using localized electron model.

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Interpretation: The formulas for the two stable oxides of carbon except carbon dioxide are to be stated. The bonding in each of these forms is to be explained using localized electron model.

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Concept introduction: When the atomic orbitals overlap with each other in the region where density of electrons is high, then molecular orbitals are formed. Overlap of the atomic orbitals determines the efficiency of the interaction between the atomic orbitals.

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To determine: The formulas for the two stable oxides of carbon except carbon dioxide and an explanation for bonding in each of these forms using localized electron model.

\r\n', 'sectionSequence': 0, 'computed': {'sectionNameWithHtmlRemoved': 'Interpretation Introduction', 'sectionTextWithHtmlRemoved': 'Interpretation: The formulas for the two stable oxides of carbon except carbon dioxide are to be stated. The bonding in each of these forms is to be explained using localized electron model. Concept introduction: When the atomic orbitals overlap with each other in the region where density of electrons is high, then molecular orbitals are formed. Overlap of the atomic orbitals determines the efficiency of the interaction between the atomic orbitals. To determine: The formulas for the two stable oxides of carbon except carbon dioxide and an explanation for bonding in each of these forms using localized electron model.'}}, {'sectionName': 'Explanation', 'sectionText': '\r\n

Explanation

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The two additional stable oxides of carbon is \r\nCO\r\n and \r\nC3O2\r\n.

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There are four valence electrons on carbon and six valence electrons on oxygen atom. Therefore the total valence electrons in \r\nCO\r\n is \r\n4+6=10\r\n. There is triple bond between carbon and oxygen atom. A lone pair of electron is present on each carbon and oxygen atom. By bonding in this way, their octet is complete. The hybridization of carbon is \r\nsp\r\n.

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Its lewis structure is,

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Figure 1

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There are four valence electrons on carbon and six valence electrons on oxygen atom. Therefore the total valence electrons in \r\nC3O2\r\n is \r\n3×4+6×2=24\r\n

', 'sectionSequence': 2, 'computed': {'sectionNameWithHtmlRemoved': 'Explanation', 'sectionTextWithHtmlRemoved': 'Explanation The two additional stable oxides of carbon is CO and C 3 O 2 . There are four valence electrons on carbon and six valence electrons on oxygen atom. Therefore the total valence electrons in CO is 4+6=10 . There is triple bond between carbon and oxygen atom. A lone pair of electron is present on each carbon and oxygen atom. By bonding in this way, their octet is complete. The hybridization of carbon is sp . Its lewis structure is, Figure 1 There are four valence electrons on carbon and six valence electrons on oxygen atom. Therefore the total valence electrons in C 3 O 2 is 3×4+6×2=24'}}]}]