This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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Question 9: How many bonding pair are present in carbon(IV) oxide molecule? Carbon(IV) oxide is commonly known as carbon dioxide (CO_2). To determine the number of bonding pairs, we draw its Lewis structure: 1. Count total valence electrons: Carbon (C) has 4 valence electrons. Oxygen (O) has 6 valence electrons. Total valence electrons = 4 + (2 × 6) = 4 + 12 = 16 electrons. 2. Arrange atoms: Carbon is the central atom, bonded to two oxygen atoms: O - C - O. 3. Form single bonds: Place a single bond between the central carbon and each oxygen atom. This uses 2 × 2 = 4 electrons. Remaining electrons = 16 - 4 = 12 electrons. 4. Distribute remaining electrons as lone pairs to outer atoms: Each oxygen needs 6 more electrons to complete its octet. O - C - O This uses 2 × 6 = 12 electrons. Remaining electrons = 12 - 12 = 0 electrons. 5. Check octets: At this point, each oxygen has an octet (2 from bond + 6 lone pair), but carbon only has 4 electrons (2 from each single bond). 6. Form multiple bonds: To satisfy carbon's octet, move one lone pair from each oxygen atom to form a double bond with the carbon atom. O = C = O 7. Final check: Each oxygen atom now has 4 electrons from the double bond and 4 lone pair electrons, totaling 8 electrons. The carbon atom has 4 electrons from each double bond, totaling 8 electrons. All atoms have complete octets. 8. Count bonding pairs: There is a double bond between the left oxygen and carbon. A double bond consists of 2 bonding pairs. There is a double bond between the right oxygen and carbon. A double bond consists of 2 bonding pairs. Total bonding pairs = 2 + 2 = 4. Therefore, there are 4 bonding pairs in a carbon(IV) oxide molecule. The correct option is B.