the type of bonds present in C2 molecule is 1. one sigma and 1 pi2. two sigma and 2 pi 3. two sigma4. two pi

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one sigma one pi

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(4) 2 pi bonds bcoz of valency

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no answer is (2) since its hybridisation will be sp3 soo sigma bonds will be 1s and 1pz remaining px and py will form pi bonds.hope that explains .

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2 pi bonds....this is explained with the help of molecular orbital theory which follows schrödinger wave equation and the wave function, psi...

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2

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1 sigma and no pie bond

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5. None of theseAns.1 sigma and 2 pi bondsBecause max no. of sigma bond in two bonded atoms is 1

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2

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2 pi bond and one sigma

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1 sigma and 2 pi bond with 1 free electron on each carbon atom

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2pi bond<div><br /><div><br /></div></div>

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2

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2 pi bond n no sigma

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opt no. 4) two pi bonds.....  and remaining valency of both carbon as pair of electrons on each in the C2 molecule....

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1 sigma bond and 2 pie bond

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Introduction:
The C2 molecule consists of two carbon atoms connected by a double bond. This molecule is known as ethylene or ethene. The type of bonds present in the C2 molecule can be explained by examining the arrangement of electrons and the hybridization of the carbon atoms.

Electronic Configuration:
Each carbon atom has an atomic number of 6, which means it has 6 electrons. The electronic configuration of carbon is 1s2 2s2 2p2. In the ground state, two electrons occupy the 1s orbital, two electrons occupy the 2s orbital, and the remaining two electrons occupy two out of the three available 2p orbitals.

Hybridization:
To form bonds, the carbon atoms undergo hybridization. In the case of ethene, each carbon atom undergoes sp2 hybridization. This hybridization involves the mixing of one 2s orbital and two 2p orbitals to form three sp2 hybrid orbitals. These orbitals are arranged in a trigonal planar geometry around each carbon atom.

Sigma and Pi Bonds:
The type of bonds present in the C2 molecule can be determined by examining the overlapping of orbitals between the carbon atoms. There are two types of overlapping that occur: sigma (σ) and pi (π) bonds.

1. Sigma Bond: A sigma bond is formed by the overlap of two sp2 hybrid orbitals, one from each carbon atom. This overlapping occurs along the internuclear axis, resulting in a head-on interaction. In the C2 molecule, there is one sigma bond formed by the overlap of one sp2 orbital from each carbon atom. This sigma bond is formed by the overlap of the two remaining unhybridized p orbitals.

2. Pi Bonds: A pi bond is formed by the overlap of two unhybridized p orbitals that are perpendicular to the internuclear axis. In the C2 molecule, there are two pi bonds formed by the overlap of the two remaining unhybridized p orbitals. These pi bonds are formed above and below the sigma bond.

Conclusion:
In summary, the type of bonds present in the C2 molecule (ethylene or ethene) are one sigma bond and two pi bonds. The sigma bond is formed by the overlap of one sp2 orbital from each carbon atom, while the two pi bonds are formed by the overlap of the remaining unhybridized p orbitals. These bonds play a crucial role in the structure and reactivity of the C2 molecule.

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how

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1.one sigma and one pi

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