The electrons in both the 2s and 2p orbitals are equivalent
The electrons in all the orbitals of carbon are equivalent
The 2s and 2p atomic orbitals hybridize
All the atomic orbitals of carbon hybridize
Explanation
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Here is an explanation:
The answer is A. When we talk of valency of an element, we are looking at the number of electrons in the outer shell f it's atom. Carbon has 4 electrons in it's outer shell i.e. it's L shell which corresponds to principal quantum number 2 of the s and p orbital in it's electronic configuration of 1s²2s²2p².
REF: Check:New school chemistry, page 51 and page 137
2S and 2P orbitals cannot be equivalent, please! The "2" there are only stating that it's the same L shell. Remember, 2S orbital is spherical and of lower energy than 2P orbitals which are at right angles to each other.
Here's why the answer is C, using New School Chemistry as a Reference:
Carbon with an electronic configuration of IS²2S²2Px¹2Py¹2px⁰ has two unpaired electrons but it shows a covalency of four instead of two. To account for this, it is proposed that the ground state carbon first absorbs energy to become excited before bonding takes place. The energy absorbed is used to promote a 2S-electron into the vacant 2P-electron. An excited excited carbon atom thus has the electronic configuration of 1S²2S¹2Px¹2Py¹2Pz¹.
Before overlap of orbitals of excited carbon atom to form its compounds, there is rearrangement of the unpaired orbitals.
This rearrangement involves an equalization in energy of the four unpaired orbitals and their spreading out, and this rearrangement is termed hybridization.
MySchool look into this question and make corrections, please.
Option A is not the correct explanation for carbon being tetravalent. Carbon is tetravalent because it forms four bonds in compounds due to the hybridization of its 2s and 2p orbitals. Hybridization involves combining different types of atomic orbitals to form new hybrid orbitals, allowing carbon to achieve four equivalent sp3 hybrid orbitals for bonding. This results in a tetrahedral arrangement and tetravalency.
The correct answer is C. The 2s and 2p atomic orbitals hybridize.
Carbon typically forms four covalent bonds, which can be explained by the process of hybridization. In carbon's ground state electron configuration, it has two electrons in the 2s orbital and two in the 2p orbital. However, to form four bonds, it needs four unpaired electrons. To achieve this, carbon undergoes sp^3 hybridization, where one 2s orbital and three 2p orbitals hybridize to form four equivalent sp^3 hybrid orbitals. These hybrid orbitals have a slightly different shape compared to the original atomic orbitals, which allows carbon to form four bonds, making it tetravalent.
The hybridization of the 2s and 2p orbitals allows carbon to form four covalent bonds. This is because the hybrid orbitals are all pointing in different directions, which allows them to overlap with the orbitals of other atoms. Covalent bonds are formed when electrons are shared between atoms.
@myschool..i think the answer is B..elect config of carbon-1s2 2s2 2p2..i.e the electrons in its orbitals are all equivalent..somebody prove me wrong please for rectification..
