Home
Class 12
CHEMISTRY
Carbon and silicon belong to group IV. T...

Carbon and silicon belong to group `IV`. The maximum coordination number of carbon in commonly occuring compounds is four whereas that of silicon is six. This is due to

A

Availability of low lying d-orbitals in silicon

B

Large size of silicon

C

More electropositive nature of silicon

D

Both (2) & (3)

Text Solution

AI Generated Solution

The correct Answer is:
To solve the question regarding the maximum coordination number of carbon and silicon, we can break it down into the following steps: ### Step 1: Understand the Group IV Elements Both carbon and silicon belong to Group IV of the periodic table. This means they have four valence electrons and can form four bonds in their most common oxidation states. **Hint:** Remember that elements in the same group have similar valence electron configurations. ### Step 2: Identify the Periods of Carbon and Silicon Carbon is in the second period, while silicon is in the third period of the periodic table. This distinction is crucial for understanding their coordination numbers. **Hint:** The period of an element indicates the number of electron shells it has. ### Step 3: Examine the Electron Configuration - **Carbon (C)**: The electron configuration is 1s² 2s² 2p². Carbon has no available d-orbitals because it is in the second period. - **Silicon (Si)**: The electron configuration is 1s² 2s² 2p⁶ 3s² 3p². Silicon has empty d-orbitals available for bonding. **Hint:** Look at the electron configuration to determine the availability of orbitals for bonding. ### Step 4: Analyze Coordination Numbers - **Carbon**: Due to the absence of d-orbitals, carbon can only utilize its s and p orbitals for bonding, leading to a maximum coordination number of 4. - **Silicon**: The presence of empty d-orbitals allows silicon to expand its coordination number to 6, as it can accommodate more than four bonds. **Hint:** Coordination number is influenced by the types of orbitals available for bonding. ### Step 5: Conclusion The difference in the maximum coordination numbers of carbon and silicon is primarily due to the availability of empty d-orbitals in silicon, which allows it to form more bonds compared to carbon. **Final Answer:** The maximum coordination number of carbon is four, while that of silicon is six, due to the availability of empty d-orbitals in silicon.
Doubtnut Promotions Banner Mobile Dark
|

Similar Questions

Explore conceptually related problems

Carbon exhibits coordination number of six.

In which of the following compounds the oxidation number of carbon is maximum

Knowledge Check

  • Carbon forms a large number of compounds due to :

    A
    tetravalency of carbon
    B
    strong catenation property of carbon
    C
    allotropic property of carbon
    D
    non-matallic character of carbon

  • Carbon shows a maximum covalency of four whereas other members can expand their cavalence due to

    A
    absence of d-orbitals in carbon
    B
    ability of carbon to form `p pi - p pi` multiple bonds
    C
    small size of carbon
    D
    catenation of carbon.

    • Similar Questions

    Explore conceptually related problems

    Formation of in-numberable compounds of carbon is due to its:

    Carbon and silicon both belong to the group 14, but inspite of the stoichiometric similarity, the dioxides, (i.e., carbon dioxide and silicon dioxide), differ in their structures. Comment.

    The number of compound(s) in which carbon atom of functional group can be counted in main chain is/are:

    Give reason for the following : a. The first ioisation eathalpy of carbon carbon is greater than that foboron, whereas the reverse is true fore the second ionisation enthalpy . b. Solid carbon dioxie is known as dry ice . c. Why does not silicon form an analogue fo graphite ?

    Butanone is a four-carbon compound with what functional group?

    Borane is an electron deficient compound. It has only six valence eletons, so the boron atom lacks an octet. Acquiring an octet is the driving force for the unusual bonding structure found in boron compounds. As an electron deficient compound, BH_(3) is a strong electrophile, capable of adding to a double bond. This hydroboration of double bond is though to oC Cur in one step, with the boron atom adding to the less highly substituted end of the double bond. In transition state, the boron atom withdraws electrons from the pi bond and the carbon at theother end of the double bond acquires a partial positive charge. This positive charge is more stable on the more highly subsituted carbon atom. The second step is the oxidation of boron atom, removing it from carbon and replacing it with hydroxyl group by using H_(2)O_(2)//OH^(bar(..)) . The simultaneous addition of boron and hydrogen to the double bond leads to a syn addition. Oxidation of the trialkyl borane replaces boron with a hydroxyl group in the same stereochemical position. Thus, hydroboration of alkenen is an example of steropecific reaction, in which different steroisomers of starting compounds react to give different steroisomers of the product. CH_(3)-underset(CH_(3))underset(|)overset(CH_(3))overset(|)C-CH=CH_(2) underset((ii)H_(2)O_(2)//OH^(bar(..)))overset((i)BH_(3)//THF)rarrZ . Z is :

    Home
    Profile