Carbon and silicon are known to have similar lattice structures. However, the four bonding electrons of carbon are present in second orbit while those of silicon are present in its third orbit. How does this difference result in a difference in their electrical conductivities
Carbon and silicon are known to have similar lattice structures. However, the four bonding electrons of carbon are present in second orbit while those of silicon are present in its third orbit. How does this difference result in a difference in their electrical conductivities
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We know that in an atoms binding energy of electron is less in highter orbit and more in lower orbit. Therefore, the energy required to remove an electron from silicon atom is much smaller than that in case of carbon atom. That is why, the number of free electrons for conduction in silicon is quite significant but very small for carbon. As a result of it, the conductivity of silicon is much higher than that of carbon.
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Molecular orbital theory as developed by Hund and Mulliken concerns with the formation of molecular orbitals formed by linear combination of atomic orbitals. The electrons are present in these molecular orbitals. The molecular orbitals are filled. The molecular orbital configuration helps us to calculate bond order which gives information about the number of bonds present between atoms. The bond order is related to bond length and bond strength. Which one of the following does not have single electron in a bonding molecular orbital?
Molecular orbital theory as developed by Hund and Mulliken concerns with the formation of molecular orbitals formed by linear combination of atomic orbitals. The electrons are present in these molecular orbitals. The molecular orbitals are filled. The molecular orbital configuration helps us to calculate bond order which gives information about the number of bonds present between atoms. The bond order is related to bond length and bond strength. Which one of the following does not have single electron in a bonding molecular orbital?
A
`CN`
B
`B_(2)`
C
`NO`
D
`N_(2)^(+)`
Molecular orbitals are formed by the overlap of atomic orbitals . Two atomic orbitals combine to form two molecular orbitals, called Bonding Molecular Orbital (BMO) and Anti - Bonding Molecular Orbital (ABMO). Different atomic orbitals of one atom combine with those atomic orbitals of the second atom which have comparable energles and proper orientation Further, if overlapping is head on, the molecular orbitals is called 'sigma' and if the overlap is lateral, the molecular orbital is called 'pi' . The molecular orbitals are filled with electrons following the same rules as followed for filling of atomic orbitals . However, the order of filling in not the same for of the most important parameter to compare a number of their characteristics In whihc of the following pair the moelcular orbitals are gerade or ungerade ?
Molecular orbitals are formed by the overlap of atomic orbitals . Two atomic orbitals combine to form two molecular orbitals, called Bonding Molecular Orbital (BMO) and Anti - Bonding Molecular Orbital (ABMO). Different atomic orbitals of one atom combine with those atomic orbitals of the second atom which have comparable energles and proper orientation Further, if overlapping is head on, the molecular orbitals is called 'sigma' and if the overlap is lateral, the molecular orbital is called 'pi' . The molecular orbitals are filled with electrons following the same rules as followed for filling of atomic orbitals . However, the order of filling in not the same for of the most important parameter to compare a number of their characteristics In whihc of the following pair the moelcular orbitals are gerade or ungerade ?
A
`sigma_(2s), pi_(2p_(x))`
B
`sigma_(2s)^(**), pi_(2p_(x))^(**)`
C
`sigma_(2s)^(**), pi_(2p_(x))`
D
`pi_(2p_(x)), pi_(2p_(x))^(**)`
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A chemical bond is an attractive force that holds the atoms together in a molecule or a compound. The element carbon is known to have the unique ability to form bonds with other similar atoms or atoms of other elements. This property of carbon has resulted in its having very large number of compounds. The carbon-carbon bond is also known to be very strong and hence stable. Answer the following questions based on above information: (i) Name the chemical bond formed between carbon-carbon atoms. How is this bond formed? (ii) Which two values are reflected in the nature of carbon resulting in its ability to form maximum number of compounds? (iii) How can these values be helpful in strengthening relationship in a family, organisation or even people of a nation?
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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.
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Silicon is the second most abundant element (~27.2%) in the earth's after oxygen (45.5 %) Carbon. Silicon, germanium, tin and lead constitute the group 14 of the periodic table. Chemistry of silicon is distinctly different from that of carbon. For example, under standard conditions CO_(2) is a gas whereas SiO_(2) is a covalent solid. The reason for the distinct difference in the properties of CO_(2) and SiO_(2) is : (a)carbon is more electronegative then O and in case of SiO_(2) oxygen is more electronegative than silicon (b)carbon has a small size and forms a pi bond with good overlap whereas silicon has larger size hence has a poor pi overlap ( c)carbon has only 'rho' orbitals and lacks 'd' orbitals whereas silicon has 'd' orbitals (d)first ionization potential of carbon is higher than that of silicon ( 1086 kJ mol^(-1) for C and 786 kJ mol^(-1) for Si ).