316137
The percentage of \({\text{p}}\) -character of the hybrid orbitals in graphite and diamond are respectively
1 33 and 25
2 50 and 75
3 67 and 75
4 33 and 75
Explanation:
In diamond, each carbon is \(\mathrm{sp}^{3}\) hybridised while in graphite each carbon has \(\mathrm{sp}^{2}\) hybridisation. In \(\mathrm{sp}^{3}, \mathrm{p}\)-character \(\rightarrow \dfrac{3}{4} \times 100=75 \%\) In \(\mathrm{sp}^{2}, \mathrm{p}\)-character \(\rightarrow \dfrac{2}{3} \times 100=66.6 \sim 67 \%\)
KCET - 2012
CHXI11:THE P-BLOCK ELEMENTS
316138
Assertion : Diamond is a bad conductor. Reason : Graphite is a good conductor.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Diamond's poor conductivity is due to each carbon atom being tetrahedrally bonded in a hybridized state with no mobile electrons. Graphite's conductivity results from a hexagonal planar structure, leaving one p-electron per carbon atom free for heat and electricity conduction. So, option (2) is correct.
CHXI11:THE P-BLOCK ELEMENTS
316139
Graphite is good conductor of current but diamond is non-conductor because
1 Diamond is hard and graphite is soft
2 Graphite and diamond have different atomic configuration
3 Graphite is composed of positively charged carbon ions
4 Graphite has hexagonal layer structure with mobile \(\pi\)-electrons while diamond has continuous tetrahedral covalent structure with no free electrons
Explanation:
Conceptual Questions
CHXI11:THE P-BLOCK ELEMENTS
316140
Which of the following types of forces bind together the carbon atoms in diamond?
1 Ionic
2 Covalent
3 Dipolar
4 van der Waals.
Explanation:
In diamond each carbon atom is \(\mathrm{sp}^{3}\) hybridized and thus forms covalent bonds with four other carbon atoms lying at the corners of a regular tetrahedron.
CHXI11:THE P-BLOCK ELEMENTS
316141
Diamond and graphite are shown to be allotropic forms of carbon by the fact that
1 Diamond is hard but graphite is soft.
2 Diamond is transparent while graphite is opaque
3 They have different crystal structures
4 Both form \(\mathrm{CO}_{2}\) when burnt.
Explanation:
Diamond and graphite are allotropes of carbon because both on burning produce \(\mathrm{CO}_{2}\) and thus show similar chemical properties.
316137
The percentage of \({\text{p}}\) -character of the hybrid orbitals in graphite and diamond are respectively
1 33 and 25
2 50 and 75
3 67 and 75
4 33 and 75
Explanation:
In diamond, each carbon is \(\mathrm{sp}^{3}\) hybridised while in graphite each carbon has \(\mathrm{sp}^{2}\) hybridisation. In \(\mathrm{sp}^{3}, \mathrm{p}\)-character \(\rightarrow \dfrac{3}{4} \times 100=75 \%\) In \(\mathrm{sp}^{2}, \mathrm{p}\)-character \(\rightarrow \dfrac{2}{3} \times 100=66.6 \sim 67 \%\)
KCET - 2012
CHXI11:THE P-BLOCK ELEMENTS
316138
Assertion : Diamond is a bad conductor. Reason : Graphite is a good conductor.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Diamond's poor conductivity is due to each carbon atom being tetrahedrally bonded in a hybridized state with no mobile electrons. Graphite's conductivity results from a hexagonal planar structure, leaving one p-electron per carbon atom free for heat and electricity conduction. So, option (2) is correct.
CHXI11:THE P-BLOCK ELEMENTS
316139
Graphite is good conductor of current but diamond is non-conductor because
1 Diamond is hard and graphite is soft
2 Graphite and diamond have different atomic configuration
3 Graphite is composed of positively charged carbon ions
4 Graphite has hexagonal layer structure with mobile \(\pi\)-electrons while diamond has continuous tetrahedral covalent structure with no free electrons
Explanation:
Conceptual Questions
CHXI11:THE P-BLOCK ELEMENTS
316140
Which of the following types of forces bind together the carbon atoms in diamond?
1 Ionic
2 Covalent
3 Dipolar
4 van der Waals.
Explanation:
In diamond each carbon atom is \(\mathrm{sp}^{3}\) hybridized and thus forms covalent bonds with four other carbon atoms lying at the corners of a regular tetrahedron.
CHXI11:THE P-BLOCK ELEMENTS
316141
Diamond and graphite are shown to be allotropic forms of carbon by the fact that
1 Diamond is hard but graphite is soft.
2 Diamond is transparent while graphite is opaque
3 They have different crystal structures
4 Both form \(\mathrm{CO}_{2}\) when burnt.
Explanation:
Diamond and graphite are allotropes of carbon because both on burning produce \(\mathrm{CO}_{2}\) and thus show similar chemical properties.
316137
The percentage of \({\text{p}}\) -character of the hybrid orbitals in graphite and diamond are respectively
1 33 and 25
2 50 and 75
3 67 and 75
4 33 and 75
Explanation:
In diamond, each carbon is \(\mathrm{sp}^{3}\) hybridised while in graphite each carbon has \(\mathrm{sp}^{2}\) hybridisation. In \(\mathrm{sp}^{3}, \mathrm{p}\)-character \(\rightarrow \dfrac{3}{4} \times 100=75 \%\) In \(\mathrm{sp}^{2}, \mathrm{p}\)-character \(\rightarrow \dfrac{2}{3} \times 100=66.6 \sim 67 \%\)
KCET - 2012
CHXI11:THE P-BLOCK ELEMENTS
316138
Assertion : Diamond is a bad conductor. Reason : Graphite is a good conductor.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Diamond's poor conductivity is due to each carbon atom being tetrahedrally bonded in a hybridized state with no mobile electrons. Graphite's conductivity results from a hexagonal planar structure, leaving one p-electron per carbon atom free for heat and electricity conduction. So, option (2) is correct.
CHXI11:THE P-BLOCK ELEMENTS
316139
Graphite is good conductor of current but diamond is non-conductor because
1 Diamond is hard and graphite is soft
2 Graphite and diamond have different atomic configuration
3 Graphite is composed of positively charged carbon ions
4 Graphite has hexagonal layer structure with mobile \(\pi\)-electrons while diamond has continuous tetrahedral covalent structure with no free electrons
Explanation:
Conceptual Questions
CHXI11:THE P-BLOCK ELEMENTS
316140
Which of the following types of forces bind together the carbon atoms in diamond?
1 Ionic
2 Covalent
3 Dipolar
4 van der Waals.
Explanation:
In diamond each carbon atom is \(\mathrm{sp}^{3}\) hybridized and thus forms covalent bonds with four other carbon atoms lying at the corners of a regular tetrahedron.
CHXI11:THE P-BLOCK ELEMENTS
316141
Diamond and graphite are shown to be allotropic forms of carbon by the fact that
1 Diamond is hard but graphite is soft.
2 Diamond is transparent while graphite is opaque
3 They have different crystal structures
4 Both form \(\mathrm{CO}_{2}\) when burnt.
Explanation:
Diamond and graphite are allotropes of carbon because both on burning produce \(\mathrm{CO}_{2}\) and thus show similar chemical properties.
316137
The percentage of \({\text{p}}\) -character of the hybrid orbitals in graphite and diamond are respectively
1 33 and 25
2 50 and 75
3 67 and 75
4 33 and 75
Explanation:
In diamond, each carbon is \(\mathrm{sp}^{3}\) hybridised while in graphite each carbon has \(\mathrm{sp}^{2}\) hybridisation. In \(\mathrm{sp}^{3}, \mathrm{p}\)-character \(\rightarrow \dfrac{3}{4} \times 100=75 \%\) In \(\mathrm{sp}^{2}, \mathrm{p}\)-character \(\rightarrow \dfrac{2}{3} \times 100=66.6 \sim 67 \%\)
KCET - 2012
CHXI11:THE P-BLOCK ELEMENTS
316138
Assertion : Diamond is a bad conductor. Reason : Graphite is a good conductor.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Diamond's poor conductivity is due to each carbon atom being tetrahedrally bonded in a hybridized state with no mobile electrons. Graphite's conductivity results from a hexagonal planar structure, leaving one p-electron per carbon atom free for heat and electricity conduction. So, option (2) is correct.
CHXI11:THE P-BLOCK ELEMENTS
316139
Graphite is good conductor of current but diamond is non-conductor because
1 Diamond is hard and graphite is soft
2 Graphite and diamond have different atomic configuration
3 Graphite is composed of positively charged carbon ions
4 Graphite has hexagonal layer structure with mobile \(\pi\)-electrons while diamond has continuous tetrahedral covalent structure with no free electrons
Explanation:
Conceptual Questions
CHXI11:THE P-BLOCK ELEMENTS
316140
Which of the following types of forces bind together the carbon atoms in diamond?
1 Ionic
2 Covalent
3 Dipolar
4 van der Waals.
Explanation:
In diamond each carbon atom is \(\mathrm{sp}^{3}\) hybridized and thus forms covalent bonds with four other carbon atoms lying at the corners of a regular tetrahedron.
CHXI11:THE P-BLOCK ELEMENTS
316141
Diamond and graphite are shown to be allotropic forms of carbon by the fact that
1 Diamond is hard but graphite is soft.
2 Diamond is transparent while graphite is opaque
3 They have different crystal structures
4 Both form \(\mathrm{CO}_{2}\) when burnt.
Explanation:
Diamond and graphite are allotropes of carbon because both on burning produce \(\mathrm{CO}_{2}\) and thus show similar chemical properties.
316137
The percentage of \({\text{p}}\) -character of the hybrid orbitals in graphite and diamond are respectively
1 33 and 25
2 50 and 75
3 67 and 75
4 33 and 75
Explanation:
In diamond, each carbon is \(\mathrm{sp}^{3}\) hybridised while in graphite each carbon has \(\mathrm{sp}^{2}\) hybridisation. In \(\mathrm{sp}^{3}, \mathrm{p}\)-character \(\rightarrow \dfrac{3}{4} \times 100=75 \%\) In \(\mathrm{sp}^{2}, \mathrm{p}\)-character \(\rightarrow \dfrac{2}{3} \times 100=66.6 \sim 67 \%\)
KCET - 2012
CHXI11:THE P-BLOCK ELEMENTS
316138
Assertion : Diamond is a bad conductor. Reason : Graphite is a good conductor.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Diamond's poor conductivity is due to each carbon atom being tetrahedrally bonded in a hybridized state with no mobile electrons. Graphite's conductivity results from a hexagonal planar structure, leaving one p-electron per carbon atom free for heat and electricity conduction. So, option (2) is correct.
CHXI11:THE P-BLOCK ELEMENTS
316139
Graphite is good conductor of current but diamond is non-conductor because
1 Diamond is hard and graphite is soft
2 Graphite and diamond have different atomic configuration
3 Graphite is composed of positively charged carbon ions
4 Graphite has hexagonal layer structure with mobile \(\pi\)-electrons while diamond has continuous tetrahedral covalent structure with no free electrons
Explanation:
Conceptual Questions
CHXI11:THE P-BLOCK ELEMENTS
316140
Which of the following types of forces bind together the carbon atoms in diamond?
1 Ionic
2 Covalent
3 Dipolar
4 van der Waals.
Explanation:
In diamond each carbon atom is \(\mathrm{sp}^{3}\) hybridized and thus forms covalent bonds with four other carbon atoms lying at the corners of a regular tetrahedron.
CHXI11:THE P-BLOCK ELEMENTS
316141
Diamond and graphite are shown to be allotropic forms of carbon by the fact that
1 Diamond is hard but graphite is soft.
2 Diamond is transparent while graphite is opaque
3 They have different crystal structures
4 Both form \(\mathrm{CO}_{2}\) when burnt.
Explanation:
Diamond and graphite are allotropes of carbon because both on burning produce \(\mathrm{CO}_{2}\) and thus show similar chemical properties.
