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a) Explain structure of diborane b) Explain two differences between diamond and
graphite on the basis of structure. Why is the graphite a good conductor of electricity
whereas diamond is an insulator?
Class 11 CBSE
Answers
Answer:
Explanation:
Diborane
Diborane is a chemical compound that consists of boron and hydrogen atoms and has a molecular formula B2H6.
Diborane is one of the simplest boron hydrides.
The Boron hydrides mix well with the air forming up explosive mixtures.
This substance will ignite rapidly at the room temperature.
(B2H6) ⇒⇒⇒see the attachment.
Differences between diamond and
graphite on the basis of structure;
Diamond and graphite are both giant covalent substances made entirely of carbon atoms. Both have chemical formula , but they do not have a molecular formula.
Molecular structure
Diamond: Giant covalent structure, with each carbon covalently bonded to four other carbon atoms in a tetrahedral arrangement to form a rigid structure.
Graphite: It is also Giant covalent structure, with each carbon covalently bonded to three other carbon atoms in a hexagonal arrangement.
Hardness
Diamond: Extremely hard. Due to rigid, tetrahedral arrangement of carbon atoms.
Graphite: Soft. Layers of hexagonally arranged carbon atoms can slide over one another.
Electrical conductivity
Diamond: Insulator. Mobile electrons are absent. All four valence electrons are used in covalent bonds.
Graphite: Conductor. Three out of four valence electrons are used for covalent bonding with other carbon atoms. Remaining valence electrons can be delocalised across the planes of carbon atoms.
Why is the graphite a good conductor of electricity whereas diamond is an insulator?
REASON
Graphite forms in layers or like sheets. Of the 4 electrons in the atom only three are bonded and one is loosely bonded in the layers . This free electron conduct electricity .
In diamonds all the 4 electrons of the atom are bonded to the atoms adjacent and this covalent bond is strong and the electrons do not move when electricity is applied like a non conductor
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Explanation:
Answer:
Explanation:
Diborane
Diborane is a chemical compound that consists of boron and hydrogen atoms and has a molecular formula B2H6.
Diborane is one of the simplest boron hydrides.
The Boron hydrides mix well with the air forming up explosive mixtures.
This substance will ignite rapidly at the room temperature.
(B2H6)
⇒⇒⇒see the attachment.
Differences between diamond and
graphite on the basis of structure;
Diamond and graphite are both giant covalent substances made entirely of carbon atoms. Both have chemical formula , but they do not have a molecular formula.
Molecular structure
Diamond: Giant covalent structure, with each carbon covalently bonded to four other carbon atoms in a tetrahedral arrangement to form a rigid structure.
Graphite: It is also Giant covalent structure, with each carbon covalently bonded to three other carbon atoms in a hexagonal arrangement.
Hardness
Diamond: Extremely hard. Due to rigid, tetrahedral arrangement of carbon atoms.
Graphite: Soft. Layers of hexagonally arranged carbon atoms can slide over one another.
Electrical conductivity
Diamond: Insulator. Mobile electrons are absent. All four valence electrons are used in covalent bonds.
Graphite: Conductor. Three out of four valence electrons are used for covalent bonding with other carbon atoms. Remaining valence electrons can be delocalised across the planes of carbon atoms.
Why is the graphite a good conductor of electricity whereas diamond is an insulator?
REASON
Graphite forms in layers or like sheets. Of the 4 electrons in the atom only three are bonded and one is loosely bonded in the layers . This free electron conduct electricity .
In diamonds all the 4 electrons of the atom are bonded to the atoms adjacent and this covalent bond is strong and the electrons do not move when electricity is applied like a non conductor
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