Samaliyesman
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I’m quite stuck on this question

explain each of the following silicon and phosphorus are both covalent substances but silicon has a much higher melting temperature than phosphorus 5marks
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charco
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(Original post by Samaliyesman)
I’m quite stuck on this question

explain each of the following silicon and phosphorus are both covalent substances but silicon has a much higher melting temperature than phosphorus 5marks
There are two forms of covalent bonding/structure

Simple covalent = small molecules, easy to separate, as intermolecular forces are weak
Giant covalent = 1 humungous molecule, v. hard to separate, as it means breaking strong covalent bonds
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η γνώση
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The simple covalent bonds is a structure that has atoms that are bonded with strong covalent bonds and molecules are bonded with weak intermolecular forces - therefore giving it a low melting point since less energy is needed to overcome the bonds (easier to break) for example CO2 or phosphorus. Whereas since Sillicon is a giant covalent structure is a giant covalent network, the molecules are bonded together with strong covalent bonds, has a higher melting point since more energy is needed to overcome the strong covalent bonds. Other example of giant covalent structure include Diamond and Graphite. Anymore issued please let me know, I may have rushed it. Goodluck in the future, take care.
Last edited by η γνώση; 2 years ago
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