Thanoswashere
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#1
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Can someone please explain why group 2 elements have a higher melting point than group 1 elements?? Does it have anything to do with increase in nuclear charge or is it something to do with London forces? Very confused 😰
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Hellllpppp
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Think about what group 2 elements are and their bonding. Hint: magnesium is a group 2 element.
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Thanoswashere
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(Original post by Hellllpppp)
Think about what group 2 elements are and their bonding. Hint: magnesium is a group 2 element.
Ohhh hold on - metallic bonding right?? So there will be a stronger attraction to the delocalised electrons in the metallic bonding lattice?
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kylalee.x
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(Original post by Thanoswashere)
Ohhh hold on - metallic bonding right?? So there will be a stronger attraction to the delocalised electrons in the metallic bonding lattice?
Has as Group 2 has 2+ ions and Group 1 has 1+ ions so group 2 has stronger metallic bonds
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Hellllpppp
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(Original post by Thanoswashere)
Ohhh hold on - metallic bonding right?? So there will be a stronger attraction to the delocalised electrons in the metallic bonding lattice?
Yeah there’s stronger attraction as the ions are 2+ instead of 1+ and there’s more delocalised electrons (2 per atom instead of 1).
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Thanoswashere
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(Original post by Hellllpppp)
Yeah there’s stronger attraction as the ions are 2+ instead of 1+ and there’s more delocalised electrons (2 per atom instead of 1).
Ok that makes so much more sense and now I understand better - thank you for your help! 😊
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