Rank the bond energies in order from lowest to highest: single bonds, double bonds, triple bonds.

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Multiple Choice

Rank the bond energies in order from lowest to highest: single bonds, double bonds, triple bonds.

Explanation:
Bond energy increases with bond order. A single bond has one shared pair of electrons, a double bond has two shared pairs, and a triple bond has three. More shared electrons and stronger attraction between the atoms make the bond shorter and harder to break, so it requires more energy. In typical diatomic bonds, single < double < triple, with approximate values like H–H (~436 kJ/mol), O=O (~498 kJ/mol), and N≡N (~941 kJ/mol) illustrating the trend. From lowest to highest bond energy: single bonds, then double bonds, then triple bonds.

Bond energy increases with bond order. A single bond has one shared pair of electrons, a double bond has two shared pairs, and a triple bond has three. More shared electrons and stronger attraction between the atoms make the bond shorter and harder to break, so it requires more energy. In typical diatomic bonds, single < double < triple, with approximate values like H–H (436 kJ/mol), O=O (498 kJ/mol), and N≡N (~941 kJ/mol) illustrating the trend. From lowest to highest bond energy: single bonds, then double bonds, then triple bonds.

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