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Why is the bond energy of HCL more than that of HF?
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+ Chemical bonds
+ Chemistry
+ Organic chemistry
+ Hydrochloric acid
Posted by
Mark Gallaway
Why is the bond energy of HCL more than that of HF?
I think your question is a bit backward. HF has greater bond energy than HCl. The bond energy of HF is 568 kJ/moL, while the bond energy of HCl is 431 kJ/moL. I will answer your question by explaining why the bond energy of HF is more than the bond energy of HCl.
To find the answer to this question, we must look toward the periodic table. We can see that fluorine is 1 period above chlorine. This is significant. It means that fluorine has less electron shielding than chlorine. Electron shielding happens when there are many electrons. The inner electrons at lower orbitals repel the outer electrons away from the nucleus. This reduces the effect of the nuclear charge to attract more electrons.
Since chlorine has more electrons at higher orbitals, it experiences this electron shielding effect more strongly. This means that its atomic radius is also larger, and any atom that it will bind to will be farther away from the nucleus. This means that the forces of attraction will be weaker due to Coulomb’s Law. Fluorine may have a weaker nuclear charge, but it does not experience this electron shielding effect very strongly. Its electrons are all on lower orbitals closer to the nucleus. This reduces fluorine’s atomic radius.
The hydrogen atom is able to move closer to the fluorine’s nucleus, experience a greater pull by the nuclear charge. Since the two atoms are closer together, the forces of attraction are greater than that of chlorine. This is just a basic explanation, but I hope it helps.
I think your question is a bit backward. HF has greater bond energy than HCl. The bond energy of HF is 568 kJ/moL, while the bond energy of HCl is 431 kJ/moL. I will answer your question by explaining why the bond energy of HF is more than the bond energy of HCl.
To find the answer to this question, we must look toward the periodic table. We can see that fluorine is 1 period above chlorine. This is significant. It means that fluorine has less electron shielding than chlorine. Electron shielding happens when there are many electrons. The inner electrons at lower orbitals repel the outer electrons away from the nucleus. This reduces the effect of the nuclear charge to attract more electrons.
Since chlorine has more electrons at higher orbitals, it experiences this electron shielding effect more strongly. This means that its atomic radius is also larger, and any atom that it will bind to will be farther away from the nucleus. This means that the forces of attraction will be weaker due to Coulomb’s Law. Fluorine may have a weaker nuclear charge, but it does not experience this electron shielding effect very strongly. Its electrons are all on lower orbitals closer to the nucleus. This reduces fluorine’s atomic radius.
The hydrogen atom is able to move closer to the fluorine’s nucleus, experience a greater pull by the nuclear charge. Since the two atoms are closer together, the forces of attraction are greater than that of chlorine. This is just a basic explanation, but I hope it helps.
I think your question is a bit backward. HF has greater bond energy than HCl. The bond energy of HF is 568 kJ/moL, while the bond energy of HCl is 431 kJ/moL. I will answer your question by explaining why the bond energy of HF is more than the bond energy of HCl.
To find the answer to this question, we must look toward the periodic table. We can see that fluorine is 1 period above chlorine. This is significant. It means that fluorine has less electron shielding than chlorine. Electron shielding happens when there are many electrons. The inner electrons at lower orbitals repel the outer electrons away from the nucleus. This reduces the effect of the nuclear charge to attract more electrons.
Since chlorine has more electrons at higher orbitals, it experiences this electron shielding effect more strongly. This means that its atomic radius is also larger, and any atom that it will bind to will be farther away from the nucleus. This means that the forces of attraction will be weaker due to Coulomb’s Law. Fluorine may have a weaker nuclear charge, but it does not experience this electron shielding effect very strongly. Its electrons are all on lower orbitals closer to the nucleus. This reduces fluorine’s atomic radius.
The hydrogen atom is able to move closer to the fluorine’s nucleus, experience a greater pull by the nuclear charge. Since the two atoms are closer together, the forces of attraction are greater than that of chlorine. This is just a basic explanation, but I hope it helps.
Sources: Bond Energies
I think your question is a bit backward. HF has greater bond energy than HCl. The bond energy of HF is 568 kJ/moL, while the bond energy of HCl is 431 kJ/moL. I will answer your question by explaining why the bond energy of HF is more than the bond energy of HCl.
To find the answer to this question, we must look toward the periodic table. We can see that fluorine is 1 period above chlorine. This is significant. It means that fluorine has less electron shielding than chlorine. Electron shielding happens when there are many electrons. The inner electrons at lower orbitals repel the outer electrons away from the nucleus. This reduces the effect of the nuclear charge to attract more electrons.
Since chlorine has more electrons at higher orbitals, it experiences this electron shielding effect more strongly. This means that its atomic radius is also larger, and any atom that it will bind to will be farther away from the nucleus. This means that the forces of attraction will be weaker due to Coulomb’s Law. Fluorine may have a weaker nuclear charge, but it does not experience this electron shielding effect very strongly. Its electrons are all on lower orbitals closer to the nucleus. This reduces fluorine’s atomic radius.
The hydrogen atom is able to move closer to the fluorine’s nucleus, experience a greater pull by the nuclear charge. Since the two atoms are closer together, the forces of attraction are greater than that of chlorine. This is just a basic explanation, but I hope it helps.
Sources: Bond Energies
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