Comparing H Bonding In H2O, HF, NH3, And CH4

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You are using an out of date browser. It may not display this or other websites correctly.You should upgrade or use an alternative browser. Comparing H bonding in H2O, HF, NH3, and CH4

• Thread starter Thread starter deleted647690
• Start date Start date Aug 12, 2016

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deleted647690

Members do not see this ad. So H2O has the highest boiling point out of these four compounds because it can potentially form 4 H bonds. Why does HF have a higher BP than NH3? Doesn't NH3 form more H bonds than HF? Same goes for CH4. Is it due to the increased EN of fluorine over N and subsequently over C? So that the H bond formed by HF is stronger than NH3's bonds which are stronger than CH4's? Sort by date Sort by votes K

kryptonxenon

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HF and NH3 can both form 2 Hydrogen bonds. But like you mentioned since Fluorine is more EN than Nitrogen, HF should have stronger IMFs and thus a higher boiling point. CH4 actually can't form any hydrogen bonds. Remember that hydrogen bonding requires a H bonded to an EN atom like F, O, or N. Upvote 0 Downvote D

deleted585480

So H2O is still the highest boiling point here? Even if HF Is the most EN?? Upvote 0 Downvote K

kryptonxenon

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JPS398 said: So H2O is still the highest boiling point here? Even if HF Is the most EN?? Click to expand...

Yes because it forms more hydrogen bonds than HF does. Upvote 0 Downvote

goodtime

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kryptonxenon said: Yes because it forms more hydrogen bonds than HF does. Click to expand...

why does it form more hydrogen bonds, i thought i would only form 2? Upvote 0 Downvote D

deleted647690

kryptonxenon said: HF and NH3 can both form 2 Hydrogen bonds. But like you mentioned since Fluorine is more EN than Nitrogen, HF should have stronger IMFs and thus a higher boiling point. CH4 actually can't form any hydrogen bonds. Remember that hydrogen bonding requires a H bonded to an EN atom like F, O, or N. Click to expand...

So two of the hydrogens on NH3 are not considered H bonded to N? Upvote 0 Downvote K

kryptonxenon

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acetylmandarin said: So two of the hydrogens on NH3 are not considered H bonded to N? Click to expand...

Remember IMFs are between 2 different molecules of NH3 and the hydrogen bonds we are talking about are between 2 different molecules. Here's a trick I learned in my TPR class to calculate the number of hydrogen bonds a compound can form: 1. Identify number of hydrogen and lone pairs 2. To calculate the number of possible hydrogen bonds take the lowest number from step 1 and multiply this by 2. Upvote 0 Downvote D

deleted647690

kryptonxenon said: Remember IMFs are between 2 different molecules of NH3 and the hydrogen bonds we are talking about are between 2 different molecules. Here's a trick I learned in my TPR class to calculate the number of hydrogen bonds a compound can form: 1. Identify number of hydrogen and lone pairs 2. To calculate the number of possible hydrogen bonds take the lowest number from step 1 and multiply this by 2. Click to expand...

Ah, I think I forgot what an H bond is. haha whoops Upvote 0 Downvote S

Songyeon 17

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kryptonxenon said: Remember IMFs are between 2 different molecules of NH3 and the hydrogen bonds we are talking about are between 2 different molecules. Here's a trick I learned in my TPR class to calculate the number of hydrogen bonds a compound can form: 1. Identify number of hydrogen and lone pairs 2. To calculate the number of possible hydrogen bonds take the lowest number from step 1 and multiply this by 2. Click to expand...

What do you mean by "take the lowest number from step 1" ? Upvote 0 Downvote You must log in or register to reply here. Share: Facebook X Bluesky LinkedIn Reddit Pinterest Tumblr WhatsApp E-mail Share Link

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