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Postby ALee_1J » Tue Dec 08, 2020 11:01 pm

Why is the preferred Lewis Structure for N2H4:
instead of a structure with a triple bond in between the two nitrogens?

Adalia 3E
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Re: N2H4

Postby Adalia 3E » Tue Dec 08, 2020 11:04 pm

I asked my TA about this, she said that Nitrogen is an element that almost never breaks the octet rule in situations like these, and if there were a triple bond not all the hydrogens would be able to bond.

Kushaal Madadi 2F
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Re: N2H4

Postby Kushaal Madadi 2F » Tue Dec 08, 2020 11:15 pm

Nitrogen cannot have an expanded octet.

Brandon Carris
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Re: N2H4

Postby Brandon Carris » Tue Dec 15, 2020 6:31 pm

Yea nitrogen in most cases likes to have 5 electrons bound

Neel Sharma 3F
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Re: N2H4

Postby Neel Sharma 3F » Tue Dec 15, 2020 7:42 pm

Nitrogen does not have access to d or f orbitals and as a result must have an octet. Oxygen and other period 2 elements are similar in this way. Hope this helps!

Melanie Krahn 1C
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Re: N2H4

Postby Melanie Krahn 1C » Tue Dec 15, 2020 7:46 pm

Nitrogen does not have an expanded octet because it is in the second period and there is no such thing as a 2d orbital for the second-period elements.

Madeline Marron 1I
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Re: N2H4

Postby Madeline Marron 1I » Tue Dec 15, 2020 8:13 pm

Nitrogen can't have more than an octet

Posts: 101
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Re: N2H4

Postby 705383815 » Tue Dec 15, 2020 8:22 pm

I believe the reason involves the total formal charges of all of the atoms in the compound.

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