Sapling week 5 & 6 #5
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Sapling week 5 & 6 #5
I got the other parts of this question right and I don't know why this one is wrong please help.
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Re: Sapling week 5 & 6 #5
Hi! The only error you have in this model is the charge on C. Carbon likes to make 4 covalent bonds, sharing 8 electrons and fulfilling its octet. However, given that it only has 2 covalent bonds, the 2 lone pairs indicate that Carbon should have a charge of -2. Hope this helps!
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Re: Sapling week 5 & 6 #5
I got that the charge on carbon is -2 because the overall molecule must not have a charge. So because there are two positive charges, carbon would be -2 to offset that. Hope this helps!
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Re: Sapling week 5 & 6 #5
Hi! The formal charge on the carbon atom would be -2, not -1. When we find the formal charge, we evaluate 4 - ((4/2)+4), which is equal to 4 - (2+4), or 4 - 6, which gives us a formal charge of -2. Additionally, the overall molecule does not have a charge so the formal charges of each individual atom should cancel each other out.
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Re: Sapling week 5 & 6 #5
Hello! First, be sure that all the charges in this molecule cancel out because the overall charge is zero. That should be a trigger that there should be an extra negative charge somewhere (or in other cases, one less +). Next, be sure to remember that carbon usually likes to have four bonds, but in this case, it only has two. Thus, the charge on the carbon atom should be -2 instead of -1. I hope this helps!
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Re: Sapling week 5 & 6 #5
Hi,
The formal charges on the atoms should add up to zero because the HCNO molecule is neutral. The most stable structure has the fewest number of, and smallest magnitude of, formal charges, and with the negative formal charges on the more electronegative elements. Both resonance structures B and C have the fewest and smallest magnitude of formal charges. Oxygen is the most electronegative atom in the molecule, so oxygen bears the negative formal charge in the most stable resonance structure. The number for C should be -2 not -1.
The formal charges on the atoms should add up to zero because the HCNO molecule is neutral. The most stable structure has the fewest number of, and smallest magnitude of, formal charges, and with the negative formal charges on the more electronegative elements. Both resonance structures B and C have the fewest and smallest magnitude of formal charges. Oxygen is the most electronegative atom in the molecule, so oxygen bears the negative formal charge in the most stable resonance structure. The number for C should be -2 not -1.
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Re: Sapling week 5 & 6 #5
So C's FC is -2. This makes sense because this cancels the other charges, giving an overall charge of 0
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Re: Sapling week 5 & 6 #5
The formal charge for carbon should be -2, since it has 4 valence electrons, and 4 lone and 4 bonded electrons, so 4 - (4 + 4/2) = -2.
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Re: Sapling week 5 & 6 #5
Hi, the formal charge on the C should be 2- because this would make the overall charge 0.
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Re: Sapling week 5 & 6 #5
C should have a formal charge of -2. Valence - free - bonding/2 = 4 - 4 - 4/2 = -2.
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Re: Sapling week 5 & 6 #5
The formal charge on Carbon should be -2. Since Crabon has 4 valence electrons, 2 pairs of shared electrons, and 2 lone pairs of electrons. 4-(2+4) = -2. Hope this helps!
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Re: Sapling week 5 & 6 #5
The formal charge of C should be -2. FC= valence electrons (4) - (long pairs (4) + sharing electrons/2 (2))
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Re: Sapling week 5 & 6 #5
the part that is incorrect about this problem is that Carbon's formal charge is -2 because it has 4 valence, 2 single bonds, and 4 lone electrons. When you plug all those numbers into the formal charge equation FC= valence- (bonds+ lone electrons), you get -2
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Re: Sapling week 5 & 6 #5
The formal charge of carbon should be -2. There are 4 bonds and 4 lone pairs so (4/2 + 4) = 6. The valence electrons of carbon is 4 so 4-6 = -2.
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Re: Sapling week 5 & 6 #5
To find resonance you would take the number of valence electrons of the respective Element, and from that subtract the number of electrons/bonds around it. A single bond counts as one, and each electron counts as one
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Re: Sapling week 5 & 6 #5
To find resonance you would take the number of valence electrons of the respective Element, and from that subtract the number of electrons/bonds around it. A single bond counts as one, and each electron counts as one
Re: Sapling week 5 & 6 #5
Since carbon only possesses two bonds, rather than the four it tends to form. Therefore, due to this abnormality, the formal charge would be -2.
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