NO molecule has 15 (odd) electrons, 8 from oxygen and 7 from nitrogen.
Yes, the nitrate ion (NO3-) is considered an odd-electron species because it has an unpaired electron. In its Lewis structure, the molecule has a total of 24 valence electrons (5 from nitrogen and 18 from three oxygen atoms, plus one extra electron for the negative charge), leading to an unpaired electron configuration. This characteristic can influence its reactivity and bonding behavior in chemical reactions.
chlorine and oxygen both have different electro negativities due to which polarity develops between the bond and one odd electron present in chlorine make different type of Dpie - Ppie bond with it
Nitrogen dioxide (NO2) does not have a conventional Lewis structure due to the presence of an odd number of valence electrons, which results in an unpaired electron. It has a total of 17 valence electrons, leading to an incomplete octet for nitrogen when attempting to satisfy the octet rule for all atoms. This unpaired electron makes NO2 a free radical, contributing to its reactivity and instability, which is not adequately represented in a simple Lewis structure. Instead, resonance structures are often used to depict its bonding and electron distribution more accurately.
1. the incomplete octet of a central atom 2. odd electron molecule 3. compound with expanded octet 4. acc. to rule atoms complete their octet to complete their octet to become stable like inert gas, but it is seen that inert gases like xenon are not stabkle they combine with fluorine and oxygen to form no. of compounds. 5. shape of molecule cant be explained 6. stability of molecule cant be explained
The structure of nitrogen dioxide (NO2) is often misrepresented due to the presence of an odd number of valence electrons, resulting in an unpaired electron. This leads to a radical species that cannot be accurately depicted using traditional Lewis structures, which typically assume a stable electron pair configuration. Instead, the resonance forms of NO2 illustrate its actual structure, where one nitrogen-oxygen bond is a double bond, and the other is a single bond, with one unpaired electron contributing to its reactivity. Thus, relying solely on a static Lewis structure fails to capture the dynamic nature of this molecule.
Yes, the nitrate ion (NO3-) is considered an odd-electron species because it has an unpaired electron. In its Lewis structure, the molecule has a total of 24 valence electrons (5 from nitrogen and 18 from three oxygen atoms, plus one extra electron for the negative charge), leading to an unpaired electron configuration. This characteristic can influence its reactivity and bonding behavior in chemical reactions.
The electronegativity variance here is not great enough to make this an ionic compound, so nitrous oxide is covalent and molecular.
Yes, NO2 is a radical species with an odd number of electrons. This is due to the unpaired electron present in the nitrogen atom, making it paramagnetic and reactive.
odd * odd = odd answer even * even = even answer odd * even = even answer
That happens because 5 is an odd number. An odd number times an odd number will give you an odd product; an odd number times an even number will give you an even product. The same happens for the multiples of any other odd number.
chlorine and oxygen both have different electro negativities due to which polarity develops between the bond and one odd electron present in chlorine make different type of Dpie - Ppie bond with it
Addition of two odd numbers will always give an even number.
No. In all likelihood, you will not break a single molecule. SO the number of molecules will remain odd or even - as it was before the breakage.
That's impossible. Adding up an odd number of odd numbers will give an answer that is an odd number. 50 is an even number. So adding up 5(5 is an odd number) odd numbers will not give 50, an even number.
This is Cu2+ and is a d9 system. It has one unpaired electron. The odd electron can be found out using magnetic susceptibility measurements or by electron paramagnetic resonance (EPR) spectroscopy.
in ClO2 ,the central Cl atom is sp2 hybridized with O-Cl-O angle of 118 degree.....the bond lengths are both 149 pm .....Cl-O bond has appreciable double bond character due to p(pi)-d(pi) bonding..the molecule is paramagnetic since it has one electron in a p-orbital... now often odd electron molecules dimerizes in order to pair the electron but ClO2 does not ...this is probably due to the reason that odd electron is delocalized as it is involved in p(pi)-d(pi) bonding.. in contrast the odd electron on N in NO2 is localized as nitrogen does not contain a d orbital...
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