It would be trigonal planar. The N central atom has a double bonded O and a single bonded O and one lone electron.
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.
NO2 readily forms a dimer because of its unpaired electron in the nitrogen atom, leading to dimerization to minimize the unpaired electron's energy. The dimer, N2O4, is more stable due to the delocalization of the electron density over both nitrogen atoms.
NO2 dimerizes to form N2O4 due to the reversible reaction between two NO2 molecules. This dimerization occurs at low temperatures and high pressures, resulting in the formation of more stable N2O4 molecules. The equilibrium between NO2 and N2O4 shifts towards the formation of N2O4 as the temperature decreases.
The electron-domain geometry of ClO4- is tetrahedral. It has four electron domains around the central chlorine atom, resulting in a tetrahedral arrangement.
The electron domain geometry for CS2 is linear, as sulfur has two bonding pairs and no lone pairs of electrons around it.
The NO2- ion has one lone electron pair.
There are 2 lone electron pairs in the NO2 ion. The nitrogen atom has one lone pair, and each oxygen atom has one lone pair, totaling to 2 lone pairs.
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.
Yes, NO2 (nitrogen dioxide) can act as an electrophile because it contains a partial positive charge on the nitrogen atom, making it attracted to electron-rich species. Electrophiles are electron-deficient species that can accept a pair of electrons in a chemical reaction.
The electron-domain geometry of PF6 is Octahedral, since the central atom Phosphorus has an electron pair geometry which is octahedral
Electron Domain is Tetrahedral Molecular Geometry is Trigonal Pyramidal
NO2 readily forms a dimer because of its unpaired electron in the nitrogen atom, leading to dimerization to minimize the unpaired electron's energy. The dimer, N2O4, is more stable due to the delocalization of the electron density over both nitrogen atoms.
NO2 dimerizes to form N2O4 due to the reversible reaction between two NO2 molecules. This dimerization occurs at low temperatures and high pressures, resulting in the formation of more stable N2O4 molecules. The equilibrium between NO2 and N2O4 shifts towards the formation of N2O4 as the temperature decreases.
The electron-domain geometry of ClO4- is tetrahedral. It has four electron domains around the central chlorine atom, resulting in a tetrahedral arrangement.
The electron domain charge cloud geometry of ICI5 s usually positively charged. This is because the process involves the loss of electrons. The electron-domain charge-cloud geometry of ICl5 is octahedral.
Though nitrogen dioxide has a single lone electron, it is not a radical, but a stable molecule.
3 bondings + 1 electron pair = 4 (electron domains)