Both O and S have the same outer electric configuration of ns2 and np4.Sulfur or iron pyrites are burnt in excess of air to produce SO 2.ĤFeS 2 + 11O 2-> 2Fe 2O 3 (solid) + 8SO 2 (gas) Similarities between Sulfur and Oxygen atoms valence electrons of oxygen = 6 (There are two oxygen atoms in the compound.).The sulfur valence electron is equal to 6.
The three pairs of bonding electrons are arranged in the plane at an angle of 120 degrees.The electron geometry of SO 2 is formed in the shape of a trigonal planner.(Sorry for including an extra question, thank you for your help so far.The molecular mass of sulfur is 32.066 g/mol. But it seems that's wrong, but I can't find a clear answer why. They would then repel each other more, causing them in turn to repel the bond electrons more, making the bond angle smaller. I would've thought that the higher the EN, the smaller the bond angle would be, because I thought higher EN means a higher electron density near the nucleus, which would bring the lone electron pairs closer to the nucleus. It is said that the higher the EN, the bigger the bond angle, but I don't exactly see why. I looked up how the central atom could affect the bond angle, and apparently electronegativity influences the bond angle too. I don't exactly see the connection between the bond angle and the magnitude of the charges yet. The larger the distance the smaller the force. The force between two charges depends on their magnitude and. There is a small difference from 'nominal' (what VSEPR predicts), because.īecause of the lone pairs that repel the shared pairs, so it should be slightly less than 120 deg. English is not my first language and I'm still getting used to the technical terms. Yes, I know about that, I misunderstood your previous question, my apologies. Is there something I missed? Or is it a trick question?īecause lone pairs spread out more, in effect, are more repulsive. SO2 (sulfur dioxide) has the same lewis structure, same resonance structures, and again all of the atoms are sp2-hybridized with one delocalized electron pair, and it leads to the same geometry: trigonal planar (120 degrees) and bent (slightly less than 120 degrees). Therefore the bond angle should be slightly less than 120 degrees. All of the atoms are sp2-hybridized (+1 delocalized electron pair), which means the electron group geometry is trigonal planar (120 degrees in between bonds), and the molecular geometry is bent. In every way I look at it, both molecules have the same structure with the same bond angle.Īfter drawing the lewis structure of NO2- (nitrite), you can see that there are 2 resonance structures. Which of these bonds has the biggest bond angle? Our chemistry teacher gave us a list of test questions to prepare ourselves for an upcoming exam, but I fail to find the answer to this one question.Įxplain the structure of NO2- and SO2- by using the VSEPR theory. A screenshot is preferable to a picture of your laptop screen. Please do not ask for help acquiring, preparing, or handling illicit substances or for help with any activity that does not fall within the confines of whatever laws apply to your particular location.īonus points: If submitting a picture please make sure that it is clear. Any infractions will be met with a temporary ban at the first instance and a permanent ban if there is another.
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