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This compound is non polar because it is symmetrical in shape which makes the vector sum equal to zero. I think the electronegativity will not play any major role as opposite vectors are cancelling each other..


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I understand your assumption of selenium disulfide being a simple molecular like that. It is similar to the mistake of silicon dioxide, which at first glance we might assign it to be a linear molecule like carbon dioxide. However the crystal structure of silicon dioxide is far more complex. In selenium disulfide, the selenium and sulfur atoms form a 8-...


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When you compute formal charges you split bonding electrons evenly between bonded atoms. This does not account for differences in electronegativity. It is similar to the difference between formal charge and oxidation state, as well explained in the Wikipedia. A better picture (closer to the real electronic distribution) is, as Pauling would probably suggest, ...


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Electronegativity is a rather slippery thing, really. Roughly speaking, it depends on both electron affinity (the tendency to take on a negative charge) and ionization enthalpy (the tendency not to assume a positive charge). Chlorine has the highest electron affinity among halogens, true; but fluorine has a much higher ionization energy, a difference of ...


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Fluorine is a rather small atom. The incoming electron is put into a region of space already crowded with electrons. So there is a significant amount of repulsion, which lessens the attraction the incoming electron feels, and so lessens the electron affinity. A similar reversal happens between Oxygen and Sulfur. The firs electron affinity of oxygen (-$142 kJ/...


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I will use electron gain enthalpy(ega) to explain this. ega becomes less negative down a group in general. However, adding an electron to 2p orbital leads to greater repulsion than adding an electron to 3 p orbital and this, chlorine has the highest ega(the magnitude) and hence, the highest electron affinity.


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