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Chemistry - Bond Angles In NH3 And NCl3

Answer : Solution 1: As Tan Yong Boon stated, it is Bent’s Rule with which we can explain the lower bond angle of \ce N F 3 \ce{NF3} \ce NF 3 when compared to \ce N H 3 \ce{NH3} \ce N H 3 . The rule as stated by Henry Bent: Atomic s character concentrates in orbitals directed towards electropositive substituents. Fluorine is more electronegative that hydrogen, and the \ce N − F \ce{N−F} \ce N − F bond would have greater p character than the \ce N − H \ce{N−H} \ce N − H bond. And more s character leads to large bond angles. Thus, the bond angle is greater in \ce N H 3 \ce{NH3} \ce N H 3 than in \ce N F 3 \ce{NF3} \ce NF 3 . Now, consider \ce N C l 3 \ce{NCl3} \ce NCl 3 . Clearly, \ce C l \ce{Cl} \ce Cl atom islarger in size than the central atom, nitrogen. Hence the higher bond angle here is due to the steric crowding caused by \ce C l \ce{Cl} \ce Cl atoms.(More pronounced than the electrongativity of \ce C l \ce{Cl} \ce Cl atom). They repel eachother and hence b...
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Are Regular VACUUM ANALYZE Still Recommended Under 9.1?

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Change The Font Size Of Visual Studio Solution Explorer

Answer : Go to Tools->Options->Environment->Fonts and Colors In "Show Settings for" chose "Environment Font" In "Font" replace Automatic to for example, Arial and change size. Change the font size of that setting, all Font size in the Explorers (Solution Explorer, Server Explorer and Toolbox) and menus will change. You can set that in Tools, Options.
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