109.5
Electron geometry for this is tetrahedral. There are two O-F single bonds, which makes 2 electron groups. There are two lone pairs around oxygen, which make up the last two electron groups. Molecules with four electron groups has a tetrahedral Electron geometry.
Trigonal pyramidal. As has 5 valence electrons. It forms single bonds with each of the F atoms, donating one electron to each bond. This leaves 2 unbonded electrons, or a single lone pair. Thus the molecule has 4 different groups attached to As, and the electron configuration is tetrahedral. A tetrahedral configuration with one lone pair results in a trigonal pyramidal molecular geometry.
False. In geometry it is helpful to group objects and look at similarities between them.
different
It promote national integration
tetrahedral
Electron geometry for this is tetrahedral. There are two O-F single bonds, which makes 2 electron groups. There are two lone pairs around oxygen, which make up the last two electron groups. Molecules with four electron groups has a tetrahedral Electron geometry.
180°
Trigonal pyramidal. As has 5 valence electrons. It forms single bonds with each of the F atoms, donating one electron to each bond. This leaves 2 unbonded electrons, or a single lone pair. Thus the molecule has 4 different groups attached to As, and the electron configuration is tetrahedral. A tetrahedral configuration with one lone pair results in a trigonal pyramidal molecular geometry.
tetrahederal
tetrahedral, if it had three electron groups it would be trigonal planar
linear
three dimensional arrangement of atoms electron-group geometry
electron-group geometry
trigonal planar
False. In geometry it is helpful to group objects and look at similarities between them.
Anything with six electron groups, keep in mind an electron group is a bonded atom or an electron pair, is an octahedral. Anything in an octahedral and a lone pair is the square pyramidal geometry. So all angles between the atoms are a little less than 90 degrees and the angle of the electron pair is greater than 90.