Select all molecular geometries (shapes) that are possible for a molecule with five electron groups an the central atom.

Do not include molecular geometries that can only be produced by having a single bonding group on the central atom (all but one of the electron groups are lone pairs.)

ocahedral

T-shaped

linear

bent

trigonal pyramidal

trigonal bipyramidal

seesaw

square pyramidal

trigonal planar

tetrahedral

square planar

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Reid WolffLv2

13 Dec 2019

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Related questions

a. Draw the Lewis structure of showing all lone pairs.

b. Is molecule polar or nonpolar?

c. Is the molecular geometry of a square planar, trigonal pyramidal, linear, trigonal planar, see-saw, square pyramidal, trigonal bipyramidal, bent, tetrahedral, T-shaped, octahedral?

d. What are the approximate bond angles in ? Select what may be applied if 90degrees, 109.5degrees, 120degrees, 180degrees

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Draw the Lewis structure for , then answer the following questions:

a. How many valence electrons does this compound have?

b. How many bonded electrons does this compound have?

c. How many lone pairs of electrons does this compound have?

d. How many single bonds does this compound have?

e. How many double bonds does this compound have?

f. What is the electron group arrangement (aka electron pair geometry) (enter one of the following: linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral)?

g. What is the molecular arrangement (aka shape) (enter one of the following: linear, trigonal planar, tetrahedral, trigonal pyramidal, bent, trigonal bipyramidal, seesaw, T-shaped, octahedral, square pyramidal, square planar)?

h. Predict the approximate bond angle (enter e.g. 90, 109.5, 120, 180, <109.5, >109.5).