Question

answer the questions in the table below about the shape of the chlorine pentafluoride (clf₅) molecule.
how many electron groups are around the central chlorine atom?
note: one electron group means one lone pair, one single bond, one double bond, or one triple bond.
what phrase best describes the arrangement of these electron groups around the central chlorine atom?
(you may need to use the scrollbar to see all the choices.)
linear
bent
t - shaped
trigonal planar
trigonal pyramidal
square planar
square pyramidal
tetrahedral
sawhorse

Explanation:

First Question (Number of Electron Groups)

Step1: Determine bonding and lone pairs

Chlorine (Cl) in $\ce{ClF5}$ has 5 single bonds with F atoms and 1 lone pair (since Cl has 7 valence electrons: 5 used in bonding, 2 left as a lone pair).

Step2: Count electron groups

Each single bond is 1 electron group, and the lone pair is 1. So total electron groups = 5 (bonds) + 1 (lone pair) = 6.

For a central atom with 6 electron groups (5 bonding, 1 lone pair), the electron - group arrangement (considering both bonding and lone pairs) follows the octahedral electron - group geometry, but the molecular shape (arrangement of atoms) is square pyramidal. Wait, no—wait, the question is about the arrangement of electron groups (including lone pairs). Wait, no, actually, when we have 6 electron groups (5 bonding, 1 lone pair), the electron - group geometry (arrangement of all electron groups) is octahedral? Wait, no, no—wait, the options given: let's re - evaluate. Wait, $\ce{ClF5}$: central Cl, 5 F atoms (single bonds) and 1 lone pair. So total electron groups: 6. The electron - group arrangement (the geometry that describes the positions of all electron groups) for 6 electron groups is octahedral? But the options don't have octahedral? Wait, no, maybe I made a mistake. Wait, the options include square pyramidal? Wait, no, the question is about the arrangement of electron groups (including lone pairs). Wait, no, maybe the question is about the molecular shape (arrangement of atoms). Wait, no, the first question is about the number of electron groups (6), the second is about the arrangement of these electron groups (including lone pairs). Wait, no, the options: let's check the options again. Wait, the options are linear, bent, T - shaped, trigonal planar, trigonal pyramidal, square planar, square pyramidal, tetrahedral, sawhorse. Wait, for 6 electron groups (5 bonding, 1 lone pair), the molecular shape (arrangement of atoms) is square pyramidal. But the question is about the arrangement of electron groups (including the lone pair). Wait, maybe the question is misphrased, and it's about the molecular shape. Wait, no, the first question is about the number of electron groups (6). For the second question, when we have 6 electron groups (5 bonding, 1 lone pair), the arrangement of the electron groups (the geometry that accounts for both bonding and lone pairs) is octahedral, but since one of the positions is a lone pair, the molecular shape (arrangement of atoms) is square pyramidal. But the options include square pyramidal. Wait, maybe the question is about the molecular shape (arrangement of atoms, i.e., the arrangement of the bonding groups and the lone pair's influence on the atom positions). So with 5 bonding groups and 1 lone pair, the shape is square pyramidal.

Answer:

6

Second Question (Electron Group Arrangement)