Textbook Question
a. Predict the electron-domain geometry around the central Xe atom in XeF2, XeF4, and XeF6.
12. Molecular Shapes & Valence Bond Theory
Electron Geometry
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Determine the number of electron groups for the following cation:AsBr2+.
A. 2
B. 3
C. 4
D. 1
A
2
B
3
C
4
D
1
Verified step by step guidance1
Identify the central atom in the cation AsBr2+. The central atom is arsenic (As).
Determine the number of valence electrons for the central atom, arsenic (As). Arsenic is in group 15 of the periodic table, so it has 5 valence electrons.
Consider the charge of the cation. AsBr2+ has a positive charge, indicating the loss of one electron. Therefore, subtract one electron from the total valence electrons of arsenic, resulting in 4 valence electrons.
Count the number of bonds formed by the central atom. Arsenic is bonded to two bromine atoms, forming two single bonds. Each bond represents one electron group.
Add the number of lone pairs on the central atom. With 4 valence electrons and 2 used for bonding, arsenic has 2 electrons left, forming one lone pair. Therefore, the total number of electron groups is the sum of bonds and lone pairs: 2 bonds + 1 lone pair = 3 electron groups.
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