Multiple Choice
Determine the molecular geometry for the following molecule:SeH2Cl2
12. Molecular Shapes & Valence Bond Theory
Molecular Geometry
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Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
What is the molecular shape of XeF4?
A
tetrahedral
B
trigonal pyramidal
C
T-shape
D
see-saw
E
square planar
Verified step by step guidance1
Identify the central atom in the molecule XeF4, which is xenon (Xe).
Determine the total number of valence electrons. Xenon has 8 valence electrons, and each fluorine (F) has 7 valence electrons. Since there are 4 fluorine atoms, the total number of valence electrons is 8 + (4 * 7) = 36.
Draw the Lewis structure for XeF4. Place xenon in the center and arrange the four fluorine atoms around it. Connect each fluorine to xenon with a single bond, using 8 electrons (4 pairs).
Calculate the remaining electrons after forming bonds. Initially, you have 36 electrons, and 8 are used in bonds, leaving 28 electrons. Distribute these electrons to satisfy the octet rule for each fluorine atom, using 24 electrons (6 per fluorine).
Determine the molecular geometry using VSEPR theory. Xenon has 4 bonded pairs and 2 lone pairs of electrons. The electron pair geometry is octahedral, but the molecular shape, considering only the atoms, is square planar.
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