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A molecule has a bond angle of 180°. Assuming that the central atom X follows the octet rule and forms no coordinate bonds, which of the following statements regarding the molecule is MOST likely FALSE?
The central atom X uses hybrid orbitals for bonding.
The molecule is linear.
The central atom X has no lone pairs of electrons.
The molecule must be polar if X and Y have different electronegativities.
Which factor does NOT contribute significantly to the difference in bond lengths between single, double, and triple bonds?
Bond Order
Atomic Size
Bond Strength
Electronegativity differences
Which of the following statements regarding the hybridization of [Ni(CN)4]2- and [NiCl4]2- is INCORRECT?
[Ni(CN)4]2- is square planar and diamagnetic
[NiCl4]2- is tetrahedral and paramagnetic
[Ni(CN)4]2- is dsp2 hybridized
[Ni(CN)4]2- is paramagnetic
A molecule AB4 has a see-saw shape. Considering Valence Bond Theory, what is the most likely hybridization of the central atom A and its likely outer electronic configuration?
sp3, ns2np2
sp3d, ns2np3
sp3d2, ns2np4
dsp3, ns2np3nd1
The complex ion [Fe(H2O)6]2+ is paramagnetic. Which of the following statements correctly explains this observation using Valence Bond Theory?
H2O is a strong field ligand, resulting in d2sp3 hybridization with no unpaired electrons.
H2O is a weak field ligand, resulting in sp3d2 hybridization with four unpaired electrons in the 3d orbitals of Fe2+.
H2O is a strong field ligand, resulting in sp3d2 hybridization with two unpaired electrons in the 3d orbitals of Fe2+.
H2O is a weak field ligand, resulting in dsp2 hybridization with two unpaired electrons in the 3d orbitals of Fe2+.
Consider the molecule SF4. According to VBT, what is the hybridization of the sulfur atom and the approximate bond angle between the axial and equatorial fluorine atoms?
sp3, 109.5°
sp3d, slightly less than 90°
sp3d2, 90°
dsp3, 120°
Which of the following offers the best explanation for the square planar geometry of XeF4 based on Valence Bond Theory?
Xe undergoes sp3 hybridization, with the two lone pairs occupying opposite corners of a tetrahedron.
Xe undergoes sp3d hybridization, with the two lone pairs occupying equatorial positions.
Xe undergoes sp3d2 hybridization, with the two lone pairs occupying axial positions to minimize repulsion, leading to a square planar arrangement of the four Xe-F bonds.
Xe undergoes dsp2 hybridization, similar to transition metal complexes.
A molecule AX has a bond angle slightly less than 109.5°. Which of the following is the most likely structure and hybridization of the central atom A?
Tetrahedral, sp
Trigonal planar, sp
Trigonal pyramidal, sp
Bent, sp
