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Chapter 9: Problem 45

For each statement, indicate whether it is true or false. (a) \(\ln\) order to make a covalent bond, the orbitals on each atom in the bond must overlap. (b) A \(p\) orbital on one atom cannot make a bond to an \(s\) orbital on another atom. \((\mathbf{c})\) Lone pairs of electrons on an atom in a molecule influence the shape of a molecule. (d) The 1 s orbital has a nodal plane. \((\mathbf{e})\) The \(2 p\) orbital has a nodal plane.

Short Answer

Expert verified
a) TRUE, b) FALSE, c) TRUE, d) FALSE, e) TRUE

Step by step solution

01

a) Orbital overlap for covalent bonds

To form a covalent bond, the orbitals of the bonded atoms must overlap, allowing electrons to be shared between the atoms. The statement is TRUE.
02

b) p orbital - s orbital bonding

It is possible for a p orbital on one atom to bond with an s orbital on another atom. For example, a carbon atom with three p orbitals and a hydrogen atom with one s orbital can form a C-H bond in a molecule like methane (CH4). The statement is FALSE.
03

c) Lone pairs' influence on molecular shape

Lone pairs of electrons on an atom can indeed influence the shape of a molecule, as they occupy space and create repulsion with surrounding electron regions. This can cause bond angles to change and result in different molecular geometries. The statement is TRUE.
04

d) 1s orbital nodal plane

A nodal plane is a region in space where electron probability density is zero. The 1s orbital is a spherical orbital surrounding the nucleus, and there is no region with zero electron probability density. Therefore, the statement is FALSE.
05

e) 2p orbital nodal plane

The 2p orbital has a dumbbell shape, with two lobes separated by a nodal plane running through the nucleus. In this nodal plane, electron probability density is zero. So, the statement is TRUE.

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Most popular questions from this chapter

What is the distinction between a bond dipole and a molecular dipole moment?

Would you expect the nonbonding electron-pair domain in \(\mathrm{NCl}_{3}\) to be greater or smaller in size than the corresponding one in $\mathrm{PCl}_{3} ?$

Methyl isocyanate, \(\mathrm{CH}_{3} \mathrm{NCO},\) was made infamous in 1984 when an accidental leakage of this compound from a storage tank in Bhopal, India, resulted in the deaths of about 3800 people and severe and lasting injury to many thousands more. (a) Draw a Lewis structure for methyl isocyanate. (b) Draw a ball-and-stick model of the structure, including estimates of all the bond angles in the compound. (c) Predict all the bond distances in the molecule. (d) Do you predict that the molecule will have a dipole moment? Explain.

The structure of borazine, \(\mathrm{B}_{3} \mathrm{~N}_{3} \mathrm{H}_{6},\) is a six-membered ring of alternating \(\mathrm{B}\) and \(\mathrm{N}\) atoms. There is one \(\mathrm{H}\) atom bonded to each \(B\) and to each \(\mathrm{N}\) atom. The molecule is planar. (a) Write a Lewis structure for borazine in which the formal charge on every atom is zero. (b) Write a Lewis structure for borazine in which the octet rule is satisfied for every atom. (c) What are the formal charges on the atoms in the Lewis structure from part (b)? Given the electronegativities of \(B\) and \(N,\) do the formal charges seem favorable or unfavorable? (d) Do either of the Lewis structures in parts (a) and (b) have multiple resonance structures? (e) What are the hybridizations at the \(\mathrm{B}\) and \(\mathrm{N}\) atoms in the Lewis structures from parts (a) and (b)? Would you expect the molecule to be planar for both Lewis structures? (f) The six \(\mathrm{B}-\mathrm{N}\) bonds in the borazine molecule are all identical in length at \(144 \mathrm{pm} .\) Typical values for the bond lengths of \(\mathrm{B}-\mathrm{N}\) single and double bonds are \(151 \mathrm{pm}\) and \(131 \mathrm{pm},\) respectively. Does the value of the \(\mathrm{B}-\mathrm{N}\) bond length seem to favor one Lewis structure over the other? (g) How many electrons are in the \(\pi\) system of botazine?

Ammonia, \(\mathrm{NH}_{3}\), reacts with incredibly strong bases to produce the amide ion, \(\mathrm{NH}_{2}\) -. Ammonia can also react with acids to produce the ammonium ion, \(\mathrm{NH}_{4}^{+}\). (a) Which species (amide ion, ammonia, or ammonium ion) has the largest \(\mathrm{H}-\mathrm{N}-\mathrm{H}\) bond angle? (b) Which species has the smallest \(\mathrm{H}-\mathrm{N}-\mathrm{H}\) bond angle?
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