Textbook Question
Dichloroethylene (C2H2Cl2) has three forms (isomers), each of which is a different substance. (b) Which of these isomers has a zero dipole moment?
Ch.9 - Molecular Geometry and Bonding Theories
Chapter 9, Problem 45
For each statement, indicate whether it is true or false. (a) In 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.
Verified step by step guidance1
Step 1: Understand the concept of covalent bonding. Covalent bonds are formed when two atoms share electrons. This sharing occurs through the overlap of atomic orbitals, which allows the electrons to be shared between the atoms.
Step 2: Analyze statement (a). Consider the requirement for orbital overlap in covalent bonding. Since covalent bonds involve the sharing of electrons through overlapping orbitals, determine if the statement about the necessity of orbital overlap is true or false.
Step 3: Understand the types of orbitals involved in bonding. Orbitals such as s, p, d, and f can participate in bonding. The s orbital is spherical, while p orbitals are dumbbell-shaped, and they can overlap with each other or with other types of orbitals.
Step 4: Analyze statement (b). Consider whether a p orbital on one atom can overlap with an s orbital on another atom. Recall that different types of orbitals can indeed overlap to form bonds, such as the overlap between an s orbital and a p orbital, which is common in many molecules.
Step 5: Evaluate the truth of each statement based on your understanding of orbital overlap and bonding. Use your knowledge of how different orbitals can interact to determine the truth value of each statement.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Covalent Bonding
Covalent bonding occurs when two atoms share one or more pairs of electrons, allowing each atom to attain a stable electron configuration. This sharing typically involves the overlap of atomic orbitals, which can include s, p, and d orbitals, depending on the atoms involved. The strength and characteristics of the bond depend on the extent of this overlap.
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02:03
Chemical Bonds
Orbital Overlap
Orbital overlap is a fundamental concept in covalent bonding, where the atomic orbitals of two atoms intersect, allowing for the sharing of electrons. The greater the overlap, the stronger the bond formed. This principle is crucial for understanding how different types of orbitals (s, p, d) can interact to form stable molecules.
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03:06Molecular Orbital Theory
Types of Atomic Orbitals
Atomic orbitals are regions in an atom where there is a high probability of finding electrons. The main types include s orbitals (spherical) and p orbitals (dumbbell-shaped). While p orbitals can indeed overlap with s orbitals to form covalent bonds, the specific orientation and energy levels of the orbitals involved can influence the bond's characteristics.
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Related Practice
Textbook Question
Dichloroethylene (C2H2Cl2) has three forms (isomers), each of which is a different substance. (c) How many isomeric forms can chloroethylene, C2H3Cl, have? Would they be expected to have dipole moments?
Textbook Question
Dihydroxybenzene, C6H6O2, exists in three forms (isomers) called ortho, meta, and para:
Which of these has a nonzero dipole moment?
Textbook Question
Draw sketches illustrating the overlap between the following orbitals on two atoms: (a) the 2s orbital on each atom
Textbook Question
Draw sketches illustrating the overlap between the following orbitals on two atoms: (b) the 2pz orbital on each atom (assume both atoms are on the z-axis) (c) the 2s orbital on one atom and the 2pz orbital on the other atom.
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Textbook Question
For each statement, indicate whether it is true or false. (d) Nonbonding electron pairs cannot occupy a hybrid orbital.