Textbook Question
In the vapor phase, BeCl2 exists as a discrete molecule. (a) Draw the Lewis structure of this molecule, using only single bonds. Does this Lewis structure satisfy the octet rule?
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Ch.8 - Basic Concepts of Chemical Bonding
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution156
- Ch.5 - Thermochemistry151
- Ch.6 - Electronic Structure of Atoms137
- Ch.7 - Periodic Properties of the Elements127
- Ch.8 - Basic Concepts of Chemical Bonding143
- Ch.9 - Molecular Geometry and Bonding Theories167
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces97
- Ch.12 - Solids and Modern Materials129
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics175
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Acid-Base Equilibria127
- Ch.17 - Additional Aspects of Aqueous Equilibria133
- Ch.18 - Chemistry of the Environment88
- Ch.19 - Chemical Thermodynamics140
- Ch.20 - Electrochemistry137
- Ch.21 - Nuclear Chemistry99
- Ch.22 - Chemistry of the Nonmetals66
- Ch.23 - Transition Metals and Coordination Chemistry69
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry11
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 8, Problem 61
Draw the dominant Lewis structures for these chlorine–oxygen molecules/ions: ClO, ClO-, ClO2-, ClO3-, ClO4-. Which of these do not obey the octet rule?
Verified step by step guidance1
Step 1: Identify the total number of valence electrons for each molecule/ion. For chlorine (Cl), it has 7 valence electrons, and for oxygen (O), it has 6 valence electrons. Consider any additional electrons due to negative charges.
Step 2: For each molecule/ion, arrange the atoms with chlorine as the central atom and connect the oxygen atoms to chlorine using single bonds initially.
Step 3: Distribute the remaining valence electrons to satisfy the octet rule for the oxygen atoms first, then place any remaining electrons on the chlorine atom.
Step 4: If the central chlorine atom does not have a complete octet, consider forming double bonds with oxygen atoms by converting lone pairs on oxygen to bonding pairs.
Step 5: Evaluate each structure to determine if the octet rule is obeyed. Note that molecules/ions with an odd number of electrons or those with expanded octets (like ClO4-) may not strictly follow the octet rule.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Lewis Structures
Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They use dots to represent valence electrons and lines to represent bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting the behavior of molecules.
Recommended video:
Guided course
04:28
Lewis Dot Structures: Ions
Octet Rule
The octet rule is a chemical rule of thumb that states atoms tend to bond in such a way that they each have eight electrons in their valence shell, achieving a stable electron configuration similar to that of noble gases. While this rule applies to many main-group elements, there are exceptions, particularly for elements in the third period and beyond, which can expand their octet.
Formal Charge
Formal charge is a concept used to determine the distribution of electrons in a molecule and to assess the stability of different Lewis structures. It is calculated by taking the number of valence electrons in an atom, subtracting the number of non-bonding electrons, and half the number of bonding electrons. Structures with the lowest formal charges on atoms are generally more stable and preferred.
Recommended video:
Guided course
01:53Formal Charge
Related Practice
Textbook Question
Mothballs are composed of naphthalene, C10H8, a molecule that consists of two six-membered rings of carbon fused along an edge, as shown in this incomplete Lewis structure:
(c) Not all of the C—C bond lengths in naphthalene are equivalent. Based on your resonance structures, how many C—C bonds in the molecule do you expect to be shorter than the others?
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Textbook Question
(a) Which of these compounds is an exception to the octet rule: carbon dioxide, water, ammonia, phosphorus trifluoride, or arsenic pentafluoride?
Textbook Question
Mothballs are composed of naphthalene, C10H8, a molecule that consists of two six-membered rings of carbon fused along an edge, as shown in this incomplete Lewis structure:
(b) Do you expect the C—C bond lengths in the molecule to be similar to those of C—C single bonds, C ═C double bonds, or intermediate between C—C single and C ═C double bonds?
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Textbook Question
Draw the Lewis structures for each of the following molecules or ions. Identify instances where the octet rule is not obeyed; state which atom in each compound does not follow the octet rule; and state how many electrons surround these atoms: (a) PF6-, (b) BeCl2, (c) NH3, (d) XeF2O (the Xe is the central atom), (e) SO42- .
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Textbook Question
In the vapor phase, BeCl2 exists as a discrete molecule. (b) What other resonance structures are possible that satisfy the octet rule?