Domanda del libro di testo
Draw Lewis structures that satisfy the octet rule for the following molecules and ions: f. HOCl
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Ch.8 - Basic Concepts of Chemical Bonding
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Capitolo 8, Problema 50
Write Lewis structures that satisfy the octet rule for the following molecules and ions: a. NH4+, b. C2F4 (the two C atoms are bonded to one another), c. COCl2 (the Cl atoms are bonded to C), d. HSO3− (H is bonded to one of the O atoms), e. HNC (H and C are both bonded to N), f. ClO3−.
Guida verificata passo dopo passo1
Step 1: Determine the total number of valence electrons for each molecule or ion. For ions, adjust the count by adding electrons for negative charges or subtracting for positive charges.
Step 2: Arrange the atoms with the least electronegative atom in the center (except for hydrogen, which is always terminal). For polyatomic ions, consider the charge distribution.
Step 3: Connect the atoms using single bonds initially, and then distribute the remaining electrons to satisfy the octet rule for each atom, starting with the outer atoms.
Step 4: If any atoms lack an octet, consider forming double or triple bonds by sharing lone pairs from adjacent atoms.
Step 5: Verify that all atoms satisfy the octet rule (or duet for hydrogen) and that the total number of electrons used matches the total valence electrons calculated in Step 1. For ions, ensure the overall charge is correct.>
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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 indicate bonds between atoms. Understanding how to draw these structures is essential for visualizing molecular geometry and predicting reactivity, especially in the context of the octet rule.
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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. This rule helps predict the types of bonds that will form in molecules and is particularly relevant when drawing Lewis structures for various compounds.
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01:36Octet Rule
Formal Charge
Formal charge is a concept used to determine the distribution of electrons in a molecule and to assess the stability of a Lewis structure. It is calculated by comparing the number of valence electrons an atom has in its free state to the number of electrons assigned to it in the Lewis structure. Minimizing formal charges across a molecule often leads to the most stable structure, guiding the correct representation of complex molecules.
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01:53Formal Charge
Pratica correlata
Domanda del libro di testo
Which one of these statements about formal charge is true? (a) Formal charge is the same as oxidation number. (b) To draw the best Lewis structure, you should minimize formal charge. (c) Formal charge takes into account the different electronegativities of the atoms in a molecule. (d) Formal charge is most useful for ionic compounds. (e) Formal charge is used in calculating the dipole moment of a diatomic molecule.
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Domanda del libro di testo
Draw Lewis structures that satisfy the octet rule for the following molecules and ions: c. SO32−
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Domanda del libro di testo
For each of the following ions of nitrogen and oxygen, write a single Lewis structure that obeys the octet rule, and calculate the oxidation numbers and formal charges on all the atoms: c. NO2+.
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Domanda del libro di testo
Draw Lewis structures that satisfy the octet rule for the following molecules and ions: d. HCN (H and N are both bonded to C),
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