Domanda del libro di testo
Draw Lewis structures for the following: (d) H2SO4 (H is bonded to O) (e) OF2
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Ch.8 - Basic Concepts of Chemical Bonding
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Capitolo 8, Problema 47f
Draw Lewis structures for the following: (f) NH2OH
Guida verificata passo dopo passo1
Step 1: Determine the total number of valence electrons. Nitrogen (N) has 5 valence electrons, Hydrogen (H) has 1 valence electron, and Oxygen (O) has 6 valence electrons. Since there are 2 Hydrogen atoms and 1 Oxygen atom, the total number of valence electrons is 5 (from N) + 2*1 (from 2 H) + 6 (from O) = 14 valence electrons.
Step 2: Draw a skeleton structure of the molecule. Nitrogen is the least electronegative atom (excluding Hydrogen), so it will be the central atom. Connect the Nitrogen atom to the Oxygen atom and each Hydrogen atom with a single bond. Each single bond represents 2 electrons.
Step 3: Distribute the remaining electrons as lone pairs. Start from the outer atoms. Hydrogen atoms are already filled because they can hold only 2 electrons. So, place the remaining electrons on the Oxygen and Nitrogen atoms. Each atom should have 8 electrons (octet rule) except Hydrogen which can only hold 2 electrons.
Step 4: If there are not enough electrons to give every atom an octet, try multiple bonds (double, triple). In this case, all atoms satisfy the octet rule, so no need for multiple bonds.
Step 5: Verify the structure. Check that the total number of electrons in the Lewis structure is the same as the total number of valence electrons calculated in step 1. Also, make sure each atom satisfies the octet rule (or duet rule for Hydrogen).
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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 represent bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting reactivity.
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04:28
Lewis Dot Structures: Ions
Valence Electrons
Valence electrons are the outermost electrons of an atom and are crucial in determining how atoms bond with each other. The number of valence electrons influences the molecule's structure and stability. For NH2OH, knowing the valence electrons of nitrogen, oxygen, and hydrogen helps in accurately constructing its Lewis structure.
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Percorso guidato
02:12Transition Metals Valence Electrons
Octet Rule
The octet rule states that atoms tend to form bonds 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 guides the arrangement of electrons in Lewis structures, ensuring that each atom, particularly carbon, nitrogen, and oxygen, satisfies this rule when possible.
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Percorso guidato
01:36Octet Rule
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