Textbook Question
a. Draw the resonance forms for SO2 (bonded O–S–O).
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Ch.1 - Structure and Bonding
Wade9th EditionOrganic ChemistryISBN: 9780135213728
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Table of contents
- Ch.1 - Structure and Bonding107
- Ch. 2 - Acids and Bases; Functional Groups115
- Ch.3 - Structure and Stereochemistry of Alkanes100
- Ch.4 - The Study of Chemical Reactions99
- Ch.5 - Stereochemistry93
- Ch.6 - Alkyl Halides; Nucleophilic Substitution118
- Ch. 7 - Structure and Synthesis of Alkenes; Elimination158
- Ch.8 - Reactions of Alkenes171
- Ch.9 - Alkynes91
- Ch.10 - Structure and Synthesis of Alcohols143
- Ch.11 - Reactions of Alcohols104
- Ch. 12 - Infrared Spectroscopy and Mass Spectrometry22
- Ch. 13 - Nuclear Magnetic Resonance Spectroscopy45
- Ch. 14 - Ethers, Epoxides, and Thioethers72
- Ch. 15 - Conjugated Systems, Orbital Symmetry, and Ultraviolet Spectroscopy89
- Ch. 16 - Aromatic Compounds74
- Ch. 17 - Reactions of Aromatic Compounds126
- Ch. 18 - Ketones and Aldehydes193
- Ch. 19 - Amines129
- Ch. 20 - Carboxylic Acids77
- Ch. 21 - Carboxylic Acid Derivatives141
- Ch. 22 - Condensations and Alpha Substitutions of Carbonyl Compounds175
- Ch. 23 - Carbohydrates and Nucleic Acids93
- Ch. 24 - Amino Acids, Peptides, and Proteins54
Chapter 1, Problem 27
Name the element that corresponds to each electronic configuration.
a. 1s2 2s2 2p2
b. 1s2 2s2 2p4
c. 1s2 2s2 2p6 3s2 3p3
d. 1s2 2s2 2p6 3s2 3p5
Verified step by step guidance1
To determine the element from an electronic configuration, count the total number of electrons, which equals the atomic number of the element.
For configuration a (1s^2 2s^2 2p^2), add the electrons: 2 (1s) + 2 (2s) + 2 (2p) = 6 electrons. The element with atomic number 6 is Carbon (C).
For configuration b (1s^2 2s^2 2p^4), add the electrons: 2 (1s) + 2 (2s) + 4 (2p) = 8 electrons. The element with atomic number 8 is Oxygen (O).
For configuration c (1s^2 2s^2 2p^6 3s^2 3p^3), add the electrons: 2 (1s) + 2 (2s) + 6 (2p) + 2 (3s) + 3 (3p) = 15 electrons. The element with atomic number 15 is Phosphorus (P).
For configuration d (1s^2 2s^2 2p^6 3s^2 3p^5), add the electrons: 2 (1s) + 2 (2s) + 6 (2p) + 2 (3s) + 5 (3p) = 17 electrons. The element with atomic number 17 is Chlorine (Cl).
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Electronic Configuration
Electronic configuration describes the distribution of electrons in an atom's orbitals. It follows the Aufbau principle, which states that electrons fill orbitals starting from the lowest energy level. Understanding electronic configurations helps identify elements based on their position in the periodic table.
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The Electron Configuration
Periodic Table
The periodic table organizes elements based on increasing atomic number and recurring chemical properties. Each element's position reflects its electronic configuration, allowing for easy identification of elements by their electron arrangement. Recognizing patterns in the table is crucial for determining the element corresponding to a given configuration.
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Valence Electrons
Valence electrons are the outermost electrons of an atom and determine its chemical properties and reactivity. For main group elements, the number of valence electrons corresponds to the group number in the periodic table. Identifying valence electrons from an electronic configuration helps pinpoint the element's group and thus its identity.
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Related Practice
Textbook Question
Both PCl3 and PCl5 are stable compounds. Draw Lewis structures for these two compounds.
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Textbook Question
There is a small portion of the periodic table that you must know to do organic chemistry. Construct this part from memory, using the following steps.
a. From memory, make a list of the elements in the first two rows of the periodic table, together with their numbers of valence electrons
b. Use this list to construct the first two rows of the periodic table.
c. Organic compounds often contain sulfur, phosphorus, chlorine, bromine, and iodine. Add these elements to your periodic table.
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Textbook Question
For each compound, state whether its bonding is covalent, ionic, or a mixture of covalent and ionic.
a. NaCl
b. NaOH
c. CH3Li
d. CH2Cl2
e. NaOCH3
f. HCO2Na
g. CF4
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1
rank
Textbook Question
b. Draw the resonance forms for ozone (bonded O–O–O)
c. Sulfur dioxide has one more resonance form than ozone. Explain why this structure is not possible for ozone.
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1
rank
Textbook Question
Give the relationship between the following pairs of structures. The possible relationships are:
same compound
constitutional isomers (structural isomers)
cis-trans isomers
not isomers (different molecular formula)
(j)
(k)
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