Textbook Question
Look at the relative positions of each pair of atoms listed here in the periodic table. How many core electrons does each have? How many valence electrons does each have?
c. nitrogen and phosphorus
d. magnesium and calcium
Ch. 1 - Remembering General Chemistry: Electronic Structure and Bonding (Part 1)
Bruice8th EditionOrganic ChemistryISBN: 9780135213711
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Table of contents
- Ch. 1 - Remembering General Chemistry: Electronic Structure and Bonding (Part 1)31
- Ch. 1 - Remembering General Chemistry: Electronic Structure and Bonding (Part 2)65
- Ch. 2 - Acids and Bases: Central to Understanding Organic Chemistry84
- Ch. 3 - An Introduction to Organic Compounds:Nomenclature, Physical Properties, and Structure183
- Ch. 4 - Isomers: The Arrangement of Atoms in Space121
- Ch. 5 - Alkenes: Structure, Nomenclature, and an Introduction to Reactivity • Thermodynamics and Kinetics83
- Ch. 6 - The Reactions of Alkenes • The Stereochemistry of Addition Reactions175
- Ch. 7 - The Reactions of Alkynes • An Introduction to Multistep Synthesis119
- Ch. 8 - Delocalized Electrons: Their Effect on Stability, pKa, and the Products of a Reaction • Aromaticity and Electronic Effects: An Introduction to the Reactions of Benzene148
- Ch. 9 - Substitution and Elimination Reactions of Alkyl Halides212
- Ch. 10 - Reactions of Alcohols, Ethers, Epoxides, Amines, and Sulfur-Containing Compounds131
- Ch. 11 - Organometallic Compounds60
- Ch. 12 - Radicals90
- Ch. 13 - Mass Spectrometry; Infrared Spectroscopy; UV/Vis Spectroscopy62
- Ch. 14 - NMR Spectroscopy95
- Ch. 15 - Reactions of Carboxylic Acids and Carboxylic Acid Derivatives123
- Ch. 16 - Reactions of Aldehydes and Ketones • More Reactions of Carboxylic Acid Derivatives141
- Ch. 17 - Reactions at the Alpha-Carbon101
- Ch. 18 - Reactions of Benzene and Substituted Benzenes144
- Ch. 19 - More About Amines • Reactions of Heterocyclic Compounds49
- Ch. 20 - The Organic Chemistry of Carbohydrates80
- Ch. 21 - Amino Acids, Peptides, and Proteins57
- Ch. 22 - Catalysis in Organic Reactions and in Enzymatic Reactions35
- Ch. 23 - The Organic Chemistry of the Coenzymes—Compounds Derived from Vitamins1
- Ch. 28 - Pericyclic Reactions58
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Bruice 8th EditionCh. 1 - Remembering General Chemistry: Electronic Structure and Bonding (Part 1)Problem 7
Bruice 8th EditionCh. 1 - Remembering General Chemistry: Electronic Structure and Bonding (Part 1)Problem 7Chapter 1, Problem 7
a. Find potassium (K) in the periodic table and predict how many valence electrons it has.
b. What orbital does the unpaired electron occupy?
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Locate potassium (K) on the periodic table. Potassium is in Group 1 (alkali metals) and Period 4.
Determine the number of valence electrons for potassium. Elements in Group 1 have 1 valence electron because they have one electron in their outermost shell.
Write the electron configuration for potassium. Potassium has an atomic number of 19, so its electron configuration is: for the outermost shell.
Identify the orbital where the unpaired electron resides. The unpaired electron in potassium occupies the 4s orbital, as the electron configuration ends with .
Conclude that potassium has 1 valence electron, and its unpaired electron is in the 4s orbital.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Valence Electrons
Valence electrons are the outermost electrons of an atom and are crucial for determining how an element will react chemically. For potassium (K), which is in group 1 of the periodic table, it has one valence electron. This single electron is responsible for potassium's reactivity and its tendency to lose this electron to form positive ions.
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Valence Electrons of Transition Metals
Periodic Table Groups
The periodic table is organized into groups (columns) that share similar chemical properties. Elements in the same group have the same number of valence electrons, which influences their reactivity. Potassium is in group 1, indicating it has one valence electron, which is characteristic of alkali metals.
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Electron Orbitals
Electron orbitals are regions around the nucleus of an atom where electrons are likely to be found. The unpaired electron in potassium occupies the 4s orbital, as potassium has an electron configuration of [Ar] 4s¹. This orbital designation helps explain the element's chemical behavior and bonding characteristics.
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Related Practice
Textbook Question
An atom with a formal charge does not necessarily have more or less electron density than the atoms in the molecule without formal charges. We can see this by examining the potential maps for H2O, H3O+, and HO−.
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a. Which atom bears the formal negative charge in the hydroxide ion?
b. Which atom has the greater electron density in the hydroxide ion?
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Textbook Question
An atom with a formal charge does not necessarily have more or less electron density than the atoms in the molecule without formal charges. We can see this by examining the potential maps for H2O, H3O+, and HO−.
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c. Which atom bears the formal positive charge in the hydronium ion?
d. Which atom has the least electron density in the hydronium ion?
Textbook Question
Give each atom the appropriate formal charge:
a.
b.
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Textbook Question
Look at the relative positions of each pair of atoms listed here in the periodic table. How many core electrons does each have? How many valence electrons does each have?
a. carbon and silicon
b. oxygen and sulfur
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Textbook Question
How many valence electrons do chlorine, bromine, and iodine have?
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