Ch.8 - Periodic Properties of the ElementsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: You may want to reference (Pages 268 - 272) Section 7.4 while completing this problem.Use electron configurations to explain the following observations:(a) The first ionization energy of phosphorus is

Problem

You may want to reference (Pages 268 - 272) Section 7.4 while completing this problem.

Use electron configurations to explain the following observations:
(a) The first ionization energy of phosphorus is greater than that of sulfur.
(b) The electron affinity of nitrogen is lower (less negative) than those of both carbon and oxygen.
(c) The second ionization energy of oxygen is greater than the first ionization energy of fluorine.
(d) The third ionization energy of manganese is greater than those of both chromium and iron.