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: Does the electron configuration [Ar]4s23d54p1 correspond to an excited state? Identify the atom and write the ground-state electron configuration if appropriate. How many unpaired electrons are presen

Solution: Does the electron configuration [Ar]4s23d54p1 correspond to an excited state? Identify the atom and write the ground-state electron configuration if appropriate. How many unpaired electrons are presen

Problem

Does the electron configuration [Ar]4s23d54p1 correspond to an excited state? Identify the atom and write the ground-state electron configuration if appropriate. How many unpaired electrons are present in this species?

Solution

1. The electron configuration of an element is the distribution of its electrons within atomic orbitals.

According to Auf Bau Principle, electrons fill in lower energy orbitals before moving to higher energy orbitals. The orbital subshells s, p, d, and f, each have a maximum number of electrons it can accommodate and are filled up according to the Auf Bau Diagram.

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