Ch.2 - Atoms & 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: Each of the following elements is capable of forming an ion in chemical reactions.By referring to the periodic table, predict the charge of the most stable ion of K.

Solution: Each of the following elements is capable of forming an ion in chemical reactions.By referring to the periodic table, predict the charge of the most stable ion of K.

Problem

Each of the following elements is capable of forming an ion in chemical reactions.

By referring to the periodic table, predict the charge of the most stable ion of K.

Solution

We have to determine the most stable ion of potassium (K).


We can start solving this problem by writing the electron configuration of potassium and the noble gas closest to it. We will write the electron configuration of K and Ar.


 


• In a neutral atom:

Atomic number= # of protons = # of electrons

K: atomic number = 19 → 19 protons & 19 electrons

Ar: atomic number = 18 → 18 protons & 18 electrons

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