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: For an isoelectronic series of ions, the ion that is the smallest is always 1. the ion with the fewest protons. 2. the least positively (or most negatively) charged ion. 3. the ion with the highest atomic number. 4. the ion with the most neutrons. 5. the ion with the most electrons.

Solution: For an isoelectronic series of ions, the ion that is the smallest is always 1. the ion with the fewest protons. 2. the least positively (or most negatively) charged ion. 3. the ion with the highest

Problem

For an isoelectronic series of ions, the ion that is the smallest is always

1. the ion with the fewest protons.

2. the least positively (or most negatively) charged ion.

3. the ion with the highest atomic number.

4. the ion with the most neutrons.

5. the ion with the most electrons.