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: How does the atomic radius of Ca compare with that of K?(a) Ca is larger because it has more electrons(b) Ca is larger because its effective nuclear charge is greater(c) K is larger because it has fewer electrons(d) K is larger because its effective nuclear charge is less(e) Ca and K are essentially the same size

Problem

How does the atomic radius of Ca compare with that of K?

(a) Ca is larger because it has more electrons

(b) Ca is larger because its effective nuclear charge is greater

(c) K is larger because it has fewer electrons

(d) K is larger because its effective nuclear charge is less

(e) Ca and K are essentially the same size

Solution

Establish the trend for atomic radius and determine which among K and Ca has a larger atomic radius 

Atomic radius represents the distance from the nucleus to the outer shell of an element. 

Trend of atomic radius in the periodic table:

decreases going from left to right of a period

increases going down a group

Solution BlurView Complete Written Solution