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 260 - 262) Section 7.2 while completing this problem.Which of the following statements about effective nuclear charge for the outermost valence electron of an atom is

Problem

You may want to reference (Pages 260 - 262) Section 7.2 while completing this problem.

Which of the following statements about effective nuclear charge for the outermost valence electron of an atom is incorrect?
(i) The effective nuclear charge can be thought of as the true nuclear charge minus a screening constant due to the other electrons in the atom.
(ii) Effective nuclear charge increases going left to right across a row of the periodic table.
(iii) Valence electrons screen the nuclear charge more effectively than do core electrons.
(iv) The effective nuclear charge shows a sudden decrease when we go from the end of one row to the beginning of the next row of the periodic table.
(v) The change in effective nuclear charge going down a column of the periodic table is generally less than that going across a row of the periodic table.