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: Group 4A elements have much more negative electron affinities than their neighbors in groups 3A and 5A (see the figure).Which of the following statements best explains this observation?(i) The group 4

Problem

Group 4A elements have much more negative electron affinities than their neighbors in groups 3A and 5A (see the figure).
A section of the periodic table shows electron affinities for select groups.
Which of the following statements best explains this observation?
(i) The group 4A elements have much higher first ionization energies than their neighbors in groups 3A and 5A.
(ii) The addition of an electron to a group 4A element leads to a half-filled np3 outer electron configuration.
(iii) The group 4A elements have unusually large atomic radii.
(iv) The group 4A elements are easier to vaporize than are the group 3A and 5A elements.