Ch.10 - Molecular Shapes & Valence Bond TheoryWorksheetSee 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: Exercise 32. Without using Fig. 3‑4, predict the order of increasing electronegativity in each of the following groups of elements.a. Na, K, Rbb. S, Se, Clc. Si, Ge, Snd. Tl, S, GeExercise 34. Without

Problem

Exercise 32. Without using Fig. 3‑4, predict the order of increasing electronegativity in each of the following groups of elements.

a. Na, K, Rb

b. S, Se, Cl

c. Si, Ge, Sn

d. Tl, S, Ge

Exercise 34. Without using Fig. 3‑4, predict which bond in each of the following groups will be the most polar.

a. C—H, Si—H, Sn—H

b. Al—Br, Ga—Br, In—Br, Tl—Br

c. C—O or Si—O

d. O—F or O—Cl

Repeat Exercises 32 and 34, this time using the values for the electronegativities of the elements given in figure below. Are there differences in your answers?