Ch.9 - Bonding & Molecular StructureWorksheetSee 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
Sections
Chemical Bonds
Lattice Energy
Lattice Energy Application
Born Haber Cycle
Dipole Moment
Lewis Dot Structure
Octet Rule
Formal Charge
Resonance Structures
Additional Practice
Bond Energy

Solution: Why does the most proper Lewis structure of BeCl 2 contain two single Be-Cl bonds instead of two double Be=Cl bonds?a. The formal charges of the atoms would be maximized, rather than minimized as requ

Problem

Why does the most proper Lewis structure of BeCl 2 contain two single Be-Cl bonds instead of two double Be=Cl bonds?

a. The formal charges of the atoms would be maximized, rather than minimized as required by the formal charge rule, if BeCl 2 contained two double bonds

b. Neither Be nor Cl could satisfy the octet rule if BeCl 2 contained two double bonds

c. Be would be surrounded by more than eight electrons if BeCl 2 had two double bonds

d. The Cl atoms would be surrounded by more than eight electrons each if BeCl contained two double bonds 

e. The formal charges could not sum to zero if BeCl 2 contained two double bonds