Chemical Bonding in Hypervalent Molecules:  Is the Octet Rule Relevant?

2002 ◽  
Vol 41 (8) ◽  
pp. 2164-2172 ◽  
Author(s):  
Stéphane Noury ◽  
Bernard Silvi ◽  
Ronald J. Gillespie
Keyword(s):  
Chemical Bonding ◽  
Hypervalent Molecules ◽  
Octet Rule

Chemical Bonding 1: Basic Concepts

2021 ◽  
pp. 81-101
Author(s):  
Christopher O. Oriakhi
Keyword(s):  
Chemical Bonding ◽  
Chemical Properties ◽  
Lattice Energy ◽  
Bond Polarity ◽  
Formal Charge ◽  
Basic Concepts ◽  
Lewis Structures ◽  
The Relationship ◽  
Octet Rule

Chemical Bonding I: Basic Concepts examines general ideas of chemical bonding between atoms and ions and how this bonding affects the chemical properties of the elements. An overview of Lewis symbols, Lewis structures and the octet rule is presented including the role of valence electrons in ionic and covalent bonding. The energy changes that accompany ionic bond formation are also discussed with emphasis on lattice energy. The chapter covers guidelines and general procedures for writing Lewis structures or electron dot formulas for molecular compounds and polyatomic ions. The concepts and applications of resonance, formal charge and exceptions to the octet rules are presented, along with coverage of the relationship between bond polarity and electronegativity.

scholarly journals The challenges of learning and teaching chemical bonding at different school levels using electrostatic interactions instead of the octet rule as a teaching model

2018 ◽  
Vol 19 (3) ◽  
pp. 932-953 ◽  
Author(s):  
Jarkko Joki ◽  
Maija Aksela
Keyword(s):  
Secondary School ◽  
Chemical Bonding ◽  
Electrostatic Interactions ◽  
Secondary Level ◽  
Teaching Model ◽  
Electrostatic Model ◽  
Upper Secondary School ◽  
Learning And Teaching ◽  
Upper Secondary ◽  
Octet Rule

Teaching chemical bonding using the octet rule as an explanatory principle is problematic in many ways. The aim of this case study is to understand the learning and teaching of chemical bonding using a research-informed teaching model in which chemical bonding is introduced as an electrostatic phenomenon. The study posed two main questions: (i) how does a student's understanding of chemical bonding evolve from lower- to upper-secondary school when an electrostatic model of chemical bonding was used at the lower-secondary level? (ii) How does the teaching of octets/full shells at the upper-secondary level affect students’ understanding? The same students were interviewed after lower-secondary school and again during their first year at upper-secondary school. Their upper-level chemistry teachers were also interviewed. The interview data were analysed using the grounded theory method. The findings showed that the students’ earlier proper understanding of the electrostatic-interactions model at the lower-secondary level did not prevent the later development of less-canonical thinking. Teachers’ pedagogical content knowledge (PCK) of the explanatory principles of chemical bonding and how to use explanations in science education needs to be promoted in both pre-service teacher education and during in-service training.

Chemical bonding in cuprous complexes with simple nitriles: octet rule and resonance concepts versus quantitative charge-redistribution analysis

2020 ◽  
Vol 22 (36) ◽  
pp. 20238-20247
Author(s):  
Simone Potenti ◽  
Lorenzo Paoloni ◽  
Surajit Nandi ◽  
Marco Fusè ◽  
Vincenzo Barone ◽  
...  
Keyword(s):  
Quantitative Analysis ◽  
Chemical Bonding ◽  
Charge Redistribution ◽  
Resonance Structures ◽  
Octet Rule

Resonance structures for six cuprous complexes with simple nitriles are interpreted by means of a quantitative analysis of charge redistribution upon copper-nitrile bonding.

Localized-orbital locator (LOL) profiles of chemical bonding

2008 ◽  
Vol 86 (7) ◽  
pp. 695-702 ◽  
Author(s):  
Heiko Jacobsen
Keyword(s):  
Energy Density ◽  
Kinetic Energy ◽  
Transition Metal Complexes ◽  
Chemical Bonding ◽  
Electron Pair ◽  
Kinetic Energy Density ◽  
Triple Bonds ◽  
Core Electrons ◽  
Localized Orbital ◽  
Hypervalent Molecules

We examine a recently introduced descriptor of chemical bonding, the localized-orbital locator (LOL), which is based on the kinetic-energy density (τ). Examples are presented for prototypical chemical bonds, such as single, double, and triple bonds, for bonding in transition metal complexes, for three-center two-electron bonds, as well as for hypervalent molecules. The topology of LOL is analyzed in terms of (3,–3) attractors (Γ). The influence of core electrons for chemical bonding is investigated, and a LOL-VSEPR (valence shell electron pair repulstion) relationship is established. Further, we compare LOL to the related electron localization function (ELF).Key words: chemical bonding, kinetic-energy density, localized-electron locator, VSEPR theory.

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