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- https://chem.libretexts.org/Courses/Duke_University/CHEM_210D%3A_Modern_Applications_of_Chemistry/3%3A_Textbook-_Modern_Applications_of_Chemistry/01%3A_Primer/1.02%3A_Chemical_Bonding_-_Electron_Pairs_and_Octets/1.2.10%3A_The_Octet_RuleA convenient method for doing this is to regard the compound as being formed from its atoms and to use Lewis diagrams. The octet rule can then be applied. Each atom must lose or gain electrons in orde...A convenient method for doing this is to regard the compound as being formed from its atoms and to use Lewis diagrams. The octet rule can then be applied. Each atom must lose or gain electrons in order to achieve an octet. Furthermore, all electrons lost by one kind of atom must be gained by the other.
- https://chem.libretexts.org/Bookshelves/Inorganic_Chemistry/Supplemental_Modules_and_Websites_(Inorganic_Chemistry)/Molecular_Geometry/Trigonal_Planar_______Molecular_GeometryAX 3 Shape: trigonal planar Steric Number: Lone Pairs: Polar/NonPolar: NonPolar Hybridization: sp 2 Examples: BF 3 , CO 3 2 - NOTES: This molecule is made up of 3 equally spaced sp 2 hybrid orbitals a...AX 3 Shape: trigonal planar Steric Number: Lone Pairs: Polar/NonPolar: NonPolar Hybridization: sp 2 Examples: BF 3 , CO 3 2 - NOTES: This molecule is made up of 3 equally spaced sp 2 hybrid orbitals arranged at 120 o angles. The shape of the orbitals is planar triangular. Since there is an atom at the end of each orbital, the shape of the molecule is also planar triangular. Contributors and Attributions Charles Ophardt, Professor Emeritus, Elmhurst College; Virtual Chembook
- https://chem.libretexts.org/Courses/University_of_North_Texas/UNT%3A_CHEM_1410_-_General_Chemistry_for_Science_Majors_I/Text/06%3A_Chemical_Bonding_-_Electron_Pairs_and_Octets/6.10%3A_The_Octet_RuleA convenient method for doing this is to regard the compound as being formed from its atoms and to use Lewis diagrams. The octet rule can then be applied. Each atom must lose or gain electrons in orde...A convenient method for doing this is to regard the compound as being formed from its atoms and to use Lewis diagrams. The octet rule can then be applied. Each atom must lose or gain electrons in order to achieve an octet. Furthermore, all electrons lost by one kind of atom must be gained by the other.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/ChemPRIME_(Moore_et_al.)/06%3A_Chemical_Bonding_-_Electron_Pairs_and_Octets/6.10%3A_The_Octet_RuleA convenient method for doing this is to regard the compound as being formed from its atoms and to use Lewis diagrams. The octet rule can then be applied. Each atom must lose or gain electrons in orde...A convenient method for doing this is to regard the compound as being formed from its atoms and to use Lewis diagrams. The octet rule can then be applied. Each atom must lose or gain electrons in order to achieve an octet. Furthermore, all electrons lost by one kind of atom must be gained by the other.
- https://chem.libretexts.org/Bookshelves/Inorganic_Chemistry/Supplemental_Modules_and_Websites_(Inorganic_Chemistry)/Molecular_Geometry/Bent_Molecular_GeometryThe molecule that is made up of 4 equally spaced sp3 hybrid orbitals forming bond angles of approximately 109.5o. The shape of the orbitals is tetrahedral. Two of the orbitals contain lone pairs of el...The molecule that is made up of 4 equally spaced sp3 hybrid orbitals forming bond angles of approximately 109.5o. The shape of the orbitals is tetrahedral. Two of the orbitals contain lone pairs of electrons. The two atoms connected to the central atom form a molecule with a bent shape.
- https://chem.libretexts.org/Bookshelves/Environmental_Chemistry/Green_Chemistry_and_the_Ten_Commandments_of_Sustainability_(Manahan)/03%3A_The_Elements_-_Basic_Building_Blocks_of_Green_Chemicals/3.06%3A_The_Magic_Octet_of_8_Outer-Shell_ElectronsThis means that a lot of the electrons will have to be shared to form a bond between the N atoms in the N2 molecule, and, in fact, 6 of the 10 outer-shell electrons available in two N atoms are shared...This means that a lot of the electrons will have to be shared to form a bond between the N atoms in the N2 molecule, and, in fact, 6 of the 10 outer-shell electrons available in two N atoms are shared between the N atoms to give a triple bond consisting of 3 pairs of shared electrons as shown by the 3 pairs of dots between the 2 N atoms in the molecule of N2 in Figure 3.6.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/08%3A_Ionic_and_Metallic_Bonding/8.04%3A_Anion_FormationThis page discusses the dangers of chlorine gas and its reaction with sodium to form safe sodium chloride. It explains the formation of anions, negatively charged ions that achieve stability by gainin...This page discusses the dangers of chlorine gas and its reaction with sodium to form safe sodium chloride. It explains the formation of anions, negatively charged ions that achieve stability by gaining electrons. The concept of isoelectronic species, where different ions have the same electron configuration, is highlighted to illustrate the differences between ions like sodium and neon. The summary emphasizes the importance of anions in ion formation.
