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- https://chem.libretexts.org/Courses/BridgeValley_Community_and_Technical_College/Fundamentals_of_Chemistry/06%3A_Molecules_and_Compounds/6.06%3A_Electron_Transfer_-_Ionic_BondsThe tendency to form species that have eight electrons in the valence shell is called the octet rule. The attraction of oppositely charged ions caused by electron transfer is called an ionic bond. The...The tendency to form species that have eight electrons in the valence shell is called the octet rule. The attraction of oppositely charged ions caused by electron transfer is called an ionic bond. The strength of ionic bonding depends on the magnitude of the charges and the sizes of the ions.
- https://chem.libretexts.org/Courses/Westfield_State_University/Chem0103_Chemistry_of_the_Life_Sciences_(Theis)/01%3A_Atoms_and_compounds/1.06%3A_Extras/1.6.04%3A_Basic_Concepts_of_Chemical_Bonding_(GenChem_Brown)/1.6.4.01%3A_Chemical_Bonds_Lewis_Symbols_and_the_Octet_RuleLewis dot symbols can be used to predict the number of bonds formed by most elements in their compounds. Lewis electron dot symbols, which consist of the chemical symbol for an element surrounded by d...Lewis dot symbols can be used to predict the number of bonds formed by most elements in their compounds. Lewis electron dot symbols, which consist of the chemical symbol for an element surrounded by dots that represent its valence electrons, grouped into pairs often placed above, below, and to the left and right of the symbol. The structures reflect the fact that the elements in period 2 and beyond tend to gain, lose, or share electrons to reach a total of 8 valence electrons in their compounds.
- https://chem.libretexts.org/Courses/Los_Angeles_Trade_Technical_College/Foundations_of_Introductory_Chemistry-1/1.10%3A_Chemical_Bonds/12.5%3A_Electron_Transfer_-_Ionic_BondsThe tendency to form species that have eight electrons in the valence shell is called the octet rule. The attraction of oppositely charged ions caused by electron transfer is called an ionic bond. The...The tendency to form species that have eight electrons in the valence shell is called the octet rule. The attraction of oppositely charged ions caused by electron transfer is called an ionic bond. The strength of ionic bonding depends on the magnitude of the charges and the sizes of the ions.
- https://chem.libretexts.org/Courses/GalwayMayo_Institute_of_Technology/Spectroscopy%3A_Background_Information_on_Electronic_Structure_of_Atoms_and_Molecules/02%3A_Chapter_2_-_Basics_of_Chemical_Bonding/2.01%3A_Basic_Concepts_of_Chemical_Bonding/2.1.07%3A_Exceptions_to_the_Octet_RuleFollowing the Octet Rule for Lewis Dot Structures leads to the most accurate depictions of stable molecular and atomic structures and because of this we always want to use the octet rule when drawing ...Following the Octet Rule for Lewis Dot Structures leads to the most accurate depictions of stable molecular and atomic structures and because of this we always want to use the octet rule when drawing Lewis Dot Structures. There are three exceptions: (1) When there are an odd number of valence electrons, (2) When there are too few valence electrons, and (3) when there are too many valence electrons
- https://chem.libretexts.org/Courses/Nassau_Community_College/General_Chemistry_1/04%3A_Chemical_Bonding_and_Molecular_Geometry/4.04%3A_Lewis_Symbols_and_StructuresValence electronic structures can be visualized by drawing Lewis symbols (for atoms and monatomic ions) and Lewis structures (for molecules and polyatomic ions). Lone pairs, unpaired electrons, and si...Valence electronic structures can be visualized by drawing Lewis symbols (for atoms and monatomic ions) and Lewis structures (for molecules and polyatomic ions). Lone pairs, unpaired electrons, and single, double, or triple bonds are used to indicate where the valence electrons are located around each atom in a Lewis structure. Most structures—especially those containing second row elements—obey the octet rule, in which every atom (except H) is surrounded by eight electrons.
- https://chem.libretexts.org/Courses/Nassau_Community_College/Principles_of_Chemistry/07%3A_Chemical_Bonds/7.03%3A_Electron_Transfer_-_Ionic_BondsThe tendency to form species that have eight electrons in the valence shell is called the octet rule. The attraction of oppositely charged ions caused by electron transfer is called an ionic bond. The...The tendency to form species that have eight electrons in the valence shell is called the octet rule. The attraction of oppositely charged ions caused by electron transfer is called an ionic bond. The strength of ionic bonding depends on the magnitude of the charges and the sizes of the ions.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/ChemPRIME_(Moore_et_al.)/06%3A_Chemical_Bonding_-_Electron_Pairs_and_Octets/6.01%3A_Prelude_to_Chemical_BondingTheories of chemical bonding invariably involve electrons. When one atom approaches another, the valence electrons, found in the outermost regions of the atoms, interact long before the nuclei can com...Theories of chemical bonding invariably involve electrons. When one atom approaches another, the valence electrons, found in the outermost regions of the atoms, interact long before the nuclei can come close together. Electrons are the least massive components of an atom, and so they can relocate to produce electrostatic forces which hold atoms together.
- 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/Courses/Westfield_State_University/Chem0103_Chemistry_of_the_Life_Sciences_(Theis)/01%3A_Atoms_and_compounds/1.06%3A_Extras/1.6.04%3A_Basic_Concepts_of_Chemical_Bonding_(GenChem_Brown)/1.5.4.07%3A_Exceptions_to_the_Octet_RuleFollowing the Octet Rule for Lewis Dot Structures leads to the most accurate depictions of stable molecular and atomic structures and because of this we always want to use the octet rule when drawing ...Following the Octet Rule for Lewis Dot Structures leads to the most accurate depictions of stable molecular and atomic structures and because of this we always want to use the octet rule when drawing Lewis Dot Structures. There are three exceptions: (1) When there are an odd number of valence electrons, (2) When there are too few valence electrons, and (3) when there are too many valence electrons
- https://chem.libretexts.org/Courses/Williams_School/Chemistry_I/06%3A_Chemical_Bonding_and_Molecular_Geometry/6.04%3A_Lewis_Symbols_and_StructuresValence electronic structures can be visualized by drawing Lewis symbols (for atoms and monatomic ions) and Lewis structures (for molecules and polyatomic ions). Lone pairs, unpaired electrons, and si...Valence electronic structures can be visualized by drawing Lewis symbols (for atoms and monatomic ions) and Lewis structures (for molecules and polyatomic ions). Lone pairs, unpaired electrons, and single, double, or triple bonds are used to indicate where the valence electrons are located around each atom in a Lewis structure. Most structures—especially those containing second row elements—obey the octet rule, in which every atom (except H) is surrounded by eight electrons.
- https://chem.libretexts.org/Workbench/OpenStax_Chemistry_Remixed%3A_Clovis_Community_College/08%3A_Chemical_Bonding_and_Molecular_Geometry/8.04%3A_Lewis_Symbols_and_StructuresValence electronic structures can be visualized by drawing Lewis symbols (for atoms and monatomic ions) and Lewis structures (for molecules and polyatomic ions). Lone pairs, unpaired electrons, and si...Valence electronic structures can be visualized by drawing Lewis symbols (for atoms and monatomic ions) and Lewis structures (for molecules and polyatomic ions). Lone pairs, unpaired electrons, and single, double, or triple bonds are used to indicate where the valence electrons are located around each atom in a Lewis structure. Most structures—especially those containing second row elements—obey the octet rule, in which every atom (except H) is surrounded by eight electrons.
