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- https://chem.libretexts.org/Courses/Los_Angeles_Trade_Technical_College/Hybrid_Chem_51_v1/10%3A_Chemical_Bonds/9.3_Covalent_BondsCovalent bonds are formed when atoms share electrons. Lewis electron dot diagrams can be drawn to illustrate covalent bond formation. Double bonds or triple bonds between atoms may be necessary to pro...Covalent bonds are formed when atoms share electrons. Lewis electron dot diagrams can be drawn to illustrate covalent bond formation. Double bonds or triple bonds between atoms may be necessary to properly illustrate the bonding in some molecules.
- https://chem.libretexts.org/Courses/Los_Angeles_Trade_Technical_College/LATTC_Hybrid_Chem_51/09%3A_Chemical_Bonds/9.3%3A_Covalent_BondsCovalent bonds are formed when atoms share electrons. Lewis electron dot diagrams can be drawn to illustrate covalent bond formation. Double bonds or triple bonds between atoms may be necessary to pro...Covalent bonds are formed when atoms share electrons. Lewis electron dot diagrams can be drawn to illustrate covalent bond formation. Double bonds or triple bonds between atoms may be necessary to properly illustrate the bonding in some molecules.
- https://chem.libretexts.org/Courses/Los_Angeles_Trade_Technical_College/DMA_Chem_51/2%3A_Beginning_Chemistry_(Ball)/09%3A_Chemical_Bonds/9.4%3A_Covalent_BondsCovalent bonds are formed when atoms share electrons. Lewis electron dot diagrams can be drawn to illustrate covalent bond formation. Double bonds or triple bonds between atoms may be necessary to pro...Covalent bonds are formed when atoms share electrons. Lewis electron dot diagrams can be drawn to illustrate covalent bond formation. Double bonds or triple bonds between atoms may be necessary to properly illustrate the bonding in some molecules.
- https://chem.libretexts.org/Under_Construction/Purgatory/CHEM_2100%3A_General_Chemistry_I_(Mink)/06%3A_Electronic_Structure_and_Periodic_Properties/6.04%3A_Electronic_Structure_of_Atoms_(Electron_Configurations)The relative energy of the subshells determine the order in which atomic orbitals are filled. Electron configurations and orbital diagrams can be determined by applying the Pauli exclusion principle (...The relative energy of the subshells determine the order in which atomic orbitals are filled. Electron configurations and orbital diagrams can be determined by applying the Pauli exclusion principle (no two electrons can have the same set of four quantum numbers) and Hund’s rule (whenever possible, electrons retain unpaired spins in degenerate orbitals). Electrons in the outermost orbitals, called valence electrons, are responsible for most of the chemical behavior of elements.
- https://chem.libretexts.org/Courses/Widener_University/Chem_145%3A_General_Chemistry_I_(van_Bramer)/07%3A_Electronic_Structure_and_Periodic_Properties/7.04%3A_Electronic_Structure_of_Atoms_(Electron_Configurations)The relative energy of the subshells determine the order in which atomic orbitals are filled. Electron configurations and orbital diagrams can be determined by applying the Pauli exclusion principle (...The relative energy of the subshells determine the order in which atomic orbitals are filled. Electron configurations and orbital diagrams can be determined by applying the Pauli exclusion principle (no two electrons can have the same set of four quantum numbers) and Hund’s rule (whenever possible, electrons retain unpaired spins in degenerate orbitals). Electrons in the outermost orbitals, called valence electrons, are responsible for most of the chemical behavior of elements.
- https://chem.libretexts.org/Courses/Brevard_College/CHE_310%3A_Inorganic_Chemistry_(Biava)/03%3A_Electronic_Structure_and_Periodic_Properties/3.05%3A_Electronic_Structure_of_Atoms_(Electron_Configurations)The relative energy of the subshells determine the order in which atomic orbitals are filled. Electron configurations and orbital diagrams can be determined by applying the Pauli exclusion principle (...The relative energy of the subshells determine the order in which atomic orbitals are filled. Electron configurations and orbital diagrams can be determined by applying the Pauli exclusion principle (no two electrons can have the same set of four quantum numbers) and Hund’s rule (whenever possible, electrons retain unpaired spins in degenerate orbitals). Electrons in the outermost orbitals, called valence electrons, are responsible for most of the chemical behavior of elements.
- https://chem.libretexts.org/Courses/Oregon_Institute_of_Technology/OIT%3A_CHE_202_-_General_Chemistry_II/Unit_3%3A_Periodic_Patterns/3.1%3A_Electron_ConfigurationsFor example, iron (1s 2 2s 2 2p 6 3s 2 3p 6 3d 6 4s 2 ) forms the ion Fe 2+ (1s 2 2s 2 2p 6 3s 2 3p 6 3d 6 ) by the loss of the 4s electrons and the ion Fe 3+ (1s 2 2s 2 2p 6 3s 2 3p 6 3d 5 ) by the l...For example, iron (1s 2 2s 2 2p 6 3s 2 3p 6 3d 6 4s 2 ) forms the ion Fe 2+ (1s 2 2s 2 2p 6 3s 2 3p 6 3d 6 ) by the loss of the 4s electrons and the ion Fe 3+ (1s 2 2s 2 2p 6 3s 2 3p 6 3d 5 ) by the loss of the 4s electrons and one of the 3d electrons.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Book%3A_Introductory_Chemistry_Online_(Young)/03%3A_Chemical_Bonding_and_Nomenclature/3.S%3A_Chemical_Bonding_and_Nomenclature_(Summary)When naming simple, binary ionic compounds, the cation is named first using the name of the element, followed by the anion, where the suffix ide is added to the root name of the element. For transitio...When naming simple, binary ionic compounds, the cation is named first using the name of the element, followed by the anion, where the suffix ide is added to the root name of the element. For transition metals in which the metal can assume a variety of oxidation states (different positive charges), the charge of the metal ion is shown in the name using Roman numerals, in parenthesis, following the name of the element (i.e., iron (III) chloride).
- https://chem.libretexts.org/Courses/Los_Angeles_Trade_Technical_College/DMA_Chem_51_Su_19/2%3A_Beginning_Chemistry_(Ball)/09%3A_Chemical_Bonds/9.4%3A_Covalent_BondsCovalent bonds are formed when atoms share electrons. Lewis electron dot diagrams can be drawn to illustrate covalent bond formation. Double bonds or triple bonds between atoms may be necessary to pro...Covalent bonds are formed when atoms share electrons. Lewis electron dot diagrams can be drawn to illustrate covalent bond formation. Double bonds or triple bonds between atoms may be necessary to properly illustrate the bonding in some molecules.
- https://chem.libretexts.org/Courses/BridgeValley_Community_and_Technical_College/Consumer_Chemistry/07%3A_Chemical_Bonds/7.05%3A_Covalent_BondsCovalent bonds are formed when atoms share electrons. Lewis electron dot diagrams can be drawn to illustrate covalent bond formation. Double bonds or triple bonds between atoms may be necessary to pro...Covalent bonds are formed when atoms share electrons. Lewis electron dot diagrams can be drawn to illustrate covalent bond formation. Double bonds or triple bonds between atoms may be necessary to properly illustrate the bonding in some molecules.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/Concept_Development_Studies_in_Chemistry_(Hutchinson)/04_The_Structure_of_an_AtomWe assume that most of the common elements have been identified, and that each element is characterized as consisting of identical, indestructible atoms. We also assume that the atomic weights of the ...We assume that most of the common elements have been identified, and that each element is characterized as consisting of identical, indestructible atoms. We also assume that the atomic weights of the elements are all known, and that, as a consequence, it is possible via mass composition measurements to determine the molecular formula for any compound of interest.
