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- https://chem.libretexts.org/Courses/Brevard_College/LNC_216_CHE/04%3A_Chemical_Bonds/4.15%3A_Metallic_BondingThe luster of a metal is due to its metallic bonds. (Credit: Courtesy of the US Mint; Source: Front: http://commons.wikimedia.org/wiki/File:2005_AEPlat_Proof_Obv.png(opens in new window); Back:...The luster of a metal is due to its metallic bonds. (Credit: Courtesy of the US Mint; Source: Front: http://commons.wikimedia.org/wiki/File:2005_AEPlat_Proof_Obv.png(opens in new window); Back: http://commons.wikimedia.org/wiki/File:American_Platinum_Eagle_2008_Proof_Rev.jpg(opens in new window); License: Public Domain)
- https://chem.libretexts.org/Bookshelves/General_Chemistry/General_Chemistry_Supplement_(Eames)/Solids/Intro_to_SolidsThere are also many solids that are on the border between covalent and ionic: they are made of metals and non-metals, but both covalent bonding and ionic bonding are important. The simplest model of m...There are also many solids that are on the border between covalent and ionic: they are made of metals and non-metals, but both covalent bonding and ionic bonding are important. The simplest model of metallic bonding is the "sea of electrons" model, which imagines that the atoms sit in a sea of valence electrons that are delocalized (spread out) over all the atoms.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Chemical_Bonding/Fundamentals_of_Chemical_Bonding/Metallic_BondingA strong metallic bond will be the result of more delocalized electrons, which causes the effective nuclear charge on electrons on the cation to increase, in effect making the size of the cation small...A strong metallic bond will be the result of more delocalized electrons, which causes the effective nuclear charge on electrons on the cation to increase, in effect making the size of the cation smaller. Metallic bonds are strong and require a great deal of energy to break, and therefore metals have high melting and boiling points. A metallic bonding theory must explain how so much bonding can occur with such few electrons (since metals are located on the left side of the periodic table and do
- https://chem.libretexts.org/Courses/Westminster_College/CHE_180_-_Inorganic_Chemistry/10%3A_Chapter_10_-_The_Transition_Metals/10.1%3A_Properties_of_Transition_Metals/Introduction_to_Transition_Metals_IIn chromium it can be shown that the 4s orbital energy is still below the 3d which suggests a configuration [Ar] 3d 4 4s 2 . However due to the effect of electronic repulsion between the outer electro...In chromium it can be shown that the 4s orbital energy is still below the 3d which suggests a configuration [Ar] 3d 4 4s 2 . However due to the effect of electronic repulsion between the outer electrons the actual configuration becomes [Ar]3d 5 4s 1 where all the electrons in the outer orbitals are unpaired.
- https://chem.libretexts.org/Courses/Northern_Alberta_Institute_of_Technology/CHEM1130_Principles_in_Chemistry_I/3%3A_Chemical_Bonding._Solubility/3.9%3A_Metallic_BondingConductivity: Since the electrons are free, if electrons from an outside source were pushed into a metal wire at one end, the electrons would be pushed into the the wire and come out at the other end ...Conductivity: Since the electrons are free, if electrons from an outside source were pushed into a metal wire at one end, the electrons would be pushed into the the wire and come out at the other end at the same rate (conductivity is the movement of charge). In insulators, the band gap between the valence band the the conduction band is so large that electrons cannot make the energy jump from the valence band to the conduction band.
- https://chem.libretexts.org/Courses/Tennessee_State_University/CHEM_4210%3A_Inorganic_Chem_II_(Siddiquee)/04%3A_d-Block_Metal_Chemistry/4.01%3A_Properties_of_Transition_Metals/4.1.04%3A_Introduction_to_Transition_Metals_IIn chromium it can be shown that the 4s orbital energy is still below the 3d which suggests a configuration [Ar] 3d 4 4s 2 . However due to the effect of electronic repulsion between the outer electro...In chromium it can be shown that the 4s orbital energy is still below the 3d which suggests a configuration [Ar] 3d 4 4s 2 . However due to the effect of electronic repulsion between the outer electrons the actual configuration becomes [Ar]3d 5 4s 1 where all the electrons in the outer orbitals are unpaired.
- https://chem.libretexts.org/Courses/Lafayette_College/CHEM_212_213%3A_Inorganic_Chemistry_(Nataro)/02%3A_Molecules/2.06%3A_The_Range_of_BondingFigure \PageIndex1: van Arkel-Ketelaar Triangle plots the difference in electronegativity (Δχ) and the average electronegativity in a bond (∑χ). the top region is where b...Figure \PageIndex1: van Arkel-Ketelaar Triangle plots the difference in electronegativity (Δχ) and the average electronegativity in a bond (∑χ). the top region is where bonds are mostly ionic, the lower left region is where bonding is metallic, and the lower right region is where the bonding is covalent.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/ChemPRIME_(Moore_et_al.)/22%3A_Metals/22.02%3A_Metallic_BondingElectrons can be fed into one end of a metal wire and removed from the other end without causing any obvious change in the physical and chemical properties of the metal. To account for this freedom of...Electrons can be fed into one end of a metal wire and removed from the other end without causing any obvious change in the physical and chemical properties of the metal. To account for this freedom of movement modern theories of metallic bonding assume that the valence electrons are completely delocalized; that is, they occupy molecular orbitals belonging to the metallic crystal as a whole. These delocalized electrons are often referred to as an electron gas or an electron sea.
- https://chem.libretexts.org/Courses/CSU_Fullerton/Chem_325%3A_Inorganic_Chemistry_(Cooley)/05%3A_d-Block_Metal_Chemistry-_General_Considerations/5.03%3A_Introduction_to_Transition_Metals_IIn chromium it can be shown that the 4s orbital energy is still below the 3d which suggests a configuration [Ar] 3d 4 4s 2 . However due to the effect of electronic repulsion between the outer electro...In chromium it can be shown that the 4s orbital energy is still below the 3d which suggests a configuration [Ar] 3d 4 4s 2 . However due to the effect of electronic repulsion between the outer electrons the actual configuration becomes [Ar]3d 5 4s 1 where all the electrons in the outer orbitals are unpaired.
- https://chem.libretexts.org/Courses/Prince_Georges_Community_College/CHEM_2000%3A_Chemistry_for_Engineers_(Sinex)/Unit_2%3A__Molecular_Structure/Chapter_4%3A_Chemical_Bonding/Chapter_4.8%3A_Metallic_BondingConductivity: Since the electrons are free, if electrons from an outside source were pushed into a metal wire at one end, the electrons would be pushed into the the wire and come out at the other end ...Conductivity: Since the electrons are free, if electrons from an outside source were pushed into a metal wire at one end, the electrons would be pushed into the the wire and come out at the other end at the same rate (conductivity is the movement of charge). In insulators, the band gap between the valence band the the conduction band is so large that electrons cannot make the energy jump from the valence band to the conduction band.
- https://chem.libretexts.org/Courses/University_of_California_Davis/Chem_4B%3A_General_Chemistry_for_Majors_II_(Larsen)/Chem_4B_Textbook/Unit_II%3A_Physical_Equilibria/III%3A_Solids_Liquids_and_Phase_Transitions/3.9%3A_Bonding_in_MetalsIn the 1900's, Paul Drüde came up with the "sea of electrons" metallic bonding theory by modeling metals as a mixture of atomic cores (atomic cores = positive nuclei + inner shell of electrons) and va...In the 1900's, Paul Drüde came up with the "sea of electrons" metallic bonding theory by modeling metals as a mixture of atomic cores (atomic cores = positive nuclei + inner shell of electrons) and valence electrons. Metallic bonds occur among metal atoms. Whereas ionic bonds join metals to non-metals, metallic bonding joins a bulk of metal atoms. A sheet of aluminum foil and a copper wire are both places where you can see metallic bonding in action.
