Metallic behavior is generally associated with
B) the second valence electron is removed. C) the eighth electron of is removed. D) the first core electron is removed. E) the last valence electron is removed. Metallic behavior is generally associated with A) elements with very negative electron affinities.B) elements with low ionization energies. C) elements with small atomic radii. D) elements with unpaired electrons.E) elements with partially filled p orbitals.) the second valence electron is removed. C) the eighth electron of is removed. D) the first core electron is removed. E) the last valence electron is removed. Metallic behavior is generally associated with A) elements with very negative electron affinities. Metallic character decreases as you move across a period in the periodic table from left to right.This occurs as atoms more readily accept electrons to fill a valence shell than lose them to remove the unfilled shell. Metallic character increases as you move down an element group in the periodic table.This is because electrons become easier to lose as the atomic radius increases, where there is less attraction between the nucleus and the valence electrons because of the increased distance between them.hare. There are trends in metallic character as you move across and down the periodic table. Metallic character decreases as you move across a period in the periodic table from left to right. This occurs as atoms more readily accept electrons to fill a valence shell than lose them to remove the unfilled shell. Share. There are trends in metallic character as you move across and down the periodic table. Metallic character decreases as you move across a period in the periodic table from left to right. This occurs as atoms more readily accept electrons to fill a valence shell than lose them to remove the unfilled shell.Metallic character increases as you move down an element group in the periodic table.This is because electrons become easier to lose as the atomic radius increases, where there is less attraction between the nucleus and the valence electrons because of the increased distance between them.hare. There are trends in metallic character as you move across and down the periodic table. Metallic character decreases as you move across a period in the periodic table from left to right. This occurs as atoms more readily accept electrons to fill a valence shell than lose them to remove the unfilled shell. 1 A metal is a lattice of positive metal 'ions' in a 'sea' of delocalised electrons. 2  Metallic bonding refers to the interaction between the delocalised electrons and the metal nuclei. 3  The physical properties of metals are the result of the delocalisation of the electrons involved in metallic bonding. The physical properties of solid metals are: 2  conduct heat. 3  conduct electricity. 4  generally high melting and boiling points. 5  strong. 6  malleable (can be hammered or pressed out of shape without breaking). 7  ductile (able to be drawn into a wire). 8  metallic lustre. 9  opaque (reflect light). 3. covalent but partially ionic. Metallic Bonds and Metallic Solids Metal atoms interact with other metal atoms to form metallic bonds, the bond type foundin pure metals, alloys, and certain intermetallic compounds. The metal cations from a lattice andthe valence electrons form a surrounding ˝sea ˛ or ˝gas.. covalent but partially ionic. Metallic Bonds and Metallic Solids Metal atoms interact with other metal atoms to form metallic bonds, the bond type foundin pure metals, alloys, and certain intermetallic compounds. The metal cations from a lattice andthe valence electrons form a surrounding ˝sea ˛ or ˝gas. Metallic bonding is not the only type of chemical bonding a metal can exhibit, even as a pure substance. For example, elemental gallium consists of covalently-bound pairs of atoms in both liquid and solid state—these pairs form a crystal lattice with metallic bonding between them.Nonmolecular' would perhaps be a better term. Metallic bonding is mostly non-polar, because even in alloys there is little difference among the electronegativities of the atoms participating in the bonding interaction (and, in pure elemental metals, none at all). More than 80 elements in the periodic table are metals. Metals are solids at ordinary temperature and pressure, with the exception (of mercury and gallium). Metals have characteristic properties such as: 1  High thermal and electrical conductivity.2  Luster and high reflectivity. 3  Malleability and ductility.ore than 80 elements in the periodic table are metals. Metals are solids at ordinary temperature and pressure, with the exception (of mercury and gallium). Metals have characteristic properties such as: 1  High thermal and electrical conductivity. 2  Luster and high reflectivity. 3  Malleability and ductility. About 91 of the 118 elements in the periodic table are metals (some elements appear in both metallic and non-metallic forms). Astrophysicists use the term metal to collectively describe all elements other than hydrogen and helium.hen a metal ore is an ionic compound of that metal and a non-metal, the ore must usually be smelted — heated with a reducing agent — to extract the pure metal. Many common metals, such as iron, are smelted using carbon as a reducing agent. The strength of the metallic bond depends on the. 1  number of electrons in the delocalised 'sea' of electrons. ( 2 More delocalised electrons results in a stronger bond and a higher melting point.). 3  packing arrangement of the metal atoms. The physical properties of solid metals are: 2  conduct heat. 3  conduct electricity. 4  generally high melting and boiling points. 5  strong. 6  malleable (can be hammered or pressed out of shape without breaking). 7  ductile (able to be drawn into a wire). 8  metallic lustre. 9  opaque (reflect light). 1 Metallic bonding refers to the interaction between the delocalised electrons and the metal nuclei. 2  The physical properties of metals are the result of the delocalisation of the electrons involved in metallic bonding. The physical properties of solid metals are: 2  conduct heat. 3  conduct electricity. 4  generally high melting and boiling points. 5  strong. 6  malleable (can be hammered or pressed out of shape without breaking). 7  ductile (able to be drawn into a wire). 8  metallic lustre. 9  opaque (reflect light).
A) Elements with very negative electron affinities.
B) Elements with low ionization energies. 
C) Elements with small atomic radii. 
D) Elements with unpaired electrons.
E) Elements with partially filled.