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What exists between a metal and a nonmetal?
Valence electrons
Do all nonmetals have a completelyfull Valence shell of electrons?
There is no set amount of valence electrons for nonmetals. The amount of valence electrons a nonmetal has is determined by the number of electrons on the outer shell of the atom.
How many valence electrons are in a stable nonmetal ion?
8
How many valence electrons would be common for an atoms of a nonmetal?
chocolate
Are electrons are used in bonding are called valence or ionic?
They are called valence electrons. Ionic is a bond between a nonmetal and a metal. A covalent bond(molecular bond) is between two or more non metals.
How is the number of valence electrons of a nonmetal related to the charge on the ion the nonmetal?
Nonmetals will undergo chemical reactions that result in a stable electron configuration of 8 electrons in the outer shell. The number of valence electrons tells you have many they have in their outer shell prior to any chemical reaction, and therefore, how many more electrons they need to get a complete set of 8. So for example, oxygen has 6 valence electrons and therefore needs 2 more to have 8, so it will form an ion with a charge of minus two, which is the charge that is carried by the additional two electrons that oxygen will acquire. Chlorine has 7 valence electrons, therefore it needs just one more electron to complete its outer shell, and as an ion will have a charge of minus one. Nitrogen has 5 valence electrons, so it needs 3 more, and will form an ion with a charge of minus three.
What is the deference between ionic bonds and covalent bonds?
covalent bonds: relatively low melting point, bond is not as strong as ionic, form between two nonmetals, valence electrons are shared between the atoms. ionic: relatively high melting point, stronger bond than covalent, form between a metal and nonmetal, valence electrons are transferred from the metal to the nonmetal, leaving the metal with a positive charge and the nonmetal with a negative charge. these charged particles are called ions. positive ion=cation, negative ion=anion.
Why are the valance electrons of metallic bonds different from other bonds?
In a metal the valence electrons delocalize into the conduction band, becoming an "electron gas" that fills the metal's bulk volume.In covalent bonds the valence electrons are shared between local pairs of atoms.In ionic bonds the valence electrons leave the "metal" and move to the "nonmetal" creating a pair of separate oppositely charged ions.In resonance bonds the valence electrons oscillate between being shared between two nearby local pairs of atoms.etc.To summarize in metals the valence electrons become delocalized, in other bonds the valence electrons stay local.
What happens to the valence electrons in a covalent bond?
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What happens to the valence electrons when new compounds are formed in covelant bonding?
valence electrons are shared in covalent bonding
What is the non metal in the third period with six outer electrons?
Oxygen is the only nonmetal with 6 Valence Electrons in period 2.
What happens to electrons after a chemical bond is formed?
If the starting point are elements then the inner shell electrons (non valence) these orbit the nuclei of the atoms and the formation of a chemical bond does not affect these materially. What happens to the valence electrons depends on the bond formed. In an ionic bond electrons are transferred from say the metal atom to the nonmetal- these electrons essentially "orbit" the nuclei of the cations and anions. They are "localised". When a covalent bond is formed the valence electrons involved are shared between the atoms, they "orbit" both nuclei. When the bond is polar covalent they spend a little more time nearer the more electronegative element. When a "delocalised"covalent bond is formed as in bezene or graphite the electrons orbit a number of atomic nuclei. In a metallic bond the valence electrons are also delocalised (the sea of electrons model) across the metal lattice, but in transition metals there is additional bonding between electrons in d orbitals (the tight bound electrons) and these electrons are essentially localised.
