Explain why metals cannot change to positive ions on its own?
Answers
Answered by
4
Answer:
The valence electrons of metals move freely in this way because metals have relatively low electronegativity, or attraction to electrons. The positive metal ions form a lattice-like structure held together by all the metallic bonds. ... When nonmetals bond together, the atoms share valence electrons and do not become ions.
Answered by
2
Answer:
A: Metal atoms readily give up valence electrons and become positive ions whenever they form bonds. When nonmetals bond together, the atoms share valence electrons and do not become ions. For example, when oxygen atoms bond together they form oxygen molecules in which two oxygen atoms share two pairs of valence electrons equally, so neither atom becomes charged.
Metallic Bonds and the Properties of Metals
The valence electrons surrounding metal ions are constantly moving. This makes metals good conductors of electricity. The lattice-like structure of metal ions is strong but quite flexible. This allows metals to bend without breaking. Metals are both ductile (can be shaped into wires) and malleable (can be shaped into thin sheets).
A: The iron ions can move within the “sea” of electrons around them. They can shift a little closer together or farther apart without breaking the metallic bonds between them. Therefore, the metal can bend rather than crack when the hammer hits it.
Metal worker shaping iron on an anvil
Summary
Metallic bonds are the force of attraction between positive metal ions and the valence electrons that are constantly moving around them. The ions form a lattice-like structure held together by the metallic bonds.
Metallic bonds explain why metals can conduct electricity and bend without breaking.
Review
What are metallic bonds?
How do metallic bonds relate to the properties of metals?
The iron in the metal working picture above (Figure above) is red hot. Infer why the metalworker heats the iron when he shapes it.
Explanation:
please mark me as brainlist and follow me
Similar questions