Which statement correctly describes metallic bonds? a. they form when certain atoms lose electrons and other atoms gain electrons. b. they involve an attraction between anions and cations. they always involvpoth a metal and a nonmetal. d. they can only form between atoms of the same element. e. they form because electrons can move freely between atoms.

Answer is     The charge of the purple circles should be positive because they represent the nuclei.

Everyone ignore this answer it is for a different question.

D

Explanation:

the atom of the metal loses one electron which becomes delocalised and is attragted by the positive nucleus leading to formation of metallic bond.

The answer is C.Many atoms give up electrons that can move among the atoms.

   B) metal ions floating in a sea of electrons

Explanation:  Metallic bonding is type of bonding which are present in the metals . It is kind of electrostatic attraction between the electrons and the positively charged metal.

Thus Metallic bonding is the not the one in which the valence electrons are rigidly held neither the pattern in which the electrons are arranged in the regular repeating pattern nor the strong electromagnetic forces which are holding the electrons together in a place.

It is that chemical bonding which is present in metals and which hold the atoms together.

D.A nonmetal atom transfers electrons to a metal atom.

Explanation:

Metals are chemical elements that have as their main physical characteristic the ability to lose electrons and, consequently, form metal cations. For this reason, they can perform two types of chemical bonds: the ionic bond and the metallic bond.

The metal bond is established between atoms of a single metal element. This type of bonding occurs only between atoms of a single metal and exclusively because a metal cannot establish chemical bond with another different metallic element.

In the metal bond, the crystalline lattices that form the metals are actually an ionic cluster (composed only of cations and electrons). The electrons present in the valence layer of the metal atoms are delocalized, that is, they leave the valence layer, causing the atom to become a cation (electron deficient).

After being delocalized, the electrons from the metal atoms surround the cations, forming a true "sea of electrons". Each of the electrons in this sea has the ability to move through the crystal lattice of the metal freely.

THE ANSWER IS D. A NONMETAL ATOM TRANSFERS ELCTRONS TO A METAL ATOM

ITS A TYPE OF ENERGY BONDING THAT ARISES FROM ELECTROSTATIC. ATTRACTIVE FORCE BETWEEN CONDUCTION ELCTRONS (A NONMETAL ATOM) AND A POSITIVELY CHARGED METAL ATOM ( WHO ATTRACTS THE NONMETALS ELECTRONS BECAUSE ITS POSITIVELY CHARGED)

There are  3 types of chemical bonds:

1) Ionic: A bond formed by the transfer of electrons from from one atom to the other

2) Covalent : A bond formed by sharing of electrons between atoms

3) Metallic: A bond formed by the electrostatic attraction between metal ions and delocalised electrons.

Metals are electropositive, i.e. they have a tendency to lose electron. In a metallic lattice, this creates positively charged ions surrounded by negatively charged electrons which are held  by electrostatic forces of attraction.

Ans: E) They form because electrons move freely between atoms.

➷ The correct option would be B. metal ions floating in a sea of electrons. The valence electrons of the metals form a sea of delocalized electrons.

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