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Is ClO4- a covalent bond or an ionic bond?

Sagot :

jenilyn26205

Answer:

The simplest one here is HClO. Its valence diagram is H—O—Cl, with each of the bonds being ordinary covalent bonds, each involving a shared pair of electrons, with one electron coming from each of the atoms at each end of the bond.

Now the perchlorate (anion) involves coordinate covalent bonds. The Lewis electron-dot structure involves Cl in the center, sharing a pair of electrons with each of the 4 oxygens — and in addition, each O atom involves 3 lone pairs. This makes 4x8 = 32 electrons, which agrees with 6 from each O & 7 from Cl & 1 to make it a 1- anion — that is, 5x4+7+1 = 32. Another way to represent perchlorate is as one covalent bond from Cl to O^1- and 3 coordinate covalent bond from each of the remaining 3 oxygens to the Cl. Note however (as suggested from the Lewis e-dot diagram) each O is equivalent, and the overall geometry is tetrahedral: each O atom at the corner of a regular tetrahedron with the Cl atom in the center of the tetrahedron.

Now ClF5 is trickier, and the Lewis octet rule is not satisfied (for the Cl), but it is satisfied for F (as in ~100% of all cases for an F atom in a stable compound). That is each F is to have an octet of electrons, so each gaining one from the central Cl. Thus Cl makes 5 electron-pair sharing bonds to each F, and has 2 valence electrons left over, which then constitute a lone pair. Thus Cl has %+1 = 6 electron pairs around it (for a total of 12 valence electrons, around the Cl), and they repel one another to end up as far apart as possible, around the Cl. That is, they end up at the corners of an octahedron (which is 2 Egyptian pyramids with their bases glued together). There is one O atom at 5 of the 6 corners of this octahedron. Thus the molecular geometry for ClF5 looks like an Egyptian pyramid with an F at each of the 5 corners, and the Cl in the middle of the base.

Explanation:

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