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Rank the members of each set of compounds in order of decreasing ionic character of their bonds. Use partial charges to indicate the bond polarity of each:

A. PCl3, PBr3, PF3
B. NF3, BF3, CF4
C. SeF4, TeF4, BrF3

Respuesta :

Answer:

Ionic character

A.  PF₃ > PBr₃ > PCl₃

B. BF₃ > CF₄ > NF₃

C. TeF₄ > BrF₃ > SeF₄

Explanation:

The most electronegative element is fluorine, followed chlorine, phosphorous nitrogen etc.

  • Atoms with high electronegativity tend to form negative ions.
  • Ionic compounds formed between elements with high electronegativity difference.
  • % ionic character is directly proportional to electronegativity difference.
  • According to Pauling Scale E.n for F(4.0), O(3.5), N(3.0), C(2.5), B(2.0), P(2.19), Se(2.55) , Te (2.1), Cl(3.16) and Br(2.96)
  • ΔE.N (Electronegativity difference) between( P and F = 4 - 2.19 = 1.81), (P and Br = 2.96 - 2.19 = 0.77) , (P and Cl = 3.16 - 2.96 = 0.2 )
  • ΔE.N (Electronegativity difference) between( N and F = 4 - 3 = 1), (B and F = 4 - 2 = 2) , (C and F = 4 - 2.5 = 1.5 )
  • ΔE.N (Electronegativity difference) between( Se and F = 4 - 2.55 = 1.45), (F and Te = 4 - 2.1 = 1.9) , (F and Br = 4 - 2.19 = 1.81 )

pstnonsonjoku

Polarity of bonds result from a high difference in electronegativity between bonding atoms.

Polarity in covalent bonds arises from the fact that the electron cloud of the bond is closer to one of the bonding atoms than the other. This in turn results from significant difference in electronegativity between the atoms in the bond. Hence, a polar covalent bond displays ionic character.

The arrangement of the compounds in each set in order of decreasing ionic character is shown below;

  • PF3 >  PCl3 > PBr3
  • BF3 >  CF4 >  NF3
  • TeF4 > SeF4 > BrF3

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