For #CCl_4#, #SiCl_4#, #PbCl4#, and #PbCl2#, which species exhibits the GREATEST ionic character?

Answer 1

Well, which beast has the highest melting point....?

And the highest melting and boiling point should correspond to the LEAST molecular.....and thus, in this scenario, the MOST ionic...and you will have to supply the physical constants, i.e. #"normal melting and boiling points,"# yourself. They should be available on the web....
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Answer 2

#"SiCl"_4# has the most ionic character.

I think "they" are asking you to determine the polarity of the bonds based on electronegativity differences (#ΔEN#).

Here is a table of the numbers:

#ulbb("Atom"_1color(white)(m)ENcolor(white)(m)"Atom"_2color(white)(m)ENcolor(white)(m)ΔENcolor(white)(m) "% Ionic")# #color(white)(m)"Cl"color(white)(mmll)3.16color(white)(mm)"C"color(white)(mmm)2.56color(white)(mll)0.61color(white)(mmml)9# #color(white)(m)"Cl"color(white)(mmll)3.16color(white)(mm)"Si"color(white)(mmm)1.90color(white)(ml)1.26color(white)(mmm)33# #color(white)(m)"Cl"color(white)(mmll)3.16color(white)(mm)"Pb"color(white)(mmll)2.33color(white)(ml)0.83color(white)(mmm)16#
The bonds are all polar covalent, and the #ΔEN# values tell us the most polar bond is #"Si-Cl"#.
The electronegativity difference corresponds to 33 % ionic character in the #"Si-Cl"# bond.
Why isn't #"PbCl"_2# the most ionic compound?
#"CCl"_4, "SiCl"_4#, and #"PbCl"_4# are liquids at room temperature but #"PbCl"_2# is a solid that melts at 501 °C.
The difference is that #"PbCl"_2# consists of #"AX"_2# linear molecules.
They can form an extended 3D crystal lattice with #stackrelcolor(blue)(δ^"+")("Pb")"···"stackrelcolor(blue)(δ^"-")("Cl")"—"stackrelcolor(blue)(δ^"+")("Pb")"—"stackrelcolor(blue)(δ^"-")("Cl"# dipole-dipole interactions.
The #"XCl"_4# compounds all have nonpolar tetrahedral molecules.

They have only weak London dispersion forces and cannot form an extended lattice with dipole-dipole interactions

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Answer 3

PbCl2 exhibits the greatest ionic character among CCl4, SiCl4, PbCl4, and PbCl2.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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