Why is that the aluminum atom is larger than the phosphorus atom, but the aluminum ion is smaller than the phosphorus ion?
Aluminum atom is larger than a phosphorus atom because aluminum has a net charge (after removing shielding electrons) of +4 and the phosphorus atom has a net charge of +5Since Phosphorus has a higher net charge, the electrons are attracted more strongly by the Phosphorus nucleus than the Aluminum nucleusBecause the outer shell is closer to the nucleus of the aluminum, thus the aluminum atom will be smaller than phosphorus atomSize of ions are determined by what kind of ions are formed (which you failed to specify)Aluminum is more likely to form cations and Phosphorus is more likely to form anionsAssuming Al+ and P- as examplesBoth atoms will still have the same net charge of +4 and +5 respectivelyHowever, since the Aluminum ion has less valence electrons, they repel each other less, hence the valence shell is closer to the Aluminum nucleusSimilarly, Phosphorus ion has more valence electrons, there is stronger inter-electron repulsion, pushing the valence shell further from the Phosphorus nucleusTherefore Al atom P atom, but Al+ P-
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