Arrange the following ions in order of increasing size:Na+1, Mg+2,Br-1?

Question

Please provide detailed answer with suitable reason/s.Which ion has the smallest size and which ion has the largest?

Answer 1

Mg2+ < Na+ < Br-

Ion size depends first on the main quantum number. Na and Mg both strip down to the Ne configuration, while Br takes up the Xe configuration, two main quantum numbers higher.

Mg2+ is smaller than Na1+ because the remaining electrons are subject to a stronger electrostatic field.

The above is true for ions in crystal lattices.

Note that in watery solutions ion size has to be calculated differently when you take the hydrate shell into account. Na+ becomes Na(H2O)6(1+), and Mg2+ becomes Mg(H2O)6(2+). Bromide won't take up a regular hydrate shell.

Answer 2

Mg+2>Na+1>Br-1

Answer 3

Mg+2, Na+1, Br-1,

Answer 4

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Answer 5

increasing orderBr-1 all three ions belong to same period
in a period as we move frm left to right atomic no increases and thus effective nuclear charge increases on valence shell thereby resulting in contraction of size
as Br-1 has the largest atomic no in a given period thus have greater effective nuclear charge and smallest in size
in case of Na and Mg ions both have same atomic no hence have similar size

Answer 6

Na, Br,Mg... from smallest to largest. Detailed answer??! Because that's the way they are and I put them in that order!

Answer 7

Br, Na, Mg

br is the smallest because it has a high electronegativity so high it can only accept electrons and not take..high electronnegativity means it it more compact

Answer 8

Mg+2 first, then sodium, then bromide

Mg, cuz it has one electron less than sodium and another proton to pull on them, then sodium cuz it's a period above bromide, then bromide

Answer 9

you typed the right order

Answer 10

u typed the correct order to ur requirment