which of the following gaseous atoms is expected to have the largest volume?
a. Sr +2
b. Sr
c. Be
d. Ca
E. Be+2
Why? what is the different between Sr. and Sr+2?
thank you
2007-03-21 12:26:49 · 3 answers · asked by carla 2 in Science & Mathematics ➔ Chemistry
You should know that, looking at the periodic table, you'll find the largest elements in the lower-left-hand corner and the smallest in the upper-right-hand corner. The reason that atom size decreases as you move left to right in the periodic table is that the atoms on the right have more protons than the atoms on the left, so the protons are pulling more on the electrons, so the electrons are closer to the center and the whole thing is smaller. Size increases as you go down a column in the table because there are more electron orbitals (a greater available space for electrons to hang out).
The difference between Sr and Sr+2 is just that Sr+2 has two fewer electrons. That's all. Therefore, it stands to reason that Sr would be bigger, because taking an electron away makes an atom smaller.
Look at the periodic table and see which element (of the choices you gave) is closest to the lower-left-hand corner of the table. As it turns out, it's strontium, Sr. And we just established that Sr is bigger than Sr+2, so Sr, (b), is the answer!
2007-03-21 12:34:03 · answer #1 · answered by dac2chari 3 · 0⤊ 0⤋
b is the answer
Sr+2 is strontium that has lost 2 electrons. the ionic radius becomes smaller as the protons try ho hold on to the remaining electrons.
Sr is the largest because it has the most number of electron shells (energy levels)
2007-03-21 19:35:50 · answer #2 · answered by The Cheminator 5 · 0⤊ 0⤋
+2 is the oxidation # (charge) and the answer should be ca (not positive but almost)
2007-03-21 19:33:58 · answer #3 · answered by 4evrpunk 2 · 0⤊ 1⤋