Cu =63.5
2 times N =28.02
6 times O =96
96=63.5=28.02=127.07
122/127.07=.96 molecules
I pick but I'm not sure about it though 1and3
We need to use the following formula
Δ
n= 4 moles
F= constant= 96500C/mol
let's plug in the values.
ΔG= -(4)(96500)(0.24)=
-92640 J or -92.6 kJ
The group on the periodic table that would have 0 electronegativity due to the fact that their valence shell is full, i.e, have a full octet would be the inert or noble gases. They have a total of 8 electrons in their valence shell and are thus inert and cannot strongly attract electrons toward itself, from neighbouring atom electrons as it does not need to.
First off chlorine is not a metal so you can ignore that one.
Sodium and Rubidium are in group 1 of the periodic table and Magnesium is in group 2.
Group one metals are more reactive than group two because it is harder for the group two metals to lose their 2 valence (outer most) electrons.
As you go down group 1 there is an increase in the reactivity this is because as you go down there is an increase in the atomic radius which leads to more shielding. This weakens the electrostatic forces of attraction making it easier to lose the outermost electrons, therefore they are more reactive.
