Elements with three p-electrons....
That would be N, P, As, Sb, and Bi -- elements in group 15
For example, energy diagram showing "empty" orbitals up through the 3p.
.....3p __ __ __
3s __
.....2p __ __ __
2s __
1s __
Energy diagram of phosphorous showing three unpaired electrons in 3p-sublevel
.....3p ↑_ ↑_ ↑_
3s ↑↓
.....2p ↑↓ ↑↓ ↑↓
2s ↑↓
1s ↑↓
According to Hund's rule, the electrons singly occupy the p-orbitals, and all have the same spin.
Answer:
The correct answers are first, fourth, fifth
Explanation:
Answer:
Explanation:
Beryllium especially, but Boron as well both exhibit metallic characteristics.
The outside ring of Beryllium contains 2 electrons. It would have to take on 6 electrons to have a ring of 8. The same statement can be made about Boron (except that it would need 5 electrons to make 8). It is easier for the atom to give up 2 or 3 than than to take on 5 or 6. It would not be easy to have a 5 or 6 minus charge on it.
N2(g)+3H2 >>>>>2NH3(g)
the mole ratio between N2, H2 and NH3. It is 1 : 3 : 2
mole N2 present
moles H2 present = 25.0 g H2 x 1 mole H2/2 g = 12.5 moles H2 present
Based on mole ratio, N2 is limiting in this situation because there is more than enough H2 but not enough N2.
moles NH3 that can be produced = 1 mole N2 x 2 moles NH3/mole N2 = 2 moles NH3 can be produced
grams of NH3 that can be produced = 2 moles NH3 x 17 g/mole = 34 grams of NH3 can be produced
