The electronic configuration of magnesium is:
1s² 2s² 2p⁶ 3s² = [Ne] 3s²
This means that for a magnesium atom, in order to have its outermost orbital full, the easiest way would be to lose the two outermost electrons. This is seen in its relatively low first two ionization energies. <u>The third ionization energy is several times higher because the ion would move from a stable form to an highly unstable form.</u> (Mg⁺² → Mg⁺³ + e⁻).
- Sodium only has one electron in its outermost orbital, so its first ionization energy would be several times lower than the second.
I will need a picture if the periodic table
Answer:
D
Explanation:
Scientific laws describe how things work with little to no exception. They do NOT provide an explanation to WHY something occurs.
Use PV =nRT. Rearrange it to n = PV/RT.
P = 202.6 kPa
V = 4.0L
R = 8.314 kPa*L/mol*K
T = 127 °C + 273 = 400 K
Plug it in and solve. I got 0.24 moles of H2.
