determine which experiences a lower effective nuclear charge. using words and/ or drawings explain why.
A) an electron in a 2s or an electron in a 2p
B) a valence electron on sulfure or a vance electron on silicon
C) a valence electron on chlorine or a valence electron on bromine
-- i don't get this at all! can somebody please explain this to me in detail. thank you!
To determine which experiences a lower effective nuclear charge, we need to understand the concept of effective nuclear charge and how it affects the electrons.
Effective nuclear charge refers to the net positive charge experienced by an electron in an atom. It is the difference between the actual nuclear charge (the number of protons in the nucleus) and the shielding effect caused by inner electrons. The more inner electrons there are, the more they shield the outer electrons from the full positive charge of the nucleus.
Now let's analyze each option to see which electron experiences a lower effective nuclear charge:
A) Electron in 2s vs. electron in 2p:
In both cases, the electrons are in the second energy level. However, the 2p electron experiences a lower effective nuclear charge than the 2s electron. This is because the 2p orbital is slightly farther from the nucleus and has a more diffuse shape compared to the 2s orbital. The electron in the 2p orbital is shielded more effectively by the inner electrons, resulting in a lower effective nuclear charge.
B) Valence electron on sulfur vs. valence electron on silicon:
Sulfur and silicon are both in the same period of the periodic table, so they have the same number of inner shells. However, silicon has a larger atomic number, meaning it has more protons in its nucleus. Therefore, the valence electron on sulfur experiences a lower effective nuclear charge than the valence electron on silicon. This is because the extra protons in the silicon nucleus exert a stronger attractive force on the outer electron, resulting in a higher effective nuclear charge.
C) Valence electron on chlorine vs. valence electron on bromine:
Chlorine and bromine are both in the same group of the periodic table, so they have the same number of valence electrons and similar atomic structures. However, bromine has a larger atomic number than chlorine, meaning it has more protons in its nucleus. As a result, the valence electron on chlorine experiences a lower effective nuclear charge than the valence electron on bromine. The extra protons in the bromine nucleus exert a stronger attractive force on the outer electron, leading to a higher effective nuclear charge.
In summary, the electron in a 2p orbital experiences a lower effective nuclear charge compared to a 2s electron. The valence electron on sulfur experiences a lower effective nuclear charge compared to a valence electron on silicon. Lastly, the valence electron on chlorine experiences a lower effective nuclear charge compared to a valence electron on bromine.