Effective nuclear charge = Zeff = the attraction of electrons to the nucleus
Zeff decreases down a group because the size of the elements increase and electrons get farther
away from the nucleus. Electron shielding reduces the charge of the outer electrons between the
nucleus.
Zeff increases across a period b/c as protons are added, valence electrons are also added and
face less shielding. Elements are also smaller as you go left to right across periods.
Cl, Na, P, S
(largest to smallest)
All the elements are in the same period and Zeff increases across the period so the order is:
Cl, S, P, Na
Solution
Effective nuclear charge = Zeff = the attraction of electrons to the nucleus
Zeff decreases down a group because the size of the elements increase and electrons get farther
away from the nucleus. Electron shielding reduces the charge of the outer electrons between the
nucleus.
Zeff increases across a period b/c as protons are added, valence electrons are also added and
face less shielding. Elements are also smaller as you go left to right across periods.
Cl, Na, P, S
(largest to smallest)
All the elements are in the same period and Zeff increases across the period so the order is:
Cl, S, P, Na.
Effective nuclear charge = Zeff = the attraction of electrons to the.pdf
1. Effective nuclear charge = Zeff = the attraction of electrons to the nucleus
Zeff decreases down a group because the size of the elements increase and electrons get farther
away from the nucleus. Electron shielding reduces the charge of the outer electrons between the
nucleus.
Zeff increases across a period b/c as protons are added, valence electrons are also added and
face less shielding. Elements are also smaller as you go left to right across periods.
Cl, Na, P, S
(largest to smallest)
All the elements are in the same period and Zeff increases across the period so the order is:
Cl, S, P, Na
Solution
Effective nuclear charge = Zeff = the attraction of electrons to the nucleus
Zeff decreases down a group because the size of the elements increase and electrons get farther
away from the nucleus. Electron shielding reduces the charge of the outer electrons between the
nucleus.
Zeff increases across a period b/c as protons are added, valence electrons are also added and
face less shielding. Elements are also smaller as you go left to right across periods.
Cl, Na, P, S
(largest to smallest)
All the elements are in the same period and Zeff increases across the period so the order is:
Cl, S, P, Na
