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What is the effective nuclear charge felt by Oxygen's valence electrons?
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What is the effective nuclear charge for the atom Mg?
the effective nuclear charge on barium is 2.
Why is atom of sulfur smaller than an atom of silicon despite sulfur having more mass?
Because as you add more electrons to the same valence shell, the effective nuclear charge increases and thus holds the valence shell closer.
Why are cation always smaller than the atoms from which they are formed?
Cations are positive ions formed by the loss of electrons. As cations have less number of electrons, the effective nuclear charge increases and as such,the remaining electrons are more tightly bound by the nucleus and there is a reduction in size. In most of the cases, the parent atom loses all the valence electrons in order to form a cation leading to the reduction of one shell(the valence shell).
The outermost electrons in an atom are called?
Valence electrons
What are the electrons in the outmost shell of an atom called?
the electrons in the outermost shell of an atom are considered to be the valence electrons.
Why do the valence electrons in nitrogen experience a greater effective nuclear charge than the valence electrons in beryllium?
valence electron in nitrogen
What is the effective nuclear charge for the atom Mg?
the effective nuclear charge on barium is 2.
What is the effective nuclear charge on Y?
Y=39 with 36 inner electrons shielding the 3 valence electrons producing a Zeff of +3
What is the chemical formula of phosphate?
PO43-.This in superscript form, hence, the formula is one phosphorous, 4 oxygens, and 3- valence electrons.
How much valence electrons does sulfur have?
The element Sulfur has 6 valence electrons. : )
What is the approximate effective nuclear charge for a valence electron in krypton?
2
In general - what happens to the atomic radius from left to right across a period?
Generally, it decreases.*As you move from left to right across a period the elements' number of protons increases, increasing the effective nuclear charge (the charge felt by the outermost [valence] electrons after taking into account the shielding electrons). As effective nuclear charge increases the attraction between the nucleus and the valence electrons increases, pulling the valence electrons closer to the nucleus, decreasing the atomic radius.*Please understand that this is not a hard and fast rule. There are other factors to take into account when determining atomic radius, this is just a general trend witnessed.
Calculating z effective?
Zeff = Z - s Z = nuclear charge (number of protons) s = (# of valence electrons x .35) + (# of electrons in next lower shell x .85) + (# of electrons on all shells 2 or more levels below the valence shell x 1.00) This calculates the screening constant
What is it called when electrons in the inner energy levels block the attraction between the nucleus and the valence electrons?
nuclear shielding
Why is an atom of sulfur smaller than an atom of silicon despite sulfur having more mass?
Because as you add more electrons to the same valence shell, the effective nuclear charge increases and thus holds the valence shell closer.
Why is atom of sulfur smaller than an atom of silicon despite sulfur having more mass?
Because as you add more electrons to the same valence shell, the effective nuclear charge increases and thus holds the valence shell closer.
What is the difference between effective valence electron and outer shell count?
Number of electrons in outer shell determines thechemical nature of the element and is unique per element. Effective Valence electrons is a calculated ratio between two concentrations of electrons. if n=resisitivity/(e*driftMobility) and n_at=density*Avogadro#/AtomicMass. Effective valence electrons is then n/n_at. Rounding this number should agree with outer shell electrons as predicted from the periodic table.
