Periodic Trend: Effective Nuclear Charge
Effective Nuclear Charge (Zeff) measures the force exerted onto an electron by the nucleus.
Periodic Trend: Effective Nuclear Charge
Higher the Effective Nuclear Charge (ZEff), greater the attractive force, which results in electrons being pulled closer to the nucleus.
Higher the Shielding Constant (S), greater the repulsive force between valence and inner core electrons, which results in valence electrons pushed away from the nucleus.
Periodic Trend: Effective Nuclear Charge
Moving towards the top right corner of the Periodic Table causes effective nuclear charge to increase.
Periodic Trend: Effective Nuclear Charge Example 1
Periodic Trend: Effective Nuclear Charge
Periodic Trend: Effective Nuclear Charge Example 2
What is the identity of an element when the effective nuclear charge of its valence electrons is 18 while its shielding constant is 5?
Periodic Trend: Effective Nuclear Charge Example 3
In which orbital does an electron in a sulfur atom experience the greatest shielding?
Using Slater’s Rules calculate the effective nuclear charge of the 4d orbital electron in iodine.
- For a multielectron atom, a 3s orbital lies lower in energy than a 3p orbital because (LO 5.16) (a) a 3p orbit...
- Among the elements N, O, P, and S, which element or elements have the smallest effect nuclear charge if we use...
- Which of the following statements about effective nuclear charge for the outermost valence electron of an atom...
- Detailed calculations show that the value of Zeff for the outermost electrons in Na and K atoms is 2.51+ and ...
- Detailed calculations show that the value of Zeff for the outermost electrons in Si and Cl atoms is 4.29+ and...
- Which will experience the greater effect nuclear charge, the electrons in the n = 2 shell in F or the n = 2 sh...
- Arrange the following atoms in order of increasing effective nuclear charge experienced by the electrons in th...
- Consider the isoelectronic ions F- and Na+. (b) Using Equation 7.1 and assuming that core electrons contribute...
- (a) From the data in Table 8.2, calculate the effective charges on the Br atom of the HBr molecule in units of...
- (a) From the data in Table 8.2, calculate the effective charges on the H atom of the HBr molecule in units of ...
- Which experience a greater effective nuclear charge: the valence electrons in beryllium or the valence electr...
- Arrange the atoms according to decreasing effective nuclear charge experienced by their valence electrons: S,...
- If core electrons completely shielded valence electrons from nuclear charge (i.e., if each core electron redu...
- If core electrons completely shielded valence electrons from nuclear charge (i.e., if each core electron redu...
- If core electrons completely shielded valence electrons from nuclear charge (i.e., if each core electron redu...
- In Section 3.6, we estimated the effective nuclear charge on beryllium’s valence electrons to be slightly grea...
- Why is energy usually released when an electron is added to a neutral atom but absorbed when an electron is re...
- Figure 7.4 shows the radial probability distribution functions for the 2s orbitals and 2p orbitals. (b) How wo...
- (b) Repeat these calculations using Slater’s rules.
- (a) If the core electrons were totally effective at screening the valence electrons and the valence electrons ...
- How does electron shielding in multielectron atoms give rise to energy differences among 3s, 3p, and 3d orbita...
- Order the electrons in the following orbitals according to their shielding ability: 4s, 4d, 4f.
- One method for calculating Zeff is to use the equation where E is the energy necessary to remove an electron ...