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Which orbital experiences the greatest effective electron charge in copper?
In copper (Cu), the 3d orbital experiences the greatest effective electron charge. This is due to the presence of a relatively high nuclear charge and the shielding effect of the 4s electrons, which results in the 3d electrons feeling a greater attraction from the nucleus. The effective nuclear charge experienced by the 3d electrons is higher compared to the 4s electrons, making them more tightly bound to the nucleus.
Why is the third ionization energy of calcium greater than that of pottasium?
The third ionization energy of calcium is greater than that of potassium because calcium has a higher effective nuclear charge and a more compact electron configuration. When removing the third electron from calcium, it involves removing an electron from a more stable, fully filled subshell (3s²) after two electrons have been removed. In contrast, potassium's third ionization energy involves removing an electron from a less stable configuration (4s¹), making it easier to remove. Consequently, the energy required to remove the third electron from calcium is higher.
Which has 2 electron in the 4s sublevel?
Ca
When comparing the energy of an electron in the 3d sub-level to that of an electron in the 4s sublevel of the same atom?
They are both capable of holding a maximum of 10
Is that 4s or 3d orbital to which an excited electron from 3p would first go?
4s, as it is lower in energy.. s then d
What will be the effective nuclear charge on 4s electron of zinc on the basis of Slater's rule?
The effective nuclear charge on the 4s electron of zinc, according to Slater's rule, would be lower than the actual nuclear charge due to shielding effects from inner electrons. It would be less than +30 (the nuclear charge of zinc) since the 3d electrons partially shield the 4s electron from the full charge of the nucleus.
What is the effective nuclear charge experienced by calcium's valence electrons?
as you know we must first have the electron configuration to get the valence electrons. the electron configuration is: 1s2 2s2 2p6 3s2 3p6 4s2. we now have the electron configuration but we dont have the v.e. the last electron in the calcium atom are in the 4s orbital so that means that since it the only electron in the 4s orbital we will use it as a v.e. so as to get the v.e. we will subtract the shielding electrons from the nuclear charge shortly expressed by the formula below. Zeff=S-Z in this case Z will be the sum of the shielding electrons and s is the nuclear charge. Zeff=20-18 Zeff=2+ so the effective nuclear charge is 2+ or 2. hope you like it.
Even though zinc is after copper in the periodic table leading to an increase in the nulear charge by 1 which should therefore decrease the radius why is it larger than copper?
Zinc has a filled 3d sublevel and 4s sublevel. There is more shielding from the effective nuclear charge within the filled 3d sublevel and also from the filled 4s sublevel. Copper does not have a filled 4s sublevel; recall that one of the 4s electrons "jumps up" to the 3d sublevel thereby stabilizing it by making it filled with 10 electrons. Because of this, the 4s is only half filled and there is not as much shielding within the 4s sublevel allowing the effective nuclear charge to pull the 4th energy level in more toward the nucleus. This will make the overall size of the atom smaller.
What is shieldin for 1s22s2p63s23p64s2?
Shielding refers to the phenomenon where inner electrons partially block the outer electrons from the full effect of the nucleus's positive charge. In the electron configuration 1s² 2s² 2p⁶ 3s² 3p⁶ 4s², the electrons in the inner shells (1s, 2s, and 2p) shield the outer 3s, 3p, and 4s electrons from the nucleus. This results in a reduced effective nuclear charge experienced by the outer electrons, which affects their energy levels and chemical behavior.
Is there nuclear energy in a iPhone 4S?
No.
Which has 2 electron in the 4s sublevel?
Ca
When comparing the energy of an electron in the 3d sub-level to that of an electron in the 4s sublevel of the same atom?
They are both capable of holding a maximum of 10
Why does a 4s electron have higher energy than a 3d electron in a chromium atom?
A 4s electron has higher energy than a 3d electron in a chromium atom because of the way electrons fill energy levels. In chromium, the 4s orbital is filled before the 3d orbital due to the stability gained from having a half-filled or fully-filled d orbital. This results in the 4s electron having higher energy than the 3d electron in a chromium atom.
What is the number of electrons in the in the outer shell of K plus?
K is potassium, and it is found in group I and period 4. It is an s block element. So, being in group I, this indicates it has ONE electron in the outer shell (4s).
4S's of effective communication?
The 4S's of communication are Shortness,Simplicity,Strength,Sincerity.
Element with a 3- charge in the 4th energy?
An element with a 3- charge in the 4th energy would have a strong, stable nucleus with a strong nuclear force holding the protons and neutrons together. This element would also have a strong, repulsive electrostatic force between the protons in the nucleus and the electrons in the 4th energy level.
An element with 20 protons and 20 electrons gains one electron The electron goes into what type of orbital?
The extra electron would go into a 4s orbital because 4s can hold up to 2 electrons before 3d can be filled.
