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What is the highest energy sublevel for tellurium?
The highest energy sublevel for tellurium (Te), which has an atomic number of 52, is the 5p sublevel. In its electron configuration, tellurium is represented as [Kr] 5s² 4d¹⁰ 5p⁴, indicating that the 5p sublevel is the outermost and highest energy level occupied by electrons.
How many 5p electrons does Ba contain?
Barium (Ba) has an atomic number of 56, meaning it has 56 electrons. The electron configuration for barium is [Xe] 6s², indicating that it does not have any electrons in the 5p subshell. Therefore, barium contains 0 electrons in the 5p subshell.
How many unpaired electrons are there in stadium?
Stadium (St) is an element with the atomic number 51. It has a ground-state electron configuration of [Kr] 4d¹⁰ 5s² 5p³. In this configuration, the 5p subshell has three electrons, which are unpaired. Therefore, there are three unpaired electrons in stadium.
In what orbital are the valence electrons of Iodine?
The valence electrons of iodine are located in the 5p orbital. Iodine has an atomic number of 53, and its electron configuration is 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 4p⁶ 5s² 5p⁵. The five valence electrons in the 5th energy level are distributed in the 5s and 5p orbitals, with the 5p orbital containing the unpaired electrons that participate in bonding.
How many unpaired electrons should you expect for Sb3 plus?
Antimony (Sb) has an atomic number of 51, and its electron configuration is [Kr] 5s² 4d¹⁰ 5p³. In the Sb³⁺ oxidation state, it loses three electrons, typically from the 5p and 5s orbitals, resulting in the configuration [Kr] 4d¹⁰. Consequently, Sb³⁺ has no unpaired electrons, as all its electrons are paired in the filled 4d subshell.
What is the highest energy sublevel for tellurium?
The highest energy sublevel for tellurium (Te), which has an atomic number of 52, is the 5p sublevel. In its electron configuration, tellurium is represented as [Kr] 5s² 4d¹⁰ 5p⁴, indicating that the 5p sublevel is the outermost and highest energy level occupied by electrons.
What element completes the 5p sub level?
The 5p sublevel is completed with 6 electrons with the addition of the element radon (Rn).
How many 5p orbitals are there in an atom?
There is 1 5s orbital
How would you justify the presence of 18 elements in the fifth of period of periodic table?
In the fifth period of the periodic table, the atoms of the elements in the first two groups are adding 1 and 2 electrons, respectively, to their highest energy 5s sublevel. Starting in group 3/IIIB and going through group 12/IIB, the atoms of those elements are adding electrons to their highest energy 4d sublevel. Since the d sublevel can contain a maxium of 10 electrons, there are 10 elements whose atoms are filling the 4d sublevel. Once the 4d sublevel is filled, the next higher energy sublevel is the 5p sublevel. Starting with the group 13/IIIA elements, the 5p sublevel is being filled. Since a p sublevel can contain a maximum of 6 electrons, there are six elements whose atoms are filling the 5p sublevel. 5s sublevel filling: 2 elements 4d sublevel filling: 10 elements 5p sublevel filling: 6 elements --------------------------------------- Total: 18 elements For a printable periodic table that includes electron configurations, go to the following link: http://www.nist.gov/pml/data/periodic.cfm
How many half filled orbitals are in Xenon?
Each orbital in Xenon has its full complement of electrons.
How many 5p electrons are in Ba?
Barium (Ba) has 2 valence electrons in its outer shell. Therefore, it does not have any 5p electrons.
What is the maximum number of electrons each of the following can hold... 2s 5p 4f 3d 4d?
2s: 2 electrons 5p: 6 4f: 14 3d: 10 4d: 10
How many unpaired electrons are there in stadium?
Stadium (St) is an element with the atomic number 51. It has a ground-state electron configuration of [Kr] 4d¹⁰ 5s² 5p³. In this configuration, the 5p subshell has three electrons, which are unpaired. Therefore, there are three unpaired electrons in stadium.
In what orbital are the valence electrons of Iodine?
The valence electrons of iodine are located in the 5p orbital. Iodine has an atomic number of 53, and its electron configuration is 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 4p⁶ 5s² 5p⁵. The five valence electrons in the 5th energy level are distributed in the 5s and 5p orbitals, with the 5p orbital containing the unpaired electrons that participate in bonding.
How many 4d electrons are in Iodine?
In iodine (I), the electron configuration is [Kr]5s²4d¹⁰5p⁵. This means that there are 10 electrons in the 4d orbital.
What are the types of sub-levels?
If the principle energy level is n=1 then the type of sublevel is 1sN=2---> type of sublevel is 2s and 2pN=3---> type of sublevel is 3s, 3p, and 3dN=4---> type of sublevel is 4s, 4p, 4d, and 4fN=5---> type of sublevel is 5s, 5p, 5d, 5f and 5gN=6---> type of sublevel is 6s, 6p, 6d, 6f, 6g, and 6hN=7---> type of sublevel is 7s, 7p, 7d, 7f, 7g, 7h, and 7iNote that:s = 1 orbitalp = 3 orbitalsd = 5 orbitalsf = 7 orbitalsg = 9 orbitalsh = 11 orbitalsIf you look closely its just adding 2 to each orbital. If you want to know the number of electrons occupying the orbitals just multiply the orbital by 2.
Element with half filled 5p level?
The element with a half-filled 5p level is antimony (Sb), which has an electron configuration of [Kr] 4d^10 5s^2 5p^3. It has five electrons in its 5p orbital, meaning it half fills the 5p level.
