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Scandium has 1 3d electron.
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How many d electrons does Hg have?
Mercury (the neutral atom) has 8o electrons.
What is the number of electrons in the sub level d?
The maximum number of electrons in a 'D' sublevel is 10
In a Bohr diagram how many electrons are in each shell?
There are 4 electron sub-shells: s, p, d, and f. These letters stand for sharp, principal, diffuse, and fundamental, but the names are not important. s subshells have 2 electons, while p subshells have 6, d subshells have 10, and f subshells have 14. There can be higher subshells, but these subshells require too much energy to fill and no element with a g subshell (the next subshell after f) has ever been synthesized. The first shell (i.e. the first period of the periodic table) has only s. Thus, the first shell has 2 electrons. The second shell has s and p subshells, so it has 2+6 or 8 electrons. The third shell has s, p, and d subshells. It ultimately has 18 electons. This can be misleading, however. The d subshell requires more energy to fill than the higher-shell s subshell. This is why the third period of the periodic table does not have a d section: the d electron subshell of the third Bohr shell does not fill until after the s subshell of the fourth Bohr shell has filled. Looking at the periodic table, you can see that the third period only has 8 electrons, while the 4th period has 18. The 18 electrons in the fourth period are the s subshell of the fourth shell, the d subshell of the 3rd shell, and the p subshell of the 4th shell. The fourth shell is similar to the third shell, but more extreme. The fourth shell has s, p, d, and f subshells, but the f subshell is not filled until two higher s shells have been filled. It does, however, fill out to 32 electrons in the 6th period of the periodic table. In the 6th period, the first period to have 32 electrons, there are 32 electrons, filling these subshells: s subshell of the 6th shell, f subshell of the 4th shell, d subshell of the 5th shell, and then the p subshell of the 6th shell. The fifth shell would ultimately fill out to a full 50 electrons and would do so in the 8th period of the periodic table. However, as previously noted, no substance has ever been found or generated with that many electrons. It would fill the s subshell of three shells above (i.e. shell 8) before it filled the g subshell of shell 5. No element in the 8th period has ever been synthesized, so a filled fifth Bohr shell has never been found. A good example for a Bohr diagram would be Astatine, which is in the 6th period. In the first shell of the Bohr diagram, you have 2 electrons (s subshell only). It is filled completely. In the second, you have 8 electrons (s and p subshells) and in the third you have 18 electrons (s, p, and d), and both shells are filled completely. In the fourth shell, you have 32 electrons (s, p, d, and f), and it is filled completely. In the fifth shell, you have 18 electrons. This is because only the s, p, and d subshells are filled. It would require too much energy to fill the f subshell of the 5th shell, so the electrons just go to the s, p, and d subshell of higher shells. The 6th shell has 7 electrons. The 2 electrons of the s subshell are filled first, and then 5 electrons go into the p shell.
Do main group metals from period 5 onward tend to lose electrons from the d subshell first?
nope :)
What is the maximum number of p orbitals that are possible?
Each of the p orbitals can hold 2 electrons due to the Pauli exclusion principle. Because there are 3 p orbitals in a given subshell, the overall p subshell can hold 6 electrons.
What is the maximum number of unpaired electrons in the s subshell and the d subshell and the p subshell and f subshell?
d subshell = 2 p subshell = 6
How many d electrons does Hg have?
Mercury (the neutral atom) has 8o electrons.
How many places are there for electrons in the third shell of an atom?
The third shell of an atom can hold a maximum of 18 electrons. This shell consists of three subshells - s, p, and d - with each subshell being able to accommodate a certain number of electrons. The s subshell can hold up to 2 electrons, the p subshell can hold up to 6 electrons, and the d subshell can hold up to 10 electrons, totaling 18 electrons in the third shell.
The maximum number of electrons in a single d subshell is?
10 electrons
What is the number of electrons in the sub level d?
The maximum number of electrons in a 'D' sublevel is 10
Why is scandium salts white?
Scandium forms compounds with the Sc3+ ion, losing both the 4s2 and 3d1 electrons. With no electrons in the d orbitalks its sakts are colorless.
How many electrons are in a copper atoms subshell?
Ah. I know what your trying to figure out. The answers silver not copper. Anyway 5 d orbitals.
What compound has the 2 plus ion that is the smallest with a filled d subshell and an anion that forms from the smallest halogen?
Ni2+, Goes from having 28 electrons to 30, giving it 10 electrons in its 3d subshell making that subshell full.
How many unpaired electrons in (d) subshell in ferric Fe3?
5 unpaired electrons There are 5 unpaired electrons in the Fe3+ ion. The reason for this is that Iron has the electron configuration Ar3d5.
How many electrons can a 5p sublevel hold?
The 5p subshell is a p-subshell, and as such is filled by 6 electrons - three pairs spinning in opposite directions.The number of electrons in each subshell is as follows:Subshell s p d f theoretical next subshellsNo. of e- 2 6 10 14 18, 22, 26, etc.
In a Bohr diagram how many electrons are in each shell?
There are 4 electron sub-shells: s, p, d, and f. These letters stand for sharp, principal, diffuse, and fundamental, but the names are not important. s subshells have 2 electons, while p subshells have 6, d subshells have 10, and f subshells have 14. There can be higher subshells, but these subshells require too much energy to fill and no element with a g subshell (the next subshell after f) has ever been synthesized. The first shell (i.e. the first period of the periodic table) has only s. Thus, the first shell has 2 electrons. The second shell has s and p subshells, so it has 2+6 or 8 electrons. The third shell has s, p, and d subshells. It ultimately has 18 electons. This can be misleading, however. The d subshell requires more energy to fill than the higher-shell s subshell. This is why the third period of the periodic table does not have a d section: the d electron subshell of the third Bohr shell does not fill until after the s subshell of the fourth Bohr shell has filled. Looking at the periodic table, you can see that the third period only has 8 electrons, while the 4th period has 18. The 18 electrons in the fourth period are the s subshell of the fourth shell, the d subshell of the 3rd shell, and the p subshell of the 4th shell. The fourth shell is similar to the third shell, but more extreme. The fourth shell has s, p, d, and f subshells, but the f subshell is not filled until two higher s shells have been filled. It does, however, fill out to 32 electrons in the 6th period of the periodic table. In the 6th period, the first period to have 32 electrons, there are 32 electrons, filling these subshells: s subshell of the 6th shell, f subshell of the 4th shell, d subshell of the 5th shell, and then the p subshell of the 6th shell. The fifth shell would ultimately fill out to a full 50 electrons and would do so in the 8th period of the periodic table. However, as previously noted, no substance has ever been found or generated with that many electrons. It would fill the s subshell of three shells above (i.e. shell 8) before it filled the g subshell of shell 5. No element in the 8th period has ever been synthesized, so a filled fifth Bohr shell has never been found. A good example for a Bohr diagram would be Astatine, which is in the 6th period. In the first shell of the Bohr diagram, you have 2 electrons (s subshell only). It is filled completely. In the second, you have 8 electrons (s and p subshells) and in the third you have 18 electrons (s, p, and d), and both shells are filled completely. In the fourth shell, you have 32 electrons (s, p, d, and f), and it is filled completely. In the fifth shell, you have 18 electrons. This is because only the s, p, and d subshells are filled. It would require too much energy to fill the f subshell of the 5th shell, so the electrons just go to the s, p, and d subshell of higher shells. The 6th shell has 7 electrons. The 2 electrons of the s subshell are filled first, and then 5 electrons go into the p shell.
What is difference between an s subshell and a d subshell orbital?
s subshell have energy more than d subshell
