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What is difference between an s subshell and a d subshell orbital?
The primary difference between an s subshell and a d subshell orbital is their shape and orientation. S subshell orbitals are spherical in shape and are found at the nucleus, while d subshell orbitals have cloverleaf or butterfly shapes and are oriented along axes passing through the nucleus. Additionally, d orbitals have more complex shapes due to their higher angular momentum quantum number.
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?
The compound with the 2+ ion that is the smallest with a filled d subshell is zinc (Zn^2+), and the anion that forms from the smallest halogen is fluoride (F^-). Therefore, the compound you are looking for is zinc fluoride (ZnF2).
The principal quantum number of the first d subshell is?
The principal quantum number of the first d subshell is 3. In the case of d orbitals, they start appearing in the n=3 energy level.
How many d orbitals can exist in a single subshell?
There are five d orbitals that can exist in a single subshell. These orbitals are usually labeled as dxy, dxz, dyz, dz^2, and dx^2-y^2. Each orbital can hold up to 2 electrons, giving a total of 10 electrons that can occupy the d subshell.
A subshell contains eight electrons. Which subshell could it be?
A subshell that contains eight electrons is the 3d subshell. The d subshell can hold a maximum of 10 electrons, but in this case, with eight electrons, it is likely filled with a combination of spin-up and spin-down electrons. Other subshells, such as p (which can hold a maximum of 6 electrons) or s (which can hold a maximum of 2 electrons), cannot contain eight electrons.
What is the maximum number of unpaired electrons in the s subshell and the d subshell and the p subshell and f subshell?
The maximum number of unpaired electrons in the s subshell is 2, in the p subshell is 6, in the d subshell is 10, and in the f subshell is 14. This is based on the maximum number of electrons that can occupy each subshell according to the Aufbau principle and the Pauli exclusion principle.
What is difference between an s subshell and a d subshell orbital?
The primary difference between an s subshell and a d subshell orbital is their shape and orientation. S subshell orbitals are spherical in shape and are found at the nucleus, while d subshell orbitals have cloverleaf or butterfly shapes and are oriented along axes passing through the nucleus. Additionally, d orbitals have more complex shapes due to their higher angular momentum quantum number.
How many electrons are in the d subshell for scandium?
Scandium has 1 3d electron.
Do main group metals from period 5 onward tend to lose electrons from the d subshell first?
Yes, main group metals from period 5 onward tend to lose electrons from the s subshell first before losing electrons from the d subshell. This is because the s subshell has lower energy levels compared to the d subshell, making it easier for the electrons to be lost from the s subshell.
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?
The compound with the 2+ ion that is the smallest with a filled d subshell is zinc (Zn^2+), and the anion that forms from the smallest halogen is fluoride (F^-). Therefore, the compound you are looking for is zinc fluoride (ZnF2).
The maximum number of electrons in a single d subshell is?
The maximum number of electrons in a single d subshell is 10.
The principal quantum number of the first d subshell is?
The principal quantum number of the first d subshell is 3. In the case of d orbitals, they start appearing in the n=3 energy level.
How many electrons does the transition metals lose?
Transition metals typically lose 1, 2, or 3 electrons to achieve a stable electron configuration. This helps them attain a full or half-full d subshell, which is more stable than an incomplete d subshell. The number of electrons lost by a transition metal depends on its position in the transition metal series and the specific chemical reaction.
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 types of electrons s p d or f are considered those involved in the make up of the outer shells of atoms?
It depends on the particular atom in question. Any of those subshells can make up the outer shells of atoms. Examples: In Mg, the outer shell is the 2s subshell. In P, the outer shell is the 3p subshell. In Fe, the outer shell is the 3d subshell, etc.
The subshell letter?
specific the 3-D shape of the orbiral
What is the full form of CFA?
d full form is Chartered Finance Analyst
