0
How many degenerate orbitals are needed to contain seven electrons with five o?
Wiki User
∙ 15y ago
There are 6
Chlorine has 7 valence electrons, and since 2 of them can occupy one s orbital, there needs to be 5 p orbitals for everything else. (5+1=6)
Wiki User
∙ 15y ago
Add your answer:
Earn +20 pts
How many degenerate orbitals are needed to contain six electrons with two of them unpaired?
4
How many degenerate orbitals are needed to contain five electrons with three of them unpaired?
4
What is the total number of electrons needed to completely fill all of the orbitals in an atoms second principal energy level?
8 electrons
Why is chlorine written as CL2 while it has valency of 1?
Valency is the number of electrons to reach the stable number of 8 electrons in its outer shell. Electrically neutral chlorine has 7 electrons its outermost shell. This means that a single bond, where two electron orbitals overlap is required to form the stable element allotrope, therefore two atoms of chlorine are needed.
How many electrons are needed to fill one orbital?
8 electrons
How many degenerate orbitals are needed to contain six electrons with two of them unpaired?
4
How many degenerate orbitals are needed to contain five electrons with three of them unpaired?
4
In the molecule chlorine makes five covalent bonds Therefore five of its seven valence electrons need to be unpaired How many degenerate orbitals are needed to contain seven electrons with five o?
6 degenerate orbitals allows for seven electrons, five of which are unpaired. ans is 6
How many orbitals can be found in a d orbital?
There are 5 d orbitals which hold 2 electrons each. Thus, 10 electrons are needed to completely fill them.
What is the total number of electrons needed to completely fill all of the orbitals in an atoms second principal energy level?
8 electrons
Why does nitrogen not support burning?
Nitrogen molecule does not contain any unpaired electron in its molecular orbitals. Unpaired electron is needed to keep up the mechanism of burning.
What is the chemical state of sulfur?
in H2S the orbitals involved are s orbitals of hydrogen atoms and s and p orbitals of S(sulfur)The electronic configuration of sulfur is 3s2,3px2,3py1,3pz1 as there are six electrons in the outer most orbit. as there are two orbitals having two electrons each and two p orbitals having one electron each, the stable orientation is obtained by sp3 hybridization,two take pair of electrons as far away as possible and two sp3 orbitals having one electron each combine with s orbital of hydrogen to form single bond. this gives an bond angle greater than 90 but less than 108 as in hydrocarbons .the bond length is also explained by this.
Why is chlorine written as CL2 while it has valency of 1?
Valency is the number of electrons to reach the stable number of 8 electrons in its outer shell. Electrically neutral chlorine has 7 electrons its outermost shell. This means that a single bond, where two electron orbitals overlap is required to form the stable element allotrope, therefore two atoms of chlorine are needed.
How many electrons are needed to fill one orbital?
8 electrons
What is the difference between d2sp3 and sp3d2 hybrid orbitals?
Good question. A lot of people use them interchangeably, and assume they are the same. They are not the same. With sp3d2, the s, p and d orbitals which are hybridized all come from the same energy level, for instance, it has been taught that when sulfur combines with six fluorine atoms to make SF6 that the 3s, 3p and two 3d orbitals hybridize to make the sp3d2 hybrid orbital set. But d2sp3 is different. In this case the d-orbitals come from the n-1 energy level. Transition metals may exhibit d2sp3 hybridization where the d orbitals are from the 3d and the s and p orbitals are the 4s and 3d. The bottom line is this, in sp3d2 hybridization all of the orbitals have the same principal quantum number. In d2sp3, the principle quantum number of the d orbitals is one less than the principal quantum numbers of the s and p orbitals. We see d2sp3 hybridization in the transitions metals and sp3d2 hybridization in the nonmetals. There is one more issue. Chemists today are finding out that in compounds like SF6 there is no involvement of d-orbitals. In other words, there is no sp3d2 hybridization in SF6. A more likely explanation involves what is called "3-center, 4-electron" bonding in which three orbitals overlap axially (in a straight line) and contain a total of 4 electrons. This means that the 3 unhybridized p-orbitals of sulfur are all that is needed to make the six bonds with fluorine atoms. Now you can be the first in your class to point out that there really isn't any sp3d2 hybridization at all.
What are electron regions called?
around the nucleous
How many electrons are needed in the outer energy levels for the atom to be stable?
Stability isn't determined by the first energy level. The only atom with less than two is hydrogen. It is a very stable atom...reactive in that it will attach to anything, but it will always be hydrogen. The atoms that readily decay (the radioactive ones) all have full first orbitals.
