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What sublevel in group 2 elements are valence electrons?
s
Which has 2 electron in the 4s sublevel?
Ca
How many electrons can 4s orbital hold?
4
Which elements have 2 electrons in their s sublevel?
If you're talking about any s sublevel at all, then any element except hydrogen would fit that. If you're talking specifically about elements that have the s orbital as their valence (outermost) orbital, and also have that valence s orbital filled with 2 electrons, then helium and anything in the second column of the periodic table will all fit that description. (He, Be, Mg, Ca, Sr, Ba, Ra)
Why 4s has one electron and 3d has 5 electrons?
The electronic configuration of atoms is based on the filling of orbitals. In the case of the 4s orbital, it is relatively lower in energy than the 3d orbital, so it is filled first. Therefore, the 4s orbital can accommodate a maximum of 2 electrons. As for the 3d orbitals, they have a higher energy level and can accommodate a maximum of 10 electrons, but in the case of transition metals, only 5 electrons fill the 3d orbitals due to electron configuration stability.
Which elements have 2 electrons in the 4s sublevel?
Ca
What element has 2 electrons in the 4s sublevel?
Ca
Which element has 2 electrons in the 4s sublevel?
Ca
What element have 2 electrons in the 4s sublevel?
Ca
What sublevel in group 2 elements are valence electrons?
s
All of the elements in period 3 have a total of 2 electrons in the?
2s Sublevel
Which has 2 electron in the 4s sublevel?
Ca
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
What elements has 2 electrons in the 4s sub level?
K
How many electrons are found in each sublevel?
Multiply the orbitals in that sublevel by 2. The s sublevel has one orbital and can contain 2 electrons. The p sublevel has three orbitals and can contain 6 electrons. The d sublevel has five orbitals and can contain 10 electrons. The f sublevel has seven orbitals and can contain 14 electrons.
Why can a p sublevel hold 6 electrons while the s sublevel can hold no more than 2 electrons?
because sublevel p has 3 orbital and each orbital can hold up to 2 electrons meanwhile sublevel s only has 1 orbital and each can hold 2 electrons therefore sublevel p can hold more
How many electrons are in the g sublevel?
There are 9 orbitals in a g sublevel. (there is 1 in an s sublevel, 3 in a p sublevel, 5 in a d sublevel, 7 in an f sublevel, 9 in a g sublevel, 11 in an h sublevel, etc.)
