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What is the value of n for the valence shells of as?
The value of n for the valence shell of arsenic (As) is 4. This means that the outermost shell of arsenic contains electrons in the fourth energy level.
What is the lowest value of 'n' that allows 'g' orbital to exist?
The lowest value of 'n' that allows a 'g' orbital to exist is 4. 'g' orbitals are part of the f sublevel, which corresponds to the fourth energy level (n=4).
What does the energy of each level n depend on?
The energy of each level n in an atom depends on the principal quantum number n. The energy increases as the value of n increases. This is due to the relationship between the distance of the electron from the nucleus and its energy.
What are the maxium number of orbitals in p sublevel?
3, each of which can hold 1 or 2 electrons. Please note that many chemists would say that there were always 3 p orbitals in the p sublevels, they may, however not all be occupied by electrons.
How many sub levels are in each energy level?
2
When did N-Sub happen?
N-Sub happened in 1000.
When was N-Sub created?
N-Sub was created in 1980-12.
Which quantum number is also called sub-shell quantum number?
The azimuthal quantum number (l) is also known as the sub-shell quantum number. It represents the sub-shell of an electron within a given energy level. The value of l determines the shape of the orbital (s, p, d, f).
Does a higher value of n mean a higher or lower energy?
A higher value of n corresponds to a higher energy level in an atom. In the context of the Bohr model of the atom, n represents the principal quantum number, which indicates the energy level of an electron in an atom.
How do you write a recursive Formula?
3,6,9,12 A sub 1 = First (3) a sub n = a sub (n-1) + change (3)
What is the number of the lowest energy level that contains an f sublevel?
The lowest energy level that contains an f sublevel is the fourth energy level (n=4).
What is the maximum of the orbitals in the p sublevel?
in a "s" sublevel there are a max of 2 electrons located on 1 orbital. in a "p" sub level there are a max of 6 electrons located on 3 orbitals. in a "d" sub level there are a max of 10 electrons located on 5 orbitals. Extra: within a level (n=2 or n=3 etc) the number of orbitals (adding all the s, p, d etc) is n^2. so in a n=2 level, there are 4 orbitals (1 for 2s, 3 for 2p..1+3=4)
What is the value of n for the valence shells of as?
The value of n for the valence shell of arsenic (As) is 4. This means that the outermost shell of arsenic contains electrons in the fourth energy level.
Why is 2d1 not possible?
A break down of 2d1:2 = the quantum energy level or electron shell denoted as 'n'd = the sub-shell of the energy level (known as a degenerate level)1 = the number of electrons occupying the sub-shell.Through extensive research by scientists, no known element has a d sub-shell in the second (n=2) energy level. In fact, the d sub-shell does not appear until the fourth period (fourth row).The first d sub-shell is known to be in the third energy level (therefore the first energy level with this sub-shell is 3d, but not 2d).Transition metals are the elements known to fill the d sub-shells. The first transition metal in the periodic table is scandium (Sc) with the electron configuration of [Ar]4s23d1.The reasons for the formation of sub-shell of d is beyond my knowledge and the scope of basic chemistry.
What element has 3 electrons and P sub level?
These would be p block elements in group 5 (XV)N, P, As, Sb, Bi
What is the lowest value of 'n' that allows 'g' orbital to exist?
The lowest value of 'n' that allows a 'g' orbital to exist is 4. 'g' orbitals are part of the f sublevel, which corresponds to the fourth energy level (n=4).
Write a program to find prime number in vb net?
Private Sub Command1_Click() Dim I, N As Integer N = Val(Text1.Text) For I = 2 To N - 1 If N Mod I = 0 Then Print "THE NUMBER IS NOT A PRIME NUMBER" Exit Sub End If Next I Print "THE NUMBER IS A PRIME NUMBER" End Sub Private Sub Command2_Click() Text1.Text = "" Text1.SetFocus End Sub Private Sub Command3_Click() End End Sub
