to morgan!!!

ikaw na lay pili sa parts nga imong i visualize...

ako na lang atong last 2 parts ....malouy ko nimo!!! T.T hehehe

The energy sequence of the first 24 subshells is given in the following table. Each cell represents a subshell with n and given by its row and column indices, respectively. The number in the cell is the subshell's position in the sequence. Empty cells represent sublevels that do not exist.

	s	p	d	f	g
1	1
2	2	3
3	4	5	7
4	6	8	10	13
5	9	11	14	17	21
6	12	15	18	22	26
7	16	19	23	27	31 morgan table ni!! important part!
8	20	24	28	32	36

3rd

Orbitals and orbits

When the a planet moves around the sun, you can plot a definite path for it which is called an orbit. A simple view of the atom looks similar and you may have pictured the electrons as orbiting around the nucleus. The truth is different, and electrons in fact inhabit regions of space known as orbitals.

Orbits and orbitals sound similar, but they have quite different meanings. It is essential that you understand the difference between them.

mao ni and 2nd!

d and f orbitals

In addition to s and p orbitals, there are two other sets of orbitals which become available for electrons to inhabit at higher energy levels. At the third level, there is a set of five d orbitals (with complicated shapes and names) as well as the 3s and 3p orbitals (3p_x, 3p_y, 3p_z). At the third level there are a total of nine orbitals altogether.

At the fourth level, as well the 4s and 4p and 4d orbitals there are an additional seven f orbitals - 16 orbitals in all. s, p, d and f orbitals are then available at all higher energy levels as well.

For the moment, you need to be aware that there are sets of five d orbitals at levels from the third level upwards

morgan mao ni ang 1st!

Visualization of Atomic Orbitals

d Orbitals

As the value of the angular momentum quantum number increases, the number of values of m increases (there are 2 l + 1 values of m) and the complexity of the orbital geometry increases. The d orbitals all possess l = 2. For this value of l, the magnetic quantum number may have values of m = -2, -1, 0, +1, and +2. Only orbitals with m = 0 are real; all other values of m give rise to complex wave functions. As is the case with p orbitals, chemists combine the m = -1 and +1 wave functions (which are complex) to obtain two new functions that are both real. Similarly, the wave functions with m = -2 and +2 are also combined to yield two new real wave functions.

The d orbital with m = 0 is designated z². The two orbitals created from the m = -1 and +1 orbitals are designated xz and yz. The two orbitals created from the m = -2 and +2 orbitals are designated xy and x²-y². These designations arise from the mathematical formulas for the wave functions and indicate the orientation of the orbital.