### s, p, d, f

Posted:

**Sun Apr 29, 2018 10:42 pm**What is the different between the orbitals?

Created by Dr. Laurence Lavelle

https://lavelle.chem.ucla.edu/forum/

https://lavelle.chem.ucla.edu/forum/viewtopic.php?f=25&t=31212

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Posted: **Sun Apr 29, 2018 10:42 pm**

What is the different between the orbitals?

Posted: **Sun Apr 29, 2018 10:46 pm**

Each orbital in a su shell has a different shape characterized by a different letter (s, p, d,f). They have electrons with different angular momentums so this sets them apart from each other.

Posted: **Sun Apr 29, 2018 11:11 pm**

Also, different orbitals are different sizes and shapes

Posted: **Sun Apr 29, 2018 11:13 pm**

What type of midterm questions/practice problems are possible for s, p, d, f?

Posted: **Sun Apr 29, 2018 11:24 pm**

I would guess that a possible problem could be giving you something like ā4dā and asking you to write out or choose the correct possible four quantum numbers (n, l, ml, and ms) that 4d could have

Posted: **Mon Apr 30, 2018 1:08 pm**

I find this to be a helpful visual:

This is a depiction of the second shell (n=2), in which there are two possible sub-shells (s and p). The s sub-shell has one orbital, which is spherical and holds a maximum of two electrons (which must have opposite spin values). The p sub-shell has 3 orbitals, which can each hold a maximum of two electrons each with opposite spin (for a total of 6 possible electrons in the p sub shell). The s sub-shell will fill first, then the p sub-shell.

In higher shells, there will be more possible sub shells and more possible orbitals. There are 5 d orbitals and therefore they can hold a total of 10 electrons, and there are 7 f orbitals meaning they can hold a total of 14 electrons.

Here is the source:

https://hackaday.com/2015/09/16/dont-kn ... c-table-2/

(Will Sweatman, 2016)

This is a depiction of the second shell (n=2), in which there are two possible sub-shells (s and p). The s sub-shell has one orbital, which is spherical and holds a maximum of two electrons (which must have opposite spin values). The p sub-shell has 3 orbitals, which can each hold a maximum of two electrons each with opposite spin (for a total of 6 possible electrons in the p sub shell). The s sub-shell will fill first, then the p sub-shell.

In higher shells, there will be more possible sub shells and more possible orbitals. There are 5 d orbitals and therefore they can hold a total of 10 electrons, and there are 7 f orbitals meaning they can hold a total of 14 electrons.

Here is the source:

https://hackaday.com/2015/09/16/dont-kn ... c-table-2/

(Will Sweatman, 2016)

Posted: **Wed May 02, 2018 7:47 pm**

Taizha 1C wrote:What type of midterm questions/practice problems are possible for s, p, d, f?

there was a homework problem where it asked us to draw it out, so we might be asked to differentiate the different orbitals (s, p, d, f)

Posted: **Fri Oct 19, 2018 4:04 am**

The difference between the orbitals of s,p,d, and f is the shape of the orbital. Within these orbitals are subshells and s=1, p=3, d=5, and f=7.

Posted: **Fri Oct 19, 2018 8:29 am**

Another distinction between the orbitals is the number of nodal planes. For examples, the s orbital has none, the p orbitals have one, the d orbitals have two, and the f orbitals have three.

Posted: **Fri Oct 19, 2018 12:04 pm**

Would it be correct to say that 4d could have n=4, l=2, ml=-1, and ms=+1/2? and if so, would it be correct to assume that each possible configuration of quantum numbers for 4d represents an electron, giving the total number of electrons in that shell?

Posted: **Fri Oct 19, 2018 1:16 pm**

505168807 wrote:Would it be correct to say that 4d could have n=4, l=2, ml=-1, and ms=+1/2? and if so, would it be correct to assume that each possible configuration of quantum numbers for 4d represents an electron, giving the total number of electrons in that shell?

You are correct that 4d could have those quantum numbers, however, if it doesn't specify otherwise and you are describing the quantum numbers of a 4d orbital, you would say n=4, l= 2, ml=-2,-1,0,1,2, and ms=+1/2 or -1/2, in which n, l, and ml give information on the orbital itself and ms signifies which electron it is referring to.

Posted: **Fri Oct 19, 2018 9:28 pm**

Orbitals are the regions of space in which electrons are most likely to be found. Each orbital is denoted by a number and a letter in which the letters (s,p,d,f), describe the shape of the orbital. An s orbital, the first energy level, is spherical and has no nodal planes. A p orbital has two lobes on either side of the nucleus and there is a nodal plane with zero probability of e- density. A d plane has 4 lobes of e- density located in xy-yz-zx planes, and there are a total of 5 orbitals. The shape of the f orbital is a little bit more complicated but still has a nodal plane.

Posted: **Sat Oct 20, 2018 3:44 pm**

The orbitals s, p, d, f have different shapes and sizes

Posted: **Sat Oct 20, 2018 3:49 pm**

The orbitals s,p,d, f have different sizes and shapes.

- s is spherical shape with 1 orbital

-p has 2 lobes on either side of nucleus with 3 orbitals

-d has 4 lobes of e- located on XY-ZX planes with 5 orbitals

f has more complicated shapes with 7 orbitals

- s is spherical shape with 1 orbital

-p has 2 lobes on either side of nucleus with 3 orbitals

-d has 4 lobes of e- located on XY-ZX planes with 5 orbitals

f has more complicated shapes with 7 orbitals

Posted: **Sat Oct 20, 2018 3:54 pm**

On Test 2, would we be required to draw the different types of orbitals or identify various diagrams of orbitals?

Posted: **Sun Oct 21, 2018 1:08 am**

If i remember correctly, Lavelle stated that he would not make us draw the different orbitals. But I would memmorize the number of lobes and planes they do have as S is spherical and does not have a nodal plane. P orbitals have 2 lobes on either side and a nodal plane. D has 44 lobes and etc.

Posted: **Mon Oct 22, 2018 9:42 am**

For test 2, do we need to know how to find the quantum numbers of an electron? How do you do that?