SPDF orbitals Explained - 4 Quantum Numbers, Electron Configuration, & Orbital Diagrams

The Organic Chemistry Tutor
27 Oct 201512:01
EducationalLearning
32 Likes 10 Comments

TLDRThis video discusses the sublevels of atomic orbitals, explaining the shapes and electron capacities of s, p, d, and f orbitals. It covers quantum numbers n, l, ml, and ms, and how they determine electron configurations. Examples include identifying quantum numbers for specific electrons and writing electron configurations for elements like phosphorus, illustrating the process with orbital diagrams.

Takeaways
  • 🌐 The shape of atomic orbitals is crucial for understanding electron behavior: S orbitals are spherical, P orbitals resemble dumbbells, D orbitals are like clover leaves, and F orbitals have complex shapes.
  • πŸ”’ The number of sublevels in an energy level (n) is equal to the principal quantum number (n). For example, n=1 has 1 sublevel (1s), n=2 has 2 sublevels (2s, 2p), and so on.
  • πŸš€ The S sublevel can hold up to two electrons, and each orbital can hold up to two electrons. This is a fundamental principle in understanding electron capacity in orbitals.
  • πŸ“š The P block in the periodic table corresponds to groups 13 to 18 and can hold up to six electrons, with three orbitals.
  • πŸ”¨ The D block, starting with elements like zinc and copper, can hold up to 10 electrons with five orbitals, as seen in the 3d sublevel.
  • 🌟 The F block can hold up to 14 electrons with seven orbitals, illustrating the complexity of higher energy levels.
  • πŸ“ˆ Quantum numbers (n, l, ml, ms) are essential for identifying electron states. n represents the principal energy level, l the sublevel (s, p, d, f), ml specifies the orbital, and ms represents electron spin.
  • πŸ” Electron configurations can be determined by filling orbitals according to the Aufbau principle, which states that electrons fill orbitals of lowest energy first.
  • πŸ“‰ Hund's rule dictates that electrons fill degenerate orbitals one at a time with parallel spins before pairing up, ensuring maximum total spin.
  • 🧩 Pauli's exclusion principle states that no two electrons can have the same set of four quantum numbers, ensuring each electron has a unique identity in an atom.
  • πŸ“š Writing electron configurations and orbital notations involves starting with the lowest energy level and filling orbitals in order, reflecting the actual electron distribution in an atom.
Q & A
  • What is the shape of the s sublevel?

    -The s sublevel has a spherical shape.

  • How many orbitals does the p sublevel have?

    -The p sublevel has three orbitals.

  • What is the maximum number of electrons that the d sublevel can hold?

    -The d sublevel can hold up to 10 electrons.

  • What is the relationship between the principal energy level (n) and the number of sublevels?

    -The number of sublevels is equal to the principal energy level (n). For example, when n is 3, there are 3 sublevels: 3s, 3p, and 3d.

  • How are the orbitals of the s, p, d, and f sublevels designated in terms of quantum numbers?

    -For the s sublevel, L = 0; for the p sublevel, L = 1; for the d sublevel, L = 2; and for the f sublevel, L = 3.

  • What is the value of ml for a p sublevel, and what does it represent?

    -The value of ml for a p sublevel varies between -1, 0, and 1. It represents the orientation of the orbital within the sublevel.

  • Explain the Pauli exclusion principle in the context of quantum numbers.

    -The Pauli exclusion principle states that no two electrons can have the same set of four quantum numbers. Each electron in an atom has a unique combination of n, L, ml, and ms.

  • What is the electron configuration for phosphorus, and how many s electrons does it have?

    -The electron configuration for phosphorus is 1s2 2s2 2p6 3s2 3p3. Phosphorus has 6 s electrons.

  • How are electrons added to degenerate orbitals according to Hund's rule?

    -According to Hund's rule, electrons are added one at a time to degenerate orbitals (orbitals with the same energy) until all are half-filled before pairing up.

  • Describe the process of identifying the four quantum numbers for a given electron, using the example of the 3p5 electron.

    -For the 3p5 electron, n is 3 (the principal energy level), L is 1 (since it's a p sublevel), ml varies between -1, 0, and 1 (the fifth electron is in the ml = 0 orbital), and ms is -1/2 (because the fifth electron is spin-down).

Outlines
00:00
🌐 Understanding Atomic Orbitals and Quantum Numbers

This paragraph introduces the basic concepts of atomic orbitals, specifically focusing on the shapes and characteristics of s, p, d, and f orbitals. It explains that the number of sublevels (s, p, d, f) corresponds to the principal quantum number (n), with s holding up to two electrons, p holding up to six, d holding up to ten, and f holding up to fourteen. The paragraph also delves into the quantum numbers n, l, ml, and ms, which are crucial for identifying the specific state of an electron within an atom. Examples are given to illustrate how to determine these quantum numbers for different electron configurations, such as 3p5 and 4d4. The importance of the Pauli Exclusion Principle is highlighted, which states that no two electrons can have the same set of four quantum numbers.

05:03
πŸ”¬ Electron Configuration and Orbital Notation

This paragraph continues the discussion on atomic orbitals by focusing on electron configuration and orbital notation. It uses the example of phosphorus, which has 15 electrons, to demonstrate how to write the electron configuration and orbital notation. The explanation covers the filling of orbitals according to the Aufbau Principle and Hund's Rule, emphasizing the importance of filling orbitals in order of increasing energy and ensuring that electrons in degenerate orbitals are filled one at a time. The paragraph concludes with a step-by-step guide on how to fill the orbital diagram for an element, starting with the lowest energy level and moving upwards.

10:04
πŸ“š Applying Electron Configuration to Phosphorus

In this paragraph, the focus shifts to applying the principles of electron configuration to the specific case of phosphorus. The video script explains how to determine the electron configuration for phosphorus, which has 15 electrons, by adding up the electrons in each sublevel (1s, 2s, 2p, 3s, 3p) until the total reaches 15. The paragraph also discusses how to answer questions related to the number of electrons in specific orbitals, such as the number of s or p electrons in phosphorus. The video concludes by reviewing the electron configuration for phosphorus and the orbital notation, reinforcing the understanding of how electrons are arranged in the atomic orbitals of an element.

Mindmap
Filling Order
3s and 3p Orbitals
2s and 2p Orbitals
1s Orbital
Example: Phosphorus
Hund's Rule
Aufbau Principle
Pauli Exclusion Principle
Ms (Spin Quantum Number)
ml (Magnetic Quantum Number)
l (Azimuthal Quantum Number)
n (Principal Quantum Number)
F Sublevel
D Sublevel
P Sublevel
S Sublevel
Orbital Notation
Electron Configuration
Quantum Numbers
Sublevels and Shapes
Quantum Numbers and Electron Configurations
Alert
Keywords
πŸ’‘SP PDF
SP PDF refers to the sublevels in atomic orbitals, specifically the s, p, d, and f sublevels. These sublevels are crucial in understanding the arrangement and behavior of electrons in an atom. In the video, the shapes and electron capacities of these sublevels are discussed, such as the spherical shape of s, the dumbbell shape of p, the clover leaf shape of d, and the complex shape of f. The video emphasizes the importance of these sublevels in determining the electron configuration of elements.
πŸ’‘Spherical shape
The term 'spherical shape' describes the geometry of the s sublevel in atomic orbitals. It is characterized by a single orbital that is symmetrical in all directions, resembling a sphere. This shape allows the s sublevel to hold up to two electrons. In the video, the s sublevel's spherical shape is contrasted with the other sublevels, highlighting its unique electron capacity and spatial arrangement.
πŸ’‘Dumbbell shape
The 'dumbbell shape' is used to describe the p sublevel in atomic orbitals. This shape is characterized by two lobes connected by a waist, resembling a dumbbell. The p sublevel can hold up to six electrons and has three orbitals. In the video, the dumbbell shape is mentioned to illustrate the spatial arrangement of electrons in the p sublevel, which is essential for understanding electron configurations.
πŸ’‘Clover leaf
The 'clover leaf' shape is an analogy used to describe the d sublevel in atomic orbitals. This shape is more complex than the s and p sublevels, with five orbitals that can hold up to ten electrons. The video script uses this analogy to help viewers visualize the spatial arrangement of electrons in the d sublevel, which is crucial for understanding the electron configurations of elements in the d-block of the periodic table.
πŸ’‘Unusual shape
The term 'unusual shape' is used in the video to describe the f sublevel in atomic orbitals. Unlike the more regular shapes of s, p, and d sublevels, the f sublevel has a more complex and varied shape. It has seven orbitals and can hold up to fourteen electrons. The video script mentions this unusual shape to emphasize the complexity of the f sublevel and its role in electron configurations, particularly in the f-block of the periodic table.
πŸ’‘Principal energy level
The 'principal energy level', denoted by the quantum number n, refers to the main energy levels in an atom. These levels are associated with the sublevels s, p, d, and f. In the video, the number of sublevels is shown to be equal to the principal energy level number (e.g., n=1 has one sublevel, n=2 has two sublevels). This concept is fundamental to understanding the electron configuration and the arrangement of electrons in atoms.
πŸ’‘Orbital
An 'orbital' is a region in an atom where an electron is most likely to be found. Each sublevel (s, p, d, f) has a specific number of orbitals, and each orbital can hold up to two electrons. The video script discusses the number of orbitals in each sublevel and how they relate to the electron capacity of that sublevel. Understanding orbitals is key to grasping how electrons are distributed in an atom.
πŸ’‘Quantum numbers
Quantum numbers are numerical values that describe the state of an electron in an atom. The video script mentions four quantum numbers: n (principal quantum number), l (azimuthal quantum number), ml (magnetic quantum number), and Ms (spin quantum number). These numbers are essential for identifying the specific location and behavior of an electron in an atom's orbital. The video provides examples of how these quantum numbers are used to describe specific electrons in different orbitals.
πŸ’‘Pauli's Exclusion Principle
Pauli's Exclusion Principle states that no two electrons in an atom can have the same set of four quantum numbers. This principle is crucial for understanding the electron configuration in atoms, as it dictates how electrons fill orbitals. The video script explains that each electron has a unique set of quantum numbers, ensuring that no two electrons occupy the same orbital in the same sublevel.
πŸ’‘Electron configuration
An 'electron configuration' describes the distribution of electrons in an atom's orbitals. The video script discusses how to write electron configurations for elements based on their atomic number and the capacities of the s, p, d, and f sublevels. For example, the electron configuration for phosphorus is given as 1s2 2s2 2p6 3s2 3p3, illustrating how electrons fill the available orbitals in increasing order of energy.
πŸ’‘Orbital notation
Orbital notation is a graphical representation of the electron distribution in an atom's orbitals. The video script explains how to create an orbital diagram for an element, starting with the lowest energy level and filling orbitals according to Hund's rule and the Aufbau principle. This notation helps visualize the electron configuration and understand the spatial arrangement of electrons in an atom.
Highlights

The s orbital has a spherical shape, similar to a sphere.

The p orbital has a dumbbell shape and can be drawn in two ways.

The d orbital resembles a clover leaf.

The f orbital has an unusual shape that varies.

The number of energy levels is equal to the number of sublevels.

When n is one, there is only one sublevel (s).

When n is two, there are two sublevels (s and p).

When n is three, there are three sublevels (s, p, and d).

When n is four, there are four sublevels (s, p, d, and f).

The s sublevel can hold up to two electrons.

Each orbital can hold up to two electrons.

The p block in the periodic table corresponds to groups 13 to 18.

The d block starts with elements like zinc, copper, and nickel.

The d sublevel can hold up to 10 electrons and has five orbitals.

The f sublevel can hold up to 14 electrons and has seven orbitals.

The s sublevel corresponds to l=0, p to l=1, d to l=2, and f to l=3.

Four quantum numbers (n, l, ml, ms) are essential for identifying electron configurations.

The Pauli Exclusion Principle states that no two electrons can have the same set of four quantum numbers.

Electron configuration for phosphorus is 1s2 2s2 2p6 3s2 3p3.

Orbital notation and electron filling follow the Aufbau principle and Hund's rule.

Transcripts
00:00

in this video we're going to talk about

00:02

um the SP PDF

00:05

sublevels um what you need to know is

00:07

that s has a spherical shape it's like a

00:10

sphere P has a dumbbell shape it can be

00:13

drawn both ways D is like a clover leaf

00:17

and F has some unusual shape which

00:20

varies and I really don't want to go

00:23

over

00:24

that but some things you need to know

00:26

the number of ngery levels is equal to

00:28

the number of su levels so when n is one

00:31

you only have one subl s when n is two

00:35

you have two sublevels s n p when n is

00:39

three you have three Su levels 3 S 3 p

00:43

3D when n is four there are four

00:46

sublevels 4 S 4 p 4 d and 4f the S

00:53

subl can hold up to two

00:57

electrons and you need to know that

00:59

every or orbital um can hold up to two

01:02

electrons so s has uh one

01:05

orbital now in a periodic

01:08

table the S block is really the first

01:10

two columns group one and group two so

01:13

that's the S

01:15

block P can hold up to six electrons if

01:19

you notice the P Block in the periodic

01:21

table it's like Group 13 to group 18 you

01:24

can see those six elements there P can

01:26

hold up to six electrons and because

01:28

every orbital can hold up to two two

01:30

electrons uh P has three

01:33

orbitals D can hold up to 10

01:36

electrons the elements in the D Block

01:39

starting with like

01:41

um you have like zinc copper nickel

01:44

those are in the 3D suev and if you look

01:47

at the periodic table there's 10

01:49

elements there D can hold up to 10

01:51

electrons and so the D suble has five

01:57

orbitals F can hold up to 14 electrons

02:01

and F has seven orbitals 1 2 3 4 5 6

02:05

7 so those are some things you want to

02:07

keep in mind by the way whenever you

02:10

have the S Sub L is equal to zero for

02:13

the P sub L is equal to one for d l is

02:17

equal to 2 and for f l is equal to

02:28

3 so you need to be familiar with these

02:31

four quantum numbers n l ML and Ms we

02:36

talked about n already this is the main

02:38

principal energy level L represents the

02:42

Su which is associated with s p d and

02:46

f ml repres it specifies the

02:52

orbital s has one orbital and it has a

02:55

value of zero P has three orbitals and

02:58

it has a value of 1 0 and 1 D has five

03:03

orbitals which varies between -2 and two

03:07

we're going to talk about that soon Ms

03:09

represents the electron spin inside an

03:11

orbital you can have an up Arrow which

03:14

stands for Plus one2 or you can have a

03:17

down arrow which has an electron spin of

03:20

negative a

03:26

half so let's talk about how to identify

03:28

these quantum numbers let's say if you

03:30

want to identify the four quantum

03:33

numbers for the 3p5

03:35

electron and it's going to be this

03:37

number n is

03:38

three now P will tell you what the value

03:42

of L is keep in mind for S L is zero for

03:45

p l is one for d l is two for f l is

03:49

three now P has uh three orbitals as we

03:53

talked about and because L is one ml is

03:57

going to vary between NE 1 Z and

04:01

one now we want to we're focused on the

04:04

fifth electron so here's the first

04:07

electron second third fourth fifth the

04:10

fifth electron lands in this orbital

04:13

where ml is zero so therefore ml is Zer

04:16

Ms is negative a half because the fifth

04:18

Arrow points down you always start by

04:21

drawing the arrows up and then down so

04:23

those are the four quantum numbers that

04:25

corresponds to the 3p5

04:27

electron let's try two more examples

04:32

let's try 4

04:35

D4 n is

04:37

4 and for d l is two because for S L is

04:41

zero for p l is one and for f l is three

04:45

now the d sub Lev has five

04:47

orbitals and so ml can vary between -2 1

04:52

0 1 and two because L is

04:55

two so here's the first Arrow second

04:57

third fourth we're interested in in the

04:59

fourth arrow and it landed on the

05:03

orbital that has a value of one and

05:06

because it's an up Arrow the spin is

05:09

positive2 all right for the sake of

05:11

practice let's try one more example

05:13

let's focus on the 5f 13 electron so n

05:18

is

05:19

five L is zero for S L is one for p l is

05:23

2 for d for f l is

05:26

three and for the F suble there are

05:29

seven

05:31

orbitals

05:33

and ml can vary between -3 and 3 because

05:38

l

05:40

is3 so we're interested in the 13th

05:42

electron 1 2 3 4 5 6 7 8 9 10 11 12 13

05:50

there it is and it landed in this

05:52

orbital so MLS

05:53

2 and it's a down arrow so the electron

05:56

spin is negative half so that's how you

05:58

could find the four quantum numbers uh

06:01

given the

06:04

electron now Paul's exclusion principle

06:08

states that no two electrons can have

06:10

the same set of four quantum numbers as

06:13

you can see these quantum numbers are

06:15

unique for each electron this one

06:18

electron has its a unique set of four

06:20

quantum numbers so if you're given these

06:23

four quantum numbers you can identify

06:25

What electron we're talking about let's

06:27

try that so let's say for example

06:29

example if uh n is 3 l is 2 ml is 1 and

06:37

Ms is negative a half What electron are

06:40

we talking about what which electron is

06:43

identified by these four um unique

06:46

quantum

06:49

numbers so we know we're in the third

06:51

enery

06:52

level when L is zero It's s when L is

06:55

one it's p when L is 2 it's D so we're

06:58

in the 3D suev D has five

07:02

orbitals and because L is 2 it varies

07:06

between -2 and 2 excuse

07:09

me now we know that the electron is in

07:12

this orbital because ml is one and we

07:16

know the arrow has to be a down arrow so

07:18

let's count it 1 2 3 start with the up

07:21

arrows four five 6 7 8 9 there's our

07:26

down arrow so these four quantum numbers

07:29

Cor Corr responds to the 3d9

07:32

electron now let's talk about electron

07:35

configuration and orbital notations and

07:38

so forth let's say if you want to write

07:42

the electron configuration

07:45

for let's go with uh

07:50

phosphorus now if I remember correctly I

07:52

believe phosphorus has 15

07:55

electrons let me just take a minute and

07:58

verify that with periodic table and yeah

08:01

that's

08:05

correct now the first energy level only

08:08

has one suel the second NG level has two

08:11

sublevels the third NG level has three

08:14

Su levels so 3s3 p3d the fourth NG level

08:18

has four Su

08:21

levels so let's say if you want to write

08:23

the electron configuration for

08:25

phosphorus the configuration the

08:28

exponents has to add up to this atomic

08:30

number now keep in mind s can hold up to

08:33

two electrons P can hold up to six D can

08:36

have up to 10 F can have up to 14 and

08:38

we're going to write it until the

08:39

exponents add up to

08:41

15 so let's begin so One S can hold up

08:45

to two electrons 2s can also hold up to

08:48

two 2p can hold up to six

08:52

electrons and 3 S can hold up to two so

08:56

right now we have 2 + 2 which is 4 + 6

08:59

which is 10 10 + 2 12 we only need three

09:01

more 3p can hold up to six but because

09:04

we only need three more we're going to

09:05

stop at 3p3 this is the electron

09:08

configuration for

09:10

phosphorus now let's say if you're given

09:12

a question and they ask you how many s

09:14

electrons are in phosphorus after you

09:17

write the configuration you can answer

09:19

the question so there are six s

09:21

electrons in phosphorus because if you

09:23

add up the exponents you get six if they

09:25

ask you hey how many P electrons are on

09:28

phosphorus simply add the P electrons 6

09:31

+ 3 there are n p electrons in

09:36

phosphorus now let's refresh the page

09:39

but let's keep the information that we

09:40

have so we said the electron

09:42

configuration for phosphorus is 1 S2 2

09:45

S2 2 P6 3 S2 and 3 P3 but now let's

09:51

write the orbital notation um for

09:54

phosphorus or the orbital

09:57

diagram so this is the 1s orbital s has

10:00

only one orbital here we have 2 s 3s

10:04

notice I keep it in the same column then

10:06

to the right of that just above 2s we

10:09

have 2p which has three orbitals and

10:15

3p now as you go up the potential energy

10:18

increases now according to offb

10:21

principle um you need to add the

10:23

electrons in increase in order which

10:26

means you start from the lowest energy

10:28

level and then you go up to the the

10:29

highest energy level so we have to start

10:31

with 1s we put the first electron here

10:34

we don't put the next one in 2s you have

10:36

to put the next one in ons you have to

10:38

go in order that's off boss principle

10:41

2s2 is filled now according to Hun's

10:44

rule whenever you're filling electrons

10:47

in degenerate orbitals you have to fill

10:49

them one at a time the word degenerate

10:51

means that the energy is equal so these

10:55

three orbitals have equal energy because

10:57

they're at the same height so therefore

11:00

they are degenerate

11:01

orbitals because they have the same

11:04

energy so whenever you're adding

11:06

electrons here you add it one at a time

11:08

according to hun rule so 1 2 3 4 five

11:12

six 2p6 is filled so next according to

11:16

off boss principle we move into 3s not

11:19

3p because we have to go in order of

11:21

increase in energy or increase in

11:23

potential energy so 3s2 and then based

11:27

on Hun's rule for degenerate orbitals

11:30

which are energy levels at the which are

11:32

orbitals that have the same energy we

11:35

have to fill these um orbitals one at a

11:37

time so 1 2 3 that's how you fill the

11:40

orbital diagram for an element write the

11:43

electron configuration

11:45

first then put the arrows in so that's

11:48

it for this video um I think we covered

11:51

a lot and uh I have other videos on

11:54

quantum numbers so feel free to search

11:55

YouTube for those and uh so that's all I

11:58

got for today that's my two cents and