How to Write the Electron Configuration for an Element in Each Block

Summary

In this educational video, Melissa Maribel guides viewers through understanding electron configurations for various elements. She explains the significance of subshells (s, p, d, and f) and their capacities, and how they are represented in the periodic table. Melissa demonstrates step-by-step electron configuration for elements in different blocks (s, p, d, and f), including beryllium, sulfur, iron, and plutonium. She also teaches how to write condensed electron configurations using noble gases as placeholders. The video concludes with resources for further learning and a practice quiz to reinforce the concepts.

Takeaways

• 🔬 Electron configuration is essential for understanding how electrons are arranged in atomic orbitals.
• 📚 There are four subshells: s, p, d, and f, each with different capacities for electrons (2, 6, 10, and 14 respectively).
• 📖 The periodic table is divided into blocks (s, p, d, f) based on the subshells where the last electron enters.
• 👩‍🏫 Melissa Maribel provides a step-by-step guide to writing electron configurations for elements in different blocks.
• 🌐 The electron configuration process starts from hydrogen and moves across the periodic table to the element of interest.
• 💡 For s-block elements, the configuration fills the s subshells first, as demonstrated with beryllium.
• 🔑 The p-block configuration, exemplified by sulfur, includes filling p subshells after the s subshells are complete.
• 🌟 Abbreviated electron configurations use noble gases as placeholders, simplifying the notation.
• 🧲 The d-block configuration, shown with iron, starts filling d subshells after the s and p subshells are filled.
• 🔋 The f-block configuration, illustrated with plutonium, is complex and involves filling f subshells after others, using noble gas placeholders.
• 📚 Melissa offers additional resources, including online tutoring and practice quizzes, to help students master electron configurations.

Q & A

What is the purpose of electron configuration?

Electron configuration helps us visualize how electrons are arranged in atomic orbitals for a specific element.

What are the four types of subshells and their capacities?

The four types of subshells are s, p, d, and f. The s subshell has one orbital holding up to two electrons, the p subshell has three orbitals holding up to six electrons, the d subshell has five orbitals holding up to ten electrons, and the f subshell has seven orbitals holding up to fourteen electrons.

How is the periodic table organized in relation to subshells?

The periodic table is organized into blocks based on subshells: s block for the first two groups, p block for the right side, d block for inner transition metals, and f block at the bottom.

What is the significance of the order in electron configuration?

The order in electron configuration is significant as it dictates the sequence in which electrons fill the orbitals, starting from hydrogen and moving left to right across the periodic table.

How do you determine the electron configuration for an element in the s block, like beryllium?

For an s block element like beryllium, you start with hydrogen (1s1) and count electrons moving left to right until you reach beryllium, which has the configuration 1s2 2s2.

Can you explain the process of finding the electron configuration for an element in the p block, such as sulfur?

For sulfur in the p block, you start with hydrogen (1s1), add electrons up to neon (2s2 2p6), then continue across the third row to sulfur with 3s2 3p4.

What is the abbreviated form of electron configuration, and how is it used?

The abbreviated form uses the noble gas configuration from the previous row as a placeholder. For sulfur, it would be [Ne] 3s2 3p4, where [Ne] represents the electron configuration of neon.

How do you find the electron configuration for an element in the d block, like iron?

For iron in the d block, start with hydrogen (1s2), add electrons up to argon (3d10 4s2), and then continue with 3d6 for iron, resulting in the configuration [Ar] 4s2 3d6.

What is the condensed electron configuration for plutonium, an element in the f block?

For plutonium, start with the noble gas radon from the sixth row and continue with 7s2 5f6, which is the condensed configuration.

Why is there a break in the periodic table for the f block elements?

There is a break in the periodic table for the f block elements because they are the last to fill their orbitals and are placed at the bottom of the table to maintain the order of atomic numbers.

What is the importance of using noble gases in condensed electron configurations?

Noble gases are used in condensed electron configurations because they represent a complete set of electrons for the previous row, simplifying the notation and making it easier to visualize the unique electron configuration of the element in question.

Outlines

00:00

🔬 Understanding Electron Configuration

This paragraph introduces the concept of electron configuration, which is essential for visualizing how electrons are arranged in atomic orbitals. Melissa Maribel, the tutor, explains the four types of subshells (s, p, d, and f) and their respective capacities for electrons. The periodic table is referenced as a guide to these subshells, with each block corresponding to a type of subshell. The s block includes the first two groups and helium, the p block is on the opposite side, the d block includes the inner transition metals, and the f block is at the bottom. The paragraph emphasizes the importance of knowing the order of electron configuration and provides examples for elements in each block, including beryllium (s block) and sulfur (p block), detailing the step-by-step process of writing their electron configurations.

05:00

📚 Electron Configuration Examples and Abbreviations

The second paragraph continues with more examples of electron configurations, focusing on the d block with iron and the f block with plutonium. It explains the process of writing full electron configurations by starting from hydrogen and moving through the periodic table to the element of interest. For iron, the configuration includes the 3d subshell, and for plutonium, it includes the 4f subshell. The paragraph also introduces the concept of condensed electron configurations, which use noble gases as placeholders to simplify the notation. Examples are provided for sulfur, iron, and plutonium, showing how to abbreviate their configurations using noble gases like neon, argon, and radon, respectively. The paragraph concludes with an offer of additional resources for homework help and a practice quiz to prepare for exams.

Keywords

💡Electron Configuration

Electron configuration refers to the distribution of electrons in an atom's orbitals. It is a fundamental concept in chemistry that helps predict an element's chemical properties and reactivity. In the video, Melissa Maribel explains how to determine electron configurations for elements in different blocks of the periodic table, using examples like beryllium, sulfur, iron, and plutonium to illustrate the process.

💡Subshells

Subshells are regions within an atom's electron cloud where electrons with similar energies are located. The four types of subshells are s, p, d, and f, each with a distinct number of orbitals and maximum electron capacity. In the script, Melissa describes the s subshell as having one orbital for up to two electrons, the p subshell with three orbitals for up to six electrons, the d subshell with five orbitals for up to ten electrons, and the f subshell with seven orbitals for up to fourteen electrons.

💡Orbitals

Orbitals are the spatial regions around an atomic nucleus where electrons are most likely to be found. They are associated with each subshell and determine the shape and orientation of electron distribution. The video script mentions that the s subshell has one orbital, the p subshell has three, the d subshell has five, and the f subshell has seven orbitals.

💡Periodic Table

The periodic table is a tabular arrangement of elements based on their atomic number, electron configurations, and recurring chemical properties. It is divided into blocks (s, p, d, f) based on the subshell that is being filled with electrons. The script uses the periodic table to guide the viewer through the electron configuration of various elements, emphasizing the importance of understanding the table's structure.

💡s Block

The s block in the periodic table includes elements where the last electron added occupies an s orbital. Melissa uses beryllium as an example in the video to explain how to write the electron configuration for an s block element, starting from hydrogen and moving across the periodic table.

💡p Block

The p block elements are characterized by the filling of p orbitals. The video script provides an example of sulfur, where Melissa explains the electron configuration, including the p orbitals filled with six electrons (2p6), as part of the process to reach sulfur's configuration.

💡d Block

The d block of the periodic table consists of the transition metals, where the d orbitals are being filled. Iron is used as an example in the script to demonstrate the electron configuration for a d block element, detailing the filling of the 3d orbitals.

💡f Block

The f block is located at the bottom of the periodic table and includes the inner transition metals and the lanthanides and actinides. Plutonium is an example used in the script to illustrate the electron configuration for an f block element, highlighting the filling of the 4f orbitals.

💡Condensed Electron Configuration

A condensed electron configuration is a shorthand representation that includes the electron configuration of the nearest noble gas followed by the remaining electrons. This method simplifies the notation and is demonstrated in the video for elements like sulfur, iron, and plutonium, where Melissa shows how to use the noble gas configuration as a starting point.

💡Noble Gases

Noble gases are a group of elements in group 18 of the periodic table, known for their full valence electron shells, making them generally unreactive. In the context of the video, noble gases serve as reference points for writing condensed electron configurations. Melissa uses neon for sulfur, argon for iron, and radon for plutonium to demonstrate this concept.

💡Atomic Orbitals

Atomic orbitals are the mathematical functions that describe the location and behavior of an electron in an atom. The video script discusses how electrons are arranged in orbitals within subshells, with specific capacities for each type (s, p, d, f), which is crucial for understanding electron configurations.

Highlights

Introduction to electron configuration and its importance in understanding atomic orbitals.

Explanation of the four types of subshells: s, p, d, and f, and their respective capacities.

Description of the s subshell's one orbital and its capacity to hold two electrons.

Details on the p subshell's three orbitals and their ability to hold up to six electrons.

Information on the d subshell's five orbitals and their capacity for ten electrons.

Clarification on the f subshell's seven orbitals and their ability to hold fourteen electrons.

Correlation of subshells with the periodic table's blocks and their respective elements.

Guidance on the specific order to follow for electron configuration and its significance.

Example 1: Step-by-step electron configuration for beryllium in the s block.

Example 2: Detailed electron configuration for sulfur in the p block, including the full and abbreviated forms.

Introduction to the abbreviated electron configuration using noble gases as placeholders.

Example 3: Electron configuration for iron in the d block, explaining the coefficient rule.

Example 4: Electron configuration for plutonium in the f block, including the full and condensed forms.

Explanation of the breaks in the periodic table and their relation to the f block.

Final condensed electron configuration for plutonium using radon as the noble gas placeholder.

Offer of additional resources for homework help, online tutoring, and practice quizzes.

Encouragement to stay determined and prepared for exams with the provided study materials.

Transcripts

We'll go over the two different ways to write the electron configuration but

don't worry I'll go over everything step by step. Hello everyone I'm Melissa Maribel

your personal tutor and here's what you really need to know for

electron configuration. Electron configuration helps us see how electrons

are arranged in atomic orbitals for a specific element. There are four types of

sub shells s, p, d and f the s subshell has one orbital that can hold up to two

electrons. The p subshell has three orbitals that can hold up to six

electrons. The d subshell has five orbitals that can hold up to 10

electrons and the f subshell has seven orbitals that can hold up to fourteen

electrons. The periodic table has all four types of subshells on it we refer

to it as a block. These first two groups are our s block and helium is also part of

the s block, on the opposite side is our p block, the inner transition metals are

our d block and finally at the bottom we have our f block.

Make sure you know these, this is the specific order that we follow for

electron configuration and yes the order does matter. Let's do an example of an

element in each block. Example 1: s block to find the electron configuration of

any element we always start from hydrogen and make our way going from

left to right to the element we are trying to find which in this case is

beryllium. So writing our electron configuration since we start with the

first row hydrogen is 1s1, we move on to helium which is 1s2 so we have 1s2.

Next we are on the second row but still in the s block so 2s1,2, 2 s2

and we stop since we reached the element we wanted. This is the electron

configuration of beryllium. Example 2: p block we'll find the electron

configuration of sulfur by starting from hydrogen and making our way to

sulfur. So 1s1, 2, 1 s2 is the first part, come back around on to the

second row 2s1, 2, 2 s2 is the second part, keep going straight across to the p

block, 2p, 1, 2, 3, 4, 5, 6, 2p6 is next, come back around onto the 3rd row to 3s1, 2

so 3s2, keep going straight across to the p block in row 3 and we will count

up until we get to sulfur so 3p, 1, 2, 3, 4, 3p4, this is our full electron

configuration for sulfur. There is an abbreviated, shorthand or condensed

electron configuration that you will need to know how to find. Let's find it

for sulfur, we always use the noble gas that is in the row before the element

we are looking for in this case it's neon and we place the noble gas in

brackets. Think of the noble gas as a placeholder or the new place to start so

we will continue after neon and write the remaining parts of the electron

configuration for sulfur. So 3s2 & 3p4, you know by placing our neon first we

are actually accounting for this entire portion of the full electron

configuration since that portion is the electron configuration of neon. Let's do

another example. Example 3: d block we'll find the electron configuration of iron

by starting from hydrogen and making our way to iron. So 1s2, 2s2,

keep going straight across to 2p6 come back around to 3s2, straight across to

3p6, come back around to the 4th row to 4s2. Now we are in the d

block and the coefficient or number in front is always 1 less than the row it

is in. So instead of 4d this is actually 3d and we will count up until we get to

iron so 3d, 1, 2, 3, 4, 5, 6, 3d6 this is our full electron configuration for iron.

Now let's find the condensed electron configuration using the noble gas in the

previous row which is argon we'll continue from argon to iron. Do 4s2 &

3d6 and this is our condensed electron configuration. Example 4: f block we'll

find the electron configuration of plutonium by starting from hydrogen and

making our way to plutonium so 1s2, 2s2 keep going straight across to 2p6, come

back around to the 3s2, straight across the 3p6, come around to the 4th row

to 4s2, remember the coefficient or number in front is always 1 number less

then the row it is in for the d block so we have 3d10. We're still in the

fourth row so 4p6 come around to the fifth row to 5s2 we're in the d block so

4d10, still in the fifth row to 5p6, come around to the sixth row to 6s2 and we

have a break in our periodic table, your clue is the change in atomic numbers we

are now in the f block which is at the bottom. Now the coefficient or number in

front is always two numbers less than the row it is in for the f block. So

instead of 6f we will write 4f and this is 4f14, now we go back up to the

d block we know this because the atomic numbers

have to go in order here we had an atomic number of 70 so next is 71, so 5d10

continue to 6p6, come around to the seventh row to 7s2. There is a break in

the table again to the f block so 5f,1, 2, 3 ,4, 5, 6 , 5f6. Here's the full electron

configuration. Now let's find the condensed electron configuration using

the noble gas that is before plutonium, so plutonium is at the bottom but would

have been in the seventh row so we will use the noble gas in the six row which

is radon and continue from there so 7s2 and 5f6 and here's the condensed

electron configuration. Now if you would like help with your homework online

tutoring or other helpful resources I have all of that and more in the

description box and if you want to make sure you're ready for your next exam

I created a practice quiz video just for you with of course step-by-step answers

you can find that right here and remember stay determined you can do this!