Konfigurasi Elektron | KIMIA KELAS 10

Summary

This educational video introduces students to electron configuration based on Bohr's atomic theory. The instructor explains that electrons orbit the nucleus in specific energy levels, with closer orbits having lower energy. The video details the maximum number of electrons per orbit, using the formula 2n², and explains how to fill electrons in orbitals following the Aufbau principle. It covers electron configurations of elements like nitrogen, magnesium, and bromine, discusses valence electrons, and contrasts main group elements with transition metals. The lesson concludes by highlighting the differences in valence electrons between these groups.

Takeaways

• 🔬 The Bohr model explains that electrons orbit the nucleus in specific energy levels, with lower energy closer to the nucleus and higher energy further away.
• ⚛️ The maximum number of electrons in a shell follows the formula 2n^2, where 'n' is the shell number.
• 🧮 In the first shell, the maximum number of electrons is 2, in the second shell it's 8, and in the third shell, it's 18, and so on.
• 📜 According to the Aufbau principle, electrons fill orbitals starting from the lowest energy level to the highest.
• 🔢 There are four types of orbitals: s, p, d, and f. S orbitals hold a maximum of 2 electrons, p holds 6, d holds 10, and f holds 14.
• 🧩 Electrons are arranged in orbitals in a specific sequence. For example, the sequence for nitrogen (atomic number 7) is 1s² 2s² 2p³.
• ⚡️ The electron configuration for magnesium (atomic number 12) is 1s² 2s² 2p⁶ 3s².
• 🛠 Electron configuration ends with s or p orbitals for main group elements and with d orbitals for transition metals.
• 💡 Valence electrons are those in the outermost shell, and they determine an element’s reactivity. For nitrogen, there are 5 valence electrons; for magnesium, there are 2.
• 🔄 Transition metals, like iron, have their electron configurations ending in d orbitals, distinguishing them from main group elements.

Q & A

What is the main topic of the video script?

The main topic of the video script is the configuration of electrons according to Bohr's atomic theory.

What does Bohr's theory state about electron movement around the nucleus?

Bohr's theory states that electrons move around the nucleus in certain orbits at specific energy levels, with closer orbits to the nucleus having lower energy levels.

What is the maximum number of electrons that can occupy the first electron shell?

The maximum number of electrons that can occupy the first electron shell is 2, as per the formula n^2 where n is the shell number.

How many types of orbitals are mentioned in the script?

Four types of orbitals are mentioned: s, p, d, and f orbitals.

What is the maximum number of electrons that can be accommodated in an s orbital?

An s orbital can accommodate a maximum of 2 electrons.

What is the Aufbau rule mentioned in the script, and what does it state?

The Aufbau rule states that electron filling begins with the orbital of the lowest energy level and proceeds to higher energy levels.

How many electrons does a p orbital hold when it is fully occupied?

A fully occupied p orbital holds 6 electrons.

What is the electron configuration for nitrogen with an atomic number of 7?

The electron configuration for nitrogen is 1s^2 2s^2 2p^3.

What is the difference between main group elements and transition elements in terms of electron configuration?

Main group elements end their electron configuration with s orbitals, while transition elements end with d orbitals.

What is the significance of valence electrons in chemical bonding?

Valence electrons are the electrons in the outermost shell that are used for bonding or chemical reactions.

How many valence electrons does magnesium have according to the script?

Magnesium has 2 valence electrons in its outermost shell.

Outlines

00:00

🔬 Electron Configuration According to Bohr's Theory

This paragraph introduces the concept of electron configuration based on Bohr's atomic theory. It explains that electrons orbit the nucleus at specific energy levels or shells. The closer the shell to the nucleus, the lower the energy level. The paragraph then discusses the maximum number of electrons that can occupy each shell, using the formula 2n^2, where 'n' is the shell number. It also describes the Aufbau principle, which dictates the order in which electrons fill orbitals starting from the lowest energy level. The paragraph details the types of orbitals (S, P, D, F) and their maximum electron capacities. It further illustrates the electron configuration process with examples, starting with the first shell having one S orbital holding a maximum of two electrons, and then moving to the second shell with one S and three P orbitals. The paragraph concludes with an example of how to write electron configurations following the Aufbau rule, emphasizing that the 4S orbital is filled before the 3D due to its lower energy level.

05:05

🌿 Electron Configuration Examples for Nitrogen, Magnesium, and Bromine

This paragraph provides detailed examples of electron configurations for specific elements: nitrogen (atomic number 7), magnesium (atomic number 12), and bromine (atomic number 35). It outlines the step-by-step process of filling electron orbitals according to the Aufbau principle, starting with the lowest energy orbitals. For nitrogen, the configuration is described as 1s^2 2s^2 2p^3, indicating two electrons in the first shell's S orbital, two in the second shell's S orbital, and three in the second shell's P orbital. The paragraph continues with magnesium's configuration, which includes filling up to the 3s orbital, and bromine's configuration, which ends with the 4p orbital. The summary also explains the concept of valence electrons, which are the electrons in the outermost shell that participate in chemical bonding. The valence electrons for nitrogen are the five in the second shell, for magnesium, the two in the third shell's S orbital, and for bromine, the seven in the fourth shell's S and P orbitals.

10:14

🌟 Understanding Valence Electrons and Transition Metals

The final paragraph focuses on valence electrons, especially in the context of transition metals. It explains that if an electron configuration ends with a 'd' orbital, the element is a transition metal, and if it ends with an 's' orbital, it belongs to the main group elements. The paragraph uses iron (atomic number 26) as an example to illustrate the electron configuration for a transition metal. It details the filling of orbitals up to the 3d orbital, which is characteristic of transition metals. The summary also clarifies the calculation of valence electrons for transition metals by adding the electrons in the 'd' orbital to those in the outermost 's' and 'p' orbitals. The paragraph concludes by emphasizing the importance of understanding electron configurations, particularly valence electrons, for grasping chemical behavior and reactivity.

Keywords

💡Electron

Electrons are subatomic particles that orbit the nucleus of an atom. In the context of the video, electrons are discussed in relation to their movement around the atomic nucleus and their energy levels, which is central to understanding atomic structure and the Bohr model.

💡Bohr Model

The Bohr Model is a theory that describes the behavior of electrons in an atom. It suggests that electrons move in specific orbits around the nucleus at certain energy levels. This model is foundational to the video's discussion on electron configuration.

💡Energy Levels

Energy levels, or shells, are specific regions around the nucleus where electrons can exist. The video explains that electrons closer to the nucleus are at lower energy levels, while those further away are at higher energy levels.

💡Shells

Shells refer to the different energy levels or layers in which electrons can be found. The script mentions that the maximum number of electrons that can occupy a shell is determined by the formula 2n^2, where n is the shell number.

💡Orbitals

Orbitals are regions within an energy level where electrons are most likely to be found. The video discusses different types of orbitals: s, p, d, and f, each with a specific capacity for electrons.

💡Aufbau Rule

The Aufbau Rule states that electrons fill orbitals starting from the lowest energy level to the highest. This rule is crucial for understanding how electrons are arranged in an atom, as explained in the video.

💡Valence Electrons

Valence electrons are the electrons in the outermost shell of an atom and play a key role in chemical bonding. The video describes how to determine the valence electrons by looking at the outermost shell of an element.

💡Transition Metals

Transition metals are elements that have their electron configuration ending in d orbitals. The video explains that elements ending in d orbitals are classified as transition metals, which have unique chemical properties.

💡Main Group Elements

Main group elements are those whose electron configuration ends in s or p orbitals. The video contrasts these with transition metals, indicating that main group elements have different chemical behaviors.

💡Electron Configuration

Electron configuration refers to the distribution of electrons in an atom's orbitals. The video provides examples of how to write electron configurations for elements like nitrogen and magnesium, following the Aufbau Rule.

💡Quantum Numbers

Quantum numbers are values that describe the state of an electron in an atom. The video implies the concept of quantum numbers when discussing the arrangement of electrons in shells and orbitals.

Highlights

Introduction to Bohr's theory of electron configuration.

Electrons orbit the nucleus at specific energy levels.

Closer orbits have lower energy levels.

The maximum number of electrons in each energy level is given by the formula n^2.

The first energy level can hold a maximum of 2 electrons.

The second energy level can hold a maximum of 8 electrons.

The Aufbau principle dictates the order of electron filling.

There are four types of orbitals: S, P, D, and F.

The S orbital can hold a maximum of 2 electrons.

The P orbital can hold a maximum of 6 electrons.

The D orbital can hold a maximum of 10 electrons.

The F orbital can hold a maximum of 14 electrons.

Electron configuration starts with the lowest energy orbitals.

Nitrogen with atomic number 7 has a specific electron configuration.

Magnesium with atomic number 12 has a specific electron configuration.

Bromine with atomic number 35 has a specific electron configuration.

Valence electrons are those in the outermost energy level.

The electron configuration of transition metals ends with d orbitals.

Iron with atomic number 26 is an example of a transition metal.

Main group elements' electron configuration ends with s orbitals.

The valence electrons of transition elements are calculated by adding s and d electrons.

The video concludes with a summary of electron configuration learning.

Transcripts

halo halo anak-anak jumpa lagi dengan

saya Pakjo hari ini kita akan belajar

konfigurasi elektron menurut teori atom

Bohr yang sudah kita pelajari pada

pertemuan sebelumnya mengatakan bahwa

elektron bergerak mengelilingi inti pada

kulit pintasan tertentu dengan tingkat

energi tertentu semakin dekat kulit

lintasan dengan inti artinya tingkat

energinya semakin rendah

Hai semakin jauh dengan inti artinya

memiliki energi yang lebih tinggi

Bagaimana dengan jumlah maksimal

elektron di setiap kulit lintasan atau

di setiap tingkat energi memiliki rumus2

n pangkat 2 jadi di kulit pertama atau

kulit kna1 maka jumlah maksimum elektron

nya yang bisa menempati kulit pertama

adalah 21 pangkat 2 sehingga jumlah

maksimal elektronnya itu dua di kulit

pertama kemudian di kulit l atau

lintasan kedua maka jumlah maksimalnya

bnr2 ^ 2 = 8 dilintasan ketika Bagaimana

23 ^ 2 = 18 dan seterusnya Bagaimana

penulisan konfigurasi elektron

berdasarkan aturan aufbau aturan aufbau

mengatakan bahwa pengisian elektron

dimulai dari orbital dengan tingkat

energi yang paling rendah kemudian

menuju ke tingkat energi yang lebih

tinggi Anda empat jenis orbital ada

orbital S orbital P orbital d dan

orbital F orbital s itu maksimal terisi

Dua elektron orbital P 6 elektron

orbital di maksimal 10

sedangkan orbital F itu maksimal 14

elektron penyusunannya Bagaimana

sekalian seperti ini di kulit pertama

itu ada satu orbital S maksimal berisi

maksimal terisi Dua elektron sedangkan

di kulit kedua ada dua orbital s dan P

dan seterusnya pengisian itu dimulai

dari yang pertama Dulu di kulit pertama

ada orbital S setelah satu SS2 itu

terisi penuh selanjutnya dua S2 setelah

2 S2 yang diisi selanjutnya adalah 26

setelah 2 p63 s23 S2 terisi penuh

setelah

ia mengisi ke-36 setelah tiga B6 tidak

ketiga D10 melainkan ke-4 S2 karena

tingkat energinya 4S dua itu lebih

rendah dibandingkan 3D setelah 4S terisi

baru ke 3D 3D selanjutnya ke-4 B dari 4b

ke 5S dari 5S menuju ke-45 P dan

kemudian ke bawah ini ada enam es jadi

pengisiannya miring contoh yang pertama

ada nitrogen dengan nomor atom 7 nomor

atom 7 artinya jumlah elektronnya

Hai bagaimana pengisian orbital dia yang

pertama adalah satu SS2 sudah Dua

elektron yang digunakan setelah satu SS2

terisi dua SS2

S1 S2 2 S2 ada empat elektron Masih sisa

3 setelah 2 S2 selanjutnya adalah 2P

berapa elektronnya tiga elektron Nah

sekarang jumlah elektron Ya sudah lucu

jadi konfigurasi elektron untuk n atau

nitrogen dengan nomor atom 7 seperti ini

selanjutnya magnesium 12 Bagaimana

konfigurasinya sama satu SS2 kemudian

dua S2 setelah 2 S2 ada 2 P6 kita hitung

Sudah berapa elektron yang digunakan

yang sudah di

Hai masukkan ke orbital 10 masih ada dua

setelah 2 P6 telah 2P ada 3S Berapa

jumlahnya 2D merupakan konfigurasi

elektron dari MG Berikutnya ber356 ini

semakin banyak 1 s22 s22 p63 s23

Hai dengan dibawahnya setelah tiga S2

ada tiga P6 setelah 36 kita hitung dulu

nih jumlah elektron yang sudah kita

masukkan ke dalam orbital Jumlahnya ada

1018 maka selanjutnya adalah empat SS2

setelah 4S dua selanjutnya itu 3 dec 10

kita hitung lagi Sudah berapa

elektronnya Sudah 30 masih ada lima lagi

telah 3D 10 selanjutnya adalah 4b berapa

elektron yang dimasukkan karena 35 maka

disini 4 P5 seperti itu cara penulisan

konfigurasi elektron Selanjutnya apa

yang

sebagai elektron valensi elektron

valensi itu elektron yang digunakan

untuk berikatan atau elektron yang

berada di kulit paling luar kita lihat

dari tiga contoh ini elektron valensinya

itu ada berapa nitrogen

di kulit terluar itu adalah kulit ke-2

sehingga elektron valensi n itu

Hai jumlahnya berapa di orbital S Ada

Dua elektron di ortopedi ada tiga

elektron jadi dari sini kita bisa

melihat bahwa jumlah elektron valensi n

itu ada dua dan tiga yaitu lima kemudian

elektron valensi mg berapa kita lihat

kulit terluar dari MG adalah kulit ke-3

di kulit ketiga ada satu orbital S

terisi Dua elektron maka elektron

valensi MG itu sama dengan dua

selanjutnya BR kulit terluar BR itu ada

empat 45 dan 4S dua sehingga jumlah

elektron valensi BR itu = 2 +

nah 7 jika konfigurasi elektron itu

berakhir di IP atau es ini merupakan

golongan utama Bagaimana dengan golongan

transisi dia akan berakhir di orbital d

Contohnya seperti ini besi dengan nomor

atom 26 kita lihat konfigurasinya yang

pertama satu SS2 kemudian diikuti kedua

ada 2 S2 2 P6 setelah 2 P6 deklit ketiga

ada tiga SS2 kemudian tiga

Hai setelah tiga B6 berikutnya ada empat

SS2 kita lihat Sudah berapa elektron

yang kita masukkan ke dalam orbital

Hai 20 masih ada 6 elektron setelah 4S

dua itu 3D elektronnya berapa 6v dari

konfigurasi elektronnya kita lihat dia

berakhir di di Karena Dia berakhir Didik

maka dia termasuk unsur transisi kalau

tadi berakhir tipe kemudian berakhir di

es itu merupakan unsur golongan utama

kalau berakhir Dede maka dia termasuk

golongan transisi

Hai elektron valensi FF berapa elektron

valensi efek karena dia golongan

transisi maka dijumlahkan dengan

Hai SD depannya dengan rumus

Hai enmind 1S kemudian Ende elektronnya

ada berapa dies ada dua sedangkan titik

ada enam Maka elektron valensinya itu =

8 demikian video pembelajaran tentang

konfigurasi elektron sampai jumpa di

video pembelajaran selanjutnya