Konfigurasi Elektron | KIMIA KELAS 10
Summary
TLDRThis 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
🔬 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.
🌿 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.
🌟 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.
Mindmap
Keywords
💡Electron
💡Bohr Model
💡Energy Levels
💡Shells
💡Orbitals
💡Aufbau Rule
💡Valence Electrons
💡Transition Metals
💡Main Group Elements
💡Electron Configuration
💡Quantum Numbers
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
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