Name: drawing lewis structures with valence electron counts
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Matter and its Interactions

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Lewis Structures of Molecular Compounds and Polyatomic Ions

Lewis yapıları, atomlar arasındaki kimyasal bağların basitleştirilmiş temsilleridir. Lewis yapılarını eten veya amonyak gibi nötr bileşikler veya hidronyum veya fosfat gibi çok atomlu iyonlar için yazmak, aşağıdaki aşamalar gereklidir. Önce moleküldeki toplam değerlik elektron sayısı hesaplanır.Örneğin eteni ele alalım. Her karbon atomunun 4 valans elektronu vardır ve her hidrojen atomunun 1 valans elektronu vardır;2 karbon ve 4 hidrojen atomlu eten, toplam 12 valans elektronuna sahiptir. Ardından, molekülün iskelet yapısını çizelim.Genel olarak kimyasal formüldeki ilk atom veya daha az elektronegatif atom merkezi olarak yerleştirilir. Bu atom aynı zamanda merkezi atom olarak adlandırılır ve en az iki bağ oluşturabilmelidir. Hidrojen atomu veya daha fazla elektronegatif atom, terminal olarak merkezi atomun etrafına yerleştirilir.Burada karbon atomları, etraflarını saran hidrojen atomları ile merkezi pozisyonları işgal ederler. Bir sonraki adım okteti tamamlamadır. İlk olarak, bağ çiftlerini temsil etmek için her iki atom arasına bir çift elektron yerleştirin.Kalan elektronlar, ikili veya sekizli konfigürasyonlarını sağlamak için terminal ve merkezi atomlara yalnız çiftler halinde dağıtılır. Bu durumda, hidrojen bir ikiliye ulaştığı için kalan elektronlar karbon atomlarına aktarılır. Şimdi, sekizli olmayan atomlar arasında çoklu bağlar oluşturmak için yalnız çiftleri kullanalım.Eten'de, karbon atomları henüz bir oklete ulaşmadı. Bu nedenle, yalnız çift, tüm atomların kararlı bir elektron konfigürasyonuna ulaşmasına izin veren bir çift bağ oluşturmak için bağlanma bölgesine taşınır. Hidronyum veya fosfat gibi yüklü çok atomlu iyonlar için Lewis yapısını yazmak için, iyonik yükü barındıracak bir modifikasyonla aynı yaklaşım izlenir.Hidronyumun Lewis yapısını çizmek için, önce iyon üzerindeki valans elektronlarının sayısını hesaplayın. Hidronyum iyonu pozitif yüke sahip olduğundan, toplam valans elektronlarından bir elektronu çıkarın ve sayıyı 8'e düşürün. Sonra molekülü iskelet yapısıyla gösterin.Şimdi her atom arasına bir elektron çifti, ardından merkez atomdaki tek elektron çiftini yerleştirin. Bu şekilde, hidrojen ve oksijen atomları sırasıyla dublet ve okteti tamamlar. Son olarak, Lewis yapısını sağ üst köşesinde pozitif bir yük ile parantez içine yazın.

moleküler bileşiklerin ve poliatomik İyonların lewis yapıları

Karmaşık moleküller ve moleküler iyonlar için Lewis yapılarını çizmek için, belirtildiği gibi adım adım bir prosedürü izlemeye yardımcı olur:
 
 <ol>
 <li>Toplam değerlik sayısını (dış kabuk) elektronlarını belirleyin. Katyonlar için her pozitif yük için bir elektronu çıkarın. Anyonlar için, her negatif yük için bir elektron ekleyin.</li>
 <li>Atomları merkezi bir atomun etrafına yerleştirerek molekülün veya iyonun iskelet yapısını çizin. (Genel olarak, en az elektronegatif eleman merkeze yerleştirilmelidir.) Her atomu tek bir bağla (bir elektron çifti) merkezi atoma bağlayın.</li>
 <li>Kalan elektronları, her bir atomun etrafında bir sekizli tamamlayarak, terminal atomları (hidrojen hariç) üzerinde yalın çiftler halinde dağıtın.</li>
 <li>Kalan tüm elektronları merkezi atom üzerine yerleştirin.</li>
 <li>Mümkün olan her yerde sekizli elde etmek için merkezi atomla çoklu bağlar oluşturmak için dış atomların elektronlarını yeniden düzenleyin.</li>
 </ol>
 
 Örneğin SiH4, CHO–2, NO+, ve OF2'yi Lewis yapılarını belirlemek için bu genel kılavuzun uygulanabileceği örnekler olarak düşünün.
 
 <ol>
 <li>Molekül veya iyondaki toplam değerlik (dış kabuk) elektron sayısını belirleyin. </li>
 </ol>
 
 SiH4 gibi bir molekül için moleküldeki her bir atomdaki değerlik elektronlarının sayısı eklenir: 
 
 = [4 değerlik e−/Si atom × 1 Si atom] + [ 1 değerlik e−/H atom × 4 H atoms] = 8 değerlik e−
 
 <h4>CHO–2</h4>
 
  CHO–2 gibi negatif bir iyon için, atomlardaki değerlik elektronlarının sayısı iyon üzerindeki negatif yüklerin sayısına eklenir (her bir negatif yük için bir elektron elde edilir):
 
 = [4 değerlik e−/C atom × 1 C atom] + [1 değerlik e−/H atom × 1 H atom] + [6 değerlik e−/O atom × 2 O atomları] + [1 ek e−] = 18 değerlik e−
 
 <h4>NO+</h4>
 
 NO+ gibi pozitif bir iyon için, iyondaki atomların üzerindeki değerlik elektronlarının sayısı eklenir, ardından iyon (her bir pozitif yük için bir elektron kaybolur) üzerindeki pozitif yüklerin sayısı toplam değerlik elektronlarının sayısından çıkarılır:
 
 = [5 değerlik e−/N atom × 1 N atom] + [6 değerlik e−/O atom × 1 O atom] + [−1 e−] = 10 değerlik e−
 
 <h4>OF2 </h4>
 
 OF2 nötr bir molekül olduğundan, değerlik elektronlarının sayısı basitçe eklenir:
 
 = [6 değerlik e−/O atom × 1 O atom] + [7 değerlik e−/F atom × 2 F atomları] = 20 değerlik e−
 
 <ol start="2">
 <li>Molekül veya iyonun iskelet yapısını çizin, atomları merkezi bir atomun etrafına düzenleyin ve her atomu tek bir (bir elektron çifti) bağ ile merkez atoma bağlayın. (İyonların yapının etrafında parantezlerle ve parantezlerin dışındaki iyonik yükün gösterildiğini unutmayın:) 
 <img alt="Figure1" src="https://www.jovecore.com/CDNSource/lessons/1063/1063Image_1.svg" style="height: 80px;" /> 
 Birkaç atom düzenlemesinin mümkün olduğu durumlarda, CHO2− için olduğu gibi, doğru olanı seçmek için deneysel kanıtlar kullanılır. Genel olarak, daha az elektronegatif elementlerin merkezi atomlar olma olasılığı daha yüksektir.  CHO2−,  'da, daha az elektronegatif karbon atomu, onu çevreleyen oksijen ve hidrojen atomları ile merkezi konumu işgal eder. Diğer örnekler arasında POCl3'te P, SO2'de S ve  ClO4−'de Cl yer alır.  Bir istisna, hidrojen neredeyse hiçbir zaman merkezi bir atom olmamasıdır. En elektronegatif element olarak flor, aynı zamanda merkezi bir atom olamaz.</li>
 <li>Kalan elektronları, bir elektron okteti ile değerlik kabuklarını tamamlamak için terminal atomlar (hidrojen hariç) üzerinde yalın çiftler olarak dağıtın. (SiH4'te elektron kalmadığından yapısı değişmez.) 
 <img alt="Figure2" src="https://www.jovecore.com/CDNSource/lessons/1063/1063image_2.svg" style="height: 80px;" /></li>
 <li>Kalan tüm elektronları merkezi atom üzerine yerleştirin. 
 <ul>
 <li>SiH4,  CHO2−  ve NO+ için kalan elektron yoktur. OF2 için kalan 16 elektrondan 12'si yerleştirilir, böylece merkez atom üzerine yerleştirilecek 4 elektron kalır: 
 <img alt="Figure3" src="https://www.jovecore.com/CDNSource/lessons/1063/1063Image_3.svg" style="height: 40px;" /></li>
 </ul>
 </li>
 <li>Mümkün olan her yerde sekizli elde etmek için merkezi atomla çoklu bağlar oluşturmak için dış atomların elektronlarını yeniden düzenleyin. 
 <ul>
 <li>SiH4: Si zaten bir sekizliye sahip, bu yüzden hiçbir şey yapılmasına gerek yok.  
 <img alt="Figure4" src="https://www.jovecore.com/CDNSource/lessons/1063/1063Image_4.svg" style="height: 70px;" /></li>
 <li>CHO−2:  Değerlik elektronları, oksijen atomlarında yalın çift olarak dağıtılır, ancak karbon atomu bir oktet yoktur.  
 <img alt="Figure5" src="https://www.jovecore.com/CDNSource/lessons/1063/1063Image_5.svg" style="height: 80px;" /></li>
 <li>Bu nedenle, tek bir yalın çift, oksijenlerin birinden bir çift bağ oluşturan karbon atomuna bağışlanır. Hangi oksijen atomunun elektronları bağışladığına bağlı olarak, aksi halde rezonans yapıları denilen iki olası yapı olabilir. </li>
 <li>NO+: Bu iyon için sekiz değerlik elektronu eklenir, ancak hiçbir atomda sekizli yoktur. Toplam elektronlar zaten kullanılmış olduğundan ek elektronlar eklenemez. Bu senaryoda, elektronlar birden fazla bağ oluşturmak için hareket ettirilmelidir. Azot atomunun iki yalın çift çifti vardır ve oksijen atomunun bir tane vardır.  
 <img alt="Figure6" src="https://www.jovecore.com/CDNSource/lessons/1063/1063Image_6.svg" style="height: 55px;" /></li>
 <li>Bu hala bir sekizli üretmez, bu nedenle üçlü bir bağ oluşturmak için başka bir çift hareket ettirilmelidir. 
  <img alt="Figure7" src="https://www.jovecore.com/CDNSource/lessons/1063/1063Image_7.svg" style="height: 50px;" /></li>
 <li>OF2'de, her atom zaten bir sekizliye sahip olduğundan hiçbir şey değişmez. 
 <img alt="Figure8" src="https://www.jovecore.com/CDNSource/lessons/1063/1063Image_8.svg" style="height: 40px;" /></li>
 </ul>
 </li>
 </ol>
 
 Bu metin bu kaynaktan uyarlanmıştır: <a href="https://openstax.org/books/chemistry-2e/pages/7-3-lewis-symbols-and-structures">Openstax, Chemistry 2e, Section 7.3: Lewis Symbols and Structures.</a>

Moleküler Bileşiklerin ve Poliatomik İyonların Lewis Yapıları

Karmaşık moleküller ve moleküler iyonlar için Lewis yapılarını çizmek için, ana hatlarıyla belirtildiği gibi adım adım bir prosedürü takip etmek faydalı olacaktır:

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drawing lewis structures with valence electron counts

Drawing Lewis structures starts with counting valence electrons and building the atom arrangement step by step. Valence electrons are the outer-shell electrons that help show how atoms bond. For ions, a positive charge means one electron is removed for each plus sign, and a negative charge means one electron is added for each minus sign.

The next step is to sketch the skeleton structure. The least electronegative atom usually goes in the center, while hydrogen is almost never central. Fluorine also cannot be a central atom because it is the most electronegative element. Ions are written in brackets, with the charge shown outside the brackets.

After the skeleton is drawn, connect the atoms to the central atom with single bonds. Each single bond represents one electron pair. Then place the remaining electrons as lone pairs on the terminal atoms, except hydrogen, until those atoms have octets when possible. Any electrons still left go on the central atom.

If the central atom still does not have an octet, move lone pairs to make double or triple bonds. This can create resonance structures, which are different valid arrangements of electrons. For the formate ion, CHO2−, one oxygen can donate a lone pair to make a double bond with carbon. That gives two possible resonance forms.

The examples in the model show how the procedure works in real cases. SiH4 has 8 valence electrons total, so its structure does not need more changes once the single bonds are drawn. CHO2− has 18 valence electrons. NO+ has 10 valence electrons, and its atoms must be rearranged into a triple bond to satisfy octets as much as possible. OF2 has 20 valence electrons, and after the lone pairs are placed, its structure stays unchanged because each atom already has an octet.

Drawing Lewis Structures with Valence Electron Counts

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Drawing Lewis structures starts with counting valence electrons and building the atom arrangement step by step. Valence electrons are the outer-shell electrons that help show how atoms bond. For ions, a positive charge means one electron is removed for each plus sign, and a negative charge means one electron is added for each minus sign. The next step is to sketch the skeleton structure. The least electronegative atom usually goes in the center, while hydrogen is almost never central. Fluorine...

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Learn the step-by-step method for drawing Lewis structures, counting valence electrons, placing lone pairs, and handling ions, resonance, and multiple bonds.

Drawing Lewis Structures with Valence Electron Counts | JoVE K12

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An ionic compound is stable because of the electrostatic attraction between its positive and negative ions. The lattice energy of a ...

Trends in Lattice Energy: Ion Size and Charge

An ionic compound is stable because of the electrostatic attraction between its positive and negative ions. The lattice energy of a compound is a measure ...

Covalent Bonding and Lewis Structures

Compared to ionic bonds, which results from the transfer of electrons between metallic and nonmetallic atoms, covalent bonds result from the mutual ...

Electronegativity

Whether a bond is nonpolar or polar covalent is determined by a property of the bonding atoms called electronegativity.&#xA0;

Electronegativity values of ...

Bond Polarity, Dipole Moment, and Percent Ionic Character

Bond Polarity

The absolute value of the difference in electronegativity (&Delta;EN) of two bonded atoms provides a rough measure of the polarity to be ...

Analyze and interpret data to explain the mechanisms and properties of the two main types of intramolecular (ionic and covalent) bonds.

Analyze the structure of atoms and isotopes.

Drawing Lewis Structures with Valence Electron Counts

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