Name: shared electrons in covalent molecules
Uploaded: 2020-09-03T13:38:28.000Z
Duration: 2 min 46 s
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K12 Standards

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North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.3.1

Covalent Bonding and Lewis Structures

Valans elektronlarının paylaşılmasıyla ametaller arasında kovalent bağlar oluşur. Peki neden ametaller iyonik bağlarda olduğu gibi elektronları transfer etmektense paylaşmayı tercih ederler? Ametaller, valans elektronlarının bir atomdan diğerine aktarılmasını zorlaştıran yüksek iyonlaşma enerjilerine sahiptir.Bir amonyak molekülü düşünün. Nitrojen atomunun bir oktete ulaşması için üç elektrona daha ihtiyaç duyar ve hidrojen atomunun bir dublete ulaşması için bir elektrona ihtiyacı vardır. Bu nedenle, nitrojen atomu, hem nitrojen hem de hidrojenin kararlı elektron konfigürasyonlarına ulaşmasını sağlayacak şekilde üç hidrojen atomuyla bağlanır.Bu bağların her biri bir çift elektron paylaştığı için buna tek bağ denir. Kovalent bağdaki paylaşılan elektron çiftine bağ çifti adı verilir. Bağlanmaya katılmayan valans elektronları, yalnız çift veya bağlanmayan elektronlar olarak adlandırılır.6 valans elektronu ile oksijen atomlarının bir oktete ulaşmak için iki elektrona daha ihtiyacı vardır. Bu nedenle, iki oksijen atomu iki elektron çiftini paylaşarak bir çift bağ oluşturur. Nitrojen ise eşlenmemiş üç elektronu diatomik formunda paylaşarak üçlü bir bağ oluşturur.Tekli ve çoklu bağlar, bağ uzunluğu ve gücü açısından farklılık gösterir. Üçlü bağlar, çift bağlardan çift bağlar da tek bağlardan daha kısadır. Bağ gücü, bağ çokluğu ile artar.Bu yüzden nitrojendeki, üçlü bağı kırmak zordur bu da onun tepkimeye girme olasılığını düşürür. Lewis modeli, moleküllerin yapısını ve kararlılığını tahmin etmeye yardımcı olur. Lewis modeline göre, H2O kararlı bir moleküldür;çünkü hem oksijen hem de hidrojen kararlı elektron konfigürasyonlarına ulaşmıştır.Oksijen elektronları yalnızca bir hidrojen atomuyla paylaşıyorsa, elde edilen OH molekülü, oksijen sadece 7 valans elektronuna sahip olduğundan stabil değildir ve oktete ulaşamaz. Bununla birlikte, okteti tamamlamak için oksijene fazladan bir elektron eklenirse, ortaya çıkan hidroksit iyonu, negatif bir yük ile stabil hale gelir. Kovalent bağlar yönlüdür çünkü paylaşılan elektronlar iki belirli atom çiftini birbirine bağlar.Buna karşılık, iyonik bağlar yönsüzdür ve kafeste birkaç iyon tutulur. Bu nedenle, kovalent bir bileşikteki moleküller ayrı birer temel birim olarak kabul edilir.

kovalent bağ ve lewis yapıları

Metal ve ametal atomlar arasında elektronların transferinden kaynaklanan iyonik bağlarla karşılaştırıldığında, kovalent bağlar, atomların “paylaşılan” bir elektron çifti için karşılıklı olarak çekilmesinden kaynaklanır. 
 
 Kovalent bağlar, her ikisi de elektronları kendilerine çekmek için benzer eğilimlere sahip olduğunda (yani, her iki atom da aynı veya oldukça benzer iyonlaşma enerjilerine ve elektron afinitelerine sahip olduğunda) iki atom arasında oluşur. 
 
 <h4>Kovalent Bileşiklerin Fiziksel Özellikleri</h4>
 
 Kovalent bağlar içeren bileşikler, iyonik bileşiklerden farklı fiziksel özellikler sergiler. Elektriksel olarak nötr olan moleküller arasındaki çekim, elektrik yüklü iyonlar arasındakinden daha zayıf olduğu için, kovalent bileşikler genellikle iyonik bileşiklere göre çok daha düşük erime ve kaynama noktalarına sahiptir. Aslında birçok kovalent bileşik, oda sıcaklığında sıvı veya gazdır ve katı hallerinde tipik olarak iyonik katılardan çok daha yumuşaktır. Ayrıca, iyonik bileşikler suda çözündüklerinde iyi elektrik iletkenleri iken, çoğu kovalent bileşik suda çözünmez; elektriksel olarak nötr olduklarından, her durumda zayıf elektrik iletkenleridirler.
 
 <h4>Kovalent Bağların Oluşumu</h4>
 
 Ametal atomlar sıklıkla diğer ametal atomlarla kovalent bağlar oluşturur. Örneğin, hidrojen molekülü H2, iki hidrojen atomu arasında kovalent bir bağ içerir. Belirli potansiyel enerjiye sahip iki ayrı hidrojen atomu birbirine yaklaşır, değerlik orbitalleri (1s) üst üste gelmeye başlar. Her hidrojen atomundaki tek elektron daha sonra her iki atom çekirdeği ile etkileşime girerek her iki atomun etrafındaki boşluğu kaplar. Paylaşılan her elektronun her iki çekirdeğe olan güçlü çekimi sistemi stabilize eder ve bağ mesafesi azaldıkça potansiyel enerji azalır. Atomlar birbirine yaklaşmaya devam ederse, iki çekirdekteki pozitif yükler birbirini itmeye başlar ve potansiyel enerji artar. Bağ uzunluğu, en düşük potansiyel enerjinin elde edildiği mesafeye göre belirlenir.
 
 Kimyasal bağları koparmak için (endotermik bir süreç) enerji gerektiğini unutmamak gerekir, oysa kimyasal bağları oluşturmak enerji açığa çıkarır (ekzotermik bir süreç). H2 durumunda, kovalent bağ çok güçlüdür; bir mol hidrojen molekülündeki bağları kırmak ve atomların ayrılmasına neden olmak için büyük miktarda enerji, 436 kJ eklenmelidir:
 
 <img alt="Eq1" src="https://www.jovecore.com/CDNSource/lessons/1059/1059_Equations-01.png" style="height: 40px;" />
 
 Tersine, iki mol H atomundan bir mol H2 molekülü oluştuğunda aynı miktarda enerji açığa çıkar:
 
 <img alt="Eq2" src="https://www.jovecore.com/CDNSource/lessons/1059/1059_Equations-02.png" style="height: 40px;" />
 
 <h4>Lewis Yapıları</h4>
 
 Lewis sembolleri, Lewis yapılarında, moleküllerdeki ve çok atomlu iyonlardaki bağlanmayı tanımlayan çizimlerde gösterilen kovalent bağların oluşumunu belirtmek için kullanılabilir. Örneğin, iki klor atomu bir klor molekülü oluşturduğunda, bir çift elektron paylaşırlar:
 
 <img alt="Figure1" src="https://www.jovecore.com/CDNSource/lessons/1059/1059Image_1.svg" style="height: 90px;" />
 
 Lewis yapısı, her bir Cl atomunun bağlanmada kullanılmayan üç çift elektrona (Yalın çift olarak adlandırılır) ve bir paylaşılan elektron çiftine (atomlar arasında yazılan) sahip olduğunu gösterir. Paylaşılan bir elektron çiftini belirtmek için bazen bir tire (veya çizgi) kullanılır:  Cl—Cl.
 
 <ul>
 <li>Paylaşılan tek bir elektron çiftine tek bağ denir. Her bir Cl atomu sekiz değerlik elektronuyla etkileşime girer: yalın çiftlerde altı ve tek bağda iki.</li>
 <li>Bununla birlikte, gerekli okteti elde etmek için bir çift atomun birden fazla elektron çiftini paylaşması gerekebilir. CH2O'daki (formaldehit) karbon ve oksijen atomları arasında ve C2H4'teki (etilen) iki karbon atomu arasında olduğu gibi bir çift atom arasında iki çift elektron paylaşıldığında bir çift bağ oluşur.  
 <img alt="Figure2" src="https://www.jovecore.com/CDNSource/lessons/1059/1059Image_2.svg" style="height: 120px;" /></li>
 <li>Karbon monoksit (CO) ve siyanür iyonunda (CN–) olduğu gibi, üç elektron çifti bir çift atom tarafından paylaşıldığında üçlü bir bağ oluşur. 
 <img alt="Figure3" src="https://www.jovecore.com/CDNSource/lessons/1059/1059Image_3.svg" style="height: 90px;" /></li>
 </ul>
 
 Periyodik tablo, bir atomdaki değerlik elektronlarının sayısını ve bir oktete ulaşmak için oluşacak bağların sayısını tahmin etmek için kullanılabilir. Argon ve Helyum gibi Grup 8A elementleri elektron konfigürasyonunu doldurmuştur ve bu nedenle nadiren kimyasal bağa katılırlar. Bununla birlikte, brom veya iyot gibi 7A grubundaki atomlar, oktete ulaşmak için yalnızca bir elektrona ihtiyaç duyar. Dolayısıyla, 7A grubuna ait atomlar tek bir kovalent bağ oluşturabilir. 6A grubunun atomlarının bir oktete ulaşması için 2 elektrona ihtiyacı vardır; dolayısıyla iki kovalent bağ oluşturabilirler. Benzer şekilde, 4A grubuna ait olan karbonun bir oktete ulaşmak için 4 elektrona daha ihtiyacı vardır; bu nedenle karbon dört kovalent bağ oluşturabilir. 
 
 Bu metin bu kaynaklardan uyarlanmıştır: <a href="https://openstax.org/books/chemistry-2e/pages/7-2-covalent-bonding">Openstax, Chemistry 2e, Section 7.2: Covalent Bonds</a> ve <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>

Kovalent Bağ ve Lewis Yapıları

Metalik ve metalik olmayan atomlar arasındaki elektron transferinden kaynaklanan iyonik bağlarla karşılaştırıldığında, kovalent bağlar karşılıklı ...

Education

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Chemical Bonding: Basic Concepts

Kimyasal Bağlanma: Temel Kavramlar

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shared electrons in covalent molecules

Covalent molecules form when atoms share electrons instead of transferring them. This bonding usually happens between nonmetal atoms with similar tendencies to attract electrons. Because the atoms pull on the electrons in a shared way, the bond is held together by mutual attraction.

Covalent compounds often have physical properties that differ from ionic compounds. The attraction between neutral molecules is weaker than the attraction between charged ions. As a result, many covalent compounds have lower melting and boiling points, and some are liquids or gases at room temperature. When they are solids, they are usually softer than ionic solids. Most covalent compounds are also insoluble in water and are poor conductors of electricity in any state.

Hydrogen gas shows how a covalent bond forms. In H2, two hydrogen atoms approach each other and their 1s valence orbitals overlap. Each electron interacts with both nuclei, which lowers the potential energy and stabilizes the molecule. If the atoms move too close, the positive nuclei repel each other, and the potential energy rises. The bond length is the distance where the potential energy is lowest. Forming a bond releases energy, so it is an exothermic process. Breaking a bond requires energy, so it is endothermic. For H2, 436 kJ must be added to break one mole of molecules, and the same amount is released when one mole forms from hydrogen atoms.

Lewis structures show covalent bonding with Lewis symbols. In chlorine gas, Cl2, the two chlorine atoms share one pair of electrons. Each chlorine atom also has three lone pairs, which are pairs not used in bonding. A shared pair can be shown with a dash, so Cl—Cl represents a single bond. Each chlorine atom then has eight valence electrons around it, including lone pairs and the bonding pair.

Some atoms need more than one shared pair to reach an octet, which is a full outer shell of eight electrons. A double bond forms when two pairs of electrons are shared, as in CH2O and C2H4. A triple bond forms when three pairs are shared, as in CO and CN−. The periodic table helps predict bonding patterns from valence electrons. Group 18 elements such as argon and helium already have filled electron configurations and rarely bond. Group 17 atoms, such as bromine and iodine, usually need one electron and can form one covalent bond. Group 16 atoms need two electrons and can form two covalent bonds. Carbon in group 14 needs four more electrons, so it can form four covalent bonds.

Shared Electrons in Covalent Molecules

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covalent bonding and lewis structures

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Explore how nonmetal atoms share electrons to form covalent bonds, from H2 and Cl2 to double and triple bonds, Lewis structures, and bonding patterns.

Shared Electrons in Covalent Molecules | JoVE K12

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Shared Electrons in Covalent Molecules

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