Name: how bond polarity shapes molecular dipoles
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Bond Polarity, Dipole Moment, and Percent Ionic Character

Polar olmayan kovalent, polar kovalent veya iyonik olsun, kimyasal bağların türü büyük ölçüde bağ atomları ve bunların bağ uzunlukları arasındaki elektronegatiflik farkı ile belirlenir. Bromda, iki brom atomu arasındaki bağ polar değildir çünkü aralarındaki elektronegatiflik farkı sıfırdır. Hidrojen bromürdeki bağ, daha elektronegatif brom elektron yoğunluğunu daha az elektronegatif hidrojen atomundan uzaklaştırdığı için kovalenttir.Potasyum bromürde bağ, elektronegatiflikteki daha büyük farktan dolayı iyonik bir bağdır ve potasyumdan bromüre tam elektron transferiyle sonuçlanır. İki eşit, ancak zıt yüklü parçacık bir mesafeyle ayrıldığında, bir çift kutup oluşur. Dipolün kantitatif büyüklüğü, coulomb cinsinden bildirilen yüklerin büyüklüğünün ve metre cinsinden bildirilen yükler arasındaki mesafenin çarpımı olan mu harfi ile temsil edilen dipol momenti olarak adlandırılır.Dipol momenti Debye birimlerinde verilir, ve bir debye 3, 34 x 10^30 Coulomb*metre'ye eşittir. Bir bileşiğin polar kovalent veya iyonik olup olmadığı, bir bağın ölçülen dipol momentinin, tam bir elektron transferini varsayan dipol momentine oranı olan yüzde iyonik karakter hesaplanarak belirlenebilir. 50'den fazla iyonik karaktere sahip bağlar iyonik olarak kabul edilir.Hidrojen ve flor atomlarının 92 pikometre mesafeyle ayrıldığı hidrojen florürü ele alalım. Bağ iyonik ise, çift kutup momenti tam bir elektron transferi varsayılarak hesaplanır. Bir elektronun yükü atomlar arasındaki mesafe ile çarpılır ve elde edilen değer bir Debye ile bölünür, bu da 4, 41 Debye dipol momentini verir.Bununla birlikte, hidrojen florürün deneysel olarak ölçülen dipol momenti 1, 18 Debye'dir. Bu nedenle, hidrojen florürün yüzde iyonik karakterini belirlemek için, 1, 18 Debye'nin ölçülen değeri 4, 41 Debye'ye bölünür ve bu da 41'lik bir yüzde iyonik karakter verir. Hidrojen florürün yüzde iyonik karakteri 50'den az olduğu için polar kovalent bir bağdır.

bağ polaritesi, dipol momenti ve yüzde İyonik karakter

<h4>Bağ Polaritesi</h4>
 
 İki bağlı atomun elektronegatifliğindeki (ΔEN) farkın mutlak değeri, bağda beklenen polaritenin ve dolayısıyla bağ türünün kaba bir ölçüsünü sağlar. Fark çok küçük veya sıfır olduğunda bağ kovalenttir ve polar değildir. Büyük olduğunda, bağ polar kovalent veya iyoniktir. H–H, H–Cl ve Na–Cl bağlarındaki atomlar arasındaki elektronegatiflik farklarının mutlak değerleri sırasıyla 0 (polar olmayan), 0,9 (polar kovalent) ve 2,1'dir (iyonik). 
 
 Elektronların atomlar arasında paylaşılma derecesi tamamen eşit (saf kovalent bağ) ile hiç (iyonik bağ) arasında değişir. 
 
 <ul>
 <li>Örneğin, HF'deki H ve F atomları 1,9'luk bir elektronegatiflik farkına sahiptir ve NH3'teki N ve H atomları 0,9'luk bir farka sahiptir, ancak bu bileşiklerin her ikisi de polar kovalent olarak kabul edilen bağlar oluşturur. </li>
 <li>Benzer şekilde, NaCl'deki Na ve Cl atomlarının elektronegatiflik farkı 2.1'dir ve MnI2'deki Mn ve I atomları 1,0'lık bir farka sahiptir, ancak bu maddelerin her ikisi de iyonik bileşikler oluşturur.</li>
 </ul>
 
 Bir bağın kovalent veya iyonik karakterine ilişkin en iyi rehber, ilgili atom türlerini ve bunların periyodik tablodaki göreceli konumlarını dikkate almaktır. 
 
 <ul>
 <li>İki ametal arasındaki bağlar genellikle kovalenttir.</li>
 <li>Bir metal ile ametal arasındaki bağ genellikle iyoniktir.</li>
 </ul>
 
 Bazı bileşikler hem kovalent hem de iyonik bağlar içerir. OH–, NO3−  ve NH4+ gibi çok atomlu iyonlardaki atomlar, polar kovalent bağlarla bir arada tutulur. Bununla birlikte, bu çok atomlu iyonlar, zıt yükteki iyonlarla birleşerek iyonik bileşikler oluşturur. Örneğin, potasyum nitrat, KNO3, K+ katyonunu ve çok atomlu NO3− anyonunu içerir. Bu nedenle, potasyum nitratta bağlanma iyoniktir, K+ ve NO3− iyonları arasındaki elektrostatik çekimden ve NO3−'daki nitrojen ve oksijen atomları arasındaki kovalenttir.
 
 <h4>Moleküler Polarite ve Dipol Moment</h4>
 
 Daha önce tartışıldığı gibi, polar kovalent bağlar, elektronlar daha elektronegatif atoma doğru çekildikçe, farklı elektronegatifliklere sahip iki atomu bağlayarak, bir atomu kısmi pozitif yüklü (δ+) ve diğer atomu kısmi negatif yüklü (δ–) bırakır. Bu yük ayrımı, bir bağ dipol momentine yol açar. Bir bağ dipol momentinin büyüklüğü Yunanca mu (µ) harfi ile temsil edilir ve burada gösterilen formülle verilir; burada Q, kısmi yüklerin büyüklüğüdür (elektronegatiflik farkı ile belirlenir) ve r yükler arasındaki mesafedir:
 
 <img alt="Eq1" src="https://www.jovecore.com/CDNSource/lessons/1062/1062_Equations-01.png" style="height: 40px;" />
 
 Bağ momenti, hem yön hem de büyüklüğe sahip olan bir vektör olarak gösterilebilir. Dipol vektörleri, daha az elektronegatif atomdan daha elektronegatif atoma doğru olan bağla birlikte işaret eden oklar olarak gösterilir. Bağın kısmen pozitif ucunu belirtmek için daha az elektronegatif uca küçük bir artı işareti çizilir. Okun uzunluğu, iki atom arasındaki elektronegatiflik farkının büyüklüğü ile orantılıdır.
 
 Tam bir molekül, moleküler yapısına ve bağlarının her birinin polaritesine bağlı olarak bir yük ayrımına da sahip olabilir. Böyle bir yük ayrımı mevcutsa, molekülün bir polar molekül (veya dipol) olduğu söylenir; aksi takdirde molekülün polar olmadığı söylenir. Dipol moment, bir bütün olarak moleküldeki net yük ayrımının kapsamını ölçer. Dipol moment, moleküler yapı dikkate alınarak üç boyutlu uzayda bağ momentleri eklenerek belirlenir.
 
 Diatomlu moleküller için yalnızca bir bağ vardır, bu nedenle bağ dipol momenti moleküler polariteyi belirler. Br2 ve N2 gibi homonükleer iki atomlu moleküllerin elektronegatiflikte hiçbir farkı yoktur, bu nedenle dipol momentleri sıfırdır. CO gibi heteronükleer moleküller için küçük bir dipol momenti vardır. HF için daha büyük bir dipol momenti vardır çünkü elektronegatiflikte daha büyük bir fark vardır.
 
 Bir molekül birden fazla bağ içerdiğinde, geometri dikkate alınmalıdır. Bir moleküldeki bağlar, bağ momentleri birbirini takip edecek şekilde düzenlenmişse (vektör toplamı sıfıra eşittir), o zaman molekül polar değildir. CO2'deki durum budur. Bağların her biri kutupsaldır, ancak molekül bir bütün olarak kutupsuzdur. Lewis yapısından ve VSEPR teorisi kullanılarak CO2 molekülünün, karbon atomunun zıt taraflarında polar C=O bağları ile doğrusal olduğu belirlenir. Bağ momentleri birbirini götürür çünkü zıt yönlere işaret ederler. Su molekülü durumunda, Lewis yapısı yine bir merkezi atoma iki bağ olduğunu gösterir ve elektronegatiflik farkı yine bu bağların her birinin sıfır olmayan bir bağ momentine sahip olduğunu gösterir. Ancak bu durumda, moleküler yapı O üzerindeki yalın çiftler nedeniyle bükülür ve iki bağ momenti birbirini götürmez. Bu nedenle, suyun net bir dipol momenti vardır ve bir polar moleküldür (dipol).
 
 Bu metin bu kaynaktan uyarlanmıştır: <a href="https://openstax.org/books/chemistry-2e/pages/7-2-covalent-bonding">Openstax, Chemistry 2e, Chapter 7.2: Covalent Bonding and  Openstax, Chemistry 2e, Chapter 7.6 Molecular Structure and Polarity.</a>

Bağ Polaritesi, Dipol Momenti ve Yüzde İyonik Karakter

Bağ Polaritesi

İki bağlı atomun elektronegatiflik (ΔEN) farkının mutlak değeri, polaritenin kaba bir ölçüsünü sağlar.

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Chemical Bonding: Basic Concepts

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how bond polarity shapes molecular dipoles

Bond polarity depends on electronegativity, the ability of an atom to attract shared electrons. The absolute value of the electronegativity difference, or ΔEN, gives a rough guide to bond type. When the difference is very small or zero, the bond is covalent and nonpolar. When it is larger, the bond may be polar covalent or ionic.

Examples show how this works in real compounds. H–H has a ΔEN of 0, so it is nonpolar. H–Cl has a ΔEN of 0.9, so it is polar covalent. Na–Cl has a ΔEN of 2.1, so it is ionic. Even so, ΔEN is only a guide. HF has a ΔEN of 1.9 and NH3 has a ΔEN of 0.9, yet both have polar covalent bonds. NaCl has a ΔEN of 2.1 and MnI2 has a ΔEN of 1.0, yet both are ionic compounds.

The type of atoms in the periodic table is often the best clue. Bonds between two nonmetals are generally covalent. Bonds between a metal and a nonmetal are often ionic. Some compounds include both kinds of bonding. Polyatomic ions such as OH−, NO3−, and NH4+ have polar covalent bonds inside the ion. They form ionic compounds when they combine with ions of the opposite charge. Potassium nitrate, KNO3, is one example. It contains K+ and NO3−, so the attraction between those ions is ionic, while the N–O bonds inside nitrate are covalent.

Polar covalent bonds create partial charges, written as δ+ and δ−. The more electronegative atom pulls the electrons closer, so one end of the bond becomes partially negative and the other becomes partially positive. This charge separation creates a bond dipole moment, symbolized by μ. A dipole is shown as a vector, or arrow, that points from the less electronegative atom toward the more electronegative atom. A small plus sign marks the positive end. A longer arrow means a larger electronegativity difference.

A whole molecule can also have a net dipole moment. That depends on both bond polarity and molecular shape. The dipole moment of the molecule is found by adding the bond moments in three-dimensional space. For diatomic molecules, there is only one bond, so the bond dipole sets the molecular polarity. Homonuclear diatomic molecules such as Br2 and N2 have no electronegativity difference, so their dipole moment is zero. Heteronuclear molecules such as CO have a small dipole moment, and HF has a larger one because its electronegativity difference is larger.

Molecular geometry can make polar bonds cancel. CO2 is linear, so its two polar C=O bond moments point in opposite directions and cancel. The molecule is nonpolar even though its bonds are polar. Water is different. Its Lewis structure shows two bonds to oxygen, and each bond has a nonzero dipole moment. Because the molecule is bent, the bond moments do not cancel. Water therefore has a net dipole moment and is a polar molecule.

How Bond Polarity Shapes Molecular Dipoles

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bond polarity, dipole moment, and percent ionic character

Bond polarity depends on electronegativity, the ability of an atom to attract shared electrons. The absolute value of the electronegativity difference, or ΔEN, gives a rough guide to bond type. When the difference is very small or zero, the bond is covalent and nonpolar. When it is larger, the bond may be polar covalent or ionic. Examples show how this works in real compounds. H–H has a ΔEN of 0, so it is nonpolar. H–Cl has a ΔEN of 0.9, so it is polar covalent. Na–Cl has a ΔEN of 2.1, so it...

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Learn how electronegativity, bond dipoles, and molecular shape determine whether a bond or molecule is polar, using examples like HCl, CO2, and water.

How Bond Polarity Shapes Molecular Dipoles | JoVE K12

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How Bond Polarity Shapes Molecular Dipoles

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