Name: lattice energy patterns in ionic solids
Uploaded: 2020-09-03T13:38:28.000Z
Duration: 2 min 54 s
Channel: JoVE

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

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Trends in Lattice Energy: Ion Size and Charge

Kafes enerjisi, iyonik bir kafesin oluşumu veya ayrılmasıyla ilişkilidir. Sodyum klorür veya magnezyum oksit oluştuğunda, kafes enerjileri önemli ölçüde farklılık gösterir. Her iyonik bileşiğin neden farklı bir kafes enerjisi vardır ve hangi bu enerji faktörlere bağlıdır?Bir iyonik bileşik, elektrostatik etkileşimlerle birbirine çekilen çok sayıda yüklü iyonun düzenli bir şekilde düzenlenmesinden oluşur. Coulomb yasasına göre, iki iyonun potansiyel enerjisi iyonlar arasındaki mesafeyle ters orantılıdır ve bu da iyon yarıçapına bağlıdır. Periyodik tabloda, alkali ve toprak alkali metallerin iyonik yarıçapı sütun boyunca artar.Metal iyonunun boyutu arttıkça iyonlar arasındaki mesafe veya bağ uzunluğu da artar. Örneğin, lityum bromür ve potasyum bromürün bağ uzunluğu sırasıyla 217 pikometre ve 282 pikometre arasında değişir. Artan çekirdek arası mesafe nedeniyle iyonlar arasındaki çekim azalır ve iyonları ayırmak çok daha kolay hale gelir.Bu nedenle, katı lityum bromürü ayırmak için kullanılan kafes enerjisi, sırasıyla 807 kilojul/mol'e karşılık 682 kilojul/mol olan potasyum bromürden daha büyüktür. İyonik yarıçapa ek olarak, kafes enerjisinin büyüklüğü de iyon yüklerine bağlıdır. Coulomb yasasına göre iyonların potansiyel enerjisi, yüklerinin çarpımı ile doğru orantılıdır.İki iyonik bileşik sodyum florür ve kalsiyum oksiti düşünün. Her iki bileşikteki iyonik mesafe benzerdir, ancak kalsiyum oksitin kafes enerjisi sodyum florürden neredeyse dört kat daha fazladır. Hem sodyum hem de florür tek değerlikli iyonlardır;yani yüklerinin çarpımı 1'dir.Bununla birlikte, kalsiyum ve oksit iyonları iki değerlidir ve yüklerinin çarpımı 4'tür, bu da sodyum florürün dört katıdır. Bu nedenle kalsiyum oksiti gaz iyonlarına ayırmak için sodyum florüre kıyasla yaklaşık dört kat daha fazla enerji gerekir. Dolayısıyla, kafes enerjisinin büyüklüğü, iyon yüklerinin çarpımı ile doğru orantılıdır ve iyonlar arasındaki mesafe ile ters orantılıdır.

Örgü enerjisindeki trendler İyon boyutu ve yükü

Bir iyonik bileşik, pozitif ve negatif iyonları arasındaki elektrostatik çekim nedeniyle stabildir. Bir bileşiğin örgü enerjisi, bu çekimin gücünün bir ölçüsüdür. Bir iyonik bileşiğin örgü enerjisi (ΔHörgü (ΔHlattice)), bir mol kristali gaz haldeki iyonlarına ayrıştırmak için gerekli olan enerji olarak tanımlanır. İyonik katı sodyum klorür için örgü enerjisi, sürecin entalpi değişimidir:
 
 <img alt="Eq1" src="https://www.jovecore.com/CDNSource/lessons/1058/1058_Equations-01.png" style="height: 40px;" />
 
 <h4>Konvansiyon</h4>
 
 Burada, iyonik katının iyonlara ayrıldığı, yani örgü enerjilerinin endotermik olacağı (pozitif değerler) konvansiyon kullanılır. Başka bir yol, eşdeğer ancak zıt bir kural kullanmaktır, burada örgü enerjisi ekzotermiktir (negatif değerler) ve iyonlar bir örgü oluşturmak için birleştiğinde açığa çıkan enerji olarak tanımlanır. Bu nedenle, başka bir referanstaki örgü enerjilerine bakarken hangi tanımın kullanıldığını doğruladığınızdan emin olun. Her iki durumda da, örgü enerjisi için daha büyük bir büyüklük, daha kararlı bir iyonik bileşiği gösterir. Sodyum klorür için ΔHörgü = 769 kJ. Bu nedenle, bir mol katı NaCl'yi gaz halindeki Na+ ve Cl– iyonlarına ayırmak 769 kJ gerektirir. Gaz halindeki Na+ ve Cl– iyonlarının her biri bir mol katı NaCl oluşturduğunda 769 kJ ısı açığa çıkar.
 
 <h4>Coulomb Yasası ve Örgü Enerjisi</h4>
 
 Bir iyonik kristalin örgü enerjisi ΔHörgü, aşağıdaki denklemle ifade edilebilir (Coulomb yasasından türetilen, elektrik yükleri arasındaki kuvvetleri yöneten): 
 
 ΔHörgü =  C(Z +)(Z−)/Ro 
 
 burada C, kristal yapının tipine bağlı olan bir sabittir; Z+ ve Z– iyonlar üzerindeki yüklerdir ve Ro interiyonik mesafedir (pozitif ve negatif iyonların yarıçaplarının toplamı). Bu nedenle, bir iyonik kristalin örgü enerjisi, iyonların yükleri arttıkça ve iyonların boyutları küçüldükçe hızla artar. Diğer tüm parametreler sabit tutulduğunda, hem katyon hem de anyonun yükünü ikiye katlamak, örgü enerjisini dört katına çıkarır. 
 
 <h4>Örnekler</h4>
 
 <ol>
 <li>LiF'nin (Z+ ve Z– = 1) örgü enerjisi 1023 kJ/mol iken, MgO'nun (Z+ ve Z– = 2) 3900 kJ/mol (Ro neredeyse aynıdır — her iki bileşik için yaklaşık 200 pm).</li>
 <li>Farklı atomlararası mesafeler farklı örgü enerjileri üretir. Örneğin, I– ile karşılaştırıldığında daha küçük iyonik F– boyutunun örgü enerjisi üzerindeki etkisini gözlemlemek için MgF2'nin (2957 kJ/mol) örgü enerjisini MgI2'ninkiyle (2327 kJ/mol) karşılaştırın.</li>
 <li>Değerli taş yakut, Cr+3 izleri içeren alüminyum oksit, Al2O3'tür. Al2Se3 bileşiği, bazı yarı iletken cihazların imalatında kullanılır. Bu iki iyonik bileşikte, Z+ ve Z– yükleri aynıdır, dolayısıyla örgü enerjisindeki fark Ro'ya bağlıdır. O2– iyonu Se2– iyonundan daha küçük olduğu için, Al2O3, Al2Se3'ten daha kısa bir interiyonik mesafeye ve dolayısıyla daha büyük örgü enerjisine sahiptir.</li>
 <li>Başka bir örnek, NaCl ile karşılaştırıldığında çinko oksit, ZnO'dur. ZnO daha büyük bir örgü enerjisine sahiptir çünkü ZnO'daki hem katyon hem de anyonun Z değerleri daha büyüktür ve ZnO'nun interiyonik mesafesi NaCl'ninkinden daha küçüktür.</li>
 </ol>
 
 Bu metin bu kaynaktan uyarlanmıştır: <a href="https://openstax.org/books/chemistry-2e/pages/7-5-strengths-of-ionic-and-covalent-bonds">Openstax, Chemistry 2e, Section 7.5: Strengths of Ionic and Covalent Bonds.</a>

Örgü Enerjisindeki Trendler İyon Boyutu ve Yükü

İyonik bir bileşik, pozitif ve negatif iyonları arasındaki elektrostatik çekim nedeniyle kararlıdır. Bir bileşiğin kafes enerjisi bir ölçüdür ...

Education

JoVE Core

Kimya

Chemical Bonding: Basic Concepts

Kimyasal Bağlanma: Temel Kavramlar

KEY TERMS AND CONCEPTS

TEMEL TERİMLER VE KAVRAMLAR

lattice energy patterns in ionic solids

Lattice energy shows how strongly ions hold an ionic solid together. It is the energy required to separate one mole of a solid into its gaseous ions. For sodium chloride, this process requires 769 kJ per mole. The opposite convention may also be used, where lattice energy is the energy released when gaseous ions form the solid. In either case, a larger magnitude means a more stable ionic compound.

For ionic crystals, lattice energy follows a pattern based on charge and ion size. The relationship can be written as ΔH lattice = C(Z+)(Z−)/Ro. In this equation, C depends on the crystal structure, Z+ and Z− are the ion charges, and Ro is the distance between the ions. Because of this, lattice energy rises quickly when ion charges increase and when ion sizes decrease. If both ion charges double, the lattice energy becomes four times larger.

Examples show these trends clearly. LiF, with ion charges of 1 and 1, has a lattice energy of 1023 kJ/mol, while MgO, with charges of 2 and 2, has a lattice energy of 3900 kJ/mol. Their interionic distances are nearly the same, at about 200 pm. Ion size also matters. MgF2 has a lattice energy of 2957 kJ/mol, while MgI2 has a lower value of 2327 kJ/mol because F− is smaller than I−.

The same idea explains differences in other compounds. Ruby is aluminum oxide, Al2O3, and it contains traces of Cr3+. Al2Se3 is used in some semiconductor devices. These compounds have the same ion charges, so the difference in lattice energy depends on Ro. O2− is smaller than Se2−, so Al2O3 has the shorter interionic distance and the larger lattice energy. ZnO also has a larger lattice energy than NaCl because the ion charges are greater and the interionic distance is smaller.

Lattice Energy Patterns in Ionic Solids

types of chemical bonds

Chemical Bonding and Bond Properties

Chemical bonding explains how atoms and ions join to form molecules and compounds. American chemist Gilbert N. Lewis pioneered chemical bonding theory with the Lewis model. This model helps explain why bonds form, why some are stronger than others, and why compounds have fixed formulas like H2O instead of H4O. Ionic bonding involves ions, which are atoms or molecules with an electrical charge. A cation is a positive ion formed when a neutral atom loses one or more electrons from its valence...

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ionic bonding and electron transfer

Ionic Compounds and Crystal Lattices

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trends in lattice energy: ion size and charge

Lattice energy shows how strongly ions hold an ionic solid together. It is the energy required to separate one mole of a solid into its gaseous ions. For sodium chloride, this process requires 769 kJ per mole. The opposite convention may also be used, where lattice energy is the energy released when gaseous ions form the solid. In either case, a larger magnitude means a more stable ionic compound. For ionic crystals, lattice energy follows a pattern based on charge and ion size. The...

covalent bonding and lewis structures

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...

bond polarity, dipole moment, and percent ionic character

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How Bond Polarity Shapes Molecular Dipoles

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lewis structures of molecular compounds and polyatomic ions

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Drawing Lewis Structures with Valence Electron Counts

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Resonance Forms in Lewis Structures

Resonance forms in Lewis structures help explain molecules and ions that cannot be shown correctly with just one drawing. In nitrite ion, NO2−, the Lewis structure can be drawn in two ways. The N-O and N=O bonds switch positions in the two drawings, but the atoms stay in the same arrangement. If nitrite really had one single bond and one double bond, the two bond lengths should be different. A double bond is shorter and stronger than a single bond between the same atoms. Experiments show that...

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exceptions to the octet rule

Octet Rule Exceptions in Lewis Structures

Some covalent molecules do not follow the octet rule in their Lewis structures. Their central atoms can fall into three groups: odd-electron molecules, electron-deficient molecules, and hypervalent molecules. These cases show why a Lewis structure may not always give every atom eight valence electrons. Odd-electron molecules have an odd number of valence electrons, so one electron remains unpaired. Molecules with an odd number of electrons are called radicals. Nitric oxide, NO, is one example,...

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key terms and concepts

Learn how ion charge and ion size affect lattice energy in ionic solids, with examples like NaCl, LiF, MgO, MgF2, MgI2, Al2O3, and ZnO.

Lattice Energy Patterns in Ionic Solids | JoVE K12

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Bonding Types: From Nonpolar Covalent to Ionic

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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.

Lattice Energy Patterns in Ionic Solids

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