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

trends-in-lattice-energy-ion-size-and-charge

Trends in Lattice Energy: Ion Size and Charge

ترتبط الطاقة الشبكية بتكوين أو انفصال الشبكة الأيونية. ومع ذلك،عندما يتكون كلوريد الصوديوم أو أكسيد المغنيسيوم،تختلف طاقتهم الشبكية بشكل كبير. لماذا لكل مركب أيوني شبكة مختلفة الطاقة وما هي العوامل التي تعتمد عليها؟يتكون المركب الأيوني من ترتيب منتظم لعدد كبير من الأيونات المشحونة،تنجذب إلى بعضها البعض عن طريق التفاعلات الكهروستاتيكية.وفقًا لقانون كولوم،الطاقة الكامنة لاثنين من الأيونات يتناسب عكسيا مع المسافة بين الأيونات،والتي بدورها تعتمد على نصف القطر الأيوني. في الجدول الدوري نصف القطر الأيوني،للفلزات الأرضية القلوية والقلويات،يزيد أسفل العمود. كلما زاد حجم أيون المعدن،تصبح المسافة بين الأيونات،أو طول الرابطة،أكبر كذلك.على سبيل المثال،طول رابطة بروميد الليثيوم وبروميدالبوتاسيوم،تختلف ما بين 217 م و 282 م،على التوالي. بسبب زيادة المسافة بين النوى،يتناقص التجاذب بين الأيونات ويصبح من الأسهل بكثير فصل الأيونات. وبالتالي،فإن الطاقة الشبكية لفصل بروميد الليثيوم الصلب أكبر من بروميد البوتاسيوم بقيمة 807 كيلوجول مول،مقابل 682 كيلوجول مول،على التوالي.بالإضافة إلى نصف القطر الأيوني،فإنّمقدار الطاقة الشبكية يعتمد أيضًا على شحنة الأيونات. وفقًا لقانون كولوم،الطاقة الكامنة للأيونات تتناسب طرديًا مع ناتج ضرب شحنتهم. لننظر في اثنين من المركبات الأيونية،فلوريد الصوديوم وأكسيد الكالسيوم.المسافة الأيونية في كلا المركبين متشابهة،لكن الطاقة الشبكية لأكسيد الكالسيوم،تساوي ما يقرب من أربع مرات أكبر من فلوريد الصوديوم. كل من الصوديوم والفلوريد عبارة عن أيونات أحادية التكافؤ؛ناتج ضرب شحنتهم هو 1. ومع ذلك،فإن أيونات الكالسيوم والأكسيد،ثنائية التكافؤ وناتج ضرب شحنتهم 4،وهو أربع مرات أكبر من فلوريد الصوديوم.هذا هو السبب في أنها تستهلك ما يقرب من أربعة أضعاف الطاقة لفصل أكسيد الكالسيوم إلى أيونات غازية بالمقارنة مع فلوريد الصوديوم. وبالتالي،فإن مقدار الطاقة الشبكية يتناسب طرديا مع ناتج ضرب الشحنات الأيونية،ويتناسب عكسيا مع المسافة بين الأيونات.

الاتجاهات في الطاقة الشبكية- حجم الأيون وشحنته

مركب أيوني مستقر بسبب الجاذبية الكهروستاتيكية بين أيونات موجبة وسالبة. الطاقة الشبكية لمركب هي مقياس لقوة هذا التجاذب. تُعرَّف طاقة شبكية (ΔHlattice) لمركب أيوني بأنها الطاقة المطلوبة لفصل مول واحد من المادة الصلبة عن أيونات الغازات المكونة له. بالنسبة لكلوريد الصوديوم الأيوني الصلب، فإن الطاقة الشبكية هي التغير في المحتوى الحراري للعملية: <img alt="Eq1" src="https://www.jovecore.com/CDNSource/lessons/1058/1058_Equations-01.png" style="height: 40px;" /><h4>الاتفاقيات </h4>هنا، يتم استخدام الإتفاقية حيث يتم فصل الصلب الأيوني إلى أيونات، مما يعني أن طاقات شبكية ستكون ماصة للحرارة (قيم موجبة). ثمة طريقة أخرى لاستخدام تقليد مكافئ لكن معاكس، حيث تكون طاقة الشبكة طاردة للحرارة (قيم سالبة)، ويُوصف بأنها الطاقة التي يتم إطلاقها عندما تتحد الأيونات لتكوين شبكية. لذلك، تأكد من تحديد التعريف المستخدم عند البحث عن مصادر شبكية في مرجع آخر. في كلتا الحالتين، يشير الحجم الأكبر للطاقة الشبكية إلى مركب أيوني أكثر ثباتًا. بالنسبة لكلوريد الصوديوم، تكون قيمة Hlattice = 769 كيلوجول. وبالتالي، يتطلب الأمر استخدام 769 كيلوجول لفصل مول واحد من NaCl الصلب إلى أيونات غازية Na+ و Cl–. عندما تتكون أيونات من أيونات غازية من نوع Na+ و Cl– من NaCl صلب، يتم تحرير 769 كيلوجول من الحرارة. <h4>قانون كولومب’ والطاقة الشبكية </h4>الطاقة الشبكية ΔHlattice لبلورة أيونية يمكن التعبير عنها بالمعادلة التالية (المستمدة من قانون كولومب’، الذي يحكم القوى بين الشحنات الكهربائية):  ΔHlattice =  C(Z +)(Z−)/Ro حيث C ثابت يعتمد على نوع البنية البلورية؛Z+ و Z– هي الشحنات على الأيونات، و Ro هو المسافة بين الأيونات (مجموع شعاع الأيونات الموجبة والسالبة). وبالتالي، تزداد الطاقة الشبكية للكريستال الأيوني بسرعة مع زيادة شحنات الأيونات وانخفاض أحجام الأيونات. عندما يتم الحفاظ على ثبات جميع المعلمات الأخرى، فإن مضاعفة شحن كل من الشحونَين إلى أربعة أضعاف الطاقة الشبكية.  <h4>أمثلة </h4><ol><li>تبلغ طاقة شبكية LiF (Z+ و Z– = 1) هي 1023 كيلوجول/مول، بينما MgO (Z+ و Z– = 2) هي 3900 كيلوجول/مول (Ro هي نفسها — تقريباً حوالي 200 pm لكلتا المركبين). </li><li> تنتج المسافات بين الذرات المختلفة طاقات شبكية مختلفة. على سبيل المثال، قارن طاقة شبكية MgF2 (2957 كيلوجول/مول) بـ MgI2 (2327 كيلوجول/مول) لملاحظة التأثير على طاقة شبكية بحجم أيوني أصغر من FF– مقارنة بـ I–.</li><li>جوهرة الياقوت الثمينة هي أكسيد الألومنيوم، Al2O3، التي تحتوي على آثار Cr3+. يُستخدم المركّب Al2Se3 في تصنيع بعض أجهزة أشباه الموصلات. في هذين المركبين الأيونيين، تكون الشحنات Z+ و Z– هي نفسها، لذا يعتمد الاختلاف في طاقة شبكية على Ro. بما أن الأيون O2– أصغر من الأيون Se2– فإن Al2O3 له مسافة أيونية أقصر من Al2Se3، وبالتالي، لديه طاقة شبكية أكبر. </li><li>ومن الأمثلة الأخرى أكسيد الزنك، ZnO، مقارنة بـ NaCl. لدى ZnO طاقة شبكية أكبر لأن قيم Z لكلٍ من الكاتيون والأنيون في ZnO أكبر، والمسافة الأيونية بين ZnO أصغر من قيمة NaCl. </li></ol>تم اقتباس هذا النص من <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>

المركب الأيوني مستقر بسبب التجاذب الكهروستاتيكي بين الأيونات الموجبة والسالبة. الطاقة الشبكية للمركب هي مقياس ...

Education

JoVE Core

الكيمياء

واحد

Chemical Bonding: Basic Concepts

الترابط الكيميائي: مفاهيم أساسية

KEY TERMS AND CONCEPTS

المصطلحات والمفاهيم الأساسية

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...

the born-haber cycle

Predicting Ionic Stability with Lattice Energy

Lattice energy helps explain why ionic compounds are stable. It measures the strength of attraction between positive and negative ions in a crystal. In one common definition, lattice energy is the energy required to separate one mole of an ionic solid into gaseous ions, so it has a positive value. Another definition uses the opposite sign and describes the energy released when gaseous ions form a lattice. When checking data, it is important to confirm which convention is being used. In either...

lewis symbols and the octet rule

Valence Electrons, Lewis Symbols, and Bonding

Chemical bonds form when atoms or ions interact in ways that lower the potential energy of a molecule. Gilbert N. Lewis created a simple model to show bond formation using valence electrons, the electrons in the outer shell. In this model, electrons are shared or transferred to help atoms reach a stable electron configuration. The Lewis model helps describe two common bond types. An ionic bond forms when electrons move from a metal to a nonmetal. A covalent bond forms when two nonmetals share...

electronegativity

Electronegativity and Polar Bonds

Electronegativity helps explain why some covalent bonds are nonpolar and others are polar covalent. It is a measure of how strongly an atom attracts shared electrons toward itself. That pull controls how electron density is distributed in a bond. Linus Pauling proposed the first electronegativity values by studying bond energies in heteronuclear molecules such as hydrogen fluoride. He expected the bond energy of HF to be about the average of the bond energies of H2 and F2, or 296 kJ/mol. The...

ionic bonding and electron transfer

Ionic Compounds and Crystal Lattices

Ionic compounds form when positive and negative ions attract each other. A cation is a positive ion, and it forms when an atom loses one or more valence electrons. An anion is a negative ion, and it forms when an atom gains one or more valence electrons. Compounds made of these ions are called ionic compounds, or salts, and the force between them is an ionic bond. The properties of ionic solids help show how strong this attraction is. They usually form rigid, brittle crystals and have high...

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

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...

lewis structures of molecular compounds and polyatomic ions

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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...

resonance

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...

formal charges

Lewis Structures with Formal Charge

Lewis structures can sometimes show more than one reasonable arrangement for a molecule or polyatomic ion. Formal charge helps chemists choose the best Lewis structure when that happens. It is a useful way to compare possible structures in chemistry. Formal charge is the hypothetical charge an atom would have if bonding electrons were shared evenly between the atoms. It can also be found by starting with the valence electrons of the neutral atom, subtracting the nonbonding electrons, and then...

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,...

bond energies and bond lengths

How Bond Energy Predicts Reaction Heat

Bond energy helps explain why molecules stay together and how much heat a reaction may release or absorb. A covalent bond is stronger when more energy is needed to separate the atoms. The energy needed to break one specific covalent bond in one mole of gaseous molecules is called bond energy, or bond dissociation energy. For a diatomic molecule, bond energy is the standard enthalpy change for an endothermic reaction that breaks that bond. The H-H bond is a common example. Its bond energy is...

bonding in metals

Electron Sea Model in Metals

Electron sea model explains how metallic bonding holds metals together. In this model, most metal atoms do not have enough valence electrons to form ionic or covalent bonds in the usual way. Their valence electrons are held loosely because metals have low electronegativity, and their ionization energy is low, so electrons are removed easily. When a metal atom loses these outer electrons, it becomes a positively charged metal ion. The freed electrons form a delocalized electron cloud around...

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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Ohio’s Learning Standards and Model Curriculum

Structure And Properties Of Matter

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CH.3

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Bonding Types: From Nonpolar Covalent to Ionic

Scientific Laws and Theories

Scientific Laws

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The Scientific Method

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Classifying Matter by State

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Classifying Matter by Composition

Matter: Pure Substances and Mixtures
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Subatomic Particles

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Use models to explain how the scientific understanding of atomic structure has evolved.

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Radioactivity and Nuclear Equations

Nuclear chemistry is the study of reactions that involve changes in nuclear structure. The nucleus of an atom is composed of protons and, except for ...

Types of Radioactivity

The most common types of radioactivity are &#945; decay, &#946; decay, &#947; decay, neutron emission, and electron capture.
Alpha (&#945;) decay is the ...

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The difference between the calculated and experimentally measured masses is known as the mass defect of the atom. In the case of helium-4, the mass defect ...

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Radioactivity is a spontaneous disintegration of an unstable nuclide and is a random process, as all the nuclei in the sample do not decay simultaneously. ...

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Many heavier elements with smaller binding energies per nucleon can decompose into more stable elements that have intermediate mass numbers and larger ...

Nuclear Power

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The process of converting very light nuclei into heavier nuclei is also accompanied by the conversion of mass into large amounts of energy, a process ...

Nuclear Transmutation

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Use models to compare nuclear reactions including alpha decay, beta decay and gamma decay; nuclear fusion and nuclear fission.

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The Energies of Atomic Orbitals

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The Aufbau Principle and Hund's Rule

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The alkali metal sodium (atomic number 11) has one more electron than the neon atom. This electron must go into the lowest-energy subshell available, the ...

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PS.Chm.1.3

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Molar Mass

The identity of a substance is defined not only by the types of atoms or ions it contains but by the quantity of each type of atom or ion. For example, ...

Use the Periodic Table as a model to predict the relative properties of elements based on the pattern of valence electrons in the outermost energy levels of atoms.

PS.Chm.2.1

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Atomic Radii and Effective Nuclear Charge

The elements in groups of the periodic table exhibit similar chemical behavior. This similarity occurs because the members of a group have the same number ...

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PS.Chm.2.2

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Lattice Energy&#xA0;

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

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 ...

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

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

Electronegativity values of ...

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Bond Polarity

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Lewis Structures of Molecular Compounds and Polyatomic Ions

To draw Lewis structures for complicated molecules and molecular ions, it is helpful to follow a step-by-step procedure as outlined:


	Determine the ...

Resonance

The Lewis structure of a nitrite anion (NO2&minus;) may actually be drawn in two different ways, distinguished by the locations of the N-O and N=O ...

Formal Charges

In some cases, there are seemingly more than one valid Lewis structures for molecules and polyatomic ions. The concept of formal charges can be used to ...

Exceptions to the Octet Rule

Many covalent molecules have central atoms that do not have eight electrons in their Lewis structures. These molecules fall into three categories:


	...

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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