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

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Trends in Lattice Energy: Ion Size and Charge

אנרגיית סריג קשורה ליצירה או לפירוק של סריג יוני. עם זאת, כאשר נוצרים נתרן כלורי או תחמוצת מגנזיום, אנרגיית הסריג שלהם שונה משמעותית. למה לכל תרכובת יונית יש אנרגיית סריג אחרת, ובאילו גורמים זה תלוי?תרכובת יונית מורכבת ממערך מסודר של מספר רב של יונים טעונים הנמשכים זה לזה באינטראקציות אלקטרוסטטיות. על פי חוק קולון, אנרגיה פוטנציאלית של שני יונים היא ביחס הפוך למרחק בין היונים, שתלוי ברדיוס היוני. בטבלה המחזורית, הרדיוס היוני של מתכות אלקליות ומתכות אלקליות עפרוריות גדל במורד הטור.ככל שיון המתכת גדל, המרחק בין היונים, או אורך הקשר, גדל אף הוא. לדוגמה, אורך הקשר של ליתיום ברומיד ואשלגן ברומיד משתנה בין 217 ל-282 פיקומטרים, בהתאמה. בגלל המרחק הבין גרעיני הגדל, המשיכה בין היונים פוחתת ונעשה הרבה יותר קל להפריד בין היונים.לכן אנרגיית הסריג הנדרשת להפרדת ליתיום ברומיד מוצק גדולה יותר מהאנרגיה הנדרשת לברומיד אשלגן, 807 לעומת 682 קילוג'ול למול, בהתאמה. בנוסף לרדיוס היוני, עוצמתה של אנרגיית הסריג תלויה גם במטענים היוניים. לפי חוק קולון, האנרגיה הפוטנציאלית של יונים עומדת ביחס ישר למכפלת המטענים שלהם.לדוגמה, שתי תרכובות יוניות של נתרן פלואוריד ותחמוצת הסידן. המרחק היוני בשתי התרכובות הוא דומה, אבל אנרגיית הסריג של תחמוצת הסידן גדולה כמעט פי ארבעה משל נתרן פלואוריד. גם נתרן וגם פלואוריד הם יונים חד-ערכיים;מכפלת המטען שלהם הוא 1.אך יוני סידן תחמוצת הם דו-ערכיים ומכפלת המטען שלהם הוא 4, גדול פי ארבעה מנתרן פלואוריד. לכן נדרשת אנרגיה רבה כמעט פי ארבעה כדי להפריד את תחמוצת הסידן ליונים גזיים בהשוואה לנתרן פלואוריד. לכן, עוצמתה של אנרגיית הסריג עומדת ביחס ישר למכפלה של מטעני היונים וביחס הפוך למרחק בין היונים.

מגמות באנרגיית הסריג: גודל ומטען של היונים

<div style="direction:rtl">

תרכובת יונית יציבה בגלל המשיכה האלקטרוסטטית בין היונים החיוביים והשליליים שלה. אנרגיית הסריג של תרכובת היא מדד לחוזקה של משיכה זו. אנרגיית הסריג (ΔHlattice) של תרכובת יונית מוגדרת כאנרגיה הנדרשת להפרדת מול אחד של המוצק ליונים הגזים המרכיבים אותו. עבור נתרן כלורי מוצק יוני, אנרגיית הסריג היא שינוי האנתלפיה של התהליך: <img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/1058/1058_Equations-01.png" style="height: 40px;"> <h4>מוסכמה</h4> 

כאן, נעשה שימוש במוסכמה שבה המוצק היוני מופרד ליונים, כלומר אנרגיות הסריג יהיו אנדותרמיות (ערכים חיוביים). דרך נוספת היא להשתמש במוסכמה מקבילה אך הפוכה, שבה אנרגיית הסריג היא אקסותרמית (ערכים שליליים) ומתוארת כאנרגיה המשתחררת כאשר יונים מתחברים ליצירת סריג. לפיכך, הקפד לאשר באיזו הגדרה נעשה שימוש בעת חיפוש אנרגיות סריג בהתייחסות אחרת. בשני המקרים, גודל גדול יותר עבור אנרגיית הסריג מצביע על תרכובת יונית יציבה יותר. עבור נתרן כלורי, ΔHlattice = 769 kJ. לפיכך, זה דורש 769 קילו-ג'ול כדי להפריד מול אחד של NaCl מוצק ליוני Na+ ו- Cl– גזיים. כאשר מול אחד של יוני Na+ ו- Cl– גזי יוצרים NaCl מוצק, 769 קילו-ג'ול של חום משתחרר. <h4>חוק קולון ואנרגיית הסריג</h4> 

ניתן לבטא את אנרגיית הסריג ΔHlattice של קריסטל יוני באמצעות המשוואה הבאה (שנגזרת מחוק קולון, השולט בכוחות בין מטענים חשמליים): ΔHlattice = C(Z +)(Z−)/Ro 

שבו C הוא קבוע התלוי בסוג מבנה הקריסטל; Z+ ו-Z– הם המטענים על היונים, ו-Ro הוא המרחק האינטריוני (סכום הרדיוסים של היונים החיוביים והשליליים). לפיכך, אנרגיית הסריג של קריסטל יוני עולה במהירות ככל שמטענים של היונים גדלים, וגדלים של היונים יורדים. כאשר כל שאר המאפיינים נשמרים קבועים, הכפלת המטען של הקטיון והאניון מכפילה פי ארבע את אנרגיית הסריג. 
<h4>דוגמאות</h4> 

<ol style="padding-right: 35px; margin: 0;"> 

 <li style="text-align: right;">אנרגיית הסריג של LiF (Z+ ו-Z– = 1) היא 1023 קילו-ג'ול/מול, ואילו זו של MgO (Z+ ו-Z– = 2) היא 3900 קילו-ג'ול/מול (Ro כמעט זהה - בערך 200 pm עבור שתי התרכובות) .</li> 
 <li style="text-align: right;">מרחקים בין-אטומיים שונים מייצרים אנרגיות סריג שונות. לדוגמה, השווה את אנרגיית הסריג של MgF2 (2957 קילו-ג'ול/מול) לזו של MgI2 (2327 קילו-ג'ול-מול) כדי לראות את ההשפעה על אנרגיית הסריג של הגודל היוני הקטן יותר של F– בהשוואה ל-I–.</li> 
 <li style="text-align: right;">אבן חן היקרה היא תחמוצת אלומיניום, Al2O3, המכילה עקבות של Cr3+. התרכובת Al2Se3 משמשת בייצור של כמה התקנים מוליכים למחצה. בשתי תרכובות יוניות אלו, המטענים Z+ ו-Z– זהים, כך שההבדל באנרגיית הסריג תלוי ב-Ro. מכיוון שיון O2– קטן יותר מיון Se2–, ל- Al2O3 יש מרחק פנימי קצר יותר מ- Al2Se3, ולכן יש לו אנרגיית סריג גדולה יותר.</li> 
 <li style="text-align: right;">דוגמה נוספת היא תחמוצת אבץ, ZnO, בהשוואה ל-NaCl. ל-ZnO יש אנרגיית סריג גדולה יותר מכיוון שערכי ה-Z של הקטיון וגם של האניון ב-ZnO גדולים יותר, והמרחק האינטריוני של ZnO קטן מזה של NaCl.</li> </ol> 

טקסט זה מותאם מ <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></div>

תרכובת יונית היא יציבה בגלל המשיכה האלקטרוסטטית בין היונים החיוביים והשליליים שלה. אנרגיית הסריג של תרכובת היא מדד ...

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Chemical Bonding: Basic Concepts

קשרים כימיים: מושגים בסיסיים

KEY TERMS AND CONCEPTS

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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...

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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...

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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...

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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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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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Bonding Types: From Nonpolar Covalent to Ionic

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Nuclear Binding Energy

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 ...

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The Pauli Exclusion Principle

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The Energies of Atomic Orbitals

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The Aufbau Principle and Hund's Rule

To determine the electron configuration for any particular atom, we can build the structures in the order of atomic numbers. Beginning with hydrogen, and ...

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Electron Configuration of Multielectron Atoms

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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Periodic Classification of the Elements

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The Periodic Table

As early chemists discovered more elements, they realized that various elements could be grouped by their similar chemical behaviors. One such grouping ...

Atomic Mass

Atoms &mdash; and the protons, neutrons, and electrons that compose them &mdash; are extremely small. For example, a carbon atom weighs less than 2 ...

Molar Mass

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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 ...

Ionic Radii

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Ionization Energy

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Electron Affinity

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PS.Chm.2.2

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Lewis Symbols and the Octet Rule

Chemical bonds are complex interactions between two or more atoms or ions, which reduce the potential energy of the molecule. Gilbert N. Lewis developed a ...

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The Born-Haber Cycle

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 ...

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 ...

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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