Name: ionic compounds and crystal lattices
Uploaded: 2020-09-03T13:38:28.000Z
Duration: 2 min 48 s
Channel: JoVE

K12 Standards

north-carolina-k-12-science-standard-course-of-study

North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.3.1

Ionic Bonding and Electron Transfer

Ýyonik baðlar, elektronlarýn metallerden ametallere aktarýlmasýyla oluþur. Elektronlarýn paylaþýldýðý kovalent baðlarla karþýlaþtýrýldýðýnda, iyonik baðlarda metaller kaybetme ve ametaller elektronlarý kabul etme eðilimindedir ama neden? Bir atomun en kararlý elektron konfigürasyonu tam oktet formudur.Potansiyel enerjileri düþürmekle birlikte bu duruma ulaþmak, bað oluþumu için önemli bir itici güçtür. Fakat elektronlarýn ne zaman transfer edilip paylaþýlmayacaðýný nasýl tahmin edebiliriz? Bunun için iyonlaþma enerjilerini ve atomlarýn elektron afinitelerini inceleriz.Periyodik tablodaki s-blok metallerin iyonlaþma enerjileri düþüktür. Bu, ayný anda katyonlar oluþtururken elektronlarýn oktete ulaþmasýný kolaylaþtýrýr. Aksine, soy gazlar dýþýnda p-bloðundan gelen ametaller yüksek elektron ilgisine sahiptir ve anyon oluþturmak için elektronlarý kolayca kabul eder.Zýt yüklü katyonlar ve anyonlar, iyonik baðlar oluþturmak için birbirlerini çekerek güçlü elektrostatik etkileþimler yaþarlar. Ýyonik bileþikler, iyonlar arasýndaki güçlü elektrostatik çekim nedeniyle genellikle yüksek erime noktalarýna sahip sert ve iyi tanýmlanmýþ kristal yapýlar oluþturur. Lityum ve flordan oluþan iyonik bir bileþik olan lityum florürü ele alalým.Lityum, bir ikili halinde lityum katyonu olmak için bir elektron kaybettiðinde, elektron flor tarafýndan alýnýr ve oktet halindeki bir anyon oluþturur. Coulomb yasasýna göre, bu iki yüklü parçacýk nötr bir bileþik olan Lityum florürü oluþturmak üzere birbirlerine çekilir. Lewis modeli, iyonik bileþiklerin kimyasal formülünü tanýmlamak ve tahmin etmek için kullanýlabilir.Lewis sembolü sað üst köþedeki yükleri gösterir ve parantez içinde yazýlý sembolle anyonlarý ve katyonlarý gösterir. Havai fiþeklerde parlak kýrmýzý bir renk elde etmek için yaygýn olarak kullanýlan bir tuz olan stronsiyum klorürü düþünelim. Stronsiyum için Lewis sembolünde iki, klorda ise bir eþleþmemiþ elektron bulunur.Stronsiyumun iki elektron kaybetmesi gerekirken, klorun bir oktete ulaþmak için bir elektron kazanmasý gerekir. Bu nedenle, bir stronsiyum katyonu 1:2 oranýnda iki klorür anyonuna baðlanýr.

İyonik bağ ve elektron transferi

İyonlar, elektrik yükü taşıyan atomlar veya moleküllerdir. Nötr atomun, değerlik kabuğundan bir veya daha fazla elektronu kaybettiğinde bir katyon (pozitif iyon) formu ve nötr atomun değerlik kabuğunda bir veya daha fazla elektron kazandığında bir anyon (negatif iyon) formu oluşur. İyonlardan oluşan bileşiklere iyonik bileşikler (veya tuzlar) denir ve bunları oluşturan iyonlar iyonik bağlarla bir arada tutulur: zıt yüklü katyonlar ve anyonlar arasındaki elektrostatik çekim kuvvetleri. 
 
 <h4>İyonik Bileşiklerin Özellikleri</h4>
 
 İyonik bileşiklerin özellikleri iyonik bağların doğasına ışık tutar.
 
 <ul>
 <li>İyonik katılar kristal bir yapı sergilerler ve sert ve kırılgan olma eğilimindedirler; ayrıca yüksek erime ve kaynama noktalarına sahip olma eğilimindedirler, bu da iyonik bağların çok güçlü olduğunu gösterir. </li>
 <li>İyonik katılar da aynı nedenle zayıf elektrik iletkenleridir — iyonik bağların gücü iyonların katı halde serbestçe hareket etmesini önler. </li>
 <li>Bununla birlikte, iyonik katıların çoğu suda kolayca çözülür. Çözündükten veya eritildikten sonra, iyonik bileşikler mükemmel elektrik ve ısı iletkenleridir, çünkü iyonlar serbestçe hareket edebilir.</li>
 </ul>
 
 <h4>İyonik Bileşiklerin Oluşumu</h4>
 
 Birçok metalik element nispeten düşük iyonlaşma potansiyellerine sahiptir ve elektronları kolayca kaybeder. Bu elemetler periyodik tabloda periyodların solunda ya da grupların alt tarafında bulunur. Ametal atomlar nispeten yüksek elektron afinitelerine sahiptir ve böylece metal atomları tarafından kaybedilen elektronları kolayca kazanırlar, böylece değerlik kabuklarını doldururlar. Ametalik elementler periyodik tablonun sağ üst köşesinde bulunur.
 
 Tüm maddeler elektriksel olarak nötr olması gerektiğinden, iyonik bir bileşiğin katyonları üzerindeki toplam pozitif yük sayısı, anyonları üzerindeki toplam negatif yük sayısına eşit olmalıdır. İyonik bir bileşiğin formülü, aynı sayıda pozitif ve negatif yük vermek için gerekli olan iyon sayılarının en basit oranını temsil eder. 
 
 <h4>İyonik Bileşikler Düzenli Ayarlanmış 3 Boyutlu Yapılar Oluşturur</h4>
 
 Bununla birlikte, bir iyonik bileşik formülünün iyonlarının fiziksel düzenlemesini temsil etmediğini not etmek önemlidir. Sodyum klorür (NaCl) "molekülü" nden bahsetmek yanlıştır çünkü herhangi bir spesifik sodyum ve klorür iyonu arasında tek bir iyonik bağ yoktur. İyonlar arasındaki çekici kuvvetler izotropiktir — her yönden aynıdır — yani herhangi bir iyon, yakınlardaki karşıt yükün tüm iyonlarına eşit derecede çekilir. Bu, iyonların kendilerini sıkı bir şekilde bağlanmış, üç boyutlu bir örgü yapısına yerleştirmesiyle sonuçlanır. Örneğin sodyum klorür, eşit sayıda Na+ katyonu ve Cl– anyonunun düzenli bir diziliminden oluşur. Na+ ve Cl– iyonları arasındaki güçlü elektrostatik çekim, onları katı NaCl içinde sıkıca bir arada tutar. Bir mol katı NaCl'yi ayrı gaz halindeki Na+ ve Cl– iyonlarına ayırmak için 769 kJ enerji gerekir. 
 
 <h4>Katyonların Elektronik Yapıları</h4>
 
 Bir katyon oluştururken, ana grup elementinin bir atomu, tüm değerlik elektronlarını kaybetme eğilimindedir, böylece periyodik tabloda kendisinden önce gelen soy gazın elektronik yapısına benzer. 
 
 <ul>
 <li>Grup 1 (alkali metaller) ve 2 (alkali toprak metalleri) için grup numaraları, tüm valans kabuğu elektronları çıkarıldığında bu elementlerin atomlarından oluşan katyonların yüklerine ve dolayısıyla valans kabuğu elektronlarının sayısına eşittir. </li>
 <li>Örneğin, kalsiyum, nötr atomları 20 elektrona ve 1s22s22p63s23p64s2 temel durum elektron konfigürasyonuna sahip olan bir grup 2 elementidir. Bir Ca atomu her iki valans elektronunu da kaybettiğinde, sonuç 18 elektronlu bir katyon, +2 yük ve 1s22s22p63s23p6 elektron konfigürasyonudur. Bu nedenle Ca2+ iyonu soy gaz Ar ile izoelektroniktir.</li>
 <li>13–17 grupları için, grup sayıları valans elektronlarının sayısını 10 aşar (dördüncü ve daha büyük periyotlardaki elementlerin atomlarında tüm d alt kabuklarının olasılığını hesaba katar). Dolayısıyla, tüm değerlik elektronlarının kaybıyla oluşan bir katyonun yükü, eksi 10 grup sayısına eşittir. Örneğin, alüminyum (grup 13'te) 3+ iyon (Al3+) oluşturur.</li>
 </ul>
 
 <h4>İstisnalar</h4>
 
 <ul>
 <li>Beklenen davranışın istisnaları, grupların altındaki elementleri içerir. </li>
 <li>Beklenen Tl3+, Sn4+, Pb4+, ve Bi5+ iyonlarına ek olarak, bu atomların valans kabuğu elektronlarının kısmi kaybı da Tl+, Sn2+, Pb2+, ve Bi3+ iyonlarının oluşumuna yol açabilir. Bu +1, +2, ve +3 katyonlarının oluşumu, 13, 14 ve 15 gruplarının ağır elementlerinin atomları için değerlik s-elektron çiftinin nispeten düşük enerjisini yansıtan inert çift etkisine atfedilir. </li>
 <li>Cıva (grup 12) de beklenmedik bir davranış sergiler: Beklenen monatomik iyon Hg+2'ye (yalnızca bir cıva atomundan oluşur) ek olarak bir diatomik iyon, Hg2+2 (bir Hg-Hg bağına sahip iki cıva atomundan oluşan bir iyon) oluşturur.</li>
 <li>Geçiş metali elemanları, ana grup elemanlarından farklı davranır. Çoğu geçiş metali katyonu, ilk önce en dıştaki s elektron(lar)ının kaybından kaynaklanan +2 veya +3 yüklere sahiptir, bunu bazen bir sonraki en dış kabuktan bir veya iki d elektronunun kaybı izler.</li>
 <li>Geçiş elemanlarının d orbitalleri—aufbau prensibine göre—elektron konfigürasyonları oluştururken en son doldurulan olmasına rağmen, en dıştaki s elektronları bu atomlar iyonlaştığında kaybedilen ilk elektronlardır. İç geçiş metalleri iyon oluşturduğunda, genellikle +3 yüke sahiptirler, bu da en dıştaki s elektronlarının ve bir d veya f elektronunun kaybından kaynaklanır.</li>
 </ul>
 
 <h4>Anyonların Elektronik Yapıları</h4>
 
 Monatomik anyonların çoğu, nötr bir ametal atom, dış s ve p orbitallerini tamamen doldurmak için yeterli elektron kazandığında oluşur ve böylece bir sonraki soy gazın elektron konfigürasyonuna ulaşır. Bu nedenle, böyle bir negatif iyon üzerindeki yükü belirlemek basittir: yük, ana atomun s ve p orbitallerini doldurmak için kazanılması gereken elektron sayısına eşittir. Örneğin oksijen 1s22s22p4 elektron konfigürasyonuna sahiptir, oksijen anyonu soy gaz neonunun (Ne) elektron konfigürasyonuna 1s22s22p6 sahiptir. Değerlik orbitallerini doldurmak için gereken iki ek elektron, oksit iyonuna –2 yükünü verir (O–2).
 
 Bu metin bu kaynaktan uyarlanmıştır: <a href="https://openstax.org/books/chemistry-2e/pages/7-1-ionic-bonding">Openstax, Chemistry 2e, Section 7.3: Ionic Bonding.</a>

İyonik Bağ ve Elektron Transferi

İyonlar, elektrik yükü taşıyan atomlar veya moleküllerdir. Nötr bir atom değerliğinden bir veya daha fazla elektron kaybettiğinde bir katyon (pozitif bir iyon) oluşur ...

Education

JoVE Core

Kimya

Chemical Bonding: Basic Concepts

Kimyasal Bağlanma: Temel Kavramlar

KEY TERMS AND CONCEPTS

TEMEL TERİMLER VE KAVRAMLAR

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 melting and boiling points. They are also poor conductors of electricity in the solid state because the ions cannot move freely. Most ionic solids dissolve readily in water. When an ionic compound is melted or dissolved, it conducts electricity and heat well because the ions can move about freely.

Ionic compounds form most easily when metals lose electrons and nonmetals gain them. Many metals have low ionization potentials, so they lose electrons easily. These elements are found on the left side of the periodic table or near the bottom of a group. Nonmetals have high electron affinities, so they readily gain the electrons lost by metals. They are found in the upper-right corner of the periodic table.

Ionic compounds must remain electrically neutral. That means the total positive charge from the cations must equal the total negative charge from the anions. The formula of an ionic compound gives the simplest ratio of ions needed to balance charge. The formula does not show the physical layout of the ions. In solid sodium chloride, for example, the ions form a tightly bound three-dimensional lattice. The attraction between Na+ and Cl- ions is strong, and it takes 769 kJ of energy to separate one mole of solid NaCl into gaseous ions.

Main-group cations often form by losing all valence electrons and taking on the electron structure of the noble gas before them. For groups 1 and 2, the group number matches the number of valence electrons and also the charge of the ion formed. Calcium is a group 2 element. A neutral calcium atom has 20 electrons, and Ca2+ has 18 electrons with the same electron configuration as argon. For groups 13 through 17, the cation charge equals the group number minus 10. Aluminum, in group 13, forms Al3+.

Some heavy main-group elements do not follow the expected pattern exactly. Thallium, tin, lead, and bismuth can also form lower-charge ions such as Tl+, Sn2+, Pb2+, and Bi3+. This is explained by the inert pair effect, which reflects the relatively low energy of the valence s-electron pair in these heavy atoms. Mercury is another exception. It can form the diatomic ion Hg2^2+, which contains a Hg-Hg bond, as well as the monatomic ion Hg2+.

Transition metals and inner transition metals form ions in a different way. Most transition metal cations have 2+ or 3+ charges. These usually come from losing the outermost s electron or electrons first, and sometimes one or two d electrons after that. Even though d orbitals fill later according to the Aufbau principle, the outermost s electrons are lost first when transition metals ionize. Inner transition metals usually form 3+ ions by losing their outermost s electrons and one d or f electron.

Most monatomic anions form when a nonmetal atom gains enough electrons to fill its outer s and p orbitals. The charge on the ion equals the number of electrons needed to reach the next noble-gas electron configuration. Oxygen is a clear example. A neutral oxygen atom has the configuration 1s2 2s2 2p4. The oxide ion, O2-, has the neon configuration, 1s2 2s2 2p6, after gaining two electrons.

Ionic Compounds and Crystal Lattices

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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electronegativity

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ionic bonding and electron transfer

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

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

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...

covalent bonding and lewis structures

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bond polarity, dipole moment, and percent ionic character

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lewis structures of molecular compounds and polyatomic ions

lewis-structures-of-molecular-compounds-and-polyatomic-ions

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resonance

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formal charges

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exceptions to the octet rule

Octet Rule Exceptions in Lewis Structures

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key terms and concepts

Explore how ions form, why ionic compounds make crystal lattices, and how charge, conductivity, and electron configurations shape ionic behavior in chemistry.

Ionic Compounds and Crystal Lattices | JoVE K12

chemistry

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Physical Science

PS.PSc.2.1

Pennsylvania State Academic Standards

Structure and Properties of Matter

3.2.9-12.B

3.2.9-12.N

Louisiana Student Standards for Science

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Matter And Its Interactions

HS-PS1-3

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Ohio’s Learning Standards and Model Curriculum

Study Of Matter

Bonding and compounds

Structure And Properties Of Matter

Chemical bonding

Physical Geology

Minerals

Chemical bonding (ionic, covalent, metallic)

Tennessee Academic Standards

Matter and Its Interactions

CHEM1.PS1.13

CHEM1.PS1.14

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Motion and Stability: Forces and Interactions

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CH.3.d

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New Jersey Student Learning Standards for Science

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Florida Department of Education

SC.912.P.8

SC.912.P.8.6

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IPC.7

IPC.7.A

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New York State Science Learning Standards

HS. Structure and Properties of Matter

HS-PS1-3.

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Georgia Standards of Excellence

SPS2.

Chemical Bonds

SC2.

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Bonding Types: From Nonpolar Covalent to Ionic

Scientific Laws and Theories

Scientific Laws

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The Scientific Method

Chemistry is an empirical science. Scientists often pose questions to understand the chemistry in everyday life and seek answers to these questions. To ...

Classifying Matter by State

Chemistry is the study of matter and the changes it undergoes. Matter is anything that has mass and occupies space. Matter is all around us; the air, ...

Classifying Matter by Composition

Matter: Pure Substances and Mixtures
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The Atomic Theory of Matter

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Subatomic Particles

Dalton was only partially correct about the particles that make up matter. All matter is composed of atoms, and atoms are composed of three smaller ...

Elements: Chemical Symbols and Isotopes

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

PS.Chm.1.1

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 ...

Nuclear Stability

Protons and neutrons, collectively called nucleons, are packed together tightly in a nucleus. With a radius of about 10&#8722;15 meters, a nucleus is ...

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 ...

Radioactive Decay and Radiometric Dating

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. ...

Nuclear Fission

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

Nuclear Power

Controlled nuclear fission reactions are used to generate electricity. Any nuclear reactor that produces power via the fission of uranium or plutonium by ...

Nuclear Fusion

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

Nuclear transmutation is the conversion of one nuclide into another. It can occur by the radioactive decay of a nucleus, or the reaction of a nucleus with ...

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

PS.Chm.1.2

Atomic Orbitals

An atomic orbital represents the three-dimensional regions in an atom where an electron has the highest probability to reside. The radial distribution ...

The Pauli Exclusion Principle

The arrangement of electrons in the orbitals of an atom is called its electron configuration. We describe an electron configuration with a symbol that ...

The Energies of Atomic Orbitals

In an atom, the negatively charged electrons are attracted to the positively charged nucleus. In a multielectron atom, electron-electron repulsions are ...

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 ...

electron-configuration-of-multielectron-atoms

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 ...

Use models to explain how electrons are distributed in atoms.

PS.Chm.1.3

Periodic Classification of the Elements

The periodic table arranges atoms based on increasing atomic number so that elements with the same chemical properties recur periodically. When their ...

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

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

atomic-radii-and-effective-nuclear-charge

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

Ionic radius is the measure used to describe the size of an ion. A cation always has fewer electrons and the same number of protons as the parent atom; it ...

Construct an explanation to infer the atomic size, reactivity, electronegativity, and ionization energy of an element based on its position in the Periodic Table.

PS.Chm.2.2

Analyze the structure of atoms and isotopes.

Ionic Compounds and Crystal Lattices

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