Name: chemical bonds: types and strength
Uploaded: 2023-04-30T18:28:31.000Z
Duration: 2 min 40 s
Channel: JoVE

K12 Standards

Louisiana Student Standards for Science

High School

Chemistry

Matter And Its Interactions

HS-PS1-1

Chemical Bonds

Atomlar birbirine yaklaştığında, elektronlar gibi çekirdekleri de birbirini iter. Aynı zamanda, her bir atomdan gelen elektronlar birbirlerinin çekirdeğine çekilir ve itme kuvvetlerini en aza indirirken atomlar arasındaki çekici kuvvetleri en üst düzeye çıkaracak şekilde düzenlenir.
Bu net bir çekici kuvvet ile sonuçlanırsa, sistemin potansiyel enerjisi düşürülür. Bu etkileşime kimyasal bağ denir.
Bununla birlikte, her atom kombinasyonu kararlı kimyasal bağlar oluşturamaz. Bir atomun kimyasal davranışı, öncelikle neyin bağ oluşturduğu ve ne tür bağlar oldukları tarafından belirlenir. Bir bileşiği oluşturan atomlar arasındaki bağı anlamak, moleküler davranışlarını anlamaya ve tahmin etmeye yardımcı olur.
Bağ enerjisi, gaz halindeki bir bileşiğin bir molündeki bir bağı kırmak için gereken enerjidir. Bağlı atomların türüne ve ilgili elektron sayısına bağlıdır. Bağ gücü bağ enerjisi ile artar.
Bağlı atomların türü ve ilgili elektron sayısı, iki bağlı atomun çekirdekleri arasındaki ortalama mesafe olan ve bağ çokluğu ve bağ kuvveti ile ters orantılı olan bağ uzunluğunu da etkiler.
En yaygın bağ etkileşimleri, zıt yüklü iyonlar arasındaki elektrostatik çekimleri içeren iyonik bağlardan, atomlar arasında değerlik elektronlarını paylaşan kovalent bağlara kadar değişen bir spektruma düşer.
İyonik bağ, iyonik bileşiklerde bulunan birincil etkileşimdir. Kurucu katyonlar ve anyonlar, elektrostatik çekim kuvvetleri ile bir arada tutulur. Genellikle, iyon oluşumundan önce, katılan atomlar arasında değerlik elektronlarının transferi yapılır.
Elektron kaybeden atom katyon olurken, elektron kabul eden atom anyon olur. Elektronların transferi tipik olarak her iyona en yakın soy gaz konfigürasyonunu verir, bu da elektron sayısındaki en küçük değişiklikle ulaşılan konfigürasyondur ve iyonları enerjik olarak daha kararlı hale getirir.
Kovalent bağda, paylaşılan elektronlar bağ atomlarının çekirdekleri ile etkileşime girer ve potansiyel enerjiyi düşürür. İkili ve üçlü bağlar, atomlar arasında sırasıyla iki ve üç çift elektronu paylaşır. Bu, diğer çekirdekten gelen ek çekici kuvvetlere maruz kalan elektron sayısını artırdığından, bağ kuvveti bağ çokluğu ile artar.

kimyasal bağlar

Atomlar, atom numarası olarak kendisine en yakın soy gazınkine benzer tamamlanmış bir değerlik kabuğu elektron konfigürasyonu elde etmek için bir kimyasal bağ oluşumuna katılırlar. İyonik, kovalent ve metalik bağlar önemli kimyasal bağ türlerinden bazılarıdır. Bağ enerjisi ve bağ uzunluğu, kimyasal bağın gücünü belirler.

Kimyasal Bağ Çeşitleri

Katyonlar ve anyonlar arasındaki elektrostatik çekim nedeniyle iyonik bir bağ oluşur. Çoğu zaman iyonlar, elektronların katılan bir atomdan diğerine aktarılması ile oluşur. Bununla birlikte, elektrostatik çekim kuvveti üç boyutlu uzay boyunca eşit olarak dağıldığı için bu bağların belirli bir yönü yoktur.

Kovalent bağ, elektron çiftlerinin komşu atomlar arasında paylaşılması ile oluşan kimyasal bir bağdır. Paylaşılan elektron çiftine bağ çifti denir. Kovalent bağlar doğası gereği yönelimlidir.

İki metal atomu arasında metalik bir bağ oluşur. Metalik bağlanma “Elektron Denizi Modeli” ile açıklanmaktadır. Metallerin düşük iyonlaşma enerjilerine dayanan model, metal atomlarının değerlik elektronlarını kolaylıkla kaybedip katyonlara dönüştüğünü belirtmektedir. Bu değerlik elektronları, tüm metal üzerinde katyonları çevreleyen serbest elektronlardan oluşan bir havuz oluşturur.

Bağ Enerjileri ve Bağ Uzunluğu

Kovalent bir bağın gücü, onu kırmak için gereken enerjiyle, yani bağlı atomları ayırmak için gereken enerjiyle ölçülür. Herhangi bir bağlı atom çiftini ayırmak enerji gerektirir. Bir bağ ne kadar güçlüyse, onu kırmak için gereken enerji de o kadar büyük olur.

Bir mol gaz molekülünde belirli bir kovalent bağı kırmak için gereken enerjiye bağ enerjisi veya bağ ayrışma enerjisi denir. İki atomlu bir molekül için bağ enerjisi, endotermik reaksiyon için standart entalpi değişimi olarak tanımlanır. Üç veya daha fazla atomlu moleküllerin iki veya daha fazla bağı vardır. Böyle bir moleküldeki tüm bağ enerjilerinin toplamı, moleküldeki tüm bağları kıran endotermik reaksiyonun standart entalpi değişimine eşittir.

İki atom arasındaki bağın kuvveti, bağdaki elektron çiftlerinin sayısı arttıkça artar. Genel olarak iki atom arasındaki bağ sayısı arttıkça bağ uzunluğu kısalır ve bağ kuvveti artar. Dolayısıyla üçlü bağlar aynı iki atom arasındaki çift bağlardan daha güçlü ve daha kısadır; aynı şekilde çift bağlar, aynı iki atom arasındaki tekli bağlardan daha güçlü ve daha kısadır. Bir atom bir gruptaki çeşitli atomlara bağlandığında, grupta aşağıya doğru ilerledikçe bağ kuvveti tipik olarak azalır.

Bu metin ABC’den uyarlanmıştır. <a href="https://openstax.org/books/chemistry-2e/pages/7-1-ionic-bonding">Openstax, Chemistry 2e, Section 7.1: Ionic Bonding</a>, <a href="https://openstax.org/books/chemistry-2e/pages/7-2-covalent-bonding">Openstax, Section 7.2: Covalent Bonding</a>, <a href="https://openstax.org/books/chemistry-2e/pages/10-5-the-solid-state-of-matter">Section 10.5: The Solid State of Matter</a>, and Section<a href="https://openstax.org/books/chemistry-2e/pages/7-5-strengths-of-ionic-and-covalent-bonds"> 7.5. Bond Strength: Covalent Bonds</a>.

Kimyasal bağlar


Atomlar, en yakın soy gazınkine benzer tamamlanmış bir değerlik-kabuk elektron konfigürasyonu elde etmek için kimyasal bir bağ oluşumuna katılırlar.

Education

JoVE Core

Organic Chemistry

Organik Kimya

Unit 1

Ünite 1

Covalent Bonding and Structure

Kovalent Bağlanma ve Yapı

KEY TERMS AND CONCEPTS

TEMEL TERİMLER VE KAVRAMLAR

chemical bonds: types and strength

Chemical bonds help atoms reach a full valence shell like the nearest noble gas. The main bond types are ionic, covalent, and metallic. Bond energy and bond length also help explain how strong a bond is.

An ionic bond forms from electrostatic attraction between cations and anions. In many cases, one atom transfers electrons to another atom, and the ions form from that transfer. Ionic bonds have no defined direction because the attraction spreads evenly through three-dimensional space.

A covalent bond forms when adjacent atoms share electron pairs. The shared pair is called the bonding pair. Covalent bonds are directional, so the atoms are linked in a specific orientation.

A metallic bond forms between two metal atoms. The electron sea model describes this type of bonding. In this model, metal atoms lose valence electrons easily and become cations, while the delocalized electrons form a pool around the cations across the metal.

The strength of a covalent bond is measured by the energy needed to break it and separate the bonded atoms. Stronger bonds require more energy. For one mole of gaseous molecules, this value is called bond energy, or bond dissociation energy. For a diatomic molecule, it is the standard enthalpy change for the endothermic reaction that breaks the bond.

Molecules with three or more atoms have more than one bond. In those cases, the total bond energy is the sum of all bond energies needed to break every bond in the molecule. Bond strength also increases as the number of electron pairs in the bond increases. Triple bonds are stronger and shorter than double bonds between the same atoms, and double bonds are stronger and shorter than single bonds. When one atom bonds to different atoms in a group, bond strength usually decreases as you move down the group.

Chemical Bonds: Types and Strength

what is organic chemistry?

Carbon Compounds in Everyday Life

Organic chemistry focuses on carbon compounds called organic compounds. These compounds may come from living things or be made by chemists. Carbon is the main element in them, and it bonds with other carbon atoms as well as hydrogen, oxygen, nitrogen, and sulfur. Carbon can form up to four strong bonds. That ability lets carbon atoms build chains and rings of many sizes, shapes, and levels of complexity. Not every carbon-containing substance is classified as organic. Carbonates, cyanides, and...

electronic structure of atoms

Atomic Orbitals and Quantum Numbers

Atomic orbitals and quantum numbers describe how electrons are arranged around the nucleus. An atom has a small, positively charged nucleus with electrons surrounding it. The nucleus contains protons and neutrons, and the quantum mechanical model gives a better picture of this structure than older models. Protons carry a +1 charge and have a mass of 1.0073 amu. Neutrons have no charge and have a mass of 1.0087 amu. Electrons carry a −1 charge and have a mass of 0.00055 amu. The number of...

electron configurations

How Electrons Fill Atomic Orbitals

Electron filling in atoms follows a set order based on orbital energy. The Aufbau principle says each new electron enters the lowest-energy subshell available. The Pauli exclusion principle says no two electrons can share the same set of four quantum numbers. Hund’s rule of maximum multiplicity says electrons stay unpaired in equal-energy orbitals when possible. The order of filling follows the relative energies of the subshells. A common sequence is 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, and so on.

chemical bonds

Chemical bonds help atoms reach a full valence shell like the nearest noble gas. The main bond types are ionic, covalent, and metallic. Bond energy and bond length also help explain how strong a bond is. An ionic bond forms from electrostatic attraction between cations and anions. In many cases, one atom transfers electrons to another atom, and the ions form from that transfer. Ionic bonds have no defined direction because the attraction spreads evenly through three-dimensional space. A...

polar covalent bonds

Electronegativity in Polar Covalent Bonds

Polar covalent bonds form when atoms share electrons unevenly. This happens in covalent bonds between atoms that have similar, but not identical, tendencies to attract electrons. Nonmetal atoms often make these bonds with other nonmetals. Hydrogen gas, H2, is a simple example of a covalent bond between two hydrogen atoms. A covalent bond begins when two atoms move close enough for their valence orbitals to overlap. In hydrogen, the 1s orbitals overlap and the single electrons on each atom...

lewis structures and formal charges

Lewis Structures, Bonds, and Formal Charge

Lewis structures show how atoms share electrons in covalent bonds and in polyatomic ions. Lewis symbols help draw these structures, and the periodic table helps predict how many valence electrons an atom has and how many bonds it can form to reach an octet. Group 18 elements, such as argon and helium, already have filled electron configurations. They rarely take part in chemical bonding. Atoms in group 17, such as bromine and iodine, need one more electron to reach an octet, so they can form...

vsepr theory

Molecular Shapes from Electron Pairs

Molecular shape can be predicted from the way electron pairs arrange around a central atom. Valence shell electron-pair repulsion theory, or VSEPR theory, uses a Lewis structure to count bonding pairs and lone electron pairs. The main idea is simple: electron pairs spread out as far as possible to reduce repulsion. In a molecule, the valence electrons around the central atom can be bonding pairs or lone pairs. Bonding pairs are found mainly between bonded atoms. Lone pairs stay on one atom and...

molecular geometry and dipole moments

Predicting Shape and Molecular Polarity

Molecular shape and molecular polarity can be predicted with VSEPR theory and dipole moments. Start by writing the Lewis structure of the molecule or polyatomic ion. Then count the electron groups around the central atom. Lone pairs and bonds both count as electron groups, and a single, double, or triple bond each counts as one region of electron density. Use that count to identify the electron-pair geometry. Next, use the number of lone pairs to determine the molecular structure. If more than...

resonance and hybrid structures

Resonance in Nitrite and Carbonate Ions

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valence bond theory and hybridized orbitals

valence-bond-theory-and-hybridized-orbitals

Covalent Bond Overlap and Orbital Hybridization

Covalent bonds form when orbitals on two atoms overlap and their single electrons pair up. The bond is stronger when the overlap is greater. Maximum overlap happens when the orbitals meet along a direct line between the two nuclei. A sigma bond, or σ bond, is the kind of covalent bond found in a single bond in a Lewis structure. In a σ bond, electron density is concentrated along the internuclear axis. A pi bond, or π bond, forms when two p orbitals overlap side by side. In a π bond, the...

mo theory and covalent bonding

Bond Order and Molecular Orbitals

Molecular orbital theory explains how electrons are arranged in molecules. It treats electron regions in a molecule much like atomic orbitals in an atom. A molecular orbital is the region of space where a valence electron is most likely to be found. Molecular orbitals form through the linear combination of atomic orbitals, or LCAO. When atomic wave functions combine in phase, they create regions with high electron density. When they combine out of phase, they create nodes, or regions with no...

intermolecular forces and physical properties

intermolecular-forces-and-physical-properties

How Intermolecular Forces Affect Matter

Intermolecular forces are the attractions between molecules, and they help explain how matter behaves. These forces influence melting points, boiling points, and whether substances mix with one another. Water has a much higher boiling point than hexane, which shows that water has stronger intermolecular forces. Three main kinds of intermolecular interactions are covered here. They include ion-dipole forces, dipole-dipole interactions, and van der Waals forces, which include London dispersion...

solubility

Why Some Substances Dissolve in Water

Solution formation depends on how solutes and solvents interact. A solution is a homogeneous mixture made of a solvent, which is the larger part, and a solute, which is the smaller part. The physical state of a solution is usually the same as the solvent. Concentration is often described as dilute for a low amount of solute or concentrated for a high amount of solute. When a solute dissolves, its particles are surrounded by solvent species. This process is called solvation. If water is the...

introduction to functional groups

Functional Groups and Organic Molecules

Functional groups are groups of atoms with specific chemical properties that appear within organic molecules. They are sometimes shown as "R." These groups sit along the carbon backbone of macromolecules, which can form chains or rings of carbon atoms. Functional groups help functionalize a compound. That means they can give the molecule different physical and chemical properties. In organic chemistry, this change in group structure can strongly affect how a compound behaves. Common...

overview of advanced functional groups

Advanced Functional Groups in Organic Chemistry

Advanced functional groups are atom clusters in organic molecules that give those molecules specific chemical properties. They are sometimes shown as "R" in formulas. By changing the atoms attached to a carbon skeleton, a functional group can make a compound behave differently in physical and chemical reactions. This topic covers several major classes of organic compounds with advanced functional groups. Aromatic hydrocarbons include benzene. Phenol is another example and is also called...

key terms and concepts

Explore ionic, covalent, and metallic bonds, plus bond energy and bond length. Learn how bond type affects strength in high school chemistry.

Chemical Bonds: Types and Strength | JoVE K12

organic chemistry

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HS-PS2-6

ohios-learning-standards-and-model-curriculum

Ohio’s Learning Standards and Model Curriculum

9-12

Physical Geology

Minerals

Chemical bonding (ionic, covalent, metallic)

Tennessee Academic Standards

Motion and Stability: Forces and Interactions

CHEM1.PS2.1

Virginia  Standards of Learning

HIgh School

Physics

PH.9

PH.9.e

Minnesota Academic Standards in Science

1.1.1 9L.4.2.1.1

3.1.1 9C.2.2.1.2

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South Carolina College and Career Ready Science Standards

Matter and Its Interactions

C-PS1-3.

C-PS2-6.

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HS-PS1-4

Chemical Bonds: Types and Strength

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