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

Kiedy atomy zbliżają się do siebie, ich jądra odpychają się nawzajem, podobnie jak elektrony. Jednocześnie elektrony z każdego atomu są przyciągane do swoich jąder i układają się w taki sposób, aby zmaksymalizować siły przyciągania między atomami, jednocześnie minimalizując siły odpychania.
Jeśli powoduje to powstanie siły przyciągania netto, energia potencjalna układu jest obniżana. Ta interakcja nazywa się wiązaniem chemicznym.
Jednak nie każda kombinacja atomów może tworzyć stabilne wiązania chemiczne. Zachowanie chemiczne atomu zależy przede wszystkim od tego, co tworzy wiązania i jakiego rodzaju są to wiązania. Zrozumienie wiązań między atomami, które tworzą związek, pomaga zrozumieć i przewidzieć ich zachowanie molekularne.
Energia wiązania to energia potrzebna do zerwania wiązania w jednym molu związku gazowego. Zależy to od rodzaju związanych atomów i liczby zaangażowanych elektronów. Siła wiązania wzrasta wraz z energią wiązania.
Rodzaj związanych atomów i liczba zaangażowanych elektronów również wpływają na długość wiązania, która jest średnią odległością między jądrami dwóch związanych atomów i jest odwrotnie proporcjonalna do liczby wiązań i siły wiązania.
Najczęstsze oddziaływania wiążące mieszczą się w spektrum od wiązań jonowych, które obejmują przyciąganie elektrostatyczne między przeciwnie naładowanymi jonami, do wiązań kowalencyjnych, które dzielą elektrony walencyjne między atomami.
Wiązanie jonowe jest podstawowym oddziaływaniem występującym w związkach jonowych. Składowe kationy i aniony są utrzymywane razem przez elektrostatyczne siły przyciągania. Często tworzenie jonów jest poprzedzone przenoszeniem elektronów walencyjnych między uczestniczącymi atomami.
Atom, który traci elektrony, staje się kationem, podczas gdy atom, który przyjmuje elektrony, staje się anionem. Przenoszenie elektronów zazwyczaj daje każdemu jonowi najbliższą konfigurację gazu szlachetnego, która jest konfiguracją osiąganą przy najmniejszej zmianie liczby elektronów, dzięki czemu jony są bardziej stabilne energetycznie.
W wiązaniach kowalencyjnych współdzielone elektrony oddziałują z jądrami wiążących atomów i obniżają energię potencjalną. Wiązania podwójne i potrójne mają odpowiednio dwie i trzy pary elektronów między atomami. Ponieważ zwiększa to liczbę elektronów podlegających dodatkowym siłom przyciągania z drugiego jądra, siła wiązania wzrasta wraz z wielokrotnością wiązania.

wiązania chemiczne

Atomy biorą udział w tworzeniu wiązań chemicznych, aby uzyskać kompletną konfigurację elektronów powłoki walencyjnej podobną do najbliższej mu pod względem liczby atomowej gazu szlachetnego. Wiązania jonowe, kowalencyjne i metaliczne to tylko niektóre z ważnych typów wiązań chemicznych. Energia wiązania i jego długość określają siłę wiązania chemicznego.

Rodzaje wiązań chemicznych

Wiązanie jonowe powstaje w wyniku przyciągania elektrostatycznego pomiędzy kationami i anionami. Często jony powstają w wyniku przeniesienia elektronów z jednego uczestniczącego atomu na drugi. Wiązania te nie mają jednak określonej kierunkowości, ponieważ elektrostatyczna siła przyciągania rozkłada się równomiernie w całej przestrzeni trójwymiarowej.

Wiązanie kowalencyjne to wiązanie chemiczne utworzone przez współdzielenie par elektronów pomiędzy sąsiadującymi atomami. Wspólna para elektronów nazywana jest parą wiążącą. Wiązania kowalencyjne mają charakter kierunkowy.

Wiązanie metaliczne powstaje pomiędzy dwoma atomami metalu. Model gazu elektronowego opisano w „modelu Morza Diraca”. Bazując na niskich energiach jonizacji metali, model stwierdza, że atomy metali łatwo tracą swoje elektrony walencyjne i stają się kationami. Te elektrony walencyjne tworzą pulę zdelokalizowanych elektronów otaczających kationy w całym metalu.

Energia wiązania i długość wiązania

Siłę wiązania kowalencyjnego mierzy się energią potrzebną do jego rozerwania, czyli energią niezbędną do oddzielenia związanych atomów. Oddzielenie dowolnej pary związanych atomów wymaga energii. Im silniejsze wiązanie, tym większa energia potrzebna do jego rozerwania.

Energia wymagana do rozerwania określonego wiązania kowalencyjnego w jednym molu cząsteczek gazowych nazywana jest energią wiązania lub energią dysocjacji wiązania. Energię wiązania cząsteczki dwuatomowej definiuje się jako standardową zmianę entalpii reakcji endotermicznej. Cząsteczki z trzema lub więcej atomami mają dwa lub więcej wiązań. Suma energii wszystkich wiązań w takiej cząsteczce jest równa standardowej zmianie entalpii dla reakcji endotermicznej, która rozrywa wszystkie wiązania w cząsteczce.

Siła wiązania między dwoma atomami wzrasta wraz ze wzrostem liczby par elektronów w wiązaniu. Ogólnie rzecz biorąc, im większa liczba wiązań między dwoma atomami, tym krótsza długość wiązania i większa siła wiązania. Zatem wiązania potrójne są silniejsze i krótsze niż wiązania podwójne między tymi samymi dwoma atomami; podobnie wiązania podwójne są silniejsze i krótsze niż wiązania pojedyncze pomiędzy tymi samymi dwoma atomami. Kiedy jeden atom wiąże się z różnymi atomami w grupie, siła wiązania zwykle maleje w miarę przesuwania się w dół grupy.

Ten tekst jest adaptacją <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>.

Wiązania chemiczne


Atomy uczestniczą w tworzeniu wiązań chemicznych w celu uzyskania kompletnej konfiguracji elektronowej powłoki walencyjnej podobnej do gazu szlachetnego znajdującego się najbliżej ...

Education

JoVE Core

Organic Chemistry

Chemia organiczna

Unit 1

Jednostka 1

Covalent Bonding and Structure

Wiązania kowalencyjne i struktura

KEY TERMS AND CONCEPTS

Kluczowe terminy i pojęcia

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

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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

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electron configurations

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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

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Lewis Structures, Bonds, and Formal Charge

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valence bond theory and hybridized orbitals

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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

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intermolecular forces and physical properties

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solubility

Why Some Substances Dissolve in Water

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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

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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.

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organic chemistry

JoVE Core Organic Chemistry explains basic concepts of stereochemistry, reactions, and mechanisms using concise and easy-to-understand animated video lessons. Additionally, the scientist-in-action videos demonstrate the application of related concepts in classical and original research experiments performed in today's laboratories worldwide.

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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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