Name: chemical bonding and bond properties
Uploaded: 2020-09-03T13:38:28.000Z
Duration: 2 min 37 s
Channel: JoVE

K12 Standards

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NC K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.3.1

Types of Chemical Bonds

Chemische bindingen zijn essentieel voor atomen om een verscheidenheid aan verbindingen te vormen, zoals zout, water of legeringen. Het begrijpen van de vorming van chemische bindingen, of specifieker, de aantrekkingskracht tussen atomen, zal helpen om moleculair gedrag te begrijpen en te voorspellen. De kern van een atoom bestaat uit neutronen en positief geladen protonen, die wordt omgeven door de negatief geladen elektronen.Wanneer twee atomen dicht bij elkaar komen, worden de elektronen van het ene atoom aangetrokken tot de kern van het andere atoom en vice versa. Tegelijkertijd stoten kernen van beide atomen elkaar af, evenals de elektronen van elk atoom. Wanneer deze interacties leiden tot een netto reductie van de potentiële energie, ontstaat er een chemische binding.Er zijn drie soorten chemische bindingen. Een metaal en een niet-metaal, zoals natrium en chloor, vormen een ionische binding. Metalen hebben lage ionisatie-energieën waardoor elektronen gemakkelijker uit het atoom kunnen worden verwijderd.Deze elektronen worden gemakkelijk geaccepteerd door niet-metalen gezien hun hoge elektronenaffiniteiten en gretigheid om een volledige valentieschil te bereiken. Daarom draagt het metaal elektronen over naar het niet-metaal en vormt het een kation en een anion. Deze geladen deeltjes trekken elkaar aan om een ionische binding te vormen.Het tweede type zijn covalente bindingen die worden gevormd tussen twee niet-metalen, zoals een koolstofatoom en twee zuurstofatomen die koolstofdioxide vormen. Niet-metalen hebben hoge ionisatie-energieën, waardoor het moeilijk is om valentie-elektronen van het ene atoom naar het andere te verwijderen en over te dragen, vandaar dat de elektronen tussen de atomen worden gedeeld. Deze gedeelde elektronen werken samen met beide kernen van de bindende atomen en verlagen de potentiële energie.Het laatste type is een metalen binding gevormd tussen twee metaalatomen. Metaalatomen verliezen gemakkelijk valentie-elektronen en vormen een pool van elektronen volgens het eenvoudigste elektronenzee-model. De valentie-elektronen worden over het hele metaal gedelokaliseerd en de positief geladen metaalatomen worden aangetrokken door deze pool van elektronen die de atomen bij elkaar houdt.

soorten chemische bindingen

Theorieën over chemische bindingen werden ontwikkeld door de Amerikaanse chemicus Gilbert N. Lewis. Hij ontwikkelde een model genaamd het Lewis-model om het type en de vorming van verschillende bindingen te verklaren. Chemische binding staat centraal in de chemie; het legt uit hoe atomen of ionen zich aan elkaar binden om moleculen te vormen. Het verklaart waarom sommige bindingen sterk zijn en andere zwak, of waarom één koolstofatoom zich bindt met twee zuurstofatomen en niet met drie; waarom water H2O is en niet H4O. <h4>Ionische bindingen</h4> Ionen zijn atomen of moleculen die een elektrische lading dragen. Een kation (een positief ion) ontstaat wanneer een neutraal atoom een of meer elektronen uit zijn valentieschil verliest, en een anion (een negatief geladen ion) ontstaat wanneer een neutraal atoom een of meer elektronen in zijn valentieschil krijgt. Verbindingen die uit ionen bestaan, worden ionische verbindingen (of zouten) genoemd, en hun samenstellende ionen worden bij elkaar gehouden door ionische bindingen: elektrostatische aantrekkingskrachten tussen tegengesteld geladen kationen en anionen. De eigenschappen van ionische verbindingen werpen enig licht op de aard van ionische bindingen. Ionische vaste stoffen vertonen een kristallijne structuur en zijn vaak stijf en bros; ze hebben ook de neiging om hoge smelt- en kookpunten te hebben, wat erop wijst dat ionische bindingen erg sterk zijn. Ionische vaste stoffen zijn om dezelfde reden ook slechte elektriciteitsgeleiders: de sterkte van ionische bindingen verhindert dat ionen vrij kunnen bewegen in de vaste toestand. De meeste ionische vaste stoffen lossen echter gemakkelijk op in water. Eenmaal opgelost of gesmolten zijn ionische verbindingen uitstekende geleiders van elektriciteit en warmte, omdat de ionen zich vrij kunnen bewegen. <h4>Covalente obligaties</h4> Niet-metaalatomen vormen vaak covalente bindingen met andere niet-metaalatomen. Covalente bindingen ontstaan wanneer elektronen worden gedeeld tussen atomen en worden aangetrokken door de kernen van beide atomen. Als de atomen die een covalente binding vormen identiek zijn, zoals in H2, Cl2 en andere diatomische moleculen, dan moeten de elektronen in de binding gelijkelijk worden verdeeld. Dit wordt een zuivere covalente binding genoemd. Wanneer de atomen verbonden door een covalente binding verschillend zijn, worden de bindende elektronen gedeeld, maar niet langer gelijk. In plaats daarvan worden de bindende elektronen meer aangetrokken door het ene atoom dan door het andere, wat aanleiding geeft tot een verschuiving van de elektronendichtheid naar dat atoom. Deze ongelijke verdeling van elektronen staat bekend als een polaire covalente binding. Verbindingen die covalente bindingen bevatten, vertonen andere fysische eigenschappen dan ionische verbindingen. Omdat de aantrekkingskracht tussen moleculen, die elektrisch neutraal zijn, zwakker is dan die tussen elektrisch geladen ionen, hebben covalente verbindingen over het algemeen veel lagere smelt- en kookpunten dan ionische verbindingen. Terwijl ionische verbindingen goede elektriciteitsgeleiders zijn wanneer ze in water worden opgelost, zijn de meeste covalente verbindingen bovendien onoplosbaar in water; omdat ze elektrisch neutraal zijn, zijn ze in welke staat dan ook slechte elektriciteitsgeleiders. <h4>Metaalverbindingen</h4> Metaalbindingen worden gevormd tussen twee metaalatomen. Een vereenvoudigd model om metaalverbindingen te beschrijven is ontwikkeld door Paul Drüde, het 'Electron Sea Model'. Gebaseerd op de lage ionisatie-energieën van metalen, stelt het model dat metaalatomen gemakkelijk hun valentie-elektronen verliezen en kationen worden. Deze valentie-elektronen creëren een pool van gedelokaliseerde elektronen die de kationen over het hele metaal omringen. Metaalachtige vaste stoffen, zoals kristallen van koper, aluminium en ijzer. worden gevormd door metaalatomen, en ze vertonen allemaal een hoge thermische en elektrische geleidbaarheid, metaalglans en kneedbaarheid. Velen zijn erg moeilijk en behoorlijk sterk. Vanwege hun kneedbaarheid (het vermogen om te vervormen onder druk of hameren) versplinteren ze niet en vormen ze daarom nuttige bouwmaterialen. De smeltpunten van metalen lopen sterk uiteen. Kwik is bij kamertemperatuur een vloeistof en de alkalimetalen smelten onder de 200 °C. Verschillende post-overgangsmetalen hebben ook lage smeltpunten, terwijl de overgangsmetalen smelten bij temperaturen boven 1000 °C. Deze verschillen weerspiegelen verschillen in de sterkte van de metaalbinding tussen de metalen. Dit artikel is aangepast van <a href="https://openstax.org/books/chemistry-2e/pages/7-1-ionic-bonding">Openstax, Chemistry 2e, Sectie 7.1: Ionische Binding</a>, <a href="https://openstax.org/books/chemistry-2e/pages/7-2-covalent-bonding">Openstax, Chemistry 2e, Sectie 7.2: Covalente Binding</a>, en <big><a href="https://openstax.org/books/chemistry-2e/pages/10-5-the-solid-state-of-matter">Openstax, Chemistry 2e, Sectie 10.5: De Vaste Toestand van Materie</a>.</big>

Soorten chemische bindingen

Chemical bonding theories were pioneered by American chemist Gilbert&nbsp;N. Lewis. He developed a model called the Lewis model to explain the type and ...

Education

JoVE Core

Scheikunde

Eén

Chemical Bonding: Basic Concepts

Chemische bindingen: basisconcepten

KEY TERMS AND CONCEPTS

BELANGRIJKE TERMEN EN CONCEPTEN

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 shell. An anion is a negative ion formed when a neutral atom gains one or more electrons in its valence shell. Ionic compounds, also called salts, are held together by electrostatic attraction between oppositely charged cations and anions.

The properties of ionic compounds show why ionic bonds are strong. Ionic solids usually have a crystalline structure and are rigid and brittle. They also tend to have high melting and boiling points. In the solid state, they are poor conductors of electricity because the ions cannot move freely. Many ionic solids dissolve readily in water. When they are dissolved or melted, they conduct electricity and heat well because the ions can move about freely.

Covalent bonding is common between nonmetal atoms. It forms when atoms share electrons, and the shared electrons are attracted by the nuclei of both atoms. When identical atoms bond, as in H2 and Cl2, the electrons are shared equally. This is called a pure covalent bond. When different atoms bond, the electrons are still shared, but not equally. This creates a polar covalent bond, where electron density shifts toward one atom.

Covalent compounds have different properties from ionic compounds. Because the attraction between neutral molecules is weaker than the attraction between charged ions, covalent compounds usually have much lower melting and boiling points. Most are insoluble in water. They are also poor conductors of electricity in any state because they are electrically neutral.

Metallic bonding forms between metal atoms. Paul Drude's electron sea model describes this bond by saying that metal atoms lose valence electrons easily and become cations. The valence electrons form a pool of delocalized electrons around the cations throughout the metal. Metallic solids, such as copper, aluminum, and iron, conduct heat and electricity well. They also have metallic luster and are malleable, so they can deform under pressure or hammering without shattering.

Metals can have very different melting points. Mercury is liquid at room temperature, and alkali metals melt below 200 degrees Celsius. Several post-transition metals also have low melting points. Transition metals, however, melt above 1000 degrees Celsius. These differences reflect differences in the strength of metallic bonding among metals.

Chemical Bonding and Bond Properties

types of chemical bonds

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

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

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

bond-polarity-dipole-moment-and-percent-ionic-character

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

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

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

Explore ionic, covalent, and metallic bonding, plus the properties of each. Learn how electrons, ions, and metals explain structure, conductivity, and melting points.

Chemical Bonding and Bond Properties | JoVE K12

chemistry

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Physical Science

PS.PSc.2.1

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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

High School

Matter and Its Interactions

CHEM1.PS1.14

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Motion and Stability: Forces and Interactions

CHEM1.PS2.1

CHEM1.PS2.2

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CH.3

CH.3.d

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PS.3.c

Minnesota Academic Standards in Science

1.2.1 9C.1.2.1.2

Arizona Science Standards

HS.P1

HS.P1U1.2

HS+C.P1

HS+C.P1U1.4

Texas Essential Knowledge and Skills

CHEM.6

CHEM.6.E

Alabama Course of Study Science

9-12.C.2.2.a

9-12.C.2.2.c

Florida Department of Education

SC.912.P.8

SC.912.P.8.6

Chemistry and Physics

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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HS-PS1-2.

HS-PS1-4.

HS-PS1-12.

Georgia Standards of Excellence

SPS2.

Chemical Bonds

SC2.

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Bonding Types: From Nonpolar Covalent to Ionic

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Radioactive Decay and Radiometric Dating

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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 ...

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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 ...

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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

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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 ...

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 ...

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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

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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

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 ...

Ionization Energy

The amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state is called its first ionization energy ...

Electron Affinity

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PS.Chm.2.2

Analyze the structure of atoms and isotopes.

Chemical Bonding and Bond Properties

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