Name: how intermolecular forces affect matter
Uploaded: 2025-05-22T09:05:33.000Z
Duration: 2 min 56 s
Channel: JoVE

K12 Standards

Louisiana Student Standards for Science

High School

Chemistry

Matter And Its Interactions

HS-PS1-3

intermolecular-forces-and-physical-properties

Intermolecular Forces and Physical Properties

Le interazioni elettrostatiche che esistono tra le molecole sono chiamate forze intermolecolari. Queste forze attrattive influenzano varie proprietà fisiche, come il punto di fusione, il punto di ebollizione e la solubilità.
I tre principali tipi di forze intermolecolari includono forti interazioni ione-dipolo tra ioni e molecole polari, interazioni dipolo-dipolo tra molecole polari e, infine, la più debole di tutte, le forze di dispersione, presenti in tutte le molecole, polari e non polari.
Le interazioni ione-dipolo sono comuni alle soluzioni. Quando un composto ionico come il cloruro di sodio viene disciolto in un solvente polare come l'acqua, gli ioni si allineano con le estremità opposte delle molecole d'acqua, consentendo la massima attrazione elettrostatica.
In alternativa, le interazioni dipolo-dipolo sono esibite da molecole polari con dipoli permanenti, dove l'estremità positiva di una molecola interagisce elettrostaticamente con l'estremità negativa della molecola vicina.
Quando un atomo di idrogeno legato all'ossigeno, all'azoto o al fluoro viene attratto dall'atomo elettronegativo di una molecola vicina, si forma un legame idrogeno, un tipo speciale di interazione dipolo-dipolo. In particolare, i composti in grado di legare idrogeno mostrano alti punti di fusione e di ebollizione.
Le forze di dispersione sono il risultato di dipoli temporanei e tendono ad aumentare con la massa molare. Gli atomi con masse più elevate hanno più elettroni e nuvole di elettroni più grandi, portando a un aumento delle forze di dispersione. Di conseguenza, è necessaria più energia per superare le forze attrattive tra gli atomi vicini, con conseguente aumento dei punti di ebollizione e fusione.
Questo spiega perché i punti di ebollizione degli alcani aumentano con la loro massa molare.
Tuttavia, la massa molare non è l'unico criterio. Nonostante abbia le stesse masse, l'n-pentano ha un punto di ebollizione più alto del neopentano a causa della maggiore superficie disponibile per le forze di dispersione.
Anche le forze intermolecolari sono cruciali nel determinare la solubilità. Liquidi di tipo e entità simili di forze intermolecolari, come l'acqua e l'etanolo, sono interamente solubili in tutte le proporzioni o sono miscibili.
Al contrario, liquidi come l'esano e l'acqua, con diversi tipi e grandezze di forze intermolecolari, sono insolubili nella maggior parte delle proporzioni o immiscibili.
Nel complesso, le forze intermolecolari sono relativamente deboli perché le cariche piccole o parziali interagiscono su grandi distanze.

forze intermolecolari e proprietà fisiche

Le forze intermolecolari sono forze di attrazione che esistono tra le molecole. Dettano diverse proprietà di massa, come punti di fusione, punti di ebollizione e solubilità (miscibilità) delle sostanze. Ad esempio, un liquido con un punto di ebollizione elevato, come l'acqua (H2O, punto di ebollizione 100 °C), mostra forze intermolecolari più forti rispetto ad un liquido con punto di ebollizione basso, come l'esano (C6H14, punto di ebollizione 68,73 °C). I tre tipi di interazioni intermolecolari includono i) forze ione-dipolo, ii) interazioni dipolo-dipolo e iii) forze di van der Waals, che includono le forze di dispersione di London.

<ol style="padding-left: 35px; margin: 0;">
	<li>Forze ione-dipolo

	Le forze ione-dipolo sono le attrazioni elettrostatiche tra uno ione e un dipolo. Sono comuni nelle soluzioni e svolgono un ruolo importante nella dissoluzione dei composti ionici, come KCl, nell'acqua. La forza delle interazioni ione-dipolo è direttamente proporzionale i) alla carica dello ione e ii) alla magnitudo del dipolo delle molecole polari.
	</li>
	<li>Interazioni dipolo-dipolo
	Le molecole polari hanno una carica parziale positiva su un'estremità e una carica parziale negativa sull'altra estremità della molecola: una separazione di carica chiamata dipolo. La forza attrattiva tra due dipoli permanenti è chiamata attrazione dipolo-dipolo, ovvero la forza elettrostatica tra l'estremità parzialmente positiva di una molecola polare e l'estremità parzialmente negativa di un'altra. Il legame idrogeno è un tipo di interazione dipolo-dipolo tra molecole con idrogeno, legate ad un atomo altamente elettronegativo, come O, N o F. L'atomo di H parzialmente caricato positivamente risultante su una molecola (il donatore nel legame idrogeno) potrebbe interagire fortemente con una coppia solitaria di elettroni di un atomo di O, N o F parzialmente caricato negativamente su molecole adiacenti (l'accettore di legame idrogeno). Il legame idrogeno aumenta considerevolmente il punto di ebollizione.
	</li>
	<li>Forze di van der Waals e forze di dispersione di London
	Le forze di van der Waals sono le più deboli di tutte le forze e dipendono dalle distanze intermolecolari tra atomi e molecole. Le forze di dispersione di London, un sottoinsieme delle forze di van der Waals, si verificano come risultato delle interazioni tra atomi/molecole non carichi a causa di cambiamenti temporanei e spontanei nella distribuzione degli elettroni. L'intensità di queste forze sembra aumentare con l'aumentare del peso molecolare a causa dell'aumento dell'area superficiale. Di conseguenza, i composti con pesi molecolari più elevati generalmente bolliranno a temperature più elevate. Va notato che un idrocarburo ramificato (neopentano) ha normalmente un'area superficiale inferiore rispetto al rispettivo isomero a catena lineare (n-pentano) e quindi un punto di ebollizione inferiore.
	</li>
	<li>Solubilità dei composti organici in acqua
	I liquidi che possono essere miscelati omogeneamente in qualsiasi proporzione si dicono miscibili. I liquidi miscibili hanno polarità simili. Ad esempio, il metanolo e l'acqua sono entrambi polari e capaci di formare legami a idrogeno. Durante la miscelazione, metanolo e acqua interagiscono attraverso legami a idrogeno intermolecolari di forza paragonabile alle interazioni metanolo-metanolo e acqua-acqua; quindi, sono miscibili. Allo stesso modo, i liquidi non polari come l'esano e il bromo sono miscibili tra loro attraverso le forze di dispersione. L’assioma chimico “il simile scioglie il simile” è utile per prevedere la miscibilità dei composti. Due liquidi che non si mescolano in misura apprezzabile sono detti immiscibili. Ad esempio, l'esano non polare è immiscibile nell'acqua polare. Le forze di attrazione relativamente deboli tra l'esano e l'acqua non superano adeguatamente le forze di legame idrogeno più forti tra le molecole d'acqua.
	</li>
</ol>

Questo testo è adattato da <a href="https://openstax.org/books/chemistry-2e/pages/10-1-intermolecular-forces"> Openstax, Chemistry 2e, Section 10.1: Intermolecular Forces</a>, <a href="https://openstax.org/books/chemistry-2e/pages/11-3-solubility">Section 11.3: Solubility</a>, e <a href="https://openstax.org/books/chemistry-2e/pages/10-introduction">Chapter 10: Liquids and Solids</a>.

Forze intermolecolari e proprietà fisiche


Le forze intermolecolari sono forze attrattive che esistono tra le molecole. Dettano diverse proprietà di massa, come i punti di fusione, i punti di ebollizione, ...

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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 forces. Each type depends on how charges are arranged in or between molecules.

Ion-dipole forces are electrostatic attractions between an ion and a dipole. They are common in solutions and are important when ionic compounds such as KCl dissolve in water. Their strength depends on the charge on the ion and the size of the dipole in the polar molecule.

Dipole-dipole interactions happen between polar molecules. A polar molecule has a partial positive end and a partial negative end, which is called a dipole. Hydrogen bonding is a strong type of dipole-dipole interaction that occurs when hydrogen is bonded to O, N, or F, and it can raise boiling points a great deal.

Van der Waals forces are the weakest intermolecular forces discussed here. London dispersion forces are a type of van der Waals force and arise from temporary shifts in electron distribution in uncharged atoms or molecules. These forces usually get stronger as molecular weight increases because surface area increases, so compounds with higher molecular weights tend to boil at higher temperatures. A branched hydrocarbon such as neopentane has less surface area than straight-chain n-pentane, so neopentane has the lower boiling point.

Intermolecular forces also help predict solubility in water. Liquids that mix in any proportion are called miscible, and they usually have similar polarities. Methanol and water are miscible because both are polar and can form hydrogen bonds. Nonpolar hexane and bromine are also miscible with each other through dispersion forces. The idea of “like dissolves like” helps explain why this happens. Hexane and water are immiscible because the weak attraction between them does not overcome the stronger hydrogen bonding among water molecules.

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How Intermolecular Forces Affect Matter

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