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

분자 사이에 존재하는 정전기 상호 작용은 분자 간 힘이라고합니다. 이러한 매력적인 힘은 융점, 비등점 및 용해도와 같은 다양한 물리적 특성에 영향을 미칩니다.

분자 간 힘의 세 가지 주요 유형은 이온과 극성 분자 사이의 강한 이온 - 이폴 상호 작용, 극성 분자 사이의 이폴 - 이폴 상호 작용, 그리고 마지막으로, 모든 분자, 극성 및 비극성에 존재하는 모든 - 분산 력의 가장 약한 것을 포함한다.

이온-이폴 상호 작용은 솔루션에 일반적입니다. 염화 나트륨과 같은 이온 화합물이 물과 같은 극성 용매에 용해되면 이온이 물 분자의 반대하의 충전 된 끝과 일치하여 최대 정전기 매력을 허용합니다.

대안적으로, 이폴-이폴 상호 작용은 1분자의 양성 끝이 인접한 분자의 음의 끝과 정전기적으로 상호 작용하는 영원한 이폴을 가진 극성 분자에 의해 전시됩니다.

산소, 질소 또는 불소에 결합된 수소 원자가 인접한 분자의 전기 음성 원자에 끌리면 특수 유형의 이폴-이폴 상호 작용인 수소 결합이 형성됩니다. 특히 수소 접합이 가능한 화합물은 높은 용융 및 끓는 점을 나타낸다.

분산력은 일시적인 이폴의 결과이며 어금니 질량으로 증가하는 경향이 있다. 질량이 높은 원자에는 전자가 더 많고 전자 구름이 커서 분산력이 증가합니다. 그 결과, 인접한 원자 사이의 매력적인 힘을 극복하기 위해서는 더 많은 에너지가 필요하며, 그 결과 더 높은 끓는 점과 융점이 발생합니다.

이것은 알케인 비등점이 어금니 질량으로 증가하는 이유를 설명합니다.

그러나, 어금니 질량만이 유일한 기준은 아니다. 동일한 질량을 가지고 있음에도 불구하고 n-펜탄은 분산력에 사용할 수 있는 표면적이 증가하여 네오펜탄보다 더 높은 비등점을 가지고 있습니다.

분자 간 힘은 또한 용해도를 결정하는 데 중요합니다. 물과 에탄올과 같은 유사한 유형의 액체와 분자 간 힘의 크기는 모든 비율로 완전히 용해되거나 오해의 소지가 있습니다.

대조적으로, 육산과 물과 같은 액체는 분자 간 힘의 다른 모형 및 규모를 가진, 대부분의 비율 또는 불굴의 에서 불용성입니다.

전반적으로, 분자 간 힘은 작은 또는 부분 전하가 먼 거리에서 상호 작용하기 때문에 상대적으로 약합니다.

분자간 힘과 물리적 특성

분자간 힘은 분자 사이에 존재하는 인력입니다. 이는 물질의 녹는점, 끓는점, 용해도(혼화성)와 같은 여러 가지 벌크 특성을 나타냅니다. 예를 들어, 물((H2, b.p. 100 °C)과 같은 끓는점이 높은 액체는 헥산(C6H14, b.p. 68.73 °C)과 같은 낮은 끓는점 액체에 비해 더 강한 분자간 힘을 나타냅니다. 세 가지 종류의 분자간 상호 작용에는 i) 이온-쌍극자 힘, ii) 쌍극자-쌍극자 상호 작용, iii) 런던 분산력을 포함하는 반 데르 발스 힘이 포함됩니다.

1. 이온-쌍극자 력

이온-쌍극자 힘은 이온과 쌍극자 사이의 정전기적 인력입니다. 이는 용액에서 흔히 발견되며 KCl과 같은 이온 화합물을 물에 용해시키는 데 중요한 역할을 합니다. 이온-쌍극자 상호작용의 강도는 i) 이온의 전하 및 ii) 극성 분자의 쌍극자의 크기에 정비례합니다.

2. 쌍극자-쌍극자 상호작용

극성 분자는 분자의 한쪽 끝에는 부분적인 양전하를, 다른 쪽 끝에는 부분적인 음전하를 가집니다. 이러한 전하 분리를 쌍극자라고 합니다. 두 개의 영구 쌍극자 사이의 인력을 쌍극자-쌍극자 인력, 즉 한 극성 분자의 부분적으로 양극인 끝과 다른 극성 분자의 부분적으로 음인 끝 사이의 정전기력이라고 합니다. 수소 결합은 O, N 또는 F와 같이 전기 음성도가 높은 원자에 결합된 수소와 분자 사이의 쌍극자-쌍극자 상호 작용의 한 유형입니다. 결과적으로 한 분자(수소 결합 공여체)에서 부분적으로 양전하를 띤 H 원자가 강하게 상호 작용할 수 있습니다. 인접한 분자(수소 결합 수용체)에 부분적으로 음전하를 띤 O, N 또는 F 원자의 비공유 전자쌍이 있습니다. 수소 결합은 끓는점을 상당히 증가시킵니다.

3. 반데르발스와 런던 분산군

모든 힘 중에서 가장 약한 힘은 반데르발스 힘으로, 이는 원자와 분자 사이의 분자간 거리에 의존합니다. 반 데르 발스 힘의 하위 집합인 런던 분산력은 전자 분포의 일시적이고 자발적인 이동으로 인해 충전되지 않은 원자/분자 간의 상호 작용의 결과로 경험됩니다. 이러한 힘의 강도는 표면적의 증가로 인해 분자량이 증가함에 따라 증가하는 것으로 보입니다. 결과적으로, 더 높은 분자량의 화합물은 일반적으로 더 높은 온도에서 끓습니다. 중요한 점은 분지형 탄화수소(네오펜탄)가 일반적으로 각각의 직쇄형(n-펜탄) 이성질체보다 표면적이 더 작으므로 끓는점이 낮다는 것입니다.

4. 물에 대한 유기화합물의 용해도

어떤 비율로든 균질하게 혼합될 수 있는 액체를 혼합성이라고 합니다. 혼합성 액체는 비슷한 극성을 가지고 있습니다. 예를 들어, 메탄올과 물은 모두 극성이며 수소 결합이 가능합니다. 혼합 시, 메탄올과 물은 메탄올-메탄올 및 물-물 상호작용과 비슷한 강도의 분자간 수소 결합을 통해 상호작용합니다. 따라서 그들은 혼합이 가능합니다. 마찬가지로, 헥산이나 브롬과 같은 비극성 액체는 분산력을 통해 서로 섞일 수 있습니다. "같은 용해"라는 화학 공리는 화합물의 혼화성을 예측하는 데 유용합니다. 어느 정도 섞이지 않는 두 액체를 섞이지 않는 액체라고 합니다. 예를 들어, 비극성 헥산은 극성 물과 섞이지 않습니다. 헥산과 물 사이의 상대적으로 약한 인력은 물 분자 사이의 강한 수소 결합력을 적절하게 극복하지 못합니다.



이 문서는에서 발췌되었습니다.<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>, and <a href="https://openstax.org/books/chemistry-2e/pages/10-introduction">Chapter 10: Liquids and Solids</a>.


분자간 힘은 분자 사이에 존재하는 인력입니다. 그들은 녹는점, 끓는점과 같은 여러 벌크 특성을 지시합니다.

Education

교육

JoVE Core

Organic Chemistry

유기 화학

Unit 1

제1단원

Covalent Bonding and Structure

공유 결합과 구조

KEY TERMS AND CONCEPTS

주요 용어 및 개념

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.

How Intermolecular Forces Affect Matter

what is organic chemistry?

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chemical bonds

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Electronegativity in Polar Covalent Bonds

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valence-bond-theory-and-hybridized-orbitals

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intermolecular forces and physical properties

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

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introduction to functional groups

Functional Groups and Organic Molecules

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Advanced Functional Groups in Organic Chemistry

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key terms and concepts

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How Intermolecular Forces Affect Matter | JoVE K12

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HS-PS2-6

Tennessee Academic Standards

Motion and Stability: Forces and Interactions

CHEM1.PS2.2

Minnesota Academic Standards in Science

9-12

1.1.1 9L.4.2.1.1

Arizona Science Standards

Physical Science

HS+C.P1

HS+C.P1U1.4

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HS-PS1-1

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Dynamic Equilibrium

A reversible chemical reaction represents a chemical process that proceeds in both forward (left to right) and reverse (right to left) directions. When ...

Construct and revise an explanation for the outcome of a simple chemical reaction based on the outermost electron states of atoms, trends in the periodic table, and knowledge of the patterns of chemical properties.  Clarification Statement: Chemistry: Examples of chemical reactions could include the reaction of sodium and chlorine, carbon and oxygen, or carbon and hydrogen. Reaction classification aids in the prediction of products (e.g. synthesis, decomposition, single displacement, double displacement, and acid-base).

HS-PS1-2

Intermolecular vs Intramolecular Forces

Intermolecular forces (IMF) are electrostatic attractions arising from charge-charge interactions between molecules. The strength of the intermolecular ...

comparison-between-electrical-and-gravitational-forces

Comparison Between Electrical And Gravitational Forces

There are four fundamental forces in nature: the gravitational force, the electromagnetic force, the strong nuclear force, and the weak nuclear force. To ...



Intermolecular forces are attractive forces that exist between molecules. They dictate several bulk properties, such as melting points, boiling points, ...

electric-field-of-two-equal-and-opposite-charges

Electric Field of Two Equal and Opposite Charges

Atoms generally contain the same number of positively and negatively charged particles, protons, and electrons. Hence, they are electrically neutral. ...

Electric Field

Consider two point charges, each exerting Coulomb force on the other. It is possible to describe the Coulomb interaction via an intermediate step by ...

Ionic Bonding and Electron Transfer

Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence ...

Electric Dipoles and Dipole Moment

Consider two charges of equal magnitude but opposite signs. If they cannot be separated by an external electric field, the system is called a permanent ...

Plan and conduct an investigation to gather evidence to compare the structure of substances at the macroscale to infer the strength of electrical forces between particles.  Clarification Statement: Emphasis is on understanding the strengths of forces between particles, not on naming specific intermolecular forces (such as dipole-dipole). Examples of particles could include ions, atoms, molecules, and network solids (such as graphite). Examples of macro-properties of substances could include the melting point and boiling point, vapor pressure, and surface tension.

bond-dissociation-energy-and-activation-energy

Bond Dissociation Energy and Activation Energy

Bond energy is the energy required to break a bond homolytically. These values are usually expressed in units of kcal/mol or kJ/mol and are referred to as ...

Bond Energies and Bond Lengths

Stable molecules exist because covalent bonds hold the atoms together. The strength of a covalent bond is measured by the energy required to break it, ...

Coupled Reactions

Cellular processes such as building and breaking down complex molecules occur through stepwise chemical reactions. Some of these chemical reactions are ...

energy-diagrams-transition-states-and-intermediates

Energy Diagrams, Transition States, and Intermediates

Free-energy diagrams, or reaction coordinate diagrams, are graphs showing the energy changes that occur during a chemical reaction. The reaction ...

What is Metabolism?

Overview

Metabolism represents all of the chemical activity in a cell, including reactions that build molecules (anabolism) and those that break ...

types-of-chemical-reactions-anabolic-and-catabolic

Types of Chemical Reactions: Anabolic and Catabolic

The first law of thermodynamics holds that energy can neither be created nor destroyed&#8212;it can only change form. An organism&#39;s essential function ...

Non-equilibrium in the Cell

An important concept in studying metabolism and energy is that of chemical equilibrium. Most chemical reactions are reversible. They can proceed in both ...

Activation Energy

Activation energy is the minimum amount of energy necessary for a chemical reaction to move forward. The higher the activation energy, the slower the rate ...

Energy Transfer in Chemical Reactions

Chemical reactions require sufficient energy to cause the matter to collide with enough precision and force that old chemical bonds can be broken and new ...

factors-influencing-the-rate-of-chemical-reactions

Factors Influencing the Rate of Chemical Reactions

A variety of factors influence the rate of chemical reactions. For a chemical reaction to happen, atoms must collide with enough energy to overcome the ...

Predicting Reaction Outcomes

Kinetics describes the rate and path by which a reaction occurs. In contrast, thermodynamics deals with state functions and describes the properties, ...

States of Matter and Phase Changes

The internal energy of a substance&#8212;the total kinetic energy of all its molecules and the potential energy of their associated forces&#8212;depends ...

Develop a model to illustrate that the release or absorption of energy from a chemical reaction system depends upon the changes in total bond energy.  Clarification Statement: Emphasis is on the idea that a chemical reaction is a system that affects the energy change.  Examples of models could include molecular-level drawings and diagrams of reactions, graphs showing the relative energies of reactants and products, and representations showing energy is conserved.

HS-PS1-4

How Intermolecular Forces Affect Matter

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