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

原子が互いに接近すると、原子核は互いに反発し、電子も反発します。同時に、各原子からの電子は互いの原子核に引き付けられ、反発力を最小限に抑えながら原子間の引力を最大化するように配置されます。
これにより正味の引力が発生すると、システムの位置エネルギーは低下します。この相互作用は化学結合と呼ばれます。
ただし、原子のすべての組み合わせが安定した化学結合を形成できるわけではありません。原子の化学的挙動は、主に結合を形成するものとそれらが結合の種類によって決まります。化合物を構成する原子間の結合を理解することは、それらの分子挙動を理解し予測するのに役立ちます。
結合エネルギーは、ガス状化合物の1モルで結合を切断するために必要なエネルギーです。結合した原子の種類と関与する電子の数によって異なります。ボンドエネルギーによりボンド強度が増加します。
結合した原子の種類と関与する電子の数も、結合した2つの原子の原子核間の平均距離であり、結合の多重度と結合強度に反比例する結合長に影響を与えます。
最も一般的な結合相互作用は、反対に帯電したイオン間の静電引力を伴うイオン結合から、原子間の価電子を共有する共有結合まで、さまざまなスペクトルに分類されます。
イオン結合は、イオン化合物に見られる主要な相互作用です。構成する陽イオンと陰イオンは、静電引力によって一緒に保持されます。多くの場合、イオン形成に先立って、関与する原子間の価電子の移動が行われます。
電子を失った原子が陽イオンになり、電子を受け入れる原子が陰イオンになります。電子の移動により、通常、各イオンに最も近い希ガス配置が与えられます。これは、電子数の変化が最も小さい場合に到達する配置であり、イオンのエネルギー安定性が向上します。
共有結合では、共有電子が結合原子の原子核と相互作用し、ポテンシャルエネルギーを低下させます。二重結合と三重結合は、それぞれ原子間で2対と3対の電子を共有します。これにより、他の原子核からの追加の引力を受ける電子の数が増えると、結合強度は結合の多重度とともに増加します。

化学結合

原子は化学結合を形成することで、最も近い原子番号を持つ希ガスと同様の価電子殻電子配置を獲得しようとします。イオン結合、共有結合、および金属結合は、重要な種類の化学結合の一部です。 結合エネルギーと結合長によって、化学結合の強さが決まります。

化学結合の種類

イオン結合は、カチオンとアニオンの間に働く静電引力によって形成されます。多くの場合、イオンは、電子がある原子から別の原子へ移動することで生成されます。 ただし、静電気引力は 3 次元空間全体に均一に分布するため、イオン結合には特定の方向性がありません。

共有結合は、隣接する原子同士が電子対を共有することで形成される化学結合です。 共有された電子対は結合対と呼ばれます。 共有結合は本質的に方向性があります。

金属結合は金属原子間で形成されます。 金属結合は「電子海モデル」で記述されます。 このモデルは、金属のイオン化エネルギーが低いことに基づいて、金属原子は容易に価電子を失い、陽イオンになると述べています。 これらの価電子は、金属全体の陽イオンを取り囲む非局在化電子のプールを作成します。

結合エネルギーと結合長

共有結合の強さは、その結合を切断するのに必要なエネルギー、つまり結合した原子を分離するのに必要なエネルギーにとして測定されます。 結合した原子のペアを分離するにはエネルギーが必要です。 結合が強ければ強いほど、それを解くのに必要なエネルギーは大きくなります。

1 モルの気体分子内の特定の共有結合を切断するのに必要なエネルギーは、「結合エネルギー」または「結合解離エネルギー」と呼ばれます。 二原子分子の結合エネルギーは、吸熱反応の標準エンタルピー変化として定義されます。 3 つ以上の原子を持つ分子には 2 つ以上の結合があります。 このような分子内のすべての結合エネルギーの合計は、分子内のすべての結合を破壊する吸熱反応の標準エンタルピー変化に等しくなります。

2 つの原子間の結合の強度は、結合内の電子対の数が増加するにつれて増加します。 一般に、2 つの原子間の結合の数が多いほど、結合長は短くなり、結合強度は大きくなります。 したがって、三重結合は、同じ 2 つの原子間の二重結合よりも強く、短いです。 同様に、二重結合は同じ 2 つの原子間の単結合よりも強くて短いです。1 つの原子が同じ族の異なる原子と結合する場合、通常、族の下にいくにつれて結合強度は低下します。

このテキストは下記から翻案されます <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>.


原子は化学結合形成に関与して、最も近い希ガスと同様の完成した価電子殻電子配置を獲得します...

Education

JoVE Core

Organic Chemistry

有機化学

Unit 1

ユニット1

Covalent Bonding and Structure

共有結合と構造

KEY TERMS AND CONCEPTS

主要用語と概念

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

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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

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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

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

JoVE Core 有機化学では、立体化学、反応、メカニズムの基本概念を、簡潔でわかりやすいアニメーション ビデオ レッスンを使用して説明します。さらに、科学者の実際のビデオでは、世界中の今日の研究室で行われている古典的および独自の研究実験における関連概念の適用を示しています。

HS-PS1-3

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Motion And Stability: Forces And Interactions

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

south-carolina-college-and-career-ready-science-standards

South Carolina College and Career Ready Science Standards

Matter and Its Interactions

C-PS1-3.

C-PS2-6.

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HS-PS1-2

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HS-PS1-4

Chemical Bonds: Types and Strength

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