Name: dalton’s laws and early atomic ideas
Uploaded: 2020-09-03T13:38:25.000Z
Duration: 2 min 59 s
Channel: JoVE

K12 Standards

north-carolina-k-12-science-standard-course-of-study

North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.1.1

The Atomic Theory of Matter

デモクリタスのような 初期のギリシャ人は 物質の最小の不可分単位である アトムという概念を 最初に提唱しました この概念は後にイギリスの 科学者ジョン・ダルトンによって 原子論として発表されました ダルトンの原子論の 第一の前提は 元素は原子と呼ばれる 小さな不可分の粒子で 構成されていることを 示唆しています 例えば 水素は2つの水素原子が 結合してできており 酸素は2つの酸素原子が 結合してできています 第2の前提は 同じ元素の原子は同一で 他の元素の原子とは 異なるということです したがって 水素の原子は すべて同じであるが 酸素の原子とは 異なるということになります 第3の前提は 異なる元素の原子は 単純な整数比で 互いに結合して化合物を 形成することができる というものです 例えば水素の2つの原子と 酸素の1つの原子が 2対1の比率で結合して H2O 水を形成します ダルトンの理論の最後の前提は 化学反応が1つの元素の原子を 別の元素の原子に 変えるのではなく その代わりに 既存の原子が 新しい物質を形成するために 自分自身を再編成 することであると述べています 水ができるとき既存の水素原子と 酸素原子は 生成も破壊されることもなく 再配列されるだけです ダルトンは 化学反応の 2つの以前の法則 質量保存の法則」と 定比例の法則」に基づいて 原子論を構築しました 質量保存の法則は 化学反応の前後の総質量が 一定であることを 示しています したがって 18グラムの水は 2グラムの水素と 16グラムの酸素に分解されます 定比例の法則とは ある化学化合物では 発生源に関係なく 構成元素の質量比が常に 一定であることを示しています 純粋な水のサンプルは 水の総質量に関係なく 酸素に対する水素の質量比が 常に1対8になります そこでダルトンは 独自の理論に基づいて 倍数比例の法則」を 提唱しました この法則によると 2つの元素が結合して 2つ以上の化合物を形成するとき 一方の元素の異なる質量は 他方の元素の固定質量と 小さな整数比で結合します つまり 2gの固定質量の 水素とは 32gまたは16gの異なる 質量の酸素が 2対1の小さな 整数比で結合して 2つの異なる化合物である 過酸化水素と水を形成します

物質の原子論

物質の基本的な構造を議論した最古の記録は、古代ギリシャの哲学者たちによるものです。 レウキッポスと デモクリトス は、すべての物質が、「見えない」ことを意味する原子と呼ばれる小さな有限の粒子で構成されていると主張しました。 後になって、 アリストテレス および他の哲学者が、物質は 4 つの「元素」 -- 火、土、空気および水の様々な組合せから成り、無限に分けることができると結論に達しました。 興味深いことに、これらの哲学者は、原子と「元素」を哲学的な概念と考えていたため、彼らの考えをテストするための実験を行うことは考えていませんでした。  
 
 アリストテレスの物質組成の見方は、イギリスの科学者ジョン・ダルトンが原子論を用いて物質の挙動を説明できるという仮説を持って化学に革命を起こすまで、 2000 年以上にわたって続いていました。 1807 年に最初に発表されたこの物質の微小な特徴に関するダルトンの仮説の多くは、現在の原子論ではまだ有効です。  
 
 ダルトンの原子理論の定理 
 
 <ol>
 <li>物質は原子と呼ばれる非常に小さい粒子で構成されています。 原子は、化学的変化に関与できる元素の最小単位です。 </li>
 <li>元素は 1 種類の原子だけで構成されています。原子はその元素に特徴的な質量を持ち、その元素のすべての原子で同じです。 元素の巨視的な試料には、非常に多くの原子が含まれており、すべて同じ化学特性を持っています。 </li>
 <li>ある1 つの元素の原子は、他のすべての元素の原子と特性が異なります。 </li>
 <li>化合物は、 2 つ以上の元素の原子を、小さな整数の比率で組み合わせたものです。 ある化合物では、各元素の原子数は常に同じ比率で存在しています。 </li>
 <li>化学変化の際に原子は生成も破壊もされず、変更前とは異なる物質を生成するように再配置されます。 </li>
 </ol>
 
 ダルトンは、化学反応の 3 つの法則を理論の基礎としました。（ 1 ）質量保存の法則、（ 2 ）定比例の法則、（ 3 ）倍数比例の法則です。 ダルトンの原子理論は、物質の多くのマクロ的性質をミクロ的に説明します。  
 
 質量保存の法則は、フランスの化学者である アントワーヌ・ラヴォアジエ によって発見されました。 これは、化学変化の際に原子は作成も破壊もされず、物質がある種類から別の種類に変化する際に存在する物質の総質量は一定であるというものです。 
 
 ダルトンは、フランスの化学者であるジョセフ・プルーストの実験についても知っていました。プルーストは、純粋な化合物のサンプルにはすべて同じ元素が同じ質量比で含まれていることを証明しました。 この記述は、定比例の法則または一定の組成の法則と呼ばれています。 特定の化合物の元素の原子数が常に同じ比率で存在するという指摘は、これらの観察結果と一致しています。  
 
 ダルトンはまた、プルーストのデータと、自身の実験結果をもとに、別の興味深い法則を導き出しました。 倍数比例の法則では、 2 つの元素が反応して複数の化合物を形成するとき、 ある要素の一定の質量は、小さい整数の比率で他の要素の質量と反応するというものです。 
 
 ダルトンの理論は、原子が素粒子で構成されており、同じ元素の原子でも質量が異なる同位体が存在することを示す枠組みを提供しました。 
 
 この文章は <a href="https://openstax.org/books/chemistry-2e/pages/2-1-early-ideas-in-atomic-theory">、 Openstax, Chemistry 2e, Section 2.1: Early Ideas in Atomic Theory から引用したものです。</a>

物質の基本構造に関する最も初期の記録された議論は、古代ギリシャの哲学者から来ています。レウキッポスとデモクリトスは、すべての問題が重要であると主張した。

Education

JoVE Core

化学

Atoms and Elements

原子と元素

KEY TERMS AND CONCEPTS

主要用語と概念

dalton’s laws and early atomic ideas

Dalton’s atomic theory explains matter with atoms, elements, and compounds. It also shows how chemical changes follow simple laws. This idea gave chemistry a microscopic model for what can be seen in the lab.

The earliest recorded ideas about matter came from ancient Greek philosophers. Leucippus and Democritus said all matter was made of tiny, finite particles called atomos, meaning “indivisible.” Aristotle and others later argued that matter was made from four elements: fire, earth, air, and water. They also believed matter could be divided forever, and these ideas were treated as philosophy rather than experiments.

That view lasted for more than two thousand years. Then English scientist John Dalton changed chemistry with an atomic theory of matter. He first published it in 1807. Many of his ideas still fit modern atomic theory.

Dalton’s postulates describe matter at the atomic level. Matter is made of extremely small particles called atoms. An atom is the smallest unit of an element that can take part in a chemical change. An element contains only one type of atom, and atoms of the same element have the same characteristic mass and chemical properties. Atoms of different elements have different properties. A compound is made of atoms of two or more elements joined in a small, whole-number ratio, and the ratio stays the same in a given compound. During a chemical change, atoms are not created or destroyed. They are rearranged into new substances.

Dalton built his theory using three key laws of chemistry. The law of conservation of mass says mass stays constant during a chemical change, a result linked to Antoine Lavoisier. The law of definite proportions, also called the law of constant composition, says every pure sample of a compound contains the same elements in the same mass ratio, as shown by Joseph Proust. Dalton also used the law of multiple proportions, which says that when two elements form more than one compound, fixed masses of one element combine with the other in small whole-number ratios.

Dalton’s atomic theory gives a microscopic explanation for macroscopic matter. It also helped later scientists show that atoms contain subatomic particles. Later work also showed that atoms of the same element can differ in mass, which are called isotopes.

Dalton’s Laws and Early Atomic Ideas

the atomic theory of matter

Dalton’s atomic theory explains matter with atoms, elements, and compounds. It also shows how chemical changes follow simple laws. This idea gave chemistry a microscopic model for what can be seen in the lab. The earliest recorded ideas about matter came from ancient Greek philosophers. Leucippus and Democritus said all matter was made of tiny, finite particles called atomos, meaning “indivisible.” Aristotle and others later argued that matter was made from four elements: fire, earth, air, and...

subatomic particles

Atomic Structure: Protons, Neutrons, and Electrons

Atomic structure is built from three subatomic particles: protons, neutrons, and electrons. Atoms make up all matter, and these particles explain an atom’s mass and charge. The electron was first identified at the end of the 19th century by J.J. Thomson. He used a cathode ray tube, a sealed glass tube with almost all the air removed and two metal electrodes. When high voltage was applied, a visible beam called a cathode ray formed. The beam bent toward positive charge and away from negative...

elements: chemical symbols and isotopes

Reading Element Symbols and Isotope Notation

Chemical symbols and isotope notation help identify elements and their atoms. A chemical symbol is an abbreviation for an element or a single atom of that element. Mercury, for example, is written as Hg. The same symbol can point to one atom in the microscopic domain or to many atoms of the element in a container or sample. Many symbols come from the element’s common English name. Others come from Latin, Greek, or German names. Aluminum uses Al, while iron uses Fe from the Latin word Ferrum.

ions and ionic charges

Predicting Ion Charges on the Periodic Table

Ion charges can often be predicted from an element’s position on the periodic table. In chemical reactions, the nucleus stays unchanged, but electrons may be transferred, lost, or shared. When atoms gain or lose electrons during compound formation, they become ions, which are electrically charged particles. A positive ion is called a cation. A cation has more protons than electrons because it lost electrons. A negative ion is called an anion. An anion has more electrons than protons because it...

the periodic table

Periodic Table Patterns and Element Groups

The periodic table organizes elements by repeating patterns in their properties. Chemists first noticed that some elements behaved alike, so they grouped them by chemical behavior. Lithium, sodium, and potassium are one example. They are shiny and conduct heat and electricity well. Calcium, strontium, and barium form another group with similar physical and chemical properties. Yet these two groups are not the same. The lithium group is much more reactive, and its elements form oxygen compounds...

atomic mass

Average Atomic Mass and Isotopes

Average atomic mass explains why many elements on the periodic table have decimal values. Atoms are extremely small, so scientists use the atomic mass unit, or amu, to measure them. A carbon atom weighs less than 2 × 10−23 g, and the amu is defined from carbon-12. One amu is exactly 1/12 the mass of one carbon-12 atom, which is 1.6605 × 10−24 g. The dalton (Da) and the unified atomic mass unit (u) mean the same thing as the amu. For a single atom, atomic mass is usually close to its mass...

molar mass

Mole, Mass, and Avogadro’s Number

The mole links mass and the number of particles in a substance. It gives chemists a standard way to count atoms and molecules in samples that are far too small to see. It also helps show why substances with the same kinds of atoms can still have very different properties, like water, H2O, and hydrogen peroxide, H2O2. The mole is an amount unit, like a pair or a dozen. One mole contains 6.02214076 × 10^23 discrete entities, such as atoms or molecules. This number is usually rounded to 6.022 ×...

key terms and concepts

Explore Dalton’s atomic theory, the laws of conservation of mass, definite proportions, and multiple proportions, plus the early ideas that shaped modern chemistry.

Dalton’s Laws and Early Atomic Ideas | JoVE K12

chemistry

JoVE Core 化学は、簡潔で理解しやすいアニメーションビデオレッスンを使用して、一般的な化学の概念を生き生きとしたものにします。さらに、活動する科学者のビデオでは、現在世界中の実験室で行われている古典的そして独創的な研究・実験をお見せします。

Physical Science

PS.PSc.1.4

PS.PSc.1.5

Louisiana Student Standards for Science

High School

Matter And Its Interactions

HS-PS1-2

HS-PS1-3

HS-PS1-7

motion-and-stability-forces-and-interactions

Motion And Stability: Forces And Interactions

HS-PS2-6

ohios-learning-standards-and-model-curriculum

Ohio’s Learning Standards and Model Curriculum

Study Of Matter

Atoms

Structure And Properties Of Matter

Atomic structure

Physical Geology

Minerals

Atoms and elements

Tennessee Academic Standards

Matter and Its Interactions

CHEM1.PS1.2

CHEM1.PS1.11

Virginia  Standards of Learning

HIgh School

CH.2

CH.2.a

PS.2

PS.2.a

Minnesota Academic Standards in Science

2.2.1 9C.1.2.1.2

Arizona Science Standards

HS.P1

HS.P1U1.1

HS+C.P1

HS+C.P1U1.1

new-jersey-student-learning-standards-for-science

New Jersey Student Learning Standards for Science

Texas Essential Knowledge and Skills

CHEM.6

CHEM.6.D

Alabama Course of Study Science

9-12.C.1.1

9-12.C.1.1.a

9-12.C.1.1.b

9-12.PS.3.4.a

Next Generation Science Standards

HS-PS1-1

Earth and Space Science

Earth’s Place in the Universe

HS-ESS1-2

Florida Department of Education

SC.912.E.5

SC.912.E.5.2

SC.912.P.8

SC.912.P.8.3

Chemistry and Physics

IPC.7

IPC.7.A

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

South Carolina College and Career Ready Science Standards

C-PS1-1

C-PS1-2

C-PS1-3.

C-PS1-7

Motion and Stability: Forces and Interactions

C-PS2-6.

Georgia Standards of Excellence

SC1.

Atomic Models: Size, Charge, and Structure

Scientific Laws and Theories

Scientific Laws

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The Scientific Method

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Classifying Matter by State

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Subatomic Particles

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Elements: Chemical Symbols and Isotopes

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Use models to explain how the scientific understanding of atomic structure has evolved.

Radioactivity and Nuclear Equations

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Types of Radioactivity

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Nuclear Stability

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Nuclear Binding Energy

The difference between the calculated and experimentally measured masses is known as the mass defect of the atom. In the case of helium-4, the mass defect ...

Radioactive Decay and Radiometric Dating

Radioactivity is a spontaneous disintegration of an unstable nuclide and is a random process, as all the nuclei in the sample do not decay simultaneously. ...

Nuclear Fission

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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 ...

Nuclear Fusion

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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 ...

Atomic Mass

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Molar Mass

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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

atomic-radii-and-effective-nuclear-charge

Atomic Radii and Effective Nuclear Charge

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Ionic Radii

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Ionization Energy

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Electron Affinity

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Construct an explanation to infer the atomic size, reactivity, electronegativity, and ionization energy of an element based on its position in the Periodic Table.

PS.Chm.2.2

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Analyze and interpret data to explain the mechanisms and properties of the two main types of intramolecular (ionic and covalent) bonds.

PS.Chm.3.1

Analyze the structure of atoms and isotopes.

Dalton’s Laws and Early Atomic Ideas

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