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

早期的希腊人，如德谟克利特，首先 提出了原子团的概念，它是物质最小的不可分割 的单位。这一概念后来被英国科学家 约翰道尔顿作为原子理论提出。道尔顿的原子理论的第一个假设 认为元素是由叫做原子的不可分割的微小 粒子组成的。例如，氢气是由两个键合在一起的氢原子 组成的，而氧气是由两个键合在一起的 氧原子组成的。第二个假设是，虽然同一元素的原子 是相同的，但它们不同于其他元素的原子。因此，所有的氢原子彼此完全相同，但不同于氧原子。第三个假设是，不同元素的原子 可以以简单的整数比相互结合，形成化合物。例如，两个氢原子和一个氧原子 以 2:1 的比例结合形成 H2O 水。道尔顿理论的最后一个假设是 化学反应不会 把一种元素的原子变成 另一种元素的原子；相反，现有的原子 会重新进行自我排列以形成新的物质。在水的形成过程中，现存的氢原子和氧原子 既没有被创造也没有被破坏，它们只是重新排列了。道尔顿把他的原子理论建立在先前的两个 化学反应定律之上 质量守恒定律 和定比例定律。质量守恒定律指出，化学反应前后的总质量 保持不变。所以，18 克的水会分解成 2 克的氢气 和16 克的氧气。定比定律指出 在一个给定的化合物中，不管是什么来源，组成元素的质量比始终保持不变。因此，不管水的总质量是多少，一个纯水样品的氢氧质量比 始终为 1:8。道尔顿根据他自己的理论 提出了多重比例定律。根据这个定律，当两种元素 结合形成一种以上的化合物时，一种元素的不同质量 与另一种元素的固定质量 以较小的整数比结合。因此，一个固定质量的氢，2 克，与不同质量的氧，32 克或 16 克，以 2：1 的小整数比结合，可以形成两种不同的化合物 过氧化氢和水。

物质的原子理论

关于物质基本结构的最早记录记载来自古希腊哲学家。勒皮普斯（Leucippus）和德谟克利斯（Democritus）争辩说，所有物质都是由有限的小颗粒组成的，它们称为 atomos ，意思是“不可切分的”。后来，亚里士多德（Aristotle）和其他人得出结论，物质由四个“元素”的各种组合组成。 ＆mdash;火，土，空气和水＆mdash;并可以无限分裂。有趣的是，这些哲学家对原子和“元素”进行了思考。作为哲学概念，但显然从未考虑过进行实验来检验其思想。
 
 亚里士多德关于物质成分的观点一直流行了两千多年，直到英国科学家约翰·道尔顿（John Dalton）以其假设可以用原子理论来解释物质的行为而彻底改变了化学。道尔顿关于物质的微观特征的许多假设首次发表于1807年，在现代原子理论中仍然有效。
 
 以下是道尔顿原子理论的假设：
 
 <ol>
 物质由称为原子的极小颗粒组成。原子是元素中可以参与化学变化的最小单元。</ li>
 <li>元素仅由一种原子组成，其质量是元素的特征，并且对该元素的所有原子都相同。元素的宏观样本包含数量惊人的原子，所有原子都具有相同的化学性质。</ li>
 <li>一种元素的原子在性质上不同于所有其他元素的原子。</ li>
 化合物由以较小的整数比例结合的两个或多个元素的原子组成。在给定的化合物中，其每个元素的原子数始终以相同的比例存在</ li>
 <li>在化学变化过程中既不会产生原子也不会破坏原子，而是将其重新排列以产生与变化之前存在的物质不同的物质。</ li>
 </ ol>
 
 道尔顿使用了三个化学反应定律作为其理论的基础：（1）质量守恒定律；（2）定比定律；（3）倍比定律。道尔顿的原子理论对物质的许多宏观特性提供了微观解释。
 
 质量守恒定律 是由法国化学家安托万·拉瓦锡（Antoine Lavoisier）发现的。它指出原子在化学变化过程中既不会产生也不会破坏。当物质从一种类型变为另一种类型时，物质的总质量保持不变。
 
 道尔顿还知道法国化学家约瑟夫·普鲁斯特（Joseph Proust）的实验，他证明了纯化合物的所有样品都包含相同质量百分比的相同元素。这种说法称为<定比定律>或成分不变定律>。关于给定化合物中元素的原子数始终以相同比例存在的建议与这些观察结果一致。
 
 道尔顿还利用普鲁斯特的数据以及他自己的实验结果来制定另一条有趣的定律。 倍比定律指出，当两个元素反应形成一个以上的化合物时，一个元素的固定质量将与其他元素的质量以较小的整数之比发生反应。 >
 
 道尔顿理论提供了一个框架，该框架后来进行了扩展，以证明该原子由亚原子粒子组成，并且同一元素的原子在质量上可以不同，称为同位素。
 
 本文改编自<a href="https://openstax.org/books/chemistry-2e/pages/2-1-early-ideas-in-atomic-theory"> Openstax，化学2e，第2.1节：原子理论的早期思想。</a> ＆nbsp;

关于物质基本结构的最早记载可追溯至古希腊哲学家。留基伯和德谟克利特提出，所有物质……

Education

教育

JoVE Core

化学

Atoms and Elements

原子与元素

KEY TERMS AND CONCEPTS

关键术语与概念

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 化学通过简单明了且通俗易懂的动画视频课程，将普通化学概念带入到现实生活当中。此外，在科学家行动视频中，我们演示了在实验室中进行的经典和原始研究实验。

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

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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

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Radioactive Decay and Radiometric Dating

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Nuclear Fission

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The Energies of Atomic Orbitals

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The Aufbau Principle and Hund's Rule

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PS.Chm.1.3

Periodic Classification of the Elements

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Atomic Mass

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PS.Chm.3.1

Analyze the structure of atoms and isotopes.

Dalton’s Laws and Early Atomic Ideas

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