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

Matter and its Interactions

PS.Chm.1.1

The Atomic Theory of Matter

Griechen wie Demokrit brachten zuerst die Idee des Atoms, der kleinsten unteilbaren Einheit der Materie, voran. Dieses Konzept wurde später von dem englischen Wissenschaftler John Dalton als Atomtheorie vorgestellt. Das erste Postulat von Daltons Atomtheorie besagt, dass Elemente aus winzigen unteilbaren Teilchen, den Atomen, bestehen.So besteht beispielsweise Wasserstoff aus zwei verbundenen Wasserstoffatomen und Sauerstoff aus zwei verbundenen Sauerstoffatomen. Das zweite Postulat besagt, dass die Atome desselben Elements zwar identisch sind, sich aber von den Atomen anderer Elemente unterscheiden. Alle Atome des Wasserstoffs sind also untereinander identisch, unterscheiden sich aber von den Atomen des Sauerstoffs.Das dritte Postulat besagt, dass sich Atome verschiedener Elemente in einfachen ganzzahligen Verhältnissen miteinander verbinden können, um Verbindungen zu bilden. Zum Beispiel verbinden sich zwei Wasserstoffatome und ein Sauerstoffatom in einem Verhältnis von 2 zu 1 zu H2O Wasser. Das letzte Postulat der Daltonischen Theorie besagt, dass chemische Reaktionen die Atome eines Elements nicht in Atome eines anderen Elements umwandeln;stattdessen ordnen sich die vorhandenen Atome neu an, um neue Substanzen zu bilden.Bei der Bildung von Wasser werden vorhandene Wasserstoff-und Sauerstoffatome weder erzeugt noch zerstört, sondern lediglich neu angeordnet. Dalton baute seine Atomtheorie auf zwei vorhergehende Gesetze über chemische Reaktionen auf:dem Gesetz der Massenerhaltung und dem Gesetz der bestimmten Proportionen. Der Gesetz der Massenerhaltung besagt, dass die Gesamtmasse vor und nach einer chemischen Reaktion konstant bleibt.So zerfällt 18 Gramm Wasser in 2 Gramm Wasserstoff und 16 Gramm Sauerstoff. Das Gesetz der bestimmten Proportionen besagt, dass unabhängig von der Quelle in einer bestimmten chemischen Verbindung das Massenverhältnis der einzelnen Elemente immer konstant bleibt. So wird eine Probe reinen Wassers immer ein Massenverhältnis von Wasserstoff zu Sauerstoff von 1 bis 8 aufweisen, unabhängig von der Gesamtmasse des Wassers.Dalton schlug dann das Gesetz der multiplen Proportionen auf der Grundlage seiner eigenen Theorie vor. Laut diesem Gesetz gilt, dass wenn sich zwei Elemente zu mehr als einer Verbindung verbinden, unterschiedliche Massen des einen Elements mit der festen Masse des anderen Elements in einem kleinen ganzzahligen Verhältnis verbinden. So verbindet sich eine feste Masse von Wasserstoff, 2 Gramm, mit verschiedenen Massen von Sauerstoff, 32 oder 16 Gramm, in einem kleinen ganzzahligen Verhältnis von 2 zu 1, um zwei verschiedene Verbindungen zu bilden Wasserstoffperoxid und Wasser.

die atomtheorie der materie

Die früheste aufgezeichnete Diskussion über die Grundstruktur der Materie stammt von antiken griechischen Philosophen. Leukipp und Demokrit argumentierten, dass alle Materie aus kleinen, endlichen Teilchen bestehe, die sie Atomos nannten, was „unteilbar“ bedeutet. Später kamen Aristoteles und andere zu dem Schluss, dass Materie aus verschiedenen Kombinationen der vier „Elemente“ – Feuer, Erde, Luft und Wasser – bestehe und unendlich unterteilt werden könne. Interessanterweise betrachteten diese Philosophen Atome und „Elemente“ als philosophische Konzepte, dachten aber offenbar nie daran, Experimente durchzuführen, um ihre Ideen zu testen. Die aristotelische Sicht auf die Zusammensetzung der Materie galt über zweitausend Jahre lang, bis der englische Wissenschaftler John Dalton die Chemie mit seiner Hypothese revolutionierte, dass das Verhalten der Materie mithilfe einer Atomtheorie erklärt werden könne. Viele von Daltons Hypothesen über die mikroskopischen Eigenschaften der Materie, die erstmals 1807 veröffentlicht wurden, sind in der modernen Atomtheorie immer noch gültig. Hier sind die Postulate von Daltons Atomtheorie: <ol> <li>Materie besteht aus äußerst kleinen Teilchen, den sogenannten Atomen. Ein Atom ist die kleinste Einheit eines Elements, die an einer chemischen Veränderung teilnehmen kann.</li> <li>Ein Element besteht aus nur einer Atomart, die eine für das Element charakteristische Masse aufweist und für alle Atome dieses Elements gleich ist. Eine makroskopische Probe eines Elements enthält eine unglaublich große Anzahl von Atomen, die alle identische chemische Eigenschaften haben.</li> <li>Atome eines Elements unterscheiden sich in ihren Eigenschaften von Atomen aller anderen Elemente.</li> <li>Eine Verbindung besteht aus Atomen von zwei oder mehr Elementen, die in einem kleinen, ganzzahligen Verhältnis kombiniert sind. In einer bestimmten Verbindung ist die Anzahl der Atome jedes ihrer Elemente immer im gleichen Verhältnis vorhanden</li> <li>Atome werden bei einer chemischen Veränderung weder erzeugt noch zerstört, sondern werden stattdessen neu angeordnet, um Substanzen zu ergeben, die sich von denen unterscheiden, die vor der Veränderung vorhanden waren.</li> </ol> Dalton verwendete drei Gesetze chemischer Reaktionen als Grundlage für seine Theorie: (1) das Gesetz der Massenerhaltung, (2) das Gesetz bestimmter Proportionen und (3) das Gesetz mehrerer Proportionen. Daltons Atomtheorie liefert eine mikroskopische Erklärung der vielen makroskopischen Eigenschaften der Materie. Das Massenerhaltungsgesetz wurde vom französischen Chemiker Antoine Lavoisier entdeckt. Es besagt, dass Atome bei einer chemischen Veränderung weder entstehen noch zerstört werden; Die Gesamtmasse der Materie, die vorhanden ist, wenn Materie von einer Art in eine andere übergeht, bleibt konstant. Dalton wusste auch von den Experimenten des französischen Chemikers Joseph Proust, der zeigte, dass alle Proben einer reinen Verbindung die gleichen Elemente im gleichen Massenverhältnis enthalten. Diese Aussage ist als Gesetz der bestimmten Proportionen oder Gesetz der konstanten Zusammensetzung bekannt. Die Annahme, dass die Anzahl der Atome der Elemente in einer bestimmten Verbindung immer im gleichen Verhältnis vorliegt, steht im Einklang mit diesen Beobachtungen. Dalton nutzte auch Daten von Proust sowie Ergebnisse seiner eigenen Experimente, um ein weiteres interessantes Gesetz zu formulieren. Das Gesetz der multiplen Proportionen besagt, dass, wenn zwei Elemente reagieren um mehr als eine Verbindung zu bilden, eine feste Masse eines Elements mit den Massen der anderen Elemente in einem Verhältnis kleiner ganzer Zahlen reagieren wird. Daltons Theorie lieferte einen Rahmen, der später erweitert wurde, um zu zeigen, dass das Atom aus subatomaren Teilchen besteht und dass Atome desselben Elements unterschiedliche Massen haben können, sogenannte Isotope. Dieser Text wurde angepasst von <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.</a>

Die Atomtheorie der Materie

Die früheste dokumentierte Diskussion über die Grundstruktur der Materie stammt von antiken griechischen Philosophen. Leucippus und Demokrit argumentierten, dass alles wichtig sei ...

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Atoms and Elements

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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.

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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...

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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...

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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

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Scientific Laws

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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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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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