Modern Version of the Experiment: Using electricity, water is electrolyzed into its components, hydrogen and oxygen. Results: Water is always found to.

Slides:

Advertisements

Similar presentations

History at a Glance Atoms.

Advertisements

The Structure of the Atom

SCH 3UY - Atomic Theory Review

3-2 Discovering Atomic Structure

2008, Prentice Hall Chemistry: A Molecular Approach, 1 st Ed. Nivaldo Tro Roy Kennedy Massachusetts Bay Community College Wellesley Hills, MA.

CHEMISTRY 161 Chapter The Early Atomic Theory pure substances compounds elements combine different elements H 2, O 2 H 2 O [O 3 ] John Dalton.

 You cannot see them, yet they make up everything…

The History of the Atom.

Atomic Theory and the Atom

Lecture 49/7/05 Homework concerns Atomic Structure.

Chpt. 2: The Atom.

11 Atomic Theory. 2 A HISTORY OF THE STRUCTURE OF THE ATOM.

Chapter 3 Atoms and Atomic Structure Write the bullets that are in black font.

Chapter 2 Atoms, Molecules, Ions.

Atomic Theory PS 9.26 PS 9.27 What is the nature of matter? The ancient Greeks pondered that question. Empedocles in 460 B.C.suggested that all matter.

Atomic Discovery Early Models of the Atom 400 B.C. – Democritus proposed the existence of fundamental particles of matter that were indivisible and indestructible.

Chemistry Sheds Light on Our Lives Unit 4 Atoms and Light

Chapter 4: Discovery of Atomic Structure. Prentice Hall © 2003Chapter 2 The Discovery of Atomic Structure An ancient Greek named Democritus was the first.

PART ONE ATOMIC THEORY. Over the course of thousands of years our idea of what matter is made of and what the atom looks like has changed dramatically.

Fundamental Chemical Laws

1 Atoms, Molecules, and Ions Chapter 2 2 John Dalton ( early 1800s): –Each element is composed of atoms –All atoms of an element are identical. –In chemical.

Atomic Structure Atoms and their structure Mr. Bruder.

, who was from was the first person to use the term atom during B.C.  Democritus defined the atom as being.  opposed Democritus because believed that.

The History of the Atom…. went against, Aristotle, who believed that matter was composed of four qualities: earth, fire, air and water all matter is composed.

A History of Atomic Theory & Basic Atomic Structure Chapter 3: The Atom Big Idea: Physical, chemical and nuclear changes are explained using the location.

Introduction to Atomic Structure Chemistry Chemistry is the study of matter and the changes it undergoes. The type of matter that is changing and what.

The Historical Development of the Atomic Model From ancient Greece philosophy, to today’s model of the atom – The model of the atom demonstrates the purpose.

Chapter 2 (Part I) Atoms, Molecules, and Ions History n Greeks n Democritus and Leucippus - atomos n Aristotle- elements n Alchemy n Robert Boyle-

Mullis1 Democritus ( B.C.) Democritus was one of a few Greek philosophers who believed that all matter in the world was made of of indivisible parts.

Chapter 4 Atomic Structure Early Atomic Theory Greeks: The world is made of two things, empty space and “atoms”. Atoms are the smallest possible stuff.

Atoms, Molecules and Ions

Chapter 3: The Atom “The Building Blocks of Matter”

HISTORY OF THE ATOM. Aristotle 400 BC 400 BC - Claimed that there was no smallest part of matter - Claimed that there was no smallest part of matter -

ATOMIC THEORY. History of the Atom  feature=related feature=related.

Lecture 3, Fall CHAPTER 2. Atoms, molecules, and ions.

Atomic Theory 15,000 kilotons.  Dismissed idea of the atom. Early Greeks Two schools of thought:  Matter is made of indestructible particles called.

Early Atomic Models Democritus –World is made of two things: empty space and indivisible particles, called atoms –There are different atoms for every material.

“How could you find the Invisible Man in Picadilly Circus?…. By the reactions of those he pushed aside.” -Ernest Rutherford’s advice to James Chadwick.

In 1782, a French chemist, Antoine Lavoisier ( ), made measurements of chemical change in a sealed container. Development of the Modern Atomic.

ATOMIC THEORY Honors Chemistry Mr. McKenzie. Atomic Structure Essential Questions: –How was the modern theory of atomic structure developed? –What are.

Going Further into Atomic Structure Thomson, Rutherford, and Millikan.

Section 4.2 Defining the Atom.

Atoms, Molecules and Ions Chapter 2. Foundations of Atomic Theory Law of conservation of mass: Antoine Lavoisier –Mass is neither created nor destroyed.

Ch. 4.2 Structure of the Nuclear Atom

Models of Atomic Structure. Dalton’s Small Dense Sphere.

EARLY ATOMIC THEORY CHAPTER 3. THE ATOM: FROM PHILOSOPHY TO SCIENTIFIC THEORY 400 BC – Democritus came up with the idea of the ________ Nature’s basic.

Evolution of the Atomic Theory. Greek Philosophy (400 BC) Democritus “All matter is made of atoms” Philosophy is knowledge gained only by observation.

History of Atomic Theory. Democritus (c. 450 BCE) Was commonly held that “something” could come from “nothing” Response to this by atomists like Democritus:

Ch 3 Atomic Theory Models of the Atom

Chapter 3 Atoms : The Building Blocks of Matter. Foundations of Atomic Theory  Several basic laws were after the 1790’s (emphasis on quantitative analysis):

The Atom - Scientists. Philosophers Democritus – believed matter was not infinitely divisible THERE WERE NO EXPERIMENTS TO TEST HIS IDEAS Matter is composed.

Mullis1 Discovery of Atomic Structure By 1850 scientists knew that atoms were composed of charged particles. Electrostatic attraction: Like charges repel.

Ch 5: Atomic Structure. warmup All matter is composed of very small particles called atoms. In middle school science you learned about the atom. 1. Draw.

Evolution of the Atomic Theory. Greek Philosophy (400 BC) Democritus “All matter is made of atoms” Philosophy is knowledge gained only by observation.

Atomic Structure Power Point First Part Chemistry I-AAHS Dr. Gray.

Atoms, Molecules and Ions Chapter 2. Foundations of Atomic Theory _________________________________________ –Mass is neither created nor destroyed. The.

Atomic Theory In 1808, the English Chemist John Dalton proposed the first theory of the nature of matter in stating that all matter was composed of atoms.

UNIT 2 Atoms, Molecules, and Ions. 1. Each element is composed of extremely small particles called atoms. 2. All atoms of a given element are identical.

CONCURRENT ENROLLMENT CHEMISTRY

History of the Atom Notes

Atomic Structure.

Chapter 4: atoms.

Chapter 3- Atomic Structure

Atomic history.

CHAPTER 3 – The Structure of the Atom

Presentation transcript:

Modern Version of the Experiment: Using electricity, water is electrolyzed into its components, hydrogen and oxygen. Results: Water is always found to contain hydrogen and oxygen in a mass ratio of 1:8 (volume ratio of 2:1) no matter how it is formed or where it is found. Scientist: Joseph Proust, 1799

Experiment: Wrote a book entitled: A New System of Chemical Philosophy (1808) Results: 1. All matter is composed of tiny indivisible particles called atoms. 2. Atoms of the same element are exactly the same; atoms of different elements are different. 3. Atoms combine in whole number ratios to form compounds. A given compound always has the same relative number and kind of atoms. 4. Atoms cannot be created or destroyed in chemical reactions, they are merely rearranged. Scientist: John Dalton, 1808

Scientist: J.J. Thomson, 1897 Experiment: An electric current is passed through an evacuated and sealed glass tube. Results: The voltage causes negative particles to move from the negative electrode to the positive electrode. The path of the electrons can be altered (deflected) by the presence of a magnetic field depending on the applied magnetic and electric fields.

Scientist: Robert Millikan, 1909 Experiment: Oil drops are sprayed above a positively charged plate containing a small hole. As the oil drops fall through the hole, they are given a negative charge. Gravity forces the drops downward. The applied electric field forces the drops upward. When a drop is perfectly balanced, the weight of the drop is equal to the electrostatic force of attraction between the drop and the positive plate. Results: Using this experiment, Millikan determined the charge on the electron to be 1.60  C.

Experiment: A radioactive substance is placed in a shield containing a small hole so that a beam of radiation is emitted from the hole. The radiation is passed between two electrically charged plates and detected. Results: Three spots are noted on the detector: –a spot in the direction of the positive plate, –a spot which is not affected by the electric field, –a spot in the direction of the negative plate. Scientist: Henri Becquerel, 1896

Experiment: A source of α- particles was placed at the mouth of a circular detector. The α -particles were shot through a piece of gold foil. Results: Most of the α - particles went straight through the foil without deflection. Some α-particles were deflected at high angles. Scientist: Ernest Rutherford, 1910

Scientist: James Chadwick, 1932 Background: At the time, it was well known that hydrogen had 1 proton, and helium had 2 protons, but the ratio of the masses of a hydrogen atom to a helium atom is 1:4. Why? Experiment: A thin sheet of beryllium was bombarded with alpha particles, and a very high energy radiation similar to gamma rays was emitted by the metal. Results: The radiation was electrically neutral. This radiation was found to be another particle which had no charge but a slightly larger mass than a proton.