The Atom.

Slides:



Advertisements
Similar presentations
Chapter 3 Atoms: The Building Blocks of Matter 3.1 The Atom:
Advertisements

The Building Blocks of Matter
Chapter 3.1. Objectives 1. Explain the law of mass, the law of definite proportions, and the law of multiple proportions 2. Summarize the five essential.
Atomic Theory History of Atom Early Greeks believed that matter consisted of tiny particles – they called the “atoms”
Chapter 2 Atoms. Greek philosopher, Democritus fifth century B.C., coined term atom, as particles that can not be cut or broken up further.
The Atom.
Early Early Atomic ideas 400 BC, Democritus – said world was made up of two things air and a basic particle called an atom. Atom was the smallest piece.
Atoms: The Building Blocks of Matter The Atom: From Philosophical Idea to Scientific Theory.
Laws of Matter & Dalton’s Atomic Theory Reviving the Ancient Idea.
Atomic Theory History of Atom Early Greeks believed that matter consisted of tiny particles – they called the “atoms”
Monday, Oct. 21 st : “A” Day Tuesday, Oct. 22 nd : “B” Day Agenda  Begin Chapter 3: “Atoms and Moles” Sec. 3.1: “Substances are Made of Atoms”  In-Class:
Unit 3: Atomic Theory. Law of Conservation of Mass Mass is neither created nor destroyed during chemical or physical changes The total mass in the reactants.
Definite Proportions, Multiple Proportions and Atomic Theory
From Philosophical Idea to Scientific Theory
Chapter 4: Atoms and Elements.  Recognize that all matter is composed of atoms.  Explain the early ideas that led to the current understanding of the.
Understanding Matter Ancient Ideas.
Courtesy: B.C. – Matter was composed of four fundamental substances: fire, earth, water, and air. Greeks considered whether matter.
Ch.4 Atomic Structure How do we know atoms exist? Picture, in your mind, what you think an atom looks like.
Bell Work On your bell work sheet, date today’s entry: 1.How many Sig. Figs. are in ? 2.Using the correct Sig. Figs, evaluate the following: 3.12.
Unit 3 Atomic Theory Chapter 3.
Atoms – Building Blocks of Matter Notes - Chapter 3 Atoms – Building Blocks of Matter Notes - Chapter 3.
Bell Work On your bell work sheet, date today’s entry: 1.If a cube has a side length of 2 m, what is it’s volume in cm 3 ? 2.Using the correct Sig. Figs,
Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Table of Contents Chapter 3 Atoms: The Building Blocks of Matter.
OUTLINE of TOPICS 1. The Story of Atom 2. Subatomic Particles 3. J.J. Thomson 4. Milikan Middle School 5. E. Rutherford 6. The Periodic Table 7. Counting.
Atoms and Moles – Chapter 3 Substances are made of atoms 3.1.
Atomic Structure PSC Chapter 3. Atomic Theory of Matter Evidence of atoms Law of Definite Proportions Law of Conservation of Mass Law of Multiple Proportions.
Foundations of Atomic Theory The transformation of a substance or substances into one or more new substances is known as a chemical reaction.
Chapter 3 Lesson Starter Young people should not smoke.
Christian Madu, Ph.D. Collin College Lecture Presentation Chapter 2-1 Atoms and Elements.
The Building Blocks of Matter. Objectives Recognize that science is a progressive endeavor that reevaluates and extends what is already known. (SPI 3221.
Ch. 3: Atoms 3.1 Foundations. History  Democritus named the most basic particle named the most basic particle atom- means “indivisible atom- means “indivisible.
Atoms & Their Structure Chapter 2 Section 1 Part 1.
 Objectives: ◦ Explain  The law of conservation of mass  The law of definite proportions  The law of multiple proportions ◦ Summarize the 5 points.
Chemical Foundations: Elements, Atoms, and Ions Atoms & Compounds.
Chapter 3 Atoms and matter. laws The transformation of a substance or substances into one or more new substances is known as a chemical reaction. Law.
 Suggested Reading pgs Pages Chapter 3, Section 1 - Atoms STM (scanning tunneling microscope) image of a single zigzag chain of cesium.
Section 1 The Atom: From Philosophical Idea to Scientific Theory
Dalton’s Atomic Theory. Law of Conservation of Mass The total mass of materials after a chemical reaction is the same as the total mass before the reaction.
Chapter 3 - Atoms: The Building Blocks of Matter.
1 History – Democritus to Dalton Mr. ShieldsRegents Chemistry U01 L01.
Atoms: PAGE 37 OF INB. Essential Question  How are Dalton’s atomic theory and modern atomic theory similar and different?
3-1 Early Models of the Atom. Atoms? ► The Greek Philosopher Democritus  Proposed that all matter is made up of small indivisible particles  Called.
ATOMIC THEORY Philosophical Idea to Scientific Theory Chapter 3 Section 1.
The Atom CHAPTER 3.1 MS. COX’S CHEMISTRY CLASS. Lesson Objectives Explain the law of conservation of mass, the law of multiple proportions and the law.
Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu The activity 1.Break into your groups and move the desks out of the.
From Philosophical Idea to Scientific Theory
Ch. 3 – Atoms: The Building Blocks of Matter
Section 3.1. Atomic Theory  400 BC – Democritus  Coined the term atom from the Greek word atomos  Philosophical Idea – No Experimental Evidence  Idea.
1. Pick up a picture from teacher 2. Conduct research using your phones and textbook to find: birth date- death date country, state, city of origin major.
Have you ever tried to observe or study something that you could not see?
Bell Work How many steps are in the scientific method? What does the atom look like? (draw a picture) What are the parts of an atom? What is the atom mostly.
The Building Blocks of Matter
Bell-Ringer How have your ideas about Santa Claus and the Easter Bunny changed as you have grown up? Is it important to keep an open mind when it comes.
The Atom.
Topic 3 Periodic Table The development of the Atomic theory.
Chapter 3: Atoms-The Building Blocks of Matter
Atomic Theory.
Foundations of Atomic Theory
Evolution of the Atomic Model
The Atom: From Philosophical Idea to Scientific Theory
The Atom: From Philosophical Idea to Scientific Theory
Chapter 3 Lesson Starter Young people should not smoke.
The History of The Atomic Theory
The Atom.
Atoms Model.
Chapter 3 Lesson Starter Young people should not smoke.
Foundations of Atomic Theory
The Atom: The Building Blocks of Matter
Atomic Structure PSC Chapter 3.
Atoms: The Building Blocks of Matter
Presentation transcript:

The Atom

Early Greek Theories Democritus 440 B.C. - Democritus thought matter could not be divided indefinitely. He called nature’s basic particle the “atom”, from the Greek word meaning “indivisible”. Aristotle 350 B.C - Aristotle modified an earlier theory that matter was made of four “elements”: earth, fire, water, air. Aristotle was wrong. However, his theory persisted for 2000 years.

Foundations of the Atom In the late 1700s chemists believed the modern definition of an element as a substance that cannot be further broken down by ordinary chemical means. It was also clear that elements combine to form compounds that have different physical and chemical properties than those of the elements that form them. Na + Cl → NaCl Different properties

Chemists at this time could not agree whether elements always combined in the same ratio when forming a particular compound. When a substance or substances are transformed into one or more new substances, it is caused by a chemical reaction. Forming lead iodide

In the 1790s, scientists began to analyze chemical reactions In the 1790s, scientists began to analyze chemical reactions. This lead to the discovery of several basic laws. The law of conservation of mass (matter (mass) is neither created nor destroyed during ordinary physical or chemical changes). Antoine Lavoisier, a French chemist, verified this law by experimentation in 1789.

The Law of Conservation Of Mass

In 1799, Joseph Proust, a French chemist, showed that a given compound always contains exactly the same proportion of elements by mass. The principle of the constant composition of compounds, originally called “Proust’s law”, is now known as the law of definite proportions.

The law of definite proportions (a chemical compound contains the same proportions by mass regardless of the size of the sample or source of the compound. For example, sodium chloride (table salt) always consists of 39.34% by mass of the element sodium, Na, and 60.66% by mass of the element chlorine, Cl.

Proust’s discovery stimulated John Dalton, an English schoolteacher, to think about atoms as the particles that might compose elements. Dalton discovered another principle that convinced him of the existence of atoms. He noted, for example, that carbon and oxygen form two different compounds that contain different relative amounts of carbon and oxygen (CO and CO2). This led to the law of multiple proportions in 1803.

The law of multiple proportions (if two or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first element is always a ratio of small whole numbers. For example, the elements carbon and oxygen form two compounds, carbon dioxide and carbon monoxide. CO molecules are always composed of one C atom and one O atom. CO2 molecules are always one C atom and two O atoms.

Law of Multiple Proportions

Dalton’s Atomic Theory In 1808, John Dalton proposed an explanation for the three laws (Atomic Theory). All matter is composed of extremely small particles called atoms. Atoms of a given element are identical in size, mass, and other properties; atoms of different elements differ in size, mass and other properties. Atoms cannot be subdivided, created, or destroyed. Atoms of different elements combine in simple whole-number ratios to form chemical compounds. In chemical reactions, atoms are combined, separated, or rearranged.

Modern Atomic Theory Aspects of Dalton’s theory have been proven incorrect (we know now that atoms are divisible and a given element can have atoms with different masses).