Chapter 2 Atoms, Molecules, and Ions semester 1/ The Structure of Atom 2.3 Atomic Number, Mass Number, and Isotopes 2.4 The Periodic Table
|
|
|
- Brooke Baker
- 5 years ago
- Views:
Transcription
1 Chapter 2 Atoms, Molecules, and Ions semester 1/ The Structure of Atom 2.3 Atomic Number, Mass Number, and Isotopes 2.4 The Periodic Table 2.5 Molecules and Ions 2.6 Chemical Formulas Ref: Raymond Chang/Chemistry/ Twelfth Edition Prepared by A. Kyi Kyi Tin
2 2.2 The Structure of Atom Atom..the basic unit of an element that can enter into chemical combination (extremely small and indivisible) Three subatomic particles electrons, protons, and neutrons. The Electron (Joseph John Thomson ( ) Negatively charged particles Source: (from cathode ray tube experiment, forerunner of the television tube) The cathode ray is attracted by the plate bearing positive charges and repelled by the plate bearing negative charges, it must consist of negatively charged particles.
3 Cathode Ray Tube
4 J.J. Thomson, measured mass/charge of e - (1906 Nobel Prize in Physics)
5 Radiation emission and transmission of energy through space in the form of waves.. Radioactivity (Antoine Henri Becquerel( ) spontaneous emission of particles and / or radiation / Any element that spontaneously emits radiation is Radioactive.
6 (Uranium compound) 2.2
7 Three types of rays produced by decay of radioactive substances such as Uranium.. (i) Alpha (α ) rays..positively charged particles (α ) particles.. deflected by positively charged plate (ii) Beta (β) rays..electrons..deflected by negatively charged plate (iii) Gamma (γ) rays..high-energy rays..no charge and are not affected by an external field.
8
9 (1908 Nobel Prize in Chemistry) α particle velocity ~ 1.4 x 10 7 m/s (~5% speed of light) 1. atoms positive charge is concentrated in the nucleus 2. proton (p) has opposite (+) charge of electron (-) 3. mass of p is 1840 x mass of e - (1.67 x g)
10 The Proton and the Nucleus 1910,Ernest Rutherford s experiment (Refer text bk. Pg.47,48) Nucleus a dense central core within the atom Proton positively charged particles in the nucleus Source: whenever α. Came close to a nucleus in the scattering experiment, it experienced a large repulsive and therefore a large deflection. (i.e nucleus is composed of positively charged particles, which called proton)
11 The Neutron (James Chadwick, 1932) -electrically neutral particles having a mass slightly greater than that of protons Particle Mass (g) Charge unit Electron Proton Neutron 9.10 x x x Source: When a thin sheet of beryllium is bombarded with α-particles, a very high-energy radiation similar to γ- rays was emitted by the metal i.e Neutron
12 mass p = mass n = 1840 x mass e - 2.2
13 2.3 Atomic Number, Mass Number, and Isotopes Atomic Number (Z) the number of protons in the nucleus of each atom of an element. Mass Number (A) the total number of neutrons and protons present in the nucleus of an atom of an element. Isotopes atoms that have the same atomic number but different mass number. 2 3 H,... 1 H,... 1 H hydrogen... deuterium... tritium 1 1 Mass number Atomic number A Z X
14 2.4 The Periodic Table -A chart in which elements having similar chemical and physical properties are grounded together. -Groups Vertical Columns -Periods.Horizontal Rows -Metals.Good conductor of Heat & Electricity -Nonmetals Poor conductor of heat & electricity -Metalloids.Intermediate b/w Metal & Non-metal -Alkali metals(1a)/ Alkaline Earth metals(2a)/ Halogens( 7A)/ Noble gases (or) Rare gases (8A)
15 Alkali Metal Alkali Earth Metal Period Group Halogen Noble Gas
16 2.5 Molecules and Ions Molecule an aggregate of at least two atoms in definite arrangement held together by chemical forces (Chemical bonds) SAME ELEMENTS (or) TWO (or) MORE ELEMENTS IN A FIXED RATIO Diatomic molecules same elements (H 2,O 2,Cl 2 ) Polyatomic molecules different elements (HCl, CO) more than two atoms (O 3, H 2 O,NH 3 ) Ions..an atom or a group of atoms that has a net positive or negative charge. Cations / Anions / monoatomic ions / polyatomic ions
17 2.6 Chemical Formulas Molecular Formula shows the exact number of atoms of each element in the smallest unit of a substance. Allotrope..one of two or more distinct forms of an element (carbon..diamond and graphite) Structural Formula shows how atoms are bonded to one another in a molecule. Empirical Formula..which elements are present and the simplest whole number ratio of their atoms..
18 Molecular formula H 2 O H 2 O 2 Empirical formula H 2 O [HO] NH 3 NH 3 H 2 C 2 O 4 [HCO 2]] O 3 [O] Ionic compounds consist of a combination of cations and an anions. (example Na + Cl - )
Chapter 2. Atoms and the Periodic Table. Chemistry: Atoms First Julia Burdge & Jason Overby
Chemistry: Atoms First Julia Burdge & Jason Overby Chapter 2 Atoms and the Periodic Table Copyright (c) The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 2 Atoms and the
Chapter 2 Atoms, Ions, and the Periodic Table. Law of Conservation of Mass. Law of Conservation of Mass
Chapter 2 Atoms, Ions, and the Periodic Table Dalton s Atomic Theory Structure of the Atom Ions Atomic Mass The Periodic Table Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction
Internal Structure of an Atom, Ions and Isotopes
Internal Structure of an Atom, Ions and Isotopes Electrons, Protons, Neutrons, Ions, Isotopes, Metals & Non-metals, Ions, Periodic Table, Thompson s Experiment, Rutherford s Experiment, Chadwick s Experiment,
10/1/2017. General Chemistry CHEM 101 (3+1+0) Dr. Mohamed El-Newehy. Chapter 2. Chemistry: Atoms, Molecules and Ions
General Chemistry CHEM 101 (3+1+0) Dr. Mohamed El-Newehy http://fac.ksu.edu.sa/melnewehy Chapter 2 Chemistry: Atoms, Molecules and Ions 1 The Structure of the Atom Dalton s Atomic Theory (1808) o Compounds
ATOMIC STRUCTURE AND THE PERIODIC TABLE. Adapted from Addison Wesley Chemistry
ATOMIC STRUCTURE AND THE PERIODIC TABLE Adapted from Addison Wesley Chemistry HISTORY OF THE ATOM 4 th Century B.C. : Democritus suggested that matter was made up of very small particles called atoms.
Atoms, Molecules and Ions
Atoms, Molecules and Ions Chapter 2 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Dalton s Atomic Theory (1808) 1. Elements are composed of extremely small
Atoms, Molecules and Ions
Atoms, Molecules and Ions Atomic Theory of Matter Modern Atomic Theory Relation to Periodic Table Isotopes & Mass Number Periodic Table Ionic Compounds Molecular Compounds Acid Compounds The Atomic Theory
Atoms, Molecules and Ions
Atoms, Molecules and Ions Chapter 2 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Dalton s Atomic Theory (1808) 1. Elements are composed of extremely small
CHEMISTRY. Matter and Change. Table Of Contents. Section 4.1 Early Ideas About Matter. Unstable Nuclei and Radioactive Decay
CHEMISTRY 4 Table Of Contents Matter and Change Section 4.1 Early Ideas About Matter Chapter 4: The Structure of the Atom Section 4.2 Section 4.3 Section 4.4 Defining the Atom How Atoms Differ Unstable
CHAPTER 4 Atomic Structure
CHAPTER 4 Atomic Structure 4.1 Early Theories of Matter Earth, Water, Air, Fire Matter was thought to be infinitely divisible No method was available to test theories Democritus (460 B.C. 370 B.C.) First
Atoms to Minerals CH 5.1
Atoms to Minerals CH 5.1 Objectives Identify the characteristics of matter Compare the particles that make up atoms of elements Describe the three types of chemical bonds Identify the characteristics of
Glencoe: Chapter 4. The Structure of the Atom
Glencoe: Chapter 4 The Structure of the Atom Section One: Early Ideas about Matter Atomists and Democritus : 400 B.C. From Thrace in Greece. Atoms- Uncut-Table Indivisible parts which cannot be broken
Chapter 2. Atoms and the Periodic Table. Chemistry: Atoms First Third Edition Julia Burdge and Jason Overby
Chemistry: Atoms First Third Edition Julia Burdge and Jason Overby Chapter 2 Atoms and the Periodic Table Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chapter
Chapter 5. Early Atomic Theory and Structure
Chapter 5 Early Atomic Theory and Structure 1 5.1 Early thoughts ~ 400 B.C. Greek philosophers Empedocles all matter was composed of four elements earth, air, water, fire Democritus all forms of matter
Updating the Atomic Theory
Updating the Atomic Theory Three major differences between modern atomic theory and Dalton s atomic theory 1. Atoms are NOT indivisible. They are made up of smaller particles: electrons, protons and neutrons.
Chapter 2. Atoms, Molecules, and Ions
Chapter 2 Atoms, Molecules, and Ions Section 2.1 The Early History of Chemistry Early History of Chemistry Greeks were the first to attempt to explain why chemical changes occur. Alchemy dominated for
Name Honors Chemistry: Atoms, protons, electrons, neutrons, and the Periodic Table
Name Honors Chemistry: Atoms, protons, electrons, neutrons, and the Periodic Table 1. In the Periodic Table below, draw or shade in the following a. the numbers for the 8 main groups (also, indicate the
4.1 Structure of the Atom
4.1 Structure of the Atom How do atoms differ from each other? What are atoms composed of? What are the subatomic particles? 2-1 Structure of the Atom Atoms actually are divisible. They are composed of
Atoms, Molecules, and Ions. Chapter 2 AP Chemistry
Atoms, Molecules, and Ions Chapter 2 AP Chemistry Building blocks of chemistry. Atom Molecule Ion Dalton s Atomic Theory 1. An element is composed of tiny particles called atoms. 2. In an ordinary chemical
Atoms, Molecules and Ions. Chapter 2
Atoms, Molecules and Ions Chapter 2 2.1 The Atomic Theory of Matter Democritus [460-370 BCE] Described tiny, indivisible particles Called them atomos Differed from Aristotle 17th century - idea of atoms
2.1 Atomic Theory of Matter
Chapter 2 2.1 Atomic Theory of Matter The theory that atoms are the fundamental building blocks of matter re-emerged in the early nineteenth century, championed by John Dalton. Law of Conservation of Mass
Atomic Structure. Chemistry Mr. McKenzie
Atomic Structure Chemistry Mr. McKenzie How was the understanding of the atom developed? John Dalton (1766-1844) - developed a model to explain observations made at the time 1. Elements are made of tiny
CHAPTER 3. Chemical Foundations
CHAPTER 3 Chemical Foundations 3.1 THE ELEMENTS 118 elements in 92 occur naturally, the rest are synthesized All matter in the universe can be chemically broken down into elements Compounds are made by
Chapter 4 Atomic Structure. Chemistry- Lookabaugh Moore High School
Chapter 4 Atomic Structure Chemistry- Lookabaugh Moore High School Section 4.1 Defining the Atom Democritus (460 B.C 370 B.C.) first used the term atomon to describe the smallest particle of matter possible.
Basic Concepts of Chemistry Notes for Students [Chapter 2, page 1] D J Weinkauff - Nerinx Hall High School
![Basic Concepts of Chemistry Notes for Students [Chapter 2, page 1] D J Weinkauff - Nerinx Hall High School](/thumbs/78/77082572.jpg "Basic Concepts of Chemistry Notes for Students [Chapter 2, page 1] D J Weinkauff - Nerinx Hall High School")
Basic Concepts of Chemistry Notes for Students [Chapter 2, page 1] Chapter 2 Chemical Foundations: Elements, Atoms and Ions Section 2-1: The Elements Ultimately all substances in the universe can be broken
Chapter 2. and Ions. Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 2 John D. Bookstaver St. Charles Community College Cottleville, MO Atomic Theory of Matter
Chapter 2. Atoms, Molecules, and Ions
Chapter 2 Atoms, Molecules, and Ions The atomic theory Topics The structure of the atom Atomic number, mass number and isotopes The Periodic Table The atomic mass scale and the average atomic mass Molecules
Chapter 2. Atoms and Ions
Chapter 2 Atoms and Ions A History of Atomic Models 400 B.C.E. (Democritus, a early atomist) 1804 (Dalton) Law of Conservation of Mass Antoine Lavoisier 1743-1794 In a chemical reaction, matter is neither
Ch 2: Atoms, Molecules, and Ions
AP Chemistry: Atoms, Molecules, and Ions Lecture Outline 2.1 The Atomic Theory of Matter Greek philosophers: Can matter be subdivided into fundamental particles? Democritus (460 370 BC): All matter can
11. The bright-line spectra produced by four elements are represented in the diagram below.
1. Which substance can not be broken down by a chemical change? A) ammonia B) ethanol C) propanal D) zirconium 2. Which particle has no charge? A) electron B) neutron C) positron D) proton 3. Which phrase
Chapter 2. Atoms, Molecules, and Ions. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO
Lecture Presentation Chapter 2 John D. Bookstaver St. Charles Community College Cottleville, MO Atomic Theory of Matter The theory that atoms are the fundamental building blocks of matter reemerged in
Chapter 1. Chemical Foundations
Chapter 1 Chemical Foundations Chapter 1 Table of Contents (1.1) (1.2) (1.3) (1.4) (1.5) (1.6) (1.7) Chemistry: An atoms-first approach The scientific method The early history of chemistry Fundamental
AP* Chapter 2. Atoms, Molecules, and Ions. Monday, September 16, 13
AP* Chapter 2 Atoms, Molecules, and Ions AP Learning Objectives LO 1.1 The student can justify the observation that the ratio of the masses of the constituent elements in any pure sample of that compound
Chapter 2 Atoms and Elements
Chapter 2 Atoms and Elements Law of Conservation of Mass in a chemical reaction, matter is neither created nor destroyed total mass of the materials you have before the reaction must equal the total mass
Atoms, Molecules, and Ions
Chapter 2 Atoms, Molecules, l and Ions Chapter 2 Table of Contents 2.1 The Early History of Chemistry 2.2 Fundamental Chemical Laws 23 2.3 Dalton s Atomic Theory 2.4 Early Experiments to Characterize the
Who came up with the first theory of atoms?
The Beginnings of Atomic Theory Who came up with the first theory of atoms? In the fourth century BCE, the Greek philosopher Democritus suggested that the universe was made of indivisible units called
Chapter 3 https://youtu.be/thndxfdkzzs?list=pl8dpuualjx tphzzyuwy6fyeax9mqq8ogr
Chapter 3 https://youtu.be/thndxfdkzzs?list=pl8dpuualjx tphzzyuwy6fyeax9mqq8ogr The smallest particle of an element that retains the chemical properties of that element. Regions: Nucleus: very small region
Updating the Atomic Theory
Updating the Atomic Theory On the basis of Dalton s Atomic Theory: An atom is the basic unit of an element that can enter into chemical combination. Three major differences between modern atomic theory
Chapter 4 The Atom. Philosophers and scientists have proposed many ideas on the structure of atoms.
Chapter4 TheAtom 4.1 Early Models of the Atom An atom is the smallest particle of an element that retains its identity in a chemical reaction. Philosophers and scientists have proposed many ideas on the
Chapter 2. Atoms, Ions, and the Periodic Table. Chapter 2 Topics. 2.1 Dalton s s Atomic Theory. Evidence for Atoms. Evidence for Atoms
Chapter 2 Atoms, Ions, and the Periodic Table Chapter 2 Topics 1. Dalton s s Atomic Theory 2. Structure of the Atom 3. Ions 4. Atomic Mass 5. The Periodic Table Copyright The McGraw-Hill Companies, Inc.
Chapter 2. Conservation of Mass. Law of Definite Proportions. Group Activity. Draw you idea of what an atom looks like.
Group Activity Draw you idea of what an atom looks like. Chapter 2 Answer the following questions: How do you know what an atom looks like at the atomic level? How do scientists know what at atom looks
2 Atomic Theory Development of Theory
Atomic Theory Development of Theory Historical Atomic Models Democritus Greek philosopher who postulated that matter is comprised of atoms as the smallest part (ca 400 BC) John Dalton Max Planck J.J. Thompson
8. atomic mass: the mass of the element and represents the. 9. Atomic number: on top of the atomic symbol; represents the.
Intro To Chemistry Study online at quizlet.com/_2xw51k 1....:... 2. alkali metals: 8. atomic mass: the mass of the element and represents the number of protons plus the number of neutrons. 9. Atomic number:
CHAPTER #2 - Atoms, Molecules, and Ions
CHAPTER #2 - Atoms, Molecules, and Ions 2.1 The Early History of Chemistry - Ancient Greeks - thought matter was composed to 4 substances earth, air, fire, water ( vs. ) Alchemy - (discovered many elements;
Accelerated Chemistry Study Guide Atomic Structure, Chapter 3
Accelerated Chemistry Study Guide Atomic Structure, Chapter 3 Terms and definitions atom ion law of constant composition isotope atomic theory of matter mass number cathode ray tube atomic mass electron
Chapter 4. The structure of the atom. AL-COS Objectives 1, 2,3,4,7, 10, 15, 20, 21, 22, 27and 28
Chapter 4 The structure of the atom AL-COS Objectives 1, 2,3,4,7, 10, 15, 20, 21, 22, 27and 28 You ll learn to Identify the experiments that led to the development of the nuclear model of atomic structure
Early Atomic Models. Atoms: the smallest particle of an element that retains the properties of that element.
Chapter 5 Early Atomic Models Atoms: the smallest particle of an element that retains the properties of that element. (Greek: atomos = indivisible) Democritus (Greek teacher in the 4 th century BC) First
Chapter 4: Atomic Structure Section 4.1 Defining the Atom
Chapter 4: Atomic Structure Section 4.1 Defining the Atom Early Models of the Atom atom the smallest particle of an element that retains its identity in a chemical reaction Democritus s Atomic Philosophy
Chapter 4. Atomic Structure
Chapter 4 Atomic Structure History: Early 1800 s Lots of introductory work with electricity Atoms are electrical in nature Have parts with + charge Have parts with charge Technology was limited until late
Teacher: Mr. gerraputa. Name: Base your answer to the question on the information below. Given the electron dot diagram:
Teacher: Mr. gerraputa Print Close Name: 1. Given the electron dot diagram: The valence electrons represented by the electron dot diagram could be those of atoms in Group 1. 13 3. 3 2. 15 4. 16 2. Which
Mass number i. Example U (uranium 235) and U (uranium 238) atomic number e. Average atomic mass weighted of the isotopes of that element i.
CP NT Ch. 4&25 I. Atomic Theory and Structure of the Atom a. Democritus all matter consists of very small, indivisible particles, which he named i. Atom smallest particle of an element that retains all
ATOMS, MOLECULES and IONS
ATOMS, MOLECULES and IONS [MH5; Ch. 2] Atoms and Atomic Theory [MH5; 2.1-2.2] The three main postulates of atomic theory are: 1) Elements are made up of atoms. 2) In chemical reactions, atoms transfer
Atomic Structure. Electricity and the Atom. Electrolyte: A compound that conducts electricity when molten or dissolved in water.
Chapter 3 Atomic Structure Electricity and the Atom Electrolyte: A compound that conducts electricity when molten or dissolved in water. Electrodes: Carbon rods of metallic strips that carry electrical
Nuclear Chemistry. Atomic Structure Notes Start on Slide 20 from the second class lecture
Nuclear Chemistry Atomic Structure Notes Start on Slide 20 from the second class lecture The Birth of an Idea Democritus, 400 B.C. coined the term atom If you divide matter into smaller and smaller pieces,
Unit 2 Chapters 5 and 6 Atoms/Periodic Table/ NOMENCLATURE NAMING AND FORMING COMPOUNDS
Unit 2 Chapters 5 and 6 Atoms/Periodic Table/ NOMENCLATURE NAMING AND FORMING COMPOUNDS Review of Atomic Structure What is an atom? The smallest particle of an element that retains the properties of that
Unit Two: Atomic Structure
Unit Two: Atomic Structure TEKS 5: The student understands the historical development of the Periodic Table and can apply its predictive power. (b) use the Periodic Table to identify and explain the properties
Atomic Theory. Democritus to the Planetary Model
Atomic Theory Democritus to the Planetary Model Democritus Greek philosopher (460-370 BCE) Believed in the philosophy of materialism With Leucippus, they though that matter can not be divided infinitely.
Early Atomic Theories and the Origins of Quantum Theory. Chapter 3.1
Early Atomic Theories and the Origins of Quantum Theory Chapter 3.1 What is Matter Made of? People have wondered about the answer to this question for thousands of years Philosophers Matter is composed
Chapter 2. Atoms, Molecules, and Ions. Lecture Outline
Chapter 2. Atoms, Molecules, and Ions Lecture Outline 2.1 The Atomic Theory of Matter Greek Philosophers: Can matter be subdivided into fundamental particles? Democritus (460 370 BC): All matter can be
Chemistry Vocabulary. These vocabulary words appear on the Chemistry CBA in addition to being tested on the Chemistry Vocabulary Test.
Chemistry Vocabulary These vocabulary words appear on the Chemistry CBA in addition to being tested on the Chemistry Vocabulary Test. atom the smallest unit of an element that still represents that element.
Chapter 2 Atoms, Molecules, and Ions
1. What name is given to the concept that different samples of a given compound always contain the same elements in the same mass ratio? A) Ration Law D) Law of Definite Proportions B) Law of Equality
DATE: NAME: CLASS: BLM 1-9 ASSESSMENT. 2. A material safety data sheet must show the date on which it was prepared.
Chapter 1 Test Goal Demonstrate your understanding of the information presented in Chapter 1. What to Do Carefully read the instructions before answering each set of questions. True/False On the line provided,
Lecture Presentation. Chapter 2. Atoms, Molecules, and Ions. James F. Kirby Quinnipiac University Hamden, CT Pearson Education, Inc.
Lecture Presentation Chapter 2 James F. Kirby Quinnipiac University Hamden, CT Atomic Theory of Matter The theory that atoms are the fundamental building blocks of matter reemerged in the early nineteenth
Second Semester Chemistry Study Guide
Second Semester Chemistry Study Guide All of the information on this review is fair game for the final Some information will be more prevalent on the test (Think about which topics we spent more time on
4-1 Notes. Defining the Atom
4-1 Notes Defining the Atom Early Models of the Atom All matter is composed of atoms Atoms are the smallest particles of an element that retains their identity in a chemical reaction Greek philosopher
DescribeDemocritus s Democritus s ideas
Atomic Structure Section 4.1 Defining the Atom DescribeDemocritus s Democritus s ideas about atoms. Section 4.1 Defining the Atom Explain Dalton s atomic theory. Section 4.1 Defining the Atom Identifywhat
Atomic Structure. ppst.com
Atomic Structure ppst.com Defining the Atom The Greek philosopher (460 B.C. 370 B.C.) was among the first to suggest the existence of atoms (from the Greek word ) He believed that atoms were and His ideas
Unit 2 Atomic Structure and Nuclear Chemistry
Chemistry 1 West Linn High School Unit 2 Packet and Goals Name: Period: Unit 2 Atomic Structure and Nuclear Chemistry Unit Goals: As you work through this unit, you should be able to: 1. describe Dalton
The History of the Atom. How did we learn about the atom?
The History of the Atom How did we learn about the atom? The Atomic Theory of Matter All matter is made up of fundamental particles. What does fundamental mean? The Greek Philosophers, 400 B.C. Democritus
Chapter 2. Atoms, Molecules, and Ions. Copyright 2017 Cengage Learning. All Rights Reserved.
Chapter 2 Atoms, Molecules, and Ions Chapter 2 Table of Contents (2.1) (2.2) (2.3) (2.4) (2.5) (2.6) (2.7) (2.8) The early history of chemistry Fundamental chemical laws Dalton s atomic theory Early experiments
AP Chemistry Chapter 2
AP Chemistry Chapter 2 Atoms, Molecules & Ions The Atomic Theory of Maer > Democritus (460 370 BC) > Greek philosopher > Thought that material was made up of ny indivisible parcles called atomos > Aristotle
Democritus of Abdera. John Dalton. Dalton s Atom. Dalton s Atomic Theory Ancient Greece - 4th century BC. Eaglesfield, England
Democritus of Abdera Ancient Greece - 4th century BC first suggested the existence of tiny fundamental particles that make up matter. atoms = indestructible did not agree with the current sci theory -
CHAPTER 2. ATOMS, MOLECULES, AND IONS REMEMBER correct in a different color. Questions
CHAPTER 2 ATOMS, MOLECULES, AND IONS REMEMBER correct in a different color Questions 17. A compound will always contain the same numbers (and types) of atoms. A given amount of hydrogen will react only
ATOMS AND ELEMENTS. Democritus 400 B.C. Atomic Theory of Matter. Dalton s Postulates (1803) Page 1
ATOMS AND ELEMENTS Democritus 400 BC Believed that matter was composed of invisible particles of matter he called atoms According to Democritus, atoms could not be broken into smaller particles Atomic
Chapter 3: Atomic Theory
Chapter 3: Atomic Theory and Elements, Atoms, Compounds & Ions A. The Elements All of the materials in the universe can be chemically broken down into about 100 different elements. 1. Element can have
Structure of matter I
Structure of matter I "Could anything at first sight seem more impractical than a body which is so small that its mass is an insignificant fraction of the mass of an atom of hydrogen?" J.J. Thomson, about
What is a theory? An organized system of accepted knowledge that applies in a variety of circumstances to explain a specific set of phenomena
Atomic Structure What is a theory? An organized system of accepted knowledge that applies in a variety of circumstances to explain a specific set of phenomena Early Theories Democritus: 4 B.C.: atom He
Unit Two Test Review. Click to get a new slide. Choose your answer, then click to see if you were correct.
Unit Two Test Review Click to get a new slide. Choose your answer, then click to see if you were correct. According to the law of definite proportions, any two samples of water, H2O, A. will be made up
Chemistry CRT Study Guide First Quarter
Number AL COS # 1. #1.0 Classify sodium chloride as an element, mixture, compound, or colloid. Compound 2. #1.0 Classify air as an element, mixture, compound, or colloid. Mixture 3. #1.0 Classify a blueberry
Chapter 2 Atoms, Molecules, and Ions. 許富銀 ( Hsu Fu-Yin)
Chapter 2 Atoms, Molecules, and Ions 許富銀 ( Hsu Fu-Yin) 1 The Atomic Theory of Matter Democritus (460 370 bce) and other early Greek philosophers described the material world as made up of tiny, indivisible
Atom Practice Test (#1) 1) What is the total number of valence electrons in an atom with the electron configuration 2-8-5? a) 2 b) 5 c) 8 d) 15
Atom Practice Test (#1) Name Multiple Choice 1 pt. each 1) What is the total number of valence electrons in an atom with the electron configuration 2-8-5? a) 2 b) 5 c) 8 d) 15 2) A Ca 2+ ion differs from
Atomic Structure. Chapters 4, 8, Bravo 15,000 kilotons
Atomic Structure Chapters 4, 8, 18.1-18.3 Bravo 15,000 kilotons What is an atom? Smallest unit of an element that retains all the properties of the element Can combine with other atoms to form compound
Chapter 2 Atoms, Molecules and Ions
Sec$on 2.1 The Early History of Chemistry Chapter 2 Atoms, Molecules and Ions Sec$on 2.1 The Early History of Chemistry Early History of Chemistry Greeks were the first to a?empt to explain why chemical
CHAPTER -4 STRUCTURE OF ATOM CONCEPT DETAILS
CHAPTER -4 STRUCTURE OF ATOM CONCEPT DETAILS KEY CONCEPTS : [ *rating as per the significance of concept] 1. Dalton s Atomic theory ** 2. J J Thomson Experiments *** 3. Rutherford s Scattering Experiments
Chapter 2. Atoms, Molecules, and Ions. Copyright 2018 Cengage Learning. All Rights Reserved.
Chapter 2 Atoms, Molecules, and Ions Chapter 2 Table of Contents (2.1) (2.2) (2.3) (2.4) (2.5) (2.6) (2.7) (2.8) The early history of chemistry Fundamental chemical laws Dalton s atomic theory Early experiments
CHAPTER 4. Atomic Structure. 4.1 Atoms. Dalton s Atomic Theory
CHAPTER 4 Atomic Structure 4.1 Atoms Democritus first suggested the idea of atoms Indivisible & Indestructible 460 B.C. 370 B.C. Dalton s Atomic Theory 1. All elements are composed of submicroscopic indivisible
SCH3U- R. H. KING ACADEMY ATOMIC STRUCTURE HANDOUT NAME:
Particle Theory of Matter Matter is anything that has and takes up. All matter is made up of very small. Each pure substance has its of particle, from the particles of other pure substances. Particles
Unit 1 Chemistry Basics
Unit 1 Chemistry Basics Estimated Time: 1 hour Terminal Objective: At the completion of this unit, the students will identify basic chemistry concepts. Enabling Objectives: The students will: 1. Define
D) A majority of α particles will pass through a thin metal sheet undeflected, while a small percentage scatter wildly.
4. What was the experimental basis for determining that the nucleus occupies a very small fraction of the volume of an atom? A) Neutral particles are emitted when a sheet of beryllium is bombarded with
9/13/2011. The Greek Philosophers. Atomic Structure & The Periodic Table. Dalton s Atomic Theory. J. J. Thomson. Thomson s Experiment
Atomic Structure & The Periodic Table The Greek Philosophers Democritus believed that all matter is made up of tiny particles that could not be divided Aristotle -- thought that matter was made of only
EDULABZ INTERNATIONAL 3 STRUCTURE OF ATOMS
3 STRUCTURE OF ATOMS I. Multiple choice questions (Tick the correct option). 1. Which one of the following proposed the atomic theory of matter? (a) John Dalton (b) J.J. Thomson (c) Rutherford (d) Niels
Chapter 2: The Structure of the Atom and the Periodic Table
Chapter 2: The Structure of the Atom and the Periodic Table 1. What are the three primary particles found in an atom? A) neutron, positron, and electron B) electron, neutron, and proton C) electron, proton,
PreAP Chemistry. Unit 4 Atomic Structure, the Periodic Table, and Nuclear Radiation
PreAP Chemistry Unit 4 Atomic Structure, the Periodic Table, and Nuclear Radiation Democritus A Greek who lived ~400 BC, was the first to suggest the existence of atoms. He believed atoms to be indivisible
Chemistry B11 Chapter 3 Atoms
Chapter 3 Atoms Element: is a substance that consists of identical atoms (hydrogen, oxygen, and Iron). 116 elements are known (88 occur in nature and chemist have made the others in the lab). Compound:
Atomic Structure and Nuclear Chemistry Multiple Choice Questions PSI Chemistry
Atomic Structure and Nuclear Chemistry Multiple Choice Questions PSI Chemistry Name: 1. What was the first particle discovered inside an atom? A. Proton C. Electron 2. What characteristic of cathode rays
Early Models of the Atom
Early Models of the Atom An atom is the smallest particle of an element that retains its identity in a chemical reaction. Although early philosophers and scientists could not observe individual atoms,
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) A 25 g sample of sugar is found to contain 51.4% oxygen by mass. Another 250 g sample
Chapter 3 Atoms: The Building Blocks of Matter. Honors Chemistry 412
Chapter 3 Atoms: The Building Blocks of Matter Honors Chemistry 412 Foundations of Atomic Theory Democritus Greek Philosopher 460-370 B.C. Stated Matter could be divided into smaller & smaller particles
Using the Periodic Table
Quick Review - Dimensional Analysis - Density - Classification of Matter (end of Chapter 1 material) - Fundamental Laws - Dalton s Atomic Theory - Cathode-Ray Tube Experiment (J.J. Thomson) - Plum Pudding
Forming Chemical Bonds
Forming Chemical Bonds Why do atoms form chemical bonds? so that the system can achieve the lowest possible potential energy Example covalent bonding in H 2 H H Potential energy 0 Distance of separation