CHEMISTRY - ZUMDAHL 2E CH.1 - CHEMICAL FOUNDATIONS.
|
|
- Kathleen Hunt
- 5 years ago
- Views:
Transcription
1 !!
2 CONCEPT: MATTER Chemistry is the study of matter and the changes it undergoes, with the being its basic functional unit. When two or more of these elements chemically bond together they form an independent structure called a molecule. Classification of Matter Under appropriate conditions of pressure and temperature, most substances can exist in 3 states of matter:, and. have a fixed shape and volume. take up the shape and volume of a container. conform to the shape of a container, but not the volume. Microscopic Explanation for the Behavior of Gases, Liquids and Solids Gas Liquid Solid Assumes the and of its container. Assumes the of the portion of its container it occupies, but not the. Maintains a fixed and compressible compressible compressible Viscosity Viscosity Viscosity Viscous Viscous Viscous Page 2
3 CONCEPT: GROUP NAMES AND CLASSIFICATIONS Ever wonder where did this periodic table ever come from? At the end of the 18 th century, Lavoisier compiled a list of the 23 elements known at the time. In 1869, Dmitri Mendeleev coined the term Periodic Table. Today the total is 114 and still counting! Now, to understand chemistry fully it will be imperative that you memorize and learn the different portions of the Periodic Table. Phase Differences At room temperature (between 20 o C to 25 o C), all elements are except: Mercury and bromine are. Hydrogen, Nitrogen, Oxygen, Fluorine, Chlorine and the Noble Gases are. Page 3
4 CONCEPT: CHARGE DISTRIBUTIONS OF THE PERIODIC TABLE A majority of the elements on the periodic table are reactive because they all want to be like the. They have the perfect number of electrons in their outer atomic shells. 1. Metals tend to electrons to become positively charged ions called. Metals that have ONLY one charge are referred to as metals. Metals that have MORE THAN one charge are referred to as metals. 2. Nonmetals tend to electrons to become negatively charged ions called. Page 4
5 CONCEPT: ELEMENT SYMBOLS Some of the names and symbols for the elements are easy to recognize like Aluminum is Al, but some others aren t. EXAMPLE 1: Identify the elements by their given symbols. a. Au b. Hg c. Pb d. Fe e. Ag Some elements exist in nature connected to their exact double. We call these chemical Siamese twins. To recall them just remember this funny phrase: Have No Fear Of Ice Cold Beer Some elements exist in nature as monoatomic elements such as &. Some elements exist in nature as polyatomic molecules such as &. Page 5
6 CONCEPT: ATOMIC MASS Whether you call it atomic mass or weight both terms tell us the combined mass of the protons and neutrons in an element. The atomic masses listed for the elements on the periodic table are the of their isotopes. Isotopes are elements with the number of protons, but number of neutrons. Atomic Mass = [(Mass of Isotope 1) x (Fractional Abundance 1)] + [(Mass of Isotope 2) x (Fractional Abundance 2)] EXAMPLE 1: Antimony has two common isotopes. If one of the isotopes 121 Sb has an isotopic mass of amu and a natural abundance of 57.25%, what is the isotopic mass (to 4 significant figures) of the other isotope? The atomic mass of antimony is g/mol. EXAMPLE 2: The atomic mass of an imaginary element A is amu. If element A consists of two isotopes that have atomic masses of 250 and 253 respectively, what is the natural abundance of each isotope? Page 6
7 CONCEPT: STRUCTURE OF THE ATOM We learned that the basic functional unit in chemistry is the. Now it s time to go into an atom to figure out its components: subatomic particles. In the center of an atom there is the, It contains the subatomic particles: and. Spinning around it we find the third subatomic particle: the. PROTONS are charged subatomic particles. ELECTRONS are charged subatomic particles.! NEUTRONS are charged subatomic particles. ATOMIC NUMBER equals the number of and determines of an element. ATOMIC MASS equals the number of in an element. EXAMPLE: Identify the unknown element. a. Element X (8 protons, 8 electrons, 8 neutrons) b. Element Y (35 protons, 36 electrons, 46 neutrons) c. Element Z (12 protons, 10 electrons, 13 neutrons) Page 7
8 CONCEPT: MODERN ATOMIC THEORY According to the Law of in a reaction matter is neither created nor destroyed. Originated in 1789 by Antoine Lavoisier. CH4 (g) + 2 O2 (g) CO2 (g) + 2 H2O (g) According to the Law of all samples of a compound, no matter on their origin or preparation has the same ratio in terms of their elements. Originated in 1797 by Joseph Proust. CO 2 Mass Ratio = (12.0gC) (32.0gO) = According to the Law of when two elements (A & B) form different compounds, the masses of element B that combine with 1 g of A are a ratio of whole numbers. Originated in 1804 by John Dalton. NO Mass Ratio = (16.0gO) (14.0g N) =1.143 NO 2 Mass Ratio = (32.0gO) (14.0g N) = The ratio of the two mass ratios obtained then gives us a whole number: = 2.0 Page 8
9 CONCEPT: MODERN ATOMIC THEORY (PRACTICE) EXAMPLE 1: A g sample of iodine reacts with g of chlorine to form iodine pentachloride, ICl5. If iodine pentachloride is the only product formed calculate its mass. EXAMPLE 2: Two samples sodium fluoride decompose into their constituent elements. The first sample produces 15.8 kg of sodium and 20.1 kg of fluorine. If the second sample produces g of sodium, how many grams of fluorine were also produced? PRACTICE: Which of the following is an example of the law of multiple proportions? a. A sample of bromine (Br) contains equal amounts of its two isotopes. b. Two different samples of H2O have the same mass ratio. c. The atomic mass of sodium (Na) is amu. d. Two different compounds composed of sulfur (S) and oxygen (O) have different mass ratios: 2.48 g O: 1 g S and 1.24 g O: to 1 g S. Page 9
10 CONCEPT: THOMSON CATHODE RAY TUBE EXPERIMENT J.J. Thomson s cathode ray tube experiments led to the discovery of the. Apply an Electric Field When an electric field is applied across the cathode ray tube, the cathode ray is attracted to the plate with a charge. Applying a Magnetic Field A moving charged body behaves like a tiny magnet, and it can interact with an external magnetic field. The electrons are by the magnetic field. Determining the Charge-To-Mass Ratio In 1897, JJ Thomson, an English Physicist, determined the charge-to-mass ratio of an electron by adjusting the electric field so that the deflection (θe) was the same as the deflection (θb), and was able to calculate the charge-to-mass ratio of an electron using the following equation: e / m ratio = Eθ E B 2 l Thomson determined the charge-to-mass ratio of an electron to be x 10 8 coulombs per gram, meaning it was approximately 2000 times lighter than hydrogen, the lightest known atom. e / m ratio = Eθ E B 2 l = coulombs per gram Page 10
11 CONCEPT: RUTHERFORD GOLD FOIL EXPERIMENT The experiment also called the Rutherford Gold Foil experiment helped to discover that any given atom had a positively charged center called the. It is there where most of the atom s mass was concentrated. Subatomic Particle Charge Mass Relative Absolute Relative (in amu) Absolute (in kg) Proton (p + ) x C x Neutron (n o ) x Electron (e ) x C 5.49 x x Page 11
12 CONCEPT: MILLIKAN OIL DROP EXPERIMENT In 1913 Robert Millikan and Harvey Fletcher discovered the charge of an electron as being. The charge of an electron When an oil droplet is suspended, mass x acceleration (m x g) due to gravity is exactly counterbalanced by the electric force applied. The electric force applied equals the applied electric field E times the charge on the drop (q). Making them equal to one another: The mass of an electron By using his discovered charge and then the charge-to-mass ratio determined by Thomson s cathode ray tube experiment we are able to calculate the mass of electron. Page 12
CHEMISTRY - TRO 4E CH.2 - ATOMS & ELEMENTS.
!! www.clutchprep.com CONCEPT: GROUP NAMES AND CLASSIFICATIONS Ever wonder where did this periodic table ever come from? At the end of the 18 th century, Lavoisier compiled a list of the 23 elements known
More informationCHEMISTRY - MCMURRY 7E CH.2 - ATOMS, MOLECULES AND IONS.
!! www.clutchprep.com CONCEPT: GROUP NAMES AND CLASSIFICATIONS Ever wonder where did this periodic table ever come from? At the end of the 18 th century, Lavoisier compiled a list of the 23 elements known
More informationCHEMISTRY - BROWN 13E CH.2 - ATOMS, MOLECULES & IONS.
!! www.clutchprep.com CONCEPT: GROUP NAMES AND CLASSIFICATIONS Ever wonder where did this periodic table ever come from? At the end of the 18 th century, Lavoisier compiled a list of the 23 elements known
More informationChapter 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
More informationA = number of protons + number of neutrons Z = number of protons
Worksheet 3 Fundamentals Objectives To understand and be able to apply the fundamental laws. The Law of Conservation of Mass Mass can be neither created nor destroyed in a chemical reaction. The Law of
More informationChapter 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.
More informationChapter 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
More informationChapter 2 Atoms and Elements
1 Chapter 2 Atoms and Elements Sec 2.3 Modern Atomic Theory and the Laws That Led to it Law of conservation of mass states that in a chemical reaction, matter is neither created nor destroyed. Law of definite
More informationUnit 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
More informationEarly 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
More informationEarly Atomic Theory. Alchemy. The atom
Early Atomic Theory Chapter 3 Democritus 460 BC- ~ 370 BC Nothing exists except atoms and empty space; everything else is opinion. Matter is composed of small indivisible particles, atomos meaning Indivisible
More informationCHE 105 Exam 1 Spring 2016
CHE 105 Exam 1 Spring 2016 Your Name: Your ID: Question #: 1 Which one of the following states of matter does not take on the shape of its container? A. solid B. liquid C. gas Question #: 2 Which statement
More informationDemocritus & Leucippus (~400 BC) Greek philosophers: first to propose that matter is made up of particles called atomos, the Greek word for atoms
AP Chemistry Ms. Ye Name Date Block The Evolution of the Atomic Model Since atoms are too small to see even with a very powerful microscope, scientists rely upon indirect evidence and models to help them
More informationAtoms, 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
More informationChapter 5 Atomic Structure and the Periodic Table
Chemistry/ PEP Name: Date: Chapter 5 Atomic Structure and the Periodic Table Chapter 5: 1 16, 20, 21, 23, 24, 27-32, 35, 42, 44, 49, 50, 55 (32 total) Section Review 5.1 1. In your own words, state the
More informationExam Accelerated Chemistry Study Sheet Chap 04 The Atom/Periodic Table
Exam Accelerated Chemistry Study Sheet Chap 04 The Atom/Periodic Table Name /87 TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. Correct the False statements by changing
More informationLesson 6: Periodic Table & Atomic Theory
Lesson 6: Periodic Table & Atomic Theory Do Now 7Hg 10.11.18 In CJ, copy info down from board. Keep CJs out and open on your desk. On Do Now page, copy and answer questions below. 1. Name 4 properties
More informationChapter Two: Early History of Chemistry. Three Important Laws. Dalton s Atomic Theory (1808) Three Important Laws (continued) Greek Explanation
Greek Explanation Chapter Two: ATOMS, MOLECULES, AND IONS Notes 2.1 In the Greek model they theorized there were four elements earth, water, air, and fire. These elements were characterized by the following
More informationAccelerated 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
More informationChapter 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
More informationChapter 3. Table of Contents. Section 1 The Atom: From Philosophical Idea to Scientific Theory. Section 2 The Structure of the Atom
Atoms: The Building Blocks of Matter Table of Contents Section 1 The Atom: From Philosophical Idea to Scientific Theory Section 2 The Structure of the Atom Section 1 The Atom: From Philosophical Idea to
More informationChapter 2: Atoms and Elements
Chapter 2: Atoms and Elements April 2003 Early Ideas about the structure of Matter Ancient Greece Leucippus and Democritus: Proposed that there were many types of atoms, different in shape and size. Aristotle:
More informationChapter 3. Chapter 3. Objectives. Table of Contents. Chapter 3. Chapter 3. Foundations of Atomic Theory, continued. Foundations of Atomic Theory
Atoms: The Building Blocks of Matter Table of Contents Philosophical Idea to Scientific Theory Objectives Explain the law of conservation of mass, the law of definite proportions, and the law of multiple
More informationChapter 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
More informationSmoking at an early age may make it more difficult to quit smoking later. Which of the above statements is an opinion and which is a theory?
Preview Lesson Starter Objectives Foundations of Atomic Theory Law of Conservation of Mass Law of Multiple Proportions Dalton s Atomic Theory Modern Atomic Theory Section 1 The Atom: From Philosophical
More informationUnit 2 continued-chemical Foundations Atoms, Ions, &Elements
Unit 2 continuedchemical Foundations Atoms, Ions, &Elements The Elements Most abundant elements in/on Earth: Oxygen 49.2% Silicon25.7% Most abundant in the human body: Oxygen65.0% Carbon18.0 % Hydrogen10.0%
More information4.1 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
More informationCHAPTER 3. Atoms: The Building Blocks of Matter
CHAPTER 3 Atoms: The Building Blocks of Matter Origins of the Atom Democritus: Greek philosopher (460 BC - 370 BC) Coined the term atom from the Greek word atomos Democritus believes that atoms were indivisible
More informationUnit 3. Atoms and molecules
Unit 3. Atoms and molecules Index. s and compounds...2.. Dalton's Atomic theory...2 2.-The atom...2 3.-Atomic number and mass number...2 4.-Isotopes, atomic mass unit and atomic mass...3 5.- configuration...3
More informationBasic 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
More informationEarly 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,
More informationTeacher: 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
More informationCHAPTER 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
More informationDATE: 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,
More informationAtoms, Ions, and the Periodic Table
Atoms, Ions, and the Periodic Table 2-1 2.1 Dalton s Atomic Theory 2-2 1 2.1 Dalton s Atomic Theory The scanning tunneling microscope, STM, invented in 1981, allows us to create images of matter at the
More informationThe 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
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Ch. 2 Practice Test Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which formula/name pair is incorrect? 1) A) Fe2(SO4)3 iron(iii) sulfide
More informationATOMIC STRUCTURE. Name: Period: Date: 1) = a generalization of scientific observations that what happens (does explain)
ATOMIC STRUCTURE Name: Period: Date: I. LAW vs. THEORY: 1) = a generalization of scientific observations that what happens (does explain) 2) (model) = a set of assumptions used to explain observations
More informationName Date Class DEFINING THE ATOM
4.1 DEFINING THE ATOM Section Review Objectives Describe Democritus s ideas about atoms Explain Dalton s atomic theory Describe the size of an atom Vocabulary atom Dalton s atomic theory Part A Completion
More informationAtoms, 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
More informationAtomic Structure. For thousands of years, people had many ideas about matter Ancient Greeks believed that everything was made up of the four elements
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, they were still able to propose
More informationPhysical Science Midterm Review
Chapter 1: Science Skills, pages 2-25 1. What is science? Science is a system of knowledge and the methods you use to find that knowledge. 2. What is the relationship between science and technology? Science
More informationA1: Atomic Structure Worksheet (Goals 1 3, Chapter 4)
Unit 3 Assignment Packet Name: Period: A1: Atomic Structure Worksheet (Goals 1 3, Chapter 4) 1. Democritus, who lived in Greece during the 4 th century B.C., suggested that is made up of tiny particles
More informationIf You Cut a Piece of Graphite
Lecture Presentation Chapter 2 Atoms and Elements If You Cut a Piece of Graphite If you cut a piece of graphite from the tip of a pencil into smaller and smaller pieces, how far could you go? Could you
More informationWhere it came from and what we know now
Where it came from and what we know now History of the Atom The first mention of the atom came from Democritus in ancient Greece He suggested that the universe was made up of small, indivisible units called
More informationChapter 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
More informationChap 4 Bell -Ringers
Chap 4 Bell -Ringers The Structure of the Atom The Atom has a Structure What we ve seen so far Chapter 1 The Science of Chemistry - Chemistry is about discovering and understanding natural laws using the
More informationChapter 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
More informationTest Review # 5. Chemistry: Form TR5-8A. Average Atomic Mass. Subatomic particles.
Chemistry: Form TR5-8A REVIEW Name Date Period Test Review # 5 Subatomic particles. Type of Particle Location Mass Relative Mass Charge Proton Center 1.67 10-27 kg 1 +1 Electron Outside 9.11 10-31 kg 0-1
More informationProperties of Atoms and The Periodic Table. Ch 16, pg
Properties of Atoms and The Periodic Table Ch 16, pg. 488-506 Today s Learning Objectives Describe the 5 models of the atom. Be able to arrange the 5 models of the atom in order. Explain why the models
More informationChemistry Chapter 3. Atoms: The Building Blocks of Matter
Chemistry Chapter 3 Atoms: The Building Blocks of Matter I. From Philosophical Idea to Scientific Theory History of the Atom The Ancient Greeks were the first to come up with the idea of the atom. Democritus
More informationATOMS 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
More informationRegents review Atomic & periodic
2011-2012 1. The diagram below represents the nucleus of an atom. What are the atomic number and mass number of this atom? A) The atomic number is 9 and the mass number is 19. B) The atomic number is 9
More informationUnit 3 Atomic Structure
Name: Unit 3 Atomic Structure Scientist Year Contribution and/ or Experimental Work Democritus Aristotle Alchemists Boyle Franklin Dalton Avogadro Mendeleev Moseley 1 Scientist Year Contribution and/ or
More informationtomic tructure Chapter 3
tomic tructure Chapter 3 Early Theories of Matter 460 BC Democritus Proposed the matter was not infinitely divisible. Believed matter composed of particles called atoms. Early Theories of Matter Aristotle
More information2.1 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
More informationYour Guide for Success Chemistry Unit Name:
Your Guide for Success Chemistry Unit Name: Chemistry Outline I. Classification Of Matter A. Elements 4 1. Identifying by Properties 2. Classifying Elements B. Compounds 4 1. Composition 2. Identifying
More informationName Date Class ATOMIC STRUCTURE
4 ATOMIC STRUCTURE SECTION 4.1 DEFINING THE ATOM (pages 101 103) This section describes early atomic theories of matter and provides ways to understand the tiny size of individual atoms. Early Models of
More informationElements. Review Questions. Copyright 2017 Pearson Canada Inc.
M02_TRO6563_02_SM_C02.qxd 1/30/16 10:17 AM Page 29 2 Atoms and Elements Review Questions 2.1 Scanning tunnelling microscopy is a technique that can image, and even move, individual atoms and molecules.
More informationDemocritus & Leucippus (~400 BC) Greek philosophers: first to propose that matter is made up of particles called atomos, the Greek word for atoms
Chemistry Ms. Ye Name Date Block The Evolution of the Atomic Model Since atoms are too small to see even with a very powerful microscope, scientists rely upon indirect evidence and models to help them
More information4.2 Structure of the Nuclear Atom > Chapter 4 Atomic Structure. 4.2 Structure of the Nuclear Atom. 4.1 Defining the Atom
Chapter 4 Atomic Structure 4.1 Defining the Atom 4.2 Structure of the Nuclear Atom 4.3 Distinguishing Among Atoms 1 CHEMISTRY & YOU How did scientists determine the structures that are inside an atom?
More informationHow to Use This Presentation
How to Use This Presentation To View the presentation as a slideshow with effects select View on the menu bar and click on Slide Show. To advance through the presentation, click the right-arrow key or
More information4-1 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
More informationAtomic Structure. Chapter 3
Atomic Structure Chapter 3 Objectives IV.B.1(a) - Describe the importance of models for the study of atomic IV.B.1(b) - Describe the crucial contributions of scientists and the critical experiments that
More informationLesson 6: Periodic Table and Atomic Theory
NOTES Name: _ Date: Class: Lesson 6: Periodic Table and Atomic Theory Element: fundamental substance that ; all matter consists of ~100 elements Atom: _ that can exist; smallest unit of an element that
More informationSection 3.1 Substances Are Made of Atoms
Section 3.1 Substances Are Made of Atoms Objectives: 1. State the three laws that support the existence of atoms. 2. List the five principles of John Dalton s atomic theory. Vocabulary: law of definite
More informationPrinciples of Chemistry: A Molecular Approach, 3e (Tro) Chapter 2 Atoms and Elements
Principles of Chemistry: A Molecular Approach, 3e (Tro) Chapter 2 Atoms and Elements 1) Which of the following is an example of the law of multiple proportions? A) A sample of chlorine is found to contain
More informationYour Guide for Success Chemistry Unit Name:
Your Guide for Success Chemistry Unit Name: Chemistry Outline I. Atoms A. Structure of an Atom 4 1. Subatomic Particles 2. Different Form b. Isotope II. Periodic Table 1. Arranging 6 a. Mendeleev b. Mosely
More informationAtomic Structure and The Periodic Table. Unit 3
Atomic Structure and The Periodic Table Unit 3 Lesson 1: Atoms Unit 5: Atomic Structure & The Periodic Table Atoms How small can things get? If you break a stone wall into smaller and smaller pieces, you
More informationChapter 8 Composition of the Atom
Chapter 8 Composition of the Atom 8-1 Scientific Modelling Scientists use models to help explain things that cannot be observed. This happens all the time; consider a globe for example. Scientific models
More informationLaw of Definite Proportion** (Proust): A given compound always contains exactly the same proportion of elements by mass.
# 10 Notes Unit 2: Laws, Properties & Mols Ch. Atoms, Molecules, Ions 5 Chemical Laws: I. Law of Conservation of Mass** (Lavoisier): Mass cannot be created or destroyed. II. III. IV. Law of Definite Proportion**
More informationRhonda Alexander IC Science Robert E. Lee
Rhonda Alexander IC Science Robert E. Lee Atom The smallest particle of an element that retains all of the chemical properties of the element. The Theory & Evidence for John Dalton s Atomic Theory: Around
More information3.01 Understanding Atoms
3.01 Understanding Atoms The Events Leading to the Discovery of the Building Block of Matter Dr. Fred Omega Garces Chemistry 111 Miramar College 1 3.02 Atomic Evolution Environmental Problems in our Lifetime
More informationChapter 2 Reading Guide AP Chemistry Date: Per:
Chapter 2 Reading Guide Name: AP Chemistry 2016-2017 Date: Per: This chapter is foundational to concepts in AP Chemistry curriculum in Big Ideas 1 and 3. These two big ideas discuss the building materials
More information4. What is the law of constant composition (also known as the law of definite proportion)?
Name: Exercises #1: 1. What is the law of conservation of mass? 2. Show that the results of the following experiments illustrate the law of conservation of mass. Experiment #1: a 5.00-g sample of pure
More informationHistory of Atomic Theory
Unit 2 The Atom History of Atomic Theory A. Democritus and Aristotle Democritus named the "atom" - means indivisible Dalton (with work of Lavoisier, Proust, and Gay-Lussac) 1. atomic theory - first based
More informationTest Review # 4. Chemistry: Form TR4-9A
Chemistry: Form TR4-9A REVIEW Name Date Period Test Review # 4 Location of electrons. Electrons are in regions of the atom known as orbitals, which are found in subdivisions of the principal energy levels
More informationAtomic Structure. 1. Democritus 2. Dalton 3. Thompson 4. Millikan 5. Moseley 6. Bohr 7. Rutherford 8. Schrodinger. October 03, 2014.
October 03, 2014 Atomic Structure Chapter 4 Democritus's Atomic Philosophy 1. Democritus 2. Dalton 3. Thompson 4. Millikan 5. Moseley 6. Bohr 7. Rutherford 8. Schrodinger Aristotle -Rejected the idea of
More informationChapter 5. Early Atomic Theory and Structure
Chapter 5 Early Atomic Theory and Structure Introduction to General, Organic, and Biochemistry 10e John Wiley & Sons, Inc Morris Hein, Scott Pattison, and Susan Arena Lightning occurs when electrons move
More informationAn atom is the smallest physical particle of an element that still retains the properties of that element.
Unit 3.1 An atom is the smallest physical particle of an element that still retains the properties of that element. At sea level, one cubic centimeter of air (size of a sugar cube, or marble) will have
More informationChapter 1: 1.7, , 1.27, 1.31, 1.35, 1.39, *1.43, 1.55, 1.59, 1.65, *1.67, 1.69*
Announcements Chapter 1: 1.7, 1.8. 1.9, 1.27, 1.31, 1.35, 1.39, *1.43, 1.55, 1.59, 1.65, *1.67, 1.69* Chapter 2: 2.17, 2.19, 2.25, 2.46, 2.85, 2.89, *2.95, 2.99, 2.101, 2.103, *2.105* Chapter 3: *3.7,*
More informationCHAPTER 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
More informationName: Block Unit 3- The Atom
Name: Block Unit 3- The Atom DEMOCRITUS 1. Was Democritus a scientist? Notes 2. In what time of history did he live? 3. Describe Democritus thoughts about gold. 4. What was Democritus word for something
More informationNuclear 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,
More informationChapter 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
More informationCHAPTER 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
More informationChapter 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
More informationUnit 2. Atoms, Molecules, and Ions
Unit 2. Atoms, Molecules, and Ions Upon successful completion of this unit, the students should be able to: 2.1 State and be able to apply the Law of Conservation of Mass, Law of Definite Proportions,
More informationChapter 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
More informationChapter 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
More informationStructure 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
More informationObservations. Qualitative: descriptive observation that is not numerical. Quantitative: Numerical observation.
Mid-Term Topics Observations Qualitative: descriptive observation that is not numerical. Example: This apple is red. Quantitative: Numerical observation. Example: The temperature of this room is 23 C.
More informationLecture Presentation. Chapter 2. Atoms and Elements. Christian Madu, Ph.D. Collin College Pearson Education, Inc.
Lecture Presentation Chapter 2 Atoms and Elements Christian Madu, Ph.D. Collin College If You Cut a Piece of Graphite If you cut a piece of graphite from the tip of a pencil into smaller and smaller pieces,
More informationUnit 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
More informationAtoms, 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
More informationMatter and Energy. Chapter 3
Matter and Energy Chapter 3 Matter Anything that has mass and takes up space Two categories Pure substances Mixtures Pure Substances Matter with a fixed composition Either an element or compound Element
More informationUnit 1 review. Chapter 1, chapter , 2.4
Unit 1 review Chapter 1, chapter 2.1-2.2, 2.4 The Organization of Matter Matter Mixtures: a) Homogeneous (Solutions) b) Heterogeneous Pure Substances Elements Compounds Atoms Nucleus Protons Quarks Electrons
More informationChemistry 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:
More information2/
Chemistry 7th Edition McMurry TEST BANK Full download at: https://testbankreal.com/download/chemistry-7th-edition-mcmurry-test-bank- 2/ Chemistry 7th Edition McMurry SOLUTIONS MANUAL Full download at:
More information