Atomic Number. Mass Number. Counting Subatomic Particles
|
|
|
- Silas Palmer
- 6 years ago
- Views:
Transcription
1 Counting Subatomic Particles Now that scientists have discovered that atoms can be subdivided into subatomic particles, there was a new problem. How do we count subatomic particles? We use terms like atomic number and mass number to do so. Atomic Number Atoms are composed of identical protons, neutrons, and electrons. How are atoms of one element different from those of another element? Each element contains a particular number of protons. The atomic number of an element is the number of protons in the nucleus. # protons in an atom = # electrons (if the atom is neutral!) Mass Number The mass number of an element is the average atomic mass of an element rounded to a whole number. Element # p # e # n Mass no. Carbon 6 Nitrogen 7 14 Mass number = 195 This number is equal to the number of protons and neutrons in the nucleus. Mass number = p + + n 0 Sodium Uranium Radon 136
2 Nuclear Symbols Contain the symbol of the element, the mass number, and the atomic number. Nuclear Symbols Find each of these a) number of protons b) number of neutrons c) number of electrons d) atomic number e) mass number Nuclear Symbols Nuclear Symbols If an element has an atomic number of 34 and a mass number of 78, what is the a) number of protons b) number of neutrons c) number of electrons d) complete nuclear symbol If an element has 91 protons and 140 neutrons, what is the a) atomic number b) mass number c) number of electrons d) complete nuclear symbol
3 Isotopes Naming Isotopes Frederick Soddy Dalton was wrong about all atoms of elements of the same type being identical. Atoms of the same element can have different numbers of neutrons. Thus, different mass numbers! These atoms are called isotopes. 1912: English radiochemist Frederick Soddy proposes the idea of isotopes. 1921: Soddy wins Nobel Prize in Chemistry for this work When referencing isotopes of an element, it is important to indicate which mass number the particular isotope has. We typically name isotopes using their element name along with their mass number. Ex. carbon-12, carbon-14, hydrogen-1, hydrogen-2 Isotope Protons Neutrons Electrons Mass number Average Atomic Mass 8 10 Elements occur in nature as a mixture of isotopes The percentage of each isotope in the naturally occurring element on Earth is nearly always the same, no matter where the element is found. This percentage is taken into account when determining the average atomic mass of a particular element. The average atomic mass is the weighted average of the atomic masses of all naturally occurring isotopes of an element.
4 Calculating Average Atomic Mass To calculate the average atomic mass of an element, two pieces of information will be needed: percent abundance of each isotope and the atomic mass of each isotope. AAM = (mass1 x %A1) + (mass2 x %A2) + *Percent abundance (%A) must be in decimal form in order to conduct calculation. Calculating AAM Ex. 1 Oxygen has three naturally occurring isotopes, oxygen-16, oxygen-17, and oxygen-18. Oxygen-16 has a percent abundance of %, oxygen-17 has an abundance of 0.038%, and oxygen-18 has an abundance of 0.200%. The atomic masses of the three isotopes are amu, amu, and amu, respectively. Calculate the average atomic mass of oxygen. Calculating AAM Ex. 2 There are three naturally occurring isotopes of neon. Their percent abundances and atomic masses are: neon-20, 90.51%, amu; neon-21, 0.27%, amu; neon-22, 9.22%, amu. Calculate the weighted average atomic mass of neon. Calculating AAM Ex.3 Naturally occurring strontium consists of the following isotopes. Isotope Atomic mass, amu Percent abundance Strontium Strontium Strontium Strontium Calculate the weighted average atomic mass of strontium.
5 Calculating AAM Ex.4 The two naturally occurring isotopes of nitrogen are nitrogen-14, with an atomic mass of amu, and nitrogen-15, with an atomic mass of amu. What are the percent abundances of these isotopes? Relating Mass to Number of Atoms How can we determine the number of atoms in a particular number of grams of a substance? We can use three concepts: the mole, Avogadro s number, and molar mass. These three concepts allow us to relate atoms and mass. The Mole Avogadro s Number (il numero d Avogadro) Remember, that the mole is the SI base unit for measuring amount of substance. In particular, one mole is equal to the number of particles as there are atoms in exactly 12 grams of carbon-12. The mole is simply a counting unit like a dozen. Italian chemist Count Amedeo Avogadro devised a way to count the number of representative particles of a substance. Avogadro s number is the number of representative particles in exactly 1 mole of a pure substance. Avogadro s number = x particles
6 Molar Mass We can also define a mole in terms of the amount of substance that contains Avogadro s number of particles. The mass of one mole of a pure substance is called the molar mass of that substance. Molar mass is measured in grams/mole. Molar Conversions We can convert between particles, moles, and grams. atoms x NA moles x molar mass grams The molar mass of an element is numerically equal to the atomic mass of the element. NA molar mass
CHAPTER 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
Chapter 3. Atomic Number. Atomic Number. Section 3. Atoms of different elements have different numbers of protons.
Section 3 Atomic Number Atoms of different elements have different numbers of protons. Atoms of the same element all have the same number of protons. The atomic number (Z) of an element is the number of
[3.2] The Atom. p in Textbook
![[3.2] The Atom. p in Textbook](/thumbs/83/88700013.jpg "[3.2] The Atom. p in Textbook")
[3.2] The Atom p. 145 149 in Textbook We will be learning about three different parts of the atom today 1. What makes up an atom 2. Where an atom s mass is found 3. What are isotopes What does the atom
VIII. Progression of the atomic model Democritus/Dalton --> Thomson --> Rutherford --> Bohr --> Quantum Mechanical
HISTORY OF ATOMIC THEORY NOTES I. Ancient Greeks A. Aristotle ~ believed there were 4 elements: B. Democritus ~ believed in the "particle theory": ~ named the small particles "atoms" which means II. Dalton
Atomic Structure. Atomic Notation. Atomic Notation. Atomic Notation. Section 3.3 Distinguishing Between Atoms. Atomic Notation
Atomic Structure Section 3.3 Distinguishing Between Atoms OBJECTIVES: Explain how the atomic number identifies an element. Use the atomic number and mass number of an element to find the numbers of protons,
Chapter 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
All atoms of an element must have the same number of protons but not neutrons.
Counting Atoms Key Terms atomic number nuclide mole isotope unified atomic mass unit Avogadro s number mass number average atomic mass molar mass Consider neon, Ne, the gas used in many illuminated signs.
Chapter 4 What are Atoms?
Chapter 4 What are Atoms? For over two thousand years, learned people wondered what matter was made of. In the 1800s, scientists found evidence that all matter was comprised of atoms. Now in the twenty-first
Smoking 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
Chapter 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
Joke of the Day. Progress of the Atom. Discovering the Atom X X. CH 4- Atoms 1. Democritus Dalton Thomson. Rutherford X X Bohr X X X.
Joke of the Day Discovering the Atom Progress of the Atom In this lesson we will take a look at the scientists who explored the wonders of the atom. QuickTime and a decompressor are needed to see this
How 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
Unit 4: The Atom, Atomic Number, Mass Number, And Isotopes
#5 PPT APE MAN AND ISOTOPES! Unit 4: The Atom, Atomic Number, Mass Number, And Isotopes LecturePLUS Timberlake 1 Atomic Theory Atoms are building blocks of elements Similar atoms in each element Different
An 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
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.
Unit 6 Chemical Analysis. Chapter 8
Unit 6 Chemical Analysis Chapter 8 Objectives 39 Perform calculations using the mole to calculate the molar mass 40 Perform calculations using the mole to convert between grams, number of particles, volume,
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
Average Atomic Mass. A new unit called the atomic mass unit (amu) was developed to deal with the very small units of mass for particles like the atom.
Average Atomic Mass Since atoms are so small and the mass of individual atoms is also very small, it is not useful to use the units of grams or kilogram. A new unit called the atomic mass unit (amu) was
6 atomic # C symbol Carbon name of element atomic mass. o Examples: # 1 mol C = g # 1 mol O = g # 1 mol H = 1.
7.1 AVOGADRO S NUMBER AND MOLAR CONVERSIONS CHEMISTRY NOTES Identify the mole as the unit used to count particles, whether atoms, ions, or molecules. Use Avogadro s number to convert between amount in
Atoms and their structure
Atoms and their structure History of atomic theory Not the history of atom, but the idea of the atom Original idea Ancient Greece (400 B.C..) Democritus and Leucippus Greek philosophers Another Greek Aristotle
Unit 6: Chemical Quantities. Understanding The Mole
Unit 6: Chemical Quantities Understanding The Mole 1 How do We Typically Measure Matter? You can measure mass, or volume, or you can count pieces. We measure mass in grams. We measure volume in liters.
Atoms and Their Isotopes
Atoms and Their Isotopes Why? Atoms and isotopes are identified by the number of protons, neutrons, and electrons that they contain. Before you can understand the properties of atoms, how atoms combine
Lesson 12: Atoms and Subatomic Particles
NOTES Name: Date: Class: Lesson 12: Atoms and Subatomic Particles Element: fundamental substance that ; all matter consists of ~100 elements Atom: that can exist; smallest unit of an element that can enter
CHEM 121 Introduction to Fundamental Chemistry. Summer Quarter 2008 SCCC. Lecture 2
CHEM 121 Introduction to Fundamental Chemistry Summer Quarter 2008 SCCC Lecture 2 Could Stephanie, Liqingqing, Huong, Sophia and Yumiko see me after class for a few minutes. Thanks. Matter, Measurements
CHAPTER 4: THE ATOM PHYSICAL SCIENCE
CHAPTER 4: THE ATOM PHYSICAL SCIENCE By C. Goodman, Doral Academy Preparatory High School, 2011-2013 Based on a PowerPoint presentation by Mrs. S. Temple, Doral Academy Preparatory High School Essential
CHAPTER 3 THE ATOM. 1. Matter is composed extremely small particles called atoms
CHAPTER 3 THE ATOM Read pgs. 107-110 I. History Democritus Greek philosopher, 400 B.C., said all matter is made up of small, indivisible particles he called atoms (Greek for indivisible ). He wasn t believed
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,
How can there be different varieties of atoms?
Chapter 4 Atomic Structure 4.1 Defining the Atom 4.2 Structure of the Nuclear Atom 4.3 Distinguishing Among Atoms 1 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. CHEMISTRY
Chapter 4: Atoms and Elements
Chapter 4: Atoms and Elements Determine atomic numbers, mass numbers, and isotope symbols for an isotope. Determine number of protons and neutrons from isotope symbols. Calculate atomic mass from percent
Drake Chemistry Isotopic Pennies Name: Atomic Structure Unit Isotopic Pennies
Introduction At the beginning of the 19 th century, John Dalton proposed a new atomic theory all atoms of the same element are identical to one another and equal in mass. It was a simple yet revolutionary
Name 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
ATOMIC 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
1. Explain the law of conservation of mass in your own words. Matter is neither created nor destroyed in a chemical reaction.
Chapter 3 Exam Review KEY I. Atomic Theory 1. Explain the law of conservation of mass in your own words. Matter is neither created nor destroyed in a chemical reaction. 2. What were Rutherford s two main
Atoms, Molecules, and the Mole
The Mole Now that we know how to write and name chemical compounds, we need to understand how chemists use these formulas quantitatively. As chemists, we need to know how many atoms or molecules are reacting
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
Atoms Section 2 Section 2: The Structure of Atoms
Section 2: The Structure of Atoms Preview Key Ideas Bellringer What Is in an Atom? Atomic Number and Mass Number Isotopes Atomic Masses Math Skills Key Ideas What is the difference between protons, neutrons,
CP/Honors Chemistry Unit 3: Atomic Theory Chapter 4, Sections 1, 2, and 3
CP/Honors Chemistry Unit 3: Atomic Theory Chapter 4, Sections 1, 2, and 3 Subatomic Particles Warm-Up Quiz 1. What are the three subatomic particles? 2. Where are the particles located in the atom? 3.
Topics in composition stoichiometry include the calculation of: Molar mass Percent Composition Molecular formula Empirical formulas
Composition Stoichiometry Composition Stoichiometry NOTES 1 So far, we ve studied the products of a chemical reaction in terms of their identity. Stoichiometry is a branch of chemistry dealing with quantities.
Title: Chem Review 2 TOPIC: DISCOVERY OF ATOM
Title: Chem Review 2 TOPIC: DISCOVERY OF ATOM EQ: How were the 3 subatomic particles discovered? Title and Highlight Topic: EQ: Date Reflect Question: Reflect on the material by asking a question (its
Chem Chapter 2.notebook October 17, 2012
Unit 1: Stoichiometry 1 Chapter 2: The Mole Atomic number the number of protons in an atom or ion Mass number the sum of the protons and neutrons in an atom 2 Isotope atoms which have the same number of
Early 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
Unit III: Quantitative Composition of Compounds
Unit III: Quantitative Composition of Compounds A. Atoms and Isotopes B. Atomic Composition of Chemical Compounds C. Formula and Molecular Mass D. Calculations using Moles of Atoms E. Calculations using
Chapter 2: Atoms and Molecules
SYMBOLS AND FORMULAS A unique symbol is used to represent each element. Formulas are used to represent compounds. Chapter 2: Atoms and Molecules ELEMENTAL SYMBOLS A symbol is assigned to each element.
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
Average Atomic Mass: How are the masses on the periodic table determined?
Chemistry Ms. Ye Name Date Block Average Atomic Mass: How are the masses on the periodic table determined? Most elements have more than one naturally occurring isotope. As you learned previously, the atoms
Vocabulary Review. Atom Cathode Ray Electrons Protons Neutrons Nucleus
2/19/16 Do Now On your half sheet of paper, identify the scientist that either discovered a part of the atom or developed a theory related to atomic structure. Vocabulary Review Atom Cathode Ray Electrons
9.1.1 CHEMICAL EQUATIONS AND STOICHIOMETRY
9.1.1 CHEMICAL EQUATIONS AND STOICHIOMETRY Work directly from Zumdahl (Chapter 3). Work through exercises as required, then summarise the essentials of the section when complete. A chemical equation is
Mass Relationships of Atoms
Mass Relationships of Atoms The Mole - the fundamental SI measure of amount of substance - the amount of substance that contains as many elementary entities as there are atoms in exactly 12 g of carbon-12
Chapter 3. Mass Relationships in Chemical Reactions
Chapter 3 Mass Relationships in Chemical Reactions In this chapter, Chemical structure and formulas in studying the mass relationships of atoms and molecules. To explain the composition of compounds and
2.1. SYMBOLS AND FORMULAS A unique symbol is used to represent each element. Formulas are used to represent compounds.
2.1. SYMBOLS AND FORMULAS A unique symbol is used to represent each element. Formulas are used to represent compounds. Symbols of Elements Atoms and Molecules ELEMENTAL SYMBOLS A symbol is assigned to
Atomic 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
THE MOLE (a counting unit)
MOLE AND MATH THE MOLE (a counting unit) A mole represents a set or group, much in the same way that a dozen represents a set of twelve. 1 dozen eggs = 12 eggs; 1 mole eggs = 6.022 x 10 23 eggs 1 dozen
Chapter 10 Chemical Quantities
Chapter 10 Chemical Quantities 10.1 The Mole: A Measurement of Matter OBJECTIVES: Describe methods of measuring the amount of something. Define Avogadro s number as it relates to a mole of a substance.
Unit 3: Atoms and Periodic Table Retake Review Packet
Name Date Block Unit 3: Atoms and Periodic Table Retake Review Packet Completing each section of the retake review packet will fulfill one of the requirements for retaking the unit 3 test. Section 1: Vocabulary
1. The mass number of the atom is the total number of &. 2. What are the three particles in an atom and what is each of their charges?
WEDNESDAY, OCT. 15 1. The mass number of the atom is the total number of &. 2. What are the three particles in an atom and what is each of their charges? 3. The symbol for elements is commonly written
Chapter 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
atomic structure practice test D) neutrons and protons B) empty space and has a small, positively charged nucleus C) neutron
atomic structure practice test 1. The major portion of an atom's mass consists of A) electrons and protons B) electrons and neutrons C) neutrons and positrons D) neutrons and protons 2. Which subatomic
Chapter 3 Mass Relationships in Chemical Reactions
Chapter 3 Mass Relationships in Chemical Reactions Semester 1/2012 3.1 Atomic Mass 3.2 Avogadro s Number and the Molar Mass of an element 3.3 Molecular Mass 3.5 Percent Composition of Compounds 3.6 Experimental
Chemistry 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
What is a Representative Particle
Chapter 7 Moles What is a Representative Particle The smallest unit into which a substance can be broken down without changing the composition of the substance. Atoms, molecules, and formula units What
History, Atomic Theory, and Atoms Review Packet HW: Due Wednesday, November 22 nd
History, Atomic Theory, and Atoms Review Packet HW: Due Wednesday, November 22 nd Name Date Period Atomic Theory Fill in the missing information in the chart below: Name of Researcher Equipment/ Experiment
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
Chapter 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
UNIT 2 - ATOMIC THEORY
UNIT 2 - ATOMIC THEORY VOCABULARY: Allotrope Electron Configuration Nuclear Charge Anion Element Nucleons Atom Excited state Nucleus Atomic Mass Ground state Orbital Atomic Mass unit (a.m.u.) Ion Proton
Unit 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%
Elements. Chem101 - Lecture 2. Elements. Elements. Elements. Elements. Atoms and Molecules
Chem101 - Lecture 2 Atoms and Molecules Elements Elements are pure substances containing only one kind of atom (homoatomic). There are at last count 114 elements. (Your book indicates 112.). - 88 of these
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
Introduction to the Mole. Advanced Chemistry Ms. Grobsky
Introduction to the Mole Advanced Chemistry Ms. Grobsky Daily Objective To understand the concept of average atomic mass To understand the mole concept and Avogadro s number Counting Units of Measurement
ب 3 18 قسم الكيمياء مصطفي عيد
memxtd@yahoo.com m.moustapha@sau.edu.sa 0115888078 ب 3 18 قسم الكيمياء مصطفي عيد The Atom Nucleus Electron Shell or Orbit The Atom. What are the 3 major parts of an atom? Proton Neutron Electron Stoichiometry
Drill What do you know? 1. Write your definition of an ATOM. 2. What is inside an atom? 3. What determines the identity of an atom?
Drill What do you know? 1. Write your definition of an ATOM. 2. What is inside an atom? 3. What determines the identity of an atom? Drill 10/6 1. What is inside an atom? 2. What determines the identity
Chemistry Chapter 3. Stoichiometry. (three sections for this chapter)
Chemistry Chapter 3 Stoichiometry (three sections for this chapter) Chemistry Chapter 3 Stoichiometry Section 1 3.1-3.4 Average Atomic Mass The Mole Molar Mass Average Atomic Mass Average mass of objects
Unit 5. Chemical Composition
Unit 5 Chemical Composition Counting by Mass Individually mass a few Calculate the average mass of one Can count large numbers of by mass Atomic Mass Unit (amu) 1 amu = 1.66 x 10-24 g Subatomic particles
Early Atomic Theory and Structure
Early Atomic Theory and Structure Chapter 5 Hein and Arena Version 1.1 Eugene Passer Chemistry Department Bronx Community 1 College John Wiley and Sons, Inc The Atom and its Subatomic Particles The atom
Chemistry for Today General Organic and Biochemistry 9th Edition Seager
Chemistry for Today General Organic and Biochemistry 9th Edition Seager TEST BANK Full download at: https://testbankreal.com/download/chemistry-today-general-organic-biochemistry-9thedition-seager-test-bank/
UNIT 2 - ATOMIC THEORY
UNIT 2 - ATOMIC THEORY VOCABULARY: Allotrope Electron Configuration Nuclear Charge Anion Element Nucleons Atom Excited state Nucleus Atomic Mass Ground state Orbital Atomic Mass unit (a.m.u.) Ion Proton
UNIT 2 - ATOMIC THEORY
UNIT 2 - ATOMIC THEORY VOCABULARY: Allotrope Anion Atom Atomic Mass Atomic Mass unit (a.m.u.) Atomic number Bohr model Cation Compound Electron Electron Configuration Element Excited state Ground state
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
Chem101 - Lecture 2. Atoms and Molecules
Chem101 - Lecture 2 Atoms and Molecules Elements Elements are pure substances containing only one kind of atom (homoatomic). There are at last count 114 elements. - 88 of them are naturally occurring.
Unit III: Quantitative Composition of Compounds
Unit III: Quantitative Composition of Compounds A. Atoms and Isotopes B. Atomic Composition of Chemical Compounds C. Formula and Molecular Mass D. Calculations using Moles of Atoms E. Calculations using
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
Elements, Atoms, and Ions
Elements, Atoms, and Ions Chemistry I: Chapter 2b Chemistry I Honors: Chapter 3 ICP: Chapter 17 SAVE PAPER AND INK!!! When you print out the notes on PowerPoint, print "Handouts" instead of "Slides" in
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
Atoms, Isotopes, and Ions
WHY? ACTIVITY 02-1 Atoms, Isotopes, and Ions Atoms are the fundamental building blocks of all substances. To begin to understand the properties of atoms and how they combine to form molecules, you must
tomic 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
CP/Honors Chemistry Unit 3: Atomic Theory Sections 4.1, 4.2, 4.3
CP/Honors Chemistry Unit 3: Atomic Theory Sections 4.1, 4.2, 4.3 Subatomic Particles Warm-Up Quiz 1. What are the three subatomic particles? 2. Where are the particles located in the atom? 3. What are
Unit 4: The MOLE & STOICHIOMETRY. Essential Question: What is a MOLE and why do we use it to measure chemical things PRECISELY?
Unit 4: The MOLE & STOICHIOMETRY Essential Question: What is a MOLE and why do we use it to measure chemical things PRECISELY? What makes a figure SIGNIFICANT? n Non-Zero DIGITS n 1.589 n 0.897 n 3600
SUMMARY (p. 44) The atom is % empty space and is composed of three particles. a. b. c.
2.1 Atomic Structure and Subatomic Particles (p. 40) There are two types of charge. 1. _ 2. Electrons In 1897 J. J. Thomson, using a cathode ray tube, measured the ratio of the charge-to-mass of the electron:
Chemistry 101 Chapter 8 Chemical Composition
Chemistry 101 Chapter 8 Chemical Composition Atomic mass unit (amu): a unit of the scale relative masses of atoms (1 amu = 1.66 10-24 g). Atomic weight (Atomic mass): the atomic weight of an element given
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
General Chemistry. Chapter 3. Mass Relationships in Chemical Reactions CHEM 101 (3+1+0) Dr. Mohamed El-Newehy 10/12/2017
General Chemistry CHEM 101 (3+1+0) Dr. Mohamed El-Newehy http://fac.ksu.edu.sa/melnewehy Chapter 3 Mass Relationships in Chemical Reactions 1 In this chapter, Chemical structure and formulas in studying
Isotopes are different forms of the that have a. Isotopes of the same element have the but. Ions are atoms that have a. In an ion, the.
Chemistry Ms. Ye Name Date Block Atomic Structure: 1. What is important about the atomic number? 2. How do you figure out the number of a. Protons in an atom? b. Electrons in an atom? c. Neutrons in an
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
Molar Mass. The total of the atomic masses of all the atoms in a molecule:
Molar Mass The total of the atomic masses of all the atoms in a molecule: Ex: H 2 O H (1.0079) x 2 atoms = 2.0158 grams O (15.999) x 1 atom = 15.999 grams 18.0148 grams (18.0 grams) Ex: Cu(NO 3 ) 2 Cu
Atomic Structure. How do you discover and study something you can t see?
Atomic Structure How do you discover and study something you can t see? WHAT IS A THEORY? A hypothesis is a proposed explanation made as a starting point for further investigation (It s bright outside
Name Period Date Engage-Atoms 1. What does Bill cut in half?
Name Period Date Engage-Atoms https://www.youtube.com/watch?v=fmuskig2exi 1. What does Bill cut in half? 2. By cutting this item in half he tries to prove that there are pieces that are uncut- table called
B. stoichiometry using balanced chemical equations to obtain info. C. mole-to-r.p. and r.p.-to-mole example problems:
Chem. Ch. 10 ~ THE MOLE NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 10.1 Notes I. Measuring Matter A. SI unit of chemical quantity = the mole (abbreviated
Molar Calculations - Lecture Notes for Chapter 6. Lecture Notes Chapter Introduction
Page 1 of 9 Page 2 of 9 Lecture Notes Chapter 6 1. Introduction a. The above equation describes the synthesis of water from hydrogen and oxygen. b. It is not balanced, however. c. Notice how the number
Collegiate Institute for Math and Science Day 57: December 9, 2016 Room 427
Unit 2: Atomic Concepts Outline Name: Period: Date: 1. The modern model of the atom has evolved over a long period of time through the work of many scientists. Dalton s Model: Elements are made of atoms
Q1. The electronic structure of the atoms of five elements are shown in the figure below.
Q1. The electronic structure of the atoms of five elements are shown in the figure below. The letters are not the symbols of the elements. Choose the element to answer the question. Each element can be
Chemistry Day 10. Monday, September 17 th Tuesday, September 18 th, 2018
Chemistry Day 10 Monday, September 17 th Tuesday, September 18 th, 2018 Do-Now Title: Brainstorm: Unit 1 1. Write down today s FLT 2. Draw what an atom looks like according to Democritus and Dalton 3.