Work hard. Be nice. Name: Period: Date: UNIT 2: Atomic Concepts Lesson 9: Calculating Average Atomic Mass
|
|
|
- Marilyn Foster
- 6 years ago
- Views:
Transcription
1 Name: Period: Date: KIPP NYC College Prep General Chemistry UNIT 2: Atomic Concepts Lesson 9: Calculating Average Atomic Mass By the end of today, you will have an answer to: How do we determine the average atomic mass of element from multiple isotopes? DO NOW: Fill out the data table using your knowledge of carbon Protons Neutrons Electrons Mass Number C What is the atomic mass number of carbon found on the periodic table? 2. Which isotope of carbon do you predict would be the most common isotope of carbon? Explain your thinking. Hint: which isotopes mass is most similar to the mass we see on the periodic table? ELEMENT vs. ATOM vs. ISOTOPE 20 Ne Ne Ne 20 Ne Ne Ne 21 Ne With a partner, answer the following questions: 1. What element is represented by the particle diagram? 2. How many atoms of the element are there? 3. How many isotopes of the element are there? 4. Fill in the following chart: Isotope Mass Number % Abundance (What percent of all the atoms represented are of this particular isotope?) 22 Ne 20 Ne 22 Ne CHECK FOR UNDERSTANDING What are the differences between an element, atom, and isotope? What are the similarities? 5. Is it possible to answer the question, What is the mass of one neon atom? Why or why not?
2 PROCESS, THINK AND WRITE: Are all atoms of the same element identical to each other? Why or why not? Catalyzing Thoughts: Below are the two naturally occurring isotopes of boron. Three key numbers are highlighted. 1) Mass number of isotope (rounded) 2) Mass number of isotope (actual) Which whole number do you predict would be closest to the atomic mass for Boron found on the periodic table and WHY? The actual atomic mass number for Boron on the periodic table is: This number is considered the average atomic mass. It is the weighted average of all of the different Boron isotopes. KEY VOCABULARY: 3) Percent Natural Abundance of that isotope ATOMIC MASS MASS NUMBER PROCESS, THINK AND WRITE: What is the difference between average atomic mass of an element and the mass number? APPLY: The atomic mass of an element is the weighted average of the (1) number of protons in the isotopes of that element (2) number of neutrons in the isotopes of that element (3) atomic masses of some of the naturally occurring isotopes of that element (4) atomic masses of all of the naturally occurring isotopes of that element
3 How to calculate average atomic mass: Work hard. Be nice. AVERAGE ATOMIC MASS = (mass of A)( % abundance of A in ratio form) + (mass of B)(% abundance of B in ratio form) +.. EXAMPLE 1: QUESTION Calculate the average atomic mass of boron. HOW TO SOLVE IT! EXAMPLE 2: Calculate the atomic mass of copper. Predict whether you think the answer will be closer to 63 or 65: Now solve: Atomic Mass = g/ mol
4 Name: Pd: Date: KIPP NYC College Prep General Chemistry 2.9 HW PART I: Complete Lab #8 Candium Lab! PART II: Be sure that all vocabulary words are in glossary sheets. The list of all words is on our website: PART III: Study all vocabulary by covering the words or definitions and quizzing yourself PART IV: Multiple choice practice 1. The gold-foil experiment led scientists to conclude that an atom s (1) Positive charge is evenly spread throughout its volume (2) Negative charge is mainly concentrated in its nucleus (3) Mass is evenly spread throughout its volume (4) Volume is mainly empty space 2. In Rutherford s gold foil experiments, some alpha particles were deflected from their original paths but most passed with no deflection. Which statement about gold atoms is supported by these experimental observations? (1) Gold atoms consist mostly of empty space. (2) Gold atoms are similar to alpha particles. (3) Alpha particles and gold nuclei have opposite charges (4) Alpha particles are more dense than gold atoms. 3. The gold foil experiment led to the conclusion that each atom in the foil was composed mostly of empty space because most alpha particles directed at the foil (1) Passed through the foil (2) Remained trapped in the foil (3) Were deflected by the nuclei in gold atoms (4) Were deflected by the electrons in gold atoms 4. Which statement correctly describes the charge of the nucleus and the charge of the electron cloud of an atom? (1) The nucleus is positive and the electron cloud is positive. (2) The nucleus is positive and the electron cloud is negative. (3) The nucleus is negative and the electron cloud is positive. (4) The nucleus is negative and the electron cloud is negative. 5. Which subatomic particle has a negative charge? (1) Proton (2) Neutron (3) Electron (4) Positron 6. Which two particles each have a mass approximately equal to one atomic mass unit. (1) electron and neutron (2) electron and positron (3) proton and electron (4) proton and neutron 7. What is the charge of the nucleus of a nitrogen atom? (1) -7 (2) 0 (3) +7 (4) The nucleus of an atom of K-42 contains (1) 19 protons and 23 neutrons (2) 19 protons and 42 neutrons (3) 20 protons and 19 neutrons (4) 23 protons and 19 neutrons
5 Name: Pd: Date: KIPP NYC College Prep General Chemistry WORK 2.7-Average Atomic Mass 10 points Summary Questions: A Nitrogen atom with 7 protons and 8 neutrons has a mass number of 15 amu. However, on the periodic table, the atomic mass for Nitrogen is Explain how this is possible. In your own words, explain the difference between Mass Number and Average Atomic Mass. Regents-Style Questions 1. The atomic mass of an element is calculated using the (1) atomic number and the ratios of its naturally occurring isotopes (2) atomic number and the half-lives of each of its isotopes (3) masses and the ratios of its naturally occurring isotopes (4) masses and the half-lives of each of its isotopes 2. Hydrogen has three isotopes with mass numbers of 1, 2, and 3 and has an average atomic mass of amu. This information indicates that (1) equal numbers of each isotope are present (2) more isotopes have an atomic mass of 2 or 3 than of 1 (3) more isotopes have an atomic mass of 1 than of 2 or 3 (4) isotopes have only an atomic mass of 1 3. What whole number do you predict the atomic mass of sulfur to be closest to? 4. Show the numerical setup for calculating the average atomic mass of sulfur. 5. State, in terms of subatomic particles, one similarity and one difference between these isotopes of sulfur:
6 6. The table below shows the number of subatomic particles in atom X and in atom Z. Atom X and atom Z are isotopes of the element (1) aluminum (3) magnesium (2) carbon (4) nitrogen 7. The table below shows the various isotopes of Chlorine Mass Number % % Natural Abundance Determine the atomic mass of Chlorine: How many protons are found in Chlorine? How many electrons are found in Chlorine? Explain why the atomic mass number is closer to 35 than to Using the information below, calculate the average atomic mass of nitrogen. Mass Number % % Natural Abundance 6
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
Name: Date: Atomic Structure 2017 Mrs. Mannion Version 1
Name: Atomic Structure 2017 1. The mass of a proton is approximately equal to the mass of A) a beta particle B) an electron C) an alpha particle D) a neutron 2. What are the characteristics of a neutron?
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
Which order of statements represents the historical development of the atomic model? A) C D A B B) C D B A C) D B A C D) D B C A
1. The mass of a proton is approximately equal to the mass of A) an electron B) a neutron C) an alpha particle D) a beta particle 2. What is the number of electrons in an atom that has 20 protons and 17
4. The mass of a proton is approximately equal to the mass of A an alpha particle C a positron. B a beta particle D a neutron
1. Which particles have approximately the same mass? A an electron and an alpha particle B an electron and a proton C a neutron and an alpha particle D a neutron and a proton 2. Which phrase describes
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
Work hard. Be nice. Name: Period: Date: UNIT 2: Atomic Concepts Lesson 3: Some go through and some don t
Name: Period: Date: UNIT 2: Atomic Concepts Lesson 3: Some go through and some don t Do Now: By the end of today, you will have an answer to: How did the gold foil experiment lead to the modern model of
CH4 HOMEWORK : ATOMIC STRUCTURE
Name Date Class 4 CH4 HOMEWORK : 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
Unit 3 Atomics Repair Problems
1. What is the charge of the nucleus in an atom of oxygen-17? A) 0 B) 2 C) +8 D) +17 2. A neutral atom contains 12 neutrons and 11 electrons. The number of protons in this atom is A) 1 B) 11 C) 12 D) 23
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
2015 Name: Test 1 Atomic Structure
2015 Name: Test 1 Atomic Structure 1. During a flame test, a lithium salt produces a characteristic red flame. This red color is produced when electrons in excited lithium atoms A) return to lower energy
Atomic Structure Practice Questions
Atomic Structure Practice Questions 1. Experiments performed to reveal the structure of atoms led scientists to conclude that an atom s (1) positive charge is evenly distributed throughout its volume (2)
Date: Hybrid Chemistry Regents Prep Ms. Hart/Mr. Kuhnau. Unit 1: All About Atoms Lesson 1.1: Parts of an atom
Unit 1: All About Atoms Lesson 1.1: Parts of an atom Do Now: By the end of today, you will have an answer to: How do we determine the number of subatomic particles in an atom? 1. A neutron has a charge
Multiple Choice Do Now!
Name: Period: Date: KIPP NYC College Prep General Chemistry Quarter 1: Let s Review Multiple Choice Do Now! 1. Which substance can be decomposed by chemical means? (1) Aluminum (2) Octane (3) Silicon (4)
Democritus & 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
Name 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
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
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,
14: BEHOLD THE POWER OF THE NUCLEUS!!!
Name: Period: Date: UNIT 14: Nuclear Chemistry Lesson 1: Let s go nuclear! By the end of today, you will have an answer to: What does it mean to be radioactive? Do Now: Final problems related to electrochemistry
Unit 3: The Atom Part 1. DUE: Friday October 13, 2017
Unit 3: The Atom Part 1 The following pages are practice questions for this unit, and will be submitted for homework! You must complete: What is in an atom? ALL QUESTIONS Calculating the Number of Protons,
Practice Packet Unit 4: Atomic Structure
Name: Regents Chemistry Practice Packet Unit 4: Atomic Structure Assess Yourself: Vocab: Lesson 1: Lesson 2: Lesson 3: Lesson 4: Lesson 5: Lesson 6: Lesson 7: 1 Vocabulary: Check your understanding. Describe
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
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
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
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
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 3. The Atom & Modern Atomic Theory
Unit 3 The Atom & Modern Atomic Theory Theories of the Atom Early Models & Thoughts: Democritus Matter is made up of tiny particles called atoms. Smallest unit that retains the identity of the element
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.
Constructing Models of Atoms
Chapter 4 Atomic Structure Investigation 4A Constructing Models of Atoms Background Information With an electron microscope, scientists can observe the arrangement of atoms on the surface of a material.
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,
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
Section Review. Development of the Atomic Theory USING VOCABULARY UNDERSTANDING CONCEPTS. Skills Worksheet
Skills Worksheet Section Review Development of the Atomic Theory USING VOCABULARY 1. In your own words, write a definition for the term atom. Correct each statement by replacing the underlined term. 2.
CHEMISTRY LAB #7 Average Atomic Mass of Candium 90 MINUTES
CHEMISTRY LAB #7 Average Atomic Mass of Candium 90 MINUTES PURPOSE: To simulate the process of calculating average atomic mass using a mythical element, candium and its three different isotopes. INTRODUCTION:
Name: Date: Pd: Unit 2: Atomic Structure: Isotopes Guided Notes. Positively charged (+1). Found in the nucleus.
_ Atoms: The Building Blocks of everything? Unit 2: Atomic Structure: Isotopes Guided Notes An atom consists of a An atom is the smallest unit of an element that is possible. All the matter around us is
Name Period. CRHS Academic Chemistry Unit 3 - Atomic Structure & Nuclear Chemistry. Homework. Due Date Assignment On-Time (100) Late (70)
Name Period CRHS Academic Chemistry Unit 3 - Atomic Structure & Nuclear Chemistry Homework Due Date Assignment On-Time (100) Late (70) 3.1 3.2 3.3 3.4 Warm-Ups EC Notes, Homework, Exam Reviews and Their
IB Chemistry : Atomic Structure & History with Boardworks Enabled Interactives
Atomic Structure Contents INTRODUCING ATOMS SUB ATOMIC PARTICLES HISTORY ATOMIC # & MASS # AVERAGE ATOMIC MASS MASS SPECTROMETER ELECTRON CONFIGURATION ISOTOPES SUMMARY ACTIVITIES ELEMENTS DIFFERENT TYPES
Chapter 2 Atoms and Elements. 2.4 The Atom
Chapter 2 Atoms and Elements 2.4 The Atom Atoms Dalton s Atomic Theory Are tiny particles of matter. Of an element are similar and different from other elements. Of two or more different elements combine
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
The structure of the Atom. Chemistry chapter 4
The structure of the Atom Chemistry chapter 4 Rutherford-Bohr Model Niels Bohr (1922) Proposed improvements to Rutherford Atomic Model. For this reason the planetary model of the atoms is sometimes called
CHEMISTRY 11 UNIT REVIEW: ATOMIC THEORY & PERIODIC TRENDS
CHEMISTRY 11 UNIT REVIEW: ATOMIC THEORY & PERIODIC TRENDS Atoms Atoms have protons and neutrons located in the nucleus of the atom. Electrons orbit around the nucleus in well-defined paths. Protons have
Practice Packet Level 3: Atomics
Name: Regents Chemistry: Mr. Palermo Practice Packet Level 3: Atomics Name: Unit Vocabulary: For each word, provide a short but specific definition from YOUR OWN BRAIN! No boring textbook definitions.
TEST REVIEW GCAA Chemistry Atoms. A. Excited B. Energy C. Orbital D. Plum Pudding Model
TEST REVIEW GCAA Chemistry Atoms From the Hangman Game-----Match the answers correctly! A. Excited B. Energy C. Orbital D. Plum Pudding Model E. Bohr F. Electron G. Frequency H. Neutron I. Thomson J. alpha
Democritus & 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
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
Atomic Structure. 1. Write one electron configuration for an atom of silicon in an excited state.
tomic Structure Name: ate: 1. Write one electron configuration for an atom of silicon in an excited state. 5. Which electron configuration represents an atom of chlorine in an excited state?. 2 8 7. 2
Atomic Concepts and Nuclear Chemistry Regents Review
1. In the late 1800s, experiments using cathode ray tubes led to the discovery of the 10.Compared to an atom of phosphorus-31, an atom of sulfur-32 contains A) electron B) neutron C) positron D) proton
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
protons electrons neutrons nucleus Center of the atom; contains protons and neutrons. The Atom Molecules are made up of two or more atoms.
_ Period: The Atom Ch. 18:1 Everything is made of atoms. Atoms are the smallest part of matter. Atoms are made up of 3 subatomic particles (particles smaller than the atom): electrons, protons, and neutrons.
Honors Chemistry Unit 2: The Atom & Its Nucleus
Honors Chemistry Unit 2: The Atom & Its Nucleus (2017-2018) Bunsen, I must tell you how excellent your study of chemical spectroscopy is, as is your pioneer work in photochemistry but what really impresses
Atomic Structure Chapter 5 Assignment & Problem Set
Atomic Structure Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Atomic Structure 2 Study Guide: Things You Must Know Vocabulary (know the definition
Unit 7 Study Guide: Name: KEY Atomic Concepts & Periodic Table
Unit 7 Study Guide: Name: KEY Atomic Concepts & Periodic Table Focus Questions for the unit... How has the modern view of the atom changed over time? How does a chemist use symbols and notation to communicate
Atomic Structure Early Theories Democritus: 4 B.C.: atom Dalton: atoms cannot Thomson: Cathode Ray Tubes Rutherford:
Atomic Structure n a well-substantiated explanation of some aspect of the natural world; n an organized system of accepted knowledge that applies in a variety of circumstances to explain a specific set
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
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 2. Atomic Structure
Atomic Structure Chapter 2 What particles compose the substances around us? When you use the term particle to explain the different properties of a solid, liquid or gas, you are referring to the simplest,
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
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
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
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
1 Development of the Atomic Theory
CHAPTER 4 1 Development of the Atomic Theory SECTION Introduction to Atoms BEFORE YOU READ After you read this section, you should be able to answer these questions: What is the atomic theory? How has
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
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%
Atomic Structure Chapter 4 Mr. Hines
Atomic Structure Chapter 4 Mr. Hines Part A Standard model of the atom Learning Targets and I can statements 1 List, label, and describe the parts of an atom. 2 Identify the atomic number and the atomic
Isotopes and Radioactive Decay
NAME PERIOD DATE CHAPTER 4 NOTES: ISOTOPES Isotopes and Radioactive Decay ISOTOPES: Atoms that contain the same number of protons but a different number of neutrons. Isotopes containing more neutrons have
A. Cu 2+ B. Fe 2+ C. Ca 2+ D. Hg Which atom in the ground state has three halffilled orbitals?
Unit 3 - Electrons, Light, and Ions 15-16 Name: ate: 1. Which is the electron configuration of a neutral atom in the ground state with a total of six valence electrons?. 1s 2 2s 2 2p 2. 1s 2 2s 2 2p 4.
Work hard. Be nice. Name: Period: Date: UNIT 3: Electrons Lesson 4: The Octet Rule. Nitrogen Neon Carbon He
Name: Period: Date: UNIT 3: Electrons Lesson 4: The Octet Rule Do Now: By the end of today, you will have an answer to: What role do valence electrons play in chemical changes? Draw the following lewis
Write the letter that best answers the question or completes the statement on the line provided.
Chapter 4 Atomic Structure Chapter Test A Multiple Choice Write the letter that best answers the question or completes the statement on the line provided. 1. Democritus thought that matter was made of
Exam 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
4.2 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?
CHEMISTRY 11 UNIT REVIEW: ATOMIC THEORY & PERIODIC TRENDS
CHEMISTRY 11 UNIT REVIEW: ATOMIC THEORY & PERIODIC TRENDS Atoms Atoms have protons and neutrons located in the nucleus of the atom. Electrons orbit around the nucleus in well-defined paths. Protons have
Democritus 460 BC 370 BC. First scholar to suggest that atoms existed. Believed that atoms were indivisible and indestructible.
Democritus 460 BC 370 BC First scholar to suggest that atoms existed. Believed that atoms were indivisible and indestructible. Democritus 460 BC 370 BC Problems with theory: 1. Did not explain chemical
Unit 2 Exam - Atomic Structure and Nuclear
1. The atomic number of an atom is always equal to the total number of. neutrons in the nucleus. protons in the nucleus 5. The mass number of an atom is equal to the number of. neutrons, only. protons,
Democritus s ideas don t explain chemical behavior & lacked experimental support.
A1: Atomic Structure Worksheet Key (Goals 1 3, Chapter 4) 1. Democritus, who lived in Greece during the 4 th century B.C., suggested that matter is made up of tiny particles that cannot be divided. He
Lesson 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
UNIT 2 - ATOMIC THEORY
*KEY* *KEY* UNIT 2 - ATOMIC THEORY *KEY* *KEY* VOCABULARY: Allotrope Anion Atom Atomic Mass Atomic Mass unit (a.m.u.) Atomic number Bohr model Cation Compound Electron Electron Configuration Element Excited
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
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
Name: Per: Date: Teacher: Official Class: Chemistry. Unit 1: The Atom
Unit 1: The Atom The following pages are practice questions for this unit, and will be submitted for homework! You must complete: Unit Vocabulary ALL QUESTIONS What is an Atom? ALL QUESTIONS Calculating
Chapter 4 Lesson 2 Notes
Chapter 4 Lesson 2 Notes How were electrons discovered? Scientists have put together a detailed model of atoms and their parts. Here is the journey of atom parts. How were electrons discovered? (cont.)
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
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
Regents Chemistry PRACTICE PACKET. Unit 2: Atomic Theory
*STUDENT* *STUDENT* Regents Chemistry PRACTICE PACKET Unit 2: Atomic Theory 2 Copyright 2015 Tim Dolgos Name History of Atomic Theory Period Fill in the missing information in the chart below: Name of
Atomic Mass And Number Worksheet Answers
ATOMIC MASS AND NUMBER WORKSHEET ANSWERS PDF - Are you looking for atomic mass and number worksheet answers Books? Now, you will be happy that at this time atomic mass and number worksheet answers PDF
Atomic Nature of Matter
Objectives: Atomic Nature of Matter 1. Define the atom and parts of the atom 2. Define the properties of an atom; molecules, compounds; states of matter Atoms Atoms are the building blocks of matter. Matter
Chapter 4. Atomic Structure
Chapter 4 Atomic Structure Warm Up We have not yet discussed this material, but what do you know already?? What is an atom? What are electron, neutrons, and protons? Draw a picture of an atom from what
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
a. According to Dalton, what is inside the atom? Nothing, the atom it the smallest
Unit 3: Review SCIENTIFIC THEORIES Dalton theorized that atoms were the smallest particle and could not be divided. Atoms can bond with one another in whole number ratios to form compounds but cannot be
Development of Atomic Theory Elements of chemistry- Atoms, the building blocks of matter Video
Development of Atomic Theory Elements of chemistry- Atoms, the building blocks of matter Video 2 CH 4- Atoms 1 Discovering the Atom In this lesson we will take a look at the scientists who explored the
UNIT 3 DENSITY STRUCTURE S AND ISOTOPES
UNIT 3 DENSITY STRUCTURE S AND ISOTOPES What is density and how to use it? A Brief History of Chemistry Structure of an Atom How to make Ions? What are Isotopes? DENSITY Density: is the mass of a substance
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
Atoms, Elements, and the Periodic Table Unit Assessment (2016) Page 1 of 13
TEST NAME:Atoms, Elements, and the Periodic Table Unit Assessment (2016) TEST ID:36063 GRADE:06-08 SUBJECT:Life and Physical Sciences TEST CATEGORY: Common Assessment Atoms, Elements, and the Periodic
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
Atomic Class Packet Unit 3
The modern model of the atom has evolved over a long period of time through the work of many scientists.(3.1a) Each atom has a nucleus, with an overall positive charge, surrounded by one or more negatively
DUE DATE: JUNE 18 TH. SUMMER REV: Atomic Structure
NAME: DUE DATE: JUNE 18 TH AP Chemistry SUMMER REV: Atomic Structure Why? Atoms and isotopes are identified by the numbers of protons, neutrons and electrons they contain. Before you can understand the
Regents 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
Test Topics: Periodic Table, Atomic Theory, Physical/Chemical Properties, Atom, Isotopes, Average Atomic Mass
Elemental Properties Review Worksheet Test Topics: Periodic Table, Atomic Theory, Physical/Chemical Properties, Atom, Isotopes, Average Atomic Mass Periodic Table 1. List the element symbols for the following
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
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,
3.1 Classification of Matter. Copyright 2009 by Pearson Education, Inc.
Chapter 3 Atoms and Elements 3.1 Classification of Matter Copyright 2009 by Pearson Education, Inc. 1 Matter Matter is the stuff that makes up all things. Copyright 2009 by Pearson Education, Inc. 2 Pure