Atoimic Structure and the Periodic Table: Unit Objective Study Guide Part 2
|
|
- Jennifer Conley
- 6 years ago
- Views:
Transcription
1 Name Date Due Atoimic Structure and the Periodic Table: Unit Objective Study Guide Part 2 Directions: Write your answers to the following questions in the space provided. For problem solving, all of the work leading up to the final answer must be shown in order to receive credit. 1. Describe the historical development of the periodic table (Döbereiner, Newland, Mendeleev, Moseley, and Seaborg). Describe the contributions made by each of the following scientists to the development of the periodic table. a. Döbereiner (What is a triad?) b. Newland (What was Newland s law of octaves?) c. Mendeleev (Why did he leave gaps in his periodic table? What were some limitations to his arrangement of the elements?) d. Moseley e. Seaborg 2. Describe the arrangement of the periodic table. The elements in the periodic table are arranged in order of increasing atomic. The vertical columns are called or. The horizontal rows are called. The elements within the same have similar chemical properties. There are periods and groups. The metals are located on the side of the periodic table. The nonmetals, with the exception of hydrogen, are located on the side of the periodic table. The metalloids are located the metals and nonmetals.
2 3. Describe the general properties of the alkali metals, alkaline earth metals, halogens, noble gases, inner transition metals (lanthanide and actinide series), and the transition metals. List at least 3 distinctive properties for each of the following. a. alkali metals b. alkaline earth metals c. halogens d. noble gases e. inner transition metals (lanthanide and actinide series) f. transition metals 4. Classify elements as metals, nonmetals or metalloids; solids, liquids or gases; alkali metals, alkaline earth metals, transition metals, halogens, noble gases or inner transition metals (lanthanides or actinides). Identify the classes of elements to which each of the following elements belongs. Each element is described by more than one term. Choose from the following classes: metal, nonmetal, metalloid; alkali metal, alkaline earth metal, transition metal, inner transition metal (lanthanide or actinide), halogen, noble gas; solid, liquid, gas (at room temperature). a. argon: b. germanium: c. mercury: d. phosphorus: e. magnesium:
3 5. Distinguish between principal energy level, energy sublevel, and atomic orbital. 1s 2 Principal energy level energy sublevel atomic orbital - 6. Use the Bohr model to draw representations for atoms. 7. Apply the aufbau principle, the Pauli exclusion principle, and Hund s rule in writing the electron configurations and orbital diagrams of elements. 8. Write the electron configuration and noble-gas notation of elements using the periodic table as a guide. Complete the following table. Nitrogen-14 Calcium-40 Xenon-131 Bohr Model Orbital Diagram Electron Configuration Bohr Notation Noble-Gas Notation
4 9. Distinguish between the ground state and the excited state of an atom. Ground state Excited state 10. Recognize the demarcation of the periodic table into an s block, p block, d block, and f block. Color the s block blue. Color the p block green. Color the d block red. Color the f block purple. For each of the following electron configurations of neutral atoms, determine if the configuration as written is the ground state, an excited state, or if it is an impossible configuration. a. 1s 2 2s 2 2p 4 b. 1s 2 2s 3 2p 6 c. 1s 2 2s 2 2p 5 3s Use electron configurations to classify elements as noble gases, alkali metals, alkaline earth metals, halogens, transition metals or inner transition metals. Explain how an element s outer electron configuration is related to its position in the periodic table. Identify the ending electron configuration for each of the following classes of elements. The first one has been done for you. a. noble gases s 2 (helium), p 6 (other noble gases) b. alkali metals - c. alkaline earth metals - d. halogens - e. transition metals - f. inner transition metals Define valence electrons and determine how many are present in atom of each maingroup (representative) element. What are valence electrons? Indicate two different ways in which the valence electrons for a main-group element can be determined. Indicate the number of valence electrons for each of the following elements. a. potassium b. magnesium c. boron d. carbon e. phosphorus f. oxygen g. fluorine h. neon
5 13. Describe the octet rule and use it to predict the charge on a stable ion. State the octet rule 14. Define isoelectronic and give examples. What does the term isoelectronic mean? Complete the following table. Element Number of Valence Electrons Charge on Stable Ion Sodium 1 +1 Calcium Aluminum Nitrogen Sulfur Iodine Is it possible for two atoms to be isoelectronic? List four ions that are isoelectronic with argon. 15. Define periodicity. Periodicity Define atomic and ionic radii, ionization energy, and electronegativity. a. atomic radii - b. ionic radii c. ionization energy Which group of elements has the highest first ionization energy? Which group of elements has the lowest first ionization energy? Why is the third ionization energy for calcium much higher than the second ionization energy? d. electronegativity Which element has the highest electronegativity value?
6 17. Describe what is meant by nuclear charge (force) and the role it plays on periodic trends. What is nuclear charge (force)? Why does nuclear charge increase as you go from left to right across a period? Why are negative ions (anions) always larger than the neutral atom from which they came? (i.e. Why is the chloride ion larger than the chlorine atom?) Why are positive ions (cations) always smaller than the neutral atom from which they came? (i.e. Why is the magnesium ion smaller than the magnesium atom?) 18. Interpret and explain period trends in atomic radii, ionic radii, ionization energies and electronegativities. Explain how nuclear charge affects each of the following period trends: a. atomic radii - Arrange the following elements in order of increasing atomic radii: calcium, bromine, arsenic, and gallium b. ionic radii - Which ion is larger, the sulfide ion or the chloride ion? Explain your answer. c. ionization energy - Arrange the following elements in order of increasing first ionization energy: rubidium, xenon, strontium, tin, and iodine. d. electronegativity - Arrange the following elements in order of increasing electronegativity: lithium, fluorine, beryllium, boron, nitrogen, and oxygen.
7 19. Describe the shielding effect and the role it plays on periodic trends. What is the shielding effect? How does the shielding effect change as you go from top to bottom within a group? How does the shielding effect change as you from left to right within a period? 20. Interpret and explain group trends in atomic radii, ionic radii, ionization energies and electronegativities. Explain how the shielding effect affects each of the following group trends: a. atomic radii - Arrange the alkali metals in order of increasing atomic radii. b. ionic radii - c. ionization energy - Arrange the alkaline earth metals in order of increasing first ionization energy. d. electronegativity Arrange the halogens in order of increasing electronegativity.
The Periodic Table & Formation of Ions
The Periodic Table & Formation of Ions Development of the Periodic Table Mendeleev: Considered to be the father of the periodic table Arranged elements by increasing atomic mass Placed elements with similar
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 informationPart I Assignment: Electron Configurations and the Periodic Table
Chapter 11 The Periodic Table Part I Assignment: Electron Configurations and the Periodic Table Use your periodic table and your new knowledge of how it works with electron configurations to write complete
More informationElectronic Structure of Atoms and the Periodic table. Electron Spin Quantum # m s
Electronic Structure of Atoms and the Periodic table Chapter 6 & 7, Part 3 October 26 th, 2004 Homework session Wednesday 3:00 5:00 Electron Spin Quantum # m s Each electron is assigned a spinning motion
More informationCHAPTER NOTES CHAPTER 14. Chemical Periodicity
Goals : To gain an understanding of : 1. Electron configurations 2. Periodicity. CHAPTER NOTES CHAPTER 14 Chemical Periodicity The periodic law states that when the elements are arranged according to increasing
More informationOrganizing the Periodic Table
Organizing the Periodic Table How did chemists begin to organize the known elements? Chemists used the properties of the elements to sort them into groups. The Organizers JW Dobereiner grouped the elements
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 information12/5/2016. Which of the following are main-group elements? Magnesium Vanadium Antimony Lead Neptunium Cesium Rutherfordium Boron Indium
Learning Target: Classify elements according to their location on the Periodic Table This is a brief review of that information. Identify the following as being an alkalai metal, alkaline earth metal,
More informationUnit 3: The Periodic Table and Atomic Theory
Name: Period: Unit 3: The Periodic Table and Atomic Theory Day Page # Description IC/HW 1 2-3 Periodic Table and Quantum Model Notes IC 1 4-5 Orbital Diagrams Notes IC 1 14 3-A: Orbital Diagrams Worksheet
More information2/15/2013. Chapter 6 6.1
Chapter 6 In a self-service store, the products are grouped according to similar characteristics. With a logical classification system, finding and comparing products is easy. You will learn how elements
More informationUNIT 3: The Periodic Table
UNIT 3: The Periodic Table Aristotle circa 300 BC Antoine Lavoisier 1770 1789 Jöns Jakob Berzelius 1828 Johann Döbereiner 1829 John Newlands 1864 Lothar Meyer 1869 Dmitri Mendeleev 1869 William Ramsay
More informationPage 1 of 9. Website: Mobile:
Question 1: Did Dobereiner s triads also exist in the columns of Newlands Octaves? Compare and find out. Only one triad of Dobereiner s triads exists in the columns of Newlands octaves. The triad formed
More information12/6/2017. Which of the following are main-group elements? Magnesium Vanadium Antimony Lead Neptunium Cesium Rutherfordium Boron Indium
Learning Target: Classify elements according to their location on the Periodic Table This is a brief review of that information. Identify the following as being an alkalai metal, alkaline earth metal,
More informationPeriodic Table and Trends Structure and Properties of Matter. Background
Background Periodic trends are the patterns observed in elemental properties across a row or down a column on the Periodic Table. Some of these trends were observed when the Periodic Table was first being
More informationNotes: Unit 6 Electron Configuration and the Periodic Table
Name KEY Block Notes: Unit 6 Electron Configuration and the Periodic Table In the 1790's Antoine Lavoisier compiled a list of the known elements at that time. There were only 23 elements. By the 1870's
More informationCHAPTER 6 The Periodic Table
CHAPTER 6 The Periodic Table 6.1 Organizing the Elements Mendeleev: listed the elements in order of increasing atomic mass and in vertical columns according to their properties. Left blank spaces for undiscovered
More informationHonors: Unit 2 : Periodic Table and Trends Study Guide
Name: Date: Period: Honors: Unit 2 : Periodic Table and Trends Study Guide Objectives to Study: Any objectives from previous assessments can possibly be on the test :-) Names of groups and their properties
More informationTest Review # 4. Chemistry: Form TR4-5A 6 S S S
Chemistry: Form TR4-5A REVIEW Name Date Period Test Review # 4 Development of the Periodic Table. Dmitri Mendeleev (1869) prepared a card for each of the known elements listing the symbol, the atomic mass,
More informationChapter 5. Preview. Lesson Starter Objectives Mendeleev and Chemical Periodicity Moseley and the Periodic Law The Modern Periodic Table
Preview Lesson Starter Objectives Mendeleev and Chemical Periodicity Moseley and the Periodic Law The Modern Periodic Table Section 1 History of the Periodic Table Lesson Starter Share what you have learned
More informationName Date Class ORGANIZING THE ELEMENTS
6.1 ORGANIZING THE ELEMENTS Section Review Objectives Explain how elements are organized in a periodic table Compare early and modern periodic tables Identify three broad classes of elements Vocabulary
More informationChemistry Chapter 9 Review. 2. Calculate the wavelength of a photon of blue light whose frequency is 6.3 x s -1.
Chemistry Chapter 9 Review 1. What is the frequency of radiation that has a wavelength of 4.7 x 10-5 cm? 2. Calculate the wavelength of a photon of blue light whose frequency is 6.3 x 10 14 s -1. 3. The
More informationColumn B 5. periodic table a. A vertical column of elements in the
Unit 4 Assignment Packet Name Period: A1: The Periodic Table: Organizing the Elements A. periodic table B. metals C. nonmetals D. periods E. alkali metals F. halogens G. columns H. periodic law I. alkaline
More informationSection 6-1 Notes. Organizing the Elements
Section 6-1 Notes Organizing the Elements Organizing the Elements As new elements were discovered chemists needed to find a logical way to organize them Properties of elements were used to sort them in
More informationPeriodic Trends. Name: Class: Date: ID: A. Matching
Name: Class: Date: Periodic Trends Matching Match each item with the correct statement below. a. electronegativity f. periodic law b. ionization energy g. atomic mass c. atomic radius h. period d. metal
More informationUnits 1, 2 study guide- atomic structure
Name: Units 1, 2 study guide- atomic structure 1) Complete the required information for each subatomic particle (T1.3) symbol name charge location Mass (AMU) p + e - n 0 2) Define the following terms:
More informationAccelerated Chemistry Study Guide The Periodic Table, Chapter 5
Accelerated Chemistry Study Guide The Periodic Table, Chapter 5 Terms, definitions, and people Dobereiner Newlands Mendeleev Moseley Periodic table Periodic Law group family period Page 1 of 38 alkali
More informationPERIODIC CLASSIFICATION
5 PERIODIC CLASSIFICATION OF ELEMENTS TEXTBOOK, QUESTIONS AND THEIR ANSWERS Q.1. Do Dobereiner s triads also exist in the columns of Newland s octaves? Compare and find out. Ans. Triad of Li, Na and K
More informationUnit 3 Periodic Table and Quantum HW Packet Name Date. Periodic Table Concepts. 1. In what family are the most active metals located?
Directions: Answer the following questions. Periodic Table Concepts 1. In what family are the most active metals located? 2. In what family are the most active non-metals located? 3. What family on the
More informationName Date Class THE PERIODIC TABLE
Name Date Class 6 THE PERIODIC TABLE SECTION 6.1 ORGANIZING THE ELEMENTS (pages 155 160) This section describes the development of the periodic table and explains the periodic law. It also describes the
More informationClassify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
ELECTRONS IN ATOMS Chapter Quiz Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 1. The orbitals of a principal energy level are lower in energy than the orbitals
More informationIdentify the five scientists that progressed atomic structure Illustrate each scientist s model of the atom
Semester Review What happens to electronegativity down a group? electrons for aluminum Identify the five scientists that progressed atomic structure Illustrate each scientist s model of the atom Circle
More informationA sample of carbon dioxide has a volume of 28.7 L and a mass of 52.5 g at 20 C. Determine the density of carbon dioxide at this temperature.
Semester Review A sample of carbon dioxide has a volume of 28.7 L and a mass of 52.5 g at 20 C. Determine the density of carbon dioxide at this temperature. 1.83 g/l Describe what defines an element s
More informationChapter 6: The Periodic Table
Chapter 6: The Periodic Table Name: Per: Test date: In-Class Quiz: Moodle Quiz: preap Learning Objectives Trace the historical development of the periodic table Identify the major groups and key features
More informationThe Periodic Table and Periodic Law
The Periodic Table and Periodic Law Periodic trends in the properties of atoms allow us to predict physical and chemical properties. Section 1: Development of the Modern Periodic Table Section 2: Classification
More informationPart I: It s Just a Trend
Part I: It s Just a Trend 1. What is the trend with the atomic numbers of the elements as you move from left to right across a period on the Periodic Table? How does this sequence continue to the next
More informationUnit Five Practice Test (Part I) PT C U5 P1
Unit Five Practice Test (Part I) PT C U5 P1 Name Period LPS Standard(s): --- State Standard(s): 12.3.1 Short Answers. Answer the following questions. (5 points each) 1. Write the electron configuration
More informationSearching for an Organizing Principle. Searching for an Organizing Principle. How did chemists begin to organize the known elements?
Searching for an Organizing Principle Searching for an Organizing Principle How did chemists begin to organize the known elements? Searching for an Organizing Principle A few elements, including copper,
More informationWARM-UP. Draw each of the three models of the atom that we learned about last unit. Who came up with each? What was wrong with each?
WARM-UP Draw each of the three models of the atom that we learned about last unit. Who came up with each? What was wrong with each? 1:59 1:58 1:57 1:56 1:55 1:54 1:53 1:52 1:51 1:50 1:49 1:48 1:47 1:46
More informationPractice Periodic Table Review
Practice Periodic Table Review Name 1. An electron will emit energy in quanta when its energy state changes from 4p to A) 5s B) 5p C) 3s D) 6p 2. Which electron configuration represents an atom in the
More informationThe Elements. ! Developed a method using x-ray spectra to identify elements
The Elements Instructions: 1. On your paper (s), copy down the given information for each of the following scientists, matter classification, or groups on the periodic table, 2. For each of the scientists,
More informationWorksheet #1: Atomic Spectra Answer the following questions using your Unit 3 notes.
Worksheet #1: Atomic Spectra 1. How did Bohr expand on Rutherford s model of the atom? 2. Compare the energy of an electron in the ground state and an electron in the excited state. 3. When an electron
More informationPeriodic Table Workbook
Key Ideas: The placement or location of elements on the Periodic Table gives an indication of physical and chemical properties of that element. The elements on the Periodic Table are arranged in order
More informationThe Atom & Periodic Table. Unit 2 Topics 4-6
The Atom & Periodic Table Unit 2 Topics 4-6 Electrons in Atoms Topic 4 Describe Bohr s model of the atom. Sketch it! Bohr - A review electrons exist in orbits around the nucleus. Bohr - IB Information
More informationPERIODIC CLASSIFICATION OF ELEMENTS
PERIODIC CLASSIFICATION OF ELEMENTS Important terms & condition: Classification of elements: the arrangement of elements in such a manner that elements with similar Properties are grouped together while
More information1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass
1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass A Br, Ga, Hg C O, S, Se B atomic number D oxidation number 2. Which list includes elements with the
More informationName: Class: Date: ID: A
Name: Class: _ Date: _ ID: A EOC review II Matching Match each item with the correct statement below. a. atomic orbital d. ground state b. aufbau principle e. Pauli exclusion principle c. electron configuration
More informationHonors Chemistry: Chapter 4- Problem Set (with some 6)
Honors Chemistry: Chapter 4- Problem Set (with some 6) All answers and work on a separate sheet of paper! Classify the following as always true (AT), sometimes true (ST), or never true (NT) 1. Atoms of
More informationSECTION 1. History of the Periodic Table
Periodic Law SECTION 1 History of the Periodic Table MENDELEEV AND CHEMICAL PERIODICITY When the Russian chemist Dmitri Mendeleev heard about the new atomic masses he decided to include the new values
More information1. Electronic Structure 2. Electron Configuration 3. Core Notation 4. EC Relationship to Periodic Table 5. Electron Configuration of Ions
Pre-AP Chemistry 11 Atomic Theory II Name: Date: Block: 1. Electronic Structure 2. Electron Configuration 3. Core Notation 4. EC Relationship to Periodic Table 5. Electron Configuration of Ions Electronic
More information1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass
1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass A Br, Ga, Hg C O, S, Se B atomic number D oxidation number 2. Which list includes elements with the
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) In nature, sulfur is most commonly found in. 1) A) pure elemental sulfur B) H2S C) sulfuric
More information5. The outermost principal energy level electron configuration of the element bromine is: a. 4s 2 c. 4s 2 4p 5 b. 4p 5 d.
1 c E = h 1. Sodium and potassium have similar properties because they have the same a. atomic radii. c. number of valence electrons. b. ionization energy. d. electronegativity. 2. Electrons must be added
More informationRegan & Johnston Chemistry Unit 3 Exam: The Periodic Table Class Period
Regan & Johnston Name Chemistry Unit 3 Exam: The Periodic Table Class Period 1. An atom of which element has the largest atomic radius? (1) Si (2) Fe (3) Zn (4) Mg 2. Which characteristics both generally
More informationThe Quantum Mechanical Model
Recall The Quantum Mechanical Model Quantum Numbers Four numbers, called quantum numbers, describe the characteristics of electrons and their orbitals Quantum Numbers Quantum Numbers The Case of Hydrogen
More informationChemistry Study Guide
Chemistry Study Guide Marking Period 3 Exam Week of 3/21/17 Study Guide due - When studying for this test, use your do nows, notes, homework, class handouts, and your textbook. Vocabulary Chapter 7 Anion
More informationNote Taking Guide: Episode 401. arranged elements by. predicted of missing. discovered that each has a unique. arranged elements by
Note Taking Guide: Episode 401 Dmitri Mendeleev: arranged elements by. predicted of missing. Henry Moseley: discovered that each has a unique. arranged elements by. now all elements fit into place based
More informationValence electron- Energy sublevel- Transition element- Period 10. Electronegativity- Alkaline earth metal- 11. Ion- Halogen- 12.
Mrs. Hilliard 1. Valence electron 2. Period 3. Alkaline earth metal 4. Halogen 5. Metalloid 6. Hund s Rule 7. Representative element 8. Energy sublevel 9. Transition element 10. Electronegativity 11. Ion
More informationPeriodic Table of Elements
Periodic Table of Elements chlorine nitrogen helium gold oxygen silver mercury hydrogen neodymium sodium niobium carbon Elements Science has come along way since Aristotle s theory of Air, Water, Fire,
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 informationAdvanced Chemistry. Mrs. Klingaman. Chapter 5: Name:
Advanced Chemistry Mrs. Klingaman Chapter 5: The Periodic Law Name: _ Mods: Chapter 5: The Periodic Law Reading Guide 5.1 History of the Periodic Table (pgs. 125-129) 1) What did Dimitri Mendeleev notice
More information: the smallest particle that has the properties of an element. In, this Greek philosopher suggested that the universe was made of.
Notes: ATOMS AND THE PERIODIC TABLE Atomic Structure: : the smallest particle that has the properties of an element. From the early concept of the atom to the modern atomic theory, scientists have built
More informationRegan & Johnston Chemistry Unit 3 Exam: The Periodic Table Class Period
Regan & Johnston Name Chemistry Unit 3 Exam: The Periodic Table Class Period 1. An atom of which element has the largest atomic radius? (1) Si (2) Fe (3) Zn (4) Mg 2. Which characteristics both generally
More informationThe orbitals in an atom are arranged in shells and subshells. orbital 3s 3p 3d. Shell: all orbitals with the same value of n.
Shells and Subshells The orbitals in an atom are arranged in shells and subshells. n=3 orbital 3s 3p 3d Shell: all orbitals with the same value of n n=3 3s 3p 3d Subshell: all orbitals with the same value
More informationElectrons and the Periodic Table:
Electrons and the Periodic Table: Development of the Periodic Table: The development of the periodic table started in the 1800 s. * By the end of the 1700 s, scientists had identified about 30 elements.
More informationYou will be responsible for answering the questions and submitting them by the END of the first week back.
PLEASE READ FIRST IB/AP Chemistry Summer Assignment Dear IB/AP Chemistry students! You all deserve a well-earned break and I wish you all a very enjoyable summer whatever you are up to. This summer assignment
More informationUnit 2 - Electrons and Periodic Behavior
Unit 2 - Electrons and Periodic Behavior I. The Bohr Model of the Atom A. Electron Orbits, or Energy Levels 1. Electrons can circle the nucleus only in allowed paths or orbits 2. The energy of the electron
More informationNotes: Electrons and Periodic Table (text Ch. 4 & 5)
Name Per. Notes: Electrons and Periodic Table (text Ch. 4 & 5) NOTE: This set of class notes is not complete. We will be filling in information in class. If you are absent, it is your responsibility to
More informationChapter 3: Electron Structure and the Periodic Law
Chapter 3: Electron Structure and the Periodic Law PERIODIC LAW This is a statement about the behavior of the elements when they are arranged in a specific order. In its present form the statement is:
More informationHistory German J. W. Dobereiner Grouped elements into triads
The Periodic Table History 1829 German J. W. Dobereiner Grouped elements into triads One of these triads included chlorine, bromine, and iodine; another consisted of calcium, strontium, and barium. In
More informationName Class Date ELECTRONS AND THE STRUCTURE OF ATOMS
The Periodic Table ELECTRONS AND THE STRUCTURE OF ATOMS 6.1 Organizing the Elements Essential Understanding Although Dmitri Mendeleev is often credited as the father of the periodic table, the work of
More informationMIDTERM STUDY GUIDE. Chapter 1 Introduction to Chemistry
MIDTERM STUDY GUIDE Chapter 1 Introduction to Chemistry What is chemistry? Chemical properties vs. physical properties examples of both States of matter Scientific method Chapter 2 Data Analysis SI measurement
More information#9 Modern Atomic Theory Quantitative Chemistry
Name #9 Modern Atomic Theory Quantitative Chemistry Student Learning Map Unit EQ: What is the current model of the atom? Key Learning: The current model of the atom is based on the quantum mechanical model.
More informationCHAPTER 6. Table & Periodic Law. John Newlands
CHAPTER 6 Table & Periodic Law 6.1 Developing a Periodic Table The periodic table was developed to show the properties of an element by simply looking at it's location. In 1860, chemists agreed on a way
More informationUnit 2 Atomic Theory and Periodicity Review
Unit 2 Atomic Theory and Periodicity Review Section I: History In each box, write the name of the scientist(s) associated with the statement. Choose from among the following: Democritus Thomson Bohr Schroedinger
More informationName: Teacher: Gerraputa
Name: Teacher: Gerraputa 1. Which list of elements contains a metal, a metalloid, and a nonmetal? 1. Ag, Si, I 2 3.K, Cu, Br 2 2. Ge, As, Ne 4.S, Cl 2, Ar 2. The elements on the Periodic Table are arranged
More informationANNOUNCEMENTS! 2. Quizzes beginning of class Must be on time to class No Excuses; tardies
ANNOUNCEMENTS! 1. Housekeeping Rules, Door, Attention signal, Bathroom Class average = seats = rule 3 2. Quizzes beginning of class Must be on time to class No Excuses; tardies 3. Tutoring 2:15 Sign log
More informationFocus Learning Targets for Periodic Trends and Bonding (1) Discuss the development of the periodic table by Mendeleev. (2) Locate and state important
Focus Learning Targets for Periodic Trends and Bonding (1) Discuss the development of the periodic table by Mendeleev. (2) Locate and state important properties of main chemical families including the
More informationPeriodic Classification of Elements
Periodic Classification of Elements Important Points: The first classification of elements is due to dobereiner in 1817. Dobereiner Triad Theory: "The atomic weight of the middle element is the arithmetic
More informationUNIT (2) ATOMS AND ELEMENTS
UNIT (2) ATOMS AND ELEMENTS 2.1 Elements An element is a fundamental substance that cannot be broken down by chemical means into simpler substances. Each element is represented by an abbreviation called
More informationOrbital Diagram Rules: 1. The Aufbau Principle: Under normal condition, each electron occupies the
Honors Chemistry Ms. Ye Name Date Block Orbital Diagram Rules: 1. The Aufbau Principle: Under normal condition, each electron occupies the 2. The Pauli Exclusion Principle: a maximum of can occupy an orbital
More informationThe Periodic Table. You have learned the names of several of the groups in previous science courses:
The Periodic Table The periodic law, which is the basis for the modern periodic table, states that when elements are arranged in order of increasing atomic number, their physical and chemical properties
More informationUnit 5 Elements and their Properties
Unit 5 Elements and their Properties 1. In 1871, Russian chemist created the forerunner of the modern periodic table. 2. The elements in Mendeleev's table were arranged in order of increasing. 3. What
More informationUnit 2 Chapters 5 and 6 Atoms/Periodic Table/ NOMENCLATURE NAMING AND FORMING COMPOUNDS
Unit 2 Chapters 5 and 6 Atoms/Periodic Table/ NOMENCLATURE NAMING AND FORMING COMPOUNDS Review of Atomic Structure What is an atom? The smallest particle of an element that retains the properties of that
More informationUnit 2: The Periodic Table
Unit 2: The Periodic Table The following pages are practice questions for this unit, and will be submitted for homework! You must complete: Unit Vocabulary ALL QUESTIONS What Group Am I? ALL QUESTIONS
More informationIonic Bonding Ionic bonding occurs when metals and nonmetals trade one or more electrons and the resulting opposite charges attract each other. Metals
Chemical Bonding Now that we know what atoms look like A very small (less than 0.001% of the volume) and massive (more than 99.99% of the mass) nucleus with protons (+) and neutrons (neutral) and electrons
More informationHistory of the Periodic Table. In this lesson, you will be introduced to a variety of attempts at classifying the elements.
History of the Periodic Table As chemists discovered more and more elements, and learned more and more about their properties, they began to see certain patterns emerge. These patterns led to a desire
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 informationUnit 02 Review: Atomic Theory and Periodic Table Review
Practice Multiple Choice Questions Unit 02 Review: Atomic Theory and Periodic Table Review 1. The number of neutrons in an atom of radioactive C 14 is: a) 6 c) 8 b) 12 d) 14 2. When a radioactive nucleus
More informationUNIT 5.1. Types of bonds
UNIT 5.1 Types of bonds REVIEW OF VALENCE ELECTRONS Valence electrons are electrons in the outmost shell (energy level). They are the electrons available for bonding. Group 1 (alkali metals) have 1 valence
More informationElectronic Structure and Bonding Review
Name: Band: Date: Electronic Structure and Bonding Review 1. For electrons: a. What is the relative charge? b. What is the relative mass? c. What is the symbol? d. Where are they located in the modern
More informationMendeleev s Periodic Table Mendeleev arranged the elements in his periodic table in order of increasing atomic mass.
6.1 Searching For an Organizing Principle Chemists used the properties of elements to sort them into groups. Mendeleev s Periodic Table Mendeleev arranged the elements in his periodic table in order of
More informationUnit 4 - Periodic Table Exam Name: PRACTICE QUESTIONS Date: 2/23/2016
Name: PRACTICE QUESTIONS Date: 2/23/2016 1. Which pair of symbols represents a metalloid and a noble gas? 1) Si and Bi 2) As and Ar 3) Ge and Te 4) Ne and Xe 2. What determines the order of placement of
More informationChapter 7. Electron Configuration and the Periodic Table
Chapter 7 Electron Configuration and the Periodic Table Topics Development of the periodic table The modern periodic table Effective nuclear charge Periodic trends in properties of elements Electron configuration
More informationName PRACTICE Unit 3: Periodic Table
1. Compared to the atoms of nonmetals in Period 3, the atoms of metals in Period 3 have (1) fewer valence electrons (2) more valence electrons (3) fewer electron shells (4) more electron shells 2. On the
More informationUnit Five: The Periodic Table Ref:
Unit Five: The Periodic Table Ref: 10.11 11.2 11.4 History of P.T. Chlorine Bromine Iodine Dobrenier- (1829) Triads groups of three elements of similar chemical and physical properties. Cannizzarro (1860)
More informationChapter Test B. Chapter: Arrangement of Electrons in Atoms. possible angular momentum quantum numbers? energy level? a. 4 b. 8 c. 16 d.
Assessment Chapter Test B Chapter: Arrangement of Electrons in Atoms PART I In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question
More informationThe Periodic Table. Tuesday 11/09/15. Friday, November 13, 15
The Periodic Table Tuesday 11/09/15 Agenda Notes on Topic 3 and Introduce Periodic Trends Computer Lab (Friday) Periodicity Periodic table Periodic Trends Ms. Thompson - SL Chemistry Wooster High School
More informationcalcium and magnesium
Section 5 5 Elements and the Periodic Table (Pages 184 187) 1. Electrolytes are the substances whose water solutions conduct electricity. Nonelectrolytes are substances that when in water do not conduct
More informationHow Electrons Determine Chemical Behavior
The Periodic Table Activity 7 How Electrons Determine Chemical Behavior GOALS In this activity you will: Investigate more patterns electron arrangements of atoms. Relate the positions s on the, their electron
More informationChemistry: Hood River Valley High School Unit 3 Note Packet and Goals. Description A1. Marble Lab. Nailon Isotope Lab A2.
Chemistry: Hood River Valley High School Unit 3 Note Packet and Goals Name: Period: Unit 3 Atomic Structure and Periodic Table Unit Goals- As you work through this unit, you should be able to: 1. describe
More information