1 THE PERIODIC TABLE & PERIODIC LAW! Development of the Modern Periodic Table!
2 Development of the Periodic Table! Main Idea: The periodic table evolved over time as scientists discovered more useful ways to compare and organize the elements.! Organizing things according to their is useful.! Scientists organize the many different of chemical in the.!
3 Development of the Periodic Table! compiled list of elements at the time (late )! Contained elements organized into categories.!
4 Development of the Periodic Table! Antoine Lavoisier compiled list of known elements at the time (late 1700s)! Contained 33 elements organized into four categories.! Increased to over elements by! Advent of.! Development of.!
5 Development of the Periodic Table! New = new scientific! Chemists needed to organize the many associated with the elements.! Agreed upon method for determining of elements.! Finding a way to the elements made it possible for scientists to determine elements they were looking for.!
6 Development of the Periodic Table! English chemist ( )! Organized elements by atomic.! Saw repeat every elements.! Called! Named relationship law of! work for every element.!
7 Development of the Periodic Table! Meyer & Mendeleev (1869)! Demonstrated connection between and elemental.! Organized elements into periodic table in order by in columns with similar.!
8 Development of the Periodic Table! Meyer & Mendeleev (1869)! Demonstrated connection between atomic mass and elemental properties.! Widely accepted b/c he predicted the existence and properties of properties that were later discovered. (left spaces in table)!
9 Development of the Periodic Table! English chemist determined that elements in Mendeleev s table were not in.! Arranging by resulted in groups of elements with properties.! Solved problem by putting elements in increasing atomic.! Resulted in clear periodic pattern of!
10 Development of the Periodic Table! English chemist Henry Moseley determined that elements in Mendeleev s table were not in correct order.! There are rows, or, in the table.! Each period corresponds to a.!
11 Development of the Periodic Table! The of the elements within a period as you move a period from left to right.! The of properties within a period as you move from one period to the next.!
12 Development of the Periodic Table! Periodic repetition of chemical and physical properties of the elements when arranged by atomic number is called the.! Elements that have chemical and physical properties end up in the in the periodic table.!
13 Modern Periodic Table! Elements classified as,, and.! Metals are, at room temp, and good of heat & electricity.! - can be drawn into.! - can be pounded into thin.!
14 Modern Periodic Table! Elements classified as metals, nonmetals, and metalloids.! Nonmetals! Occupy side of periodic table.! There is a in properties among nonmetals than among metals.! Generally or, dull solids.! conductors of heat & electricity.!
15 Modern Periodic Table! Elements classified as metals, nonmetals, and metalloids.! Nonmetals! The variation among nonmetals makes it to describe one set of general that will apply to all nonmetals.!
16 Modern Periodic Table! Elements classified as metals, nonmetals, and metalloids.! Metalloids ( )! Border line on periodic table.! Have & properties of both and.! Under some conditions, metalloids may behave like. Under other conditions, they may behave like.!
17 Classification! of the Elements! Main Idea: Elements are organized in different in the periodic table according to their.! Chemical are identified according to about the of their.!
18 Classification! of the Elements! Main Idea: Elements are organized in different blocks in the periodic table according to their electron configurations.! What can you learn about each element from the periodic table?!
19 Modern Periodic Table! What information can be displayed in a periodic table?! The periodic table usually displays the and of the elements, along with information about the of their atoms.!
20 Modern Periodic Table! In the center is the for aluminum (Al).! The for aluminum ( ) is the symbol.! The element and atomic are the symbol.! 2, 8, and 3 indicate the number of in each occupied.!
21 Modern Periodic Table! Periodic Table is according to of at room temperature.! Black =! Red =! Blue =! Gray =!
22 Modern Periodic Table! Some groups of elements have names! 1A=! 2A=! Very ; usually exist as (ie~ ).! Highly (not as much as Group ).!
23 Modern Periodic Table! Some groups of elements have special names! 7A=! that are very ; usually exist as compounds (ie~ NaCl).! 8A= Noble gases! Nonmetals that are.!
24 Modern Periodic Table! Representative Elements! Groups! Display a wide range of and properties.! Most are ; few ; one.!
25 Modern Periodic Table! Transition Elements! Group elements are transition elements.! types that are based on their configurations.!! Usually displayed in of Periodic Table.! Characterized by the presence of electrons in orbitals.!
26 Modern Periodic Table! Transition Elements! Group B elements are transition elements.! Two types that are based on their electron configurations.!! Appear the main body of the periodic table.! Characterized by the presence of electrons in orbitals.!
27 Organizing Elements by Electron Configuration! determines the properties of an element.! play a key role in determining the of elements.!.! are electrons in the of an atom.! Elements can be sorted into, elements, metals, or metals based on their configurations.!
28 Organizing Elements by Electron Configuration! Valence electrons are electrons in the highest energy level of an atom.! of valence electrons of an atom = number in which the atom is located!
29 Organizing Elements by Electron Configuration! Valence electrons are electrons in the highest energy level of an atom.! Noble gas electron configurations.! The and sublevels are completely filled with electrons electrons in the s sublevel and electrons in the p sublevel.! Helium (He) 1s 2 Neon (Ne) 1s 2 2s 2 2p 6 Argon (Ar) 1s 2 2s 2 2p 6 3s 2 3p 6 Krypton (Kr) 1s 2 2s 2 2p 6 3s 2 3p 6 2d 10 4s 2 4p 6
30 Organizing Elements by Electron Configuration! Valence electrons are electrons in the highest energy level of an atom.! Representative elements configurations.! The and sublevels of the highest occupied energy level are.!
31 Organizing Elements by Electron Configuration! Valence electrons are electrons in the highest energy level of an atom.! Representative elements configurations.! In atoms of these Group elements, there is only electron in the highest occupied energy level.! Have chemical properties b/c all have the number of valence electrons.! Lithium (Li) 1s 2 2s 1 Sodium (Na) 1s 2 2s 2 2p 6 3s 1 Potassium (K) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1
32 Organizing Elements by Electron Configuration! Valence electrons are electrons in the highest energy level of an atom.! Representative elements configurations.! In atoms of the Group elements, there are electrons in the highest occupied energy level.! For any representative element, its equals the of in the highest occupied energy level.! Carbon (C) 1s 2 2s 2 2p 2 Silicon (Si) 1s 2 2s 2 2p 6 3s 2 3p 2 Germanium (Ge) 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 2
33 Valence Electrons & Period! of an element s electrons indicates the on the periodic table in which it is found.! Lithium (Li) = 2s 1 =! Gallium (Ga) = [Ar] 4s 2 3d 10 4p 1 =!
34 s-, p-, d-, & f-block Elements! Periodic table is divided into ( ) representing the atom s energy being filled with valence electrons! different energy sublevels (,,, & ), so periodic table divided into distinct blocks.! Reason for the table s odd shape!
35 s-, p-, d-, & f-block Elements! Periodic table is divided into sections (blocks) representing the atom s energy sublevel being filled with valence electrons!
36 s-block Elements! Consists of Groups &.! Group elements have filled s orbitals.! Contain valence electron & configuration ends in! Group elements have filled s orbitals.! Contain valence electron & configuration ends in!
37 p-block Elements! Comprised of Groups! Contain elements with filled or partially filled _ orbitals.! Spans groups b/c three p orbitals can hold a maximum of electrons.! Group elements are unique members of p-block! Atoms so they don t undergo chemical.!
38 Contains metals & is block.! Usually characterized by a outermost s orbital and filled or partially-filled orbital.! d-block Elements! d orbital = orbital - 1! ie~! d orbitals can hold a total of electrons, so d- block spans groups on periodic table.!
39 f-block Elements! Contains metals! Characterized by a filled / partially-filled outermost s orbital and filled or partially-filled & orbitals.! f orbitals can hold a total of electrons, so f- block spans columns on periodic table.!
40 Each on the periodic table corresponds to a.! Blocks of Elements!
41 Review Time! What does the period an element is located in tell you about that element s electron configuration? What does the group tell you?!
42 Periodic Trends! Main Idea: among elements in the periodic table include their and their ability to or electrons.! of periodic table tells about the of many of the.! Much like patterns of a calendar.!
43 Atomic Radius! What are the trends among the elements for atomic size?! Atomic size is a periodic trend influenced by.! Size is defined by how an atom lies to a atom.! This size is expressed as an.! The atomic radius is of the distance between the of two atoms of the same element.!
44 Atomic Radius! What are the trends among the elements for atomic size?! The atomic radius is one-half of the distance between the nuclei of two atoms of the same element.!
45 Atomic Radius! Trends in Atomic Radius! In general, atomic size from top to bottom within a, and from left to right across a.!
46 Trends in Atomic Radius! Atomic Radius! Atomic size increases from top to bottom within a group, and decreases from left to right across a period.! Atomic radius (pm) Atomic number
47 Trends within Groups! Atomic radii as you move down a group.! Atomic Radius! on the nucleus.! Number of occupied.! Variables affect atomic size in ways.!
48 Trends within Groups! Atomic radii increase as you move down a group.! The in the number of occupied orbitals electrons in the highest occupied energy level from the of protons in the nucleus.! The is than the effect of the increase in nuclear charge, so the atomic size.! Atomic Radius!
49 Trends within Periods! in atomic radii as you move left to right across period.! Caused by positive charge in.! Shielding effect is for all elements in a period.! Increasing nuclear charge pulls the electrons to the nucleus! Atomic size.! Atomic Radius!
50 Practice with Atomic Radius! Which alkali metal has an atomic radius of 238 pm?! Atomic Radius! Based on the data for alkali metals and noble gases, how does atomic size change within a group?! Is an atom of barium, atomic number 56, smaller or larger than an atom of cesium, Cs?!
51 Formation of Ions! An atom is electrically because it has numbers of and.! Atoms or electrons to form and acquire.! Positive and negative ions form when electrons are between atoms.!
52 Formation of Ions! Atoms gain or lose electrons to form ions and acquire charges.! Atoms that electrons and form charged ions.! An ion with a positive charge is called a.! The charge for a is written as a number followed by a sign.!
53 Formation of Ions! Atoms gain or lose electrons to form ions and acquire charges.! Atoms that electrons and form charged ions.! An ion with a negative charge is called an.! The charge for an is written as a number followed by a sign.!
54 Ionization Energy! Forming an ion requires.! Energy is needed to overcome b/t positive charge of and negative charge of.! energy is defined as the energy required to an from a gaseous atom.! The energy required to remove the electron from an atom is called the ionization energy.!
55 Ionization Energy! Ionization energy tends to from top to bottom within a and from left to right across a.!
56 Ionizing Energy! Indication of how an atom s nucleus holds onto its electrons.! ionization energy = hold.! likely to form ions.!
57 Ionization Energy! Group Trends in Ionization Energy! First ionization energy generally from top to bottom within a group.! Size of atom = nuclear charge on electrons.! Less to remove electrons.! First ionization energy (kj/ mol) Atomic number
58 Ionization Energy! Period Trends in Ionization Energy! First ionization energy generally from left to right across a period.! Nuclear charge ; shielding effect remains.! Increased between nucleus and electrons = to remove electrons.! First ionization energy (kj/ mol) Atomic number
59 Ionizing Energy! The graph reveals group and period trends for ionization energy.! Which element in period 2 has the lowest first ionization energy? In period 3?! What are the group and period trends for first ionization for noble gases and alkali metals?!
60 Ionizing Energy! It is possible to remove e - s from an atom.! Amount of energy = ionization energies! What are the values for the first, second and third ionization energies for sodium and aluminum?!
61 Ionizing Energy! It is possible to remove multiple e - s from an atom.! Amount of energy = ionization energies! Is it easier to remove an electron from an sodium or aluminum atom? From Na + or Al +? From Na 2+ or Al 2+?! Which ion is most common - Na 3+ or Al 3+?!
62 Ionic Radius! Atoms gain or lose electrons to form ions and acquire charges.! Atoms that lose electrons and form positively charged cations ALWAYS become.! Atoms that gain electrons and form negatively charged anions ALWAYS become.!
63 Ionic Radius! What are the trends among the elements for ionic size?! Ionic size tends to from top to bottom within a.! Size of cations and anions from left to right across a.!
64 Ionic Radius! Trends within Groups: from Top to Bottom.!
65 Ionic Radius! Trends within Periods: from Left to Right!
66 Octet Rule! Atoms tend to gain, lose, or share electrons in order to acquire a full set of valence electrons.! Useful for determining what type of ions an atom might form.! Elements on side form ions & electrons.! Elements on side form ions & electrons.!
67 Electronegativity! There is a property that can be used to predict the type of that will form during a reaction.! = ability of an atom of an element to electrons when the atom is in a compound.! H 2.1 Li 1.0 Na 0.9 K 0.8 Rb 0.8 Cs 0.7 Electronegativity Values for Selected Elements Be 1.5 Mg 1.2 Ca 1.0 Sr 1.0 Ba 0.9 B 2.0 Al 1.5 Ga 1.6 In 1.7 Tl 1.8 C 2.5 Si 1.8 Ge 1.8 Sn 1.8 Pb 1.9 N 3.0 P 2.1 As 2.0 Sb 1.9 Bi 1.9 O 3.5 S 2.5 Se 2.4 Te 2.1 F 4.0 Cl 3.0 Br 2.8 I 2.5
68 Electronegativity! Trends in Electronegativity! as you move top to bottom within a.! as you move left to right across a.!
69 Electronegativity! Trends in Electronegativity! Least electronegative element in the table is.! tendency to electrons.! electrons and forms.!
70 Electronegativity! Trends in Electronegativity! electronegative element in the table is.! tendency to electrons.! electrons and forms.!
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,
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
1 63 Periodic Trends > Chapter 6 The Periodic Table 61 Organizing the Elements 62 Classifying the Elements 63 Periodic Trends 2 63 Periodic Trends > CHEMISTRY & YOU How are trends in the weather similar
63 Periodic Trends > 63 Periodic Trends > CHEMISTRY & YOU Chapter 6 The Periodic Table 61 Organizing the Elements 62 Classifying the Elements 63 Periodic Trends How are trends in the weather similar to
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
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
Chapter 6 The Periodic Table Section 6.1 Organizing the Elements OBJECTIVES: Explain how elements are organized in a periodic table. Section 6.1 Organizing the Elements OBJECTIVES: Compare early and modern
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
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
Name: Chemistry, PERIODIC TABLE 1. A solid element that is malleable, a good conductor of electricity, and reacts with oxygen is classified as a (1) noble gas (2) metalloid (3) metal (4) nonmetal 2. Which
Chapter 6 - The Periodic Table and Periodic Law Objectives: Identify different key features of the periodic table. Explain why elements in a group have similar properties. Relate the group and period trends
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
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
Chemical Periodicity Periodic Table Classification of the Elements OBJECTIVES: Explain why you can infer the properties of an element based on those of other elements in the periodic table. Classification
The Modern Periodic Table 1. An arrangement of the elements in order of their numbers so that elements with properties fall in the same column (or group). Groups: vertical columns (#1-18) Periods: horizontal
THE PERIODIC TABLE Is an arrangement of elements in which the elements are separated into groups based on a set of repeating properties EXPANSION OF THE ELEMENTS French scientist Lavoisier complied a list
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
1. The arrangement of the elements from left to right in Period 4 on the Periodic Table is based on A) atomic mass B) atomic number C) the number of electron shells D) the number of oxidation states 2.
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,
Topic 3: Periodicity OBJECTIVES FOR TODAY: Fall in love with the Periodic Table, Interpret trends in atomic radii, ionic radii, ionization energies & electronegativity The Periodic Table What is the periodic
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
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
Unit 5 The Periodic Table I. Development of Periodic Table Periodic law: when elements are arranged in order of increasing atomic number, their physical and chemical properties show a periodic pattern.
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
6.1 Development of the Modern Periodic Table Objectives: 1. Describe the major advancements in development of the periodic table 2. Describe the organization of the elements on the periodic table 3. Classify
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
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
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
CHEM 1305: Introductory Chemistry The Periodic Table From Chapter 5 Textbook Introductory Chemistry: Concepts and Critical Thinking Seventh Edition by Charles H. Corwin Classification of Elements By 1870,
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
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
The Periodic Law Notes (Chapter 5) I. History of the Periodic Table About 70 elements were known by 1850 (no noble gases) but there didn t appear to be a good way of arranging or relating them to study.
*KEY* *KEY* Regents Chemistry PRACTICE PACKET Unit 3: Periodic Table 1 Copyright 2015 Tim Dolgos 2 Copyright 2015 Tim Dolgos 3 Copyright 2015 Tim Dolgos It s Elemental DIRECTIONS: Use the reading below
*STUDENT* *STUDENT* Mr. Dolgos Regents Chemistry PRACTICE PACKET Unit 3: Periodic Table 2 3 It s Elemental DIRECTIONS: Use the reading below to answer the questions that follow. We all know by now that
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
Regents Chemistry: Practice Packet Unit: 5 Periodic Table 1 VOCABULARY For each word, provide a short but specific definition from YOUR OWN BRAIN! No boring textbook definitions. Write something to help
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
Assessment Chapter 5 Pre-Test Chapter: The Periodic Law Use the periodic table below to answer the questions in this Chapter Test. In the space provided, write the letter of the term or phrase that best
Chapter 6 Organizing the Elements THE PERIODIC TABLE AND PERIODIC LAW Periodic Table Summary Sheet For the Periodic Table above indicate each of the following TRENDS: atomic size and ionic size Na Na +
Chapter 5 Lecture Chapter 5 Electronic Structure and Periodic Trends 5.6 Trends in Periodic Properties Learning Goal Use the electron configurations of elements to explain the trends in periodic properties.
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
Chapter 5 Notes Chemistry; The Periodic Law The Periodic Table The periodic table is used to organize the elements in a meaningful way. As a consequence of this organization, there are periodic properties
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
Trends in the Periodic Table Effective nuclear charge: < effective nuclear charge is the attraction felt by the valence electrons from the nucleus < increases across a period : increases across because
CHAPTER 5 THE PERIODIC LAW What types of useful information can you find on the Periodic Table? I. History of the Periodic Table A. Before the Periodic Table was invented, about 63 elements were known.
PERIODIC TRENDS AND THE PERIODIC TABLE THE PERIODIC TABLE The row tells us how many energy levels are in that atom The row is also the group The column tells us how many electrons are in the outer energy
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
A few elements, including copper, silver, and gold, have been known for thousands of years There were only 13 elements identified by the year 1700. Chemists suspected that other elements existed. As chemists
Honors Chemistry Unit 4 (2017-2018) Families (research and present) Metals/nonmetals Trends o Atomic radius o Electronegativity o Ionization energy o Metallic and nonmetallic character Review Ions Oxidation
AP Chemistry Ms. Ye Name Date Block Do Now: 1. Complete the table based on the example given Location Element Electron Configuration Metal, Nonmetal or Semi-metal Metalloid)? Group 1, Period 1 Group 11,
The Periodic Table Why is it called a periodic table? The properties of the elements in the table repeat in a "periodic" way (specific pattern). Periodic law: There is a periodic repetition of chemical
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
Periodic Table and Periodicity BHS Chemistry 2013 In 1869, Dmitri Mendeleev, a Russian chemist noticed patterns in certain elements. He discovered a way to arrange the elements so that they were organized
Ch. 5 - The Periodic Table 250 Atomic Radius (pm) 200 150 100 50 0 0 5 10 15 20 Atomic Number III. Periodic Trends (p. 140-154) I II III A. Periodic Law When elements are arranged in order of increasing
Modern Atomic Theory Review of the Discovery of the Atom 1803 John Dalton discovered that elements are made of atoms. He thought that atoms were solid, like a marble. 1875 Crooks discovered the electron.
10/25 Chapter 8: Periodic Relationships Among the Elements Development of the Periodic Table Early chemists: chemical properties related to atomic mass Newlands: Law of octaves >Didn t work past Ca Mendeleev
CHAPTER 6 Elements and the Periodic Table 6.1 The Periodic Table Are you made of star dust? Are you made of star dust? The Big Bang produced hydrogen and helium and a tiny bit of lithium Are you made of
Name: Date: Chemistry ~ Ms. Hart Class: Anions or Cations 4.8 Ions and Ionic Radius Directions: As we watch the video, answer these questions. 1. What is it called when an atom gains or loses an electron?
The Periodic Table Introduction The periodic table is made up of rows of elements and columns. An element is identified by its chemical symbol. The number above the symbol is the atomic number The number
C h e m i s t r y 1 A : C h a p t e r 8 P a g e 1 Chapter 8: Periodic Properties of the Elements Homework: Read Chapter 8. Work out sample/practice exercises Check for the MasteringChemistry.com assignment
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
UNIT 1 ATOMIC STRUCTURE AND THE PERIODIC TABLE PART 2 INTRODUCTION TO THE PERIODIC TABLE Contents 1. The Structure of the Periodic Table 2. Trends in the Periodic Table Key words: group, period, block,
Chapter 7 Electron Configuration and the Periodic Table Copyright McGraw-Hill 2009 1 7.1 Development of the Periodic Table 1864 - John Newlands - Law of Octaves- every 8th element had similar properties
Chapter 7 Electron Configuration and the Periodic Table Copyright McGraw-Hill 2009 1 7.1 Development of the Periodic Table 1864 - John Newlands - Law of Octaves- every 8 th element had similar properties
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
CHEMICAL BONDING Chemical bonds are strong attractive force that exists between the atoms of a substance Chemical Bonds are commonly classified into 3 types: 1. IONIC BONDING Ionic bonds usually form between
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
Periodic Trends: tomic Radius Ionization nergy lectronegativity Metallic haracter Ionic Radius Periodic Trends Five main trends in the periodic table will be discussed: The sizes of atoms Ionization energy
SAMPLE PROBLEMS! 1. From which of the following is it easiest to remove an electron? a. Mg b. Na c. K d. Ca 2. Which of the following influenced your answer to number one the most? a. effective nuclear
Unit 2 Part 2: Periodic Trends Outline Classification of elements using properties Representative elements, transition elements Metals, nonmetals and metalloids Classification of elements using electron
The Periodic Table Beyond protons, neutrons, and electrons It wasn t always like this Early PT Folks n Johann Dobereiner n Triads- groups of 3 with similarities/ trends n Cl, Br, I the properties of Br
Slide 1 / 54 1 Put the following elements in order of increasing atomic size: P, Cs, Sn, F, Sr, Tl Slide 2 / 54 2 Put the following elements in order of increasing atomic size: Ca, Rb, K, O, Al, As Slide
2-1 Unit 2 Periodic Table At the end of this unit, you ll be able to Describe the origin of the periodic table State the modern periodic law Key the periodic table according to metals vs. nonmetals and
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
Why all the repeating Why all the repeating Why all the repeating Why all the repeating Patterns What Patterns have you observed in your life? Where to Get Help If you don t understand concepts in chapter
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
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
Electron Configurations and the Periodic Table The periodic table can be used as a guide for electron configurations. The period number is the value of n. Groups 1A and 2A have the s-orbital filled. Groups
Periodic Table Mendeleev s Table (1871) While it was the first periodic table, Mendeleev had very different elements, such as the very reactive potassium and the very stable copper, in the same family.
Reminder & Announcement Starting the week of October 15 th Group 1 is doing the tutorial on Strong Acids and Bases and Redox. Group 2 is doing the Acid/Base lab. I am away next Monday thru Wednesday. Professor