E3 Describe the development of the modern periodic table E4 Draw conclusion about the similarities and trends in the properties of elements, with
|
|
- Audrey Lang
- 6 years ago
- Views:
Transcription
1
2 E3 Describe the development of the modern periodic table E4 Draw conclusion about the similarities and trends in the properties of elements, with reference to the periodic table
3 By elements had been discovered. By discovered With 62 elements, scientists decided it was time to organize them. They started with the most obvious property atomic mass but soon realized this didn t work because of isotopes (the mass changed depending on which type of an element was present)
4 Dimitri Mendeleev was one of the first to publish a table. (1869) He used similar chemical properties as well as atomic mass to arrange the elements. (Ie some were solids, some very reactive, some high melting points, some very brittle, etc ) He noticed that when elements are listed according to their mass certain properties occur periodically (so in certain vertical families they all seem to have similar properties )
5 As more data became available we actually changed the table to increasing atomic number, which made the whole table make sense!!! (Isotopes no longer caused a problem to the pattern!) The PERIODIC LAW summarizes the organization of the periodic table: When elements are arranged in order of increasing atomic number, their properties are repeated periodically. Henry Mosely came up with the concept of atomic number.
6 Period- a horizontal row on the periodic table Sodium (Na) Family Name: Alkali metals Family #: 1 Group #: 3 How many elements in the 6 th period? 36
7 Families (a.k.a. Groups)- vertical columns on the periodic table in which elements have similar properties and chemical reactivity (because of similar electron configurations in the outermost energy levels (ie. Valence shells p-orbitals) Stability is achieved by having a full outer valence shell (full p or s-orbital), or even half full.
8 How many families on the periodic table? There are 18 families on the periodic table Interesting pattern: The last digit of the family # indicates how many valence e- there are in all elements in that family (works for Families 1-2, 13-18) How many e- would family 17 like to gain or lose? Family 2??
9
10 H = 1s 1 Li = [He]2s 1 Na = [Ne]3s 1 K = [Ar]4s 1 Rb = [Kr]5s 1 Cs = [Xe]6s 1 All elements in the same family end with the same valence configuration. (in this case 1s 1 ), same # of valence e-. Also, notice that the principle quantum number of the s orbital is the same as the period #
11 Because they have the same number of valence e-. And we know that it is the valence e- that are responsible for the way elements interact!
12 Metals (to the left of the staircase line ) Non-metals (to the right of the staircase line ) Metalloids/semi-metals/Semiconductors, along the staircase line (the line between metals and non-metals starts under Boron) Metalloids have properties of both metals and non-metals. The properties of elements change from metallic to non-metallic going from left to right across the table * Elements become more metallic going down a family in the periodic table
13
14 Recall: Properties of metals versus non-metals: Metals - Have a metallic shine/ luster - Usually solid at room temperature - Are malleable (don t shatter) - Are ductile (can be formed into sheets or wires) - Are good conductors of electricity Non-metals - Usually have a dull appearance/ lack luster - Usually gases at room temperature - Are brittle solids (i.e. are not malleable) - Are not ductile Do not conduct electricity
15 Increasing Metallic character Increasing Metallic character LEAST METALLIC MOST METALLIC
16 Include Li, Na, K, Rb, Cs, Fr most chemically reactive of the metals (must be stored under oil as they will react with air) react explosively with water
17
18 Includes Be, Ca, Mg, etc. very chemically reactive and are never found free in nature (same as alkali metals)
19 are highly reactive with metals, especially alkali metals highly toxic
20 Include He, Ne, Xe, etc EXTREMELY STABLE and only rarely react to form compounds (because of their full valence shell) All other elements want to be like these ones, and they will lose or gain electrons to become iso-electric (having some electron composition) as them. all are gases when given energy (with electricity or extreme heat) each gives off a unique color
21
22 Energy Levels So Li, Be, B, C, N, O, F, Ne are all in the same energy level, n=2, and as you move across from left to right, there are more e-)
23 Pretty Protons Excited Electrons
24 If there are more Pretty p+ in the nucleus, do you think they would have a greater pull on the exited e- who were all the same distance away? Heck yes! If there were a lot of e-(all at different distances) around the p+, would the outer e- be pulled in by the protons to the same extent as the ones that are closer? Out of sight out of mind??
25 Going across the row or period, the atomic size/radius decreases. Why do you think? This is because: e - and p+ are being added to the same energy level (same distance from the nucleus) which means more attractive forces between them (the p+ in the nucleus are pulling e- more strongly into the center because there are more of them and the e- are still at some distance away).
26 Pretty Protons Excited Electrons
27 Going down a group or family, the atomic size increases. Why? This is because: e - are being added to E.L. further away from the p+ in the nucleus. The p+ are not as close to all the e- anymore, and therefore don t exert as much pull on them. More e - means more e - repulsion between them. More e - shielding of the outer e - from the nucleus by the inner e -. Basically, you are adding more energy levels, and therefore the atom gets bigger!
28 The middle electrons (electrons in the energy levels between the nucleus and the valence electrons) are called the Shielding electrons, they "shield" the valence electrons from the force of attraction exerted by the positive charge of the p+ in the nucleus.
29 Excited Electrons are in each other s way (e- shielding= there s a lot of e- between the p+ and the outside e-. Likes repel, so there is more repulsion of e- than pulling by p+ outside e- are not being pulled in as much!! Pretty Protons
30
31 The smaller an atom is, the closer the p+ are to the valence e- and therefore, the e- are held more tightly by the force of attraction so it take a lot of energy to remove e- in smaller atoms. If the atom is larger, the nucleus is farther from the valence e-, and therefore they are held less tightly, so it is easier to remove e- from larger atoms.
32
33 Metallic ions, which are positive, lose electrons, so they are smaller than their atom forms. A) This is because the ions have more protons than electrons, which exert a stronger pull on the outer electrons. B) They might also lose an energy level (making it smaller)
34 For non-metallic ions, which are negative, the opposite is true(they gain more e-) The non-metallic ions are larger than their atoms because there are more electrons being added than protons so there is less attraction and more electron repulsion.
35 Going across a period, the ionization energy increases because: The atoms get smaller as you go across (attractive forces are greater within the atom), therefore, it s harder to pull the electrons away so more energy is needed to do that. Metallic nature of elements (Ability to Give up e-) decreases as you go across! Because the additional protons in the nucleus attract the e-, they cause the electrons to be less readily released.
36 Going down a group ionization energy decreases because: The atom gets bigger as you go down, so the electrons are further away from nucleus and not held tightly so they are easier to steal! Metallic nature increases! (e- are further away from the nucleus, and can be more easily removed) There is more electron repulsion between the e-, There is more electron shielding
37 Down a family more energy levels further from nucleus Electron shielding and repulsion!! Pretty Protons Low ionization energy won t take much to steal that valence e-!!!
38 In general ionization energy increases; as you go across a period, and decreases as you go down a family. There is a slight decrease in ionization energy for which a loss of an electron produces a full or half full orbital (because of their additional stability). Notice: The greatest ionization energies for a period are for the noble gases (they are VERY unreactive and do not want to lose an electron.
39
40 1 st Ionization energy means energy needed to remove 1 electron 2 nd Ionization energy means energy needed to remove a second electron 3 rd Ionization energy means energy needed to remove a third electron
41 Note: Which tend to attract/take electrons? Metals or Non-metals? NON-METALS!!! Elements get more non-metallic as you go across the table. As the atomic radius decreases, the protons pull electrons in more strongly (more + s pulling s) So as the radius gets smaller the tendency to pull in other e- increases. So going across the periodic table Electronegativity INCREASES!! (see the back of your periodic table)
42 Electronegativity (ability to attract e- to itself) Decreases as you move down the families, the atomic radius is increasing (atom getting bigger and not holding the e- so tightly), there is not a great tendency to pull in other e-.
43 Electronegativity
44 As you become more non-metallic your affinity for an e- increases. (non-metals are takers). If you are a metal you don t want extra e-, so your affinity is typically low. So in general, the affinity increases across a period, and decreases down a family.
45 Electronegativity
46 True or False Elements in the same family have similar properties? True! Elements in the same family will react in the same way? True! Why do they react the same way? Same # of valence e-!!
47 If Mg reacts with Cl - what will the formula be? MgCl 2 So then what will the formula be of Ca and Br (without doing any work?) CaCl 2 What about Ba and F? BaF 2 See the pattern!?
48 If Ca binds with P to form Ca 3 P 2 Predict the formula for Sr bonding with N? Sr 3 N 2 So the big idea is elements in the same family will make the same compounds because of their similar valence e-!!!
[3.4] The Periodic Table and Periodic Trends
[3.4] The Periodic Table and Periodic Trends Father of the Periodic Table Dmitri Mendeleev: Scientist who did a lot of work in the development of the modern periodic table Early periodic tables were arranged
More informationChapter 6 The Periodic Table The how and why History. Mendeleev s Table
Chapter 6 The Periodic Table The how and why History 1829 German J. W. Dobereiner grouped elements into triads Three elements with similar properties Properties followed a pattern The same element was
More informationUnit 5. The Periodic Table
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.
More information2. Why do all elements want to obtain a noble gas electron configuration?
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,
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 informationChapter 6 The Periodic Table
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
More informationPeriodic Table Trends. Atomic Radius Ionic Radius Ionization Energy Electronegativity
Periodic Table Trends Atomic Radius Ionic Radius Ionization Energy Electronegativity 1. Atomic Radius Atomic Radius - distance from nucleus to outermost atom Measured by dividing the distance between 2
More informationChapter 6 - The Periodic Table and Periodic Law
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
More informationPeriods: horizontal rows (# 1-7) 2. Periodicity the of the elements in the same group is explained by the arrangement of the around the nucleus.
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
More informationThe Periodic Table and Periodic Trends
The Periodic Table and Periodic Trends The properties of the elements exhibit trends and these trends can be predicted with the help of the periodic table. They can also be explained and understood by
More information7. What is the likeliest oxidation number of an element located in Period 3 and Group 16? a. +2 b. +3 c. -3 d The amount of energy required to
1. Which of the following is the most important factor in determining the properties of an element? a. Atomic mass b. Atomic radius c. Periodic table position d. Electron configuration 2. Similar properties
More informationRegents Chemistry PRACTICE PACKET
*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
More informationCHAPTER 5 THE PERIODIC LAW. What types of useful information can you find on the Periodic Table?
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.
More informationRegents Chemistry Unit 2 The Periodic Table Text Chapter 5
Regents Chemistry Unit 2 The Periodic Table Text Chapter 5 I. Historical Development of the Periodic Table Stanislao Cannizzarro- In1860 presented a convincing method for accurately measuring relative
More informationChapter #2 The Periodic Table
Chapter #2 The Periodic Table Mendeleeve (1834 1907), arranged the elements within a group in order of their atomic mass. He noted repeating patterns in their physical and chemical properties Periodic
More informationPeriodic Trends. Elemental Properties and Patterns
Periodic Trends Elemental Properties and Patterns The Periodic Law Dimitri Mendeleev was the first scientist to publish an organized periodic table of the known elements. He was perpetually in trouble
More informationPeriodic Trends. Elemental Properties and Patterns
Periodic Trends Elemental Properties and Patterns History of the Periodic Table 1871 Mendeleev arranged the elements according to: Increasing atomic mass Elements w/ similar properties were put in the
More informationChemical Periodicity. Periodic Table
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
More informationPeriodic Table of Elements
Name: Periodic Table of Elements Block: The periodic table is a scientific work of art, hidden within it are multiple trends, groups, families, and patterns It took a few tries to get to this current masterpiece
More informationThe Periodic Law Notes (Chapter 5)
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.
More informationThe Periodic Table. Beyond protons, neutrons, and electrons
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
More informationA few elements, including copper, silver, and gold, have been known for thousands of years
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
More informationPeriodic Table and Periodicity. BHS Chemistry 2013
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
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 informationMr. Dolgos Regents Chemistry PRACTICE PACKET. Unit 3: Periodic Table
*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
More informationUNIT 5 THE PERIODIC TABLE
UNIT 5 THE PERIODIC TABLE THE PERIODIC TABLE EARLY ATTEMPTS OF CLASSIFICATION Many chemists started to organize and classify the elements according to their properties. In the 1790s, Antoine LaVoisier
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. 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 informationThe Periodic Table. Chapter 5. I. History II. Organization III. Periodic Trends
The Periodic Table Chapter 5 I. History II. Organization III. Periodic Trends I. History P. 101-103 5a: The Periodic Table Material in chapter 5 is critical to understanding chapter 6! Early Organization
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 informationGetting to know the Periodic Table: Recall: Elements are organized based on atomic number and similar properties
Getting to know the Periodic Table: Recall: Elements are organized based on atomic number and similar properties 1. Find your staircase on the right side of the periodic table. Feel free to make the lines
More informationSAMPLE PROBLEMS! 1. From which of the following is it easiest to remove an electron? a. Mg b. Na c. K d. Ca
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
More informationHydrogen (H) Nonmetal (none)
Honors Chemistry Ms. Ye Name Date Block Do Now: 1. Complete the table based on the example given Location Element Metal, Nonmetal or Group/Family Name Semi-metal (Metalloid)? Group 1, Period 1 Hydrogen
More informationIntroduction: Periodic Table of Elements. Introduction: Valence Electrons: 3/30/2014
Introduction: Periodic Table of Elements Science Links 2013-2014 The periodic table arranges information in a logical way. The columns of elements are called groups or families. Elements in the same family
More informationElectron Configuration and Periodic Trends - Chapter 5 section 3 Guided Notes
Electron Configuration and Periodic Trends - Chapter 5 section 3 Guided Notes There are several important atomic characteristics that show predictable that you should know. Atomic Radius The first and
More informationUnit 2 Periodic Table
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
More informationnumber. Z eff = Z S S is called the screening constant which represents the portion of the nuclear EXTRA NOTES
EXTRA NOTES 1. Development of the Periodic Table The periodic table is the most significant tool that chemists use for organising and recalling chemical facts. Elements in the same column contain the same
More informationChapter 5 Notes Chemistry; The Periodic Law The Periodic Table The periodic table is used to organize the elements in a meaningful way.
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
More informationChemistry B11 Chapter 3 Atoms
Chapter 3 Atoms Element: is a substance that consists of identical atoms (hydrogen, oxygen, and Iron). 116 elements are known (88 occur in nature and chemist have made the others in the lab). Compound:
More informationDiscovery of Elements. Dmitri Mendeleev Stanislao Canizzaro (1860) Modern Periodic Table. Henry Moseley. PT Background Information
Discovery of Elements Development of the Periodic Table Chapter 5 Honors Chemistry 412 At the end of the 1700 s, only 30 elements had been isolated Included most currency metals and some nonmetals New
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 informationChapter 5 Trends of the Periodic Table Diary
Chapter 5 Trends of the Periodic Table Diary A Brief History of the Periodic Table I began to look about and write down the elements with their atomic weights and typical properties, analogous elements
More informationThe Periodic Table. Unit 4
The Periodic Table Unit 4 I. History A. Dmitir Mendeleev Russian chemist, 19th century Arranged elements by their properties Arranged by increasing atomic mass Groups: vertical groups-elements have similar
More informationMendeleev s Table (1871) While it was the first periodic table, Mendeleev had very different elements, such as the very reactive potassium and the
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.
More informationShapes of the orbitals
Electrons Review and Periodic Table Trends Unit 7 Electrons Shapes of the orbitals Electron Configuration Electrons spin in opposite direction Background Electrons can jump between shells (Bohr s model
More informationChapter 7. Periodic Properties of the Elements. Lecture Outline
Chapter 7. Periodic Properties of the Elements Periodic Properties of the Elements 1 Lecture Outline 7.1 Development of the Periodic Table The periodic table is the most significant tool that chemists
More informationUnit 7:Periodic Table Notes. Essential Question: Describe the differences between nonmetals, metalloids and metals.
Unit 7:Periodic Table Notes Essential Question: Describe the differences between nonmetals, metalloids and metals. 1 Red stair step line separates metals from nonmetals Groups/families vertical Have similar
More informationDobereiner developed concept of Triads (groups of 3 elements with similar chemical properties) Average of 1st and 3rd
Unit Early 800's Dobereiner developed concept of Triads (groups of elements with similar chemical properties) atomic mass atomic mass Ca 0. S. Sr Average of st and rd Se Ba 7. Te 7. *useful for predicting
More informationPeriodic Trends. 1. Why is it difficult to measure the size of an atom? 2. What does the term atomic radius mean? 3. What is ionization energy?
Periodic Trends 1. Why is it difficult to measure the size of an atom? 2. What does the term atomic radius mean? 3. What is ionization energy? 4. What periodic trends exist for ionization energy? 5. What
More informationPeriodic Trends. More than 20 properties change in predictable way based location of elements on PT
Periodic Trends Periodic Trends More than 20 properties change in predictable way based location of elements on PT Some properties: Density Melting point/boiling point Atomic radius Ionization energy Electronegativity
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 informationDevelopment of the Periodic Table
Development of the Periodic Table John Newlands - Law of Octaves 1864 When arranged in order of atomic mass, every eighth element had similar properties. Dimitri Mendeleev / Lothar Meyer 1869 organized
More informationHistory of The Periodic Table
History of The Periodic Table Organizing the Elements Chemists used the properties of elements to sort them into groups. JW. Dobreiner grouped elements into triads. A triad is a set of three elements with
More informationTrends in the Periodic Table
Trends in the Periodic Table OBJECTIVES FOR TODAY: Fall in love with the Periodic Table, Interpret group and period trends in atomic radii, ionization energies and electronegativity The Periodic Table
More informationTHE PERIODIC TABLE. Is an arrangement of elements in which the elements are separated into groups based on a set of repeating properties
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
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 informationPERIODIC PROPERTIES OF THE ELEMENTS
PERIODIC PROPERTIES OF THE ELEMENTS DEVELOPMENT OF PERIODIC TABLE Elements in the same group generally have similar chemical properties. Properties are not identical, however. DEVELOPMENT OF PERIODIC TABLE
More informationChapter 8. Periodic Properties of the Element
Chapter 8 Periodic Properties of the Element Mendeleev (1834 1907) Ordered elements by atomic mass Saw a repeating pattern of properties Periodic law when the elements are arranged in order of increasing
More informationPeriodicity SL (answers) IB CHEMISTRY SL
(answers) IB CHEMISTRY SL Syllabus objectives 3.1 Periodic table Understandings: The periodic table is arranged into four blocks associated with the four sublevels s, p, d, and f. The periodic table consists
More informationPeriodic Table. Metalloids diagonal between metals and nonmetals. Have metallic and non-metallic properties
Chapter 6 Periodic Table Most elements are metals Metals are shiny, malleable, ductile, and good conductors of heat and electricity Most metals are solid at room temperature Non-metals in upper right corner,
More informationSCH3U- R. H. KING ACADEMY ATOMIC STRUCTURE HANDOUT NAME:
Particle Theory of Matter Matter is anything that has and takes up. All matter is made up of very small. Each pure substance has its of particle, from the particles of other pure substances. Particles
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 informationExplaining Periodic Trends
Explaining Periodic Trends! Many observable trends in the chemical and physical properties of elements are observable in the periodic table.! On trends you may be familiar with is reactivity, which is
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 9: Elements are the Building blocks of Life
Chapter 9: Elements are the Building blocks of Life Section 9.1- Elements and the Periodic Table Keep Scale in mind Animation: http://htwins.net/scale2/ I. ELEMENTS All matter is made up of one or more
More informationName: Date: Blk: Examine your periodic table to answer these questions and fill-in-the-blanks. Use drawings to support your answers where needed:
Name: Date: Blk: NOTES: PERIODIC TRENDS Examine your periodic table to answer these questions and fill-in-the-blanks. Use drawings to support your answers where needed: I. ATOMIC RADIUS (Size) Going from
More informationHonors Chemistry Unit 4 ( )
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
More informationPeriodic Trends. Elemental Properties and Patterns
Periodic Trends Elemental Properties and Patterns The Periodic Law Dimitri Mendeleev was the first scientist to publish an organized periodic table of the known elements. Henry Moseley Discovered the proton
More informationGroup Trends: the trend that the atoms follow going down any particular group
Trends of the Periodic Table Basics Trends are patterns of behaviors that atoms on the periodic table of elements follow. Trends hold true most of the time, but there are exceptions, or blips, where the
More informationLecture Presentation. Chapter 8. Periodic Properties of the Element. Sherril Soman Grand Valley State University Pearson Education, Inc.
Lecture Presentation Chapter 8 Periodic Properties of the Element Sherril Soman Grand Valley State University Nerve Transmission Movement of ions across cell membranes is the basis for the transmission
More informationChapter 8: Periodic Properties of the Elements
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
More informationChemical symbols. Know names and symbols of elements #1 30, plus. Rb, Cs, Sr, Ba, Ag, Au, Cd, Hg, Pt, Ga, Ge, As, Sn, Pb, Se, Br, I, and U
Chemical symbols Know names and symbols of elements #1 30, plus Rb, Cs, Sr, Ba, Ag, Au, Cd, Hg, Pt, Ga, Ge, As, Sn, Pb, Se, Br, I, and U Coulomb s Law F = attractive/repulsive force Q 1, Q 2 = charges
More informationCh 7: Periodic Properties of the Elements
AP Chemistry: Periodic Properties of the Elements Lecture Outline 7.1 Development of the Periodic Table The majority of the elements were discovered between 1735 and 1843. Discovery of new elements in
More informationCh. 4 Sec. 1-2, Ch. 3 sec.6-8 ENERGY CHANGES AND THE QUANTUM THEORY THE PERIODIC TABLE
Ch. 4 Sec. 1-2, Ch. 3 sec.6-8 ENERGY CHANGES AND THE QUANTUM THEORY THE PERIODIC TABLE What Makes Red Light Red? (4.1) Electromagnetic Radiation: energy that travels in waves (light) Waves Amplitude: height
More informationPowerPoint to accompany. Chapter 6. Periodic Properties of the Elements
PowerPoint to accompany Chapter 6 Periodic Properties of the Elements Development of the Periodic Table Elements in the same group generally have similar chemical properties. Properties are not identical,
More informationUnit 4: The Periodic Table Text Questions from Corwin
Unit 4: The Periodic Table Name: KEY Text Questions from Corwin 4.4 1. List five properties of metals. solid, has luster, highly dense, has high melting point, and is a good conductor of heat and electricity
More informationChapter 4. Periodic Trends of the Elements. Chemistry: Atoms First Second Edition Julia Burdge & Jason Overby
Chemistry: Atoms First Second Edition Julia Burdge & Jason Overby Chapter 4 Periodic Trends of the Elements M. Stacey Thomson Pasco-Hernando State College Copyright (c) The McGraw-Hill Companies, Inc.
More informationFor the Periodic Table above indicate each of the following TRENDS: atomic size and ionic size. Na Na + F F - Ne < < < <
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 +
More informationChapter 7 Electron Configuration and the Periodic Table
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
More information1869 Mendeleev: method of organizing the elements according to both their masses and their properties. The Old Table
The Periodic Table 1869 Mendeleev: method of organizing the elements according to both their masses and their properties. The Old Table Vertical Columns: Elements arranged in groups each group shares similar
More informationIntroduction period group
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
More informationPeriodic Nomenclature Columns are called groups or families o 18 columns in standard periodic table o Traditionally numbered I-VIII, followed by A or
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
More informationRegents Chemistry NOTE PACKET. Unit 3: Periodic Table
*STUDENT* *STUDENT* Regents Chemistry NOTE PACKET Unit 3: Periodic Table 1 *STUDENT* Unit 3 - The Periodic Table *STUDENT* VOCABULARY: Ionization energy Electronegativity Atomic Radius Ionic Radius Chemical
More informationTHE PERIODIC TABLE & PERIODIC LAW! Development of the Modern Periodic Table!
THE PERIODIC TABLE & PERIODIC LAW! Development of the Modern Periodic Table! Development of the Periodic Table! Main Idea: The periodic table evolved over time as scientists discovered more useful ways
More informationUnit 3 - The Periodic Table
Unit 3 - The Periodic Table Unit Objectives - At the completion of this unit you will be able to: Describe the origin of the periodic table State the modern periodic law Explain how an element s electron
More informationCh. 7- Periodic Properties of the Elements
Ch. 7- Periodic Properties of the Elements 7.1 Introduction A. The periodic nature of the periodic table arises from repeating patterns in the electron configurations of the elements. B. Elements in the
More informationPERIODIC TRENDS AND THE PERIODIC TABLE
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
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 informationChapter 6: Periodic Trends
Chapter 6: Periodic Trends Development of the Periodic Table Dmitri Mendeleev designed the first periodic table in 1869 by grouping elements with similar chemical & physical properties in rows according
More informationChapter 7 Electron Configuration and the Periodic Table
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
More informationHonors Chemistry. If an element has a LOW ionization energy, what does that tell you about its tendency to lose electrons?
Do Now: Location on Periodic Table Lose or Gain electrons to obtain noble gas electron configuration? Form cations or anions? Relative ionization energy Relative electronegativity Metals Nonmetals If an
More informationPeriodic Properties of the Elements
Chapter 7 Periodic Properties of the Elements DEVELOPMENT OF THE PERIODIC TABLE Elements in the same group generally have similar chemical properties. Properties are not identical, however. Brown, LeMay,
More informationChapter 5 The Periodic Law
z Chapter 5 The Periodic Law z Section 5-1 History of the Periodic Table Mendeleev noticed that when the elements were arranged in order of increasing atomic mass, certain similarities in their chemical
More informationElectron Configurations and the Periodic Table
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
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 informationChapter 7 Periodic Properties of the Elements
Chapter 7 Periodic Properties of the Elements Development of Periodic Table Elements in the same group generally have similar chemical properties. Properties are not identical, however. Development of
More informationUnit 4: The Periodic Table
Unit 4 Periodic Table Notes (filled in).notebook Unit 4: The Periodic Table Review Book: Topic 2 Textbook: Ch. 5 & 14 What is an example of something that is "periodic"? school schedule, sunrise/sunset
More informationTrends in the Periodic Table
Trends in the Periodic Table A trend is a predictable change in a particular direction. Example: There is a trend in the alkali metals to increase in reactivity as you move down a group. Atomic Radius
More informationAssessment Chapter 5 Pre-Test Chapter: The Periodic Law Use the periodic table below to answer the questions in this Chapter Test.
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
More informationPeriodic classification of elements
Periodic classification of elements Elements are classified on the basis of similarities in their properties. Classification makes the study of elements easier and systematic. 1817: Law of triads (Johann
More information