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Bellwork : Thursday 2/16/2012

Bellwork : Thursday 2/16/2012. Which elements are important for our body/health ? Oxygen, Calcium, Potassium, Iron Which elements are valuable or precious? Gold, Platinum, Silver How do elements get their names?

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Bellwork : Thursday 2/16/2012

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  1. Bellwork: Thursday 2/16/2012 • Which elements are important for our body/health? • Oxygen, Calcium, Potassium, Iron • Which elements are valuable or precious? • Gold, Platinum, Silver • How do elements get their names? • Find at least 3 element names on the periodic table that have names that are odd or recognizable. Where do you think the name came from? • Named after places discovered/created • Germanium- Germany • Berkelium- Berkeley, California • Americium – named after the country America, where the element was created (in Chicago, Illinois) • Europium – named after the continent Europe • Named after famous scientists • Rutherfordium- Ernest Rutherford • Einsteinium- Albert Einstein • Named using words from other languages • Copper (Cu) – “cuprum,” derived from Greek; named after the island in Cyprus in which it was mined • Gold (Au) – “aurum,” derived from Latin; called the solar metal; associated with the Sun (Sol) • Iron (Fe) – “ferrous,” derived from Latin; associated with the celestial body, Mars

  2. Objective 02/11/2013 Page 82 SWBAT recognize the first 20 elements of the periodic table. Jumpstart • 6 protons • 6 electrons • Atomic number: 6 • Carbon • 34 electrons • 34 protons • Atomic number: 34 • Selenium • 29 protons & 35 neutrons • Atomic mass: 64 amu • Copper Find the # of protons, neutrons, electrons, atomic mass, or atomic number when given certain information. • 6 protons • # electrons? • Atomic number? • Element? • 34 electrons • # protons? • Atomic number? • Element? • 29 protons & 35 neutrons • Atomic mass? • Element? • Hints: • # of protons = # of electrons • # of protons = Atomic number • Protons + Neutrons = Atomic Mass

  3. The Periodic Table Notebook Page 83 Packet 9 Page 8

  4. Periodic Table Scavenger Hunt- pg 6 • Periodic Table Scavenger Hunt • Blue Handout • Textbook pages 91-103

  5. Nickel- Ni Tin- Sn Neon- Ne Iron- Fe Mercury- Hg Copper- Cu Periodic Table Scavenger Hunt- pg 6 • O- Oxygen • H- Hydrogen • S- Sulfur • C- Carbon • Co- Cobalt • Cl- Chlorine • Ca- Calcium • He- Helium • Zn- Zinc • Au- Gold • Ag- Silver • N- Nitrogen

  6. Periodic Table Scavenger Hunt- pg 6 • All contain 1, 2, or 3 letters; first one capitalized, second lowercase • Because they can’t all start with the same letter; There are more elements than there are letters in the alphabet! • Groups: • 1- Alkali Metals; • 2- Alkaline Earth Metals; • 3-12- Transition Metals; • 17- Halogens; • 18- Noble Gases • Atomic size/mass INCREASES as you move right. • Atomic size INCREASES as you go down.

  7. Periodic Table Scavenger Hunt- pg 6 • Elements are arranged numerically by their atomic number. • The majority of the elements are METALS. • Mendeleev designed the first periodic table in 1869. • Solve the riddles… • 1st place medal- Gold Au • Bones strong- Calcium Ca • Write on paper- Lead Pb • Worth five, bigger than ten- Nickel Ni

  8. Evolution of the Periodic Table- It’s Elementary- Video 6.34 • The properties of the elements repeat in each period (row) of the table • An element’s properties can be predicted from its location in the periodic table! MAJOR IDEA:

  9. Organizing the Elements: Arrangement of the Periodic Table • Mendeleev: discovered that patterns appeared when the elements were arranged in order of increasingatomic mass. • Sometimes this method didn’t work, so he would put the elements in a “best fit” location. • Mendeleev Song

  10. Organization of the Modern Periodic Table Label these on your blue and white PT! Periods- horizontal rows (1-7)

  11. Groups- vertical columns (1-18) Label these on your blue and white PT!

  12. Modern Periodic Table • Organized based on atomic number(discovered in the 1900’s) rather than atomic mass • British scientist, Henry Mosley, created the modern periodic table of elements • At 27 years old he was killed in WWI What are examples (10!) of some elements that don’t fit Mendeleev’s original model (organized by increasing atomic mass)? Cobalt/Nickel- 27/28 Tellurium/Iodine- 52/53 Argon/Potassium- 18/19 Thorium/Protactinium- 90/92 Uranium/Neptunium- 92/93 Plutonium/Americium- 94/95

  13. February 12, 2013 • Take out Packet 9, Page 7 for corrections • Atom Property’s Quiz

  14. Packet 9, Page 7- Memorization • The 1st 20 Elements to Memorize…and a few more • Fill in the symbols of the missing elements with the correct element and fill in the blanks below the periodic table. These elements are the ones you need to memorize. You should take a few minutes every day to look over them and commit them to memory. • Common Compounds to Memorize • The following is a list of compounds that you need to memorize. You need to know all three columns. • You will be tested on these next week, and will take the test for 3 weeks in a row until you achieve 100% accuracy.

  15. Objective 02/13/2013 No Page SWBAT familiarize themselves with the Periodic Table of Elements by recognizing an element’s different properties .

  16. Extra Credit? • If you can sing this song…in front of the class…then I will give you extra credit….I mean Harry Potter can do it! • Daniel Radcliffe (Harry Potter) Sings Element Song • And yes it has been done, once….!

  17. Page 8- Introduction to the Periodic Table Modern Periodic Table • Period (def) – The horizontal rows; determine the number of orbitals in an atom. • Group (def) – The vertical columns; the number of valence electrons in the atom. 5.6 TSW RECOGNIZE THAT WITHIN A PERIOD ON THE PERIODIC TABLE, THE ATOMIC NUMBER OF ELEMENTS INCREASE BY ONE PROTON GOING FROM LEFT TO RIGHT. • Organized based on atomic number(discovered in the 1900’s) rather than atomic mass • British scientist, Henry Mosley, created the modern periodic table of elements

  18. Patterns in the Periodic Table Valence Electrons (def) – the electrons in the outermost orbital. • The # can vary from 1-8; to be happy, it wants 8**Octet Rule** • True/False. Each element has a typical number of valence electrons. • Important: What is the pattern that exists in the periodic table that predicts the number of valence electrons an atom will have? • It depends on the group number!!!!

  19. Patterns in the Periodic Table • 5.7- TSW RECOGNIZE THAT GROUPS ON THE PERIODIC TABLE CONTAIN ELEMENTS WITH SIMILAR PROPERTIES. • The properties of the elements repeat in each period (row) of the table. • An element’s properties can be predicted from its locationin the periodic table!

  20. Trends in the Periodic Table: Physical Properties of Elements • When elements are arranged in order of increasing atomic number, their physical and chemical properties show a periodic pattern.

  21. Groups in the Periodic Table

  22. Reminders Atomic Number Atomic Mass Sum of the number of protons and neutrons in the nucleus of an atom • Number of protons in the nucleus of an atom • Atoms are neutral • # protons = # electrons • Elements are arranged in Periodic Table according to increasing atomic number

  23. Reading the Periodic Table of the Elements • Each square of the Periodic Table usually includes the element’s name, atomic number, chemical symbol, and atomic mass.

  24. Reading the Periodic Table of the Elements Element’s Name NOTE: They can be organized different ways. What is an easy way to tell the difference between the atomic mass and the atomic number?? Chemical (Atomic) Symbol Atomic Number Atomic Mass

  25. The Periodic Table of Elements CYOPT- Create Your Own Periodic Table… …as well as labeling and taking notes on each group of elements

  26. Create-Your-Own Periodic Table (CYOPT) Atomic number Artificially Made 6 C 12.01 Carbon Radioactive • Fill in the Key at the top for Carbon • Begin filling in the atomic symbol, atomic mass, and atomic number for the elements in group 1 & 2—be sure to use the same order as the key! Chemical symbol Atomic mass Element Name

  27. CYOPT- Structure of the Atom Valence Electron Negatively Charged Outside the Nucleus; in the outside shell Electron Negatively Charged Outside the Nucleus Charge of atom: Neutral Charge of nucleus: Positive Majority of the atom is empty space. Proton Positively Charged Inside the Nucleus Neutron Neutrally Charged Inside the Nucleus

  28. CYOPT- Reading the Periodic Table • Atomic Mass = # of protons + # of neutrons • Atomic Number = # of protons • Organized by increasing atomic number • Valence Electrons • [Sketch Table] • An element’s properties can be predicted from its location in the periodic table • Group/Family = column (up/down) • # of valence electrons • Period = row (left to right) • # of orbitals/shells

  29. Create-Your-Own (CYO) Periodic Table (PT) • Man Made: : ) Radioactive:  • Coloring: Letters: Black (s), Red (g), Blue (l) • Coloring: Outline each in a different color—see my example for help!!

  30. Metals • 75% of elements are metals • Physical properties of metals: • hardness • luster(shininess) • malleability (can be pounded or rolled into shapes or flat sheets) • ductility (can be pulled out or drawn into wires) • Conductors(transmit heat and electricity easily) • Magnetic (attracted to magnets) • ex. iron (Fe), cobalt (Co), and nickel (Ni) • State of Matter- Most metals are solids at room temperature • Melting point- high temperature; except Mercury (Hg)--liquid at room temperature

  31. Group 1: Alkali Metals 1

  32. Group 1: Alkali Metals • Group 1 • 1 valence electron • which it readily loses to become a cation • Extremely reactive – NEVER found alone in nature • Only found in compounds, combined with other elements • Reacts violently with water to produce explosions • Causes skin burns if you come into contact with it • Physical Properties: • Soft- can be cut with a plastic knife • Shiny • Lightweight • Good conductors of electricity and heat • Low melting points • Tarnishes rapidly • Alkali Metals Video (1.30)

  33. Group 2: Alkaline Earth Metals 2

  34. Group 2: Alkaline Earth Metals • Group 2 • 2 valence electrons • 2nd most reactive group of elements in the periodic table • Chemically bond very easily by giving away 2 electrons • Physical Properties: • Fairly hard • bright white • good conductors of electricity • high melting points • high densities • Called Alkaline? When mixed in solutions = pH greater than 7 • Those pH levels are defined as 'basic' or 'alkaline' solutions • Alkaline Metals Video

  35. Groups 3-12: Transition Metals 3 4 5 6 7 8 9 10 11 12

  36. Groups 3-12: Transition Metals • Groups 3-12 • Largest group of elements • Most commonly found • Follows NO rules when finding valence electrons • Use the two outermost shells/orbitals to bond with other elements • Most elements only use the valence shell • Physical Properties: • Hard and shiny • Good conductors of heat & electricity • Are fairly stable, reacting slowly or not at all with air and water • Most have very high melting and boiling points • Most dissolve in acids • Gold Malleability Video • Copper + Zinc = Brass Video • Iron in a Dollar Video

  37. Rare Earth Metals Lanthanides Actinides

  38. Rare Earth Metals: Lanthanides • Top row (Rare Earth Metals) • Fits in period 6 • Named after the first element in the row (Lanthanum) • Physical Properties: • Soft • Malleable • Shiny/high luster • High conductivity • Found naturally on Earth • Only 1 element in the series is radioactive

  39. Rare Earth Metals: Actinides • Bottom row (Rare Earth Metals) • Fits in period 7 • Named after the first element in the row (Actinium) • All are radioactive • Nucleus is very unstable • last for only a fraction of a second after they are made • Some not found in nature • Only thorium and uranium exist on Earth in significant amounts • All the elements after uranium were created artificially in the lab

  40. Other Metals (Metals in Mixed Groups) 13 14 15

  41. Other Metals (Metals in Mixed Groups) • Located in groups 13, 14, 15 • Includes 7 Elements – Al, Ga, In, Sn, Tl, Pb, Bi • Follow “rules” when finding valence electrons • Possess many of the same Physical Properties as the Transition Metals: • Solid & Opaque • Ductile & Malleable • High densities

  42. Metalloids 13 14 15 16

  43. Metalloids • Possess properties of both metals and non-metals • Semi-conductors • Found along the “stair-step” or “ladder” (between metals/non-metals) • Physical Properties: • Solids • Shiny or dull • Will conduct heat and electricity (but not as well as metals) • Metalloids: • Boron • Silicon • Germanium • Arsenic • Antimony • Tellurium • Polonium

  44. Non-Metals 1 18 14 15 16 17

  45. Nonmetals • 17 nonmetals • Found to the right of the “stair step” on the periodic table & Hydrogen • Lack most of the properties of metals • Physical Properties: (most) • Solid nonmetals are brittle (not malleable/ductile) • Poor conductors of heat & electricity • Dull • Chemical Properties: (most) • Form compounds easily • EXCEPT Group 18 (Noble Gases)

  46. Group 17: Halogens 17

  47. Halogens- Group 17 • Group 17 • 7 valence electrons • 1 away from a full shell • Very close to being happy • Combine with many different elements • Often bond with elements from Group One • “Very reactive! – Only need 1 more electron to fulfill the “Octet Rule” • Never found alone in nature • All are poisonous non-metals

  48. Group 18: Noble Gases 18

  49. Noble Gases- Group 18 • Group 18 • Full valence shell • Hydrogen & Helium: full with 2 electrons • Others: full with 8 electrons • Happiest elements of all!! • Will never combine with other elements (too stable) • Colorless, tasteless, odorless gases • When electricity passes through them, they glow different colors

  50. Gas Discharge Spectrum Tubes- Noble Gases • Spectrum tubes contain atoms of gas elements • Energy is supplied through an electric field between electrodes at the ends of the tubes. • In an electric field, a free electron will accelerate away from the negative electrode and toward the positive electrode. • When such an electron collides with a gas molecule in its path, it may transfer some of its energy to the gas molecule, producing a gas molecule in an excited (high-energy) state. e-(high energy) + Hg --> Hg* + e-(lower energy) • In this equation, Hg* represents an atom of mercury in an excited state. • The excited gas molecule does not remain in a high-energy state for long. It can return to its lowest-energy state, the ground state, by emitting its excess energy as light. Hg* --> Hg + light • This is the source of the glow of a discharge tube. The gas emits a characteristic particular color of light. The identity of the gas in the tube determines the color of the glow.

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