1 / 31

Periodic Table

Periodic Table. Dmitri Mendeleev organized the known elements into a table called the periodic table. He organized them by their increasing atomic masses. Today we organize the elements by their increasing Atomic Number. Insert copy of the periodic table.

julianna-larya
Download Presentation

Periodic Table

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Periodic Table

  2. DmitriMendeleevorganized the known elements into a table called the periodic table. He organized them by their increasing atomic masses.

  3. Today we organize theelementsby their increasingAtomicNumber.

  4. Insert copy of the periodic table.

  5. Rows on the periodic table are called periods. All the elements listed in a row belong to the same period. There are 7 (seven) periods.

  6. Columns in the periodic table are called groups or families. All elements in a group have similar properties.

  7. Insert copy of the periodic table. The columns have been given an Arabic number. The columns are numbered 1 – 18 starting at the left and moving to the right. Please make sure that your periodic table has them numbered like this.

  8. Valence Electrons The outer most energy level is usually not full or complete . These electrons in the outer energy level are called Valenceelectrons. Valence electrons are important because they determine how an element will react with other substance.

  9. Insert picture of periodic table. Group 1 and 2 the number of Valence electrons in the outer energy level willmatchthe group number.

  10. Insert picture of periodic table. Groups 3 through 12 do not follow any particular rule to determine the number of Valence electrons.

  11. Insert picture of periodic table. Group 13 to 18 – The Valence electrons for each of these is the group number less10.For example Group 14 –10= 4 Valence electrons.

  12. Elements whose atoms gain, lose or shareelectrons are reactive and they combine to form the many compounds we use in our daily lives.

  13. Elements are categorized as metals, nonmetals or metalloids. Metals: Anelementthat has luster, ismalleableandductile, and is said to be a good conductor of heat andelectricity.

  14. What is luster, malleable and ductile? Luster describes the way a surface reflects light…therefore metallic luster would be shiny like a metal object. Malleable means to be able to press or pound the substance into sheets or different shapes. Ductile means that the substance can be drawn out into thin wires.

  15. Elements are categorized as metals, nonmetals or metalloids (cont’). Nonmetals: an element that is usually agasor abrittlesolid at room temperature. It is a poor conductor of heat andelectricity.

  16. Elements are categorized as metals, nonmetals or metalloids (cont’). Metalloid: an element thatsharessome characteristics or properties with bothmetalsand nonmetals.

  17. Group 1 and 2 Elements: These elements are so reactive that they are only found combined with other elements in nature.

  18. Group 1: Alkali Metals • Soft – can be cut with a knife • Shiny andsilver colored • LowDensity (some will even float) • Mostreactiveof the metals • Valence electrons = 1 • Reactsviolentlywith water forming a hydrogen gas • Compounds from these are very useful such as NaCl

  19. Group 2:Alkaline- Earth Metals • Very reactivebut not as reactive as Alkali Metals. • Silver colored • Moredensethan Group 1 metals • Valence electrons =2 • Useful compounds include: Calcium compounds such as cement, plaster, chalk, and YOU.

  20. Group 3 to 12:TransitionMetals • Do not lose their valenceelectrons as easily as groups 1 & 2. • Less reactive thanAlkaliandAlkalineEarth metals • Shiny • Goodconductorsof electricity • Higherdensity and melting points (except mercury) than Group 1 and 2

  21. Group 3 to 12: Transition Metals (cont’.) • Lanthanides: The first row underneath the periodic table: Shiny, reactive, many are used in the production of steel. • Actinides: The second row underneath the periodic table: These elements are allradioactiveand unstable.. Note: Elements found after 94 (Plutonium) are man made and not found in nature

  22. Group 13:BoronGroup • Reactive • Valence electrons = 3 • Contains1Metalloid and4Metals • Solidat room temperature • Aluminumis the most abundant in this group and the most common in the Earth’s crust

  23. Group 14:Carbon Group • Reactivityvariesin this group depending on the element • Valence electrons =4 • This group contains2metals, 1nonmetal and2metalloids. • Many forms founduncombinedin nature such as diamonds • Compounds are very useful:proteins, fats, carbohydrates, computer chips.

  24. Group 15:Nitrogen Group • Reactivityvariesin this group depending on the element • Valence electrons =5 • Group contains1metal, 2Nonmetals, and2metalloids • Phosphorous is veryreactiveand only found in naturecombinedwith other elements. • All butnitrogenare solid at room temperature. • Nitrogen makes up78%of our atmosphere. • Generallyunreactive.

  25. Group 16: Oxygen Group • More reactivethan group 15 • Valence electrons =6 • Group contains1Metals, 3Nonmetals and1Metalloids • Sulfur is found in nature and is used to makesulfuricacid, a very commonly used chemical in industry. • All butoxygenare solid at room temperature. • Oxygen makes up21%of the Earth’s Atmosphere • Oxygen is very reactive and combines with many other elements especially metals • Rustis the result of the oxidation of metal.

  26. Group 17:Halogen Group • Veryreactive • Valence electrons = 7 • Nonmetal group • PoorConductors of electricity and heat • Reactviolently with alkali metals to form salts • Never founduncombinedin nature • Atoms of these elements only need to gain 1 electron to fill their outer shell • Chlorine andIodineare both in this group and can be combined to make disinfectants.

  27. Group 18:Noble Gas Group • Non-reactant • Valence electrons =8 • Outermostenergy shell is full • Colorless, odorlessgases at room temp. • Under normal conditions they do notreactwith other elements • All found on Earth in very small amounts • Argonis the most common in the group • Their non-reactivity makes them very useful forlightbulbs, helium for blimps andweatherballoons.

  28. Hydrogen Stands Alone: • Properties do not match the properties of any single group • Valence Electrons = 1 • Easily looses that one valence electron • Physical properties are like the nonmetal group • Most abundant element in the Universe • Its reactive nature makes it useful as a fuel for rockets.

  29. Insert picture of periodic table.

More Related