1 / 21

PERIODIC TABLE OF ELEMENTS NOTES

PERIODIC TABLE OF ELEMENTS NOTES. Atoms vs. Ions. Atoms = same number P + & E - Ex: (+3) + (-3) = 0 charge is ZERO Ions = same # P + , …but more or less E - Ex: (+3) + (-4) = -1 Ex: (+3) + (-2) = +1 Charge is (+ or -).

torn
Download Presentation

PERIODIC TABLE OF ELEMENTS NOTES

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 OF ELEMENTS NOTES

  2. Atoms vs. Ions • Atoms = same number P+ & E- • Ex: (+3) + (-3) = 0 • charge is ZERO • Ions = same # P+, …but more or less E- • Ex: (+3) + (-4) = -1 • Ex: (+3) + (-2) = +1 • Charge is (+ or -) *sodium ion laser is used to determine the temperature in the mesosphere and the lower thermosphere

  3. Quick Electron Lesson • Electrons are found in the energy levels. • Electrons affect the properties of elements • Remember atoms have a ZERO CHARGE • If an atom has a charge  ONLY affects ELECTRONS • # P+ ≠ #E- • If Positive (+) charge, TAKE AWAY electrons • If Negative (-) charge, ADD ON electrons

  4. Ions: What and Why? • An Ion is an atom with a + or -charge • Cation = ion with + charge • Anion = ion with - charge • Goal: fill outermost shell (Octet Rule) • Ex. Na = 11 electrons (7 more until full shell) • Na+1 = 10 electrons (outermost shell full) • Valence Electrons (outermost shell electrons) are used for bonding

  5. How to organize elements? • Early scientists used the properties of elements to sort them into groups. • Elements are arranged in order of increasing atomic number.

  6. How It Works • Rows (across) = PERIODS • Goes in order of ATOMIC NUMBER • Determines # energy levels • Elements within a period = PROPERTIES CHANGE Periodic law: the pattern of properties within a period repeats as you move from one period to the next

  7. How It Works • Columns (up and down) = GROUPS or FAMILIES • Determines the # valence electrons • Elements within a group = SIMILAR PROPERTIES

  8. 3 Broad Classes of Elements Metals Metalloids Nonmetals “Staircase”

  9. 3 Broad Classes of Elements • Metals: • Good Conductors • High Luster or Sheen (Shiny) • Ductile • Malleable • Nonmetals: (Opposite of metals) • Metalloids: Act as a metal or nonmetal

  10. Metallic Trend • Most metallic elements are Cesium (Cr) and Francium (Fr) In your journal, outline the periodic table and include the trends.

  11. Main Groups • Alkali Metals • Alkaline Metals • Transition Metals • Metalloids • Nonmetals • Halogens • Noble Gasses • Lanthanides • Actinides

  12. Group 1: Alkali Metals“The Gentlemen” • Except Hydrogen • Traits: • 1 valence electron • Lose valence electron +1 charge • VERY REACTIVE • (Almost) always bonds with halogens

  13. Group 7: Halogens “The Ladies” • Common Salts: • Chlorine (Cl) • Bromine (Br) • Iodine (I) • Traits: • 7 valence electrons • Gains 1 valence electrons -1 charge • VERY REACTIVE • Almost awalysbonds with Alkali gentlemen

  14. Why They Make Such a Cute Couple…Reason for Bonding Goal: To settle down Meet the OCTET RULE Valence electrons = bonding Alkali Gentlemen= 1 valence electron Halogen Ladies= 7 valence electrons

  15. In Addition…Charge • No Charge = No Drama! • Alkali (Sodium) = +1 charge • Halogens (Chlorine) = -1 charge • NaCl = (+1) + (-1) = 0

  16. Find a Partner Who… • What charge do alkali metals have? Halogens? • What are valence electrons? • Why do alkali and halogens go so well together (two reasons)?

  17. Group 2: Alkaline Earth Metals “Players” Players: • Traits: • 2 valence electrons • Loses 2 valence electrons +2 charge • (Almost) always bonds with TWO halogensistas OR 1 Group 6 nonmetal

  18. Group 8: Noble Gases“The Snobs” The Snobs: • Traits: • 8 valence electrons (Octet Rule) • NO CHARGE (no drama) •  NOT REACTIVE • Bonds with NO ONE • Too good for anyone else.

  19. In between Groups:Transition Metals • Scandium to Zinc • Zinc to Mercury • Found in middle of table • Ones in each column = similar properties • Different charges • Some are synthetic • Inner Transition Metals • Lanthanides and Actinides • Rare Earth Elements

  20. Elbow Partner • What do metalloids separate (what are the found between)? • Why are the noble gasses “snobs?” • Describe the traits of alkaline earth metals (charge, number of valence electrons).

More Related