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Agenda: 3/10

Agenda: 3/10. To predict properties of an element using Periodic Trends (Reactivity and Bonding) Warm-up: Reviewing trends: sketch PT showing trends Predicting properties based on trends Practice Video Using Electronegativity to determine type of bonds .

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Agenda: 3/10

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  1. Agenda: 3/10 • To predict properties of an element using Periodic Trends (Reactivity and Bonding) • Warm-up: Reviewing trends: sketch PT showing trends • Predicting properties based on trends • Practice • Video • Using Electronegativity to determine type of bonds

  2. What are the Trends on the Periodic Table? Label the trends Increases Decreases Periodic Table Increases Decreases

  3. Predicting Properties of Elements - based on the position on the Periodic Table : Size; IE; EN Property: which element has the largest value? Ca vs. Br C vs. SnF vs. I Si vs. Cl Na vs. P Li vs. K Be vs. O S vs. Ar Al vs. S Ne vs. Kr B vs. Al B vs. Ne

  4. Predicting Properties of Elements - based on the position on the Periodic Table : Size; IE; EN Property: which element has the largest value? Ca vs. Br C vs. SnF vs. I Si vs. Cl Na vs. P Li vs. K Be vs. O S vs. Ar Al vs. S Ne vs. Kr B vs. Al B vs. Ne

  5. Predicting Properties of Elements - based on the position on the Periodic Table : Size; IE; EN Property: which element has the largest value? Ca vs. Br C vs. SnF vs. I Si vs. Cl Na vs. P Li vs. K Be vs. O S vs. Ar Al vs. S Ne vs. Kr B vs. Al B vs. Ne

  6. Predicting Properties using the PT • How does the organization of the Periodic Table help us make predictions? • https://www.teachingchannel.org/videos/periodic-table • 14 minutes • Starts with low reactivity metals: copper, silver & gold • Very reactive metals • Non-metals

  7. Compounds & Bonds – Unit 5 Why do atoms bond to form compounds? How are bonds formed? How do we represent compounds (names and formulas)?

  8. Chemical Bonds • Review sources • http://bcs.whfreeman.com/thelifewire/content/chp02/02020.html • http://www.sciencegeek.net/Chemistry/taters/directory.shtml • http://ed.ted.com/lessons/the-science-of-macaroni-salad-what-s-in-a-mixture-josh-kurz

  9. Bonding Essentials • Bonds are formed when valence electrons are gained, lost or shared by atoms • There are 3 major types of bonds • Ionic, Covalent, Metallic • Compounds are 2 or more atoms bonded together, with different properties than their elements.

  10. Metals and Non-metals Act Differently

  11. Atomic Theater • Demonstrating bonding • Ionic – 2 students • Covalent – 2 students • Metallic – 4 students

  12. Chemical Bonds • http://ed.ted.com/lessons/how-atoms-bond-george-zaidan-and-charles-morton

  13. Electronegativity • Ability of an atom in a compound to attract electrons from another atom. • Difference between electronegativity of atoms is used to determine the bond type.

  14. Electronegativity Differences • Electronegativity Differences = ∆EN O 3.2

  15. Determining bond type Determine the absolute difference (either + or -) Type? O ___ - N____= _____ O ___ - O____=_____ O ___ - H____=_____ F____- Li ____=_____

  16. Periodic Table with Electronegativities Electronegativity Values for Elements Circle elements with highest & lowest value & label. Show trends for EN using arrows.

  17. Electronegativity Learning Guide • Determine absolute differences • Classify each bonding pair of elements as: • Ionic • Covalent • If covalent, determine if the bond is: non-polar (∆ 0 – 0.3) or polar (∆0.4 – 1.7)

  18. Types of Bonds Ionic Covalent Metallic

  19. Ionic Bond • Ionic Bond: formed with Bonds a __________ with a ____________ Valence electrons are ________________ from the ___________ to the __________. Therefore, when the valence electron(s) are transferred to the ____-______, the NM become _______ charged (a ________).

  20. Ionic Bond∆EN = 1.8 – 3.2

  21. Ionic bonds • The electronegativity difference must be equal to or greater than __________. • Ionic bonds look like: • Na Cl

  22. Opposite charges attract= electrostatic attraction Like the attraction of magnets Formula unit

  23. Ionic compounds • Ionic bonds form ionic compounds. An ionic compound is composed of positive (cations) and negative (anions) ions that are combined so that the negative and positive charges are equal. • Note: Ionic compounds form lattice structures

  24. Why do some atoms in formulas have subscripts and others do not? Use electron dot notation to show bonds and compounds Lewis structures

  25. Ionic Bonds – Transfer of electrons • Show formula unit • Strength of bonds (bond energy)

  26. Ionic Bonds & Compounds • Using electron dot to show the transfer of electrons • A metal must lose all its valence electrons • A non-metal must gain enough valence electrons to meet the Octet Rule. • Additional atoms (ions) of each type of element may be needed to form the correct compound.

  27. Ionic Formula • Ionic formula units: The charges of the atoms in the compound must equal to zero. • Na ion (Na ) and Cl ion (Cl ) _______ + ________ = 0 Na ion (Na ) and Ca ion (Ca ) _______ + ________ = 0

  28. Ionic compound names • Metal name + Non-metal (ide) • Prefix?? • Note: will practice names & formulas after determining bonds

  29. Properties of Ionic Compounds

  30. Video: Discovery Ed • Ionic bonds

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