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Physical Science Date :2/16/11

Physical Science Date :2/16/11. Instructional Objective: 1.identify the difference between ionic and covalent compounds 2.Learn about the bonds Review Questions: Name the following Np______ Er_______ Other instructions: Lab .Rolling for a compound. Homework:

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Physical Science Date :2/16/11

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  1. Physical ScienceDate :2/16/11 Instructional Objective:1.identify the difference between ionic and covalent compounds 2.Learn about the bonds Review Questions:Name the following Np______ Er_______ Other instructions: Lab .Rolling for a compound. Homework: Do Work sheet for naming compound

  2. Physical Science09/29/10 Instructional Objective: 1.Reteach the element’s place in the periodic chart2.Reteach naming and writing the formula for compounds Review Questions:1. Explain a cation Other instructions: Lab.Submit the work sheet before you leave Homework: Do the work sheet

  3. Ions • An atom with a charge. • It can be positive or negative in charge. • It can be obtain by loosing or gaining electrons. (Protons never change)

  4. Cations • Are always positive in charge. • Obtain by loosing electrons. • Always going to be a metal • Written using the symbol with a + sign • Ex. Na+ Proton – 11, electron -10 • Roman numerals are used to show the charge of certain metals. • Ex: Fe 3+ is named as Iron III

  5. Anions • Are always negative in charge. • Obtain by gaining electrons • Always going to be a nonmetal • Written using a symbol with a negative sign. • Ex: Cl – (Proton -17 ,electron -18)

  6. What is an oxidation number? • valence electron: electron in the outermost energy level of an atom • oxidation number: number of electrons an atom gains, loses, or shares when it forms a chemical bond

  7. What is a chemical equation? chemical equation: *chemical formula that describe a chemical reaction coefficient: • number that shows how many molecules of a substance are in a chemical reaction • Used to balance an equation

  8. Ionic Compound • Metal and a nonmetal combined. • Always a cation and anion • Net charge will be zero. • Named as metal first ,then the nonmetal that ends with ide,ite,ate. • Ex. Sodium Chloride (Name) NaCl (Symbol) • To write the symbol use the crisscross method to cancel the charges. • Ex:

  9. Physical ScienceDate :2/17/11 Instructional Objective:1.understsnd to name compounds that contain polyatomic ions 2.Learn to write the formula for a chemical compounds Review Questions:1.Three exceptions of polyatomic ions. _______________________________________ Other instructions: Finish the Open book pre test Homework: Do Work sheet for polyatomic ions

  10. Physical ScienceDate :2/17/11 Instructional Objective:1.understsnd to name compounds that contain polyatomic ions 2.Learn to write the formula for a chemical compounds Review Questions:1.Explain cations. _______________________________________ Other instructions: Finish the work sheet with the teacher Homework: Do Work sheet for polyatomic ions

  11. Physical ScienceDate 02/21/11 Instructional Objective:1.Learn about the covalent compounds 2.Identify the ionic and covalent bonds Review Questions:1.Write the formula for sodium phosphide? _______________________________________ Other instructions: 1.Finish the “October Sky” and submit the work sheet 2.Do Work sheet with the teacher Homework: Do the work sheet for the compounds.

  12. Metals with multiple ions • Many transition metals have more than one oxidation number. • It is always indicated with roman Numeral number. • Ex: Copper II Copper I Chromium II Chromium III

  13. Two types of ionic compounds • Binary ionic compound • *Contain two elements • *Contain a metal and a nonmetal • Ex: NaCl

  14. Polyatomic ion • is a group of atoms that acts as a single atom. • have an overall electrical charge. • atoms are held together by covalent bonds. • If there is more than one polyatomic ion in a molecule, the polyatomic ion is written in parentheses. . End with ite or ate EX: SO32- Sulfite (one less Oxygen than the ate) (Charge will be same) SO42- Sulfate (Charge will be same)

  15. 3 Exceptions in the polyatomic ions • Ammonium polyatomic cation that not ending with “ite” or “ate” ending NH+4 - Ammonium NH+3 -Ammonia • Cyanide CN- • Hydroxide OH-

  16. Ternary Ionic compound • Contain a metal and a polyatomic ion • Contain three or more elements • Or contain a poly atomic cation and a nonmetal • Or contain two polyatomic ions. • Ex: Na2 SO4 ( 3 elements) • Ex: Ca(SO4)2 (more than one polyatomic ions, you must use a parenthesis around it)

  17. Covalent Compounds (Molecular compounds) • Always going to be nonmetals combined • Identify or name using prefix for the number of atoms. • Ex:

  18. Prefix for covalent compound • Mono -1 • Di-2 • Tri-3 • Tetra-4 • Penta-5 • Hexta-6 • Septa-7 • Octa-8 • Nano-9 • Deca-10

  19. Physical ScienceDate :2/16/09 Instructional Objective:1.Learn about the Chemical bond 2.Identify the ionic and covalent bonds Review Questions:1.An atom’s mass number equals the number of ________________________ Other instructions: Lab. Chemical bonding Homework: Do the work sheet

  20. Chemical bonds • are the force that join two or more atoms. • A stable compound occurs. • a net (total) attractive force between the atoms .

  21. Two types of bonds • Covalent bond: one or more pairs of electrons are shared by two atoms. • Ionic bond: one or more electrons from one atom are removed and attached to another atom. • resulting in positive and negative ions which attract each other.

  22. Covalent Bonds • involve the sharing of a pair of valence electrons by two atoms

  23. Ionic Bonds • one or more atoms lose electrons and other atoms gain

  24. Ionization energy • The amount of energy used to remove an electron is known as the ionization energy • Varies from element to elements • Energy increases from left to right(less reactive) • Energy decreases from top to bottom(easy to remove the electron, so it will be more reactive) • Ex: K is more reactive than Na

  25. Crystal Lattices • an ionic compound particles are arranged in a repeating pattern • The attractions keeps the ions in a fixed position in a frame work (lattice) • Ex:LiCl

  26. (metal) (nonmetal) CHARGE OF ATOM CHARGE OF ATOM neutral neutral Cl 17 Na 11

  27. (metal) (nonmetal) CHARGE OF ATOM CHARGE OF ATOM neutral neutral Cl 17 Na 11

  28. (metal) (nonmetal) CHARGE OF ATOM CHARGE OF ATOM neutral neutral Cl 17 Na 11

  29. (metal) (nonmetal) CHARGE OF ATOM CHARGE OF ATOM neutral neutral Cl 17 Na 11

  30. (metal) (nonmetal) CHARGE OF ATOM CHARGE OF ATOM neutral neutral Cl 17 Na 11

  31. (metal) (nonmetal) CHARGE OF ion CHARGE OF ion negative positive Ionic Bond (cation) (anion) [Cl] 1- 17 [Na] 1+ 11

  32. (metal) (nonmetal) CHARGE OF ion CHARGE OF ion negative positive Ionic Bond (cation) (anion) [Cl] 1- 17 [Na] 1+ 11

  33. (metal) (nonmetal) CHARGE OF ion CHARGE OF ion negative positive Ionic Bond (cation) (anion) [Cl] 1- 17 [Na] 1+ 11

  34. (metal) (nonmetal) CHARGE OF ion CHARGE OF ion negative positive Ionic Bond (cation) (anion) [Cl] 1- 17 [Na] 1+ 11

  35. (metal) (nonmetal) CHARGE OF ion CHARGE OF ion negative positive Ionic Bond (cation) (anion) [Cl] 1- 17 [Na] 1+ 11

  36. (metal) (nonmetal) CHARGE OF ion CHARGE OF ion negative positive Ionic Bond (cation) (anion) [Cl] 1- 17 [Na] 1+ 11

  37. (metal) (nonmetal) CHARGE OF ion CHARGE OF ion negative positive Ionic Bond (cation) (anion) [Cl] 1- 17 [Na] 1+ 11

  38. What is a diatomic molecule? • is made up of two atoms of the same element • is usually held together by a covalent bond. • Most gaseous elements form diatomic molecules.

  39. 7 diatomic molecules • Hydrogen( H2), • Oxygen ( O2), • Nitrogen (N2), • Fluorine (F2), • Chlorine(Cl2), • Bromine (Br2) • Iodine(I2)

  40. Metallic Bonds • Is the attraction between a metal cation and the shared electrons that surround it • More valance electrons in a metal-stronger the metallic bond

  41. Physical ScienceDate :2/25/2010 Instructional Objective:1.Name the ionic and covalent compounds 2. Formula for ionic and covalent compounds Review Questions:write the formula for the following 1.Sodiumphosphate_________________________________ Other instructions: Finish the work sheet (Use the rollercoaster book from under your desk). Homework: Study for the unit test

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