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Elements

Elements. Simplest form of matter that retains its properties Known by common names and abbreviations. Compounds. Made of two or more elements chemically combined in definite proportions Law of definite proportions : pure compounds always have the same ratio of elements

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Elements

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  1. Elements Simplest form of matter that retains its properties Known by common names and abbreviations

  2. Compounds • Made of two or more elements chemically combined in definite proportions • Law of definite proportions: pure compounds always have the same ratio of elements H2O = 2 Hydrogen for every 1 Oxygen (Chemical Formula) • Two Types: • Ionic Compounds • Molecular Compounds (Molecules)

  3. Paper Clip Lab • Elements vs. Compounds vs. Mixtures

  4. Ionic Compounds • Made up of Ions: Charged atoms Cations: Positive charge Ex: Na (Atom) Na+ (Cation) 11 protons (+) 11 protons (+) 11 electrons (-) 10 electrons (-) Anions: Negative Charge Ex: Cl (Atom) Cl- (Anion) 17 protons (+) 17 protons (+) 17 electrons (-) 18 electrons (-)

  5. Ions Vs. Atoms • There are chemical differences between ions and atoms…. Na+ vs. Na University of Nottingham http://www.periodicvideos.com/videos/011.htm Army disposing of Na http://www.youtube.com/watch?v=HY7mTCMvpEM

  6. Ions and Periodic Table

  7. 2 Types of Ions • Monatomic Ions: Single elements Na+ Zn2+ Br- Cl- O2- • Polyatomic Ions: Two or more different elements NH4+ CO32- CrO42- Cr2O72- See your handout for the list

  8. Ionic Compounds • Cation + Anion = Ionic Compound Na+ + Cl- = NaCl Ni2+ + 2(IO3-) = Ni(IO3)2 The positive cation and negative anion attract each other to form neutral compound Usually solids with high melting and boiling points Usually form from metal and nonmetal

  9. Naming Ionic Compounds • Binary Ionic Compounds: 2 different ions K+ + Cl- KCl • Cation is ALWAYS first • Net charge is ALWAYS zero • Cation name doesn’t change. • Change anion name by using the “ide” ending KCl = Potassium Chloride

  10. Naming Ionic Compounds • NaCl = • MgO = • KF = • CaBr2 =

  11. Naming Ionic Compounds • Some elements (called transition metals) can form more than one type of positive ion. The positive charge of the ion is then indicated by a roman numeral. Fe2+ = iron(II) Fe3+ = iron(III) Cu+ = copper(I) Cu2+ = copper(II)

  12. Naming Ionic Compounds • CuBr = • PbCl2 = • FeN = • CrP =

  13. Naming Ionic Compounds • Polyatomic ions: • Have special names • Are treated as one unit (they don’t break apart) • Most end in “ite” or “ate” Ba2+ + CO32- BaCO3 Barium Carbonate Barium carbonate

  14. Naming Ionic Compounds • FePO4 = • CaCrO4 = • NaNO3 • SnSO4

  15. Naming Ionic Compounds • Zinc chloride = • Iron(II) oxide = • Tin(IV) sulfite = • Aluminum hypochlorite =

  16. Molecule • Neutral groups of non-metallic elements joined by covalent bonds (electrons are shared) NO IONS – NO CHARGE • Low melting and boiling points • Liquids and gases at room temperature • Ex: H2O, CO2, O2, and Cl2

  17. Naming Molecular Compounds • Name them in the order that they appear • Element with more positive chemical nature will be first • “More positive” means towards the left side of periodic table • Second element: drop the last syllable and add “ide” • If there is more than one atom of an element, add a numerical prefix: CO = Carbon Monoxide CO2 = Carbon Dioxide N2O3 = Dinitrogen Trioxide

  18. Naming Molecular Compounds • Dinitrogen monoxide = • Silicon carbide = • N2O4 = • Cl2O8 =

  19. Naming Acids and Bases • Acid: Produces hydrogen ion (H+) when dissolved in H2O • Formula = (H+ to balance the anion charge) + (anion) Ex: H2S HCl • Base: Produces hydroxide ion (OH-) when dissolved in H2O • Formula= cation metal + hydroxide ion to balance charge Ex: NaOH Al(OH)3

  20. Naming Acids • When the anion…. • Ends with “ide”: acid name begins with “hydro” the suffix “ic” is added to the anion Ex: HCl = hydrochloric acid • Ends with “ite”: the suffix “ous” is added to the anion Ex: H2SO3 = sulfurous acid • Ends with “ate”: the suffix “ic” is added to the anion Ex: HNO3 = nitric acid

  21. Naming Bases • Named the same way as ionic compounds • Al(OH)3 = aluminum hydroxide • Fe(OH)3 = iron(III) hydroxide

  22. Naming Acids and Bases • H2CO3 = • Phosphoric acid = • KOH = • Strontium hydroxide =

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