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 H 2 O = 2 Hydrogen for every 1 Oxygen (Chemical Formula) Two Types: ①Ionic Compounds ②Molecular 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 electrons (-)10 electrons (-) Anions: Negative Charge Ex:Cl (Atom)Cl - (Anion)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.htmhttp://www.periodicvideos.com/videos/011.htm Army disposing of Na http://www.youtube.com/watch?v=HY7mTCMvpEMhttp://www.youtube.com/watch?v=HY7mTCMvpEM

6. Ions and Periodic Table

7. 2 Types of Ions Monatomic Ions: Single elements Na + Zn 2+ Br - Cl - O 2- Polyatomic Ions: Two or more different elements NH 4 + CO 3 2- CrO 4 2- Cr 2 O 7 2- See your handout for the list

8. Ionic Compounds Cation + Anion = Ionic Compound Na + + Cl - = NaCl Ni 2+ + 2(IO 3 - ) = Ni(IO 3 ) 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 ①Cation is ALWAYS first ②Net charge is ALWAYS zero ③Cation name doesn’t change. ④Change anion name by using the “ide” ending KCl = Potassium Chloride

10. Naming Ionic Compounds ①NaCl = ②MgO = ③KF = ④CaBr 2 =

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. Fe 2+ = iron(II) Fe 3+ = iron(III) Cu + = copper(I) Cu 2+ = copper(II)

12. Naming Ionic Compounds ①CuBr = ②PbCl 2 = ③FeN = ④CrP =

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” Ba 2+ + CO 3 2-  BaCO 3 BariumCarbonateBarium carbonate

14. Naming Ionic Compounds ①FePO 4 = ②CaCrO 4 = ③NaNO 3 ④SnSO 4

15. Naming Ionic Compounds ①Zinc chloride = ②Iron(II) oxide = ③Tin(IV) sulfite = ④Aluminum 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: H 2 O, CO 2, O 2, and Cl 2

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 CO 2 = Carbon Dioxide N 2 O 3 = Dinitrogen Trioxide

18. Naming Molecular Compounds ①Dinitrogen monoxide = ②Silicon carbide = ③N 2 O 4 = ④Cl 2 O 8 =

19. Naming Acids and Bases Acid: Produces hydrogen ion (H + ) when dissolved in H 2 O – Formula = (H + to balance the anion charge) + (anion) Ex: H 2 S HCl Base: Produces hydroxide ion (OH - ) when dissolved in H 2 O 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: H 2 SO 3 = sulfurous acid -Ends with “ate”: the suffix “ic” is added to the anion Ex: HNO 3 = 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 ①H 2 CO 3 = ②Phosphoric acid = ③KOH = ④Strontium hydroxide =