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ION FORMATION

ION FORMATION. an atom there are the same number of protons and electrons it is electrically neutral. ION FORMATION. An ion is an atom that has lost or gained electrons and now has an electric charge. ION FORMATION.

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ION FORMATION

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  1. ION FORMATION an atom there are the same number of protons and electrons it is electrically neutral.

  2. ION FORMATION An ion is an atom that has lost or gained electrons and now has an electric charge

  3. ION FORMATION The net charge of an ion that has lost or gained electrons is shown as a superscript to the right of the atomic symbol It is also called the oxidation number

  4. ION FORMATION Bismuth will gain 3 electrons and have a negative 3 charge Bi = Bi-3 Oxidation number Sodium will lose its electron and become positively charged Na = Na+1

  5. ION FORMATION The number of electrons that an atom will gain or lose depends on its position on the periodic table (group number)

  6. Ca+ion An atom that has lost electrons and now has a net positively charged Sodium will lose its electron and become positively charged Na = Na+1

  7. Anion An atom that has gained an electron and now has a net negative charge Bismuth will gain 3 electrons and have a negative 3 charge Bi = Bi -3

  8. ION FORMATION Metals, elements to the left of the staircase, will form cations (+ charge) Nonmetals, elements to the right of the staircase will form anions (- negative)

  9. ION FORMATION group “B” elements The oxidation numbers of the “B” group elements are variable. They do not follow a pattern like the Group “A” elements.

  10. ION FORMATION group “B” elements Oxidation numbers will be given to you as a Roman Numeral in parentheses following the name of the element.

  11. ION FORMATION group “B” elements • Practice 1. Write the ion formed by these element. • iodine I-1 d. cobalt (II)Co+2 b. potassium K+1 e. gallium Ga+3 c. sulfur S-2 f. chromium (III) Cr+3

  12. ION FORMATION group “B” elements Writing Ions Practice

  13. ION Oxidation Cation Number or Anion Bromine 1 Anion Rubidium 1 Cation Barium 2 Cation Sulfur 2 Anion Tin (IV) 4 Cation Iodine 1 Anion Argon 0 Neither Aluminum 3 Cation Magnesium 2 Cation

  14. ION Oxidation Cation Number or Anion Strontium 2 Anion Lead (II) 2 Cation Antimony (V) 5 Cation Phosphorus 3 Anion Copper (I) 1 Cation Selenium 2 Anion

  15. BONDING Remember that a compound consist of two or more elements chemically combined together H2O, NaCl, Sb3(PO4)5

  16. BONDING The smallest unit of a compound is a molecule Only electrons move during bonding It is the movement of valence electrons that determines how one atom will bond with another

  17. BONDING Octet Rule- all atoms need 8 valence electrons to be stable

  18. BONDING, FOUR TYPES IONIC- Transfer of electrons COVALENT- sharing of electrons POLAR COVALENT- uneven sharing of electrons METALLIC- bonds between cations and free electrons

  19. IONIC BONDS Electrons are transferred from one atom to another This creates a Cation (+) and an Anion (-) Opposite charges attract

  20. IONIC BONDING Na Cl Na+1 -1 Cl

  21. -1 Na+1 Cl The Cation (Na) is attracted to the Anion (Cl)

  22. IONIC BONDING Ionic Bonds are the strongest bonds Form between Metals and Non-Metals

  23. BONDING The stair case separates Metals (Left) from Non-Metals (Right)

  24. IONIC BONDINGLewis Dot Na Cl -1 Na+1 Cl

  25. BONDINGEnergy Levels Cl Na -1 +1 Na Cl

  26. Writing Formulas for Ionic Compounds Ion- an atom that has lost or gained electrons Cation- Lost electrons positive charge Anion- Gained electrons negative charge

  27. Writing Formulas for Ionic Compounds Oxidation number- indicates the number of electrons lost or gained during bonding To be stable- oxidation number must be zero (no charge) Binary Compound– formed between metal and non-metal

  28. Writing Formulas for Ionic Compounds • Write the ion of the Cation – Mg+2 • Write the ion of the Anion – O-2 • Write the subscripts (bottom numbers) to indicate how many ions of each element is needed to make the sum of the oxidation numbers zero (do not write 1’s)

  29. Magnesium (Mg) Group II Loses two electrons Mg+2 Oxygen (O) Group VI Gains two electrons O-2 Writing Formulas for Ionic Compounds

  30. Writing Formulas for Ionic Compounds Mg+2 + O -2 = net charge of 0 Formula = MgO

  31. Magnesium (Mg) Group II Loses two electrons Mg+2 Bromine (Br) Group IIV Gains one electrons Br -1 Writing Formulas for Ionic Compounds

  32. Writing Formulas for Ionic Compounds Mg+2 + Br -1 = net charge of +1 We need 2 Br -1 ions to even out the charge Mg+2 + Br2-1 = net charge of 0 (Mg+2 + Br -1 + Br -1 = net charge of 0) Formula = MgBr2

  33. Sodium (Na) Group I Loses one electrons Na+1 Oxygen (O) Group VI Gains two electrons O -2 Writing Formulas for Ionic Compounds Combine Sodium and Oxygen

  34. Writing Formulas for Ionic Compounds Na+1 + O -2 = net charge of -1 We need 2 Na +1 ions to even out the charge Na2+2 + O -2 = net charge of 0 (Na+1 + Na+1 + O -2 = net charge of 0) Formula = Na2O

  35. Calcium (Ca) Group II Loses two electrons Ca+2 Fluorine (F) Group VII Gains one electrons F -1 Writing Formulas for Ionic Compounds Combine Calcium and Fluorine

  36. Writing Formulas for Ionic Compounds Ca+2 + F -1 = net charge of +1 We need 2 F -1 ions to even out the charge Ca+2 + F2-1 = net charge of 0 (Ca+2 + F-1 + F -1 = net charge of 0) Formula = CaF2

  37. Iron (II) (Fe II) Fe (II) Loses two electrons Fe+2 Sulfur (S) Group VI Gains two electrons S -2 Writing Formulas for Ionic Compounds Combine Iron (II) and Sulfur

  38. Writing Formulas for Ionic Compounds Fe+2 + S -2 = net charge of 0 Formula = FeS

  39. Writing Formulas for Ionic Compounds: Crisscross A SHORTCUT to figure out then number of each ion needed to form a neutral compound

  40. Writing Formulas for Ionic Compounds: Crisscross • Write each Cation first followed by the Anion • Cross the oxidation numbers (superscript) to be the subscript of the other • Reduce the subscripts if they aren’t already

  41. Magnesium (Mg) Group II Loses two electrons Mg+2 Bromine (Br) Group IIV Gains one electrons Br -1 Writing Formulas for Ionic Compounds: Crisscross

  42. Writing Formulas for Ionic Compounds: Crisscross Mg+2 Br -1 Mg1 Br2 Formula = MgBr2

  43. Magnesium (Mg) Group II Loses two electrons Mg+2 Oxygen (O) Group VI Gains two electrons O-2 Writing Formulas for Ionic Compounds: Crisscross

  44. Writing Formulas for Ionic Compounds Mg+2 + O -2 Mg+2 + O-2 Formula = Mg2 O2 (REDUCE) =MgO

  45. Sodium (Na) Group I Loses one electron Na+1 Oxygen (O) Group VI Gains two electrons O -2 Writing Formulas for Ionic Compounds: Crisscross Combine Sodium and Oxygen

  46. Writing Formulas for Ionic Compounds Na+1 + O -2 Na2 + O1 Formula = Na2O

  47. Iron (II) (Fe II) Fe (II) Loses two electrons Fe+2 Sulfur (S) Group VI Gains two electrons S -2 Writing Formulas for Ionic Compounds Combine Iron (II) and Sulfur

  48. Writing Formulas for Ionic Compounds Fe+2 + S -2 Fe2 + S2 Fe2S2 REDUCE to FeS

  49. Naming Ionic Compounds • Write the name of the cation first

  50. Naming Ionic Compounds 2. If the cation is a transition metal add a Roman Numeral in parentheses to indicate oxidation number • Use crisscross method in reverse FeS = Fe+1 S-1

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