1 / 24

Chemical Bonding and Nomenclature

Chemical Bonding and Nomenclature. Ch. 6 & 7. Chemical Bond. Mutual electrical attraction between the nuclei and valence electrons of different atoms Atoms bond to reduce potential energy Atoms become more stable when they are bonded. Types of Chemical Bonds.

oscarjones
Download Presentation

Chemical Bonding and Nomenclature

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Chemical Bonding and Nomenclature Ch. 6 & 7

  2. Chemical Bond • Mutual electrical attraction between the nuclei and valence electrons of different atoms • Atoms bond to reduce potential energy • Atoms become more stable when they are bonded

  3. Types of Chemical Bonds • Metallic – Attraction between metal atoms and the surrounding electrons • Ionic – Electrical attraction between cations and anions • Covalent – Sharing of electrons between atoms • Nonpolar Covalent – Electrons are shared equally between the atoms • Polar Covalent – Electrons are not shared equally between the atoms

  4. Metallic Bonding • Empty d orbitals are overlapping – electrons flow between these empty orbitals creating a ‘sea of electrons’ • A network of metal atoms forms in which the atoms attract the ‘sea of electrons’

  5. Metals have Unique Properties • High electrical conductivity • Absorb and emit light – shiny • Malleable – can be hammered into thin sheets (Layers of atoms just slide past one another) • Ductile – can be drawn into a string

  6. Ionic or Covalent??? • Check the electronegativity difference between two atoms… • If the EN difference is greater than 1.7, the bond will be ionic. • If the EN difference is 0.3 to 1.7, the bond is polar covalent • If the EN difference is 0 to 0.3, the bond is nonpolar covalent

  7. Ionic Bonding • Cation transfers electrons to anion • Creates a crystalline solid – 3-D network of cations and anions • Lowest ratio of the cations to anions is represented by the formula unit

  8. Formation of Ionic Compounds • Electron-dot notation – represents transfer of electrons

  9. Example • Draw the electron dot diagram representing the formation of an ionic bond between • potassium and iodine • aluminum and oxygen

  10. Characteristics of Ionic Bonds • Ions have strong attractions between them – this results in: • High melting point, high boiling point • Hard, but brittle • Layers of ions will break apart • Only electrical conductors in molten state • Many ionic compounds will dissolve in water

  11. Things to know about ions before naming/writing ionic formulas • Cations can be monatomic or polyatomic ions • Monatomic charges are on the PT and polyatomic ions must be memorized (p. 210 of textbook) • Cations can also be transition metals – lose a varying amount of electrons – must use Roman numerals to indicate charge • Exceptions: Zn+2, Cd+2, Ag +1 • Lead and Tin also use Roman numerals to indicate charge • Anions can be monatomic or polyatomic ions

  12. Practice - Naming Ions • Write the names the following ions: • Ca+2 • I-1 • Cu+2 • Zn+2 • Pb +4 • NO3-1 • NH4+1

  13. Answers • Calcium Ion • Iodide • Copper (II) • Zinc • Lead (IV) • Nitrate • Ammonium

  14. Ionic Nomenclature • To name an Ionic Compound • Step 1: Name the cation • Check to see if it needs Roman numerals • Step 2: Name the anion

  15. NaBr CaI2 K2O CuCl CuCl2 ZnBr2 K2SO4 Ca(NO3)2 NH4Cl (NH4)2SO4 Pb(ClO3)4 BaSO3 MnO AgCl Examples

  16. Sodium bromide Calcium iodide Potassium oxide Copper (I) chloride Copper (II) chloride Zinc bromide Potassium sulfate Calcium nitrate Ammonium chloride Ammonium sulfate Lead (IV) chlorate Barium sulfite Manganese (II) oxide Silver chloride Answers

  17. Writing Ionic Formulas • To write an ionic compound’s formula • Step 1: Write the formula for the cation – including charge • Step 2: Write the formula for the anion – including charge • Step 3: Balance the charges. • Be sure to use parenthesis if more than one polyatomic ion is needed

  18. Calcium chloride Barium sulfide Ammonium nitride Iron (II) chloride Lead (IV) sulfate Barium phosphate Calcium hydroxide Iron (III) permanganate Ammonium nitrite Calcium carbonate Copper (II) sulfate Sodium acetate Potassium sulfite Sodium hydroxide Examples

  19. Acid Nomenclature • The first element is Hydrogen – H____ • To name an acid, look at the anion: • If the anion ends in –ide, change the name of the acid to hydro-ic acid • If the anion ends in –ite, change the name of the acid to –ous acid. • If the anion ends in –ate, change the name of the acid to –ic acid.

  20. HCl H2SO4 HClO3 HBr H2S HClO4 H2CO3 HNO2 Examples

  21. Hydrochloric acid Sulfuric acid Chloric acid Hydrobromic acid Hydrosulfuric acid Perchloric acid Carbonic acid Nitrous acid Answers

  22. Acids – Writing Formulas • To write the formula for an acid • Step 1: Decide which ion is needed based on the ending • Step 2: Add H+1 in front of the anion • Step 3: Balance the charges

  23. Hydroiodic acid Phosphorous acid Sulfurous acid Nitric acid Acetic acid Phosphoric acid Hypochlorous acid Examples

  24. HI H3PO3 H2SO3 HNO3 HCH3COO or CH3COOH H3PO4 HClO Answers

More Related