1 / 22

Chemical Formulas and Chemical Compounds

Chemical Formulas and Chemical Compounds. 7.1. Naming Binary Ionic Compounds. Binary Ionic Compound (BIC) -ionic compound made up of two ions To name cation – use name of atom Na + = sodium K + = potassium Ca 2+ = calcium Ba 2 + = barium. Naming Anions.

jasia
Download Presentation

Chemical Formulas and Chemical Compounds

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 Formulas and Chemical Compounds 7.1

  2. Naming Binary Ionic Compounds • Binary Ionic Compound (BIC) -ionic compound made up of two ions • To name cation – use name of atom • Na+ = sodium K+ = potassium • Ca2+ = calcium Ba2+ = barium

  3. Naming Anions • To name anions, use the atom’s base name and –ide at the end • Cl- = Chloride S2- = Sulfide • P3- = Phosphide O2- = Oxide • KBr = Potassium bromide • Mg3N2 = Magnesium nitride

  4. Naming • FrF • SrBr2 • Li2Se

  5. Writing Ionic Formulas • Write the symbol and charge of each ion side by side (cation first) • If total = 0, just write symbols & you are done! • If total does not = 0, criss cross charges to have overall 0 charge

  6. Formula Writing Practice • Magnesium sulfide • Rubidium Oxide • Strontium Bromide • Aluminum Oxide

  7. Multiple Charge Cations/Transitions & Group 14 • If cation has multiple charges, use a roman numeral to indicate charge • Cu+ =Copper (I) Cu+2 =Copper (II) • I = 1 II = 2 III = 3 IV = 4 • V = 5 VI= 6 VII = 7 VIII = 8 • IX = 9 X = 10

  8. Determining Charge on Transition Metals • The charge on ionic compounds has to be electrically neutral • Figure out overall charge on anion and then determine what charge cation has to be • CuCl2 ~Each Cl has a charge of -1 (needs 1 e-) and since there are 2 of them, the overall charge of Cl is -2. Cu must be +2 = Copper (II) chloride

  9. Determining Charge on Transition Metals • PbO2 Charge on O is -2 and there are 2 of them so overall on O is -4. • Pb has to be +4 • Lead (IV) oxide

  10. Practice • CuO • Hg2O • Cu2O • Vanadium (III) Iodide • Platinum (IV) oxide

  11. Polyatomic Ions • Polyatomic Ion – an ion made of 2 or more atoms that behave like a single ion • Bonded covalently • Bond ionically with other simple ions as salts

  12. Naming Compounds w/polyatomics • Name the ion that is not a polyatomic like simple cations or anions and then name the polyatomic as the chart says • NaOH = Sodium hydroxide • CaCO3 = Calcium carbonate

  13. Polyatomic Ions • AlPO3 • LiSCN • FeSO4 • Mn(Cr2O7)2

  14. Formula Writing w/polyatomics • Determine charge of overall polyatomic and then the other ion. • Follow same rules as before. • Beryllium cyanide • Copper (II) nitrate

  15. Polyatomic Ions • Barium sulfide • Potassium oxalate • Chromium (III) cyanide • Vanadium (V)silicate

  16. Oxyanions • Name changes as number of O changes • Gain 1 O = perchlorate ClO4- • Base Name = chlorate ClO3- • Lose 1 O = chlorite ClO2- • Lose 2 O = hypochlorite ClO-

  17. Hydrogen and Sulfur • The name usually starts with the word hydrogen, but use mono- and di- • HPO4 –monohydrogen phosphate • H2PO4 – dihydrogen phosphate • Thio – replace O with S • K2S2O3 – Potassium thiosulfate

  18. Naming Covalent Compounds • Inorganic molecular compounds • Specify # of each type of atom • P4O6 – Tetraphosphorus hexoxide • P4O10 – Tetraphosphorus decoxide

  19. Cova l en t p r e f ixes

  20. Naming Covalent Compounds • If there is 1 of the first element, mono is omitted from the word • CO – carbon monoxide • CO2 – carbon dioxide

  21. Naming Covalent Compounds • 1st element – named 1st – usually least e-neg • 2nd element – named 2nd – usually most e-neg – add ide ending • Drop vowels o and a from prefix before adding it to a root that starts with a vowel

  22. Naming Covalent Compounds • N2O4 – Dinitrogen tetroxide • SF6 – Sulfur hexafluoride • Some common names are used instead of technical name • H2O – water – not dihydrogen monoxide

More Related