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Chemical Nomenclature

Chemical Nomenclature. How to write and say chemical formulas General Chemistry 10-11. Elements. Elements are said with just their name Mg = magnesium Ca = calcium Some elements never exist by themselves These are called diatomic molecules

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Chemical Nomenclature

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  1. Chemical Nomenclature How to write and say chemical formulas General Chemistry 10-11

  2. Elements • Elements are said with just their name • Mg = magnesium • Ca = calcium • Some elements never exist by themselves • These are called diatomic molecules • There are seven of them and they make a seven on the periodic table

  3. The Diatomic Molecules • These would still be said by their elemental name but would be written with a subscript of 2 • N2 • O2 • F2 • Cl2 • Br2 • I2 • H2

  4. Compounds • Most elements are not found separately but combined in a compound with something else • The reason for this is the octet rule We want 8…eight is great!

  5. Octet Rule • Noble gases are what all elements aspire to be like electronically • These elements have 8 electrons in highest energy level

  6. Na Cl Ionic Bond • Atoms will either give up or take electrons to get to have eight in their highest energy level

  7. Na Cl Hey, can you help me out and gimme an electron?

  8. Na Cl Why certainly, I have one I don’t want anyway.

  9. Na Cl Give up/take away electrons

  10. - + Na Cl Charges • Sodium now has a +1 charge since it has lost an electron • Chlorine a minus charge since it gained an electron

  11. - NaCl 4Eva + Na Cl (or until water breaks us apart) Ionic Bond • Opposites attract, so a bond is formed between the two of them.

  12. Ionic Compound • The combination of Na+ and Cl- form the compound NaCl • An ionic compound will always consist of: • A metal ion (also called a cation, the + one) • A non-metal ion (also called an anion, the - one) • CATION ALWAYS COMES BEFORE THE ANION; both in the name and the formula

  13. Naming Ionic Compounds • When naming ionic compounds • Just say the name of the metal • For the non-metal, drop the ending and add -ide to it. • NaCl = sodium chloride

  14. Name the following ionic compounds ZnO LiBr Mg3N2 BaS K3P Zinc oxide Lithium bromide Magnesium nitride Barium sulfide Potassium phosphide Practice Problem #1

  15. Determining metal and non-metal charge • Where are the metals on the periodic table? • Metals always have what charge? • Where are the nonmetals? • Nonmetals always have what charge? We’ll see the charges of the different families on the following slide.

  16. +1 -3 -1 +2 -4 -2 Using the periodic Table to find an ion’s charge We’re going to forget all about the middle of the table for now.

  17. You must balance out the overall charge! Combining metals and nonmetals • When combining a metal and a non-metal, the overall charge of the compound must be zero.

  18. Combining metals and nonmetals • Take for instance calcium nitride. • What is the charge of the calcium ion? • What is the charge of the nitride ion?

  19. N Ca Combining metals and nonmetals • Ca+2 means each calcium ion has 2 more electrons than it wants • N-3 means each nitride ion needs 3 more electrons.

  20. N Ca Hey buddy, can you spare 3 electrons?

  21. N Ca Sorry, I only have two.

  22. N Ca Ca Maybe I can help!

  23. N Ca Ca

  24. Ca -3 N +2 Ca HEY, What about me? YEAH! YEAH!

  25. Ca -3 N +2 Ca Hang loose, man. I’ll get one of my buddies.

  26. Ca -3 N N +2 Ca YO, YO, YO. Your hero has arrived.

  27. -1 -3 N N YEAH! +2 Ca +2 Ca

  28. -1 -3 N N I still need two more. +2 Ca +2 Ca

  29. -1 -3 N N Ca I need to get rid of two more. +2 Ca +2 Ca

  30. -1 -3 N N Ca +2 Ca +2 Ca

  31. +2 Ca -3 +2 Ca -3 N N +2 Ca The ions found they were still attracted to one another due to their opposing charges. And they all lived happily ever after.

  32. Practice Problem #2 • Give the formulas for the following compounds • Beryllium iodide • Potassium sulfide • Magnesium oxide • Strontium fluoride BeI2 K2S MgO SrF2 Now is the time to learn “SWITCHY SWITCHY” and reduce!

  33. Transition Metals • The middle block of elements • All cations • Most can take on multiple charges • Some Exceptions • Zn = +2 • Ag = +1

  34. Transition metal compounds • In order to tell what charge a transition metal has, put its charge in parenthesis • For instance Copper (II) Oxide means… • the copper ion here has a +2 charge • For instance Copper (I) Oxide means… • the copper ion here has a +1 charge What are the formulas of these two ionic compounds?

  35. Practice Problem #3 • Give the formula of the following compounds: • Tungsten (IV) Chloride • Gold (III) phosphide • Tin (II) fluoride • Zinc sulfide WCl4 AuP SnF2 ZnS

  36. Polyatomic Ions • Sometimes, atoms get together but can’t quite get to an overall zero charge. • This is where they become a polyatomic ion • They’re still a charged particle (mostly anions) so they can combine with an opposing charged ion to produce a compound • Naming is easy, we just say the name of the polyatomic ion With polyatomic ions we don’t have to change the ending

  37. [ [ H N H H H Ionic Compounds involving a polyatomic ion 1N = -5 4H = -4 Total -9 One extra electon

  38. [ [ H Cl N H H H Ionic Compounds involving a polyatomic ion

  39. +1 -1 [ [ [ [ H Cl N H H H Ionic Compounds involving a polyatomic ion Opposites attract

  40. +1 -1 [ [ [ [ H Cl N H H NH Cl = Ammonium Chloride H 4 Another happy compound formed!

  41. Practice Problem #4 Ammonium sulfide Calcium sulfate Barium nitrate Potassium carbonate Magnesium phosphate • Name the following compounds • (NH4)2S • CaSO4 • Ba(NO3)2 • K2CO3 • Mg3(PO4)2

  42. Practice Problem #5 • Write formulas for the following compounds • Aluminum nitrate • Beryllium sulfate • Calcium phosphite • Ammonium sulfite • Strontium nitrite Al(NO3)3 BeSO4 Ca3(PO3)2 (NH4)2SO3 Sr(NO2)2

  43. Cl Cl Covalent Bonds • Compounds formed by two non-metals • More of a sharing of electrons rather than a give-take relationship

  44. Cl Cl Can you spare an electron?

  45. Cl Cl JINX!

  46. Why don’t you share an electron? You know sharing is caring! Cl Cl

  47. Co=together Valent=valence electrons… therefore, covalent is sharing electrons! Cl Cl Shared pair of electrons = Covalent Bond

  48. Naming Covalent Bonds • Prefixes on back of periodic table • If there is only one of the first element, no prefix. Otherwise attach prefix • Second always gets prefix and -ide ending (just like ionic anion) • Name these • ICl5 • N2O

  49. Practice Problem #7 Carbon dioxide Phosphorous pentachloride Carbon monoxide Triphosphorous hexaflouride • Name the following covalent compounds • CO2 • PCl5 • CO • P3F6

  50. Practice Problem #8 • Give the formula for the following compounds • Sodium acetate • Nickel (II) chloride • Carbon dioxide • Sulfur trioxide • Triphosphorous tetrachloride NaC2H3O2 NiCl2 CO2 SO3 P3Cl4

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