1 / 23

Write the electron configuration for K and Br.

Write the electron configuration for K and Br. Circle the Valence Electrons. NOMENCLATURE. OF IONIC. COMPOUNDS. A John Modica Production. Ionic Compounds. Because electrons are negatively charged…

lesley-matthews
Download Presentation

Write the electron configuration for K and Br.

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. Write the electron configuration for K and Br. Circle the Valence Electrons

  2. NOMENCLATURE OF IONIC COMPOUNDS A John Modica Production

  3. Ionic Compounds • Because electrons are negatively charged… • an atom becomes positively or negatively charged as it loses or gains an electron, respectively. • Any atom or group of atoms with a net charge (whether positive or negative) is called an ion. • A positively charged ion is a cation • A negatively charged ion is an anion. +2 Mg positively t negatively n n -2 O

  4. Compounds are two or more elements that are held together by opposite charge attraction. IONIC COMPOUNDS 8 (+)10 (-)-2 Charge Oxygen-8 Magnesium-12 12 (+)10 (-)+2 Charge Metal Non-metal

  5. Ionic Formulas • Ions combine in small, whole number proportions so that the sum of oxidation numbers will be zero! • Electrons are transferred from the metal to the non-metal • The metal become a cation (+ charge) • Why? • The non-metal becomes an anion (- charge) • Why?

  6. Metals combine with non-metals Metals loose electrons to non-metals They attract because their charges are opposite. Metals Non-metals

  7. Ionic Formulas • These are called Binary Compounds • The prefix “bi” meaning two • Two elements bonding to form a compound • The metal ion ALWAYS goes first, followed by the non-metal ion

  8. So what does this look like? Mg -2 +2 O Magnesium Oxide

  9. So what does this look like? Al -2 +3 S 3 2 Aluminum Sulfide

  10. So what does this look like? Na -1 +1 Cl Sodium Chloride A.k.a. Table Salt

  11. Your Turn! -1 F -1 Ba +2 Cl +1 Na Br Al +3 -1 +1 -2 +1 -2 K O S Li

  12. Your Turn! F Ba Cl Na 2 Br Al 3 K O S Li 2 2

  13. Now let’s Kick it up a notch!

  14. Polyatomic Ions • A group of 2 or more atoms that act as a single unit • When a metal and a polyatomic ion bond this forms a tertiary compound • 3 or more elements reacting to form a compound

  15. POLYATOMIC IONS Polyatomic ions are mostly made of two non-metals. Ions with -1 charge perbromate BrO4-1 bromate BrO3-1 bromite BrO2-1 hypobromite BrO-1 perchlorate ClO4-1 chlorate ClO3-1 chlorite ClO2-1 hypochlorite ClO-1 periodate IO4-1 iodate IO3-1 iodite IO2-1 hypoiodite IO-1 nitrate NO3-1 nitrite NO2-1 hydroxide OH-1 cyanide CN-1 acetate C2H3O2-1 Permanganate MnO4-1 bicarbonate HCO3-1 Ions with a -2 Charge carbonate CO3-2 sulfate SO4-2 sulfite SO3-2 chromate CrO4-2 dichromate Cr2O7-2 oxalate C2O4-2 Ions with a -3 Charge phosphate PO4-3 phosphite PO3-3 arsenate AsO4-3 Ions with +1 charge ammonium ion NH4+1 Yes, I can read your minds…

  16. No you do not have to memorize these polyatomic ions. You will receive a chart with these Obviously!!!

  17. Tertiary Compounds • Polyatomics ions react as one unit, so you treat them the same when writing formulas • Use the criss-cross method Na PO +1 -3 4 3 Sodium Phosphate

  18. Tertiary Compounds Mg SO ( ) -2 +2 4 Magnesium Sulfate

  19. Tertiary Compounds NO Al ( ) -2 +3 2 2 3 Aluminum Nitrite Yeah, I’ve got nothing.

  20. Your Turn! -2 -1 SO Ba +2 ClO +1 Na 2 4 PO Al +3 -3 4 -1 -2 +1 +1 K NO SO Li 2 3

  21. Your Turn! ( ) ClO SO Ba Na 2 2 4 2 ( ) PO Al 4 K NO SO Li 2 2 3

  22. How do we know the charge of the elements? Glad you asked!

  23. Oxidation Numbers (most common) +2 +2 +1 +3 +2 +4 0 -4 -3 -2 -1 +1 +2 +3 1A 7A 8A H H He 3A 4A 5A 6A 2A Li Be B C N O F Ne Click on element to see its oxidation number(s) Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Ce Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Rf Db Sg Rh Hs Mt Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu return Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr

More Related