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Multi-Valent Transition Metals and Polyatomic ions

Multi-Valent Transition Metals and Polyatomic ions. Subscripts and Superscripts. Superscripts (above) = charge (+ or -) of the ion Cl -1 or Ca +2 Subscripts (below) = the number of ions Cl 2 or H 4. Transition Metals:.

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Multi-Valent Transition Metals and Polyatomic ions

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  1. Multi-Valent Transition Metals and Polyatomic ions

  2. Subscripts and Superscripts • Superscripts (above) = charge (+ or -) of the ion Cl-1 or Ca+2 • Subscripts (below) = the number of ions Cl2 or H4

  3. Transition Metals: • Nearly all the transition metals are able to form more than one cation or are multi-valent. • Ex: iron can form Fe2+ and Fe3+. Given the formula of an ionic compound you can use the reverse cross-over method to determine the charge of the cation. Ex: FeCl3

  4. Scientists use two ways to name these type of compounds: • Stock System • Classical System

  5. Classical System: • We will not use the classical system for grade 10 science. We will only look at it and how it works. • The classical system is based on latin names for elements. Ex: iron is ferrum. We add an “ic” to the end of this to indicate the higher charge and we add an “ous” to the end to indicate the lower charge. Ex: Iron

  6. Stock System: • The charge of the cation is written in brackets as a roman numeral. Ex: Fe3+ would be iron (III) and Fe2+ would be iron (II). • Remember roman numerals: 1-(I), 2- (II), 3-(III), 4-(IV), 5-(V).

  7. Example: • Both CuO and Cu2O are real compounds • We know that O always has a charge of -2 • For CuO, we know that it is the Cu+2 ion (sum to zero)  copper (II) oxide • And for the Cu2O, we know that there is 2 x the Cu+1 ion (to sum to zero)  copper (I) oxide

  8. Try to write names for these (don’t forget the roman numberial for the metal) : • CrO • Au3P • SnCl4

  9. Given the name we can write the formula: • Nickel (III) bromide • We know that Br is always Br-1 • We also know that this is the Ni3+ ion (it tell us in the brackets) • Therefore we need 3 x Br-1 with Ni3+ for the compound to be neutral (sum to zero)  NiBr3

  10. Try these: • lead (II) chloride • mercury (I) arsenide • cobalt (II) chloride.

  11. Quote of the day: “Our young people aren’t so bad; it’s just they have more critics than models.” Anon

  12. Polyatomic Ions • Have a charge ( + or - ) • Consists of two or more non-metal atoms (or metal complex) joined by a covalent bond • Act as a single unit

  13. Polyatomic Ions • See your table of ions on the periodic table for a list • Please add ammonium: NH4+ to the list

  14. Write names for ionic compounds containing polyatomic ions: • Na2CO3 • KOH • Sn3(PO4)4

  15. Writing chemical formulas for ionic compounds containing polyatomic ions: (remember to use parentheses to indicate the correct number of ions) • ammonium sulfide • lead (IV) hydrogen carbonate • calcium hydroxide • magnesium nitrate

  16. Practice: handouts

  17. Give chemical formula: A) Nickel (III) bromide B) antimony (V) nitride C) platinum (II) phosphide D) lead (II) chloride E) mercury (I) arsenide F) cobalt (II) chloride. Practice: (use stock system)

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