3. take the amount of charge (again, ignoring the sign) from the negative ion and make this the subscript…

3. take the amount of charge (again, ignoring the sign) from the negative ion and make this the subscript for the positive ion in the formula. 4. the subscripts represent a ratio, so they should be expressed in lowest terms. for example, when writing the formula for magnesium oxide (mgo), the amount of charge for mg and o is the same. to express this in lowest terms, you divide by two. again, remember that you do not write subscripts of 1. writing the chemical formula for magnesium chloride determine the subscripts by “crossing over” the amount of charge from each ion. remember that you do not write the number 1. practice 1. write the formula for the compound formed by each pair of elements. a. gold(iii) and nitrogen b. copper(ii) and sulfur c. tin(ii) and chlorine d. lead(iv) and oxygen 2. write the names of the following binary ionic compounds. a. aucl3 b. pbo2 c. cu2o d. ascl3 on science 10 blackline masters blm 4 - 6 multivalent ionic compounds copyright © 2010 mcgraw - hill ryerson lim 978 - 0 - 07 - 031859 - 5

3. take the amount of charge (again, ignoring the sign) from the negative ion and make this the subscript for the positive ion in the formula. 4. the subscripts represent a ratio, so they should be expressed in lowest terms. for example, when writing the formula for magnesium oxide (mgo), the amount of charge for mg and o is the same. to express this in lowest terms, you divide by two. again, remember that you do not write subscripts of 1. writing the chemical formula for magnesium chloride determine the subscripts by “crossing over” the amount of charge from each ion. remember that you do not write the number 1. practice 1. write the formula for the compound formed by each pair of elements. a. gold(iii) and nitrogen b. copper(ii) and sulfur c. tin(ii) and chlorine d. lead(iv) and oxygen 2. write the names of the following binary ionic compounds. a. aucl3 b. pbo2 c. cu2o d. ascl3 on science 10 blackline masters blm 4 - 6 multivalent ionic compounds copyright © 2010 mcgraw - hill ryerson lim 978 - 0 - 07 - 031859 - 5

Answer

Explanation:

Step1: Determine ion charges

  • Gold(III) ion ($Au^{3 +}$) has a charge of + 3, nitrogen ion ($N^{3 -}$) has a charge of - 3. Crossing - over charges gives $AuN$.
  • Copper(II) ion ($Cu^{2+}$) has a charge of + 2, sulfur ion ($S^{2 -}$) has a charge of - 2. Crossing - over charges gives $CuS$.
  • Tin(II) ion ($Sn^{2+}$) has a charge of + 2, chlorine ion ($Cl^{-}$) has a charge of - 1. Crossing - over charges gives $SnCl_{2}$.
  • Lead(IV) ion ($Pb^{4+}$) has a charge of + 4, oxygen ion ($O^{2 -}$) has a charge of - 2. Dividing by 2 (to get lowest terms), gives $PbO_{2}$.

Step2: Name ionic compounds

  • For $AuCl_{3}$, gold has a + 3 charge, so it is gold(III) chloride.
  • For $PbO_{2}$, lead has a + 4 charge, so it is lead(IV) oxide.
  • For $Cu_{2}O$, copper has a + 1 charge here, so it is copper(I) oxide.
  • For $AsCl_{3}$, arsenic has a + 3 charge, so it is arsenic(III) chloride.

Answer:

a. $AuN$ b. $CuS$ c. $SnCl_{2}$ d. $PbO_{2}$ 2. a. gold(III) chloride b. lead(IV) oxide c. copper(I) oxide d. arsenic(III) chloride