Ionic and Metallic Compounds Review Sheet
Remember to look over all homework, notes and daily questions. 1. Vocabulary to define a. anion b. cation c. ionic bond substance d. ionic compound ion with a negative charge; formed by gaining electrons ion with a positive charge; formed by losing electrons formed from the transfer of electrons from a metallic substance to a nonmetallic compound containing ionic bonds

e. metallic bond metal atoms donate valence electrons to the “sea” of electrons, which are able to move among all of the atoms; metallic cations are attracted to the sea of valence electrons 2. In terms of energy and electron configurations, explain why ionic bonds form. Atoms will gain or lose electrons to form the stable electron configuration of a noble gas; when atoms reach this configuration, they are in a lower energy state, making them stable 

3. On the periodic table above, write the charge that an element in each group will form. Column A – 1+ Column B – 2+ Column C – 3+ Column D – skip Column E – 3Column F – 2Column G – 1Column H - skip 4. Based on the periodic table shown: a. elements from columns A and E will combine in which ratio? b. elements from columns B and G will combine in which ratio? c. elements from columns B and C will combine in which ratio? d. elements from columns A and F will combine in which ratio? e. elements from columns C and F will combine in which ratio?

A3E BG2 They won’t. A2F C2F3

5. List and describe 3 properties about ionic compounds. a. Poor conductors of heat/electricity in the solid state, Good conductors of heat/electricity when dissolved in water i. When in solid state, they do not move and so they cannot transfer heat or electricity. b. They are hard and brittle, due to the strong attractive forces holding the ions together. c. They are found in a 3-d crystal lattice. i. All ions are surrounded by ions of the opposite charge.

6. Draw the formation of an ionic bond between the following elements using electron dot symbols. a. sodium and oxygen b. calcium and nitrogen c. lithium and chlorine

7. Write chemical formulas for the following ionic compounds. a. sodium nitrate NaNO3 b. aluminum chloride e. sodium phosphide f. magnesium nitrate AlCl3 Na3P Mg(NO3)2 PbSO3 Ca3(PO4)2 (NH4)2SO4

c. silver(I) sulfate d. iron(III) oxide k. aluminum sulfide l. beryllium chloride

Ag2SO4 Fe2O3 Al2S3 BeCl2 Cu3As GaN FeBr2

g. lead(II) sulfite h. calcium phosphate i. j. ammonium sulfate silver(I) cyanide

m. copper(I) arsenide n. gallium nitride o. iron(II) bromide

8. Name the following ionic compounds. a. TiSe titanium(II) selenide b. Cu2O c. V3P5 copper(I) oxide vanadium(V) phosphide

d. Co(ClO3)3 e. Pb(SO4)2 f. CuCrO4

cobalt(III) chlorate lead(IV) sulfate copper(I) chromate

g. (NH4)3PO4 h. Cu(NO2)2 i. j. KCN Zn3N2

ammonium phosphate copper(II) nitrite potassium cyanide zinc(II) nitride sodium permanganate

l.

Co3(PO4)2

cobalt(II) phosphate lithium oxide iron(III) acetate strontium hydroxide

m. Li2O n. Fe(C2H3O2)3 o. Sr(OH)2

k. NaMnO4

9. Using the model of metallic bonding, explain 2 properties of metals. a. High melting/boiling points – strong attraction between metallic cations and the delocalized electrons make it so that a lot of energy is required to separate the atoms b. Malleability [ability to be pounded into thin sheets] – a shift in the elements doesn’t change the attraction; look at figure 7.12 on page 226 c. Ductility [ability to be drawn into wires] – a shift in the elements doesn’t change the attraction; look at figure 7.12 on page 226 d. Conductivity as solid – electrons free to move as a current; delocalized electrons move heat from one place to another much more quickly than something that doesn’t contain mobile electrons [ionic or covalent compounds]