UNIT 0 – Review, The Structure of the Atom, Bonds and Naming 6. Naming Covalently Bonded Compounds a) carbon dioxide _____________ b) nitrogen monoxide __________ c) sulfur trioxide _____________ d) antimony tribromide_____________ e) chlorine dioxide __________________ f) hydrogen iodide_________________ g) iodine pentafluoride _____________ h) water _________________ i) ammonia __________________ j) sulfur hexafluoride _____________ 7. Write the names for the following covalent compounds a) P4S5 ___________________________________________________________ b) O2 _____________________________________________________________ c) SeF6 ____________________________________________________________ d) Si2Br6 __________________________________________________________ e) SCl4 _____________________________________________________________ f) NF3 ______________________________________________________________ g) CH4 ______________________________________________________________ 8. Complete the table for the common polyatomic ions. Pg. 422 Formula Name Formula Name Phosphate OH-­‐ SO42-­‐ Sulphate Permanganate 2-­‐
2-­‐
CO3 C2O4 Oxalate Nitrate SiO32-­‐ NO2-­‐ Ammonium -­‐
Perchlorate HCO3 Chlorate Cyanide Cr2O72-­‐ C2H3O2-­‐ UNIT 0 – Review, The Structure of the Atom, Bonds and Naming 9. Name the following polyatomic ions listed below a) NaOH _______________________________________ b) NaClO3 ______________________________________ c) NaC2H3O2 ____________________________________ d) Ca(OH)2 _____________________________________ e) BaSO4 _______________________________________ f) ZnCO3 _______________________________________ g) AlPO4 _______________________________________ h) AgNO3 _______________________________________ i) K2C2O4 _______________________________________ j) (NH4)2SO4 ____________________________________ k) Na2SO4 ______________________________________ l) KNO3 ________________________________________ 10. Write the names for the following polyatomic ions. Use Table 8.10 on page 422 a) sodium nitrate _______________ b) potassium acetate _____________ c) aluminum sulfate _____________ d) lithium chlorate ______________ e) magnesium nitrate____________ f) ammonium acetate _____________ g) silver nitrate___________________ h) sodium hydroxide _____________ UNIT 0 – Review, The Structure of the Atom, Bonds and Naming 11. List the 7 diatomic gases 12. Lewis Bonding Diagrams (1) Count up the total number of valence electrons you have to work with. (2) Try forming all single bonds with all atoms involved first (include your lone pairs). Make sure you follow the octet rule with all atoms (remember exceptions). (3) Count the number of electrons you used. If the number is the same as your count in step (1), you are done. If you have counted more electrons than the number in step (1), you must begin forming multiple bonds. (1)NH3 (2)O2 (3)CF4 (4)CO (5)SI2 (6)BCl3 (7)BeBr2 (8)PF3 (9)C2H4 UNIT 0 – Review, The Structure of the Atom, Bonds and Naming 13. Families in the Periodic Table Label these families on the periodic table by filling in the element symbols and labeling it with the family name. The families include; Alkali metals, earth alkaline metals, transition metals, halogens, and nobel gases. Below, list 3 properties for each family. Homework pg. 29 # 39041