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Name: Date: Group: UNIT 0 Review 1. Structure of the Atom. atomic number a) All elements of the same type have the same _______________ ________________. protons b) This number represents the amount of positively (+) charged ___________________ electrons and negatively () charged _____________________ in the atom. c) Neutrally charged particles, which keep an atom stable, are called proton neutrons _____________________. They have the same mass as a ___________________________. d) In general on periodic table elements in the same column have the same number family (group) valence of ____________________ electrons and are in the same __________________. electron shells e) Elements in a row have the same number of ______________ _________________ and are period in the same _______________________. Atomic number Atomic Mass (AMU Atomic # Protons Electrons Valence Electrons Preferred Ion Atomic Mass Neutrons Aluminum 13 13 13 3 Al 3+ 26.981 14 Potassium 19 Chlorine 17 19 17 19 17 1 7 K+ Cl 39.098 35.453 20 18 Draw the BohrRutherford Diagram for: a) Carbon b) Lithium 2. Ionic Bonds c) Phosphorous a) This type of _________________________ molecular force forms between a intrametal non-metal ___________________________ and a ____________________________. oppositely b) The bond forms between two ______________________________ charged ions. Electrons are ____________________________ by the more electronegative atom. Stolen Cation c) A positive ion is known as a ________________________. A negative ion is known as an Anion _____________________________. high Crystalline d) Ionic compounds form ____________________________ structures with _______________ melting points and _________________ boiling points. high Conduct e) When dissolved in water ionic compounds _______________________ into electricity _________________. 3. Covalent Bonds share a) In covalent bonds the atoms _______________________ electrons to form stable octet electron shells that satisfy the ________________________ rule. non-metals b) This type of bond occurs between two ______________________________. covalent c) All organic molecules contain ________________________ bonds. Covalent compounds not conduct do _________________________________ electricity. Polyatomic ions d) _______________________________________________ are charged molecules containing covalent bonds. F-F Single e) A _________________ bond is used when atoms share 2 electrons: __________ O=0 Double f) A _________________ bond is used when atoms share 4 electrons: ___________ Triple N (three lines) N g) A _________________ bond is used when atoms share 6 electrons: __________ 4. Naming Compounds: Possible Prefixes: 1 Mono 3 Tri 5 Penta 7 2 4 Tetra 6 Hexa 8 Di Hepta Octa 9 10 Deca 5. Writing Chemical Formulas: EX. Lithium Oxide Step 1 Write the chemical symbols for each element with the metal first. Step 2 Write the ionic charges above each symbol Nona Step 3 Crossover the ionic charges and write them below, removing the (+ or ) Step 4 Simplify the numbers ( if necessary). Remove the “1’s”. Activities: 1) Write the names for the following covalent compounds: Phosphorus Pentasulfide a) P4S 5Tetra ___________________________________________________ Oxygen b) O2 ___________________________________________________ Sellinium hexafluoride c) SeF6 ________________________________________________ Disilicon hexabromide d) Si2Br 6 _______________________________________________ sulfur tetrachloride e) SCl4 ________________________________________________ methane (carbon tetrahydride) f) CH4 ________________________________________________ Diboron monosilicide g) B2Si _______________________________________________ 2) Write the formulas for the following covalent compounds: SbBr3 a) antimony tribromide __________________________________ b) hexaboron silicide _____________________________________ c) chlorine dioxide _______________________________________ d) hydrogen iodide _______________________________________ e) iodine pentafluoride __________________________________ f) dinitrogen trioxide ____________________________________ g) ammonia(nitrogen trihydride) _______________________ h) phosphorus triiodide __________________________________ 3) Write the formulas for the following ionic compounds. MgO a) magnesium oxide __________________ c) aluminum nitride __________________ e) potassium sulfide __________________ g)calcium bromide __________________ i) sodium sulfide __________________ k) beryllium oxide __________________ SnF2 b) tin (II) fluoride _________________ d) lead (IV) nitride _________________ f) iron (III) chloride _________________ h) copper (I) oxide _________________ j) antimony (III) sulfide _____________ l) mercury (II) oxide ________________ 5. Write the names for the following compounds. Lithium Oxide a) Li2O _____________________________ chloride b) AlCl3Aluminum ____________________________ Magnesium Sulfide c.) MgS _____________________________ Calcium Fluoride d) CaF2_____________________________ oxide e.) Al2O _____________________________ 3 Aluminum Beryllium fluoride f.) BeF2 ______________________________ Potassium Phosphide g) K3P ______________________________ Water g) H2O ______________________________ Lead (II) sulfide j) PbS _____________________________ Tin (IV) oxide k) SnO2 _____________________________ Nickle (II) oxide l). NiO _____________________________ Copper Iodide m) CuI2 _____________________________ n) PbCl4 ____________________________ Lead (IV) chloride Iron (II) phosphate o) FeP _____________________________ (III) bromide p) AuBr3Gold ___________________________ p) NH3Ammonia _____________________________ homework: pg. 4#1 pg. 5#3abc,4, 5 pg.12 #9
