Review - Mr. Swan`s Class
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Mr. Swan Name: __________________ GRADE 10 CHEMISTRY REVIEW C1 - Student’s must be able to use the periodic table to determine the number of valence electrons an element has, and predict the way elements would combine with each other by gaining, losing, or sharing electrons. 1) Draw Bohr model diagrams for the following atoms (neutral charge) or ions (+ or - charge) Lithium atom Oxygen ion Neon atom Magnesium ion Silicon atom Chlorine ion 2) Draw Lewis dot diagrams for the following atoms or ions Beryllium atom Nitrogen ion Fluorine ion Sodium ion Aluminium ion Argon atom Mr. Swan Name: __________________ 3) Determine the number of valence electrons present on the following elements Carbon ______ Magnesium ______ Phosphorus ______ Oxygen ______ Bromine ______ Helium ______ Neon ______ Strontium ______ Chlorine ______ Sulfur ______ Boron ______ Potassium ______ 4) Identify those elements that want to… lose/gain electrons Lose 1 e- Lose 2 e- Lose 3 e- Gain 3 e- Gain 2 e- Gain 1 e- 5) Identify a good partner for each of the following elements; and draw Lewis dot diagrams of them Lithium Magnesium Nitrogen Oxygen Chlorine Aluminum Mr. Swan Name: __________________ C2 - Student’s must be able to demonstrate an understanding of molecular compounds by determining the ratios that they combine to form compounds, writing formulas, and naming compounds 1) Describe a molecular compound. (What elements are involved? What happens to electrons?) 2) One oxygen forms a compound with an unknown number of chlorine; draw the resulting Lewis dot diagram of the compound. (What ions will oxygen and chlorine form? How many electrons does oxygen need to share?) 3) One nitrogen forms a compound with an unknown number of fluorine; draw the resulting Lewis dot diagram of the compound. 4) One selenium forms a compound with an unknown number of phosphorus; draw the resulting Lewis dot diagram of the compound. 5) Write the name for each of the following molecular compounds Mono Di Tri Tetra Penta Hexa CO2 _____________________________________ N2O3 _____________________________________ CO _____________________________________ PCl5 _____________________________________ PBr3 _____________________________________ NH3 _____________________________________ SO3 _____________________________________ P2O5 _____________________________________ N2O _____________________________________ SCl6 _____________________________________ Mr. Swan Name: __________________ 6) Write the chemical formula for each of the following molecular compounds Hydrogen iodide _______________________ Arsenic tribromide _______________________ Chlorine dioxide _______________________ Hexaboron silicide _______________________ Phosphorus triiodide_______________________ Phosphorus pentabromide _______________________ Dinitrogen trioxide Selnium tetrachloride _______________________ _______________________ C3 - Student’s must be able to demonstrate an understanding of ionic compounds by determining the ratios they combine to form compounds, writing formulas, and naming compounds 1) Describe an ionic compound. (What elements are involved? What happens to electrons?) 2) One sodium forms a compound with an unknown number of chlorine; draw the resulting Lewis dot diagram of the compound. (What ions will sodium and chlorine form? How many of each will be required to produce a neutral compound?) 3) One calcium forms a compound with an unknown number of bromine; draw the resulting Lewis dot diagram of the compound. 4) One aluminum forms a compound with an unknown number of sulfur; draw the resulting Lewis dot diagram of the compound. Mr. Swan Name: __________________ 5) One copper (transition metal) forms a compound with 2 chlorine number of chlorine; draw the resulting Lewis dot diagram of the compound. 6) One titanium (transition metal) forms a compound with 2 oxygen number of chlorine; draw the resulting Lewis dot diagram of the compound. 7) Name each of the following ionic compounds (Identify those compounds that have transition metals? You must specify the charge on the metal with a roman numeral) (I) + One (II) + Two (III) + Three (IV) + Four (V) Na3N _____________________________________ PbS _____________________________________ KBr _____________________________________ MnF2 _____________________________________ BeF2 _____________________________________ AlCl3 _____________________________________ CaS _____________________________________ CuCl2 _____________________________________ NiO _____________________________________ FeBr3 _____________________________________ + Five 8) Write the chemical formula for each of the following ionic compounds (Roman numeral represents charge) Magnesium oxide _______________________ Sodium fluoride _______________________ Potassium sulfide _______________________ Tin (IV) sulfide _______________________ Lithium iodide _______________________ Lead (II) oxide _______________________ Magnesium Nitride _______________________ Copper (I) Bromide _______________________ Mr. Swan Name: __________________ C4 - Student’s must be able to demonstrate an understanding of chemical reaction by balancing and classifying different reaction types. 1) Describe how the chemical reactions below are similar and different. Explain why only one reaction abides by the Law of conservation of mass. (What elements are involved? How many of each are present before the reaction? What about after the reaction?) A) B) 2) Balance each of the following chemical equations Al + N2 Fe + O2 KI + Cl2 BaO2 CH4 + ZnS + Na Fe Cl2 O2 → → FeCl3 Fe3O4 → KCl + I2 → BaO → CHCl3 → ZnO → H2 -→ FeCl2 + H2O + AlN + O2 + + + HCl SO2 NaOH 3) Write the chemical equation for each of the following word equations; then balance Chlorine + potassium bromide → potassium chloride and bromine zinc sulfide + oxygen → . zinc oxide + sulfur dioxide Calcium + oxygen → calcium oxide Mr. Swan Magnesium bromide + chlorine Name: __________________ → magnesium chloride + bromine Iron(III) oxide + carbon monoxide → iron + carbon dioxide 4) Label each of the following diagrams as a type of chemical reaction. (Synthesis, Decomposition, Single Displacement, Double Displacement) is a _____________________ reaction is a ____________________ reaction is a ____________________ reaction is a _____________________ reaction 5) Label each of the following as a type of chemical reaction. (S, D, S.D., D.D.) ________ CO2 → C + O2 ________ NaCl + AgNO3 → NaNO3 + AgCl ________ S + Cl2 → SCl2 ________ 2C2H2 + 5O2 ________ CH4 ________ Mg + ________ 2O2 + N2 ________ 3CaBr2 + 2Na3P → Ca3P2 ________ 2KI + Br2 ________ C6H12O6 → ________ 2NaF 2Na + F2 ________ Si + O2 ________ CS2 + 2F2 ________ NaI + Cs → CsI + Na → → 4CO2 + 2 H2O C + 2H2 2 HCl → → N2O4 → → → MgCl2 + H2 2KBr + I2 6C + 6H2O SiO2 → CF4 + 2S + 6NaBr Mr. Swan 6) Predict the reaction products for the following reactions by a. identifying the type of reaction b. writing the products for the reactions potassium + iodine zinc oxide sodium iodide + chlorine barium chloride + lithium sulfate iron(III) oxide + hydrogen Name: __________________
