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Year 10 - Chemistry Revision

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Year 10 - Chemistry Revision Year 10 - Chemistry Revision 1) Name the following compounds: (a) PBr 3 (b) CBr 4 (c) Na 2SO 4 (d) Cu(NO 2)2 (e) CaCl 2 (f) Fe 2O3 (g) P2O5 (h) N2O3 (i) P3O6 (j) Mg 3(PO 4)2 (k) IF 5 (l) Li 2O (m) CuS (n) CrPO 4 (o) K 3N (p) Fe 2(CO 3)3 (q) (NH 4)3PO 4 (r) SnS (s) NaHSO 3 (t) NaC 2H3O2 (u) SnS 2 (v) N 2S3 (w) B 4H10 (x) PbCl 2 (y) Ag 3PO 4 (z) Ca(CN) 2 2) Write the formula for the following compounds. (a) Potassium chloride (b) Calcium nitrate (c) Silicon tetrachloride (d) Diphosphorus pentoxide (e) Lead (IV) sulfide (f) Dihydrogen sulfide (g) Carbon Tetrabromide (h) copper (I) sulfide (i) Tin (II) chloride (j) Dinitrogen Trihydride (k) Barium oxide (l) Aluminium sulfide (m) Zinc (II) phosphide (n) Iron (II) oxide (o) Potassium permanganate (p) Hydrogen Peroxide (q) Potassium dichromate (r) Tin (II) perchlorate (s) Diboron hexahydride (t) Titanium (IV) chloride 3) Write word equations and then balanced formula for the following reactions: (a) Magnesium burns in the presence of oxygen to produce magnesium oxide. (b) Aluminium metal reacts with chlorine gas to produce Aluminium chloride. (c) Electrolysis can be used to split water into hydrogen and oxygen. (d) Nitrogen dioxide gas dissolves in water to produce nitric acid (HNO 3) and nitrogen monoxide. (e) A solution of lead (II) nitrate is mixed with sodium phosphate to produce sodium nitrate and a precipitate of lead (II) phosphate. (f) Sodium metal ignites in the presence of chlorine gas to produce sodium chloride. (g) Mercury (II) oxide decomposes into mercury and oxygen. (h) Aluminium metal is displaced by copper (II) sulfate solution producing copper metal and aluminium sulfate. (i) Gallium is heated in the presence of oxygen gas to produce gallium (III) oxide. (j) Aluminium sulfate reacts with sodium hydroxide to produce an aluminium hydroxide precipitate and sodium sulfate. (k) Nitrogen triiodine explodes to produce nitrogen gas and iodine gas. (l) Potassium permanganate reacts violently with hydrogen peroxide to produce potassium peroxide, manganese (IV) oxide, water and oxygen gas. 4) Determine what type of reaction each reaction is in question 3 (exclude d and l). 5) Determine the number of electrons, proton and neutrons in each of the following. (a) C (b) S (c) Fe (d) Na (e) Be 2+ (f) Ca (g) Ca 2+ (h) O (i) I - (j) Mg 2+ (k) Na + (l) S 2- 6) What is an isotope? 7) (a) Distinguish between ionic, covalent and metallic bonding. (b) The following table shows the properties of ionic, covalent and metallic substances. Property Ionic Covalent Metallic Melting and Boiling Point High Low High Malleability Brittle Soft Soft Conductivity None as solid None High High in solution (i) Why are metals able to conduct electricity? (ii) Explain why metals are malleable and ductile. (iii) Explain why ionic compounds can only conduct electricity when dissolved in solution. (iv) *Challenge* Explain why ionic compounds are brittle. 8) Why noble gases are said to be inert (stable)? 9) (a) What is the difference between an endothermic and an exothermic reaction? (b) *Challenge* Is the breaking of chemical bonds an endothermic or an exothermic process? What about the formation of new bonds? 10) Distinguish between elements, compounds and mixtures. 11) On the periodic table: a) Label the group numbers. b) Shade the transition metals blue. c) Shade the metalloids green. d) Shade the non-metals yellow. e) Identify the valency of each group. Answers 1) (a) Phosphorous tribromide (b) carbon tetrabromide (c) sodium sulfate (d) copper (I) nitrite (e) calcium chloride (f) iron (III) oxide (g) diphosphorous pentaoxide (h) dinitrogen trioxide (i) triphosphorous hexaoxide (j) magnesium phosphate (k) iodine pentafluoride (l) lithium oxide (m) copper (II) sulfide (n) chromium phosphate (o) potassium nitride (p) iron (III) carbonate (q) ammonium phosphate (r) tin (II) sulfide (s) sodium hydrogen sulfite (t) sodium acetate (u) tin (IV) sulfide (v) dinitrogen trisulfide (w) tetraboron decahydride (x) lead (II) chloride (y) silver (I) phosphate (z) calcium cyanide 2) (a) KCl (b) Ca(NO 3)2 (c) SiCl 4 (d) P2O5 (e) PbS 2 (f) H 2S (g) CB 4 (h) Cu 2S (i) SnCl 2 (j) N 2H3 (k) BaO (l) Al 2S3 (m) Zn 3(PO 3)2 (o) KMnO 4 (p) H 2O2 (q) K 2Cr 2O7 (r) Sn(ClO 4)2 (s) B 2H6 (t) TiCl 4 3) a) Magnesium + oxygen magnesium oxide 2Mg + O 2 2MgO b) Aluminium + chlorine Aluminium chloride 2Al + 3Cl 2 2AlCl 3 c) water hydrogen + oxygen 2 H 2O 2H 2 + O2 d) nitrogen dioxide + water nitric acid + nitrogen monoxide 3NO 2 + H2O 2HNO 3 + NO e) lead (II) nitrate + sodium phosphate sodium nitrate + lead (II) phosphate 3Pb(NO 3)2 + 2Na 3PO 4 6NaNO 3 + Pb 3(PO 4)2 f) sodium + chlorine sodium chloride 2Na + Cl 2 2NaCl g) Mercury (II) oxide mercury + oxygen 2HgO 2Hg + O 2 h) Aluminium + copper (II) sulfate copper + aluminium sulfate 2Al + 3CuSO 4 3Cu + Al 2(SO 4)3 i) Gallium + oxygen gallium (II) oxide 2Ga + O2 2GaO j) Aluminium sulfate + sodium hydroxide Aluminium hydroxide + sodium sulfate Al 2(SO 4)3 + 6NaOH 2Al(OH) 3 + 3Na 2SO 4 k) nitrogen triiodide nitrogen + iodine 2NI 3 N2 + 3I2 l) Potassium permanganate + hydrogen peroxide potassium peroxide + manganese (IV) oxide + water + oxygen 2KMnO 4 + 2H 2O2 K2O2 + 2MnO 2 + 2H 2O + 2O 2 4) a) combination b) combination c) decomposition e) double replacement f) combination g) decomposition h) single replacement i) combination j) double replacement (k) decomposition .
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