CHEMISTRY – CHEMICAL PROCESSES
1.Briefly describe the tests for the following gases: (a) carbon dioxide turns limewater milky - precipitates (b) oxygen causes glowing splint to re-ignite (c) hydrogen causes burning splint to produce a pop sound.
2.Sketch a periodic table and label the main regions of the table. See pg 184
3.Draw Bohr diagrams for the following atoms: (a) boron (b) sulphur (c) calcium. [pic]
4.How many protons, neutrons, and electrons, do the following particles have: (a) C, (b) Fe, (c) Cl-1, (d) Ca+2, (e) N-3?
5.Use Bohr diagrams or Lewis dot diagrams to show how an ionic bond forms between sodium and chlorine. [pic]
6.Use Bohr diagrams or Lewis dot diagrams to draw the molecules produced when the following atoms join with each other: (a) fluorine joining with fluorine;; (b) carbon joining with hydrogen; (c) oxygen joining with hydrogen; (e) nitrogen joining with fluorine. In each case write the formula of the molecule produced.
(a) silver oxide(b) zinc fluoride(c) calcium chloride(d)strontium phosphide (e) barium iodide(f) sodium nitride(g) lead (II) chloride(h)tin(IV) fluoride (i) copper(I)sulfide(j) silver nitrate(k) lead (II) chlorate(l) calcium sulphate (m) sodium carbonate(n)copper(II)hydroxide (o) aluminum bicarbonate
8.Give the formula for the following compounds:
(a) sodium oxide Na2O(b) calcium nitride Ca3N2
(c) lithium iodide LiI(d) potassium phosphide K3P
(e) aluminum nitride AlN(f) sodium fluoride NaF
(g) iron(II) bromide FeBr2(h) copper(I) nitride Cu3N
(i) lead(II) oxide PbO(j) magnesium carbonate MgCO3
(k) tin(II) nitrate Sn(NO3)2(l) lead(IV) chlorate Pb(ClO3)4
(m) potassium sulphate K2SO4(n) calcium hydrogen carbonate
(o) calcium phosphate Ca3(PO4)2p)hydrochloric acid HCl(aq)
q) sulfuric acid H2SO4(aq)
9.Balance the following chemical equations:
(a)Cl2 + 2 KI ( 2 KCl + I2
(b)4 FeO + O2 ( 2 Fe2O3
(c)2 Al2O3 + 3 Si ( 3 SiO2 + 4 Al
(d)2 NaOH + H2SO4 ( Na2SO4 + 2 H2O
(e)2 K + 2 H2O ( 2 KOH + H2
(f)Ca + 2 HClO3 ( Ca(ClO3)2 + H2
(g)N2O5 + 3 Li2O ( 2 Li3NO4
(h)2 C2H6 + 7 O2 ( 4 CO2 + 6 H2O
(i)2 H3PO4 + 3 Sr(OH)2 ( Sr3(PO4)2 + 6 H2O
(j)B2(SO4)3 + 3 Mg(HCO3)2 ( 2 B(OH)3 + 6 CO2 + 3MgSO4 10.State the Law of Conservation of Mass. In any chemical reaction, the total mass of the reactants equals the total mass of the products
11.When 16.0 grams of sulphur is reacted with copper, 31.8 grams of copper is used up producing copper(II) sulphide. (a) Write out the word equation for this reaction.
Sulphur + copper ( copper (II) sulphide
(b) What is the mass of copper(II) sulphide produced? Show your work! 16 g + 31.8 g = 47.8 g
c) What type of reaction occurred? synthesis
12.List three observations that would indicate that a chemical reaction had occurred. Change in colour, precipitate forms, heat/light is produced or absorbed, gas produced
13.Name the four types of chemical reactions. Write the general form for each. Synthesis: A + B ( AB
Decomposition: AB ( A + B
Single displacement: A + BC ( AC + B
Double displacement: AB + CD ( AD + CB
14.What is (a) an endothermic reaction absorbs heat (b) an exothermic reaction releases heat
15.State (a) three properties of acids sour, react with metals and carbonates, conduct electricity (b) three properties of bases bitter, feel slippery, conduct electricity
16.What is the pH...