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SCH3U Sample Chapter 2 Test This test may be longer than the test you get on Thursday. Thursday’s test also may contain questions of slightly different formats. The basic information will be the same. 1) How is an ordinary covalent bond different from a co-ordinate covalent bond. In a co-ordinate bond, both electrons come from the same atom. 2) Draw a Lewis diagram for the molecule HO. Label one of each of the following types of electrons: lone pair, bonded pair, and unpaired (3 points). 3) State whether the following bonds will be ionic, polar covalent, or covalent. If the bond is polar covalent or ionic, state which atom will have the partial or full negative charge. a) Br-S b) N-I c) O-O d) H-F non-polar polar non-polar polar 4) Use Lewis diagrams to show the molecules that would form between the following atoms. a) Cl & itself b) C & S c) O & I d) Si & Cl 5) Use Lewis diagrams to show how the following elements could combine to form ionic compounds and then give the formula that results. a) Li & I b) Ca & Br c) Rb & S LiI CaBr2 Rb2S 6) Draw a Lewis structure for the following molecule following the rules for complex molecules. Give the number of ordinary and co-ordinate covalent bonds present. PO33- There are no co-ordinate covalent bonds. 7) Give the Lewis structure, compound type (ionic, polar, non-polar), shape and shape code (if molecular), for each of the following. a) CH4 b) KI c) CH2F2 d) SO3 e) N2 non-polar ionic polar non-polar non-polar tetrahedral tetrahedral flat triangle diatomic AX4E0 AX4E0 AX3E0 AX1E1 (1 bond, but it is a triple bond) 2 single bond 1 double bond f) HCl polar diatomic AX1E3 g) BeH2 non-polar linear AX2E0 h) H2S polar bent AX2E2 i) HCN polar linear AX2E0 j) NH3 polar trigonal pyramid AX3E1 8) Identify one compound from question 7 that would have each of the following inter-particle forces. Chose a different compound for each force. a) ionic bonds b) London forces c) Hydrogen bonds d) dipole/dipole forces KI CH4 NH3 H2S 9) a) Give an example of a substance that would be held together entirely by covalent bonds. Diamonds, Quartz b) Give one physical property that would result from such a configuration. Very hard, high melting point. 10) Arrange the forces in question 8 and 9 in order from weakest to strongest (some may be the same). London forces; dipole/dipole forces; Hydrogen bonds; Covalent and Ionic 11) Which compound in each of the following pairs of compounds will have the higher melting point? Give the deciding factor in each case. a) NH3 and PH3 b) LiBr and SBr2 c) BCl3 and BCl2F d) C4H10 and C12H26 NH3; polar PH3 is not polar e) H2O and H2S H2O; H-bonds H2S dipole/dipole LiBr; ionic SBr2 is polar BCl2F; polar BCl3 is non-polar f) CO2 and HCN HCN; polar CO2 non-polar g) H2O and C45H92 C45H92 the large London forces are stronger than H2O H-bonds C12H26; larger molecule h) OCl2 and CO2 OCl2; polar CO2 is non-polar 12) Identify each of the following compounds as being soluble in water or soluble in cyclohexane (a non-polar solvent). a) O2 b) KCl c) C2H5OH d) C3H8 e) CCl4 f) NH3 cyclohexane non-polar water ionic water polar cyclohexane non-polar cyclohexane non-polar water polar You also should be able to generate chemical formulas given the compound name and to name a compound if given its formula. Questions 15, 16, and 17 on pages 103 and 104 are good practice for this. 15) a) NaHSO4 f) NaClO k) Al2O3 b) NaOH g) S8 l) KOH c) CO2 h) KNO3 m) H2CO3 d) HC2H3O2 i) H3PO4 e) not on our list j) I2 16) a) MgBr2 f) Ag2CO3 k) MgO p) Zn(ClO)2 u) NaClO z) BaCO3 b) CS2 g) Al(ClO4)3 l) N2O q) Pb(ClO4)4 v) OCl2 c) Hg(NO2)2 h) CuSO4 m) FeSO5 r) PBr5 w) SnBr2 d) HCl i) SO3 n) H2CO3 s) AsCl5 x) H2SO4 e) LiOH j) NiPO4 o) Ca(OH)2 t) Bi(NO3)3 y) KOH