1. Science 10 Review Part 1: Chemical Compounds

2. Ionic Compounds

3. Metal and non-metal combination

5. Ionic Compounds Metal and non-metal combination

6. Ionic Compounds Metal and non-metal combination Contains charged ions (atoms or group of atoms that have lost or gained electrons) e.g O 2-, PO 4 3- K +, NH 4 +

7. Ionic Compounds Metal and non-metal combination Contains charged ions (atoms or group of atoms that have lost or gained electrons) e.g O 2-, PO 4 3- K +, NH 4 + Ionic bond forms as a result of electron transfer.

8. Ionic bond is a force of attraction between positive and negative ions

9. Cu 2+ O 2-

10. Ionic bond is a force of attraction between positive and negative ions E.g. CuO, NaHC 2 O 4 Cu 2+ O 2-

11. Ionic bond is a force of attraction between positive and negative ions E.g. CuO, NaHC 2 O 4 Ionic compounds form 3D crystals that contain many ions Cu 2+ O 2-

12. Ionic bond is a force of attraction between positive and negative ions E.g. CuO, NaHC 2 O 4 Ionic compounds forms 3D crystals that contain many ions CuO, a formula unit, represents the lowest ratio of positive to negative ions Cu 2+ O 2-

13. Molecular compounds

14. Non-metal and non-metal combination

16. Molecular compounds Non-metal and non-metal combination

17. Molecular compounds Non-metal and non-metal combination Form molecules

18. Molecular compounds Non-metal and non-metal combination Form molecules Contain covalent bonds that result from electron sharing

19. Molecular compounds Non-metal and non-metal combination Form molecules Contain covalent bonds that result from electron sharing E.g. CH 4, SO 2

21. Acids, Bases and Salts

22. Acids are molecular compounds that contain hydrogen atoms. They produce the H + ion.

23. Acids, Bases and Salts Acids are molecular compounds that contain hydrogen atoms. They produce the H + ion. E.g. HCl = hydrochloric acid H 2 SO 4 = sulphuric acid

24. Acids, Bases and Salts Acids are molecular compounds that contain hydrogen atoms. They produce the H + ion. E.g. HCl = hydrochloric acid H 2 SO 4 = sulphuric acid Bases contain the hydroxide ion, OH - E.g NaOH

25. Acids, Bases and Salts Acids are molecular compounds that contain hydrogen atoms. They produce the H + ion. E.g. HCl = hydrochloric acid H 2 SO 4 = sulphuric acid Bases contain the hydroxide ion, OH - E.g NaOH Salts are ionic compounds that form from reacting acids and bases. E.g. NaCl

26. Phase Symbols

27. Are subscripts that indicate the phase of the chemical

28. Phase Symbols Are subscripts that indicate the phase of the chemical E.g (s) solid state; Fe (s)

29. Phase Symbols Are subscripts that indicate the phase of the chemical E.g (s) solid state; Fe (s) (l) liquid state; H 2 O (l)

30. Phase Symbols Are subscripts that indicate the phase of the chemical E.g (s) solid state; Fe (s) (l) liquid state; H 2 O (l) (g) gaseous state; O 2 (g)

31. Phase Symbols Are subscripts that indicate the phase of the chemical E.g (s) solid state; Fe (s) (l) liquid state; H 2 O (l) (g) gaseous state; O 2 (g) (aq) means aqueous or substance is dissolved in water; NaCl ( aq)

32. Dissociation equations

33. All ionic compounds and acids dissociate or break up into ions when dissolved in water Dissociation equations

34. All ionic compounds and acids dissociate (break up into ions) when dissolved in water E.g. Ca and NO 2 Polyatomic ion Dissociation equations

35. All ionic compounds and acids dissociate or break up into ions when dissolved in water E.g. Ca and NO 2 Ca 2+ Dissociation equations

36. All ionic compounds and acids dissociate or break up into ions when dissolved in water E.g. Ca and NO 2 Ca 2+ NO 2 - Dissociation equations

37. All ionic compounds and acids dissociate or break up into ions when dissolved in water E.g. Ca and NO 2 Ca 2+ NO 2 - NO 2 - Dissociation equations

38. All ionic compounds and acids dissociate or break up into ions when dissolved in water E.g. Ca and NO 2 Ca 2+ NO 2 - NO 2 - Ca(NO 2 ) 2(s) Dissociation equations

39. All ionic compounds and acids dissociate or break up into ions when dissolved in water E.g. Ca and NO 2 Ca 2+ NO 2 - NO 2 - Ca(NO 2 ) 2(s) calcium nitrite Dissociation equations

40. All ionic compounds and acids dissociate or break up into ions when dissolved in water E.g. Ca and NO 2 Ca 2+ NO 2 - NO 2 - Ca(NO 2 ) 2(s) Ca 2+ calcium nitrite Dissociation equations

41. All ionic compounds and acids dissociate or break up into ions when dissolved in water E.g. Ca and NO 2 Ca 2+ NO 2 - NO 2 - Ca(NO 2 ) 2(s) Ca 2+ + calcium nitrite Dissociation equations

42. All ionic compounds and acids dissociate or break up into ions when dissolved in water E.g. Ca and NO 2 Ca 2+ NO 2 - NO 2 - Ca(NO 2 ) 2(s) Ca 2+ + 2 NO 2 - calcium nitrite Dissociation equations

43. All ionic compounds and acids dissociate or break up into ions when dissolved in water E.g. Ca and NO 2 Ca 2+ NO 2 - NO 2 - Ca(NO 2 ) 2(s) Ca 2+ (aq) + 2 NO 2 - calcium nitrite Dissociation equations

44. All ionic compounds and acids dissociate or break up into ions when dissolved in water E.g. Ca and NO 2 Ca 2+ NO 2 - NO 2 - Ca(NO 2 ) 2(s) Ca 2+ (aq) + 2 NO 2 - (aq) calcium nitrite Dissociation equations

45. E.g. Ga and S Ga 3+ S 2-

46. S 2-

47. E.g. Ga and S Ga 3+ S 2- Ga 3+ S 2-

48. E.g. Ga and S Ga 3+ S 2- Ga 3+ S 2- S 2-

49. E.g. Ga and S Ga 3+ S 2- Ga 3+ S 2- S 2- Ga 2 S 3(s)

50. E.g. Ga and S Ga 3+ S 2- Ga 3+ S 2- S 2- Ga 2 S 3(s) 2 Ga 3+ (aq)

51. E.g. Ga and S Ga 3+ S 2- Ga 3+ S 2- S 2- Ga 2 S 3(s) 2 Ga 3+ (aq) + 3 S 2- (aq)

52. E.g. Ga and S Ga 3+ S 2- Ga 3+ S 2- S 2- Ga 2 S 3(s) 2 Ga 3+ (aq) + 3 S 2- (aq) gallium sulphide ending change to ide

53. Science 10 Review Part 2: Balancing Equations

54. Study Guide p. 110 Writing and Balancing Chemical Equations Step 1 Write chemical equation with phase symbols if not already done.

55. Study Guide p. 110 Writing and Balancing Chemical Equations Step 1 Write chemical equation with phase symbols if not already done. e.g. Al (s) + I 2(g)  AlI 3(s)

56. Study Guide p. 110 Step 2 Assign every chemical species a coefficient of ONE.

57. Study Guide p. 110 Step 2 Assign every chemical species a coefficient of ONE.

58. Study Guide p. 110 Step 2 Assign every chemical species a coefficient of ONE. e.g. __Al (s) + __ I 2(g)  __ AlI 3(s)

59. Study Guide p. 110 Step 2 Assign every chemical species a coefficient of ONE. e.g. 1 Al (s) + 1 I 2(g)  1 AlI 3(s)

60. Study Guide p. 110 Step 3 Count the number of each atom on reactant and product side of equation (multiply coefficient and subscript).

61. Study Guide p. 110 Step 3 Count the number of each atom on reactant and product side of equation (multiply coefficient and subscript). Al 2 (SO 3 ) 3

62. Study Guide p. 110 Step 3 Count the number of each atom on reactant and product side of equation (multiply coefficient and subscript). Al 2 (SO 3 ) 3 2 Aluminum 3 Sulphur 9 Oxygen

63. Study Guide p. 110 Step 3 Count the number of each atom on reactant and product side of equation (multiply coefficient and subscript). Al 2 (SO 3 ) 3 3 Al 2 (SO 3 ) 3 2 Aluminum 3 Sulphur 9 Oxygen

64. Study Guide p. 110 Step 3 Count the number of each atom on reactant and product side of equation (multiply coefficient and subscript). Al 2 (SO 3 ) 3 3 Al 2 (SO 3 ) 3 6 Aluminum 9 Sulphur 27 Oxygen 2 Aluminum 3 Sulphur 9 Oxygen

65. e.g. __Al (s) + __ I 2(g)  __ AlI 3(s) Study Guide p. 110 Step 4 Increase or change the coefficients to make numbers of atoms balance on both sides of equation. 3 22

66. Study Guide p. 110 Step 5 Always double check your answer. Reactants Al = 2 I = 6 Products Al = 2 I = 6 e.g. __Al (s) + __ I 2(g)  __ AlI 3(s) 3 22

67. Helpful Hints: Balance elements in elemental form (Fe, O 2, S 8, P 4 ) last. Study Guide p. 110

68. Helpful Hints: Balance elements in elemental form (Fe, O 2, S 8, P 4 ) last. Balance polyatomic ions (e.g. SO 4 2- ) as a group if they don’t break apart. Study Guide p. 110

69. Helpful Hints: Balance elements in elemental form (Fe, O 2, S 8, P 4 ) last. Balance polyatomic ions (e.g. SO 4 2- ) as a group if they don’t break apart. Balance oxygen and hydrogen last. Study Guide p. 110

70. __C 8 H 18(s) + __ O 2(g)  __ CO 2(g) + __ H 2 O (g) 25 9 8 16 Oxygen 9 25 Oxygen + Example: 50 Oxygen Must double all other coefficients

71. __C 8 H 18(s) + __ O 2(g)  __ CO 2(g) + __ H 2 O (g) 25 9 8 50 Oxygen 16 Carbon 36 Hydrogen Example: 216 18 50 Oxygen 16 Carbon 36 Hydrogen

72. Science 10 Review Part 3: Names & Formulas of Compounds

73. Formulas of Ionic Compounds

74. Roman Numeral in name indicates ion charge

75. Formulas of Ionic Compounds Roman Numeral in name indicates ion charge e.g mercury (II) phosphate

76. Formulas of Ionic Compounds Roman Numeral in name indicates ion charge e.g mercury (II) phosphate Hg 2+ PO 4 3-

77. Formulas of Ionic Compounds Roman Numeral in name indicates ion charge e.g mercury (II) phosphate Hg 2+ PO 4 3- Hg 2+

78. Formulas of Ionic Compounds Roman Numeral in name indicates ion charge e.g mercury (II) phosphate Hg 2+ PO 4 3- Hg 2+ PO 4 3-

79. Formulas of Ionic Compounds Roman Numeral in name indicates ion charge e.g mercury (II) phosphate Hg 2+ PO 4 3- Hg 2+ PO 4 3- Hg 2+

80. Formulas of Ionic Compounds Roman Numeral in name indicates ion charge e.g mercury (II) phosphate Hg 2+ PO 4 3- Hg 3 (PO 4 ) 2 Hg 2+ PO 4 3- Hg 2+

81. Naming Ionic Compounds

82. Must use a roman numeral to indicate the charge of metal ions with more than one possible ion charge

83. Naming Ionic Compounds Must use a roman numeral to indicate the charge of metal ions with more than one possible ion charge e.g Cr 2 O 3 +3 or +2

84. Naming Ionic Compounds Must use a roman numeral to indicate the charge of metal ions with more than one possible ion charge e.g Cr 2 O 3 Cr Cr +3 or +2

85. Naming Ionic Compounds Must use a roman numeral to indicate the charge of metal ions with more than one possible ion charge e.g Cr 2 O 3 Cr O 2- Cr O 2- O 2- +3 or +2

86. Naming Ionic Compounds Must use a roman numeral to indicate the charge of metal ions with more than one possible ion charge e.g Cr 2 O 3 Cr 3+ O 2- Cr 3+ O 2- O 2- +3 or +2

87. Naming Ionic Compounds Must use a roman numeral to indicate the charge of metal ions with more than one possible ion charge e.g Cr 2 O 3 Cr 3+ O 2- Cr 3+ O 2- O 2- +3 or +2 chromium (III) oxide

88. A roman numeral is not required when a metal has only one ion charge

89. e.g K 2 SO 4

90. A roman numeral is not required when a metal has only one ion charge e.g K 2 SO 4 +1 only

91. A roman numeral is not required when a metal has only one ion charge e.g K 2 SO 4 potassium sulphate +1 only

92. Formulas of Molecular Compounds

93. Binary compounds use prefix system to indicate the number atoms of each element

94. Formulas of Molecular Compounds Binary compounds use prefix system to indicate the number atoms of each element The element furthest to the left or farthest down the periodic table is written first

95. Greek prefixes 1 – mono 6 - hexa 2 – di 7 - hepta 3 – tri8 - octa 4 – tetra 9 - nona 5 – penta 10 - deca

96. Formulas of Molecular Compounds

97. sulphur dioxide

98. Formulas of Molecular Compounds sulphur dioxide SO 2

99. Formulas of Molecular Compounds sulphur dioxide SO 2 tetranitrogen nonaoxide

100. Formulas of Molecular Compounds sulphur dioxide SO 2 tetranitrogen nonaoxideN 4 O 9

101. Formulas of Molecular Compounds sulphur dioxide SO 2 tetranitrogen nonaoxideN 4 O 9 diphosphorus pentoxide

102. Formulas of Molecular Compounds sulphur dioxide SO 2 tetranitrogen nonaoxideN 4 O 9 diphosphorus pentoxideP 2 O 5

103. Naming Molecular Compounds

104. Mono is never used for the first element

105. Naming Molecular Compounds Mono is never used for the first element Second element changes to –ide ending

106. Naming Molecular Compounds Mono is never used for the first element Second element changes to –ide ending Vowels (a, o) on prefix are sometimes omitted if followed by vowels (a, o)

107. Naming Molecular Compounds Mono is never used for the first element Second element changes to –ide ending Vowels (a, o) on prefix are sometimes omitted if followed by vowels (a, o) e.g. carbon monooxide  carbon monoxide

108. Naming Molecular Compounds

109. SiO 2

110. Naming Molecular Compounds SiO 2 silicon dioxide

111. Naming Molecular Compounds SiO 2 silicon dioxide N 2 S

112. Naming Molecular Compounds SiO 2 silicon dioxide N 2 Sdinitrogen monosulphide

113. Naming Molecular Compounds SiO 2 silicon dioxide N 2 Sdinitrogen monosulphide P 4 Cl 6

114. Naming Molecular Compounds SiO 2 silicon dioxide N 2 Sdinitrogen monosulphide P 4 Cl 6 tetraphosphorus hexachloride

115. Science 10 Review Part 4: Chem/Phys Change Chemical Equations

116. Chemical & Physical Change

117. Physical change: no new substance is formed

118. Chemical & Physical Change Physical change: no new substance is formed Chemical change: new substance is formed

119. Chemical & Physical Change Physical change: no new substance is formed Chemical change: new substance is formed Evidence for chemical change:

120. Chemical & Physical Change Physical change: no new substance is formed Chemical change: new substance is formed Evidence for chemical change: energy change colour change formation of a precipitate (solid) formation of a gas

121. Energy Changes Endothermic Reactions : energy absorbed e.g ice pack Exothermic Reactions: energy released e.g. combustion

122. Chemical equations from Word Equations

123. In Chemistry 11, a solution means something is dissolved in water. Therefore, the phase is aqueous.

124. Chemical equations from Word Equations In Chemistry 11, a solution means something is dissolved in water. Therefore, the phase is aqueous. Must include phase symbols and balance the equation

125. Chemical equations from Word Equations In Chemistry 11, a solution means something is dissolved in water. Therefore the phase is aqueous. Must include phase symbols and balance the equation Diatomic molecules: H 2, N 2, O 2, F 2, Cl 2, Br 2, I 2

127. Chemical equations from Word Equations

128. E.g. A solution of barium phosphate is mixed with aqueous sodium sulphate to yield solid barium sulphate and aqueous sodium phosphate.

129. Chemical equations from Word Equations E.g. A solution of barium phosphate is mixed with aqueous sodium sulphate to yield solid barium sulphate and aqueous sodium phosphate.

130. Chemical equations from Word Equations E.g. A solution of barium phosphate is mixed with aqueous sodium sulphate to yield solid barium sulphate and aqueous sodium phosphate. Ba 3 (PO 4 ) 2(aq)

131. Chemical equations from Word Equations E.g. A solution of barium phosphate is mixed with aqueous sodium sulphate to yield solid barium sulphate and aqueous sodium phosphate. Ba 3 (PO 4 ) 2(aq) + Na 2 SO 4(aq) 

132. Chemical equations from Word Equations E.g. A solution of barium phosphate is mixed with aqueous sodium sulphate to yield solid barium sulphate and aqueous sodium phosphate. Ba 3 (PO 4 ) 2(aq) + Na 2 SO 4(aq)  BaSO 4(s)

133. Chemical equations from Word Equations E.g. A solution of barium phosphate is mixed with aqueous sodium sulphate to yield solid barium sulphate and aqueous sodium phosphate. Ba 3 (PO 4 ) 2(aq) + Na 2 SO 4(aq)  BaSO 4(s) + Na 3 PO 4(aq)

134. Chemical equations from Word Equations E.g. A solution of barium phosphate is mixed with aqueous sodium sulphate to yield solid barium sulphate and aqueous sodium phosphate. Ba 3 (PO 4 ) 2(aq) + Na 2 SO 4(aq)  BaSO 4(s) + Na 3 PO 4(aq) 332