Upload
alexander-morris
View
40
Download
2
Tags:
Embed Size (px)
DESCRIPTION
What You Will Learn Today. Write balanced ionic equations. Note: Please ensure that you’ve downloaded and printed the accompanied notes before you embark on this e-learning journey. Ionic equations. A chemical equation shows the number of atoms and molecules of the reactants and products. - PowerPoint PPT Presentation
Citation preview
1
a) Write balanced ionic equations.
Note:Please ensure that you’ve
downloaded and printed the accompanied notes before you
embark on this e-learning journey.
2
Ionic equations
A chemical equation shows the number of atoms and molecules of the reactants and products.
Also shows physical state of reactants and products.
However, does not show clearly the reactions of ionic compounds.
3
Ionic equations
An ionic equation shows only the ions taking part in the reaction and leaves out the ions that do not
react.
4
Writing ionic equations
Procedure is similar as writing chemical equations.
A) Ionic compounds when dissolved in water dissociate completely into ions.
B) Spectator ions i.e ions that do not take part in the reaction are omitted on both sides of the
ionic equation.
5
Writing ionic equations Example 1
Step 1 Write word equation and chemical formula. Silver nitrate + sodium chloride silver chloride
+ sodium nitrate
AgNOAgNO33 (aq) + NaCl (aq) (aq) + NaCl (aq) AgCl (s) + Na AgCl (s) + Na
NONO3 (aq)(aq)
6
Writing ionic equations Example 1
Step 2 Write formula of ions formed
AgAg++ (aq) + NO (aq) + NO33-- (aq) (aq) + + NaNa++ (aq) + Cl (aq) + Cl-- (aq) (aq)
AgCl (s) + AgCl (s) + NaNa++ (aq) + (aq) + NONO3- (aq)(aq)
AgNOAgNO33 (aq) + NaCl (aq) (aq) + NaCl (aq) AgCl (s) + AgCl (s) +
NaNa NONO3 (aq)(aq)
Not able to dissolve in water to form ions
7
Writing ionic equations Example 1 Step 3 Omit spectator ions (NONO33
-- and and NaNa++ appear both sides. Do not take part in the reaction. Can be cancelled)
AgAg++ (aq) + NO (aq) + NO33-- (aq) (aq) + + NaNa++ (aq) + Cl (aq) + Cl-- (aq) (aq)
AgCl (s) + AgCl (s) + NaNa++ (aq) + (aq) + NONO3- (aq)(aq)
AgAg++ (aq) (aq) + Cl+ Cl-- (aq) (aq) AgCl (s) AgCl (s)
8
Writing ionic equationsExample 2
Step 1 Write word equation and chemical formula. Sodium hydroxide + hydrochloric acid sodium
chloride + water
NaOH (aq)+ HCl (aq) NaOH (aq)+ HCl (aq) NaCl (aq) NaCl (aq)
+ H+ H22O (l)O (l)
9
Writing ionic equationsExample 2
Step 2 Write formula of ions formed
NaNa++ (aq) + OH (aq) + OH-- (aq) (aq) + + HH++ (aq) + Cl (aq) + Cl-- (aq) (aq)
NaNa++ (aq) + (aq) + ClCl- (aq) + (aq) + HH22O (l)O (l)
NaOH (aq)+ HCl (aq) NaOH (aq)+ HCl (aq) NaCl (aq) NaCl (aq)
+ H+ H22O (l)O (l)
Covalent compound. Does not form ions
10
Writing ionic equationsExample 2 Step 3 Omit spectator ions (Na++ and Cl and Cl-- appear both
sides. Do not take part in the reaction. Can be cancelled)
HH++ (aq) + OH (aq) + OH-- (aq) (aq) H2O (l)
NaNa++ (aq) + OH (aq) + OH-- (aq) (aq) + + HH++ (aq) + Cl (aq) + Cl-- (aq) (aq)
NaNa++ (aq) + (aq) + ClCl- (aq) + (aq) + HH22O (l)O (l)
11
Writing ionic equationsExample 3
Step 1 Write word equation and chemical formula. Sodium carbonate + dilute hydrochloric acid
sodium chloride + water + carbon dioxide
NaNa22COCO33 (aq)+ 2HCl (aq) (aq)+ 2HCl (aq) 2NaCl 2NaCl (aq)(aq) + H+ H22O (l) + COO (l) + CO22 (g) (g)
12
Writing ionic equationsExample 3
Step 2 Write formula of ions formed
22NaNa++ (aq) + CO (aq) + CO33-- (aq) (aq) + + 22HH++ (aq) + (aq) + 22ClCl--
(aq)(aq) 22NaNa++ (aq) + (aq) + 22ClCl- (aq) + (aq) + HH22O (l) + O (l) +
COCO22 (g) (g)
NaNa22COCO33 (aq)+ (aq)+ 22HCl (aq) HCl (aq) 22NaCl NaCl (aq)(aq) + H+ H22O (l) + COO (l) + CO22 (g) (g)
13
Writing ionic equationsExample 3 Step 3 Omit spectator ions (Na++ and Cl and Cl-- appear both
sides. Do not take part in the reaction. Can be cancelled)
2H2H++ (aq) + CO (aq) + CO33-- (aq) (aq) CO CO22 (g) + (g) + H2O (l)
22NaNa++ (aq) + CO (aq) + CO33-- (aq) (aq) + + 22HH++ (aq) + (aq) + 22ClCl--
(aq)(aq) 22NaNa++ (aq) + (aq) + 22ClCl- (aq) + (aq) + HH22O (l) + O (l) +
COCO22 (g) (g)
14
1 Magnesium + sulfuric acid magnesium sulfate + hydrogen
2 Sodium hydroxide + nitric acid Sodium nitrate + water
Write balanced chemical equations and then the ionic equations (with state symbols) for the following questions.
15
3 Magnesium oxide + hydrochloric acid Magnesium chloride + water
4 Silver nitrate solution + potassium iodide solution silver iodide (AgI is insoluble) + potassium nitrate
Write balanced chemical equations and then the ionic equations (with state symbols) for the following questions.
16
Answers in red box
(take a peek only after you’ve done the questions in your notes. Your integrity counts!)
17
1. Magnesium + sulfuric acid magnesium sulfate + hydrogen
Mg (s) + H2SO4 (aq) MgSO4 (aq) + H2 (g)
Mg (s) + 2H+ (aq) + SO42- (aq) Mg2+ (aq) +
SO42- (aq) + H2 (g)
Mg (s) + 2H+ (aq) Mg2+ (aq) + H2 (g)
18
2. Sodium hydroxide + nitric acid Sodium nitrate + water
NaOH (aq) + HNO3 (aq) NaNO3 (aq) + H2O (l)
Na+ (aq) + OH- (aq) + H+ (aq) + NO3- (aq)
Na+ (aq) + NO3- (aq) + H2O (l)
OH- (aq) + H+ (aq) H2O (l)
19
3. Magnesium oxide + hydrochloric acid Magnesium chloride + water
MgO (s) + 2HCl (aq) MgCl2 (aq) + H2O (l)
MgO (s) + 2H+ (aq) + 2Cl- (aq) Mg2+ (aq) +
2Cl- (aq) + H2O (l)
MgO (s) + 2H+ (aq) Mg2+ (aq) + H2O (l)
4. Silver nitrate + potassium iodide silver iodide + potassium nitrate
AgNO3 (aq) + KI (aq) AgI (s) + KNO3 (aq)
20
Ag+ (aq) + NO3- (aq) + K+ (aq) + I- (aq)
AgI (s) + K+ (aq) + NO3- (aq)
Ag+ (aq) + I- (aq) AgI (s)