expoeriment f4

8/13/2019 expoeriment f4

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1. Empirical formula of copper(II) oxide2. Empirical formula of magnesium oxide3. Chemical equations

Number Activity 3.4

Pg. 23Title Empirical formula of copper(II) oxide

Aim To determine the empirical formula of copper(II)

oxide

Problem

Statement

How does the formula of copper(II) oxide

determine?

Hypothesis The empirical formula of copper(II) oxide can be

determined by finding out the mass of copper and

oxygen in a sample of copper(II) oxide

Apparatus U tube Stoppers Glass tube Combustion tube with a small hole at the

end

Retort stand and clamp Spatula Porcelain dish Bunsen burner Balance

Preparation for hydrogen gas

Thistle funnel Flat-bottomed flask

Material Hydrogen gas, H2 Copper(II) oxide Anhydrous calcium chloride, CaCl2 Wooden splinter

Preparation for the hydrogen gas

Dilute hydrochloric acid Zinc pieces

Variables Manipulated variable: Mass of copperoxide

Responding variable: Mass of copperformed

Controlled / Fixed variable: An excess of


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hydrogen gas

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Number Activity 3.5Pg. 25

Title Empirical formula of magnesium oxide

Aim To determine the empirical formula of magnesiumoxide

ProblemStatement

How does the formula of magnesium oxidedetermine?

Hypothesis The empirical formula of magnesium oxide is

MgO

Apparatus Crucible with lid

Tongs Bunsen burner Tripod stand Pipe-clay triangle

Material 10 cm magnesium ribbon Sandpaper

Variables Manipulated variable: Magnesium ribbon Responding variable: Mass of magnesium

oxide

Controlled / Fixed variable: Length / Massof magnesium ribbon and excess air

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Number Activity 3.6

Pg. 27

Title Chemical equations

Aim To construct balanced chemical equations

A. Heating of copper(II) carbonate

B. Reaction of ammonia gas and hydrochloric acid

/ Formation of ammonium chloride

C. Reaction of lead(II) nitrate and potassium iodide

/ Precipitation of lead(II) iodide


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ProblemStatement

How does the chemical equations determine?

Hypothesis A. The chemical equation of copper(II) carbonate

is CuCO3> CuO + CO2

B. The chemical equation ofApparatus Boiling tube

Test tubes Rubber bung with delivery tube Test tube rack Test tube holder Stoppers Bunsen burner

Material Copper(II) carbonate powder Lime water Concentrated ammonia solution Concentrated hydrochloric acid Lead(II) nitrate solution Potassium iodide solution

Variables A. Heating of copper(II) carbonate

Manipulated variable: Mass of copper(II)carbonate

Responding variable: Mass of copper oxideformed / Volume of carbon dioxide

liberated Controlled / Fixed variable: Pressure

B. Reaction of ammonia gas and hydrochloric acid

/ Formation of ammonium chloride

Manipulated variable: Concentration ofammonia and hydrochloric acid

Responding variable: Ammonium chlorideformed

Controlled / Fixed variable: Temperatureand pressure

C. Reaction of lead(II) nitrate and potassium iodide

/ Precipitation of lead(II) iodide

Manipulated variable: Volume of lead(II)nitrate solution and volume of potassium

iodide solution


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Responding variable: Mass of lead(II)iodide formed

Controlled / Fixed variable: Temperatureand pressure

List of PEKA experiments:

1. Chemical properties of lithium, sodium and potassium2. Chemical properties of Group 17 elements3. Properties of the oxides of elements in Period 3

Number Experiment 4.1

Pg. 35

Title Chemical properties of lithium, sodium and

potassium

Aim To investigate the chemical properties of lithium,

sodium and potassium

Problem

Statement

How does the reactivity of Group 1 elements

change when they react with water and oxygen gas,

O2?

Hypothesis When going down Group 1, alkali metals become

reactive in their reactions with water

Apparatus Water troughs Small knife

Forceps Gas jars Gas jar spoons Gas jar covers

Material Small pieces of lithium, sodium andpotassium

Filter paper Distilled water Red litmus paper Three gas jars filled with oxygen gas, O2

Variables Manipulated variable: Different types ofalkali metals

Responding variable: Reactivity of metals Controlled / Fixed variable: Water, size of

metals

Operational An alkali metal that reacts more vigorously with


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Definition water is more reactive metal

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Number Experiment 4.2

Pg. 39Title Chemical properties of Group 17 elements

Aim To investigate the chemical properties of Group 17

elements

(A) Reactions of halogens with water

(B) Reactions of halogens with iron

(C) Reactions of halogens with sodium hydroxide,NaOH solution

ProblemStatement

How do halogens react with water, iron andsodium hydroxide, NaOH solution?

Hypothesis (A) Reactions of halogens with water

1. Halogens forms acidic solutions when theyreact with water

2. Halogens show bleaching properties whenthey react with water


Halogens form iron(III) halides when they react

with iron / When going down Group 17, halogens

become less reactive in their reactions with iron

(C) ) Reactions of halogens with sodium

hydroxide, NaOH solution

Halogens form sodium halide, sodium halite(I) and

water when they react with sodium hydroxide /

When going down Group 17, halogens become lessreactive in their reactions with sodium hydroxide

solution

Apparatus Test tubes Dropper Test tube holders Stoppers Combustion tubes Delivery tubes


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Bunsen burner Retort stand and clamp

Material Chlorine gas, Cl2(produce after mixingpotassium manganate(VII) salts with

concentrated hydrochloric acid) Liquid bromine, Br2 Solid iodine, I2 Blue litmus paper Water Iron wool Soda lime 2 mol dm-3sodium hydroxide, NaOH

solution

Variables (A) Reactions of halogens with water

Manipulated variable: Type of halogens Responding variable: Change in colour of

the blue litmus paper / Reactivity of

halogens

Controlled / Fixed variable: Water(B) Reactions of halogens with iron

Manipulated variable: Types of halogens Responding variable: Appearance of brown

solid / Reactivity of halogens Controlled / Fixed variable: Iron



Manipulated variable: Types of halogens Responding variable: Formation of a

colourless solution from a coloured halogen

/ Reactivity of halogens

Controlled / Fixed variable: Sodiumhydroxide solution

OperationalDefinition

(A) Reactions of halogens with water

1. When blue litmus paper turns red, thesolution formed shows acidic property

2. When blue litmus paper turns white, the


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solution formed shows bleaching property


The appearance of a brown solid shows the

formation of iron(III) halides



The formation of a colourless solution indicates

that salts of sodium halide, sodium halite(I) and

water are formed

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Number Experiment 4.3Pg. 45

Title Properties of the oxides of elements in Period 3

Aim To study the properties of the oxides of elements in

Period 3

Problem

Statement

How do the acid-base properties of the oxides of

elements change across Period 3?

Hypothesis Acidic properties of the oxides of elements

increase whereas basic properties of the oxides ofelements decrease across Period 3

Apparatus

Boiling tubes Test tubes Test tube holder Glass rod Spatula Gas jar Gas cover 100 cm3measuring cylinder

Material Sodium oxide, Na2O Magnesium oxide, MgO

Aluminium oxide, Al2O3 Silicon(IV) oxide, SiO2 Phosphorus pentoxide, P2O5 Sulphur dioxide gas, SO2 Dichlorine heptoxide, Cl2O7 Universal Indicator 2 mol dm-3nitric acid, HNO3 2 mol dm-3sodium hydroxide, NaOH


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solution

Variables Manipulated variable: Oxides of elementsof Period 3

Responding variable: pH values in waterand solubility in acid or alkali

Controlled / Fixed variable: Water or nitricacid, HNO3 or sodium hydroxide, NaOH

solution

OperationalDefinition

1. Oxide that dissolves in water to formsolution with pH less than 7 is acidic and

pH more than 7 is alkaline

2. Oxide that can dissolve in an acid exhibitsbasic properties

3. Oxide that can dissolve in an alkali exhibitsacidic properties

4. Oxide that can dissolve in both acid andalkali exhibits amphoteric properties

List of PEKA experiments:

1. Ionic compound2. Properties of ionic and covalent compounds

Number Activity 5.1

Pg. 52

Title Ionic compound

Aim To prepare ionic compounds(A) Preparation of

magnesium oxide, MgO

(B) Preparation of sodium chloride, NaCl

(C) Preparation of iron(III) chloride, FeCl3

Apparatus (A) Preparation of magnesium oxide, MgO

Sandpaper Crucible Spatula Pipe-clay triangle Tripod stand Bunsen burner


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(B) Preparation of sodium chloride, NaCl

Knife Forceps Filter paper Spatula Gas jar spoon / Deflagrating spoon Gas jar cover Gas jar


Spatula Asbestos paper Combustion tube Stopper with delivery tube Retort stand and clamp Bunsen burner

Material (A) Preparation of magnesium oxide, MgO

Magnesium ribbon(B) Preparation of sodium chloride, NaCl

Sodium Chlorine gas, Cl2


Iron filling Chlorine gas, Cl2

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Number Activity 5.3

Pg. 55

Title Properties of ionic and covalent compounds

Aim To compare the properties of ionic and covalentcompounds(A) Melting point and boiling point

(B) Solubility in water and organic solvents

(C) Electrical conductivity


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Apparatus (A) Melting point and boiling point

Spatula Evaporating dish Dropper


Spatula Glass rod Test tubes Test tube rack


Spatula Glass rod Switch Connecting wires with crocodile clips Batteries Bulb Carbon electrodes Beakers Crucible Tripod stand Pipe-clay triangle Bunsen burner

Material (A) Melting point and boiling point

Magnesium chloride, MgCl2 Sodium sulphate, Na2SO4 Diethyl ether, (C2H5)2O Hexane, C6H14


Distilled water Magnesium chloride, MgCl2 Cyclohexane, C6H12 Sodium sulphate, Na2SO4 Diethyl ether, (C2H5)2O Hexane, C6H14



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Solid lead(II) bromide, PbBr2 Magnesium chloride, MgCl2solution Naphthalene, C10H8

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expoeriment f4