WAEC SSCE - Chemistry - 2005

Which of the following molecules has a linear structure?

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The molecule with a linear structure is CO2. A molecule's structure depends on the arrangement of atoms in the molecule and the bonds between them. In CO2, there are two oxygen atoms bonded to a central carbon atom. The bond between each oxygen atom and the carbon atom is double-bonded, which means they share two pairs of electrons. This double bond arrangement forces the molecule to be linear in shape. In contrast, NH3 and CH4 have a tetrahedral shape due to the presence of lone pairs on the central atom, which cause the atoms to spread out. Water (H2O) also has a bent shape because of its lone pairs and its two single bonds.

What process is involved in the reaction represented by the following equation? AICI₃ + 3H₂O_(l) → AI(OH) _3(s) + 3HCI_(g)

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The process involved in the reaction represented by the given equation is hydrolysis. In this reaction, a compound (AICI3) reacts with water, and as a result, it breaks down into two products, AI(OH)3 and HCI. This reaction is called hydrolysis because water is used to break down the compound. Specifically, the AICI3 is split into AI(OH)3 and HCI through the addition of water molecules, which causes the chemical bonds in AICI3 to break. The resulting AI(OH)3 is a solid precipitate that falls out of the solution, while the HCI is a gas that is released into the air.

Which of the following reactions is sulphur (IV) oxidizing agent?

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The electronic configuration of an element X is 1s²2s ²2s⁶3p ² 3p⁴. It can be deduced that X

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Consider the reaction represented by the equation below, xNH_3(g) + yCI_2(g) → zHCI_(g) + N_2(g) The values of x,y and z are respectively

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Which of the following sets of elements are arranged in order of decreasing atomic size in the Periodic Table?

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When X is heated with manganese (IV) oxide, oxygen is produced X is

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The substance X reacts with manganese (IV) oxide when heated, and produces oxygen gas. Among the options given, the only substance that fits this description is KCIO₃, also known as potassium chlorate. When potassium chlorate is heated with manganese (IV) oxide, the following chemical equation takes place: 2KClO₃ → 2KCl + 3O₂ In this equation, manganese (IV) oxide acts as a catalyst, which means it helps to speed up the reaction without being consumed in the process. The result is the production of oxygen gas, which is released as a byproduct. Therefore, the answer to this question is KCIO₃ (potassium chlorate).

Hardness in water can be removed by adding

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Which of the following is not an acid anhydride?

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Which of the following statements is not a postulate of the kinetic theory of gases?

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The statement that "Molecules move with the same speed" is not a postulate of the kinetic theory of gases. According to the kinetic theory of gases, gas molecules are in constant random motion, and they move with different speeds and in different directions. The average kinetic energy of the gas molecules is directly proportional to the temperature of the gas. This means that at higher temperatures, the gas molecules will have a higher average speed. The other postulates of the kinetic theory of gases are that intermolecular forces between gas molecules are negligible, and collisions between gas molecules are elastic, which means that no energy is lost during the collision. These postulates help to explain the macroscopic properties of gases, such as their pressure, temperature, and volume, in terms of the behavior of their constituent molecules.

The activation energy of a reaction can be altered by

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The activation energy of a chemical reaction is the amount of energy that needs to be supplied to start the reaction. It is an energy barrier that must be overcome for a reaction to occur. There are different ways to alter the activation energy of a reaction, and one of them is by using a catalyst. A catalyst is a substance that lowers the activation energy of a reaction, making it easier for the reaction to occur. Catalysts do not change the overall energy change of the reaction, but they make it happen faster and with less energy input. Another way to alter the activation energy is by changing the temperature. When the temperature is increased, the particles of the reactants move faster, and they collide with more energy, which makes it more likely for the reaction to occur. This increase in kinetic energy of the particles can overcome the activation energy barrier, and the reaction can proceed. On the other hand, adding a reducing agent or applying high pressure does not directly alter the activation energy of a reaction. A reducing agent is a substance that donates electrons to another chemical species, while high pressure can affect the equilibrium of a reaction. However, neither of these methods directly changes the energy barrier required to start the reaction. In summary, the activation energy of a reaction can be altered by using a catalyst or changing the temperature, but not by adding a reducing agent or applying high pressure.

When ice is changing to water, its temperature remains the same because the heart gained is

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When ice changes into water, it goes through a process called melting. During melting, the ice absorbs heat from the surroundings without increasing its temperature. This is because the heat energy is used to break the bonds between the molecules of ice, which are held together by strong forces. The heat energy that is absorbed during melting is called the "heat of fusion". It is the amount of heat energy required to change a solid into a liquid, or vice versa, without any change in temperature. In the case of ice melting, the heat of fusion is absorbed from the surroundings, which keeps the temperature of the ice constant at 0°C (32°F) until all of the ice has melted. Therefore, the reason why the temperature of ice remains the same during the melting process is that the heat gained is being used to separate the molecules and break the bonds between them, rather than increasing the temperature of the ice.

The colour of the solution formed when ethyne reacts with an acidic solution of potassium tetraoxomanganate (VII) is

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When ethyne, also known as acetylene, reacts with an acidic solution of potassium tetraoxomanganate (VII), also known as potassium permanganate, a chemical reaction occurs. The purple colour of the potassium permanganate solution fades away, and the solution becomes colourless. This happens because the potassium permanganate oxidizes the ethyne, which breaks down into carbon dioxide and water. This reaction converts the potassium permanganate into manganese(II) ions, which are colourless, hence the colour of the solution changes from purple to colourless. Therefore, the correct answer is "colourless."

Which of the following methods is suitable for preparing insoluble salts?

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The method suitable for preparing insoluble salts is double decomposition. Double decomposition is a chemical reaction in which two ionic compounds exchange ions to form two new compounds. This reaction can occur when one of the products is insoluble in water, leading to the formation of an insoluble salt. In the process of double decomposition, the cations of one compound switch places with the cations of the other compound, resulting in the formation of two new compounds. If one of these new compounds is insoluble in water, it will precipitate out of the solution as a solid. The insoluble compound can then be collected through filtration and washed with water to remove any remaining soluble impurities. Thermal decomposition involves breaking down a compound into simpler substances by heating it. Oxidation involves adding oxygen or removing hydrogen from a compound. Neutralization is a reaction between an acid and a base to form a salt and water. These methods are not suitable for preparing insoluble salts. Therefore, double decomposition is the suitable method for preparing insoluble salts.

NaHCO_3(s) can be distinguished from Na₂CO_3(s) by the action of

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Which of the following substances is a non-reducing sugar?

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Sucrose is a non-reducing sugar. A reducing sugar is a sugar that has a free aldehyde or ketone functional group, which can reduce certain chemicals such as Benedict's solution or Fehling's solution. When a reducing sugar is heated with these chemicals, they are oxidized and reduce the chemical reagent, leading to the formation of a colored precipitate. Sucrose is a disaccharide composed of glucose and fructose linked by a glycosidic bond. It does not have a free aldehyde or ketone functional group, so it cannot act as a reducing sugar. In contrast, glucose, fructose, and maltose all have a free aldehyde or ketone functional group, so they can act as reducing sugars. Therefore, among the options given, sucrose is the non-reducing sugar.

The volume occupied by a given mass of gas depends on its

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The volume occupied by a given mass of gas depends on its temperature and pressure. This is because gas molecules are constantly moving and colliding with each other and with the walls of their container. When the temperature of a gas increases, the molecules move faster and collide with each other more frequently, which increases the pressure of the gas. Similarly, when the pressure of a gas increases, the molecules are pushed closer together, which decreases the volume of the gas. Therefore, temperature and pressure are the main factors that determine the volume occupied by a given mass of gas.

Which of the following changes is characteristic of an alpha-particle emission?

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An alpha-particle emission is characterized by the nucleus losing two protons and two neutrons. An alpha particle is a type of radiation that consists of two protons and two neutrons, which is equivalent to the nucleus of a helium atom. During alpha-particle emission, a nucleus will eject an alpha particle from its structure. This process causes the nucleus to lose two protons and two neutrons, which changes its atomic number and mass number. This type of radioactive decay occurs in heavy nuclei that are unstable due to having too many protons and neutrons, and it allows the nucleus to become more stable by reducing the number of particles in its structure.

Which of the following factors does not affect the rate of reaction of CaCO₃ with HCI?

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The factor that does not affect the rate of reaction of CaCO₃ with HCI is the solubility of CaCO₃. When CaCO₃ reacts with HCI, it produces carbon dioxide, water, and calcium chloride. The rate of this reaction is affected by several factors, such as temperature, concentration of HCI, and surface area of CaCO₃. However, the solubility of CaCO₃ does not affect the rate of reaction because it is a solid and does not dissolve in the reaction mixture. In other words, the reaction rate depends on the number of collisions between CaCO₃ and HCI molecules, and the solubility of CaCO₃ does not influence this collision process. Therefore, it is safe to say that the solubility of CaCO₃ does not affect the rate of reaction of CaCO₃ with HCI.

Which of the following can be used to predict the type of bonding in HCI?

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The correct option to predict the type of bonding in HCl is electronegativity difference. Bonding occurs when atoms share or transfer electrons to achieve a more stable electron configuration. The electronegativity of an atom is its ability to attract electrons towards itself in a chemical bond. When two atoms with different electronegativity values come together, the atom with higher electronegativity will pull the electrons closer to itself, creating a polar covalent bond. In the case of HCl, hydrogen has an electronegativity value of 2.1, while chlorine has an electronegativity value of 3.0. The difference between these two values is 0.9, which falls in the range of a polar covalent bond. To summarize, the electronegativity difference between two atoms is a measure of their tendency to form a bond and the type of bond that will form.

Which of the following substance is an alloy of lead?

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The substance that is an alloy of lead is called soft solder. Soft solder is a type of metal alloy that is commonly used to join together two or more metal pieces by melting the solder and allowing it to flow into the joint. Soft solder typically contains a combination of lead and tin, although other metals may also be added to achieve specific properties. The reason why soft solder is considered an alloy of lead is because lead is one of the main components in the mixture. The lead in the soft solder helps to lower the melting point of the alloy, making it easier to work with and allowing it to flow more easily into the joint. It is worth noting that while soft solder is commonly used in various applications such as plumbing, electronics, and jewelry-making, it is also important to handle it with care since lead is a toxic metal.

Which of the elements will burn in excess oxygen to form a product that is neutral to litmus?

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Reaction undergone by compounds with the general formula C_n H_2n+2 include

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Fats are classified as

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Fats are classified as "alkanoates". Alkanoates are a type of organic compound consisting of a long chain of carbon atoms (called an alkyl group) and a carboxyl group (-COO-) at one end. Fats are made up of glycerol molecules (a type of alcohol) and three alkanoic acids (also known as fatty acids) that are attached to the glycerol backbone, forming a molecule known as a triglyceride. Therefore, fats are classified as alkanoates because they contain these alkyl groups and carboxyl groups.

What is the mass number of an element having 20 neutrons, 15 protons and 15 electrons?

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The mass number of an element is the sum of its protons and neutrons. In this case, the element has 15 protons and 20 neutrons, so the mass number would be: Mass number = protons + neutrons Mass number = 15 + 20 Mass number = 35 Therefore, the correct option is 35. To summarize, the mass number of an element can be found by adding the number of protons and neutrons in the nucleus of an atom.

An element X has an atomic number of 16. What is its most likely oxidation state in its binary compounds?

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The most likely oxidation state of element X in its binary compounds can be determined by looking at its position in the periodic table and its electron configuration. Element X has an atomic number of 16, which places it in group 16 (also known as the oxygen group) of the periodic table. This group includes elements such as oxygen, sulfur, and selenium. The elements in this group have six valence electrons, meaning they need two more electrons to complete their outermost shell and attain a stable octet configuration. Based on this information, the most likely oxidation state for element X in its binary compounds would be -2. This is because in binary compounds, the element will typically gain two electrons to achieve a stable octet configuration. Therefore, it will have a charge of -2 to balance the positive charge of the other element in the compound. So, option -2 is the correct answer.

An element which can exist in two or more forms in the same physical state, exhibits

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The correct term that describes an element which can exist in two or more forms in the same physical state is allotropy. Allotropy is a type of property that some elements have, where they can exist in different structural forms known as allotropes. Each allotrope has different physical and chemical properties, even though they are made up of the same atoms. For example, carbon is an element that exhibits allotropy. It can exist in several different allotropes, including diamond, graphite, and fullerenes. Diamond is a hard, transparent substance used in jewelry and cutting tools, while graphite is a soft, dark substance used in pencils and lubricants. Both diamond and graphite are made up of carbon atoms, but their structures are different, which results in their different physical and chemical properties. Isotopy refers to the property of having the same atomic number but a different atomic mass due to a different number of neutrons. Structural isomerism refers to the property of having the same chemical formula but different structural arrangements. Variable valency refers to the property of having different valences, or combining capacities, depending on the chemical reaction.

Which of the following pairs of solutions will produce a precipitate when mixed?

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In which of the following processes is biotechnology not applied?

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Biotechnology is not applied in the Electroplating of metals process. Biotechnology is the use of living organisms or biological processes for industrial, medical, or environmental applications. In the manufacture of drugs, biotechnology is used to produce medications such as insulin, vaccines, and antibodies. In the treatment of domestic sewage, biotechnology is used to break down organic matter in wastewater using microorganisms. In the production of alcoholic beverages, biotechnology is used to ferment sugars into alcohol using yeast. However, in electroplating, a process used to coat one metal with another by passing an electric current through a solution containing ions of the coating metal and the metal to be coated, biotechnology is not involved. This process involves chemical and electrical reactions, but not biological ones.

HNO₃ does not usually react with metals to liberate hydrogen because HNO₃ is

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Ethyne undergoes the following reactions except

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Ethyne (also known as acetylene) can undergo polymerization, addition, and substitution reactions. However, it does not undergo esterification reactions. Polymerization involves the combination of many ethyne molecules to form a long-chain polymer. Addition reactions involve the addition of atoms or groups to the double bond of ethyne to form a saturated compound. Substitution reactions involve the replacement of one or more hydrogen atoms in ethyne with another atom or group. Esterification, on the other hand, involves the reaction between an alcohol and a carboxylic acid to form an ester. Ethyne does not have a functional group that can react with carboxylic acids or alcohols to form esters, so it cannot undergo esterification reactions.

What is the major product formed when C₂H₅OH reacts with CH₃COOH?

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The major product formed when C₂H₅OH reacts with CH₃COOH is CH₃COOC₂H₅. This reaction is a type of esterification, where an alcohol and a carboxylic acid react to form an ester and water. In this case, the ethyl alcohol (C₂H₅OH) reacts with acetic acid (CH₃COOH) to form ethyl acetate (CH₃COOC₂H₅) and water (H₂O) as a byproduct. The reaction takes place due to the acidic nature of the carboxylic acid, which donates a proton (H⁺) to the hydroxyl group (-OH) of the alcohol, forming water and a carboxylate ion. The carboxylate ion then reacts with the electrophilic carbon atom of the carboxylic acid, leading to the formation of the ester. To summarize, the reaction between C₂H₅OH and CH₃COOH leads to the formation of CH₃COOC₂H₅ and H₂O as a byproduct, making CH₃COOC₂H₅ the major product of the reaction.

In which of the following reactions is the position of equilibrium not affected by an increase in pressure?

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The main difference between a primary cell and a secondary cell is that the primary cell

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The main difference between a primary cell and a secondary cell is that the primary cell cannot be recharged, while the secondary cell can be recharged. A primary cell is a battery that generates electrical energy through an irreversible chemical reaction. Once the reactants are used up, the cell cannot produce electricity anymore and must be replaced. On the other hand, a secondary cell, also known as a rechargeable battery, can be recharged by reversing the chemical reactions that occur during discharge. Both primary and secondary cells are types of electrochemical cells, which convert chemical energy into electrical energy through an oxidation-reduction reaction. They both contain two electrodes and an electrolyte, which allows the flow of charged particles between the electrodes.

Which of the following compounds dissolves readily in water?

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Among the given compounds, only NH4Cl dissolves readily in water. This is because NH4Cl is an ionic compound, composed of ammonium (NH4+) and chloride (Cl-) ions. When NH4Cl is added to water, the water molecules surround the ions, separating them from each other and forming a solution. This process is called hydration or solvation. On the other hand, BaSO4, CuSO3, and AgCl are insoluble or only slightly soluble in water. BaSO4 and AgCl are both ionic compounds, but they have very low solubility in water. CuSO3 does not exist as a stable compound under normal conditions, and it is usually synthesized as a complex or in a solution of a different solvent. Therefore, the compound that dissolves readily in water among the given options is NH4Cl.

Determine the mass of copper deposited by 4.0 moles of electrons in the reaction represented by the equation below: Cu²_(aq) + 2e^- → Cu_(s)

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To determine the mass of copper deposited, we need to use the concept of Faraday's law of electrolysis. This law states that the amount of substance produced at an electrode is directly proportional to the quantity of electricity passed through the electrolyte. The quantity of electricity is measured in coulombs (C) and is related to the number of moles of electrons (n) by the equation: Q = nF where Q is the quantity of electricity, n is the number of moles of electrons, and F is the Faraday constant, which is equal to 96,485 C/mol. In this case, we have 4.0 moles of electrons, so the quantity of electricity is: Q = nF = 4.0 mol x 96,485 C/mol = 385,940 C The reaction involves the reduction of Cu2+ ions to Cu metal, which requires two electrons per ion. So, for every two electrons that pass through the electrolyte, one Cu atom is produced. This means that the number of moles of Cu produced is half the number of moles of electrons: n(Cu) = 0.5 x n(e-) = 0.5 x 4.0 mol = 2.0 mol The molar mass of copper is 63.55 g/mol, so the mass of copper produced is: m = n x M = 2.0 mol x 63.55 g/mol = 127.1 g Therefore, the mass of copper deposited is approximately 127.1 g. The closest option to this value is which is 128 g.

A salt that absorbs moisture from the atmosphere without forming a solution is said to be

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A salt that absorbs moisture from the atmosphere without forming a solution is said to be hygroscopic. Hygroscopic substances have a strong affinity for water molecules and can absorb water vapor from the surrounding atmosphere. This can cause the substance to become damp or even dissolve in the absorbed water. In contrast, efflorescent substances release water molecules into the surrounding atmosphere and can become dry and powdery. Deliquescent substances can absorb so much water that they dissolve and form a solution. Insoluble substances cannot dissolve in water and will not absorb moisture from the atmosphere.

(a)(i) State Graham's law of diffusion

(ii) If 100 cm\(^3\) of oxygen diffused in 4 seconds and 50cm\(^3\) of gas Y diffused in 3 seconds, calculate the relative molecular mass of gas Y. (0 = 16)

(b) Consider the following equilibrium reaction: X + 2Y\(_{(g)}\) \(\rightleftharpoons\) XY\(_{2(9)}\)     \(\Delta\)H = -52KJ mol\(^{-1}\)

(i) State what happens to the yield of XY\(_2\) when the temperature is increased

(ii) Explain the effect of decrease in pressure on the equilibrium position.

(iii) State the effect of a catalyst on the I. position of equilibrium II. activation energy

(c)(i) State the differences between the solubilities of solids and gases in liquids.

(ii) Name the physical-properties used it choosing separation techniques for the following mixtures:

I. kerosene and petrol II. calcium trioxocarbonate (IV) and potassium chloride. III. ammonium chloride and sodium chloride.

(d)(i) State a method of preparing each of the following salts:

(iii) State the difference between anhydrous and hydrated salts.

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(a)(i) State the two types of hardness in water.

(ii) Name a salt that causes each type of hardness.

(ii) Write a balanced equation for the removal of each type of hardness.

(iv) State one effect of hard water on soap.

(b)(i) State whether the pH of each of the following is less than, equal to, or greater than 7.

I. Glucose solution II. Chlroine water III. Lime water IV. Sour milk

(ii) Give the difference between the following compounds: I. an acidic oxide and an amphoteric oxide; II. concentrated acid and a dilute acid; Ill. a normal salt and an acid salt

(c)(i) Iron reacts with H\(_2\)SO\(_4\) according to the equation: Fe\(_{(s)}\) + H\(_2\)SO\(_{4(aq)}\) ---> FeSO\(_{4(aq)}\) + H\(_{2(g)}\)

Calculate the mass of FeSO\(_4\) that would be produced by 0.5 mole of Fe. [H = 1, S = 32, Fe = 56]

(ii) List two allotropes of sulphur

(d)(i) State what would La observed when a damp starch-iodide paper is dropped into a gas jar of chloride

(ii) Explain your ansv.er in (d)(i) above.

(iii) State the products formed when ammonia reacts with excess chlorine.

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(a)(i) List three observable changes that take place when a dilute solution of copper (II) chloride is electrolysed using platinum electrodes. Stage III

(ii) Calculate the quantity of electricity used during electrolysis when a current of 0.21 ampere flows for 2 hours.

(iii) State what is meant by the term preferential discharge of ions in electrolysis

(iv) Give one factor which influences the preferentia! discharge of ions during electrolysis.

(v) State one Q difference between-a conductor and an electrolyte.

(b) Consider the reaction represented by the equation below: Na\(_2\)S\(_2\)O\(_{3(aq)}\) + 2HCI\(_{(aq)}\) \(\to\) 2NaCI\(_{(aq)}\) + H\(_2\)O\(_{(l)}\) + SO\(_{2(g)}\) + S\(_{(s)}\)

(i) List two factors that can affect the rate of this reaction.

(i) Which of the products can be readily used to measure the rate of the reaction. Give a reason for your answer.

(iii) Name two instruments that can be used to measure factors in (b)(i) above.

(c)(i) State the reasons for regarding rusting and burning as oxidation processes.

(ii) I. Write the balanced half equations for the following redox reaction: Mg\(_{(s)}\) + Fe\(^{2+}_{(aq)}\)  ----> Mg\(^{2+}_{(aq)}\) + Fe\(_{(s)}\)

II. Which of the reactants is the oxidizing agent?

Ill. State the change in the oxidation number of the oxidizing agent.

(d)(i) State one ore from which each of the following metals can be extracted. I. Tin II. Iron (ii) List two uses of copper (iii) Name one alloy of tin.

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TEST OF PRACTICAL KNOWLEDGE QUESTION

All your burette readings (initial and final), as well as the size of your pipette, must be recorded but no account of experimental procedure is required. All calculations must be done in your answer book.

A is a solution of H\(_2\)SO\(_4\) containing 4.9 gdm-3, B is a solution containing X g dm\(^{-3}\) of Na\(_2\)CO\(_3\).

(a) Put A into the burette and titrate it against 20.0 cm\(^3\) or 25.0 cm\(^3\) portions of B using methyl orange as an indicator. Record the volume of your pipette. Tabulate your burette readings and calculate the average volume of A used. The equation for the reaction involved in the titration is; H\(_2\)SO\(_{4(aq)}\) + Na\(_2\)CO\(_{3(aq)}\) \(\to\) Na\(_{2}\)SO\(_{4(aq)}\) + H\(_2\)O\(_{(l)}\) + CO\(_{2(g)}\)

(b) From your results and information provided above, calculate the:

(i) Concentration of A In mol dm\(^{-3}\)

(ii) concentration of B in mol dm\(^{-3}\)

(iii) mass of salt formed when 500 cm\(^3\) of B is Completely neutralized by A.

(v) volume of carbon (IV) oxide liberated in (b) (ii) above at s.t.p. [O = 16, Na = 23, S = 32, 1 mole or a gas occupies 22.4 dm\(^3\) at s.t.p.]

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(i) Write the structure of 2—chloro-2—methylpropane.

(ii) Consider the compound X represented by the structure below:

I. State the functional group in X; II. Give the IUPAC name of X; Ill. State the homologous series to which X belongs. IV. Give the names of two compounds from which X is formed. V. State one physical characteristt of X.

 (b)(i) List two products obtained from fractional distillation of petroleum;

(ii) State one use of each product in (b)(i) above,

(iii) Mention one disadvantage of crude oil production

 (c)(i) Mention the monomer of protein (ii) A compound has an empirical formula of CHO\(_2\) and its molar mass is 90. Deduce the molecular formula of the compound. [H = 1, C = 12, O = 16].

(d) Use the reaction scheme below to answer questions (i).— (iv).

(i) State the reagents needed for stages II and V;

(ii) Nanie the product Q of reaction in stage IV;

(iii) State the conditions required for stage III;

(iv) Give the names of the processes in stages I, II, Ill and V respectively.

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TEST OF PRACTICAL KNOWLEDGE QUESTION

(a) State what would be observed when:

(i) Chlorine is passed through a freshly prepared solution of FeCl\(_2\).

(ii) SO\(_2\) is bubbled into a solution of FeCl\(_3\);

(iii) A few drops of water Is added to sodium hydroxide pellets in a test tube;

(iv) Dilute H\(_2\)SO\(_4\) is added to CaCO\(_{3(s)}\)

(b) Three test tubes contain solutions of SO\(_3^{2-}\), CO\(^{2-}_3\) and SO\(_4^{2-}\) respectively. Describe one chemical method that you would use to identify the solution containing SO\(_4^{2-}\) 

(c)(i) Draw and label a diagram to illustrate the separation of a mixture of petrol and water

(ii) Which of the following will dissolve faster? 10g of NaOH pellets in 100 cm\(^3\) of water; 10g of NaOH powder in 50 cm\(^3\) of water. Give the reason for your answer.

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TEST OF PRACTICAL KNOWLEDGE QUESTION

Credit will be given for strict adherence to instructions, for observations precisely recorded, and for accurate inferences. All tests, observations, and inferences must be clearly entered in your answer book, in ink, at the time they are made.

C Is an inorganic salt. D is an organic compound. Carry out the following exercises on C and D. Record your observations and identify any gases evolved. State the conclusion you draw from the result of each test.

(a) (i) Put C in a test tube and add about 10 cm\(^3\) of distilled water. Stir well.

(ii) Divide the resulting solution into two portions. To the first portion add sodium hydroxide solution in drops and then in excess.

(iii) To the second portion add dilute trioxonitrate (V) acid. Then add silver trioxonitrate (V) solution followed by aqueous ammonia in excess. tube and odd about 2- 5 cm\(^3\) of 'Xn'.

(ii) Identify the functional group present in D.

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(a) The electronic configurations of atoms of elements A, B, C and D are given as follows: A. Is\(^2\)2s\(^2\)2p\(^2\); B. 1s\(^2\)2s\(^2\)2sp\(^1\) ; C. 1s\(^2\)2s\(^2\) 2p\(^1\) ; D. 1s\(^2\) 2s\(^2\)

(I) Arrange the elements in order of increasing atomic size, giving reasons

(ii) State which of the elements I. is divalent II. contains atoms with two unpaired electrons in the grouped state. Ill, readily loses one electron from its atom during chemical bonding IV. belongs to group Ill in the Periodic Table.

(b)(i) State one difference between electrovalent and covalent bonds.

(ii) Name two other bonds apart from the ones in (b)(i) above which bind atoms and molecules together.

(iii) State two characteristics of a covalent compound.

(c)(i) What is isotopy?

(ii) Illustrate with suitable example

(iii) Two isotopes of Z with mass numbers 18 and 20 are in the ratio 1:2 Determine the relative atomic mass of Z.

(d)(i) Which of the following elements: calcium, fluorine, iodine neon, magnesium and helium are I. halogens II. noble gases Ill. alkaline earth metals.

(ii) Write a balanced equation for the bombardment of \(^7_3Li\) with protons to produce \(^8_4\beta\) and \(\gamma\)-rays
(iii) State one use of radioactive isotopes.

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(i) Name two amorphous forms of carbon

(ii) State the reason why graphite is a lubricant but diamond is not.

(iii) Draw and label a diagram for the laboratory preparation of a dry sample of carbon (IV) oxide.

(b)(i) Give one example of the following: I. Soil pollutant; II. Water pollutant; III. Air pollutant.

(ii) State the major use of sulphur (IV) oxide in a chemical industry.

(c)(i) Explain in terms of the kinetic theory why petrol is volatile

(ii) State two criteria for determining the purity of a substance.

(iii) Mention one use of each of the following gases: I. Krypton; II. Argon

(d)(i) When zinc metal was added to aqueous copper (I) tetraoxosulphate (VI), the solution turned colourless. I. Name the compound in the colourless solution. II. Write the ionic equation for the reaction. Ill. State what would be observed when a few drops of sodium hydroxide solution is added to a portion of the colourless solution.

(ii) Calculate the volume of CO\(_2\) produced when 5.3g of Na\(_2\)CO\(_3\) reacted with excess HNO\(_{3(aq)}\) + Na\(_2\)CO\(_3\) + 2HNO\(_{3(aq)}\) \(\to\) 2NaNO\(_{3(aq)}\) + CO\(_{2(g)}\) + H\(_2\)O\(_{(l)}\) [H = 1, C = 12, N = 14, O = 16, Na = 23, 1 mole of a gas occupies 22.4 dm\(^3\) at s.t.p.]

Antwoorddetails

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