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Form 2 Chemistry Sample Revision Questions With Answers
State the color of the indicators in the solutions given in the table below:
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1.
Dilute sulphuric (VI) acid does not react fully with calcium carbonate while dilute hydrochloric acid reacts fully with calcium carbonate liberating carbon (IV) oxide.
2.
The table below shows PH values of some solutions
3.
Using dots (•) and crosses (×) show bonding in Ammonium ion (N=14, H=1)
4.
Name the process that occur when anhydrous calcium chloride is left in an open beaker overnight and a solution is formed.
5.
The grid below represents part of the periodic table. Study it and answer the questions that follow. (The letters are not the actual symbols of the elements). a).Which letter represents the element that is least reactive? A b) What type of bond is formed when B and E react? Explain your answer.
6.
Clean iron fillings were weighed and then place on a watch glass containing water as shown. i).State the observation made on the iron ii).With a reason compare the mass of iron fillings at the start of the experiment with that of the product after three days. iii).Give general chemical formula of the product formed in this experiment.
7.
The table below shows some elements and their atomic numbers. The letters do not represent the actual symbols of the elements.
8.
When Magnesium is reacted in steam it forms a white solid and hydrogen gas.
9.
The set-up below was used to electrolyze aqueous copper (II) sulphate. a).Explain why the bulb light brightly at the beginning of the experiment and becomes dim after sometime. b).Write the ionic equation of the reaction that took place at the cathode.
10.
The diagram shows the apparatus used to separate different dyes in food coloring.
11.
The peaks below show the mass spectrum of element X.
12.
The following diagrams show the structures of two allotropes of carbon. Study them and answer the questions that follow.
13.
An ion of oxygen is larger than oxygen atom. Explain.
14.
Carbon (IV) Oxide sublimes at #-78^o# C. It is called dry ice a).Why is it called dry ice? b).It is used for keeping ice cream cold. Why is it preferred to ordinary ice? c).Name two other substances that behave as dry ice
15.
The following diagram represents a non-luminous flame of the Bunsen burner a).Name the parts of the flame labeled A, B and C b).Which of the parts in (a) above is the hottest? c).A non-luminous flame is preferred for heating. Explain d).i) Name the other type of flame produced by
16.
Define the following terms as used in medicine i).Drug ii).Prescription iii).Dosage iv).Drug abuse
17.
Balance the following chemical equations i). #Mg + O_2 -> MgO# ii). #Mg + N_2 -> Mg_3N_2# iii). #Al + HCl -> AlCl_3 + H_2# iv) #C_3H_8 + O_2 -> CO_2 + H_2 0#
18.
Hydrated Copper (II) Sulphate is heated in a boiling tube as shown. i).State the color of Copper (II) Sulphate ii).Explain why the boiling tube was slanted iii).How can the purity of the colorless liquid be confirmed?
19.
Define the following terms; a).Ionization energy b) Electron affinity
20.
The table below shows some properties and electronic arrangements of common ions of elements represented by letters P to X. Study the information in the table and answer the questions that follow i).Give the atomic numbers of the elements P and Q ii).Select the most reactive metallic element iii).Select 3 elements that belong to the same group of periodic table iv).Select 3 elements that would
21.
Observe the equation below #Fe_2 O_(3(s)) + CO_(g) ->Fe_(s) + CO_(2(g))# i).Balance the equation ii).Select the following from the above equation Oxidizing agent Reducing agent
22.
Elements X and Y have atomic numbers 11 and 17 respectively. Which one of the elements is a metal? Give a reason for your answer.
23.
The table below shows the atomic numbers of four elements W, X, Y and Z.Which two elements belong to the same group?
24.
Two elements M and N have atomic numbers 17 and 20 respectively. Write the formula of the compound formed when M and N react.
25.
An element B consists of three isotopes of mass, 28, 29 and 30 and percentage abundances of 92.2, 4.7 and 3.1 respectively. Show that the relative atomic mass of element is 28.11
26.
When lead (II) Carbonate is reacted with dilute Sulphuric (VI) acid, the reaction takes place for a short time and then stops. Explain.
27.
Starting with lead (II) oxide, describe how you would prepare a solid sample of Lead (II) Carbonate.
28.
Study the information in the table below and answer the questions that follow:- (a) Complete the table by filling in the blank spaces (i) , (ii) (iii), and (iv) (b) Identify the particles which are electrically charged
29.
Sodium Carbonate Decahydrate crystals were left exposed on a watch glass for two days. a).State the observations made on the crystals after two days. b).Name the property of salts investigated in the above experiment
30.
Starting with sodium oxide, describe how a sample of crystals of sodium hydrogen carbonate may be prepared.
31.
A piece of marble chips was strongly heated in air for about 30 minutes. Some drops of water were added drop by drop to the product when it was still warm. Using equation, explain: i).What happens when the piece of marble chips is heated? ii) The reaction that takes place when water
32.
When exposed to air, crystals of hydrated sodium carbonate loses water of crystallizations;- i).Name this process ii) Write the formula of hydrated sodium carbonate
33.
A burning magnesium continues to burn inside a gas jar full of carbon (IV) oxide. Explain.
34.
a).Identify two substance that are reacted to regenerate ammonia gas in the Solvay process. b). Write down a balanced chemical equation for the reaction above
35.
Explain how you would obtain solid lead carbonate from a mixture of lead carbonate and sodium carbonate powders.
36.
Describe how the following reagents can be used to prepare copper (II) hydroxide, solid copper (II) sulphate, solid sodium hydroxide and distilled water.
37.
The table below shows the relative molecular masses and the boiling points of methane and water Explain why the boiling point of water is higher than that of methane.
38.
State with reasons whether the changes below are physical or chemical.
39.
A student set-up the apparatus below in order to determine the percentage by volume of oxygen in air. a) Why did water rise when the reaction had stopped? b) The student wrote the expression for the percentage by volume of oxygen in air as #(y-x)/x times 100%# Why the volume of oxygen was calculated using the above expression incorrect? c) What should have been done after the reaction had stopped
40.
Explain why air is considered as a mixture
41.
State the color of the indicators in the solutions given in the table below:
×
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