HYDROGEN
1) Name or state with reference to hydrogen- the first element of the Periodic table.
a) The periodic of the periodic table to which the element hydrogen belongs.
b) The two subgroups of the periodic table in which hydrogen can be placed.
c) The element in period-3 which is electropositive and shows similarity to hydrogen.
d) The element in period-4 which is electronegative and shows similarity to hydrogen.
e) An element in period-2 which has the same atomicity as hydrogen.
f) An element which combines with both hydrogen and halogens forming covalent compounds.
g) An electrovalent compound formed from an element in period-3 and hydrogen.
h) A covalent gaseous compound formed from an element in period-3 and hydrogen.
i) A covalent gaseous compound formed from an element in group IV A and hydrogen.
j) An oxide of hydrogen which is neutral in nature.
k) The number of shared pairs of electrons in a diatomic molecule of hydrogen.
l) A non metallic element in group IA of the periodic table.
2) Complete the following sentences that filling in the blanks with appropriate word/s.
a) The first element hydrogen of the periodic table shows similarity with __ metals of group IA and _____ of group VIIA.
b) Hydrogen shows electropositive character. Elements in group IA are considered electropositive since they have a tendency to ___ one electron from its valence shell.
c) Hydrogen also shows electronegative character. Elements in group VIIA are considered electronagative since they have a tendency to ____ one electron forming an electronegative element.
d) The electronic configuration of the elements in period-3 which has the same number of valence electrons as hydrogen is _____ .
e) The element in group IA which has one electron less than the noble gas present in period-1 of the periodic table is _____ .
f) Hydrogen is a diatomic molecule which has two atoms linked by a ____ covalent bond. The element in group VIIA which is also diatomic and exists in the liquid state at room temperature is ____ .
g) Halides of hydrogen and alkali metals yield____ ions in aqueous solution. During electrolysis these ions of discharged at the negative electrode i.e., cathode .
3) Give reasons for the following:
a) Hydrogen can be positioned in group IA and group VIIA of the periodic table.
b) Hydrogen can be represented as H¹⁺ or as H¹⁻.
4) Match the points pertaining to the occurrence and discovery of hydrogen in column I with the concluding facts in column II
COLUMN I
A) Lavoisier in 1783 established the name 'hydrogen'
B) Hydrogen does not occur
C) Hydrogen is present in traces in
D) A compound, one ninth by mass of which is hydrogen in the combine state is
COLUMN II
a) the atmosphere around the sun and stars.
b) water
c) meaning 'water producer'
d) in the free state on Earth.
5) Hydrogen is prepared from cold water, boiling water or steam by reaction with certain metals involving potassium, sodium, calcium and magnesium, aluminium, zinc, iron. Complete and balance the equations for the reactions of the above metals with water by substituting the correct symbols in each case.
a) Reaction with cold water
i) X + H₂O --> XOH + H₂ [X- burns in air with a lilac flame].
ii) Y + H₂O --> YOH + H₂ [Y-burns in air with a golden yellow flame].
iii) Z + H₂O --> Z(OH₂)+ H₂ [Z-burns in air with a brick red flame].
b) Reaction with boiling water or steam
i) Q + H₂O --> QO + H₂ [QO - is a basic oxide].
ii) R + H₂O --> RO + H₂ [RO- is an amphoteric oxide].
iii) S + H₂O --> S₂O₃ + H₂ [S- is a trivalent metal].
iv) T+ H₂O <==> T₃O₄ + H₂ [Reaction of T with steam is reversible]
6) Hydrogen is also prepared by the action of metals and dilute acids and on alkalis. The metal is converted to its salt and gaseous hydrogen is liberated.
Complete and balance the equation for the conversions of the following metal to their salts using an acid or an alkaline.
Metal Acid/Alkali Salt Hydrogen
a) Mg ___--> _______ + H₂
ᵐᵃᵍⁿᵉˢᶦᵘᵐ ᶜʰˡᵒʳᶦᵈᵉ
b) Al + ___ --> ________ + H₂
ᵃˡᵐᵘⁿᶦᵘᵐ ˢᵘˡᵖʰᵃᵗᵉ
c) Fe + ___ --> ________ + H₂
ᶠᵉʳʳᵒᵘˢ ᶜʰˡᵒʳᶦᵈᵉ
d) Zn + ___ --> ________ + H₂
ˢᵒᵈᶦᵘᵐ ᶻᵘⁿᶜᵃᵗᵉ
e) Pb + ___ --> ________ + H₂
ˢᵒᵈᶦᵘᵐ ᵖˡᵘᵐᵇᵃᵗᵉ
f) Al + ___ --> ________ + H₂
ˢᵒᵈᶦᵘᵐ ᵃˡᵘᵐᶦⁿᵃᵗᵉ
g) Al + ___ --> ________ + H₂
ᵖᵒᵗᵃˢˢᶦᵘᵐ ᵃˡᵘᵐᶦⁿᵃᵗᵉ
7) Give reasons for the following:
a) Sodium and potassium are not preferred as the starting metals in the preparation of hydrogen from cold water.
b) Amalgamated sodium can be used in place of sodium in the above preparation.
c) Reaction of magnesium or aluminium with boiling water is comparitively slow and the reaction later comes to stop.
c) Reaction of magnesium or aluminium with boiling water is comparitively slow and the reaction later comes to stop.
d) The reaction in (c) above can be made to proceed again by passage of steam over the red hot metal.
e) Reaction of magnesium with water moves in the forward direction only while that of iron with water (steam) is a reversible reaction.
f) Dilute nitric acid is generally not used in the preparation of hydrogen from metals, however, magnesium reacts with very dilute nitric acid at low temperatures liberating hydrogen.
g) Dilute acids react with metals liberating hydrogen, even then lead is not used in the reaction with dilute hydrochloric or Sulphuric acid.
8) Name the following:
a) A metal which reacts explosively with cold water liberating hydrogen.
b) A metal alloyed with sodium to give amalgamated sodium.
c) A metal which reacts very slowly with boiling water to liberate hydrogen.
d) A trivalent metal which displaces hydrogen from dilute sulphuric acid.
e) The salt formed when iron reacts with dilute hydrochloric acid displacing hydrogen from it.
f) A metal which reacts with dilute hydrochloric acid to form a salt insoluble in cold water but soluble in hot water.
g) The salt formed when zinc reacts with caustic potash liberating hydrogen..
h) A metal other than magnesium which reacts with very dilute nitric acid laborating hydrogen.
i) A metal which reacts with cold water forming a tarbid solution.
j) Two metals which do not displace hydrogen from dilute acids.
9) Give reasons for the following
a) Granulated zinc is preferred to pure zinc for the reaction with dilute acid.
b) The initial gas bubbles of hydrogen are allowed to escape out before the actual collection of hydrogen gas.
c) Highly electropositive metals are not used in place of zinc in the preparation.
d) Concentrated hydrochloric acid is not preferred to dilute acid for reaction with zinc in the laboratory preparation.
e) A naked flame is never brought near the apparatus used in the laboratory preparation.
f) The lower end of the thistlle funnel should dip below the level of the dilute acid in the flask.
g) Traces of copper [II] sulphate maybe added to the reaction medium.
h) Hydrogen gas prepared in the laboratory has a peculiar smell.
i) Hydrogen is lighter than air, even then it is not collected over air, but by downward displacement of water.
10) Pure hydrogen is prepared by passage of the gas through various solutions which respectively absorbs each impurity. Match the impurity with the solution which absorbs it.
11) Pure hydrogen is prepared by passage of the gas through various solution which respectively absorb each impurity . Match the impurity with solution which absorbs it.
Impurity
A) Arsine[AgH₃]
B) Phosphine [PhH₃]
C) Hydrogen sulphide[H₂S]
D) Nitrogen dioxide [NO₂]
E) Sulphur dioxide [SO₂]
F) Moisture
Removed by
a) Potassium hydroxide solution
b) Fused calcium chloride
c) Silver nitrate solution
d) Lead nitrate solution
12) Complete the table pertaining to the production of hydrogen by the Bosch process involving three main steps.
Step I : Production of Water gae
X + H₂O ---°C---> XO + H₂ ∆
• Equation : ___''
• X is white/ red hot ______
• Temperature of the reaction ______°C.
• Reaction involves passage of ____[ water/ steam] over X.
• Reaction is____[ exothermic/ endospermic]
• Resultant product of the reaction is water gas is a mixture of ____[XO] and hydrogen in the ratio ___ : ____ .
Step -II Reduction of steam to hydrogen by XO
XO + H₂ + H₂O ---°C--> XO₂+ 2H₂
• Equation : _____
• The reactant are water gas and ___[ limited/excess] steam.
• Temperature of the reaction is around ____ °C.
• The catalyst used is ____ [Y₂O₃].
• The promoter used is____[Z₂O₃].
• The catalyst also used other than the one used in (d) above is ____.
• _____[XO] is ______[oxidized/reduced] to ___[XO₂] with a further yield of hydrogen in the reaction in Step II .
• Reaction in Step II is _____[exothermic/endothermic]
Step- III: Removal of carbon monoxide and carbon dioxide from the above mixture.
Using X, Y and Z how are the gases separated.
X= Potassium hydroxide, Y= Water , Z= Ammoniacal Cuprous chloride.
Solution Gas absorbed Equation
X = KOH
Y= Water
Z= Ammoniacal CuCl₂
13) A method other than the one used above for manufacture of hydrogen involves electrolysis of neutral liquid [X] as the starting reactant.
a) Name the neutral liquid [X].
b) Give the equation for the electrolysis of the same.
c) Name the electrode at which hydrogen is liberated.
d) State the reason for acidification of the neutral liquid.
e) Name another solution which on electrolysis liberate hydrogen as a by product.
14) Using hydrogen as one of the reactants how do you obtain:
a) A neutral liquid using a neutral gas.
b) An acidic gas using another acidic gas.
c) A basic gas using an unreactive gas.
d) A acidic gas using vapours of nonmetal
e) A hydride using a monovalent active metal.
15) Hydrogen reduces certain metallic oxides to free metals. Give an equation of each of the following reductions.
Metallic oxide Equation for reduction
a) a black basic oxide
b) a yellow amphoteric oxide.
c) an oxide of iron.
16) Name the following :
a) The condition in which equal volumes of hydrogen and chlorine react slowly producing hydrogen chloride.
b) The catalyst ar promoter used in the conversion of Nitrogen to ammonia using H₂.
c) The state of sulphur which reacts with hydrogen forming hydrogen sulphide.
d) The phenomenon due to which certain metals eg., palladium adsorb large volume of hydrogen on their surface.
e) A catalyst used in hydrogenation reactions.
f) A product manufactured using the process of hydrogenation of oils.
g) The product of oxidation of hydrogen formed during reduction of zinc oxide by hydrogen.
h) The product formed when pure hydrogen burns in oxygen.
i) A metallic oxide which is not reduced to its metal by hydrogen.
j) Two colourless gases one of which is hydrogen which combines under suitable conditions to give another Colourless gas.
17) Give reasons for the following:
a) Nickel finds application in hydrogenation reaction eg., hydrogenation of oil.
b) Passage of hydrogen through vegetable oils under suitable conditions results in their solidification.
c) Pure hydrogen burns quietly while a hydrogen -air mixture does not.
d) Hydrogen can be separated from a mixture of hydrogen and carbon dioxide by liquefaction.
18) The table below represent the metal activities series with the most active metal at the top of the series and the least active below. Name the following:
Activity series Name of metal which _
K 1. Reacts violently with water liberating hydrogen.
Na 2. Does not react with steam or dil. HCl.
Ca 3. Is divalent and displaces hydrogen from water.
Mg 4. Displaces hydrogen from caustic soda but does not react with dil HCl .
Al
Zn 5. Displaces hydrogen from very dilute to nitric acid.
Fe 6. Does not react with the dil. sulphuric acid but reacts with steam liberating hydrogen
Pb 7. Displaces hydrogen from dil. HCl and dil H₂SO₄ but not from dil nitric acid.
[H]
Cu 8. Reacts violently when placed in any dilute acid.
Hg 9. Displaces hydrogen from cold water forming a Colourless solution.
Ag
Au 10. Displaces hydrogen from steam leaving behind an amphoteric residue.
19) Give reasons for the following:
a) Hydrogen gas can be tested by its combustibility in air.
b) If a jar containing hydrogen-carbon dioxide mixture is placed over an empty porous pot, the porous pot gets filled with hydrogen initially.
c) Two gas jars, one containing 'oxygen' and the other 'hydrogen' can be identified with a glowing splinter, but not with a moist litmus paper.
d) Hydrogen finds application as a constituent of important fuels.
e) Hydrogen gas was initially used to study weather conditions.
e) Hydrogen gas was initially used to study weather conditions.
f) Extraction of certain metals from their oxides may be carried out using hydrogen.
g) Oxy-hydrogen flames used in welding and cutting of metals produce high temperatures.
h) Hydrogen finds application in the conversion of palm oil to solid fats.
THE PERIODIC TABLE
1) Complete the statements given below pertaining to different Chemists and their contributions towards classification of elements by chosing the correct words from the following list.
(Mendeleeff, Robert Boyle, Early Chemists, Newland, Lavoisier, Doberenier, Carl Scheele, Moseley, Humphry Davy)
a) _______attempted to classify elements on basis of their properties, metallic and non metallic nature, valency etc, but the classification was discarded and atomic weight and not properties were considered for further classification .
b) ______ classified elements into groups of three on observing a relationship between atomic weights of certain elements and their properties. He arranged elements in increasing order of atomic weights in groups of three called triads.
c) ______ are arranged elements in series in ascending order of their atomic weights and suggested a resemblance between the eighth and first element similar to the 8th and first notes on a musical scale.
d) _______ arranged elements in increasing order of their atomic weights and observed that elements with similar properties appear at regular intervals on arrangement. Such properties are called periodic properties and are those which appear at regular intervals in a periodic table. Examples of such properties are valency, electronegativity, metallic and nonmetallic character.
e) _____ stated that atomic number and not atomic weight of an element should be taken into consideration for classification of elements .
f) _______periodic law states that the physical and chemical properties of elements are periodic functions of their atomic weights.
g) ______arranged elements in increasing order of atomic numbers in seven horizontal rows called periods and 18 vertical columns called groups.
2) State the following with respect to Table A and Table B pertaining to classification of elements by different scientists
Table - A
Elements lithium sodium potassium carbon nitrogen oxygen
At. Weight 7.0 23.0 39.0 12.0 14.0 16.0
Table B
Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine
Sodium Magnesium Aluminium Silicon Phosphorus sulphur Chlorine
23.0 24 27 28 31 32 35.5
a) Name the scientist whose law pertains to classification of elements as seen in Table A.
b) State the law which pertains to classification of elements as seen in Table A .
c) Name the scientist whose law pertains to classification of elements as seen in Table B.
d) State the law which pertains to classification of elements as seen in Table B.
3) Give reasons for the following:
a) Classification of elements by early chemists on basis of properties, valencies and Metallic and nonmetallic nature of elements was soon discarded.
b) Dobereinier's Law of Trials did not hold weightage as a standard for classification for all elements.
c) Newland's classification of elements led to much criticism.
4) Name or state the following reference to Mendeleef's periodic table:
a) On what basis was the classification of elements made by Mendeleeff.
b) State the terms used for the following pertaining to Mendeleef's periodic table.
i) The horizontal rows of elements in the periodic table.
ii) The vertical columns of elements in the periodic table.
iii) The properties which repeat themselves at regular intervals in the periodic table.
c) State three contributions made by Mendeleef's which significantly helped to form the basis of the Modern Periodic Table.
d) Give reasons why Mendeleeff Periodic Table was not completely accepted as the Modern Periodic Table.
5) Name or state the following pertaining to the Modern Periodic Table.
a) The fundamental characteristics of an element which formed the basis of classification of elements in the Modern Periodic Table.
b) The number of horizontal rows - periods in the table.
c) The number of vertical columns - groups in the table.
d) The period which contains only two elements.
e) The period which contains 8 elements each .
f) The period which contains the element having stable electronic configuration 2,8,8.
g) The first element of the periodic table,
h) The type of elements present in the zero group of the periodic table.
i) The last element of the third short period.
j) The period which contains the lanthanide series which is situated at the bottom of the periodic table.
k) The group which are further divided into subgroups A and B.
6) Name or state the following pertaining to the elements of the periodic table.
a) The number of electron shell in the elements of periods one, two or three respectively.
b) The electronic configuration of the zero group element of period-1.
c) The number of valence electrons of the element in group IV of period-2 of the periodic table.
d) The valency of the elements of group IA, VIIA and zero group.
e) The group to which the elements carbon (at no. 6), nitrogen (at no, 7) and oxygen (at no 8) belong.
f) The period to which sulphur (at no 16) and chlorine (at no 17) belong.
g) The electronegative element from the element sodium, magnesium and sulphur.
h) The type of bonding seen in the oxide of the element in period-3, group IIIA.
i) An element in period-3, group VA whose chloride exists in two different physical states.
j) The groups of the periodic table which contains the alkali metals , alkaline earth metals and the halogens respectively.
k) The grouping name given to the type of elements present in groups
i) IB to VIIB and VIII
ii) IA to VIIA
l) The non metal positioned in group IA.
m) The series of chemically reactive metals of period -7 placed at the bottom of the periodic table.
n) The least electronegative elements from the elements chlorine, bromine and Iodine in group VIIA.
o) The element in period-2, group IA, which shows similarity with a divalent metal in period-3 group IIA.
p) The non metallic element in period-2 to which is diatomic and unreactive at ordinary temperatures.
7) State whether the following statements of true or false. If false rewrite the correct statement.
a) Element with similar outer electronic configuration are placed in the same period of the periodic table.
b) If properties of one member of a group is known the properties of other members of the group could be correlated due to similarity or gradation in properties of elements in a group.
c) Non metals occupy the upper right hand corner of the periodic table.
d) The two sub groups A and B accommodate elements with similar properties.
e) Properties of elements remain the same on moving from left to right in the modern periodic table,
f) Electronegativity and nonmetallic character of elements increases across a period from left to right and decreases down a group.
8) Write i) Electronic configuration ii) Group Assigned iii) Metallic/ nonmetallic iv) Electronegative/Electropositive of the following:
Element Atomic number
a) Hydrogen. 1
b) Carbon 6
c) Nitrogen 7
d) Oxygen 8
e) Sulphur 16
f) Chlorine 17
g) Lead 82
h) Bismuth 83
i) Polonium 84
j) Astatine 85
TEST- PAPER (Chemistry)-1
SECTION - A (40 Marks)
(Attempt all)
1) Complete the statements by filling in the blanks with the correct word/s: (10x1=10)
a) Direct combination reaction Sulphur dioxide with water gives _____. (H₂SO₄/H₂SO₃/H₂S₂O₇).
b) Formation of hydrogen chloride from hydrogen and chlorine is an example of ____. ( photochemical reaction/ electrochemical reaction)
c) The reaction of hydrogen burning in oxygen to give a neutral liquid is an example of ____ (exothermic/ endothermic) reaction.
d) The neutral gas evolved when lead nitrate undergoes thermal decomposition is ____( nitrogen dioxide/ oxygen/ nitrogen).
e) The reddish brown precipitation obtained during a double decomposition - precipitation reaction between an iron salt and an alkali is (iron(II) hydroxide/iron(III) hydroxide).
f) Isotopes have same ____(number of neutrons/ electronic configuration/ atomic masses).
g) An____(atom/ ion) is capable of independent existence in solution.
h) An atom with electronic configuration 2, 7 and mass number 19 will have ____ neutrons (8/10/12).
i) The most reactive halogen from group 17_____ (Chlorine/fluorine/ bromine)
j) _____(group-1/group -2.group-3) is the number of the elements atomic number 4.
2) Select the correct answer from given option (1×14=14)
(Decreases , increases , remains same, increases by one, electropositive, electronegative, ammonia, hydrogen chloride, hydrogen, nitrogen dioxide, nitric oxide.
a) Across a period from left to right in the Modern Periodic Table.
Number of electron shells ____. Number of valence electrons____. Electronegativity___ characters of the element changes from ____to____.
b) Down a group in the modern periodic table.
Number of electron shells______. Number of valence electrons___. Electronegativity _____character of elements changes from _____to ____.
c) State the gases products formed, when--
i) An active metal reacts with dilute sulphuric acid.
ii) A metallic nitrate undergoes thermal decomposition giving a coloured gas.
iii) Two gases one of them neutral, combines by absorption of light energy.
iv) An ammonium salt reacts with an alkali.
v) An exothermic reaction takes place between ammonia and a neutral gas.
3) Match the column (10)
Column I
A) Highly reactive, univalent metals.
B) Highly reactiva, univalent non metals
C) Unreactive inert elements
D) Elements of group 3 to 12(1B to VIIB, VIII)
E) Radioactive elements
F) AB <=> A+ B
G) AB--> A+ B
H) X⁺Y⁻ + A⁺B⁻--> X⁺B⁻ + A⁺Y⁻
I) X + YZ--> XZ + Y
J) X+ Y --> XY - ∆
ʰᵉᵃᵗ
Column II
P) halogens
Q) transition elements
R) alkali metals
S) lanthanide series
T) Nobel gases
U) actinide series
V) double decomposition
W) thermal dissociation
X) endothermic reaction
Y) displacement reaction
Z) decomposition reaction
4) Give balanced equations for reaction involving evolution of a gas on addition of dilute acid to-- (4)
a) sodium sulphite
b) calcium carbonate
SECTION - II
5) a) Define: (2×3==6)
i) Decomposition reaction
ii) alkaline earth metals
iii) Isotopes
b) Draw the geometric atomic structure of each of the following atoms showing the number of electrons, protons and neutrons in each of them: (2×2)
a) ¹²₆C
b) ³¹₁₅P
6) Name or state the following: (Any 10) (10×1=10)
a) The three isotopes of hydrogen.
b) Two elements having same number of protons and electrons but different number of neutrons .
c) The valency of an element whose electronic configuration is 2, 8, 3.
d) The shell closest to the nucleus of an atom.
e) An element having valency 'zero'
f) The non-metallic element present in period 3 other than Sulphur and chlorine.
g) A nonmetal in period 2 having electronic configuration 2, 6.
h) An electrovalent compound formed between an alkali metal and a halogen.
i) A covalent compound formed between an element in period 1 and a halogen.
j) An alkali metal in period 3 which dissolves in water giving a strong alkali.
k) A metal in period 3 having valency.
l) The bridge elements of period 3 of group 1 [1A], 2[IIA], 13[IIIA].
7) a) State the following: (5)
i) The group to which the element with electronic configuration of 2, 8, 2 belongs.
ii) The group from groups 1[1A], 2[IIA], 16[VIA] , 17[VIIA] whose elements are most electronegative.
iii) The group which contains highly electropositive metals including sodium.
iv) The group whose elements are unreactive or inert.
iv) The group which contains highly reactive electronegative non-metals including Chlorine.
b)
State the number of neutrons in each of the atoms A to E. Also state which of the atoms A to E is a metal. (5)
8)a) Differentiate between the following terms: (6)
i) Valence shell and penultimate shell.
ii) Atomic number and mass number.
iii) Octet and duplet
b) Name the solid residual product formed in each reaction and state it's colouring during-- thermal decomposition of the following substances. (4)
i) copper nitrate.
ii) ammonium dichromate.
iii) zinc carbonate.
iv) lead nitrate.
9) a) Explain : 'silver nitrate solution is kept in coloured reagent bottle in the laboratory. (2)
b) Give a balanced equation for conversion of--
i) an ammonium salt to a basic gas.
ii) a soluble lead salt to an insoluble lead salt - formed as a white precipitate. (2)
c) Why noble gases do not found compounds readily . (2)
d) Represent each of the following: (2)
i) a proton 'p'.
ii) an electron 'e'.
iii) a neutron 'n' in terms of its symbols showing the subscript and superscript values. (2)
e) Explain the octet rule for formation of -
i) sodium chloride from a sodium atom and a chlorine atom.
ii) nitrogen molecule from two nitrogen atoms. (2)
ANIMAL TISSUE
A) State whether the following statement are true or false:
1) Epithelial cells rest upon a thin basement membrane.
2) Animal tissues are less diverse than plant tissues.
3) Epithelium protects the organs from the mechanical injury.
4) Epithelial cells are exclusively protective tissues .
5) Epithelial cells lack intercellular speces.
6) Tendons and Ligaments connect two bones and provide movement.
7) Blood plasma is straw-coloured fluid.
8) External ear is made up of flexible cartilage.
9) Ligaments allows the tissues to resist mechanical stress.
10) Haemoglobin provides red colour to the blood.
11) Lymph is straw-coloured because of the presence of WBC s.
12) The muscles of limbs are striped in work at our will.
13) Cardiac muscles work continuously.
14) The axons bundle together to form a muscle.
15) Nerves receive the message through dendrons .
16) Smooth muscles are cylinderical and elongated.
17) Blood and lymph constitute the fibrous connective tissue.
18) Cardiac muscles and skeletal muscles have striated apreence.
19) Voluntary muscles are found in the internal organs of the body.
20) The dendrons of nerves transmits messages to the other nerves.
21) Adipose tissue protects us from external socks.
22) Lymph is straw-coloured and lacks WBCs
B) Choose the correct option :
1) Which of the following is not a connective tissue ?
a) Adipose tissue b) blood c) cartilage d) Nerves
2) Tendons is a tissue that connects
a) a bond to another bone.
b) a nerve to a muscle
c) a muscle to a bone
d) a muscles to another muscle.
3) Cardiac muscles are
a) branched and voluntary
b) branched and involuntary
c) unbranched and voluntary
d) unbranched and involuntary
4) The cells responsible for blood clotting are
a) erythrocytes
b) leukocytes
c) chondrocytes
d) thrombocytes
5) Which of the following is not a connective tissue
a) bone b) blood c) cartilage d) epithelium
C) Fill in the blanks with missing words:
1) Cartilage consists of____ cells while the cells of bones are called____.
2) ____ muscles help in the moment of the food in food pipe.
3) _____ blood cells protect the body against pathogens.
4) The nervous tissue helps in the ____and____ of body.
5) ____ muscles never take rest.
6) The adipose tissue is responsible for the storage of ______.
D) Match the following
Column A
1) spindle-shaped
2) Sendrites
3) Haemoglobin
4) Blood clotting
5) Striated muscles
6) Heart
Column B
a) Erythrocytes
b) Platelets
c) Skeletal muscles
d) Neuron
e) Cardiac muscles
f) Smooth muscles
E) Pick out odd one out
1) Bone, blood, tendon, nerve.
2) Involuntary, cardiac, skeletal, smooth.
3) Cardiac, axon, smooth, skeletal.
4) Areolar , ligament, adipose, cartilage
F) Name the type of tissue found in
1) brain and spinal cord.
2) between two bones.
3) On the surface of human skin.
4) between muscles in bones.
5) hands and legs.
6) the wall of the heart.
G) Identify the following tissue :
1) Muscular tissue that works at our will.
2) Straw-coloured fluid connective tissue lacking RBCs.
3) Muscles that does not get tired.
4) Muscles that helps to pick up objects .
5) Skeletal connective tissue composed of chondrocytes.
6) Fluid connective tissue on containing RBCs.
H) Observe the figure carefully and answer the questions given below.
a) Identify the muscular tissue.
b) Write any two features by which you identified the tissue.
c) Where will you find this tissue in your body.
d) Are these muscles voluntary or involuntary ?
e) Name the other two kinds of muscles present in our body. Write two features and at least one function of each kind of muscle.
CLASSIFICATION OF ORGANISMS
A) Fill in the blanks with appropriate words
1) The arrangement of the organisms into groups on the basis of their features is known as____
2) ____ is the lowest category of classification.
3) _____ kingdom classification is the oldest system of classification.
4) Kingdom____ was included in three kingdom classification.
5) Five kingdom classification proposed by ______
6) _____helpd us to understand the life from basic features.
7) _____Kingdom contains prokaryotic organisms.
8) ______and____ bacteria present in the curd help in its formation.
9) Amoeba reproduces by the process of____ fission .
10) Bacteria are of industrial importance to produce____and____.
11) Protists are ____organisms because of the presence of well-defined____.
12) ____is used in bakeries for making bread and cakes .
13) Two common fungi are _____and____.
14) _____ is saprophytic fungus.
15) All the organisms including Kingdom____ are autotrophic.
16) The cell wall of all plants is made up of _____.
17) The new Kingdom proposed by Haeckel includes____ eukaryotes.
18) Classification arranges organisms into groups on the basis of their____.
19) The animals which feed on dead organic matter are____.
20) The organisms belonging to the kingdom____ are Prokaryotes.
21) The antibiotics, penicillium, is obtained from a ____.
B) Choose the correct option:
1) All protozoans are
a) unicellular prokaryotes.
b) unicellular eukaryotes.
c) multicellular prokaryotes
d) multicellular eukaryotes .
2) Staphylococcus belongs to Kingdom Monera as it is
a) unicellular eukaryote.
b) multicellular prokaryote.
c) unicellular prokaryote.
d) multicellular eukaryote.
3) The lowest category of classification is
a) family b) order c) genius d) species
4) Identify the correct group.
a) Monera - Yeast, mushroom, spirogyra
b) Protista -- Paramesium, Euglena, amoeba
c) Fungi -- Rhizopus, penicillium, Escherichia
d) Plantae---- Pea, amoeba, yeast
5) Only Kingdom comprising all autotrophs is
a) fungi b) Monera c) protista d) plantae
C) State whether the following statements are true or false:
1) Species is the highest category of classification.
2) All protists are unicellular, eukaryotic, autotrophs.
3) Two Kingdom classification was proposed by Linnaeus.
4) Whittaker added Monera and Protists as new Kingdoms .
5) All fungi are parasitic organisms which derive nutrition from other organisms.
D) Pick out the odd one out:
1) Fungi, Yeast, bacteria, mushrooms.
2) Agaricus, Amoeba, Paramesium, Euglena .
3) Linnaeus, protista, plantae, Animalia.
4) Lactobacillus, Amoeba, Bacillus, Staphylococcus.
E) Identify the following picture and answer the following questions.
a) Name the organism and the kingdom it belongs to.
b) Write any two characteristic features of the Kingdom .
c) Give two more examples of the above Kingdom.
CLASSIFICATION OF ANIMAL
A) Name the group to which the following animals belong:
Hydra, Amoeba , Earthworm, Ascaris, Tapeworm, Sycon, Euglena, Liver fluke.
B) Identify the group of animals from the following characteristics :
1) Gut with a single opening.
2) Body divided into segments.
3) Body unsegmented and flattened.
4) Excretion takes placed by nephridia
5) Presence of Cnidoblasts.
6) Spines on the body.
7) Body covered by exoskeleton.
8) Pores on the body.
9) Nephridia as respiratory organs.
10) Presence of joints in appendages.
11) is segmented into ring-like segments.
12) has jointed legs .
13) is enclosed in a calcareous shell.
14) has a flat body
15) moves with the help of the tube feet .
16) moves with the help of pseudopodia.
C) Fill in the blanks with appropriate words:
1) The tentacles of Hydra have____ cells .
2) Excretion in leech takes place through_____.
3) Ascaris lives in the____ of human beings.
4) Molluscs have ____ for locomotion.
5) ____ have three pairs of legs for movement.
6) The tube feet help in____ and capture of food.
7) The____ have a soft body and are covered with a hard____.
8) Hydra belongs to the phylum_____.
9) The backbone of animals is made up of small_____.
10) The body of arthropods is____and covered with____.
11) Earthworm has a____ body and has____ for excretion.
D) Name an organism which has the following features:
1) Spines on skin.
2) unsegmented soft body enclosed in a shell .
3) Body divided into head, thorax and abdomen.
4) Head with two pairs of antennae.
E) Choose the correct option
1) Earthworm is an annelid because of the presence of
a) tube feet
b) pores on body
c) nephridia
d) hard exoskeleton
2) The Echinoderms have
a) many jointed appendages
b) a single foot for locomotion
c) small tube feet for movement
d) a well developed brain.
3) Identify the correct group.
a) Porifera-- Leech , Hydra, Tapeworm
b) Annelida--- Crab, Lobster, Earthworm
c) Arthropoda--- Cockroach, Prawn, Ant
d) Echinodermata--- Star fish, Prawn, Snail
4) Cnidoblasts are the characteristic feature of
a) cnidarians b) arthropods c) nematodes d) Molluscs
5) Tube feet help in the moment of
a) starfish
b) earthworm
c) roundworm
d) flatworm
F) State whether the following statements are true or false
1) Body of Echinoderms has a large number of spines.
2) Ascaris is a parasitic form which lives in the human intestine.
3) Annelids have flame cells as excretory structures .
4) Invertebrates have tube-like structures in their body for blood flow.
5) Liver fluke is roundworm and has only one opening.
G) Pick the odd one out:
1) Earthworm, leech, roundworm , Annelida.
2) Octopus, slugs, snails , starfish
3) Tube feet, starfish, jellyfish,
4) Annelids, Mollusca, vertebrae, porifera.
5) exoskeleton, joints , foot, prawn
H) Identify the picture and answer the following questions.
a) Name the organism and the phylum it belongs to.
b) Write any two characteristic features of the Phylum.
c) Give two more examples of the above Phylum
ATOMIC STRUCTURE
1) Define the terms
a) Atomic number
b) Mass number
c) Electron
2) From the symbol ⁴₂He for the elements helium, write down the mass number and the atomic number of the element.
3) a) Sulphur as an atomic number of 16 and a mass number of 31. State the number of protons and neutrons present in the nucleus of sulphur.
b) Give a simple diagram to show the electrons in an atom of sulphur.
4) ²⁴₁₂Mg and ²⁶₁₂ Mg are symbols of two isotopes and magnesium. compare the atoms of these isotopes with respect to:
a) the composition of their nuclei.
b) their electronic configurations .
c) give the reason why the two isotopes of magnesium have different mass numbers.
5) Chlorine is an element of atomic number 17. It is a mixture of two Isotopes having mass number of 35 and 37.
a) What is meant by "atomic number of an element"? What do you understand by an 'atom'.
b) Write down the electronic configuration the chlorine atom.
c) State the number of protons , electrons and a neutrons in the following isotopes: ³⁷Cl₁₇, ³⁷Cl₁₇.
d) Explain why the two atoms in (c) above have the same chemical reactions.
e) If molten magnesium chloride is electrolysed suggest suitable electrode(anode). Carbon
6) Five atoms are labelled V to Z
Atoms mass number. Atomic number
V 40 20
W 19 9
X 7 3
Y 16 8
Z 14 7
i) Which one of these atoms (a) contains 7 protons (b) has an electronic configuration 2.7 ? Z, W
ii) Write down the formula of the compound formed by atoms X and Y. X₂Y
7) Element X, Y, Z have atomic numbers 6, 9 and 12 respectively, Which one:
a) forms anions - negative ion.
b) forms cation - positive ion.
c) has 4 electrons in the outermost orbit.
8) The atoms of aluminium is represented by ²⁷Al₁₃. Write down the number of
a( electrons
b) protons
c( neutrons
d) the arrangement of electrons in the different orbits or shells in one atom of aluminium.
9) Name the element which does not contain any neutrons in its nucleus.
10) Elements A, B, C have atomic number 9, 20 and 10 respectively.
a) State which one is (i) a nonmetal (b) a metal (c) a chemically insert
b) Write down the formula of the compound formed by two of the above elements.
11) Write down the electronic configuration of the following:
a) ²⁷₁₃X
b) ³⁵₁₇Y.
Write down the number of electrons in X and neutrons in Y and the formula of the compound formed by X and Y. XY₃
12) Write down:
a) The mass number of the atom having 20 neutrons and 15 protons.
b) The number of neutrons in the nucleus of an atom having atomic number 17 and mass number 37.
13) What is the relation between the number of protons and the number of electrons in an atom.
14) Copy and complete the following table relating to the atomic structure of some elements.
Element At. No Mass.no pro neu elect
Beryllium 4. 9
Fluorine 9 10
Sodium 12 11
Phosphate. 31 15
15) The electronic structure (configuration) of fluorine can be written as 2,7. In a similar way give the electronic configuration of:
a) aluminium
b) phosphorus
16) Represent each of the following:
a) a proton 'p'.
b) an electron 'e'.
c) a neutron 'n' in terms of its symbols showing the subscript and superscript values.
17) An element 'A' has mass number 23 and atomic number 11. State the
a) number of neutrons in its shell.
b) electronic configuration of the element 'A'.
18) The following elements U and Z are given :
₃U, ₆V, ₉W, ₁₄X, ₁₈Y, ₂₀Z.
State the electronic configuration of each and state whether they are metals, non metals or insert gases.
19) Draw the geometrical atomic structure of each of the following atoms showing the number of electrons, protons and neutrons in each of them:
a) ¹²₆C
b) ²³₁₁Na
c) ³¹₁₅P
d) ³⁹₁₉K
e) ⁴⁰₂₀Ca
20) Four elements A, B, C, D are given :
A shows the presence of 20 neutrons and 17 electrons.
B shows the presence of 18 neutrons, 17 protons and 17 electrons.
C shows the presence of 10 neutrons, 9 protons and 10 electrons.
D shows the presence of 4 neutrons , 3 protons and 1 electrons.
State which of the above is-
a) an atom
b) a cation
c) a pair of isotopes.
Write the formula of the compound formed between D and C.
21) Difference between the terms -
a) stable and unstable electronic configuration
b) Duplet and octet rule
c) Electron and proton
d) atomic number and mass number
e) nucleus and nucleons
f) Valence shell and penultimate shell
22) Select the correct answer from the answers in brackets to complete each sentence.
a) An element has electronic configuration 2, 8, 1 and 12 neutrons. Its mass number is ____( 11/23 /12).
b) The maximum number of electrons in M shell is _____(8/32/18).
c) Isotopes have same____( number of neutrons/ electronic configuration/ atomic masses).
d) An___( atom/ion) is capable of independence existence in solution.
e) An atom with electronic configuration 2,7 and mass number 19 will have____ (8/10/12).
23) Give reasons for the following:
a) the physical properties of isotopes of the same element are not identical.
b) the mass number of an atom is slightly less than the actual atomic mass.
c) the shells surrounding the nucleus of an atom are also called 'energy levels'.
d) Helium is chemically extremely unreactive.
e) Mass number is slightly less than the actual atomic mass.
24) Name the state the following:
a) the three isotopes of hydrogen.
b) Two elements having same number of protons and electrons but different number of neutrons.
c) the valency of an element whose electronic configuration is 2, 8, 3.
d) the shell closest to the nucleus of an atom.
e) An element having valency zero.
25)
State the number of neutrons in each of the atoms A to E. Also state which of the atoms A to E is a metal.
26) Match the elements A to E in list 1 with their valencies in list 2 and with their nature in list 3.
List : 1
A) Atomic number 7, mass number 14
B) Electronic configuration 2,8.
C) neutrons 14, electrons 13
D) neutrons 22, protons 18.
E) electronic configuration 2,8,1
List: 2
1) -3
2) +1
3) +3
4) +2
5) 0
List: 3
X: metal
Y: nonmetal
Z: noble gas
RESPIRATION IN PLANTS
A) Fill in the blanks with missing words:
1) The reaction of sugars with oxygen is called _____
2) Plants exchange gases with the ____passively.
3) Barks of woody stems of plants have___ for gaseous exchange.
4) Stomata are the opening present on the surface of ____ for gaseous exchange.
5) Roots have thin_____ which help the plant in oxygen intake.
6) The energy is released in the body by the____ of food .
7) _____produced in anaerobic respiration is used in the brewing industry.
8) The energy produced in____ respiration is less than the energy produced in____ respiration.
9) _____ is always produced in respiration, whether aerobic or anaerobic.
10) _____ is added to the moist dough of the flour to make bread and cake.
11) _____rrespiration takes place in the absence of oxygen.
12) The roots takes up_____present in the speces between the____ particles.
13) _____and ____ are essential processes in plants which are complementary to each other.
14) Respiration is an____ process, while photosynthesis is an___ process.
15) Oxidation of food releases energy in the form of____ energy.
16) Leaves of the plants have _____for gaseous exchange.
B) Choose the correct option:
1) End products of anaerobic respiration are
a) ethyl alcohol and carbon dioxide
b) ethyl alcohol and water
c) carbon dioxide and water
d) water and energy
2) After heavier exercise, human muscles cramp because of the accumulation of
a) alcohol b) carbon dioxide c) lactic acid d) uric acid
3) Lenticels are the special structures of gaseous exchange in
a) succulent stems b) soft stems c) green stems d) woody stems
4) choose the correct statement.
a) respiration in plants occurs day and night irrespective of photosynthesis.
b) respiration plants occurs only in night when plants do not for photosynthesis .
c) Rrespiration in plants occurs only during day time as plants use carbon dioxide released by photosynthesis .
d) plants do not need to respire as they use oxygen released during photosynthesis.
5) lactic acid produce during
a) photosynthesis
b) aerobic respiration
c) anaerobic respiration
d) fermentation
C) State whether the following statements are true or false:
1) Respiration in plants can take place only in nights in the absence of photosynthesis.
2) Leaves of plants respire with the help of the Lenticels.
3) Each part of the plant can respire indivisually.
4) Yest respire aerobically as well as anaerobically depending on the conditions.
5) Roots of Water-logged plants respire anaerobically .
D) Identify the figure given below and answer the following questions.
a) What does the above figure show ?
b) Name the pores present in the above figure.
c) Write the function of these pores.
d) Name the similar pores present in the leaves
___________&&&&______&&&&&&__&___
1) The cells of a tissue are similar in structure but different and function.
2) Apical meristem is responsible for the elongation of the stem.
3) Meristem tissues can be called as growth tissues .
4) The meristematic cells are thick-walled.
5) The shoot apex contains lateral meristem.
6) Xylem and phloem are supporting tissues.
7) Phloem is made up of mainly dead cells.
8) Xylem helps to transport water in upward direction.
9) Phloem is present outside the xylem tissue.
10) Xylem and phloem consist of living cells.
11) Permanent tissue have definite form in size.
12) Meristematic tissue are also called growth tissues .
13) Intercalary meristem increases the diameter of the plant parts.
14) Parenchyma serves as the packing material in the body of an organism.
15) Sclerenchyma tissue is composed of live cells without any spaces in between.
16) Phloem is a living tissue while xylem is a dead tissue.
B) Name the simple permanent tissue which
a) is composed of thin-walled cells .
b) comprises dead cells
c) has cells with large spaces in between.
d) is made up of cells whose cell wall is thickened at corners.
e) is present in the hard coverings of nuts.
C) Choose the correct option.
1) The thin-walled living cells found in the soft parts of a plant are
a) parenchyma b) collenchyma c) xylem d) phloem
2) The plant tissue that helps in transportation of water is
a) xylem b) phloem c) sclerenchyma d) parenchyma
3) In potato, starch is stored in the
a) phloem b) parenchyma c) sclerenchyma d) chlorenchyma
4) Lignin is present in the cell walls of
a) sclerenchyma b) parenchyma c) chlorenchyma d) collenchyma
5) The cells of sclerenchyma are
a) living and thin-walled
b) living and thick-walled
c) dead and thin-walled
d) dead and thick-walled
D) Fill in the blanks with missing words.
1) Potato tubers store starch in_____ cells.
2) ____acts as cement and makes sclerenchyma hard.
3) Parenchyma containing chloroplasts is known as____
4) ____ tissue is responsible for the elongation of the stem .
5) The increase in the diameter the root occurs by the division of___ tissue.
E) Match the following:
Column A
1) Lignin deposit
2) Manufacture of food
3) Transportation of food
4) Base of leaves
5) Thickened corners
Column B
a) Collenchyma
b) intercalary meristem
c) Sclerenchyma
d) Chlorenchyma
e) Phloem
F) Pick the odd one out :
1) Meristem , parenchyma, apical, intercalary
2) Xylem, vascular, food, phloem.
3) Sclerenchyma , lignin, coconut, parenchyma.
4) Flexible , tissue, thickened corners , leaf stalk, thin-walled
G) Name the type of the tissue found:
1) At the top of the plant roots.
2) At the base of the leaves.
3) On the outer side of vascular bundle.
4) In the inner side of The vuscular bundle.
5) In the leaf stalks.
6) In the hard covering of seeds.
H) Identify the following tissue:
1) plyant tissue consisting of cells with thickened corners.
2) Permanent plant issue with intercellular spaces.
3) Plant tissue that has lost its stability to divide.
4) Simple permanent plant tissue consisting of cells with thick cell walls.
5) Tissue responsible for the transportation of water in plants.
I) Observe the figure carefully and answer the questions given below :
a) identify the tissue.
b) Write any two features by which you identified this tissue.
c) Where will you find this tissue ?
d) Give any two functions of this tissue.
e) Name two more tissues which have similar structure and function.
ANIMAL TISSUE
A) State whether the following statement are true or false:
1) Epithelial cells rest upon a thin basement membrane.
2) Animal tissues are less diverse than plant tissues.
3) Epithelium protects the organs from the mechanical injury.
4) Epithelial cells are exclusively protective tissues .
5) Epithelial cells lack intercellular speces.
6) Tendons and Ligaments connect two bones and provide movement.
7) Blood plasma is straw-coloured fluid.
8) External ear is made up of flexible cartilage.
9) Ligaments allows the tissues to resist mechanical stress.
10) Haemoglobin provides red colour to the blood.
11) Lymph is straw-coloured because of the presence of WBC s.
12) The muscles of limbs are striped in work at our will.
13) Cardiac muscles work continuously.
14) The axons bundle together to form a muscle.
15) Nerves receive the message through dendrons .
16) Smooth muscles are cylinderical and elongated.
17) Blood and lymph constitute the fibrous connective tissue.
18) Cardiac muscles and skeletal muscles have striated apreence.
19) Voluntary muscles are found in the internal organs of the body.
20) The dendrons of nerves transmits messages to the other nerves.
21) Adipose tissue protects us from external socks.
22) Lymph is straw-coloured and lacks WBCs
B) Choose the correct option :
1) Which of the following is not a connective tissue ?
a) Adipose tissue b) blood c) cartilage d) Nerves
2) Tendons is a tissue that connects
a) a bond to another bone.
b) a nerve to a muscle
c) a muscle to a bone
d) a muscles to another muscle.
3) Cardiac muscles are
a) branched and voluntary
b) branched and involuntary
c) unbranched and voluntary
d) unbranched and involuntary
4) The cells responsible for blood clotting are
a) erythrocytes
b) leukocytes
c) chondrocytes
d) thrombocytes
5) Which of the following is not a connective tissue
a) bone b) blood c) cartilage d) epithelium
C) Fill in the blanks with missing words:
1) Cartilage consists of____ cells while the cells of bones are called____.
2) ____ muscles help in the moment of the food in food pipe.
3) _____ blood cells protect the body against pathogens.
4) The nervous tissue helps in the ____and____ of body.
5) ____ muscles never take rest.
6) The adipose tissue is responsible for the storage of ______.
D) Match the following
Column A
1) spindle-shaped
2) Sendrites
3) Haemoglobin
4) Blood clotting
5) Striated muscles
6) Heart
Column B
a) Erythrocytes
b) Platelets
c) Skeletal muscles
d) Neuron
e) Cardiac muscles
f) Smooth muscles
E) Pick out odd one out
1) Bone, blood, tendon, nerve.
2) Involuntary, cardiac, skeletal, smooth.
3) Cardiac, axon, smooth, skeletal.
4) Areolar , ligament, adipose, cartilage
F) Name the type of tissue found in
1) brain and spinal cord.
2) between two bones.
3) On the surface of human skin.
4) between muscles in bones.
5) hands and legs.
6) the wall of the heart.
G) Identify the following tissue :
1) Muscular tissue that works at our will.
2) Straw-coloured fluid connective tissue lacking RBCs.
3) Muscles that does not get tired.
4) Muscles that helps to pick up objects .
5) Skeletal connective tissue composed of chondrocytes.
6) Fluid connective tissue on containing RBCs.
H) Observe the figure carefully and answer the questions given below.
a) Identify the muscular tissue.
b) Write any two features by which you identified the tissue.
c) Where will you find this tissue in your body.
d) Are these muscles voluntary or involuntary ?
e) Name the other two kinds of muscles present in our body. Write two features and at least one function of each kind of muscle
CHEMISTRY TERMINOLOGY - CHEMICAL REACTIONS
THE LANGUAGE OF CHEMISTRY
1) A symbol represents a short form of an element.
a) In most cases the first letter of an element was taken as the symbol for that element. Give two examples of the same.
b) In certain cases in the first letter along with the its small letter from its name were used as the symbols. Give two examples of the same.
c) In some cases the symbols were derived from their Latin names. Name two metals . Whose symbols are derived from the same.
d) Sulphur is represented by the symbol 'S'. State how the symbol represents the elements i) qualitatively [i.e., representation in terms of an atom] ii) quantitatively, [i.e., representation in terms of weight].
2) Give reasons for the following:
a) In hydrogen chloride the valency of the element chlorine is considered as one.
b) Certain metals exhibit more than one valency and showing 'variable valency '.
c) All equations must be balanced.
d) A chemical equation provides useful information about a reaction.
e) All chemical equations have their limitations.
3) State the valency and name the ion or radical in each of the following cases given below (The first example is completed for you):
Electrical ent positive ions or radicals
Symbol/Valency Name
a) K¹⁺ Potassium
b) Na
c) H
d) NH₄
e) Ca
f) Mg
g) Zn
h) Ba
i) Ni
i) Co
j) Al
k) Cr
Variable valencies
a) Cu¹⁺
b) Cu
c) Hg¹⁺
d) Hg
e) Fe²⁺
f) Fe
g) Mn²⁺
h) Mn
i) Pb²⁺
j) Pb
k) Pt²⁺
l) Pt
Electrovalent negative ion or radicals
Symbol/valency Name
a) Cl¹⁻ Chloride
b) ClO₃
c) ClO
d) Br
e) I
f) OH
g) NO₂
h) NO₃
i) HCO₃
j) HSO₃
k) HSO₄
l) AlO₂
m) MnO₄
n) SO₃
o) SO₄
p) S
q) CO₃
r) O
s) CrO₄
t) Cr₂O₇
u) ZnO₂
v) PbO₂
w) PO₄
x) N
y) C
4) State the valency of each of the elements in the respective compounds:
a) Sulphur in (i) sulphur dioxide
ii) sulphur trioxide
b) Nitrogen in i) Nitrogen monoxide
ii) Nitrogen dioxide
iii) dinitrogen oxide
iv) dinitrogen pentoxide
c) Copper in i) cupric oxide
ii) Cuprous oxide
5) Give the formulas of the following compounds whose metallic radical exhibits variable valency.
a) Cupric nitrate.
b) Cuprous chloride.
c) Iron(II) sulphate.
d) Mercuric nitrate.
e) Plumbous chloride.
f) Stannous chloride.
g) Mangannic sulphate.
h) Platinic chloride.
i) Mercurous chloride.
j) Iron [II] nitrate.
6) Give the name of the compounds whose formulas are listed below:
a) HNO₂ ___
b) HCO₃ |
c) H₂C₂O₄. |
d) H₃PO₄ | --- Acids
e) CH₃COOH _ |
g) Al(OH)₃
h) CaSiO₃.
i) Na₂ZnO₂.
j) K₂CrO₄.
k) Mg₃N₂.
7) A chemical equation is a shorthand form for a chemical change
a) 2KClO₃ ---∆--> 2KCl + 3O₂.
i) In the above reaction name the reactant and the products.
ii) State what the arrow in between indicates.
8) Balance the following equations.
a) CuO+ NH₃ --> Cu + H₂O + N₂.
b) NH₃ + Cl₂ --> HCl + NCl₃.
c) Mg₃N₂ + H₂O --> Mg(OH)₂ + NH₃.
d) Pb₃O₄ + HCl --> PbCl₂ + H₂O + Cl₂.
e) Manganese [IV] + Hydrochloric acid --> Manganese (II) Chloride+ Water + Chlorine.
f) Potassium hydroxide + Chlorine --> Potassium chloride + Potassium hypochlorite + Water.
g) Ammonium dichromate --> Chromiumoxide + Water+ Nitrogen.
h) Potassium sulphite + Nitric acid --> Potassium nitrate+ Water+ Sulphur dioxide.
i) Iron [II] chloride + Water + Sulphur dioxide --> Iron [II] Chloride+ Sulphuric acid+ Hydrochloric acid.
j) Copper+ Sulphuric acid --> Copper sulphate + Water+ Sulphur dioxide.
k) Iron [III] oxide + Carbon monoxide --> Iron + Carbon dioxide.
l) Sodium sulphite+ Sulphuric acid --> Sodium sulphate+ Water+ Sulphur dioxide.
m) Zinc + Sodium hydroxide --> Sodium zincate --> Hydrogen.
n) Aluminium+ Carbon dioxide --> Aluminium oxide + Carbon.
o) Sodium bicarbonate+ Aluminium sulphate --> Sodium sulphate+ Aluminium hydroxide+ Carbon dioxide.
p) Calcium hydroxide+ Ammonium sulphate --> Calcium sulphate+ Water+ Ammonia.
q) Nitric acid+ Magnesium carbonate --> Magnesium nitrate+ Water+ Carbon dioxide.
r) Iron [III] oxide+ Sulphuric acid --> Iron [III] sulphate+ Water.
s) Zinc sulphide+ Oxygen --> Zinc oxide+ Sulphur dioxide.
t) Carbon+ Nitric acid --> Carbon dioxide+ Water+ Nitrogen dioxide.
7) Match the different types of chemical reactions in column II with the meaning of the type of reactions in column I.
COLUMN I
a) A chemical reaction in which two or more elements or compounds react to form one new compound as a product.
b) A chemical reaction in which a chemical compound decomposes or splits up into two or more simpler substances. It is generally brought about by heat.
c) A chemical reaction which takes place when an element [or radical] has replaced another element in a compound.
d) A chemical reaction in which two reactants are both the decomposed to form new substances by exchanging their radicals.
e) A chemical reaction which employes a catalyst to alter the rate of a reaction.
f) A chemical reaction in which the products formed react together to form the original reactants depending on the conditions of the reaction.
g) A reaction in which a substance dissociates into two or more simpler substances on application of heat and is a reversible reaction.
h) A reaction which involves addition of oxygen or electronegative element or removal of hydrogen or electropositive element.
i) A reaction which involves addition of hydrogen or electropositive elements or removal of oxygen or electronegative element.
j) A chemical reaction which proceeds with evolution of heat energy.
k) A chemical reaction which proceeds with absorption of heat energy.
l) A chemical reaction which proceeds with absorption of light energy.
COLUMN II
A) Double decomposition
B) Exothermic reaction
C) Reversible reaction
D) Displacement reaction
E) Combination or synthesis
F) Decomposition reaction
G) Thermal dissociation
H) Endothermic reaction
I) Catalytic reaction
J) Oxidation reaction
K) Photochemical reaction
L) Reduction reaction.
8) With reference to the reaction -- A to L in column II of the previous question no. 7 state the type of reaction/s to which each of the following belongs :
a) Addition of zinc to copper sulphate solution.
b) Heat on lead nitrate crystals.
c) Preparation of oxygen from potassium chlorate.
d) Conversion of ferrous chloride to ferric chloride using chlorine.
e) Formation of ammonia from nitrogen and hydrogen.
f) Liberation of hydrogen at the cathode acidified water.
g) Manufacture of glucose by green plants.
h) Formation of nitric oxide from Nitrogen and oxygen.
i) Addition of zinc to dilute sulphuric acid.
j) NH₄Cl <=> NH₃ + HCl.
k) 2KNO₃ --∆--> 2KNO₂ + O₂.
l) 2H₂O₂ --H₃PO₄--> 2H₂O + O₂.
m) PbBr₂ --> Pb²⁺ + 2Br¹⁻ [ions].
n) 2HgO --∆--> 2Hg + O₂.
o) N₂O₄ <=∆=> 2NO₂.
p) AgNO₃ + KCl --> AgCl + KNO₃.
q) Fe + S --> FeS.
r) H₂ + Cl₂ --> 2HCl.
ˢᵘⁿˡᶦᵍʰᵗ
s) C + H₂O --> CO.
t) Cl₂ + 2KI --> 2KCl + I₂.
u) 3Fe + 4H₂O <==∆=> Fe₃O₄ + 4H₂.
v) 2Cu + O₂ --> 2CuO.
w) Fe₂O₃ + 2Al --> Al₂O₃ + 2Fe.
x) KNO₃ + H₂SO₄ --> HNO₃ + KHSO₄.
y) 2FeCl₂ + Cl₂ --> 2FeCl₃.
z) Fe+ H₂SO₄ --> FeSO₄ + H₂.
a) SO₂ + Cl₂ --> SO₂Cl₂.
b) 3Ca + N₂ --> Ca₃N₂.
c) CuSO₄ + Fe --> FeSO₄ + Cu.
d) 4HNO₃ --> 2H₂O + 4NO₂ + O₂.
8) Oxidation and reduction reactions are generally termed as redox reactions . In the examples given below underline the oxidised product or reduced product in the respective reactions. Underline substance is the oxidising or reducing agent respectively.
Oxidation reactions
a) Cu + O₂ --> 2CuO.
b) H₂S + Cl₂ --> S + 2HCl.
c) 2FeCl₂ Cl₂ --> 2FeCl₃.
d) SO₂ + H₂O + Cl₂ --> H₂SO₄ + 2HCl.
e) H₂S + 2FeCl₃ ---> 2FeCl₂ + 2HCl + S.
f) Zn + H₂SO₄ --> ZnSO₄ + H₂.
g) Fe + S --> FeS.
h) 2Mg + SO₂ --> MgO + S.
i) 2H₂S + SO₂ --> 3S + 2H₂O.
j) S + 2H₂SO₄ ---> 3SO₂ + 2H₂O.
Reduction reactions
a) CuO + H₂ --> Cu + H₂O.
b) Br₂ + H₂S --> 2HBr + S.
c) 2FeCl₃ + H₂S --> 2FeCl₂ + 2HCl + S.
d) 2HgCl₂ + SnCl₂ --> Hg₂Cl₂ + SnCl₄.
e) 2FeCl₃ + SO₂ + 3H₂O --> 2FeCl₂ + 2HCl + H₂SO₄.
f) Fe₂(SO₄)₃ + 2H₂O + SO₂ --> 2FeSO₄ + 2H₂SO₄.
g) Cl₂ + 2H₂O + SO₂ --> 2HCl + H₂SO₄.
h) 2HNO₃ + SO₂ --> 2NO₂ + H₂SO₄.
i) 2KMnO₄ + 2H₂O + 5SO₂ --> 2MnSO₄ + K₂SO₄ + 2H₂SO₄.
j) K₂Cr₂O₇ + H₂SO₄ + 3SO₂ --> Cr₂(SO₄)₃+ K₂SO₄ + H₂O.
9) Name the following:
a) A coloured gaseous oxidising agent.
b) A liquid oxidising agent which on thermal decomposition in presence of a catalyst liberates oxygen.
c) A gaseous reducing agent containing Oxygen.
d) An acidic other than nitric and Sulphuric Acid which is an oxidizing agent.
e) A gaseous reducing agent neutral in nature other than carbon monoxide.
f) An oxidizing agent which liberates chlorine on heating with concentric hydrochloric acid.
g) Two neutral gases which react to give a basic gas and the reaction is exothermic.
h) Two neutral gases which react to give a neutral oxide and the reaction is exothermic.
i) A substance which decomposes by absorption of sound energy.
j) Two substances which react explosively on close physical contact.
