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ICSE Revision 2016 : Chemistry (Good Earth School, Kanchipuram)

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Anirudh Giri
Good Earth School, Kanchipuram

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Good Earth School Naduveerapattu Date: Class: X Chemistry Revision I. Fill in the blanks: (1) The modern Periodic Table has ______________ periods. (2) Each ______________ in the Periodic Table is comprised of elements having the same number of electron shells. (3) Elements in a period, all have the same number of ______________ in their atoms. (4) Elements in a group, all have the same number of ______________. (5) The most active metals are located in ______________ 1 and 2 of the Periodic Table. (6) The most reactive non-metals comprise group ______________ of the Periodic Table. (7) The elements of ______________ are known as transition elements. (8) The elements occupying left and right side groups of Periodic Table are called ______________ elements. (9) The rare gases are placed in ______________ group at the end. (10) Elements from atomic number 57 to ______________ occupy same place in Periodic Table. These elements are called ______________. (11) The properties of elements are periodic function of their ______________. (12) The atomic size ______________ as we move left to right across the period, because the ______________ increases but the ______________ remains the same. (13) The metallic character ______________ in a group as one moves from top to bottom. (14) The metallic character ______________ in a group as one moves from right to left. (15) In a period or in a group, the larger the atomic size of an element, the ______________ metallic is the element. (16) Moving across a ______________ of the periodic table, the elements show increasing ______________ character. (17) The amount of energy involved in the reaction X + energy X+ + C is known as the ______________ of the element X. (18) Across a period, the ionization potential ______________. (19) Down the group, electron affinity ______________. (20) The higher the electron affinity of a non-metal, ______________ the chemically reactive the non-metal is. (21) The tendency to gain an electron ______________ on moving down a group and ______________ on moving across a period in the Periodic Table. (22) Elements having high ionization potential have ______________ electron affinities. (23) The electronegativity of elements ______________ across a period and ______________ down a group. (24) In general, non-metals are ______________ electronegative than metals. (25) On moving from left to right in a given period, the number of shells ______________. (26) Elements X belongs to group 2 and period 3 of the Periodic Table. It has ______________ electrons in the outer most shell. (27) Each period except period 1 in the Periodic Table begins with ______________ and ends up with a ______________. (28) The metallic and non-metallic character depends upon the ______________ and ______________ of the elements. (29) Ionic compounds consist of ______________ charged ions. (30) Ionic compounds have ______________ melting points due to ______________ ionic bonds. (31) (32) (33) (34) (35) (36) (37) (38) (39) (40) (41) (42) (43) (44) (45) (46) (47) (48) (49) (50) (51) (52) (53) (54) (55) (56) The physical state of ionic compounds is ______________. Ionic compound conduct electricity in their ______________. The nature of bond in compounds of alkali and alkaline earth metals is ______________. ______________ compounds have low boiling points because of ______________ intermolecular forces. In covalent compounds, the bond is formed due to the ______________ of electrons. Melting and boiling points of covalent compounds are generally ______________. Covalent bond is rigid and directional, it is responsible for ______________. Most covalent compounds have density ______________ than that of water. The electronegativities of atoms giving covalent molecules are generally _____________. Atoms of the same element combine to form molecules by means of ___________ bonds. A solution of a __________ electrolyte will contain both ions and molecules of the solute. In the sodium chloride crystal, each Na+ ion is surrounded by ______________ Cl ions and each Cl ion by ______________ Na+ ions. In sodium chloride, the Na+ ion has the ______________ configuration and the Cl ion has the ______________ configuration. A compound conducted electricity in the fused state. The compound is made-up of ______________. The duplet or octet structure of valence shell makes ______________ of an element chemically ______________. The atomic number of oxygen is 8. The total number of electrons in the O2 ion is ______________. The atomic number of oxygen is 8. The number of protons in the O2 ion is ___________. Two nitrogen atoms join together by sharing ___________ pairs of electrons. In all the four bonds are ___________. The water molecules easily break the ___________ bonds between the oppositly charged ions. The ions drift in water in all possible directions and hence electrovalent compounds ___________ in water. A molecule of ___________ contains a triple bond. ___________ are identical to a normal covalent compound. Salts of strong acids and strong bases in water produce ___________ solution of sodium carbonate in water is ___________ in nature, while the solution of ferric chloride is ___________ in nature. A solution X turns blue litmus red, soit must contain: (a) _________ ions. Another solution Y turns red litmus blue and therefore, must contain. (b) ___________ ions. When solutions X and Y are mixed together, the products will be a ___________ and (c) ___________ if a piece of magnesium was put into solution X. ___________ gas would be evolved. In making copper sulphate crystals, a black powder called ___________ is added to dilute ___________ acid and the mixture is warmed. Excess black powder is added to a small volume of acid so as to ___________. The excess insoluble black powder is got rid by ___________. The resulting clear solution looks ___________ in colour. This solution is heated to get rid of some of the ___________. Slow cooling of the remaining solution ___________ of pure copper sulphate. Deliquescence takes place because of the difference in ___________ of atmospheric ___________ and that of the deliquescent substance. The vapour pressure of atmospheric humidity is ___________ than that of the deliquescent substance. The substances which take up water on exposure to atmosphere, without forming a solution are known as ___________ substances. (57) An acid is a compound which when dissolved in water gives ___________ ions as the only ___________ ions. (58) A ___________ acid undergoes almost complete dissociation on dissolving in water. (59) An example of mineral acid is ___________. (60) Vinegar contains ______________________ acid. (61) Sodium acetate on hydrolysis forms sodium hydroxide and ___________. (62) The basicity of Acetic Acid is ______________________. (63) Metal A reacts with cold water forming hydrogen and new compound B. The anion combined with A in a substance B is named ___________. (64) The solution of sodium carbonate is alkaline due to ___________. (65) The pH value of a neutral solution is ______________________. (66) As the pH of solution decreases, its acidic strength progressively ___________. (67) As the pH of solution increases, the ___________ strength of the solution progressively decreases. (68) pH value of lemon juice is ___________ than 7. (69) Ammonium hydroxide is a ___________ base. (70) Methyl orange turns ___________ in acidic solution. (71) The formation of a salt from an acid and a base involves the combination of ___________ from the acid and the ___________ from the ___________ to form ___________ molecules. (72) A salt which absorbs moisture from the air, but does not change in physical state in called ___________ salt. (73) Ammonium chloride is a ___________ salt. (74) Sodium hydrogen sulphate is ___________ salt. (75) The salt of the acid HNO2 are called ___________ and those of the acid HNO3 are called ___________. (76) Sodium sulphite reacts with dilute sulphuric acid to form sodium sulphate ___________ gas and water. (77) Copper (II) chloride reacts with sodium hydroxide to form ___________ copper hydroxide and sodium chloride. (78) A chemical reaction between hydronium ions of an acid and OH ions of a base to form unionized water is called ___________. (79) Dissolving of aluminium foit in HCl as well as NaOH shows that it is ___________ in nature. (80) An example of a deliquescent salt is ___________. (81) Superphosphate is an example of a compound called ___________. (82) The number of H+ ions of an acid which react completely with one molecule of a base is called its ___________. II. Reasoning based questions: (1) Explain why the elements placed in the same group of the Periodic Table have the same chemical properties. (2) Why group IA elements are called Alkali metals? (3) Why sodium is a metal while sulphur is a non-metal? (4) Alkali metals are good reducing agents. (5) Why are the elements sodium and chlorine in the same period of the Periodic Table? (6) Sodium atom, Na forms the positive ion Na+, but chlorine atom Cl, does not form the positive Cl+ ion. (7) Potassium atom is larger than sodium atom. Why? (8) Magnesium atom is smaller than calcium atom. Why? (9) Magnesium atom is smaller than sodium atom. Why? (10) Which is larger Na+ or K+? Why? (11) Mg2+ ions is smaller than O2 ion although both are iso-electronic. Explain. (12) Why the atomic size decreases in a period as we move from left to right? (13) The reducing power of elements increases as one goes down a group. (14) The reducing power of elements decreases as on one move from left to right in a period. (15) Why the oxidizing power of elements increases on moving from left to right along a period in the periodic table? (16) Why ionization potential of the element increases across a period? (17) Why the second ionization energy of an element is greater than its first ionization energy? (18) Why is ionization energy of O less than that of N? (19) Noble gases have zero electron affinity values. (20) Why elements with low ionization potential exhibit metallic properties? (21) Why atoms combine with one another? (22) Why do certain elements from ions? (23) Why are all atoms other than noble gas atoms, reactive? (24) Why a molecule of hydrogen is more stable than the uncombined atoms? (25) Why is hydrogen ion called proton? (26) A cation is smaller than the atom from which it is formed. Why? (27) An anion carries negative charge. Why? (28) Why electrovalent compounds form hard crystals? (29) Why electrovalent compounds have high melting, boiling points and low volatility? (30) Why electrovalent compounds in crystalline state do not conduct electricity? (31) Why do electrovalent compounds usually dissolve in water and molecular compounds dissolve in organic solvents? (32) Why ionic compounds are generally soluble in water, but insoluble in organic solvents? (33) Why molten NaCl conduct electricity but, CCl4 does not? (34) Why is sodium ion (Na+) not reactive, but sodium metal is very reactive? (35) Why covalent compounds are generally liquids or gases? (36) Why all covalent compounds are bad conductor of electricity? (37) Why covalent compounds have low melting point and boiling point? (38) Why most of the covalent compounds have density less than that of water? (39) Why do covalent compounds exist as gases, liquids or soft solids? (40) Why hydrogen chloride can be termed as a polar covalent compound? (41) Why is methane molecule regarded as a non-polar covalent compound? (42) Why the melting and boiling points of co-ordinate compounds are higher than covalent compounds and lower than ionic compounds?

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