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Solution: In case of diamond, each carbon atom of a single crystal is surrounded by four other carbon atoms by covalent bonds such that they form four corners of a regular tetrahedron. Because of four covalent bonds with each carbon atoms there are no free electrons available.
Due to the non-availability of free electrons within crystalline structure, diamond acts as a bad conductor of electricity. In case of graphite, every carbon atom in a single crystal is covalently bonded to three carbon atoms.
As each carbon atoms has four valence electrons one valence electron is left free for each carbon atom. These free electrons can be easily made to flow within the crystalline structure of graphite by applying electric potential.
Thus, graphite is a good conductor of electricity. Question-3 Write three important uses of ethanol. Solution: Ethanol is used as a solvent to dissolve varnishes, medicines and other organic compounds It is used as beverage for drinking as an intoxicant in different forms, viz; Brandy, Whisky etc.
Question-4 State what you will observe when sugar crystals is heated strongly. State what you will observe when sugar crystals is treated with conc. Sulphuric acid. Solution: The sugar crystal will initially melt. Gradually, they turn brown and start swelling up. They give off large amount of steam. Finally black porous residue of Ch 8 Maths Class 10 Extra Questions Youtube carbon is left behind.
The sugar crystals will initially turn brown. Lot of frothing takes place with the evolution of large amount of heat and steam is given off. Finally a black porous residue of carbon is left behind.
Question-5 How are the molecules of aldehyde and Ketone structurally different? Solution: In aldehyde, the carbon atom of the carbonyl group is attached to one alkyl group R and one hydrogen atom but in ketone, the carbonyl group is attached to two alkyl groups. Question-6 What change has been Ch 7 Maths Class 10 Extra Questions Vba made in the composition of detergents to make them biodegradable? Solution: Detergents made from long chain hydrocarbons having the minimum branching in their molecules are degraded more easily.
Calculate the mass of one atom of hydrogen atom. How many moles are present in 4 g of sodium hydroxide? A sample of ammonia weighs 3. What mass of sulphur trioxide contains the same number of molecules as are in 3.
Answer: Number of moles of ammonia in 3. Carbon dioxide produced by action of dilute hydrochloric acid on potassium hydrogen carbonate is moist whereas that produced by heating potassium hydrogen carbonate is dry. What would be the difference in the composition of carbon dioxide in the two cases? State the associated law. Answer: The composition of CO 2 in both the cases would be same, i.
The law associated is law of constant proportion. How many atoms would be present in a black dot marked on the paper with graphite pencil as a full stop at the end of a sentence. Does the solubility of a substance change with temperature? Explain with the help of an example. The solubility generally, increases with increase in temperature. For example, you can dissolve more sugar in hot water than in cold water.
Calculate the mass percentage of oxygen present in the following compounds and state the law of chemical combination associated. Classify each of the following on the basis of their atomicity. What are ionic and molecular compounds? Give examples. For example, water, ammonia, carbon dioxide. Compounds composed of metals and non-metals contain charged species.
The charged species are known as ions. An ion is a charged particle and can be negatively or positively charged. A negatively charged ion is called an anion and the positively charged ion is called cation. For example, sodium chloride, calcium oxide. How many a molecules b hydrogen atoms c oxygen atoms are there in 0. Answer: a 1 mol of water contains 6. Calculate the number of moles present in: i 3. Calculate the mass per cent of each element of sodium chloride in one mole of it.
Calculate the number of particles in each of the following: a 46 g of Na atom b 8 g of O 2 molecules c 0. Raunak took 5 moles of carbon atoms in a container and Krish also took 5 moles of sodium atoms in another container of same weight.
Arrange the following in order of decreasing masses: i 10 23 molecules of CO 2 gas ii 0. Calculate the mass per cent of each element present in the molecule of calcium carbonate. Verify by calculating that a 5 moles of CO 2 and 5 moles of H20 do not have the same mass. Calcium chloride when dissolved in water dissociates into its ions according to the following equation. What is a mole? What is the unit of mole? How many molecules are there in a certain mass of a substance? Answer: A mole is the amount of a substance which contains the same number of chemical units atoms, molecules or ions as there are atoms in exactly 12 g of carbon We know that Avogadro number is 6.
The difference in the mass of moles each of sodium atoms and sodium ions is 5. Compute the mass of an electron. For moles each of sodium atoms and ions there would be a difference of moles of electrons. The mass of one steel screw is 4.
Find the mass of one mole of these steel screws. Compare this value with the mass of the Earth 5. Which one of the two is heavier and by how many times? The Earth is times heavier than one mole of screws. Compute the number of ions present in 5. Each NaCl particle is equivalent to 2 ions, i. How many atoms of gold are present in one gram of this sample of gold? Compute the difference in masses of one mole each of aluminium atoms and one mole of its ions.
Mass of an electron is 9. Which one is heavier? An aluminium atom needs to lose three electrons to become an ion. Compute the ratio of the number of atoms of gold and silver in the ornament. A sample of ethane C 2 H 6 gas has the same mass as 1. How many C 2 H 6 molecules does the sample of gas contain? In photosynthesis, 6 molecules of carbon dioxide combine with an equal number of water molecules through a complex series of reactions to give a molecule of glucose having a molecular formula C 6 H 12 O 6.
How many grams of water would be required to produce 18 g of glucose?
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