What are the major differences between metals and non-metals?
METALS |
NON METALS |
Metals can lose electrons easily. |
Non-metals cannot lose electrons easily |
Metals are solids at room ( Exceptions – Hg, Ga ). |
temperature Non – metals may be solids, liquids or gases at room temperature |
Metals generally form ionic compounds. |
Non–metals generally form covalent compounds. |
Metals have low ionization enthalpies. |
Non–metals have high ionization enthalpies. |
Metals are less electronegative. They are rather electropositive elements. |
Non–metals are electronegative. |
Metals have a high reducing power. |
Non–metals have a low reducing power |
Metals have luster. They reflect light from polished or freshly cut surface |
Non-metals do not have luster.( Exceptions – Diamond and Iodine ) |
Metals generally have high density |
Non-metals generally have low density |
They are good conductors of heat and and electricity.
|
They are usually bad conductors of heat electricity. (exception – carbon in the form of gas carbon and graphite ) |
Metals are malleable and ductile. They can be beaten into sheets and drawn into wires. |
Non-metals are not malleable and ductile They are brittle when solid.They can be crushed into powder |
They have a three dimensional crystal structure with metallic bonds |
They have different types of structures with covalent and van-der-Walls’ bonds |
Metals usually have high tensile Strength |
Non- metals usually have low tensile strength |
Metals generally have 1 to 3 electrons in outermost shell of their atoms |
Non-metals generally have 4 to 8 in their outermost shell of the atom |
They generally form basic oxides. |
They generally form acidic oxides |
They act as reducing agents |
They act as oxidizing agents. |
The mass of an electron is 9.1 × 10–31 kg. If its K.E. is 3.0 × 10–25 J, calculate its wavelength.
Calculate the amount of carbon dioxide that could be produced when
(i) 1 mole of carbon is burnt in air.
(ii) 1 mole of carbon is burnt in 16 g of dioxygen.
(iii) 2 moles of carbon are burnt in 16 g of dioxygen.
Calculate the wavelength of an electron moving with a velocity of 2.05 × 107 ms–1.
Balance the following redox reactions by ion – electron method :
(a) MnO4 – (aq) + I – (aq) → MnO2 (s) + I2(s) (in basic medium)
(b) MnO4 – (aq) + SO2 (g) → Mn2+ (aq) + HSO4– (aq) (in acidic solution)
(c) H2O2 (aq) + Fe 2+ (aq) → Fe3+ (aq) + H2O (l) (in acidic solution)
(d) Cr2O7 2– + SO2(g) → Cr3+ (aq) + SO42– (aq) (in acidic solution)
In a process, 701 J of heat is absorbed by a system and 394 J ofwork is done by the system. What is the change in internal energy for the process?
What will be the minimum pressure required to compress 500 dm3 of air at 1 bar to 200 dm3 at 30°C?
In a reaction A + B2 → AB2 Identify the limiting reagent, if any, in the following reaction mixtures.
(i) 300 atoms of A + 200 molecules of B
(ii) 2 mol A + 3 mol B
(iii) 100 atoms of A + 100 molecules of B
(iv) 5 mol A + 2.5 mol B
(v) 2.5 mol A + 5 mol B
At 0°C, the density of a certain oxide of a gas at 2 bar is same as that of dinitrogen at 5 bar. What is the molecular mass of the oxide?
Which one of the following will have largest number of atoms?
(i) 1 g Au (s)
(ii) 1 g Na (s)
(iii) 1 g Li (s)
(iv) 1 g of Cl2(g)
Density of a gas is found to be 5.46 g/dm3 at 27 °C at 2 bar pressure. What will be its density at STP?
Write the favourable factors for the formation of ionic bond.
The ionization constant of nitrous acid is 4.5 x 10-4. Calculate the pH of 0.04 M sodium nitrite solution and also its degree of hydrolysis.
Give one method for industrial preparation and one for laboratory preparation of CO and CO2 each.
What happens when
(i) sodium metal is dropped in water ?
(ii) sodium metal is heated in free supply of air ?
(iii) sodium peroxide dissolves in water ?
Suggest reasons why the B-F bond lengths in BF3 (130 pm) and BF-4(143 pm) differ.
A sample of HI(g) is placed in flask at a pressure of 0.2 atm. At equilibrium the partial pressure of HI(g) is 0.04 atm. What is Kp for the given equilibrium ?
2HI (g) ↔ H2 (g) + I2 (g)
A certain salt X, gives the following results.
(i) Its aqueous solution is alkaline to litmus.
(ii) It swells up to a glassy material Yon strong heating.
(iii) When conc. H2SO4 is added to a hot solution of X, white crystal of an acid Z separates out.
Write equations for all the above reactions and identify X, Y and Z.
Explain why the following systems are not aromatic?
Is there any change in the hybridisation of B and N atoms as a result of the following reaction?
BF3 + NH3 → F3B.NH3
Distinguish between a sigma and a pi bond.