Indicate the σ and π bonds in the following molecules :
(i) C6H6,
(ii) C6H12,
(iii) CH2Cl2,
(iv) CH2=C=CH2,
(v) CH3NO2,
(vi) HCONHCH3
(i) C6H6
There are six C-C sigma (σC-C) bonds, six C-H sigma (σC-H) bonds and three C=C pi (πC-C) resonating bonds in this compound.
(ii) C6H12
There are six C-C sigma (σC-C) bonds and twelve C-H sigma (σC-H) bonds in this compound.
(iii) CH2Cl2
There two C-H sigma (σC-H) bonds and two C-Cl sigma (σC-Cl) bonds in this compound.
(iv) CH2=C=CH2
There are two C-C sigma (σC-C) bonds, four C-H sigma (σC-H) bonds, and two C=C pi (πC-C) bonds in this compound.
(v) CH3NO2
There are three C-H sigma (σC-H) bonds, one C-N sigma (σC-N) bond, one N-O sigma (σN-O) bond and one N=O pi (πN-O) bond in this compound.
(vi) HCONHCH3
There are two C-N sigma (σC-N) bonds, four C-H sigma (σC-H) bonds, one N-H sigma bond, and one C=O pi (πC-O) bond in this compound.
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?
Calculate the entropy change in surroundings when 1.00 mol of H2O(l) is formed under standard conditions. ΔfH0 = –286 kJ mol–1.
Elements of group 14
(a) exhibit oxidation state of +4 only
(b) exhibit oxidation state of +2 and +4
(c) form M2-and M4+ion
(d) form M2+and M4+ions
How are 0.50 mol Na2CO3 and 0.50 M Na2CO3 different?
What do you mean by green chemistry? How will it help decrease environmental pollution?
Write bond line formulas for : Isopropyl alcohol, 2,3-Dimethyl butanal, Heptan-4- one.
In Rutherford’s experiment, generally the thin foil of heavy atoms, like gold, platinum etc. have been used to be bombarded by the α-particles. If the thin foil of light atoms like aluminium etc. is used, what difference would be observed from the above results?
Nitrogen laser produces a radiation at a wavelength of 337.1 nm. If the number of photons emitted is 5.6 × 1024, calculate the power of this laser.
Draw the structure of (i) BeCl2 (vapour) (ii) BeCl2 (solid).
Neon gas is generally used in the sign boards. If it emits strongly at 616 nm, calculate
(a) the frequency of emission,
(b) distance traveled by this radiation in 30 s
(c) energy of quantum and
(d) number of quanta present if it produces 2 J of energy.
An aqueous solution of borax is
(a) neutral (b) amphoteric (c) basic (d) acidic
VERY HELPFUL!!!!