Ionisation Energy

Q.

If the radius of a metal atom (A) is 5 pm and the radius of an electronegative atom (B) is 20 pm, then in the unit cell

(1) A in octahedral voids, B in FCC unit

(2) A in FCC unit, B in the tetrahedral void

(3) A in BCC unit, B in the cubic void

(4) A in the tetrahedral void, B in FCC unit

Q.

The anomalous behaviour of first element of s and p block elements of each group as compared to other group members is due to following reasons:

1. Small size of atom

2. Large charge/radius ratio

3. High electronegativity and non availability of d-orbitals in their valence shell

4. All of the these

Q.

20 L of H₂ gas at S.T.P weigh about:

1. 20 g

2. 448 g

3. 12.2 g

4. 1.8 g

Q. 6.5 g of an impure sample of limestone liberates2.2 g of CO2 on strong heating. The percentagepurity of CaCO3 in the sample is(1) 85.2%(2) 76.9%(3 72.5%(4)925%

Q. In which of the following molecules/ions all bonds are not equal? a.sf4 b.sif4 c.xef4 d.bf4-

Q. 39 Which of the following is true for nitrate anion (1) formal charge on N is 0 (2) bond order of NO bond is 4/3 (3) average formal charge on oxygen is -1/3 (4) there are 2 pi bonds in the ion Which one is correct option Also explain ?

Q. A sample of oxygen gas at STP occupies 2.8 L. The number of oxygen atoms in the sample is

Q.

If the number of atomic orbitals undergoing hybridisation is 4, number of hybrid orbitals formed is:

1. 4

2. 8

3. 6

4. 2

Q. In a hypothetical atom, the number of electrons inshell and subshell are x and y, respectively, whereeach electron has three possible spin states repre-sented as s +1/2, -1/2 and 0.Then the value of x + y is(A) 2n^2+ 4l+2(B) 3n^2+ 3l + 1(C) 3n^2 + 6l +3(D) 6n^{} +3l +3

Q. The electronegativity of H and Cl are 2.1 and 3.0 respectively .The nature of HCl is

Q. Radius of second orbit of an element is 0.070nm. The energy asspciated with this ( in J) will

Q. 100 mL of 0.1N hypo decolourised iodine by the addition of x g of crystalline copper sulphate to excess of KI. The value of x is(mol. weight of CuSO4.5H2O is 250)-1)5.0g, 2)1.25g, 3)2.5g, 4)4g.

Q. 29.Why are the melting and boiling points of group 14 elements higher than the corresponding group 13 elements?

Q. 41.The volumes of ozone and chlorine diffusing during the same time are 35mL and 29ml respectively. If the molecular weight of chlorine is 71, Calculate the molecular weight of ozone.

Q. 0.) If radius of a metal atom (A) is 5 pm and radius ofan electronegative atom (B) is 20 pm, then in theunit cell(1) A in octahedral voids, B in FCC unit(2) A in FCC unit, B in tetrahedral void(3) A in BCC unit, B in cubic void(4) A in tetrahedral void, B in FCC unit

Q. 42. Effective number of atom(s) present on the faces广of FCC unit cell of a metallic crystal is ( 2 or 4 or 1 or

Q. Draw Lewis dot structures of SO3 molecule and (SO3)2- ion and mention Co-ordinate bonds wherever required.

Q.

Which of the following is largest

1. Cl^-

2. S^2-

3. Na⁺

4. F^-

Q. How many moles of magnesium phosphate will contain 0.25 mole of oxygen atom

Q. 10. The equivalent weight of a metal is 100. If the specific heat of metal is 0.09 J/g calculate the exact atomic weight of the metal

Q. Which of the following is the correct reason for the anomalous behaviour of Boron?

1. Smallest size in the group
2. Low Ionisation Energy
3. None of these
4. Low Electronegativity

Q. 1. Why do the melting points of Group 15 of the Modern Periodic Table increase from Nitrogen to Arsenic, but decrease Arsenic onwards?

Q. Which of the following species has lowest ionisation enthalpy?

1. $O$
2. $O^{+}$
3. $O^{-}$
4. $O^{2-}$

Q. Which of the following isoelectronic ions have lowest ionization?

1. $F^{-}$
2. $N{a}^{+}$
3. $O^{2-}$
4. $M{g}^{2+}$

Q. 41. If average molecular mass of air is 29 , than assuming that n2 and o2 are there , calculate mile percent of n2 mass percent of n2

Q. 37.Explain about covalent or molecular hydrides

Q.

Among the following elements element with highest ionisation enthalpy is:

1. B

2. O

3. N

4. C

Q. In the transformation, $Na\left(s\right)\to N{a}^{+}\left(g\right)$, the energies involved are:

1. Ionization energy and sublimation energy
2. Bond dissociation energy
3. Sublimation energy
4. Ionization energy

Q. why does thermal stability of oxides, hydroxides etc of 2nd group elements increases down the group ?? and shouldnt it decrease down the group as the size of atom is increasing ??

Q. The decreasing order of the first ionization energy of group 16 elements is:

1. $O>S>Se<Te>Po$
2. $O>S>Se>Te>Po$
3. $O<S<Se<Te<Po$
4. None of the above