11 chem liquid and solids

1. Isotopes differ in:

• Properties with respect to their mass number
• Properties with respect to their proton number
• Isotopes don’t differ as they have same number of electrons and protons
• All of the above

2. Isotopes are:

• Chemically similar
• Physically dissimilar
• Chemically dissimilar
• Both a and b

3. Ionization energy depends upon:

• Atomic/ionic radii
• Proton to electron ratio
• Shielding effect
• All of the above

4. 2nd ionization energy of Mg is higher than the first because:

• Metallic character of Mg+1 is less than that of Mg
• Nuclear pull for Mg+1electron is more than that for the Mg atom
• Size of Mg+1 is greater than Mg+2
• Both a and b

5. With the increasing atomic number, ionization energy increases along a period because:

• No change in shielding effect along a period
• Nuclear pull increases with the increase in the number of protons
• Atomic/ionic size decreases along a period
• All of the above

6. The correct set of four quantum numbers for the valence electron of rubidium (Z = 37) is:

• n = 5, 1 = 0, m = 0 and s = +1/2
• n = 5, 1 = 1, m = 1 and s = +1/2
• n = 5, 1 = 1, m = 0 and s = +1/2
• n = 6, 1 = 0, m = 0 and s = +1/2

7. The electron configuration of K(19) is:

• 1s3 2s3 2p5 3s3 3p5
• 1s2 2s2 2p6 3s2 2p5 4s2
• 1s2 2s2 2p6 3s2 3p6 4s1
• None of the above

8. The number of d-electrons in Fe+2 (Z=26) is not equal to:

• p electrons in Ne (Z = 10)
• d electrons in Fe (Z = 26)
• s electrons in Mg (Z = 12)
• p electrons in Ar (Z = 17)

9. The electronic configuration of an element is 1s2 2s2 2p3. This represents a/an:

• Ground state
• Hybridized state
• Excited-state
• Molecular state

10. In which of the following, all have the same number of electrons:

• Cl–, Br– and I–
• H–, H and H+
• F–, Ne and Na+
• Li+, Na+ and K+