The position of elements with an outer electronic configuration as
1. 6th period and 10th group.
2. 7th period and 3rd group.
3. 6th period and 3rd group.
4. 7th period and 9th group.
1st (∆H1) and 2nd (∆H2) Ionization Enthalpies (in kJ mol–1) and the (∆egH) Electron Gain Enthalpy (in kJ mol–1) of a few elements are given below:
Elements | ΔH1 | ΔH2 | ΔegH |
I | 520 | 7300 | –60 |
II | 419 | 3051 | –48 |
III | 1681 | 3374 | –328 |
IV | 1008 | 1846 | –295 |
V | 2372 | 5251 | +48 |
VI | 738 | 1451 | –40 |
The most reactive metal is:
1. | VI | 2. | III |
3. | I | 4. | II |
The formula of the stable binary compounds that would be formed by
an element having atomic number 71 and fluorine:
1. | LuF6
|
2. | LuF2
|
3. | LuF3
|
4. | LuF4 |
The factor that does not affect the valence electron is:
1. | Azimuthal quantum number |
2. | Nuclear charge (Z) |
3. | Nuclear mass |
4. | Number of core electrons |
The size of isoelectronic species: F–, Ne and Na+, is affected by :
1. | Nuclear charge (Z) |
2. | Valence principal quantum number (n) |
3. | Electron-electron interaction in the outer orbitals |
4. | None of the above factors because their size is the same |
The incorrect statement about ionization enthalpy is:
1. | Ionization enthalpy increases for each successive electron. |
2. | Noble gases have the highest ionization enthalpy. |
3. | A big jump in ionization enthalpy indicates a stable configuration. |
4. | Ionization enthalpy of oxygen is higher than that of nitrogen. |
Match the following isoelectronic species in Column I and Column II:
Column I | Column II | ||
i. | a. | ||
ii. | Ar | b. | |
iii. | c. | ||
iv. | d. |
i | ii | iii | iv | |
1. | b | c | a | d |
2. | c | b | a | d |
3. | c | d | b | a |
4. | b | c | d | a |
The general outer electronic configuration of s, p, d , and f-block elements respectively would be :
1. | ns1-2, nd2np1-6, (n-1)d1-10np0-2, (n-2)f1-14(n-1)d0-10ns2 |
2. | ns1-2, ns2np1-6, (n-1)f1-10ns0-2, (n-2)g1-14(n-1)d0-1ns2 |
3. | ns1-2, ns2np1-6, (n-1)d1-10ns1-2, (n-2)f1-14(n-1)d0-1 ns2 |
4. | np1-2, nd2np1-6, (n-1)d1-10ns0-2, (n-2)f1-14(n-1)d0-10ns2 |
The reactivity of alkali metals increases, whereas halogen decreases down the group, because:
1. | On moving down, ionization enthalpy decreases in group 1 while the electron gain enthalpy becomes less negative in group 17. |
2. | On moving down, ionization enthalpy increases in group 1 while the electron gain enthalpy becomes less negative in group 17. |
3. | On moving down, ionization enthalpy increases in group 1 while the electron gain enthalpy becomes less positive in group 17. |
4. | On moving down, ionization enthalpy decreases in group 17 while the electron gain enthalpy becomes less negative in group 1. |
The values of the first ionization enthalpies for two isotopes would be:
1. | Same. |
2. | Different. |
3. | Same values but positive for the first and negative for the second. |
4. | Same values but negative for the first and positive for the second. |