Q. No.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.
Among the following, the elements that can show covalency greater than 4 is/are:
(a) Be
(b) P
(c) S
(d) B
Choose the correct option
1. (a), (d)
2. (b), (c)
3. (c), (d)
4. (b), (d)
In which following options of arrangement does not agree with the variation of the property indicated against it?
| (a) | Al3+< Mg2+< Na+< F– (Increasing ionic size) |
| (b) | B < C < N (Increasing atomic size) |
| (c) | I < Br < Cl (Increasing atomic size) |
| (d) | Li < Na < K (Metallic character) |
Choose the correct option
| 1. | (a), (d) | 2. | (b), (c) |
| 3. | (c), (d) | 4. | (b), (d) |
The properties among the following can be shown by the element belonging
to the 3rd period and group 13 of the periodic table:
(a) Good conductor of electricity
(b) Liquid, metallic
(c) Solid, metallic
(d) Solid, non-metallic
Choose the correct option :
1. (a), (c)
2. (b), (c)
3. (c), (d)
4. (b), (d)
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 general outer electronic configuration of s, p, d , and f-block elements respectively would be :
| 1. | ns1-2, ns2np1-6, (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)f1-14nd0-1ns2 |
| 3. | ns1-2, ns2np1-6, (n-1)d1-10ns1-2, (n-2)f1-14(n-1)d0-1 ns2 |
| 4. | ns1-2, ns2np1-6, (n-1)d1-10ns0-2, (n-2)f1-14(n-2)d0-10ns2 |
The statement that "the electronegativity of N on the Pauling scale is 3.0 in all the nitrogen compounds" is incorrect because:
| 1. | Electronegativity of an element is a variable property. |
| 2. | Pauling scale is not used to measure electronegativity. |
| 3. | The electronegativity of N on the Pauling scale is 12.0 |
| 4. | None of the above. |
The basic difference between the electron gain enthalpy (Ea) and electronegativity (EN) is:
| 1. | Ea is the tendency to lose electrons, while EN is the tendency to repel the shared pairs of electrons. |
| 2. | Ea is the tendency to gain neutrons, while EN is the tendency to attract the shared pairs of electrons. |
| 3. | Ea is the tendency to donate electrons, while EN is the tendency to attract the shared pairs of molecules. |
| 4. | Ea is the tendency to gain electrons, while EN is the tendency to attract the shared pairs of electrons. |
An element with higher negative electron gain enthalpy in the given pair is:
(i) O or F (ii) F or Cl
1. O, Cl
2. F, F
3. O, F
4. F, Cl
The trend of atomic radius in a period and a group is :
| 1. | Generally decreases from right to left across a period and increases down a group. |
| 2. | Generally increases from left to right across a period and decreases down a group. |
| 3. | Generally decreases from left to right across a period and increases down a group. |
| 4. | Generally remains same from left to right across a period and increases down a group. |
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