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प्रश्न
State the trends in ionization energy down the group.
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उत्तर
The greater the nuclear charge, the stronger the attraction between valence electrons and the nucleus and the greater the energy needed to remove the electron(s).
संबंधित प्रश्न
Represent ionisation potential in the form of an equation. In which unit it is measured?
Choose the correct answer.
An element with highest ionization potential
(i) Calesium
(ii) Fluorine
(iii) Helium
(iv) Neon
Li, K, Na, H (In the decreasing order of their ionization potential)
A, B, C are three elements in which B is an inert gas other than helium.With this information complete the following table.
| Element | Atomic number | No. of electrons in the valence shell | Group to which the element belongs |
| A | Z - 1 | ||
| B | Z | ||
| C | Z + 1 |
Also, explain the following : Ionization energy of element C is less than that of element A.
Arrange the following in increasing order of property indicated
Li, Be, B (ionization energy)
State whether the ionization potential increases or decreases on going down a group.
Arrange the following as per instruction given in the bracket.
Na, K, Cl, S, Si (increasing ionisation potential)
First ionisation enthalpy of two elements X and Y are 500 kJ mol−1 and 375 kJ mol−1 respectively. Comment about their relative position in a group as well as in a period.
Arrange the following in order of increasing ionisation energy:
F, O, Ne
Explain your choice.
This question refers to the elements of the Periodic Table with atomic numbers from 3 to 18. Some of the elements are shown by letters, but the letters are not the usual symbols of the elements.
| 3 | 4 | 5 | 6 | 7 | 8 | 9 | 10 |
| A | B | C | D | E | F | G | H |
| 11 | 12 | 13 | 14 | 15 | 16 | 17 | 18 |
| I | J | K | L | M | N | O | P |
Which of these have least Ionisation Energy?
