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प्रश्न
Choose the correct answer from the options given below:
Ionisation potential increases over a period from left to right because of the
(A) Atomic radius increases and nuclear charge increases
(B) Atomic radius decreases and nuclear charge decreases
(C) Atomic radius increases and nuclear charge decreases
(D) Atomic radius decreases and nuclear charge increases
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उत्तर
Atomic radius decreases and nuclear charge increases
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संबंधित प्रश्न
Arrange the following as per the instruction given in the brackets:
Na, Li, K (Increasing Ionisation Energy)
Define the term ‘ionisation potential`.
Arrange the elements of second and third period in increasing order of ionization energy.
Which element from the following has the highest ionization energy?
Explain your choice.
Ne, He, Ar
Li, K, Na, H (In the decreasing order of their ionization potential)
Among the elements of the second period, Li to Ne, pick out the element with highest first ionization energy
The metals of group 2 from top to bottom are: Be, Mg, Ca, Sr, Ba. Which of these metals will form ions most readily and why?
Arrange the following as per instruction given in the bracket.
Na, K, Cl, S, Si (increasing ionisation potential)
Arrange the following as per the instruction given in the bracket:
Potassium, Lithium, Sodium (increasing order of ionization potential).
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?
