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प्रश्न
Give reason for the following:
Ionisation potential of the element increases across a period.
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उत्तर
As atomic size decreases and nuclear charge increases, it becomes more difficult to remove electrons, requiring more energy and increasing electron potential.
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संबंधित प्रश्न
Arrange the following as per the instruction given in the brackets:
Na, Li, K (Increasing Ionisation Energy)
What do you understand by successive ionization energies?
State the trends in ionization energy across the period.
Which element from the following has the highest ionization energy?
Explain your choice.
P, Na, CI
Choose the correct answer.
An element with highest ionization potential
(i) Calesium
(ii) Fluorine
(iii) Helium
(iv) Neon
Among the elements of the second period, Li to Ne, pick out the element with highest first ionization energy
Fill in the blank from the choice given in bracket.
The energy required to remove on electron from a natural isolated gaseous atom and convert it into a positively charged gaseous ion is called ____________
Arrange the following in order of increasing ionisation energy:
F, O, Ne
Explain your choice.
Across a period, the 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?
