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Question
State the trends in ionization energy across the period.
Solution
Ionization energy increases as we move from left to right across a period as the atomic size decreases.
RELATED QUESTIONS
The energy required to remove an electron from a neutral isolated gaseous atom and convert it into a positively charged gaseous ion is called ____________. (electron affinity, ionization potential,
electronegativity)
Arrange the following as per the instruction given in the brackets:
Na, Li, K (Increasing Ionisation Energy)
A process of formation of ions from molecules which are not in the ionic state
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)
Among the elements of the second period, Li to Ne, pick out the element with highest first ionization energy
Choose the correct answer from the choice given:
Ionisation potential increases over a period from left to right because the
Give reason:
Ionisation potential of the element increases across a period from left to right.
Ionisation Potential values depend on atomic size. Explain.
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?
