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Question
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?
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Solution
I (11)
RELATED QUESTIONS
Represent ionisation potential in the form of an equation. In which unit it is measured?
State the trends in ionization energy down the group.
Give reason for the following:
Ionisation potential of the element increases across a period.
Which element from the following has the highest ionization energy?
Explain your choice.
Ne, He, Ar
Choose the correct answer.
An element with highest ionization potential
(i) Calesium
(ii) Fluorine
(iii) Helium
(iv) Neon
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.
In a group, a particular element has the lowest ionization potential; does it ionize most easily or least easily? Explain with example.
Arrange the following as per instruction given in the bracket.
Na, Mg, Cl, S, Si (increasing ionisation potential)
Across a period, the ionization potential ______.
The element with highest ionisation potential is ______.
