Advertisements
Advertisements
Question
Arrange the following in order of increasing ionisation energy:
F, O, Ne
Explain your choice.
Advertisements
Solution
Ne is the rightmost element in period 2 and an inert gas. Hence, it has the highest ionisation energy.
RELATED QUESTIONS
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
Give a reason for Ionisation potential increases across a period, from left to right
State the trends in ionization energy down the group.
Name the elements with highest and lowest ionization energies in the first three periods.
Which element from the following has the highest ionization energy?
Explain your choice.
Ne, He, Ar
In a group, a particular element has the lowest ionization potential; does it ionize most easily or least easily? Explain with example.
Supply the missing word from those in the brackets:
If an element has a low ionization energy then it is likely to be ______ (metallic/ non-metallic).
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.
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?
