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प्रश्न
Arrange the following in order of increasing ionisation energy:
F, O, Ne
Explain your choice.
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उत्तर
Ne is the rightmost element in period 2 and an inert gas. Hence, it has the highest ionisation energy.
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संबंधित प्रश्न
Give a reason for Ionisation potential increases across a period, from left to right
What do you understand by successive ionization energies?
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
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.
With reference to the variation of properties in the Periodic Table, which of the following is generally true?
Ionization potential increases from left to right across a period.
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 the instruction given in the bracket
Na,Li,K (Increasing ionization energy)
The changes in the properties of elements on moving from left to right across a period of the Periodic Table. For the property, choose the correct answer.
The ionization potential:
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.
