Arrange the elements of second and third period in increasing order of ionization energy.

Short/Brief Note

Second period: Neon > Fluorine > Oxygen > Nitrogen > Carbon > Boron > Beryllium > Lithium

Third Period: Argon > Chlorine > Sulphur > Phosphorus > Silicon > Aluminum > Magnesium > Sodium

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Chapter 1: Periodic Table, Periodic Properties and Variations of Properties - lntext Questions [Page 15]

Chapter 1 Periodic Table, Periodic Properties and Variations of Properties
lntext Questions | Q 5. (a) | Page 15

Name the periodic property which relates to the amount of energy required to remove an electron from an isolated gaseous atom.

Arrange the elements of group 17 and group 1 according to the given conditions.

Increasing ionization potential

Arrange the following in increasing order of property indicated
Li, Be, B (ionization energy)

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?

Fill in the blank from the choices given below
Across a period, the ionisation potential ____________.

which element has the highest ionisation potential.

Fill in the blank by selecting the correct word from the option.
If an element has a low ionization energy then it is likely to be ________

Arrange the following as per the instruction given in the bracket
Na,Li,K (Increasing ionization energy)

Arrange the following in order of increasing ionisation energy:

P, Na, Cl

Explain your choice.

Ionisation Potential values depend on atomic size. Explain.