Advertisements
Advertisements
Question
Give reason.
Inert gases have exceptionally high ionization enthalpies.
Advertisements
Solution
- Across a period, the screening effect is the same, and the effective nuclear charge increases.
- As a result, the outer electron is held more tightly, and hence, the ionization enthalpy increases across a period.
- Inert gases are present on the extreme right of the periodic table i.e., in group 18. Also, inert gases have stable electronic configurations i.e., complete octet or duplet. Due to this, they are extremely stable and it is very difficult to remove electrons from their valence shell.
Hence, inert gases have exceptionally high ionization enthalpies.
APPEARS IN
RELATED QUESTIONS
Explain the following.
The atomic radii of Cl, I, and Br are 99, 133, and 114 pm, respectively.
Explain the following.
13Al is a metal, 14Si is a metalloid and 15P is a nonmetal.
Explain the following.
Cu forms coloured salts while Zn forms colourless salts.
Answer the following.
Ionization enthalpy of Li is 520 kJ mol-1 while that of F is 1681 kJ mol-1. Explain.
Answer the following.
Why the second ionization enthalpy is greater than the first ionization enthalpy?
Answer the following.
Why the elements belonging to the same group do have similar chemical properties?
Answer the following.
Explain electronegativity and electron gain enthalpy. Which of the two can be measured experimentally?
Choose the correct option.
Consider the elements B, Al, Mg, and K predict the correct order of metallic character:
Choose the correct option.
If the valence shell electronic configuration is ns2np5, the element will belong to
Choose the correct option.
Which of the following pairs is isoelectronic?
Answer the following question.
For the following pair, indicate which of the two species is of large size:
Fe2+ or Fe3+
Answer the following question.
Select the smaller ion form the following pair:
K+, Li+
Answer the following question.
Select the smaller ion form the following pair:
N3–, F–
With the help of a diagram answer the questions are given below:
- Which atom should have smaller ionization energy, oxygen, or sulphur?
- The lithium forms +1 ions while beryllium forms +2 ions?
Define electronegativity
Name the factors on which ionization enthalpy depends?
How does ionization enthalpy vary down the group and across a period?
How the atomic size vary in a group and across a period? Explain with suitable example.
Give reason.
Alkali metals have low ionization enthalpies.
Give reason.
Noble gases possess relatively large atomic size.
