Advertisements
Advertisements
Question
Answer the following question.
Select the smaller ion form the following pair:
N3–, F–
Solution
F– has a smaller ionic radius than N3–.
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.
Answer the following.
Explain the screening effect with a suitable example.
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?
Choose the correct option.
Consider the elements B, Al, Mg, and K predict the correct order of metallic character:
Choose the correct option.
The lanthanides are placed in the periodic table at
Choose the correct option.
If the valence shell electronic configuration is ns2np5, the element will belong to
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+
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
What are the valence electrons?
Define ionization enthalpy.
Name the factors on which ionization enthalpy depends?
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.
Inert gases have exceptionally high ionization enthalpies.
Give reason.
Fluorine has less electron affinity than chlorine.
