Advertisements
Advertisements
प्रश्न
Answer the following.
Ionization enthalpy of Li is 520 kJ mol-1 while that of F is 1681 kJ mol-1. Explain.
Advertisements
उत्तर
- Both Li and F belong to period 2.
- Across a period, the screening effect is the same while the effective nuclear charge increases.
- As a result, the outer electron is held more tightly, and therefore, the ionization enthalpy increases across a period.
- Hence, F will have higher ionization enthalpy than Li.
Thus, the ionization enthalpy of Li is 520 kJ mol-1 while that of F is 1681 kJ mol-1.
APPEARS IN
संबंधित प्रश्न
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.
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.
For the following pair, indicate which of the two species is of large size:
Mg2+ or Ca2+
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 ionic radius
Define electronegativity
What are the valence electrons?
Define ionization enthalpy.
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.
Fluorine has less electron affinity than chlorine.
Give reason.
Noble gases possess relatively large atomic size.
