The Elements in a Periodic Table are arranged so that the properties of these elements repeat periodically as a function of their atomic numbers. The size of the atoms is one such example of the repetition in properties of the elements. The Atomic Size decreases on moving to the right in a row or period; the Atomic Size increases on moving down a group.
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Definition: The Atomic Radius in a Periodic Table follows a common trend for all the elements in the periodic table. It is the function of the Atomic Number of the elements, and the size of the elements depends on the electronic configuration of the elements. |
Atomic Radius in Periodic Table Questions with Solutions
Q1: Why does the size of the elements increase on moving down the groups in a Periodic Table?
Answer: This is because there takes place an addition of energy levels as we move down in a group in the Periodic Table. As the number of energy levels increases, the size of the atoms also increases.
Q2. How can the Atomic Size be measured?
Answer: The Atomic Size of an element can be measured by measuring the distance between the nuclei of two atoms that are directly in contact with each other. This distance is noted and halved to determine the approximate size of an atom.
Q3. What is an Atomic Radius?
Answer: Atomic Radius is the distance between the nucleus of an atom to its outermost electronic energy level (outermost orbital). The Atomic Radius can also be defined as the mean distance from the nucleus of an atom to the boundary of subshells containing electrons.
Q4. What is the unit of measurement of the Atomic Radius?
Answer: The Atomic Radius of elements is so small that it is measured on an Angstrom (Å) scale.
1 Å = 10-10 m = 10-8 cm
Q5. How does the Atomic Radius change within a group and in a period in a Periodic Table?
Answer: On moving to the right of a period, the Atomic Radius of elements decreases with an increase in the atomic number. And on moving down the group, the Atomic Radius increases due to the increase in the number of energy levels.
Q6. What is an Ionic Radius? How can it be measured?
Answer: Ionic Radius is the distance measured from the nucleus of an atom to the point where it has an influence on its electronic cloud. The Ionic Radius can be measured by measuring the distance between the two neighbouring ions in a crystal structure.
Q7. What is the range of the Atomic Radius of the Periodic Table Elements?
Answer: The Atomic Radius of the elements is too small and limited to some extent. The Atomic Radius of elements ranges from 30 PM to 300 PM.
Q8. _____ has the largest Atomic Radius.
- Francium
- Rubidium
- Chlorine
- Fluorine
Answer: (a)
Explanation: Francium has the largest Atomic Radius in the Periodic Table.
Q9. Pick the correct order of the Atomic Radius.
- K > Na
- F > Cl
- Fr < Cl
- Fe < C
Answer: (a)
Explanation: Potassium (K) lies in the fourth period, while Sodium (Na) lies in the third period. As the radius of elements increases on moving down in a group, the Atomic Radius of K is bigger than Na. So, option (a) is correct.
Q10. Comment on the sizes of metals and non-metals.
Answer: The non-metals exist in the right-most corner of the periodic table, and the metals exist in the left-most corner of the periodic table. As the Atomic Radius decreases on moving from left to right in a period, the size of non-metals is smaller than the size of the metals. The metals, in fact, have the largest size in a period.
Q11. Compare the sizes of Fluorine and Chlorine on the basis of their electronic configurations.
Answer: Fluorine exists in the second period, while Chlorine exists in the third period. The electronic configuration of Fluorine and Chlorine is given below.
F: [He] 2s2 2p5
Cl: [Ne] 3s2 3p5 = [He] 2s2 2p6 3s2 3p5
The above two electronic configurations show that Chlorine has 1 extra energy level than Fluorine. Due to this reason, Chlorine is larger in size than Fluorine.
Q12. The Atomic Radius increases due to an increase in the ______.
- Number of Electrons
- Number of Protons
- Number of Electronic Shells
- None of the above
Answer: (c)
Explanation: The Electronic Shells are the energy levels of an atom in which the electrons are present. As the number of electronic shells increases, the size of an atom also increases.
Q13. The decrease in Atomic Size is very prominent in ______.
- The First Period
- The Second Period
- The Third Period
- The Fourth Period
Answer: (b)
Explanation: The decrease in the Atomic Size on moving from left to right is most prominent in the Second Period. This is because of the following factors:
- The electronegativity of elements increases significantly towards the right.
- The Atomic Radius of the elements decreases.
- The Ionization Enthalpy increases.
Q14. The Ionic Species O2-, F–, Na+, and Mg2+ are:
- Isoelectronic Species
- Isotopes
- Isomers
- None of the above
Answer: (a)
Explanation: All of the given species have 10 electrons. Thus, they are Isoelectronic Species.
Q15. The condition required for the chemical reaction: X → X+ + e– is_____.
- The use of a Catalyst
- Electron Affinity
- Ionization Energy
- None of the above
Answer: (c.)
Explanation: Ionization Energy is the energy given to isolate or remove an electron from the neutral gaseous atom.
Practice Questions on Atomic Radius in Periodic Table
Q1. Why does the Radius of atoms decreases on going from left to right in a period?
Q2. State whether the following statement is true or false.
The value of Ionization Enthalpy is always positive for a reaction.
- True
- False
Q3. The Oxidation State of Mn in KMnO4 is _____.
- 4
- 5
- 6
- 7
Q4. The compounds that can be tested with a litmus paper are:
- Only acids
- Only bases
- Both acids and bases
- None of the above
Q5. The elements Li, Mg, Be, and Al, are in a ______ relationship.
- Diagonal
- Triangular
- Periodical
- Group
Click the PDF to check the answers for Practice Questions.
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