Indicate which one of the two species in each of the following pairs is smaller: (a) Cl or Cl−; (b) Na or Na+; (c) O2− or S2−; (d) Mg2+ or Al3+; (e) Au or Au3+.
(a)
Interpretation:
In the given set of species which will be smaller in size has to be identified.
Concept Introduction:
- The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
- As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
- An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
- Anions will have larger size compared to cations.
- The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
- When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
- A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
- If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
- The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.
To identify: The species which will have smaller size from the given species.
Answer to Problem 4.89QP
Answer
In (a)
Explanation of Solution
The number of electrons and protons in the given set of species (a) is,
Species | Total number of Electrons | Total number of Protons |
| 17 | 17 |
| 18 | 17 |
The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total number of protons in all the given species is same, but the total numbers of electrons are different.
By comparing the total number of protons and electrons in the table given in the previous step and as comparing to the size of atom size of anion is larger. And also here the proton number is lesser than the electron in
(b)
Interpretation:
In the given set of species which will be smaller in size has to be identified.
Concept Introduction:
- The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
- As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
- An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
- Anions will have larger size compared to cations.
- The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
- When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
- A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
- If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
- The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.
To identify: The species which will have smaller size from the given species.
Answer to Problem 4.89QP
Answer
In (b)
Explanation of Solution
The number of electrons and protons in the given set of species (b)
Species | Total number of Electrons | Total number of Protons |
| 11 | 11 |
| 10 | 11 |
The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total numbers of protons in all the given species are same, but the total numbers of electrons are different.
By comparing the total number of protons and electrons in the table given in the previous step it is clear that the number of proton is greater than the electron in
(c)
Interpretation:
In the given set of species which will be smaller in size has to be identified.
Concept Introduction:
- The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
- As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
- An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
- Anions will have larger size compared to cations.
- The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
- When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
- A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
- If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
- The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.
To identify: The species which will have smaller size from the given species.
Answer to Problem 4.89QP
Answer
In (c)
Explanation of Solution
The number of electrons and protons in the given set of species (c)
Species | Total number of Electrons | Total number of Protons |
| 8 | 10 |
| 16 | 18 |
The total number of electrons and protons present for the given species are found out and presented in the above table.
The given two species belong to group “6A” of periodic table. The oxygen atom comes before the sulphur atom when we move down the periodic table. As discussed above, when we move down the group the ionic radius increases because the electrons are added to a new subshell. Hence,
(d)
Interpretation:
In the given set of species which will be smaller in size has to be identified.
Concept Introduction:
- The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
- As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
- An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
- Anions will have larger size compared to cations.
- The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
- When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
- A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
- If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
- The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.
To identify: The species which will have smaller size from the given species.
Answer to Problem 4.89QP
Answer
In (d)
Explanation of Solution
The number of electrons and protons in the given set of species (d)
Species | Total number of Electrons | Total number of Protons |
| 10 | 12 |
| 10 | 13 |
The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total number of electrons in all the given ions is same, but the total numbers of protons are different.
The number of proton in
(e)
Interpretation:
In the given set of species which will be smaller in size has to be identified.
Concept Introduction:
- The distance between the nucleus and the valence shell of a cation or an anion is known as ionic radius. An ion is formed by either loss or gain of electrons from its valence shell.
- As we move down the group in periodic table the ionic radius increases as the electrons are added to new subshell. As we move across the period the ionic radius increases as the electrons are added to the same subshell.
- An anion is formed when an electron is added to the valence shell of an atom. The anion has a net negative charge in it. In anion the extra electron added occupies more space and maximizes the shielding.
- Anions will have larger size compared to cations.
- The reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons in the nucleus is known as shielding effect
- When the proton number is greater than the electron, the size of the ion will be smaller due to less shielding. When the proton number is lesser than the electron, the size of the ion will be larger due to more shielding.
- A cation is formed when an electron is lost by an atom from its valence shell. The cation has a net positive charge. In cation the shielding decreases as the electron is removed from the valence shell.
- If the total number of electrons is less than the total number of protons in the ion, then the protons present can effectively attract the valence shell decreasing the size of the ion and vice-versa.
- The trend in periodic table can be described as well. As we move down the group the ionic radius decreases as the electrons are added to a new shell. But as we move across a period in periodic table the ionic radius increases as the electrons are added to the same subshell.
To identify: The species which will have smaller size from the given species.
Answer to Problem 4.89QP
Answer
In (e)
Explanation of Solution
The number of electrons and protons in the given set of species (e)
Species | Total number of Electrons | Total number of Protons |
| 79 | 79 |
| 76 | 79 |
The total number of electrons and protons present for the given species are found out and presented in the above table. From this we can see that total number of protons in the given species is same, but the total numbers of electrons are different.
By comparing the total number of protons and electrons in the table given in the previous step it is clear that the number of proton is greater than the electron in
Want to see more full solutions like this?
Chapter 4 Solutions
Chemistry: Atoms First - With Solutions and Access
- Which of the four atoms Na, P, Cl, or K (a) has the largest atomic radius? (b) has the highest ionization energy? (c) is the most electronegative?arrow_forwardAt first glance, we expect the Zeff of a valence electron of sodium (Z = 11) to be 1 but in reality, it is closer to 2.667 because _____.arrow_forwardSince the first ionization energy of rubidium is +403 kJ mol, how many kJ of energy is it required to convert 22.90 g gaseous rubidium to +1 monoatomic ion at constant temperature?arrow_forward
- Na+, Ne, O2-, Mg2+, F- Which isthe smallest in size? Which has the lowest ionization energy?arrow_forwardThe experimentally determinded Bi-Cl bond distance in bismuth trichloride is 2.48Å . Given the tablulated value of 0.99Å for the atomic radius of Cl, predict the atomic radius of Bi?arrow_forward7.104 The energy needed for the following process is1.96 × 104kJ/mol: If the first ionization energy of lithium is 520 kJ/mol,calculate the second ionization energy of lithium, that is,the energy required for the processarrow_forward
- A) Which of the halogen elements has the highest density in its standard state? B) Which of the elements of the third period should have the highest 2nd ionization energy? C) For which of Al, Si or P is the absolute value of the Electron Affinity greatest? D) Which of the ions Mg2+, Sr2+, Ca2+, Be2+, Ba2+, or Ra2+ is the smallest? E) For the elements: X = Br, I, Cl, or H, which has the the smallest average X-C bond energy?arrow_forwardWrite any two multiplicities of higher energy in the form 2s+1L J, giving a diagrammatic illustration of each.arrow_forward7.5 B What must the distance be between charges of +2.25 and −1.86 for the attractive force between them to be the same as that between charges of +4.06 and −2.11 separated by a distance of 2.16 pm?arrow_forward
- Please, give simple words explenation. Additional examples very helpful. Please, write the answer clear or typed. Thank you Ionic radii Why is there an overall contraction in ionic radii? Why is radius of Ti^ 2+ less than theoretical value? Why is the radius of Cr^ 2+ larger than that of V^ 2+.arrow_forwardArrange the following in order of decreasing size? Mg2+, K+ and Ar?arrow_forwardArrange the following seven atoms or ions in order of size,from smallest to largest: K, F+, Rb, Co25+, Br, F, Rb-.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningPrinciples of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning