Explain the important distinctions between each pair of terms: (a) actinide and lanthanide element; (b) covalent and metallic radius; (c) atomic number and effective nuclear charge; (d) ionization energy and electron affinity; (e) paramagnetic and diamagnetic.

Short Answer

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The key distinctions are as follows. Actinides and lanthanides differ by atomic number and several physical properties; covalent radius refers to the approximate half-distance in a covalent bond while metallic radius refers to the same in a metallic crystal; atomic number is the count of protons while effective nuclear charge considers electron-electron repulsion; ionization energy is the energy to remove an electron, while electron affinity refers to the energy when gaining one; paramagnetic materials are attracted to magnetic fields and diamagnetic ones are repelled by them.

Step by step solution

01

Actinide and Lanthanide Element

First, define each. Actinides are 15 metallic chemical elements with atomic numbers from 89 to 103, actinium through lawrencium. They make up the f-block of the periodic table. Lanthanides are 15 metallic chemical elements with atomic numbers from 57 through 71, from lanthanum through lutetium. They form another part of the f-block. These two differ not only in their atomic numbers but also in their electron configurations, oxidation states, and other chemical and physical properties.
02

Covalent and Metallic Radius

The covalent radius is approximately half the distance between the nuclei of two similar atoms bonded together, while the metallic radius is half the distance between the nuclei of two adjacent atoms in a metallic crystal. The covalent radius reflects the size of an atom that forms part of a covalent bond, whereas the metallic radius reflects the size of an atom in a metallic crystal structure.
03

Atomic Number and Effective Nuclear Charge

The atomic number is the number of protons in an atom's nucleus, which defines the chemical characteristics of the element and its place in the periodic table. Effective nuclear charge is the net positive charge experienced by the valence electrons in an atom. It differs from the atomic number because it takes into account the effect of electron-electron repulsion. Atomic number identifies an element, while effective nuclear charge impacts an atom's reactivity and size.
04

Ionization Energy and Electron Affinity

Ionization energy is the energy required to remove an electron from an atom or ion. Electron affinity is the energy change when an atom or ion gains an electron. Ionization energy measure the tendency of an atom to lose electrons, while electron affinity indicates an atom's desire to gain electrons. Both quantities relate to the energy changes associated with electrons, but in opposite ways.
05

Paramagnetic and Diamagnetic

Paramagnetic materials are attracted to magnetic fields due to the presence of unpaired electrons and their spin; diamagnetic materials, with no unpaired electrons, are slightly repelled by magnetic fields. The main difference lies in their reaction to external magnetic fields: paramagnetic substances get attracted and diamagnetic substances get repelled.

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Most popular questions from this chapter

Describe how the ionization energies of the ions \(\mathrm{He}^{-}, \mathrm{Li}^{-}, \mathrm{Be}^{-}, \mathrm{B}^{-}, \mathrm{C}^{-}, \mathrm{N}^{-}, \mathrm{O}^{-},\) and \(\mathrm{F}^{-}\) vary with atomic number.

Is it possible for two different atoms to be isoelectronic? two different cations? two different anions? a cation and an anion? Explain.

A method for estimating electron affinities is to extrapolate \(Z_{\text {eff }}\) values for atoms and ions that contain the same number of electrons as the negative ion of interest. Use the data in the table on the next page to answer the questions that follow. $$\begin{array}{lll} \hline \begin{array}{l} \text { Atom or lon: } \\ \text { I(kJmol }^{-1} \text {) } \end{array} & \begin{array}{l} \text { Atom or lon: } \\ \text { I(kJmol }^{-1} \text {) } \end{array} & \begin{array}{l} \text { Atom or lon: } \\ \text { I(kJmol }^{-1} \text {) } \end{array} \\ \hline \text { Ne: 2080 } & \text { F: 1681 } & \text { O: } 1314 \\ \text { Na }^{+}: 4565 & \text { Ne }^{+}: 3963 & \text { F }^{+}: 3375 \\ \text { Mg }^{2+} \text { : 7732 } & \text { Na }^{2+}: 6912 & \text { Ne }^{2+}: 6276 \\ \text { A1 }^{\text {3 }^{+}: 11,577} & \text { Mg }^{3+}: 10,548 & \text { Na }^{3+}: 9540 \\ \hline \end{array}$$ (a) Estimate the electron affinity of \(F\), and compare it with the experimental value. (b) Estimate the electron affinities of \(\mathrm{O}\) and \(\mathrm{N}\) (c) Examine your results in terms of penetration and screening.

Must all atoms with an odd atomic number be paramagnetic? Must all atoms with an even atomic number be diamagnetic? Explain.

Explain why the first ionization energy of \(\mathrm{Mg}\) is greater that of \(\mathrm{Na},\) whereas the second ionization of Na is greater than that of Mg.

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