Describe and define the oboffered patterns in atomic dimension, ionization power, and electron affinity of the elements

The facets in groups (vertical columns) of the periodic table exhibit similar chemical habits. This similarity occurs bereason the members of a group have the exact same number and also circulation of electrons in their valence shells. However before, tright here are additionally other patterns in chemical properties on the routine table. For instance, as we relocate down a group, the metallic character of the atoms boosts. Oxygen, at the height of group 16 (6A), is a colormuch less gas; in the middle of the group, selenium is a semiconducting solid; and, toward the bottom, polonium is a silver-grey solid that conducts electrical power.

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As we go throughout a period from left to ideal, we include a proton to the nucleus and also an electron to the valence shell through each succeeding element. As we go down the aspects in a group, the number of electrons in the valence shell remains continuous, however the primary quantum number boosts by one each time. An understanding of the digital structure of the aspects permits us to research some of the properties that govern their chemical behavior. These properties vary periodically as the digital framework of the aspects transforms. They are (1) dimension (radius) of atoms and also ions, (2) ionization energies, and also (3) electron affinities.


Explore visualizations of the periodic fads discussed in this section (and many kind of even more trends). With simply a couple of clicks, you have the right to create three-dimensional versions of the periodic table reflecting atomic size or graphs of ionization energies from all measured facets.

Variation in Covalent Radius

The quantum mechanical image provides it challenging to develop a definite dimension of an atom. However before, there are several handy methods to define the radius of atoms and also, for this reason, to recognize their family member sizes that give approximately similar worths. We will certainly use the covalent radius (Figure 1), which is defined as one-fifty percent the distance between the nuclei of two identical atoms as soon as they are joined by a covalent bond (this measurement is feasible because atoms within molecules still retain much of their atomic identity). We know that as we sdeserve to down a team, the major quantum number, n, boosts by one for each aspect. Hence, the electrons are being added to an area of room that is progressively remote from the nucleus. Consequently, the dimension of the atom (and also its covalent radius) have to boost as we boost the distance of the outermany electrons from the nucleus. This trfinish is shown for the covalent radii of the halogens in Table 5 and also Figure 1. The fads for the entire periodic table deserve to be watched in Figure 1.

AtomCovalent radius (pm)Nuclear charge
Table 5. Covalent Radii of the Halogen Group Elements
Figure 1. (a) The radius of an atom is characterized as one-fifty percent the distance in between the nuclei in a molecule consisting of two similar atoms joined by a covalent bond. The atomic radius for the halogens increases down the group as n boosts. (b) Covalent radii of the elements are shown to scale. The basic trfinish is that radii rise down a team and decrease throughout a period.
Figure 2. Within each duration, the trend in atomic radius decreases as Z increases; for instance, from K to Kr. Within each team (e.g., the alkali metals displayed in purple), the trend is that atomic radius rises as Z rises.

As presented in Figure 2, as we relocate throughout a period from left to ideal, we mainly find that each facet has a smaller covalent radius than the facet coming before it. This could seem counterintuitive because it means that atoms via even more electrons have a smaller atomic radius. This can be described via the idea of reliable nuclear charge, Zeff. This is the pull exerted on a particular electron by the nucleus, taking right into account any kind of electron–electron repulsions. For hydrogen, tbelow is just one electron and also so the nuclear charge (Z) and also the reliable nuclear charge (Zeff) are equal. For all various other atoms, the inner electrons partly shield the outer electrons from the pull of the nucleus, and also thus:

Shielding is identified by the probcapability of one more electron being in between the electron of interemainder and also the nucleus, as well as by the electron–electron repulsions the electron of interest encounters. Core electrons are adept at shielding, while electrons in the exact same valence shell do not block the nuclear attraction knowledgeable by each other as effectively. Therefore, each time we relocate from one element to the following across a period, Z boosts by one, but the shielding rises only slightly. Hence, Zeff increases as we relocate from left to best throughout a period. The stronger pull (better reliable nuclear charge) knowledgeable by electrons on the ideal side of the routine table draws them closer to the nucleus, making the covalent radii smaller sized.

Therefore, as we would certainly mean, the outerthe majority of or valence electrons are most basic to rerelocate bereason they have actually the highest possible energies, are shielded even more, and also are farthest from the nucleus. As a general rule, as soon as the representative facets create cations, they carry out so by the loss of the ns or np electrons that were included last in the Aufbau process. The transition facets, on the other hand also, lose the ns electrons before they begin to shed the (n – 1)d electrons, even though the ns electrons are included initially, according to the Aufbau principle.

Example 1

Sorting Atomic RadiiPredict the order of raising covalent radius for Ge, Fl, Br, Kr.

SolutionRadius increases as we relocate dvery own a group, so Ge Give an instance of an atom whose size is smaller than fluorine.

Variation in Ionic Radii

Ionic radius is the meacertain used to define the dimension of an ion. A cation always has fewer electrons and the same variety of proloads as the parent atom; it is smaller sized than the atom from which it is derived (Figure 3). For example, the covalent radius of an aluminum atom (1s22s22p63s23p1) is 118 pm, whereas the ionic radius of an Al3+ (1s22s22p6) is 68 pm. As electrons are removed from the external valence shell, the staying core electrons occupying smaller shells suffer a better efficient nuclear charge Zeff (as discussed) and also are attracted also closer to the nucleus.

Figure 3. The radius for a cation is smaller than the parent atom (Al), as a result of the lost electrons; the radius for an anion is larger than the parent (S), as a result of the gained electrons.

Cations with larger charges are smaller than cations through smaller charges (e.g., V2+ has an ionic radius of 79 pm, while that of V3+ is 64 pm). Proceeding down the groups of the routine table, we uncover that cations of successive aspects via the exact same charge mostly have actually bigger radii, matching to a rise in the primary quantum number, n.

An anion (negative ion) is created by the enhancement of one or even more electrons to the valence shell of an atom. This outcomes in a higher repulsion among the electrons and a decrease in Zeff per electron. Both results (the increased variety of electrons and the lessened Zeff) cause the radius of an anion to be bigger than that of the parent atom (Figure 3). For example, a sulhair atom (3s23p4) has actually a covalent radius of 104 pm, whereas the ionic radius of the sulfide anion (3s23p6) is 170 pm. For consecutive facets proceeding down any kind of group, anions have actually larger primary quantum numbers and also, for this reason, larger radii.

Atoms and also ions that have actually the exact same electron configuration are shelp to be isoelectronic. Instances of isoelectronic species are N3–, O2–, F–, Ne, Na+, Mg2+, and also Al3+ (1s22s22p6). Another isodigital series is P3–, S2–, Cl–, Ar, K+, Ca2+, and also Sc3+ (3s23p6). For atoms or ions that are isoelectronic, the number of prolots determines the size. The greater the nuclear charge, the smaller the radius in a series of isodigital ions and also atoms.

Variation in Ionization Energies

The amount of power compelled to rerelocate the a lot of loosely bound electron from a gaseous atom in its ground state is called its initially ionization energy (IE1). The initially ionization energy for an aspect, X, is the power required to form a cation with +1 charge:

The power required to remove the second most loosely bound electron is called the second ionization power (IE2).

extX^+ (g) longrightarrow extX^2+(g) + exte^- ;;;;; extIE_2

The power forced to rerelocate the third electron is the 3rd ionization energy, and so on. Energy is always forced to rerelocate electrons from atoms or ions, so ionization procedures are endothermic and also IE values are always positive. For larger atoms, the most loosely bound electron is situated farther from the nucleus and also so is much easier to rerelocate. Therefore, as size (atomic radius) rises, the ionization energy have to decrease. Relating this logic to what we have actually simply learned about radii, we would intend first ionization energies to decrease down a group and also to boost throughout a duration.

Figure 4 graphs the connection in between the initially ionization power and the atomic variety of several elements. The values of initially ionization energy for the elements are provided in Figure 5. Within a period, the IE1 generally boosts via increasing Z. Dvery own a team, the IE1 value mainly decreases through boosting Z. Tright here are some methodical deviations from this trend, yet. Note that the ionization power of boron (atomic number 5) is less than that of beryllium (atomic number 4) even though the nuclear charge of boron is higher by one proton. This deserve to be described bereason the energy of the subshells rises as l increases, as a result of penetration and also shielding (as discussed formerly in this chapter). Within any type of one shell, the s electrons are lower in power than the p electrons. This suggests that an s electron is harder to remove from an atom than a p electron in the exact same shell. The electron removed throughout the ionization of beryllium (2s2) is an s electron, whereas the electron removed throughout the ionization of boron (2s22p1) is a p electron; this outcomes in a lower initially ionization energy for boron, even though its nuclear charge is higher by one proton. Therefore, we view a tiny deviation from the predicted trfinish developing each time a new subshell starts.

Figure 4. The initially ionization power of the facets in the initially 5 periods are plotted against their atomic number.
Figure 5. This variation of the regular table shows the initially ionization power of (IE1), in kJ/mol, of selected aspects.

Another deviation occurs as orbitals end up being more than one-fifty percent filled. The initially ionization energy for oxygen is slightly less than that for nitrogen, despite the trend in enhancing IE1 worths across a period. Looking at the orbital diagram of oxygen, we have the right to watch that removing one electron will certainly eliminate the electron–electron repulsion caused by pairing the electrons in the 2p orbital and also will certainly bring about a half-filled orbital (which is energetically favorable). Analogous transforms take place in succeeding periods (note the dip for sulhair after phosphorus in Figure 5).


Removing an electron from a cation is even more tough than rerelocating an electron from a neutral atom bereason of the higher electrostatic attraction to the cation. Likewise, removing an electron from a cation through a higher positive charge is more tough than rerelocating an electron from an ion via a reduced charge. Hence, succeeding ionization energies for one facet always increase. As viewed in Table 6, tright here is a huge increase in the ionization energies (color change) for each element. This jump coincides to removal of the core electrons, which are harder to remove than the valence electrons. For example, Sc and Ga both have 3 valence electrons, so the rapid boost in ionization power occurs after the 3rd ionization.

Ge762.21537.53302.14410.69021.4Not availableNot available
As944.51793.62735.54836.86042.912311.5Not available
Table 6. Successive Ionization Energies for Schosen Elements (kJ/mol)

Example 2

Ranking Ionization EnergiesPredict the order of raising power for the following processes: IE1 for Al, IE1 for Tl, IE2 for Na, IE3 for Al.

SolutionRerelocating the 6p1 electron from Tl is simpler than removing the 3p1 electron from Al bereason the better n orbital is farther from the nucleus, so IE1(Tl) 1(Al). Ionizing the third electron from extAl ;;;;; ( extAl^2+ longrightarrow extAl^3+ + exte^-) calls for even more energy bereason the cation Al2+ exerts a stronger pull on the electron than the neutral Al atom, so IE1(Al) 3(Al). The second ionization energy for sodium clears a core electron, which is a much better power procedure than removing valence electrons. Putting this all together, we obtain: IE1(Tl) 1(Al) 3(Al) 2(Na).

Check Your LearningWhich has the lowest value for IE1: O, Po, Pb, or Ba?

Variation in Electron Affinities

The electron affinity is the power change for the process of adding an electron to a gaseous atom to create an anion (negative ion).

This process can be either endothermic or exothermic, relying on the aspect. The EA of some of the aspects is offered in Figure 6. You can check out that many kind of of these facets have negative values of EA, which means that power is released when the gaseous atom accepts an electron. However before, for some elements, energy is forced for the atom to end up being negatively charged and also the value of their EA is positive. Just as via ionization power, subsequent EA values are connected through creating ions with more charge. The second EA is the power associated through adding an electron to an anion to form a –2 ion, and also so on.

As we could predict, it becomes simpler to include an electron throughout a collection of atoms as the effective nuclear charge of the atoms increases. We find, as we go from left to best throughout a period, EAs tend to become more negative. The exceptions discovered among the elements of team 2 (2A), group 15 (5A), and also group 18 (8A) can be understood based upon the digital structure of these groups. The noble gases, group 18 (8A), have actually a completely filled shell and also the incoming electron have to be added to a higher n level, which is more hard to do. Group 2 (2A) has a filled ns subshell, and also so the next electron added goes into the greater power np, so, again, the observed EA worth is not as the trfinish would certainly predict. Finally, group 15 (5A) has a half-filled np subshell and the next electron must be paired with an existing np electron. In every one of these cases, the initial relative stcapacity of the electron configuration disrupts the trfinish in EA.

We likewise could intend the atom at the height of each team to have actually the biggest EA; their first ionization potentials suggest that these atoms have actually the largest effective nuclear charges. However before, as we relocate down a group, we view that the second facet in the group most regularly has the greatest EA. The reduction of the EA of the initially member deserve to be attributed to the tiny size of the n = 2 shell and the resulting huge electron–electron repulsions. For instance, chlorine, with an EA worth of –348 kJ/mol, has the highest possible value of any element in the regular table. The EA of fluorine is –322 kJ/mol. When we add an electron to a fluorine atom to develop a fluoride anion (F–), we add an electron to the n = 2 shell. The electron is attracted to the nucleus, yet tright here is additionally significant repulsion from the various other electrons already present in this small valence shell. The chlorine atom has actually the same electron configuration in the valence shell, yet bereason the entering electron is going into the n = 3 shell, it occupies a substantially larger region of room and also the electron–electron repulsions are decreased. The entering electron does not experience as much repulsion and also the chlorine atom accepts a secondary electron more conveniently.

Figure 6. This variation of the periodic table display screens the electron affinity worths (in kJ/mol) for selected elements.

The properties discussed in this section (size of atoms and ions, effective nuclear charge, ionization energies, and also electron affinities) are central to knowledge chemical reactivity. For instance, bereason fluorine has an energetically favorable EA and also a big energy barrier to ionization (IE), it is much less complicated to create fluorine anions than cations. Metallic properties including conductivity and mallecapability (the capacity to be developed into sheets) depend on having electrons that can be removed conveniently. Thus, metallic character increases as we relocate dvery own a team and decreases across a period in the exact same trfinish oboffered for atomic size because it is easier to remove an electron that is farther amethod from the nucleus.

See more: Which Of The Following Is A Strong Electrolyte? ? (A)$Hcl$ (B)$Hbr

Key Concepts and also Summary

Electron configurations enable us to understand many kind of routine patterns. Covalent radius rises as we move dvery own a group bereason the n level (orbital size) rises. Covalent radius greatly decreases as we relocate left to right throughout a duration bereason the reliable nuclear charge proficient by the electrons boosts, and the electrons are pulled in tighter to the nucleus. Anionic radii are bigger than the parent atom, while cationic radii are smaller, because the variety of valence electrons has actually adjusted while the nuclear charge has actually stayed consistent. Ionization energy (the power linked via developing a cation) decreases down a team and also largely increases across a duration because it is easier to remove an electron from a larger, higher energy orbital. Electron affinity (the energy connected via forming an anion) is even more favorable (exothermic) when electrons are inserted into reduced power orbitals, closer to the nucleus. As such, electron affinity becomes increasingly negative as we move left to right throughout the periodic table and decreases as we move dvery own a group. For both IE and also electron affinity data, tright here are exceptions to the patterns as soon as taking care of totally filled or half-filled subshells.

Chemistry End of Chapter Exercises

Based on their positions in the routine table, predict which has actually the smallest atomic radius: Mg, Sr, Si, Cl, I.Based on their positions in the periodic table, predict which has actually the largest atomic radius: Li, Rb, N, F, I.Based on their positions in the regular table, predict which has actually the largest initially ionization energy: Mg, Ba, B, O, Te.Based on their positions in the periodic table, predict which has the smallest initially ionization energy: Li, Cs, N, F, I.Based on their positions in the regular table, rank the following atoms in order of enhancing first ionization energy: F, Li, N, RbBased on their positions in the regular table, rank the complying with atoms or compounds in order of boosting first ionization energy: Mg, O, S, SiAtoms of which group in the periodic table have a valence shell electron configuration of ns2np3?Atoms of which team in the routine table have actually a valence shell electron configuration of ns2?Based on their positions in the routine table, list the adhering to atoms in order of enhancing radius: Mg, Ca, Rb, Cs.Based on their positions in the periodic table, list the following atoms in order of enhancing radius: Sr, Ca, Si, Cl.Based on their positions in the routine table, list the following ions in order of enhancing radius: K+, Ca2+, Al3+, Si4+.List the complying with ions in order of increasing radius: Li+, Mg2+, Br–, Te2–.Which atom and/or ion is (are) isoelectronic with Br+: Se2+, Se, As–, Kr, Ga3+, Cl–?Which of the complying with atoms and ions is (are) isodigital through S2+: Si4+, Cl3+, Ar, As3+, Si, Al3+?Compare both the numbers of prolots and electrons current in each to rank the complying with ions in order of enhancing radius: As3–, Br–, K+, Mg2+.Of the five aspects Al, Cl, I, Na, Rb, which has actually the the majority of exothermic reaction? (E represents an atom.) What name is given to the power for the reaction? Hint: note the process illustrated does not correspond to electron affinity extE^+(g) + exte^- longrightarrowhead extE(g)Of the 5 aspects Sn, Si, Sb, O, Te, which has the a lot of endothermic reaction? (E represents an atom.) What name is given to the power for the reaction? extE(g) longrightarrow extE(g)^+ + exte^-The ionic radii of the ions S2–, Cl–, and also K+ are 184, 181, 138 pm respectively. Explain why these ions have actually different sizes even though they contain the same number of electrons.Which primary team atom would be supposed to have actually the lowest second ionization energy?Exordinary why Al is a member of group 13 rather than team 3?


covalent radiusone-half the distance between the nuclei of two similar atoms when they are joined by a covalent bondefficient nuclear chargecharge that leads to the Coulomb pressure exerted by the nucleus on an electron, calculated as the nuclear charge minus shieldingelectron affinityenergy forced to add an electron to a gaseous atom to develop an anionionization energyenergy forced to rerelocate an electron from a gaseous atom or ion. The associated number (e.g., second ionization energy) corresponds to the charge of the ion produced (X2+)isoelectronicteam of ions or atoms that have actually similar electron configurations


Answers to Chemisattempt End of Chapter Exercises