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Chapter 7: Problem 41

(a) What is the general relationship between the size of an atom and its first ionization energy? (b) Which element in the periodic table has the largest ionization energy? Which has the smallest?

Short Answer

Expert verified
(a) As the atomic size increases, the ionization energy decreases. This is because larger atoms have their outermost electrons farther from the nucleus and experience less attractive force from the protons in the nucleus, requiring less energy to be removed. (b) The element with the largest ionization energy is Helium (He), while the element with the smallest ionization energy is Francium (Fr).

Step by step solution

01

(a) Understanding ionization energy and atomic size

Ionization energy is the energy required to remove an electron from a neutral atom in the gaseous state. Atomic size is the distance from the center of an atom's nucleus to its outermost electron shell.
02

(a) Relationship between atomic size and ionization energy

As the atomic size increases, the ionization energy decreases. This is because the outermost electrons are farther from the nucleus, and thus, they experience less attractive force from the protons in the nucleus. Consequently, it requires less energy to remove an electron from a larger atom as compared to a smaller atom. Now, let's move to the second part of the question.
03

(b) Identifying the element with the largest ionization energy

In the periodic table, ionization energy generally increases as one moves from left to right across a period and decreases as one moves downwards in a group. The reason for this is that when moving from left to right, the number of protons in the nucleus increases, making the positive charge of the nucleus stronger. This increases the attractive force between the nucleus and the electrons, making it harder to remove an electron. The element with the largest ionization energy is the one that has the smallest atomic size and is located in the upper-right corner of the periodic table. The element is Helium (He), located in group 18 and period 1.
04

(b) Identifying the element with the smallest ionization energy

Conversely, the element with the smallest ionization energy is the one that has the largest atomic size and is located in the lower-left corner of the periodic table. The element is Francium (Fr), located in group 1 and period 7. In summary: - There is an inverse relationship between atomic size and ionization energy: as atomic size increases, ionization energy decreases. - The element with the largest ionization energy is Helium (He), while the element with the smallest ionization energy is Francium (Fr).

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Most popular questions from this chapter

Some ions do not have a corresponding neutral atom that has the same electron configuration. For each of the following ions, identify the neutral atom that has the same number of electrons and determine if this atom has the same electron (d) \(\mathrm{Zn}^{2+}\) configuration. (a) \(\mathrm{Cl}^{-}\), (b) \(\mathrm{Sc}^{3+}\) (c) \(\mathrm{Fe}^{2+}\) (e) \(\mathrm{Sn}^{4+}\)

Detailed calculations show that the value of \(Z_{\text {eff }}\) for the outermost electrons in \(\mathrm{Na}\) and \(\mathrm{K}\) atoms is \(2.51+\) and \(3.49+\), respectively. (a) What value do you estimate for \(Z_{\text {eff }}\) experienced by the outermost electron in both \(\mathrm{Na}\) and \(\mathrm{K}\) by assuming core electrons contribute 1.00 and valence electrons contribute 0.00 to the screening constant? (b) What values do you estimate for \(Z_{\text {eff }}\) using Slater's rules? (c) Which approach gives a more accurate estimate of \(Z_{\text {eff }}\) ? (d) Does either method of approximation account for the gradual increase in \(Z_{\text {eff }}\) that occurs upon moving down a group? (e) Predict \(Z_{\text {eff }}\) for the outermost electrons in the \(\mathrm{Rb}\) atom based on the calculations for \(\mathrm{Na}\) and \(\mathrm{K}\).

Elements in group 17 in the periodic table are called the halogens; elements in group 16 are called the chalcogens. (a) What is the most common oxidation state of the chalcogens compared to the halogens? (b) For each of the following periodic properties, state whether the halogens or the chalcogens have larger values: atomic radii, ionic radii of the most common oxidation state, first ionization energy, second ionization energy.

(a) One of the alkali metals reacts with oxygen to form a solid white substance. When this substance is dissolved in water, the solution gives a positive test for hydrogen peroxide, \(\mathrm{H}_{2} \mathrm{O}_{2}\). When the solution is tested in a burner flame, a lilac-purple flame is produced. What is the likely identity of the metal? (b) Write a balanced chemical equation for the reaction of the white substance with water.

We will see in Chapter 12 that semiconductors are materials that conduct electricity better than nonmetals but not as well as metals. The only two elements in the periodic table that are technologically useful semiconductors are silicon and germanium. Integrated circuits in computer chips today are based on silicon. Compound semiconductors are also used in the electronics industry. Examples are gallium arsenide, GaAs; gallium phosphide, GaP; cadmium sulfide, CdS; and cadmium selenide, CdSe. (a) What is the relationship between the compound semiconductors' compositions and the positions of their elements on the periodic table relative to \(\mathrm{Si}\) and Ge? \((\mathbf{b})\) Workers in the semiconductor industry refer to "II-VI" and "III-V" materials, using Roman numerals. Can you identify which compound semiconductors are II-VI and which are III-V? (c) Suggest other compositions of compound semiconductors based on the positions of their elements in the periodic table.
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