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Chapter 7: Problem 12

Moseley's experiments on \(\mathrm{X}\) rays emitted from atoms led to the concept of atomic numbers. (a) If arranged in order of increasing atomic mass, which element would come after chlorine? (b) Describe two ways in which the properties of this element differ from the other elements in group $8 \mathrm{~A}$.

Short Answer

Expert verified
The element that comes after Chlorine when arranged in order of increasing atomic mass is Argon (Ar). Argon differs from other elements in group 8A in terms of its lower atomic mass and lower boiling point.

Step by step solution

01

From the periodic table, we can find the atomic mass of Chlorine (Cl), which is approximately 35.5 atomic mass units (amu). ##Step 2: Identify the element after Chlorine##

After identifying Chlorine's atomic mass, we need to look for the next element in the periodic table with a higher atomic mass. The next element with higher atomic mass is Argon (Ar) with an atomic mass of approximately 39.95 amu. ##Step 3: Identify Argon's properties##
02

Argon (Ar) is a noble gas and belongs to the 8A group in the periodic table. It has an electron configuration of \(1s^2 2s^2 2p^6 3s^2 3p^6\). Argon is colorless, odorless, and an inert gas. ##Step 4: Compare Argon's properties with other elements in group 8A##

We need to describe two ways in which Argon's properties differ from other elements in group 8A. Difference 1:
03

Argon has a lower atomic mass compared to other elements in group 8A. The atomic masses of the elements in group 8A increase as we go down the periodic table (e.g., Krypton, Xenon, and Radon). Difference 2:

Argon has the lowest boiling point (-302.6°F or -185.9°C) among the elements in group 8A. As we go down the group, the boiling points of the elements increase (Krypton's boiling point: -244.2°F or -153.4°C, Xenon's boiling point: -162.2°F or -108.1°C, and Radon's boiling point: - 81.8°F or -63.1°C). In conclusion, the element which comes after Chlorine when arranged in order of increasing atomic mass is Argon (Ar), and it differs from other elements in group 8A in terms of its lower atomic mass and lower boiling point.

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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) \(\mathrm{Sn}^{4+}\)

Which of the following statements about effective nuclear charge for the outermost valence electron of an atom is incorrect? (i) The effective nuclear charge can be thought of as the true nuclear charge minus a screening constant due to the other electrons in the atom. (ii) Effective nuclear charge increases (iii) Valence going left to right across a row of the periodic table. electrons screen the nuclear charge more effectively than do core electrons. (iv) The effective nuclear charge shows a sudden decrease when we go from the end of one row to the beginning of the next row of the periodic table. (v) The change in effective nuclear charge going down a column of the periodic table is generally less than that going across a row of the periodic table.

For each of the following pairs, indicate which element has the smaller first ionization energy: (a) $\mathrm{Cs}, \mathrm{Cl} ;(\mathbf{b}) \mathrm{Fe}, \mathrm{Zn} ;\( (c) \)\mathrm{I}, \mathrm{Cl} ;(\mathbf{d}) \mathrm{Se}, \mathrm{Sn}$

Which will experience the greater effect nuclear charge, the electrons in the \(n=2\) shell in \(\mathrm{F}\) or the \(n=2\) shell in \(\mathrm{B}\) ? Which will be closer to the nucleus?

Chlorine reacts with oxygen to form \(\mathrm{Cl}_{2} \mathrm{O}_{7} .\) (a) What is the name of this product (see Table 2.6)? (b) Write a balanced equation for the formation of \(\mathrm{Cl}_{2} \mathrm{O}_{7}(l)\) from the elements. (c) Would you expect \(\mathrm{Cl}_{2} \mathrm{O}_{7}\) to be more reactive toward \(\mathrm{H}^{+}(a q)\) or \(\mathrm{OH}^{-}(a q) ?(\mathbf{d})\) If the oxygen in \(\mathrm{Cl}_{2} \mathrm{O}_{7}\) is considered to have the -2 oxidation state, what is the oxidation state of the \(\mathrm{Cl}\) ? What is the electron configuration of \(\mathrm{Cl}\) in this oxidation state?
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