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Chapter 9: Problem 92

Arrange the following elements in order of decreasing metallic character: $\mathrm{Sc}, \mathrm{Fe}, \mathrm{Rb}, \mathrm{Br}, \mathrm{O}, \mathrm{Ca}, \mathrm{F}, \mathrm{Te}.$

Short Answer

Expert verified
The elements arranged in order of decreasing metallic character are: \( \mathrm{Rb}, \mathrm{Ca}, \mathrm{Sc}, \mathrm{Fe}, \mathrm{Te}, \mathrm{Br}, \mathrm{O}, \mathrm{F} \).

Step by step solution

01

Identify the position of each element on the periodic table

First, find each element in the periodic table and assess its position relative to others. Sc (Scandium) belongs to group 3, period 4. Fe (Iron) is in group 8, period 4. Rb (Rubidium) is in group 1, period 5. Br (Bromine) is in group 17, period 4. O (Oxygen) is in group 16, period 2. Ca (Calcium) is in group 2, period 4. F (Fluorine) is in group 17, period 2. Te (Tellurium) is in group 16, period 5.
02

Apply the rules of periodic trends

We know that the metallic character decreases from left to right across a period and increases from top to bottom in a group. Order them accordingly.
03

Order the elements

Following these periodic trends, the final arrangement in order of decreasing metallic character is: Rb (Rubidium), Ca (Calcium), Sc (Scandium), Fe (Iron), Te (Tellurium), Br (Bromine), O (Oxygen), F (Fluorine).

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Most popular questions from this chapter

Refer only to the periodic table on the inside front cover and indicate which of the atoms, \(\mathrm{Bi}, \mathrm{S}, \mathrm{Ba}, \mathrm{As}\) and \(\mathrm{Ca},\) (a) is most metallic; (b) is most nonmetallic; (c) has the intermediate value when the five are arranged in order of increasing first ionization energy.

Compare the elements \(\mathrm{Na}, \mathrm{Mg}, \mathrm{O},\) and \(\mathrm{P}.\) (a) Place the elements in order of increasing ionization energy. (b) Place the elements in order of increasing electron affinity.

Consider a nitrogen atom in the ground state and comment on whether the following statements are true or false. (a) \(\mathrm{Z}_{\text {eff }}\) for an electron in a 2 s orbital is greater than that for the 1 s orbital. (b) The \(Z_{\text {eff for the } 2 p \text { and } 2 s \text { orbitals is the same. }}\) (c) More energy is required to remove an electron from a 2 s orbital than from the \(2 p\) orbital. (d) The 2 s electron is less shielded than the \(2 p\) electron.

Briefly describe each of the following ideas or phenomena: (a) the periodic law; (b) ionization energy; (c) electron affinity; (d) paramagnetism.

In estimating the boiling point and melting point of bromine in Example \(9-5,\) could we have used Celsius or Fahrenheit instead of Kelvin temperature? Explain.
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