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Chapter 3: Problem 61

What element seems poorly placed in group IA (1), the alkali metals? Why?

Short Answer

Expert verified
Hydrogen (H) seems to be poorly placed in Group IA (1), the alkali metals, because it is a non-metal with high ionization energy and electronegativity, unlike other alkali metals. Although it shares the property of having one electron in its outermost shell, its overall properties significantly differ from those of alkali metals.

Step by step solution

01

Identify the elements in Group IA (1)

To find the poorly placed element, first, we must know the elements in Group IA (1). Group IA consists of the following elements: Hydrogen (H), Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb), Cesium (Cs), and Francium (Fr).
02

Evaluate the properties of alkali metals

Alkali metals have certain properties in common which include: 1. They are soft metals that can be cut easily. 2. They are highly reactive, especially with water and oxygen. 3. They have one valence electron in the outermost shell. 4. They have low ionization energy and electronegativity.
03

Compare the properties of elements in Group IA (1)

Now, let's compare the properties of the elements in Group IA (1) to find the poorly placed element: 1. Hydrogen is a non-metal and exists as a diatomic gas, while other alkali metals are soft metals. 2. Hydrogen is reactive, but its reactivity is quite different from other alkali metals. 3. Hydrogen has one electron in its outermost shell, so it shares this property with alkali metals. 4. Hydrogen has a high ionization energy and electronegativity, in contrast to alkali metals.
04

Determine the poorly placed element and explain the reason

Based on the comparison of properties, Hydrogen (H) seems to be poorly placed in Group IA (1), the alkali metals. The reason for this is because hydrogen is a non-metal, and its ionization energy and electronegativity are very different from the properties of other alkali metals. Although it shares the property of having one electron in its outermost shell, its overall properties significantly differ from those of alkali metals.

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Most popular questions from this chapter

Scandium (Sc) is a metal that tends to lose three electrons. Copper (Cu) and zinc \((Z n)\) are also metals that tend to lose one and two electrons, respectively. Knowing this, explain why the first group in the transition metals is numbered IIIB, whereas the last two groups in the transition series are numbered IB and IIB, respectively.

Why is the atomic mass of carbon not listed as 12 on the periodic table if the universal standard is that \({ }_{6}^{12} \mathrm{C}\) has an atomic mass of exactly 12 amu?

Atom A has 35 protons and 44 neutrons in its nucleus. Atom \(\mathrm{B}\) has 35 protons and 46 neutrons in its nucleus. Should we expect similar or different chemical properties for these atoms? Explain.

Calcium reacts with fluorine to form the compound \(\mathrm{CaF}_{2}\). In the reaction, each atom of one of the elements loses two electrons, and each atom of the other element gains one electron. (a) Atoms of which element gain electrons? (b) Atoms of which element lose electrons? (c) What is the charge on the atoms that gain one electron? (d) What is the charge on the atoms that lose two electrons? (e) Write the full atomic symbol, including charges, for each element. Give Ca 20 neutrons and F 10 neutrons.

Fill in the following table: $$ \begin{array}{lcccc} & { }_{8}^{15} \mathrm{O}^{+} & ? & ? & ? \\ \hline \text { Mass number } & ? & 27 & ? & 58 \\ \text { Atomic number } & ? & ? & 15 & ? \\ \text { Number of protons } & ? & 13 & ? & ? \\ \text { Number of neutrons } & ? & ? & 16 & 30 \\ \text { Number of electrons } & ? & ? & ? & 27 \\ \text { Charge on ion } & ? & +3 & -3 & +1 \\ \hline \end{array} $$
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