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Chapter 22: Problem 21

Give a reason why hydrogen might be placed along with the group lA elements of the periodic table.

Short Answer

Expert verified
Hydrogen might be placed along with the group 1A elements in the periodic table because it shares similar properties, such as having one electron in the outermost shell, a valency of 1, and the ability to form positively-charged ions (cations) by losing this electron. The reactivity of hydrogen also resembles that of the group 1A elements.

Step by step solution

01

Identify properties of hydrogen

Hydrogen is the first element in the periodic table and has one electron in its outermost shell (1s1 configuration). It has a valency of 1 and forms a single covalent bond with other elements to achieve a stable configuration. Hydrogen can also lose this electron to form a positively-charged hydrogen ion (H+).
02

Identify properties of group 1A elements

Elements in group 1A of the periodic table (alkali metals) have one electron in their outermost shell (ns1 configuration, where n is the principal quantum number). They have a valency of 1 and are highly reactive, losing this electron to form positively-charged ions (cations).
03

Compare hydrogen to group 1A elements

Hydrogen and group 1A elements share the same valence electron configuration (having one electron in their outermost shell). They both have a valency of 1 and can form positively-charged ions by losing this electron. Their reactivity also arises from the desire to lose one electron and achieve a stable electronic configuration.
04

Reason for placing hydrogen in group 1A

Hydrogen might be placed along with the group 1A elements in the periodic table because it shares similar properties, such as having one electron in the outermost shell, a valency of 1, and the ability to form positively-charged ions (cations) by losing this electron. The reactivity of hydrogen also resembles that of the group 1A elements.

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Most popular questions from this chapter

Explain the following observations: (a) The highest fluoride compound formed by nitrogen is \(\mathrm{NF}_{3}\), whereas phosphorus readily forms \(\mathrm{PF}_{5}\). (b) Although \(\mathrm{CO}\) is a well-known compound, SiO does not exist under ordinary conditions. (c) \(\mathrm{AsH}_{3}\) is a stronger reducing agent than \(\mathrm{NH}_{3} .\)

Write the chemical formula for each of the following, and indicate the oxidation state of the halogen or noble-gas atom in each: (a) calcium hypobromite, (b) bromic acid, (c) xenon trioxide, (d) perchlorate ion, (e) iodous acid, (f) iodine pentafluoride.

Give the chemical formula for (a) hydrocyanic acid, (b) nickel tetracarbonyl, (c) barium bicarbonate, (d) calcium acetylide (e) potassium carbonate.

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Complete and balance the following equations: (a) \(\mathrm{CO}_{2}(g)+\mathrm{OH}^{-}(a q) \longrightarrow\) (b) \(\mathrm{NaHCO}_{3}(s)+\mathrm{H}^{+}(a q) \longrightarrow\) (c) \(\mathrm{CaO}(s)+\mathrm{C}(s) \stackrel{\Delta}{\longrightarrow}\) (d) \(\mathrm{C}(s)+\mathrm{H}_{2} \mathrm{O}(g) \stackrel{\Delta}{\longrightarrow}\) (e) \(\mathrm{CuO}(s)+\mathrm{CO}(g) \longrightarrow\)
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