Which of the following elements (X) will form a covalent hydride with the formula XH 3 that is a gas at room temperature? (LO 22.4) (a) Al (b) As (c) Ba (d) Se

All right. Hi, everyone. So this question is asking us at room temperature, which element would form a gaseous covalent hydride with the formula A two option A says gallium. Option B says beryllium, option C says sulfur and option D says nitrogen. Now recall a covalent hydride involves two nonmetals, right? Because one other non metal is going to combine with hydrogen via a covalent bond in which electrons are being shared between them. Now, the formula of the hydride itself, meaning the ratio of hydrogen to the other nonmetal depends on the group in which the other nonmetal resides in in the periodic table. No, earlier, I mentioned the fact that covalent hydride must involve two nonmetals. So therefore, I can go ahead and actually eliminate any metals that I happen to have in my answer choices. So gallium and beryllium are going to be removed for this reason. So at this point, we can compare and contrast sulfur and nitrogen to start off recall that sulfur is found in group six a of the periodic table in which it normally has six valence electrons. Now because it has six valence electrons, two more electrons are required to complete its octet. So because of this sulfur generally forms two covalent bonds with other atoms to complete its octet, which means that a hydride that contains sulfur would generally have a chemical formula of HS two or otherwise known as H two S. Now nitrogen, on the other hand, resides in group five a of the periodic table, which means that it has five valence electrons. So therefore, nitrogen generally forms three covalent bonds with other atoms to complete its octet. This means that a hydride containing nitrogen would have a chemical formula of NH three. So based on this right, we can see that it's sulfur that would form a hydride, a gaseous covalent hydride with the formula of HS two because sulfur is capable of forming two covalent bonds due to the fact that it already has six valent electrons. So our answer here is going to be option c in the multiple choice. And with that being said, thank you so very much for watching. And I hope you found this helpful.

Ch.22 - The Main Group Elements

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McMurry 8th Edition

Ch.22 - The Main Group Elements

Problem 22.3

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Chapter 22, Problem 22.3

Which of the following elements (X) will form a covalent hydride with the formula XH₃ that is a gas at room temperature? (LO 22.4)
(a) Al (b) As (c) Ba (d) Se

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Identify the elements that can form covalent bonds with hydrogen to create a hydride.

Consider the periodic table position of each element: Al, As, Ba, and Se.

Recall that covalent hydrides are typically formed by nonmetals or metalloids.

Determine which of the given elements is likely to form a gaseous hydride at room temperature.

Recognize that As (arsenic) is a metalloid that can form a covalent hydride, AsH_3, which is a gas at room temperature.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Covalent Bonding

Covalent bonding occurs when two atoms share one or more pairs of electrons, typically between nonmetals. This type of bond results in the formation of molecules, such as hydrides, where the hydrogen atom bonds with another element. Understanding the nature of covalent bonds is essential for predicting the properties of compounds, including their state at room temperature.

Hydrides

Hydrides are compounds formed between hydrogen and another element. They can be classified into ionic and covalent hydrides, with covalent hydrides being formed by nonmetals. The physical state of hydrides at room temperature can vary; for instance, covalent hydrides of lighter nonmetals tend to be gases, while those of heavier elements may be liquids or solids.

Periodic Trends

Periodic trends refer to the predictable patterns in the properties of elements as you move across or down the periodic table. These trends influence factors such as electronegativity, atomic size, and the ability to form covalent bonds. Recognizing these trends helps in determining which elements are likely to form gaseous hydrides, as lighter elements in specific groups tend to form such compounds.

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Periodic Trends

Related Practice

Look at the location of elements A, B, C, and D in the following periodic table:

(e) Which of these oxides has the highest melting point? Which has the lowest melting point?

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Textbook Question

Consider the six second- and third-row elements in groups 4A–6A of the periodic table:

Possible structures for the binary fluorides of each of these elements in its highest oxidation state are shown below.

(a) Identify the nonfluorine atom in each case, and write the molecular formula of each fluoride.

117

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Textbook Question

Consider the six second- and third-row elements in groups 4A–6A of the periodic table:

Possible structures for the binary fluorides of each of these elements in its highest oxidation state are shown below.

(b) Explain why the fluorides of nitrogen and phosphorus have different molecular structures but the fluorides of carbon and silicon have the same molecular structure.

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Textbook Question

The following pictures represent various silicate anions. Write the formula and charge of each anion.

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Textbook Question

Which element in each of the following pairs has more nonmetallic character?

(a) Se or Te

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Textbook Question

Which compound in each of the following pairs is more ionic?

(b) P4O6 or Ga2O3