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Chapter 8: Problem 135

Match each of the elements on the right with its description on the left: (a) A pale yellow gas that reacts with water. (b) A soft metal that reacts with water to produce hydrogen. (c) A metalloid that is hard and has a high melting point. (d) A colorless, odorless gas. (e) A metal that is more reactive than iron, but does not corrode in air. Nitrogen \(\left(\mathrm{N}_{2}\right)\) Boron (B) Aluminum (Al) Fluorine \(\left(\mathrm{F}_{2}\right)\) Sodium (Na)

Short Answer

Expert verified
(a) Fluorine \(\left(\mathrm{F}_{2}\right)\), (b) Sodium (Na), (c) Boron (B), (d) Nitrogen \(\left(\mathrm{N}_{2}\right)\), (e) Aluminum (Al).

Step by step solution

01

Match elements with properties

Firstly, let's go through each element one by one and match its properties with the descriptions given. \n\n- Nitrogen \(\left(\mathrm{N}_{2}\right)\): This is a colourless, odourless gas, so it matches with description (d).\n- Boron (B): Boron is a metalloid, hard and has a high melting point, so it matches with description (c). \n- Aluminum (Al): This is a metal that is more reactive than iron but does not corrode in air. It matches description (e).\n- Fluorine \(\left(\mathrm{F}_{2}\right)\): Fluorine is a pale yellow gas that reacts with water, so it matches with description (a). \n- Sodium (Na): This is a soft metal that reacts with water to produce hydrogen. This matches with description (b).
02

Final Matching

Now, let's finalize the matches as per our analysis: \n\n(a) Fluorine \(\left(\mathrm{F}_{2}\right)\) \n(b) Sodium (Na) \n(c) Boron (B) \n(d) Nitrogen \(\left(\mathrm{N}_{2}\right)\)\n(e) Aluminum (Al).

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Most popular questions from this chapter

When magnesium metal is burned in air, it forms two products \(A\) and \(B\). A reacts with water to form a basic solution. B reacts with water to form a similar solution as that of A plus a gas with a pungent odor. Identify A and \(\mathrm{B}\) and write equations for the reactions. (Hint: See Chemistry in Action essay "Discovery of the Noble Gases" in Section \(8.6 .\) )

Write the formulas and names of the oxides of the second-period elements (Li to \(\mathrm{N}\) ). Identify the oxides as acidic, basic, or amphoteric.

How does atomic radius change (a) from left to right across a period and (b) from top to bottom in a group?

The ionization energies of sodium (in \(\mathrm{kJ} / \mathrm{mol}\) ), starting with the first and ending with the eleventh, are 495.9,4560,6900,9540,13,400,16,600,20,120 \(25,490,28,930,141,360,170,000 .\) Plot the \(\log\) of ionization energy ( \(y\) axis) versus the number of ionization \((x\) axis \() ;\) for example, log 495.9 is plotted versus 1 (labeled \(I E_{1}\), the first ionization energy), \(\log 4560\) is plotted versus 2 (labeled \(I E_{2}\), the second ionization energy), and so on. (a) Label \(I E_{1}\) through \(I E_{11}\) with the electrons in orbitals such as \(1 s, 2 s, 2 p\) and \(3 s .\) (b) What can you deduce about electron shells from the breaks in the curve?

An element X reacts with hydrogen gas at \(200^{\circ} \mathrm{C}\) to form compound Y. When \(Y\) is heated to a higher temperature, it decomposes to the element \(X\) and hydrogen gas in the ratio of \(559 \mathrm{~mL}\) of \(\mathrm{H}_{2}\) (measured at STP) for \(1.00 \mathrm{~g}\) of \(\mathrm{X}\) reacted. \(\mathrm{X}\) also combines with chlorine to form a compound \(Z,\) which contains 63.89 percent by mass of chlorine. Deduce the identity of \(X\).
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