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Chapter 8: Problem 5

Which of these elements are metals, nonmetals, and metalloids: \(\mathrm{As}, \mathrm{Xe}, \mathrm{Fe}, \mathrm{Li}, \mathrm{B}, \mathrm{Cl}, \mathrm{Ba}, \mathrm{P}, \mathrm{I}, \mathrm{Si} ?\)

Short Answer

Expert verified
Arsenic, Boron, and Silicon are metalloids; Xenon, Chlorine, Phosphorus, and Iodine are nonmetals; Iron, Lithium, and Barium are metals.

Step by step solution

01

Identify element type for Arsenic (As)

Looking at the periodic table, Arsenic (As) is found under metalloids, so it is a metalloid.
02

Identify element type for Xenon (Xe)

Locating Xenon (Xe) on the periodic table, it falls under the noble gases which are nonmetals, so it's a nonmetal.
03

Identify element type for Iron (Fe)

Iron (Fe) is located under metals on the periodic table, so it's a metal.
04

Identify element type for Lithium (Li)

Lithium (Li) is found under alkali metals on the periodic table, so it's a metal.
05

Identify element type for Boron (B)

According to the periodic table, Boron (B) is a metalloid.
06

Identify element type for Chlorine (Cl)

Chlorine (Cl) falls under halogens on the periodic table which are nonmetals, so it's a nonmetal.
07

Identify element type for Barium (Ba)

Using the periodic table, Barium (Ba) is found under alkaline earth metals, so it's a metal.
08

Identify element type for Phosphorus (P)

Phosphorus (P) falls under nonmetals on the periodic table, so it's a nonmetal.
09

Identify element type for Iodine (I)

Iodine (I) is located under halogens which are nonmetals, so it's a nonmetal.
10

Identify element type for Silicon (Si)

Silicon (Si) is found under metalloids on the periodic table, so it's a metalloid.

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Most popular questions from this chapter

Little is known of the chemistry of astatine, the last member of Group \(7 \mathrm{~A}\). Describe the physical characteristics that you would expect this halogen to have. Predict the products of the reaction between sodium astatide (NaAt) and sulfuric acid. (Hint: Sulfuric acid is an oxidizing agent.).

Define valence electrons. For representative elements, the number of yalence electrons of an element is equal to its group number. Show that this is true for the following elements: \(\mathrm{Al}, \mathrm{Sr}, \mathrm{K}, \mathrm{Br}, \mathrm{P}, \mathrm{S}, \mathrm{C}\).

In the late 1800 s the British physicist Lord Rayleigh accurately determined the atomic masses of a number of elements, but he obtained a puzzling result with nitrogen. One of his methods of preparing nitrogen was by the thermal decomposition of ammonia: \( 2 \mathrm{NH}_{3}(g) \longrightarrow \mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \) Another method was to start with air and remove oxygen, carbon dioxide, and water vapor from it. Invariably, the nitrogen from air was a little denser (by about 0.5 percent) than the nitrogen from ammonia. Later the English chemist Sir William Ramsay carried out an experiment in which he passed nitrogen, which he had obtained from air by Raleigh's procedure, over red-hot magnesium to convert it to magnesium nitride: \(3 \mathrm{Mg}(s)+\mathrm{N}_{2}(g) \longrightarrow \mathrm{Mg}_{3} \mathrm{~N}_{2}(s)= \)= After all of the nitrogen had reacted with magnesium, Ramsay was left with an unknown gas that would not combine with anything. The atomic mass of this gas was determined to be 39.95 amu. Ramsay called the gas argon, which means "the lazy one" in Greek. (a) Later Rayleigh and Ramsay, with the help of Sir William Crookes, the inventor of the discharge tube, showed that argon was a new element. Describe the type of experiment performed that led them to the conclusion. (b) Why did it take so long to discover argon? (c) Once argon had been discovered, why did it take relatively little time to discover the rest of the noble gases? (d) Why was helium the last noble gas to be discovered on Earth? (e) The only confirmed compound of radon is radon fluoride, \(\mathrm{RnF}\). Give two reasons why there are so few known radon compounds.

Write the outer electron contigurations for (a) the alkali metals, (b) the alkaline earth metals, (c) the halogens, (d) the noble gases.

Why do elements that have high ionization energies usually have more positive electron affinities?
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