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Chapter 2: Problem 39

For each of the following elements, write its chemical symbol, determine the name of the group to which it belongs (Table 2.3 ), and indicate whether it is a metal, metalloid, or nonmetal: (a) potassium, (b) iodine, (c) magnesium, (d) argon, (e) sulfur.

Short Answer

Expert verified
(a) Potassium: K, Alkali Metals (Group 1), Metal. (b) Iodine: I, Halogens (Group 17), Nonmetal. (c) Magnesium: Mg, Alkaline Earth Metals (Group 2), Metal. (d) Argon: Ar, Noble Gases (Group 18), Nonmetal. (e) Sulfur: S, Chalcogens (Group 16), Nonmetal.

Step by step solution

01

(a) Potassium

Potassium's chemical symbol is 'K'. It belongs to Group 1, also known as Alkali Metals. Potassium is classified as a metal.
02

(b) Iodine

Iodine's chemical symbol is 'I'. It belongs to Group 17, also known as Halogens. Iodine is classified as a nonmetal.
03

(c) Magnesium

Magnesium's chemical symbol is 'Mg'. It belongs to Group 2, also known as Alkaline Earth Metals. Magnesium is classified as a metal.
04

(d) Argon

Argon's chemical symbol is 'Ar'. It belongs to Group 18, also known as Noble Gases. Argon is classified as a nonmetal.
05

(e) Sulfur

Sulfur's chemical symbol is 'S'. It belongs to Group 16, also known as Chalcogens. Sulfur is classified as a nonmetal.

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Most popular questions from this chapter

(a) What isotope is used as the standard in establishing the atomic mass scale? (b) The atomic weight of boron is reported as 10.81 , yet no atom of boron has the mass of 10.81 amu. Explain.

Gallium (Ga) consists of two naturally occurring isotopes with masses of 68.926 and 70.925 amu. (a) How many protons and neutrons are in the nucleus of each isotope? Write the complete atomic symbol for each, showing the atomic number and mass number. (b) The average atomic mass of Ga is 69.72 amu. Calculate the abundance of each isotope.

A cube of gold that is \(1.00 \mathrm{~cm}\) on a side has a mass of \(19.3 \mathrm{~g} . \mathrm{A}\) single gold atom has a mass of 197.0 amu. (a) How many gold atoms are in the cube? (b) From the information given, estimate the diameter in \(\AA\) of a single gold atom. (c) What assumptions did you make in arriving at your answer for part (b)?

The radius of an atom of gold \((\mathrm{Au})\) is about \(1.35 \AA\). (a) \(\mathrm{Ex}\) press this distance in nanometers (nm) and in picometers (pm). (b) How many gold atoms would have to be lined up to span \(1.0 \mathrm{~mm} ?\) (c) If the atom is assumed to be a sphere, what is the volume in \(\mathrm{cm}^{3}\) of a single Au atom?

The element lead (Pb) consists of four naturally occurring isotopes with atomic masses 203.97302,205.97444,206.97587 , and 207.97663 amu. The relative abundances of these four isotopes are 1.4,24.1,22.1 , and \(52.4 \%\), respectively. From these data, calculate the atomic weight of lead.
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