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Chapter 8: Problem 3

Describe the general layout of a modern periodic table.

Short Answer

Expert verified
A modern periodic table is divided into s-, p-, d-, and f-blocks, with elements arranged in increasing order of atomic numbers. Each cell contains an element's chemical symbol, atomic number, and atomic weight, and possibly its state of matter at room temperature. Special groups include alkali metals, alkaline earth metals, halogens, and noble gases, along with transition metals.

Step by step solution

01

Identify the Main Divisions

The modern periodic table is generally divided into 4 blocks: the s-block, the p-block, the d-block, and the f-block. The s-block and p-block collectively form the representative elements (main group), while the d-block forms the transition metals, and the f-block houses the lanthanides and actinides.
02

Understand the Arrangement

Elements within the periodic table are arranged in increasing order according to their atomic numbers. They are placed in specific periods (rows) and groups (columns). There are seven periods and 18 groups in the modern periodic table. The group number signifies the number of valence electrons in an element's outermost shell, whereas the period number indicates the number of shells or energy levels in an atom.
03

Acknowledge the Info within Cell

Each cell or box of the periodic table contains detailed information about an element. This typically includes the element's chemical symbol, atomic number, atomic weight, and (in some versions) other properties such as the element鈥檚 state of matter (solid, liquid, gas) at room temperature.
04

Note the Special Groups

There are specific groups on the periodic table that have given names due to shared properties. These include group 1 (alkali metals), group 2 (alkaline earth metals), group 17 (halogens), and group 18 (noble gases). The elements in groups 3-12 are known as transition metals.

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Most popular questions from this chapter

Write ground-state electron configurations for these transition metal ions: (a) \(\mathrm{Sc}^{3+}\) (b) \(\mathrm{Ti}^{4+}\) (c) \(\mathrm{V}^{5+}\) (d) \(\mathrm{Cr}^{3+}\) , (e) \(\mathrm{Mn}^{2+},\) (f) \(\mathrm{Fe}^{2+}\) (h) \(\mathrm{Co}^{2+}\) (g) \(\mathrm{Fe}^{3+}\) (i) \(\mathrm{Ni}^{2+}\) (i) \(\mathrm{Cu}^{+}\) (k) \(\mathrm{Cu}^{2+}\) (1) \(\mathrm{Ag}^{+}\) \((\mathrm{m}) \mathrm{Au}^{+}\) (n) \(\mathrm{Au}^{3+},\) (o) \(\mathrm{Pt}^{2+}\)

Explain why the first electron affinity of sulfur is \(200 \mathrm{~kJ} / \mathrm{mol}\) but the second electron affinity is \(-649 \mathrm{~kJ} / \mathrm{mol}\),

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 \(I_{1}\), the first ionization energy), log 4560 is plotted versus 2 (labeled \(I_{2}\), the second ionization energy), and so on. (a) Label \(I_{1}\) through \(I_{11}\) 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?

What factors account for the unique nature of hydrogen?

In each of the following pairs, indicate which one of the two species is smaller: (a) \(\mathrm{Cl}\) or \(\mathrm{Cl}^{-},\) (b) Na or \(\mathrm{Na}^{+}\), (c) \(\mathrm{O}^{2-}\) or \(\mathrm{S}^{2-},\) (d) \(\mathrm{Mg}^{2+}\) or \(\mathrm{Al}^{3+},\) (e) \(\mathrm{Au}^{+}\) or \(\mathrm{Au}^{3+}\).
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