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Chapter 9: Problem 74

In your own words, define the following terms: (a) isoelectronic; (b) valence- shell electrons; (c) metal; (d) nonmetal; (e) metalloid.

Short Answer

Expert verified
(a) Isoelectronic refers to two different entities having identical electron configurations. (b) Valence-shell electrons are in the outermost shell of an atom and determine its chemical reactivity. (c) A metal is a substance with properties like luster, good conduction of heat and electricity, malleability, and ductility. (d) Nonmetals are opposite to metals, generally poor conductors of heat and electricity. (e) Metalloids have properties intermediate between metals and nonmetals.

Step by step solution

01

Define Isoelectronic

The term 'isoelectronic' refers to two different atoms, ions, or molecules that have identical electron configurations, that is, the same number of electrons and the same structure of their electron shells.
02

Define Valence-shell Electrons

Valence-shell electrons refer to the electrons in the outermost shell of an atom. These electrons play a key role in determining the chemical behavior and reactivity of an element.
03

Define Metal

A metal is a substance that generally is lustrous, good conductor of heat and electricity, malleable, and ductile. Metals tend to lose electrons during chemical reactions, forming positive ions.
04

Define Nonmetal

Nonmetals are elements that are generally poor conductors of heat and electricity, and tend not to form positive ions in their chemical reaction. Nonmetals usually have properties opposite to those of metals.
05

Define Metalloid

Metalloids are elements with properties intermediate between metals and nonmetals. They can have the appearance of metals, but like nonmetals, they are poor conductors of heat and electricity. Silicon and germanium are examples of metalloids.

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Most popular questions from this chapter

The element whose atoms have the electron configuration \([\mathrm{Kr}] 4 d^{10} 5 \mathrm{s}^{2} 5 p^{3}(\mathrm{a})\) is in group 13 of the periodic table; (b) bears a similarity to the element Bi; (c) is similar to the element \(\mathrm{Te} ;\) (d) is a transition element.

All the isoelectronic species illustrated in the text had the electron configurations of noble gases. Can two ions be isoelectronic without having noble-gas electron configurations? Explain.

Listed below are two atomic properties of the element germanium. Refer only to the periodic table on the inside front cover and indicate probable values for each of the following elements, expressed as greater than, about equal to, or less than the value for Ge. $$\begin{array}{lcc} \hline \text { Element } & \text { Atomic Radius } & \begin{array}{c} \text { First lonization } \\ \text { Energy } \end{array} \\ \hline \mathrm{Ge} & 122 \mathrm{pm} & 762 \mathrm{kJ} / \mathrm{mol} \\ \mathrm{Al} & ? & ? \\ \mathrm{In} & ? & ? \\ \mathrm{Se} & ? & ? \\ \hline \end{array}$$

Write electron configurations consistent with the following data on numbers of unpaired electrons: \(\mathrm{Ni}^{2+}, 2 ; \mathrm{Cu}^{2+}, 1 ; \mathrm{Cr}^{3+}, 3.\)

Plot a graph of the square roots of the ionization energies versus the nuclear charge for the two series \(\mathrm{Li}, \mathrm{Be}^{+}, \mathrm{B}^{2+}, \mathrm{C}^{3+},\) and \(\mathrm{Na}, \mathrm{Mg}^{+}, \mathrm{Al}^{2+}, \mathrm{Si}^{3+} .\) Explain the observed relationship with the aid of Bohr's expression for the binding energy of an electron in a one electron atom.
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