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Chapter 8: Problem 6

Compare the physical and chemical properties of metals and nonmetals.

Short Answer

Expert verified
The physical and chemical properties of metals and nonmetals differ greatly. Metals typically have a shiny appearance, are malleable, have high melting and boiling points, and are good conductors of electricity and heat. They also usually react with oxygen to form basic oxides. Nonmetals, in contrast, lack a metallic shine, are brittle, have low melting and boiling points, are poor conductors, and form acidic oxides when they react.

Step by step solution

01

Appearance

Begin by describing the appearance. Most metals have a shiny appearance, since they're good reflectors of light. Nonmetals, on the other hand, lack this metallic shine, and can appear dull or even transparent.
02

Melting and Boiling Points

Next, compare melting and boiling points. Generally, metals have high melting and boiling points, excluding mercury which is a liquid at room temperature. Nonmetals typically have lower melting and boiling points, and, at room temperature, they can exist as solids, liquids, or gases
03

Malleability

Discuss malleability. Metals are malleable (they can be beaten into thin sheets). Nonmetals are not malleable; instead, they are typically brittle.
04

Conductivity

Discuss conductivity. Metals are good conductors of electricity and heat, while most nonmetals are poor conductors.
05

Reactivity

Lastly, compare reactivity. Both metals and nonmetals can be reactive, but show reactivity in different ways. Metals often react with oxygen to form basic oxides, while nonmetals will typically form acidic oxides.

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Most popular questions from this chapter

Give the physical states (gas, liquid, or solid) of the representative elements in the fourth period at 1 atm and \(25^{\circ} \mathrm{C}: \mathrm{K}, \mathrm{Ca}, \mathrm{Ga}, \mathrm{Ge}, \mathrm{As}, \mathrm{Se}, \mathrm{Br}\).

Explain what is meant by the diagonal relationship. List two pairs of elements that show this relationship.

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 do we mean when we say that two ions or an atom and an ion are isoelectronic?

Define ionization energy. Ionization energy is usually measured in the gaseous state. Why? Why is the second ionization energy always greater than the first ionization energy for any element?
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