YES or NO - would you be able to conduct electricity, bend, shape and flatten any elements in group 18?
Answers
Answer:
I think YES....YES.
Explanation:
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Answer: All elements except hydrogen, which form positive ions by losing electrons during chemical reactions are called metals. Thus metals are electropositive elements. They are characterized by bright luster, hardness, ability to resonate sound and are excellent conductors of heat and electricity. Metals are solids under normal conditions except for Mercury.
Physical Properties of Metals
Metals are lustrous, malleable, ductile, good conductors of heat and electricity. Other properties include:
State: Metals are solids at room temperature with the exception of mercury, which is liquid at room temperature (Gallium is liquid on hot days).
Luster: Metals have the quality of reflecting light from its surface and can be polished e.g., gold, silver and copper.
Malleability: Metals have the ability to withstand hammering and can be made into thin sheets known as foils (a sugar cube chunk of gold can be pounded into a thin sheet which will cover a football field).
Ductility: Metals can be drawn into wires. 100 gm of silver can be drawn into a thin wire about 200 meters long.
Hardness: All metals are hard except sodium and potassium, which are soft and can be cut with a knife.
Valency: Metals have 1 to 3 electrons in the outermost shell of their atoms.
Conduction: Metals are good conductors because they have free electrons. Silver and copper are the two best conductors of heat and electricity. Lead is the poorest conductor of heat. Bismuth, mercury and iron are also poor conductors
Density: Metals have high density and are very heavy. Iridium and osmium have the highest densities where as lithium has the lowest density.
Melting and Boiling Points: Metals have high melting and boiling point. Tungsten has the highest melting point where as silver has low boiling point. Sodium and potassium have low melting points.
Chemical Properties of Metals
Metals are electropositive elements that generally form basic or amphoteric oxides with oxygen. Other chemical properties include:
Electropositive Character: Metals tend to have low ionization energies, and typically lose electrons (i.e. are oxidized) when they undergo chemical reactions They normally do not accept electrons. For example:
Na0→Na++e−(2.11.1)
Mg0→Mg2++2e−(2.11.2)
Al0→Al3++3e−(2.11.3)
Alkali metals are always 1+ (lose the electron in s subshell)
Alkaline earth metals are always 2+ (lose both electrons in s subshell)
Transition metal ions do not follow an obvious pattern, 2+ is common, and 1+ and 3+ are also observed
Compounds of metals with non-metals tend to be ionic in nature
Most metal oxides are basic oxides and dissolve in water to form metal hydroxides:
Metal oxide + water -> metal hydroxide
Na2O(s) + H2O(l) -> 2NaOH(aq)
CaO(s) + H2O(l) -> Ca(OH)2(aq)
Metal oxides exhibit their basic chemical nature by reacting with acids to form salts and water:
Metal oxide + acid -> salt + water
MgO(s) + HCl(aq) -> MgCl2(aq) + H2O(l)
NiO(s) + H2SO4(aq) -> NiSO4(aq) + H2O(l)
Explanation: