![]() The metals above hydrogen will react with aqueous hydrogen ion to form hydrogen gas. ![]() Notice the position of hydrogen in the activity series. The aluminum is a stronger reducing agent than silver and will reduce the Ag + ion to solid Ag.ģ Ag 2S (s) + 2 Al(s) → 6 Ag (s) + Al 2S 3 (s) Tarnish can be removed chemically with aluminum. Silver tarnishes according to the following reaction with H 2S gas.Ģ Ag (s) + H 2S (gas) → Ag 2S (s) + H 2 (g)Ĭommercial silver polishes will remove the tarnish from silver, but some of the silver is lost because these polishes are abrasive. Chromium can reduce Cu 2+ ion, but it cannot reduce Mn 2+. A metal can reduce any ion below it in the series. For example, zinc is a weaker reducing agent than sodium, but it is a stronger reducing agent than copper. Gold is at the end of the list and is not as easily oxidized and is therefore the weakest reducing agent on this activity series.īoth the ease of oxidation and the reducing strength of the metals decrease going down the column. Lithium is at the top of the list and is the most easily oxidized metal which means it is the strongest reducing agent in the activity series below. Below is a table of a partial activity series for metals in aqueous solution. ![]() Metals are strong reducing agents, but their reducing power decreases going across a period of the periodic table. This means metals lose electrons more easily than nonmetals. ![]() Metals are more easily oxidized than nonmetals. ![]()
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