Identify the species oxidized and the species reduced?
a.) 3Cu(s) + 2Au(NO3)3(aq)--->3Cu(NO3)2(aq) + 2Au(s) reduced: oxidized: b.) Mg(s) + Ni(NO3)2(aq)---> Mg(NO3)2(aq) + Ni(s) reduced: oxidized:
How do I identify the reducing agent in a reaction of magnesium with oxygen?
The reducing agent is the substance that is oxidized, in this case the Mg. Mg loses 2 electrons to O, reducing O to O-2. Since Mg caused this reduction, it is the reducing agent.
Is nitric acid a strong oxidizing agent?
Oxidizing propertiesNitric acid is a strong oxidizing agent as shown by its large positive E◦ values.NO3- (aq) + 2H+ (aq) e- → NO2 (g) + H2O (l) E◦ = 0.79 VNO3- (aq) + 4H+ + 3e- → NO (g) 2H2 (l) E◦ = 0.96 VBeing a powerful oxidizing agent, nitric acid reacts violently with many non-metallic compounds and the reactions may be explosive. Depending on the acid concentration, temperature and the reducing agent involved, the end products can be variable. Reaction takes place with all metals except the precious metal series and certain alloys. As a general rule, oxidizing reactions occur primarily with the concentrated acid, favoring the formation of nitrogen dioxide (NO2).Reactions with metalsNitric acid dissolves most metals including iron, copper, and silver, with generally the liberation of lower oxides of nitrogen rather than hydrogen. It can also dissolve the noble metals with the addition of hydrochloric acid.Cu + 4HNO3 → Cu(NO3)2 + 2NO2 + 2H2OThe acidic properties tend to dominate with dilute acid, coupled with the preferential formation of nitrogen oxide (NO).3Cu + 8HNO3 → 3Cu(NO3)2 + 2NO + 4H2OSince nitric acid is an oxidizing agent, hydrogen (H) is rarely formed. Only magnesium (Mg) and calcium (Ca) react with cold, dilute nitric acid to give hydrogen:Mg(s) + 2HNO3 (aq) → Mg(NO3)2 (aq) + H2 (g)Reactions with nonmetalsReaction with non-metallic elements, with the exception of silicon and halogen, usually oxidizes them to their highest oxidation states as acids with the formation of nitrogen dioxide for concentrated acid and nitrogen oxide for dilute acid.C + 4HNO3 → CO2 + 4NO2 + 2H2Oor3C + 4HNO3 → 3CO2 + 4NO + 2H2OPassivationAlthough chromium (Cr), iron (Fe), and aluminum (Al) readily dissolve in dilute nitric acid, the concentrated acid forms a metal oxide layer that protects the metal from further oxidation, which is called passivation
Why is Cr²⁺ is a good reducing agent but Mn³⁺ is a good oxidising agent?
[math]Cr^{2+}[/math] - [math]d^{4}[/math] configuration gets converted to [math]Cr^{3+}[/math] - [math]d^{3}[/math] has half-filled [math]t_{2g}[/math] orbital makes it good reducing agent while In case of [math]Mn^{3+}[/math] - [math]d^{4}[/math] Configuration gets converted to [math]Mn^{2+}[/math] - [math]d^{5}[/math] configuration giving half –filled d-configuration has more stability which makes it good oxidising agent.Edit: [math]Cr^{2+}[/math] gives negative CFSE while [math]Cr^{+}[/math] having Zero CFSE makes it less stable compared to [math]Cr^{2+}[/math].In case of Mn, it always forms low spin complexes. So, it will have more negative CFSE in case of [math]Mn^{2+}[/math] than [math]Mn^{3+}[/math] .[math]Mn^{4+}[/math] is highly charged which make it unstable and highly oxidising.
I need a feature article on earths structure does anybody have one?!?
http://scign.jpl.nasa.gov/learn/plate1.h...
How can you prove that oxygen is needed for burning?
Burning candle.Cup.Put cup over candle.There is oxygen inside the cup, but in a limited amount.Flame out.Also, carbon is from the fuel and oxygen is the oxidiser, with the waste, carbon mon/dioxide as supporting evidence. Magnesium can burn too, magnesium oxide is its product and the Earth’s surface and atmosphere is not hot enough for gaseous carbon to exist naturally (supporting that oxygen is not from fuels and carbon is not the ambient oxidiser), suggesting that not only is oxygen crucial for a flame, but even more important than the fuel’s elements, for multiple elements can burn with oxygen and heat.Well, there is such thing as a fluorine fire, but still, in most contexts, oxygen is needed.
Do all metals react with hydrochloric acid to produce hydrogen?
For a metal to react with an acid to form a salt and hydrogen gas, it has to be above hydrogen in the electrochemical series (ECS). The Electrochemical Series is a list of elements in order of their reactivity (high to low). The list is as follows: Potassium(most reactive), Sodium, Calcium, Magnesium, Aluminium, Zinc, Carbon, Iron, Tin, Hydrogen, Lead, Copper, Silver, gold(least reactive) In your experiment, the Magnesium reacted most vigorously hence producing a lot of Hydrogen gas, which when lit with a glowing splint burned with a pop. Mg + 2HCl ------------------->MgCl2 + H2 Zinc should also have produced hydrogen gas quickly, however not as quickly or vigorously as Magnesium. Maybe a smaller amount of zinc was used in the experiment - hence the proportion of Hydrogen gas produced would be less. Zn + 2HCl --------------------> ZnCl2 + H2 Aluminium should also produce hydrogen gas when reacted with HCl acid, however the aluminium may have been coated in Aluminium Oxide (due to corrosion with oxygen in the air). This coating has to be dissolved by the Hydrochloric Acid before the main reaction proceeds. So the reaction takes longer to start but when it does it will produce Hydrogen gas. To dissolve the Al2O3 (aluminium oxide coating the aluminium metal) Al2O3 + 6HCl---------------------------> 2AlCl3 + 3H2O The main reaction then is: 2Al + 6HCl -----------------------> 2AlCl3 + 3H2 Finally Copper will not react with Hydrochloric Acid to produce Hydrogen gas as it is below Hydrogen in the Electrochemical Series.
What is sodium? For example, what is it made of and what it is used for.?
Sodium is an element made of 100% sodium. You seldom see it by itself, as it will spontaneously ignite on contact with the oxygen in the air. It combines with almost everything including chlorine to make sodium chloride, common salt. Try wikipedia to learn more