Fill in the blanks, word bank is provided:Compounds of elements in high oxidation states tend to act as a(n) _____ and _____ in chemical reactions.Give two examples: _____ and ______Compounds of elements in low oxidation states tend to act as a(n) _____ and _____ in chemical reactions.Give two examples:Word Bank:- become oxidized- oxidizing agent- become solvated- reducing agent- become reduced- change coordination- solvent- ClO4-, MnO, Cu2O, Mg, Cr2O72-, CrO3, MnO4-, TiO

Why is it that when something gains electrons, it is said to be reduced? What is being reduced?

If electricity of sufficient voltage is passed into a solution of potassium iodide in water, a reaction takes place in which elemental hydrogen gas and elemental iodine are produced, leaving a solution of potassium hydroxide. Write the unbalanced equation for this process.

Write equations for respiration and photosynthesis. For each reaction, label the substances that are oxidized and reduced. Why are these reactions important?

. For each of the following unbalanced oxidation-reduction chemical equations, balance the equation by inspection, and identify which species is the reducing agent. a.Fe(s)+O2(g)Fe2O3(s)b.Al(s)+Cl2(g)AlCl3(s)c.Mg(s)+P4(s)Mg3P2(s)

In an ordinary flashlight battery, an oxidation reaction and a reduction reaction rake place at different locations to produce an electric current that consists of electrons. In one of the reactions, the zinc container of the battery slowly dissolves as it is converted into zinc ions. Is this the oxidation or the reduction reaction? Is this reaction the source of electrons, or are electrons used to carry out the reaction? Explain your answers with a reaction equation.

You have probably had the unpleasant experience of discovering that a flashlight battery has gotten old and begun to leak. Is there evidence that this change is due to a chemical reaction?

The element carbon undergoes many inorganic reactions, as well as being the basis for the field of organic chemistry. Write balanced chemical equations for the reactions of carbon described below. l type='a'> Carbon burns in an excess of oxygen (for example. in the air) to produce carbon dioxide. If the supply of oxygen is limited, carbon will still burn but will produce carbon monoxide rather than carbon dioxide. molten lithium metal is treated with carbon, lithium car bide, Li2C2 , is produced. i>Iron(II) oxide reacts with carbon above temperatures of about 700 °C to produce carbon monoxide gas and molten elemental iron. i>Carbon reacts with fluorine gas at high temperatures to make carbon tetrafluoride.

Write balanced chemical equations for the reactions used to prepare each of the following compounds from the given starting material(s). In some cases, additional reactants may be required. (a) solid ammonium nitrate from gaseous molecular nitrogen via a two-step process (first reduce the nitrogen to ammonia, then neutralize the ammonia with an appropriate acid) (b) gaseous hydrogen bromide from liquid molecular bromine via a one-step redox reaction (c) gaseous H2S from solid Zn and S via a two-step process (first a redox reaction between the starting materials, then reaction of the product with a strong acid)

When heated to 700—800 C, diamonds, which are pure carbon, are oxidized by atmospheric oxygen. (They burn!) Write the balanced equation for this reaction.