1. is it easy to distinguish between between the different oxidation states of copper? why?

2. You synthesized copper (I) chloride and copper (I) oxide. How do they differ from their copper (II) analogs? comment on the stability of these moist solids in air. If unstable, what is the likely product of decomposition?

3. calculate the percent recovery of copper from 10 mL of .10M of Cu(NO3)2? (how would you do this question?)

4. Is it necessary to synthesize the various copper compounds in order to recover copper metal?

Also, how can you write word equations for reactions? For example, adding HCl to CuO.

Any help with these questions would be greatly appreciated! even telling me how to go about them!!! thank you!!!

1. I suggest you think of the various compounds of copper and ask yourself how you distinguish between them. The question is ambiguous to begin with because it doesn't specify by physical means or chemical means.

2. Again, if you synthesized these compounds you must have seem what they look like. Compare them with the (II) analogs and you have your answer.

3. How many grams do you if Cu? That's
mols Cu(NO3)2 = M x L = ?
mols Cu = the same since there is 1 mol Cu in 1 mol Cu(NO3)2.
Grams Cu = mols Cu x atomic mass Cu = ? This is the theoreticalyield (TY)

% recovery. You need to know how much Cu you recovered. Call that actual yield (AY). Then
% recovery = (AY/TY)*100 = ?

4. I don't understand 4.

word equation. There isn't a reaction in your example but it does dissolve so I would write it this way.
hydrochloric acid + copper(II) ==> copper 2+ ion(aq) + oxide ion(aq) + hydrogen ion(aq) + chloride ion(aq).

For a real reaction like this,
2HCl(aq) + CuS(s) ==> H2S(g) + CuCl2(aq)

hydrochloric acid + copper(II) sulfide yields hydrogen sulfide gas + copper(II) chloride

1. To distinguish between different oxidation states of copper, you can look at their physical and chemical properties. Copper has several common oxidation states, including +1 and +2. One way to distinguish between them is by observing their colors. Copper (I) compounds are typically white or pale yellow, while copper (II) compounds are usually blue or green. However, this method may not be foolproof as the color can be affected by other factors.

Another way to distinguish between the oxidation states is through their reactivity. Copper (I) compounds tend to be more reactive than copper (II) compounds. For example, copper (I) chloride (CuCl) is soluble in water and is readily oxidized to copper (II) when exposed to air, while copper (II) chloride (CuCl2) is more stable and less reactive.

2. Copper (I) chloride (CuCl) and copper (I) oxide (Cu2O) differ from their copper (II) analogs, copper (II) chloride (CuCl2) and copper (II) oxide (CuO), in terms of their oxidation states. Copper (I) compounds have copper in the +1 oxidation state, while copper (II) compounds have copper in the +2 oxidation state.

Regarding the stability of these moist solids in air, copper (I) compounds are generally less stable and more prone to oxidation compared to copper (II) compounds. Copper (I) chloride, for example, readily reacts with air oxygen and moisture to form copper (II) chloride. Copper (I) oxide can also decompose in the presence of moisture and oxygen to form copper (II) oxide.

If these compounds are unstable, the likely product of decomposition would be the higher oxidation state compound. For example, copper (I) chloride decomposes to form copper (II) chloride, while copper (I) oxide decomposes to form copper (II) oxide.

3. To calculate the percent recovery of copper from 10 mL of 0.10 M Cu(NO3)2, you will need to know the molar mass of copper (Cu). Let's assume it is 63.55 g/mol.

First, calculate the number of moles of copper in 10 mL of 0.10 M Cu(NO3)2:
moles of Cu = volume (in L) × concentration (in mol/L)
moles of Cu = 10 mL ÷ 1000 mL/L × 0.10 mol/L

Once you have the number of moles of copper, you can calculate the mass of copper using its molar mass:
mass of Cu = moles of Cu × molar mass
percent recovery = (mass of Cu recovered ÷ mass of Cu in initial solution) × 100

4. It is not necessary to synthesize various copper compounds in order to recover copper metal. Copper can be obtained from its ores through smelting and refining processes. These processes involve heating the ores to high temperatures, separating impurities, and obtaining pure copper.

To write word equations for reactions, you need to represent the reactants and products using their chemical formulas and express the reaction in words. For example, adding hydrochloric acid (HCl) to copper (II) oxide (CuO) can be written as follows:
Copper (II) oxide + Hydrochloric acid → Copper (II) chloride + Water
CuO + 2HCl → CuCl2 + H2O

Remember to balance the equation by adjusting the coefficients in front of each compound to ensure the conservation of atoms.