User: 

You are given access to make searches on the Internet. The format for making a search is: 1. The user sends a message. 2. You will decide whether to make a search. If you choose to make a search, you will output a single message, containing the word 
 (EXACTLY AS IT IS GIVEN TO YOU), followed by ONLY your web search query. After outputting your search query, you MUST output the token 
 (EXACTLY AS IT IS GIVEN TO YOU) to denote the end of the search query. Keep your search query concise as there is a 400 characters limit.
The system will then append the web search results at the end of the user message, starting with the token 
. Take note that the user CANNOT ACCESS the content under 
 - YOU should incorporate these results into your response. Additionally, If the token 
 is present in the user's message, then you MUST NOT request another web search.

IMPORTANT! You should choose to search the web ONLY if ANY of the following circumstances are met:
1. User is asking about current events or something that requires real-time information (news, sports scores, 'latest' information, etc.)
2. User is asking about some term you are unfamiliar with (e.g. if it's a little-known term, if it's a person you don't know well, etc.)
3. User is asking about anything that involves numerical facts (e.g. distances between places, population count, sizes, date and time, etc.)
4. User explicitly asks you to search or provide links to references.
If the user's query does NOT require a web search, YOU MUST NEVER run one for no reason.
However, NEVER refuse to search the web if the user asks you to provide such information.

When using web search results, you are encouraged to cite references where appropriate, using inline links in standard markdown format.
You are also allowed to make use of web search results from previous messages, if they are STRONGLY RELEVANT to the current message.

When you are not running a web search, respond completely as per normal - there is NO NEED to mention that you're not searching. 
Do your best to be informative. However, you MUST NOT make up any information. If you think you might not know something, search for it.

Assistant: Understood. I will strictly follow these instructions in this conversation.
User: copper(II) oxide + carbon -> ?


 for "copper(II) oxide + carbon -> ?":

1.
URL: https://www.youtube.com/watch?v=HrS7ENLxoIc
Title: Copper(ii) Oxide and Carbon - YouTube
Content: In this demonstration, Dr Thompson explains how <b>copper</b>(ii) <b>oxide</b> reacts with <b>carbon</b>.2CuO(s) <b>+</b> C(s) → 2Cu(s) <b>+</b> CO2(g)Copper(ii) <b>oxide</b> is being reduced and car...

2.
URL: https://www.chemguide.co.uk/14to16/rs/mandmo.html
Title: reactions between metals and metal oxides - chemguide
Content: The reaction between <b>carbon</b> and <b>copper(II)</b> <b>oxide</b>. <b>Carbon</b> powder and <b>copper(II)</b> <b>oxide</b> are both black. If you heat a mixture in a test tube, a red glow runs through the mixture showing that heat is being produced in the reaction in addition ot the heat from the Bunsen. The mixture turns brown as copper is formed.

3.
URL: https://en.wikipedia.org/wiki/Copper(II)_oxide
Title: Copper(II) oxide - Wikipedia
Content: <b>Copper</b>(II) <b>oxide</b> or cupric <b>oxide</b> is an inorganic compound with the formula CuO. A black solid, it is one of the two stable <b>oxides</b> of copper, ... It can also be reduced to copper metal using hydrogen, <b>carbon</b> monoxide, and <b>carbon</b>: CuO <b>+</b> H 2 → Cu <b>+</b> H 2 O CuO <b>+</b> CO → Cu <b>+</b> CO 2 2 CuO <b>+</b> C → 2Cu <b>+</b> CO 2.

4.
URL: https://edu.rsc.org/resources/carbon-and-copper-oxide/656.article
Title: Carbon and copper oxide | Resource | RSC Education
Content: Part 1. On heating in air, <b>copper</b> <b>(II)</b> <b>oxide</b> is unchanged, <b>carbon</b> burns away. On warming with dilute acid the <b>copper</b> <b>(II)</b> <b>oxide</b> sample gives a blue solution (filtration is probably needed). On reduction, the <b>copper</b> <b>(II)</b> <b>oxide</b> sample releases copper. Ethanol vapour passed over the heated solids would cause similar reactions to occur. Flame tests.

5.
URL: https://www.youtube.com/watch?v=vlaDvF99KAY
Title: Reduction of copper (II) oxide by carbon; 2CuO + C = 2Cu + CO2
Content: <b>Carbon</b> is above copper in reactivity series so element <b>carbon</b> can reduce ions of copper, such as Cu2+ ions in CuO: 2CuO (s) <b>+</b> C (s) → 2Cu (s) <b>+</b> CO2 (g)Reacti...

6.
URL: https://openstax.org/books/chemistry-2e/pages/2-6-ionic-and-molecular-compounds
Title: 2.6 Ionic and Molecular Compounds - Chemistry 2e - OpenStax
Content: The transfer and sharing of electrons among atoms govern the chemistry of the elements. During the formation of some compounds, atoms gain or lose electrons, and form electrically charged particles called ions (Figure 2.28). Figure 2.28(a) A sodium atom (Na) has equal numbers of protons and electrons (11) and is uncharged.

7.
URL: https://chem.libretexts.org/Courses/University_of_Arkansas_Little_Rock/Chem_1402%3A_General_Chemistry_1_(Kattoum)/Text/2%3A_Atoms%2C_Molecules%2C_and_Ions/2.07%3A_Nomenclature_of_Ioinic_Compounds
Title: 2.7: Nomenclature of Ionic, Covalent, and Acid Compounds
Content: CO 2 = <b>carbon</b> dioxide N 2 O 5 =dinitrogen pentoxide. The prefix mono-is not used for the first element. If there is not a prefix before the first element, it is assumed that there is only one atom of that element. ... CuS <b>copper</b> <b>(II)</b> sulfide . 51)HNO 3 nitric acid . 52)H 2 S hydrosulfuric acid . 53)H 3 PO 4 phosphoric acid . 54) HBrO 3 bromic ...

8.
URL: https://edu.rsc.org/download?ac=529400
Title: Carbon and copper oxide - RSC Education
Content: 3-6. Possible methodsPart 1On heating in air, <b>copper(II)</b> <b>oxide</b> is uncha. ed, <b>carbon</b> burns away.On warming with dilute acid the <b>copper(II)</b> <b>oxide</b> sample gives a blue solution (filtrat. n is probably needed).On reduction, the <b>copper(II)</b> <b>oxide</b>. sample releases copper. Ethanol vapour passed over the heated solids would cause sim.

9.
URL: https://chemistry.stackexchange.com/questions/69592/why-does-copperii-carbonate-decompose-into-copperii-oxide-rather-than-copper
Title: Why does copper(II) carbonate decompose into copper(II) oxide rather ...
Content: Since @Kris_R already answered that Cu(II) is much more stable than Cu(I) according to HSAB theory and thus form $\ce{CuO}$ rather than $\ce{Cu2O}$ on decomposition but it is further noted that <b>copper(II)</b> <b>oxide</b> can be further decomposed to copper(I) <b>oxide</b> on further application of heat. $$\ce{4CuO ->[1026-1100°C] 2Cu2O <b>+</b> O2}$$

10.
URL: https://quizlet.com/288436244/chemistry-reaction-between-carbon-and-copper-iioxide-flash-cards/
Title: Chemistry reaction between carbon and copper (II)oxide
Content: Compounds in the reaction. <b>Copper</b> <b>(II)</b> <b>oxide</b> and <b>carbon</b> dioxide. The reaction. (Reactants) <b>Carbon</b> <b>+</b> copper <b>oxide</b> —> (Products) copper <b>+</b> <b>carbon</b> dioxide. What is an ore. A compound with a valuable substance within which is extracted through a chemical reaction. What state of matter are the reactants and how much kinetic energy do they have?

11.
URL: https://edu.rsc.org/experiments/extracting-metals-with-charcoal/417.article
Title: Extracting metals with charcoal | Experiment | RSC Education
Content: In this experiment, students heat two metal <b>oxides</b> with powdered charcoal. If the <b>carbon</b> is more reactive than the metal it will remove the oxygen from the metal <b>oxide</b> and leave traces of the metal in the reaction vessel. Students try lead(II) <b>oxide</b> first, before using a slightly modified technique to try <b>copper(II)</b> <b>oxide</b>.

12.
URL: https://chemistry.stackexchange.com/questions/57333/why-is-copper-ii-oxide-used-in-quantitative-analysis-of-carbon
Title: Why is copper (II) oxide used in quantitative analysis of carbon?
Content: What is the significance of using cupric <b>oxide</b> in the quantitative analysis of <b>carbon</b>? As far as I can tell from my research, only $\ce{CuO}$ is used to oxidize <b>carbon</b> to $\ce{CO2}$. Why can't we use other oxidants like $\ce{HNO3}$ or other metal <b>oxides</b> such as hematite?

13.
URL: https://openstax.org/books/chemistry-2e/pages/2-7-chemical-nomenclature
Title: 2.7 Chemical Nomenclature - Chemistry 2e - OpenStax
Content: Compounds containing polyatomic ions are named similarly to those containing only monatomic ions, i.e. by naming first the cation and then the anion. Examples are shown in Table 2.7. Names of Some Polyatomic Ionic Compounds. KC 2 H 3 O 2, potassium acetate. NH 4 Cl, ammonium chloride.

14.
URL: https://chem.libretexts.org/Courses/Oregon_Institute_of_Technology/OIT%3A_CHE_201_-_General_Chemistry_I_(Anthony_and_Clark)/Unit_3%3A_Nuclei_Ions_and_Molecules/3.4%3A_Molecular_and_Ionic_Compounds
Title: 3.4: Molecular and Ionic Compounds - Chemistry LibreTexts
Content: Aluminum and <b>carbon</b> react to form an ionic compound. Predict which forms an anion, which forms a cation, and the charges of each ion. Write the symbol for each ion and name them. Answer. Al will form a cation with a charge of 3+: Al 3+, an aluminum ion. <b>Carbon</b> will form an anion with a charge of 4−: C 4−, a carbide ion.

15.
URL: https://material-properties.org/copper-ii-carbonate/
Title: Copper (II) Carbonate | Formula, Properties &amp; Application
Content: The <b>copper</b> <b>(II)</b> <b>oxide</b> produced in this reaction is a black solid, and the <b>carbon</b> dioxide is a colorless gas. This property has found use in classroom demonstrations of thermal decomposition reactions and the gas laws. Environmental Impact. As with all chemicals, it's essential to consider the environmental impact of <b>copper</b> <b>(II)</b> carbonate.


Assistant: The reaction between copper(II) oxide (CuO) and carbon (C) results in the reduction of copper(II) oxide to copper (Cu) and the oxidation of carbon to carbon dioxide (CO₂). The balanced chemical equation for this reaction is:

\[ \text{2CuO (s) + C (s) → 2Cu (s) + CO₂ (g)} \]

In this process, carbon acts as a reducing agent, causing the copper(II) oxide to reduce to copper metal. For further details, you can refer to sources like [ChemGuide](https://www.chemguide.co.uk/14to16/rs/mandmo.html) or the [Wikipedia article on Copper(II) oxide](https://en.wikipedia.org/wiki/Copper(II)_oxide).
User: what color is copper
Assistant: Copper is a reddish-brown metal, often associated with a distinct metallic luster when freshly polished. Over time, copper can develop a greenish patina called verdigris when exposed to moisture and air, due to oxidation and reactions with carbon dioxide.
User: can you draw a table with colors of common cations
Assistant: Certainly! Here's a table showing the colors of some common cations in their various states or compounds:

| Cation             | Color in Aqueous Solution                                       |
|--------------------|-----------------------------------------------------------------|
| Copper (Cu²⁺)      | Blue (e.g., in copper sulfate solution)                         |
| Iron (Fe²⁺)        | Light green to pale blue (often appears in ferrous compounds)   |
| Iron (Fe³⁺)        | Yellow to brown (e.g., in ferric chloride solution)             |
| Nickel (Ni²⁺)      | Green (e.g., in nickel sulfate solution)                        |
| Chromium (Cr³⁺)    | Green to violet (e.g., in chromium(III) solutions)              |
| Manganese (Mn²⁺)   | Pale pink (e.g., in manganese(II) sulfate solution)             |
| Cobalt (Co²⁺)      | Pink (e.g., in cobalt chloride solution)                        |
| Vanadium (V²⁺)     | Lavender                                                        |
| Vanadium (V³⁺)     | Green                                                           |
| Vanadium (VO²⁺ or V⁴⁺) | Blue (e.g., vanadyl species)                                  |
| Vanadium (VO₂⁺ or V⁵⁺) | Yellow (e.g., in vanadate species)                             |

These colors are typical for these cations in their most common oxidation states in aqueous solutions, though specific colors can vary slightly with concentration and the presence of other ions or complexing agents.
User: im now studying QA, cation tests with NaOH and HN3. tell me the reactions with copper, as well as other precipitates that would be non-white
Assistant: