These are some possible ionic equation for CuSO4 plus H2O:
Cu2+ + 6 H2O --> Cu(H2O)6
Cu(H2O)62+ + H2O <--> Cu(OH)(H2O)5+ + H3O+
This makes a solution of copper sulfate weakly acidic.
Unbalanced equation is calles skeletal equation. The difference between these equations is that the skeleton equation doesnot show the no. of atoms and molecules in the equation whereas the balanced chemical equation shows. Also the balanced chemical equation shows that the products and the reactants are solid, liquid, gas or aqueous.
No, but both describe the same chemical reaction.
CuSO4 is ionic.
CuSO4 is an ionic compound. This is because it is composed of a metal (Cu) and a nonmetal (S and O), which typically form ionic bonds through the transfer of electrons.
A really good link below has amazing net ionic equations, balanced too! Sorted by type of reaction, really useful. Also try Chemfiesta.com
Yep. Cu is positively charged, and SO4 is negatively charged.
The chemical reaction is:2 NaOH + CoCl2 = 2 NaCl + Co(OH)2
Balanced Molecular:2HBr + Mg = MgBr2 + H2Net Ionic:2Br- + Mg = Mg2+ + 2 Br-
Yes, CuSO4 is an ionic compound. It is made up of copper (Cu) ions carrying a positive charge and sulfate (SO4) ions carrying a negative charge.
CuSO4 is an ionic compound composed of a metal (Cu) and a non-metal group (SO4). In this compound, copper gives up electrons to oxygen and sulfur atoms, forming positively charged ions (Cu2+) and negatively charged ions (SO4 2-) that are held together by ionic bonds.
Copper is a single element so it is nonpolar. A polar substance forms when two or more elements with different electronegativities bond form a compound.
Redox reactions are often written as net ionic equations to focus on the species that actually participate in the reaction, eliminating spectator ions that do not undergo any change. This simplification highlights the transfer of electrons between oxidizing and reducing agents, making it easier to analyze the underlying chemical processes. Additionally, net ionic equations provide a clearer representation of the reaction's chemistry in solution, which is particularly useful in contexts like electrochemistry and analytical chemistry.