You can mix them together (alloying) but these noble metals do NOT react, thus no bond is made
The reaction is:Ag+ + Cl- = AgCl(s)Silver chloride is an insoluble, white, photosensitive precipitate.
AgCl (silver chloride) is primarily an ionic bond. It forms when silver (Ag) donates an electron to chlorine (Cl), resulting in the formation of positively charged silver ions (Ag⁺) and negatively charged chloride ions (Cl⁻). This electrostatic attraction between the oppositely charged ions creates the ionic compound AgCl.
The empirical formula of the compound would be AgCl, as the ratio of silver to chlorine in the compound is 3:1 based on the given mass percentages (75% Ag and 25% Cl). This ratio simplifies to AgCl when expressed in the simplest whole number ratio.
Ag-N bond in Ag(NH3)2+ is a coordinate covalent bond. Cu-Cl bond in CuCl2 is an ionic bond. N-H bond in NH3 is a polar covalent bond. Ag-Ag bond in Ag2 is a metallic bond. Cl-Cl bond in Cl2 is a pure covalent bond.
slightly
slightly
The oxidation number of Ag in AgClO4 is +1, as it is a common oxidation state for silver in compounds. The oxidation number of Cl in AgClO4 is +7, as it is in the ClO4- ion which has a total charge of -1.
One mole of chloride (Cl-) to one mole of Ag+ ions: Cl- + Ag+ --> AgCl(s)
The oxidation number of Ag in AgCl is +1. AgCl is an ionic compound where Cl has an oxidation number of -1, so for the compound to be neutral, the oxidation number of Ag must be +1.
Ag, Hg, Pb
It actually reacts with AgCl to produce NaCl (which is soluble), and some Na3[Ag(S2O3)2]complexes which are also soluble in water.
A linear ionic bond is formed
in the AgCl molecule two atoms present one is Ag (i.e.Ag in +1oxidation state) & another is Cl atom(Cl in -1).
The oxidation number of silver (Ag) in AgCl is +1. This is because chlorine (Cl) has an oxidation number of -1 in most compounds, so the overall sum of the oxidation numbers must be zero for a neutral compound like AgCl.
Ag-Cl is an ionic compound formed between silver (Ag) and chlorine (Cl) ions. Ionic compounds are composed of a metal cation and a nonmetal anion, where the metal donates electrons to the nonmetal to achieve a stable electron configuration.
CuCl2(aq) + 2AgNO3(aq) = Cu(NO3)2(aq) + 2AgCl(s)