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Silver has a charge of 1+ and CO3 has a charge of 2-, compounds must have charges of 0. (1+)+(1+)+(2-)=0, therefore, you get Ag2CO3. Hope this helps.
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How many atoms in Ag2O?
i believe 3 because Ag2 has two atoms and O only has one atom. so, 2+1=3
Enter the letter of the description from column 2 that best matches the term in column 1?
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.
What is the Formula for Silver carbonate?
Silver = Ag+1 Carbonate = CO3-2 Formula is: Ag2(CO3)
What is the formula silver carbonate?
Silver = Ag+1 Carbonate = CO3-2 Formula is: Ag2(CO3)
What is the chemical formula for silver sulphate?
Ag2( SO4)3
Ag plus CO3 equals Ag2 plus Co3?
Ag is going to exist in nature as Ag2--no doubt about it. The actual reaction with carbonate is 2AgNO3 (silver nitrate) + Na2CO3 (sodium carbonate) = Ag2CO3 (silver carbonate) plus NaNO3. For some reason you get elemental silver out of this too--which you shouldn't because it's a balanced equation, but Ag2CO3 is yellowish and it's normally got gray flecks in it when you get it.
What type of ion does silver form?
Mainly Silver(I) or Ag+ ion. It can also form Silver(II) or Ag2+ ion.
Why is the symbol for the atom silver Na?
The symbol for Silver is 'Ag' not 'Na' 'Ag' is taken from its Latin name Argentinum. 'Na' is the symbol for Sodium (latin name: Natrium) Silver is an Element. Atom is the smallest unit of any substance. Two silver atom would be present in Ag2
Are silver ions examples of ionic bonds?
Silver ions are only one half of a ionic bond. Take a simple ionic compound, one half of which is silver, for example silver bromide. This contains both Ag2+ (silver) and Br-(Bromine) ions. The bonds between these two different ions are ionic bonds
What is the balanced equation for silver chlorine silver chloride?
Silver oxide --> silver and (+) oxygenAg2O --> Ag2 + O2BALANCED =2Ag2O --> 2Ag2 + O2
What is the balanced equation for silver nitrate and iron II sulfate?
AgNO3 + CoSO4 --> Co(NO3)2 + Ag2 SO4 Double displacement reaction This is not balanced quick fix is 2AgNO3 + CoSO4 = Co(NO3)2 + Ag2SO4
What is the chemical reaction for silver nitrate and potassium chromate solutions?
the chemical reaction between silver nitrate and potassium chromate in generally used in a titration to look for chloride ions , and is a two step reaction: i will give you the ionic equations, which is pretty much all you need Ag+(aq) + Cl-(s) --> AgCl(s) this part of the equation caused the solution to go cloudy. when all the chloride ions are used up then the silver reacts with the chromate ions to produce the red colour you see when the end point of the precipitation is reached: 2Ag+(aq) + CrO4 2-(aq) --> Ag2 CrO4(s) which produces the red colour the amount of silver nitrate relates directly to the chloride ion concentration as it is a 1:1 ration reaction. i hope this answers your question =)
Where can you find a wiring diagram square d 2601 ag2 drum switch?
Did you find this diagram? I need it also to install a Hobart Disposer
What is the chemical property of silver?
Silver is in group 11, it has an electronic configuration of [Kr]4d105s1Silver metal is chemically relatively inert hence its use as a coinage metal. It is sensitive to sulfur compounds forming a black tarnish of silver sulfide Ag2SSilver(I)It has some similarities to the alkali metals as it loses one electron to form the Ag+ ion. One difference is that the Ag+ ion is small and therefore polarising (Fajans rules) and the salts such as AgCl are more covalent in character than their alkali metal analogues. AgCl unlike NaCl is quite insoluble in water. Precipitation of AgCl and weighing the precipitate ("gravimetric" analysis) is a method of determining chloride. AgBr is particularly sensitive to light, producing Ag metal and was used in photographic film. The silver mirror test for for aldehydes which reduce the Ag+ ion to Ag metal depositing it on the side of the vessel shows how easily Ag+ is reduced. (Note ketones do not reduce Ag+)The oxide Ag2O is known readily forming when precipitated AgOH is allowed to dry.Many compounds of silver(I) are best described as covalent, for example silver cyanide, silver sulfate where the coordination number of silver is 2 with linear bonding. Silver (I) forms many complexes with nitrogen ligands for example AgCl dissolves in liquid ammonia to form [Ag(NH3)2]+Silver(II)Ag can form other compounds where it loses a further one or two electrons (from the 4d shell). The Ag2+ ion is produced in aqueous solution by oxidation of AgI compounds with ozone. These ions are not stable, unlike copper where Cu2+ is well known. e.g. copper sulfate. AgF2 is known but AgCl2, AgBr2 are not. The oxide which appears to contain AgII is in fact a mixed valence oxide silver(I, III) oxideSilver(III)Some silver(III) compounds are known, AgF3 which is red. This oxidises xenon the inert gas to form XeF2. Then [Ag(OH)4]- ion containing Ag3+ is produced electrolytically in strong (12M) KOH solution. It gives the solution a yellow color which fades slowly, half life 100 mins or so.The wikipedia article on silver is not very good imho and most text books are weak on summarising trends.
