Which of the following are ionic, and which are molecular? (a) Sc2O3 ionic molecular (b) NaI ionic molecular (c) SCl2 ionic mole
1 answer:
Answer :
Ionic compound : (a), (b), (d), (e), (f), (g) and (h)
Molecular compound : (c)
Explanation :
Ionic compound : It is defined as the compound which is formed when electron gets transferred from one atom to another atom.
Ionic compound are usually formed when a metal reacts with a non-metal.
Covalent compound : It is defined as the compound which is formed by the sharing of electrons between the atoms forming a compound.
The covalent compound are usually formed when two non-metals react.
All the polyatomic ions always form an ionic compound.
Polyatomic ions : It is a charged species that composed of two or more atoms and these charged species are bonded by the covalent bond.
As we know that the molecular compounds are the covalent compounds.
(a) Sc₂O₃
This is an ionic compound because it is made up of scandium metal and oxygen non-metal elements.
(b) NaI
This is an ionic compound because it is made up of sodium metal and iodine non-metal elements.
(c) SCl₂
This is an molecular compound because it is made up of sulfur and chlorine non-metal elements.
(d) Ca(NO₃)₂
This is an ionic compound because it is made up of calcium metal and polyatomic ion non-metal elements.
(e) FeCl₃
This is an ionic compound because it is made up of iron metal and chlorine non-metal elements.
(f) LaP
This is an ionic compound because it is made up of lanthanum metal and phosphorous non-metal elements.
(g) CoCO₃
This is an ionic compound because it is made up of cobalt metal and polyatomic ion non-metal elements.
(h) (NH₄)₂SO₄
This is an ionic compound because it is made up of ammonium ion and sulfate ion.
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Answer:
5.0x10⁻⁵ M
Explanation:
It seems the question is incomplete, however this is the data that has been found in a web search:
" One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate. Suppose a EPA chemist tests a 250 mL sample of groundwater known to be contaminated with nickel(II) chloride, which would react with silver nitrate solution like this:
NiCl₂ + 2AgNO₃ → 2AgCl + Ni(NO₃)₂
The chemist adds 50 mM silver nitrate solution to the sample until silver chloride stops forming. She then washes, dries, and weighs the precipitate. She finds she has collected 3.6 mg of silver chloride. Calculate the concentration of nickel(II) chloride contaminant in the original groundwater sample. Round your answer to 2 significant digits. "
Keep in mind that while the process is the same, if the values in your question are different, then your answer will be different as well.
First we <u>calculate the moles of nickel chloride found in the 250 mL sample</u>:
- 3.6 mg AgCl ÷ 143.32 mg/mmol *
= 0.0126 mmol NiCl₂
Now we <u>divide the moles by the volume to calculate the molarity</u>:
- 0.0126 mmol / 250 mL = 5.0x10⁻⁵M