Which actions are part of the dissolution process of an ionic solute in water? (more than one)
1 answer:
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Answer: a) Sodium and nitrogen : : sodium nitride.
b) Oxygen and strontium :
: strontium oxide.
c) Aluminum and chlorine : : aluminium chloride.
d) Cesium and bromine : : cesium bromide.
Explanation:
For formation of a neutral ionic compound, the charges on cation and anion must be balanced. The cation is formed by loss of electrons by metals and anions are formed by gain of electrons by non metals.
a) Sodium and nitrogen : Here sodium is having an oxidation state of +1 called as cation and nitrogen forms an anion
with oxidation state of -3. Thus they combine and their oxidation states are exchanged and written in simplest whole number ratios to give neutral
named as sodium nitride.
b) Oxygen and strontium : Here strontium is having an oxidation state of +2 called as cation and oxygen forms an anion
with oxidation state of -2. Thus they combine and their oxidation states are exchanged and written in simplest whole number ratios to give neutral
named as strontium oxide.
c) Aluminum and chlorine : Here aluminium is having an oxidation state of +3 called as cation and chlorine forms an anion
with oxidation state of -1. Thus they combine and their oxidation states are exchanged and written in simplest whole number ratios to give neutral
named as aluminium chloride.
d) Cesium and bromine : Here cesium is having an oxidation state of +1 called as cation and bromine forms an anion
with oxidation state of -1. Thus they combine and their oxidation states are exchanged and written in simplest whole number ratios to give neutral
named as cesium bromide.
An oxide of nitrogen contains 30.45 mass % N, if the molar mass is 90± 5 g/mol the molecular formula is N₂O₄.
<h3>What is molar mass?</h3>The molar mass of a chemical compound is determined by dividing its mass by the quantity of that compound, expressed as the number of moles in the sample, measured in moles. A substance's molar mass is one of its properties. The compound's molar mass is an average over numerous samples, which frequently have different masses because of isotopes.
<h3>How to find the molecular formula?</h3>The whole-number multiple is defined as follows.
Whole-number multiple =
The empirical formula mass is shown below.
Mw of empirical formula = Mw of N+ 2 x (Mw of O)
= 14.01 g/mol + 2 x (16.00 g/mol)
= 46.01 g/mol
With the given molar mass or the molecular formula mass, we can get the whole-number multiple for the compound.
Whole-number multiple = ≈ 2
Multiplying the subscripts of NO2 by 2, the molecular formula is N(1x2)O(2x2)= N2O4.
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