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:
In the kinetic molecular theory, the molecules of an ideal gas are in constant random motion inside the container of the gas, and the pressure of the gas (which is the pressure exerted by the molecules in their collisions with the walls of the container) arise from this random motion of the molecules.
The main assumptions of the kinetic theory of gases are:
- The gas consists of a large number of molecules that collide between each other and the walls of the container; all these collisions are elastic
- The duration of the collisions is negligible compared to the time between the collisions
- The number of molecules is so large that statistics can be applied
- Intermolecular forces between the molecules are negligible (except during the collisions)
- The volume of the molecules is negligible compared to the volume of the container
In particular, the pressure of the gas is directly proportional to the average kinetic energy of the molecules, according to the equation:
where
p is the pressure of the gas
V is the volume of the container
K is the average kinetic energy of the molecules in the gas
We see that as the pressure is higher, the higher the kinetic energy of the particles: this means that the molecules will move faster, on average.
Therefore in this problem, the gas that exerts a pressure of 1.5 atm will have molecules moving faster than the molecules of the gas exerting a pressure of only 1.0 atm.