Somebody help me with this please very much appreciated
1 answer:
The answer for the following answer is explained below.
The answer is NH_{4} ^{+}
Explanation:
Bronsted-Lowry acid :
It is a solution that donates protons, and is known as a proton donor.It donates protons in the form of hydrogen ion().This is reinforced by the definition of an acid ,which is a solution that has hydrogen ions.
In Bronsted-Lowry aci it must contain a hydrogen io that it can give up.When the acid gives a hydrogen ion,the charge of an acid decreases.
Here,
NH_{4} ^{+} loses one hydrogen ion and forms ammonia molecule.
So therefore the Bronsted-Lowry acid is NH_{4} ^{+}.
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Answer:
Explanation:
General representation of an element is given as:
where,
Z represents Atomic number
A represents Mass number
X represents the symbol of an element
Beta decay : In this process, a neutron gets converted into a proton and an electron releasing a beta-particle. The beta particle released carries a charge of -1 units.
The given reaction would be represented as:
Explanation:
Polarity is defined as the development of partial charges on the atoms of a molecule. In a water molecule, there are hydrogen and oxygen atoms.
Due to the difference in electronegativity of both hydrogen and oxygen atom there is development of partial positive charge on hydrogen atom and a partial negative charge on oxygen atom.
So, when bond between hydrogen and oxygen will break down then it will form hydrogen ions () and oxygen ions (
).
Ion-dipole interactions are defined as the interactions that occur when an ion interacts with the dipole of a molecule.
When an electron is added to a neutral atom to convert it into a negative ion then the amount of change taking place in its energy is known as electron affinity.
So, oxygen atom has an affinity towards cations and hydrogen atom has an affinity for anions.
Thus, we can conclude that following interactions and processes contribute to the dissolution of ionic compounds in water:
1. Affinity of oxygen towards cations
2. Ion–dipole interactions
4. Hydration
6. Affinity of hydrogen towards anions