How does ionic radius affect the conductivity of an electrolyte solution?

How does ionic radius affect the conductivity of an electrolyte solution?

Radius decreases, smaller ions carrying current in small area, more associations with anions & due to this, the ions become heavy & they move with reduced speed as compared to less associated ones, & thus conductivity decreases.

What does ionic radius tell you?

The ionic radius is the distance between the nucleus and the electron in the outermost shell of an ion. When an electron is added to an atom, forming an anion, the added electron repels other electrons, resulting in an increase in the size of the atom.

What is the relationship between ionic radius and the charge of the ion?

In general, ionic radius decreases with increasing positive charge. As the charge on the ion becomes more positive, there are fewer electrons. The ion has a smaller radius. In general, ionic radius increases with increasing negative charge.

How does ions affect ionic radius?

Ionic size (for the same ion) also increases with increasing coordination number, and an ion in a high-spin state will be larger than the same ion in a low-spin state. In general, ionic radius decreases with increasing positive charge and increases with increasing negative charge.

How does ionic charge affect conductivity?

The conductivity is determined by the number of charge carriers, how fast they move, and how much charge each one carries. Hence, for most aqueous solutions, the higher the concentration of dissolved salts, which will lead to more ions, the higher the conductivity.

Why does the ionic radius increase?

As you move down a column or group, the ionic radius increases. This is because each row adds a new electron shell. Ionic radius decreases moving from left to right across a row or period. But for the nonmetallic elements, the ionic radius increases because there are more electrons than protons.

What happens if ionic radius increases?

Ionic radii increases down a group. In a group, all the ions have the same charge as they have the same valency (that is, the same number of valence electrons on the highest energy level sub-orbital). Therefore, ionic radii increase down a group as more shells are added (per period).

Why does the ionic radius increase down the group?

As you move down a column or group, the ionic radius increases. This is because each row adds a new electron shell. More protons are added, but the outer valence shell remains the same, so the positively charged nucleus draws in the electrons more tightly.

Does ionic radius increase or decrease down a group?

As you move down a column or group, the ionic radius increases. This is because each row adds a new electron shell. Ionic radius decreases moving from left to right across a row or period. While the atomic radius follows a similar trend, ions may be larger or smaller than neutral atoms.

Why does the ionic radius increase down a group?

Down a group, the number of energy levels (n) increases, so there is a greater distance between the nucleus and the outermost orbital. This results in a larger atomic radius. Ionic radius is the distance from the nucleus to the outer edge of the electron cloud of an ion.

What are the factors that affect an electrolysis reaction?

Describe factors that affect an electrolysis reaction. effect of concentration. nature of electrolyte. nature of electrodes. Change: Effect on Reaction: Increased current. Increased rate of electrolysis. Increased voltage.

Why does the conductivity of an ionic compound decrease with increasing radius?

Radius decreases, smaller ions carrying current in small area, more associations with anions & due to this, the ions become heavy & they move with reduced speed as compared to less associated ones, & thus conductivity decreases. The explanation is different to the what the book says. Could someone please explain this?

What happens to ionic radius as you move across a period?

Ionic radius decreases moving from left to right across a row or period. More protons are added, but the outer valence shell remains the same, so the positively charged nucleus draws in the electrons more tightly. But, for the nonmetallic elements, ionic radius increases because there are more electrons than protons.

What is the relationship between ionic radius and effective nuclear charge?

As you move across a row of period of the periodic table, the ionic radius decreases for metals forming cations, as the metals lose their outer electron orbitals. The ionic radius increases for nonmetals as the effective nuclear charge decreases due to the number of electrons exceeding the number of protons.