Which Of The Following Properties Decreases Down The Group From Fluorine To Iodine?

Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons. … As shown in the figure above, electronegativity decreases from fluorine to iodine; the atoms become less effective at attracting bonding pairs of electrons as they grow larger.

Which of the following property decreases down the group in the halogens?

Answer Expert Verified. Atomic radius increases down the group. Hence nuclear attraction for the valence electron decreases down the group.

What decreases in going down the halogen group?

This means the shared electrons are further from the halogen nucleus, which increases the shielding of inner electrons. This means electronegativity decreases down the group.

Why is fluorine more reactive compared to iodine?

The electron affinity of fluorine is much larger, which makes reduction to fluoride much easier. E−F bonds are stronger than E−I bonds, in both an ionic and covalent sense. Fluoride has a larger solvation enthalpy than iodide.

Which of the following decreases down the group from F to I?

As we move down the group from fluorine to iodine, electronegativity decreases due to corresponding increases in the size of the atom. Hence, this option is correct. So, the correct answer is “Option B,C and D”.

Which character decreases down a group?

As we move down the group, the non-metallic character decreases due to increase in the atomic size.

Which of the following properties of the halogens increases from F to I?

The melting points increase from F → I for the halogens.

Which of the following decreases down the group in the periodic table?

Electronegativity decreases as we go down the group and atomic radius increases as we go down the group.

Which is smaller iodine or fluorine and why?

Simply put, fluorine atoms will occupy less space than iodine atoms, which are considerably bulky when compared with fluorine atoms. … On the other hand, placing the larger iodine atom as the central atom will allow the smaller fluorine atoms to bond without too much repulsion.

Does fluorine or iodine have a higher electronegativity?

Fluorine has greater EN than iodine (in fact, F is the most EN atom in the periodic table). Fluoride has a high EN due to a combination of two effects, but the reason why iodine has a lower EN value is due to reason #2 alone.

Why is electronegativity of iodine less than fluorine?

1. Atomic Size: The smaller the size of an atom the greater its tendency to attract the shared pair of electrons. So smaller atoms have more electronegativity. … So as we move down the group from fluorine, chlorine, bromine to iodine the electronegativity decreases.

Which of the following properties increases going down in group 17 elements?

As you go down group 17 from top to bottom, the melting point of the elements increases and the boiling point increases.

Why do halogens show positive oxidation state?

Halogens show positive oxidation state when they combine with oxygen and fluorine atoms. 29. Halogens are good oxidizing agent and oxidizing power (reactivity decreases with the increase in a number.

Which of the property of halogens is maximum among the members of their period?

Answers. Electronegativity increases across a period, and decreases down a group. Therefore, fluorine has the highest electronegativity out of all of the elements. Because fluorine has seven valence electrons, it only needs one more electron to acheive a noble gas configuration (eight valence electrons).

Which property of halogens decreases with increase in atomic number?

In MX2 (M= metal X = halogen), covalent properties decrease. Ionisation potential decreas.

Which properties of halogens increase with increasing atomic number?

Physical Properties of Halogens

Chlorine and Fluorine are in the gaseous state, whereas bromine is in the liquid state and iodine is in the solid-state. The melting and boiling points of the halogens increase with an increase in their atomic numbers.

Which of the following properties of halogens increases with increase in atomic number?

In the halogen family on moving down the group from chlorine to iodine, atomic and ionic radius increases with increasing number of shells and shielding effect in halogen atom.

Why electron affinity decreases down the group?

Electron affinity decreases down the groups and from right to left across the periods on the periodic table because the electrons are placed in a higher energy level far from the nucleus, thus a decrease from its pull. … The increased nuclear charge as you go down the group is offset by extra screening electrons.

Does electronegativity decrease down a group?

Electronegativity is the measure of the ability of an atom in a bond to attract electrons to itself. Electronegativity increases across a period and decreases down a group. … Down a group, the number of energy levels (n) increases, and so does the distance between the nucleus and the outermost orbital.

Why does metallic character decrease?

– The metallic character is depending upon the losing of valence electrons. Due to this reason, the ability of an element to lose valence electrons from top to bottom increases. Whereas, in the case of across the period it decreases due to the decrease in the ability to lose valence electrons.

Which of the following parameter decreases down a group?

Answer: Moving down in a group, the electronegativity decreases due to an increase in the distance between the nucleus and the valence electron shell, thereby decreasing the attraction, making the atom have less of an attraction for electrons or protons.

What is the atomic size when moving down a group?

When moving down a group of the periodic table, the atomic radius increases because of the presence of additional principal energy levels, which are further away from the nucleus.

What is the trend for ionization energy going down the groups?

Ionization energy decreases as we go down a group. Ionization energy increases from left to right across the periodic table.