The boiling points of halogens increase down the group due to the increasing strength of Van der Waals forces as the size and relative atomic mass of the atoms increase. This change manifests itself in a change in the phase of the elements from gas (F2, Cl2) to liquid (Br2), to solid (I2).

Atoms of group 17 gain one electron and form anions with a 1− charge; atoms of group 16 gain two electrons and form ions with a 2− charge, and so on.

Halogens share many similar properties including:

• They all form acids when combined with hydrogen.
• They are all fairly toxic.
• They readily combine with metals to form salts.
• They have seven valence electrons in their outer shell.
• They are highly reactive and electronegative.

Like other nonmetals, halogens cannot conduct electricity or heat. Compared with most other elements, halogens have relatively low melting and boiling points.

Halogens are good conductors of heat and electricity. False as halogens belongs to 17(A) group so they are non metal nad as u know non metal are poor conductor of heat and electricity. Hence, the statement is false.

Anhydrous HF (or H2F2) is a bad conductor of electricity. HF is the weakest halogen acid and as such do not provide ions for carrying electric current.

Fluorine is a bad conductor of electricity as it remains incapable of giving out free electrons that remain localized on fluorine. This happens mainly due to two reasons: The reactivity of fluorine atom is high as it needs only one electron to fill its outermost orbit.

Pure sulfur is a tasteless, odourless, brittle solid that is pale yellow in colour, a poor conductor of electricity, and insoluble in water. It reacts with all metals except gold and platinum, forming sulfides; it also forms compounds with several nonmetallic elements.

Chlorine is a non-metal substance and hence it is a bad conductor of heat and electricity. Since the ions or electrons in a non-metal are bonded with covalent bonds therefore, their electron does not have a tendency to move in the outer nucleus. Therefore, it cannot work as a conductor.

In a silicon lattice, all silicon atoms bond perfectly to four neighbors, leaving no free electrons to conduct electric current. This makes a silicon crystal an insulator rather than a conductor. A pure silicon crystal is nearly an insulator — very little electricity will flow through it.

Graphite. Graphite is a form of carbon in which the carbon atoms form covalent bonds with three other carbon atoms. Graphite conducts electricity due to the ‘spare’ electrons being delocalised between the layers. This conductivity makes graphite useful as electrodes for electrolysis .

Melting point: Iodine is liquid so it doesn’t have a melting point. Conductor of Eletricity: Iodine does not conduct electricity since each molecule of iodine comprises two iodine atoms joined by a covalent bond that cannot be excited sufficiently to transfer electrical energy.

Conductor of Eletricity: Iodine does not conduct electricity since each molecule of iodine comprises two iodine atoms joined by a covalent bond that cannot be excited sufficiently to transfer electrical energy.