Identify which of the following is mainly responsible for holding bromine molecules relatively close together in the liquid state?

Question

BlackTom AI · Accepted Answer

First, let's restate what the question is asking:Identify which force mainly holds bromine molecules relatively close together in the liquid state, and consider the given options.
Option: Polar covalent bonds
This choice would imply that the attraction comes from polar covalent bonding between atoms within a molecule or between molecules. Bromine (Br2) is a diatomic molecule with nonpolar covalent bonds internally, and the molecule-ligand attractions in liquid Br2 are not governed by polar covalent interactions between different Br2 molecules. So this option does not explain why Br2 liquid is held together.
Option: Dispersion forces
Dispersion (London) forces arise from temporary fluctuations in electron distribution, creating instantaneous dipoles that induce neighboring dipoles. In nonpolar, symmetric molecules like Br2, these dispersion forces are the primary intermolecular attraction. They are responsible for keeping Br2 molecules relatively close in the liquid state by providing weak, temporary attractions that add up across many molecules.
Option: Hydrogen bonds
Hydrogen bonding requires hydrogen atoms bonded to highly electronegative atoms such as fluorine, oxygen, or nitrogen. Bromine is not capable of forming hydrogen bonds in Br2, so this option does not apply to liquid bromine.
Option: Ionic bonds
Ionic bonds involve full transfer of electrons and electrostatic attraction between oppositely charged ions. Bromine in Br2 remains as neutral molecules with covalent bonds; there are no ions formed to create ionic attractions in liquid bromine. Therefore, this option is inaccurate for explaining Br2's liquid-state cohesion.
In summary, the key reasoning is that bromine is a nonpolar diatomic molecule, and the dominant intermolecular force between its molecules in the liquid state is the dispersion (London) force, not hydrogen bonding, polar covalent inter-molecular interactions, or ionic bonding. The incorrect choices rely on bond types that do not govern Br2–Br2 interactions in the liquid phase.

Identify which of the following is mainly responsible for holding bromine molecules relatively close together in the liquid state?

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Identify which of the following is mainly responsible for holding bromine molecules relatively close together in the liquid state?

查看解析

登录即可查看完整答案

类似问题

Choose which of the following statements explains why benzoic acid is soluble in water.[Fill in the blank]

Rank the following compounds from lowest boiling point to highest boiling point.

Question at position 34 Select all of the weak types of bonds.IonicHydrogenVan der WaalsCovalent

Match the following properties of liquids with their best definition 1: Surface tension ____ 2: Cohesive force ____ 3: Capillary action ____ 4: Adhesive forces ____

What type of intermolecular forces are due to the attraction between temporary dipoles and their induced temporary dipoles?

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Compared to the melting points of ionic compounds, the melting points of molecular solids tend to be ____.

What is the key difference between a liquid and a gas?

更多留学生实用工具

希望你的学习变得更简单

Match the following properties of liquids with their best definition 1: Surface tension 2: Cohesive force 3: Capillary action 4: Adhesive forces