Evaluate the statement. bromine (br) is a halogen. given the information in the statement, what can be inferred as true about bromine? hint: look at your periodic table. a) bromine has seven electrons and seven protons b) bromine tends to form covalent bonds when in chemical reactions with metals c) bromine tends to form anions when in chemical reactions with metals d) bromine does not react easily with other atoms.

            Option-C (Bromine tends to form anions when in chemical reactions with metals) is the correct answer.

Explanation:
                   Bromine belongs to Group VII called as Halogens in the periodic table. It has seven valence electrons in its valence shell. In order to obtain noble gas configuration, Bromine tends to gain one electron from metals.
                   Therefore, Bromine forms ionic bond when treated with metals as the electronegativity difference is greater than 1.7. When Bromine gains electron from any metal it converts into Bromide (Br⁻) as follow,

                                     M +  Br₂      →     MBr₂

Reduction of Bromine,

                                     Br₂  +  2 e⁻     →     2 Br⁻     ∴ Br⁻  =  Anion

Oxidation of Metal:
                                     M     →     M²⁺  +  2 e⁻

During the seventeenth and especially eighteenth centuries, driven both by a desire to understand nature and a quest to make balloons in which they could fly (Figure 1), a number of scientists established the relationships between the macroscopic physical properties of gases, that is, pressure, volume, temperature, and amount of gas. Although their measurements were not precise by today’s standards, they were able to determine the mathematical relationships between pairs of these variables (e.g., pressure and temperature, pressure and volume) that hold for an ideal gas—a hypothetical construct that real gases approximate under certain conditions. Eventually, these individual laws were combined into a single equation—the ideal gas law—that relates gas quantities for gases and is quite accurate for low pressures and moderate temperatures. We will consider the key developments in individual relationships (for pedagogical reasons not quite in historical order), then put them together in the ideal gas law.

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