Describe why atoms of bromine, Br, are so reactive. To which family does bromine belong.

Bromine is a halogen and it is very reactive because it needs only one more electron to comoplete a "shell".

Ah, bromine, the lively rebel of the periodic table! You know, bromine atoms are quite reactive because they have a bit of a "halogen personality." They belong to the halogen family, along with their mischievous buddies like chlorine and fluorine.

Now, bromine is always on the lookout for some extra electrons to make itself more stable. Since it only has 7 electrons in its outermost energy level, it wants to grab another electron to fill up that octave and achieve the noble gas configuration.

This eagerness to gain an extra electron makes bromine a bit of a "bonding bandit." It loves to snatch electrons from other atoms, forming strong bonds and creating compounds. This reactive behavior can be both exciting and unpredictable, just like a spontaneous party crasher!

So, bromine's reactivity is all about its electron-hungry nature, which is common among the halogens. Just like a playful prankster at a family gathering, bromine brings an unpredictable and lively spark to the periodic table party!

Atoms of bromine (Br) are highly reactive due to their electron configuration and position in the periodic table. Bromine belongs to the halogen family (Group 17) in the periodic table.

One key factor that makes bromine reactive is its electron configuration. Bromine has seven valence electrons, and its electron configuration is 2-8-18-7. Like other halogens, it is only one electron away from having a stable noble gas electron configuration. Atoms tend to be more stable when they have a complete outer energy level, typically with eight electrons (the octet rule).

To achieve a stable configuration, bromine readily reacts with other elements by gaining or sharing one electron. By gaining an electron, bromine forms a negatively charged ion called a bromide ion (Br-). This ion has achieved a stable noble gas configuration by having a full outer energy level with eight electrons.

Bromine's reactivity also stems from its strong electronegativity. Electronegativity refers to an atom's ability to attract electrons towards itself in a chemical bond. Bromine has a relatively high electronegativity among elements, which means it has a strong tendency to attract electrons. This makes it more likely to participate in chemical reactions, as it can easily form covalent bonds with other atoms.

In summary, bromine's reactivity is primarily due to its electron configuration, where it is only one electron away from achieving a stable noble gas configuration. Its strong electronegativity also contributes to its reactivity. Consequently, bromine readily reacts with other elements to fulfill its electron needs, making it a highly reactive element.

Atoms of bromine, Br, are highly reactive due to their electron configuration and their position in the periodic table. Bromine belongs to the halogen family, which is located in Group 17 (Group VIIA) of the periodic table.

Bromine has an atomic number of 35, meaning it has 35 protons and electrons. Its electron configuration is 2-8-18-7, with the outermost energy level containing 7 valence electrons. Valence electrons are the electrons involved in chemical bonding and determining an atom's reactivity.

Atoms tend to become more stable by achieving a full outer electron shell. In the case of bromine, it only needs one additional electron to complete its outer level and reach the stable configuration of the noble gas argon. This electron deficiency makes bromine highly reactive, as it seeks to gain an electron from other atoms to complete its octet.

Bromine's reactivity is especially evident in reactions with metals. It readily reacts with metals to form ionic compounds, where bromine gains an electron from the metal to become a negatively charged ion called a bromide ion. This reactivity is essential in many chemical reactions, including organic synthesis, water disinfection, and flame retardants.

In summary, the reactivity of bromine is due to its electron configuration, specifically its need to gain one electron to achieve stability by completing its outer electron shell. This reactivity places bromine in the halogen family, whose members similarly have a strong tendency to gain one electron to reach a stable configuration.