Question

Compare For each of the given elements, list two other elements with similar chemical properties a. iodine (I) b. barium (Ba) c. iron (Fe)

Short answer

Elements with similar chemical properties to iodine (I) are Fluorine (F) and Chlorine (Cl), as they are also part of the halogen group (Group 17). Elements with similar chemical properties to barium (Ba) are Calcium (Ca) and Magnesium (Mg), as they are also part of the alkaline earth metals group (Group 2). Elements with similar chemical properties to iron (Fe) include Cobalt (Co) and Nickel (Ni), as they are also part of the same group (Group 8) and period and have incompletely filled d-orbitals.

Step-by-step solution

(Listing elements with similar properties to Iodine (I))

(Iodine belongs to Group 17 (VIIA), which is also known as the halogen group. Elements in the same group have similar chemical properties due to having the same number of valence electrons. The elements with similar chemical properties to iodine are other halogens, such as Fluorine (F) and Chlorine (Cl).)

(Listing elements with similar properties to Barium (Ba))

(Barium is a part of Group 2 (IIA) in the periodic table, known as the alkaline earth metals. Elements in the same group have similar chemical properties due to having the same number of valence electrons. Therefore, elements with similar chemical properties to barium include other alkaline earth metals such as Calcium (Ca) and Magnesium (Mg).)

(Listing elements with similar properties to Iron (Fe))

(Iron belongs to Group 8 (VIIIB) of the periodic table and is a part of the transition metals. Elements in the same group do not necessarily have the same number of valence electrons, but they share similar properties due to having incompletely filled d-orbitals. Some elements with similar chemical properties to iron include Cobalt (Co) and Nickel (Ni) as they are also part of the same group and period.)

Key concepts

Halogens

Halogens form a fascinating and reactive group in the periodic table known as Group 17. They are non-metals and have seven electrons in their outermost shell, which significantly influences their chemical behaviors and reactions.

For instance, iodine (I), a member of this group, shares chemical properties with other halogens such as fluorine (F), chlorine (Cl), bromine (Br), and astatine (At). They are all eager to gain one more electron to achieve a full outer shell, which is why they form salts when they react with metals. One of the most well-known examples is sodium chloride (table salt), which is a compound of chlorine.

Halogens are also known for their distinct colors and states at room temperature - from the gaseous fluorine and chlorine, to the liquid bromine, and the solid iodine and astatine. These elements are used in many applications due to their reactivity, such as in disinfection, pharmaceuticals, and the production of halogen lamps.

Alkaline Earth Metals

The alkaline earth metals, situated in Group 2 of the periodic table, are comprised of beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra).

Similar to barium (Ba), these metals contain two electrons in their outermost shell, which they can readily lose to form cations with a +2 charge. This characteristic electron configuration leads to their shared chemical properties, including high reactivity, especially with water, to form hydroxides and release hydrogen gas.

Alkaline earth metals play crucial roles in various fields. Calcium, for example, is essential for biological organisms in building bones and teeth. Magnesium is a core component in chlorophyll, enabling plants to perform photosynthesis. Moreover, these metals find use in diverse applications such as aerospace construction, fireworks, and batteries.

Transition Metals

Transition metals form a broad group in the center of the periodic table, extending from groups 3 to 12. These metals, including iron (Fe), cobalt (Co), nickel (Ni), copper (Cu), and others, are defined by their partially filled d-orbitals.

The chemical properties of transition metals are complex due to the variety of oxidation states they can adopt, unlike the predictable +1 of the halogens or +2 of the alkaline earth metals. For instance, iron can exist in the +2 or +3 oxidation states allowing it to form various compounds, from hemoglobin in our blood to rust on an old car.

These elements' versatility means they are fundamental in industry and manufacturing. They are used to construct buildings, make jewelry, and even catalyze reactions in chemical processes. Their magnetic and conductive properties further position them as key materials in electronic devices and other high-tech applications.