Question

Of the elements \(\mathrm{Sn}, \mathrm{Xe}, \mathrm{Te}, \mathrm{Sr}, \mathrm{I}\), and \(\mathrm{Rb}\), identify one that fits each of the following: a. smallest atomic size b. an alkaline earth metal c. a metalloid d. lowest ionization energy e. in Group \(4 \mathrm{~A}(14)\) f. least metallic character g. seven valence electrons

Short answer

a. Xe, b. Sr, c. Te, d. Rb, e. Sn, f. Xe, g. I

Step-by-step solution

- Identify smallest atomic size

The smallest atomic size typically corresponds to an element that is furthest to the right and towards the top of the periodic table. Among the given elements \(\text{Sn, Xe, Te, Sr, I, Rb}\), Xenon (Xe) fits this description as it is a noble gas in period 5.

- Identify the alkaline earth metal

Alkaline earth metals are found in Group 2 of the periodic table. Among the given elements, Strontium (Sr) is an alkaline earth metal.

- Identify the metalloid

Metalloids are elements that have properties intermediate between metals and nonmetals. Among the given elements, Tellurium (Te) is a metalloid.

- Identify element with lowest ionization energy

The element with the lowest ionization energy is typically the one that is furthest to the left and towards the bottom of the periodic table. Among the given elements, Rubidium (Rb) has the lowest ionization energy.

- Identify element in Group 4A (14)

Group 4A (or Group 14) on the periodic table includes elements like Carbon, Silicon, Germanium, Tin, and Lead. Among the given elements, Tin (Sn) is in Group 4A.

- Identify element with least metallic character

The least metallic character corresponds to elements on the right side of the periodic table. Among the given elements, Xenon (Xe), a noble gas, has the least metallic character.

- Identify element with seven valence electrons

Elements with seven valence electrons are in Group 17 (or Group 7A). Among the given elements, Iodine (I) has seven valence electrons.

Key concepts

atomic size

Atomic size, also known as atomic radius, refers to the distance from the center of the nucleus to the outermost electron shell. As you move down a group in the periodic table, the atomic size increases because additional electron shells are added. Conversely, as you move from left to right across a period, the atomic size decreases because the effective nuclear charge increases, pulling the electron shells closer to the nucleus.
In the original exercise, Xenon (Xe) was identified to have the smallest atomic size among the given elements because it is located furthest to the right and towards the top of the periodic table.

alkaline earth metals

Alkaline earth metals belong to Group 2 of the periodic table. These metals include Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), Barium (Ba), and Radium (Ra). These elements have two valence electrons, which they tend to lose easily to form +2 cations. This makes them quite reactive, though not as reactive as the alkali metals in Group 1.
In the exercise, Strontium (Sr) is identified as the alkaline earth metal among the given elements.

metalloids

Metalloids have properties intermediate between metals and nonmetals. They are often semiconductors, meaning they can conduct electricity better than nonmetals but not as well as metals. Common metalloids include Boron (B), Silicon (Si), Germanium (Ge), Arsenic (As), Antimony (Sb), and Tellurium (Te).
In the exercise, Tellurium (Te) is identified as the metalloid among the given elements. It exhibits both metallic and nonmetallic properties.

ionization energy

Ionization energy is the energy required to remove an electron from an atom in its gaseous state. It generally increases as you move from left to right across a period due to increasing effective nuclear charge. However, it decreases as you move down a group because the electrons are further from the nucleus, making them easier to remove.
In the exercise, Rubidium (Rb) is identified as having the lowest ionization energy among the given elements. It's located in Group 1, where the elements have a single electron in their outer shell that is easy to remove.

Group 4A elements

Group 4A, or Group 14, elements include Carbon (C), Silicon (Si), Germanium (Ge), Tin (Sn), and Lead (Pb). These elements have four valence electrons, which makes them versatile in forming various types of bonds. They can react with both metals and nonmetals.
In the exercise, Tin (Sn) is correctly identified as the element in Group 4A among the given options. Tin has several common oxidation states, making it useful in a variety of chemical reactions.

metallic character

Metallic character refers to the degree to which an element exhibits the characteristics of metals, such as being lustrous, ductile, malleable, and good conductors of heat and electricity. This character generally decreases as you move from left to right across a period and increases as you move down a group.
In the exercise, Xenon (Xe) is identified as having the least metallic character among the given elements. Being a noble gas, Xenon is non-metallic and largely inert.

valence electrons

Valence electrons are the electrons in the outermost shell of an atom. These electrons are important because they are involved in chemical bonding. Elements in the same group have the same number of valence electrons, which gives them similar chemical properties. For example, elements in Group 17 (or Group 7A) have seven valence electrons and include Fluorine (F), Chlorine (Cl), Bromine (Br), Iodine (I), and Astatine (At).
In the exercise, Iodine (I) is identified as the element with seven valence electrons among the given options.