Chapter 3: Problem 81
Of the elements \(\mathrm{Na}, \mathrm{Mg}, \mathrm{Si}, \mathrm{S}, \mathrm{Cl}\), and \(\mathrm{Ar}\), identify one that fits each of the following: a. largest atomic size b. a halogen c. electron arrangement \(2,8,4\) d. highest ionization energy e. in Group \(6 \mathrm{~A}(16)\) f. most metallic character g. two valence electrons
Short Answer
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a. Na, b. Cl, c. Si, d. Ar, e. S, f. Na, g. Mg
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Atomic Size
Atomic size, also known as atomic radius, is the distance from the nucleus of an atom to the boundary of its electron cloud. The atomic size generally increases as you move down a group on the periodic table. This is because each row adds a new electron shell, making the atom larger. In contrast, atomic size decreases from left to right across a period due to the increasing charge of the nucleus, which pulls the electron cloud closer. For example, sodium (Na) has the largest atomic size among the elements Na, Mg, Si, S, Cl, and Ar.
Halogen
Halogens are found in Group 17 of the periodic table. They have seven valence electrons, making them highly reactive, especially with alkali metals and alkaline earth metals. Their reactivity decreases as you move down the group. Among the elements provided (Na, Mg, Si, S, Cl, Ar), chlorine (Cl) is the halogen. Halogens often form salts when combined with metals, such as sodium chloride (table salt).
Electron Arrangement
Electron arrangement refers to the distribution of electrons in an atom's electron shells. Each element has a specific electron configuration that shows the number of electrons in each shell. For example, the configuration 2,8,4 corresponds to silicon (Si). This means silicon has 2 electrons in its first shell, 8 in the second, and 4 in the third, totaling 14 electrons. This configuration helps determine the chemical properties and reactivity of the element.
Ionization Energy
Ionization energy is the energy required to remove an electron from a gaseous atom or ion. It generally increases across a period (from left to right) due to the higher nuclear charge, which holds the electrons more tightly. Conversely, ionization energy decreases as you move down a group because the electrons are farther from the nucleus and thus easier to remove. Argon (Ar) has the highest ionization energy among the given elements (Na, Mg, Si, S, Cl, Ar) because it is a noble gas with a full outer electron shell, making it very stable.
Group 16 Elements
Group 16 elements, also known as Group 6A, have six valence electrons. These elements include oxygen, sulfur, selenium, tellurium, and polonium. They are crucial for many biological and industrial processes. Sulfur (S) is the Group 16 element among the given elements (Na, Mg, Si, S, Cl, Ar). These elements tend to form compounds by gaining or sharing electrons to complete their valence shell.
Metallic Character
Metallic character refers to an element's ability to lose electrons and form positive ions (cations). This property increases as you move down a group and decreases from left to right across a period on the periodic table. Elements with high metallic character are typically shiny, malleable, conductive, and have high melting and boiling points. Sodium (Na), out of the elements given (Na, Mg, Si, S, Cl, Ar), exhibits the most metallic character, making it highly reactive and typical of metals.
Valence Electrons
Valence electrons are the outermost electrons of an atom and determine its chemical properties and reactivity. Elements in the same group typically have the same number of valence electrons. For example, magnesium (Mg) has two valence electrons, placing it in Group 2 of the periodic table. These electrons are crucial for forming bonds with other atoms. Elements with similar valence electrons exhibit similar chemical behavior.
