Question

Write the condensed electron configurations for the following atoms and indicate how many unpaired electrons each has: (a) \(\mathrm{Mg},(\mathbf{b}) \mathrm{Ge},(\mathbf{c}) \mathrm{Br},(\mathbf{d}) \mathrm{V},(\mathbf{e}) \mathrm{Y},(\mathbf{f}) \mathrm{Lu}\)

Short answer

The condensed electron configurations and unpaired electrons for the given elements are as follows: (a) Mg: \([\mathrm{Ne}]\ 3s^2\], 0 unpaired electrons (b) Ge: \([\mathrm{Ar}]\ 4s^2 3d^10 4p^2\], 2 unpaired electrons (c) Br: \([\mathrm{Ar}]\ 4s^2 3d^10 4p^5\], 1 unpaired electron (d) V: \([\mathrm{Ar}]\ 4s^2 3d^3\], 3 unpaired electrons (e) Y: \([\mathrm{Kr}]\ 5s^2 4d^1\], 1 unpaired electron (f) Lu: \([\mathrm{Xe}]\ 6s^2 4f^14 5d^1\], 1 unpaired electron

Step-by-step solution

Determine the atomic numbers

Look up the atomic numbers of the given elements using the periodic table: (a) Mg (magnesium) has an atomic number of 12. (b) Ge (germanium) has an atomic number of 32. (c) Br (bromine) has an atomic number of 35. (d) V (vanadium) has an atomic number of 23. (e) Y (yttrium) has an atomic number of 39. (f) Lu (lutetium) has an atomic number of 71.

Write the condensed electron configurations

Using the periodic table, determine the condensed electron configurations for the given elements: (a) Mg: \[1s^2 2s^2 2p^6 3s^2\] or \[[\mathrm{Ne}]\ 3s^2\] (b) Ge: \[1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^2\] or \[[\mathrm{Ar}]\ 4s^2 3d^10 4p^2\] (c) Br: \[1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^5\] or \[[\mathrm{Ar}]\ 4s^2 3d^10 4p^5\] (d) V: \[1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^3\] or \[[\mathrm{Ar}]\ 4s^2 3d^3\] (e) Y: \[1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^1\] or \[[\mathrm{Kr}]\ 5s^2 4d^1\] (f) Lu: \[1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^6 6s^2 4f^14 5d^1\] or \[[\mathrm{Xe}]\ 6s^2 4f^14 5d^1\]

Determine the number of unpaired electrons

Count the number of unpaired electrons in the electron configurations: (a) Mg: 0 unpaired electrons (b) Ge: 2 unpaired electrons (c) Br: 1 unpaired electron (d) V: 3 unpaired electrons (e) Y: 1 unpaired electron (f) Lu: 1 unpaired electron In summary, we have the following condensed electron configurations and unpaired electrons: (a) Mg: \[[\mathrm{Ne}]\ 3s^2\], 0 unpaired electrons (b) Ge: \[[\mathrm{Ar}]\ 4s^2 3d^10 4p^2\], 2 unpaired electrons (c) Br: \[[\mathrm{Ar}]\ 4s^2 3d^10 4p^5\], 1 unpaired electron (d) V: \[[\mathrm{Ar}]\ 4s^2 3d^3\], 3 unpaired electrons (e) Y: \[[\mathrm{Kr}]\ 5s^2 4d^1\], 1 unpaired electron (f) Lu: \[[\mathrm{Xe}]\ 6s^2 4f^14 5d^1\], 1 unpaired electron

Key concepts

Atomic Number

The atomic number is truly a cornerstone in chemistry and physics, representing the unique identity of an element. It is defined as the number of protons in the nucleus of an atom. This number not only identifies an element but also determines its position in the periodic table.

Each element has a distinct atomic number. For example, magnesium (Mg) has an atomic number of 12, meaning it has 12 protons in its nucleus. Similarly, germanium (Ge) has an atomic number of 32. This concept is crucial because it tells us how many electrons an atom has in a neutral state, since the number of protons equals the number of electrons.

The atomic number not only determines the element's identity but also its chemical properties and placement on the periodic table. As you move across the table from left to right, each consecutive element has an atomic number one greater than the previous one.

Unpaired Electrons

Unpaired electrons have a significant role in the chemistry of an element. They are electrons that remain single in an atom's electron configuration. These unpaired electrons reside in orbitals that are not completely filled.

Unpaired electrons often indicate the magnetic properties of an element, contributing to paramagnetism, where atoms are attracted to a magnetic field. For example, in the bromine (Br) atom, there is 1 unpaired electron, revealing its magnetic nature.

To determine the number of unpaired electrons, examine the electron configuration of an atom, and identify if any orbitals contain unpaired electrons. For instance, vanadium (V) has three unpaired electrons in the 3d subshell according to its configuration \[\mathrm{[Ar] 4s^2 3d^3}\], making vanadium exhibit paramagnetic properties.

Remember, the presence of unpaired electrons is key in understanding the chemical reactivity and bonding behavior of elements.

Periodic Table

The periodic table is an essential tool for organizing elements that shows physical and chemical properties in a systematic way. Composed of rows called periods and columns known as groups or families, the periodic table allows us to predict the behavior and properties of elements.

Elements are arranged in increasing order of their atomic numbers. For instance, magnesium (Mg) is in the second period and group 2, indicating its place in the table with an atomic number 12.

The periodic table reveals trends such as atomic radii, ionization energy, and electronegativity. It also highlights categories like metals, nonmetals, and metalloids. This organization helps us understand not only individual elements but also their interactions.

The table is our guide to writing electron configurations and determining an element's valence electrons, which affect its chemical behavior. For instance, looking at yttrium (Y) in group 3, we see it typically forms 3+ ions, consistent with losing its three outermost electrons in the 5s and 4d subshells.