How can atoms with fewer than 8 valence electrons fill their outermost energy level? (If you can, can you please help me use either sulfur or magnesium to explain the process please?) Thank You!

They can either share electrons with other atoms (forming covalent bonds) or gain/lose electrons with other atoms (forming ionic bonds).

An atom of sulfer has six valence electrons. It can have eight valence electrons by sharing two electrons with or gaining two electrons from other atoms.

Atoms with fewer than 8 valence electrons can fill their outermost energy level through a process called ionization or through the formation of chemical bonds.

Let's take the example of sulfur, which has 6 valence electrons (in its 3rd energy level). Sulfur needs 2 more electrons to fill its outermost energy level, so it can achieve a stable electron configuration.

1. Ionization:
Sulfur can gain 2 electrons to achieve a stable electron configuration. This can be done by ionization - the process of gaining or losing electrons. Sulfur can gain 2 electrons by accepting them from other atoms that have a tendency to lose electrons. For example, sulfur can react with a metal like sodium (Na) that readily loses 1 electron. The resulting sulfur ion (S^2-) will now have 8 electrons in its outermost energy level.

2. Chemical Bonding:
Sulfur can also achieve a stable electron configuration by forming chemical bonds with other atoms. For example, sulfur can form a covalent bond by sharing its 2 valence electrons with 2 atoms of another element, such as oxygen (O). Sulfur and oxygen atoms can each contribute 1 electron to form a double bond, resulting in the formation of sulfur dioxide (SO2). In this case, sulfur shares its 2 electrons with the 2 oxygen atoms, which fills the outermost energy level of both sulfur and oxygen atoms.

Now, let's take the example of magnesium, which has 2 valence electrons in its 3rd energy level. Magnesium needs to lose these 2 electrons to achieve a stable electron configuration.

1. Ionization:
Magnesium can lose its 2 valence electrons through ionization. It can donate these electrons to an atom that readily accepts them, such as oxygen. When magnesium reacts with oxygen, it loses its 2 valence electrons and forms magnesium oxide (MgO). The resulting magnesium ion (Mg^2+) will now have a complete outermost energy level.

2. Chemical Bonding:
Magnesium can also achieve a stable electron configuration by forming chemical bonds. For example, magnesium can react with chlorine (Cl) to form magnesium chloride (MgCl2). Magnesium donates its 2 valence electrons to chlorine, which fills the outermost energy level of both atoms.

In summary, atoms with fewer than 8 valence electrons can fill their outermost energy level by either gaining or losing electrons through ionization, or by forming chemical bonds through electron sharing.

To understand how atoms with fewer than eight valence electrons fill their outermost energy level, let's take two examples: sulfur and magnesium.

Sulfur (atomic number 16) has six valence electrons in its outermost energy level. To fill its outermost energy level, it needs to gain two more electrons. Sulfur achieves this by undergoing a chemical reaction, typically forming a compound with another element that donates electrons. Sulfur often reacts with metals to achieve a stable electron configuration.

For example, when sulfur reacts with magnesium (atomic number 12), which has two valence electrons in its outermost energy level, the following reaction occurs:

S + Mg -> MgS

In this reaction, magnesium donates its two valence electrons to sulfur, completing the outermost energy level of sulfur. Magnesium loses its two electrons, forming a cation (Mg2+), while sulfur gains two electrons, forming an anion (S2-). The resulting compound, magnesium sulfide (MgS), has a stable electron configuration for both sulfur and magnesium.

So, sulfur fills its outermost energy level by gaining two electrons from another element.

On the other hand, let's consider magnesium itself. It only needs to lose its two valence electrons to achieve a stable electron configuration. Magnesium achieves this by undergoing a reaction in which it donates its two valence electrons to another atom or group of atoms.

For example, magnesium could react with chlorine (atomic number 17) to form magnesium chloride:

Mg + Cl2 -> MgCl2

In this reaction, each chlorine atom takes one electron from magnesium, resulting in the transfer of two electrons from magnesium to the two chlorine atoms. Magnesium loses its two valence electrons and forms a 2+ cation (Mg2+), while chlorine gains one electron each, forming two chloride anions (Cl-).

So, in the case of magnesium, it fills its outermost energy level by losing two electrons to another atom or group of atoms.

In summary, atoms with fewer than eight valence electrons fill their outermost energy level by either gaining or losing electrons through chemical reactions with other elements.