How many valence shell electrons do each of the following elements contain? How many new bonds can each form? (c) O

Verified step by step guidance

1. Identify the group number of oxygen in the periodic table. Oxygen is in group 16.
2. Determine the number of valence electrons for oxygen. Elements in group 16 have 6 valence electrons.
3. To find out how many new bonds oxygen can form, consider the number of electrons needed to complete its octet. Oxygen needs 2 more electrons to complete its octet.
4. Oxygen can form 2 new bonds to achieve a stable electron configuration, typically forming two single bonds or one double bond.
5. Visualize the bonding: Oxygen often forms two single bonds (e.g., in H2O) or one double bond (e.g., in O2) to satisfy the octet rule.

Key Concepts

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial for determining how an element interacts with others. For oxygen (O), which is in group 16 of the periodic table, there are six valence electrons. These electrons are involved in chemical bonding, influencing the element's reactivity and the types of bonds it can form.

Covalent Bonds

Covalent bonds are formed when two atoms share pairs of electrons, allowing them to achieve a full outer shell. Oxygen typically forms two covalent bonds to satisfy the octet rule, which states that atoms tend to bond in such a way that they have eight electrons in their valence shell. This characteristic is essential for understanding how oxygen interacts with other elements.

Octet Rule

The octet rule is a chemical principle that states atoms tend to bond in a way that results in eight electrons in their valence shell, achieving a stable electronic configuration. For oxygen, this means it will seek to gain or share two additional electrons to complete its octet. Understanding this rule helps predict the bonding behavior of oxygen and its compounds.