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

Verified step by step guidance

1. Identify the group number of carbon in the periodic table. Carbon is in group 14.
2. Determine the number of valence electrons for carbon. Elements in group 14 have 4 valence electrons.
3. Understand that the number of valence electrons determines how many bonds an element can form. Carbon can form 4 bonds because it has 4 valence electrons.
4. Consider the octet rule, which states that atoms tend to form bonds until they are surrounded by 8 valence electrons. Carbon needs 4 more electrons to complete its octet.
5. Conclude that carbon can form 4 new covalent bonds to achieve a full valence shell, typically forming single, double, or triple bonds in organic compounds.

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 carbon (C), which is in group 14 of the periodic table, there are four valence electrons. These electrons are involved in forming chemical bonds, influencing the element's reactivity and bonding capacity.

Bond Formation

Bond formation refers to the process by which atoms connect to create molecules. The number of bonds an element can form is typically equal to the number of unpaired valence electrons. In the case of carbon, it can form four covalent bonds by sharing its four valence electrons with other atoms, allowing for a variety of molecular structures.

Covalent Bonds

Covalent bonds are a type of chemical bond where two atoms share one or more pairs of electrons. This sharing allows each atom to attain a full outer shell, achieving greater stability. Carbon's ability to form four covalent bonds enables it to create complex organic molecules, making it a fundamental element in organic chemistry.