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

Verified step by step guidance

1. Identify the group number of nitrogen in the periodic table. Nitrogen is in group 15.
2. Determine the number of valence electrons. Elements in group 15 have 5 valence electrons.
3. To find out how many new bonds nitrogen can form, consider the number of electrons needed to complete its octet. Nitrogen needs 3 more electrons to reach 8.
4. Conclude that nitrogen can form 3 new covalent bonds to achieve a full octet.
5. Remember that the typical bonding pattern for nitrogen is to form three single bonds or one triple bond, as seen in ammonia (NH₃) or nitrogen gas (N₂).

Key Concepts

Valence Electrons

Valence electrons are the electrons located in the outermost shell of an atom. They play a crucial role in chemical bonding and determine how an element interacts with others. For nitrogen (N), which is in group 15 of the periodic table, there are five valence electrons, which are essential for forming bonds with other atoms.

Covalent Bonds

Covalent bonds are formed when two atoms share one or more pairs of electrons. The number of covalent bonds an atom can form is typically determined by the number of unpaired valence electrons it has. Since nitrogen has five valence electrons, it can form three covalent bonds by sharing its three unpaired electrons with other atoms.

Octet Rule

The octet rule is a chemical principle that states atoms tend to bond in such a way that they have eight electrons in their valence shell, achieving a stable electron configuration similar to that of noble gases. For nitrogen, which has five valence electrons, it seeks to gain three more electrons through bonding to fulfill the octet rule, thus forming stable compounds.