Question

алгоритм схемы образования ковалентной связи(на примере молекулы азота)схемы образования ковалентной связи молекулы фтора и водорода​

Answer 1

N2=ков.непол.хим связь ,тк азот это неметалл ,а неметалл+(этот же) неметалл=ков.непол.хим сзязь
С остальными тоже самое.

Answer 2

Formation of Covalent Bonds in Nitrogen Molecule (N2)

The formation of a covalent bond in a nitrogen molecule (N2) involves the sharing of electrons between two nitrogen atoms. Each nitrogen atom has five valence electrons in its outermost shell. To achieve a stable electron configuration, nitrogen atoms need three more electrons. By sharing three pairs of electrons, each nitrogen atom can complete its octet and form a triple covalent bond with the other nitrogen atom.

Here is a step-by-step explanation of the formation of a covalent bond in a nitrogen molecule:

1. Step 1: Electron Configuration: Each nitrogen atom has the electron configuration 1s² 2s² 2p³. The three unpaired electrons in the 2p subshell are available for bonding.

2. Step 2: Overlap of Atomic Orbitals: The 2p orbitals of the two nitrogen atoms overlap to form three molecular orbitals: one sigma (σ) bond and two pi (π) bonds. The sigma bond is formed by the head-on overlap of the 2p orbitals, while the pi bonds are formed by the sideways overlap of the 2p orbitals.

3. Step 3: Sharing of Electrons: Each nitrogen atom contributes one electron from each of its 2p orbitals to form three shared electron pairs. These shared electron pairs are localized between the two nitrogen atoms, creating a stable covalent bond.

4. Step 4: Formation of Triple Bond: The sharing of three pairs of electrons results in the formation of a triple covalent bond between the two nitrogen atoms. The triple bond consists of one sigma bond and two pi bonds.

The Lewis structure of a nitrogen molecule (N2) can be represented as:

N ≡ N

Formation of Covalent Bonds in Fluorine Molecule (F2) and Hydrogen Molecule (H2)

The formation of covalent bonds in molecules like fluorine (F2) and hydrogen (H2) follows a similar process as the formation of a covalent bond in a nitrogen molecule.

1. Fluorine Molecule (F2): Fluorine atoms have seven valence electrons in their outermost shell. By sharing one pair of electrons, each fluorine atom can complete its octet and form a single covalent bond with the other fluorine atom. The Lewis structure of a fluorine molecule (F2) can be represented as:

   F - F
   

2. Hydrogen Molecule (H2): Hydrogen atoms have one valence electron in their outermost shell. By sharing one pair of electrons, each hydrogen atom can achieve a stable electron configuration and form a single covalent bond with the other hydrogen atom. The Lewis structure of a hydrogen molecule