Chemical Bonding And Molecular Structure

The correct option is (C): Lone pair-bond pair repulsion.

The correct option is (C): .

The correct option is (B): 3.35Å.

The correct option is (C): 2, 2.

The correct option is (B): .

An ionic bond is formed when an electron is transferred from a metal atom to a non-metal atom, resulting in the formation of ions that are held together by electrostatic forces.

BeCl has a linear structure because beryllium forms two bonds with chlorine atoms, resulting in an angle of 180 between the bonds. Therefore, the bond angle in BeCl is 180 .

O has a double bond between the oxygen atoms, where two pairs of electrons are shared. This is the correct answer, as other molecules listed have single bonds.

In NH , nitrogen has 3 bond pairs (from the three N-H bonds) and 1 lone pair of electrons in its valence shell. Thus, the correct answer is 3 bond pairs and 1 lone pair.

NaCl forms a polar covalent bond because sodium (Na) is a metal and chlorine (Cl) is a non-metal, leading to an unequal sharing of electrons, resulting in a polar bond.

Step 1: Understanding molecular geometry.
The H O molecule consists of two hydrogen atoms covalently bonded to a central oxygen atom. The oxygen atom has two lone pairs of electrons, which cause the molecule to adopt a bent or V-shape. Step 2: Explanation of the shape.
The lone pairs on oxygen repel the bonding pairs of electrons, which forces the molecule to adopt a bent geometry. The bond angle is approximately 104.5°, which is less than the ideal tetrahedral angle of 109.5° due to the lone pair repulsion. Step 3: Conclusion.
Thus, the shape of the H O molecule is bent or V-shaped.

Step 1: Understanding polar covalent bonds.
A polar covalent bond occurs when two atoms with different electronegativities form a bond, resulting in an unequal sharing of electrons. Step 2: Explanation.
In HCl (hydrogen chloride), chlorine is more electronegative than hydrogen, so the electrons in the bond are more attracted to chlorine, creating a partial negative charge on chlorine and a partial positive charge on hydrogen. Step 3: Conclusion.
Thus, HCl has a polar covalent bond due to the difference in electronegativity between hydrogen and chlorine.

Step 1: Definition of Sigma Bond.
A sigma bond is formed by the head-on overlapping of atomic orbitals along the internuclear axis. This overlap results in a bond with high electron density between the nuclei. Step 2: Characteristics of Sigma Bond.
Sigma bonds are stronger than pi bonds due to the direct overlap of orbitals. They are formed in single bonds and are responsible for the bonding between atoms in molecules. Step 3: Conclusion.
The bond formed by the overlapping of orbitals along the internuclear axis is called a sigma bond.

Step 1: Definition of Ionization Energy.
Ionization energy is the energy required to remove an electron from an atom or ion in the gas phase. It is influenced by atomic size and effective nuclear charge. Step 2: Trend Across a Period.
As you move across a period from left to right, the number of protons increases, leading to a higher effective nuclear charge. This stronger attraction makes it more difficult to remove electrons, and thus, the ionization energy increases. Step 3: Conclusion.
Therefore, ionization energy generally increases from left to right in a period.