HYBRIDIZATION

Multiple Choice

What is hybridization?

• Formation of covalent bonds through electron sharing

• Formation of metallic bonds in a crystal lattice

• Formation of new hybrid orbitals by combining atomic orbitals of different energies and shapes

• Formation of ionic bonds between atoms

Multiple Choice

Which of the following is NOT a common type of hybridization?

• sp

• sp²

• sp³

• dsp²

Multiple Choice

sp³ hybridization occurs when

• one s orbital and two p orbitals combine
• two s orbitals and two p orbitals combine
• three s orbitals and one p orbital combine
• one s orbital and three p orbitals combine

Multiple Choice

Hybridization occurs to

• form new atomic orbitals suitable for bonding
• increase atomic weight
• break existing bonds
• create new elements

Multiple Choice

Why do sp³ hybrid orbitals have varying bond angle?

• Temperature variations
• Presence of lone pairs of electrons
• Electronegativity of the atoms
• Presence of double bonds

Multiple Choice

What is the average bond angle of sp³ hybrid orbitals?

• 120 degrees
• 105 degrees
• 109.5 degrees
• 100 degrees

Multiple Choice

Why does water have a bent shape?

• Attraction between lone pairs of electrons on the oxygen atom
• Hydrogen bonding between water molecules
• Ionic bonding between hydrogen and oxygen atoms
• Repulsion between lone pairs of electrons on the oxygen atom

Multiple Choice

What type of hybrid orbital exist on the central atom of water?

• sp²

• sp
• sp³

• sp³d

Multiple Choice

Sp² hybridization is formed when

• two s orbitals and one p orbital combine
• three s orbitals combine
• one s orbital and one p orbital combine
• one s orbital and two p orbitals combine

Multiple Choice

The bond angle between sp² hybrid orbitals is

• 180 degrees
• 150 degrees
• 90 degrees
• 120 degrees

Multiple Choice

What is the shape of sp² hybrid orbital molecules?

• octahedral
• trigonal planar
• tetrahedral
• linear

Multiple Choice

Which of the following compounds has sp² hybridization?

• Methane (CH₄)

• Acetylene (C₂H₂)

• Ethylene (C₂H₄)

• Propane (C₃H₈)

Multiple Choice

sp hybrid orbital involves the combination of

• one s orbital and one d orbital
• two s orbitals
• one p orbital and one d orbital
• one 2s orbital and one 2p orbital

Multiple Choice

What is the shape of sp hybrid orbitals?

• Linear
• Square
• Tetrahedral
• Octahedral

Multiple Choice

How does the one 2s orbital gets hybridized with a 2p orbital?

• The 2s orbital remains unchanged
• The 2s orbital combines with a 3p orbital
• Through the process of hybridization, the one 2s orbital and one 2p orbital combine to form two sp hybrid orbitals.
• The 2s orbital combines with a 1s orbital

Multiple Choice

What is the bond angle between an sp orbital?

• 180 degrees
• 270 degrees
• 120 degrees
• 90 degrees

Multiple Choice

What is the shape of sp³ hybrid orbitals?

• Linear
• Square
• Tetrahedral
• Octahedral

Multiple Choice

What is the mixing ratio of an sp³ hybrid orbital?

• 1:2
• 1:4
• 1:3
• 1:5

Multiple Choice

An sp³ has how many hybrid orbitals?

• 2
• 6
• 4
• 8

Multiple Choice

What is an electron orbital?

• A region around the nucleus of an atom where an electron is likely to be found.
• A region around the nucleus of an atom where a photon is likely to be found.
• A region around the nucleus of an atom where a neutron is likely to be found.
• A region around the nucleus of an atom where a proton is likely to be found.

Multiple Choice

What is the hybridization of CO₂?

• dsp2
• sp3
• sp2
• sp

Multiple Choice

Though CO₂ is a compound with an sp2 hybridization, yet it has a linear shape. What accounts for that?

• Repulsion between lone pairs of electrons
• Tetrahedral geometry
• Attraction between lone pairs of electrons
• Presence of double bonds

Multiple Choice

What accounts for trigonal pyramidal shape of ammonia (NH₃)?

• Absence of lone pairs on the nitrogen atom
• Presence of a double bond between nitrogen and hydrogen atoms
• Linear arrangement of hydrogen atoms
• Presence of a lone pair of electrons on the nitrogen atom

Multiple Choice

How does the presence of lone pair(s) affect the shape and bond angle of covalent compounds?

• Lone pairs have no effect on the shape or bond angle of covalent compounds.
• Lone pairs result in linear molecular shapes with ideal bond angles.
• Lone pairs always lead to a symmetrical molecular shape.
• Lone pairs cause deviations from the ideal bond angles and can result in a non-linear or distorted molecular shape.

Multiple Choice

Water is bent because

• absence of lone pairs of electrons on the oxygen atom
• presence of two lone pairs of electrons on the oxygen atom
• presence of three lone pairs of electrons on the oxygen atom
• linear molecular geometry

Multiple Choice

What is the hybridization of water?

• sp²

• sp
• sp³d

• sp³

Multiple Choice

What is a sigma bond?

• A sigma bond is a type of covalent bond formed by the overlap of atomic orbitals along the bond axis.
• A sigma bond is a type of metallic bond
• A sigma bond is a type of hydrogen bond
• A sigma bond is a type of ionic bond

Multiple Choice

Ethyne (C₂H₂) has how many pi bonds?

• 1
• 4
• 2
• 3

Multiple Choice

The difference between pi bond and sigma bond is that

• Pi bond is stronger than sigma bond.
• Pi bond is formed by the end-to-end overlap of p orbitals, while sigma bond is formed by the side-to-side overlap of atomic orbitals.
• Pi bond is always present in single bonds.
• Pi bond is formed by the side-to-side overlap of p orbitals, while sigma bond is formed by the end-to-end overlap of atomic orbitals.

Multiple Choice

Why does pi-bond limit free rotation of molecules?

• Pi-bonds allow free rotation by aligning with the molecule's axis
• Pi-bonds restrict free rotation due to the sideways overlap of p-orbitals.
• Pi-bonds have no effect on the rotation of molecules
• Pi-bonds enhance free rotation by stabilizing the molecule

Multiple Choice

In pi-bonds, where is electron density concentrated?

• Above and below the plane of the bonded atoms
• Within the plane of the bonded atoms
• In the nucleus of the bonded atoms
• Distributed equally around the bonded atoms

Multiple Choice

In sigma-bonds, where is electron density concentrated?

• Above and below the plane of the bonded atoms
• Within the plane of the bonded atoms
• In the nucleus of the bonded atoms
• Distributed equally around the bonded atoms

Multiple Choice

Why is pi-bond always accompanied by a sigma bond?

• A pi-bond can exist independently without a sigma bond
• A pi-bond is weaker when accompanied by a sigma bond
• A pi-bond is always accompanied by a sigma bond to provide stability and strength to the overall bond.
• A sigma bond is not necessary for a pi-bond to exist

Multiple Choice

Sigma bond is stronger than the pi bond because

• Pi bonds have a greater overlap of atomic orbitals along the bond axis.
• Sigma bonds involve weaker electrostatic interactions.
• Pi bonds are more stable due to their structure.
• Sigma bonds have a greater overlap of atomic orbitals along the bond axis.