HYBRIDIZATION

Presentation

•

Chemistry

•

10th Grade

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Practice Problem

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Medium

Samuel ATONGO

Used 10+ times

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16 Slides • 34 Questions

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?

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

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 sp³has how many hybrid orbitals?

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

Multiple Choice

Though CO₂is 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

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?

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.

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