Chemistry Chapter on Hybridisation and Aromaticity

False (B)

It states that a compound must contain 4n + 2 pi bonds, where n is a whole number.

<p>cyclic</p> Signup and view all the answers

<p>Cyclic = Must have a ring structure Planar = All atoms lie in the same plane Conjugated = Alternating single and double bonds Huckel's rule = 4n + 2 pi bonds for stability</p> Signup and view all the answers

<p>sp3 (D)</p> Signup and view all the answers

<p>True (A)</p> Signup and view all the answers

<p>sigma (σ) bond</p> Signup and view all the answers

<p>180</p> Signup and view all the answers

<p>sp = Linear sp2 = Trigonal Planar sp3 = Tetrahedral sp3d = Trigonal Bipyramidal</p> Signup and view all the answers

<p>3 (C)</p> Signup and view all the answers

<p>Spherical (D)</p> Signup and view all the answers

<p>True (A)</p> Signup and view all the answers

<p>True (A)</p> Signup and view all the answers

<p>2p orbitals</p> Signup and view all the answers

<p>Aufbau Principle</p> Signup and view all the answers

<p>Atoms become more stable when bonds are formed. (D)</p> Signup and view all the answers

<p>True (A)</p> Signup and view all the answers

<p>unpaired</p> Signup and view all the answers

<p>Four</p> Signup and view all the answers

<p>sp3 (C)</p> Signup and view all the answers

<p>Aufbau Principle = Fill orbitals from lowest to highest energy Pauli’s Exclusion Principle = Maximum of two electrons per orbital with paired spins Hund’s Rule = One electron in each degenerate orbital before pairing Degenerate Orbitals = Orbitals at the same energy level</p> Signup and view all the answers

<p>False (B)</p> Signup and view all the answers

<p>orbital hybridisation</p> Signup and view all the answers

<p>Each set contains three orbitals at right angles to each other. (A)</p> Signup and view all the answers

<p>Bond Length = The optimum distance between two bonded atoms Bond Strength = The energy required to break a bond Hybrid Atomic Orbitals = New orbitals formed from the combination of s and p orbitals Valence Shell = The outermost shell of an atom that contains electrons</p> Signup and view all the answers

<p>Delocalization increases thermodynamic stability and decreases reactivity.</p> Signup and view all the answers

<p>False (B)</p> Signup and view all the answers

<p>3</p> Signup and view all the answers

<p>aromatic</p> Signup and view all the answers

<p>They have identical lengths and strengths. (C)</p> Signup and view all the answers

<p>False (B)</p> Signup and view all the answers

<p>sp = Triple bond sp2 = Double bond sp3 = Single bond sp3d = Pyramidal bond</p> Signup and view all the answers

<p>Multiple double bonds separated by a single bond (C)</p> Signup and view all the answers

<p>sp3</p> Signup and view all the answers

<p>False (B)</p> Signup and view all the answers

<p>It illustrates the alternating double bonds in aromatic compounds.</p> Signup and view all the answers

A spherical region around the nucleus where there is a high probability of finding an electron. Each S orbital can hold a maximum of two electrons.

A dumbbell-shaped region around the nucleus where there is a high probability of finding an electron. Each P orbital can hold a maximum of two electrons.

A set of orbitals within the same electron shell that have the same energy level. For example, the three p orbitals (Px, Py, Pz) are degenerate because they have the same energy level.

The process of combining atomic orbitals to form new hybrid orbitals. It helps explain the geometry and bonding properties of molecules.

A phenomenon where electrons are delocalized over a ring of atoms, leading to increased stability. This occurs when the molecule contains a cyclic system of alternating single and double bonds.

Orbitals are filled starting with those of lowest energy level. For example, 1s orbital is filled before 2s orbital

Each orbital can contain a maximum of two electrons, and they must have opposite spins.

When degenerate orbitals are available, electrons are filled one by one into each degenerate orbital before pairing up in the same orbital.

A cyclic molecule with conjugated double bonds that exhibits increased stability compared to other conjugated systems due to electron delocalization.

A rule that states that a cyclic molecule with 4n + 2 pi electrons, where n is a whole number (1, 2, 3, etc.), is considered aromatic.

A planar molecule with a continuous ring of overlapping p orbitals, allowing for the delocalization of electrons in a pi system. This delocalization contributes to increased stability.

The ability of a molecule to be stable due to the delocalization of electrons, resulting in the molecule being less reactive than expected. It's related to aromaticity.

A compound that is a cyclic molecule with a continuous ring of overlapping p orbitals, containing 4n + 2 pi electrons, leading to a planar structure with enhanced stability. Benzene is a classic example.

The process of combining atomic orbitals to form new hybrid orbitals with different properties.

It's the outermost electron shell of an atom, which participates in chemical bonding.

A three-dimensional representation of a molecule, showing how atoms are connected and arranged in space.

A type of covalent bond formed by the overlap of one s and three p atomic orbitals, resulting in four equivalent sp³ hybrid orbitals.

The energy released during the formation of a chemical bond between two atoms.

The energy required to break a chemical bond between two atoms.

The distance between the nuclei of two bonded atoms.

The strength of a chemical bond, measured by the amount of energy required to break it.

When multiple double bonds are separated by only a single bond, their pi electrons are delocalized over the entire system.

A type of bonding in which atomic orbitals combine to form a hybrid orbital, resulting in different bond angles and shapes.

In a conjugated system, all p orbitals overlap equally, creating a continuous delocalized π system. This allows for electron interaction across the entire molecule.

Double bonds that are separated by two or more single bonds, or not separated at all, resulting in localized pi electrons.

The distribution of electrons over multiple atoms instead of being localized on a single atom or bond.

A simplified representation of aromatic compounds showing alternating double and single bonds, which is a static representation.

The process of mixing the 2s orbital and three 2p orbitals in a carbon atom to form four equivalent sp3 hybrid orbitals. These orbitals point to the corners of a tetrahedron and give the carbon atom a tetrahedral geometry.

sp2 hybridization occurs when one 2s and two 2p orbitals mix together to form three SP2 hybrid orbitals, leaving one pure p orbital.

sp hybridization is a process where one 2s orbital mixes with one 2p orbital to generate two sp hybrid orbitals. This process leaves two unhybridized 2p orbitals.

A sigma (σ) bond is formed by the head-on overlap of hybridized orbitals, while a pi (π) bond is formed by the sideways overlap of unhybridized p orbitals.

A single bond, sigma (σ) bond is formed by the head-on overlap of sp3 orbitals, while a pi (π) bond is formed by the sideways overlap of unhybridized p orbitals.

Hybridization occurs because it leads to the formation of stronger bonds and provides better directional properties than non-hybridized orbitals.

Hybridization can occur with elements other than carbon, including nitrogen, oxygen, and sulfur. The electron configurations of these atoms in their compounds can be determined based on their hybridization state.