Ultimate Quiz On Hybridisation

The correct answer is Lewis structure. Lewis structures are diagrams that show the bonding and lone pair electrons in a molecule. Lone pairs are represented by pairs of dots placed next to the atom. By looking at the Lewis structure, we can determine the presence and location of lone pairs in a molecule. Pauling's theory is related to chemical bonding, Archimedes principle is related to buoyancy, and Pauli's exclusion principle is related to electron configuration and the behavior of electrons in atoms. None of these theories or principles directly provide information about lone pairs.

Oxygen has 6 valence electrons. Valence electrons are the electrons in the outermost energy level of an atom, and they determine the atom's chemical properties. Oxygen is in group 16 of the periodic table, which means it has 6 valence electrons.

The correct answer is "Because of the bent shape of the molecule." This is because the water molecule (H2O) has a bent or V-shaped structure due to the two lone pairs of electrons on the oxygen atom. This arrangement causes an uneven distribution of charge, with the oxygen atom being slightly negatively charged and the hydrogen atoms being slightly positively charged. As a result, the bond between the oxygen and hydrogen atoms is polar, meaning there is an unequal sharing of electrons.

Linus Pauling is the correct answer because he was the first to develop the hybridization theory. This theory explains the mixing of atomic orbitals to form new hybrid orbitals during the bonding process. Pauling's work on hybridization greatly contributed to our understanding of chemical bonding and molecular structure.

A sigma bond is the strongest covalent chemical bond. It is formed by the overlap of atomic orbitals along the axis between the two bonding atoms. This overlap allows for maximum electron density between the atoms, resulting in a strong bond. In contrast, a pi bond is formed by the sideways overlap of atomic orbitals, which is weaker than the head-on overlap of a sigma bond. Bent bonds and metal-to-metal bonding are not covalent bonds and are not as strong as sigma bonds.

Pi-bonds are chemical bonds where two lobes of an orbital on one atom overlap two lobes of an orbital on another atom laterally. This type of bond is formed by the sideways overlap of p orbitals, resulting in the formation of a bond with electron density above and below the plane of the atoms. Pi-bonds are commonly found in double and triple bonds and are weaker than sigma bonds. They play a crucial role in the formation of organic molecules and are important for the stability and reactivity of compounds.

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The bond axis refers to the imaginary line that connects the two nuclei in a molecule. This axis represents the direction along which the atoms are bonded together. It helps to define the orientation and geometry of the molecule, as well as the arrangement of the atoms around the bond axis.

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In ethene (ethylene), C2H4, each carbon atom forms five sigma (σ) bonds.

Each carbon atom forms a sigma bond with one hydrogen atom and a sigma bond with the other carbon atom. This results in a total of five sigma bonds in ethene.

So, in ethene, there are five sigma (σ) bonds.