Generate Quiz 68E06AC8DE0B4

With a total of 12 valence electrons—four between the two central carbons and two between each of the four carbon-hydrogen bonds—C2H4 has the most shared electrons of any compound.

N2 has 3 shared pairs of electron (6 electrons in total)

CO2 has 4 shared pairs of electrons (8 electrons in total).

NH3 has 3 shared pairs of electrons. (6 total electrons)

The cation Na+ and the anion OH- combine to form NaOH. It has ionic bonds as a result. However, if we only look at the hydroxyl group (-OH), we will see that there is a covalent bond.

Since the octet rule describes an atom’s propensity to favor having eight (8) electrons in its valence shell, Option C is accurate.

This is the right choice.

the force that binds the atoms that comprise a compound or molecule together. Chemical bonds like ionic, covalent, and metallic bonds are examples of intramolecular forces.

It serves as an illustration of intermolecular forces.

Types of Intermolecular Forces: Ion-Dipole, Dipole-Dipole, Dispersion, and Hydrogen Bonding

The trend of electronegativity is F>O>N. The strength of the bond increases with the difference in the electronegativity of the linked atoms. The strongest hydrogen bond is formed by fluorine because it is the most electronegative.

The weakest intermolecular forces are London dispersion forces, also known as van der Waals forces. They occur when transient changes in the distribution of electrons cause transient dipoles to form in nonpolar molecules. The London forces get stronger as a molecule’s size and electron count increase. The strength of London forces increases as the molecular weight of the halogens rises from F2 to Cl2 to Br2 to I2. The main cause of the shift in the states of halogens at room temperature is this increase in London forces.

The relationship between conductivity and hydration is inverse. Ions’ conductance drops after hydration because they are encircled by water molecules. Therefore, hydration must decrease to let electron movement (to transmit electricity) in order to enhance conductance.

The arrangement of carbon atoms in a diamond is tetrahedral. With a C-C-C bond angle of 109.5 degrees, each carbon atom is sp3 hybridized and joined to four more carbon atoms that are 1.544 x 10-10 meters apart. It is a robust, inflexible three-dimensional structure that produces an endless atomic network.

A is accurate since ionization energy drops down the group and group 1A atoms are big and quickly lose electrons.