Introductory Chemistry Study Set 7

The Lewis electron diagram of an atom is shown below. This atom has a valence shell configuration of ns²np¹.

Electronegativity is a unitless number

The following is the accurate Lewis electron diagram for a P atom.

When electrons are transferred to a central atom to form a compound, a covalent bond is formed.

Lone electron pairs are electrons that do not make covalent bonds.

BeCl₂ is an example of an electron deficient molecule.

O is the central atom in an H₂O molecule.

The equal sharing of electrons in a covalent bond is called a nonpolar covalent bond.

Most odd electron compounds are chemically inactive.

The measured strength of ionic bonding is called the lattice energy.

A Cl^- ion has fulfilled the octet rule of valence electrons.

NO₂ is an example of an odd electron molecule.

A Na atom needs to gain two electrons to fulfill the octet rule.

The H−H bond is an example of a covalent bond.

A C-H bond is a nonpolar covalent bond.

A Lewis electron dot diagram represents only the protons of an atom.

The following is the accurate Lewis electron diagram for a carbon atom.

A bond will definitely be polar covalent if the electronegativity difference between the atoms involved is 1.4.

An ionic bond is formed between two atoms with the same charge.

Strength of an ionic bond decreases with an increase in the magnitude of the charge.