Jan 17 Chemical Bonding Overview

The compound formed when magnesium (Mg) loses two electrons and chlorine (Cl) gains one electron each, forming a 1:2 ratio.

Sodium (Na) loses one electron, while sulfur (S) gains two electrons, resulting in a transfer of two electrons.

A positively charged ion formed when an atom loses electrons.

The simplest whole number ratio of atoms in a compound, in this case, two aluminum (Al) atoms to three oxygen (O) atoms.

Ionic compounds are formed through the transfer of valence electrons from a metal to a nonmetal, leading to the formation of oppositely charged ions which attract each other.

The ionic radius is smaller than the atomic radius of the neutral atom because the loss of electrons results in a stronger attraction between the remaining electrons and the nucleus.

The electronic configuration of Mg2+ ([Ne]) is similar to the noble gas neon because it has lost its two valence electrons.

Ionic compounds are formed primarily by the electrostatic attraction between positively charged metal ions and negatively charged nonmetal ions.

Group VIIA, also known as halogens, have a high tendency to gain an electron to achieve a stable noble gas configuration.

Calcium (Ca) belongs to Group IIA and loses two electrons to form a +2 cation.

Nonmetals from Group V, like phosphorus (P), gain three electrons to form a -3 anion (P3-).

When a Group IIA element forms a cation, it loses all its s and p valence electrons, resulting in the outermost shell becoming empty.

Carbon (C) can share its valence electrons with other atoms to form covalent bonds, unlike typical metals which form ionic bonds by electron transfer.

Ionic bonding involves the transfer of electrons from a metal to a nonmetal, resulting in the formation of oppositely charged ions that attract each other.

Covalent bonds are formed when two nonmetals share electrons.

H2O (water) is a molecule formed by the sharing of electrons between hydrogen (H) and oxygen (O), indicating covalent bonding.

Metals are known for their ability to conduct electricity due to their delocalized valence electrons, forming a 'sea of electrons' that can move freely.

Metals and nonmetals have a significant difference in electronegativity, leading to a transfer of electrons and formation of ionic bonds.

Valence electrons are the outermost electrons in an atom and participate in chemical bonding.

Ionic bonds are formed by the electrostatic attraction between oppositely charged ions.

Lewis Electron-Dot Symbols represent the valence electrons of an atom.

HCl is formed by the sharing of electrons between hydrogen and chlorine, indicating a covalent bond.

Ionic compounds are generally crystalline solids at room temperature due to the strong electrostatic forces holding the ions together.

Covalent bonds are formed by the sharing of electrons between nonmetals.

Lewis Electron-Dot Symbols represent the valence electrons of an atom and the noble gas core. They do not correspond to the noble gas configuration.

Salts are ionic compounds formed from the reaction of an acid and a base.

A cation's size decreases with an increase in its positive charge due to a stronger attraction between the remaining electrons and the nucleus.

Ca2+ has the same number of electrons as argon.

Anions become larger with increasing negative charges due to greater electron-electron repulsion.