- Ionic bonding
- 2.6 Molecular and Ionic Compounds
- Covalent Bonds vs Ionic Bonds
- Ionic and Covalent Bonds
Naming Ionic Compounds with Transition Metals Introductionand how season episode
There are two types of atomic bonds - ionic bonds and covalent bonds. They differ in their structure and properties. Covalent bonds consist of pairs of electrons shared by two atoms, and bind the atoms in a fixed orientation. Whether two atoms can form a covalent bond depends upon their electronegativity i. This results in a positively charged ion cation and negatively charged ion anion.
Ionic bonding is a type of chemical bonding that involves the electrostatic attraction between oppositely charged ions , and is the primary interaction occurring in ionic compounds. It is one of the main bonds along with Covalent bond and Metallic bonding. Ions are atoms that have gained one or more electrons known as anions , which are negatively charged and atoms that have lost one or more electrons known as cations , which are positively charged. This transfer of electrons is known as electrovalence in contrast to covalence. In the simplest case, the cation is a metal atom and the anion is a nonmetal atom, but these ions can be of a more complex nature, e. In simpler words, an ionic bond is the transfer of electrons from a metal to a non-metal in order to obtain a full valence shell for both atoms.
There are many types of chemical bonds and forces that bind molecules together. The two most basic types of bonds are characterized as either ionic or covalent. In ionic bonding, atoms transfer electrons to each other. Ionic bonds require at least one electron donor and one electron acceptor. In contrast, atoms with the same electronegativity share electrons in covalent bonds, because neither atom preferentially attracts or repels the shared electrons. Ionic bonding is the complete transfer of valence electron s between atoms. It is a type of chemical bond that generates two oppositely charged ions.
In ordinary chemical reactions, the nucleus of each atom and thus the identity of the element remains unchanged. Electrons, however, can be added to atoms by transfer from other atoms, lost by transfer to other atoms, or shared with other atoms. The transfer and sharing of electrons among atoms govern the chemistry of the elements. During the formation of some compounds, atoms gain or lose electrons, and form electrically charged particles called ions Figure 1. You can use the periodic table to predict whether an atom will form an anion or a cation, and you can often predict the charge of the resulting ion.
Atomic radii generally decrease along each period row of the periodic table and increase down each group column. The atomic radius of a chemical element is a measure of the size of its atoms. It represents the mean distance from the nucleus to the boundary of the surrounding cloud of electrons. Atomic radii vary in a predictable manner across the periodic table. Radii generally decrease along each period row of the table from left to right and increase down each group column.
2.6 Molecular and Ionic Compounds
Covalent Bonds vs Ionic Bonds
Ionic and Covalent Bonds