This particular resource used the following sources:. Skip to main content. Nonmetallic Elements. Search for:. Types of Bonds. Learning Objective Describe the types of bonds formed between atoms. Key Points Nonmetals can form different types of bonds depending on their partner atoms. A covalent bond involves a pair of electrons being shared between atoms. An example of an ionic compound is the sodium chloride , NaCl. An ionic compound will be made up of both positive and negative ions. Therefore, the oppositely charges ions in an ionic compound combines and balancing each other out resulting in a net charge of zero 0.
Conversely, an ionic compound that has hydroxide OH — or oxide O 2- is classified as a base. An ionic compound formed by acid-base reactions and without those ions is called a salt. While covalent bond involves the sharing of electrons between atoms, an ionic bond involves the transferring of electrons from one to another in order to achieve the stable configuration. Here is a tabulated summary of the major differences between ionic bond and covalent bond: 1.
It is argued that no absolute transferring of electrons exists and that an ionic bonding has some sort of covalent character in it. Nevertheless, a chemical bond that appears to be more of an ionic than a covalent, then it is deliberated as an ionic bond. One of the ways to tell that a bond is ionic is by looking at the electronegativity.
The larger the difference in electronegativity between the two atoms is, the more ionic it is. As the name implies, a hydrogen bond is a chemical bond wherein hydrogen serves as a bridge between two atoms. Similar to the ionic bond, the hydrogen bond entails an electrostatic force. To form ionic bonds, Carbon molecules must either gain or lose 4 electrons.
This is highly unfavorable; therefore, carbon molecules share their 4 valence electrons through single, double, and triple bonds so that each atom can achieve noble gas configurations. Covalent bonds include interactions of the sigma and pi orbitals; therefore, covalent bonds lead to formation of single, double, triple, and quadruple bonds.
In this example, a phosphorous atom is sharing its three unpaired electrons with three chlorine atoms. In the end product, all four of these molecules have 8 valence electrons and satisfy the octet rule. Ionic and covalent bonds are the two extremes of bonding. Polar covalent is the intermediate type of bonding between the two extremes. Some ionic bonds contain covalent characteristics and some covalent bonds are partially ionic.
For example, most carbon-based compounds are covalently bonded but can also be partially ionic. Polarity is a measure of the separation of charge in a compound. A compound's polarity is dependent on the symmetry of the compound and on differences in electronegativity between atoms. Polarity occurs when the electron pushing elements, found on the left side of the periodic table, exchanges electrons with the electron pulling elements, on the right side of the table.
This creates a spectrum of polarity, with ionic polar at one extreme, covalent nonpolar at another, and polar covalent in the middle. Both of these bonds are important in organic chemistry.
Ionic bonds are important because they allow the synthesis of specific organic compounds. Scientists can manipulate ionic properties and these interactions in order to form desired products. Covalent bonds are especially important since most carbon molecules interact primarily through covalent bonding.
Learn about the basic structure of an ion, related to atomic number and mass. Ionic bonds are formed between a metal and non-metal, for example sodium chloride. An atom of sodium will lose an electron and form a positive ion.
An atom of chlorine will gain an electron and form a negative ion. The ionic bond is the electrostatic force of attraction between a positively charged metal ion and a negatively charged non-metal ion.
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