Define each chemical bond. Explain the differences of each bond. In an ionic bond, a positive and a negative atom are attracted. These atoms have a charge and are known as ions. A positive ion has less electrons, and a negative ion has more electrons. Lithium iodide is an ionic bond. In a covalent bond, the electrons are shared. Hydrogen bromide is a covalent bond. Bromine has seven valence electrons, and hydrogen has one. The single valence electron of hydrogen completes the octet of bromine. In a metallic bond, the electrons move freely. Cesium has metallic bonds. A hydrogen bond describes the attraction between hydrogen and nitrogen, oxygen and fluorine. Nitrogen, oxygen and fluorine have high electronegativity and therefore strongly attract the less-electronegative hydrogen.
Explain single, double and triple bonds. Covalent bonds can be formed eitherby sharing one pair of electrons, two pairs of electrons or three pairs of electrons. Bromine is a single bond and shares one pair of electrons. Carbon can be double bonded to another carbon and therefore shares two pairs of electrons. One atom of nitrogen is triple bonded to another atom of nitrogen, forming a triple bond.
Describe bond polarity. The polarity refers to a difference in positive charge or negative charge for a compound that has a covalent bond. A compound does not have a dipole moment, or any overall polarity, if it is a diatomic molecule. Therefore, bromine bonded to bromine is nonpolar. However, hydrogen bromide is polar. The bromine is more electronegative than the hydrogen. The bromine has a partial negative charge, and the hydrogen has a partial positive charge.
Explain intermolecular forces, which are attractions between molecules. Van der Waals forces are examples of intermolecular forces and also are known as dispersion forces. Hydrogen bonds may be classified as intermolecular forces.