Difference between a Mixture and a Compound - Essay Example

Another way to differentiate mixtures and compounds is the ease of separation of elements (“Elements, Compounds and Mixtures”, n.d.). Mixtures can be separated easily through physical separation while chemical compounds can only be separated by destroying the compound.

Element is any substance that contains only one kind of atom and cannot be broken down into simpler types of matter either by physical or chemical means (“Elements, Compounds and Mixtures”, n.d.). If we have a pure substance, we can tell whether it is a compound or an element by asking the question “Can the substance be further decomposed by chemical means?” If the answer is yes, then it is a compound. If the answer is no, then it is an element.

An ionic bond is a bond in which one or more electrons from one atom are removed and attached to another atom, resulting in positive and negative ions which attract each other (“Chemical Bonding”, n.d.). A covalent bond is a bond in which one or more pairs of electrons are shared by two atoms (“Chemical Bonding”, n.d.). These two bonds differ in structure and properties.

Covalent bonds have low polarity while ionic bonds have high polarity. Covalent bonds have a definite shape and ionic bond has no definite shape. When it comes to the melting point, covalent bonds have a low melting point while ionic bond has a high one. Another difference between the two bonds is their boiling point a covalent bond has a low boiling point while an ionic bond has a high boiling point (“Covalent Bonds vs. Ionic Bonds”, 2011).

An ionic bond is formed when a metal attracts a non-metal. Non-metals are “stronger” than metal and can get electrons very easily from that metal. These two opposite ions attract each other to form an ionic bond (“Covalent Bonds vs. Ionic Bonds”, 2011).

Examples: Sodium chloride (NaCl), Sulphuric Acid (H2SO4).

A covalent bond is formed when non-metals from the right side of the periodic table bond with each other because they have similar electronegativities. This is because there are no atoms strong enough to attract electrons from others. They share their electrons from outer molecular orbit with others (“Covalent Bonds vs. Ionic Bonds”, 2011).

Examples: Water (H2O), Methane (CH4).