Different Types Of Compounds In Chemistry

Binary Compounds

A binary compound is a chemical compound that contains exactly two different elements.[1][2] Examples of binary ionic compounds include calcium chloride (CaCl2), sodium fluoride (NaF), and magnesium oxide (MgO), whilst examples of a binary covalent compounds include water (H2O), and sulfur hexafluoride (SF6).

Ternary Compounds

In chemistry, a ternary compound is a compound containing three different elements. An example of this is sodium phosphate, Na3PO4. The sodium ion has a charge of 1+ and the phosphate ion has a charge of 3-. Therefore, three sodium ions are needed to balance the charge of one phosphate ion. Another example of a ternary compound is calcium carbonate . In naming and writing the formulae for ternary compounds, we follow rules that are similar to binary compounds.(CaCO3).

Polyatomic Compounds

A compound made up of a polyatomic ion. Most compounds are neutrally charged, such as NaCl (salt). A polyatomic ion is a compound of several atoms that leave a charge after formation (such as hypochlorite, ClO, or permanganate, MnO4). These ion compounds must form with another ion to neutralize the charge (such as sodium hypochlorite, NaClO). Hope this helps.

Acids

An acid (from the Latin acidus/acēre meaning sour[1]) is a chemical substance whose aqueous solutions are characterized by a sour taste, the ability to turn blue litmus red, and the ability to react with bases and certain metals (likecalcium) to form salts. Aqueous solutions of acids have a pH of less than 7. A lower pH means a higher acidity, and thus a higher concentration of positive hydrogen ions in the solution. Chemicals or substances having the property of an acid are said to be acidic.

Bases

In chemistry, a base is a substance that, in aqueous solution, is slippery to the touch, tastes bitter, changes the color of indicators (e.g., turns red litmus paper blue), reacts with acids to form salts, and promotes certain chemical reactions (base catalysis). Examples of bases are the hydroxides of the alkali and alkaline earth metals (NaOH, Ca(OH)2, etc.). Such substances produce hydroxide ions (OH-) in aqueous solutions, and are thus classified as Arrhenius bases.

Oxides

An oxide /ˈɒksaɪd/ is a chemical compound that contains at least one oxygen atom and one other element[1] in its chemical formula. Metal oxides typically contain an anion of oxygen in the oxidation state of −2. Most of the Earth's crust consists of solid oxides, the result of elements being oxidized by the oxygen in air or in water. Hydrocarbon combustion affords the two principal carbon oxides: carbon monoxide and carbon dioxide. Even materials considered pure elements often develop an oxide coating. For example, aluminium foil develops a thin skin of Al2O3 (called a passivation layer) that protects the foil from further corrosion.[2] Different oxides of the same element are distinguished by Roman numerals denoting their oxidation number, e.g. iron(II) oxide versus iron(III) oxide.

Ionic Bonding

Ionic bonding is a type of chemical bond that involves the electrostatic attraction between oppositely charged ions. These ions represent atoms that have lost one or more electrons (known as cations) and atoms that have gained one or more electrons (known as an anions). 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.g. molecular ions like NH4+ or SO42-

It is important to recognize that clean ionic bonding – in which one atom "steals" an electron from another – cannot exist: All ionic compounds have some degree of covalent bonding, or electron sharing. Thus, the term "ionic bonding" is given when the ionic character is greater than the covalent character—that is, a bond in which a large electronegativity difference

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