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Introduction
 
Matters and Properties of Matters
 
--Classification of Matters with Examples
 
--Decomposition of Compounds and Mixtures
 
--Phases(States) of Matters with Example
 
--Properties and Naming Simple Compounds (Nomenculature) with Example
 
--Matters and Properties of Matters Cheatsheet
 
Atomic Structure with Examples
 
Periodic Table
 
The Mole Concept with Examples
 
Gases with Examples
 
Chemical Reactions with Examples
 
Nuclear Chemistry (Radioactivity)
 
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Properties and Naming Simple Compounds (Nomenculature) with Example


Properties and Naming Simple Compound with Examples

More than one element come together and comprise compounds. As we discussed in previous topics, compounds are pure substances. Building blocks of compounds are molecules including more than one elements.

H2O

H2+1/2O2→H2O

H2: Molecule

O2: Molecule

We examine naming in two steps, first we learn how to write simple formula, then we learn real (compound, molecule) formula.

1. Simple Formula: We can understand types of elements and ratio of them from simple formula. On the contrary, we can not understand physical and chemical properties of matter by looking at its simple formula.

(NO2)n

(CH2)n

(NO2)n

where n is variable.

2. Real Formula: Types of elements and "n" number in the simple formula is given in real formula.

C6H12O6: Real Formula

(CH2O)n: Simple Formula where n=6

Real formula gives us:

  • Types of compound
  • Types of elements
  • Molecule mass of compound
  • "n" number in the simple formula

We first examine compounds formed by two elements or binary compounds. One metal can not form compound with another metal. Thus, if one of the elements is metal, then other one must be nonmetal or two of the elements must be nonmetal to form compound. Oxygen is one of the elements joining structure of most of the compounds. Let me explain compounds including oxygen first.

a) Nonmetal+Oxygen Compounds:

We first say name of nonmetal element then number of oxygen atoms in the compound and word "oxide". For example;

I. CO: Carbon Monoxide (one carbon atom and one oxygen atom)

II. CO2: Carbon Dioxide (one carbon atom and two oxygen atoms)

III. P2O5: Phosphor Penta Oxide (two Phosphor atom and 5 oxygen atoms)

In first example, we do not write mono in front of Carbon atom, in general number of atoms does not written in front of first element. However, there are some exceptions;

NO, N2O

If we say nitrogen monoxide to first compound, and second compound we can mix them. Thus, we must put "di" in front of nitrogen in second compound.

NO: nitrogen monoxide

N2O: di nitrogen monoxide

Prefixes we use in naming compounds are;

one: mono            five: penta              nine: nona

two: di                  six: hexa                ten: deca

three: tri               seven: hepta

four: tetra             eight: octa

b) Metal+Oxygen Compounds:

Naming these compounds are different from naming nonmetal+oxygen compounds. Prefixes given above are not used in naming these compounds. On the contrary, oxidation number of metals are given in these compounds if necessary. Better understanding examine following examples;

CaO: Calcium Oxide (Since calcium has one oxidation number +2, we do not write it.)

Cu2O :Copper I Oxide

CuO: Copper II Oxide   (Since copper has two oxidation number we write them.)

Na2O: Sodium Oxide

Al2O3 aluminum oxide

FeO: Iron (II) Oxide

Fe2O3: Iron (III) Oxide  (Iron has two oxidation numbers +2 and +3 thus we must mention oxidation numbers)

c) Nonmetal+Nonmetal Compounds:

In these types of compounds, you must first write element having "+" oxidation number and then "-" number of atoms in second nonmetal element or more metallic element is written first. You must also add "ide" suffix after second element.

CS2: Carbon disulphide

CCl4: Carbon tetra chloride

ICl: Iode mono chloride

PI3: Phosphorus tri iodide

P2S5:(Di) Phosphorus pentasulfide

d) Metal+Nonmetal Compounds:

In naming metal+nonmetal compounds, we do not say number of atoms in elements, however, we must say oxidation number of elements if it has more than one oxidation number. Finally, as in the previous examples, we must ad "ide" suffix after second element. Examine following examples for better understanding;

MgI2: Magnesium Iodide

FeBr2 : Iron II Bromide

FeBr3: Iron III Bromide

NaCl: Sodium Chloride

e) Naming Binary Acids:

If a binary compound dissolves in water and contains H atom, we call these compounds as acid. When naming these acids we follow given steps. Hydro+nonmetal element+"ic" suffix+ acid

Examples:

HCl: Hydrochloric acid

HBr: Hydrobromic acid

HI: Hydroiodic acid

H2S: Hydro sulfuric acid

f) Some Common Polyatomic Ions:

NH4+ Ammonium

OH- Hydroxide

CO3-2 Carbonate

PO4-3 Phosphate

SO4-2 Sulfate

SO3-2 Sulfide

NO3- Nitrate

NO2- Nitrite

Example: Which one of the following name of compound is false.

I. Hg2Cl2 Mercury I Chloride

II. NO3 Nitrogen Trioxide

III. K2S Potassium Sulfide

IV. CO Carbon Monoxide

V. NaCl Sodium Chlore

In ionic compounds we first write cation then write anion. We add "ide" suffix after anion, thus in V. Name of compound must be;

NaCl=Sodium Chloride

I, II, III and IV are true.


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