Group 14 elements: the carbon family

Introduction:
The carbon family elements in the periodic table that belong to the Group 14 or the IV A family are carbon (C), silicon (Si), germanium (Ge), tin (Sn), lead (Pb) and Ununquadium (Uuq). The carbon family is unique in having one metal, three metals and two metalloids.

Properties of individual elements of the carbon family may be represented by the table below

Name of the Element	Represented by symbol	Atomic number	Atomic weight	Type	Electronic configuration of the elements
Carbon	C	6	12.011	Non-metal	[He]2s22p2
Silicon	Si	14	28.0855	Metalloid	[Ne]3s23p2
Germanium	Ge	32	72.61	Metalloid	[Ar]3d104s24p2
Tin	Sn	50	118.710	Metal	[Kr]4d105s25p2
Lead	Pb	82	207.2	Metal	[Xe]4f145d106s26p2
Ununquadium	Uuq	114	289	Metal	[Rn]5f146d107s27p2

The electronic configuration in the valence shells of the carbon family elements is ns², np².  Sharing of electrons is seen in most of the elements of the carbon family. As the size of the atom is increased, the tendency of the elements to lose electrons decreases. Similarly, the tendency of losing electrons decreases with the increase in the atomic number among the elements of the carbon family. The oxidation states of the elements in the carbon family are usually +4 and +2 for heavier elements because of the inert pair effect.

Individual elements in the carbon family:

Carbon: The first element known to humans and is the fourth most abundantly found element. Carbon exists both in elemental form and as allotropes, the most common being diamond and graphite.
Silicon: Crystalline metalloid that forms the foundation for the age of semiconductors. The common compound SiO₂ is abundantly found in earth’s crust.
Germanium: Used in manufacturing of semi-conductor devices. Rarely present in earth’s crust.
Tin: When pure, the metal is silvery white and is very soft. Forms low-melting alloys called solders that connect electric circuits.
Lead: Readily combines with the oxygen in the air forming Pb₂O, which results in the dulling of the surface on exposure to air.

Conclusion on carbon family:

The elements in the carbon family include a non-metal, two metalloids and three metals, varying greatly in their physical and chemical properties. These elements occur as elemental forms and in the form of compounds in nature. The elements of Group 14 are relatively non-reactive and usually tend to form covalent compounds with exceptions of tin and lead that form ionic compounds.

Common chemical formulas

Introduction: 

In order to study or describe the elements and molecules in simpler forms, chemical formulas are extensively used. For example simplest formula for water is H₂0, where H represents hydrogen and O is oxygen and subscript ₂ indicates the two atoms of hydrogen element joined together to form a molecule.

Applications of chemical formulas

• It is used to explain the kinds of atoms and their numbers in compound (or an element).
• The atoms of every element are characterized by different letters.
• A subscript is used when more than one atom present in a specific element
• It states the chemical composition of a compound by means of chemical symbols

Common chemical formulas for everyday substances and some common acids

NaCl- Table salt, NH₃ (Ammonia) and CH₄ (methane) used for cleanser and a gaseous fuel, C₆H₁₂O₆ - table sugar or glucose, Air contains mixture of N₂, O₂, CO₂, and other traces gas, H₂O₂ (hydrogen per oxide)- used as a antiseptic and to bleach or lighten hair, Aspirin - C₉H₈O₄, Hydrochloric acid (HCl),Nitric acid (HNO₃),Hydrocyanic acid (HCN), Perchloric acid (HClO₄), Sulfuric acid (H₂SO₄),Carbonic acid (H₂CO₃)

Some important common chemical formulas are given below

Acetic acid - CH₃COOH, Acetone - CH₃COCH₃, Ammonium hydroxide - NH₄OH, Aspirin - C₉H₈O₄, Benzene - C₆H₁₂, Boric acid - H₃BO₃,Butane - C₄H₁₀, Caffeine - C₈H₁₀N₄O₂, Calcium carbonate - CaCO₃, Calcium chloride - CaCl₂, Calcium hydroxide - Ca(OH)2, Calcium oxide – CaO, Calcium sulfate - (CaSO₄), Glucose - C₆H₁₂O₆, Hydrochloric acid - HCl, Hydrofluoric acid - HF, Magnesium sulfate - MgSO₄, Manganese dioxide - MnO₂, Methane - CH₄, Naphthalene - C₁₀H₈, Oxalic acid - H₂C₂O₄ , Potassium nitrate - KNO₃, Potassium sodium tartrate - NaKC₄H₄O₆ , Potassium oxide - K₂O, Potassium sulfate - K₂SO₄, Sodium bicarbonate - NaHCO₃, Sodium chloride – NaCl, Sodium hydroxide - NaOH, Sodium sulfate - Na₂SO₄, Sodium phosphate - Na₃PO₄, Sodium tetraborate - Na₂B₄O₇, Sucrose - C₁₂H₂₂O₁₁, Sulfuric acid - H₂SO₄, Water - H₂0, Zinc chloride- ZnCl

Chemical compounds

Introduction:
We are going to see about the important chemical compounds.  A chemical compound is one of the pure chemical substance composed of molecules and formed combination of more than one different chemically bonded chemical elements.  Elements are more stable when the compounds are combined to form together.  Some important chemical compound names are organic compound, inorganic compound, biomolecules, organometallic compounds and so on.

Organic compound- Important chemical compound

Some important chemical compounds are
Acetaldehyde:  It is an organic chemical compound and also occurs in coffee.  The general formula is CH₃CHO.
Benzene:  Benzene is also an organic chemical compound and it is flammable liquid.  General formula is C₆H₆.
Butene:  Butylene or butene is an chemical compound.  It is colorless gas.  General formula is C₄H₈.
Ethene:  Ethylene or ethene is one of the chemical compound.  It is flammable gas and colourless.  The general formula of ethene is C₂H₄.
Formic acid:  Methanoic acid or formic acid is the carboxylic acid.  The general formula of formic acid is HCOOH.

Inorganic compound- Important chemical compound

Some important chemical compounds are
Aluminium chloride:  Aluminium chloride (AlCl₃) is the combination of aluminium and chlorine.
Ammonia:  Ammonia (NH₃)is the chemical compound.  It is colourless gas and pungent odour.
Calcium chloride:  It is one of the important chemical compound.  CaCl₂ is the combination of calcium and chlorine compounds.
Chromic acid:  Collection of compounds. It is a powerful oxidized agent.
Gallium phosphate:  GaPO₄ or (gallium orthophosphate) is a colourless crystal.
Hydrogen chloride:  HCl  combination of hydrogen and chlorine atom and soluble in water.
Magnesium oxide:  MgO is a moisture absorbent.  It used as raw material for making cement.
Nitrogen monoxide:  It is a chemical compound with chemical formula NO.
Biomolecules:

Some important chemical compounds are
Acetic acid:  The general formula is CH₃COOH.  It is pungent smell and sour taste.
Cellulose:  The general formula is C₆H₁₀O₅.  It is one of the organic compound.

Air chemical equation

Introduction :

Air is usually made up of a mixture of so many gases. Air comprises slightly over 20% of oxygen (O₂) and in relation to 78% nitrogen (N₂). Air also contains surplus quantities of Carbon Dioxide (about 0.03%) and even smaller quantities of other inert gases like Helium, Neon, Argon, etc. It has some low level Ozone O₃. Air usually exists as a mixture of all these gases it does exist in the compound form. It also contains small and varying quantity of water vapor. Which we are looking as clouds in the sky.The air chemical equation are give in Table 1

Air chemical equation:Chief constituent of gases

The chief constituent of air is nitrogen gas followed by oxygen

The first two gases nitrogen and oxygen make up 99.0% of the atmosphere by volume.

Nitrogen is moderately inert because of its strong triple bond holding the atoms jointly in the molecule. Whereas, the oxygen gas is synthesized by photosynthesis and removed by combustion and respiration.

Types of Air chemical equation:

The types of air chemical equation as follows

Reaction with Acetaldehyde: Oxygen gas is used in the preparation of acetaldehyde (ethanol) involves the following steps.

2CH₃CH₂OH + O₂ →2CH₃CHO + 2H₂O

Further oxidation of ethanoic acid with give rise to acetic acid which on further oxidation with carbon dioxide and water takes place on burning.

2CH₃CHO + O₂ → 2CH₃COOH

Reaction with Aluminum: Secondly oxygen reacts with aluminum metal

Aluminum metal undergoes a combination reaction with O₂ (g).

4Al + 3O₂ →2Al₂O₃

Reaction with Copper hydroxide: Copper (II) hydroxide degraded into copper (II) oxide and water when heated.

Cu (OH) ₂ → CuO + H₂O

Reaction with Heptanes: Heptanes, burns in air to give carbon dioxide

C₇H₁₆ + 11O₂ → 7CO₂ + 8H₂OH

Reaction with methyl ter butyl ether: The gasoline additive MTBE (methyl tert-butyl ether), C₅H₁₂O₂ (l), burns in air.

C₅H₁₂O₂ + 7O₂ →5CO₂ + 6H₂O

Physical properties of Air chemical equation:

• Oxygen exhibits its Compressibility that is isothermal properties with the chemical compounds.
• Oxygen shows high conductivity towards air, water, and other fluids.
• It has high density gradient against air, water and other fluids, various solids and other common liquids.
• It is relatively rough to handle because of its high tensile strength.

Check my best blog Types of chemical reactions.

Types of chemical reactions

Introduction :
Chemical reaction is defined as the changing one set chemical reactions into other set of chemical reactions. There is no need to give input to the chemical reactions. Chemical reactions involves the transfer of electrons and the formation of chemical bonds. Reactants are the substance which are involved in the chemical reactions. Nuclear reactions are also takes place in the chemical reactions. There are three types of chemical reactions are present.

Different Types of Chemical Reactions:

There are three types of chemical reactions are present. The three types are defined in the following,
Oxidation reaction and reduction reaction:
Oxidation and reduction reaction are defined as one substance gets oxidised and the other substance gets reduced. Simply it is defined as the loss or gain of electrons. Some of the examples involves in this type of chemical reaction are,
1. Iron and oxygen reaction:
In this example, the ion reacts with the oxygen and it produces oxide. In this the oxidised substance is iron. The chemical reaction is as follows,
4Fe + 3O₂ `->`  2Fe₂O₃
Where
            Fe = iron
            O₂ = oxygen
            2Fe₂O₃  = oxide
2. Ethanol and oxygen reaction:
In this example, the ethanol reacts with the oxygen, thus producing an acid called ethanol. In this the oxidised substance is ethanol.
CH₃ CH₂ OH + [ O ]    `->` CH₃COOH
Where,

CH₃ CH₂ OH = ethanol

[ O ] = other chemicals

CH₃COOH = ethanoic acid

Acid – Metal oxide Reaction:
The formation of salt and water by using the reaction of acid and the metal oxide is called as the acid – metal reaction. The example of chemical reaction is, The acid hydrochloric acid reacts with the metal oxide iron oxide,thus producing  iron chloride and solvent water
3HCl + Fe₂O₃ `->` FeCl₃ + 3H₂O

HCl = hydrochloric acid

Fe₂O₃ = iron oxide

FeCl₃ = iron chloride

H₂O = water

Three types of chemical reaction

Acid – Base Reactions:
The formation of salt and water by using the reaction of acid and base are called as the Acid-Base reactions. The examples for this chemical reaction are ,
The acid hydrochloric acid reacts with the base sodium hydroxide, thus producing a salt called sodium chloride and solvent water
HCl + NaOH NaCl + H₂O
Where,
HCl = hydrochloric acid
NaOH = sodium hydroxide
NaCl = sodium chloride
H₂O = water

Another example,
The acid sulphuric acid reacts with the base potassium hydroxide, thus producing a potassium sulphate and the solvent water
H₂SO₄ + 2KOH K₂SO₄ + 2H₂O
Where,
H₂SO₄ = sulphuric acid
KOH = potassium hydroxide
K₂SO₄ = potassium sulphate
H₂O = water

Ionization energy periodic table

Ionization energy is the electrostatic attraction that changes the trend in the groups and periods of a periodic table

Introduction to Ionization energy periodic table

Ionization energy is the minimum amount of energy required to remove an electron from the outermost orbit of an atom to the minimum distance from the atom so that no electrostatic interaction exists between the separated electron and the cation so formed.

explanation for Ionization energy from periodic table

Electrons present in an atom are attracted towards the nucleus due to the positive charge of protons. Therefore, some energy is required to remove an electron from an atom. This energy is referred to as the "Ionization Energy", as when the electron is removed from an atom, the atom is converted to a positively charged ion.
THe energy required to remove the first electron from a neutral atom is called the First Ionization energy, the energy required to remove the second electron from a positive cation is called the Second Ionization Energy, and so on.

Factors on which the ionization energy of an atom depends(periodic table)

1. Atomic size:- The greater the atomic size, the greater is the distance of the outermost shell from the protons inside the nucleus. Thus, there is lesser pull of the protons on the electrons of the last shell. Thus, the greater the atomic size, the lesser is the ionization energy of that element.
2. Nuclear charge:- Greater nuclear charge means greater attraction of the elecrons by the protons inside the nucleus. Thus, if the nuclear charge is greater, it becomes difficult to remove electrons from the outermost shell. Thus, the greater the nuclear charge, the greater is the Ionization Energy.

Varation of ionization energy in the Periodic table:-

1. Across a Period:- 
   Ionization energy of elements increases as one moves from left to right in a row of the Periodic Table.
   Reason:-As we move from left to right in a row of the Periodic Table, the number of rows in the atoms of successive elements remains the same whereas the nuclear charge increases. This causes the electrons to be attracted more strongly towards the nucleus, and hence, the ionization energy increases.
2. In a Group:-
   As one moves down a group in the Periodic Table, the ionization energy of successive elements decreases.
   Reason:-As we move down a group, the number of shells in the atoms of elements increases and the atomic number also increases. This causes an increase in the atomic size as well as in the nuclear charge. But the increase in atomic size overcomes the increase in nuclear charge, and thus it becomes more easier to remove electrons from atoms of elements as one moves down a group.

Atomic size

Introduction
 Let us discuss about the atomic size. According to modern the Atomic Theory, an atom is the minimum particle of an element which takes part in chemical reactions it maintains its identity all the way through every physical changes and chemical changes. Atoms of elements are quite reactive. They, therefore, normally do not exist in the free state except the atoms of noble or rare gases. Next we see the size of an atomic.

Atomic size

It has been found that the atoms of all elements are made up from three basic particles and that the atoms of different elements contain different numbers of these three particles. The particles are electron, proton and neutron. Since an atom has in general no charge, the many electrons external the nucleus is similar to the number of protons inside the nucleus. The even with microscope, they do not perceive them atoms are small.
               The atoms are generally declaring the building blocks of matter. They are very very small and do not be seen even by the majority of powerful microscope. An idea of the extremely small size of the atom can be had from the fact that 1cm of space can accommodate about 35,000,000 atoms arranged end to end in a line. The atomic radius is called as size of the atom is indicated by its radius. The atomic radius of the smallest atom, hydrogen is 0.37 x 10^-10 m or 0.037 nm. The nm is normally declaring the nanometer.
              The 1nm is normally declare the 1nm=10^-9 m or 10⁹ nm = 1 m. The small dimensions of hydrogen atom or atoms in general can be seen as compared with the size of some common objects given in the following table.

Relative sizes of some common objects

Relative sizes
Radii	Examples
10-1 m 10-2 m 10-4 m 10-8 m 10-9 m 10-10 m	Watermelon Ant Grain of sand A molecule of haemoglobin A molecule of water An atom of hydrogen