Hydrogen bond

 Hydrogen bond is a weak bond between two molecules by the weak attraction between a partially charged positive ion with partially charged negative ion. Though, vander walls attraction force is also a weak attraction force, but it have a wide difference from hydrogen bond.

Hydrogen bond occurs between two polar compound. The molecules that shows polarity undergoes into hydrogen bond.

How water molecules are bonded with each other? Why water molecules are not gaseous? 

Vaporization can make water to undergo into gaseous state. Water is exist as liquid state. When water is heated the temperature increases, kinetic energy of particles increases. At the same time inter molecular attraction force decreases. When temperature reaches into melting point, each molecules aparts from each other. In that case hydrogen bond breaks down.

Ionic bond

 Ionic bond is a type of chemical bond that forms by attraction between two oppositely charged ion.

Positively charged ion and negatively charged ion attract each other and forms a bond.

According to octate rule each atom wants to be highest level of stable, to do this atom tend to achieve stable outer most electronic configuration.

Metal releases electron and turn into positive ion, non metal element accept this electron and turns into negative ion. Positive ion and negative ion attract each other.

Octate role

 Octate role is a principle of electron being number eight in outer most electronic shell. Any atom tends to be highest stable electronic configuration. When outer most electronic shell of an atom be eight in number or two in number it became highest stable. 

To be stabilise any atom tends to donate electron or accept electron and to form ion. When atom donate electron the number of proton in nucleus became greater than the electrons in orbits. Hence, atom looses its neutrality and be cation. When atom accepts electron then it convert into anion which is negatively charged. 

In a covalent bond when electrons of different atom in covalent bond share electrons then each atom became stable electronic configuration. 

Periodic table

Periodic table is an arrangement of elements with its properties as same way that chemical properties of elements belongs same in same group and same period. for example, all hallogen are placed in group 17. All of the innert gas are in group 18. 

 Atomic number is the basis of periodic table, though at the innitial stage of development of periodic table atomic mass was the basis of periodic table.

Periodic table is a table of rearrangement of chemical elements with the basis of these properties. 

In a periodic table elements are rearranged with their properties.

Periodic table consists with period and coloumn.

The horrizontal line is period and the verticle line is coloumn.

Left to right in a period atomic number increases as same as top to bottom in a group atomic number increases.

Left to right in a period atomic size decreases on the other hand top to bottom in a group atomic size increases.

Innert gas are placed in group zero.

In a period table  there also exist diagonal relationship.

The electronegativity increases by top to bottom in a group and decreases left to right in a period.

Ionization energy also increases top to bottom in a group and increases  left to right in a period.

Outer most electronic shell

 According to Rutherford atomic model within an atom central positive charged ion is nucleus that consists with proton, neutron and other essential elementary particles. Nucleus is surrounded by electron by same number of proton exist. Electron revolve surrounding nucleus by an elliptical path. Eleptical paths are preserved for specific number of electron. These are called electronic shell. 

The electronic shell are identified as K, L, M, N

The most farest electronic shell is called outer most electronic shell.

Innert gas

 Elements of group 18 in a periodic table is called innert gas. Innert gas is chemically inactive and does not go into chemical reaction.  Due to its inactivity in chemical reaction it is called innert gas. 

The examples of innert gas is Helium, Neon, Argon, Crypton, Xenon and Redon.

Elements wants to be achieve highest stability outer most electronic configuration will follow Octate rule. In case of Helium doublet rule is observed. 

Due to its stable electronic configuration it does not form any cation or anion. Hence, no ionic bond is formed. Not only that no electron sharing caused to form any covalent bond. 

This is noticeable that highest stabilised elements are usually gaseous elemens. There have certain cause of highest stable elements be gaseous.

Atomic Number

 Atomic number is an unique identification number of any atom that determines the properties of atom. Atomic number is considered as the basis of periodic table. 

Though, atomic mass was considered as the basis of periodic table at the innitial stage of periodic table. But in that case, potassium is placed in innert gas group and Argon is placed with alkaline metal. 

When rearrangement is done by atomic number the problem solved.

Basically, Atomic number is nothing but a proton numbet. Though, proton number and electron number is considered as same in a neutral atom, electron number is not the atomic number. Electron number may change, but proton number may not change.

Electron affinity

 Electron affinity is the capability of an atom to convert into negatively charged ion by attracting eletron in its outer most electronic shell from outside. 

To being a stable outermost electronic configuration atom tends to accept or donate electron. 

The difference between electronegativity and electron affinity is that, electron affinity is capability to accept any outershell electron to convert into negative ion. But electronegativity is capability of attracting electron cloud from an atomic bond. 

Ionization energyis opposed to electron affinity. While energy to form positive charge is ionization energy, the required energy to form negative ion is called electron affinity.

Atomic size

 Atomic size is determined by the radius of outermost electronic shell. According to Rutherford atomic model, electron revolve surrounding the nucleus in a circular orbit. Nucleus is the center of circle, the distence between nucleus and outermost electron is called atomic radius. The more atomic radius indicates bigger atomic size. 

If atomic number increases, but electronic shell remain same, atomic radius decreases due to increased electrostatic force of attraction.

On the other hand more atomic number with the number of electronic shell or orbit increases the atomic size.

Electronegativity is dependent on atomic size. The bigger the atomic size indicates highest electronegativity. But with the increase of size ionization energy decreases.

Due to electronegativity difference electron cloud within a covalent bond tends to closer to more electronegative atom. Hence, dipole creates as a results of polarity. 

Hence, Ionic properties of covalent compound excerts for the polarity of compound.

Electron affinity also depends with atomic size. The more bigger atom shows less electron affinity.

Ionization energy

Ionization energy is required energy for an isolated atom to release an electron from its outer shell orbit to make ion converting into innert gas stabilized condition. The required energy is measured as coulamb or Jole. When a one electron is released from an atom then atom convert into positively charged ion. Ionization energy may be First ionization energy and second ionization energy or more. The required energy to release only one loosely bounded electron is called First ionization energy.

Ionic properties of covalent bond

Covalent bond is a bond build up two or more atoms only with sharing of electron. Here, no electron donation and acceptation occurred. Though, no atom electron donate and no atom electron accept, atoms are in covalent bond usually should charged neutral. But, due to electronegativity differrence more electronegative atom became partially negatively charged. Hence, it shows a little bit of ionic characteristics.

Polarity in a covalent compound is a cause of parially being charged of atom due to difference of electronegativity electron cloud being difference in different atom.

Polarity

Polarity is a characteristics of any molecule of creating two oppositely charged portion in a covalent bond compound. Due to difference in electronegativity in a covalent compound, more electronegative atom or molecule belongs more electron density. Electron cloud tends more closer to more electronegative atom. Hence, it is partially negatively charged. partially charged atom is not as same as charged atom in ionic bond. Another atom in the compound are in partially positive charged. The compound that have polarity is called dipole. Polarity creates

Ion

Ion is the charged state of an atom. On the other hand any charged atom or molecule is called ion. Molecule or single atom is charged nutral, the number of proton and number of electron is equal in number. Any deviation in that number is termed as charged. When molecule or atom belongs electron number than proton number, then it is negatively charged ion. When molecule or atom belongs greater proton number than electron is termed positively charged ion. Both a single element or molecule can form Ion except innert gas, because it does not do any reaction and maintain its highly stable condition. In octate rule and doubled rule elements rends to be highly stabilised to their outer most electronic configuration.