What types of bonding are present in H3O+?

Covalent and co-ordinate.

Related Questions:

(1) The maximum number of hydrogen bonds formed by a water molecule in ice is.

(2) What is the temperature at density of water is maximum ?

(3) Why ice floats on water at room temperature ?

(4) Why density of water is greater than ice ?

(5) What is "Nascent" Hydrogen ?

(6) How many hydrogen bonded water molecules are present?

(7) Water is generally a good solvent for ionic compounds. Why?

Water is generally a good solvent for ionic compounds. Why?

Water is a polar compound with a high dielectric constant (81). Hence, it decreases the electrostatic forces of attraction acting between the oppositely charged ions in an electrovalent compound. Therefore, the ions are separated and dissolution occurs. Dissolution of electrolytes in water is also favoured due to hydration of ions.

Related Questions:

(1) The maximum number of hydrogen bonds formed by a water molecule in ice is.

(2) What is the temperature at density of water is maximum ?

(3) Why ice floats on water at room temperature ?

(4) Why density of water is greater than ice ?

(5) What is "Nascent" Hydrogen ?

(6) How many hydrogen bonded water molecules are present?

 

Oxy acids of Sulphur:

 Oxidation state of sulphur atom and respective oxy-acids:

Oxidation state	Series name	Prefix of acid	Name of acids
(+2)	“us”series	Hypo	Hyposulphurous acid
(+4)	“us”series	…….	Sulphurous acid
(+5)	“ic”series	Hypo	Hyposulphuric acid
(+6)	“ic”series	…….	Sulphuric acid
(+7)/(+8)Cal/ava	“ic”series	Peroxy	Peroxysulphuric acid

Important Note:

(1) Ortho and meta form of sulphurous and sulphuric acid not exist but both have pyro form only.

(2) Hyposulphurous acid start thionous series and while hyposulphuric acid start thionic series;

(1) Sulphurous Series:

(A) Sulphurous acid:

(B) Hyposulphurous acid(H₂SO₂/S(OH)₂):

(C) Thiosulphurous acid(H₂S₂O₂):

(D) Pyrosulphurous acid(H₂S₂O₅=H₂SO₃+SO₂):

(2) Sulphuric acid series:

(A) Sulphuric acid(H₂SO₄):

(B) Pyrosulphuric acid(H₂S₂O₇=H₂SO₄+SO₃): Oleum:

(C) Peroxomonosulphuric acid(H₂SO₅):Caro’s acid:

(D) Peroxodisulphuric acid(H₂S₂O₈): Marshall’s acid:

(3) Thionous acid series

(4) Thionic acid series:

(A) Dithionic acid(H₂S₂O₆):

(B) Trithionic acid (H₂S₃O₆):

(C) Tetrathionic acid(H₂S₄O₆):

Related Topics:

(1) What are the oxy-acids?

(2) What are "Ortho" or "Meta" oxyacids?

(3) What are "pyro" oxy acids?

(5) Suffix – “ic-acids” , ‘us-acids” :

(6) Prefix “Hypo-acids”, and “Per-acids”:

(7) How to find oxy-linkage present in a given oxy-acid:

(8) How to pridict cyclic structure given compound/oxy-acid:

Related Questions: 

(1) What is Use of Boric Acid?

(2) What is use of Orthoboric acids?

(3) What is basicity of "Boric acid" ?

(4) Why Boric acid exist in solid state ?

(5) What is structure of solid Ortho Boric acid ?

(6) What is effect of heat on Borax?

(7) What is the structure of trimetaboric acid and trimetaborate ion?

(8) What is the Sodium per borate ,give the structure and its uses?

(9) Why aqueous solution of borax reacts with two moles of acids ?

(10) What is the molecular formula of Borax ?

(11) Why Boric acid become strong acid in the presence of cis 1,2-diol or 1,3-diol ?

(12) Why Borazine is more reactive than benzene towards Electrophic Aromatic substitution reactions ?

(13) Why Borazine (B3N3H6) is also known as inorganic benzene ?.

Why radii of Ar is greater than the radii of chlorine?

In chlorine, the radii mean the atomic or covalent radii which is actually half the intermolecular distance between 2 atoms whereas in Argon the radii means the Vander waals radii as Argon is not a diatomic molecule. Vander Waal’s radii are actually half the distance between adjacent molecule. So Vander Waal’s radii being larger than atomic radii, Argon has a larger radii than chlorine.

Related Questions:

(1) What are the Amphoteric metals ? gives Examples.

(2) Name of total metalloids present in periodic table ?

(3) Total numbers of elements which are liquid at normal temperature is ?

(4) What is Mendeleev's periodic table ? give important features and draw back of Mendeleev's table.

(5) What is atomic volume ? and what is periodicity of atomic volume in groups and periods ?

(6) Why there are 2, 8 and 8 elements in first, second and third periodic of periods table respectively ? Explain.

(7) In alkali metal group which is the strongest reducing agent in aqueous solution and why?

(8) The electron affinity of sulphur is greater than oxygen. Why?

(9) The first ionization energy of carbon atom is greater than that of boron atom, whereas reverse is true for the second ionization energy. Explain.

(10) The electronegativities of B, Al, Ga are 2.0, 1.5, 1.6 respectively. The trend is not regular. Explain.

(11) Li2CO3 decomposes on heating but other alkali metal carbonates don’t. Explain.

(12) Of all noble metals, gold has got a relatively high electron affinity. Explain.

(13) Ionization energy of Boron is smaller than Beryllium even though effective nuclear charge is higher?

(14) What are the increasing order of ioni radii of first group elements in water ?

(15) What are the increasing order of molar conductivity of first group elements in water ?

Atomic Radius:

(1)     The radius of an atom may be taken as the distance between atomic nucleus and the outermost shell of electrons of the atom.

(2)     According to the Heisenberg’s uncertainty principle the position of a moving electron cannot be accurately determined. So the distance between the nucleus and the outermost electron is uncertain.

(3)     Atomic radius can be determined indirectly from inter nuclear distance between the two atoms in a gaseous diatomic molecule. This internuclear distance between the two atoms is called bond length.

(4)     The internuclear distance between the two atoms can be measured by X– ray diffraction or spectroscopic studies and also nuclear magnetic resonance (NMR) spectrum.

(5)     Atomic radius depends on the type of chemical bond between atoms in a molecule. These are:

(i)   Covalent radius

(ii) Metallic radius or crystal radius

(iii) Vander Waal’s radius

(iv) Ionic radius or Collision radius

(6) Periodicity in Atomic Radius and Ionic Radius: 

Related Questions:

(1) What are the Amphoteric metals ? gives Examples.

(2) Name of total metalloids present in periodic table ?

(3) Total numbers of elements which are liquid at normal temperature is ?

(4) What is Mendeleev's periodic table ? give important features and draw back of Mendeleev's table.

(5) What is atomic density ? give the periodicity of atomic density in periods and groups.

(6) What is atomic volume ? and what is periodicity of atomic volume in groups and periods ?

(7) Why there are 2, 8 and 8 elements in first, second and third periodic of periods table respectively ? Explain.

(8) In alkali metal group which is the strongest reducing agent in aqueous solution and why?

(9) The electron affinity of sulphur is greater than oxygen. Why?

(10) The first ionization energy of carbon atom is greater than that of boron atom, whereas reverse is true for the second ionization energy. Explain.

(11) The electronegativities of B, Al, Ga are 2.0, 1.5, 1.6 respectively. The trend is not regular. Explain.

(12) Li2CO3 decomposes on heating but other alkali metal carbonates don’t. Explain.

(13) Of all noble metals, gold has got a relatively high electron affinity. Explain.

(14) What are the increasing order of ioni radii of first group elements in water ?

(15) What are the increasing order of molar conductivity of first group elements in water ?