Gaurav Gupta sir

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2021-10-12 12:08:33 Some Important Increasing Order :

1. Bond Angle :

(i) CH4 , C2H4 , C2H2
(ii) H2O, NH3 , CH4 , CO2
(iii) H2O, NH3 , CH4 , BH3
(iv) NO2—, NO2 , NO2+
(v) H2Se, H2S, H2O
(vi) AsH3 , PH3 , NH3
(vii) PF3 , PCl3 , PBr3 , PI3
(viii) NF3 , NCl3
(ix) NF3 , NH3 , NCl3
(x) OF2 , OH2 , Cl2O

2. Melting Point :

(i) Cs, Rb, K, Na, Li
(ii) Mg, Ba, Sr, Ca, Be
(iii) CaI2 , CaBr2 , CaCl2 , CaF2
(iv) BeCl2 , MgCl2 , CaCl2 , SrCl2 , BaCl2
(v) NaI, NaBr, NaCl, NaF
(vi) CsCl, RbCl, KCl, NaCl
(vii) AlCl3 , MgCl2 , NaCl

3.Boiling Point :

(i) PH3 , AsH3 , NH3 , SbH3
(ii) H2S, H2Se, H2O
(iii) HCl, HBr, HI, HF
(iv) NH3 , HF, H2O
(v) He, Ne, Ar, Kr
(vi) H2O, D2O
(vii) H2 , Cl2 , Br2

4.Dipole moments :

(i) CCl4 , CHCl3 , CH2Cl2 ,CH3Cl
(ii) NF3 , NH3 , H2O, HF
(iii) Cis-chloropropene, Trans-chloropropene
(iv) p, m, o-dichlorobenzene
(v) CH3I, CH3Br, CH3F, CH3Cl
(vi) NH3 , SO2 , H2O, HF
(vii) H2S, H2O
(viii) HI, HBr, HCl, HF
(ix) PH3 , ASH3 , SbH3 , NH3
(x) H2O, H2O2 Open / Comment

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2021-10-09 11:51:07 Important One Liners on Electric Charges
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If an object is attracted by another charged body, the first object may be oppositely charged or not charged because we know both an uncharged object and an oppositely charged object are attracted by another charged object.

If an object is positively charged it loses some of its electrons. The mass of an electron is 9.11*10^-31 kg. So, if a positively charged body loses ‘n’ number of electrons, it mass decrease by the amount n*9.11E^-31kg.

Though gold is a costly metal it is used in electroscope because of the property malleability. This means very thin and light sheets can be formed from gold simply by hammering or rolling and hence the deflection of the light gold plates increases.

The divergence of the plates of the Gold-leaf oscilloscope depends only on the presence of a charge, not on the quality of charge i.e. positive or negative. So, if the charge changes from positive to negative and vice versa the degree of divergence of the plates remains the same.

The same charges repel each other. So, they try to maintain maximum distance from each other and hence they try to remain at the outer surface of an object. If the charge remains on the inner surface or throughout the body, they will repel each other with greater force.

The human body is a good conductor and hence the charge produced by friction flew through his body to the ground. We can tackle the problem simply by holding the brass rod with the help of some insulated holder.

If the apparatus is initially in contact with some positively charged body and then comes in contact with another charged body and if the divergence increases we can deduce that the second body is also positively charged. If the divergence decreases then the second body must be negatively charged.

According to electrostatic series, glass is situated above silk. So, if the glass is rubbed with silk, the positive charge on glass and negative charge on silk is produced. Similarly, we can predict what is the nature of charge if we rub two di-electric substances together.

1 Coulomb means 3*10^9 Electro Static Unit of charge. Coulomb and ESU are two different units of charge and their conversion formula is necessary. Coulomb is the unit of charge in the SI system and esu is the unit of charge in the CGS system.

The two spheres are oppositely charged by the same amount. So if they come in contact, both of their charges are neutralized. So they become uncharged and don’t attract or repel each other. Open / Comment

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2021-10-08 10:26:54 Classification of solids as ionic, metallic, molecular, network (covalent) or amorphous.

(i) Tetra phosphdecoxide(P4O10) → Molecular

(ii) Ammonium phosphate(NH4)3PO4 → ionic

(iii) SiC → Network (Covalent)

(iv) I2 → molecular

(v) P4 → Molecular

(vi) Plastic → amorphous

(vii) Graphite → Network (Covalent)

(viii) Brass → metallic

(ix) Rb → metallic

(x) LiBR → ionic

(xi) Si → Network (Covalent) Open / Comment

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2021-10-07 10:12:06 Atoms & Molecules

Around 500 BC, an Indian Philosopher Maharishi Kanad, first time postulated the concept of indivisible part of matter and named it ‘pramanu.’

In 1808, John Dalton used the term ‘atom’ and postulated the atomic theory to the study of matter.


Dalton’s Atomic Theory
According to Dalton’s atomic theory, all matter, whether an element, a compound or a mixture is composed of small particles called atoms.
According to Dalton’s atomic theory, all matters, whether they are elements, compounds, or mixtures, are composed of small particles known as atoms.

Salient features of Dalton’s Atomic Theory
All matter is made of very miniscule particles known as atoms.
Atom is an indivisible particle, which cannot be created or destroyed through chemical reaction.
All atoms of an element are identical in mass and chemical properties whereas, atoms of different elements have different masses and chemical properties.
To form a compound, atoms are combined in the ratio of small whole numbers.
In a given compound, the relative number and kinds of atoms are constant.

Atomic Mass
The mass of an atom of a chemical element; it is expressed in atomic mass units (symbol is u).
The atomic mass is roughly equivalent to the number of protons and neutrons present in the atom.
One atomic mass unit is a mass unit equal to the exactly one-twelfth (1/12th) the mass of one atom of carbon-12 and the relative atomic masses of all elements have been calculated with respect to an atom of carbon-12.

Molecule
The smallest particle of an element or a compound, which is capable to exist independently and shows all the properties of the respective substance.
A molecule, normally, is a group of two or more atoms which are chemically bonded together.
Atoms of the same element or of different elements can join (with chemical bond) together to form molecules.
The number of atoms that constitute a molecule is known as its atomicity.

Ion
A charged particle is known as ion; it could be either negative charge or positive charge.
The positively charged ion is known as a ‘cation’.
The negatively charged ion is known as an ‘anion.’

Chemical Formulae
A chemical formula of a compound demonstrations its constituent elements and the number of atoms of each combining element.
The chemical formula of a compound is the symbolic representation of its Composition.
The combining capacity of an element is known as its ‘valency.’

Molecular Mass
The molecular mass of a substance is calculated by taking the sum of the atomic masses of all the atoms in a molecule of respective substance. For example, the molecular mass of water is calculated as −
Atomic mass of hydrogen = 1u
Atomic mass of oxygen = 16 u

The water contains two atoms of hydrogen and one atom of oxygen.
Molecular Mass of Water is = 2 × 1+ 1×16 = 18 u (u is the symbol of molecular mass).

Formula Unit Mass
The formula unit mass of a substance is calculated by taking the sum of the atomic masses of all atoms in a formula unit of a compound.

Avogadro Constant or Avogadro Number
Avogadro was an Italian scientist who had given the concept of Avogadro Number (also known as Avogadro Constant).
The number of particles (atoms, molecules, or ions) present in 1 mole of any substance is fixed, and its value always calculated as 6.022 × 1023.
In 1896, Wilhelm Ostwald had introduced the concept of ‘mole;’ however, mole unit was accepted to provide a simple way of reporting a large number in 1967.

Law of Conservation of Mass
During a chemical reaction, sum of the masses of the reactants and products remains unchanged, which is known as the ‘Law of Conservation of Mass.’

Law of Definite Proportions
In a pure chemical compound, its elements are always present in a definite proportion by mass, which is known as the ‘Law of Definite Proportions.’

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