File No.33/05/18/11/2014
IX CLASS - IIT/N.T.S.E FOUNDATION - TECHNO
ANDHRA PRADESH - TELANGANA
2014-2015 PROGRAM M E
CHEMISTRY - 2ND CHAPTER - SOLUTION
CHEMICAL BONDING
1.
The dots in Lewis symbols represents Valence electrons in an atom.
2.
Inert nature of noble gases can be explained by octet theory.
3.
Electrons involved in bond formation are commonly called as Valence electrons & Core electrons.
4.
3 number of electrons transferred from one atom to another during bond formation in Aluminium Nitride:
5.
An element of low is Ionic bond is formed ionisation potential combines with an element of very high
electron affinity:
6.
CaI2 is least ionic compound.
7.
Ca3N2 is more ionic compound.
8.
Bond formation is Always exothermic.
9.
A covalent bond is likely to be formed between two elements which have similar electronegativities
10.
The maximum number of covalent bonds by which the two atoms can be bonded to each other is Three.
11.
The molecule which contains maximum number of electrons is BCl3.
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12.
2014 solvents.
- 2015
Covalent compounds are soluble in non-polar
13.
If the electron pair forming a bond between two atoms A and B is not the centre, then the bond is
polar covalent bond.
14.
Ammonium ion contains co-ordinate bond.
15.
Bond present in iodinemonochloride is covalent bond.
16.
The strength of a covalent bond between two atoms is determined by bond energy.
17.
N  bond in N2 largest amount of bond energy to dissociate the atoms concerned.
18.
Sigma bonds are Cylindrically symmetrical about the bond axis.
19.
The strength of sigma bonds by s – s, p – p, s – p overlap is in the order: s – s < s – p < p – p.
20.
 bond always exists with sigma bond
1.
Many ionic crystals dissolve in water because water decreases the inter ionic attraction in the crystal lattice
due to solvation.
2.
Most of the ionic substances are soluble in polar solvents like water.
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IX CLASS - IIT/N.T.S.E FOUNDATION - TECHNO
2+
2–
ion and S ion is larger than Cl– ion, which of the following will be least
3.
If Na ion is larger than Mg
soluble in water is MgS.
4.
The electronic configuration of the four elements A, B, C and D are (A) 1s2 (B) 1s2 2s2 2p2 (C) 1s2 2s2 2p5 (D)
1s2 2s2 2p6.
Tendency to form electrovalent bond is largest in C .
5.
Two elements ‘X’ and ‘Y’ have the following configurations
X = 1s2 2s2 2p6 3s2 3p6 4s2
Y = 1s2 2s2 2p6 3s2 3p5
The compound formed by the combination of ‘X’ and ‘Y’ will be XY2.
6.
The covalency of Hydrogen, Chlorine, Oxygen and Nitrogen in their elementary molecules respectively is
H  H, Cl  Cl, O  O, N  N .
7.
Silicon has 4 electrons in the outermost orbit. In forming the bonds: it shares electrons
8.
An element ‘Y’ has the ground state electronic configuration 2, 8, 7. The type of bond that exists between
the atoms of ‘Y’ is Covalent.
9.
The electronegativity values of C, H, O, N and 2.5, 2.1, 3.5 and 2.5 respectively. The most polar bond is
O - H.
10.
Dative bonds do present in NH4Cl.
11.
Covalent bond is directional, ionic compounds do not exhibit space isomerism are statement is incorrect.
12.
The single, dou ble and triple bond lengths o f carbon in carbon dioxide are respctively:
1.22, 1.15 and 1.10 Ao
13.
The bond energies of H-H and Cl-Cl are 430 Kj/mol and 242 Kj/mol respectively.  Ht for HCl is 91 KJ mol1.The bond energy of HCl will be 245KJ.
14.
 bonds are formed by hybrid orbitals is not characteristic of  bond?
15.
A triple bond is made of one  and two  bonds
16.
Shape of the molecule is decided by  bonds.
17.
Number of sigma and pi bonds present in O = C =O are 2  , 2  .
18.
Number of sigma and pi bonds present in calcium carbide are 3  , 2 
19.
Lattice energy of BeCO3 (I), MgCO3(II) and CaCO3 (III) is in order is I > II > III.
20.
Electronegativity values of elements help in predicting is polarity of the molecules
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BRAIN TWISTERS
1.
High electron affinity, less size, less anion charge & high electro negativity are features of acceptors required
to form ionic bond.
2.
Sodium chloride, Copper chloride & Magnesium oxide are substance not having covalent bonding.
3.
Covalent bond is it is formed by sharing of the electrons and when two non-metals are combined, then a
covalent bond is formed.
4.
The bond formed between two non-metallic elements is covalent bond, the bond formed between two inert
gas elements is van der Wall’s bond & the bond formed between a metal and a non-metal is electrovalent
bond. are correct.
5.
A Pi –bond is formed when a sigma bond is already formed, pi-bonds may be formed by the overlapping of
P-Orbitals & pi-bonds results form lateral overlap of atomic orbitals are characteristics of Pi bond.
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6.
7.
IX CLASS - IIT/N.T.S.E FOUNDATION - TECHNO
a) Ionic compounds in aqeous
-
Good conductor of electricity
b) Ionic compounds in solid state
-
Bad conductor of electricity
c) ZnSO4. 7H2O and FeSO4. 7H2O
-
Isomorphs
d) Best polar solvent
-
Water
-
CHCl3
a) Covalent compounds
-
H2, SO2, PCl3, Covalent bond is formed
b) Valence electrons in the
-
Five
-
Zero
-
Covalent bond is formed
a) Highly covalent material
-
Diamond, Graphite
b) Conductor of electricity
-
Graphite
c) Good ionic solid
-
Potassium chloride, Zeolite
d) Hydrogen bonded solid
-
Ice
a) Sigma bond
-
Linear overlap of atomic orbitals, Fluorine molecule, Nitrogen
molecule, Carbondioxide molecule
b) Pi bond
-
Side wise overlap of atomic orbitals , Nitrogen molecule,
Carbondioxide molecule, Linear overlap of atomic orbitals
c) H2
-
Side wise overlap of atomic orbitals, Linear overlap of atomic
orbitals, Fluorine molecule, Nitrogen molecule
d) N2
-
elements of VA group
c) Electronegativity between
two H-H atoms
d) If electronegativity difference
between two non-metals is less
than 1.7
8.
9.
Nitrogen molecule, Linear overlap of atomic orbitals,
molecule, Linear overlap of atomic orbitals,
2014Carbondioxide
- 2015
Fluorine molecule
10.
11.
a) H2O
-
sp3
b) SF6
-
sp 3d 2
c) C2H4
-
sp 2
d) C2H2
-
sp
The electrons in the outermost orbit of an atom are called valency electrons. Nitrogen atomic number=7,
E.C 1s22s22p2 nitrogen atom = 5. The electrons in the outermost orbit of an atom are called
Valency shell is 2nd shell no. of valency electrons = 5.
Both Assertion and Reason are correct, and Reason is correct reason of Assertion.
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12.
Elements which lose electrons are called electropositive elements and which given electrons are called
electronegative elements.
Both Assertion and Reason are correct, and Reason does not explain Assertion.
13.
The covalency of nitrogen in N2 molecule is 3 and in HNO2 is 3.
Both are correct and Reason does not explain Assertion.
14.
Graphite being a non metal it has free electrons to conduct electricity. So, Assertion and Reason both are
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IX CLASS - IIT/N.T.S.E FOUNDATION - TECHNO
correct and reason explains Assertion.
15.
Bond length increases with increase in the size of the atom. In an ionic compound bond length is the some
of the ionic radii.
Both Assertion and Reason are correct, and Reason explains Assertion.
16.
Element X is strongly electropositive and the element Y is strongly electronegative. Both are univalent. The
compound formed would be X+ Y–.
17.
An element with atomic number 11 will form a strong ionic compound with an element of atomic number is
10.
18.
During the formation of an ionic bond, the atom that receives electrons is the atom with higher ionisation
energy
19.
The group number of atoms which could not form a chemical bond is zero group.
20.
The maximum number of covalent bonds that could be formed between two carbon atoms is 3.
1
A, B, C are the elements of group IA, IIA, IIIA respectively they Lewis dot diagram of A, B ,C is
A belongs to IA group, i.e, A 
B belongs to IIA group i.e, B
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
C belongs to IIIA group i.e, C
2.
The correct statement is the shared pair of electrons, which result in the formation of a bond is called
bonded pair, the pair of electrons present in the valence shell but not involved in the bonding is lone pair.
3.
CuSO4.5H2O are
Cu - SO4 – electrovalent bond
H2O – covalent bond.
CuSO4.5H2O co-ordinate covalent bond.
4.
E1 – E . C. 1s2
E2 – 1s22s22p2
E3 – 1s22s22p5
E4 – 1s22s22p6
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E3 element is capable of forming both ionic as well as covalent bonds.
5.
Given X, Y, Z elements
 X does not conduct electricity in solid (or) liquid state i.e, it is non metal and forms non polar covalent
bond
 Y conducts electricity in both fused and solution state forms ionic bond.
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IX CLASS - IIT/N.T.S.E FOUNDATION - TECHNO
 Z conducts electricity only in solution state so, it forms polar covalent bond.
6.
Lewis acods are always in a position to donate electrons pair and lewis bases are accept an electron pair,
so, in between lewis acid and lewis base dative bond is formed.
7.
a) C2H6
Covalent bond
b) Iron wire
Metallic bond
c) H2O
Covalent bond
d) H3O+
Coordinate, covalent bonds
8.
Ethene CH2  CH2
H C  C H
| |
H H
9.
Number of

bonds = 5 
Number of

bond = 1 
CH  CH, H  C  C  H
Number of

bonds = 3 
Number of

bonds = 2 
10.
Sigma bond is stronger then  bond.
11.
Generally  bond is formed from the lateral overlap of P-P Orbital and d-d orbital .
12.
When orbitals overlap unsymmetrically2014
formed
 bond- is2015
13.
Number of sigma and pi bonds present in C2H4 are 5  , 1 
14.
Number of sigma and pi bonds present in C2H2 are 3  , 2 
15.
NH3,
4  N H
number of
|

bonds = 3 
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H
16.
When two atoms containing electrons of same spin then bonding will not occur.
17.
Strongest covalent bond is observed in N  N
18.
Shape molecule is decided by  bonds
19.
Valence bond theory of L. Pauling and J.E. Slater accounts for strength characteristics of covalent bond.
20.
The double bond between the two carbon atoms in ethylene consists of one sigma bond and one pi bond
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