EAMCET QUESTIONS FROM CHAPTER  GASEOUS STATEPART-1

1.The average kinetic energy of one molecule of an ideal gas at 27^oC and 1 atm. Pressure is

1) 900 cals K-1 mol-1	2.	6.21×10-21 J K-1 molecule-1
3) 336.7 J.K-1 molecule -1	4. 374.3 J.k-1 mol-1

2.The vapor of a substance effuses through a small hole at the rate of 1.3 times faster than SO₂gas at 1 atm. pressure and 500K The molecule weight of the gas is

1) 49.2                        2) 37.9                         3) 41.6                        4) 83.2

3.40 grams of a sample of carbon on combustion left 10% of it unreached. The volume of oxygen required at STP for this combustion reaction is

1. 22.4l                       2. 67.2 l                       3. 11.2 l                      4. 44.8 l

4.In a flask of ‘V’ litres , 0.2 moles of O₂, 0.4 moles of N₂, 0.1 moles of NH₃and 0.3 moles of He gases are present at 27^oC. If total pressure exerted by these non-reacting gases is 1 atm, the partial pressure exerted by N₂gas is

1. 0.4 atm                   2. 0.3 atm                    3. 0.2 atm                   4. 0.1 atm

5.What is the temperature at which the kinetic energy of 0.3 moles of Helium is equal to the kinetic energy of 0.4 moles of Argon at 400 K ?

	1) 400 K	2) 873 K	3) 533 K	4) 300K
43.

6.A certain mass of a gas occupies a volume of 2 litres at STP. To what temperature the gas must be heated to

double its volume, keeping the presure constant?

1) 100 K                     2) 273 K                      3) ₂₇₃⁰ _C                  4)

7.Which of the following set of variables give a straight line with a negative slope when plotted ?

(P = vapour pressure. T = Temperature in K)

y-axis	x-axis	y-axis	x-axis
1) P	T	2)	T
3)	P	4)

8.At. T(K), 100 L of dry oxygen is present in a sealed container. It is subjected to silent electric discharge, till the volumes of oxygen and ozone become equal. What is the volume (in litres) of ozone formed at T (K)?

1) 50                           2) 60                            3) 30                           4) 40

9.A and B are ideal gases. The molecular weights of A and B are in the ratio of 1 : 4, the pressure of a gas mixture containing equal weights A and B is P atm. What is the partial pressure of 'B' in the mixture?

(1)                               (2)                               (3)                               (4)

10.What is the ratio of kinetic energies of 3 gm. of hydrogen and 4 grams of oxygen at T K?

(1) 12 : 1                     (2) 6 : 1                       (3) 1 : 6                       (4) 24 : 1

EAMCET QUESTIONS FROM CHAPTER PERIODIC TABLE PART-2

1.Which one of the following order is correct for the first ionization energies of the elements ?

1. B < Be < N< O    2. Be < B < N < O   3. B< Be < O < N    4. B < O < Be < N

2.The elements ‘X’,’Y’ and ‘Z’ from oxides which are acidic, basic and amphoteric respectively. The correct order of their electro – negativity is

1. X > Y >Z               2) Z > Y > X               3) X > Z > Y              4) Y > X > Z

3.The atomic numbers of elements A, B, C and D are z – 1, z, z+1 and z+2 , respectively. If B is a nobles gas, choose the correct answers from the following statements:

a) A has higher electron affinity b) C exists in +2 oxidation state c) D is an alkaline Earth metal

1) a and b                   2) b and c                    3) a and c                    4) a,b and c

4.Element with Atomic number 38, belongs to

1) II A group and 5^th period                                     2) II A group and 2^nd period

3) V A group and 2^nd period                                     4) III A group and 5^th period

5.An oxide of an element is a gas and dissolves in water to give an acidic solution. The element belong to

1) II group                  2) IV group                3) VIII group              4) zero group

6.Observe the following statements :

I) The physical and chemical properties of elements are periodic functions of their electronic configuration

II)Electronegativity of fluorine is less than the electronegativity of chlorine

III)Electropositive nature decreases from top to bottom in a group The correct answer is

1) I, II and III are correct                              2) only I is correct

3) only I and II is correct                               4) only II and III are correct

7.Identify the correct order in which the covalent radius of the following elements increases.

	(I) Ti	(II) Ca	(III) Sc
	(1) I, II, III	(2) III, II, I	(3) II, I, III	(4) I, III, II
8.	Identify the correct order in which the ionic radius of the following ions increases
			−3+
	(I)	(II)	FNa
			(III)
	(1) III, I, II	(2) I, II, III	(3) II, III, I	(4) II, I, III

 CHEMICAL BOND IMPORTANT POINTS

 Atoms combine to form molecules.
 Formation of chemical bond involves redistribution of electrons.
 Ionic Bond: "The chemical bond formed by the complete transfer of one or more
electrons from one atom to other".
Eg: NaCl, MgO

Covalent Bond: "The bond formed by the sharing of electrons between two atoms".
Eg: H2, Cl2, F2, H2O
Octet configuration: "The filling up of valence orbital with 8 electrons".
As the atoms approach each other, the attractive forces between electrons of one atom
and the nucleus of other atom increases, results in the decrease of combined potential
energy of combined atoms.
At the critical internuclear distance, the energy of the molecule (or) combined atoms is
less than the sum of the energies of individual atoms and thus a chemical bond is
formed.
Potential- Energy Level Diagram: Zero group elements have stable electronic configuration having 2 (or) 8 electrons.
A covalent bond is formed by the overlap of two pure atomic orbitals (or) two hybridised
orbitals (or) one hybridized and one atomic orbital.
Strong bond is formed by the maximum overlap of orbitals.
 Sigma-bond: End-on-end overlap of orbitals lead to the formation of sigma bond. It is
formed by the overlap of s-s orbitals, p-p orbitals and s-p orbital overlap.
Pi-bond: Partial overlap of orbitals lead to the formation of pi (ð) bond.
 Sigma bond is stronger than pi-bond, sigma bond exists independently.
Eg: H2, HCl, Cl2, CH4
ð-bond has no independent existence. It exists only after the formation of ó bond.
In a double bond, one sigma and one ð bond are present.
Eg: C2H4, O2, CO2, etc.,
 In a triple bond, one sigma and two pi-bonds are present.
Eg: N2, C2H2, HCN etc.,
 In a co-ordinate covalent bond, both the electrons are supplied by one atom and shared
between two atoms.
The primary requirement for the formation of a covalent bond is that one atom shouldhave a lone pair of electrons (with octet configuration) to donate and another atom
should have an empty orbital to receive it.
Eg:Molecules having linear structure are
Eg: CO2, BeCl2, C2H2, HCN etc.,
 Molecules having pyramidal structure are
Eg: NH3, PCl3, PH3, ....
Molecules having double bond are
Eg: O2, CO2, C2H4, ....
 Molecules having triple bond are
Eg: N2, HCN, C2H2...
Water molecule have "V" - shape.
 PCl5 has trigonal bi-pyramidal shape.
   Periodic Classification of ElementsImportant Points:The first classification of elements is due to dobereiner in 1817.
 Dobereiner Triad Theory: "The atomic weight of the middle element is the
arithmetic mean of first and third elements (or) the atomic weights of all the three
elements are approximately the same"
Eg: i) Li, Na, K ii) Fe, Co, Ni iii) Cl, Br, I.
Newland's Concept of Octaves: Every eighth element is having the similar
properties to that of the first element like in octave of music.
 Mendeleef, Lother Meyer used atomic property. Atomic weight for classification
elements.
 Mendeleef's Periodic Law: The properties of the elements are the periodic
functions of their atomic weights".
 Modern Periodic Law: The properties of the elements are the periodic functions of
their atomic number (or) electronic configuration.
 Modern Periodic Table is called long form of periodic table.
Long form of periodic table is divided into seven horizontal rows called "Periods" and
eighteen vertical columns called "Groups"
 The first period has only two elements.
The second and third period have 8 elements each.
 Fourth, Fifth and sixth periods have 18 elements each.
 Lanthanides and actinides are placed at the bottom of the periodic table.
 Seventh period is incomplete.
 Based on electronic configuration, the elements are classified into 4 types. They are
inert gases, representative elements, transition elements representative elements
and inner transition elements.
 Atomic radius: It is the distance between the centre of the nucleus and outermost
orbital.
 It is expressed in units of Angstroms.
 Ionization energy: It is the energy required to remove an electron from the
outermost orbital in the gaseous state.
 IE is expressed in ev or KCal.mol–1 or K.J.mol–1.
 Electronegativity: The ability of the bonded atom to attract the electron density of
the shared electrons.
 Electronegativity is expressed ... pauling scale.
 In a period, Atomic radius decreases and ionisation energy and electronegativity
increases.
In a group, atomic radius increases and IE and EN value decreases.

 ATOMIC STRUCTURE IMPORTANT POINTS

:1. Electrons, protons and neutrons are called sub-atomic particles.
2. J.J. Thomson's atomic model could not explain the atomic spectra.
3. Rutherford proposed "Planetary atomic model" based on á-ray scattering
experiments.

4. According to this model, electrons are subjected to two types of forces that is
1) The force of attraction between electrons and the nucleus

2) The centrifugal force
These two forces are equal and opposite.
5. Max Planck proposed the Quantum theory of radiation.
6. E = hí Planck's constant h = 6.625 × 10–27 erg.sec. (or) 6.625 × 10–34 J.sec.
7. Bohr proposed his atomic model based on Planck's Quantum theory.
8. Bohr model explains stationary orbits, angular momentum and radiation of energy.
9. Bohr model could not explain the atomic spectra of higher elements, Zeeman effect,
quantization of angular momentum.
10. Sommerfeld proposed the elliptical orbits and sub-stationary states.
11. Orbits are indicated by "Principal Quantum number" ie 'n', sub-stationary states are
indicated by "Azimuthal Quantum number i.e 'l', orientation of orbitals is indicated by
"magnetic Quantum number" i.e, 'm' and spinning of electrons of "Spin Quantum
number" 's'.
12. l value = (n – 1), the number of 'm' values is equal to (2l + 1) and ranges from
–l....0....+l. s is +1/2 or –1/2.13. "The region in space where there is finite probability of finding electron" is called
"atomic orbital".
14. s, p, d and f orbitals are present in the orbits. 1, 2, 3 and 4 onwards (or) K, L, M and
N onwards successively.
15. Orbitals having same energy are called degenerate orbitals.
16. "Electron occupies the orbital whose (n + l) value is minimum. If (n + l) value is same,
it occupies the orbital having less 'n' value" ____ Aufbau Principle.
17. "No two electrons will have all the four Quantum numbers same" ___ Pauli exclusionprinciple.
18. "Pairing of electrons takes place when all the degenerate orbitals are occupied by one
electron each" ____ Hund's rule.
19. Atomic radius is the distance between the nucleus and outermost orbital.
Units: A° ; 1A° = 10–8 cm or 10–10m.
20. Ionization potential is "the minimum energy required to remove an electron from
outermost orbital in the gaseous state".
Units: ev (or) K.J. mol–1 (or) K.Cal.mol–1.
21. Electron affinity is "the energy released when an electron is added to a neutral
gaseous atom in the ground state".
Units: ev (or) K.J. mol–1 (or) K.Cal.mol–1.

EAMCET QUESTIONS FROM CHAPTER TRANSITION ELEMENTS PART-1

1.Which one of the following sets correctly represent the increase in the paramagnetic property of the ions ?

1) Cu 2+ < V 2+ < Cr2 + < Mn2+	2) Cu2+ < Cr 2+ < V2 + < Mn2+
3) Cu 2+ < V 2+ < Cr2 + < Mn2+	4) V 2 + < Cu 2 + < Cr 2 + < Mn 2+

2.Which one of the following statements is correct ?

1)  Ionic radius of Fe³⁺ is greater than Fe²⁺

2)  Atomic radius of chlorine atom is greater than the ionic radius of chloride ion.

3)  Electron affinity of phosphorus is greater than nitrogen

4)   Cs₂O is strongly acidic in nature

3.

éCo

(

NH

3 )5

SO

ù Br

and éCo

(

NH

3 )

Br ù SO

are pair of ____ isomers

ë

4

û

ë

5û

4

1) lonization

2) Ligand

3) Co-ordination

4) Hydrate

4.Which one of the following pairs of complexes has the effective atomic number equal to 36 for the transition element ?

1) ëéCo (NH3 )6 ûù Cl3 ; K3 ëé Fe (CN )6 ûù	2) ëéCo( NH3 )6 ûù Cl3 ; ëéCr (H2 O )6 ûù Cl3
3) ëéFe (CO )5 ûù ; K 4 ëé Fe(CN )6 ûù	4) ëéFe (CO )5 ûù ; K 3 ëé Fe (CN )6 ûù

5.When AgNO₃solution is added in excess to 1M solution of CoCl₃xNH₃, one mole of AgCl is formed. What is the value of ‘x’?

1) 1                               2) 2                               3) 3                               4) 4

6.Which of the following pair of Transition metal ions, have the same calculated values of spin only

	magnetic moment ?
	1) Ti +2  and V +2	2) Fe+2  and Cu +2	3) Cr+2  and Fe+2	4) Co+2  and Ti +2
7.	What is the correct order of spin only magnetic moment (in BM) of Mn2 + , Cr 2+ and V 2+  ?
	1) Mn2+ > V 2 + > Cr2+ 2) V 2 + > Cr 2 + > Mn 2+		3) Mn2+ > Cr 2 + > V 2+	4) Cr 2+ > V 2 + > Mn2+

8.A complex compound of _CO⁺³ with molecular formula CoClX , YNH₃ gives a total of 3 ions when dissolved in water. How many _Cl ^- ions satisfy both primary and secondary valencies in this complex?

 (1) 3                             (2) 1                              (3) 4                              (4) Zero

9.Assertion (A) : The spin only magnetic moment of _Sc⁺³ is 1.73 BM.

Reason (R) : The spin only magnetic moment (in BM) of an ion is equal to  n (n + 2)

(1)  Both A and R are true and R is the correct explanation of A.

(2)  Both A and R are true and R is not the correct explanation of A.

(3) A is true but R is not true.                           (4) A is not true but R is true.