Which of the following arrangements shows the correct order of decreasing paramagnetism?
The outer electronic structure of lawrencium ( atomic number 103) is:
1. Rn 5f137s27p2
2. Rn 5f136d17s17p2
3. Rn 5f147s17p2
4. Rn 5f146d17s2
Which of the following sets of atomic numbers corresponds to elements of group 16?
Sodium generally does not shown oxidation state of +2, because of its:
1. High first ionisation potential
2. High second ionization potential
3. Large ionic radius
4. High electronegativity
Assuming that elements are formed to complete the seventh period, what would be the atomic number of alkaline earth metal of the eighth period?
Which one of the following is a different pair?
2. Be, Ba
Zn and Cd metals do not show variable valency because:
1. They have only two electrons in the outermost subshells
2. Their d-subshells are completely filled
3. Their d-subshells are partially filled
4. They are relatively soft metals
Which of the following is not a representative element?
Which of the following species must have maximum number of electrons in 'dxy' orbital?
4. Both (a) and (b)
Which of the following graph is correct representation between atomic number (Z) and magnetic moment of d-block elements? [Outer electronic configuration : (n-1)dxns1or 2 ]
If IUPAC name of an element is "unununium" then correct statement regarding element is :
1. It is a inner transition element
2. It belongs to 8th period in periodic table
3. It is transition element
4. It is a non-transition element
Consider the following information about element P and Q:
Period number Group number
P 2 3
Q 3 2
Then formula of the compound formed by P and Q element is:
Largest in size out of Na+, Ne and F- is:
4. All are equal
Which of the following is arranged in decreasing order of size?
The size of the species , Pb, Pb2+, Pb4+ decreases as:
Incorrect order of radius is:
The first ,second and third ionisation energies (E1, E2 and E3) for an element are 7 eV, 12.5 eV and 42.5 eV respectively. The most stable oxidaition state of the element will be:
Which of the following metal is expected to have the highest third ionization enthalpy?
1. Cr (Z = 424)
2. V (Z = 23)
3. Mn (Z =25)
4. Fe (Z = 26)
The ionization energy boron is less than that of beryllium because :
1. beryllium has a higher nuclear charge than boron
2. beryllium has a lower nuclear charge than boron
3. the outermost electron in boron occupies a 2p-orbital
4. the 2s and 2p-orbitals of boron are degenerate
Which of the following isoelectronic ion has the lowest ionization energy is :
Which of the following electronic configuration is associated with the biggest jump between the second and third ionization energies?
An element has successive ionization enthalpies as 940 (first), 2080, 3090, 4140, 7030, 7870, 16000 and 19500 KJ mol-1. To which group of the periodic tables does this element along?
The correct order of I.E.2. is :
(1) Na >F > O > N
(2) O > F > Ne > N
(3) Ne > O > F > N
(4) O > Ne > F > N
Which of the following processes involves absorption of energy?
(1) S(g) + e-→ S-(g)
(2) S- + e-→ S2-(g)
(3) Cl(g) + e-→ Cl-(g)
(4) None of these
Among the following configuration, the element which has the highest electron affinity is :
The electronegativity of the following element increases in the order :
(1) C < N < Si < P
(2) Si < P < C < N
(3) N < C < P < Si
(4) C < Si < N < P
Which of the following order is incorrect ?
(1) Electronegativity of central atom : CF4> CH4> SiH4
(2) Hydration energy : Al3+> Be2+> Mg2+> Na+
(3) Electrical conductance : F-(aq.)>Cl-(aq.)> S2-(aq.)
(4) Magnetic moment : Ni4+> V3+> Sr2+
Among the following, which has the maximum hydration energy?
Among the following oxides, which has the maximum lattice energy?
Which of the following compound has a positive enthalpy of solution?
Born-Haber cycle can be used to, estimate :
1. Lattice energy of ionic crystals
2. Electron, gain enthalpy
4. Both (1) and (2)
Select the amphoteric substance in the following :
Which of the following ionic is most unlikely to exist?
The electronic configuration of four elements are :
Consider the following statements :
(i) I Shows variable oxidation state
(ii) II is a d-block element
(iii) The compound formed between I and III is covalent
(iv) IV shows single oxidation state
Which statement is True (T) or False (F)?
The correct order of ionic size of N3-, Na+, F-, Mg2+ and O2-is :
(1) Mg2+> Na+> F-> O2-< N3-
(2) N3-< F-> O2> Na+> Mg2+
(3) Mg2+< Na+< F-< O2-< N3-
(4) N3-> O2-> F-> Na+< Mg2+
If the ionic radii of K+ and F- are nearly the same (i.e, 1.34 ), then the atomic radii of K and F respectively are :
(1) 1.34 , 1.34
(2) 0.72 , 1.96
(3) 1.96 , 0.72
(4) 1.96 , 1.34
X(g)→ X+(g) + e- , ∆H = +720 KJ mol-1
Calculate the amount of energy required to convert 110 mg of ‘X’ atom in gaseous state into X+ion. (Atomic wt. for X = 7 g/mol)
(1) 10.4 kJ
(2) 12.3 kJ
(3) 11.3 kJ
(4) 14.5 kJ
Which is the correct order of ionization energies?
(1) F-> F >Cl->Cl
(2) F >Cl>Cl-> F-
(3) F->Cl->Cl> F
(4) F->Cl-> F >Cl
The third ionization energy is maximum for :
Consider the following ionisation reactions :
I.E. (kJ mol-1) I.E. (kJ mol-1)
If monovalent positive ion of A, divalent positive ion of B and trivalent positive ion of C have zero electron. Then incorrect order of corresponding I.E. is :