Transition elements exhibit variable oxidation states because they release electrons from the following orbits:

 

  • ns and np orbits

  • (n-1)d and ns orbits

  • (n-1)d orbits

  • ns orbits

According to Moseley, a straight-line graph is obtained on plotting-

  • The frequencies of characteristic X-rays of elements against their atomic numbers.

  • The square of the frequencies of characteristic X-rays of elements against their atomic numbers

  • The square root of the frequencies of characteristic X-rays of elements against their atomic numbers

  • The reciprocal of the frequencies of characteristic X-rays of elements against their atomic numbers.

The tenth element in the periodic table resides in:

  • the second period

  • the fourth period

  • the fifth period

  • the eight period

Which of the following order is not in accordance with the property stated against it?                                                                                                      

  • F2 > Cl2 > Br2 > l2 Oxidising Power

  • Hl > HBr >HCl >HF Acidic property in water

  • F2 > Cl2 > Br2 > l2 Electronegativity

  • F2 > Cl2 > Br2 > l2 Bond dissociation energy

An element X occurs in short period having configuration ns2np1 . The formula and nature of its oxide are:

  • XO3, basic

  • XO3, acidic

  • X2O3, amphoteric

  • X2O3, basic

The outermost electronic configuration of the most electronegative element is :

  • ns2np3

  • ns2np4

  • ns2np5

  • ns2np6

The elements X, Y, Z and J have the indicated electron configurations starting with the innermost shell. The most metallic element is :

  •  X = 2, 8, 3

  •  Y = 2, 8, 8

  •  Z = 2, 8, 8, 1

  •  j = 2, 8, 8, 7

Which statement is true?

  • The electronegative nature of elements increases along the period

  • The electropositive nature of elements increases along the period

  • The chemical reactivity of elements increases along the period

  • The I.E  of element decreases along the period

The most non-metallic element among the following is:

  • Be

  • B

  • Mg

  • Al

58Ce is a member of which block?

  •  s-block elements.

  •  p-block elements.

  •  d-block elements.

  •  f-block elements.

The screening effect of 'd' electrons is:

  • Much less than s-electrons.

  • Much more than s-electrons.

  • Equal to s-electrons.

  • Equal to p-electrons.

Correct statement regarding transuranic elements is :

  • They have higher atomic number than uranium.

  • They are lighter than uranium.

  • They have lower atomic number than uranium.

  • They have same atomic number as uranium.

The correct  sequence of increasing order of density is:

  • Li < K< Na < Rb < Cs

  • Li < Na < K < Rb < Cs

  • Cs < Rb < K < Na < Li

  • K < Li < Na < Rb < Cs

General electronic configuration of outermost and penultimate shell of an atom is
(n - 1)s2 (n - 1) p6 (n - 1)dx ns2. If n = 4 and x = 5, the number of proton in the nucleus is:

  • > 25

  • < 24

  • 25

  • 30

The maximum number of valence electrons possible for atoms in the second period of the periodic table is:

  • 18

  • 10

  • 8

  • 2

The element having atomic number 19, is:

  • an inert gas

  • a metal with oxidation number +1

  • a non-metal with oxidation number -3

  • a metal with oxidation number -3

Which of the following has the least density?

  • Na

  • Li

  • Mg

  • K

Eka aluminium and Eka silicon are now known as:

  • Ga and Ge

  • Al and Si

  • Fe and S

  • H+ and Si

An element having the electronic configuration of its atom ns2 np2 should have similar properties to those of:

  • Sodium

  • Carbon

  • Magnesium

  • Oxygen

The order of basic character of given oxides is:

  • Na2O > MgO > Al2O3 > CuO

  • MgO > Al2O3 > CuO > Na2O

  • Al2O3 > MgO > CuO > Na2O

  • CuO > Na2O > MgO > Al2O3

A variable oxidation state is shown by which of the following?

  • Na

  • Cu

  • Mg

  • Al

The lightest metal in the periodic table is:

  • H

  • Mg

  • Ca

  • Li

Which of the following electronic configurations represents the d-block element? 

  • 1s2 2s2 2p6 3s23p63d10 4s24p6

  • 1s2 2s2 2p6 3s23p63d10 4s24p1

  • 1s2 2s2 2p6 3s23p63d10 4s2

  • 1s2 2s2 2p6 3s23p6 4s2

The most common oxidation state of cerium (Ce) is:

  • +5, +3

  • +5, +4

  • +3, +4

  • +3, +5

Which of the electronic configuration of an atom has the lowest ionization enthalpy? 

  • 1s2,2s22p5

  • 1s2,2s22p3

  • 1s2,2s22p6,3s1

  • 1s2,2s22p6

A common trend in both groups I and II elements in the periodic table, as the atomic number increases, is :

  • Maximum valency increases

  • Reactivity with water decreases

  • Oxidizing power increases

  • Atomic radius increases

The difference between ions and atoms is of:

  • presence of charge

  • All of these

  • relative size

  • Configuration

The expected trend of change in atomic radius down the group is:

  • Continuous decrease

  • Continuous increase

  • Periodic one, an increase followed by a decrease

  • Periodic one, a decrease followed by an increase

An element R forms the highest oxide R2O5. R belongs to:

  • 13th  group

  • 15th group

  • 16 th group

  • 2nd group

Amongst the following electronic configurations, highest ionisation energy is represented by- 

  • [Ne]3s23p3

  • [Ne]3s23p2

  • [Ar]3d104s24p3

  • [Ne]3s23p1

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