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Daily Practice Problems
Class 11 Chemistry
Classification of Elements and Periodicity in Properties
daily practice problem

Question1.

Given below are few statements related to Mendeleev’s Periodic table:

  1. Mendeleev ignored the order of atomic weights at some instances and placed the elements with similar properties together in same group.
  2. He proposed that some of the elements were still undiscovered and, therefore, left several gaps in the table.
  3. Mendeleev arranged elements in horizontal rows and vertical columns of a table in order of their increasing atomic weights in such a way that the elements with similar properties occupied the same vertical column or group.
  4. Mendeleev relied on the similarities in the empirical formulas and properties of the compounds formed by the elements.

Which of the above statement/statements are incorrect?

  1. a
  2. b
  3. d
  4. none of the above

 

 Question2.

How Henry Moseley showed that the atomic number is more fundamental

property of an element than its atomic mass?

 

Question3.

Find out group, period & block of element having Z = 82.

 

Question4.

Write the IUPAC name & symbol for the element with atomic number 115?

 

Question5.

Why 4f- & 5f-inner transition series of elements placed separately in periodic table?

 

Question6.

Write the general outer electronic configuration of d-block & f-block elements.

   

Question7.
 

Which one of the following groups represent a collection of isoelectronic species? (At. Numbers, Cs = 55 and Br = 35)

  1. N3-, F-, Na+
  2. Ca2+, Cs+, Br
  3. Be, Al3+, Cl-
  4. Na+, Ca2+, Mg2+

 

Question8.

Atomic radii of noble gases are measured in terms of

  1. Metallic radius
  2. Covalent radius
  3. Van der waals radii
  4. Ionic radii

 

Question9.

Arrange the following species in increasing order of their sizes: I-, I, Cl, Br

 

Question10.

B has lower first Ionisation enthalpy than Be because, energy required to remove

  1. s-electron is less than p-electron.
  2. p-electron is less than s-electron.
  3. None of the above

 

Question11.

X(g)  →   X+(g) + e-             Ionisation enthalpy = +320 kJ mol-1

Calculate the amount of energy required to convert 140mg of ‘X’ atom in gaseous state into X+ ion.

(1 mole of X = 7g)

  1. 10.6 kJ
  2. 7.2 kJ
  3. 6.8 kJ
  4. 6.4 kJ

 

Question12.

Define Ionization enthalpy. How does it vary across period and down the group in case of main group elements? Why?

 

Question13.

Given below are the statements related to electron gain enthalpy:

  1. Electron gain enthalpy provides a measure of the ease with which an atom adds an electron to form anion.
  2. Depending on the element, Electron gain enthalpy can be either endothermic or exothermic.
  3. Group 17 elements (the halogens) have low negative electron gain enthalpies.
  4. Group 18 elements have large positive electron gain enthalpies.
  5. Electron gain enthalpy becomes less negative as we go down a group.

Which of the following statement/statements are incorrect?

  1. Both a & d
  2. e
  3. c
  4. b

 

Question14.

According to Pauling scale, arbitrary value of 4.0 is given to certain element X which is considered to have greatest ability to attract shared electrons in chemical compound. Select the correct element X from given options:

  1. O
  2. Cl
  3. F
  4. N

 

Question15.

Which of the following statement/statements concerning element having atomic number 11 are correct?

  1. It forms Ionic compounds.
  2. It has very high reactivity.
  3. It has large positive electron gain enthalpy.
  4. It has low ionisation enthalpy.

Options:

  1. a & b
  2. c
  3. d & a
  4. a, b & d

 

Question16.

Which of the following oxide is amphoteric?

  1. Na2O
  2. Al2O3
  3. Cl2O
  4. CO

 

Question17.

The formula of the binary compound formed by the element (Z = 56) and sulphur is

  1. XS
  2. X2S
  3. XS2
  4. X3S

 

Question18.

Among the following elements C, Al, Na, and Cs, the correct order of their metallic character is:

  1. Cs > Na > Al > C
  2. Cs > Al > Na > C
  3. Na > Cs > Al > C
  4. Cs > Na > C > Al

 

Question19.

What are the reasons for the different chemical behaviour of the first member of a group of elements in the s- and p-blocks compared to that of the subsequent members in the same group?

 

Question20.

Why electronegativity of any given element is not constant? Explain giving an example.

**********

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