Home
Class 11
CHEMISTRY
Construct a table comparing metals with ...

Construct a table comparing metals with non-metals in terms of
(a) The sign of the charges possible on monoatomic ions
(b) The possibility of reaction with other elements of the same class
(c ) The range of the possible number of valence electrons
(d) The ability of the elecments to conduct electricity in the elementary state .

Text Solution

Verified by Experts

Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • CHEMICAL BONDING AND MOLECULAR STRUCTURE

    CENGAGE CHEMISTRY|Exercise Ex 2 .2 Subjective (Intermolecular Forces And H-Bonding)|7 Videos
  • CHEMICAL BONDING AND MOLECULAR STRUCTURE

    CENGAGE CHEMISTRY|Exercise Ex 2 .2 Subjective (Molecular Orbital Theory)|4 Videos
  • CHEMICAL BONDING AND MOLECULAR STRUCTURE

    CENGAGE CHEMISTRY|Exercise Archives Subjective|15 Videos
  • ATOMIC STRUCTURE

    CENGAGE CHEMISTRY|Exercise Concept Applicationexercise(4.3)|19 Videos
  • CHEMICAL EQUILIBRIUM

    CENGAGE CHEMISTRY|Exercise Archives (Subjective)|11 Videos

Similar Questions

Explore conceptually related problems

An element X belongs to 3rd period and group 2 of the periodic table. State: (a) number of valence electrons (b) valency (c) metal or non-metal (d) name of the element

An element E has following electronic configuration : {:(K,L,M,),(2,8,6,):} (a) To which group of the periodic table does element E belong ? (b) To which period of the periodic table does element E belong ? (c) State the number of valence electrons present in element E. (d) State the valency of the element E.

Which of the following statements is not a correct statement about the trends when going from left to right across the periods of Periodic Table ? (a) The elements become less metallic in nature. (b) The number of valence electrons increases. (c) The atoms lose their electrons more easily. (d) The oxides become more acidic.

An element belongs to third period and second group in the periodic table. (a) State number of valence electrons in it. (b) Is it a metal or non-metal ? (c) Name the element (d) Write the formula of its oxide

Compare metals and non-metals based on the following properties (i) Electrical conductivity (ii) Tensile strength (c) Formation of ions (iv) Reaction with acids

An electron is in a state with n=4. What are (a) the number of possible values of l, (b) the number of possible values of m_(l) , (c ) the number of poosible values of m_(s) , (d) the number of states in the n=4 shell, and (e) the number of subshells in the n=4 shell?

Two elements X and Y belong to groups 1 and 2 respectively in the same period. Compare them with respect to (a) the number of electrons in the outermost shell, (b) the number of valence electrons , (c) metallic character, (d) size of the atoms and ( e) formulae of the oxdies , hydrides and chlorides.

The atomic number of an element X is 17. Predict (a) its valency, (b) whether it is a metal or nonmetal (c ) the nature of the element, (d) the name of the element and ( e) the relative size with respect to other members of its group .

Rohan was told that six elements A,B, C,D,E and F have atomic numbers of 2,12,20,18,4 and 10 respectively (where A,B,C,D,E and F are not the chemical symbols of these elements). Based on this information, Rohan was asked to answer the following questions: (a) Which of these elements belong to the same groups of the periodic table? Why? (b) Which of these element belong tothe same periods of the periodic table? Why? (c) Which of these elements are (i) metals, and (ii) non-metals? (d) Which of these elements are chemically (i) reactive and (ii) unreactive? (e) What values are displayed by Rohan in answering the above questions?

Read the given passage and answer the questions number 1 to 5 that follow : The d-block of the periodic table contains the elements of the groups 3 - 12 and are known as transition elements. In general, the electronic configuration of these elements is (n - 1) d^(1-10)ns^(1-2) . The d-orbitals of the penultimate energy level in their atoms receive electrons giving rise to the three rows of the transition metals i.e., 3d, 4d and 5d series. However, Zn Cd and Hg are not regarded as transition elements. Transition elements exhibit certain characteristic properties like variable oxidation states, complex formation, formation of coloured ions and alloys, catalytic activity, etc. Transition metals are hard (except Zn, Cd and Hg) and have a high melting point. Which transition metal of 3d series does not show variable oxidation states ?