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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 .

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(a) Electropositive nature of the element(s) increases down the group and decreases across the period (b) Electronegativity of the element decreases down the group and increases across the period (c) Atomic size increase down the group and decreases across a period (left to right) (d) Metallic character increases down the group and decreases across a period On the basis of the above trends of the periodic table, answer the following about the electron with atomic number 3 to 9 (a) Name the most electropositive element among them (b) Name the most electronegative element (c) Name of the element with smallest atomic size (d) Name the element which is a metalloid (e) Name the element which shows maximum valency.

Oxidation number is the charge which an atom of an element has in its ion or appears to have when present in the combined state. It is also called oxidation state. Oxidation number of any atom in the elementary state is zero. Oxidation number of a monoatomic ion is equal to the charge on it. In compounds of metals with non metals, metals have positive oxidation number while non metals have negative oxidation numbers. In compounds of two difference elements, the more electronegative element has negative oxidation number whereas the other has positive oxidation number. In complex ions, the sum of the oxidation number of all the atoms is equal to the charge on the ion. If a compound contains two or more atoms of the same element, they may have same or different oxidation states according as their chemical bonding is same or different. The oxidation state of the most electronegative element in the products of the reaction between BaO_(2) and H_(2)SO_(4) are

Oxidation number is the charge which an atom of an element has in its ion or appears to have when present in the combined state. It is also called oxidation state. Oxidation number of any atom in the elementary state is zero. Oxidation number of a monoatomic ion is equal to the charge on it. In compounds of metals with non metals, metals have positive oxidation number while non metals have negative oxidation numbers. In compounds of two difference elements, the more electronegative element has negative oxidation number whereas the other has positive oxidation number. In complex ions, the sum of the oxidation number of all the atoms is equal to the charge on the ion. If a compound contains two or more atoms of the same element, they may have same or different oxidation states according as their chemical bonding is same or different. A compound of Xe and F is found to have 53.3% Xe (atomic weight =133). Oxidation number of Xe in this compound is

Mendeleev predicted the existence of certain elements not known at that time and named two of them as Eka-Silicon and Eka-aluminium (a) Name the elements which have taken the place of these elements (b) Mention the group and the period of these electron in the modern periodic table (c) Classify these elements as metals, non-metals or metalloids (d) How many valence electrons are present in each one of them ?

(a) How is the valency of an element determined if its electronic configuration is known? Determine the valency of an element of atomic no. 9 (b) Given below are some elements of the Modern Periodic Table. Atomic numbers of the elements are given in the parentheses: A(4), B(9), C(14), D(19), E(20) (i) With the help of the electronic configuration, find out which one of the above elements will have one electron in its outermost shell? (ii) Which rwo elements belong to the same group? Give reasons for your answer. (iii) Which one of the above elements belonging to the fourth period has bigger atomic radius and why?.

In a metal in the solid state, such as a copper wire, the atoms are strongly bound to one another and occupý fixed positions. Some electrons (called the conductor electrons) are free to move in the body of the metal while the other are strongly bound to their atoms. In good conductors, the number of free electrons is very large of the order of 10^(28) electrons per cubic metre in copper. The free electrons are in random motion and keep colliding with atoms. At room temperature, they move with velocities of the order of 10^5 m/s. These velocities are completely random and there is not net flow of charge in any directions. If a potential difference is maintained between the ends of the metal wire (by connecting it across a battery), an electric field is set up which accelerates the free electrons: These accelerated electrons frequently collide with the atoms of the conductor, as a result, they acquire a constant speed called the drift speed which is given by V_e = 1/enA where I = current in the conductor due to drifting electrons, e = charge of electron, n = number of free electrons per unit volume of the conductor and A = area of cross-section of the conductor. A current of 1 A flows through a copper wire. The number of electrons passing through any cross-section of the wire in 1.6 sec is (charge of a electron = 1.6 xx 10^(-19 c) .

Study the following table in which positions of six elements A,B,C,D,E and F are shown as they are in the modern periodic table. On the basis of the above table, answer the following question : (i) Name the element which form only covalent compounds. (ii) Name the element which is a metal with valency three. (iii) Name the element which is a non-metal with valency three. (iv) Out of D and E, which is bigger in size and why ? (iv) Write the common name for the family to which the elements C and F belongs.

Choose the correct answer: In the periodic table alkali metals are placed in group - A:1, B:11, C:17, D:18 Which of the following properties: do not match with elements of the halogen family, A : They have seven electrons in their valence shell, B : They are highly reactive chemically, C: They are metallic in nature, D: They are diatomic in their molecular form.

The colours of the transition metal are due to d-d excitation. The energy required for d-d electron axcitation is available in the visible range. Transition metal ions have the tendency to absorb certain rediations from the visible region and exhibit the complementary colour. The transition metal ions which have completely filled d-orbitals are colourless as the excitation of electron or electrons is not possible within d-orbitals. The transition metal ions which have completely empthy d-orbitals are also colourless. In KMnO_4 and K_2Cr_2O_7 , there are no unpaired electrons at the central atom but they are dep in colour. The colour of these compounds is due to charge transfer spectrum. for example in MnO_4 electron is momentrily transferred from O to the metal and thuys oxygen changes from O^(2-) and O^(ɵ) maganese from Mn^(7+) to Mn^(6+) . Q. Which of the following is paramagnetic as well as coloured ion?

The colours of the transition metal are due to d-d excitation. The energy required for d-d electron axcitation is available in the visible range. Transition metal ions have the tendency to absorb certain rediations from the visible region and exhibit the complementary colour. The transition metal ions which have completely filled d-orbitals are colourless as the excitation of electron or electrons is not possible within d-orbitals. The transition metal ions which have completely empthy d-orbitals are also colourless. In KMnO_4 and K_2Cr_2O_7 , there are no unpaired electrons at the central atom but they are dep in colour. The colour of these compounds is due to charge transfer spectrum. for example in MnO_4 electron is momentrily transferred from O to the metal and thuys oxygen changes from O^(2-) and O^(ɵ) maganese from Mn^(7+) to Mn^(6+) . Q. Which is a coloured ion?

CENGAGE CHEMISTRY ENGLISH-CHEMICAL BONDING AND MOLECULAR STRUCTURE-Solved Examples
  1. Construct a table comparing metals with non-metals in terms of (a) T...

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  2. Write the formula for a compound of CI which contains Ionic bonds only

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  3. Pure liquid H(2)SO(4) solidifies below 10.4^(@)C Neither the pure liqu...

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  4. Write electron dot and line structure for (a) SeO(3)^(2-) ,(b) Li(3)...

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  5. By completing the following structures, adding unshared e^(-) pairs wh...

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  6. (a) In each of the following parts select the species having the great...

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  7. Arrange in decreasing polarity of bonds SbH(3),AsH(3),PH(3),NH(3)

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  8. The dipole moment of HBr is 2.60 xx 10^(-30)Cm and the interatomic spa...

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  9. The single and multiple bond radii of some elements given in the follo...

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  10. Arrange C-C,C=C and C-=C in order of (i) Decreasing bond dissociatio...

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  11. The Pt-Cl distance is 2.32 A in several crystalline compounds What i...

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  12. The averge (C C) bond energy is 343 kJ mo1^(-1). What do you predict f...

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  13. What is the hybridisation state of each C-atom in the following molecu...

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  14. How many sigma and pi bonds are present in a benzene molecule ? .

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  15. (a) What is the number of molecular orbitals obtained by mixing of two...

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  16. Compare and contrast the concepts of hybrid orbitals and molecular orb...

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  17. Which of the following molecules has the highest IE (i) Ne (ii) F

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  18. Select the species with the largest IE in each (i )Na,K,Rb (ii) F,Ne

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  19. Select from following gropus, the one which has the largest radius Li,...

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  20. Distinguish using the property mentioned in brackets (e) NF(3),NH(3) ...

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