In order to be stable, they easily lose this electron and get oxidized. (ii) Alkali metals have one electron in their valence shell. (i) The ionization potential of element increases across a period because the atomic size decreases due to an increase in nuclear charge and electrons in the outermost shell are more strongly held because of which greater energy is required to remove the electron. (ii) Alkali metals are good reducing agents. (i) Ionization potential of element increases across a period. Electron affinity of inert gases is zero. Reason - Electron affinity of argon is zero as Argon is in 3rd period and is an inert gas. Select the element in period 3 whose electron affinity is zero. The element having three shells with three electrons in the valence shell is in group 13 and period 3. State the group and period of the element having three shells with three electrons in the valence shell. Reason - Halogens are non-metallic in character. Reason - In the periodic table, alkali metals are placed in the group 1 as they have one electron in the outer most shell. They are diatomic in their molecular form.They have seven electrons in their valence shell.(ii) Which of the following properties do not match with elements of the halogen family? (i) In the periodic table, alkali metals are placed in the group. (ii) Down the group, the electron affinity decreases Question 3 (i) Across a period, the ionization potential increases. (ii) Down the group, the electron affinity. (i) Across a period, the ionization potential. As oxidizing power depends on tendency to gain electrons and non-metals are good oxidizing agents hence oxidizing power of elements increases across a period. The oxidizing power of elements increases from left to right along a period because electro-negativity and the non metallic character increases from left to right. Give reasons - The oxidizing power of elements increases from left to right along a period. (ii) Electron affinity is the amount of energy released when an atom in the gaseous state accepts an electron to form an anion. (i) Ionization Potential is the amount of energy required to remove an electron from the outer most shell of an isolated gaseous atom. (ii) The number of valence electrons are 6. (iii) Is the element a metal or a non metal. (ii) The number of valence electrons in the element. Question 2Ītomic number of an element is 16. (iii) Non metallic character down the group - decreases. (ii) Electro negativity across a period - increases. (i) The number of electrons in the valence shell of halogen is 7. (iii) Non metallic character down the group - increases/decreases. (ii) Electro negativity across the period - increases/decreases. (i) The number of electrons in the valence shell of a halogen is : Ionization Potential is the amount of energy required to remove an electron from the outer most shell of an isolated gaseous atom. (v) Electron dot structure for the compound formed between C and K is shown below:ĭefine the following term - Ionization Potential. (iv) Covalent bond will be formed between F and J. (iii) B 2H is the name of the compound between B and H. (v) Draw the electron dot structure for the compound formed between C and K. (iv) In the compound between F and J, what type of bond will be formed? (iii) Write the formula of the compound between B and H. (ii) How many valence electrons are present in G? Some elements are given in the above table in their own symbol and position in the periodic table, while others are shown with a letter. Question 2Ĭonsider the section of the periodic table given below: Group Chapter 1 Periodic Table - Periodic Properties & Variation of Properties Class 10 - Dalal Simplified ICSE Chemistry SolutionsĪmong Period-2 elements - Lithium Carbon Fluorine Neon - State the one which has high electron affinity.įluorine has the highest electron affinity.
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