Chemistry
With reference to period 3 of the periodic table — State :
- The type of bonding of the element with electronic configuration 2, 8, 7.
- The formula of the chloride of the element with electronic configuration 2, 8, 4.
- The nature of the oxide of the alkaline earth metal in the period.
- The number of electrons in the penultimate shell of the element with valency -1.
- The electronic configuration of the element whose hydroxide is a weak base.
Periodic Table
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Answer
- The element with electronic configuration 2, 8, 7 will form ionic bonds with metals and with non-metal it will form covalent bond.
- The element with electronic configuration is 2, 8, 4 is Si and with chloride it forms SiCl4.
- The alkaline earth metal in the period 3 is Mg and it's oxide is basic in nature (i.e. MgO is basic is nature).
- The number of electrons in the penultimate shell of the element with valency -1 is 8.
- The element is Magnesium and electronic configuration is (2, 8, 2)
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Related Questions
Give reasons for the following:
Atomic size decreases across a period but increases down a group of the periodic table.
In period 2, element 'A' is to the right of element 'B'
- The element 'A' would probably have a …………… [smaller/larger] atomic size than 'B'.
- The element 'B' would probably have …………… [lower/higher] ionization potential than 'A'.
- The element 'A' would have …………… [lesser/higher] electron affinity than 'B'.
- Nuclear charge of element 'B' would be …………… [less/more] than element 'A'.
- If an element 'C' had a low electronegativity and ionization potential it would have more tendency to …………… [gain/lose] electrons.
With reference to group 1 [IA] of the periodic table – fill in the blanks with the correct word:
The elements are …………… [light/heavy] …………… [metals/non metals] since their atomic size is …………… [large/small]. The energy binding the atoms is …………… [high/low] and hence the elements have …………… [high/low] melting points. The melting points of the elements …………… [increases/decreases] down the subgroup. The electropositive character …………… [increases/decreases] down the subgroup and the elements are strong …………… [reducing/oxidizing] agents. The element with electronic configuration 2, 8, 1 will have …………… [higher/lower] electron affinity and …………… [smaller/larger] atomic size than the element with electronic configuration 2, 1.
Match the elements in column 'X' with the correct group they belong from column 'Y'
X Y 1: Element with atomic number 19 A: Group 18 [0 group] 2: Element with electronic configuration 2 B: Group 16 [VI A] 3: Element with a valency of -2 C: Group 1 [IA] 4: Element 'P' which loses 3 electrons to form a cation D: Group 17 [VII A] 5: Element 'Q' in period-3 which has the highest electron affinity E: Group 13 [III A]