EN generally increases across the period and decrease down the group.Give reasons.
Asked by surajsubedi14 | 16th Jul, 2014, 09:46: AM
Electronegativity trend across group: The positively charged protons in the nucleus attract the negatively charged electrons. As the number of protons in the nucleus increases, the electronegativity or attraction will increase. Therefore electronegativity increases from left to right in a row in the periodic table.
Electronegativity trend across period: The electronegativity increases from bottom to top because the bonding pair of electrons is increasingly distant from the attraction of the nucleus.
Answered by Prachi Sawant | 16th Jul, 2014, 11:06: AM
- pls explain
- Give the name of the hardest element of group 13.
- Give the type of hybridization involved in BCl3NH3.
- Name one electron deficient compound formed by Boron.
- Give the electronic configuration of Boron.
- Aluminum can form [AlF6]− but Boron cannot form [BF6]−. Why?
- Why does boron triflouride behave as a Lewis acid?
- Why Boron forms only covalent compounds?
- Suggest reasons why the B–F bond lengths in BF3 (130 pm) and BF4- (143 pm) differ.
- If B–Cl bond has a dipole moment, explain why BCl3 molecule has zero dipole moment.
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