Which anion is larger se2 or te2

Please explain why you chose this order. Jacob T. Jun 23, Explanation: All five ions have an equal number of electrons and therefore share the same electron configuration.

Related questions What happens to ionic size down a group? What happens to ionic size across a period? How does ionic size change? How does ion size affect conductivity? Can I determine the ion size by charge? Question 78b The primary reason sodium ions are smaller than sodium atoms is that the ion has only two shells Which arrangement is in the correct order of radius size?

Study lib. Upload document Create flashcards. Flashcards Collections. Documents Last activity. Add to Add to collection s Add to saved. Chem 2 AP Homework Problems pg. For elements in the same group, the most important relationship is having the same number of valence electrons, so they have similar chemical properties. Metals: malleable, ductile, generally shiny, electrically and thermally conductive, medium to high melting points, lose electrons in chemical reactions.

Non-metals: dull, brittle, electrically and thermally insulating, low melting and boiling points, generally gain electrons in chemical reactions. For representative elements, the number of valence electrons of an element is equal to its group number. Al: 3 v. Explain why hydrogen can resemble the Group 1A and the Group 7A elements.

Two species are isoelectronic if they have the same number of electrons. Can two neutral atoms of different elements be isoelectronic? How does the size of an atom change when it is converted to a and anion and b a cation? The ionic radius is the radius of a cation or anion. Cs is below Na in the same group, so its valence electrons are in a more shielded orbital at a higher energy, thus experience less coulombic attraction to the nucleus..

The electron configuration of lithium is 1s22s1. The two 1s electrons shield the 2s electron effectively from the nucleus. Consequently, the lithium atom is considerably larger than the hydrogen atom. Explain the trend. The atomic radius is largely determined by how strongly the outer-shell electrons are held by the nucleus. The larger the effective nuclear charge, the more strongly the electrons are held and the smaller the atomic radius.