Question

Create representations using each of the following methods to show the formation of lithium oxide, Li2O.

a. Electron configurations

b. Orbital diagrams

c. Lewis diagrams

d. Shell models

Answer 1

To represent the formation of lithium oxide (Li2O) utilizing electron configurations, we should consider the electronic structures of lithium (Li) and oxygen (O) atoms. Lithium has an atomic number of 3, which designates it has 3 electrons. Its electron configuration is 1s^2 2s^1. Oxygen has an atomic number of 8, with an electron configuration of 1s^2 2s^2 2p^4. During the formation of Li2O, one lithium atom will transer its valence electron to an oxygen atom. This electron transfer leads to the formation of Li+ and O2- ions. The resulting electron configurations are Li+: 1s^2 and O2-: 1s^2 2s^2 2p^6. b. Orbital diagrams: To represent the formation of Li2O utilizing orbital diagrams, we can illustrate the electron distribution in the orbitals of both the lithium and oxygen atoms. In the case of lithium (Li), its orbital diagram would show one electron in the 2s orbital. Oxygen (O), on the other hand, has two electrons in the 2s orbital and four electrons in the 2p orbitals (two in each). Upon the formation of Li2O, one electron from the 2s orbital of lithium is transferred to oxygen's 2p orbitals. This results in Li+ with a vacuous 2s orbital (1s^2 2s^0), and O2- with a filled 2s and 2p orbitals (1s^2 2s^2 2p^6). c. Lewis diagrams: Lewis diagrams, additionally kenned as Lewis dot structures, can be acclimated to represent the formation of Li2O by exhibiting the valence electrons of the elements. In the case of lithium (Li), it has one valence electron, which is represented by a single dot. Oxygen (O) has six valence electrons, which would be shown as six dots (two dots paired with one another and the remaining four placed individually). When Li2O is composed, one valence electron from lithium is transferred to oxygen. This results in Li+ depicted with no dots and O2- with eight valence electrons (the pristine six, plus the transferred electron). d. Shell models: Shell models represent the energy levels or shells occupied by electrons in an atom or ion. To illustrate the formation of Li2O utilizing shell models, we can depict the electron distribution in the shells of lithium and oxygen. Lithium (Li) has two shells: the first shell (K shell) contains two electrons, and the second shell (L shell) contains one electron. Oxygen (O) has two shells as well, with the first shell containing two electrons and the second shell containing six electron. During the formation of Li2O, one electron fromm the L shell of lithium is transferred to the second shell of oxygen. This results in Li+ with only one shell (the K shell) and O2- with three shells (the pristine two, plus the transferred electron occupying the second shell).