Electronic Structure 0.0 / 5 ? ChemistryElectronic StructureASWJEC Created by: zoolouiseCreated on: 28-03-16 13:31 What do electrons within atoms occupy? Fixed energy levels, or shells. They're numbered 1, 2, 3, 4, etc and the numbers are known as principle quantum numbers, or n. 1 of 13 What does the lower the value of n mean? The lower the value of n, the closer the shell is to the nucleus and therefore the lower the energy level. 2 of 13 What are atomic orbitals? Regions of space around the nucleus where there's a high probability you'll find an electron with a given energy. 3 of 13 What's the definition of an atomic orbital? An atomic orbital is a region in an atom that can hold up to two electrons with opposite spins. 4 of 13 What are subshells? Orbitals of the same type being grouped together. 5 of 13 How many electrons can each orbital hold? Each orbital can hold two electrons with opposing spins, reducing the effect of repulsion. 6 of 13 What is an S orbital? An S orbital is spherical and often drawn as a circle. 7 of 13 An S orbital is spherical and often drawn as a circle. P orbitals come in three different types, they are dumbell shaped probes. They're known as px, py and pz. They're at right angles to eachother. 8 of 13 How many electrons can each different subshell hold? S subshells can hold 2 electrons, P subshells can hold 6 electrons, D subshells can hold 10 electrons and F subshells can hold 14 electrons. 9 of 13 What is Aufau principle? Electrons fill atomic orbitals in order of increasing energy. 10 of 13 What is the Pauli exclusion principle? A maximum of two electrons can occupy each orbital with opposing spins. 11 of 13 What is Hund's rule? The orbitals will first fill with one electron each with parallel spins, before a second electron is added with the paired spin. 12 of 13 What is the variation when filling subshells? An order is followed up until the 3p subshell, the 4s subshell is filled before the 3d subshell. 13 of 13
Comments
No comments have yet been made