That's correct! Sulfur (S) is in the third row, so it has electrons in the third energy level. The first two levels are completely filled, giving 1s22s22p6 and it has six electrons in the third level, giving 3s23p4.
Solutions are mixtures of one or more solutes dissolved in a solvent. They do not have electron configurations. Only atoms and ions have electron configurations.
Electron configurations are only made for pure elements. The electron configuration for Hydrogen is 1s1. The electron configuration for Oxygen is 1s2 2s2 2p4
unpredictable and pattern contradict one and other. and they follow the periodic table if they are elements, ions will not
Periodicity reflects the properties of elements and represents similar electron configurations. Just took the test and got a 100% :)
Copper and Chromium have 1 electron in the 4s subshell, and 5 and 10 in the 3d subshell respectively. You needn't know beyond that until University.
All of the representative elements (s and p block) have predictable electron configurations. However, many of the transition elements have electron configurations that are not predicted by the rules for determining electron configuration.
The elements with the electron configurations that end in ns 2 and np 5 are halogens, group VII A elements.
The elements with the electron configurations that end in ns 2 and np 5 are halogens, group VII A elements.
halogens
Elements with similar electron configurations are placed in the same group.
Group 18
Each neutral atom has a specific electron cofiguration.
scandium
All halogens or group 17 elements.
electrons
protons
what column of the periodic table contains elements whose electron configurations end with d4