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Answer:
The electron configuration for Copper (Co) is: 1s2 2s2 2p6 3s3 3p6 4s2 3d7.
The atom is the building block of matter. It is not indivisible, though, as the Greek origin of its name indicates. Over the past two centuries, experimentalists have identified numerous particles that comprise an atom. For the purposes of chemistry, we are interested in three of these particles: the proton, the neutron, and the electron.
An atom consists of a central nucleus of protons and neutrons, and electrons that orbit the nucleus.
The proton has an electric charge of +1e, or 1.602 x 10-19 Coulombs (a Coulomb is a unit of electric charge. For convenience, the charges of subatomic particles are usually described as multiples of the value e, the charge of one electron, called the elementary charge.)
The neutron has no charge (it is electrically neutral.)
The electron carries a negative charge: -1e. Electrons are bound to the nucleus by their electromagnetic attraction to the positively-charged protons. An atom in its neutral state always has the same number of protons as electrons. The positive and negative charges cancel, and thus the net charge of the atom is zero.
The true nature of the electrons' movement around the nucleus is complex. As an introduction, it's useful to present the Classical Model of atomic structure. This is a simplified scenario in which we regard the electrons as discrete objects orbiting at known, fixed distances from the nucleus.
THE CLASSICAL MODEL OF ELECTRON ORBITAL CONFIGURATION
The electrons orbit only in certain "allowed" regions around the nucleus. The farther an electron orbits from the nucleus, the higher the energy associated with it. Through energy transfers during collisions with other particles or with light, it is possible for electrons to move up to orbitals of higher energy. In this case, we say that the atom is in an excited state. Here, we will only describe ground state electron configurations.
Each energy level, or shell, contains one or more orbitals. Each orbital contains one or more subshells. A subshell has a place for up to two electrons. Electrons "fill up" orbitals from the lowest energy up -- that is, the second orbital does not contain an electron unless the first orbital is already full.