Quantum numbers<span> allow us to both simplify and dig deeper into electron configurations. Electron configurations allow us to identify energy level, subshell, and the number of electrons in those locations. If you choose to go a bit further, you can also add in x,y, or z subscripts to describe the exact orbital of those subshells (for example </span><span>2<span>px</span></span>). Simply put, electron configurations are more focused on location of electrons then anything else.
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Quantum numbers allow us to dig deeper into the electron configurations by allowing us to focus on electrons' quantum nature. This includes such properties as principle energy (size) (n), magnitude of angular momentum (shape) (l), orientation in space (m), and the spinning nature of the electron. In terms of connecting quantum numbers back to electron configurations, n is related to the energy level, l is related to the subshell, m is related to the orbital, and s is due to Pauli Exclusion Principle.</span>
If an atom gains electrons, it develops a negative charge equal to the number of electrons gained.
So the net charge on the copper atom which gained 2 electrons will be -2.
Answer:
V = V0 + a t
V = 75 - 9.8 * 3 = 45.6 m/s
<span> A pure substance is an material which contains atoms of only one kind.
It has fixed physical and chemical properties such as boiling point, melting point, valency, density and more.</span>
