The subshells of 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 4f act like core orbitals. This understanding of the configuration of the atom helps us to understand why electrons and atoms behave the way they do.
6s orbital and 5d orbital are the subshells in the electron configuration of valence orbitals.
Excepting the valence electrons shell all other shells are considered core orbitals.
All have the same nuclear charge and consequently the same electron configuration.
electron pairs move away from each other to more electrostatically balanced positions
There is no metal like you describe in your question. Hydrogen is in Group 1, but is not an alkali metal. It is a gas at standard temperature. It does rarely behave like an alkali metal, and it does have only one electron. Hydrogen is in Group 1 primarily because of its electron configuration, which is 1s1. All of the alkali metals also have one electron in their outermost s orbital.
Sodium chloride has got electron configuration of 2,8,1. Potassium chloride has got electron configuration of 2,8,8,1. They behave identically in almost all the chemical reactions. But then you have potassium chloride molecule inside the cell. You need to have sodium chloride molecules out side the body cell to make them survive. If you get intravenous injection of sodium chloride, nothing will happen to you. If you give intravenous injection of potassium chloride, you will die instantly. How body cells recognize the difference between sodium chloride and potassium chloride in no time is the big question mark.
Well, the act of measuring an electron's momentum changes its position, rendering the measurement invalid. This is the Heisenberg Uncertainty Principle.
Erwin Schrodinger proposed the modern atomic model, known as the "wave-mechanical" model. Essentially, he said that atoms behave like both waves and particles, and purported the concept of electron shells, subshells, and orbitals. Electrons are found on "shells" of charge outside the atom. These shells divide into subshells, which divide into orbitals.
how electrons behave in their orbitals
Yes, chemical similarities exist between hydrogen and alkali metals; also the electron configuration has a parallel.
All have the same nuclear charge and consequently the same electron configuration.
a spinning electron produces a magnetic field that makes the electron behave like a tiny magnet
electron pairs move away from each other to more electrostatically balanced positions
the power from te cord go on the metal so when you touch it you get shocked
Hydrogen
An electron cloud surrounding an atom is a visualization tool to allow for the discussion of atomic proberties. Since electrons behave with wavelike properties, the "cloud" is a representaion of the probability density of the electron's wavefunctions.
Hydrogen is on the left side because it has the same valence electron configuration as all the other elements in its family/group. Hydrogen, Lithium, Sodium, Potassium, Rubidium, Cesium, and Francium all contain one valence electron.
There is no metal like you describe in your question. Hydrogen is in Group 1, but is not an alkali metal. It is a gas at standard temperature. It does rarely behave like an alkali metal, and it does have only one electron. Hydrogen is in Group 1 primarily because of its electron configuration, which is 1s1. All of the alkali metals also have one electron in their outermost s orbital.
Any particle, such as an electron, also behaves as a wave (as well as behaving like a particle).