is energy level depend on electrons, i means is the shell having more electrons have more energy?
the ocean absorbes solar energy because it has a low albedo.
same
For low energy bulbs the usual saving in input energy is a factor of 5, so a 95 watt bulb should consume about 20 watts. However this should be shown on the box, if you have it.
The electron configuration is why they react. The Alkali metals have one electron in their outer shell and to complete their outer shell need 7 more electrons. They can give, take or share electrons with other atoms. This is when the Halogens come in handy. The Halogens have 7 electrons in their outer shells, and need one more to complete the outer shell. These can react very easily because they have both the perfect amounts to fill their outer shells and become compounds. Other atoms with other amounts to become atoms not ions needs another element to react with. Hope this helps, Matt.
Low energy beta particles, say, from tritium, are called soft beta particles.
magnesium has a 2 valence electrons. because the third electron is not a valence electron, or in the outer shell, much more energy would be needed to remove it
The size of xenon allows the inner electrons to shield the valence shell electrons reducing the ionization energy. The ionization energy is only low enough to allow reactions with the most electronegative elements.
The ionization energy tells us about the energy required (and thus the ease) with which an atom/ion can give away an electron (in the outermost shell). So, atoms with low ionization energies ( lowest for Caesium) give away the electron with ease
have completely filled valence shell obey octet rule generally chemically inert
they have few valence electrons and aren't close to having eight valence electrons
Group A1 of the Periodic Table (Hydrogen, Lithium, Sodium . . . ) is an Alkali Metal and only has one valance electron. If the element were to lose that electron, it forms an ion. Each element violently reacts when combined with water.
The fewer numbers of valence electrons, and the farther away those valence electrons are from the nucleus, the lower the ionization energy will be. So your group 1 and 2 metals toward the bottom of those groups will have low ionization energies, and therefore be very reactive.
Since the electrons in a smaller atom are closer to the protons in the nucleus, the pull is stronger, so it tends to hold on the the electrons rather than release them during a reaction. Think of a magnet trying to lift a paper clip from far away instead of close up; that's why larger atoms tend to only loosely hold their electrons.
If you're asking how will an atom with 5 valence electrons will achieve a full set of valence electrons, then the answer would be that they bond with other atoms to gain a full set of the valence electrons by sharing or gaining 3 electrons.
The alkali metals easily yield the one electron found in their valence shell, to bond with other elements. Since it takes so little energy to remove this electron from an alkali metal (i.e., they have a low ionization energy) these metals are never found in nature in their elemental forms (they are too reactive; i.e., their atoms so easily bond to other atoms).
The valence electron shell of noble gases id completely filled; as a consequence the affinity for electrons and the chemical reactivity are at an extremely low level.
If there is an extra electron in the valence level then the electron is in the excited state and is carrying more energy. If the atom is normal then it is in the ground stte and contains low energy.