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2021-06-17

What is the number of electrons in the outermost energy level of an oxygen atom?

What is the number of electrons in the outermost energy level of an oxygen atom?

8

How many electrons does oxygen have in its outer shell?

six valence electrons

How do you describe element with 8 electrons in their outermost shell?

Answer. Answer: Elements with the same number of electrons in their outermost shell show similar chemical properties Example: Helium (with its 2), neon, argon, and krypton (each with 8) have “filled” their outermost shells. They are the so-called inert or “noble” gases.

What is the maximum number of electrons in the 8th energy level?

A. Energy Levels Each principal energy level can contain up to 2n2 electrons, where n is the number of the level. Thus, the first level can contain up to 2 electrons, 2(12) = 2; the second up to 8 electrons, 2(22) = 8; the third up to 18, 2(32) = 18; and so on.

What is a high energy electron?

High-energy electrons are released from NADH and FADH2, and they move along electron transport chains, like those used in photosynthesis. The electron transport chains are on the inner membrane of the mitochondrion. As the high-energy electrons are transported along the chains, some of their energy is captured.

How do electrons have energy?

The electron can gain the energy it needs by absorbing light. If the electron jumps from the second energy level down to the first energy level, it must give off some energy by emitting light. The atom absorbs or emits light in discrete packets called photons, and each photon has a definite energy.

How many energy levels are there in an atom?

Explanation: Every atom has an infinite number of energy levels available, depending on how much energy has been absorbed. In the ground state, there are seven (known/most-often-seen) energy levels which may contain electrons. The period number is the same as the highest energy level in that period at ground state.

Why are energy levels quantized?

Quantized energy levels result from the relation between a particle’s energy and its wavelength. Only stationary states with energies corresponding to integral numbers of wavelengths can exist; for other states the waves interfere destructively, resulting in zero probability density.