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Electrons reside in shells and orbitals The arrangement of electrons around the atomic nucleus is complex, and electrons do not simply orbit the nucleus as a planet would orbit a star. Broadly speaking, electrons are located in concentric shells that surround the nucleus. The shells that are closer to the nucleus are generally lower
A sodium atom spontaneously loses an electron to get a full shell of electrons. A Na7- ion is more stable than a sodium atom because it has a full shell of electrons. A Cl7+ ion is just as stable as a Cl- ion because they both have a full shell of electrons.
23 wrz 2022 · The tendency to form species that have eight electrons in the valence shell is called the octet rule. The attraction of oppositely charged ions caused by electron transfer is called an ionic bond. The strength of ionic bonding depends on the magnitude of the charges and the sizes of the ions.
Sodium readily gives up that single third-shell electron, and when it loses this one negative charge, it becomes positively charged (because it now has 11 protons and only 10 electrons). By giving up its lone third-shell electron, sodium ends up with a full outer shell.
20 lip 2023 · These elements, including hydrogen (H), lithium (Li), and sodium (Na), all have one electron in their outermost shells. That means that they can achieve a stable configuration and a filled outer shell by donating or sharing one electron with another atom or a molecule such as water.
Sodium has 11 electrons: two in the first shell, eight in the second, and one in the third (Figure 2.2.1). Sodium readily gives up that single third-shell electron, and when it loses this one negative charge, it becomes positively charged (because it now has 11 protons and only 10 electrons). By giving up its lone third-shell electron, sodium ...
15 sty 2024 · Most of the elements that make ionic compounds form an ion that has a characteristic charge. For example, sodium makes ionic compounds in which the sodium ion always has a 1+ charge. Chlorine makes ionic compounds in which the chloride ion always has a 1− charge. Some elements, especially transition metals, can form ions of multiple charges.
