Noble gasses are historically known as inert gasses - so true
TRUE (apex)
No, the electron configuration for an ion is not always the same as that of its nearest noble gas. When an atom loses or gains electrons to form an ion, its electron configuration changes. For example, a sodium ion (Na⁺) has the electron configuration of [Ne], which is the same as neon, but a chloride ion (Cl⁻) also has the same configuration as argon ([Ar]). Thus, while some ions can have configurations similar to noble gases, this is not universally true for all ions.
Noble gases have completely filled orbitals. They generally have 8 valence electrons (helium has only 2) and obey octet rule (stable electronic configuration). Hence they are chemically inert (or do not react with other elements).
Ions that are formed when metals gain electrons are called anions. This process allows metals to achieve a stable electron configuration by filling their outermost energy level, similar to noble gases.
Noble gasses are historically known as inert gasses - so true
TRUE (apex)
No, the electron configuration for an ion is not always the same as that of its nearest noble gas. When an atom loses or gains electrons to form an ion, its electron configuration changes. For example, a sodium ion (Na⁺) has the electron configuration of [Ne], which is the same as neon, but a chloride ion (Cl⁻) also has the same configuration as argon ([Ar]). Thus, while some ions can have configurations similar to noble gases, this is not universally true for all ions.
Noble gases have completely filled orbitals. They generally have 8 valence electrons (helium has only 2) and obey octet rule (stable electronic configuration). Hence they are chemically inert (or do not react with other elements).
Ions that are formed when metals gain electrons are called anions. This process allows metals to achieve a stable electron configuration by filling their outermost energy level, similar to noble gases.
The pseudo noble-gas electron configuration has the outer three orbitals filled, the s, p and d- s2p6d10 (18 electrons total) and so is fairly stable. Elements that attain this electron configuration are at the right side of the transition metals (d-block). Br-, I-, Se2-
False. Alkali metals lose one electron to form a stable electron configuration with a full outer shell of electrons, which is the stable electron configuration for these elements.
Krypton and argon both have 8 valence electrons. This is true of all noble gases except helium, which has only 2 valence electrons.
True. Elements of the halogen family readily lose one electron to attain a stable electron configuration and become halide ions with a negative charge. This makes them highly reactive and likely to form ionic bonds with other elements.
They all have a full set of valence electrons.
All elements tend to react with other elements so as to attain a noble gas electronic configuration in their ions, because such a configuration usually has the lowest energy for a particular atom or ion, other factors being equal. The drive to form such an ion is strongest when the electron configuration of an elemental atom differs from the closest noble gas configuration by only one electron, and this criterion is true for both group and group 17 elements: Group 1 elements can attain a noble gas electron configuration by donating one electron to another atom, and Group 17 elements can attain a noble gas configuration by accepting one electron, thereby filling their valence shell.
The valence electron shell of noble gases is full.