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What else can I help you with?
What have stable electron configurations?
any time there are as many electrons and protons and they fill each orbital optimally.
What is true of electron configurations of the noble gases?
They all have a full set of valence electrons.
The elements Li and F combine to form an ionic compound The electron configurations in this compound are the same as the electron configurations of atoms in which group?
The electron configurations of LiF will be the same as the electron configurations of atoms in Group 18 (noble gases) because Li will lose its single electron to attain a stable octet similar to the noble gases, while F will gain an electron to achieve a complete valence shell.
Which noble gas has 5 sublevels?
None of the noble gases have 5 sublevels. All noble gases have electron configurations that end in an s or p sublevel.
Ions of CaFMg and iodine have electron configurations that are similar to which noble gases?
socks answer should be D
What is true about the electron configurations of the noble gases Decent levels are partially filled be the electrons with the highest energy you sublevel see the highest occupied SN?
The valence electron shell of noble gases is full.
Is true about the electron configurations of the noble gases?
the elections with the highest energy are in an f sub level. your welcome :))
What group attains Electron Configuration of noble gases by gaining one electron?
The group attains electron configuration of noble gases by gaining one electron is the halogens. They have seven valence electrons and need one more electron to complete their outer shell, resulting in a full valence shell like the noble gases.
Why are electron affinity values for the noble gases endothermic?
Electron affinity values for noble gases are endothermic because these elements have stable electron configurations and do not readily accept additional electrons. This makes it energetically unfavorable for them to gain an extra electron, resulting in a positive electron affinity value.
How do electron configurations of noble gases give them high unreactivity?
Noble gases have completely filled orbitals, are stable and chemically inert (non-reactive). So generally they will not form compounds.
How do the electron configurations of the noble gases make them all highly unreactive?
Noble gases have completely filled orbitals / electron energy shells. They are stable and chemically inert (non-reactive). So generally they will not accept / gain / share electrons and they do not form compounds.
What do the electron configurations for all the group 18 noble gases have in common?
All group 18 noble gases have a completely filled outer electron shell, which gives them stability and inertness. Their electron configurations end in s2p6, meaning they have a full s orbital and a full p orbital in their outermost shell.
