What does a closed shell mean? + Example - Socratic
2018年3月30日 · That's just another way to say that there are zero unpaired electrons in all occupied orbitals. Atoms like "Kr" (noble gas), "Zn"^(2+) (argon configuration), etc. are closed-shell. "O"_2^(2-) is an example of a closed-shell molecule, whereas "O"_2 is an open-shell molecule. Various open-shell cases exist.
What is a noble gas electron configuration? - Socratic
2017年8月24日 · Well, helium has a closed shell, 1s^(2) electronic configuration.... In order to save some time when writing the configuration of the next element, Li, Z=3, I could write [He]2s^(1); all the reactivity is going to occur in the valence shell. And likewise for say sulfur, Z=16, which builds on a neon core, we could write, [Ne]3s^(2)3p^4, instead of the long 1s^(2)2s^(2)2p^(6)3s^(2)3s^4. The ...
How do valence electrons affect chemical bonding? | Socratic
2014年2月13日 · The number of electrons in an atom's outermost valence shell governs its bonding behaviour. Elements whose atoms have the same number of valence electrons are grouped together in the Periodic Table. Generally, elements in Groups 1, 2, and 13 to 17 tend to react to form a closed shell with the electron configuration s²p⁶. METALS The most reactive metals are those from Groups 1 and 2. They ...
How do valence electrons affect reactivity? + Example - Socratic
2014年1月10日 · The valence electrons are the electrons in the outermost electron shell of an atom. That is why elements whose atoms have the same number of valence electrons are grouped together in the Periodic Table. Generally, elements in Groups 1, 2, and 13 to 17 tend to react to form a closed shell, corresponding to the electron configuration #s^2p^6#.
How do valence electrons determine chemical properties?
2014年2月13日 · It is not the valence electrons themselves, but the number of valence electrons that determines the chemical properties of an element. Elements whose atoms have the same number of valence electrons are grouped together in the Periodic Table. Generally, elements in Groups 1, 2, and 13 to 17 tend to react to form a closed shell with a noble gas electron configuration ending in ns^2 np^6. METALS ...
How do you determine the electron configuration of Cl?
2016年7月5日 · In most cases, you can tell the electron configuration from the position in the Periodic Table, but sometimes there are exceptions. Fortunately, Cl is easy. Chlorine (Cl) is element 17, and it lies in the third row (period) in the next-to-last column. The previous rare gas element is neon (Ne, element 10), which has a closed-shell configuration: [Ne] = (1s)^2(2s)^2(2p)^6 Chlorine has this core ...
How do you do shorthand notation for electron configuration?
2017年9月14日 · Well, we know that the elements build on a closed-shell inert gas configuration.... And thus we have for He, Z=2, i.e. 1s^(2). For Li, Z=3, we could write [He]2s^1; or for Na, Z=11, Mg, Z=12, we could write....[Ne]3s^1, or [Ne]3s^2 respectively. All the chemistry is going to occur with respect to the valence electrons, and the inner core in largely inert.....
What is the electron configuration of Au+? - Socratic
2016年1月3日 · [Xe] 4f^14 5d^10 The atomic number of Au is 79. Therefore, its configuration is: 1s^2 2s^2 2p^6 3s^2 3p^6 3d^10 4s^2 4p^6 4d^10 5s^2 5p^6 4f^14 5d^10 6s^1 or, [Xe] 4f^14 5d^10 6s^1 For Au^+, one electron is removed from the outermost 6s orbital, making the configuration, [Xe] 4f^14 5d^10
How do valence electrons determine chemical reactivity?
2014年1月7日 · The valence electrons are the electrons in the outermost electron shell of an atom. > The number of electrons in an atom's outermost valence shell governs its bonding behaviour. That is why elements whose atoms have the same number of valence electrons are grouped together in the Periodic Table. Generally, elements in Groups 1, 2, and 13 to 17 tend to react to form a closed shell ...
Valence Electrons - Chemistry - Socratic
Generally, elements in Groups 1, 2, and 13 to 17 tend to react to form a closed shell with a noble gas electron configuration ending in #ns^2 np^6#. METALS. The most reactive metals are those from Groups 1 and 2. They need to lose only one or two valence electrons to form positive ions with a noble gas configuration. NONMETALS