Ni tends to lose the 2 e - in the 4s orbital ⇒ Ni 2+ ⇒ 16 electrons in the outer shell Electron configurations with 16 electrons or half-filled orbitals can also be observedĪg: Z = 47 ⇒ 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 4d 10 5s 1Īg tends to lose the e - in the 5s orbital ⇒ Ag + ⇒ 18 electrons in the outer shell Order of orbitals that lose electrons first: 1s < 2s < 2p < 3s < 3p < 3d < 4s < 4p < 4d < 5sĪ relatively stable electron configuration for transition metals is one with 18 electrons in the outer shell.
PERIODIC TABLE OF ELEMENTS WITH TRENDS HOW TO
How to write the electron configuration of a main group element ion: ⇒ F -: 1s 2 2s 2 2p 6 (10 electrons total, isoelectronic with Ne) ⇒ Fluorine tends to gain one electron to have the number of electrons as neon Species with identical electron configuration are called isoelectronic speciesį: 1s 2 2s 2 2p 5 The nearest noble gas is neon Ne: 1s 2 2s 2 2p 6 The main group elements tend to lose or gain the number of electrons needed to get the same number of electrons as the nearest noble gas. The greater the Z eff, the higher the positive charge of the nucleus, the easier it is to add a negatively charged electron ⇒ electron affinity follows the trend of Z eff: EA increases across a period and decreases down a group.The amount of energy released when an electron is attached to a neutral atom or molecule in the gaseous state: Noble gases: great Z eff values and no valence electrons (very stable electronic structures) ⇒ high first ionization energyĪlkali metals: they want to lose one electron to have the same electronic configuration as the nearest noble gas ⇒ relatively low ionization energy Core electrons are very attracted by the nucleus ⇒ high IE ⇒ significant jump in ionization energies occurs after the outermost electrons are removed.Each additional electron is more difficult to remove (less e - e - repulsion) ⇒ the second ionization energy is greater than the first ionization energy.The greater the Z eff, the more tightly bound an electron is to an atom ⇒ ionization energy follows the trend of Z eff: IE increases across a period and decreases down a group.The closer an electron is to the nucleus, the more difficult it is to remove.Mg+ (g) → Mg 2+ (g) + e - (second ionization) Mg (g) → Mg + (g) + e - (first ionization) Second ionization energy: the minimum energy required to remove an electron from a gaseous ion X + (g)įirst and second ionization energies of Mg:.First ionization energy: the minimum energy required to remove an electron from a neutral gaseous atom X (g).The energy required to remove an electron from a gaseous atom or ion The principal quantum number n describes the size of the orbital: the larger n, the larger the orbital is ⇒ the atomic radius increases down a group.Z eff increases across a period ⇒ the atomic radius decreases across a period The higher the effective nuclear charge Z eff, the more attracted the outer electrons are to the nucleus and the closer they are to the it.
The distance between the nucleus and the outermost electrons Elements of the same period have similar valence electron configurations and therefore behave in the same way during a chemical reaction The properties of elements depend on their valence electrons.
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