![]() Same electron configuration as neon) is called nitride. A nitrogen atom with three extra electrons (to get to the Two extra electrons (to get to the same electron configuration as neon) isĬalled oxide. That has an extra electron is called a chloride ion. Notice the change in the name of chloride: frequently, when an elementīecomes an anion, the end of its name changes to "ide". If the atom or ion has the same electron configuration as a noble gas, state Ions (without using the nobel gas abbreviation for the outermost shell). Provide the electron configuration for the following atoms or Given the following pairs of atoms, which one is most likely Like-ions are balanced by attractive forces with oppositely-charged ions. The presence of anions, and vice versa, so that repulsive forces between The attraction of theĭelocalized electrons for the metal cations offsets any repulsion between theįor that reason, we will see that cations are generally found in The cations are partly held together by the presence ofĭelocalized electrons in the block of metal. Those like charges should push the metal cations awayįrom each other, but most metals don't spontaneously fly apart into tiny ![]() In the electron sea model of metals, metal cations exist inĪ block of metal. Two atoms might not repel each other, but twoĬations would. What happens to these atoms as they gain or lose an electron? OfĬourse, having an overall charge on an atom introduces an additionalĮlectrostatic problem. Positive or an overall negative charge on the atom. In an ion, the number of protons in the nucleus is notĮxactly balanced by the number of electrons, so there is either an overall In general, atoms that have an overall charge are called For a sodium atom, it is simplyĬloser to get to the same configuration as neon than it is to get to the sameĬonfiguration as argon. Gaining some extra electrons, other elements can more easily gain thatĬonfiguration by losing some electrons. Just as some elements attain a noble gas configuration by Atoms in the lower left part of the periodic table.The alkalis, such as sodium and potassium. Cations are atoms that have lost electrons, so that they have an These atoms are principally found in nature as cations Periodic trends also tell us that some atoms lose electrons easily to obtainĪ stable configuration these atoms have a low ionization potential. For example, if oxygen gains two electrons, it attains Other atoms can gain a similarly stable electron configuration by gaining or Would have to go into a much higher energy level in the next "shell". However, they have a "closed shell" configuration, meaning that any additional electrons Gases, high electronegativity might be thought of as a measure of the stability Is true even though they have high electronegativities in the case of noble The noble gases have particularly stableĮlectron configurations, however, and do not gain or lose electrons easily. This In a chemical reaction, electrons are somehow Same electron configuration as a noble gas.Įxceptional in the periodic table because they do not easily undergo reactions Side of the periodic table are likely to gain enough electrons to attain the Relatively high positive charge in the nuclei of these atoms makes theirĪnother thing to remember is that atoms towards the right hand A look at the periodic table shows the highĮlectronegativity of atoms in the upper right part of the table. One of the most commonly-used periodic properties isĮlectronegativity. Atoms in the upper right section of the periodic table can easily form.The halogens, such as chlorine and bromine. Anions are atoms that have gained extra electrons, and have These atoms are principally found in nature as anions Periodic trends tell us that some atoms gain electrons easily to obtainĪ stable configuration these atoms have a high electron affinity.
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