![]() ![]() Explain to Mendeleev, in 3 to 4 sentences, how and why the periodic table has changed. The noble gases do not have electronegativity values because they have a complete valence level.ĩ.ĝescribe and explain the pattern in atomic radius for the first 18 elements.Ītomic radius decreases across a period and increases down a group.Īs you go across a period from left to right, the nuclear charge increases so the valence level electrons are attracted more strongly to the nucleus, decreasing the distance from the nucleus, which in turn decreases the atomic radius.ġ1. Describe and explain the pattern in electronegativity for the first 18 elements.Įlectronegativity increases across a period and decreases down a group.Ĩ.Ğxplain how electronegativity is related to electron configuration.Īs the valence level fills with electrons, it requires more energy to attract bonding pairs of electrons because there must be enough energy to overcome the repulsion of electrons already in the valence level. As an electron gets further from the nucleus, the weaker the nuclear attraction becomes, requiring less energy to remove an electron. Removing an electron requires more energy. The larger the positive charge of the nucleus is, (more protons), the greater the nuclear charge and attraction for electrons. Explain how ionization energy is related to electron configuration. If electrons are lost, the charge is positive, and if electrons are gained, the charge is negative.ĥ.ĝescribe and explain the pattern in first ionization energy for the first 18 elements.įirst ionization energy increases across a period (row) and decreases down a group (family or column).Ħ. The number of electrons lost or gained determines the magnitude of the charge. Explain how ionic charge is related to the number of valence level electrons. If electrons are gained, there is a negative ionic charge.Ĥ. If electrons are lost, there is a positive ionic charge. The general pattern for ionic charge going horizontally across a period is 1+, 2+, 3+, 4+, 4-, 3-, 2-, 1-, 0. Since He, Ne, and Ar all have full valence levels and do not gain nor lose electrons, they have an ionic charge of 0. It will neither gain nor lose electrons because its valence level is also full. He has a full valence level with just 2 electrons, since all of its electrons are in level 1. Ne and Ar have a full valence level with 8 electrons, so they will neither gain nor lose electrons. He, Ne, and Ar are all found in column 18. They lose a single valence electron, giving a 1- charge, and are in column 17. O and S gain 2 electrons, resulting in a 2- charge, and are found in column 16. They are in column 15 on the periodic table. ![]() Nitrogen can lose all 5 electrons, resulting in a 5+ charge. N and P have 5 valence level electrons, so they will likely gain 3 electrons, resulting in a 3- charge. They are in column 14 of the periodic table. They have an ionic charge of 4- or 4+ respectively. C and Si have 4 valence level electrons, which means they can gain 4 electrons or lose 4 electrons. They are in column 2 of the periodic table.ī and Al have 3 valence level electrons, an ionic charge of 3+, and lose 3 valence level electrons. Excepting helium, elements with 2 valence level electrons (Be and Mg) have an ionic charge of 2+ and lose 2 electrons. ![]() They are in column 1 of the periodic table. Level 3, elements 11 to 18, follow the same pattern as level 2-1 to 8 valence level electrons.ģ.ĝescribe and explain the pattern in ionic charge for the first 18 elements.Įlements with 1 valence level electron (H, Li, Na) have an ionic charge of 1+ and lose 1 electron. Level 2, elements 3 to 10, have 1 to 8 valence level electrons respectively. The first row, H and He, has 1 and 2 valence level electrons. Describe and explain the pattern in the number of valence level electrons for the first 18 elements. Eight electrons need to be added to the third level to complete it.Ģ. Elements 11 to 18 follow the same pattern as elements 3 to 10, except electrons are placed in the third level instead of the second level. Elements 3 to 10 fill 1s, 2s, and 2p, totaling 8 electrons for the level. Describe and explain the pattern in electron configurations for the first 18 elements. ![]()
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