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chem periodic table
table and trends
| Question | Answer |
|---|---|
| pattern with group | elements with similar properties would be in the same group (up and down) |
| how does the periodic table fit into patterns best | when arranged by increasing atomic # rather than average atomic mass |
| Valence electrons | elements in the same group (up and down) have the same number of valence electrons. valence electrons are used for bonding |
| Octet rule | elements create bonds to have 8 valence electrons |
| metal properties | (left of staircase), shiny, high density, good conductors of heat and electricity, malleable, and ductile |
| non-metal properties | (right of staircase), gas at room temp, brittle & dull when solid, poor conductors of heat and electricity. |
| group 1 | alkali metals: (hydrogen is a non-metal and doesn't count) - very reactive metals, have 1 valence electron and from 1+ ions (looses 1) |
| group 2 | alkaline earth metals: lightly less reactive then alkali metals, have 2 valence electrons and form 2+ ins (losses 2) |
| group 3-12 | transition metals: (big middle box) moderate range of reactivity and wide range of properties, varied charge but always positive - 13 -16 (the bo at the bottom) are also transition metals |
| group 13 | have 2 valence electrons and form 3+ ions (loses 3) |
| group 14 | have 4 valence electrons, varied reactivity |
| group 15 | have 5 valence electrons, varied reactivity, can form 3- ions (gains 3) |
| group 16 | oxygen is in this group, have 6 valence electrons, reactive, can from 2- ions (gains 2) |
| group 17 | halogens: nonmetals, very reactive, 7 valence electrons, can form 1- ions (gains 1) |
| group 18 | noble gases: unreactive inert nonmetals, all colorless, odorless gasses at room temperature, have 8 valence electrons and don't form ions |
| lanthanides and actinides | also transition metals at bottom of table sp table wouldn't be wide |
| atomic radius definition | measures from center of atom to edge of electron cloud |
| atomic radius periodic trend | decreases left to right as atomic radius decrease, atomic # increases stronger effective nuclear charge pulls e- closer |
| atomic radius group trend | increases up to down going down adds energy levels more shielding effect - e- doesn't feel the pull of nucleus. like charges repel |
| what element has the largest atomic radius | francium |
| ionic radius cations | positively charged ions (1+ loses e-) radius gets smaller, same number of p+ but less e- to put;; |
| ionic radius anions | negatively charged ions (1- gains e-) radius gets bigger, same number of p+ but more e- to feel the pull |
| ionization energy periodic trend | (horizontal) increases left to right stronger effective nuclear charge, e- held tighter |
| ionization energy definition | the energy needed to remove 1 electron from an atom of an element (1st, 2nd, 3rd exist) |
| ionization energy group trend | (vertical) decreases up to down adds energy levels, e- further from nucleus, more e- shielding |
| element with the largest ionization energy | helium |
| removing electrons ionization energy | the next ionization energy always requires more energy than the one before once you remove all the valence, bug just in ionization energy e.g. Mg has 2 ve-, removing the 3rd requires A LOT of energy |
| electronegativity definition | the ability of an atom to attract electrons to itself wen part of a compound |
| electronegativity periodic trend | increases left to right stronger effective nuclear charge, stronger ability to attract another atoms e- |
| electronegativity group trend | decreases going down more energy levels. greater shielding effect weakens pull for another atoms e- |
| what to remember about electronegativity | noble ashes are exempt |
| which element is the most electronegative | fluorine (noble gases don't count) |
Created by:
Cookie~Monster