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unit three
chemical periodicity
| Question | Answer |
|---|---|
| the periodic laws | the properties of the elements are a periodic function of their atomic number |
| metals are... | lustrous, good conductors of hear/electricity, ductile, tenacious, malleable |
| nonmetals are... | dull, poor conductors of heat/electricity, brittle |
| malleable | hammered into a sheet |
| tenacious | bendable rather than breakable |
| ductile | form it into a wire |
| brittle | breaks away |
| ionization energy | energy required to remove an electron from an atom /or the energy required to remove an electron from a gaseous atom |
| cation | + ion |
| anion | - ion |
| atomic radius | distance (nucleus to the edge of the electron cloud) of an atom |
| atomic radius increases... | down the group due to increasing electron shells |
| atomic radius decreases... | across the period due to increasing effective nuclear charge |
| how to find effective nuclear charge? | number of protons - core electrons |
| What do core electrons shield? | valence electrons so that valence electrons don't feel the full attrition of the nucleus |
| zeff | effective nuclear charge |
| What are cations? | smaller than their atom due to fewer electron shells |
| What are anions? | larger than their atom due to more electron shells |
| ionization energy decreases... | down a group because valence electron are further from the nucleus |
| ionization energy increases... | across a period, due to increasing effective nuclear charge making it harder to remove electrons |
| more electron shells = | less attraction of the nucleus for the electrons |
| electronegativity | the tendency of an atom to attract electrons to itself in a bond |
| electronegativity decreases... | down a group because bonded electrons are further from the nucleus and therefore less strongly attracted to it |
| electronegativity increases... | across a period die to increases effective nuclear charge making increases attraction |
| what to talk about if it is atom smaller than atom (apsq)? | same group - different amount of electron shells (talk about each atom) same period - different zeff causing atom with higher zeff to have higher force of attraction (smaller atomic radius) |
| what to talk about if it is atom higher ionization energy than atom (same groups)(apsq)? | same group - valence electrons, electron shells, valence electrons closer to nucleus because of electron shells, more energy to remove electron because of closer |
| what to talk about if it is atom higher ionization energy than atom (same period)(apsq)? | same period - different zeff, higher one has a greater force of attraction, electrons held more tightly needing higher ionization level to remove valence electron |
| what to talk about if it is ion of atom (negative) larger ionic radius than regular of the same atom (apsq)? | same protons, extra electron, more repulsion, ion with expand to larger radius |
| representative elements | elements in which all the inner shells are complete but outer shell is incomplete |
Created by:
kyla_snyder_
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