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| atomic number--equals number of protons |
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| mass number--number of protons and neutrons |
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| isotopes differ in the number of ______ so they have a different ____ ___ |
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| formula for angular momentum of an electron: |
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| angular momentum = nh/2pi |
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| equation for Energy of an electron |
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| equation for energy of a photon |
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| pauli exclusion principle: |
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| no two electrons in a given atom can possess the same set of four quantum numbers |
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| principle quantum number means |
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| equation for the maximum number of electrons in an energy level: |
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| angular momentum: subshells: s,p,d,f |
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| magnetic quantum number stands for: |
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Definition
| orbit, so for example: px, py, pz |
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Definition
| bus rule: orbitals fill sot hat there are a maximum half filled orbitals with parallel spins |
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Definition
| material has unpaired electrons |
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| material has NO unpaired electrons |
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| chemical properties of elements are dependent upon their atomic numbers |
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| non-representative elements |
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| transition elements have partly filled ______ |
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| lanthanide and actinide series have partly filled _____ |
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| noble gases also called... |
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| atomic radii increases across the periodic table: |
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| ionization energy increases across the periodic table: |
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Definition
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| electronegativity increases across the periodic table: |
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Definition
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| electron affinity increases across the periodic table: |
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Definition
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| effective charge increases across the periodic table: |
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Term
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Definition
| energy required to completely remove an electron from a gaseous atom or ion |
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| second ionization is always ____ than the first ionization energy |
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Definition
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Term
| atomic radii trend is due to... |
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Definition
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| ionization energy trend is due to the fact that |
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Definition
| it is harder to remove an electron if it is closer and more tightly bound |
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Term
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Definition
| energy change that occurs when an electron is added to a gaseous atom--- also the ease with which the atom can accept an electron |
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Term
| the stronger the attractive pull of the nucleus for electrons.... |
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Definition
| the greater the electron affinity will be |
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| electron affinity of noble gases is... |
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Definition
| about zero because they already possess a stable octet |
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Definition
| measure of the attraction an atom has for electrons in a chemical bond |
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| the greater the electronegativity of an atom the greater its attraction for... |
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Definition
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| electronegativity is related to |
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| categories of elements on periodic table: |
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| 1. metals 2. nonmetals 3. metalloids |
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| metals have ____ melting points |
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| metals have ___ densities |
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Definition
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| metals are shiny or dull? |
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Definition
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| metals are malleable or brittle? |
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| _____ is the largest, most metallic and least electronegative of all naturally occurring elements |
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Definition
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Definition
| ability to be drawn into wires |
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characteristics of metals:
____ atomic radius
____ ionization energy
____ electronegativity |
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Definition
| large, low, low---- because the few electrons in the valence shell of a metal can easily be removed |
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| are metals good conductors? |
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Definition
| yes--of heat and electricity |
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| most reactive metals are where on the periodic table? |
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Definition
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| most electronegative element? |
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Definition
| flourine F, largest electron affinity |
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| are nonmentals malleable or brittle? |
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Definition
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| are nonmetals shiny or dull |
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Definition
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characteristics of nonmetals:
____ ionization energies
_____ electronegativities |
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Definition
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| are nonmetals good conductors? |
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Definition
| no-of neither heat nor electricity |
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| can nonmetals gain electrons easily? |
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Definition
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| _____ can explain all periodic trends as well as chemical properties |
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Definition
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| properties of metalloids: |
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Definition
| vary considerably--- densities, bp and mp fluctuate widely |
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Term
| metalloids have characteristics of |
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Definition
| both metals and nonmetals mixed--- very dependent on element |
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| characteristics of metalloids depends greatly on |
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Definition
| what element they are being reacted with |
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| elements that are metalloids: |
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Definition
| boron (B), silicon (Si), germanium (Ge), arsenic (As), antimony (Sb), and tellurium (Te) |
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Definition
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| alkali metals have densities ____ than of other metals |
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Definition
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| alkali metals are highly reactive because they have |
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Definition
| low ionization energies and easily lose their valence electron |
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Definition
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| removing electrons from alkaline earth metals produces: |
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Definition
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| halogens have _____ physical properties |
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Definition
| varying: gas to liquid to solid |
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Term
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Definition
| alkali metals and alkaline earth metals because they want to donate electrons to the halogens |
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| halogen + alkali metal or alkaline earth metal = |
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| fairly nonreactive because of complete valence shell |
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noble gas characteristics:
____ boiling points |
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characteristics of transition metals:
____ melting points
____ boiling points |
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Definition
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| transition metals can exist in a variety of positively charged forms called |
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Definition
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| the formation of complexes by the transition metals causes the orbitals to |
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Definition
| split into two energy sublevels |
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Term
| rule for filling orbitals: |
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Definition
(n+ l) of each orbital and then see whatever one is a lower number--- fill that one first
so 4s vs. 3d
4 + 0 = 4 and 3 + 2 =5 so fill 4s first |
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| if the (n + l) rule results in a tie fill orbital with |
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Definition
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Definition
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Definition
| number of protons + number of neutrons |
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Definition
| weighted average of all isotopes |
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Definition
| fully filled and half filled subshells |
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| effective nuclear charge: |
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Definition
| attractive, positive charge of the nucleus perceived by a valence electron |
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Definition
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| O has a lower ionization energy than N because |
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Definition
| N is already half filled, removing one from O gives a half filled |
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Term
| electron affinity is a ___ number so energy is ____ when an electron is added |
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Definition
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Term
| noble gases and half filled orbitals will have a ____ delta E relating to electron affinity because |
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Definition
| positive, it doesn't want electrons |
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Term
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Definition
| energy emitted as electromagnetic radiation from matter exists in discrete bundles called quanta |
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Term
| heisenberg uncertainty principle |
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Definition
| impossible to know the momentum and position of an electron at the same time |
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