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| Distribution of electrons in an atom/molecule in their orbitals |
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| Electron configuration with the lowest energy levels |
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| A diagram of the electron population within the orbitals |
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| m sub s, an upwards or downwards arrow |
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| Pauli exclusion principle |
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| no two electrons can have the same quantum numbers |
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| Elements with sumilar physical/chemical properties fall within the same column (up and down on per. table) |
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| Fill the lowest energy levels first |
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| Electrons in the outermost shell |
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| Electrons are placed individually in orbital diagrams until full |
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| Noble gas orbital diagrams are |
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| Created the modern periodic table |
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| What did the periodic law do? |
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| It allowed for predictions not yet discovered |
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| electrons that are not valence electrons |
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| How do valence electrons explain periodic law? |
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| Elements in the same column/family have same v.e. #, similar properties |
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| Anomalous electron config. |
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Definition
| S-orbital partially fills before d-orbital begins to fill, or s-orbital is skipped |
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| How do valence electrons explain periodic law? |
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Definition
| Elements in the same column/family have same v.e. #, similar properties |
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| Anomalous electron config |
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Definition
| S-orbitals only partially filled before electrons move to d-orbital, or s-orbital skipped |
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Definition
| Chromium, copper, silver, gold, and paladium. |
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| Config of the 5 anomalous elements |
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Definition
Cr= [Ar] 4s1 3d5
Cu= [Ar] 4s1 3d10
Ag= [Kr] 5s1 4d10
Au= [Xe] 6s1 5d10
Pd= [Kr] 4d10 |
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| Element with a positive charge due to losing an electron |
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| Element with a negative charge due to gaining an electron |
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| 2 valence electrons (helium) |
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| What tends to form cations? |
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| What tends to form anions? |
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| Group 1A and 2A lose what valence electrons to form cations? |
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| D-block (transition metals) lose what electrons first, and then the next? |
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| Attracted to magnetic field because of unpaired electrons |
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| Repelled by magnetic field due to all paired electrons |
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Definition
| Pull/force an electron "feels" from the nucleus due to protons |
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| The pull on electrons is greater when |
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Definition
| closer to the nucleus, or less core electrons |
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| the pull on electrons is weaker when |
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Definition
| farther from nucleus, or more core electrons |
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Term
| which electrons feel more Zeff? |
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Definition
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| which electrons feel less Zeff? |
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Definition
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Definition
| Outer valence e- don't feel the charge of the nucleus due to core e- |
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| Gives indication of size of atom |
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| The atomic radius is larger when what is weaker? |
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Definition
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| The atomic radius is smaller when |
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| What causes the atomic radius to be larger or smaller? |
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Definition
| The number of electrons inbetween the valence and nucleus |
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| Which ion is smaller and why |
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Definition
| Cations- they lose electrons |
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| Which ion is larger and why |
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Definition
| Anions- they gain electrons |
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| Which is larger- Br- or Kr? |
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Definition
| Bromine, both have the same amount of electrons but Krypton has more protons, so Bromine is larger |
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| Which is larger- Li or Ne? |
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Definition
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| Energy required to remove an electron from an atom |
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| As Zeff increases, what gets stronger? |
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Definition
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| Why does IE become stronger when Zeff increases? |
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Definition
| When an electron is pulled away, the Zeff force gets stronger due to protons, so the energy required to pull away an electron is greater. |
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| IE means it's doing work on the system in order to remove the electron |
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| Change in energy when an atom gains an electron to form an anion |
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| In terms of heat, electron affinity is |
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Definition
| either exothermic or endothermic |
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| When it comes to electron affinity, what family tends to be exothermic? |
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Definition
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| EA becomes more _____ across a period |
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| Negative energy in terms of EA tells us what? |
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| It's an exothermic reaction |
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Definition
| Trend occurring from left to right- rows |
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| Periodic trend for atomic radius |
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Definition
| As the # of electrons goes up, the radius becomes larger. |
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| Periodic trend for ionization energy |
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Definition
| As you go from left to right, ionization energy takes less force because there are more electrons and less force from Zeff |
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| Achieving an octet maximizes ______ and minimizes ______ |
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| Bond between a metal and nonmetal where the electron(s) are transferred. |
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| Bond between two nonmetals- shared. |
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| Bond among metals, communal sharing |
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| Polar bonds are inbetween what? |
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| Important physical property of ionic compounds |
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Definition
| Conducive of electricity in aqueous conditions |
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| Covalent bonding is a result of what? |
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Definition
| Overlap of atomic orbitals |
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| Physical property of covalent compounds |
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Definition
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| Examples of metallic bonders |
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Definition
| Iron, copper, silver, gold |
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| Physical properties of metallic bonders |
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| Malleable, ductile, can conduct heat and electricity |
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| Ability of an atom in a bond to attract electrons to itself |
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| When does a dipole occur? |
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Definition
| One side of a molecule is +, and the other side is - |
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| Electronegativity increases across a _____ and up a _____ |
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| > or equal to 2.0 (electronegativity) |
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| Why do chemical bonds form? |
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Definition
| They lower the potential energy between the charged particles. |
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