Gen Chem 2- Test 2 – Flashcards
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| Electron configuration |
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| Distribution of electrons in an atom/molecule in their orbitals |
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| Ground state |
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| Electron configuration with the lowest energy levels |
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| Orbital diagram |
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| A diagram of the electron population within the orbitals |
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| Electron spin |
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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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| Periodic law |
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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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| Aufbau principle |
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| Fill the lowest energy levels first |
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| Valence electrons |
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| Electrons in the outermost shell |
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| Hund's rule |
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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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| Stable (full) |
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| n |
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| energy level |
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| l |
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| orbital type |
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| m sub l |
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| orientation |
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| m sub s |
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| electron spin |
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| Dmitri Mendeleev |
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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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| order of energy levels |
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| s, p, d, f |
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| core electrons |
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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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| 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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| Elements in the same column/family have same v.e. #, similar properties |
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| Anomalous electron config |
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| S-orbitals only partially filled before electrons move to d-orbital, or s-orbital skipped |
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| 5 anomalous elements |
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| Chromium, copper, silver, gold, and paladium. |
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| Config of the 5 anomalous elements |
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| Cr= [Ar] 4s1 3d5 Cu= [Ar] 4s1 3d10 Ag= [Kr] 5s1 4d10 Au= [Xe] 6s1 5d10 Pd= [Kr] 4d10 |
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| Cation |
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| Element with a positive charge due to losing an electron |
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| Anion |
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| Element with a negative charge due to gaining an electron |
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| Octet |
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| 8 valence electrons |
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| Duet |
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| 2 valence electrons (helium) |
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| What tends to form cations? |
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| Metals |
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| What tends to form anions? |
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| Nonmetals |
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| Group 1A and 2A lose what valence electrons to form cations? |
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| S-orbital |
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| D-block (transition metals) lose what electrons first, and then the next? |
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| S, then D |
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| Paramagnetism |
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| Attracted to magnetic field because of unpaired electrons |
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| Dimagnetism |
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| Repelled by magnetic field due to all paired electrons |
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| Effective nuclear charge |
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| 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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| closer to the nucleus, or less core electrons |
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| the pull on electrons is weaker when |
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| farther from nucleus, or more core electrons |
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| which electrons feel more Zeff? |
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| core |
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| which electrons feel less Zeff? |
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| valence |
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| Shielding/screening |
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| Outer valence e- don't feel the charge of the nucleus due to core e- |
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| Atomic radius |
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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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| Zeff |
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| The atomic radius is smaller when |
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| The Zeff is greater |
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| What causes the atomic radius to be larger or smaller? |
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| The number of electrons inbetween the valence and nucleus |
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| Which ion is smaller and why |
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| Cations- they lose electrons |
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| Which ion is larger and why |
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| Anions- they gain electrons |
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| Which is larger- Br- or Kr? |
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| 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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| Ne |
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| Ionization energy |
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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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| Ionization energy |
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| Why does IE become stronger when Zeff increases? |
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| 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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| In terms of heat, IE is |
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| endothermic |
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| Why is IE endothermic? |
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| IE means it's doing work on the system in order to remove the electron |
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| Electron affinity |
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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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| either exothermic or endothermic |
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| When it comes to electron affinity, what family tends to be exothermic? |
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| noble gases |
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| EA becomes more _____ across a period |
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| negative |
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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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| Periodic trend |
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| Trend occurring from left to right- rows |
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| Periodic trend for atomic radius |
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| As the # of electrons goes up, the radius becomes larger. |
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| Periodic trend for ionization energy |
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| 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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| Why do atoms bond? |
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| Achieve octet |
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| Achieving an octet maximizes ______ and minimizes ______ |
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| Attraction, repulsion |
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| Ionic bond |
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| Bond between a metal and nonmetal where the electron(s) are transferred. |
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| Covalent bond |
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| Bond between two nonmetals- shared. |
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| Metallic bond |
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| Bond among metals, communal sharing |
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| Most molecular bonds are |
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| Polar |
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| Polar bonds are inbetween what? |
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| Covalent and ionic |
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| Important physical property of ionic compounds |
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| Conducive of electricity in aqueous conditions |
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| Covalent bonding is a result of what? |
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| Overlap of atomic orbitals |
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| Physical property of covalent compounds |
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| Poor conductors |
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| Examples of metallic bonders |
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| 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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| Electronegativity |
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| Ability of an atom in a bond to attract electrons to itself |
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| Dipole moment |
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| Separation of charges |
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| When does a dipole occur? |
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| 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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| Period, column |
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| 0-.4 |
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| Nonpolar |
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| .5-1.9 |
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| Polar |
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| > or equal to 2.0 (electronegativity) |
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| ionic |
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| Why do chemical bonds form? |
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| They lower the potential energy between the charged particles. |
