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Chemistry Exam 2
Exam 2
| Question | Answer |
|---|---|
| How many Oxygens does "ide" have... | Negative 3 - Oxygens (from ate) |
| How many Oxygens does "hypo ______ ite" have... | Negative 2 - Oxygens (from ate) |
| How many Oxygens does "ite" have... | Negative 1 - Oxygens (from ate) |
| How many Oxygens does "ate" have... | No added or subtracted Oxygens (from ate) |
| How many Oxygens does "per _____ ate" have... | Positive 1 - Oxygens (from ate) |
| flour- | F^- |
| chlor- | CIO3^- |
| brom- | Br03^- |
| iod | IO3^- |
| sulf(ur)- | SO4^-2 |
| selen- | SeO4^-2 |
| nitr- | NO3^- |
| phosoh(or)- | PO4^-3 |
| arsen- | AsO4^-3 |
| carb(on)- | CO3^-2 |
| silic- | SiO4^-4 |
| bor- | BO3^-3 |
| acet- | CH3COO^- |
| chrom- | CrO4^-2 |
| dichrom- | Cr2O7^-2 |
| mangan- | MnO4^- |
| Cations: Ammonium | NH4^+ |
| Anions: Hydroxide | OH^- |
| Anions: Cyanide | CN^- |
| Anions: Peroxide | O2^-2 |
| Where is the S-block | Left 2 columns of the periodic table |
| Where is the P-Block | Right 6 columns of the periodic table |
| Where is the F-Block | Bottom two rows of the periodic table |
| Where is the D-Block (transition metals) | Middle portion of the periodic table |
| S-Block | Lambda = 0 |
| P-Block | Lambda = 1 |
| F-Block | Lambda = 3 |
| D-Block | Lambda = 2 |
| What subshell do transition metals start at | 3d subshell |
| How many electrons can the S-Orbital Hold? | 2 Electrons |
| How many electrons can the P-Orbital Hold? | 6 Electrons |
| How many electrons can the D-Orbital Hold? | 10 Electrons |
| How many electrons can the F-Orbital Hold? | 14 Electrons |
| List the EM Spectrum in order... | Gamma -> X-Ray -> Ultraviolet -> Visible spectrum -> infrared -> Microwave -> Radio |
| Visible spectrum (Strongest to Weakest) | VIBGYOR - (ROYGBIV Backwards) |
| What does n mean in the electron configuration? | Row |
| What does s mean in the electron configuration? | Block |
| What does m1 or (L) mean in the electron configuration? | Magnetic Quantum number -1 -> 0 -> 1 |
| What does ms mean in the electron configuration? | Spin -1/2 or +1/2 (This can be determined if there is a down arrow) |
| What happens if there is a small frequency | There is less power |
| For an electron in the 4d orbital identify its shell and subshell | Shell = 4 Subshell = 2 (d=2) |
| How to calculate MAX electrons | 2n^2 |
| How is L situated? | 0, 1, 2, 3, 4 |
| Why can these sets of numbers not exist? n=3 l=2 m1=0 ms=1 | ms can only be -1/2 or +1/2 |
| Why can these sets of numbers not exist? n=2 l=2 m1=-1 ms=-1/2 | 2d does not exist (transition metals (d) starts at the 3rd level) |
| Why can these sets of numbers not exist? n=4 l=1 m1=-2 ms=+1/2 | m1 can only exist from -1 < 0 < 1 |
| Molecular Compounds | Does not contain metals |
| Ionic Compounds | Contains metals |
| How to calculate moL | Mass / Molar Mass |
| Empirical Formula | Mass / Molar Mass (of all elements) then divide moL by the smallest MoL to get the ratio - Use the ratio to get number of elements |
| Ionization energy | The ability to lose an electron from an atom - si is more stable |
| Effective nuclear charge | The net positive nuclear charge on an electron - Chlorine has more protons which allow for a higher charge |
| MoL x Molar mass = | Mass |
| Avogadro's number | 6.022 x 10^23 |
| Mol x Avag # = | number of atoms |
| Percent composition | Add all the elements, / by the molar mass, calc total molar mass, divide element by total = % |
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