CHEM 115
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CHEM 115 - Details
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55 questions
| 🇬🇧 | 🇬🇧 |
| Acetate | C2H3O2 (-) |
| NA | NA |
| Carbonate | CO3 (2-) |
| Nitrate | NO3 (-) |
| Phosphate | PO4 (3-) |
| Sulfate | SO4 (2-) |
| Hydroxide | OH (-) |
| Permanganate | MnO4 (-) |
| Hypochlorite | ClO (-) |
| Chlorite | ClO2 (-) |
| Chlorate | ClO3 (-) |
| Perchlorate | ClO4 (-) |
| Bromate | BrO3 (-) |
| Iodate | IO3 (-) |
| Ammonium | NH4 (+) |
| Acetate | C2H3O2 (-) |
| How were neutrons discovered? | Through understanding radioactive decay |
| Gold Foil Experiment | Discovered the proton and nucleus |
| Cathode Ray Tube Experiment | Discovered the electron |
| Oil Drop Experiment | Discovered the negative charge of the electron |
| When can you use the equation to calculate concentrations/volumes necessary for a dilution? | ONLY when the solute and solvent are the same |
| Define concentration | The amount of solute in a solution |
| What is Molarity? | Moles of solute/Liters of solution (M) |
| In general, metals form ________ | Cations (+ charge) |
| In general, nonmetals form ________ | Anions (- charge) |
| General trend of Groups 1-3 | Metals: +1, +2, +3 |
| General trend of Groups 16-17 | Nonmetals: -2, -1 |
| Major trend of ionic size | Period 1-7 = increases |
| Minor trend of ionic size | Cations = decreases anions = increases |
| Major trend of ionization energy | Period 1-7 = 1st IE decreases |
| Minor trend of ionization energy | Group 1-18 = 1st IE increases |
| What is the exception to the minor trend of ionization energy? | Going group 15-16 |
| 2nd ionization energy is _________, but depends on __________________ | Always greater than the first; whether you're removing valence or core electrons |
| Major trend of atomic size | Period 1-7 = increases |
| Minor trend of atomic size | Group 1-18 = decreases |
| Major trend of effective nuclear charge | Period 1-7 = decreases |
| Minor trend of effective nuclear charge | Group 1-18 increases |
| Major trend of electron affinity | Group 1-17 = decreases |
| Isoelectric | When two atoms/ions have the same number of electrons |
| Coloumb's Law | The attractive force between atoms is proportional to the distance between atoms and the magnitude of charges |
| Binary compounds | Composed of 2 elements/components |
| Formal charge | The hypothetical charge if all bonding e- were shared 100% equally |
| Equation for formal charge | Formal charge = # of VE - # of non-bonding e- - 1/2(# of bonding e-) |
| Formal charge must be calculated... | For each individual atom in the structure |
| Guideline 1 of formal charge and Lewis dot structures | Any structure where 1+ atom has less than a full octet is low quality |
| Guideline 2 of formal charge and Lewis dot structures | Structures with a formal charge of 0 across the board are better |
| Guideline 3 of formal charge and Lewis dot structures | Structures with a formal charge of smaller magnitude are better |
| Guideline 4 for formal charge and Lewis dot structures | More negative formal charge should be on the more electronegative atom |
| Electron Geometry: 2 e- regions | Linear (180º) |
| Electron Geometry: 3 e- regions | Trigonal planar |