Chemistry- 1st semester exam
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71 terms
Terms | Definitions |
|---|---|
 Left | in scientific notation, positive power |
| Right | in scientific notation, negative power |
| Extensive Properties | depends on how much you have, volume and mass |
| Intensive Properties | doesnt depend on how much you have, density, boiling, and melting point |
| Homogenous mixture | becomes 1 |
| Heterogenous mixture | doesnt mix together |
| Physical Change | change without changing identity |
| Chemical Changes | substance transform in differemt substance through chemical bonding |
| Alkali metals | group 1, metal, soft, silvery, highly reactive, missing 1 electron |
| Alkaline Earth Metals | group 2, missing 2 electrons, highly reactive |
| Transitional Metals | center, normal metals, unreactive, conducts electricity, stablE |
| Simi Conductors | conduct electricity in small amounts |
| Gray Area | make up substances of living things |
| Halogens | highly violate, missing 1 proton |
| Metals | group1- Al, Ga, In, Ti, Sn, Pb, Bi, and Po |
| Metalloids | B, Si, Ge, As, Sb, Te |
| Nonmetals | C, N, O, P, Se- Group 6 |
| mass/volume | density equation |
| volumeXDensity | Mass equation |
| mass/density | volume equation |
| Proton charge | positive |
| Electron charge | negative |
| Nucleus | Protons and neutrons are located in the_____ and surrounded by electrons |
| Alpha Particles | subtract 4 from the top and 2 from the bottom |
| Beta Particles | add 1 to the bottom |
| Atomic number | number of protons, determines the position on the periodic table |
| Atomic Mass Number | sum of protons and neutrons in the nucleus |
| Gold foil experiment | designed by ernest rutherford, proed nucleus was at the center of atom, electrons werent evenly distributed |
| Aufbau principle | each electron occupies the lowest energy orbital available |
| Pauli Exclusion Principle | maximum of 2 electrons may occupy single atomic orbital, but of the electrons have opposite spins |
| Hunds Rule | single electrons with the same spin must occupy each equal energy orbitak before additional electrons with opposite spins can occupy the same orbitals |
| Valence Electrons | electrons in the outermost orbitals |
| Valence Configuration | last s and last p |
| Cation | positive |
| Anion | negative |
| 4 oxygens | per+root+ate |
| 3 oxygens | root+ate |
| 2 oxygens | roote+ite |
| 1 oxygen | hypo+root+ite |
| Sigma bonds | longest weakest, single bond |
| Pi bonds | shorter and stronger, double bonds |
| Tripple Bonds | shortest and strongest, 3 bonds |
| hydo+element+ic+acid | Covalently bonded acids |
| Resonance Structure | more that one valid Lewis structure can be written for a molecule or an ion |
| H2, N2, O2, F2, Cl2, Br2, I2 | Diatomical Molecules |
| N2 | bonds 3 times |
| Oxidation state | charge |
| Bonding atoms | the electrons bond |
| Stable atoms | need 8 valence electrons |
| Electron arrangement | delocalized an sea of an electron |
| Oxygen | bent shape |
| Group 1&2 | positive ions, bond with far side of table |
| Transition metals | have 8 valence electrons |
| Sigma bond | the 1st bond in a multiple bond |
| Salt | all ionically formed units |
| Properties of ionic compounds | when put in water or melted, the ionic compound conducts |
| VESPR | valence electron pair repulsion model, takes shape because of opposites attracts |
| Atomic radii | decrease as you move right to left and increase as you go down |
| Isotopes | different number of neutrons |
| Larger pair | the element with the most electrons |
| Wavelength and frequency | C=(funky h)(v) |
| Energy | E=(h)(v) |
| C | 3.0X108 |
| H | 6.626X10-34 |
| Polar molecules | extra electrons left over after the bond, not an even amount of pair |
| Non-polar molecule | no extra electrons, even amount of pairs |
| Binary acids | hydro+element+ic acid |
| Oxyacids | contain hydrogen and an oxyanion |
| EMS | violet, blue, green, yellow, orange, red |
| Qualitative | descriptive |
| Quantitative | numerical |
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