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EXAM 2 GEN CHEM
| Term | Definition |
|---|---|
| Electromagnetic Spectrum | the entire spectrum of sunlight including, gamma rays, x-rays, UV, visible, infrared (IR), microwave, and radio |
| Gamma Rays | highest energy, highest frequency, shorter wavelength |
| Visible Rays | violet, indigo, blue, green, yellow, orange, red. 400-700nm |
| Radio | lowest energy, lowest frequency, longest wavelength |
| With the smallest first, what is the order of increasing wavelength? | X-Ray < Ultraviolet < Visible < IR |
| IR | infrared, warms earth and oceans |
| With the smallest first, what is the order of increasing energy? | IR < Visible <Ultraviolet < X-Ray |
| One Wavelength | distance between any point on wave to the exact same point on the next wave. Curvy thing |
| Frequency | represented by a V, measure of how many waves pass by in one second |
| s(-1), 1/s, Hz (Hertz) | measurements of frequency |
| Lewis Dot Symbol | consists of the element symbol surrounded by dots each dot represents a valence electron |
| Speed | wavelength x frequency |
| Speed of light is constant | 3x10^8(m/s) or 3x10^17(nm/s) |
| Photoelectric Effect | particle nature of light. |
| E = h x v | Energy (J) = Plancks Constant x frequency (1/s, s^-1, Hz) |
| c = | speed of light |
| Photons | a stream of particles of light |
| v = | frequency |
| E = | energy |
| squiggle | wavelength |
| outermost electrons | valence electrons |
| # of valence electrons = | the elements group # |
| Octet Rule | main group elements tend to form 8 valence electrons to be stable, forms a covalent bond |
| Covalent Bond | pair of shared valence electrons |
| The Lewis Structure explain why | each atom is structured the way it is. For example CH4 is not CH3 or CH5. |
| A hydrogen element needs to have ... | 1 covalent bond |
| Carbon is in group __, and needs ___. | Group 4A and needs 4 covalent bonds |
| Nitrogen is in group __, and needs ___. | Group 5A and needs 3 covalent bonds |
| Oxygen and Sulfur are in group __, and needs ___. | Group 6A and needs 2 covalent bonds |
| F, Cl, Br, and I are in group ___, and needs ___. | Group 7A and needs 1 covalent bond |
| Lewis Structure represents | covalent bonding |
| Lone Pair | Valence electrons not bonded, represented by dots |
| Double Bond | forms when 2 pairs of electrons (4 in total) are shared (CO2) |
| Triple Bond | forms when 3 pairs of electrons (6 in total) are shared (N2) |
| 1st Step of Drawing Lewis Structure | determine total # of valence electrons (cations and anions) |
| 2nd Step of Drawing Lewis Structure | draw skeletal structure of molecule, central atom is written first and least electronegative. H can only be a terminal. |
| 3rd Step of Drawing Lewis Structure | Distribute electrons as ion pair on terminal atoms, completing octet rule |
| 4th Step of Drawing Lewis Structure | If any electrons remain place them as lone pairs on central atom |
| 5th Step of Drawing Lewis Structure | If the central atom has less than 8 electrons move 1+ lone pairs from the terminal atom to form multiple bonds between the central atom and terminal atom |
| cation | ions with a positive charge, subtract one electron for each positive charge |
| anion | ions with a negative charge, add one electron for each negative charge |
| Resonance Structure | one of two or more equally valid Lewis Structures. Differ only in position of electrons, not in the position of the atoms. |
| Free Radicals | odd number of electrons. They are very reactive and will try to get 1 from another. Very strong tendency to react. |
| UVA | lowest energy, longest wavelength |
| UVB | medium energy, medium wavelength, breaks single bond |
| UVC | highest energy, shortest wavelength, breaks double bond |
| shorter wavelength = | high frequency = high energy |
| UV | in this region photons have enough energy to remove electrons from neutral molecules, breaking chemical bonds. In living things this is birth defects and cancers. |
| Ozone Layer | blocks out UV radiation, has a smell |
| Ozone (O3)= | Energy +3 O2, produced through welding and lightening |
| Ozone is more reactive than | oxygen |
| 90% of ozone is in stratosphere, but when it is in the troposphere it is | considered a pollutant |
| Chlorofluorocarbons (CFC's) | compounds composed of chlorine, fluorine, and carbon. Includes trichloromethane, dichloromethane |
| Chlorine containing molecules | are bad and deplete ozone by producing a radical |
| Ozone and Chlorine | inverse relationship as one increases the other decreases |
| Montreal Protocol | regulate CFC's to restore ozone by replacing chlorine hydrocarbons with fluorine |
| fluorine is | friendlier to ozone |
| VSEPR (Valence Shell Electron-Pair Repulsion ) | opposite charges (+,-) attract and same charges (-,-) and (+,+) repel. All electrons are negative so they maximize distance between each other |
| Electron Grouping/Regions of Electron Densities | only looking at the central atom. Single bond, double bond, triple bond, and lone pair, are all each their own individual one group |
| Electron Group of 2 | linear, with an 180 degree bond angle |
| Electron Group of 3 | trigonal planar with 120 degree bond angle |
| Electron Group of 4 | tetrahedral with 109.5 degree bond angle |
| # of lone pairs 0 | tetrahedral |
| # of lone pairs 1 | trigonal planar |
| # of lone pairs 2 | bent |
| Isotopes | atoms of the same atomic # but different mass # due to different # of neutrons. Most elements have them, similar chemical qualities. |
| what's on the periodic table | is the weighted average mass |
| abundance % will always = | one |
| Mole | the amount of a substance containing the same # of discrete entities (such as atoms, molecules, and ions) as the # of C |
| NA Avogadro's: | 6.02214179x 10^23 |
| # of atoms or molecules/ NA # | # of moles |
| mass in g/ molar mass = | # of moles |
| Greenhouse Effect | natural process by which atmospheric gases absorb and re-radiate a major portion (about 80%) of IR radiation radiated by the earth |
| Greenhouse Gases | capable of absorbing and emitting IR radiation, thus warming the atmosphere |
| Greenhouse gases include | CO2, H2O, NO2, CH4 |
| Electronegativity | measure of ability of an atom to attract bonded electrons |
| Cations | metals that lose electrons and become + charged |
| Anions | nonmetals that gain electrons and become - charged |
| Ionic Bond | chemical bond formed when oppositely charged ions attract in the solid state |
| Losing electrons | means a more positive charge |
| Gaining electrons | means a more negative charge |
| Monoatomic Ions | ions formed from only one atom |
| Transition metals | exhibit variable changes, charge is shown by roman numerals |
| Polyatomic ions | 2 or more ions covalently bonded together with a positive or negative charge. Includes NH4 +, OH -, CO3 2-, NO3 -, PO4 3-, SO4 2- |
| Ammonium | NH4 + |
| Hydroxide | OH - |
| Carbonate | CO3 2- |
| Nitrate | NO3 - |
| Phosphate | PO4 3- |
| Sulfate | SO4 2- |
| Formula of ionic compounds | write metal (cation) first then the nonmetal (anion) the charges must be equal to zero. NaCl, Na2O, AlCl3 |
| Naming Monoatomic Ions: main group metals | the name is the same |
| Naming Monoatomic Ions: transition metals | same name, indicate charge with roman numeral |
| Naming Monoatomic Ions: anions | name ends in -ide |
| Naming Ionic Compounds | metal (cation) is named first, then nonmetal |
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