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| What is the speed of ligth? |
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Definition
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| HOw are frequency and wavelength related? |
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Definition
| they are inversely proportional |
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| The shorter the wavelength, the _____the frequency. |
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| The longer the wavelength, the _____the frequency. |
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Definition
| lower (remember double Ls) |
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| As wavelength inceases, what happens to frequency? |
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| as wavelength decreases, what happens to frequency? |
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Definition
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| HOw are frequency and energy related? |
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Definition
| they are directly proportional. AS frequency increases, so does energy. AS frequency decreases, so does energy. |
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| Black areas on a line spectrum mean _____. Lines on a line spectrum mean _____. |
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| What does it mean if something is quantized? |
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Definition
| used or distributed in discrete amounts; whole numbers no fractions |
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| What is Planck's constant (h)? |
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| What is Planck's equation? |
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| What does the photoelectric effect basically state? |
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Definition
| high frequency, high energy, and a short wavelength means that something will have mass. Low freqency, low energy, and a long wavelength means that something will most likely not have mass. |
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| how would you find the energy of a photon with a wavelength of 415 nm. |
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Definition
| E=hc/wavelength. Plug in the values for each and then multiply by 10^9 nm/m to get rid of nanometers and meters and your answer will come out in Joules |
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| What does the principal quantum number tell? What is the symbol? |
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Definition
| describes the main energy level of the electron; n=1 is the first level away from the nucleus |
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| What does the angular momentum quantum number tell? What is it's symbol? |
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Definition
| descibes the shape or type of orbital; there are 4 types of orbitals: s=0, p=1, d=2, and f=3 (symbol=l) |
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| What does the magnetic quantum number tell? What is its symbol? |
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Definition
| describes the electron's position in the orbital; s has one possible position; p has three possible positions; d has five possible positions; f has seven possible positions |
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| What does the spin quantum number tell? |
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Definition
| describes the electron's spin (m sub s); +1/2 (counter clockwise) and -1/2 for clockwise |
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| the maximum number of electrons in any one energy level can be determined by... |
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Definition
| 2n^2. For n=1, 2(1)^2=2 so maxium of 2 electrons in the n=1 energy level or shell. |
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| The number of sub energy levels in any main energy level is equal to the value of ___. |
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Definition
| n. For n=1, there is only one subshell (s)and l=0. For n=2, there are two subshells, (s and p) so l=0,1 |
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| How many orbitals does the s, p, d, and f subshell have? |
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Definition
| s has 1 oribital, p has 3 orbitals, d has 5 orbitals, f has 7 orbitals (oribitals=positions) |
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| What is the maximum number of electrons that each orbital can hold? |
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Definition
| any orbital/position can only hold 2 electrons. The s subshell has 1 oribtial so it can hold 2 electrons. The p subshell has 3 positions so it can hold 6 electrons. The d subshell has 5 orbitals so it can hold 10 electrons and the f subshell has 7 positions so it can hold 14 electrons. |
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| If n=2, then there are 2 sub shells s and p. interepret this in terms of the periodic table. |
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Definition
| If n=2, then there are two sub shells, s and p. The principle quantum number corresponds to the period. In period 2, there is only a possibility of having an s and p subshell. |
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| What does Hund's rule say? |
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Definition
| one electron must be in each orbital for pairing ( use this when doing orbital notation) |
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| angular quantum number (l) means what? |
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Definition
| the type of orbital: s, p, d, f |
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Term
| When doing electron configurations for transition metals (d subshell and f susbhell) what do you need to remember? |
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Definition
| always subrtract one from the period for the principal quantum number for the d subshell. For the f subshell, always subrtract two. The f subshell will always START with periods 6 and 7. |
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Term
| How do you calculate the number of valence electrons? (mulitiple ways) |
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Definition
| Look at the largest coefficient in the electron configuration and the exponent will be the number of valence electrosn. IF there are two coefficients with the same number, just add these exponents. It doesn't matter if one is s and d and p or whatever...just pay attention to the coefficent. Or the group number corresopnds to the number of valence electrons (except transition metals). |
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| How do you do electron configurations for transition metals? |
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Definition
| normal configurations except for elements in the 4th and 9th group of the transition metals (not the 4th and 9th group of the whole periodic table) |
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| How do you handle electron configurations for the transition metals in the 4th and 9th group (of the transition metals)? |
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Definition
| Do the condensed electron configuration. The electrons that are "left" the valence electrons.... take one from the largest coefficient and add it to the next one (the one that is almost full or half full) |
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| HOw do you do electron configurations for ions? |
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Definition
| if it is a positive ion (cation), remove an electron. If its Na+, remove one. IF its Mg2+, remove 2. If it's a negative ion (anion), add electrons to make it full. If its F-, add 1 one electrons. IF its N3-, add electrons. Add to make it full. |
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| HOw do you do electron configurations for transition metal ions? |
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Definition
| same process for transition metals. All transitions metals are cations so you will always be removing electrons, make sure you know the charge on the transition metals though |
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| Also when doing electron configurations for cations, what shell do you subtract from? |
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Definition
| the shell with the largest coefficient. |
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| What is the periodic trend for electronegativty? |
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Definition
| flourine is the most electronegative; Increases as you go across a period, decreases as you go down a group. |
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| What is the periodic trend for atomic radius? |
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Definition
| helium has the smallest. Atomic radius increases as you move towards group 1, and decreases as you go down groups. |
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| What is the periodic trend for ionization energy? |
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Definition
| Helium has the largest. It takes more energy to remove an electron from the noble gase. This increases as you move towards the noble gases, and up a group |
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| know the periodic trend for electron affinity |
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Definition
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| What are the trends for ion sizes? |
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Definition
| the radius of a cation (positive ion) is always smaller than the radius of its original element....Li+ is smaller than Li. The radius of an anion is always larger than the radius of its original element...F- is larger than F. |
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