Term
| What scientist develeloped atomic theory in the early 1800s? |
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Definition
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| How does the energy of an electron change when it moves closer to the nucleus? |
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| The pricipal quantum number indicated what property of an electron? |
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| How many energy sublevels are in the second principal energy level? |
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Definition
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| What is the max number of electrons in the second principal energy level? |
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Definition
| 8. (4 orbitals*2 energy sublevels=8) |
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Term
| In Rutherford's model of an atom, where are the electrons and protons located? |
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Definition
| Moving throughout the atom. |
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Term
| In the Bohr model of the atom, an electron in orbit has a fixed _____ ? |
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Definition
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Term
| What did Rutherford's experiment demonstrate? |
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Definition
| That most of an atom's mass in concentrated in a relatively small portion of the atom's entire volume. |
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Term
| What is the probability of finding an electron within the region indicated by the drawn electron cloud? |
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Term
| The SHAPE of an electron cloud is determined by the electron's ____? |
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Definition
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Term
| Formula 2n squared represents ____? |
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Definition
| The max number of electrons that can be in an energy level. |
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Term
| The letter P in 4p cubed indicates _________? |
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Definition
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Term
| If 2 electrons occupy 2 p orbitals, what is the directions of the spins of these 2 electrons? |
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Definition
| Both clockwise or both counterclockwise. |
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Term
| Unpaired electrons in Sulfur? |
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Definition
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Term
| What orbital is filled when iodine gas gains an electron to become a negative ion? |
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Definition
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Term
| What is true about the electron configurations of the noble gases? |
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Definition
| The outermost s and p sublevels are partially filled. |
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Term
| Representative elements are in what group? |
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Definition
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Term
| Each period number in the periodic table corresponds to ______? |
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Definition
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Term
| The category of elements that is characterized by the filling of the f orbitals is the _____? |
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Term
| Ni, Fe and Zn all belong to what group of elements? |
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Definition
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Term
| How does atomic radius change down a group in the periodic table? |
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Definition
| First increases, then decreases. |
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Term
| Why is the radius of a negative ion always greater than the radius of it's neutral atom? |
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Definition
| Because the number of principal energy levels is always reduced. |
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Term
| What contributes to the relatively greater atomic size of the higher-atomic-number elements within a particular family of the periodic table? |
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Definition
| more shielding of the outer electrons by the inner electrons |
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Term
| How to calculate which element has the least atomic radius? |
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Definition
| Atomic radius- the lower the period, the greater the atomic radius. (the higher period has the least atomic radius) |
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Term
| What electron configurations are particularly stable? |
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Definition
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Term
| What factor contributes to lower ionization energy of the higher-atomic-number elements in a family in the periodic table? |
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Definition
| Greater distance from the nucleus. |
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