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Chemistry
| Question | Answer |
|---|---|
| The relative overall energy of each orbital is referred to as what number? | Principal quantum number(n) |
| This quantum number distinguishes the orbitals available within a subshell ie s, p, d and f | Magnetic quantum number(m) |
| This quantum number describes the angular momentum of an electron. It has both a magnitude of 1/2 and direction(+ or-) | Spin quantum number(s) |
| It is the secondary or azimuthal quantum number(l). It describes the shape of the orbital an electron occupies | Angular momentum quantum number |
| It states that every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin | Hund's rule |
| It states that in the ground state of an atom or ion, electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels | Aufbau principle |
| nounCHEMISTRY a law stating that the elements, when listed in order of their atomic numbers, fall into recurring groups, so that elements with similar properties occur at regular intervals. | Periodic law |
| How many elctrons can the s, p, d and f subshells contain....respectively | s- 2 p-6 d- 10 f- 14 |
| What are the angular momentum quantum numbers(l) for the s, p, d and subshells? | l=0 s subshell l=1 p subshell l=2 d subshell l=3 f subshell |
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Tunrayo