Term
| What charge do protons have? |
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Definition
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Term
| What is the single letter abbreviation for atomic number and what does atomic number represent? |
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Definition
| Z and the number of protons |
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Term
| What is the abbreviation for mass number? |
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Definition
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Definition
| atoms that share an atomic number but have different mass numbers |
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Definition
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Definition
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Definition
| hydrogen with one proton; mass of 1 amu |
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Definition
| hydrogen with 1 proton and 1 neutron; mass of 2 amu |
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Definition
| hydrogen with one proton and two neutrons; mass of 3 amu |
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Definition
| 6.02 x 1023; in on mole of an element there are that many atoms of that element |
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Term
| What is the equation to determine the energy of a quantum? |
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Definition
E = hf
E is the energy of a quantum
H is Planck's constant 6.626 x 10-34 J·s
f is the frequency of the radiation |
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Term
| What equation represents the possible values for the angular momentum of an electron orbiting a hydrogen nucleus? |
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Definition
L = nh/2π
L is angular momentum
n is the principal quantum number (any positive integer)
h is Planck's constant
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Term
| What equation describes the energy of a photon? |
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Definition
E = hc/λ
E is the energy
h is Planck's constant 6.626 x 10-34 J·s
c is the speed of light 3.00 x 108 m/s |
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Term
| Heisenberg uncertainty principle |
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Definition
| it is impossible to simultaneously determine, with perfect accuracy, the momentum and the position of an electron; if we want to assess position of an electron is has to stop thus throwing off momentum and vice versa |
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Term
| Pauli exclusion principle |
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Definition
| no two electrons in a given atom can possess the same set of four quantum numbers |
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Definition
| denoted by n; any positive integer; higher n equals higher energy level and radius of electron's shell |
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Term
| What is the maximum number of electrons within a shell? |
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Definition
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Definition
| angular momentum quantum number; denoted by l (lowercase L); describes the shape and number of subshells within a principal energy level (shell); range for l is n-1 |
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Term
| What is spectroscopic notation? |
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Definition
Using a number for the principal quantum number and designated letters for the azimuthal quantum number
- l = 0 is s
- l = 1 is p
- l = 2 is d
- l = 3 is f
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Term
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Definition
| designated by ml; specifies the particular orbital within a subshell where an electron is most likely to be found; possible values are -l to +l |
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Definition
| denoted by ms; describes an elecrons spin orientation within an orbital; two possible values of +1/2 and -1/2 |
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Term
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Definition
| each subshell will fill completely before electrons begin to enter the next one |
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Term
| How to do electron configuration for cations and anions |
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Definition
- cations - remove electrons from the subshells with highest value for n first, the higher l is the tie breaker
- anions - just add according to regular rules
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Term
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Definition
| states that within a given subshell orbitals are filled such that there are a maximum number of half filled orbitals with parallel spins |
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Term
| Half-filled and fully filled orbitals have lower energies (higher stability) than other states. What are the two exceptions to this? |
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Definition
Chromium (and other elements in its group) and Copper (and other elements in its group)
- Chromium should be 4s23d4 but is 4s13d5
- Copper should be 4s23d9 but is 4s13d10
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Term
| Half-filled and fully filled orbitals have lower energies (higher stability) than other states. What are the two exceptions to this? |
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Definition
Chromium (and other elements in its group) and Copper (and other elements in its group)
- Chromium should be 4s23d4 but is 4s13d5
- Copper should be 4s23d9 but is 4s13d10
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Term
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Definition
| materials composed of atoms with unpaired electrons will be slightly attracted to magnetic field |
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Term
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Definition
| materials of only paired electrons will be slightly repelled |
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