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32 Cards in this Set
- Front
- Back
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What is the Rydberg equation for the spectral lines of hydrogen? |
1/y = 𝑅∞ (1 /𝑛^ 2 −1/𝑚^2) |
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What is the equation to be able to calculate the energy of a single photon? |
𝐸 = ℎv Einstein’s equation |
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How do you calculate the energy of a mole of photons? Why is this needed? |
By using Avogadro’s constant. (6.022 x 10^23) This is needed because chemists most often report energies in kJ/mol. |
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What is Schrodinger waveequation? |
It is an equation for the orbits of the electrons. There are four quantum numbers that obey specific rules. |
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What is the Principal quantum number, its value, and meaning? |
Principal quantum number = n Value = Any positive integer Meaning = Energy level in Hydrogen atom |
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What is the Angular momentumquantum number, its value, and meaning? |
Angular momentumquantum number = l Value = l = 0 … N-1 in steps of 1 Meaning = Roughly determines number of lobes(actually nodes) in an orbital. 0 = S1 = P2 = D3= F4 = G5 = H… and so on |
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Give the number of lobes/nodes in an orbital. |
0 = S 1 = P 2 = D 3= F 4 = G 5 = H … and so on |
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What is the Azimuthal quantum number, its value, and meaning? |
Azimuthal quantum number = ml Value = ml =-l … l in steps of 1 Meaning = Determines the orientation of theorbitals in space such as Px, Py and Pzfor L=1 |
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What is the Spin quantum number, its value, and meaning? |
Spin quantum number = ms Value = +½ or -½ Meaning = Spin on the electron |
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What is the Pauli-Exclusion principle? |
It states that no two electrons may have the same set of quantum numbers. This basically limits each orbital to holding just two electrons. |
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What is Hund’s rule? |
It states that if several orbitals are degenerate (have the same energy) then nature will first put one electron in each orbital before it total fills any one of them. |
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How many different types of bonds are there? Name them. |
1. Ionic 2. Covalent 3. Polar Covalent |
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Define ionic bonds. |
the electronegativity difference is so great that one atom rips the electron off theother to form ions. These ions are then held together in a crystal lattice by electrostaticforces |
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Define covalent bonds. |
the electronegativity difference is slight and the atoms share the electrons |
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Define polar covalent bonds. |
the electronegativity difference is enough that the electrons are not shared equally and they tend to spend more time near the more electronegative atom |
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Ammonium |
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Acetate |
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Cyanide |
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Phosphite |
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Phosphate |
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Hydrogen Phosphate |
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Dihydrogen Phosphate |
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Sulfite |
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Sulfate |
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Thiosulfate |
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Peroxide |
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Hydroxide |
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Permanganate |
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Carbonate |
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Hydrogen Carbonate |
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Nitrite |
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Nitrate |
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