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Chem Ch 2
| Question | Answer |
|---|---|
| Electromagnetic radiation | The way energy is transferred through space. Travels as both waves and particles. |
| Wavelength | The distance between corresponding points on adjacent waves. |
| Amplitude | The height of the crest. |
| Wavelength can affect both ___ and ___ "color" | Visible and non-visible. |
| Amplitude can affect ___ | Brightness. |
| Frequency | The number of waves passing a given point per unit of time. |
| Speed of light | 3.00 x 10^8 m/s |
| Interference | Waves are isolated but interact with each other. |
| Constructive interference | The alignment of waves in phase, thus increasing amplitude. |
| Destructive interference | The alignment of waves out of phase, thus canceling the waves. |
| Diffraction | When a wave encounters an obstacle that is comparable in size, it bends around it. |
| Energy comes in packets called _____ | Quanta |
| Energy is proportional to ____ | Frequency |
| Energy of a photon equation | E=hv |
| Bohr model included | Explained the spectra of hydrogen, quantum numbers, and energy transitions. |
| Bohr model limitations | Why doesn't an electron fall into the nucleus? Doesn't fully explain other atomic spectra. Doesn't explain wavelike properties. |
| The relationship between mass and wavelength | wavelength = h/mv |
| X-ray diffraction | X-rays passed through a crystal produced an interference pattern. |
| The more precisely the momentum of a particle is known... | The less precisely its position is known. |
| Quantum mechanics | A mathematical method into which both the wave and particle nature of matter could be incorporated. |
| Orbital | Describes a spatial distribution of electron density. Described by a set of 3 quantum numbers. |
| Principle quantum number | n: describes the energy level on which the orbital resides. The values are integers greater than or equal to 1. |
| Angular momentum | l: defines the shape of the orbital. The values are integers ranging from 0 to n-1 |
| L=0 | s |
| L=1 | p |
| L=2 | d |
| L=3 | f |
| Magnetic quantum number | ml: describes the 3-dimensional orientation of the orbital. Allowed values are integers ranging from -L to L |
| Spin quantum number | ms: describes its magnetic field, which affects its energy. Only has 2 allowed values: +1/2 and -1/2 |
| The lowest energy level an electron can attain is n=_ or the __ orbital | 1, 1s |
| Shape of s orbital | Spherical |
| Each principle level with n=2 or greater contains __ __ orbitals | 3 p, (ml=-1, 0, 1) |
| The p orbital should consist of __ ___ on either side of the nucleus. What is the shape? | 2 lobes. Dumbbell |
| Each principle level with n=3 or greater contains __ __ orbitals | 5 d, (ml=-2, -1, 0, 1, 2) |
| Based on the quantum numbers, four of the five d orbitals have __ lobes; the other resembles a __ orbital with a donut around the center. | 4, p |
| Each principle level with n=4 or greater contains __ __ orbitals | 7 f, (ml=-3, -2, -1, 0, 1, 2, 3) |
| F orbitals are much more complex, and have more __ and __ than d orbitals | Lobes, nodes |
| Why do we depict atoms as spherical if there are so many different shapes to the electron orbitals? | Most atoms have so many electrons occupying different orbitals that superimposing them leads to a mostly spherical shape. |
| Shape of d orbital | 4-leaf clover |
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