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GEN CHEM
Reviewer for semi-final exam
| Question | Answer |
|---|---|
| Did not explain why metal compounds give off characteristic colors when they are flame tested. | Problem with Rutherford's model |
| Did not explain why metals glow when heated | Problem with Rutherford's model |
| Did not explain the chemical properties of elements | Problem with Rutherford's model |
| Bohr's Theory | Electrons are located at specific energy levels surrounding the nucleus. |
| What is not true on Bohr's theory? | Electrons moved in fixed orbits around the nucleus. |
| A key in understanding the atom | Bohr Model |
| Electrons have a specific amount of energy. The distance between rungs on the ladder were not consistent, they get closer together as you move higher up. | Schrodinger's Theory |
| Amount of energy needed to move from one energy level to another. | Quantum |
| It is also called wave mechanics. It describes the arrangement and space occupied by electrons | Quantum Theory |
| Three dimensional regions in space where there is high probability of finding an electron around an atom. | Orbitals |
| Characteristics of Electron | -Extremely small in mass -Located outside the nucleus -Moving at extremely high speeds in a sphere -Have a specific energy levels |
| What do you call the bright line that appears when atoms are heated? | Line Spectra |
| Electrons in atoms are arranged in? | Discrete levels |
| What happens when electron absorbs energy? | It jumps to a higher energy level |
| What happens when electron emits energy? | It falls to a lower energy level |
| The electrons move in regions of probability around the nucleus called? | Orbitals |
| What do you call the one that defines the energy of electron, the electron's relative distance from nucleus, the size and shape of orbital and the pairing of electrons. | Quantum numbers |
| Defines the energy of electron | Principle Quantum Numbers (n) |
| Four Sublevels | Sphere, Pear, Dumbbell, and Fundamental |
| The value of ____ tells you how many sublevels are present in that energy. | n |
| Size and energy of orbital | Principal quantum number 'n' |
| Shape of atomic orbitals | Angular momentum quantum number ( l ) |
| Orientation of the orbital in space relative to the other orbitals in the atom | Magnetic quantum number (m) |
Created by:
Berlinda
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