Term
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Definition
| The number of electrons in the atom's highest numbered or outermost shell. |
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Term
| Valences of elements in family: IA |
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Definition
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Term
| Valences of elements in family: IIA |
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Definition
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Term
| Valences of elements in family: IIIA |
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Definition
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Term
| Valences of elements in family: IVA |
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Definition
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Term
| Valences of elements in family: VA |
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Definition
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Term
| Valences of elements in family: VIA |
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Definition
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Term
| Valences of elements in family: VIIA |
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Definition
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Term
| Valences of elements in family: VIIIA |
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Definition
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Definition
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Term
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Definition
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Definition
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Term
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Definition
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Term
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Definition
| The distribution of electrons into shells and sub levels for an atom of an element. Each element has a unique electron configuration. |
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Term
| Write the electron configuration: lithium |
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Definition
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Term
| Write the electron configuration: iron |
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Definition
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Term
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Definition
| Within a sub level, the order of filling orbitals is chosen to maximize half filled orbitals. All single electrons have parallel spins. |
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Term
| Describe the shape of the orbital: s |
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Definition
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Term
| Describe the shape of the orbital: p |
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Definition
| dumbbell shape with 2 lobes (p for parallel axes) |
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Term
| Describe the shape of the orbital: d |
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Definition
| double dumbbell; most have 4 lobes (d for diagonals) |
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Term
| Describe the shape of the orbital: f |
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Definition
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Term
| Pauli Exclusion Principle |
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Definition
| No two electrons in an atom can have an identical set of four quantum numbers |
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Term
| How does the Pauli Exclusion Principle apply to electron spin? |
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Definition
| The two electrons in any orbital must have opposite spins. (+1/2 or -1/2) |
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Term
| What is the order for filling sub levels (Aufbau Process) from lowest to highest energy? |
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Definition
| 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d |
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Term
| Which sublevels are present in energy level: 1 |
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Definition
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Term
| Which sublevels are present in energy level: 2 |
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Definition
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Term
| Which sublevels are present in energy level: 3 |
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Definition
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Term
| Which sublevels are present in energy levels: 4, 5, 6, 7 |
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Definition
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Term
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Definition
| An orbital is contained in a sublevel and holds two electrons. |
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Term
| How many orbitals in sublevel: s |
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Definition
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Term
| How many orbitals in sub level: p |
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Definition
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Term
| How many orbitals in sub level: d |
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Definition
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Term
| How many orbitals in sub level: f |
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Definition
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Term
| List the names of the four sub levels and their electron capacities. |
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Definition
Sublevel s holds two electrons
Sublevel p holds 6 electrons
Sublevel d holds 10 electrons
Sublevel f holds 14 electrons |
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Term
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Definition
| Electron is at its lowest energy level, as close to the nucleus as possible. |
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Term
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Definition
| An electron absorbs energy and moves to a higher energy level above the ground state. |
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Term
| List the three basic postulates of the Bohr Model for the hydrogen atom. |
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Definition
1. e- are present only in specific energy states.
2. A quantum of energy is absorbed or emitted to change energy levels.
3. A quantum is the smallest amount of energy that can be gained or lost. |
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Term
| Lyman, Balmer and Paschen Series |
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Definition
Groups of lines in the emission spectrum of hydrogen. Lyman- ultraviolet, six lines
Balmer- visible, five lines
Paschen- infra-red, four lines |
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Term
| Quantum theory equation relating energy to frequency. |
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Definition
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Term
| Quantum theory equation relating wavelength to frequency |
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Definition
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Term
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Definition
| A bright line spectrum formed when energy absorbed by an element is emitted at specific wavelengths. Each element has a unique spectrum. |
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Term
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Definition
| A dark-line spectrum formed when white light is passed through a vaporized element and a few specific wavelengths are absorbed. |
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Term
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Definition
| h = 6.63 X 10-34 J·sec/particle |
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Term
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Definition
| A packet of energy associated with a specific wavelength of electromagnetic radiation. |
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Term
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Definition
| A number used to describe the energy levels available to an electron. Each electron in an atom has a unique set of four. |
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Term
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Definition
| Consists of the atom's symbol surrounded by the same number of dots as the atom's valence. May be used for elements, compounds, or polyatomic ions. |
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Term
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Definition
| An individual packet or quantum of radiant energy of a specific wavelength. |
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Term
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Definition
| An atom or group of atoms which has magnetic properties due to unpaired electrons in its orbitals. |
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Term
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Definition
| A term indicating a substance which does not contain unpaired electrons and is therefore not attracted to a magnetic field. |
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Term
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Definition
| Instrument which disperses light emitted by energized atoms and allows examination of their spectra. |
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