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Chemisty
| Question | Answer |
|---|---|
| Electron | The negative subatomic particle in the electron cloud of an atom |
| Electromagnetic radiation | A form of energy that exhibits wavelike behavior as it travels through space |
| Wavelength | - A unit of distance for measuring waves |
| Frequency | The number of waves that pass a given point in a certain time |
| Emission spectrum | The spectrum of light released from excited atoms of an element |
| Heisenberg uncertainty principle | It is impossible to determine the position and velocity of an electron or other particle simultaneously |
| •Valence electrons | Electrons in the outermost energy level of the electron cloud |
| •Octet rule | The tendency of atoms to prefer to have 8 valence electrons |
| •Ions | Atoms or molecules that have a charge due to having lost or gained electrons |
| •Lewis structures | A convenient and simple way to represent an element and its valence electrons |
| •Quantum theory | A mathematical description for the wave properties of electrons and other tiny particles |
| •Orbital | - A 3D region around the nucleus that shows were an electron probably is |
| •Electron configuration | The most stable arrangement of electrons in an atom’s electron cloud |
| Periodic trends | Specific patterns in the periodic table that make it possible to make predictions about an element’s properties |
| Coulomb’s law | As the atomic number increases, the nuclear attraction for electrons increases, thus pulling the electrons in more tightly to the nucleus |
| Atomic radius | One-half the distance between the nuclei of two identical atoms bonded together |
| Reactivity | A measure of how readily an atom will react |
| Shielding effect | When electrons in the inner energy levels block the attraction of the nucleus to the valence electrons |
| •Electronegativity | A measure of the ability of an atom in a bond to attract electrons |
| •Ionization energy | The energy required to remove one electron from a neutral atom of an element |
| •Oxidation numbers | The charge of an ion |
| •Ionic radius | The radius of a monoatomic ion in an ionic compound |
| Explain both the wave and particle natures of electrons. | Electrons are the negative subatomic particles in the atom but they behave more like waves • They can have different amounts of energy and thus different frequencies. |
| Explain the relationship between electrons, energy, and electromagnetic radiation. | Electrons can absorb and release energy in the form of electromagnetic radiation. |
| mathematical relationship between the speed, wavelength and frequency of electromagnetic radiation. | Speed of light is constant • Wavelength and frequency have an inverse relationship |
| Cations: | atoms that lose e- in order to become stable − Results in a positive charge − Usually metals |
| Anions: | atoms that gain e- in order to become stable − Results in a negative charge − Usually nonmetals |
| Differentiate between Bohr’s model of the atom and the quantum model of the atom. | While Bohr’s model does show the arrangement of protons, neutrons, and electrons in the atom, it does not show the 3D nature of the electron cloud, or accurately depict the nature of electrons being in constant motion. |
| Aufbau principle: | electrons fill the lowest energy orbital first |
| Hund’s rule: | orbitals of equal energy each get 1 e- before any orbital gets a second pair |
| Pauli exclusion principle: | no two e- in the same atom can have the same set of quantum numbers |
| how the shielding effect works. | This occurs when electrons in the inner energy levels block the attraction of the nucleus to the valence e- and thus they become more loosely held. • It increases as you go down a group as the atomic size is increasing. |
Created by:
Levygobrrr