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Chemistry
1st Semester
| Term | Definition |
|---|---|
| Atomic number | the total number of protons in the nucleus of an atom; determines the identity of an atom |
| Atomic radius | the distance from the nucleus to the valence electrons |
| Average atomic mass | the weighted average mass of all isotopes of an element |
| Chemical property | a characteristic of an element that can be observed during or after a chemical reaction |
| Electron configuration | a model that describes the distribution and pattern of electrons in an atom |
| Electronegativity | the ability or tendency of an atom or ion to attract a shared electron in a bond |
| Ionization energy | the energy required to remove an electron from an atom or ion |
| Lewis Dot Structure | a model that utilizes the octet rule to show the placement of bonds and lone pairs of electrons between atoms in a molecule |
| Physical property | characteristics of an element; can be observed or measured without changing its chemical composition |
| Representative elements | elements located in families 1, 2, 13 – 18; have very predictable patterns of valence electron behavior compared to the transition metals |
| Valence electrons | electrons in the outermost energy level of an atom |
| atom | the smallest unit of matter that retains the chemical identity of the element |
| Electromagnetic spectrum | the range of all types of electromagnetic radiation, including the wavelengths or frequencies of visible and invisible forms of energy, including radio, microwaves, infrared, visible, ultraviolet, X-rays, and gamma |
| Electron | a negatively charged subatomic particle that is responsible for an atom’s reactivity |
| Electron cloud | the region of space outside the nucleus of an atom where electrons are located; contains the vast majority of an atom’s volume |
| Emission spectrum | the discrete energies of light, or quantized frequencies, that an atom emits as an electron transitions from a higher energy state to a lower energy state |
| Heisenberg's Uncertainty Principle | showed mathematical evidence that we cannot simultaneously know both the position and speed of a particle (e.g., electron and photon) with accuracy |
| Ion | an atom that has a charge due to the gain or loss of electrons |
| Proton | a positively charged subatomic particle in the nucleus that gives an atom its identity |
| Quantization of Energy | the concept that energy can only exist in specific, discrete amounts, rather than being continuous |
| 0th (Zeroth) Law of Thermodynamics | If both systems A and B are in thermodynamic equilibrium with system C, systems A and B must be in thermodynamic equilibrium with each other. |
| 1st Law of Thermodynamics | Energy can transform from one form into another, but cannot be created nor destroyed in an isolated system. The total energy of a system and its surroundings always remains the same. |
| 2nd Law of Thermodynamics | the combined entropy of the system and its environment will always increase |
| 3rd Law of Thermodynamics | As temperature approaches absolute zero, the entropy of a system approaches a constant value. |
| Dalton’s law of partial pressure | In a mixture of gases, the pressures of each component gas, called partial pressures, add up to give the total pressure of the entire gas mixture. |
| Entropy | a measure of the disorder or randomness of particles in a system |
| Heat | the transfer of thermal energy |
| Ideal gas | a hypothetical gas that perfectly follows the postulates of kinetic molecular theory |
| Kinetic molecular theory | a model that describes the movement and interactions of particles in an ideal gas; serves as a simplified approximation of real gas behavior |
| Mole | a scientific unit of measurement used to count large amounts of extremely small particles, such as atoms, molecules, or compounds |
| Temperature | a measurement of the average amount of energy or speed of particles in a system |
| Charles' Law | states that the volume of a given mass of gas varies directly with the absolute temperature of the gas when pressure is kept constant. |
| Boyle's Law | states that the volume of a given mass of gas varies inversely with the pressure when the temperature is kept constant |
| STP | Standard Temperature and Pressure in Chemistry, It is the temperature at which the pressure of a gas is equal to 1 atmosphere and the temperature is equal to 273.15 K |
| Alpha decay | the emission of a helium nucleus (2 protons and 2 neutrons, called an alpha particle) from an unstable nucleus of a radioactive isotope |
| Beta decay | the emission of an electron or positron (called a beta particle, beta minus or beta plus) from an unstable nucleus of a radioactive isotope |
| Fission | the splitting of a radioactive (unstable) nucleus into smaller, more stable atoms, which results in a large release of energy |
| Fusion | the combining of two less stable (radioactive) nuclei of atoms into one more stable atom, which results in a tremendous release of energy |
| Gamma decay | the emission of super high-energy photon (packets of electromagnetic radiation, called a gamma ray / photon) from an unstable nucleus of a radioactive isotope |
| Radioactive | a sample of something that contains an isotope; unstable; emits at least one type of radiation as it decays into a more stable isotope |
| Chemical bonding | a relatively strong attraction between atoms or ions resulting from shared or transferred valence electrons |
| Covalent bond | a chemical bond between two atoms sharing electrons |
| Electron dot structure (Lewis dot structure) | a model that utilizes the octet rule to show the placement of bonds and lone pairs of electrons between atoms in a molecule |
| Ionic bond | a chemical bond between two atoms when one or more electrons are transferred from one atom to the other |
| Metallic bond | a bond where delocalized electrons are shared among positively charged metal ions, holding the metal atoms together |
| Valence Shell Electron Pair Repulsion (VSEPR) theory | a model used to describe the shape of molecules; based on the idea that electrons in bonds and lone pairs form a shape that allows them to stay as far away from each other as possible (repulsion between electrons) |
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