CHEMISTRY REGENTS OVERVIEW – Flashcards
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| PROTONS |
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| POSITIVELY CHARGED (+) |
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| NEUTRONS |
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| NO CHARGE |
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| ELECTRONS |
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| - ARE SMALL AND ARE NEGATIVELY CHARGED(-) - FOUND IN "CLOUDS" ORBITALS AROUND AN ATOM'S NUCLEUS |
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| NUCLEONS |
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| PROTONS AND NEUTRONS THAT ARE IN AN ATOM'S NUCLEUS |
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| MASS NUMBER |
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| - IS EQUAL TO AN ATOM'S NUMBER OF PROTONS AND NEUTRONS ADDED TOGETHER |
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| ATOMIC NUMBER |
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| - equal to the # of protons in the nucleus of an atom |
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| NUMBER OF NEUTRONS |
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| - equal to mass number - atomic number |
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| ISOTOPES |
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| - atoms with equal number of protns, but diifer in neutron number |
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| CATIONS |
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| - positively charged ions (+) - forms when a neutral atom loses electrons - smaller than their parent atom (anion) |
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| ANIONS |
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| - negatively charged ions (-) - forms when a neutral atom gains electrons - larger than their parent atom (cations) |
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| ERNEST RUTHERFORD - GOLD-FOIL EXPERIMENT |
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| - showed that an atom is consisted of empty space with a small, dense, positively charged nucleus |
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| DALTON'S MODEL OF ATOM |
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| - showed solid sphere of matter that was uniform throughout |
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| BOHR MODEL OF ATOM |
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| - in model of atom, placed electrons orbiting around the nucleus |
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| CURRENT WAVE - MECHANICAL MODEL |
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| - shows atoms with electrons in clouds around the atom's nucleus |
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| STP |
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| - standard temperature & pressure (273 kelvin and 1 atm) |
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| BRIGHT LINE SPECTRA |
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| - electrons emit energy as light when they jump from the higher energy levels back to the ground state. |
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| ELEMENTS |
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| - pure substances composed of only one kind of atom |
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| BINARY COMPOUNDS |
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| - substances made up of two kinds of atoms (ex: H20, NH3, CO2) |
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| DIATOMIC COMPOUNDS |
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| - elements that form two atom molecules in their natural form at STP * REMEMBER THE PHRASE - " BrINCIHOF" (BR2, I2, N2, CL2, H2, O2, F2) |
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| SOLUTIONS |
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| homogenous mixtures (air, salt water, etc.) |
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| HOMOGENOUS |
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| - A class of matter with definite properties whose members are composed of two or more substances, each retaining its own identifying properties (e.g., mixed vegetables). |
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| HETEROGENEOUS |
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| A heterogeneous compound, mixture, reaction or other such object is one that consists of many different items, which are often not easily sorted or separated, though they are clearly distinct. |
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| SOLUTE |
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| - substance being dissolved |
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| SOLVENT |
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| - substances that dissolves the solute |
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| PHYSICAL CHANGES |
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| - do not from new substances - merely change the appearance of the original substance (melting of ice) |
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| CHEMICAL CHANGES |
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| - results in the formation of new substances (ex: the burning of hydrogen gas to produce water vapor) |
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| REACTANTS AND PRODUCTS |
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| - REACTANTS = left side of the reaction arrow - PRODUCTS = right side of the reaction arrow |
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| ENDOTHERMIC REACTIONS |
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| - absorb heat - the energy value is on the left side of the reaction arrow in a forward reaction |
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| EXOTHERMIC REACTIONS |
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| - releases energy - energy is the product in the reaction |
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| SYNTHESIS REACTIONS |
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| - when two or more reactants combine to become one |
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| DECOMPOSITION REACTIONS |
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| - occurs when a single reactant forms two or more products |
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| SINGLE REPLACEMET REACTIONS |
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| - when one element replaces another element in a compound |
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| DOUBLE REPLACEMENT REACTIONS |
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| - occurs when two compounds react to form to new compounds |
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| LAW OF CONSERVATION OF MASS |
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| - masses of reactants = masses of products |
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| GRAM FORMULA MASS |
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| - sum of the atomic masses of all the atoms in a substance |
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| Use this diagram to help determine the number of significant figures in a measured value… |
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| Pacific Atlantic If the decimal point is present, start counting digits from the Pacific (left) side, starting with the first non-zero digit. 1 2 3 0.00310 (3 sig. figs.) If the decimal point is absent, start counting digits from the Atlantic (right) side, starting with the first non-zero digit. 3 2 1 31,400 (3 sig. figs.) |
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| ELECTRON CONFIGURATION |
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| Electron configurations are written in the bottom center of an element’s box on the periodic table in your reference tables. # of electrons in 3rd principal energy level # of electrons in 2nd principal energy level # of electrons in 1st principal energy level |
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| ISOTOPES |
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| Isotopes are written in a number of ways: C-14 is also Carbon-14, and is also mass number 14C atomic number 6 |
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| SOLIDS |
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| - definite shape and volume |
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| LIQUIDS |
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| - no definite shape, but definite shape |
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| GASES |
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| - no definite shape or volume - random particle motion |
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| SUBLIMATION |
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| - substances that turn from a solid directly to a gas (CO2, I2) |
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| SUBLIMATION |
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| - substances that turn from a solid directly to a gas (CO2, I2) |
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| DEGREES KELVIN |
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| - C + 273 |
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| HEAT OF FUSION |
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| - the heat absorbed or released when 1 gram of substances changes from a solid to liquid phase |
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| HEAT OF VAPORIZATION |
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| - heat absorbed or releases when 1 gram of substance moves from liquid phase to gas phase |
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| PRESSURE/VOLUME |
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| - pressure of gas increases, volume decreases - pressure of gas decreases, volume increases |
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| REAL GASES |
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| - real gas particles have volume - attracted to one another - not behave like ideal gases - will behave like ideal gases under low pressure and high temp. |
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| DISTILLATION |
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| - SEPARATING MIXTURES WITH DIFFERENT BOILING POINTS |
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| FILTRATION |
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| - separating mixtures of solids and liquids -chromotography can also be used |
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| NOBLE GASES (GROUP 18) |
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| - (GROUP 18) - inert and stable |
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| IONIZATION |
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| - increases as you GO UP AND TO THE RIGHT OF TABLE |
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| ATOMIC RADII |
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| - decreases left to right - due to increasing nuclear charge - increases as you go downa group |
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| ELECTRONEGATIVITY |
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| - measure of an element's attractions to electrons |
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| ALKALI METALS |
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| - Group 1 |
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| ALKALINE EARTH METALS |
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| - Group 2 |
