Chemistry Vocab Test Questions – Flashcards
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| Atomic Radius |
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| one half the distance between the nuclei of two atoms of the same element when they are joined |
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| non metals |
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| poor conductors of heat and electricity |
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| periodic law |
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| when elements are arranged in order of increasing atomic # there is periodic repetition of physical and chemical properties |
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| halogens |
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| elements found in group 7A |
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| transition metals |
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| elements with s and d orbitals of the highest occupied energy level containing electrons |
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| cation |
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| ion with a positive charge |
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| ionization energy |
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| energy required to remove an electron from an atom |
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| electronegavity |
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| the ability of an atom of an element to attract electrons when the atom is in a compound |
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| anion |
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| ion with negative charge |
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| base |
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| an ionic compound that produces hydroxide ions when dissolved in water |
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| binary compound |
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| composed of two elements and can be either ionic or molecular |
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| law of definite proportions |
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| in samples of any chemical compound, masses of elements are always in same proportions |
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| acid |
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| compound that contains one or more hydrogen atoms and produces hydrogen ions when dissolved in water |
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| polyatomic ion |
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| ions composed of more than one atom |
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| law of multiple proportions |
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| whenever the same two elements form more tahn one compound, the different masses of one element that combine with the same mass of the other element are in the ratio of small whole #'s |
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| monatomic ions |
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| ions consisting of a single atom |
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| matter |
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| anything that has a mass and occupies space |
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| technology |
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| which society.... |
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| biotechnology |
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| applies science to the production of biological products or processes |
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| pollutant |
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| material found in air, water, or soul that is harmful to humans etc |
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| scientific method |
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| scientific approach to the solution of a scientific problem |
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| observation |
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| using your senses to obtain info |
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| experiment |
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| procedure that is used to test a hypothesis |
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| manipulated variable |
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| variable that you change during experiment |
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| responding variable |
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| variable that is observed during the experiment |
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| theory |
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| well-tested explanation for a broad range of observations |
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| scientific law |
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| concise statement that summarizes the results of many observations and experiments |
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| mass |
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| measure of the amount of matter the object contains |
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| volume |
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| measure of space occupied by the object |
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| extensive property |
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| property that depends on the amount of matter in a sample |
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| intensive property |
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| property that depends on the type of matter in a sample not amount of matter |
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| substance |
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| matter with uniform and definite composition |
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| physical property |
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| quality or condition of a substance that can be observed or measured without changing the substance's composition |
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| solid |
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| definite shape definite volume not easily compresed |
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| liquid |
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| indefinite shape definite volume not easily compressed |
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| Gas |
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| indefinite shape indefinite volume easily compressed |
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| physical change |
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| some properties of material change, but the composition of the material does not change |
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| mixture |
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| physical blend of two or more components |
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| heterogeneous mixture |
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| mixture where composition is not uniform throughout |
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| homogeneous mixture |
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| compostition is uniform throughout |
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| solution |
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| homogeneous mixture |
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| phase |
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| any part of a sample with uniform composition and properties |
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| filtration |
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| process separating solid from a liquid in a heterogeneous mixture |
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| distillation |
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| liquid boiled to produce vapor then condenced to for a liquid |
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| element |
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| simplist form of matter that has a unique set of properties |
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| compound |
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| substance that contains two or more elements chemically combined in a fixed porportion |
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| chemical change |
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| change that produces matter of a dif composition than the one before |
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| chemical symbol |
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| one or two lettered symbol |
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| chemical property |
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| ability of a substance to undergo a specific chemical change |
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| product |
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| substance produced in the reaction |
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| reactant |
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| substance present at the start of the reaction |
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| chemical reaction |
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| one of more substances change into one or more new substances |
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| precipitate |
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| sold that forms and settles out of a liquid mixture |
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| law of conservation of mass |
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| states that in any physical change or chemical reaction, mass is conserved. Mass is neither created nor distroyed |
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| measurement |
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| quantity that has both a # and a unit |
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| scientific notation |
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| given # is written as the product of two numbers ex) 6.02 X 10^23 |
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| accuracy |
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| measure of how close a measurement comes to the actual or true value of whatever is measured |
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| precision |
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| measure of how close a series of measurements are to one another |
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| accepted value |
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| correct value based on reliable references |
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| experimental value |
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| value measured in the lab |
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| error |
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| difference between experimental value and accepted value |
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| percent error |
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| absolute value of the error divided by the accepted value, multiplies by 100% ex) percent error= |error|/accepted value X 100% |
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| significant figure |
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| include all digits that are known, plus last digit that is estimated |
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| SI |
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| revised version of the metric system |
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| weight |
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| force that measures the pull on a given mass by gravity |
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| temperature |
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| measure of how hot or cold an object is |
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| the celsius scale |
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| sets the freezing point of water to zero and boiling point to 100 |
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| kelvin scale |
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| freezing point 273.15 K boililng 373.15 K |
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| absolute zero |
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| zero point on the Kelvin scale -273.15 degrees celsius |
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| energy |
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| capacity to do work or to produce heat |
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| Joule (J) |
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| SI unit of energy 1 J=0.2390 cal 1cal= 4.184 J |
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| Calorie(cal) |
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| quantity of heat that raises the temp of 1 g of pure water by 1 degree celsius |
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| conversion factor |
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| ratio of equivalent measurements |
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| dimensional analysis |
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| way to analyze and solve problems using units, or dimensions, of the measurements |
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| Density |
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| ratio of mass of an object to its volume ex) D=M/V |
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| atom |
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| smallest particle of an element that retains its identity in a chemical reaction |
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| electrons |
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| negatively charged subatomic particles |
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| cathode ray |
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| glowing beam |
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| protons |
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| positively charged subatomic particles |
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| neutrons |
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| subatomic particles with no charge but with a mass nearly equal to that of a proton |
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| nucleus |
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| tiny central core of an atom and is composed of protons and neutrons |
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| atomic # |
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| # of protons in the nucleus |
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| mass # |
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| total # of protons and neutrons in atom |
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| Number of neutrons |
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| = mass #- atomic # |
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| isotopes |
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| atoms that have the same# of protons but different # of neutrons |
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| atomic mass unit (amu) |
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| defined as 1/12th of the mass of a carbon-12 atom. |
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| atomic mass |
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| weighted average mass of the atoms in a naturally occurring sample of the element. |
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| period |
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| row --> |
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| group |
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| | | V |
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| energy levels |
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| fixed energies electron can have |
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| quantum |
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| amount of energy required to move an electron from one energy lever to another |
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| atomic orbital |
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| often thought of as a region of space in which there is a high probability of finding an electron |
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| electron configuration |
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| electrons arranged in various orbitals around the nuclei of atoms |
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| aufbau principle |
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| electrons occupy the orbitals of lowest energy first |
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| pauli exclusion principle |
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| atomic orbital may describe at most two electrons |
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| hund's rule |
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| electrons occupy orbitals of the same energy in a way that makes the # of electrons with the same spin direction as large as possible |
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| amplitude |
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| wave's height from zero to the crest |
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| wavelenth |
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| distance between the crests |
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| frequency |
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| v;# of wave cycles to pass a given point per unit of time |
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| electromagnetic radiation |
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| includes radio waves, microwaves, light etc |
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| spectrum |
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| different frequencies |
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| atomic emission spectrum |
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| frequencies of light emitted by electron |
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| ground state |
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| electron has lowest possible energy |
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| photons |
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| light quanta |
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| heisenberg uncertainty principle |
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| it is impossible to know exactly both the velocity and the position of a particle at the same time |
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| periodic law |
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| when elements are arranged in order of increasing atomic #, there is a periodic repetition of their physical and chemical properties |
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| metals |
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| good conductors of heat and electric currents |
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| metalloid |
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| generally has properties that are similar to those of metals and nonmetals |
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| noble gases |
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| elements in group 8A |
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| representative elements |
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| display a wide range of physical and chemical properties |
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| inner transition metal |
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| highest occupied s sublevel and a nearby f sublevel generally contain electrons |
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| transition metals |
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| highest occupied s and d sublevel contain electrons |
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| anion |
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| ion with negative charge |
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| valence electrons |
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| are the electrons in the highest occupied energy level |
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| electron dot structures |
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| diagrams that show valence electron dots |
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| octet rule |
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| in forming compounds atoms tend to achieve the electron configuration of a noble gas |
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| halide ions |
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| ions produced when atoms of chlorine and other halogens gain electrons |
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| ionic compounds |
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| compounds composed of cations and anions |
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| ionic bond |
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| electrostatic forces that hold ions together in ionice compounds |
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| chemical formula |
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| shows the kinds and #'s of atoms in the smalles representative unit of a substance |
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| formula unit |
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| lowest whole number ration of ions in an ionic compound |
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| coordination # |
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| # of ions of opposite charge that surround the ion in a crystal |
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| Metallic bonds |
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| consist of the attraction of free-floating valence electrons for the positively charged metal ions |
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| alloys |
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| mixtures composed of two or more elements at least one of which is a metal |
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| covalent bond |
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| atoms held together by sharing electrons |
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| molecule |
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| neutral group of atoms joined together by covalent bonds |
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| diatomic molecule |
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| molecule consisting of 2 oxygen atoms |
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| molecular compound |
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| compound composed of molecules |
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| molecular formula |
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| chemical formula of a molecular compound |
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| single covalent bond |
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| 2 atoms held together by sharing a pair of electrons |
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| structural formula |
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| represents the covalent bonds by dashes and shows the arrangements of covalently bonded atoms |
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| unshared pair |
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| pair of valence electrons that is not shared between atoms |
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| double covalent bond |
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| bond involving two shared pairs of electrons |
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| triple covalent bond |
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| bond formed by sharing 3 pairs of electrons |
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| coordinate covalent bond |
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| covalent bond in which one atom contributes both bonding electrons |
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| bond dissociation energy |
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| energy required to break the bond between two covalently bonded atoms |
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| resonance structure |
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| structure that occurs when it is possible to draw two or more valid electron dot structures that have the same # of electron pairs for a molecular molecule or ion |
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| molecular orbital |
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| orbitals that apply to the entire molecule |
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| molecular orbital |
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| orbitals that apply to the entire molecule |
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| bonding orbital |
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| molecular orbital that can be occupied by two electrons of a covalent bond |
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| sigma bond |
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| when 2 atomic orbitals combine to for a molecullar orbital that is symmetrical around the axis connecting two atomic nuclei |
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| pi bond |
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| bonding electrons are most likely to be found in a sausage shaped regions above and below the bond axis of the bonded atom |
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| tetrahedral angle |
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| 109.5 |
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| hybridization |
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| several atomic orbitals mix to for the same total # of equivalent hybrid orbitals |
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| nonpolar covalent bond |
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| bonding electrons share equally |
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| polar covalent bond |
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| covalent bond between atoms in which the electrons are shared unequally |
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| polar molecule |
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| one end of the molecule is slightly negative and the other end is slightly positive |
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| dipole interactions |
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| occur when polar molecules are attracted to one another |
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| dispersion forces |
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| the weakest of all molecular interactions, are caused by the motion of electrons |
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| hydrogen bonds |
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| are attractive forces in which a hydrogen covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom |
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| network solids |
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| solids in which all the atoms are covalently bonded to each other |
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| binary compound |
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| composed of 2 elements and can be either ionic or molecular |
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| mole |
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| representative particles measuring the amount of a substance |
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| representative particle |
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| refers to the species present in a substance |
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| avagadros # |
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| 6.02 X10^23 |
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| molar mass |
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| mass of mole |
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| STP |
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| temp of 0 |
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| percent composition |
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| percent by which mass of each element in the compound |
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| empirical formula |
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| gives the lowest whole-number ratio of atoms of the elements in a compound |
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| chemical equation |
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| representation of a chemical reaction |
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| skeleton equation |
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| chemical equation that does not indicate the relative amounts of the reactants and products |
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| catlyst |
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| substance that speeds up |
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| coefficients |
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| small whole numbers placed in front of |
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| balanced equation |
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| each side of the equation has the same # of atoms |
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| combo reaction |
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| chemical change in which two or more substances react to form a single new substance |
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| single replacement reaction |
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| chemical change in which one element replaces a second element in a compound |
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| activity series |
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| lists metals of decreasing reactivity |
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| combustion reactions |
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| reacts with oxygen |
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| complete ionic equation |
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| equation that shows dissolved ionic compounds as dissociated free ions |
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| spectator ion |
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| ion appears on both sides |
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| net ionic equation |
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| directly involved |
