chem. finals Word Scramble
|
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
Question | Answer |
manipulated variable | variable that changes |
responding variable | variable that is observed as the result of an experiment |
scientific method | observe, hypothesize, predict, experiment |
matter | anything that has mass and takes up space |
chemical change | creating a new substance by changing the composition, irreversible |
physical change | properties of materials change but composition does not |
chemical reaction | reactants yield product |
compound | 2 or more elements chemically combined in fixed proportions |
element | purest form of matter, made of 1 substance |
reactant | substance that undergo a chemical reaction |
product | result of a chemical reaction |
heterogeneous | mixture of 2 or more substances that are not uniform |
homogeneous | 2 or more substances uniformly mixed |
law of conservation of mass | mass can not be created of destroyed |
precipitate | solid formed from 2 aqueous reactants in a chemical reaction |
vapor | gaseous state of substance that is a liquid of solid at room temperature |
accuracy | how close to the expected value |
conversion factor | ratio of equivalent measurements |
dimensional analysis | use of conversion factors to solve problems |
percent error | % error=|accepted-experimented|/accepted*100 |
precision | how close measurements are to each other |
scientific notation | a base number times a power of 10 |
significant figures | accurate measurements by the right number of digits |
atom | smallest part of matter that still holds all properties of an element |
atomic mass | weighted average of all isotopes of that atom |
atomic number | number of protons |
electrons | negatively charges, JJ Thompson |
proton | positively charged, Goldstein |
nucleus | protons + neutrons, center of atom |
group | up and down periodic table |
period | left and right of periodic table |
isotope | same number of protons but different number of neutrons |
mass number | protons + neutrons |
neutron | no charge, Rutherford |
atomic orbital | 1s, 3p, 5d, 7f |
atomic sublevels | s,p,d,f |
aufbau's principle | electrons enter orbitals in the lowest energy level |
electron configuration | 1s22s23p6 . . . |
energy levels | quantum number, n=1, 2, 3, 4 . . . |
ground state | electron is in the lowest energy level possible |
hund's rule | electrons enter orbitals with up spin then go back and fill up with down spin |
pauli exclusion principle | each orbital holds 2 electrons with opposite spins |
anion | nonmetals, receive electrons, negatively charged ion |
cation | metals, give away electrons, positively charged ion |
periodic law | along a period elements have similar properties |
atomic radius | distance between 2 nuclei of the same element |
electronegativity (electron affinity) | ability to attract an electron |
ionization energy | amount of energy it takes to remove an electron |
metalloids | along the staircase and has both properties of metals and nonmetals |
metals | left of staircase, good conductor, malleable, strong |
transition metals | groups 1b to 8b |
representative elements | groups 1a to 8a, short form |
nonmetals | right of staircase, not good conductors, mostly gases, brittle |
chemical formula | use symbols to show element and the number of each in a ionic compound |
electron dot structure | element symbol surrounded by dots representing valence electrons |
formula unit | another name for ionic compound |
ionic bond | transfer of electrons from cation to anion |
ionic compound | made up of metal cations and nonmetal anions |
metallic bond | formed by attraction of free flowing valence electrons for positively charged metal ions, "sea of electrons" |
octet rule | all elements want stable electron configuration like noble gases |
valance electrons | electrons in the outer most shell |
covalent bond | bonding of 2 or more nonmetals |
diatomic molecule | H2, N2. O2, F2, Cl2, Br2, I2, nonmetals that bonds with itself |
molecule | covalent compound |
nonpolar | covalent bond where atoms have equal pull (0-.4) |
polar | covalent bond in which electron are being pulled towards one atom over another (ex. H2O mickey mouse shaped) |
pi bond | double bond, 2nd bond formed |
sigma bond | single bond, 1st bond formed |
polyatomic ion | covalent compound with charge |
resonance | write 2 or more different lewis structures for the same compound |
unshared pair electrons | lone electrons not active in bond |
VSEPR theory | repulsion between lone electrons causes shape to bend |
structural formula | lewis structure with dots and dashes |
acids | H+ in front |
bases | OH- at the end |
binary compound | 2 elements bonded together either ionic or covalent |
monatomic ion | single element with charge |
law of definite proportions | chemical compounds have the same composition despite sample size |
law of multiple proportions | elements combine in whole number rations not decimals |
avagadro's number | 6.02*10^23 |
empirical formula | smallest ratio of a molecular formula |
molar mass | mass of 1 mole on an element or compound |
percent composition | % composition = (mass of element/mass of compound)*100 |
representative particles | atom, molecule, formula unit |
activity series | ability of an element to replace another in a single replacement |
balanced equation | has coefficients |
chemical equations | uses symbols for reactants and products, separated by ----> |
catalyst | speeds up chemical reaction but not involved |
synthesis/combination | A+B--->AB |
combustion | A+O2--->CO2+H20+heat |
decomposition | AB--->A+B |
single replacement | A+BC--->B+AC |
double replacement | AB+CD--->AD+CB |
skeleton equation | no coefficients |
spectator ion | not involved in net ionic equations |
actual yield | what it actually produces |
excess reagent | left over after chemical reaction |
limiting reagents | used up in chemical reaction, determines the amount of product produced |
mole ration | obtained by coefficients in balance equation |
percent yield | (actual/theoretical)*100 |
stoichiometry | calculating quantities from info provided in balanced equation |
theoretical yield | what it should produce, have to figure it out using mole island and not given |
measure the level of lead in the blood | analytical chemistry |
study non carbon based chemicals in rocks | inorganic chemistry |
investigate changes that occur as food is digested in the stomach | biochemistry |
study of carbon based chemicals in coal | organic chemistry |
explain the energy transfer that occurs when ice melts | physical chemistry |
what is density of water? | 1 g/mL = 1 g/cm3 |
why is an atom positively charged when it loses an electron? | more protons than electrons |
why is an atom electrically neutral | same number of protons and electrons |
name 2 ways that isotopes of the same element differ | number of neutrons and mass |
how many orbitals are in 2p energy level? | 3 |
how many sublevels are in the n=1 principle energy level? n=4 energy level | 1(s), 4(s, p, d, f) |
what is the max number of electrons that can go into the 3p sublevel? 4f sublevel? 3d sublevel? | 6,14,10 |
what are 2 ways an ion can form from an atom | gain of lose electrons |
compare the size of cations to its original element | cations are always smaller than the original element because it lost electrons |
compare the size of anions to its original element | anions are alway bigger because it gained electons |
why are ionic compounds chemically neutral? | charges on ions balance out |
what is the different between ionic bond and covalent bond? | ionic=transfer electrons covalent=share electrons |
what are the molecular shapes? | linear, bent, trigonal planar, trigonal pyramid, square planar, tetrahedral |
extensive properties | properties dependent on sample size (ex. mass, volume) |
intensive properties | properties that are not dependent on sample size but the type of matter (ex. density, color hardness, melting point, malleability) |
democritus | 1st to suggest idea of atoms, particles that were indestructable and indivisible, no evidence |
chadwick | neutron |
who used the gold foil experiment? to find what? | Rutherford used it to find the nucleus |
what were the curies responsible for | discovery of radioactivity |
Bohr's model | electrons orbit around nucleus in a fixed path, did not work for any atom than hydrogen |
electrons behave like _________. | waves of motion |
quantum | the amount of energy required to move an electron from one energy level to the next |
what happens when electrons get excited | electron gains energy and move up energy levels, when they return to ground state they emit light as result of electron transition |
bond dissociation energy | energy needed to break a bond |
van der waal forces (intermolecular forces) | dipole interactions, dispersion forces |
dipole | similar properties of an ionic or polar covalent bond but much weaker, 2 polar molecules are attracted to one another |
dispersion forces | momentary attraction of electrons due to the random motion of electron in an atom |
Created by:
sapphiresun
Popular Chemistry sets