Honors Chem Midterm Review Sheet
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77 terms
Terms | Definitions |
|---|---|
 chemistry | the study of matter and it's changes |
| modern world: age of _____ | plastics |
| matter | anything that has mass and takes up space |
| vapor | gaseous state of a substance that is generally a liquid or a solid at room temp. |
| solid | particles tightly packed, defined shape and volume |
| liquid | expands when heated, takes shape of the container, particles are semi-flexible |
| gas | takes shape and volume of container, particles are far apart |
| scientific method | observation>hypothesis>experiment>theory |
| theory | braod and extensively tested explanation of why experiments give certain results. can't be proven |
| law | concise statement that summerizes the results of many observations and experiments. can be proven, but can't be explained |
| hypothesis | a proposed explanation or reason for what is observed |
| how to study chemistry | understand and apply concepts by using your textbook, experiments tests and quizzes |
| physical properties | state, color, meling point, boiling point, density |
| physical changes | cutting, grinding, bending, etc. |
| distillation | boiling liquid to produce a vapor that is then condensed again into a liquid. it purifies the liquid |
| homogeneous mixtures | completely uniform in composition (ex. salt water) also called a solution |
| heterogeneous mixtures | not uniform in composition (ex. chocolate chip cookie) |
| mixture | either hetero. or homo. a physical blend of two or more substances that is seperable by hand |
| compound | a substance that can be separated into simpler substances only by chemical means |
| qualitative | results given in a descriptive, nonnumeric form |
| quantitative | results given in definite numbers and units |
| accuracy | the measure of how close a measurement is to the actual, true value |
| precision | the measure of how close measurements are to one another |
| sigfig rule on leading zeros | they don't count ever (sigfigs) |
| sigfig rule on in-between zeros | they always count (sigfigs) |
| sigfig rule on zeros at the end | they only count if there is a decimal (sigfigs) |
| mega(M) | 10^6 |
| kilo(k) | 10^3 |
| deci(d) | 10^-1 |
| centi(c) | 10^-2 |
| milli(m) | 10^-3 |
| micro(μ) | 10^-6 |
| nano(n) | 10^-9 |
| pico(p) | 10^-12 |
| how to become a better problem solver | develop a plan |
| the heart of problem solving | analyze>calculate>evaluate |
| density (equation) | m/v |
| relationship b/w numerator and denominator in a conversion factor | numerator is equivalent to denominator |
| smallest particle of an element that retains all its properties | atom |
| Democritus | first suggested the idea of atoms |
| Dalton's Atomic Theory | •invisible particles •atoms of same element are identicle •atoms of different elements can physically mix together in simple whole-number ratios •atoms of 1 element are never changed into atoms of another element as a result of a chemical reaction |
| JJ Thompson | discovered the electron |
| Robert A. Millikan | discovered the quantity carried by electron |
| E. Goldstein | discovered protons |
| James Chadwick | discovered neutrons |
| Ernest Rutherford | discovered the nucleous |
| Rutherford Experiment | Gold foil method** |
| nucleus | center of an atom, heaviest part, made up of protons and electrons |
| electron | negatively charged, form a cloud around the nucleus |
| proton | positively charged |
| neutron | no charge at all |
| atomic number | •the number over the chemical symbol of the periodic table •tells how many protons are in the element |
| mass number | •the sum of the number of neutrons and protons in an atomic nucleus •under the chemical symbol |
| finding isotopes | different number of neutrons=different number of mass (ex. Ne-20: 10p, 10n, 10e; Ne-21: 10p, 11n, 10e; Ne-22: 10p, 12n, 10e) |
| isotopes | atoms that have the same number of protons but a different number of neutrons |
| how to find the atomic mass of a series of isotopes | average the masses |
| anion | ions that end in "-ide" |
| the electrical charge of a cation | positive charge |
| cation | any atom or group of atoms that has a positive charge, meaning one or more electron has been taken away ⁺sign is directly after the chemical symbol |
| anion | any atom or group of atoms that has a negative charge, meaning one or more electrom has been added ⁻sign is directly after the chemical symbol |
| ionic compounds | composed of metal cations and nonmetal anions (ex. sodium chloride) |
| molecular compounds | composed of atoms of 2 nonmetal anions (ex. carbon monoxide) |
| when a group of the periodic table becomes ions | ionic charge is positive and numerically equal to the group when positive/when negative subtract the group number from 8 to get the number** see pages 143-145 |
| Avagadro's number | 6.23*10^23 number of representative particles |
| 1 mole (quantity) | 6.022*10^23 atoms 6.022*10^23 molecules 6.022*10^23 ions |
| diatomic elements | (NIH) N₂O₂F₂Cl₂Br₂I₂H₂ |
| volume of 1 mole of liquid at STP | 22.4 L |
| chemical reaction symbols | + add reactants --> yield; products come after this symbol <--> reversable (s) (l) (g) (aq) states arrow with triangle on top heat was used arrow with "Pt" on top catalyst used |
| types of chemical reactions | combination decomposition combustion single displacement double displacement (acid-base or precipitate) |
| chemical equations must be balanced so that they:_______ (reason) | obey the the law of conservation of mass |
| catalyst | something that speeds up a chemical reaction, but isn't used up |
| the calculation of quantities in chemical equations | stoichiomentry |
| what is conserved in a chemical reation | atoms and mass |
| relationship between mass of reactants and products | they are equal |
| percent yield (equation) | (actual yield (given) ÷ theoretical yield (found in lab))*100% |
| limiting reagent | determines the amount of product that can be formed in a reaction |
| excess reagent | reactant not completely used in a reaction |
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