| Question | Answer |
| Rules for naming acids with oxygen | 1. anion ends in -ate, suffix -ic acid. 2. anion ends in -ite, suffix = -ous acid |
| Rules for naming acids without oxygen | Anion ends in -ide: Hydro-root-ic acid |
| Acids | certain molecules that contain free H+ ions. One of more H+ attatched to an anion |
| Name the prefixes for naming nonmetalic binary compounds | mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca |
| Naming binary covalent compounds: 2 nonmetals | 1. first element in formula named first. 2. 2nd element named as anion (-ide) 3. prefixes denote numbers of atoms present. 4. mono never used for naming first element |
| Naming oxyanions | Smallest number = Hypo-root-ite. Small number = root-ite. Large number = root-ate. Largest number = Per-root-ate. |
| Oxyanions | series of anions that contain atoms of given element and different numbers of O atoms |
| Naming binary compounds: Metals sometimes form more than 1 type of cation. | Charge on metal ion must be specified by roman numeral. Elements that only form 1 cation don't need roman numerals. Expections: Ag+ always the same and Zn+2 always the same. |
| To name binary compounds, + monoatomic cation, - monoatmic anion | 1. cation always named first. 2. monoatomic cation takes name from name of element. 3. monoatomic anion root + -ide |
| periods | horizontal row of elements |
| noble gases | group 8A, monoatomic gases, little chemical reactivity |
| Halogens | Group 7A, diatomic molecules, ions charge 1- |
| alkaline earth metals | Group 2A, 2+ charged ions |
| alkali metals | group 1A, active elements that form ions with +1 charge |
| groups/families | vertical columns, similar chemical properties |
| nonmetals | upper right corner of table. Tend to gain electrons. lack physical properties of metals. form negative ions. bond to each other with covalent bonds |
| metals | efficient conductors of heat and electricity. malleable (into thin sheets). ductile (into wires). lustrous appearance. majority of elements. |
| periodic table | shows all known elements, gives information about each. letters in boxes = symbols for the elements |
| polyatomic ions | many atom ions, can be in ionic compounds |
| ionic solid | solid consisting of oppositely charged ions |
| ionic bonding | force of attraction between oppositely charged ions. cation and anion. |
| anion | ion with negative charge, takes electron |
| cation | one electron stripped off. positive ion. |
| ion | atom or group of atoms that has a net positive or negative charge |
| space-filling model | relative sizes of atoms as well as relative orientations in molecule |
| structural formula | individual bonds shown, may not indicate actual shape of molecule. line = individual bonds. to show shape: dotted lines behind plane of paper, wedges in front of plane of paper |
| chemical formula | symbols for elements to indicate types of atoms present. subscripts = number of atoms. |
| molecules | held together by covalent bonds. move around as independent units. |
| covalent bonds | sharing electrons |
| chemical bonds | hold together atoms in a compound |
| mass number | number of protons + neutrons, in superscript |
| Atomic number | number of protons, in subscript |
| Isotopes | Atoms with the same number of protons, but different numbers of neutrons. Almost exactly the same properties. |
| Neutrons | Same mass at p+, but not charge. |
| Protons | Positive charge = electon's negative charge |
| Modern atom model | Tiny nucleus with electrons moving about. Chemistry of atom results from electrons. Nucleus made of P+ and N0. Number and arrangement of e- accounts for chemical properties. |
| Nuclear atom | Rutherford. Center = positive charge (Nucleus) with electrons moving arorund nucleus at large distance relative to nuclear radius |
| Gold foil experiment | Tests Thomson's plum pudding model. Directs alpha particles at thin sheet of gold foil. Alpha particles should crash right though foil with minor deflects. Many particles deflected at large angles, some reflected, majority go through. Huge surprise. Plum pudding model could not be correct. Results could only have been caused by center of concentrated positive charge that contains most of atom's mass. Deflected particles = "close encounters" with nucleus |
| Ernest Rutherford | Gold foil test, nuclear atom |
| 3 types of radioactive emissions | Gamma (high energy light), Beta (High speed electron), Alpha (2+ charge, helium nucleus) |
| Radioactivity | Spontaneous emission of radiation. |
| Plum Pudding model | JJ Thompson. After doing cathode-ray experiment with various types of metals, hypothesized that all atoms have electrons. Atoms neutral, therefore also had to have some positive charge. Atom = Diffuse cloud of positive charge with negative electrons imbedded in it. |
| Cathode-ray tube experiment | Partially evacuated tube. High voltage through tube, a 'ray' or cathode ray produced. Produced at - electrode, repelled by negative pole of magnet. Thought ray was negatively charged particles called electrons. Develops charge-to-mass ratio of electron. e/m = -1.76 x 10^8 C/g |
| JJ Thompson | Discovers electrons, plum pudding model |
| Avogardo's Hypothesis | At the same temperature and pressure, equal volumes of different gases contain the same number of particles. Volume of a gas determined by number of particles present. |
| Dalton's atomic theory. | 1. Each element is made up of tiny particles called atoms. 2. Atoms of a given element are identical. Atoms of different elements are different in some fundamental way or ways. 3. Chemical compounds are formed when atoms of different elements combine with each other. compounds always the same relative numbers and types of atoms. 4. Chemical reactions involve reorganization of atoms. Changes the way they are bound together. Atoms themselves are not changed. |
| Law of multiple proportions | If elements composed of tiny individual particles, given compound always the same combination of these atoms. Why same relative masses of elements were always found in a given compound. When two elements form a serries of compounds, the ratios of the first masses of the second element that combine with 1 gram of the first element can always be reduced to small whole numbers. Leads to hypothesis that each element consisted of certain type of atom and compounds were formed by specific combinations of these atoms. |
| John Dalton | Law of multiple proportions, atomic theory, atomic masses |
| Law of Definite Proportions | A given compound always contains exactly the same proportion of elements by mass. |
| Phlogiston | Stahl thought it flowed out of burning material. Things stop burning because container filled up with phlogiston. Discovered phlogiston actually oxygen. |
| Robert Boyle | First "chemist." Relationship between pressure and volume. End of Greek 4 system. ideas about chemical elements |
| Greeks believed matter composed of | Fire, earth, air, water |
| Fahrenheit to Celsius | TF = TC x 9F/5C + 32F |
| Elements | Substances that cannot be decomposed into simple substances by physical or chemical means. Composed of atoms with nuclei and electrons. |
| Chemical change | Given substance becomes new substance or substances with different properties and different composition |
| Compound | Substance with constant composition. Can be broken down into elements by chemical processes |
| Paper chromatography | porous paper and drop of mixture |
| Chromatography | Mobile phase, either gas or liquid. Stationary phase, solid. Components with high affiinity for mobile phase move quickly thorugh chromatographic system |
| Filtration | Solid and liquid. Put through mesh paper, liquid leaves solid behind |
| Distillation | Depends on volatility (how readily substances become gases). Boil through cool tube into flask. Sometimes required multi-step distillation |
| physical changes | eg. boiling/freezing |
| pure substance | one with constant composition |
| solution | homogeneous mixture |
| Heterogeneous mixture | visibly distinguishable parts, can be usually separated into 2 or more homogeneous parts |
| Homogeneous mixture | visiblely indistinguishable parts |
| Gas | No fixed volume or shape, compressible |
| Liquid | Definite volume, no specific shape |
| Solid | rigid, fixed volume and shape |
| Density | mass/volume |
| Converting Temperature (Kelvin) to Temperature (Celsius) | T(K) = T(C) + 273.15 |
| Unit factor | Doesn't change value, only units |
| Dimensional analysis/unit factor method | Convert a given result from one system of units to another |
| Sig fig calculations: Rounding | Use only the first number to the right of the last sig fig, don't round until the end. |
| Sig fig calculations: Addition or subtraction | Same number of decimal places as limiting term |
| Sig fig calculations: Multiply or divide | Number of sig figs same as least precise measurement (limiting term) |
| Rules for counting sig figs: definitions | yes, infinite sig figs |
| Rules for counting sig figs: counted numbers | yes, infinite sig figs |
| Rules for counting sig figs: trailing zeros | only with decimal point |
| Rules for counting sig figs: captive zeros | yes |
| Rules for counting sig figs: leading zeros | no |
| Rules for counting sig figs: nonzero integers | yes |
| Systematic error | AKA Determinate error. Either always high or low. If systematic error absent, precision indication of accuracy. |
| Random error | AKA Indeterminate error. Equal probability of being high or low. |
| Precision | Degree of agreement among several measurements of the same quantity. Reproductability. |
| Accuracy | Agreement of particular value to true value |
| Significant Figures | Uncertanty of last number |
| Uncertain digits | Vary |
| Certain digits | Remain the same regardless of who makes the measurements |
| Weight | Force g exerts on an object to measure mass. Varies with gravity. |
| Mass | Resistance of an object to change |
| SI System | System Internationale. Prefixes change size. |
| Natural Law vs. Theory | Natural Law: Summy of observed (measurable) behavior. Theory: Attempt to explain WHY it happened. |
| Natural law | See that same observation applies to many different system. Generalized. Eg. Law of Conservation of Mass |
| What is a theory, or a model | Created by many tested hypotheses. Interpretation for why an observation my have occured. Subject to change. Future predictions can lead to experiments which can lead to a modified theory. An educated guess. |
| quantitative observations | numbers and units, measurements |
| Qualitative observations | no numbers |
| Hypothesis | Possible explanation |
| What is the scientific method? | 1. Collect data (observations) 2. Formulate hypothesis (suggest possible explanations) 3. Test hypothesis (do experiments) |
| Microscopic world | World we cannot see |
| Macroscopic world | World we can see |
| What is a scanning tunnel microscope (STM) | Uses e- current to see very small objects |
| Described why the cooled melted wax had a hole in the middle. | Hardened from the outside in, as outside hardens, volume of inside decreased, and therefore density increased and it sank to the bottom |
| What is the densest element? | Osnium |
| What is rheoscopic fluid? | Shows dynamics, tests pressures, made up of different densities |
| Describe centrifugation | Rheoscopid fluid spins around in centrifuge, denser things go to the bottom, sepparates based on density |
| Describe the wax density demo | Solid wax sinks in liquid wax -- more dense |
| femto (f) | 10^-15 |
| pico (p) | 10^-12 |
| nano (n) | 10^-9 |
| micro (ยต) | 10^-6 |
| milli (m) | .001 |
| centi (c) | .01 |
| deci (d) | .1 |
| deca (dk) | 10 |
| hecta (h) | 100 |
| kilo (k) | 1000 |
| mega (M) | 10^6 |
| giga (g) | 10^9 |
| tera (t) | 10^12 |
| What happened in the stoplight reaction? | Orangish yellowish liquid, shaken, turns amber red, goes quickly back to orange. Shake up and own, from orange to green, to blackish purple. |
120 cards - created sep 13, 4:36pm