Help
Options
Didn't know it?
click below
click below
Knew it?
click below
click below
Don't Know
Remaining cards (0)
Know
retry
shuffle
restart
0:00
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
Exam Chem Ch 1
| Question | Answer |
|---|---|
| chemistry definition | the study of matter and the changes that matter undergoes. |
| why do chemists determine the properties of matter | to study matter (classify, describe, explain the behavior of) |
| property definition | any characteristic that allows one to recognize or distinguish a particular type of matter. (color, state of matter) |
| Chemist determine the properties of matter through | experimental observations |
| Experimental observerations are used to explain and model the world around us usingq | the scientific method |
| Data definition | Observations of material pieces from experiments undertaken under controlled conditions |
| chemists use controlled conditions in their experiments so they are | reproducible (can be repeated) |
| What is data used for in an experiment | to draw conclusions about what is occurring during an experiment |
| Scientific laws | statements/equations that summarize the results of MANY experiments (what happens) |
| Theoretical models (theories) | explanations (why) certain phenomena is observed |
| theories originate from | hypotheses |
| A hypothesis will become a theory if it survuves | repeated testing |
| the scientific method being iterative means | its never ending as no result is considered unrefinable |
| qualitative observations | do not involve numerical information (color, hot or cold, bubbles formed, strong smell) |
| quantitative observations | measurements with numbers associated with them |
| two essential parts of a measurement | number and unit |
| element definition | substance that cannot be decomposed into simpler substances |
| compounds definition | substances that can be decomposed into simpler substances |
| solid state of matter properties | has fixed shape and volume |
| liquid state of matter properties | takes shape of the container; forms horizontal surface; has fixed volume |
| gas state of matter properties | expands to fill container |
| pure substance properties | made of one element or compound; composition and properties are the same in any sample; always homogenous |
| elements or compounds used to create a mixture are | components |
| homogenous and heterogenous classifications are on a scale dependent categorization. meaning that | its a classification that can change depending on scale |
| homogenous mixtures | same uniform appearance (no visible boundaries) referred to as solutions |
| heterogenous mixture | visible boundaries |
| true or false mixtures can be separated into their pure components | true |
| intensive property | physical property that does not depend on the size of a substance |
| extensive property | depends on size of substance |
| chemical properties | how a substance undergoes a chemical change (composition) into a different type of matter |
| homogenous mixtures can be separated into their components by processes that use | the differences in physical properties of the components |
| derived units | combination of 2 or more base units of si system |
| english system of units uses | inches |
| fahrenheit to celsius | (180/100)(Celsius temp) + 32 F |
| celsius to fahrenheit | (100/180)(fahrenheit temp) -32 |
| in kelvins water freezes and boils at | 273.15, 373.15 |
| kelvins to celsius | (1K/1C)(Celsius temp) + 273.15 |
| Celsius to kelvins | 1C/1K(temp in kelvin - 273.15) |
| measurement always has | a number, unit, and uncertainty |
| exact numbers | relationships between units |
| all quantitative observations involve | inexact numbers |
| most digits equals | least uncertain number |
| last digit in a measurement is always | an estimate |
| true or false no device can provide an exact measurement | true |
| accuracy | how close a measurement is to the accepted value of the property being measured |
| precision | how close the measurements are for repeated measurements |
| sig fig notation | method of writing a number with minimum uncertainty |
| when rounding off 5 to two decimal places round to closest | even number |
| other name for dimensional analysis | factor label method |
| density | intensive physical property that is a ratio of mass/volume |
| exact numbers arent considered for | sig figs |
| law of definite proportions (constant composition) | for any known compound, the elements making up that compound are always combined in the same portion by mass |
| law of conservation of mass | no detectable gain or loss of mass occurs in a chemical transformation |
| dalton's atomic theory of matter | matter must be made of some invisible unit (he called atom), atoms must possess certain properties that explain these two laws |
| Dalton's postulates 1-3 | Matter consists of atom (smallest unit that can experience change) In a pure element all atoms are identical in mass and properties atoms of a different element vary in mass and other properties |
| daltons postulates 4-5 | 4. When atoms of different elements combine to form compounds, new particles form (same ratio of atoms for compound) 5. atoms are indestructible in chemical reactions, atoms rearrange but do not break themselves apart |
| law of multiple proportions | if two elements A and B can combine to form more than one compound, the masses of B that combine with masses of A are in the smallest ratio |
| representational viewpoint | uses special language (equations, symbols) to characterize components of matter and changes they undergo |
| daltons hypothesis of atoms being indestructible was proven | wrong, atoms consist of subatomic particles |
| who discovered the grouping for the periodic table | dmitri mendeleev and julius meyer |
| Mendeleev was able to preidct | some elements that werent discovered |
| main grp elements | 1,2,13-18 |
| transition metals | 3-12 |
| inner transition metals | bottom of the table |
| alkali metals | group 1 |
| alkaline earth metals | group 2 |
| halogens | group 17 |
| noble gases | group 18 |
| hydrogen has properties of which two groups | 1, 17 |
| metals properties | can conduct heat and electricity well, shiny, left hand side of table |
| nonmetal properties | gases at room temp, dull, poor conductors, not malleable, low melting and boiling points, right hand side of table |
| metalloids properties | properties of metals and nonmetals, semiconductors of heat and electricity, right hand side of the table (except hydrogen) |
| average atomic mass is calculated by | using masses of its known isotopes and their fractional abundances |
| percentage abundance equals | fractional abundance x 100 |
| pure substances (molecules) | two or more atoms of same element |
| seven naturally molecular elements | hydrogen, nitrogen, oxygen, fluorine, bromine, iodine, chlorine |
| molecular compound | contains molecules with two or more types of atoms |
| for all ionic compounds there is no | individual molecule of that compound |
| formula unit | describes what types and the amount of each atom in a substance |
| rules for wriiting chemical formulas of ionic compounds | positive ion first, leave off subscripts of 1, electrically neutral, smallest set of whole numbers, charges not shown in formula |
| monatomic cation rule | name of atom + ion |
| metal can form more than one ion, what must be added to name | element name (charge) |
| ammonium | NH4+ |
| Ammonium | H3O+ |
| phosphonium | PH4+ |
| monatomic anions rule | replace suffix of atom with ide |
| hydroxide | OH- |
| cyanide | CN- |
| Peroxide | O2- |
| oxyanions | polyatomic anions containing oxyge (-ite or -ate as suffix, -ate for most common oxyanion) |
| depending on whether an oxyanion has one or 2 H atoms u should say | hydrogen (ion name) or dihydrogen (ion name) |
| inorganic compound | composed principally of non carbon elements |
| binary ionic compounds | element name for cation + anion with ide suffix |
| hydrates use | prefixes to indicate number of water molecules |
| binary molecular compounds | element name for first element + ide suffix to stem of elements name + prefixes use to indicate number of atoms in molecule |
| when a molecular compound contains hydrogen and only one other nonmetal atom binded to it you do not use | prefixes for hydrogen |
| examples of inorganic compounds | ionic, molecular, hydrates, acids/bases |
| acids | release H+ ions into a solution |
| binary acids naming | Add hydro to nonmetal name and ic to stem (chloric) + acid |
| acids containing three elements (oxoacids) | anion name from ate to ic, or ite to ous + acid |
| formula mass (molecular mass) | sum of all average masses in a chemical formula |
| mole is equal to the number oif | atoms in a sample of matter |
| Avogrado's number | 6.022 x 10*23 (number of moles for any entity) |
| molar mass | mass in g/1 mol |
| for pure elements, the molar mass is the same as | atomic mass |
| all compounds with same elements and molar ratio will have the same | percent composition |
| empirical formula only accepted for | ionic compounds |
| molecular mass is always a multiple of its | empirical formula |
| for subscripts in chemical formula, you can round to .5 if number is between | x.35-x.65 |
| can round to 1 for subscript if number is between | x.8-2.2 |
| concentration | amount of a component in a solution |
| dilute solution | small amount of solute compared to solvent |
| concentrated solution | large amount of solute compared to solvent |
| molarity (molar concentration) | moles/liters of solution |
| volume of dilute solution x molarity of dilute solution is = to | volume of concentrated solution x molarity of concentrated solution |
Created by:
taylerw613
Popular Biochemistry sets