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Chemistry Exam 1- BL
| Question | Answer |
|---|---|
| accuracy | measure of how close the measurement is to the "true"value |
| precision | measure of how close together repeated measurements are to eachother |
| volume | measure of how much three dimensional space a substance, especially gas or liquid occupies |
| electrolytes | ions dissolved in water |
| formula unit for ionic compounds | of an ionic compound represents the ration of cation to anion in the lattice |
| formula mass for ionic compounds | sum of atomis masses of ions in formula unit (amu) |
| molecular mass for covalent compounds | sum of atomic masses of atoms in molecular formula (amu) |
| properties of nonmetals | -low melting point -hydrogen=nonmetal -own color -brittle -nonconductive -reduction |
| element | substance somposed of only one type of atom, cannot be broken down into simpler form -109 known elements -90 unknown elements |
| lattice structure | every cation is surrounded by anions; every anion surrounded by cations |
| matter | anything that has maass and occupies volume |
| momatomic ion | ion formed from a single atom |
| diatomic molecules | molecules composed of two atoms |
| molecular formula | a covalent compound that has definite & unique composition -gives limited info -doesnt indiciate arrangement of atoms or covalent bonds |
| NH4 | ammoniun (cation) |
| H3O | Hydronuim (cation) |
| OH | hydroxide (anion) |
| NO3 | nitrate(anion) |
| CN | cyanide (anion) |
| HCO3 | hydrogen carbonate (anion) |
| HSO4 | hydrogen sulfate (anion) |
| CO3 (2-) | carbonate ion (anion) |
| PO4 (3-) | phosphate ion (anion) |
| Guidelines for determining formula unit for ionic compound | 1. determine charge on cation 2. determine charge of anion (group #-8) 3.insert subscripts CA2+cl = CaCl2 4.divide by common divisor Mg2O2= MgO 5. Double check if neutral or not (cation charge x subscript) + anion charge x subscript) |
| naming ionic compounds | -metal first, nonmetal second -take off ending add -ide to nonmetal -if multiple #, NaCl3; add the charge as roman numeral- Sodium (III0 Chloride -if compound has lower charge add-ous -if compound has higher chharge add- ic |
| naming covalent compounds | prefixes 1-mono 2-di 3-tri 4-tetra 5-penta 6-hexa 7-hecta 8-oct 9-nona 10-deca ex: nitrogen oxide =NO nitrogen dioxide =NO2 |
| polyatomic ions | ions made up of a group of atoms then a single atom |
| allotrope | different forms of the element within the same phase -O2 & O3 -P- white; burns in air (r &b exist) Carbon - grahite, diamond, c60 (soccerball) |
| density | physical property of mater often used to characterize a substance or material ... d=m/v |
| properties of metals | -solids -metallic luster -malleability -ductile -conduct electricity -dense -oxidation |
| covalent bonds | two nonmetals come together & share valence E -neutral -E are shared -2 or more nonmetals -discrete(individual) |
| ionic compound | formed when a metal atom transfers some or all of its valence electrons to a nonmettal -cation/anion -metal and nonmetal -electrostatic -dimensional lattice of oppisitely charged atoms |
| mass | measure of the amt of matter |
| mass, location & charge of: P , E, & N | P= nuclues, positive, 1.6726x 10^-24 E= electron cloud, negative, 9.108 x10 ^-28 N=nuetral, nucleus, 1.750 x 10 ^24 |
| average atomic mass | weighted average of the mass of its isoptopes based on their natural adundance |
| calcuate average mass | avg=(%x100)(mass1) + (%x100)(mass2) |
| ion | atom that has lost or gained one or more valence electrons -positive or negative |
| compound | substance composed of two or more diff types of atoms held together in a unique proportion -broken down through chemical reactions |
| nonbonding or lone pairs | electrons that dont share an electron |
| ionic bond | electrostatic attraction that holds ions together |
| ionization | process when metals lose electrons |
| molar mass | mass of one mole of an element or comound |
| pure substance | substance composed of only one compound or element |
| change F to C | (f-32)5/9 |
| Change C to F | 9/5(C + 32) |
| Change C to K | add 273 |
| Change K to C | -273 |
| isotopes | atoms with the same number of protons but a different # of neutrons |
| atoms | smallest particle that retains the properties of an element - atom is to element as molecule is to compound |
| molecule | smallest particle retainnig properties of the compound, but, some elements exist as molecules in their stable form |
| a-s=us | unshared atoms |
| atomic number | # of protons an atom contains |
| dimensional analysis | considers the units (dimensions) to set-up the calculation supplied x req/supplied = req |
| chemical properties | refer to its behavior in the presence of other chemical substances -transorms substances into new substance |
| every measurement consists of: | # & a unit |
| nanoscale & atomic scale | describes matter too small to be seen even with a microscope |
| scientific notation | used to express really small # or really big # |
| SF: x & / | never give more SF in the answer than least # given |
| SF: + & - | never give more after the decimal than the least number given after the decimal |
| micronutrients | required in quanities of less than 100mg/day |
| the mole | 6.02 x 10^23 aka avagrados number |
| anion | # of electrons greater than the number of protons -neg charged -nonmetals gain electrons to becom anions |
| cation | less than the number of protons -positively charged -metals lose electrons to becom cations |
| electron orbital | region of space where electrons are found |
| energy levels | lower the lectrons on the shells; lower the energy -three orbitals |
| elements to the right of the periodic table... | gain electrons |
| temperature | measure of the intensity of heat |
| diatomic molecules found in nature | BrINClHOF bromine iodine nitrogen chlorine hydrogen oxygen flourine |
| bohr model | thought electroms orbitied around the nucleus like planets around the sun |
| electron configuration levels | 1s2 2s2 2p6 3s2 3p6 4s2 4p6 |
| outershell & innershell electrons | outer- valence electrons inner- core lelectrons |
| elements on the left of the periodic table.. | drop electrons |
| heat | form of energy |
| inert | unreactive |
| octect rule | prediction of a molecule structure of a molecule by arranging electrons so that each atoom has a full outermost shell |
| significant figures | all the certian digits as well as the one uncertian digit |
| electrostatic attraction | "glue" that holds ions together - force of attraction btwn oppositely charged entities (cation & anion) |
| physcial properties | properties we observe or measure without considering how the element interacts |
| weight | weight depends on gravitational pull |
| macronutrients | elements required in large quanities . more than 100mg/day |
| lewis dot structure | represent a pair of bonding electrons with dots or lines |
| mass number | sum of protons & neurons of the isotopes |
| metric conversion | mathemetical transformation of a value in one metric unit (supplied unit) into another metric unit( requested unit) |
| macroscopic scale | all material you can see |
| covalance | how many bonds commonly found |
| periodicity | property of elements in the same column ( similiar physical & chemical) |
| margin of error | conveyed in the number of digits reported in the # -10lb -10.0lb -10.00lb |
| valence electrons | # of electrons in the outermost shell of an atom -equal to group # |
| N-A=S | n= # of E needed A= # of E available S= # of E shared |
| microscopic scale | cannot be seen by the naked eye |
| guidelines for sig figs | 1.nonzeros sig (3.45= 3SF) 2.Trap zeros are sig ( 3.05 =3 SF) 3. zeros following nonzero & decimal pt sig (0.400 = 3SF)(4.0 - 2 SF) 4. no decimal -zeros not sig (6,000 = 1 SF) 5. Zeros that appear before nonzeros not sig (0.00040 = 2 SF) 6. all # in SN |
Created by:
britlat
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