Honors Chemistry Semester one
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
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| 314.721 | 6 significant figures
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| 0.001775 | 4 significant figures(place-holding zeroes are NOT significant)
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| 23.12 | 4 significant figures
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| 7.9303 | 5 significant figures
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| 63000 | 2 significant figures
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| 0.0091 | 2 significant figures
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| 34.00 | 4 significant figures (zeroes to the right of the decimal are significant)
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| 20.02 | 4 significant figures (zeroes betweend two non-zeroes are significant)
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| 12 books | unlimited significant figures (exactly counted things have unlimited significant figures)
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| 200.740 | 6 significant figures
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| 0.007 | 1 significant figures
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| 39.0 | 3 significant figures
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| 61.2+9.35+8.6=(find answer with correct significant figures) | 79.2
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| 34.61-17.3= | 17.3
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| ROUND TO THREE SIG FIGS: 87.073 | 87.1
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| ROUND TO THREE SIG FIGS: .001552 | .oo155
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| ROUND TO THREE SIG FIGS:6.999 | 7.oo
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| 6051.00 | 6 significant figures
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| 0.0005 | 1 significant figures
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| 0.1020 | 4 significant figures
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| 5000 | 1 significant figures
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| 0.020 | 2 significant figures
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| 501 | 3 significant figures
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| 2 liquid elements in room temp | mercury(Hg) and bromine(Br)
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| metalloids | boron(B) silicon(Si) germanium(Ge) arsenic(As) antimony(Sb) tellurium(Te) polonium(Po) astatine(At)
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| diatomic elements | hydrogen, nitrogen oxygen fluorine, chlorine, bromine, iodine
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| valence electrons | electrons on the outer most shell
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| family | vertical column of elements
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| period | horizontal row of electrons
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| mass | sum of protons and neutrons
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| atomic number | number of protons
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| matter | has mass and takes up space
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| heterogeneous mixture | mixture that is not thorough throughout
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| element | most basic form
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| compound | 2 or more combined elements
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| aristotle | 350BC, 4 elements=earth, wind, fire, water
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| dalton's atomic theory | 1808 matter consists of atoms,indestructible, rearrange but never break apart, identical in mass. can be identified by their weights. different elements can combine to form compounds. atoms are always presented in the same whole number ratio.
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| Thompson | 1895-Thompson, plum pudding model. filled container with gas and attached a battery charge to both ends and can glowed, added a wall with a small opening on one side of the can and a line/strip of green went from one end to the other.
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| Rutherford | 1909-shot alpha particles into gold foil. came up with idea that there are positive and negative particles. came up with model that is very close to what we use today
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| Bohr | 1913-came up with the basis for the present day model of the atom(excluding the neutrons)
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| chadwick | 1932-found out that the protons and electrons aren't adding up to the elements mass. he noticed that there must be neutrons in the nucleus with the protons and the electron clouds around it. present day model.
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| (NH4)+ | ammonium
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| (NO2)- | nitrite
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| (NO3)- | nitrate
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| (SO3)2- | sulfite
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| (SO4)2- | sulfate
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| (HSO4)- | hydrogen sulfate
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| (OH)- | hydroxide
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| (CN)- | cyanide
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| (PO4)3- | phosphate
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| (HPO4)2- | hydrogen phosphate
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| (H2PO4)- | dihydrogen phosphate
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| (CO3)2- | carbonate
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| (HCO3)- | hydrogen carbonate
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| (ClO)- | hypochlorite
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| (ClO2)- | chlorite
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| (ClO3)- | chlorate
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| (ClO4)- | perchlorate
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| (C2H3O2)- | acetate
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| (MnO4)- | permanganate
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| (Cr2O7)2- | dichromate
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| (CrO4)2- | chromate
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| (O2)2- | peroxide
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| density | mass per unit of volume 1g/ml
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| element | simplest substance, only one type of atom
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| compound | 2 or more elements
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| molecule | smallest unit of chemistry compounds
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| mixture | mix of two or more substances
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| 3 states of matter | solid, liquid, gas
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| Dalton's atomic theory | 1)elements are made of atoms, 2)atoms of the same element are the same exact, 3)atoms cannot be created, subdivided or destroyed, 4)atoms from different elements can combine to compounds, 5)atoms are combined, separated, or rearranged in chemical reaction
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| valence electrons | the electrons in the outermost ring
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| core electrons | the combined electrons minus the outermost ring
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| period | horizontal rows in the periodic table
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| group | vertical rows on the periodic table
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| ion | charged particle
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| polyatomic ion | charged compound
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| cation | positive ion
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| anion | negative ion
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| 7 diatomic molecule symbols | H, N, O, F, Cl, Br, I, Hg
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| Hg^2+ | diatomic ion, called mercury 1
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| acids | when there is an "H" in a chemical compound
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| law of conservation of matter | matter cannot be created or destroyed
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| synthesis | reactants combine
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| sing;e-replacement | an element replaces another in the equation
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| double-replacement | 2 elements that replace each other in the equation
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| combustion | combine oxygen, carbon, and hydrogen
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| spectator ions | Same ions on both sides of an equation
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| avagadro's number | 6.022*10^23
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| empirical formula | simplest formula of atoms in a formula
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| molecular formula | shoes all the atoms in a formula
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| convert moles to grams | moles * weight
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| convert grams to moles | grams / weight
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| convert moles to molecules | moles * 6.022*10^23
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| convert molecules to moles | number of atoms / 6.022*10^23
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| theoretical yield | amount of product which is predicted in a reaction
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| experimental yield | amount is actually formed
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| percent yield | percent of the product formed
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| formula for percent yield | theoretical / actual
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| limiting reagent | reactant that is used up
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| endothermic reaction | energy is taken in
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| exothermic reaction | energy in given off
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| conservation of energy | idea that energy is not created or destroyed
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| equation to find the heat of an object | q=Mc^T
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| specific heat | amount of energy it takes to raise the temperature of 1 gram 1 degree Celsius
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| calorimeter | measures heat in a given liquid
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| Hess' Law | the change of reactants to a given product doesn't depend on the steps
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| calories=>joules | calories * 4.184
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| How much energy that goes into a calorimeter comes out of it? | none
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| group one | alkali metals
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| group 2 | alkali earth metals
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| group 3-12 | transition metals
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| group 17 | halogens
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| group 18 | noble gases
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| metalloids | properties of nonmetals and metals
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| lanthanides | upper section of the inner transition metals
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| actinides | lower section of the inner transition metals
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| 2 elements that are liquid at room temperature | mercury and bromine
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| the gold foil experiment was done by which scientist and it caused the discovery of what? | Rutherford, protons
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| km | kilometer
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| cm | centimeter
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| mm | millimeter
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| um | micrometer
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| n | nanometer
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| pm | picometer
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| kg | kilogram
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| cg | centigram
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| mg | milligram
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| ug | microgram
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| ng | nanogram
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| pg | picogram
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| measure distance | meter
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| measure mass | kilogram
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| measure volume | liters
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| measure time | second
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| gig- | 10^9
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| mega | 10^6
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| kilo | 10^3
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| centi | 10^-2
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| milli | 10^-3
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| micro | 10^-6
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| nano | 10^-9
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| pico | 10^-12
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| soluble | all nitrates, all NO3, group 1, NH4, (all Cl, Br, I except with(Ag, Hg2, Pb)), (all SO4, except with(Ba, Pb, Ca))
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| insoluble | S, CO3, PO4, (all OH except with(group 1, and Ca and down in group 2))
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| coefficients | the whole numbers in a balanced equations
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| subscripts | cannot be changed in a formula, or have atoms added or subtracted from it
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| soluble solid | to mean a solid that readily dissolves in water; the solid disappears as the ions are dispersed in the water
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| insoluble and slightly soluble solid | same thing; a solid where sure a tiny amount dissolves in water that it is undetectable with the naked eye
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| molecular equation | it shows the complete formulas of all reactants and products
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| complete ionic equation | molecular equation plus the ions of each substance
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| spectator ions | ions which do not participate directly in a reaction in solution
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| net ionic equation | includes only those components tat are directly involved in the reaction
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| acid | substance that produces H ions when it is dissolved in water
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| base | a substance that produces OH ions in water
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