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AP Chemistry Chapter 2 Flashcards

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10635835942John DaltonProposed that matter is composed of tiny particles called atoms. He postulated that all atoms of one element are the same but are different from atoms of another element. Atoms combine to form compounds.0
10635835943Wilhelm Rontgenphysicist who discovered X-rays1
10635835944JJ ThomsonShowed that cathode rays are streams of negative particles. He is credited with discovering the electron and measured its charge to mass ratio. He postulated that all atoms contain electrons.2
10635835945Robert MillikanMeasured the charge of an electron and calculated its mass.3
10635835946Henri Becquerelfrench physicist who discovered radioactivity in uranium4
10635835947Ernest RutherfordHe discovered the atomic nucleus and the proton and showed that atoms were mostly empty space - investigations in to the structure of the atomic nucleus - father of nucleur physics5
10635835948AtomsConsist of a tiny dense positively charged nucleus surrounded by a cloud of negative electrons. They are electrically neutral because each contains equal numbers of protons and electrons.6
10635835949NucleusContains positively charged protons and neutral neutrons.7
10635835950AnionsWhen atoms gain electrons to form negatively charged ions8
10635835951CationsWhen atoms lose electrons to form positively charged ions9
10635835952Atomic numberthe number of protons in the nucleus10
10635835953Elementa substance all of whose atoms contain the same number of protons. Each element is defined by its atomic number11
10635835954Mass numbernumber of protons and neutrons in the nucleus12
10635835955Isotopesatoms of identical atomic numbers but different mass numbers13
10635835956Atomic Mass Unitamu. One amu equals 1.66054 * 10^24g. It is more useful to compare the masses of atoms to the masses of one carbon-12 isotope. One C12 atom has a defined mass of exactly 12 amu.14
10635835957Atomic MassThe weighted average mass of all the isotopes of an element based on the abundance of each isotope found on earth. Atomic masses are expressed in amu. All atomic masses reported on the periodic table are based on the carbon 12 standard.15
10635835958Groups of familiesvertical column on the periodic table16
10635835959Periodshorizontal rows on the periodic table17
10635835960Alkali MetalsGroup 118
10635835961Alkali Earth MetalsGroup 219
10635835962HalogensGroup 1720
10635835963Noble GasesGroup 1821
10635835964Diatomic MoleculesA molecule made up of two atoms. 7 elements occur this way: Hydrogen, Nitrogen, fluorine, chlorine, bromine and iodine. (H, O, N, F, Cl, Br, I)22
10635835965Molecular Compoundcomposed of molecules and usually contain only nonmetals. A molecular formula indicates the actual number and type of atoms in the molecule and is the most often used formula for a molecular compound.23
10635835966Monatomic Ionssingle atoms24
10635835967Polyatomic Ionsaggregates of atoms25
10635835968Ionic Compoundsmade up of ions containing both metals and nonmetals26
10635835969Empirical FormulaGives the relative number of atoms or each type in the compound. Mainly used for ionic compounds.27
10635836009Potassium ion28
10635836010Calcium ion29
10635836011cobalt(II) ion30
10635836012Cobalt(III) ion31
10635835970Scandium ionSc3+32
10635836013Silver ion33
10635836014zinc ion34
10635836015Cadmium ion35
10635836016Tin(II) ion36
10635836017tin (IV) ion37
10635836018lead (II) ion38
10635836019lead (IV) ion39
10635835971Names of monoatomic anionsWhen an atom gains electrons, the end of the element name is replaced with -ide. ex. H- is hydride, O^2- is oxide.40
10635836020Hydroxide41
10635836021Cyanide42
10635836022Peroxide43
10635835972Names of polyatomic cationsWhen polyatomic cations form from nonmetals lose electrons, their new names end in -ium. ex. NH4+ is ammonium.44
10635835973OxyanionsPolyatomic anions ending in -ate, which also contain oxygen.45
10635836023Phosphate46
10635836024Hydrogen Phosphate47
10635836025Sulfate48
10635836026Carbonate49
10635836027Dihydrogen Phosphate50
10635836028Hydrogen sulfate51
10635836029Hydrogen carbonate52
10635836030Nitrate53
10635836031Acetate/ethanoate54
10635835974Oxyanions ending in -iterefers to oxyanions having the same charge but one fewer oxygen55
10635835975Hypochloritehypo denotes one fewer oxygen56
10635836032Chlorite57
10635836033Chlorate58
10635835976perchlorateper denotes one more oxygen59
10635836034Magnesium bromide60
10635835977Calcium phosphateCa₃(PO₄)₂61
10635836035Iron (III) Oxide62
10635836036Iron (II) oxide63
10635835978Hydrofluoric acidHF64
10635835979Hydrochloric acidHCl65
10635835980Hydrobromic acidHBr66
10635835981Hydroiodic acidHI67
10635836037Nitric acid68
10635836038Sulfuric acid69
10635836039Phosphoric Acid70
10635836040Acetic acid71
10635836041Hydrosulfuric acid72
10635836042Hydroselenic acid73
10635835982Carbonic acidH₂CO₃74
10635836043Nitrous acid75
10635835983Sulfurous acidH₂SO₃76
10635835984Perchloric acidHClO₄77
10635835985Chloric acidHClO₃78
10635835986Chlorous acidHClO₂79
10635835987Hypochlorous acidHCIO80
10635835988Naming binary acidsreplace the -ide ending of the anion with -ic acid and add the prefix hydro. ex. Bromide, Br-, becomes hydrobromic acid, HBr.81
10635835989Naming oxyacidsReplace the -ate ending of the oxyanion with the ic acid or the -ite ending of the oxyanion with the -ous acid. Examples include Nitrate, NO3-, become nitric acid, HNO3-, and hypochlorite, ClO-, becomes hypochlorous acid, HClO. Exceptions include Phosphate, PO4^3-, becomes Phosphoric acid, H3PO4, and sulfate, SO4^2-, becomes sulfuric acid, H2SO4.82
10635835990Naming binary molecular compoundsBinary molecular compounds contain 2 nonmetals. 1. Name the first element 2. Name the second element giving it an -ide ending 3. Use prefixes that denote how many of each element are in the formula83
10635835991Mono184
10635835992Di285
10635835993Tri386
10635835994Tetra487
10635835995Penta588
10635835996Hexa689
10635835997Hepta790
10635835998Octa891
10635835999Nona992
10635836000Deca1093
10635836001Hydrocarbonscompounds containing only carbon and hydrogen94
10635836002Alkaneshydrocarbons containing only C-C single bonds. For naming alkanes, the prefix indicates the numbers of carbons in the formula, and the -ane indicates it is an alkane.95
10635836003Functional Groupsgroups of atoms that give rise to the structure and properties of an organic compound. Examples include alcohols, -OH, and carboxyl acid, -COOH.96
10635836044Methanol97
10635836045Ethanol98
106358360461-propanol99
106358360472-propanol100
106358360041-butanolCH3CH2CH2CH20H101
106358360052-butanolCH3CH2CHOHCH3102
10635836006methanoicH2COOH103
10635836048ethanoic acid104
10635836007propane acidCH3CH2COOH105
10635836008butanoic acidCH3CH2CH2COOH106
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