Chapter 1 CHM 1045 FINAL REVIEW CHS 1 3 Chemistry is the study of matter and the changes it undergoes Scientific Method a systematic approach to research o Types of data collected Qualitative general observations found in the experiment Quantitative numbers that are obtained by measure during the experiment Hypothesis tentative explanation for a set of observations Law concise verbal or mathematical statement of a relationship between phenomena that is always the same under the same conditions Matter something that occupies or has space o Element cannot be separated o Compound atoms made up of two or more elements that are chemically united in fixed proportions Intensive does not depend on how much matter there is Extensive depends on how much matter there is Solid Liquid Gas o Physical Mixture substance o Chemical compound element Physical property done without changing the composition or identity of the substance o Ex melting point boiling point Chemical property must carry out a chemical change o Ex burning something a boiled egg inside starts as watery ends in a solid state SI Base Units o Length m o Mass kg o Time s o Electrical current A o Temperature K o Amount of a substance mol o Luminous intensity cd Basic conversions o 1kg 1000 g or 1x10 3g o 1 g cm 3 1 g mL o 1000 kg m 3 1 g L 001 g mL Temperature conversions o C F 32F x 5C 9F o F 9F 5C x C 32F o K C 273 15 density mass volume o volume length 3 Scientific Notation Nx10 n o Add or subtract write N1 and N2 with the same exponents then combine The exponents stay the same o Multiplication multiply N1 and N2 then add the exponents o Division divide N1 and N2 then subtract the exponents Significant figures meaningful digits o Addition or subtraction the number cannot have more digits to the right of the decimal than either of the original numbers o Multiplication or division the final answer has the number of significant figures that the original number that has the smallest number of significant figures Accuracy how close to the real value Precision how closely two or more measures of the same quantity agree with Convert between units when solving chemical problems by using dimensional one another o Less deviation analysis Conversion factors o 1 in 2 54 cm 2 54 cm 1in 12in x 2 54cm 1 in 30 48 cm Chapter 2 properties Elements extremely small particles called atoms same size mass chemical o Subatomic particles smaller than atoms Compounds atoms of more than one element o Chemical reaction separation combination or rearrangement of atoms not the creation or destruction Laws of conservation of mass matter can be neither created nor destroyed Negatively charged particles electrons o 1 76 x 10 8 c g o Charge of electron 1 6022 x 10 19 c o Mass of e 9 10 x 10 28 g Radiation and radioactivity o Alpha ray positively charged particles a particles o Beta rays electrons that are deflected by a negatively charged plate b o Gamma rays radioactive radiation that consist of high energy rays no particles charge Positively charged particles protons o Mass of proton 1 672 x 10 24 g 1840 times the mass of an electron o 1 6022 x 10 19 c neutrons neutral particles with mass slightly greater than a proton Atomic number number of protons in the nucleus of each atom Mass number total number of neutrons protons present in the nucleus of an o Mass number number of protons number of neutrons o Mass number atomics number number of neutrons o Number of neutrons mass number atomic number Isotopes atoms that have the same atomic number but different mass numbers atom Periodic table o Metal Good conductor o Nonmetal o Metalloids Poor conductor o Horizontal periods o Vertical groups Cation net positive charge Has properties of both metal and nonmetal o Lose an electron to become Anion net negative charge o Gain an electron to become Ionic compound formed from cations and anions Monoatomic ion only one atom Polyatomic contains more than one ion Chemical formulas written in terms of chemical symbols o Molecular exact number of atoms of each element o Allotrope 1 or 2 or more distinct forms of elements o Structural formula shows how atoms bonded to one another in the o Empirical formula tells us which elements are present and the simplest molecule whole number ration Organic compounds contain C usually in combination with elements o Ex H O N S ALL others are inorganic compounds Binary compounds formed from 2 elements Ternary 3 elements ide for binary molecular compounds prefixes for second element o mono o di o tri o etc o ends in ide o hydro prefix and ic HCl HCl acids substances that yield H when dissolved in water Hydrogen chloride hydrochloric acid o Oxoacids contain H O and another element Ex HClO chloric acid Oxoanions anions and oxoacids o H3PO4 phosphoric acids o H2PO4 dihydrogen phosphate o HPO4 2 hydrogen phosphate o PO4 3 phosphate Hydrates have a specific number of H2O molecules attached o 7 H2O heptahydrate o 2 HO dehydrate hydrocarbons H and C only o alkalines Chapter 3 Atomic mass the mass of one atom in amu o one amu a mass 1 12 mass of 1 carbon 12 atom o carbon 12 6 protons 6 neutrons The mole mol is the amount of a substance that contains as man atoms molecules or other parts as thwew are atoms of exactly 12 g of thee C 12 isotope Avogadro s number 6 0221415 x10 23 atoms o The mass of carbon 12 is it molar mass 1 mole of units of a substance 12g carbon 12 atoms 6 022x10 23 carbon 12 atoms 1 993x10 23 g o Carryout conversions between the mass and moles of atoms and between moles and number of atoms 1 mol X molar mass X 1 mol X 6 022 x 10 23 X atoms Molecular mass the sum of the atomic masses in the molecule o Molar mass g numerically molecular mass amu Collisions between electrons and gaseous atoms ions o By dislodging an electron from each atom or molecule Percent composition by mass percent of each element in a compound o Percent compound of element n x molar mass element molar mass compound x 100 Empirical formula o Chemical analysis tells the number of grams in each element of a given compound o Convert quantities in grams to number of moles Ex CO2 and H2O Mass C 22g CO2 x 1 mol CO2 44 01g CO2 x 1 molC 1 mol CO2 x 12 01 g C 1 mol C 6g C Mass H 13 5 g H20 x 2 mol H 1 mol H20 x 1 008 g H 1 mol H 1 51 g H Mass O 11 5 6g 1 51g 4g O Chemical reaction process in which a substance is changed into 1 or more substances o Chemical equation uses chemical symbols to show what happens during a chemical reaction H2 O2 H2O o …
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