SPCHEM 1ST QUARTER PDF

Lesson 1: Matters and its Properties 2. Distillation – purifies liquid mixture by using boiling points of its substance --------------------------PROPERTIES OF MATTER------------------------...

Lesson 1: Matters and its Properties 2. Distillation – purifies liquid mixture by using boiling points of its substance --------------------------PROPERTIES OF MATTER------------------------ Residue – higher boiling point 1. Physical Properties – determined/ measured Distillate without changing the chemical composition of matter - Volume, mass, density, boiling point, temp 2. Chemical Properties – only be measured by changing the chemical composition of the matter - Combustible, radioactivity, reactivity (𝐻2 𝑂 + 𝑂2) = rust 3. Filtration – separates solid from liquid using a porous material Intensive (intrinsic) – do not depend with the amount of matter but with the type - Temp, density, boiling point Extensive (extrinsic) – depend with the amount of matter 4. Evaporation – separates by allowing the liquid to evaporate and solid particle remain -----------------------PROPERTIES AND CHANGES---------------------- Ex. Salt farms 1. Physical change – only physical properties (no chemical composition) - Melting of ice, moist from the window 2. Chemical change – chemical composition is changed (process) - Changed when matter produced has different set of properties 5. Chromatography – separates component of a mixture by passing the mixture through stationary States of Matter phase 1. Solid Gas chromatography – separate gas 2. Liquid 3. Gas ------------CLASSIFICATION OF MATTER (composition)------------ 6. Use of Magnet – separate mixtures of magnetic and non-magnetic matter 7. Electrolysis – separate ------------METHODS AND TECHNIQUES IN SEPARATING----------- compounds like water 1. Decantation – separates using electricity undissolved solid from liquid Ex. Cooking rice  Lesson 2: Measurements ------COMMON MEASUREMENT AND UNIT CONVERSIONS------ Density – mass per unit volume Measurement – quantifies the characteristics of matter 𝑚 𝐷= - Compare to standard quantity (units) 𝑣 1. Given: SI Base Unit Base Quantity Name of Unit Symbol 𝑉 = 15 𝑐𝑚3 𝑚 = 45 𝑔 Length Meter m Mass kilogram kg Find: 𝐷 = ? Time Second s Solution: 𝑚 Electrical current Ampere A 𝐷= 𝑣 Temperature Kelvin K 45𝑔 Amount of substance Mole mol 𝐷= 15 𝑐𝑚3 Luminous intensity candela cd 𝐷 = 3𝑔 /𝑐𝑚3 ------------------------ACCURACY VS PRECISION------------------------ 2. Given: 𝑉 = 8 𝑐𝑚3 𝑚 = 40 𝑔 Find: 𝐷 = ? Solution: 𝑚 𝐷= 𝑣 40𝑔 𝐷= 8 𝑐𝑚3 -----------UNCERTAINTY AND ERROR IN MEASUREMENT---------- 𝐷 = 5𝑔 /𝑐𝑚3 Error – difference between “measured value” and “true value” Volume - 1000ml = 1L - 14.79mL = 1tbsp 1. Systematic errors – naturally occur, assume correct - 1mL = 1𝑐𝑚3 - 4.93mL = 1 tsp and accurate - 29.57mL = 1oz 2. Random errors – “human error” Temperature Uncertainty – quantification of the doubt about the C to F 9 𝐹 = 𝐶 + 32 measurement result 5 K to F 9 𝐹 = (𝐾 − 273.15) + 32 ---------------------LIMITATION IN MEASUREMENT-------------------- 5 K to C 𝐶 = 𝐾 − 273.15 Significant figures – reporting proper number of digits in F to C 5 measurement or calculation 𝐶 = (𝐹 − 32) 9 C to K 𝐾 = 𝐶 + 273.15 F to K 5 𝐾 = (𝐹 − 32) + 273.15 9 -----------------------------------RULES--------------------------------------- Lesson 3: Compositions of Matter 1. Any nonzero – significant Ex. 12345(5), 98(2), 854879(6) -----------------ATOMIC MODEL & THEORY TIMELINE---------------- 1. Democritus – matter is divided into smaller pieces 2. Any zeroes between nonzero digits – significant forever Ex. 10005(5), 2005406(7), 2000001(7) - “atom” 3. Zeros at the end w/o decimal – not significant 2. John Dalton – first atomic theory Ex. 34000(2), 10000(1), 34.500(5) - “atom” – tiny, solid balls 4. Zeros at the beginning of decimal number – not 3. JJ. Thompson – atom was made smaller things significant - “Raisin bun model” Ex. 0.03(1), 0.0004(1), 0.0090(2)  4. Ernest Rutherford – protons & nucleus ATOM – basic unit of an element that can enter to chemical - Atoms have (+) particles in the center and combination mostly empty space - Internal structure - Subatomic particles 5. Niels Bohr – electrons move around the nucleus in o Proton (𝑝+ ) shells o Electron (𝑒 − ) Erwin Schrodinger – Quantum Mechanical o Neutron (𝑛0 ) Model (orbitals) 6. James Chadwick – with Rutherford 𝑝+ = 𝑒 − - Particles w/ no charge (neutrons) --------------------------REPRESENTING AN ATOM---------------------- 7. Modern – electrons moving around nucleus in a Nuclide – atomic number and mass number cloud ------------------DALTON’S ATOMIC THEORY (1808)------------------- Atoms – elements composed of extremely small particle - Identical (size, mass, and chemical properties) - Atom of 1 element differ from another Atomic number (z) – number of protons (identity) in the nucleus of each atom of an element Compounds – composed of atoms more than 1 element 3𝑝+ = 𝐿𝑖 - Relative number of atoms of each element in a given compound is the same Neutral atom – number of protons = number of electrons - Ground state atoms Chemical reaction – rearrangement of atoms - Not created/ destroyed Mass Number (A) – mass of an atom - amu (atomic mass unit) -----------------------------------LAWS--------------------------------------- - number of protons + number of neutrons 1. Law of Definite Proportion Joseph Proust (1754 - 1826) – same compound IONS – an atom/ group of an atom (with + and – net charge) always the same proportion by mass - number of protons are the same after process Ex. Water – 11% H, 89% O → 18g of water = 1.98g H, 16.02g O 𝑝+ ≠ 𝑒 ↑↓ 2. Law of Multiple Proportion a. Cation – positive - 2 elements combine to form more than 1 compound - Loses electrons - Masses of 1 element that combine with a fixed mass of other element are in ratios of small whole b. Anion – negative numbers - Gain electrons Ex. 27 3+ 13𝐴𝑙 𝑝+ = 13 𝑒 − = 10 (13 − 3) (cation) 𝑛0 = 14 78 34𝑆𝑒 2− 𝑝+ = 34 𝑒 − = 36 (34 + 2) (anion) 𝑛0 = 44 3. Law of Conservation of Mass - Total mass of substance present at the end of chem Monoatomic Ion – only 1 atom process is the same as the mass of substances before 𝑁𝑎+ , 𝐶𝑙 − , 𝐶𝑎2+ , 𝑂2− , 𝐴𝑙 3+ , 𝑁 3− the process Ex. 1.00g H + 8.00g O = 9.00𝐻2 𝑂 Polyatomic Ion – more than 1 atom 4.03 MgO – 2.43g Mg = 1.6g O 𝑂𝐻 − , 𝐶𝑁 − , 𝑁𝐺4 +  ISOTOPES – defined by the number of protons Diatomic Molecule – 2 atoms - Different mases 𝐻2 , 𝑁2 , 𝑂2 , 𝐵𝑟2 , 𝐹2 , 𝐼2 , 𝐶𝑙2 , 𝐶𝑂, 𝐻𝐶𝐼 - Different number of neutrons Polyatomic Molecule – more than 2 atoms 𝑂3 , 𝐻2 𝑂, 𝑁𝐻3 , 𝐶𝐻4 Lesson 4: Electronic Structure of Atom and Electron Configuration *Unstable = radioactive decay 1. Bohr’s Atomic model 2. The Dual Nature of Electron (Louis de Broglie) Ex. 3. The concept of quantum H-1 𝑝+ = 1 𝑒− = 1 𝑛0 = 0 4. Heisenberg’s Uncertainty Theory H-2 𝑝+ = 1 𝑒− = 1 𝑛0 = 1 H-3 𝑝+ = 1 𝑒− = 1 𝑛0 = 2 Quantum number 1. Principal number – floor number Fractional abundance – fraction of total number of atoms 2. Azimuthal/ Angular – rooms that is composed of an isotope 3. Magnetic (“orbital”) – number of beds (2 only) 1 1 4. Spin – only 2 (+ 2 , − 2) Ex. Isotopic Mass Fractional Abundance 49.9461 0.0435 2.17 51.9405 0.8379 43.52 52.9407 0.0950 5.029 53.9389 0.0236 1.27 Cr = 51.989 amu S p d f g h --------------COMMON ISOTOPES AND THEIR USES------------------ 2 6 10 14 18 Radioactive Isotopes Applications in Medicine Quantum number 1. Cobalt-60 Radioactive therapy for cancer n l ml # of Orbital # of 2. Iodine-131 Brain tumors, cardiac liver, and orbital name electrons thyroid 1 0 0 1 1s 2 3. Carbon-14 Diabetes, gout, and anemia 4. Carbon-11 Glucose monitors during PET scan 2 0 0 1 2s 2 5. Sodium-24 Blood circulation 1 -1, 0, +1 3 2p 6 6. Thallium-201 Heart tissue and tumors 7. Technetium-99m Brain tumors, heart cells, radiotracer 3 0 0 1 3s 2 1 -1, 0, +1 3 3p 6 Radioactive Isotopes Industrial Applications 2 -2, -1, 0, +1, +2 5 3d 10 1. Americium-241 Rolling steel and paper, oil wells 2. Sodium-24 Oil well, leaks in pipe lines 4 0 0 1 4s 2 3. Iridium-192 Boilers and aircraft parts 1 -1, 0, +1 3 4p 6 4. Uranium-235 Nuclear power plant, fuel, fluorescent 2 -2, -1, 0, +1, +2 5 4d 10 glassware and wall tiles 3 -3, -2, -1, 0, +1, +2, +3 7 4f 14 5. Californium-252 Moisture content of soil, road and bldgs. 5 0 0 1 5s 2 1 -1, 0, +1 3 5p 6 MOLECULES – aggregate of 2 or more atoms in a definite 2 -2, -1, 0, +1, +2 5 5d 10 arrangement held together by chemical bonds (molecule vs 3 -3, -2, -1, 0, +1, +2, +3 7 5f 14 compound) 4 -4, -3, -2, -1, 0, +1, +2, +3, +4 9 5g 18 - Neutral - May contain atoms of the same element/ atoms of 2 or more elements joined in a fixed ratio -----------------RULES IN ELECTRON CONFIGURATION--------------- c. Orbital Diagram 1. Aufbau Principle 1. Li = 3 – paramagnetic 2. Hund’s Rule 3. Pauli Exclusion Principle *Exemption to Aufbau Principle: EC ending in d4, d9, f6, f13 2. Ag = 47 – paramagnetic 3. Mn = 25 – paramagnetic 4. Al+3 = 10 – diamagnetic Electron Configuration a. Longhand 1. Li = 3 1𝑠 2 2𝑠1 2. Ag = 47 1𝑠 2 2𝑠1 2𝑝6 3𝑠 2 3𝑝6 4𝑠 2 3𝑑10 4𝑝6 5𝑠1 4𝑑10 3. Mn = 25 1𝑠 2 2𝑠1 2𝑝6 3𝑠 2 3𝑝6 4𝑠 2 3𝑑 5 4. Al+2 = 10 1𝑠 2 2𝑠1 2𝑝6 Valence electron – highest principal the electron occupied 1. 1 2. 1 3. 2 4. 8 b. Shorthand 1. 𝐿𝑖 = [𝐻𝑒] 2𝑠1 2. 𝐴𝑔 = [𝐾𝑟] 5𝑠1 4𝑑10 3. 𝑀𝑛 = [𝐴𝑟] 4𝑠 2 3𝑑 5 4. 𝐴𝑙 +3 = [𝑁𝑒] 3𝑠 2 3𝑝1