General Chemistry 1 1st Quarter 1st Semester PDF

GENERAL CHEMISTRY 1 1st Quarter | 1st Semester 3. 999 = PRECISION AND ACCURACY 4. 8008 = ★ Accuracy - the closeness of the...

GENERAL CHEMISTRY 1 1st Quarter | 1st Semester 3. 999 = PRECISION AND ACCURACY 4. 8008 = ★ Accuracy - the closeness of the 5. 4.80 x10³ = measured value to a standard or true value ★ Multiplication/Division - determine the ★ Precision - the closeness of the one with the least significant figures. measurements to each other ★ Example: ○ 500N x 1.2m = 600Nm (1 sig) x (2 sig) = (1 sig) ○ 500.0N x 1.2m = 6.0 x10²Nm (4 sig) x (2 sig) = (2 sig) ○ 96.752 / 3.541 = 27.32 (5 sig) / (4 sig) = (4 sig) ★ Addition/Subtraction - determine the one with the least decimal places. ★ Example: ○ 200.5m + 150.255m + 201m = 551.755m ~ 552m SIGNIFICANT FIGURES (1 dec) + (3 dec) + (0 dec) = (0 dec) 1. All non-zero numbers ○ 2.36 + 12.1 = 14.46 ~ 14.5 2. Sandwiched zero (2 dec) + (1 dec) = (1 dec) ★ Example: 101, 501, 1001, 4009 ○ 1.27 - (-1.1) = 2.37 ~ 2.4 3. Trailing zero (with decimal point) (2 dec) - (1 dec) = (1 dec) ★ Example: 2.80, 1400.0, 0.660 Non-significant zero SCIENTIFIC NOTATION ★ Trailing zero (without decimal ★ The number between 1-10 times a power point) of ten. ○Example: 10000 (1 sig fig) ★ Example: / 1.0 x10⁴ (2 sig fig) / 1.00 ○ 0.0125 x10³ - not a scientific x10⁴ (3 sig fig) notation, so move a point ★ Leading zero (with decimal point) ○ 1.25 x10⁻² - it becomes -2 to have ○ Example: 0.0028 (2 sig the same value fig) / 0.0123 (3 sig fig) ○ 2.56 x10⁸ = 2.56000000 PRACTICE TEST ○ 4.6000 = 4.6 x10⁴ 1. 300 = 2. 14.60 =  GENERAL CHEMISTRY 1 1st Quarter | 1st Semester PROPERTIES OF SUBSTANCES PRACTICE TEST ★ Intrinsic Property - independent of the 1. You have a rock with a volume of 15 cm³ amount of material and a mass of 45 g. What is its density? ○ Specific gravity, Chemical properties, Malleability, Luster 2. What is the mass of the ethyl alcohol that exactly fills a 200.0 mL container? ★ Extrinsic Property - dependent on the The density of ethyl alcohol is 0.789 amount of material; easier to change g/mL. (can cut) ○ Mass, Volume, Length, Width, 3. What volume of silver metal will weigh Height, Radius, Texture exactly 2500.0 g. The density of silver is 10.5 g/cm³. DENSITY NAMING AND WRITING CHEMICAL ★ Mass per unit volume FORMULAS ★ Also known as (ρ) rho. NAMING CHEMICAL FORMULAS ★ Formula: ρ = M/V; M=ρV; V=M/ρ ★ If the chemical bond has hydrogen, then it is an acid. ★ Specific gravity - is to compare a ○ Binary acid - hydrogen is relationship between 2 substances bonded to a nonmetallic element 𝑑𝑒𝑛𝑠𝑖𝑡𝑦 𝑜𝑓 𝑠 ○ Specific Gravity = or a polyatomic ion without 𝑑𝑒𝑛𝑠𝑖𝑡𝑦 𝑜𝑓 𝑤 oxygen. EXAMPLE: Name: Hydro-___ acid 1. How many kg of gasoline are there in a 10.0m³ tanker? The density of gasoline ○ Oxy-acid - hydrogen is bonded is given by ρ = 719.7 kg/m³. to a polyatomic ion with oxygen. M = ρV Name: M = (719.7 kg/m³) (10.0m³) ___-ous acid (replace -ite) M = 7197 kg ___-ic acid (replace -ate) M = 7.20 x10³ kg (3 sig fig) 2. How much space will be needed by 7,200 metric tons of rice? The density of rice is given by ρ = 770 kg/m³. V = M/ρ 7,200 𝑡𝑜𝑛 1000 𝑘𝑔 V= 770 𝑘𝑔/𝑚³ × 1 𝑡𝑜𝑛 V = 9350.65 m³ V = 9400 m³ (2 sig fig)  GENERAL CHEMISTRY 1 1st Quarter | 1st Semester NAMING ACIDS ○ SnF4 - Tin (IV) fluoride HCl (g) Hydrogen Chloride ★ If the chemical bond consists of at least HCl (aq) Hydrochloric Acid one polyatomic ion (either cation or anion), do not change the name of the SO4-2 Sulfate polyatomic ion. Add Roman Numerals H2SO4 Sulfuric Acid at the end of the cation corresponding to its charge. HClO Hypochlorous Acid ★ Example: HClO2 Chlorous Acid ○ Ba(ClO2)2 - Barium chlorite ○ Pb(C2H3O2)2 - Lead (II) acetate HClO4 Perchloric Acid ○ (NH4)2C2O4 - Ammonium oxalate ★ If the chemical bond consists of both nonmetals, use prefixes (mono, di, tri, tetra, etc) and use -ide at the end of the anion. 1 - mono 6 - hexa 2 - di 7 - hepta 3 - tri 8 - octa 4 - tetra 9 - nona 5 - penta 10 - deca PRACTICE TEST ★ Example: 1. HI ○ NO - Nitrogen monoxide 2. H2SO3 ○ N2H4 - Dinitrogen tetrahydride 3. MgSO4 ○ P4O10 - Tetraphosphorus 4. FeSO4 decoxide 5. Al2O3 6. H3BO3 ★ If the chemical bond consists of a metal 7. FeBr3 cation and (a) a nonmetal or (b) another 8. SO2 metal anion, simply pair the name of the 9. KMn04 cation, and use -ide at the end of the 10. N2H4 anion. Add Roman Numerals at the end of the cation corresponding to its WRITING CHEMICAL FORMULAS charge. ★ Example: ★ Example: ○ Sodium Chloride: Na+1 Cl-1 = NaCl ○ LiBr - Lithium bromide (The goal is to have zero charge. ○ Fe2O3 - Iron (III) oxide the atoms must be equal to zero)  GENERAL CHEMISTRY 1 1st Quarter | 1st Semester ○ Magnesium Chloride: Mg+2 Cl-1 (2) = MgCl2 (Since the charges are 2 STEP BY STEP HOW TO GET THE TOTAL MASS and 1, it must equal to 0. So, the OF THE FORMULA: chloride charge was multiplied 1. Get the atomic mass by 2 for us to have zero) 2. Multiply how many atoms are there ○ Aluminum Oxide: Al+3(2)=+6 3. Add the elements O-2(3)=-6 = Al2O3 (Like magnesium chloride, both charges are ★ Example: Sulfuric Acid multiplied to have an equal value Step 1: H+1(2) = +2 S-2O-2 to zero.) Step 2: H2SO4 - Sulfuric Acid Step 3: PRACTICE TEST H=1x2=2 1. Ammonium Nitrate S = 32 x 1 = 32 2. Copper (II) Nitrate O = 16 x 4 = 64 3. Hypochlorous Acid Step 4: amu = 94 g/mol 4. Nickel (II) Chloride 5. Sodium Borate ★ Example: Sodium Phosphate 6. Perchloric Acid Step 1: Na+1(3) = +3 PO4-3 7. Sulfur Dioxide Step 2: Na3PO4 8. Copper Sulfide Step 3: 9. Nickel Phosphate Na = 23 x 3 = 69 10. Boronic Acid P = 31 x 1 = 31 O = 16 x 4 = 64 Step 4: amu = 164 g/mol FORMULA MASS ★ Atomic Number - whole number PRACTICE TEST because atoms are in a series 1. Fe2(SO4)3 ★ Mass Number - decimal number (but will 2. Nitrogen Hydrate be rounded off to whole number when 3. Potassium Permanganate computing) 4. NaSCN ★ amu = atomic mass unit or μ 5. Ammonium Chloride 6. Zn(ClO3)3 ★ Example: Hydrochloric Acid 7. Oxygen Gas Step 1: H+1Cl-1 8. Aluminum Perchlorate Step 2: HCl 9. PbSO4 Step 3: 10. Na3BO3 H-1x1=1 Cl - 35 x 1 = 35 ISOTOPIC SYMBOL Step 4: amu = 36 g/mol ○ Atomic Mass Neutrons = Atomic Mass - Atomic Number (Z) ○ Atoms per molecule  GENERAL CHEMISTRY 1 1st Quarter | 1st Semester ★ Example: C614 H= 2 × 100 = 2.04% 98 ○ 14 - Atomic Mass 32 ○ 6 - Atomic Number = No. of S= 98 × 100 = 32.65% protons 64 O= 98 × 100 = 65.31% = 100.00% ± 0.01 = 99.99 or Isotopic Atomic Atomic # of 100.01, tolerable Symbol Mass Number Neutrons (Z) ★ Example: (NH4)2SO4 N714 14 7 7 N = 14 x 2 = 28 H=1x8=8 Fe1226 26 12 14 S = 32 x 1 = 32 O = 16 x 4 = 64 Ba2656 56 26 30 amu = 132 g/mol PRACTICE TEST 28 N= 132 × 100 = 21.21 Isotopic Atomic Atomic # of 8 Symbol Mass Number Neutrons H= 132 × 100 = 6.06 (Z) 32 S= 132 × 100 = 24.24 Ar ? 18 22 64 O= 132 × 100 = 48.49 ? 51 ? 28 = 100.00% ± 0.01 = 99.99 or 100.01 Ga 70 ? 39 Mg 24 12 ? PRACTICE TEST 1. Mn2O3 ? 209 83 ? 2. CuCl2 3. Na2S PERCENT COMPOSITION 4. Cs2O 5. Fe2O3 𝑇𝑜𝑡𝑎𝑙 𝑚𝑎𝑠𝑠 × 100 MASS TO MOLE, MOLE TO MASS CONVERSION ★ If not whole number, round off to 2 decimal places MASS TO MOLE ★ Example: H2SO4 ★ Example: 16g of Oxegen Gas (O2) H=1x2=2 O2 = 16 x 2 = 32 g/mol S = 32 x 1 = 32 1 𝑚𝑜𝑙 O = 16 x 4 = 64 16g of O2 x 32𝑔 𝑜𝑓 𝑂₂ amu = 98 g/mol = 0.50 mol O2 ★ Example: 0.5g FeSO4  GENERAL CHEMISTRY 1 1st Quarter | 1st Semester Fe = 56 x 1 = 56 1 𝑚𝑜𝑙 𝑁₂ 2 𝑚𝑜𝑙 𝑁𝐻₃ 200.0 g N2 x x x S = 32 x 1 = 32 26 𝑔 𝑁₂ 1 𝑚𝑜𝑙 𝑁₂ O = 16 x 4 = 64 17 𝑔 𝑁𝐻₃ = 242.9 g NH3 1 𝑚𝑜𝑙 𝑁𝐻₃ amu = 152 g/mol 1 𝑚𝑜𝑙 𝐻₂ 2 𝑚𝑜𝑙 𝑁𝐻₃ 1 𝑚𝑜𝑙 200.0 g H2 x x x O.5g of FeS04 x 2 𝑔 𝐻₂ 3 𝑚𝑜𝑙 𝐻₂ 152𝑔 𝑜𝑓 𝐹𝑒𝑆𝑂₄ 17 𝑔 𝑁𝐻₃ = 3 x10-3 =0.003 mol of FeSO4 = 1133 g NH3 1 𝑚𝑜𝑙 𝑁𝐻₃ MOLE TO MASS CHEMICAL REACTIONS/PREDICTING ★ Example: 0.50 mol of HCl(aq) PRODUCTS H=1 Cl = 35 ★ Any metal combined with water will ` amu = 36 g of HCl(aq) produce metal hydroxide or base. ★ Any non-metal gas combined with water, 36 𝑔 𝑜𝑓 𝐻𝐶𝑙 will produce acid. 0.50 mol HCl(aq) x 1 𝑚𝑜𝑙 𝐻𝐶𝑙 = 18g HCl(aq) STEP-BY-STEP 1. Identify the type of reaction ★ Example: 2.0 mol NH4NO3 2. Write down the reactants N = 14 x 1 = 14 3. Use charge H=1x4=4 4. Balance the reaction N = 14 x 1 = 14 5. Predict the state of products O = 16 x 3 = 48 amu = 80 g of NH4NO3 ★ Examples: ★ MgO (s) + H2O (l) -> Mg(OH)2 (aq) 2.0 mol NH4NO3 x ★ SO2 (g) +H2O (l) -> H2SO3 (aq) 80 𝑔 𝑜𝑓 𝑁𝐻₄𝑁𝑂₃ ★ 2Al2O3 (s) + 6H2O (l) -> 4Al(OH)3 1 𝑚𝑜𝑙 𝑁𝐻₄𝑁𝑂₃ = 160 g of NH4NO3 SEPARATION TECHNIQUES FOR MIXTURES HABER PROCESS ｡ﾟﾟ･｡･ﾟﾟ｡ ★ Formula: N2 + 3H2 = 2NH3 ﾟ。 to be updated ★ Method used to create ammonia by ﾟ･｡･ﾟ reaction of Nitrogen and Hydrogen 2 𝑚𝑜𝑙 𝑁𝐻₃ ★ Mole Ratio: 1 𝑚𝑜𝑙 𝑁₂ ★ Example: Given: 200.0 g N2 / 200.0 g H2