Chemistry 11 Midterm Review

Name: ___________________ Chemistry 11 Chemistry 11 (Midterm Review) Block: _________ Midterm Review Unit 1.1 – 1.8 Review Write the chemical name or formula for the given formula. Classify the compound as an Acid, Base, Hydrate, Ionic, or Covalent Compound FORUMLA 1) CoF3 2) PBr5 3) KMnO4 4) FeC2O4 5) HNO3 (aq) 6) Sn(CN)2 7) LiOH 8) Na2HPO4 9) Cu(NO3)2•6H2O 10) NH4NO3 11) N2S5 12) CuSO4 13) V2O5 14) Ni3(PO4)2•8H2O 15) H3PO4 (aq) 16) S4N2 17) CS2 18) W(CN)3 TYPE I NAME Cobalt (III) Fluoride C Phosphorus Pentabromide I Potassium Permanganate I Iron (II) Oxalate A Nitric Acid I Tin (II) Cyanide B Lithium Hydroxide I Sodium Hydrogen Phosphate H Copper (II) Nitrate Hexahydrate I Ammonium Nitrate C Dinitrogen Pentasulfide I Copper (II) Sulfate I Vanadium (V) Oxide H Nickel (II) Phosphate Octahydrate A Phosphoric Acid C Tetrasulfur Dinitride C Carbon Disulfide I Tungsten (III) Cyanide Name: ___________________ Chemistry 11 (Midterm Review) A 19) H2S (aq) NAME 1) chlorine tetroxide Block: _________ TYPE C 2) chlorine tetroxide C 3) iron (III) hydroxide B 4) radium carbonate I 5) hydrobromic acid A 6) disilicon hexaiodide C 7) sulfurous acid A 8) chromium (II) oxalate I 9) zinc (II) carbonate tetrahydrate H 10) dinitrogen pentoxide C 11) tungsten (V) bromide I 12) tin (II) bicarbonate I 13) mercury (I) nitrate I 14) copper (I) phosphate I 15) sulfuric acid A 16) beryllium oxide I 17) molybdenum(VI) iodide I 18) ammonia C Hydrosulfuric Acid FORMULA ClO4 ClO4 Fe(OH)3 RaCO3 HBr Si2I6 H2SO3 CrC2O4 ZnCO3 • 4H2O N2O5 WBr5 Sn(HCO3)2 Hg2(NO3)2 Cu3PO4 H2SO4 BeO MoI5 NH3 Balancing Equations and Reaction Types Review Using the different types of reactions (Synthesis, Decomposition, Single Replacement, Double Replacement, Neutralization, and Combustion) predict the products and balance the equation. 1) ___ H3PO4 + _3_ KOH → ___ K3PO4 + ___ H2O Type of Reaction: ____________ Neutralization____________ 2) _2_ C2H2 + _5_ O2 → _2_ H2O + _4_ CO2 Type of Reaction: _____________Combustion________________ Name: ___________________ Chemistry 11 (Midterm Review) Block: _________ Exothermic and Endothermic Reactions 1. Draw a diagram of an Exothermic and Endothermic Reaction. Label the Reactant, Products, Enthalpy Change (∆H), and Activation Energy (Ea) ENDOTHERMIC EXOTHERMIC 2. List the following Reactions as Exothermic or Endothermic: a. 2H2O2(l) → 2H2O(l) + O2(g) + 200kJ Answer: ____Exothermic___ b. Mn(s) + 2 HCl(aq) → MnCl2(aq) + H2(g) + 221 kJ Answer: ____Exothermic___ c. 2 N2O5 (g) + 110 kJ → 4NO2(g) + O2(g) Answer: ___Endothermic__ d. P4O10(g) + 6H2O(l) → 4 H3PO4(aq) + 424 kJ Answer: ____Exothermic__ Atomic Structure and Periodic Trends: 1. Which atom is bigger: Bi or P? Why? Bi – electrons fill up the higher energy level orbitals which makes the atomic radius much larger 2. Complete the following table: Atom/Ion Atomic # Mass # a) 39 b) 41 Protons Neutrons Electrons K+1 19 39 19 20 18 Ca 20 41 20 21 20 Ga+3 31 69 31 38 28 Cl-1 17 37 17 20 18 O 8 18 8 10 8 U+4 92 235 92 143 88 c) 69 d) 37 e) 18 f) 235 3. Naturally occurring silver consists of 51.8% Ag-107 and 48.2% Ag-109. What is the average atomic mass (AAM) of a sample of natural silver, expressed to 3 decimal places? AAM = (107 amu)(0.518) + (109 amu)(0.482) = 107.964 amu Name: ___________________ Chemistry 11 (Midterm Review) Block: _________ 4. Write the electron configuration and core notation for the following: a. P Electron Configuration: ____1s2 2s2 2p6 3s2 3p3_________ Core Notation: _________[Ne] 3s2 3p3________________ b. F- Electron Configuration: ________1s2 2s2 2p6 ___________ Core Notation: ____________[Ne] or [He] 2s2 2p6 _______ c. Pd Electron Configuration: __1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d8 _ Core Notation: ________________[Kr] 5s2 4d8 ______________ d. Se Electron Configuration: ____1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4 ___ Core Notation: ___________[Ar] 4s2 3d10 4p4 _______________ e. S2- Electron Configuration: ____1s2 2s2 2p6 3s2 3p6____________ Core Notation: ______[Ar] or [Ne] 3s2 3p6 ___________ 1. Draw the energy level diagrams for: Mg P3- S- 2. Name the corner of the periodic table would have the largest of the following trends. Explain why. a. Atomic Size/Radius _____Bottom Left Corner_____ b. Electronegativity _____Top Right Corner_______ c. Ionization Energy _______Top Right Corner_____ Name: ___________________ Chemistry 11 (Midterm Review) Block: _________ 3. Circle the metalloid: Be Rb Os Ge Pb Al 4. Circle the most reactive element in the following: Na Mg Si Al Ar 5. Circle the element with the largest atomic radius of these: Na Mg Si Al Ar 6. Circle the element with the largest atomic radius of these: N P As Sb Bi 7. Circle the element with the largest ionization energy of these: C Si Ge Sn Pb 8. Define ionization energy? • Ionization Energy: The amount of energy needed to remove the outermost electron 9. Circle the element with the highest electronegativity of these: F Cl Br I 10. Define electronegativity? • Electronegativity: Tendency of an atom to attract electrons from a neighboring atom Lewis Structures and Bonding: 1. With respect to electronegativity, how does an ionic bond differ from a covalent bond? Non-polar covalent Bond - electronegativity difference between 0 – 0.4 Polar Covalent Bond - electronegativity difference is between 0.5 – 1.6 Ionic Bond – electronegativity difference is greater than 1.7 2. Indicate whether the following compounds are ionic, non-polar covalent, or polar covalent: Explain why. a. NaCl – Ionic bond (metal + non-metal) – electronegativity difference = 2.1 b. H2O – Covalent bond (non-metal + non-metal) c. NO2 – Covalent bond (non-metal + non-metal) d. CS2 – Covalent bond (non-metal + non-metal) 3. Out of CaO, NaCl, NaF, and LiF, which would have the highest melting point? Why? CaO has the highest melting point – it has a stronger ionic bond 4. List the number of valence electrons for: a. Si __4__ c. Ne + b. K __8__ d. O2- __8__ __8__ e. H-1 f. N __0__ __5__ Name: ___________________ Chemistry 11 (Midterm Review) Block: _________ 5. Which intermolecular force is responsible for the fact that H2Se has a higher boiling point than H2S? Explain how. Se has a larger atomic radius than S, therefore Se will have a stronger Dipole-Dipole force and greater London forces 6. Which intermolecular force is responsible for the fact that H2O has a higher boiling point than H2S? Explain how. H2O will have Hydrogen Bonding and H2S will not - See section [4.1] 7. What is considered the weakest intermolecular force? Why? London Forces – they are only a temporary intermolecular force 8. How can you tell if a molecule is polar or non-polar? Check the electronegativity difference (ΔEN) or by drawing the molecule to check the symmetry 9. Write the intermolecular forces from strongest to weakest. London Forces < Dipole-Dipole < Hydrogen Bonding 10. What is the ΔEN and say the type of bond for the following: 1. Na-Br 2. CS2 Name SiO2 ΔEN = __1.9_ Bond-Type:__ Ionic___ ΔEN = __0__ Bond-Type: NonPolar __ 2D Lewis Structure Bonds: Ionic, Polar, or Non Polar Overall molecule: Ionic, Polar, NonPolar Bonds Si-O bond = Polar (ΔEN=1.7) Molecule Overall molecule = NonPolar (symmetrical) NH3 BCl3 3. H-F ΔEN = __1.9_ Bond-Type:_Polar 4. Ca-F ΔEN = __1.9_ Bond-Type:__Ionic Types of Intermolecular Forces (LD/DD/HB) Shape Name Forces London Forces Shape Linear Bonds N-H bond = Polar (ΔEN=0.9) Forces London Forces Hydrogen Bonding Molecule Overall molecule = Polar (Non symmetrical) Shape Trigonal Pyramidal Bonds B-Cl bond = Polar (ΔEN=1.0) Forces London Forces Molecule Shape Trigonal Planar Overall molecule = NonPolar (symmetrical) * * Exception 3-D Structure Name: ___________________ Chemistry 11 (Midterm Review) H2O Bonds Forces O-H bond = Polar London Forces Hydrogen Bonding (ΔEN=1.4) SF4 Block: _________ Molecule Overall molecule = Polar (Non symmetrical) Shape Angular / Bent Bonds S-F bond = Polar (ΔEN=1.5) Forces London Forces Dipole-Dipole Molecule Overall molecule = Polar (Non symmetrical) Shape Trigonal Bipyramidal / Seesaw 11. Given the following graph of Temperature vs. Time for warming substance “X” which starts out as a solid, answer the questions below: Temperature oC 90oC Gas Boiling Point 77oC Liquid Melting Point 43oC Solid 15oC 0.0 5.0 15.0 20.0 Time (minutes) 28.0 a) During time 0.0 – 5.0 minutes, the added heat energy is being used to _________________Heat up / add energy to the solid _____________ b) During time 5.0 – 15.0 minutes, the added heat energy is being used to _______Change from a solid to a liquid (melting point - fusion)____ c) During time 15.0 – 20.0 minutes, the added heat energy is being used to __________________ Heat up / add energy to the liquid__________ d) During time 20.0 – 28.0 minutes, the added heat energy is being used to ______ Change from a liquid to a gas (Boiling Point - vaporization)__ e) The melting point of substance “X” is _______43 oC___________ f) The boiling point of substance “X” is _______77 oC____________ Name: ___________________ Chemistry 11 (Midterm Review) Block: _________ Solutions Chemistry 1. Why are some solvents polar and some non-polar? Which would you use to dissolve salt? As like dissolve like , polar compound is soluble in polar solvent and non polar compound in non polar solvent. NaCl is ionic compound and it can be soluble in only that solvent which can dissociate it into its components. [Na]+[Cl]- will dissolve in a polar solvent due to the charges on the ionic compound. 2. Which of the following would you except to form conducting (“ionic”) solutions when added to water, and which would form non-conducting (“non-ionic”) solutions? (a) KI (b)HBr (c)CH4 (d)CsF (e) H2CO3 (f)ICl (g)CaBr2 (h)CH3COOH 3. Which of the following conduct electricity? (a)HCl(aq) (b)Ag(s) (c)BaBr2(aq) (d)LiCl(s) (e)CO2(s) (f)LiOH(l) (g)C14H10(l) (h) CH3COOH(l) 4. Which should melt at a higher temperature? Why? (a) He or Xe (b)F2 or Br2 Why: Electrons further from Nucleus (c)CH4 or CH3F Why: Electrons further from Nucleus (e)HI or HCI (d) HBr or Kr Why: Polar (f)H2O or H2Te (g) CH3-CH3 or HO-CH2CH2-OH Why: Hydrogen Bonding Why: Stronger London Forces 5. Calculate the molarity of 0.289 moles of FeCl3 dissolved in 120 ml of solution? Answer: 𝑀= 𝑛 𝑉 = 0.289 𝑚𝑜𝑙 0.120 𝐿 = 2.41 𝑚𝑜𝑙 𝐿 6. If a 0.075 liter solution contains 0.0877 moles of CuCO3, what is the molarity? Answer: 𝑀= 𝑛 𝑉 = 0.0877 𝑚𝑜𝑙 0.075 𝐿 = 1.17 𝑚𝑜𝑙 𝐿