Chem 11 Exam Preparation

Transcription

1 Chem 11 Exam Preparation Format: You won t be surprised it looks like a longer version of your quizzes Part A: Multiple Choice without calculations. 60 questions worth ½ pt each. 30 points total. Part B: Multiple Choice with calculations. 20 questions worth 1 pt each. 20 points total. Part C: Problem Section. Each problem is made up of a mix of questions. Do 5 problems worth 10 points each. 50 points total. To prepare for the problem section, look at the problem sections from the three unit tests. Here is a list of topics found in the problem section of past exams: Average atomic mass Molar conversions (Particle/moles/mass/volume) % Composition Empirical Formula Molecular Formula Hydrate Stoichiometric Mass to Mass Problem Limiting Reactant Bond types Lewis Diagrams Intramolecular forces (covalent, ionic and metallic bonds) and properties Intermolecular forces and properties (ex. Melting and boiling points) Drawing and naming alkanes, alkenes, alkynes, cyclic hydrocarbons, benzene, and hydrocarbon derivatives including alcohols and compounds with chloro and bromo groups. Substitution reactions of alkanes Complete and incomplete combustion of any hydrocarbon Addition reactions of alkenes and alkynes. Markovnikov s Rule Find the average atomic mass for chromium from the data provided.

2 A sample of platinum, Pt, contains (8.43)(10 25 ) atoms. How many moles of platinum are present? The simple sugar glucose has the chemical formula C 6H 12O 6. (a) How many molecules of glucose are present in mol of this sugar? (b) What is the mass of mol of glucose? (c) How many molecules of glucose are present in a mg sample? (d) How many hydrogen atoms are in a mg sample? Find the molar mass of ammonium sulfide,(nh 4) 2S. The gem, garnet, has the chemical formula, Ca 3Al 2(SiO 4) 3. How many atoms of aluminum are in a piece of garnet having a mass of g? What is the volume of 4.92 mol of helium gas at STP? Which sample occupies at greater volume at STP? (a) 30.0 g of CH 4 or (b) molecules of H 2? Analysis of 24.1 g of calcium oxide revealed that it contained 17.2 g of calcium. What mass of this compound would contain 60 g of calcium? A compound of chromium and oxygen is 68.4% Cr and 31.6% O. What is its empirical formula? A 3.00 g sample of CoC1 2 xh 2O was heated and after the water was driven off, 1.64 g of CoC1 2 remained. Find the value of x. The poison coniine can be recovered from the hemlock plant. A g sample of this compound contains g of carbon, g of hydrogen, and the remainder is nitrogen. The molar mass of this compound is g/mol. Determine the molecular formula of coniine. What volume of H 2(g) will be produced at STP when 4.28 g of calcium metal reacts with water as shown by the following equation. Ca (s) + 2H 2O (l) Ca(OH) 2(aq) + H 2(g)

3 The following single displacement reaction occurs when the solid mixture of aluminum and manganese are heated. 2Al (s) + 3MnO (s) Al 2O 3(s) + 3Mn (s) What mass of manganese solid will be produced when g of Al (s) and g of MnO (s) are allowed to react? For each set of atoms listed, use a Lewis structure to illustrate how they can combine by sharing electrons to form a compound. (a) 2 carbon atoms and 6 hydrogen atoms (b) 2 carbon atoms, 4 hydrogen atoms, and 2 fluorine atoms (c) 2 carbon atoms, 4 hydrogen atoms and one oxygen atom (d) 1 carbon atom, 1 hydrogen atom, and 3 chlorine atoms Use the table of electronegativities listed in the student textbook to predict whether the bond formed between each pair of atoms will be non-polar covalent, polar covalent, or ionic. (a) Cs and O (b) Fe and N (c) H and Br (d) Ag and S, (e) O and Cl Polar covalent bonds are caused by (a) the donation of a pair of electrons by one atom (b) the unequal sharing of a pair of electrons (c) the union of atoms of the same electronegativity (d) the complete transfer of electrons from one atom to another (e) the equal sharing of electrons Which of the following best explains metallic bonding? (a) Metal atoms are covalently bonded to one another. (b) Metals have the ability to form both anions and cations; these form ionic-type bonds (c) Metallic bonds involve an attraction between metal anions and a sea of mobile valence electrons. (d) Metallic bonds involve an attraction between metal cations and a sea of mobile valence electrons. (e) Metallic bonds involve an attraction between metal cations and the nuclei of nearby atoms. Draw an electron dot (Lewis) diagram for each of the following. (a) Al (b) CaF 2

4 (c) a compound in which two oxygen atoms are bonded to each other and one hydrogen atom is also bonded to each oxygen (d) a compound in which 2 C atoms are bonded to one another. Each carbon atom is also bonded to two hydrogen atoms. (e) a carbon atom is bonded to a hydrogen atom and to a nitrogen atom. Which of the following in the liquid state is expected to be the best conductor of electricity? (a) CCl 4 (b) CaF 2 (c) I 2 (d) CS 2 Which of the following compounds in liquid state has the strongest hydrogen bonding? (a) PH 3 (b) CH 4 (c) NH 3 (d) H 2S Indicate which of the following molecules are polar and which are non-polar. (a) CO 2 (c) CH 3OH (d) CH(OH)O (e) PCl 3 (f) CCl 4 Predict the shape of the following molecules. (a) NF 3 (e) PCl 3 (f) CHCl 3 Determine the intermolecular forces for following molecules. (a) NF 3 (e) PCl 3 (f) CHCl 3 (a) CO 2 (d) HCl + Cl 2 You melt ice by heating it to 0 0 C. You melt NaCl by heating it to C.Why does salt have the higher melting point? Draw the condensed structural diagram and then name each of the following molecules represented by a line structural diagram Name the compounds that are represented below. (a) CH 3(CH 2) 4CH 3 (b) (CH 3) 2CHCH 2CH 2CH(CH 3) 2 (c) (CH 3) 4C

5 Draw condensed structural diagrams and line structural diagrams for the following molecules: (a) 3-ethyl-4-methyl-1-octene (b) 4-propyl-3-methyl-1-heptyne (c) 5-ethyl-2,3-dimethylheptane Use condensed structural diagrams to represent the addition of 1-butene to HCl. Name the products and use Markovnikov s rule to determine the major and minor products. Use condensed structural diagrams to represent the substitution reaction between methane and chlorine. Balance the complete and incomplete combustion of ethene.

6 Find the average atomic mass for chromium from the data provided. A sample of platinum, Pt, contains (8.43)(10 25 ) atoms. How many moles of platinum are present? The simple sugar glucose has the chemical formula C 6H 12O 6. (a) How many molecules of glucose are present in mol of this sugar? (b) What is the mass of mol of glucose? (c) How many molecules of glucose are present in a mg sample? (d) How many hydrogen atoms are in a mg sample? Find the molar mass of ammonium sulfide,(nh4)2s.

7 The gem, garnet, has the chemical formula, Ca 3Al 2(SiO 4) 3. How many atoms of aluminum are in a piece of garnet having a mass of g? What is the volume of 4.92 mol of helium gas at STP? Which sample occupies at greater volume at STP? (a) 30.0 g of CH 4 or (b) molecules of H 2? Analysis of 24.1 g of calcium oxide revealed that it contained 17.2 g of calcium. What mass of this compound would contain 60 g of calcium? A compound of chromium and oxygen is 68.4% Cr and 31.6% O. What is its empirical formula?

8 A 3.00 g sample of CoC12 xh2o was heated and after the water was driven off, 1.64 g of CoC12 remained. Find the value of x. The poison coniine can be recovered from the hemlock plant. A g sample of this compound contains g of carbon, g of hydrogen, and the remainder is nitrogen. The molar mass of this compound is g/mol. Determine the molecular formula of coniine. What volume of H 2(g) will be produced at STP when 4.28 g of calcium metal reacts with water as shown by the following equation. Ca (s) + 2H 2O (l) Ca(OH) 2(aq) + H 2(g) The following single displacement reaction occurs when the solid mixture of aluminum and manganese are heated. 2Al (s) + 3MnO (s) Al 2O 3(s) + 3Mn (s) What mass of manganese solid will be produced when g of Al (s) and g of MnO (s) are allowed to react?

9 For each set of atoms listed, use a Lewis structure to illustrate how they can combine by sharing electrons to form a compound. (a) 2 carbon atoms and 6 hydrogen atoms (b) 2 carbon atoms, 4 hydrogen atoms, and 2 fluorine atoms (c) 2 carbon atoms, 4 hydrogen atoms and one oxygen atom (d) 1 carbon atom, 1 hydrogen atom, and 3 chlorine atoms Use the table of electronegativities listed in the student textbook to predict whether the bond formed between each pair of atoms will be non-polar covalent, polar covalent, or ionic. (a) Cs and O (b) Fe and N (c) H and Br (d) Ag and S, (e) O and Cl Polar covalent bonds are caused by (a) the donation of a pair of electrons by one atom (b) the unequal sharing of a pair of electrons (c) the union of atoms of the same electronegativity (d) the complete transfer of electrons from one atom to another (e) the equal sharing of electrons Which of the following best explains metallic bonding? (e) (a) Metal atoms are covalently bonded to one another. (b) Metals have the ability to form both anions and cations; these form ionic-type bonds (c) Metallic bonds involve an attraction between metal anions and a sea of mobile valence electrons. (d) Metallic bonds involve an attraction between metal cations and a sea of mobile valence electrons. Metallic bonds involve an attraction between metal cations and the nuclei of nearby atoms.

10 Draw an electron dot (Lewis) diagram for each of the following. (a) Al (b) CaF2 (c) a compound in which two oxygen atoms are bonded to each other and one hydrogen atom is also bonded to each oxygen (d) a compound in which 2 C atoms are bonded to one another. Each carbon atom is also bonded to two hydrogen atoms. (e) a carbon atom is bonded to a hydrogen atom and to a nitrogen atom. Which of the following in the liquid state is expected to be the best conductor of electricity? (a) CCl4 (b) CaF2 (c) I2 (d) CS2 Which of the following compounds in liquid state has the strongest hydrogen bonding? (a) PH3 (b) CH4 (c) NH3 (d) H2S Indicate which of the following molecules are polar and which are non-polar. (a) CO2 (c) CH3OH (d) CH(OH)O (e) PCl3 (f) CCl4 Predict the shape of the following molecules. (a) NF3 (e) PCl3 (f) CHCl3

11 Determine the intermolecular forces for following molecules. (a) NF3 (e) PCl3 (f) CHCl3 (a) CO2 (d) HCl + Cl2 You melt ice by heating it to 0 0 C. You melt NaCl by heating it to C.Why does salt have the higher melting point?

12 Draw the condensed structural diagram and then name each of the following molecules represented by a line structural diagram (a) (b) Name the compounds that are represented below. (a) CH 3(CH 2) 4CH 3 (b) (CH 3) 2CHCH 2CH 2CH(CH 3) 2 (c) (CH3)4C Draw condensed structural diagrams and line structural diagrams for the following molecules: (a) 3-ethyl-4-methyl-1-octene (b) 4-propyl-3-methyl-1-heptyne (c) 5-ethyl-2,3-dimethylheptane

13 Use condensed structural diagrams to represent the addition of 1-butene to HCl. Name the products and use Markovnikov s rule to determine the major and minor products. Use condensed structural diagrams to represent the substitution reaction between methane and chlorine. Balance the complete and incomplete combustion of ethene.