SOLUTION CLASS-XII / (CBSE)
|
|
|
- Cynthia Deborah Flowers
- 7 years ago
- Views:
Transcription
1 CBSE XII EXAMINATIN-016 SLUTIN CBSE 1 th Board (Chemistry) SET- Corporate ffice : CG Tower, A-46 & 5, IPIA, Near City Mall, Jhalawar Road, Kota (Raj.) PCCP Head ffice: J-, Jawahar Nagar, Main Road, Kota (Rajasthan)-4005 Contact : , Toll Free : CIN: U800RJ007PLC0409 P.T.. PAGE # 1
2
3 CBSE XII EXAMINATIN-016 Ans 1. Pb(N ) (s) Pb (s) 4N(g) (g) N gas dimeriz on cooling N N 4 Ans. (i) Reaction (i) is SN Reaction because is this Reaction Inversion of configuration occur. Ans. Ans 4. Colloidal solution are stable due to random motion (Brownian motion) of Colloidal particles. Zn heating 1 Zn e Zinc oxide is white in colour at room temp. n heating it loses oxygen and turn yellow. Ans 5. 1 CH NH CH CH CH CH N-methyl--methyl Propanamine Ans 6. (i) (H P ) XeF 4 P H P H P H F F Xe F F Ans 7. (i) osmotic pressure Minimum boiling azeotropes are show positive deviation from Raoult Law. Examples mixture of water + Ethanol Corporate ffice : CG Tower, A-46 & 5, IPIA, Near City Mall, Jhalawar Road, Kota (Raj.) PCCP Head ffice: J-, Jawahar Nagar, Main Road, Kota (Rajasthan)-4005 Contact : , Toll Free : CIN: U800RJ007PLC0409 P.T.. PAGE #
4 CBSE XII EXAMINATIN-016 Ans 8. (i) Kolbe Reaction :- n Reacting sodium salt of phenol with carbon dioxide gas, salicylic acid (-hydroxy benzoic acid) is formed. H Na H H NaH C CNa CH H+ under 4-7atm Pressure 400k Phenol Sod. phenate Sod. Salicylate Salicylic acid Friedal - Carft acetylation of anisole on Reacting alkyl halide [ Ex. CH Cl] in presence of Anhydrous AlCl with anisole, ortho-methyl anisole and para methyl anisole is formed as product. Anisole CH +CH Cl Anh.AlCl CH + CH CH -methyl anisole CH P-methyl anisole (i) Phenol to toluene : H r CH Phenol Zn dust - Zn CH Cl Anh.AlCl Toluene Forma ldehyde to Ethanol H H H CH C + CH Mg X C H H MgX H CH CH H + Mg Ethanol X H Formaldehyde Methyl megnesium halide Ans 9. (i) When chlorine atoms are removed from coordination sphere, moles of AgCl precipitated out. So the formula of complex will be : [Ni (H ) 6 ] Cl Hexaamine nickle (II) Chloride Ans 10. Pt NH(g) N(g) H(g) (i) rder of Reaction = Zero order molecularity = unit of k = mol l sec Corporate ffice : CG Tower, A-46 & 5, IPIA, Near City Mall, Jhalawar Road, Kota (Raj.) PCCP Head ffice: J-, Jawahar Nagar, Main Road, Kota (Rajasthan)-4005 Contact : , Toll Free : CIN: U800RJ007PLC0409 P.T.. PAGE #
5 CBSE XII EXAMINATIN-016 Br UV light Ans 11. (i) Br Cyclo hexene Br 1,-di bromo Cyclohexane CH C H = CH Peroxide HBr CH CH CH Br -phenyl propene 1-Bromo--phenyl propane CH H CH Cl (iii) H heat HCl H + H -Chloromethyl Phenol Ans 1. Volume of unit cell = a [ a = edge length) = (400 Pm) = ( m) = ( cm) = cm Volume of 08 g of the Element mass 08 g density = 9.71 cm 7g cm = vol of given amount Number of unit cells in this volume = vol of one unit cell 9.71 = 4 = Since each f.c.c unit cell contain 4 atoms therefore, total number of atoms in 08 g = = atoms Ans 1. (a) In phenol the lone pair of e on oxygen involves in delocalization not available freely for the protonation, where as in ethanol the e lone pairs on oxygen atom are not dellocalized, so they avoilable for protonation. (b) Due to the presence of H-bond in ethanol, intermolecular force of attractions are more in ethanol rather than alcohol. P.T.. Corporate ffice : CG Tower, A-46 & 5, IPIA, Near City Mall, Jhalawar Road, Kota (Raj.) PCCP Head ffice: J-, Jawahar Nagar, Main Road, Kota (Rajasthan)-4005 Contact : , Toll Free : CIN: U800RJ007PLC0409 PAGE # 4
6 CBSE XII EXAMINATIN-016 (c) Bacause in case of anisole, methyl phenyl oxinium ion C6H5 CH is formed by protonation H of ether. The bond between -CH is weaker than the bond between -C 6 H 5 because the carbon of phenyl group is Sp hybridised and there is partial double bond character. Therefore the attack by I ion breaks -CH bond to form CH -I. Ans 14. (i) The open chain structure fails to Explain the following reaction s (iii) (a) Despite having aldehyde ( CH), glucose does not react with sodium bisulphite (NaHS ) (b) Glucase does not give, 4 DNP Test and schiff test. (c) The pentaacetate of glucose does not react with hydroxylamine. This indicates the absence of free CH group. Phosphodiaester linkage present in Nucleic acids. Example of fat soluble vitamine Vitamine A, D, E, K Examples of water soluble vitamine Vitamine B and C Ans 15. weight of solute (w) = g molar mass (M W ) = 14 g/mol weight of solvent (w) = 50 g K b For Complete Ionization i = n Na S 4 i = = 0.5 K kg mol w K So Elevation in Boiling point T b = i b 1000 M W T b = T b = 0.4 W So boiling of solution = Boiling point of solvent + Elevation in B.P = 100 C C Ans 16. (i) Chromatography Some time, it is possible to separate two sulphide ores by adjusting proportion of oil to water or by using depressants. For Examples, in case of an ore containging ZnS and PbS, the depressant used in NaCN. It selective prevents Zn S from coming to the froth but allow PbS to come with the forth. (iii) CaC Ca C Ca Si flux Impurity CaSi Slag lime stone provide Ca on decomposition, Ca which work as flux to Remove Impurity of silica as slag (CaSi ) Corporate ffice : CG Tower, A-46 & 5, IPIA, Near City Mall, Jhalawar Road, Kota (Raj.) PCCP Head ffice: J-, Jawahar Nagar, Main Road, Kota (Rajasthan)-4005 Contact : , Toll Free : CIN: U800RJ007PLC0409 P.T.. PAGE # 5
7 CBSE XII EXAMINATIN-016 Ans 17. (i) o/w Emulsions : In this system water acts as dispession medium and oil act as disphersed phase. for e.g. - milk and vanishing cream. In milk, liquid fat is dispired in water (iii) Zeta potential :- Separation of charge is a set of potential, the charges of opposite signs on the fixed and diffused parts of the double layer results in a difference in potential between these layers. This potential difference between the fixed layer and the diffused layer of opposite charges is called the zeta potential. Multimolecular colloids :- A large number of atoms or smaller molecules of a substance aggregate together to form species having size in the colloidal range. The species thus formed are called multimolecular colloids. Ans 18. (a) [Fe(CN) 6 ] 4.N. of Fe = x + 6 ( 1) = 4 x = + Fe + = 1s, s, p 6, s, p 6, d 6, 4s in the presence of CN d 4s 4p d 4s 4p d sp hybridisation - Hybridisation d sp - magnetic character all the electrons are paired because CN is a low spin ligand as a result it is diamagnetic is Nature - low spin complex (b) Cl Cl C en en Ans 19. (a) In H P, there are P-H bonds whereas in H P there is only 1 P-H bond. P H H H P H H P H H Corporate ffice : CG Tower, A-46 & 5, IPIA, Near City Mall, Jhalawar Road, Kota (Raj.) PCCP Head ffice: J-, Jawahar Nagar, Main Road, Kota (Rajasthan)-4005 Contact : , Toll Free : CIN: U800RJ007PLC0409 P.T.. PAGE # 6
8 CBSE XII EXAMINATIN-016 (b) (c) This is because S-S bond is stronger than - bond. due decrease in bond dissociation Enthalpy from HF to HI Ans 0. (i) C6H 5 C N H 4 C H CNH 6 5 Benzanaide C H NH 6 5 Aniline ( H CCl ) Pyridine ( Acetylation) NH C-CH N-phenylethanamide N NH NC C H N BF Benzene diazonium Fluoroborate NaN Cu Ä Nitrobenzene Sn HCl Aniline CHCl alc.koh phenylisocyanide Ans 1. H H Ea log10k log10 A.0 RT Given log k 14. T 4 k E a = R (activation Energy) E a = = J mol half life (t 50% ) = 00 minutes k = t 50% k = sec (Rate constant) Ans. (i) Benzoyl peroxide is free radical generater. In the presence of benzoyl peroxide phenyl free radical formed which is responsible of chain initiating step. (a) H N (CH ) 6 NH (Hexamethydiamine) and adipic acid CH (CH ) 4 CH (iii) Polythene < Buna S < Nylon 6, 6 P.T.. Corporate ffice : CG Tower, A-46 & 5, IPIA, Near City Mall, Jhalawar Road, Kota (Raj.) PCCP Head ffice: J-, Jawahar Nagar, Main Road, Kota (Rajasthan)-4005 Contact : , Toll Free : CIN: U800RJ007PLC0409 PAGE # 7
9 CBSE XII EXAMINATIN-016 Free radical mechanism : R (i) Chain initiation steps C6H5 C C C6H5 C 6H5 C C 6 H5 Benzoyl peroxide ( initiator ) phenyl radical Chain propagating step :- C 6 H 5 CH CH C6H5 CH C H Chain terminating step :- C 6H5CH C H CH CH C6H5 CH CH C H Chain termination C H CH CH CH CH CH CH CH CH C H 6 5 n n 6 5 Polythene Ans. (i) (a) Mr. Roy is a good friend of Mr. Awasthi, and He is a responsible person. (b) Mr. Roy is concern about the health of his friend. It is not advisable to take sleeping pills without consulting doctor because the main ingredient of most of the sleeping pills is barbiturates. These chemicals make you to breathe showly and less deeply. That can be dengerous for people who have asthma or some other heart problems. (iii) Transquillizers are drugs which are used for treatment of stress, fatigue, mild and severe mental diseases. eg. Chlordiazepoxide and meprobamate Ans 4. (a) CH CN (i) Sncl HCl H CH CH Ethanal CH C HCN H CN - Hyodroxy propannitrile dil NaH CH CH CH H CH Hydroxy bu tanal CH CH CH CH but en1al (A) CH CH (B) CH CH CH H CH Corporate ffice : CG Tower, A-46 & 5, IPIA, Near City Mall, Jhalawar Road, Kota (Raj.) PCCP Head ffice: J-, Jawahar Nagar, Main Road, Kota (Rajasthan)-4005 Contact : , Toll Free : CIN: U800RJ007PLC0409 P.T.. PAGE # 8
10 CBSE XII EXAMINATIN-016 (C) CH CH = CH CH (D) CH C H CN (b) (i) homologous members of same series. homologous members of same series (c) CH CH > CH CH H > CH CCH carboxylic acids are having high boiling point due to hydrogen bonding. R (a) Etard Reaction CH C H(CrHCl ) CH Toluene CS Cl cromyl chloride Cr chromium complex H Benzeldehyde (b) HCH > CH CH > C 6 H 5 CCH (c) Because in Cl CH CH, I effective group is present which decreases the electron density of C. that s why Cl CH CH is more acidic than CH CH. (d) CH CH CH = CH CH CN Hex en 1 nitrile (i) i. Bu AlH CH CH CH = CH CH CH H Hex -en 1 al (e) two isomers are CH C CH and CH CH CH (A) CH C CH Ketone (B) CH CH CH aldehyde P.T.. Corporate ffice : CG Tower, A-46 & 5, IPIA, Near City Mall, Jhalawar Road, Kota (Raj.) PCCP Head ffice: J-, Jawahar Nagar, Main Road, Kota (Rajasthan)-4005 Contact : , Toll Free : CIN: U800RJ007PLC0409 PAGE # 9
11 CBSE XII EXAMINATIN-016 NaH I CHCCH CH CNa CHI (A) Yellow ppt NaH I CH CHCH No reaction (B) Ans 5. (a) E cell = E cell E cell = E cell n log [Product] 10 [Reactant] log = log = log [ log = 1] = = = V (b) Given [ E (Fe + / Fe) = 0.44 V ] E (A + / A) =.7 V E (B + / B) = 0.14 V A will prevent iron from corrosion, so we can coat the iron metal by element A because it is having more negative value of reduction potential then iron (a) Given Molarity (M) = mol / L R Conductivity = cm 1 ( H + ) = cm mol (CH C ) = cm mol 1000 Molar Conductivity ( m ) = Conductivity M = cm mol = Molar conduc tance at specific concontration Molar conduc tance at inf inite ditation Corporate ffice : CG Tower, A-46 & 5, IPIA, Near City Mall, Jhalawar Road, Kota (Raj.) PCCP Head ffice: J-, Jawahar Nagar, Main Road, Kota (Rajasthan)-4005 Contact : , Toll Free : CIN: U800RJ007PLC0409 P.T.. PAGE # 10
12 CBSE XII EXAMINATIN-016 = = 0.1 = 10% CH CH H CH (b) Electro chemical cell :- Cell which convert chemical Energy into Electrical Energy (i) If E cell [External] > E cell Electron flow from Cathode to anode and current flow from anode to cathode. Ans 6. (a) (i) The ability of oxygen to stabilise the high oxidation state exceeds that of fluorine. Due to lanthanoid contraction Zr and Hf show similar properties. (iii) Due to variable oxidation state, transition metals act as good catalyst. (b) (i) Mn + 4KH + Fuse K Mn 4 + H Cr H I Cr + + 7H + I R (i) (iii) (iv) Zn because Zn does not show variable oxidation State Cr chromium is having highest melting point due to high enthalpy of atomisation Copper (Cu). Mn Mn Ar 4s d 5 4 Ar 4s d Mn + having 4 electrons in d subshell, it required one electron to half filled configuration in d subshell it act as strong oxidising agent. Corporate ffice : CG Tower, A-46 & 5, IPIA, Near City Mall, Jhalawar Road, Kota (Raj.) PCCP Head ffice: J-, Jawahar Nagar, Main Road, Kota (Rajasthan)-4005 Contact : , Toll Free : CIN: U800RJ007PLC0409 PAGE # 11
Code number given on the right hand side of the question paper should be written on the title page of the answerbook by the candidate.
Series ONS SET-3 Roll No. Candiates must write code on the title page of the answer book Please check that this question paper contains 15 printed pages. Code number given on the right hand side of the
Chapter 4 Chemical Reactions
Chapter 4 Chemical Reactions I) Ions in Aqueous Solution many reactions take place in water form ions in solution aq solution = solute + solvent solute: substance being dissolved and present in lesser
SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001
SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001 1. A small pin contains 0.0178 mol of iron. How many atoms of iron are in the pin? 2. A sample
neutrons are present?
AP Chem Summer Assignment Worksheet #1 Atomic Structure 1. a) For the ion 39 K +, state how many electrons, how many protons, and how many 19 neutrons are present? b) Which of these particles has the smallest
ATOMS. Multiple Choice Questions
Chapter 3 ATOMS AND MOLECULES Multiple Choice Questions 1. Which of the following correctly represents 360 g of water? (i) 2 moles of H 2 0 (ii) 20 moles of water (iii) 6.022 10 23 molecules of water (iv)
Stoichiometry. Lecture Examples Answer Key
Stoichiometry Lecture Examples Answer Key Ex. 1 Balance the following chemical equations: 3 NaBr + 1 H 3 PO 4 3 HBr + 1 Na 3 PO 4 2 C 3 H 5 N 3 O 9 6 CO 2 + 3 N 2 + 5 H 2 O + 9 O 2 2 Ca(OH) 2 + 2 SO 2
IB Chemistry. DP Chemistry Review
DP Chemistry Review Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant Assessment statement Apply the mole concept to substances. Determine the number of particles and the amount
APPENDIX B: EXERCISES
BUILDING CHEMISTRY LABORATORY SESSIONS APPENDIX B: EXERCISES Molecular mass, the mole, and mass percent Relative atomic and molecular mass Relative atomic mass (A r ) is a constant that expresses the ratio
Bonding Practice Problems
NAME 1. When compared to H 2 S, H 2 O has a higher 8. Given the Lewis electron-dot diagram: boiling point because H 2 O contains stronger metallic bonds covalent bonds ionic bonds hydrogen bonds 2. Which
= 11.0 g (assuming 100 washers is exact).
CHAPTER 8 1. 100 washers 0.110 g 1 washer 100. g 1 washer 0.110 g = 11.0 g (assuming 100 washers is exact). = 909 washers 2. The empirical formula is CFH from the structure given. The empirical formula
Which substance contains positive ions immersed in a sea of mobile electrons? A) O2(s) B) Cu(s) C) CuO(s) D) SiO2(s)
BONDING MIDTERM REVIEW 7546-1 - Page 1 1) Which substance contains positive ions immersed in a sea of mobile electrons? A) O2(s) B) Cu(s) C) CuO(s) D) SiO2(s) 2) The bond between hydrogen and oxygen in
INTI COLLEGE MALAYSIA A? LEVEL PROGRAMME CHM 111: CHEMISTRY MOCK EXAMINATION: DECEMBER 2000 SESSION. 37 74 20 40 60 80 m/e
CHM111(M)/Page 1 of 5 INTI COLLEGE MALAYSIA A? LEVEL PROGRAMME CHM 111: CHEMISTRY MOCK EXAMINATION: DECEMBER 2000 SESSION SECTION A Answer ALL EIGHT questions. (52 marks) 1. The following is the mass spectrum
B) atomic number C) both the solid and the liquid phase D) Au C) Sn, Si, C A) metal C) O, S, Se C) In D) tin D) methane D) bismuth B) Group 2 metal
1. The elements on the Periodic Table are arranged in order of increasing A) atomic mass B) atomic number C) molar mass D) oxidation number 2. Which list of elements consists of a metal, a metalloid, and
Calculating Atoms, Ions, or Molecules Using Moles
TEKS REVIEW 8B Calculating Atoms, Ions, or Molecules Using Moles TEKS 8B READINESS Use the mole concept to calculate the number of atoms, ions, or molecules in a sample TEKS_TXT of material. Vocabulary
4. Using the data from Handout 5, what is the standard enthalpy of formation of BaO (s)? What does this mean?
HOMEWORK 3A 1. In each of the following pairs, tell which has the higher entropy. (a) One mole of liquid water or one mole of water vapor (b) One mole of dry ice or one mole of carbon dioxide at 1 atm
Candidate Style Answer
Candidate Style Answer Chemistry A Unit F321 Atoms, Bonds and Groups High banded response This Support Material booklet is designed to accompany the OCR GCE Chemistry A Specimen Paper F321 for teaching
Cambridge International Examinations Cambridge International General Certificate of Secondary Education
Cambridge International Examinations Cambridge International General Certificate of Secondary Education *0123456789* CHEMISTRY 0620/04 Paper 4 Theory (Extended) For Examination from 2016 SPECIMEN PAPER
Instructions Answer all questions in the spaces provided. Do all rough work in this book. Cross through any work you do not want to be marked.
GCSE CHEMISTRY Higher Tier Chemistry 1H H Specimen 2018 Time allowed: 1 hour 45 minutes Materials For this paper you must have: a ruler a calculator the periodic table (enclosed). Instructions Answer all
Question Bank Electrolysis
Question Bank Electrolysis 1. (a) What do you understand by the terms (i) electrolytes (ii) non-electrolytes? (b) Arrange electrolytes and non-electrolytes from the following substances (i) sugar solution
Chapter 1: Moles and equations. Learning outcomes. you should be able to:
Chapter 1: Moles and equations 1 Learning outcomes you should be able to: define and use the terms: relative atomic mass, isotopic mass and formula mass based on the 12 C scale perform calculations, including
AP Chemistry 2008 Free-Response Questions
AP Chemistry 008 Free-Response Questions The College Board: Connecting Students to College Success The College Board is a not-for-profit membership association whose mission is to connect students to college
Chem 1A Exam 2 Review Problems
Chem 1A Exam 2 Review Problems 1. At 0.967 atm, the height of mercury in a barometer is 0.735 m. If the mercury were replaced with water, what height of water (in meters) would be supported at this pressure?
1. How many hydrogen atoms are in 1.00 g of hydrogen?
MOLES AND CALCULATIONS USING THE MOLE CONCEPT INTRODUCTORY TERMS A. What is an amu? 1.66 x 10-24 g B. We need a conversion to the macroscopic world. 1. How many hydrogen atoms are in 1.00 g of hydrogen?
ORGANIC CHEMISTRY I PRACTICE PROBLEMS FOR BRONSTED-LOWRY ACID-BASE CHEMISTRY
RGANIC CHEMISTRY I PRACTICE PRBLEMS FR BRNSTED-LWRY ACID-BASE CHEMISTRY 1. For each of the species below, identify the most acidic proton and provide the structure of the corresponding conjugate base.
Cambridge International Examinations Cambridge International Advanced Subsidiary and Advanced Level
Cambridge International Examinations Cambridge International Advanced Subsidiary and Advanced Level *0123456789* CHEMISTRY 9701/02 Paper 2 AS Level Structured Questions For Examination from 2016 SPECIMEN
Chemistry 65 Chapter 6 THE MOLE CONCEPT
THE MOLE CONCEPT Chemists find it more convenient to use mass relationships in the laboratory, while chemical reactions depend on the number of atoms present. In order to relate the mass and number of
6 Reactions in Aqueous Solutions
6 Reactions in Aqueous Solutions Water is by far the most common medium in which chemical reactions occur naturally. It is not hard to see this: 70% of our body mass is water and about 70% of the surface
Chemistry B11 Chapter 4 Chemical reactions
Chemistry B11 Chapter 4 Chemical reactions Chemical reactions are classified into five groups: A + B AB Synthesis reactions (Combination) H + O H O AB A + B Decomposition reactions (Analysis) NaCl Na +Cl
Stoichiometry Review
Stoichiometry Review There are 20 problems in this review set. Answers, including problem set-up, can be found in the second half of this document. 1. N 2 (g) + 3H 2 (g) --------> 2NH 3 (g) a. nitrogen
stoichiometry = the numerical relationships between chemical amounts in a reaction.
1 REACTIONS AND YIELD ANSWERS stoichiometry = the numerical relationships between chemical amounts in a reaction. 2C 8 H 18 (l) + 25O 2 16CO 2 (g) + 18H 2 O(g) From the equation, 16 moles of CO 2 (a greenhouse
CHEMICAL REACTIONS. Chemistry 51 Chapter 6
CHEMICAL REACTIONS A chemical reaction is a rearrangement of atoms in which some of the original bonds are broken and new bonds are formed to give different chemical structures. In a chemical reaction,
Chapter 13. Properties of Solutions
Sample Exercise 13.1 (p. 534) By the process illustrated below, water vapor reacts with excess solid sodium sulfate to form the hydrated form of the salt. The chemical reaction is Na 2 SO 4(s) + 10 H 2
Chemistry B11 Chapter 6 Solutions and Colloids
Chemistry B11 Chapter 6 Solutions and Colloids Solutions: solutions have some properties: 1. The distribution of particles in a solution is uniform. Every part of the solution has exactly the same composition
Chemistry: Chemical Equations
Chemistry: Chemical Equations Write a balanced chemical equation for each word equation. Include the phase of each substance in the equation. Classify the reaction as synthesis, decomposition, single replacement,
Aqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions.
Aqueous Solutions and Solution Stoichiometry Water is the dissolving medium, or solvent. Some Properties of Water Water is bent or V-shaped. The O-H bonds are covalent. Water is a polar molecule. Hydration
REVIEW QUESTIONS Chapter 8
Chemistry 101 ANSWER KEY REVIEW QUESTIONS Chapter 8 Use only a periodic table to answer the following questions. 1. Write complete electron configuration for each of the following elements: a) Aluminum
Formulae, stoichiometry and the mole concept
3 Formulae, stoichiometry and the mole concept Content 3.1 Symbols, Formulae and Chemical equations 3.2 Concept of Relative Mass 3.3 Mole Concept and Stoichiometry Learning Outcomes Candidates should be
Chemistry Diagnostic Questions
Chemistry Diagnostic Questions Answer these 40 multiple choice questions and then check your answers, located at the end of this document. If you correctly answered less than 25 questions, you need to
2. Write the chemical formula(s) of the product(s) and balance the following spontaneous reactions.
1. Using the Activity Series on the Useful Information pages of the exam write the chemical formula(s) of the product(s) and balance the following reactions. Identify all products phases as either (g)as,
In the box below, draw the Lewis electron-dot structure for the compound formed from magnesium and oxygen. [Include any charges or partial charges.
Name: 1) Which molecule is nonpolar and has a symmetrical shape? A) NH3 B) H2O C) HCl D) CH4 7222-1 - Page 1 2) When ammonium chloride crystals are dissolved in water, the temperature of the water decreases.
(1) e.g. H hydrogen that has lost 1 electron c. anion - negatively charged atoms that gain electrons 16-2. (1) e.g. HCO 3 bicarbonate anion
GS106 Chemical Bonds and Chemistry of Water c:wou:gs106:sp2002:chem.wpd I. Introduction A. Hierarchy of chemical substances 1. atoms of elements - smallest particles of matter with unique physical and
Sample Test 1 SAMPLE TEST 1. CHAPTER 12
13 Sample Test 1 SAMPLE TEST 1. CHAPTER 12 1. The molality of a solution is defined as a. moles of solute per liter of solution. b. grams of solute per liter of solution. c. moles of solute per kilogram
Chemical Calculations: The Mole Concept and Chemical Formulas. AW Atomic weight (mass of the atom of an element) was determined by relative weights.
1 Introduction to Chemistry Atomic Weights (Definitions) Chemical Calculations: The Mole Concept and Chemical Formulas AW Atomic weight (mass of the atom of an element) was determined by relative weights.
Questions on Chapter 8 Basic Concepts of Chemical Bonding
Questions on Chapter 8 Basic Concepts of Chemical Bonding Circle the Correct Answer: 1) Which ion below has a noble gas electron configuration? A) Li 2+ B) Be 2+ C) B2+ D) C2+ E) N 2-2) Of the ions below,
Amount of Substance. http://www.avogadro.co.uk/definitions/elemcompmix.htm
Page 1 of 14 Amount of Substance Key terms in this chapter are: Element Compound Mixture Atom Molecule Ion Relative Atomic Mass Avogadro constant Mole Isotope Relative Isotopic Mass Relative Molecular
Name Class Date. In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question.
Assessment Chapter Test A Chapter: States of Matter In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. The kinetic-molecular
Unit 10A Stoichiometry Notes
Unit 10A Stoichiometry Notes Stoichiometry is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations
K + Cl - Metal M. Zinc 1.0 M M(NO
Redox and Electrochemistry This section should be fresh in your minds because we just did this section in the text. Closely related to electrochemistry is redox chemistry. Count on at least one question
Moles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations
Moles Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations Micro World atoms & molecules Macro World grams Atomic mass is the mass of an
Page 1. 6. Which hydrocarbon is a member of the alkane series? (1) 1. Which is the structural formula of methane? (1) (2) (2) (3) (3) (4) (4)
1. Which is the structural formula of methane? 6. Which hydrocarbon is a member of the alkane series? 7. How many carbon atoms are contained in an ethyl group? 1 3 2 4 2. In the alkane series, each molecule
Exam 4 Practice Problems false false
Exam 4 Practice Problems 1 1. Which of the following statements is false? a. Condensed states have much higher densities than gases. b. Molecules are very far apart in gases and closer together in liquids
Chapter 8 Atomic Electronic Configurations and Periodicity
Chapter 8 Electron Configurations Page 1 Chapter 8 Atomic Electronic Configurations and Periodicity 8-1. Substances that are weakly attracted to a magnetic field but lose their magnetism when removed from
48 Practice Problems for Ch. 17 - Chem 1C - Joseph
48 Practice Problems for Ch. 17 - Chem 1C - Joseph 1. Which of the following concentration measures will change in value as the temperature of a solution changes? A) mass percent B) mole fraction C) molality
Chapter 3 Mass Relationships in Chemical Reactions
Chapter 3 Mass Relationships in Chemical Reactions Student: 1. An atom of bromine has a mass about four times greater than that of an atom of neon. Which choice makes the correct comparison of the relative
Identification of Unknown Organic Compounds
Identification of Unknown Organic Compounds Introduction The identification and characterization of the structures of unknown substances are an important part of organic chemistry. Although it is often
Atomic Structure. Name Mass Charge Location Protons 1 +1 Nucleus Neutrons 1 0 Nucleus Electrons 1/1837-1 Orbit nucleus in outer shells
Atomic Structure called nucleons Name Mass Charge Location Protons 1 +1 Nucleus Neutrons 1 0 Nucleus Electrons 1/1837-1 Orbit nucleus in outer shells The number of protons equals the atomic number This
The Periodic Table: Periodic trends
Unit 1 The Periodic Table: Periodic trends There are over one hundred different chemical elements. Some of these elements are familiar to you such as hydrogen, oxygen, nitrogen and carbon. Each one has
10. Calculate the mass percent nitrogen in (NH 4 ) 2 CO 3 (molar mass = 96.09 g/mol). a. 29.1 % c. 17.9 % e. 14.6 % b. 35.9 % d. 0.292 % f. 96.
Chem 171-2-3: Final Exam Review Multiple Choice Problems 1. What is the molar mass of barium perchlorate, Ba(ClO 4 ) 2? a. 189.90 g/mol c. 272.24 g/mol e. 336.20 g/mol b. 240.24 g/mol d. 304.24 g/mol f.
Chem 112 Intermolecular Forces Chang From the book (10, 12, 14, 16, 18, 20,84,92,94,102,104, 108, 112, 114, 118 and 134)
Chem 112 Intermolecular Forces Chang From the book (10, 12, 14, 16, 18, 20,84,92,94,102,104, 108, 112, 114, 118 and 134) 1. Helium atoms do not combine to form He 2 molecules, What is the strongest attractive
Unit 2: Quantities in Chemistry
Mass, Moles, & Molar Mass Relative quantities of isotopes in a natural occurring element (%) E.g. Carbon has 2 isotopes C-12 and C-13. Of Carbon s two isotopes, there is 98.9% C-12 and 11.1% C-13. Find
States of Matter CHAPTER 10 REVIEW SECTION 1. Name Date Class. Answer the following questions in the space provided.
CHAPTER 10 REVIEW States of Matter SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Identify whether the descriptions below describe an ideal gas or a real gas. ideal gas
Electronegativity and Polarity MAIN Idea A chemical bond s character is related to each atom s
Section 8.5 Objectives Describe how electronegativity is used to determine bond type. Compare and contrast polar and nonpolar covalent bonds and polar and nonpolar molecules. Generalize about the characteristics
Coimisiún na Scrúduithe Stáit State Examinations Commission
2015. M33 Coimisiún na Scrúduithe Stáit State Examinations Commission LEAVING CERTIFICATE EXAMINATION, 2015 CHEMISTRY ORDINARY LEVEL TUESDAY, 16 JUNE AFTERNOON 2.00 TO 5.00 400 MARKS Answer eight questions
Chapter 17. The best buffer choice for ph 7 is NaH 2 PO 4 /Na 2 HPO 4. 19)
Chapter 17 2) a) HCl and CH 3 COOH are both acids. A buffer must have an acid/base conjugate pair. b) NaH 2 PO 4 and Na 2 HPO 4 are an acid/base conjugate pair. They will make an excellent buffer. c) H
Chemistry Post-Enrolment Worksheet
Name: Chemistry Post-Enrolment Worksheet The purpose of this worksheet is to get you to recap some of the fundamental concepts that you studied at GCSE and introduce some of the concepts that will be part
100% ionic compounds do not exist but predominantly ionic compounds are formed when metals combine with non-metals.
2.21 Ionic Bonding 100% ionic compounds do not exist but predominantly ionic compounds are formed when metals combine with non-metals. Forming ions Metal atoms lose electrons to form +ve ions. Non-metal
AROMATIC COMPOUNDS A STUDENT SHOULD BE ABLE TO:
A STUDENT SHULD BE ABLE T: ARMATIC CMPUNDS 1. Name benzene derivatives given the structures, and draw the structures given the names. This includes: Monosubstituted benzenes named as derivatives of benzene:
CHM1 Review Exam 12. Topics REDOX
CHM1 Review Exam 12 Topics REDOX REDOX Reactions Oxidation Reduction Oxidizing agent Reducing agent Galvanic (Voltaic) Cells Anode Cathode Salt bridge Electrolyte Half-reactions Voltage o Positive voltages
Assessment Schedule 2013 Chemistry: Demonstrate understanding of the properties of organic compounds (91391)
NCEA Level 3 Chemistry (91391) 2013 page 1 of 8 Assessment Schedule 2013 Chemistry: Demonstrate understanding of the properties of organic compounds (91391) Evidence Statement Q Evidence Achievement Achievement
NOTE: This practice exam contains more than questions than the real final.
NOTE: This practice exam contains more than questions than the real final 1 The wavelength of light emitted from a green laser pointer is 532 10 2 nm What is the wavelength in meters? 532 10-7 m 2 What
Getting the most from this book...4 About this book...5
Contents Getting the most from this book...4 About this book....5 Content Guidance Topic 1 Atomic structure and the periodic table...8 Topic 2 Bonding and structure...14 Topic 2A Bonding....14 Topic 2B
Chapter 3! Stoichiometry: Calculations with Chemical Formulas and Equations. Stoichiometry
Chapter 3! : Calculations with Chemical Formulas and Equations Anatomy of a Chemical Equation CH 4 (g) + 2O 2 (g) CO 2 (g) + 2 H 2 O (g) Anatomy of a Chemical Equation CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2
1332 CHAPTER 18 Sample Questions
1332 CHAPTER 18 Sample Questions Couple E 0 Couple E 0 Br 2 (l) + 2e 2Br (aq) +1.06 V AuCl 4 + 3e Au + 4Cl +1.00 V Ag + + e Ag +0.80 V Hg 2+ 2 + 2e 2 Hg +0.79 V Fe 3+ (aq) + e Fe 2+ (aq) +0.77 V Cu 2+
Chemical Calculations: Formula Masses, Moles, and Chemical Equations
Chemical Calculations: Formula Masses, Moles, and Chemical Equations Atomic Mass & Formula Mass Recall from Chapter Three that the average mass of an atom of a given element can be found on the periodic
Chemistry 151 Final Exam
Chemistry 151 Final Exam Name: SSN: Exam Rules & Guidelines Show your work. No credit will be given for an answer unless your work is shown. Indicate your answer with a box or a circle. All paperwork must
Chemistry Ch 15 (Solutions) Study Guide Introduction
Chemistry Ch 15 (Solutions) Study Guide Introduction Name: Note: a word marked (?) is a vocabulary word you should know the meaning of. A homogeneous (?) mixture, or, is a mixture in which the individual
Chemical Proportions in Compounds
Chapter 6 Chemical Proportions in Compounds Solutions for Practice Problems Student Textbook page 201 1. Problem A sample of a compound is analyzed and found to contain 0.90 g of calcium and 1.60 g of
CHEM5 Energetics, Redox and Inorganic Chemistry Mark scheme
AQA Qualifications A-LEVEL CHEMISTRY CHEM5 Energetics, Redox and Inorganic Chemistry Mark scheme 2420 June 204 Version. Final Mark schemes are prepared by the Lead Assessment Writer and considered, together
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Chemistry 1C-Dr. Larson Chapter 20 Review Questions MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) is reduced in the following reaction: Cr2O7
Chemical Equations & Stoichiometry
Chemical Equations & Stoichiometry Chapter Goals Balance equations for simple chemical reactions. Perform stoichiometry calculations using balanced chemical equations. Understand the meaning of the term
7. 1.00 atm = 760 torr = 760 mm Hg = 101.325 kpa = 14.70 psi. = 0.446 atm. = 0.993 atm. = 107 kpa 760 torr 1 atm 760 mm Hg = 790.
CHATER 3. The atmosphere is a homogeneous mixture (a solution) of gases.. Solids and liquids have essentially fixed volumes and are not able to be compressed easily. have volumes that depend on their conditions,
Part B 2. Allow a total of 15 credits for this part. The student must answer all questions in this part.
Part B 2 Allow a total of 15 credits for this part. The student must answer all questions in this part. 51 [1] Allow 1 credit for 3 Mg(s) N 2 (g) Mg 3 N 2 (s). Allow credit even if the coefficient 1 is
Question Bank Organic Chemistry-I
Question Bank Organic Chemistry-I 1. (a) What do you understand by the following terms : (i) Organic chemistry (ii) Organic compounds (iii) Catenation? [3] (b) Why are there very large number of organic
HOMEWORK 4A. Definitions. Oxidation-Reduction Reactions. Questions
HOMEWORK 4A Oxidation-Reduction Reactions 1. Indicate whether a reaction will occur or not in each of following. Wtiring a balcnced equation is not necessary. (a) Magnesium metal is added to hydrochloric
Chapter 12: Oxidation and Reduction.
207 Oxidation- reduction (redox) reactions Chapter 12: Oxidation and Reduction. At different times, oxidation and reduction (redox) have had different, but complimentary, definitions. Compare the following
CHEMISTRY 101 EXAM 3 (FORM B) DR. SIMON NORTH
1. Is H 3 O + polar or non-polar? (1 point) a) Polar b) Non-polar CHEMISTRY 101 EXAM 3 (FORM B) DR. SIMON NORTH 2. The bond strength is considerably greater in HF than in the other three hydrogen halides
NET IONIC EQUATIONS. A balanced chemical equation can describe all chemical reactions, an example of such an equation is:
NET IONIC EQUATIONS A balanced chemical equation can describe all chemical reactions, an example of such an equation is: NaCl + AgNO 3 AgCl + NaNO 3 In this case, the simple formulas of the various reactants
Chapter 3: Stoichiometry
Chapter 3: Stoichiometry Key Skills: Balance chemical equations Predict the products of simple combination, decomposition, and combustion reactions. Calculate formula weights Convert grams to moles and
Concept 1. The meaning and usefulness of the mole. The mole (or mol) represents a certain number of objects.
Chapter 3. Stoichiometry: Mole-Mass Relationships in Chemical Reactions Concept 1. The meaning and usefulness of the mole The mole (or mol) represents a certain number of objects. SI def.: the amount of
Chapter 5 Classification of Organic Compounds by Solubility
Chapter 5 Classification of Organic Compounds by Solubility Deductions based upon interpretation of simple solubility tests can be extremely useful in organic structure determination. Both solubility and
Chapter 1 The Atomic Nature of Matter
Chapter 1 The Atomic Nature of Matter 6. Substances that cannot be decomposed into two or more simpler substances by chemical means are called a. pure substances. b. compounds. c. molecules. d. elements.
Molarity of Ions in Solution
APPENDIX A Molarity of Ions in Solution ften it is necessary to calculate not only the concentration (in molarity) of a compound in aqueous solution but also the concentration of each ion in aqueous solution.
Sample Exercise 3.1 Interpreting and Balancing Chemical Equations
Sample Exercise 3.1 Interpreting and Balancing Chemical Equations The following diagram represents a chemical reaction in which the red spheres are oxygen atoms and the blue spheres are nitrogen atoms.
CHAPTER 3 Calculations with Chemical Formulas and Equations. atoms in a FORMULA UNIT
CHAPTER 3 Calculations with Chemical Formulas and Equations MOLECULAR WEIGHT (M. W.) Sum of the Atomic Weights of all atoms in a MOLECULE of a substance. FORMULA WEIGHT (F. W.) Sum of the atomic Weights
Chapter 3. Chemical Reactions and Reaction Stoichiometry. Lecture Presentation. James F. Kirby Quinnipiac University Hamden, CT
Lecture Presentation Chapter 3 Chemical Reactions and Reaction James F. Kirby Quinnipiac University Hamden, CT The study of the mass relationships in chemistry Based on the Law of Conservation of Mass
Chemistry 1050 Chapter 13 LIQUIDS AND SOLIDS 1. Exercises: 25, 27, 33, 39, 41, 43, 51, 53, 57, 61, 63, 67, 69, 71(a), 73, 75, 79
Chemistry 1050 Chapter 13 LIQUIDS AND SOLIDS 1 Text: Petrucci, Harwood, Herring 8 th Edition Suggest text problems Review questions: 1, 5!11, 13!17, 19!23 Exercises: 25, 27, 33, 39, 41, 43, 51, 53, 57,
Metals and Non-metals. Comparison of physical properties of metals and non metals
Metals and Non-metals Comparison of physical properties of metals and non metals PHYSICAL PROPERTY METALS NON-METALS Physical State Metallic lustre (having a shining surface) Mostly solids (Liquid -mercury)
Chem 115 POGIL Worksheet - Week 4 Moles & Stoichiometry
Chem 115 POGIL Worksheet - Week 4 Moles & Stoichiometry Why? Chemists are concerned with mass relationships in chemical reactions, usually run on a macroscopic scale (grams, kilograms, etc.). To deal with
PART I: MULTIPLE CHOICE (30 multiple choice questions. Each multiple choice question is worth 2 points)
CHEMISTRY 123-07 Midterm #1 Answer key October 14, 2010 Statistics: Average: 74 p (74%); Highest: 97 p (95%); Lowest: 33 p (33%) Number of students performing at or above average: 67 (57%) Number of students
Element of same atomic number, but different atomic mass o Example: Hydrogen
Atomic mass: p + = protons; e - = electrons; n 0 = neutrons p + + n 0 = atomic mass o For carbon-12, 6p + + 6n 0 = atomic mass of 12.0 o For chlorine-35, 17p + + 18n 0 = atomic mass of 35.0 atomic mass