# Chapter 3: Stoichiometry

Save this PDF as:

Size: px
Start display at page:

Download "Chapter 3: Stoichiometry"

## Transcription

1 Chapter 3: Stoichiometry Chem 6A Michael J. Sailor, UC San Diego 1 Announcements: Thursday (Sep 29) quiz: Bring student ID or we cannot accept your quiz! No notes, no calculators Covers chapters 1 and 2 Need to know your name, PID, and section # Chem 6A Michael J. Sailor, UC San Diego 2

2 Cover page of Thursday s quiz Chem 6A 2010 (Sailor) Name: Student ID Number: Section Number: QUIZ H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Lanthanides Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Actinides Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Some useful constants and relationships: Ideal gas constant: L. atm. mol -1. K -1 = J. mol -1. K -1 Avogadro constant: x mole -1 Planck's constant = h = x J. s speed of light: 3.00 x 10 8 m/s J = 1 L. atm 1J = 1kg. m 2 /s 2 1 atm = 760 Torr 1 ev = x J E = -RHh/n 2 RH = 3.29 x Hz C2 = second radiation constant = 1.44 x 10-2 K. m Emitted power (W) = (constant)t 4 Surface area (m 2 ) max = 1 5 C 2 E = hc " Chem 6A Michael J. Sailor, UC San Diego 3 The Periodic Table of the Elements QUIZ THURS Oct 20 (front page) Chem 6A Michael J. Sailor, UC San Diego 4

3 The Periodic Table of the Elements QUIZ THURS Oct 20 (back page) Provide the names of the following elements: Element H Li Fr Pt Ag Sb Etc 20 elements total Name hydrogen lithium francium platinum silver antimony Chem 6A Michael J. Sailor, UC San Diego 5 Problem: Mass-to-mass calculations Since the bronze age (4000 b.c.), copper metal has been produced by smelting, in which Cu 2 O ore is reduced with excess carbon (charcoal). How much copper can be produced from smelting of 1.00 kg of pure Cu 2 O? a) 222 g b) 888 g c) 444 g d) 2252 g e) none of the above Chem 6A Michael J. Sailor, UC San Diego 6

4 Solution: Mass-to-mass calculations (1) The balanced equation for the reaction is: 2Cu 2 O + C 4Cu + CO 2 (2) Find out how many moles of Cu are there, then convert to grams Cu: 1000 g Cu 2 O Mol Cu 2 O 4 mol Cu g Cu g Cu 2 O 2 mol Cu 2 O 1 mol Cu = 888 g Cu Chem 6A Michael J. Sailor, UC San Diego 7 Problem: Limiting reactant In the Haber process, hydrogen (H 2 ) reacts with nitrogen (N 2 ) in a reactor to make ammonia. The reactor is initially charged with 2 mol of H 2 and 3 mol of N 2 and the reaction is allowed to go to completion. Fill out the table below indicating the amounts of reactants and products present after the reaction is complete. 3 H 2 + N 2 2 NH 3 Moles H 2 Moles N 2 Moles NH 3 Chem 6A Michael J. Sailor, UC San Diego 8

5 Solution: Limiting reactant The reactor is initially charged with 2 mol of H 2 and 3 mol of N 2 Balanced equation: 3 H 2 + N 2 2 NH 3 If all 2 mol of H 2 reacts, how many moles of N 2 are needed? Before reaction Moles H 2 2 Moles N 2 3 Moles NH 3 0 After reaction Chem 6A Michael J. Sailor, UC San Diego 9 Solution: Limiting reactant The reactor is initially charged with 2 mol of H 2 and 3 mol of N 2 Balanced equation: 3 H 2 + N 2 2 NH 3 If all 2 mol of H 2 reacts, how many moles of N 2 are needed? = 2/3 mol N 2 needed We have 3 mole of N 2, so N 2 is in excess and H 2 is limiting Chem 6A Michael J. Sailor, UC San Diego 10

6 Solution: Limiting reactant The reactor is initially charged with 2 mol of H 2 and 3 mol of N 2 and the reaction is allowed to go to completion. Balanced equation: 3 H 2 + N 2 2 NH 3 Before reaction What s used? What s left? After reaction, Moles H 2 = 2-2 = 0 Moles H Moles N 2 3 2/ Moles NH Moles N 2 = 3-2/3 = 7/3, or 2.33 Moles NH 3 = mol H 2 2 mol NH 3 = 4/3, or mol H 2 Chem 6A Michael J. Sailor, UC San Diego 11 Solution: Limiting reactant What if we chose to calculate it assuming the N 2 is limiting? Balanced equation: 3 H 2 + N 2 2 NH 3 If all 3 mol of N 2 reacts, how many moles of H 2 are needed? Before reaction Moles H 2 2 Moles N 2 3 Moles NH 3 0 After reaction Chem 6A Michael J. Sailor, UC San Diego 12

7 Solution: Limiting reactant If all 3 mol of N 2 reacts, how many moles of H 2 are needed? Balanced equation: 3 H 2 + N 2 2 NH 3 = 9 mol H 2 needed We only have 2 mole of H 2, so H 2 is limiting Chem 6A Michael J. Sailor, UC San Diego 13 Chapter 3: Stoichiometry (cont) Chem 6A, Section D Sept 29, 2011 Chem 6A Michael J. Sailor, UC San Diego 14

8 Problem: Limiting reactant Since the bronze age (4000 b.c.), copper metal has been produced by smelting, in which Cu 2 O ore is reduced with excess carbon (charcoal). How much copper can be produced from smelting of 1.00 kg of pure Cu 2 O with 25 g of charcoal? Assume the byproduct of the reaction is CO2. a) 222 g b) 888 g c) 444 g d) 2252 g e) none of the above Chem 6A Michael J. Sailor, UC San Diego 15 Solution: Limiting reactant The balanced equation for the reaction is: 2Cu 2 O + C 4Cu + CO 2 Find out how many moles of Cu 2 O we have: 1000 g Cu 2 O Mol Cu 2 O g Cu 2 O Find out how many moles of C we have: 25 g C Mol C g C how many moles of C are needed: = 6.99 mol Cu 2 O = 2.08 mol C 1000 g Cu 2 O Mol Cu 2 O 1 mol C g Cu 2 O 2 mol Cu 2 O = 3.49 mol C needed Chem 6A Michael J. Sailor, UC San Diego 16

9 Solution: Limiting reactant We have 2.08 mol C. We need 3.49, so all of the C will be used up before all of the Cu 2 O has reacted. So C (carbon) is the limiting reactant. how many moles of Cu will be produced using this much C? 25 g C Mol C 4 mol Cu g Cu g C 1 mol C Mol Cu = 529 g Cu Chem 6A Michael J. Sailor, UC San Diego 17 Problem: Combustion analysis Combustion analysis is carried out on g of a compound that contains only carbon, hydrogen, and oxygen. The masses of water and carbon dioxide produced are g and g, respectively. What is the empirical formula of the compound? See problem 3.34 from the book Chem 6A Michael J. Sailor, UC San Diego 18

10 Solution: Combustion analysis Like excess-limiting reagent problem except the oxygen is never limiting: C x H y O z + xs O 2 x CO 2 + y/2 H 2 O Figure out number of moles and mass of carbon, hydrogen: g CO 2 1mol CO 2 1 mole C g CO 2 1 mol CO 2 = moles C moles C g C 1 mol C = g C g H 2 O 1mol H 2 O 2 mole H g H 2 O 1 mol H 2 O = moles H moles H g H 1 mol H = g H Chem 6A Michael J. Sailor, UC San Diego 19 Solution: Combustion analysis C x H y O z + xs O 2 x CO 2 + y/2 H 2 O Mass left over = = g mass C x H y O z mass H mass C So g is the mass of O (NOT O 2 ) in the sample. The number of moles of O is: g O 1mol O g O = mol O Chem 6A Michael J. Sailor, UC San Diego 20

11 Solution: Combustion analysis C x H y O z + xs O 2 x CO 2 + y/2 H 2 O Dividing by the least common denominator (O in this case): Element Moles Fraction C H O So the empirical formula is C 2 H 6 O Chem 6A Michael J. Sailor, UC San Diego 21 Water: H!+ 2!- O 105 H!+ Chem 6A Michael J. Sailor, UC San Diego 22

12 Sodium Chloride (NaCl) Crystal Cl - Na + Unit Cell Chem 6A Michael J. Sailor, UC San Diego 23 Dissolution of NaCl in water ion-dipole interactions replace ion-ion interactions Solvent Solute = H 2 O = Na + = Cl - Chem 6A Michael J. Sailor, UC San Diego 24

13 Ethanol in water dipole-dipole interactions: Like Dissolves Like Hydrogen Bonds Chem 6A Michael J. Sailor, UC San Diego 25 Problem: Determine molar concentration What is the molarity of a solution made by adding enough water to 20.0 g of NaCl to make 50.0 ml of solution? MW of NaCl is g/mol. Set up but do not solve. Chem 6A Michael J. Sailor, UC San Diego 26

14 Solution: Determine molar concentration Molarity is defined as moles of solute/liter of solution: 20.0 g NaCl mol NaCl g NaCl L solution (= 6.84 M) Chem 6A Michael J. Sailor, UC San Diego 27 Problem: Dilution calculations What volume of M sucrose solution is needed to make 2.00 L of a 0.05 M sucrose solution? Set up but do not solve. Chem 6A Michael J. Sailor, UC San Diego 28

15 Solution: Dilution calculations 1. How many moles of sucrose are needed? 0.05 mol sucrose 2 Liters Liter = 0.1 mol sucrose 2. What volume of solution do I need? 0.1 mol sucrose Liter mol sucrose = L of solution Chem 6A Michael J. Sailor, UC San Diego 29 Problem: Dilution calculations Calculate the volume (in liters) of a 0.1 M KMnO 4(aq) stock solution that is needed to prepare 250 ml of 1.50 x 10-3 M KMnO 4(aq) (set up but do not solve). Chem 6A Michael J. Sailor, UC San Diego 30

16 Solution: Dilution calculations Volume = 1.5 x 10-3 mol KMnO ml L L L 1000 ml 0.1 mol KMnO 4(aq) (= 3.75 x 10-3 L) Chem 6A Michael J. Sailor, UC San Diego 31 Problem: Titration calculations A g sample of iron ore (mixture of Fe 2 O 3 and SiO 2 ) is dissolved in hydrochloric acid and 22.3 ml of M KMnO 4 are required to reach the stoichiometric point. What is the percent by mass of iron present in the sample? The balanced net ionic equation for the titration reaction is given below: 5Fe 2+ + MnO H + 5Fe 3+ + Mn H 2 O a) 63.6 % b) 7.28 % c) 36.4 % d) 100 % e) none of the above Chem 6A Michael J. Sailor, UC San Diego 32

17 Solution: Titration calculations Find out how many moles of Fe are there: 1.18 x 10-2 mol KMnO ml L 5 mol Fe 2+ L 1000 ml - 1 mol MnO 4(aq) = x 10-3 mol Fe 2+ = x 10-3 mol Fe. How many grams of Fe were there? x 10-3 mol Fe g Fe Mol Fe = grams Fe. So the % by mass Fe is: g/0.202g x 100% = 36.4% Chem 6A Michael J. Sailor, UC San Diego 33 Sections SECTION TIME LOCATION D01 M 2-2:50 pm WLH 2115 D02 M 3-3:50 pm WLH 2115 D03 M 4-4:50 pm WLH 2115 D04 W 2-2:50 pm WLH 2115 D05 W 3-3:50 pm WLH 2115 D06 W 4-4:50 pm WLH 2115 D07 F 2-2:50 pm WLH 2115 D08 F 3-3:50 pm WLH 2115 D09 F 4-4:50 pm WLH Chem 6A Michael J. Sailor, UC San Diego

### INSTRUCTIONS: Exam III. November 10, 1999 Lab Section

CHEM 1215 Exam III John III. Gelder November 10, 1999 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 7 different pages. The last page includes a periodic table and

More information

### 8. Relax and do well.

CHEM 1314.03 Exam I John I. Gelder September 25, 1997 Name TA's Name Lab Section Please sign your name below to give permission to post, by the last 4 digits of your student I.D. number, your course scores

More information

### Fall 2011 CHEM Test 4, Form A

Fall 2011 CHEM 1110.40413 Test 4, Form A Part I. Multiple Choice: Clearly circle the best answer. (60 pts) Name: 1. The common constituent in all acid solutions is A) H 2 SO 4 B) H 2 C) H + D) OH 2. Which

More information

### The Periodic Table of Elements

The Periodic Table of Elements 8 Uuo Uus Uuh (9) Uup (88) Uuq (89) Uut (8) Uub (8) Rg () 0 Ds (9) 09 Mt (8) 08 Hs (9) 0 h () 0 Sg () 0 Db () 0 Rf () 0 Lr () 88 Ra () 8 Fr () 8 Rn () 8 At (0) 8 Po (09)

More information

### 7. Relax and do well.

CHEM 1215 Exam II John II. Gelder October 13, 1999 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 5 different pages. The last page includes a periodic table and a solubility

More information

### Chemistry 1 Second Lecture Exam Fall Abbasi Khajo Kruft Levine Mathias Mathias/Ortiz Metlitsky Rahi Sanchez-Delgado Vasserman

Page 1 of 9 Chemistry 1 Second Lecture Exam Fall 2011 Name Circle the name of your recitation/lab instructor(s) Abbasi Khajo Kruft Levine Mathias Mathias/Ortiz Metlitsky Rahi Sanchez-Delgado Vasserman

More information

### Atoms and the Periodic Table

Atoms and the Periodic Table Parts of the Atom Proton Found in the nucleus Number of protons defines the element Charge +1, mass 1 Parts of the Atom Neutron Found in the nucleus Stabilizes the nucleus

More information

### Chemistry Standard level Paper 1

M17/4/EMI/SPM/ENG/TZ1/XX hemistry Standard level Paper 1 Thursday 11 May 2017 (afternoon) 45 minutes Instructions to candidates Do not open this examination paper until instructed to do so. Answer all

More information

### CHEM 130 Exp. 8: Molecular Models

CHEM 130 Exp. 8: Molecular Models In this lab, we will learn and practice predicting molecular structures from molecular formulas. The Periodic Table of the Elements IA 1 H IIA IIIA IVA VA VIA VIIA 3 5

More information

### Ch. 9 NOTES ~ Chemical Bonding NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.

Ch. 9 NOTES ~ Chemical Bonding NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. I. Review: Comparison of ionic and molecular compounds Molecular compounds Ionic

More information

### Circle the letters only. NO ANSWERS in the Columns!

Chemistry 1304.001 Name (please print) Exam 5 (100 points) April 18, 2018 On my honor, I have neither given nor received unauthorized aid on this exam. Signed Date Circle the letters only. NO ANSWERS in

More information

### 8. Relax and do well.

CHEM 1225 Exam I John I. Gelder February 4, 1999 Name KEY TA's Name Lab Section Please sign your name below to give permission to post your course scores on homework, laboratories and exams. If you do

More information

### Made the FIRST periodic table

Made the FIRST periodic table 1869 Mendeleev organized the periodic table based on the similar properties and relativities of certain elements Later, Henri Moseley organized the elements by increasing

More information

### Circle the letters only. NO ANSWERS in the Columns! (3 points each)

Chemistry 1304.001 Name (please print) Exam 4 (100 points) April 12, 2017 On my honor, I have neither given nor received unauthorized aid on this exam. Signed Date Circle the letters only. NO ANSWERS in

More information

### Chemistry Standard level Paper 1

Chemistry Standard level Paper 1 Thursday 12 May 2016 (morning) 45 minutes Instructions to candidates Do not open this examination paper until instructed to do so. Answer all the questions. For each question,

More information

### A little history. When and How? Sir William Ramsey. ü 12/5/13. ü 1. Who put together the first useable Periodic Table?

ü // A little history Johahann Dobereiner (80-89) o Triads John Newlands (8-898) o Law of Octaves Who put together the first useable ic Table? Mendeleev you remember him right? When and How? You know it

More information

### 30 Zn(s) 45 Rh. Pd(s) Ag(s) Cd(s) In(s) Sn(s) white. 77 Ir. Pt(s) Au. Hg(l) Tl. 109 Mt. 111 Uuu. 112 Uub. 110 Uun. 65 Tb. 62 Sm. 64 Gd. 63 Eu.

Enthalpy changes: experimentally it is much easier to measure heat flow at const pressure - this is enthalpy q p = )H : also nearly all chemical reactions are done at constant pressure. Enthalpy (heat)

More information

### Chemistry 126 Final Examination, Prof. Hanson, May, Section B or D (circle one) Seat Coordinate Name

Chemistry 126 Final Examination, Prof. Hanson, May, 2004 Section B or D (circle one) Seat Coordinate Name DO NOT OPEN THIS EXAM UNTIL INSTRUCTED TO DO SO Each asterisk () is 5 points. There are 40 s, for

More information

### SCIENCE 1206 UNIT 2 CHEMISTRY. September 2017 November 2017

SCIENCE 1206 UNIT 2 CHEMISTRY September 2017 November 2017 UNIT OUTLINE 1. Review of Grade 9 Terms & the Periodic Table Bohr diagrams Evidence for chemical reactions Chemical Tests 2. Naming & writing

More information

### Atomic Structure & Interatomic Bonding

Atomic Structure & Interatomic Bonding Chapter Outline Review of Atomic Structure Atomic Bonding Atomic Structure Atoms are the smallest structural units of all solids, liquids & gases. Atom: The smallest

More information

### 9/20/2017. Elements are Pure Substances that cannot be broken down into simpler substances by chemical change (contain Only One Type of Atom)

CAPTER 6: TE PERIODIC TABLE Elements are Pure Substances that cannot be broken down into simpler substances by chemical change (contain Only One Type of Atom) The Periodic Table (Mendeleev) In 1872, Dmitri

More information

### NAME: SECOND EXAMINATION

1 Chemistry 64 Winter 1994 NAME: SECOND EXAMINATION THIS EXAMINATION IS WORTH 100 POINTS AND CONTAINS 4 (FOUR) QUESTIONS THEY ARE NOT EQUALLY WEIGHTED! YOU SHOULD ATTEMPT ALL QUESTIONS AND ALLOCATE YOUR

More information

### Chapter 12 The Atom & Periodic Table- part 2

Chapter 12 The Atom & Periodic Table- part 2 Electrons found outside the nucleus; negatively charged Protons found in the nucleus; positive charge equal in magnitude to the electron s negative charge Neutrons

More information

### Modified from: Larry Scheffler Lincoln High School IB Chemistry 1-2.1

Modified from: Larry Scheffler Lincoln High School IB Chemistry 1-2.1 The development of the periodic table brought a system of order to what was otherwise an collection of thousands of pieces of information.

More information

### 6.3 Classifying Elements with the Periodic Table

6.3 Classifying Elements with the Periodic Table The Periodic Table was developed by scientists to organize elements in such a way as to make sense of the growing information about their properties. The

More information

### Atomic Emission Spectra. and. Flame Tests. Burlingame High School Chemistry

Atomic Structure Atomic Emission Spectra and Flame Tests Flame Tests Sodium potassium lithium When electrons are excited they bump up to a higher energy level. As they bounce back down they release energy

More information

### E5 Lewis Acids and Bases: lab 2. Session two lab Parts 2B, 3, and 4. Session one lab Parts 1and 2A. Aquo Complex Ions

E5 Lewis Acids and Bases: lab 2 Session one lab Parts 1and 2A Session two lab Parts 2B, 3, and 4 Part 2B. Complexation, Structure and Periodicity Compare the reactivity of aquo complex ions containing

More information

### What is the periodic table?

The periodic table of the elements represents one of the greatest discoveries in the history of science that certain elements, the basic chemical substances from which all matter is made, resemble each

More information

### Grade 11 Science Practice Test

Grade 11 Science Practice Test Nebraska Department of Education 2012 Directions: On the following pages of your test booklet are multiple-choice questions for Session 1 of the Grade 11 Nebraska State Accountability

More information

### CHEMISTRY 102 Fall 2014 HOUR EXAM I Page 1

OUR EXAM I Page 1 1. Draw the Lewis structure for ICl5. ow many of the following four statements (I-IV) is/are true regarding ICl5? I. The central atom in ICl5 has one lone pair of electrons. II. Some

More information

### Chemistry 12 Name Exam I Form A Section February 7, 2001 Student No.

Chemistry 12 Name Exam I Form A Section February 7, 2001 Student No. IMPRTANT: n the scantron (answer sheet), you MUST clearly fill your name, your student number, section number, and test form (white

More information

### Stoichiometry. Mole Concept. Balancing Chemical Equations

Stoichiometry The story so far The structure of an atom protons, neutrons & electrons Electron structure & the Periodic Table Shapes of electron orbitals (Quantum Numbers) Essential and toxic elements

More information

### UNIVERSITY LE CAMPUS. Moderators Dr D. Reddy Dr B. Moodley. Dr L. Pillay Dr G. Birungii. This paper inclusive). answer booklet.

SCHOOL OF CHEMISTRY & PHYSICS UNIVERSITY OF KWAZULU-NATAL, WESTVILL LE CAMPUS APCH231 : CHEMICAL ANALYSIS NOVEMBER 2013 MAIN EXAMINATIONN DURATION: 3 HOURS TOTAL MARKS: 100 Moderators Dr D. Reddy Dr B.

More information

### single-layer transition metal dichalcogenides MC2

single-layer transition metal dichalcogenides MC2 Period 1 1 H 18 He 2 Group 1 2 Li Be Group 13 14 15 16 17 18 B C N O F Ne 3 4 Na K Mg Ca Group 3 4 5 6 7 8 9 10 11 12 Sc Ti V Cr Mn Fe Co Ni Cu Zn Al Ga

More information

### Experiment Three. Lab two: Parts 2B and 3. Halogens used in Parts 2 and 3. Lab one: Parts 1 and 2A. Halogens (Family VIIA) used in Parts 2 and 3

Experiment Three Lab one: Parts 1 and 2A Lab two: Parts 2B and 3 1 1A 1 H 1s 1 2 IIA 3 Li 2s 1 1 1 Na 3s 1 1 9 K 4s 1 3 7 Rb 5s 1 5 5 Cs 6s 1 8 7 Fr 7s 1 4 Be 2s 2 1 2 Mg 3s 2 3 IIIB 4 IVB 5 VB 6 VIB 7

More information

### Halogens HALOGENS. Parts 2A and 2B. Chem : Feb. 19, 20 and March 3. Compare the properties and reactivity of the halogens and halides

Chem. 125-126: Feb. 19, 20 and March 3 Experiment 3 Session 2 (Three hour lab) Complete Experiment 3 Parts 2B and 3 Complete team report Complete discussion presentation Parts 2A and 2B Compare the properties

More information

### CHEM 108 (Fall-2003) Exam Final (100 pts)

CHEM 108 (Fall-2003) Exam Final (100 pts) Name: -------------------------------------------------------------------------------, SSN -------------------------------- LAST NAME, First (Circle the alphabet

More information

### [ ]:543.4(075.8) 35.20: ,..,..,.., : /... ;. 2-. ISBN , - [ ]:543.4(075.8) 35.20:34.

.. - 2-2009 [661.87.+661.88]:543.4(075.8) 35.20:34.2373-60..,..,..,..,.. -60 : /... ;. 2-. : -, 2008. 134. ISBN 5-98298-299-7 -., -,,. - «,, -, -», - 550800,, 240600 «-», -. [661.87.+661.88]:543.4(075.8)

More information

### Reporting Category 1: Matter and Energy

Name: Science Teacher: Reporting Category 1: Matter and Energy Atoms 8.5A Fill in the missing information to summarize what you know about atomic structure. Name of Subatomic Particle Location within the

More information

### Spin Cut-off Parameter of Nuclear Level Density and Effective Moment of Inertia

Commun. Theor. Phys. (Beijing, China) 43 (005) pp. 709 718 c International Academic Publishers Vol. 43, No. 4, April 15, 005 Spin Cut-off Parameter of Nuclear Level Density and Effective Moment of Inertia

More information

### Chemistry Higher level Paper 1

hemistry igher level Paper 1 Thursday 11 May 2017 (afternoon) 1 hour Instructions to candidates Do not open this examination paper until instructed to do so. Answer all the questions. For each question,

More information

### VIIIA H PREDICTING CHARGE

58 IA PREDICTING CHARGE VIIIA H IIA IIIA IVA VA VIA VIIA You can reliably determine the charge using our method for Groups IA, IIA, IIIB, Aluminum, and the Group VA, VIA, and VIIA NONMETALS Li Be B C N

More information

### Thermochemistry. Chapter 6. Chemistry E1a

Thermochemistry Chapter 6 Chemistry E1a Energy: What is it? How is it transformed? What is energy? What are the SI units for energy? Give examples of some energy What types of energy are we going to be

More information

### Chemistry 51 Exam #3. Name KEY November 20, 2001

Chemistry 51 Exam #3 Name KEY November 20, 2001 This exam has nine (9) questions. Please check before beginning to make sure no questions are missing. All scratch work must be done on the attached blank

More information

### (FIRST) IONIZATION ENERGY

181 (FIRST) IONIZATION ENERGY - The amount of energy required to remove a single electron from the outer shell of an atom. - Relates to reactivity for metals. The easier it is to remove an electron, the

More information

### EXAMPLES. He VIA VIIA Li Be B C N O F Ne

59 IA EXAMPLES VIIIA H IIA IIIA IVA VA He VIA VIIA Li Be B C N O F Ne Na Mg IIIB IVB VB Al Si P VIB VIIB VIIIB IB IIB S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru

More information

### Principles of Chemistry I 3150: EXAM I Thursday, 5:10PM EXAM FOR PRACTICE USE FALL 2017

Name Bubble on your scan sheet the Test Number and Test Form below: Principles of Chemistry I 3150:151-800 EXAM I Thursday, 5:10PM EXAM FOR PRACTICE USE FALL 2017 TEST 6, FORM A September 29, 2016 200+

More information

### 8. Relax and do well.

EM 1515.001 Exam III John III. Gelder November 7, 2001 Name TA's Name Lab Section INSTRUTIONS: 1. This examination consists of a total of 9 different pages. The last three pages include a periodic table,

More information

### - Some properties of elements can be related to their positions on the periodic table.

179 PERIODIC TRENDS - Some properties of elements can be related to their positions on the periodic table. ATOMIC RADIUS - The distance between the nucleus of the atoms and the outermost shell of the electron

More information

### 1. Following Dalton s Atomic Theory, 2. In 1869 Russian chemist published a method. of organizing the elements. Mendeleev showed that

20 CHEMISTRY 11 D. Organizing the Elements The Periodic Table 1. Following Dalton s Atomic Theory, By 1817, chemists had discovered 52 elements and by 1863 that number had risen to 62. 2. In 1869 Russian

More information

### Chemistry 1 Final Exam Dec Circle one: Abassi Castillo Ciskowska Jarzecki Kahanda Shakya

Chemistry 1 Final Exam Dec. 2005 Name Circle one: Abassi Castillo Ciskowska Jarzecki Kahanda Shakya Write your name on this page and on the next page. For questions 33 45 you must show work. The exam adds

More information

### The 18 Electron Rule. References: Gray: chapter 5 OGN: chapter 18

The 18 Electron Rule References: Gray: chapter 5 OGN: chapter 18 Element Groups Alkali metals nert or Noble gases Alkali earths alogens e Li Na Be Mg Transition metals B Al Si N P O S F l Ne Ar K Rb s

More information

### ... but using electron configurations to describe how aluminum bromide forms is a bit cumbersome! Can we simplify the picture a bit?

193... but using electron configurations to describe how aluminum bromide forms is a bit cumbersome! Can we simplify the picture a bit? LEWIS NOTATION / ELECTRON-DOT NOTATION - Lewis notation represents

More information

### Lewis dot structures for molecules

1 Lewis dot structures for molecules In the dot structure of a molecule, - SHARED valence electrons are shown with dashes - one per pair. - UNSHARED valence electrons ("lone pairs") are represented by

More information

### UW CHEM 120 Summer ALWAYS express any numerical value with units and significant figures. This includes intermediate values in calculations!

Exam 3 Review Tips for Success on Exams: Show ALL YOUR WORK when solving numerical problems. ALWAYS express any numerical value with units and significant figures. This includes intermediate values in

More information

### Bronsted: Acids are proton donors. Session one Pre-lab (p.151) due 1st hour discussion of E4 Lab (Parts 1and 2A)

E5 Lewis Acids and Bases (Session 1) November 5-11 Acids Bronsted: Acids are proton donors. Session one Pre-lab (p.151) due 1st hour discussion of E4 Lab (Parts 1and 2A) Problem Compounds containing cations

More information

### Chem 6 Sample exam 2 (150 points total) NAME:

hem 6 Sample exam 2 (150 points total) @ This is a closed book exam to which the onor Principle applies. @ The last page contains equations and physical constants; you can detach it for easy reference.

More information

### Electrons. Unit H Chapter 6

Electrons Unit H Chapter 6 1 Electrons were discovered by 1. Dalton 2. Lavoisier 3. Proust 4. Mendeleev 6. Rutherford 7. Bohr 8. Schrodinger 9. Dirac 5. Thomson 2 Electrons were discovered by 1. Dalton

More information

### Atoms and The Periodic Table

Atoms and The Periodic Table A. Early Models of the Atom 1. The earliest models of the atom came in the 5 th century B.C. when In the 4 th century, B.C., rejected this idea and proposed that earthly matter

More information

### - Some properties of elements can be related to their positions on the periodic table.

179 PERIODIC TRENDS - Some properties of elements can be related to their positions on the periodic table. ATOMIC RADIUS - The distance between the nucleus of the atoms and the outermost shell of the electron

More information

### Chapter 3: Compounds

Chapter 3: Compounds Chapter 3 Educational Goals 1. Understand where electrons are located in atoms and how the locations of electrons affect the energy of the atom. 2. Define the term valence electron

More information

### NAME: 3rd (final) EXAM

1 Chem 64 Winter 2003 AME: 3rd (final) EXAM THIS EXAM IS WORTH 100 POITS AD COTAIS 9 QUESTIOS THEY ARE OT EQUALLY WEIGHTED! YOU SHOULD ATTEMPT ALL QUESTIOS AD ALLOCATE YOUR TIME ACCORDIGLY IF YOU DO'T

More information

### 8. Relax and do well.

CHEM 1515 Name Exam III TA's Name John III. Gelder April 7, 1993 Lab Section INSTRUCTIONS: 1. This examination consists of a total of 8 different pages. The last 2 pages include important mathematical

More information

### VIIIA He IIA IIIA IVA VA VIA VIIA. Li Be B C N O F Ne. Na Mg VIB VIIB VIIIB IB IIB S. K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br

188 THE FIRST TWO PERIODIC TRENDS IN A NUTSHELL LARGER IONIZATION ENERGY SMALLER RADIUS IA H IIA IIIA IVA VA VIA VIIA VIIIA He Li Be B C N O F Ne Na Mg IIIB IVB VB Al Si P VIB VIIB VIIIB IB IIB S Cl Ar

More information

### Chemistry 112 Name Exam I Form A Section January 29,

Chemistry 112 Name Exam I Form A Section January 29, 2013 email IMPORTANT: On the scantron (answer sheet), you MUST clearly fill your name, your student number, section number, and test form (white cover

More information

### INSTRUCTIONS: (1) Write your name in the blank titled "NAME" on the scantron form provided.

INSTRUCTIONS: (1) Write your name in the blank titled "NAME" on the scantron form provided. (2) Write your section number in the blank titled "SUBJECT" on the scantron form. (3) Write your Student ID number

More information

### Chapter 2 Lecture Notes: Atoms

Educational Goals Chapter 2 Lecture Notes: Atoms 1. Describe the subatomic structure of an atom. 2. Define the terms element and atomic symbol. 3. Understand how elements are arranged in the periodic table

More information

### Polar bonds, polar molecules and the shape of molecules.

Chapter 3 Polar bonds, polar molecules and the shape of molecules. Polar and non-polar bonds In homonuclear diatomic molecules such as H 2 or Cl 2 electrons are shared equally between equal atoms. The

More information

### E4 Acids, Bases, and Salts

E4 Acids, Bases, and Salts Session One of two session lab Complete Parts 1 and 2 in lab. If time allows, start or complete Part 3. Acids and Bases Q. Are acid-base properties of substances predictable

More information

### - Some properties of elements can be related to their positions on the periodic table.

186 PERIODIC TRENDS - Some properties of elements can be related to their positions on the periodic table. ATOMIC RADIUS - The distance between the nucleus of the atoms and the outermost shell of the electron

More information

### Name Date Class STUDY GUIDE FOR CONTENT MASTERY. covalent bond molecule sigma bond exothermic pi bond

Covalent Bonding Section 9.1 The Covalent Bond In your textbook, read about the nature of covalent bonds. Use each of the terms below just once to complete the passage. covalent bond molecule sigma bond

More information

### Atomic terms. Example: Helium has an atomic number of 2. Every helium atom has two protons in its nucleus.

Atomic terms - ATOMIC NUMBER: The number of protons in the atomic nucleus. Each ELEMENT has the SAME NUMBER OF PROTONS in every nucleus. In neutral atoms, the number of ELECTRONS is also equal to the atomic

More information

### Periodic Table. Modern periodic table

41 Periodic Table - Mendeleev (1869): --- When atoms are arranged in order of their atomic weight, some of their chemical and physical properties repeat at regular intervals (periods) --- Some of the physical

More information

### Mass Relationships in Chemical Reactions

Mass Relationships in Chemical Reactions Chapter 3 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Micro World atoms & molecules Macro World grams Atomic mass

More information

### c. K 2 CO 3 d. (NH 4 ) 2 SO 4 Answer c

Chem 130 Name Exam 2, Ch 4-6 July 7, 2016 100 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct units and

More information

### History of the Periodic Table

SECTION 5.1 History of the Periodic Table By 60, more than 60 elements had been discovered. Chemists had to learn the properties of these elements as well as those of the many compounds that the elements

More information

### PROOF/ÉPREUVE ISO INTERNATIONAL STANDARD. Space environment (natural and artificial) Galactic cosmic ray model

INTERNATIONAL STANDARD ISO 15390 First edition 2004-##-## Space environment (natural and artificial) Galactic cosmic ray model Environnement spatial (naturel et artificiel) Modèle de rayonnement cosmique

More information

### CHEMISTRY 1A SPRING 2011 EXAM 1 KEY CHAPTERS 1-4

You might find the following useful. Electronegativities H 2.2 CHEMISTRY 1A SPRING 2011 EXAM 1 KEY CHAPTERS 1- Li Be B C N O F 0.98 1.57 2.0 2.55.0..98 Na Mg Al Si P S Cl 0.9 1.1 1.61 1.9 2.19 2.58.16

More information

### 1.02 Elements, Symbols and Periodic Table

.0 Elements, Symbols and Periodic Table Dr. Fred O. Garces Chemistry Miramar College.0 Elements, Symbols and the Periodic Table January 0 The Elements: Building block of Matter The periodic table of the

More information

### 4.01 Elements, Symbols and Periodic Table

.0 Elements, Symbols and Periodic Table Dr. Fred O. Garces Chemistry 00 Miramar College.0 Elements, symbols and the Periodic Table Aug The Elements: Building block of Matter The periodic table of the chemical

More information

### Name Section Signature TA ID #

FIRST LETTER OF YOUR LAST NAME CHEMISTRY 118 EXAM II March 8, 014 Name Section Signature TA ID # PLEASE READ THE FOLLOWING INSTRUCTIONS Do NOT begin the exam until asked to do so. There are 8 numbered

More information

### Example: Helium has an atomic number of 2. Every helium atom has two protons in its nucleus.

59 Atomic terms - ATOMIC NUMBER: The number of protons in the atomic nucleus. Each ELEMENT has the SAME NUMBER OF PROTONS in every nucleus. In neutral atoms, the number of ELECTRONS is also equal to the

More information

### E4 Acids, Bases, and Salts

E4 Acids, Bases, and Salts Session One of two session lab Complete Parts 1 and 2 in lab. If time allows, start or complete Part 3. Reminder: Pre-lab report, page 112, due at start of lab. Acids and Bases

More information

### Steward Fall 08. Moles of atoms/ions in a substance. Number of atoms/ions in a substance. MgCl 2(aq) + 2 AgNO 3(aq) 2 AgCl (s) + Mg(NO 3 ) 2(aq)

Dealing with chemical stoichiometry Steward Fall 08 of Not including volumetric stoichiometry of Chapter 6.0x10 A 6.0x10 Mol/mol ratio from balanced equation B 6.0x10 6.0x10 s, Equations, and Moles: II

More information

### 1. The arrangement of the elements from left to right in Period 4 on the Periodic Table is based on

1. The arrangement of the elements from left to right in Period 4 on the Periodic Table is based on A) atomic mass B) atomic number C) the number of electron shells D) the number of oxidation states 2.

More information

### Writing Chemical formula with polyatomic groups

Writing Chemical formula with polyatomic groups 1. Use the Periodic table to determine the combining powers of single elements. Eg. Magnesium is in Group 2 and has a combining power of 2. 2. Use Table

More information

### Attention: Please study problem set 1, 2, 5 and 6 as well. This review does not contain these chapters.

Chemistry 101 Review for Final Attention: Please study problem set 1, 2, 5 and 6 as well. This review does not contain these chapters. 1. Use the following ions to write the chemical formula for each ionic

More information

### E4 Acids, Bases, and Salts

E4 Acids, Bases, and Salts Session One of two session lab Complete Parts 1 and 2 in lab. If time allows, start or complete Part 3. Reminder: Prelab report, page 112, due at start of lab. Acids and Bases

More information

### ICP/MS Multi-Element Standards

Standards Ultra Pure Matrix Special Packaging Traceability to National Reference Materials AccuStandard s ICP/MS Standards are formulated to meet the needs of this very special instrument. As matrix effect

More information

### CHAPTER 7: CHEMICAL FORMULAS AND CHEMICAL COMPOUNDS. Chemistry 1-2 Enriched Mr. Chumbley

CHAPTER 7: CHEMICAL FORMULAS AND CHEMICAL COMPOUNDS Chemistry 1-2 Enriched Mr. Chumbley SECTION 1: CHEMICAL NAMES AND FORMULAS While the bulk of the content will come from the Naming Chemical Compounds

More information

### Class XI Chapter 1 Some Basic Concepts of Chemistry Chemistry

Question 1.1: Calculate the molecular mass of the following: (i) H 2 O (ii) CO 2 (iii) CH 4 (i) H 2 O: The molecular mass of water, H 2 O = (2 Atomic mass of hydrogen) + (1 Atomic mass of oxygen) = [2(1.0084)

More information

### 5. [7 points] What is the mass of gallons (a fifth) of pure ethanol (density = g/cm 3 )? [1 gallon = Liters]

1 of 6 10/20/2009 3:55 AM Avogadro s Number, N A = 6.022 10 23 1. [7 points] Given the following mathematical expression: (15.11115.0)/(2.154 10 3 ) How many significant figures should the answer contain?

More information

### Exploration Geochemistry Basic Principles and Concepts Coordinator: Bill Coker BHP Billiton World Exploration Inc

Exploration In The New Millenium Exploration Geochemistry Basic Principles and Concepts Coordinator: Bill Coker BHP Billiton World Exploration Inc Introduction Exploration Geochemistry - Definition Basic

More information

### Chapter 2 Atoms and the Periodic Table

Chapter 2 1 Chapter 2 Atoms and the Periodic Table Solutions to In-Chapter Problems 2.1 Each element is identified by a one- or two-letter symbol. Use the periodic table to find the symbol for each element.

More information

### !!! DO NOT OPEN THIS EXAM BOOK UNTIL TOLD TO DO SO BY THE INSTRUCTOR!!!

CHEM 142 - Exam 1 Version B!!! DO NOT OPEN THIS EXAM BOOK UNTIL TOLD TO DO SO BY THE INSTRUCTOR!!! Instructor: Dr. Kari Pederson NO GRAPHING CALCULATORS ALLOWED Date: Friday, July 15 ONLY CALCULATORS MAY

More information

### Unit 4: Reactions and Stoichiometry

Unit 4: Reactions and Stoichiometry Reactions Chemical equation Expression representing a chemical reaction Formulas of reactants on the left side Formulas of products on the right side Arrow(s) connect(s)

More information

### 1 Arranging the Elements

CHAPTER 12 1 Arranging the Elements SECTION The Periodic Table BEFORE YOU READ After you read this section, you should be able to answer these questions: How are elements arranged on the periodic table?

More information

### Chemistry 101 Chapter 4 STOICHIOMETRY

STOICHIOMETRY Stoichiometry is the quantitative relationship between the reactants and products in a balanced chemical equation. Stoichiometry allows chemists to predict how much of a reactant is necessary

More information

### Problem Set III Stoichiometry - Solutions

Chem 121 Problem set III Solutions - 1 Problem Set III Stoichiometry - Solutions 1. 2. 3. molecular mass of ethane = 2(12.011) + 6(1.008) = 30.07 g 4. molecular mass of aniline = 6(12.011) + 7(1.008) +

More information

### Honors text: Ch 10 & 12 Unit 06 Notes: Balancing Chemical Equations

Notes: Balancing Chemical Equations Effects of chemical reactions: Chemical reactions rearrange atoms in the reactants to form new products. The identities and properties of the products are completely

More information