8. Relax and do well.

Save this PDF as:
 WORD  PNG  TXT  JPG

Size: px
Start display at page:

Download "8. Relax and do well."

Transcription

1 CHEM Exam II KEY ohn II. Gelder October 23, 1997 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 9 different pages. The last four pages include a periodic table, a solubility table, a table of enthalpy's of formation, an activity series and some useful equations. All work should be done in this booklet. 2. PRINT your name, TA's name and your lab section number now in the space at the top of this sheet. DO NOT SEPARATE THESE PAGES. 3. Answer all questions that you can and whenever called for show your work clearly. Your method of solving problems should pattern the approach used in lecture. You do not have to show your work for the multiple choice or short answer questions. 4. No credit will be awarded if your work is not shown in problems Point values are shown next to the problem number. 6. Budget your time for each of the questions. Some problems may have a low point value yet be very challenging. If you do not recognize the solution to a question quickly, skip it, and return to the question after completing the easier problems. 7. Look through the exam before beginning; plan your work; then begin. 8. Relax and do well. Page 2 Page 3 Page 4 Page 5 TOTAL SCORES (34) (25) (21) (20) (100)

2 CHEM 1314 EXAM II PAGE 2 (12) 1. Write the chemical formula(s) of the product(s) and balance the following reactions. Identify all products phases as either (g)as, (l)iquid, (s)olid or (aq)ueous. If no reaction occurs write NR. a) 2Al(s) + Fe 2 O 3 (s) Al 2 O 3 (s) + 2Fe(l) b) Na 2 SO 4 (aq) + 2NH 4 Cl(aq) (NH 4 ) 2 SO 4 (aq) + 2NaCl(aq) c) Mg(s) + Cu 2+ (aq) Mg 2+ (aq) + Cu(s) d) 3Na 2 CO 3 (aq) + 2Fe(NO 3 ) 3 (aq) 6NaNO 3 (aq) + Fe 2 (CO 3 ) 3 (s) (12) 2. Write the ionic and net ionic chemical equations for 1b) and 1d). 1b) Ionic equation: 2NH 4 + (aq) + SO 4 2 (aq) + 2Na + (aq)) + 2Cl (aq) 2NH 4 + (aq) + SO 4 2 (aq) + 2Na + (aq)) + 2Cl (aq) Net Ionic equation: 2NH 4 + (aq) + SO 4 2 (aq) + 2Na + (aq) + 2Cl (aq) 2NH 4 + (aq) + SO 4 2 (aq) + 2Na + (aq) + All ions cancel..no net ionic equation...no 2Cl (aq) reaction. 1d) Ionic equation: 6Na + (aq) + 3CO 3 2 (aq) + 2Fe 3+ (aq) + 6NO 3 (aq) 6Na + (aq) + Fe 2 (CO 3 ) 3 (s) + 6NO 3 (aq) Net Ionic equation: 6Na + (aq) + 3CO 3 2 (aq) + 2Fe 3+ (aq) + 6NO 3 (aq) 6Na + (aq) + Fe 2 (CO 3 ) 3 (s) + 6NO 3 (aq) 2Fe 3+ (aq) + 3CO 3 2 (aq) Fe 2 (CO 3 ) 3 (s) (10) 3. An explosive, trinitrotoluene, is prepared by reacting toluene with nitric acid according to the equation C 7 H 8 (l) + 3HNO 3 (aq) C 7 H 5 (NO 2 ) 3 (l) + 3H 2 O(l) What mass of toluene and nitric acid are required to produce 50.0 g of trinitrotoluene? 50.0 g TNT 1 mol = Mol TNT 227 g Mol TNT 1 mol C 7 H 8 1 mol TNT 92.0 g 1 mol C 7 H = 20.3 g C 7 H Mol TNT 3molHNO 3 1molTNT 63.0 g 1 mol HNO = 41.6 g HNO 3 3

3 CHEM 1314 EXAM II PAGE 3 (15) 4. Boric acid is formed in the reaction between boron trifluoride and water. The reaction is, 4BF 3 + 3H 2 O H 3 BO 3 + 3HBF 4 What is the maximum number of grams of boric acid which can be obtained when 150. g of boron trifluoride is reacted with 35.0 g of water? 150. g BF 3 1 mol BF g = 2.21 mol B 35.0 g H 2 O 1 mol H 2 O = g mol H 2 O 2.21 mol BF 3 3 mol H 2 O = 1.66 mol H 4 mol BF 2 O required mol H 2 O required and 1.94 mol H 2 O are available. So the water is in excess and BF 3 is limiting mol BF 3 1 mol H 3 BO g 4 mol BF 3 1 mol H 3 BO = 34.1 g H 3 BO 3 3 Calculate the final mass of both reactants after the reaction has gone to completion. 0 g of BF 3 left 1.66 mol H 2 O 18.0 g H 2 O 1 mol H 2 O = 29.9 g H O reacted g 29.9 g = 5.1 g H 2 O remain unreacted. (10) 5. Calculate the mass of oxalic acid that reacts with mls of 2.44 x 10-3 M KMnO 4 in excess sulfuric acid. The equation which describes the reaction between oxalic acid, potassium permanganate and sulfuric acid is, 2KMnO 4 (aq) + 5H 2 C 2 O 4 (aq) + 3H 2 SO 4 (aq) K 2 SO 4 (aq) + 2MnSO 4 (aq) + 10CO 2 (g) + 8H 2 O(l) mls 1 L 1000 mls 2.44 x 10 3 mol KMnO 4 1 L 5 mol H 2 C 2 O 4 2 mol KMnO g 1 mol H 2 C 2 O g of H 2 C 2 O 4

4 CHEM 1314 EXAM II PAGE 4 (9) 6. The industrial preparation of nitric acid, the Ostwald Process, converts ammonia to nitric acid. Using the following standard enthalpy of reaction data and Hess' Law determine the enthalpy for production of nitric acid from ammonia. (Note: While ammonia and nitric acid are the only two substances mentioned it should be realized other substances may be needed to obtain a balanced chemical equation which describes the conversion of ammonia to nitric acid.) Reaction 4NH 3 (g) + 5O 2 (g) 4NO(g) + 6H 2 O(g) 2NO(g) + O 2 (g) 2NO 2 (g) 3NO 2 (g) + H 2 O(g) 2HNO 3 (aq) + NO(g) H 907 k 114 k 182 k Clearly demonstrate how the given equations are to be manipulated to obtain the final equation. 4NH 3 (g) + 5O 2 (g) 4NO(g) + 6H 2 O (g) 907 k 3 (2NO(g) + O 2 (g) 2NO 2 (g)) 114 k 3 2 (3NO 2 (g) + H 2 O(g) 2HNO 3 (aq ) + NO(g)) 182 k 2 4NH 3 (g) + 8O 2 (g) 4HNO 3 (aq ) + 4H 2 O (g) 1613 k (12)7a. When a sulfide is combusted sulfur dioxide is a product. Calculate H rxn for the combustion of zinc sulfide. 2ZnS(s) + 3O 2 (g) 2ZnO(s) + 2SO 2 (g) H rxn = Σ H f (products) - Σ H f (reactants) H rxn = 2 mol -348 k mol + 2 mol -297 k mol - 2 mol -206 k + 3 mol mol 0 k = -878 k (2 mol ZnS) mol 1

5 CHEM 1314 EXAM II PAGE 5 (20)8a g of water at 33.0 C are added to 24.0 g of water, in a calorimeter, at 21.0 C. The final temperature of the mixture is 27.8 C. Calculate the heat capacity of the calorimeter. q hot = (q cold + q calorimeter ) g (27.8 C 33.0 C) = (4.184 g C g C 24.0 g (27.8 C 21.0 C) + HC calorimeter (27.8 C 21.0 C)) 979 = (682 + HC calorimeter 6.8 C) HC calorimeter = C = 43.7 C b g of KOH are added to the same calorimeter used in the experiment in part a) above which now holds 50.0 mls of water. The initial temperature of the water in the calorimeter 22.6 C. If the final temperature of the solution in the calorimeter after adding the KOH is 31.2 C, calculate the molar heat of solution for KOH. (Assume the specific heat of the solution is equal to the specific heat of pure water.) q reaction = (q solution + q calorimeter ) q reaction = (4.184 g C g (31.2 C 22.6 C) C C)) 2246 = 1.98 g KOH 56.0 g 1 mol KOH = 63.5 k mol 1 (31.2 C 22.6

6 CHEM 1314 EXAM II PAGE IA 1 H Li IIA 4 Be Na Mg K Ca Rb Sr Cs Ba Fr (223) Ra IIIA IVA VA VIA VIIA B C N O F 9 10 Ne IIIB IVB VB VIB VIIB VIII IB IIB Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe (98) La Periodic Table of the Elements Hf Al Si P S Cl VIIIA 2 Ta W Re 75 Os Ir Pt Au Hg 80 Tl Pb Bi Po At Rn (209) (210) Ac Rf Db Sg Bh Hs Mt (261) (262) (263) (262) (265) (266) He Ar (222) Lanthanides Actinides Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu (145) Th Pa U Np Pu AmCm Bk Cf Es Fm Md No Lr (244) (243) (247) (247) (251) (252) (257) (258) (259) (260) Useful Information Specific heat of H 2 O(s) = 2.09 g C Specific heat of H 2 O(l) = g C Specific heat of H 2 O(g) = 1.84 g C Heat of fusion of H 2 O(s) = 6.01 k mol Heat of vaporization of H 2 O(l) = k mol R = L. atm mol. K or R = mol. K q(heat flow) = mass specific heat T q reaction = (q calorimeter + q solution ) q reaction = (q calorimeter + q water ) H rxn = Σ n H f (products) - Σ m H f (reactants) H = E + nrt

7 CHEM 1314 EXAM II PAGE 7 Solubility Table Ion Solubility Exceptions NO 3 soluble none ClO 4 soluble none Cl soluble except Ag +, Hg 2+ 2, *Pb 2+ I soluble except Ag +, Hg 2+ 2, Pb 2+ SO 2 4 soluble except Ca 2+, Ba 2+, Sr 2+, Hg 2+, Pb 2+, Ag + CO 3 2 insoluble except Group IA and NH 4 + PO 3 4 insoluble + except Group IA and NH 4 - OH insoluble except Group IA, *Ca 2+, Ba 2+, Sr 2+ S 2 insoluble except Group IA, IIA and NH + 4 Na + soluble none NH + 4 soluble none K + soluble none *slightly soluble

8 CHEM 1314 EXAM II PAGE 8 Table of Standard Heats of Formation Substance H f Substance H f and State (k/mol) and St ate (k/mol) C(s) (graphite) 0 HCl(g) C(s) (diamond) 2 HBr(g) CO(g) HI(g) 26.5 CO 2 (g) I 2 (g) CH 4 (g) 75 O 2 (g) 0 CH 3 OH(g) -201 O(g) 249 CH 3 OH(l) -239 O 3 (g) 143 H 2 CO(g) -116 CCl 4 (l) N 2 (g) 0 HCOOH(g) -363 NH 3 (g) -46 HCN(g) NH 3 (aq) -80 CS 2 (g) NH 4 + (aq) -132 CS 2 (l) 89.7 N 2 H 3 CH 3 (l) 54 C 2 H 2(g) 227 N 2 H 4 (l) 50.6 C 2 H 4 (g) 52 NO(g) CH 3 CHO(g) -166 NO 2 (g) C 2 H 5 OH(l) -278 N 2 O(g) 82.0 C 2 H 5 O 2 N(g) -533 N 2 O 4 (g) 9.16 C 2 H 6 (g) N 2 O 4 (l) 20 C 3 H 6 (g) 20.9 HNO 3 (aq) C 3 H 8 (g) -104 HNO 3 (l) C 4 H 10 (g) -126 NH 4 ClO 4 (s) -295 CH 2 = CHCN(l) 152 CH 3 COOH(l) -484 S 2 Cl 2 (g) -18 C 6 H 12 O 6 (s) SO 2 (g) TiO 2 (s) -945 H 2 S(g) Cl 2 (g) 0 SOCl 2 (g) -213 Cl 2 (aq) -23 Cl - (aq) -167 SiCl 4 (g) -657 SiO 2 (s) SiF 4 (g) H 2 (g) 0 H(g) 217 TiO 2 (s) H + (aq) 0 TiCl 4 (g) -763 OH - (aq) -230 H 2 O(l) -286 ZnO(s) -348 H 2 O(g) -242 ZnS(s) -206

9 CHEM 1314 EXAM II PAGE 9 Metal Half-Reaction Reaction Lithium Li Li + + e Potassium K K + + e Barium Ba Ba e Calcium Ca Ca e Sodium Na Na + + e Magnesium Mg Mg e Aluminum Al Al e Manganese Mn Mn e Zinc Zn Zn e Chromium Cr Cr e Iron Fe Fe e Cobalt Co Co e Nickel Ni Ni e Tin Sn Sn e Lead Pb Pb e Hydrogen H 2 2H + + 2e Copper Cu Cu e Silver Ag Ag + + e Mercury Hg Hg e Platinum Pt Pt e Gold Au Au e

10 CHEM 1314 EXAM II PAGE 10

INSTRUCTIONS: Exam III. November 10, 1999 Lab Section

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

7. Relax and do well.

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

8. Relax and do well.

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

8. Relax and do well.

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 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

Circle the letters only. NO ANSWERS in the Columns!

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.

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

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

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

8. Relax and do well.

8. Relax and do well. CHEM 55.00-006 Exam I John I. Gelder February 5, 2002 Name TA's Name Section INSTRUCTIONS:. This examination consists of a total of 8 different pages. The last three pages include a periodic table, a table

More information

8. Relax and do well.

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

Chapter 3: Stoichiometry

Chapter 3: Stoichiometry 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

More information

Chapter 12 The Atom & Periodic Table- part 2

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

Marks for each question are as indicated in [] brackets.

Marks for each question are as indicated in [] brackets. Name Student Number CHEMISTRY 140 FINAL EXAM December 10, 2002 Numerical answers must be given with appropriate units and significant figures. Please place all answers in the space provided for the question.

More information

CHEM 130 Exp. 8: Molecular Models

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

VIIIA H PREDICTING CHARGE

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

Grade 11 Science Practice Test

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

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

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

Using the Periodic Table

Using the Periodic Table MATH SKILLS TRANSPARENCY WORKSHEET Using the Periodic Table 6 Use with Chapter 6, Section 6.2 1. Identify the number of valence electrons in each of the following elements. a. Ne e. O b. K f. Cl c. B g.

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.

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

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 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

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

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

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 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

The Periodic Table of Elements

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

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 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

SCIENCE 1206 UNIT 2 CHEMISTRY. September 2017 November 2017

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

Made the FIRST periodic table

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

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

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

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

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

Circle ONLY the LETTER of your answer.

Circle ONLY the LETTER of your answer. hemistry 1304 Name (please print) Exam 5 (105 points) May 3, 2017 n my honor, I have neither given nor received unauthorized aid on this exam. Signed Date ircle NLY the LETTER of your answer. 1. (3 points)

More information

Chemistry Standard level Paper 1

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

Lewis dot structures for molecules

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

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

... 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

6.3 Classifying Elements with the Periodic Table

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

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

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

(FIRST) IONIZATION ENERGY

(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

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

- 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

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. 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

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

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

Chemistry Standard level Paper 1

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

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

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

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

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

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

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

Periodic Table. Modern periodic table

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

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

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

What is the periodic table?

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

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

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

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

- 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

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

- 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

1.02 Elements, Symbols and Periodic Table

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

E4 Acids, Bases, and Salts

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

materials and their properties

materials and their properties materials and their properties macroscopic properties phase state strength / stiffness electrical conductivity chemical properties color / transparence spectroscopical properties surface properties density

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. 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

4.06 Periodic Table and Periodic Trends

4.06 Periodic Table and Periodic Trends 4.06 Periodic Table and Periodic Trends Dr. Fred Omega Garces Chemistry 100, Miramar College 1 4.06 Periodic Table and Periodic Trend The Periodic Table and the Elements What is the periodic table? What

More information

4.01 Elements, Symbols and Periodic Table

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

Atomic Structure & Interatomic Bonding

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

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

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

NAME: SECOND EXAMINATION

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

single-layer transition metal dichalcogenides MC2

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

Thermochemistry. Chapter 6. Chemistry E1a

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

E4 Acids, Bases, and Salts

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

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

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

E4 Acids, Bases, and Salts

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

Writing Chemical formula with polyatomic groups

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

CHEMISTRY 102 Fall 2014 HOUR EXAM I Page 1

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

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

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

Chemistry Higher level Paper 1

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

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

[ ]: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

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

Chapter 2 Lecture Notes: Atoms

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

1 Arranging the Elements

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 112 Name Exam I Form A Section January 29,

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

Chapter 6. Electronic Structure of Atoms. The number & arrangement of e - in an atom is responsible for its chemical behavior.

Chapter 6. Electronic Structure of Atoms. The number & arrangement of e - in an atom is responsible for its chemical behavior. Chapter 6 Electronic Structure of Atoms The number & arrangement of e - in an atom is responsible for its chemical behavior I) The Wave Nature of Light A) Electromagnetic Radiation Radiant Energy light,

More information

ICP/MS Multi-Element Standards

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

An Introduction to Atoms

An Introduction to Atoms An Introduction to Atoms Matter (stuff) is made of atoms. John Dalton (1776-1884) Check your current model: Draw a carbon atom Model of the Atom Atoms are made of subatomic particles. There are three types

More information

Chapter 2 Atoms and the Periodic Table

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

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

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

Name Section Signature TA ID #

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

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

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

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

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

Single-Element Standards for AAS

Single-Element Standards for AAS Single-Element Standards for AAS for AAS Flame Silver Ag in 2-5% HNO 3 Aluminium Al in 2-5% HCl Aluminium Al in 2-5% HNO 3 Arsenic As in 2-5% HCl Arsenic As in 2-5% HNO 3 Gold Au in 2-5% HCl Boron B in

More information

Stoichiometry. Mole Concept. Balancing Chemical Equations

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

NAME: 3rd (final) EXAM

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

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

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

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

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

Review. 8th grade science STAAR. Name Class. Underline your strong TEKS and circle your weak TEKS: 8.5A Atoms. 7.5C Energy Flow Through Ecosystems

Review. 8th grade science STAAR. Name Class. Underline your strong TEKS and circle your weak TEKS: 8.5A Atoms. 7.5C Energy Flow Through Ecosystems 8th grade science STAAR Review Name Class Underline your strong TEKS and circle your weak TEKS: 8.5A Atoms 7.5C Energy Flow Through Ecosystems 8.5B Reactivity 8.5C Periodic Table 8.5D Chemical Formulas

More information

AP Chapter 6: Thermochemistry Name

AP Chapter 6: Thermochemistry Name AP Chapter 6: Thermochemistry Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. AP Chapter 6: Thermochemistry 2 Warm-Ups (Show your work for credit)

More information

Chapter 4. The Major Classes of Chemical Reactions 4-1

Chapter 4. The Major Classes of Chemical Reactions 4-1 Chapter 4 The Major Classes of Chemical Reactions 4-1 The Major Classes of Chemical Reactions 4.1 The Role of Water as a Solvent 4.2 Writing Equations for Aqueous Ionic Reactions 4.3 Precipitation Reactions

More information

Chapter 3: Compounds

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

Teacher Workbooks. Science and Nature Series. Atomic Structure, Electron Configuration, Classifying Matter and Nuclear Chemistry, Vol.

Teacher Workbooks. Science and Nature Series. Atomic Structure, Electron Configuration, Classifying Matter and Nuclear Chemistry, Vol. Teacher Workbooks Science and Nature Series Atomic Structure, Electron Configuration, Classifying Matter and Nuclear Chemistry, Vol. 1 Copyright 23 Teachnology Publishing Company A Division of Teachnology,

More information

Inorganic Chemistry review sheet Exam #1

Inorganic Chemistry review sheet Exam #1 Inorganic Chemistry review sheet Exam #1 Ch. 1 General Chemistry review reaction types: A/B, redox., single displacement, elimination, addition, rearrangement and solvolysis types of substances: elements,

More information

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

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

UNIT (2) ATOMS AND ELEMENTS

UNIT (2) ATOMS AND ELEMENTS UNIT (2) ATOMS AND ELEMENTS 2.1 Elements An element is a fundamental substance that cannot be broken down by chemical means into simpler substances. Each element is represented by an abbreviation called

More information

Chemistry 112 Name Exam I Form A Section February 3,

Chemistry 112 Name Exam I Form A Section February 3, Chemistry 112 Name Exam I Form A Section February 3, 2015 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

Chem 1412 SU06 Exam 4

Chem 1412 SU06 Exam 4 Chem 1412 SU06 Exam 4 Student: 1. Which of the following is necessary for a process to be spontaneous? A. H sys < 0 B. S sys > 0 C. S surr < 0 D. S univ > 0 E. G sys = 0 2. Which of the following is always

More information

Chemical Formulas and Chemical Nomenclature. Mr. Matthew Totaro Legacy High School Honors Chemistry

Chemical Formulas and Chemical Nomenclature. Mr. Matthew Totaro Legacy High School Honors Chemistry Chemical Formulas and Chemical Nomenclature Mr. Matthew Totaro Legacy High School Honors Chemistry 1 Molecular View of Elements and Compounds 2 Atomic Elements Atomic Elements = elements whose smallest

More information

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

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

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 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

OCN 201: Origin of the Earth and Oceans. Waimea Bay, Jan 2002

OCN 201: Origin of the Earth and Oceans. Waimea Bay, Jan 2002 OCN 201: Origin of the Earth and Oceans Waimea Bay, Jan 2002 Periodic Table of the Elements Noble IA IIA IIIA IVA VA VIA VIIA VIIIA IB IIB IIIB IVB VB VIB VIIB gases H He Li Be B C N O F Ne Na Mg Al Si

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 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