1. The relative molecular mass of a gas is 56 and its empirical formula is CH 2. What is the molecular formula of the gas? D. C 4 H 8 (Total 1 mark)
|
|
- Dwight Lawrence
- 6 years ago
- Views:
Transcription
1 1. The relative molecular mass of a gas is 56 and its empirical formula is CH 2. What is the molecular formula of the gas? A. CH 2 B. C 2 H 4 C. C 3 H 6 D. C 4 H 8 2. A fixed mass of gas has a certain volume at a temperature of 50 C. What temperature is required to double its volume while keeping the pressure constant? A. 100 K B. 323 K C. 373 K D. 646 K 3. Which sample has the greatest mass? A. 1 mol of SO 2 B. 2 mol of N 2 O C. 2 mol of Ar D. 4 mol of NH 3 IB Questionbank Chemistry 1
2 4. What is the coefficient of Fe 3 O 4 when the following equation is balanced using the lowest whole numbers? A. 2 B. 3 C. 4 Al(s) + Fe 3 O 4 (s) Al 2 O 3 (s) + Fe(s) D cm 3 of water is added to a solution of 200 cm 3 of 0.5 mol dm 3 sodium chloride. What is the concentration of sodium chloride in the new solution? A mol dm 3 B. 0.1 mol dm 3 C. 0.2 mol dm 3 D. 0.3 mol dm 3 6. What is the maximum mass, in g, of magnesium oxide that can be obtained from the reaction of oxygen with 2.4 g of magnesium? A. 2.4 B. 3.0 C. 4.0 D. 5.6 IB Questionbank Chemistry 2
3 7. Brass is a copper containing alloy with many uses. An analysis is carried out to determine the percentage of copper present in three identical samples of brass. The reactions involved in this analysis are shown below. Step 1: Cu(s) + 2HNO 3 (aq) + 2H + (aq) Cu 2+ (aq) + 2NO 2 (g) + 2H 2 O(l) Step 2: 4I (aq) + 2Cu 2+ (aq) 2CuI(s) + I 2 (aq) Step 3: I 2 (aq) + 2S 2 O 3 2 (aq) 2I (aq) + S 4 O 6 2 (aq) (a) (i) Deduce the change in the oxidation numbers of copper and nitrogen in step 1. Copper: Nitrogen: (2) (ii) Identify the oxidizing agent in step 1. (1) (b) A student carried out this experiment three times, with three identical small brass nails, and obtained the following results. Mass of brass = g ± g Titre Initial volume of mol dm 3 S 2 O 2 3 (± 0.05 cm 3 ) Final volume of mol dm 3 S 2 O 2 3 (± 0.05 cm 3 ) Volume added of mol dm 3 S 2 O 2 3 (± 0.10 cm 3 ) Average volume added of mol dm 3 S 2 O 2 3 (± 0.10 cm 3 ) IB Questionbank Chemistry 3
4 (i) Calculate the average amount, in mol, of S 2 O 2 3 added in step 3. (2) (ii) Calculate the amount, in mol, of copper present in the brass. (1) (iii) Calculate the mass of copper in the brass. (1) (iv) Calculate the percentage by mass of copper in the brass. (1) (v) The manufacturers claim that the sample of brass contains 44.2 % copper by mass. Determine the percentage error in the result. (1) IB Questionbank Chemistry 4
5 (c) With reference to its metallic structure, describe how brass conducts electricity (1) (Total 10 marks) 8. Smog is common in cities throughout the world. One component of smog is PAN (peroxyacylnitrate) which consists of 20.2 % C, 11.4 % N, 65.9 % O and 2.50 % H by mass. Determine the empirical formula of PAN, showing your working. (Total 3 marks) 9. Consider the following sequence of reactions. RCH 3 reaction 1 RCH 2 Br reaction 2 RCH 2 OH reaction 3 RCOOH RCH 3 is an unknown alkane in which R represents an alkyl group. (a) The alkane contains 81.7 % by mass of carbon. Determine its empirical formula, showing your working. (3) IB Questionbank Chemistry 5
6 (b) Equal volumes of carbon dioxide and the unknown alkane are found to have the same mass, measured to an accuracy of two significant figures, at the same temperature and pressure. Deduce the molecular formula of the alkane. (1) (c) (i) State the reagent and conditions needed for reaction 1. (2) (ii) State the reagent(s) and conditions needed for reaction 3. (2) (d) Reaction 1 involves a free-radical mechanism. Describe the stepwise mechanism, by giving equations to represent the initiation, propagation and termination steps. (4) (e) The mechanism in reaction 2 is described as S N 2. (i) State the meaning of each of the symbols in S N 2. (1) (ii) Explain the mechanism of this reaction using curly arrows to show the movement of electron pairs, and draw the structure of the transition state. (3) (Total 16 marks) IB Questionbank Chemistry 6
7 10. What is the correct Lewis structure for hypochlorous acid, a compound containing chlorine, hydrogen and oxygen?.... A. : Cl : O : H : B. : Cl : H : O : C. : Cl : O : H D. O : Cl : H How do the bond angles in CH 4, NH 3 and H 2 O compare? A. CH 4 = NH 3 = H 2 O B. CH 4 < NH 3 < H 2 O C. NH 3 < CH 4 < H 2 O D. H 2 O < NH 3 < CH Which species does not contain delocalized electrons? A. CH 3 CH 2 O B. CH 3 CO 2 C. O 3 D. NO 3 IB Questionbank Chemistry 7
8 13. How many σ and π bonds are present in a molecule of propyne, CH 3 CCH? σ π A. 5 3 B. 6 2 C. 7 1 D What are the correct formulas of the following ions? Ammonium Hydrogencarbonate Phosphate A. NH HCO 3 PO 4 B. NH 3 + C. NH 4 + D. NH 4 + HCO 3 HCO 3 2 HCO 3 PO 4 3 PO 4 2 PO Which molecule has an octahedral shape? A. SF 6 B. PCl 5 C. XeF 4 D. BF 3 IB Questionbank Chemistry 8
9 16. Which order is correct when the following compounds are arranged in order of increasing melting point? A. CH 4 < H 2 S < H 2 O B. H 2 S < H 2 O < CH 4 C. CH 4 < H 2 O < H 2 S D. H 2 S < CH 4 < H 2 O 17. The graph below shows the first four ionization energies of four elements A, B, C and D (the letters are not their chemical symbols). Which element is magnesium? IB Questionbank Chemistry 9
10 18. Describe and compare three features of the structure and bonding in the three allotropes of carbon: diamond, graphite and C 60 fullerene. (Total 6 marks) 19. Describe the structure and bonding in SiO 2. (Total 2 marks) IB Questionbank Chemistry 10
11 20. Describe the delocalization of pi (π) electrons and explain how this can account for the structure and stability of the carbonate ion, CO 3 2. (Total 3 marks) 21. Ammonia, NH 3, is a weak base. (i) Draw the Lewis structure of ammonia and state the shape of the molecule and its bond angles (3) IB Questionbank Chemistry 11
12 (ii) The conjugate acid of ammonia is the ammonium ion, NH 4 +. Draw the Lewis structure of the ammonium ion and deduce its shape and bond angles (3) (Total 6 marks) 22. (i) Define the term first ionization energy of an atom. (2) (ii) Explain the general increasing trend in the first ionization energies of the period 3 elements, Na to Ar. (2) (iii) Explain why sodium conducts electricity but phosphorus does not. (2) (Total 6 marks) 23. Draw the Lewis structures, state the shape and predict the bond angles for the following species. (i) PCl 3 (3) (ii) NH 2 (3) IB Questionbank Chemistry 12
13 (iii) XeF 4 (3) (Total 9 marks) 24. Explain, using diagrams, why CO and NO 2 are polar molecules but CO 2 is a non-polar molecule. (Total 5 marks) IB Questionbank Chemistry 13
14 1. D 2. D 3. B 4. B 5. C 6. C 7. (a) (i) Copper: 0 to +2 / increases by 2 / +2 / 2+; Allow zero/nought for 0. Nitrogen: +5 to +4 / decreases by 1 / 1 / 1 ; Penalize missing + sign or incorrect notation such as 2+, 2 + or II, once only. 2 (ii) nitric acid/hno 3 / NO 3 /nitrate; Allow nitrogen from nitric acid/nitrate but not just nitrogen. 1 (b) (i) ; (mol); Award [2] for correct final answer. 2 (ii) (mol); 1 IB Questionbank Chemistry 1
15 (iii) ( ) = g; Allow (iv) = % 1 (v) = 10/10.2 %; 44.2 Allow 11.3 % i.e. percentage obtained in (iv) is used to divide instead of 44.2 %. 1 (c) Brass has: delocalized electrons / sea of mobile electrons / sea of electrons free to move; No mark for just mobile electrons. 1 [10] 8. C N O H = 1.68 = = 4.12 = 2.48 ; = 2 = = 5 C 2 NO 5 H 3 ; = 3 ; No penalty for use of 12, 1 and/or 14. Award [1 max] if the empirical formula is correct, but no working shown. 3 [3] 9. (a) n C = = 6.80 and n H = = 18.1; ratio of 1: 2.67 /1: 2.7; C 3 H 8 ; No penalty for using 12 and 1. 3 (b) C 3 H 8 ; 1 (c) (i) Br 2 /bromine; UV/ultraviolet light; Accept hf/hv/sunlight. 2 (ii) Cr 2 O 7 2 /MnO 4 and acidified/ H + /H 3 O + ; IB Questionbank Chemistry 2
16 Accept names. heat / reflux; 2 (d) Initiation: Br 2 2Br ; Propagation: Br + RCH 3 HBr + RCH 2 ; RCH 2 + Br 2 RCH 2 Br + Br ; Termination: [1 max] Br + Br Br 2 ; RCH 2 + Br RCH 2 Br; RCH 2 + RCH 2 RCH 2 CH 2 R; Award for any termination step. Accept radical with or without throughout. Do not penalize the use of an incorrect alkane in the mechanism. 4 max (e) (i) substitution and nucleophilic and bimolecular/two species in rate-determining step; Allow second order in place of bimolecular. 1 (ii) curly arrow going from lone pair/negative charge on O in OH to C; Do not allow curly arrow originating on H in OH curly arrow showing Br leaving; Accept curly arrow either going from bond between C and Br to Br in bromoethane or in the transition state. representation of transition state showing negative charge, square brackets and partial bonds; Do not penalize if HO and Br are not at 180 to each other. Do not award M3 if OH ---- C bond is represented unless already penalized in M1. Do not penalize the use of an incorrect alkyl chain in the mechanism. 3 [16] IB Questionbank Chemistry 3
17 10. C 11. D 12. A 13. B 14. D 15. A 16. A 17. B IB Questionbank Chemistry 4
18 18. Award [2 max] for three of the following features: Bonding Graphite and C 60 fullerene: covalent bonds and van der Waals /London/ dispersion forces; Diamond: covalent bonds (and van der Waals /London/dispersion forces); Delocalized electrons Graphite and C 60 fullerene: delocalized electrons; Diamond: no delocalized electrons; Structure Diamond: network/giant structure / macromolecular / three-dimensional structure and Graphite: layered structure / two-dimensional structure / planar; C 60 fullerene: consists of molecules / spheres made of atoms arranged in hexagons/pentagons; Bond angles Graphite: 120 and Diamond: 109 ; C 60 fullerene: bond angles between ; Allow Graphite: sp 2 and Diamond: sp 3. Allow C 60 fullerene: sp 2 and sp 3. Number of atoms each carbon is bonded to Graphite and C 60 fullerene: each C atom attached to 3 others; Diamond: each C atom attached to 4 atoms / tetrahedral arrangement of C (atoms); 6 max [6] 19. network/giant structure / macromolecular; each Si atom bonded covalently to 4 oxygen atoms and each O atom bonded covalently to 2 Si atoms / single covalent bonds; 2 Award [1 max] for answers such as network-covalent, giant-covalent or macromolecular-covalent. Both M1 and M2 can be scored by a suitable diagram. [2] IB Questionbank Chemistry 5
19 20. delocalization/spread of pi/π electrons over more than two nuclei; equal bond order/strength/length / spreading charge (equally) over all three oxygens; gives carbonate ion a greater stability/lower potential energy; 3 M3 can be scored independently. Accept suitable labelled diagrams for M1 and M2 e.g. OR Do not penalize missing brackets on resonance structure but 2 charge must be shown. Allow 2 for charge on resonance structure. [3] 21. (i) Accept any combination of dots/crosses and lines to represent electron pairs. (trigonal/triangular) pyramid; Allow 3D representation using wedges and dotted bonds of trigonal pyramidal molecule. 107 ; 3 Accept any angle between 105º and 108.5º. No ECF for shape based on incorrect Lewis structure. IB Questionbank Chemistry 6
20 (ii) Charge needed for mark. tetrahedral; Allow a 3D representation using wedges and dotted bonds of tetrahedral molecule /109 /109 28'; 3 No ECF for shape based on incorrect Lewis structure. [5] 22. (i) energy/enthalpy change/required/needed to remove/knock out an electron (to form +1 /uni-positive/ M +1 ion); in the gaseous state; Award for M(g) M + (g) + e. Award [2] for M(g) M + (g) + e with reference to energy/enthalpy change. 2 (ii) increasing number of protons/atomic number/z/nuclear charge; atomic radii/size decreases / same shell/energy level / similar shielding/ screening (from inner electrons); No mark for shielding/screening or shielding/screening increases. 2 (iii) Na: delocalized electrons / mobile sea of electrons / sea of electrons free to move; No mark for just mobile electrons. P: atoms covalently bonded / no free/mobile/delocalized electrons; 2 [6] 23. (i) trigonal pyramid; in the range of ; 3 IB Questionbank Chemistry 7
21 (ii) Must include minus sign for the mark. bent/v shaped; in the range of ; 3 (iii) square planar; 90 ; Penalize once only if electron pairs are missed off outer atoms. 3 [9] 24. CO: Award for showing the net dipole moment, or explaining it in words (unsymmetrical distribution of charge). NO 2 : Award for correct representation of the bent shape and for showing the net dipole moment, or explaining it in words (unsymmetrical distribution of charge). CO 2 : Award for correct representation of the linear shape and for showing the two equal but opposite dipoles or explaining it in words (symmetrical distribution of charge). For all three molecules, allow either arrow or arrow with bar for representation of dipole moment. Allow correct partial charges instead of the representation of the vector dipole moment. Ignore incorrect bonds. Lone pairs not needed. 5 [5] IB Questionbank Chemistry 8
D. 1.0 (Total 1 mark) 2. The relative molecular mass of a gas is 56 and its empirical formula is CH 2. What is the molecular formula of the gas?
1. 1.7 g of NaNO 3 (M r = 85) is dissolved in water to prepare 0.20 dm 3 of solution. What is the concentration of the resulting solution in mol dm 3? A. 0.01 B. 0.1 C. 0.2 D. 1.0 2. The relative molecular
More informationSL Score. HL Score ! /30 ! /48. Practice Exam: Paper 1 Topic 4: Bonding. Name
Name Practice Exam: Paper 1 Topic 4: Bonding SL SL Score! /30 HL Score! /48 1. What is the correct Lewis structure for hypochlorous acid, a compound containing chlorine, hydrogen and oxygen? A. B. C. D.
More informationIB Topics 4 & 14 Multiple Choice Practice
IB Topics 4 & 14 Multiple Choice Practice 1. Which compound has the shortest C N bond? CH 3NH 2 (CH 3) 3CNH 2 CH 3CN CH 3CHNH 2. Which of the following series shows increasing hydrogen bonding with water?
More informationReview for Chapter 4: Structures and Properties of Substances
Review for Chapter 4: Structures and Properties of Substances You are responsible for the following material: 1. Terms: You should be able to write definitions for the following terms. A complete definition
More informationAnswers. Chapter 4. Exercises
Answers hapter 4 Exercises 1 lead nitrate, Pb( 3 ) 2 barium hydroxide, Ba() 2 potassium hydrogencarbonate, K 3 magnesium carbonate, Mg 3 copper sulfate, u 4 calcium phosphate, a 3 (P 4 ) 2 ammonium chloride,
More informationAnswers. Chapter 4. Exercises. lead nitrate, Pb(NO3)2. 10 barium hydroxide, Ba(OH)2 potassium hydrogencarbonate, KHCO3.
Answers hapter 4 Exercises 1 lead nitrate, Pb(N3)2 10 barium hydroxide, Ba()2 potassium hydrogencarbonate, K3 12 D 11 (a) (e) copper sulfate, us4 N 3 (d) 13 (a) KBr (b) Zn (c) Na2S4 (d) ubr2 (e) r2(s4)3
More information1. What is the sum of all coefficients when the following equation is balanced using the smallest possible whole numbers? D.
1. What is the sum of all coefficients when the following equation is balanced using the smallest possible whole numbers? A. 5 B. 7 C. 11 C 2 H 2 + O 2 CO 2 + H 2 O D. 13 2. 1.7 g of NaNO 3 (M r = 85)
More informationN10/4/CHEMI/SP2/ENG/TZ0/XX CHEMISTRY STANDARD LEVEL PAPER 2. Thursday 11 November 2010 (afternoon) Candidate session number.
N10/4/CHEMI/SP2/ENG/TZ0/XX 88106105 CHEMISTRY STANDARD LEVEL PAPER 2 Thursday 11 November 2010 (afternoon) 1 hour 15 minutes 0 0 Candidate session number INSTRUCTIONS TO CANDIDATES Write your session number
More informationMultiple Choice Identify the letter of the choice that best completes the statement or answers the question.
CHAPTER 4 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. A substance is a brittle crystal that conducts electricity in molten liquid state
More informationChapter 6 Chemistry Review
Chapter 6 Chemistry Review Multiple Choice Identify the choice that best completes the statement or answers the question. Put the LETTER of the correct answer in the blank. 1. The electrons involved in
More information1. What is the formula for the compound formed by calcium and nitrogen?
IB Chem 1 Name Topic 4 Bonding - Sample Test Problems 1. What is the formula for the compound formed by calcium and nitrogen? A. CaN B. Ca 2 N C. Ca 2 N 3 D. Ca 3 N 2 2. Element X is in group 2, and element
More informationCovalent bonding does not involve electrostatic attraction between oppositely charged particles.
SCH3U7 - Topic 4: Bonding Review SL Which of these bonding types would not be classified as strong? Metallic Covalent Ionic Dipole dipole The bond dissociation energy of NaCl is 411 kj mol -1, while that
More information1. What is the formula for the compound formed by calcium and nitrogen? D. Ca 3 N 2 (Total 1 mark)
1 2 3 1. What is the formula for the compound formed by calcium and nitrogen? A. CaN B. Ca 2 N C. Ca 2 N 3 D. Ca 3 N 2 2. Element X is in group 2, and element Y in group 7, of the periodic table. Which
More information2 Bonding and structure Answers to Exam practice questions
Pages 77 80 Exam practice questions 1 a) Bonding between atoms in a metal is the result of electrostatic attractions between positive metal ions in a lattice and delocalised electrons in the outer shell
More informationIB Chemistry 11 Kahoot! Review Q s Bonding
IB Chemistry 11 Kahoot! Review Q s Bonding 1. What is the best description of the carbon-oxygen bond lengths in CO3 2-? A. One short and two long bonds B. One long and two short bonds C. Three bonds of
More information2. Write the electron configuration notation and the electron dot notation for each: (a) Ni atom (b) Ni 2+ ion (c) Ni 3+ ion
EXTRA HOMEWORK 2A 1. Predict whether each of the following types of matter will be bonded with ionic, covalent, or metallic bonds, and identify whether each will be composed of atoms, ions, or molcules
More informationUnit Six --- Ionic and Covalent Bonds
Unit Six --- Ionic and Covalent Bonds Electron Configuration in Ionic Bonding Ionic Bonds Bonding in Metals Valence Electrons Electrons in the highest occupied energy level of an element s atoms Examples
More information6 Shapes of molecules and intermolecular forces Answers to practice questions. OCR Chemistry A. Question Answer Marks Guidance
1 (a) (i) HI, HBr, HCl, HF 1 (a) (ii) CF 4, CH 3 I, CH 2 Br 2, CHCl 2 F 1 (b) (i) CO 2 and HCN: linear H 2 O and SCl 2 : non-linear BF 3 and SO 3 : trigonal planar NH 3 and H 3 O + : pyramidal AlCl 4 and
More informationMarkscheme November 2017 Chemistry Higher level Paper 2
N7/4/CHEMI/HP/ENG/TZ0/XX/M Markscheme November 07 Chemistry Higher level Paper 9 pages N7/4/CHEMI/HP/ENG/TZ0/XX/M This markscheme is the property of the International Baccalaureate and must not be reproduced
More informationSave My Exams! The Home of Revision For more awesome GCSE and A level resources, visit us at Covalent bonding.
Covalent bonding Mark Scheme Level Subject Exam Board Topic Booklet Pre U Chemistry Cambridge International Examinations Covalent bonding-chemical forces Mark Scheme Time Allowed: 72 minutes Score: /60
More informationChapter 16 Covalent Bonding
Chemistry/ PEP Name: Date: Chapter 16 Covalent Bonding Chapter 16: 1 26; 28, 30, 31, 35-37, 40, 43-46, Extra Credit: 50-53, 55, 56, 58, 59, 62-67 Section 16.1 The Nature of Covalent Bonding Practice Problems
More informationCHAPTER 6: CHEMICAL NAMES AND FORMULAS CHAPTER 16: COVALENT BONDING
CHAPTER 6: CHEMICAL NAMES AND FORMULAS CHAPTER 16: COVALENT BONDING 6.1 Introduction to Chemical Bonding A chemical bond is a mutual electrical attraction between the nuclei and valence electrons of different
More informationChemical bonding & structure
Chemical bonding & structure Ionic bonding and structure Covalent bonding Covalent structures Intermolecular forces Metallic bonding Ms. Thompson - SL Chemistry Wooster High School Topic 4.3 Covalent structures
More informationTopic 4: Bonding. Adapted from Mr Field
Topic 4: Bonding Adapted from Mr Field 4.1 Ionic Bonding and Structure Ionic bonding An ionic bond is: The electrostatic attraction between two oppositely charged ions sodium fluoride lithium oxide F -
More informationCHEMISTRY 110 EXAM 2 Oct.
EMISTRY 110 EXAM 2 ct. 15, 2012 FRM A 1. Which of the following is an incorrect formula for a neutral compound made from the given ions?! "#$%&'! #'%&'! (&)*+,#! -.!! aluminum oxide Al 2 3 /.!! magnesium
More informationF321: Atoms, Bonds and Groups Structure & Bonding
F321: Atoms, Bonds and Groups Structure & Bonding 1. This question is about different models of bonding and molecular shapes. Magnesium sulfide shows ionic bonding. What is meant by the term ionic bonding?
More information1. Which response contains all the molecules below that violate the octet rule, and no others? SF 4, SiCl 4, H 2Te, AsF 5, BeI 2
Chem 1100 Pre-Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which response contains all the molecules below that violate the octet rule, and no
More informationClass Period. 4. What distinguishes a polar covalent bond from a nonpolar covalent bond?
Cut along dotted line. Name Assignment #1 Chemical Bonding (Predicting Bond Types) 1. What is a chemical bond? 2. Why do atoms form chemical bonds? 3. What distinguishes an ionic bond from a covalent bond?
More informationM10/4/CHEMI/SP2/ENG/TZ1/XX+ CHEMISTRY. Wednesday 12 May 2010 (afternoon) Candidate session number. 1 hour 15 minutes INSTRUCTIONS TO CANDIDATES
M10/4/CHEMI/SP2/ENG/TZ1/XX+ 22106111 CHEMISTRY standard level Paper 2 Wednesday 12 May 2010 (afternoon) 1 hour 15 minutes 0 0 Candidate session number INSTRUCTIONS TO CANDIDATES Write your session number
More informationThe dative covalent bond acts like an ordinary covalent bond when thinking about shape so in NH 4. the shape is tetrahedral
1.3 Bonding Definition Ionic bonding is the electrostatic force of attraction between oppositely charged ions formed by electron transfer. Metal atoms lose electrons to form ve ions. Non-metal atoms gain
More informationAdvanced Subsidiary Unit 1: The Core Principles of Chemistry
Write your name here Surname Other names Pearson Edexcel International Advanced Level Centre Number Chemistry Advanced Subsidiary Unit 1: The Core Principles of Chemistry Candidate Number Thursday 14 January
More informationUnit 1 Module 1 Forces of Attraction page 1 of 10 Various forces of attraction between molecules
Unit 1 Module 1 Forces of Attraction page 1 of 10 Various forces of attraction between molecules 1. Ionic bonds 2. Covalent bonds (also co-ordinate covalent bonds) 3. Metallic bonds 4. Van der Waals forces
More informationCh 10 Chemical Bonding, Lewis Structures for Ionic & Covalent Compounds, and Predicting Shapes of Molecules
Fructose Water Ch 10 Chemical Bonding, Lewis Structures for Ionic & Covalent Compounds, and Predicting Shapes of Molecules Carbon Dioxide Ammonia Title and Highlight TN Ch 10.1 Topic: EQ: Right Side NOTES
More informationCHAPTER 3 CHEMICAL BONDING NUR FATHIN SUHANA BT AYOB SMK SULTAN ISMAIL, JB
CHAPTER 3 CHEMICAL BONDING NUR FATHIN SUHANA BT AYOB SMK SULTAN ISMAIL, JB LEARNING OUTCOMES (ionic bonding) 1. Describe ionic (electrovalent) bonding such as NaCl and MgCl 2 LEARNING OUTCOMES (metallic
More information51. Pi bonding occurs in each of the following species EXCEPT (A) CO 2 (B) C 2 H 4 (C) CN (D) C 6 H 6 (E) CH 4
Name AP Chemistry: Bonding Multiple Choice 41. Which of the following molecules has the shortest bond length? (A) N 2 (B) O 2 (C) Cl 2 (D) Br 2 (E) I 2 51. Pi bonding occurs in each of the following species
More informationMemorize: Understand: Know how to:
NAME: CLASS PERIOD: REVIEW FOR HONORS CHEMISTRY SEMESTER 1 EXAM Memorize: Understand: Know how to: 1 SI units for different measurements (length, volume, number, mass, temperature, density) Definition
More informationChapter 7. Chemical Bonding I: Basic Concepts
Chapter 7. Chemical Bonding I: Basic Concepts Chemical bond: is an attractive force that holds 2 atoms together and forms as a result of interactions between electrons found in combining atoms We rarely
More informationSTRUCTURE AND BONDING
NAME SCHOOL INDEX NUMBER DATE 1. 1989 Q 6 STRUCTURE AND BONDING The table below gives the distance between atoms (bond lengths) in halogen molecules and the energies required to break the bonds (bond energies)
More informationUnit Test: Bonding. , is best described as: A. bent. B. linear. C. T-shaped. D. triangular.
Unit Test: Bonding SCH3UE_2009-2010_V1 NAME: Multiple Choice ( 10) 1. Which substance has the lowest electrical conductivity? A. Al (s) B. Al 2 O 3(s) C. KCl (aq) D. HCl (aq) 2. Which bond has the lowest
More informationCHEMISTRY 110 EXAM 2 Feb 25, 2013 FORM A
EMISTRY 110 EXAM 2 Feb 25, 2013 FORM A 1. ow many valence electrons and lone pairs are in the structure of the ammonium ion? # valence electrons # lone pairs A. 8 0 B. 10 1. 8 1 D. 10 2 E. 12 3 2. Which
More informationIB Chemistry 2 Summer Assignment
Name IB Chemistry 2 Summer Assignment 1. What is the sum of all coefficients when the following equation is balanced using the smallest possible whole numbers? C 2 H 2 + O 2 CO 2 + H 2 O A. 5 B. 7 C. 11
More information* one of these choices is not used
IONIC BONDING REVIEW WORKSHEET Part 1 - Complete each of the following sentences by filling in the appropriate word or phrase from the list below. negative noble gas octet anion positive electrons ions
More informationPRACTICE EXAMINATION QUESTIONS FOR 1.1 ATOMIC STRUCTURE (includes some questions from 1.4 Periodicity)
PRACTICE EXAMINATION QUESTIONS FOR 1.1 ATOMIC STRUCTURE (includes some questions from 1.4 Periodicity) 1. At room temperature, both sodium metal and sodium chloride are crystalline solids which contain
More informationDefinition: An Ionic bond is the electrostatic force of attraction between oppositely charged ions formed by electron transfer.
3 Bonding Definition An Ionic bond is the electrostatic force of attraction between oppositely charged ions formed by electron transfer. Metal atoms lose electrons to form +ve ions. on-metal atoms gain
More informationHonors Chemistry Unit 6 ( )
Honors Chemistry Unit 6 (2017-2018) Lewis Dot Structures VSEPR Structures 1 We are learning to: 1. Represent compounds with Lewis structures. 2. Apply the VSEPR theory to determine the molecular geometry
More information2.2.2 Bonding and Structure
2.2.2 Bonding and Structure Ionic Bonding Definition: Ionic bonding is the electrostatic force of attraction between oppositely charged ions formed by electron transfer. Metal atoms lose electrons to form
More informationChemistry 121: Topic 4 - Chemical Bonding Topic 4: Chemical Bonding
Topic 4: Chemical Bonding 4.0 Ionic and covalent bonds; Properties of covalent and ionic compounds 4.1 Lewis structures, the octet rule. 4.2 Molecular geometry: the VSEPR approach. Molecular polarity.
More informationEdexcel Chemistry A-level
Edexcel Chemistry A-level Topic 2 - Bonding and Structure Flashcards What are ions? What are ions? Charged particles that is formed when an atom loses or gains electrons What is the charge of the ion when
More informationBonding. Honors Chemistry 412 Chapter 6
Bonding Honors Chemistry 412 Chapter 6 Chemical Bond Mutual attraction between the nuclei and valence electrons of different atoms that binds them together. Types of Bonds Ionic Bonds Force of attraction
More informationChemical Bonds. Chapter 6
Chemical Bonds Chapter 6 1 Ch. 6 Chemical Bonding I. How and Why Atoms Bond A. Vocabulary B. Chemical Bonds - Basics C. Chemical Bonds Types D. Chemical Bonds Covalent E. Drawing Lewis Diagrams F. Bond
More informationSigma Pi Hybridization A. 4 1 sp 2 B. 4 1 sp 3 C. 3 2 sp 3 D. 3 1 sp 2
IB Chemistry HL Topic4 Questions 1. What is the best description of the carbon-oxygen bond lengths in CO 3 2? A. One short and two long bonds B. One long and two short bonds C. Three bonds of the same
More informationChemical Bonds, Lewis Structures, Bond Order, and Formal Charge
Chemical Bonds, Lewis Structures, Bond Order, and Formal Charge PRELAB ASSIGNMENT Read the entire laboratory write up. Write an objective, any hazards associated with this lab, and answer the following
More informationShapes of molecules & ions
.1..5 Shapes of molecules & ions 54 minutes 50 marks Page 1 of 6 Q1. (a) The shape of the molecule BCl and that of the unstable molecule CCl are shown below. (i) Why is each bond angle exactly 10 in BCl?
More informationWeek 8 Intermolecular Forces
NO CALCULATORS MAY BE USED FOR THESE QUESTIONS Questions 1-3 refer to the following list. (A) Cu (B) PH 3 (C) C (D) SO 2 (E) O 2 1. Contains instantaneous dipole moments. 2. Forms covalent network solids.
More informationTest Bank for Introductory Chemistry Essentials 5th Edition by Tro
Test Bank for Introductory Chemistry Essentials 5th Edition by Tro Sample Introductory Chemistry, 5e (Tro) Chapter 10 Chemical Bonding 10.1 True/False Questions 1) Bonding theories are used to predict
More informationTOPIC: Chemical Bonds
TOPIC: Chemical Bonds H O bond H a water molecule In elements and compounds, the atoms are held together by chemical bonds. Forming a bond makes an atom more stable, so atoms form as many bonds are they
More informationAP CHEMISTRY CHAPTERS 5 & 6 Problem Set #4. (Questions 1-13) Choose the letter that best answers the question or completes the statement.
NAME: AP CHEMISTRY CHAPTERS 5 & 6 Problem Set #4 (Questions 1-13) Choose the letter that best answers the question or completes the statement. (Questions 1-2) Consider atoms of the following elements.
More informationFind the difference in electronegativity between the hydrogen and chlorine atoms
Answers Questions 16.2 Molecular polarity 1. Write a dot diagram for the HCl molecule. Find the difference in electronegativity between the hydrogen and chlorine atoms Difference in electronegativity =
More informationChapter 8 Covalent Boding
Chapter 8 Covalent Boding Molecules & Molecular Compounds In nature, matter takes many forms. The noble gases exist as atoms. They are monatomic; monatomic they consist of single atoms. Hydrogen chloride
More informationUNIT F321: ATOMS, BONDS AND GROUPS REVISION CHECKLIST. Miscellaneous Questions
UNIT F321: ATOMS, BONDS AND GROUPS REVISION CHECKLIST Miscellaneous Questions 1.1 Module 1: Atoms and Reactions 1.1.1 Atoms Candidates should be able to: Atomic structure (a) describe protons, neutrons
More informationAll chemical bonding is based on the following relationships of electrostatics: 2. Each period on the periodic table
UNIT VIII ATOMS AND THE PERIODIC TABLE 25 E. Chemical Bonding 1. An ELECTROSTATIC FORCE is All chemical bonding is based on the following relationships of electrostatics: The greater the distance between
More informationExam Review Questions - Multiple Choice
Exam Review Questions - Multiple Choice The following questions are for review. They are in no particular order. 1. An atom of iron 56 26Fe has... a) 26 protons, 26 electrons, 30 neutrons b) 30 protons,
More informationChemistry Chapter 6 Test Review
Chemistry Chapter 6 Test Review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. A mutual electrical attraction between the nuclei and valence electrons
More informationCh 6 Chemical Bonding
Ch 6 Chemical Bonding What you should learn in this section (objectives): Define chemical bond Explain why most atoms form chemical bonds Describe ionic and covalent bonding Explain why most chemical bonding
More informationChapter 7. Ionic & Covalent Bonds
Chapter 7 Ionic & Covalent Bonds Ionic Compounds Covalent Compounds 7.1 EN difference and bond character >1.7 = ionic 0.4 1.7 = polar covalent 1.7 Electrons not shared at
More information[2]... [1]
1 Carbon and silicon are elements in Group IV. Both elements have macromolecular structures. (a) Diamond and graphite are two forms of the element carbon. (i) Explain why diamond is a very hard substance....
More informationChapter 7 Chemical Bonding and Molecular Structure
Chapter 7 Chemical Bonding and Molecular Structure Three Types of Chemical Bonding (1) Ionic: formed by electron transfer (2) Covalent: formed by electron sharing (3) Metallic: attraction between metal
More informationName AP CHEM / / Chapter 8 Outline Bonding: General Concepts
Name AP CHEM / / Chapter 8 Outline Bonding: General Concepts Types of Chemical Bonds Information about the strength of a bonding interaction is obtained by measuring the bond energy, which is the energy
More informationVSEPR & Molecular Geometry
Bonding Packet Page 1 of 10 Chemistry Bonding Revisited and molecular structures PLEASE BRING YOUR OLD BONDING PACKET, too! VOCABULARY: 1. ionic bonds 2. covalent bonds 3. molecule 4. metallic bond 5.
More informationAtoms have the ability to do two things in order to become isoelectronic with a Noble Gas.
CHEMICAL BONDING Atoms have the ability to do two things in order to become isoelectronic with a Noble Gas. 1.Electrons can be from one atom to another forming. Positive ions (cations) are formed when
More informationSPECIMEN. Candidate Number
Advanced Subsidiary GCE CHEMISTRY A F321 QP Unit F321: Atoms, Bonds and Groups Specimen Paper Candidates answer on the question paper. Additional Materials: Data Sheet for Chemistry (Inserted) Scientific
More information1.3 Bonding. They have full outer shells and the electrons are paired with opposite spins fulfilling the 'octet rule'.
1.3 Bonding Electron configuration: They have full outer shells and the electrons are paired with opposite spins fulfilling the 'octet rule'. Bonding: All other elements on the periodic table will combine
More informationMultiple Choice Identify the choice that best completes the statement or answers the question.
Covalent Practice CP November 2015 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Bromine, atomic number 35, belongs to Group 17. How many electrons does
More informationAS LEVEL CHEMISTRY BONDING AND STRUCTURE PERIODICITY
AS LEVEL CHEMISTRY BONDING AND STRUCTURE PERIODICITY Answer all questions Max 90 marks Name.. Mark../90...% Grade Paddington Academy 1 1. Draw a dot-and-cross diagram for CaCl 2. [Total 2 marks] 2. Magnesium
More informationCHAPTER 12: CHEMICAL BONDING
CHAPTER 12: CHEMICAL BONDING Problems: 1-26, 27c, 28, 33-34, 35b, 36(a-c), 37(a,b,d), 38a, 39-40, 41-42(a,c), 43-58, 67-74 12.1 THE CHEMICAL BOND CONCEPT chemical bond: what holds atoms or ions together
More informationAmerican International School of Johannesburg. Quantitative Revision Questions II
American International School of Johannesburg Quantitative Revision Questions II 1. A toxic gas, A, consists of 53.8 % nitrogen and 46.2 % carbon by mass. At 273 K and 1.01 10 5 Pa, 1.048 g of A occupies
More informationIGCSE Double Award Extended Coordinated Science
IGCSE Double Award Extended Coordinated Science Chemistry 3.5 & 3.6 - Covalent Bonds Covalent Bond You need to know what covalent bonding is. Like ionic bonds, covalent bonds are another type of chemical
More informationChemical Bonds In elements and compounds, the atoms are held together by chemical bonds.
Chemical Bonds In elements and compounds, the atoms are held together by chemical bonds. Forming a bond makes an atom more stable, so atoms form as many bonds are they are able to. Bonds are made using
More informationName Unit Three MC Practice March 15, 2017
Unit Three: Bonding & Molecular Geometry Name Unit Three MC Practice March 15, 2017 1. What is the hybridization of the oxygen atom in water? a) sp b) sp 2 c) sp 3 d) It is not hybridized 2. When a double
More informationForm Code X. (1) 2.56 x photons (2) 5.18 x photons (3) 9.51 x photons (4) 5.15 x photons (5) 6.
Form Code X CHM 1025, Summer 2018 NAME Final Review Packet (Teaching Center) Final Packet Instructions: Do your best and don t be anxious. Read the question, re-read the question, write down all given
More informationUNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level *156507654 3 * CHEMISTRY 9701/21 Paper 2 Structured Questions AS Core May/June
More information5072 CHEMISTRY (NEW PAPERS WITH SPA) BASIC TECHNIQUES 5067 CHEMISTRY (NEW PAPERS WITH PRACTICAL EXAM) BASIC TECHNIQUES
5072 CHEMISTRY (NEW PAPERS WITH SPA) BASIC TECHNIQUES 5067 CHEMISTRY (NEW PAPERS WITH PRACTICAL EXAM) BASIC TECHNIQUES LEARNING OUTCOMES a) Be able to write formulae of simple compounds b) Be able to write
More informationMarkscheme May 2017 Chemistry Standard level Paper 2
M7/4/CHEMI/SP/ENG/TZ/XX/M Markscheme May 07 Chemistry Standard level Paper pages M7/4/CHEMI/SP/ENG/TZ/XX/M This markscheme is the property of the International Baccalaureate and must not be reproduced
More informationQuantitative chemistry Atomic structure Periodicity
IB chemistry Units 1-3 review Quantitative chemistry Significant figures The mole- be able to convert to number of particles and mass Finding empirical and molecular formulas from mass percentage States
More informationAdvanced Subsidiary Unit 1: The Core Principles of Chemistry
Write your name here Surname Other names Pearson Edexcel GCE Centre Number Chemistry Advanced Subsidiary Unit 1: The Core Principles of Chemistry Candidate Number Friday 27 May 2016 Morning Time: 1 hour
More informationAdvanced Subsidiary Unit 1: The Core Principles of Chemistry
Write your name here Surname Other names Pearson Edexcel International Advanced Level Centre Number Chemistry Advanced Subsidiary Unit 1: The Core Principles of Chemistry Candidate Number Friday 26 May
More informationBonding/Lewis Dots Lecture Page 1 of 12 Date. Bonding. What is Coulomb's Law? Energy Profile: Covalent Bonds. Electronegativity and Linus Pauling
Bonding/Lewis Dots Lecture Page 1 of 12 Date Bonding What is Coulomb's Law? Energy Profile: Covalent Bonds Electronegativity and Linus Pauling 2.1 H 1.0 Li 0.9 Na 0.8 K 0.8 Rb 0.7 Cs 0.7 Fr 1.5 Be 1.2
More informationNOTES: Unit 4: Bonding
Name: Regents Chemistry: Mr. Palermo Student Version NOTES: Unit 4: Bonding Name: 1. Ion 2. Positive/Negative ion 3. Stable Octet 4. Diatomic Molecules 5. Electronegativity 6. Ionic Bond 7. Covalent Bond
More informationCHEMICAL BONDING IONIC BONDS COVALENT BONDS HYDROGEN BONDS METALLIC BONDS
CHEMICAL BONDING IONIC BONDS COVALENT BONDS HYDROGEN BONDS METALLIC BONDS IONIC BONDING When an atom of a nonmetal takes one or more electrons from an atom of a metal so both atoms end up with eight valence
More informationChapter 9. Lewis Theory-VSEPR Valence Bond Theory Molecular Orbital Theory
Chapter 9 Lewis Theory-VSEPR Valence Bond Theory Molecular Orbital Theory Problems with Lewis Theory Lewis theory generally predicts trends in properties, but does not give good numerical predictions.
More informationMOLECULAR ORBITAL DIAGRAM KEY
365 MOLECULAR ORBITAL DIAGRAM KEY Draw molecular orbital diagrams for each of the following molecules or ions. Determine the bond order of each and use this to predict the stability of the bond. Determine
More informationTHE ST. MICHAEL SCHOOL THIRD FORM CHEMISTRY MANUAL 3 SYMBOLS AND FORMULAE, CHEMICAL BONDING AND CHEMICAL EQUATIONS
1 THE ST. MICHAEL SCHOOL THIRD FORM CHEMISTRY MANUAL 3 SYMBOLS AND FORMULAE, CHEMICAL BONDING AND CHEMICAL EQUATIONS COMPILED BY G.WALKER, L.WORRELL, T. HARDING REFERENCE BOOKS Anne Tindale Chemistry A
More informationT2-1P1 [187 marks] [1 mark] How many protons, neutrons and electrons are present in each atom of 31 P? [1 mark]
T2-1P1 [187 marks] 1. How many protons, neutrons and electrons are present in each atom of 31 P? 2. What is the atomic number of a neutral atom which has 51 neutrons and 40 electrons? A. 40 B. 51 C. 91
More informationCHEMISTRY Matter and Change Section 8.1 The Covalent Bond
CHEMISTRY Matter and Change Section Chapter 8: Covalent Bonding CHAPTER 8 Table Of Contents Section 8.2 Section 8.3 Section 8.4 Section 8.5 Naming Molecules Molecular Structures Molecular Shapes Electronegativity
More informationUse the concept of electronegativity to justify why the acid strengths of ethanedioic acid and ethanoic acid are different
Which molecule has the largest dipole? A ClF 3 B BF 3 C SF 6 D CF 4 (Total mark) 2 Which of these atoms has the highest electronegativity? A B C D Na Mg Cl Ar (Total mark) 3 Ethanedioic acid is a weak
More informationName 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 informationMolecular Geometry and intermolecular forces. Unit 4 Chapter 9 and 11.2
1 Molecular Geometry and intermolecular forces Unit 4 Chapter 9 and 11.2 2 Unit 4.1 Chapter 9.1-9.3 3 Review of bonding Ionic compound (metal/nonmetal) creates a lattice Formula doesn t tell the exact
More informationChemistry and the material world Lecture 3
Chemistry and the material world 123.102 Lecture 3 Electronic bookkeeping we need a way of finding out in which proportions two or more atoms make up a molecule is it CH 3 or CH 4 or CH 5? counting valence
More informationSubtopic 4.2 MOLECULAR SHAPE AND POLARITY
Subtopic 4.2 MOLECULAR SHAPE AND POLARITY 1 LEARNING OUTCOMES (covalent bonding) 1. Draw the Lewis structure of covalent molecules (octet rule such as NH 3, CCl 4, H 2 O, CO 2, N 2 O 4, and exception to
More informationIB Chemistry. Chapter 4.1
IB Chemistry Chapter 4.1 Chemical Bonds Atoms or ions that are strongly attached to one another Chemical bonds will form if potential energy decreases (becomes more stable) 2 Valence Electrons Valence
More information