# Complete the table to show the relative charge of each particle and the number of each particle found in a 140 Ce 2+ ion.

Save this PDF as:

Size: px
Start display at page:

Download "Complete the table to show the relative charge of each particle and the number of each particle found in a 140 Ce 2+ ion."

## Transcription

1 1 This question is about the elements with atomic numbers between 58 and 70 (a) Cerium, atomic number 58, is a metal Complete the table to show the relative charge of each particle and the number of each particle found in a 140 Ce 2+ ion Particle proton neutron Relative charge of each particle Number of each particle present in a 140 Ce 2+ ion electron [2] (b) Cerium behaves as a typical metal when it reacts with dilute sulfuric acid to form the salt cerium(iii) sulfate and a second product Identify the second product (ii) Write the formula of cerium(iii) sulfate and, explain what has happened to the cerium in this reaction in terms of the number of electrons transferred Formula Explanation [2] (iii) How has a salt been formed in this reaction?

2 (c) Europium, atomic number 63, reacts with oxygen at room temperature 4Eu + 3O 2 2Eu 2 O 3 Calculate the volume of oxygen, in cm 3, required to fully react with 912 g of europium at room temperature and pressure Volume = cm 3 [2] (d) A compound of thulium, atomic number 69, has the following composition by mass: O 307% S 154% Tm 539% State what is meant by the term empirical formula (ii) Determine the empirical formula of the compound Show your working Empirical formula = [2]

3 (e) Ytterbium, atomic number 70, is the first element in the Periodic Table to have the first four shells full State the number of electrons in the fourth shell of ytterbium [1] (ii) How many orbitals are there in the third shell of ytterbium? [1] [Total: 13]

4 2 This question is about Group 7 elements (a) Chlorine can be made by the redox reaction below MnO 2 (s) + 4HCl(aq) MnCl 2 (aq) + 2H 2 O(l) + Cl 2 (g) Using oxidation numbers, show what has been oxidised and what has been reduced in this reaction Oxidised Reduced [2] (b) Complete the electron configuration of a manganese atom 1s 2 (c) Chlorine gas can be added to a cold, dilute alkaline solution to form bleach Write the equation for this reaction [1] (d) A student bubbles chlorine gas through aqueous potassium iodide A reaction takes place State what the student would observe (ii) Write the ionic equation for this reaction Include state symbols

5 (e) Chlorine gas reacts with methane One of the products is dichloromethane, CH 2 Cl 2 Chlorine is more electronegative than carbon and hydrogen, which have approximately equal electronegativity values Explain what is meant by the term electronegativity [2] (ii) Draw a 3-D diagram of a molecule of CH 2 Cl 2 Use partial charges to indicate polar bonds [2] (iii) Explain why a CH 2 Cl 2 molecule is polar (f) Bromine has two isotopes, Br 79 and Br 81 The relative atomic mass of bromine is 799 Calculate the percentage of Br 79 atoms in a sample of bromine Answer = % [1] [Total: 12]

6 3 A student was given 200 cm 3 of solution X in which sodium hydroxide, NaOH, and sodium hydrogencarbonate, NaHCO 3, had both been dissolved The student carried out two different titrations on samples of solution X using 0100 mol dm 3 sulfuric acid, H 2 In the first titration, both NaOH and NaHCO 3 were neutralised In the second titration, only NaOH was neutralised The student s results for the titrations of 250 cm 3 samples of solution X are shown volume of H 2 needed to neutralise both NaOH and NaHCO cm 3 volume of H 2 needed to neutralise only NaOH 1800 cm 3 2NaOH(aq) + H 2 (aq) 2NaHCO 3 (aq) + H 2 (aq) Na 2 (aq) + 2H 2 O(l) Na 2 (aq) + 2H 2 O(l) + 2CO 2 (g) (a) Calculate the amount, in mol, of H 2 used to neutralise only the NaOH in 250 cm 3 of solution X Amount = mol [1] (ii) Calculate the concentration, in mol dm 3, of NaOH in solution X Concentration = mol dm 3 [1]

7 (b) Calculate the amount, in mol, of NaHCO 3 in the 200 cm 3 of solution X 11 (ii) Calculate the mass of NaHCO 3 in the 200 cm 3 of solution X Give your answer to three significant figures Amount = mol [2] Mass = g [1] [Total: 5]

8 4 Calcium is in Group 2 of the Periodic Table The diagram shows some reactions of calcium and its compounds Calcium Calcium carbonate Reaction 1 Reaction 2 Calcium oxide Calcium hydroxide (a) Reactions 1 and 2 both form calcium oxide Write the equation for reaction 1 (ii) What type of reaction is reaction 2? (b) Calcium hydroxide is both a base and an alkali Refer to any relevant ions in your answer Explain what is meant by the terms base and alkali Base Alkali [2]

9 (c) A student prepared some calcium hydroxide by adding a small piece of calcium to a large excess of water Describe what the student would observe and write the equation for the reaction Observation Equation [2] (d) A student prepares a solution of calcium nitrate from calcium carbonate What reagent would the student need to use? Write the equation for the reaction Reagent Equation [2] [Total: 8]

10 5 Antimony, Sb, has atomic number 51 (a) Complete the table below to show where antimony is found in the Periodic Table Period Block [1] (b) Antimony exists as a mixture of isotopes What is meant by the term isotopes? (ii) Different isotopes of antimony have the same chemical properties Explain why (iii) Complete the table below to show the atomic structure of 121 Sb Protons Neutrons Electrons [1] (c) The relative atomic mass of antimony is 1218 Define the term relative atomic mass [3]

11 (ii) A sample of antimony, A r = 1218, was analysed and was found to consist of 60% 121 Sb and one other isotope Determine the mass number of the other isotope in the sample of antimony mass number of the other antimony isotope = [1] (d) Antimony chloride, SbCl 3, exists as simple covalent molecules A dot-and-cross diagram of SbCl 3 is shown below Cl Sb Cl Cl Predict the shape of a molecule of SbCl 3 Explain your answer name of shape: explanation: [3] (ii) SbCl 3 molecules are polar Explain why [2] [Total: 13]

12 6 This question is about compounds used in fertilisers (a) A compound used as a fertiliser has the following composition by mass: C, 2000%; H, 667%; N, 4667%; O, 2666% Calculate the empirical formula of this compound empirical formula = [2] (b) A salt used as a fertiliser has the empirical formula H 4 N 2 O 3 Suggest the formulae of the ions present in this salt [2] (c) Calcium phosphate(v), Ca 3 (PO 4 ) 2, is another salt used in fertilisers Calcium phosphate(v) can be prepared by reacting together an acid and a base Suggest the formula of the acid used to prepare Ca 3 (PO 4 ) 2 (ii) Name a base which could be used to prepare Ca 3 (PO 4 ) 2 [Total: 6]

13 7 An aqueous solution of aluminium chloride can be prepared by the redox reaction between aluminium metal and dilute hydrochloric acid A student reacts mol of aluminium completely with dilute hydrochloric acid to form an aqueous solution of aluminium chloride The equation for this reaction is shown below 2Al(s) + 6HCl(aq) 2Al Cl 3 (aq) + 3H 2 (g) (a) In terms of electron transfer, explain whether aluminium is being oxidised or reduced [1] (b) Calculate the volume of hydrogen gas formed, in dm 3, at room temperature and pressure volume of hydrogen gas formed = dm 3 [2] (c) Calculate the mass of Al Cl 3 formed Give your answer to three significant figures mass of Al Cl 3 formed = g [2] (d) Calculate the volume, in cm 3, of 120 mol dm 3 hydrochloric acid needed to react completely with mol of aluminium volume = cm 3 [2] [Total: 7]

14 8 Silicon and potassium are two elements found in the Earth s crust (a) Silicon and potassium both exist as several isotopes Define the term relative isotopic mass [2] (ii) Complete the table below for an atom and an ion of two different isotopes of potassium Protons Neutrons Electrons 39 K [2] (b) Complete the electron configuration of a silicon atom 1s 2 (c) Silicon reacts with chlorine to form molecules of silicon tetrachloride, SiCl 4 How many molecules are present in 8505 g of SiCl 4? answer = molecules [3]

15 (ii) Potassium reacts with chlorine to form an ionic lattice of potassium chloride, KCl A diagram of part of the potassium chloride lattice is shown below Add labels to each circle in the diagram to show the particles present in the lattice The diagram assumes all particles have the same size [2] [Total: 10]

### ... [1] (ii) Draw a dot-and-cross diagram to show the bonding in NH 3

1 Chemists have developed models for bonding and structure which are used to explain different properties. (a) Ammonia, NH 3, is a covalent compound. Explain what is meant by a covalent bond. Draw a dot-and-cross

### F321: Atoms, Bonds and Groups Moles and Equations

F321: Atoms, Bonds and Groups Moles and Equations 108 Marks 1. (a) A student carries out a titration to find the concentration of some sulfuric acid. The student finds that 25.00 cm 3 of 0.0880 mol dm

### 1 Sulfur, atomic number 16, is found within the Earth s crust. Sulfur is released into the atmosphere at times of volcanic activity.

1 Sulfur, atomic number 16, is found within the Earth s crust. Sulfur is released into the atmosphere at times of volcanic activity. A sample of sulfur from a volcano was analysed to give the following

### F321: Atoms, Bonds and Groups Redox

F321: Atoms, Bonds and Groups Redox 39 Marks 1. The element strontium forms a nitrate, Sr(NO 3 ) 2, which decomposes on heating as shown below. 2Sr(NO 3 ) 2 (s) 2SrO(s) + 4NO 2 (g) + O 2 (g) Using oxidation

### For the element X in the ionic compound MX, explain the meaning of the term oxidation state.

1. (a) By referring to electrons, explain the meaning of the term oxidising agent.... For the element X in the ionic compound MX, explain the meaning of the term oxidation state.... (c) Complete the table

### , are both bases., can be prepared by reacting ammonia with sulfuric acid, H 2. Why can ammonium sulfate be described as a salt?......

1 Ammonia, NH 3, and hydrazine, N 2 H 4, are both bases. (a) Ammonium sulfate, (NH 4 ) 2, can be prepared by reacting ammonia with sulfuric acid, H 2. Why can ammonium sulfate be described as a salt?..

### Elements in the Periodic Table show a periodic trend in atomic radius. In your answer you should use appropriate technical terms, spelled correctly.

1 The Periodic Table is arranged in periods and groups (a) Elements in the Periodic Table show a periodic trend in atomic radius State and explain the trend in atomic radius from Li to F In your answer

### London Examinations IGCSE

Centre No. Candidate No. Paper Reference 4 3 3 5 2 H Paper Reference(s) 4335/2H London Examinations IGCSE Chemistry Paper 2H Higher Tier Wednesday 21 May 2008 Afternoon Time: 2 hours Surname Signature

### UNIT 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

1 Chlorine and bromine are elements in Group 7 of the Periodic Table. (a) Chlorine is used in water treatment. State one advantage and one disadvantage of using chlorine in water treatment. advantage:...

### Subject: Chemistry Foundation Code: Session: January Year: Final Mark Scheme

Subject: Code: 2811 Session: January Year: 2001 Final Mark Scheme 14th Jan 2001 MAXIMUM MARK 90 Page 1 of 1 3882 January 2001 Answer all questions 1. Lithium was discovered in 1817 by the Swedish chemist

### PRACTICE EXAMINATION QUESTIONS FOR 1.2 AMOUNT OF SUBSTANCE

PRACTICE EXAMINATION QUESTIONS FOR 1.2 AMOUNT OF SUBSTANCE 1. Nitroglycerine, C 3 H 5 N 3 O 9, is an explosive which, on detonation, decomposes rapidly to form a large number of gaseous molecules. The

### Write down everything that the word equation tells you about the reaction (Total 4 marks)

Q1. Here is a word equation for a chemical reaction. copper oxide + sulphuric acid copper sulphate + water Write down everything that the word equation tells you about the reaction.......... (Total 4 marks)

### SPECIMEN. 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

### Personalised Learning Checklists AQA Chemistry Paper 1

AQA Chemistry (8462) from 2016 Topics C4.1 Atomic structure and the periodic table State that everything is made of atoms and recall what they are Describe what elements and compounds are State that elements

### burette filled with sulphuric acid conical flask 25.0 cm 3 of sodium hydroxide(aq) concentration 2.24 mol / dm 3

1 Crystals of sodium sulphate-10-water, Na 2 SO 4.10H 2 O, are prepared by titration. burette filled with sulphuric acid conical flask 25.0 cm 3 of sodium hydroxide(aq) concentration 2.24 mol / dm 3 (a)

### Personalised Learning Checklists AQA Trilogy Chemistry Paper 1

AQA TRILOGY Chemistry (8464) from 2016 Topics T5.1 Atomic structure and the periodic table State that everything is made of atoms and recall what they are Describe what elements and compounds are State

### 6V d.c. supply. State the form of energy used to carry out the electrolysis. (1)

1 (a) Water, acidified with a small amount of dilute sulfuric acid, can be decomposed by electrolysis using the apparatus shown. oxygen hydrogen acidified water + (i) 6V d.c. supply State the form of energy

### Atoms, Elements, Atoms, Elements, Compounds and Mixtures. Compounds and Mixtures. Atoms and the Periodic Table. Atoms and the.

Atoms, Elements, Compounds and Mixtures Explain how fractional distillation can be used to separate a mixture. 1 Atoms, Elements, Compounds and Mixtures Fractional distillation is used to separate components

### (i) Calculate the amount, in moles, of HCl in 33.2 cm 3 of mol dm 3 hydrochloric acid. Give your answer to 3 significant figures. ...

Q1. (a) An unknown metal carbonate reacts with hydrochloric acid according to the following equation. M 2CO 3(aq) + 2HCl(aq) 2MCl(aq) + CO 2(g) + H 2O(l) A 3.44 g sample of M 2CO 3 was dissolved in distilled

### Page 1. Exam 2 Review Summer A 2002 MULTIPLE CHOICE. 1. Consider the following reaction: CaCO (s) + HCl(aq) CaCl (aq) + CO (g) + H O(l)

Page 1 MULTIPLE CHOICE 1. Consider the following reaction: CaCO (s) + HCl(aq) CaCl (aq) + CO (g) + H O(l) The coefficient of HCl(aq) in the balanced reaction is. a) 1 b) 2 c) 3 d) 4 e) 0 2. Given the information

### Shapes 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?

### Chemical Reactions. Ch. 11 Chemical Reactions. Chemical Reactions. Chemical Reactions

Chemical Reactions Ch. 11 Chemical Reactions when a substance changes identity Reactants - original Products - resulting law of conservation of mass total mass of reactants = total mass of products In

### Chapter 4 Types of Chemical Reaction and Solution Stoichiometry

Chapter 4 Types of Chemical Reaction and Solution Stoichiometry Water, the Common Solvent One of the most important substances on Earth. Can dissolve many different substances. A polar molecule because

### CH 221 Chapter Four Part II Concept Guide

CH 221 Chapter Four Part II Concept Guide 1. Solubility Why are some compounds soluble and others insoluble? In solid potassium permanganate, KMnO 4, the potassium ions, which have a charge of +1, are

Questions and Mark Scheme from OCR AS GCE CHEMISTRY A with links to video explanations on Youtube F321/01 Atoms, Bonds and Groups January 2013 Duration: 1 hour Click here to start Note: The material presented

### NSS Chemistry Part 2 The Microscopic World I HKCEE Past Paper Questions Structural Questions

NSS Chemistry Part 2 The Microscopic World I HKCEE Past Paper Questions Structural Questions 1. HKCEE 1994 Q7b The table below lists some physical properties of lead, bromine and lead(ii) bromide. Lead

### Show by calculation that the starting concentration of the manganate(vii) ions was mol dm 3.

1. Manganate(VII) ions react with ethanedioate ions in acidic solution. MnO 4 (aq) + 16H + (aq) + 5C O 4 (aq) Mn + (aq) + 8H O(l) + 10CO (g) (a) In a particular experiment 00 cm of aqueous potassium manganate(vii),

### , are both macromolecules. They have similar physical properties but silicon(iv) oxide is acidic and zirconium(iv) oxide is amphoteric

1 Silicon(IV) oxide, SiO 2, and zirconium(iv) oxide, ZrO 2, are both macromolecules. They have similar physical properties but silicon(iv) oxide is acidic and zirconium(iv) oxide is amphoteric. (a) Defi

### States of matter

3.1.3.4 States of matter 261 minutes 257 marks Page 1 of 30 Q1. (a) Describe the bonding in a metal. Explain why magnesium has a higher melting point than sodium. (4) (b) Why do diamond and graphite both

### Titration curves, labelled E, F, G and H, for combinations of different aqueous solutions of acids and bases are shown below.

Titration curves, labelled E, F, G and H, for combinations of different aqueous solutions of acids and bases are shown below. All solutions have concentrations of 0. mol dm 3. (a) In this part of the question,

### AQA Chemistry (Combined Science) Specification Checklists. Name: Teacher:

AQA Chemistry (Combined Science) Specification Checklists Name: Teacher: Paper 1-4.1 Atomic structure and the periodic table 4.1.1 A simple model of the atom, symbols, relative atomic mass, electronic

### AS Paper 1 Group VII: The Halogens

AS Paper 1 Group VII: The Halogens South Axholme School Q1.Which one of the following statements is true? A B C D Bromine liberates iodine from aqueous sodium iodide. Chlorine liberates fluorine from aqueous

### FACTFILE: GCE CHEMISTRY

FACTFILE: GCE CHEMISTRY HALOGENS Halogens Students should be able to: 1.8.1 recall the colours of the elements and explain the trends within the Group, limited to physical state at room temperature, melting

### 1.24 Calculations and Chemical Reactions

1.24 Calculations and Chemical Reactions Converting quantities between different substances using a balanced equation A balanced chemical equation tells us the number of particles of a substance which

### A student adds the following volumes of aqueous sodium thiosulfate, dilute hydrochloric acid and distilled water to the conical flask.

1 When aqueous sodium thiosulfate and dilute hydrochloric acid are mixed, a precipitate of insoluble sulfur is produced. This makes the mixture difficult to see through. Na 2 S 2 O 3 (aq) + 2HCl (aq) S(s)

### Hydrated nickel(ii) salts are green in colour. Give the electron configuration of a nickel(ii) ion and hence state why the ion is coloured.

1. This question is about nickel compounds. (a) Hydrated nickel(ii) salts are green in colour. Give the electron configuration of a nickel(ii) ion and hence state why the ion is coloured.......... (b)

### Chapter 4 Reactions in Aqueous Solution

Chapter 4 Reactions in Aqueous Solution Homework Chapter 4 11, 15, 21, 23, 27, 29, 35, 41, 45, 47, 51, 55, 57, 61, 63, 73, 75, 81, 85 1 2 Chapter Objectives Solution To understand the nature of ionic substances

### Additional Science. Chemistry CH2FP. (Jun13CH2FP01) General Certificate of Secondary Education Foundation Tier June 2013.

Centre Number Surname Candidate Number For Examiner s Use Other Names Candidate Signature Examiner s Initials Additional Science Unit Chemistry C2 Chemistry Unit Chemistry C2 Monday 20 May 2013 General

### 1. Hydrochloric acid is mixed with aqueous sodium bicarbonate Molecular Equation

NAME Hr Chapter 4 Aqueous Reactions and Solution Chemistry Practice A (Part 1 = Obj. 1-3) (Part 2 = Obj. 4-6) Objective 1: Electrolytes, Acids, and Bases a. Indicate whether each of the following is strong,

### Chemical 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

### TOPIC 7. CHEMICAL CALCULATIONS I - atomic and formula weights.

TOPIC 7. CHEMICAL CALCULATIONS I - atomic and formula weights. Atomic structure revisited. In Topic 2, atoms were described as ranging from the simplest atom, H, containing a single proton and usually

### State the strongest type of interaction that occurs between molecules of hydrogen peroxide and water.

Q1.A hydrogen peroxide molecule can be represented by the structure shown. (a) Suggest a value for the H O O bond angle. (b) Hydrogen peroxide dissolves in water. (i) State the strongest type of interaction

### Concentration Units. Solute CONCENTRATION. Solvent. g L -1. (M, molarity) concentration in. mol / litre of solution. mol L -1. molality. molality.

CHAPTER 4 REACTIONS IN AQUEOUS SOLUTION CONCENTRATION Solute Solvent Concentration Units mass NaCl / unit volume of solution g L -1 (M, molarity) concentration in moles per litre of solution c NaCl c B

### 3.2.6 Group II. Trends in Chemical properties. 164 minutes. 161 marks. Page 1 of 19

3.2.6 Group II Trends in Chemical properties 164 minutes 161 marks Page 1 of 19 Q1. (a) A small sample of barium metal was added to water in a flask. When the reaction had ceased, the contents of the flask

### Practice I: Chemistry IGCSE

Practice I: Chemistry IGCSE cristian.obiol@gmail.com 1) Explain the following processes related to changes of states of matter. -Melting:... -Vaporization:... -Freezing:... -Condensation:... -Sublimation:...

### TOPIC: 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

### AQA GCSE CHEMISTRY (9-1) Topic 1: Atomic Structure and the Periodic Table

AQA GCSE CHEMISTRY (9-1) Topic 1: Atomic Structure and the Periodic Table 4.1.1 Atoms, elements and compounds 4.1.1.1 Atoms, elements and compounds All substances are made of atoms. An atom is the smallest

### 2014 Chemistry 1 st Semester Exam Review Packet

Name: Date: Hour: 2014 Chemistry 1 st Semester Exam Review Packet 1. What percentage of the water on Earth is salt water? (1 point) A. 97.2% B. 0.009% C. 2.11% D. 2.8 % 2. One similarity between all mixtures

### PHYSICAL SCIENCES: PAPER II

NATIONAL SENIOR CERTIFICATE EXAMINATION NOVEMBER 2017 PHYSICAL SCIENCES: PAPER II Time: 3 hours 200 marks PLEASE READ THE FOLLOWING INSTRUCTIONS CAREFULLY 1. This question paper consists of 19 pages, a

### Types of chemical reaction

Chemical misconceptions 57 Types of chemical reaction Target level Topics Rationale This probe is primarily designed for students in the 14 16 age range who have been introduced to the range of reaction

### Unit IV: Stoichiometry

Unit IV: Stoichiometry D. Calculations from chemical equations 1. Mol-mol calculations 2. Mol-gram calculations 3. Gram-gram calculations E. Limiting reactant (or reagent) F. Other applications of stoichiometry

### Identify the reaction type, predict the products, and balance the equations. If it is a special decomposition or synthesis, identify which kind.

Identify the reaction type, predict the products, and balance the equations. If it is a special decomposition or synthesis, identify which kind. 1. calcium + oxygen 2. cupric carbonate 3. aluminum + hydrochloric

### Advanced Subsidiary Unit 1: The Core Principles of Chemistry

Write your name here Surname Other names Edexcel GCE Centre Number Chemistry Advanced Subsidiary Unit 1: The Core Principles of Chemistry Candidate Number Thursday 23 May 2013 Morning Time: 1 hour 30 minutes

### 1 Carbon occurs in a wide range of compounds and is essential to living systems [1] Isotopes of carbon have the same chemical properties....

1 Carbon occurs in a wide range of compounds and is essential to living systems. (a) Two isotopes of carbon are 12 C and 13 C. State what is meant by the term isotopes. Isotopes of carbon have the same

### Write an overall equation for the first stage in the rusting of iron.

1. (a) Define the term standard electrode potential............. (b) When a metal is placed in a solution of its ions, the electrical potential set up between the metal and the solution cannot be measured

### THE BRIDGING COURSE TO SIXTH FORM CHEMISTRY AT Myton School

THE BRIDGING COURSE TO SIXTH FORM CHEMISTRY AT Myton School Introduction Before you start the AS Chemistry course in September you should have completed this new bridging course for Chemists. It has been

### Chemistry *P42864A0120* P42864A. Unit: KCH0/4CH0 Paper: 2C. Thursday 16 January 2014 Afternoon Time: 1 hour. Instructions. Information.

Write your name here Surname Other names Pearson Edexcel Certificate Pearson Edexcel International GCSE Chemistry Unit: KCH0/4CH0 Paper: 2C Centre Number Candidate Number Thursday 16 January 2014 Afternoon

### 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)

### NATIONAL 5 CHEMISTRY. Unit 1 Chemical Changes and Structure. Exam Questions

NATIONAL 5 CHEMISTRY Unit Chemical Changes and Structure Exam Questions Rates of Reaction 202 Int2 2. Rapid inflation of airbags in cars is caused by the production of nitrogen gas. The graph gives information

### , for C 2. COOH is mol dm [1] COOH by adding water until the total volume is cm 3. for C 2 COOH.

1 A student is supplied with 0.500 mol dm 3 potassium hydroxide, KOH, and 0.480 mol dm 3 propanoic acid, C 2 COOH. The acid dissociation constant, K a, for C 2 COOH is 1.35 10 5 mol dm 3. (a) C 2 COOH

### 2.3 Group 7 The Halogens

2.3 Group 7 The Halogens Physical properties of the Halogens: The melting and boiling point of the halogens increases with atomic number due to increased van der Waals (from increased number of electrons).

### Chapter 6: Chemical Bonding

Chapter 6: Chemical Bonding Learning Objectives Describe the formation of ions by electron loss/gain to obtain the electronic configuration of a noble gas. Describe the formation of ionic bonds between

### Reactions in Aqueous Solutions

Reactions in Aqueous Solutions 1 Chapter 4 General Properties of Aqueous Solutions (4.1) Precipitation Reactions (4.2) Acid-Base Reactions (4.3) Oxidation-Reduction Reactions (4.4) Concentration of Solutions

### Chapter 2: Mass Relations in Formulas, Chemical Reactions, and Stoichiometry

Previous Chapter Table of Contents Next Chapter Chapter 2: Mass Relations in Formulas, Chemical Reactions, and Stoichiometry Section 2.1: The Atomic Mass The atomic mass is the mass of 1 atom. Atoms are

### This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24

Name Hour January Exam Practice A This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24 This practice exam will be graded in the exam portion of the grade book. Objectives

### [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....

### Q1. The diagram shows the apparatus for an experiment. Hydrated copper sulphate crystals were heated. They became anhydrous copper sulphate.

Q1. The diagram shows the apparatus for an experiment. Hydrated copper sulphate crystals were heated. They became anhydrous copper sulphate. (a) Name a suitable piece of equipment to heat tube A.... (b)

### 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

### Ch 9 Stoichiometry Practice Test

Ch 9 Stoichiometry Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1. A balanced chemical equation allows one to determine the a. mole ratio

Please write clearly in block capitals. Centre number Candidate number Surname Forename(s) Candidate signature GCSE ADDITIONAL SCIENCE CHEMISTRY Foundation Tier Unit Chemistry C2 F Wednesday 15 June 2016

### 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

### No Brain Too Small. Credits: Four

No Brain Too Small Level 1 Science 2015 90944 Demonstrate understanding of aspects of acids and bases Credits: Four Achievement Achievement with Merit Achievement with Excellence Demonstrate understanding

### Bonding Review Worksheet

Bonding Review Worksheet 1. Complete the following chart: (first line is done as an example) isotope symbol isotope name atomic number (Z) mass number (A) protons neutrons 235 92 U uranium-235 92 235 92

### 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

### Complete and balance these equations to show the reactions during electrolysis. Na Na (2)

Q1. The diagram shows electrolysis of sodium chloride solution. (a) Complete and balance these equations to show the reactions during electrolysis. At the positive electrode Cl e Cl At the negative electrode

### SIR MICHELANGELO REFALO SIXTH FORM

SIR MIELANGELO REFALO SIXT FORM alf-yearly Exam 2016 Subject: hemistry ADV 1 ST Time: 3 hours Answer 6 questions. All questions carry equal marks. You are reminded of the importance of clear presentation

### EXAM 3 CHEM 1310 WS09 Key Version #2

EXAM 3 CHEM 1310 WS09 Key Version #2 1. (p. 116) Select the correct name and chemical formula for the precipitate that forms when the following reactants are mixed. CuCl 2 (aq) + Na 2 CO 3 (aq) A. copper(ii)

### Stoichiometry. Introduction. Rx between Hydrogen and Oxygen can be described as: Balanced equation: Or Avogadros Number: (number of Molecules)

Stoichiometry Introduction Rx between Hydrogen and Oxygen can be described as: Balanced equation: Or Or Avogadros Number: (number of Molecules) Or Moles (amount of a substance containing avogadros number

### (ii) Describe the structure of solid potassium iodide. You may draw a diagram. (iii) Explain why potassium iodide has a high melting point.

1 (a) Potassium iodide is an ionic compound. (i) Describe what happens, in terms of electron loss and gain, when a potassium atom reacts with an iodine atom. (ii) Describe the structure of solid potassium

### National 5 Chemistry

National 5 Chemistry Identified Past Paper Questions from SQA Credit and Intermediate 2 papers Unit : Chemical Changes and Structure March 204 Transforming lives through learning Chemistry N5 Past Paper

### PMT. GCE Chemistry A. Unit F321: Atoms, Bonds and Groups. Advanced Subsidiary GCE. Mark Scheme for June Oxford Cambridge and RSA Examinations

GCE Chemistry A Unit F321: Atoms, Bonds and Groups Advanced Subsidiary GCE Mark Scheme for June 2015 Oxford Cambridge and RSA Examinations OCR (Oxford Cambridge and RSA) is a leading UK awarding body,

### 1 Zirconium (Zr) is a metal in Period 5. Its main oxidation state is +4.

1 Zirconium (Zr) is a metal in Period 5. Its main oxidation state is +4. (a) The following are all zirconium atoms: 90 40Zr, 91 40Zr and 92 40Zr. In terms of numbers of electrons, neutrons and protons,

### TOPIC 9. CHEMICAL CALCULATIONS III - stoichiometry.

TOPIC 9. CHEMICAL CALCULATIONS III - stoichiometry. Stoichiometric calculations. By combining a knowledge of balancing equations with the concept of the mole, it is possible to easily calculate the masses

### Chapter 14 Acids and Bases

Properties of Acids and Bases Chapter 14 Acids and Bases Svante Arrhenius (1859-1927) First to develop a theory for acids and bases in aqueous solution Arrhenius Acids Compounds which dissolve (dissociate)

### Transition Pack for A Level Chemistry

Transition Pack for A Level Chemistry A guide to help you get ready for A-level Chemistry. You will be tested on this material in the week beginning 12 th September 2016 1 This booklet contains background

### M08/4/CHEMI/SP2/ENG/TZ2/XX CHEMISTRY. Thursday 8 May 2008 (afternoon) Candidate session number. 1 hour 15 minutes INSTRUCTIONS TO CANDIDATES

M08/4/CHEMI/SP2/ENG/TZ2/XX 22086117 CHEMISTRY standard level Paper 2 Thursday 8 May 2008 (afternoon) 1 hour 15 minutes 0 0 Candidate session number INSTRUCTIONS TO CANDIDATES Write your session number

### Atoms What subatomic particles make up the atom?

Atoms What subatomic particles make up the atom? What are the masses of the subatomic particles? What do atomic and mass number represent? What does 7 3 Li represent? How are elements arranged in the periodic

### 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

### Quantitative Chemistry

Quantitative Chemistry When we do experiments to measure something in Chemistry, we: Repeat experiments (usually 3 times) to improve the reliability of the results, by calculating an average of our results.

### Figure 1. Describe what happens when two atoms of potassium react with one atom of sulfur. Give your answer in terms of electron transfer

Q1.Figure 1 shows the outer electrons in an atom of the Group 1 element potassium and in an atom of the Group 6 element sulfur. Figure 1 (a) Potassium forms an ionic compound with sulfur. Describe what

### CHEMISTRY HONORS LEOCE Study Guide

BENCHMARK: N.1.1-1.2, N.1.6, N.3.1, N.3.3, N.3.4 CHEMISTRY HONORS CHEMISTRY AND SCIENTIFIC MEASUREMENT TEXTBOOK: Glencoe, Chemistry: Matter and Change, Chapters 1-3 ESSENTIAL QUESTION: How is measurement

### (Ex. from Past Exam Questions)

(Ex. from Past Exam Questions). CO 2 and SiO 2 are oxides of Group IV elements. (i) Account for the fact that CO 2 is a gas while SiO 2 is a high melting solid under room temperature and atmospheric pressure.

### Section B: Some Essential Background Chemistry

Section B: Some Essential Background Chemistry Soluble and insoluble salts The importance of knowing whether a salt is soluble or insoluble in water You will remember that acids react with carbonates to

### Molecule smallest particle of a substance having its chemical properties Atoms connected via covalent bonds Examples:

Ionic equations, calculations involving concentrations, stoichiometry MUDr. Jan Pláteník, PhD Molecule smallest particle of a substance having its chemical properties Atoms connected via covalent bonds

### ph calculations MUDr. Jan Pláteník, PhD Brønsted-Lowry concept of acids and bases Acid is a proton donor Base is a proton acceptor

ph calculations MUDr. Jan Pláteník, PhD Brønsted-Lowry concept of acids and bases Acid is a proton donor Base is a proton acceptor HCl(aq) + H 2 O(l) H 3 O + (aq) + Cl - (aq) Acid Base Conjugate acid Conjugate

### Advanced Subsidiary Unit 1: The Core Principles of Chemistry

Write your name here Surname Other names Edexcel GCE Centre Number Chemistry Advanced Subsidiary Unit 1: The Core Principles of Chemistry Candidate Number Tuesday 15 May 2012 Afternoon Time: 1 hour 30

### Chemistry Study Guide

Chemistry Study Guide Marking Period 3 Exam Week of 3/21/17 Study Guide due - When studying for this test, use your do nows, notes, homework, class handouts, and your textbook. Vocabulary Chapter 7 Anion