This document contains a chemistry exam with multiple choice and short answer questions testing knowledge of atomic structure, isotopes, ionization energies, and calculations involving relative atomic mass. The exam covers topics including:
- Completing tables of atomic and isotopic data
- Calculating relative atomic masses from isotopic abundances
- Defining terms like ionization energy, isotopes, and relative atomic mass
- Writing equations to represent changes in ionization state and electron affinity
- Explaining trends in ionization energies and relating atomic structure to reactivity
This document is a thesis submitted by Oded Bar-Lev towards a Doctor of Philosophy degree from Tel Aviv University. The thesis is focused on developing the kinetic and hydrodynamic theory of granular gases under the supervision of Prof. Philip Rosenau and Prof. Isaac Goldhirsch. It contains an abstract, introduction providing background on granular materials and granular gases, and outlines the structure of the thesis which includes chapters on kinetic theory, the homogeneous cooling state, hydrodynamics of nearly smooth granular gases, and conclusions.
This document is a textbook on drilling engineering that covers topics such as rotary drilling rig components and systems, geomechanics, drilling hydraulics, drill bits, and drillstring design. It provides detailed explanations of concepts and calculations with examples. The textbook is intended for a master's level course on petroleum engineering and drilling.
Here are explanations for the phenomena described:
a) Walking on wet ice is difficult because ice is very slippery when wet, providing little friction between the feet and surface.
b) It is difficult to strike a match on a smooth surface because friction is needed to generate enough heat from the striking surface to light the match head. A rough surface provides more friction.
c) Pulling a boat on land is more difficult than in water because water provides less resistance (friction) than sand or rocks on a beach. The boat slides more easily through water.
d) Wet floors and roads are dangerous because water reduces the friction between shoes/tires and the surface, making it easier to slip and lose traction.
An explosion inside the Pantheon in Rome was simulated using three numerical models to calculate blast pressures (JWL, TM5-1300, CONWEP) and finite element analysis to model the structure's response. The pressure fields and structural damage evolution over time were examined. For the aircraft fuselage case, the aluminum alloy material behavior and a proposed passive protective device were modeled. Numerical simulations assessed the device's ability to mitigate in-cabin blast effects on the fuselage. Mesh sensitivity studies were performed for both fluid and structural domains. The simulations provide insight into protecting historic structures and aircraft from explosive blasts.
Thomas E. Brown is seeking a manager position that will challenge his personal and career growth. He has over 30 years of experience in facilities maintenance, including preventative maintenance, repair of equipment, and ensuring reliability. His background encompasses electrical systems, automation, hydraulics, pneumatics, and more.
IQANZ Presentation to Enterprise Architecture Meet UP Group Cover page LIKobus Dippenaar
The document provides an overview of IQANZ, a professional services organization that specializes in independent assurance services for business and ICT initiatives. It discusses IQANZ's technical quality assurance services, which include reviewing initiatives to ensure alignment with standards and best practices. The services cover the project lifecycle from requirements through implementation and include specialized areas like Agile projects, solution design, and data governance. IQANZ takes a continuous improvement approach and has expertise reviewing a wide range of technical and enterprise areas.
Este documento proporciona una lista de 4 personas admitidas a una convocatoria con su nombre, fecha de nacimiento y estatura. También incluye la liquidación de una cuenta bancaria con los movimientos, saldos y días de cada operación, así como los intereses acreedores y la retención a cuenta aplicada.
This document is a thesis submitted by Oded Bar-Lev towards a Doctor of Philosophy degree from Tel Aviv University. The thesis is focused on developing the kinetic and hydrodynamic theory of granular gases under the supervision of Prof. Philip Rosenau and Prof. Isaac Goldhirsch. It contains an abstract, introduction providing background on granular materials and granular gases, and outlines the structure of the thesis which includes chapters on kinetic theory, the homogeneous cooling state, hydrodynamics of nearly smooth granular gases, and conclusions.
This document is a textbook on drilling engineering that covers topics such as rotary drilling rig components and systems, geomechanics, drilling hydraulics, drill bits, and drillstring design. It provides detailed explanations of concepts and calculations with examples. The textbook is intended for a master's level course on petroleum engineering and drilling.
Here are explanations for the phenomena described:
a) Walking on wet ice is difficult because ice is very slippery when wet, providing little friction between the feet and surface.
b) It is difficult to strike a match on a smooth surface because friction is needed to generate enough heat from the striking surface to light the match head. A rough surface provides more friction.
c) Pulling a boat on land is more difficult than in water because water provides less resistance (friction) than sand or rocks on a beach. The boat slides more easily through water.
d) Wet floors and roads are dangerous because water reduces the friction between shoes/tires and the surface, making it easier to slip and lose traction.
An explosion inside the Pantheon in Rome was simulated using three numerical models to calculate blast pressures (JWL, TM5-1300, CONWEP) and finite element analysis to model the structure's response. The pressure fields and structural damage evolution over time were examined. For the aircraft fuselage case, the aluminum alloy material behavior and a proposed passive protective device were modeled. Numerical simulations assessed the device's ability to mitigate in-cabin blast effects on the fuselage. Mesh sensitivity studies were performed for both fluid and structural domains. The simulations provide insight into protecting historic structures and aircraft from explosive blasts.
Thomas E. Brown is seeking a manager position that will challenge his personal and career growth. He has over 30 years of experience in facilities maintenance, including preventative maintenance, repair of equipment, and ensuring reliability. His background encompasses electrical systems, automation, hydraulics, pneumatics, and more.
IQANZ Presentation to Enterprise Architecture Meet UP Group Cover page LIKobus Dippenaar
The document provides an overview of IQANZ, a professional services organization that specializes in independent assurance services for business and ICT initiatives. It discusses IQANZ's technical quality assurance services, which include reviewing initiatives to ensure alignment with standards and best practices. The services cover the project lifecycle from requirements through implementation and include specialized areas like Agile projects, solution design, and data governance. IQANZ takes a continuous improvement approach and has expertise reviewing a wide range of technical and enterprise areas.
Este documento proporciona una lista de 4 personas admitidas a una convocatoria con su nombre, fecha de nacimiento y estatura. También incluye la liquidación de una cuenta bancaria con los movimientos, saldos y días de cada operación, así como los intereses acreedores y la retención a cuenta aplicada.
This document describes an experiment to determine the empirical formula of copper oxide. The combustion tube containing porcelain dish and oxide of copper is weighed before and after heating. The following data is obtained: mass of combustion tube + porcelain dish = 19.60 g, mass after adding oxide of copper = 25.68 g, mass after heating = 24.46 g. The student is asked to calculate the empirical formula of copper oxide using this data. Additional questions relate to the apparatus setup, chemical equation, and determining empirical formulas of other substances.
The document is a chemistry exam paper containing multiple questions on topics related to electricity and chemistry. It includes questions about the extraction of zinc from zinc blende, the purification of zinc by electrolysis, corrosion of steel and its prevention, the extraction of iron in the blast furnace, and catalysts in chemical reactions. The questions require students to write word and ionic equations, explain observations, complete descriptions, and suggest explanations.
AQA AS Chemistry Atomic Structure QuestionsGodschild24
This document contains sample chemistry problems and questions regarding various topics:
1) Using the ideal gas equation to calculate the volume of ethanol vapor under certain pressure and temperature conditions.
2) Balancing a chemical equation and calculating moles of a substance produced.
3) Calculating the maximum mass of a product formed from a given mass of a reactant over two reaction stages.
4) Stating the relative charge and mass of an electron, identifying properties of chromium isotopes, and explaining mass spectrometry.
5) Calculating an empirical formula from elemental composition percentages.
The document contains a 9 question exam paper assessing knowledge of the periodic table and properties of group 1 metals, transition metals such as vanadium, and elements in period 2 such as carbon, nitrogen, fluorine and neon. Questions cover trends in physical and chemical properties, electronic configurations, oxidation states, bonding and structures.
This document contains information about atomic hydrogen energy levels and the photoelectric effect. It provides:
1) A simplified energy level diagram for atomic hydrogen showing the ground state at -13.6 eV and first excited state at -3.4 eV.
2) An explanation of how the photon model of light enabled scientists to understand why electrons are emitted instantly from metal surfaces when light above a certain frequency is used, resolving issues with the wave theory of light.
3) Information about the work function of magnesium and how the photon model explains photoemission beginning immediately when radiation is applied, unlike predictions from treating light as a wave.
1. The document discusses types of nuclear radiation (alpha, beta, gamma) and their properties. It provides examples of how radioactive sources can be used in experiments and demonstrations.
2. Safety precautions are important when using radioactive sources. Radiation can penetrate materials differently depending on its type, and sources decay over time.
3. Radiation detection equipment such as Geiger counters are used to measure radiation levels and identify isotopes. Properties like half-life can be calculated from decay data.
The document describes several experiments related to chemistry concepts:
1) An experiment to determine the empirical formula of copper(II) oxide by calculating mass changes before and after combustion.
2) Properties of elements in Period 3 of the periodic table such as electron configuration and reactivity.
3) The components and reactions occurring in a chemical cell using copper and zinc plates.
4) Characteristics and reactions of common salts like sodium carbonate and zinc nitrate.
5) The industrial process for producing ammonia through catalytic hydrogenation of nitrogen.
This document is an exam paper for the International General Certificate of Secondary Education (IGCSE) Chemistry exam. It consists of 5 questions testing knowledge of chemistry concepts and calculations. The first question covers topics related to iron production and properties of iron and steel. The second question covers essential minerals and properties of elements like boron. The third question covers alkene hydrocarbons and their reactions. The fourth question covers nitrogen dioxide and oxides of nitrogen. The final question covers properties of elements in Period 6 of the periodic table.
The document provides information about electrolysis experiments using different electrolyte solutions and electrodes. In the first experiment, a sodium sulfate solution is electrolyzed using carbon electrodes. Ions move to the electrodes and gases are produced. Hydrogen gas is collected at one electrode. In the second experiment, dilute sodium chloride solution is electrolyzed and chlorine gas is collected at one electrode.
This document contains sample questions from past science exams on various topics:
1. An experiment on the electrical conductivity of lead bromide, measuring the current through an ammeter.
2. An experiment using a concave lens to form an image.
3. An experiment culturing bacteria to study the relationship between colony growth and time.
4. An experiment comparing the elasticity of natural rubber and processed rubber.
It also provides multi-part questions testing the ability to form hypotheses, design experiments, analyze data, and apply science concepts. Questions cover topics like food processing, polymer properties, and classifying materials as conductors, insulators and thermoplastics/thermosets.
This document summarizes Ali Farzanehfar's research on mitigating anomalous spike signals observed in the CMS barrel electromagnetic calorimeter. Spikes mimic real electron and photon signals and can reduce the efficiency of the CMS trigger system if not addressed. The document investigates the distinguishing properties of spikes, current mitigation techniques, and uses a Monte Carlo simulation to evaluate potential improvements like optimizing the shaping time, digitization phase, and number of digitized samples. Tuning these parameters was found to better separate spike and electromagnetic shower pulses and improve the efficiency of spike rejection while maintaining high acceptance of real signals.
This document summarizes a master's thesis that studied irradiation-induced swelling in two ODS steels. Samples of a 15CRA-3 alloy and a PM2000 alloy were irradiated with helium ions from room temperature to 800°C to a dose of 0.84 dpa with 4000 appm helium/dpa. Surface displacements were measured using white light interferometry. Low swelling was found in both alloys, with the PM2000 showing slightly higher swelling of around 0.8%/dpa at 600°C compared to 0.3%/dpa for 15CRA-3 over the full temperature range. The higher swelling resistance of 15CRA-3 is attributed to its finer
Electricity is generated in a nuclear power station through nuclear fission. In a nuclear reactor, a chain reaction occurs where neutrons cause additional nuclear fissions, releasing energy. Moving the control rods up and down affects the number of neutrons absorbed and thus controls the energy released by the chain reaction.
This thesis examines swirling reactive flow in gas turbines and industrial burners. The author develops equations to model flame flashback using the Burgers-Rott vortex model. Experimental data on vortex velocities is used to determine unknown properties of the flow. This improves understanding of the back-pressure flame propagation mechanism and how to reduce flame instability in multi-fuel systems, supporting greener energy production.
This thesis analyzes the effect of N2 vibrational energy on flow characteristics in high-speed flight using computational fluid dynamics (CFD). The author validates relaxation models for N2 vibrational energy transfer and compares results with and without including vibrational energy effects. A key finding is that including N2 vibrational energy shows different thermal energy redistribution over a blunt body, with significant impacts on pressure and temperature profiles.
The document provides examples and problems related to chemical formulas and equations. It includes questions about relative atomic masses, empirical formulas, molecular formulas, stoichiometric calculations involving moles, masses and volumes. Specifically, it asks students to determine empirical formulas from experimental data on reactants and products, write balanced chemical equations, and perform stoichiometric calculations using molar masses and mole ratios.
This document contains 6 problems involving springs and Hooke's law. Problem 1 involves drawing a graph of extension vs. load for a spring obeying Hooke's law and calculating the initial speed of a model train stopped by a spring. Problem 2 involves calculating the kinetic energy and maximum height of an athlete bouncing on a trampoline and identifying points on a spring graph. Problem 3 involves completing a graph, calculating work done on a spring, and forces on an object suspended by a spring.
Characterization Studies of a CdTe Pixelated Timepix Detector for Applicatio...Costa Papadatos
This document summarizes a master's thesis that characterized a CdTe pixelated Timepix detector for applications in particle physics and medical physics. The thesis studied polarization effects in the detector to determine if detectors with ohmic contacts exhibit polarization. It was observed that the effective bias of the detector decreased over a 38-hour period, indicating polarization. The detector was exposed to gamma rays and its energy resolution was measured to be within 1.18% and 0.03% for the energies studied. Both per-pixel and global energy calibrations were implemented and compared when measuring proton energies between 0.8-10 MeV. The global calibration improved energy resolution by an average of 8.6% for protons. The presence of traps in Cd
This document contains information about a physics module, including:
1. A table to be filled in with SI prefixes and their symbols/values.
2. A word problem involving mass, diameter, height, acceleration, temperature increase, and heat energy.
3. Figures and questions about a milliammeter, including correcting zero error and explaining how a mirror strip increases accuracy.
4. Figures and questions about a measuring instrument, including identifying parts and measuring thickness.
5. A velocity-time graph problem involving initial velocity, acceleration, and motion characteristics.
6. Questions about measuring wire diameter using a meter rule or other suitable instrument.
7. An explanation and
The document provides an overview of atomic and nuclear physics concepts. It discusses the atomic structure of matter, including subatomic particles and the Bohr model of the atom. It also covers the chart of nuclides, mass defect and binding energy, modes of radioactive decay including alpha, beta, gamma emission and electron capture. Additionally, it summarizes key topics in radioactivity such as decay rates, half-life and equilibrium. Neutron interactions like scattering and absorption reactions are also briefly described. The goal is to introduce fundamental physics principles relevant to nuclear processes and radiation.
This document describes an experiment to determine the empirical formula of copper oxide. The combustion tube containing porcelain dish and oxide of copper is weighed before and after heating. The following data is obtained: mass of combustion tube + porcelain dish = 19.60 g, mass after adding oxide of copper = 25.68 g, mass after heating = 24.46 g. The student is asked to calculate the empirical formula of copper oxide using this data. Additional questions relate to the apparatus setup, chemical equation, and determining empirical formulas of other substances.
The document is a chemistry exam paper containing multiple questions on topics related to electricity and chemistry. It includes questions about the extraction of zinc from zinc blende, the purification of zinc by electrolysis, corrosion of steel and its prevention, the extraction of iron in the blast furnace, and catalysts in chemical reactions. The questions require students to write word and ionic equations, explain observations, complete descriptions, and suggest explanations.
AQA AS Chemistry Atomic Structure QuestionsGodschild24
This document contains sample chemistry problems and questions regarding various topics:
1) Using the ideal gas equation to calculate the volume of ethanol vapor under certain pressure and temperature conditions.
2) Balancing a chemical equation and calculating moles of a substance produced.
3) Calculating the maximum mass of a product formed from a given mass of a reactant over two reaction stages.
4) Stating the relative charge and mass of an electron, identifying properties of chromium isotopes, and explaining mass spectrometry.
5) Calculating an empirical formula from elemental composition percentages.
The document contains a 9 question exam paper assessing knowledge of the periodic table and properties of group 1 metals, transition metals such as vanadium, and elements in period 2 such as carbon, nitrogen, fluorine and neon. Questions cover trends in physical and chemical properties, electronic configurations, oxidation states, bonding and structures.
This document contains information about atomic hydrogen energy levels and the photoelectric effect. It provides:
1) A simplified energy level diagram for atomic hydrogen showing the ground state at -13.6 eV and first excited state at -3.4 eV.
2) An explanation of how the photon model of light enabled scientists to understand why electrons are emitted instantly from metal surfaces when light above a certain frequency is used, resolving issues with the wave theory of light.
3) Information about the work function of magnesium and how the photon model explains photoemission beginning immediately when radiation is applied, unlike predictions from treating light as a wave.
1. The document discusses types of nuclear radiation (alpha, beta, gamma) and their properties. It provides examples of how radioactive sources can be used in experiments and demonstrations.
2. Safety precautions are important when using radioactive sources. Radiation can penetrate materials differently depending on its type, and sources decay over time.
3. Radiation detection equipment such as Geiger counters are used to measure radiation levels and identify isotopes. Properties like half-life can be calculated from decay data.
The document describes several experiments related to chemistry concepts:
1) An experiment to determine the empirical formula of copper(II) oxide by calculating mass changes before and after combustion.
2) Properties of elements in Period 3 of the periodic table such as electron configuration and reactivity.
3) The components and reactions occurring in a chemical cell using copper and zinc plates.
4) Characteristics and reactions of common salts like sodium carbonate and zinc nitrate.
5) The industrial process for producing ammonia through catalytic hydrogenation of nitrogen.
This document is an exam paper for the International General Certificate of Secondary Education (IGCSE) Chemistry exam. It consists of 5 questions testing knowledge of chemistry concepts and calculations. The first question covers topics related to iron production and properties of iron and steel. The second question covers essential minerals and properties of elements like boron. The third question covers alkene hydrocarbons and their reactions. The fourth question covers nitrogen dioxide and oxides of nitrogen. The final question covers properties of elements in Period 6 of the periodic table.
The document provides information about electrolysis experiments using different electrolyte solutions and electrodes. In the first experiment, a sodium sulfate solution is electrolyzed using carbon electrodes. Ions move to the electrodes and gases are produced. Hydrogen gas is collected at one electrode. In the second experiment, dilute sodium chloride solution is electrolyzed and chlorine gas is collected at one electrode.
This document contains sample questions from past science exams on various topics:
1. An experiment on the electrical conductivity of lead bromide, measuring the current through an ammeter.
2. An experiment using a concave lens to form an image.
3. An experiment culturing bacteria to study the relationship between colony growth and time.
4. An experiment comparing the elasticity of natural rubber and processed rubber.
It also provides multi-part questions testing the ability to form hypotheses, design experiments, analyze data, and apply science concepts. Questions cover topics like food processing, polymer properties, and classifying materials as conductors, insulators and thermoplastics/thermosets.
This document summarizes Ali Farzanehfar's research on mitigating anomalous spike signals observed in the CMS barrel electromagnetic calorimeter. Spikes mimic real electron and photon signals and can reduce the efficiency of the CMS trigger system if not addressed. The document investigates the distinguishing properties of spikes, current mitigation techniques, and uses a Monte Carlo simulation to evaluate potential improvements like optimizing the shaping time, digitization phase, and number of digitized samples. Tuning these parameters was found to better separate spike and electromagnetic shower pulses and improve the efficiency of spike rejection while maintaining high acceptance of real signals.
This document summarizes a master's thesis that studied irradiation-induced swelling in two ODS steels. Samples of a 15CRA-3 alloy and a PM2000 alloy were irradiated with helium ions from room temperature to 800°C to a dose of 0.84 dpa with 4000 appm helium/dpa. Surface displacements were measured using white light interferometry. Low swelling was found in both alloys, with the PM2000 showing slightly higher swelling of around 0.8%/dpa at 600°C compared to 0.3%/dpa for 15CRA-3 over the full temperature range. The higher swelling resistance of 15CRA-3 is attributed to its finer
Electricity is generated in a nuclear power station through nuclear fission. In a nuclear reactor, a chain reaction occurs where neutrons cause additional nuclear fissions, releasing energy. Moving the control rods up and down affects the number of neutrons absorbed and thus controls the energy released by the chain reaction.
This thesis examines swirling reactive flow in gas turbines and industrial burners. The author develops equations to model flame flashback using the Burgers-Rott vortex model. Experimental data on vortex velocities is used to determine unknown properties of the flow. This improves understanding of the back-pressure flame propagation mechanism and how to reduce flame instability in multi-fuel systems, supporting greener energy production.
This thesis analyzes the effect of N2 vibrational energy on flow characteristics in high-speed flight using computational fluid dynamics (CFD). The author validates relaxation models for N2 vibrational energy transfer and compares results with and without including vibrational energy effects. A key finding is that including N2 vibrational energy shows different thermal energy redistribution over a blunt body, with significant impacts on pressure and temperature profiles.
The document provides examples and problems related to chemical formulas and equations. It includes questions about relative atomic masses, empirical formulas, molecular formulas, stoichiometric calculations involving moles, masses and volumes. Specifically, it asks students to determine empirical formulas from experimental data on reactants and products, write balanced chemical equations, and perform stoichiometric calculations using molar masses and mole ratios.
This document contains 6 problems involving springs and Hooke's law. Problem 1 involves drawing a graph of extension vs. load for a spring obeying Hooke's law and calculating the initial speed of a model train stopped by a spring. Problem 2 involves calculating the kinetic energy and maximum height of an athlete bouncing on a trampoline and identifying points on a spring graph. Problem 3 involves completing a graph, calculating work done on a spring, and forces on an object suspended by a spring.
Characterization Studies of a CdTe Pixelated Timepix Detector for Applicatio...Costa Papadatos
This document summarizes a master's thesis that characterized a CdTe pixelated Timepix detector for applications in particle physics and medical physics. The thesis studied polarization effects in the detector to determine if detectors with ohmic contacts exhibit polarization. It was observed that the effective bias of the detector decreased over a 38-hour period, indicating polarization. The detector was exposed to gamma rays and its energy resolution was measured to be within 1.18% and 0.03% for the energies studied. Both per-pixel and global energy calibrations were implemented and compared when measuring proton energies between 0.8-10 MeV. The global calibration improved energy resolution by an average of 8.6% for protons. The presence of traps in Cd
This document contains information about a physics module, including:
1. A table to be filled in with SI prefixes and their symbols/values.
2. A word problem involving mass, diameter, height, acceleration, temperature increase, and heat energy.
3. Figures and questions about a milliammeter, including correcting zero error and explaining how a mirror strip increases accuracy.
4. Figures and questions about a measuring instrument, including identifying parts and measuring thickness.
5. A velocity-time graph problem involving initial velocity, acceleration, and motion characteristics.
6. Questions about measuring wire diameter using a meter rule or other suitable instrument.
7. An explanation and
The document provides an overview of atomic and nuclear physics concepts. It discusses the atomic structure of matter, including subatomic particles and the Bohr model of the atom. It also covers the chart of nuclides, mass defect and binding energy, modes of radioactive decay including alpha, beta, gamma emission and electron capture. Additionally, it summarizes key topics in radioactivity such as decay rates, half-life and equilibrium. Neutron interactions like scattering and absorption reactions are also briefly described. The goal is to introduce fundamental physics principles relevant to nuclear processes and radiation.
1. NT Exampro 1
1. (a) Complete the following table.
Atom Number of
protons
Number of
neutrons
Number of
electrons
Ir
Mo
191
77
96
42
(2)
(b) The element gallium consists of two types of atom of relative mass 69.0 and 71.0
respectively. The percentage abundance of the atoms of relative mass 69.0 is 60.2.
(i) Calculate the relative atomic mass of gallium.
(ii) What name is given to these different atoms of gallium?
..........................................................................................................................
(2)
(c) Define the term second ionisation energy. Write an equation, using the element
potassium, to show this change.
....................................................................................................................................
....................................................................................................................................
....................................................................................................................................
....................................................................................................................................
(3)
(d) The first seven ionisation energies (kJ mol–1) for two elements A and B in the same Period
of the Periodic Table are:
Element
A
B
1
1012
578
2
1903
1817
3
2912
2745
4
4957
11578
5
6274
14831
6
21269
18378
7
25398
23296
(i) Explain the relative magnitude of the first and second ionisation energies of
element B.
..........................................................................................................................
..........................................................................................................................
..........................................................................................................................
www.chemactive.com
2. NT Exampro 2
(ii) Explain the relative magnitude of the first ionisation energy for elements A and B.
..........................................................................................................................
..........................................................................................................................
..........................................................................................................................
(4)
(Total 11 marks)
2. Complete the following table.
Atom Number of
protons
Number of
neutrons
Number of
electrons
Ir
Mo
191
77
96
42
(2)
3. The element gallium consists of two types of atom of relative mass 69.0 and 71.0 respectively.
The percentage abundance of the atoms of relative mass 69.0 is 60.2.
(i) Calculate the relative atomic mass of gallium.
(ii) What name is given to these different atoms of gallium?
................………….....................................................................................................
(2)
4. Define the term isotope.
....................................................................................................................................
(1)
5. From the position of radium in the Periodic Table, predict the following:
(a) the formula of radium carbonate;
…….......................……….........................................................................................
www.chemactive.com
3. NT Exampro 3
(b) the equation for the thermal decomposition of solid radium carbonate;
…….......................……….........................................................................................
(c) how the decomposition temperature required in (d)(ii) would compare with that required
for magnesium carbonate.
…….......................……….........................................................................................
(Total 4 marks)
6. (a) Define the terms
(i) atomic number;
..........................................................................................................................
(1)
(ii) mass number;
..........................................................................................................................
(1)
(iii) relative atomic mass.
..........................................................................................................................
..........................................................................................................................
(1)
(b) In 1919 F. W. Aston, using an early form of the mass spectrometer, showed that neon
exists as a mixture of isotopes.
The mass spectrum is shown below; determine the relative atomic mass of neon.
100
80
60
40
20
18 20 22 24
relative
abundance
m/e
....................................................................................................................................
....................................................................................................................................
(2)
(c) (i) Define the second ionisation energy of fluorine.
www.chemactive.com
4. NT Exampro 4
..........................................................................................................................
..........................................................................................................................
(2)
(ii) Sketch a graph on the axes below to show the successive ionisation energies of
fluorine. Give reasons for the shape of the line you draw.
log
ionisation
energy
number of ionisation
..........................................................................................................................
..........................................................................................................................
..........................................................................................................................
(4)
(Total 11 marks)
7. Define the terms
(a) atomic number;
...........………..............................................................................................................
(1)
(b) mass number;
...........………..............................................................................................................
(1)
(c) relative atomic mass.
...........………..............................................................................................................
...........………..............................................................................................................
(1)
(Total 3 marks)
8. (i) Give the electronic configuration of an atom of the isotope of calcium, 20
45
Ca.
……..………...................………...............................................................................
www.chemactive.com
5. NT Exampro 5
(1)
(ii) Give the names and numbers of each type of particle present in a nucleus of this isotope.
……..………...................………...............................................................................
……..………...................………...............................................................................
(2)
(iii) State one reason why the information in (i) is usually more useful to chemists than
that in (ii).
……..………...................………...............................................................................
……..………...................………...............................................................................
(1)
(Total 4 marks)
9. The species X, Y and Z are atoms or ions.
species X Y Z
atomic number 16 16 16
mass number 32 35 32
net charge 0 0 –2
(a) (i) State the number of electrons, protons and neutrons X
electrons .......................... protons ......................... neutrons .......................
(1)
(ii) What is the relationship between X and Y?
……………………………………………………………………………..…
(1)
(iii) Identify Z
……………………………………………………………………………..…
(1)
(b) 332 kJ of energy are required to convert a mole of gaseous atoms of X to a mole of
gaseous Z
(i) Represent by equations the two steps which make up this energy change.
……………………………………………………………………………..…
……………………………………………………………………………..…
(2)
(ii) Explain why the second step is endothermic
……………………………………………………………………………..…
……………………………………………………………………………..…
(1)
www.chemactive.com
6. NT Exampro 6
(c) Y is radioactive, decaying by beta (β) emission.
When a sample of the product form the β decay of Y was passed into a mass spectrometer
it produced only one peak, at m/e = 35 whereas a naturally occurring sample of this
element gave an extra peak at m/e = 37.
Account for this difference between the sample of the element made from Y and the
naturally occurring sample of the same element.
.....................................................................................................................................
.....................................................................................................................................
.....................................................................................................................................
(2)
(Total 8 marks)
10. (a) (i) Define the terms:
atomic number ...............................................................................................
......................................................................................................................
mass number .................................................................................................
......................................................................................................................
(2)
(ii) Identify the particle which contains 11 protons, 12 neutrons and 10 electrons.
......................................................................................................................
(1)
www.chemactive.com
7. NT Exampro 7
(b) Bromine consists of two isotopes, mass numbers 79 and 81. A sample of bromine gas,
Br2, was examined in a mass spectrometer. The mass spectrum showing the molecular
ions is given below.
100
50
Relative
intensity
158 160 162
m/e
(i) Identify the species responsible for the peak at m/e = 160.
......................................................................................................................
(1)
(ii) Deduce the relative abundances of the two isotopes,
(2)
(c) Define the term first electron affinity for bromine atoms, illustrating your answer with an
equation.
................................................................................................................................
................................................................................................................................
................................................................................................................................
................................................................................................................................
(3)
www.chemactive.com
8. NT Exampro 8
(d) The graph showing the variation of the first ionisation energies of the elements neon to
potassium is given below.
2500
2000
1500
1000
500
0
First
ionisation
energy/kJ mol–1
Ne Na Mg Al Si P S Cl Ar K
(i) Define the term first ionisation energy with reference to neon.
......................................................................................................................
......................................................................................................................
......................................................................................................................
(2)
(ii) Explain the general trend in the first ionisation energies of the elements sodium to
argon.
......................................................................................................................
......................................................................................................................
......................................................................................................................
(2)
(iii) Explain why the first ionisation energy of neon is greater than the first ionisation
energy of argon.
......................................................................................................................
......................................................................................................................
......................................................................................................................
(2)
(Total 15 marks)
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9. NT Exampro 9
11. (a) Iron has several isotopes. One of them has the electronic configuration [Ar]3d64s2 , an
atomic number of 26 and a mass number of 56.
(i) Which of these pieces of information would be the most use in helping a chemist
decide on the likely chemical reactions of iron?
............................................................................................................................
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(1)
(ii) State how many of each of the following particles is found in an atom of 56Fe.
Protons ................ electrons ................ neutrons ................
(2)
(iii) What are isotopes?
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(2)
(b) The relative atomic mass of a sample of iron may be found by using a mass spectrometer
to determine the isotopic composition.
(i) The diagram below represents a low-resolution mass spectrometer in which four
areas have been identified. State what happens in each of these areas.
(+)
Sample
B
CA
D
To vacuum pump
Area A ..............................................................................................................
Area B ..............................................................................................................
Area C ..............................................................................................................
Area D ..............................................................................................................
(4)
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10. NT Exampro 10
(ii) In such a determination the following isotopic composition was found.
Isotope Percentage composition
54Fe 5.8
56Fe 91.6
57Fe 2.2
58Fe 0.33
Calculate the relative atomic mass of this sample of iron, giving your answer to two
decimal places.
(2)
(Total 11 marks)
12. (a) (i) Complete the electronic configuration of a sulphur atom.
1s2...................................................................................................................
(1)
(ii) Deduce the number of neutrons in the nucleus of an atom of 32S.
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(1)
(b) (i) Define the term first electron affinity.
......................................................................................................................
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(3)
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11. NT Exampro 11
(ii) The following equation represents the change occurring when the second electron
affinity of sulphur is measured.
S–(g) +e–→ S2– (g)
Explain why the second electron affinity of an element is endothermic.
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(2)
(Total 7 marks)
13. (a) (i) What is meant by the mass number of an atom?
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(1)
(ii) Define the term relative atomic mass.
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(2)
(iii) What are isotopes?
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(2)
(b) Magnesium has three isotopes. The mass spectrum of magnesium shows peaks at m/e 24
(78.60%), 25 (10.11%), and 26 (11.29%). Calculate the relative atomic mass of
magnesium to 4 significant figures.
(2)
(Total 7 marks)
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12. NT Exampro 12
14. (a) Complete the following table:
Particle Relative charge Relative mass
Proton 1
Electron –1
Neutron 1
(3)
(b) State the number of each of the above particles present in one molecule of CH4, showing
clearly how you arrive at your answer.
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(3)
(c) Complete the electronic configuration of a chlorine atom.
1s2 ............................................................................................................................
(1)
(d) Give the formula of the chlorine species composed of 17 protons, 20 neutrons and 16
electrons.
....................................................................................................................................
(2)
(e) Write one equation in each case to represent the change occurring when the following
quantities are measured.
(i) The first electron affinity of sulphur.
............................................................................................................................
(2)
(ii) The first ionisation energy of sulphur.
........................................................................................................................
(1)
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13. NT Exampro 13
(f) Explain why the first ionisation energy of chlorine is higher than that of sulphur.
....................................................................................................................................
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....................................................................................................................................
....................................................................................................................................
(2)
(Total 14 marks)
15. (a) (i) Write the equation for the reaction of lithium with water.
………………………………………………………………………………..
(2)
(ii) Describe what you would expect to see during the reaction.
………………………………………………………………………………..
………………………………………………………………………………..
(2)
(b) State the number of protons, neutrons and electrons in a +Li
3
7
ion.
protons: ……………… neutrons: ……………… electrons: ………………
(3)
(c) The mass spectrum of lithium shows two peaks. Their mass/charge ratios and
percentage abundance are shown below.
Mass/charge % Abundance
6.02 7.39
7.02 92.61
Calculate the relative atomic mass of lithium, giving your answer to three
significant figures.
(2)
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14. NT Exampro 14
(d) Describe a test that you would do to distinguish between solid lithium chloride and
solid sodium chloride. Clearly state what you would do and what you would see with both
substances.
………….…………………………………………………………………………….
………….…………………………………………………………………………….
………….…………………………………………………………………………….
………….…………………………………………………………………………….
(3)
(Total 12 marks)
16. (a) State the meaning of the terms
(i) relative atomic mass
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(2)
(ii) mass number
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(1)
(iii) isotopes
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(2)
(b) The isotopic composition of a sample of sulphur is found using a mass spectrometer.
(i) Explain how atoms of the sample of sulphur are ionised.
..........................................................................................................................
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..........................................................................................................................
(2)
(ii) State the type of charge on the sulphur ions formed in the mass spectrometer.
..........................................................................................................................
(1)
(iii) State how the resulting sulphur ions are then accelerated.
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15. NT Exampro 15
..........................................................................................................................
(1)
(c) For a particular sample of sulphur atoms the following isotopic composition was recorded.
Isotope Percentage composition
32S 95.00
33S 0.76
34S 4.24
Calculate the relative atomic mass of this sample of sulphur. Give your answer to two
decimal places.
(2)
(d) Predict the electronic configuration of a 34S atom, using s, p and d notation.
1s2 .........................................................................................................................
(1)
(Total 12 marks)
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