Ark Elvin Academy Year 10 Science Study Pack Spring assessment 2018 Cumulative content part 1 Name
Biology Cell Biology: structure and transport Part 1: Glossary 1. active transport the movement of substances from a dilute solution to a more concentrated solution against a concentration gradient, requiring energy from respiration 2. algae simple aquatic organisms (protista) that make their own food by photosynthesis 3. alveoli tiny air sacs in the lungs that increase the surface area for gaseous exchange 4. bacteria single-celled prokaryotic organisms 5. cell membrane the membrane around the contents of a cell that controls what moves in and out of the cell 6. cell wall the rigid structure around plant and algal cells. It is made of cellulose and strengthens the cell 7. cellulose the complex carbohydrate that makes up plant and algal cell walls and gives them strength 8. chlorophyll the green pigment contained in the chloroplasts 9. chloroplasts the organelles in which photosynthesis takes place 10. cytoplasm the water-based gel in which the organelles of all living cells are suspended and most of the chemical reactions of life take place 11. diffusion the spreading out of the particles of any substance in a solution, or particles in a gas, resulting in a net movement of particles from an area of higher concentration to an area of lower concentration down a concentration gradient 12. eukaryotic cells from eukaryotes that have a cell membrane, cytoplasm, and genetic cells material enclosed in a nucleus 13. hypertonic a solution that is more concentrated than the cell contents (osmosis) 14. hypotonic a solution that is less concentrated than the cell contents (osmosis) 15. isotonic a solution that is the same concentration as the cell contents (osmosis) 16. mitochondria the site of aerobic cellular respiration in a cell 17. nucleus organelle found in many living cells containing the genetic information surrounded by the nuclear membrane 18. osmosis the diffusion of water through a partially permeable membrane from a dilute solution (which has a high concentration of water) to a concentrated solution (with a low concentration of water ) down a concentration gradient 19. partially a membrane that allows only certain substances to pass through permeable membrane 20. permanent space in the cytoplasm filled with cell sap vacuole 21. phloem the living transport tissue in plants that carries dissolved food (sugars) around the plant
22. plasmolysis the state of plant cells when so much water is lost from the cell by osmosis that the vacuole and cytoplasm shrink and the cell membrane pulls away from the cell wall 23. prokaryotic cells from prokaryotic organisms have a cytoplasm surrounded by a cell membrane, and a cell wall that does not contain cellulose. The genetic material is a DNA loop that is free in the cytoplasm and not enclosed by a nucleus. Sometimes there are one or more small rings of DNA called plasmids 24. resolving power 25. ribosomes the site of protein synthesis in a cell a measure of the ability to distinguish between two separate points that are very close together 26. sperm the male sex cells or gametes that carry the genetic material from the male parent 27. stomata openings in the leaves of plants, particularly on the underside and opened and closed by guard cells, allowing gases to enter and leave the leaf 28. turgor the pressure inside a plant cell exerted by the cell contents pressing on the cell wall 29. ventilated movement of air or water into and out of the gas exchange organ, for example lungs or gills 30. xylem the non-living transport tissue in plants that transports water from the roots to the leaves and shoots Part 2: Key knowledge 1. Animal and plant cells Key information: Most animal cells have the following parts: a nucleus, cytoplasm, a cell membrane, mitochondria to carry out aerobic respiration which releases energy for the cell, ribosomes to carry out protein synthesis by joining many amino acids. In addition to the parts found in animal cells, plant cells often have: chloroplasts filled with chlorophyll to absorb light for photosynthesis a permanent vacuole filled with cell sap to provide support to the cell Plant and algal cells also have a cell wall made of cellulose, which strengthens the cell. Figure 1: structure of an animal cell Figure 2: structure of plant cell
2. Eukaryotes and prokaryotes Key information: Plant and animal cells (eukaryotic cells) have: genetic material enclosed in a nucleus to control the activity of the cell a cell membrane to control what enters and exits the cell cytoplasm to allow reactions to take place Bacterial cells (prokaryotic cells) are much smaller in comparison. The genetic material is not enclosed in a nucleus. It is a single DNA loop and there may be one or more small rings of DNA called plasmids. They also have cytoplasm, a cell membrane and a cell wall to provide strength and support to the cell. 3. Cell differentiation and specialised cells Key information: Figure 3: structure of a prokaryote cell Cells may be specialised to carry out a particular function: sperm cells, nerve cells and muscle cells in animals root hair cells, xylem and phloem cells in plants. As an organism develops, cells differentiate to form different types of cells. Most types of animal cell differentiate at an early stage. Many types of plant cells can differentiate throughout life. In mature animals, cell division is mainly restricted to repair and replacement. As a cell differentiates it gets different sub-cellular structures so it can carry out a certain function. It has become a specialised cell.
Figure 4: summary of the structure and function of specialised cells
4. Microscopes Key information: A light microscope shines a beam of light across a thin, dead, stained specimen. The resolution (ability to distinguish between two points) and magnification of a light microscope is high enough the view the nucleus and cell membrane. Most organelles are too small to be viewed with a light microscope. Figure 5: image of a microscope Figure 6: equation triangle to calculate magnification 1. Magnification = image size / size of real object 2. Image size = magnification x size of real object 3. Size of real object = image size / magnification
5. Diffusion Key information: Diffusion is the spreading out of the particles of any substance in solution, or particles of a gas, resulting in a net movement from an area of higher concentration to an area of lower concentration. Figure 7: explanation of diffusion in terms of particles 6. Osmosis and investigating osmosis Key information: 1. Water may move across cell membranes via osmosis. 2. Osmosis is the diffusion of water from a dilute solution to a concentrated solution through a partially permeable membrane. Plant tissue can be used to measure the rate of uptake of water in different solutions. During these experiments, only the water moves. Salt and sugar molecules are too large to pass across the partially permeable membranes. The higher the concentration of salt or sugar, the lower the concentration of water.
Figure 8: a model of osmosis in hypertonic and hypotonic solutions Figure 9: osmosis in plant cells 7. Active transport Key information: Active transport moves substances from a more dilute solution to a more concentrated solution (against a concentration gradient). This requires energy from respiration. Active transport allows mineral ions to be absorbed into plant root hairs from very dilute solutions in the soil. Plants require ions for healthy growth. It also allows sugar molecules to be absorbed from lower concentrations in the gut into the blood which has a higher sugar concentration. Sugar molecules are used for cell respiration. Figure 10: the uptake of mineral ions in roots via active transport
Part 3: Key questions 1. Animal and plant cells a. Label the cells: b. Fill in the table with the functions of each organelle. Organelle Nucleus Cytoplasm Cell membrane Mitochondria Ribosomes Chloroplasts Vacuole Cell wall Function c. Identify three organelles found in plant cells but not animal cells. 2. Eukaryotes and prokaryotes a. What type of cells are eukaryotic cells b. What type of cells are prokaryotic cells? c. Outline 3 differences between prokaryotes and eukaryotes. 3. Cell differentiation and specialised cells a. Describe how the structure of a sperm cell relates to its function. b. Describe how the structure of a root hair cell relates to its function. c. what is meant by the term differentiation. d. Describe why cell division is important for animals. e. Explain how the xylem is specialised to carry out its function. f. State the name of the tissue in plants which allows plant cells to differentiate throughout life. 4. Microscopes a. The image shows human cheek cells. In the space below, draw a biological drawing of this image. Label the organelles which are visible. b. Describe how the slide of cheek cells would have been prepared. c. State what is meant by the term resolution. d. Give the equation that links magnification, image size and actual size. 5. Diffusion
a. Define the term diffusion. b. Give two examples of molecules which diffuse in and out of cells. Name the process these molecules are involved in. c. State three factors that affect the rate of diffusion. d. Describe the relationship between surface area: volume ratio and the rate of diffusion. e. Complete the table to show how the following are adapted for exchanging materials. Organ Lungs How it is adapted for exchange Small intestine Gills Leaves Roots 6. Osmosis and investigating osmosis a. Define the term osmosis b. Why is salt water an example of a hypertonic solution? c. In what type of solution would water movement be equal? d. Outline the similarities and differences between osmosis and diffusion e. Describe why the water moves from the left to the right side. f. Explain why the sugar molecules do not move. 7. Active transport a. Outline the main differences between diffusion and active transport. b. Explain, using examples, the importance of active transport for plant growth. c. Explain why active transport cannot occur in the absence of oxygen. d. Describe when active transport is used by the cells lining the small intestine.
Chemistry Atomic structure Part 1: Glossary 1. aqueous solution the mixture made by adding a soluble substance to water 2. atom the smallest part of an element that can still be recognised as that element 3. atomic number the number of protons (which equals the number of electrons) in an atom. It is sometimes called the proton number a symbol equation in which there are equal numbers of each type of atom on either side of the equation 4. balanced symbol equation 5. chromatography the process whereby small amounts of dissolved substances are separated by running a solvent along a material such as absorbent paper 6. compound a substance made when two or more elements are chemically bonded together 7. electron a tiny particle with a negative charge. Electrons orbit the nucleus of atoms or ions in shells 8. electronic structure a set of numbers to show the arrangement of electrons in their shells (or energy levels) 9. element a substance made up of only one type of atom. An element cannot be broken down chemically into any simpler substance 10. group all the elements in the columns (labelled 1 to 7 and 0) in the periodic table 11. ion a charged particle produced by the loss or gain of electrons 12. isotope atoms that have the same number of protons but different number of neutrons, i.e., they have the same atomic number but different mass numbers 13. law of conservation 14. of mass. the total mass of the products formed in a reaction is equal to the total mass of the reactants 15. mass number the number of protons plus neutrons in the nucleus of an atom 16. neutron a dense particle found in the nucleus of an atom. It is electrically neutral, carrying no charge 17. noble gases the very unreactive gases found in Group 0 of the periodic table. Their atoms have very stable electronic structures 18. nucleus (of an atom) the very small and dense central part of an atom that contains protons and neutrons 19. periodic table an arrangement of elements in the order of their atomic numbers, forming groups and periods 20. product a substance made as a result of a chemical reaction 21. proton a tiny positive particle found inside the nucleus of an atom
22. reactant a substance we start with before a chemical reaction takes place 23. shell an area in an atom, around its nucleus, where electrons are found 24. state symbol. the abbreviations used in balanced symbol equations to show if reactants and products are solid (s), liquid (l), gas (g) or dissolved in water (aq) 25. symbol equation an equation that helps you see how much of each substance is involved in a chemical reaction by showing the chemical symbols and formulae of all the reactants and products involved. 26. word equation a way of describing what happens in a chemical reaction by showing the names of all reactants and the products they form Part 2: Key knowledge 1. Elements, compounds and chemical formulae All substances are made up of atoms. Atoms can be joined together by chemical bonds. If atoms of the same type are joined together, the substance is called an element. The periodic table lists all the chemical elements, with eight main groups each containing elements with similar chemical properties. If different types are joined together, the substance is called a compound. The names of the elements can be found on the periodic table. Compounds are not found on the periodic table. The chemical formulae of a molecular substance tells you which atoms, and how many of them, are present. 2. Chemical equations Chemical equations show the reactants (the substances your start with) and the products (the substances made) in a reaction. Word and symbol equations can be used to represent chemical reactions. Symbol equations help you see ow much of each substance is involved in a reaction. The law of conservation of mass states: no new atoms are ever created or destroyed in a chemical reaction (the total mass of reactants = the total mass of products) State symbols can be included in chemical equations to tell you more information: (s) solids (l) liquids (aq) aqueous solutions (g) gases
3. Separating mixtures A mixture is made up of two or more substances that are not chemically combined. Mixtures can be separated by physical techniques: filtration, crystallisation and simple distillation. a. Filtration This technique is used to separate substances that are insoluble in a particular solvent from those that are soluble in the solvent. E.g. sand and water b. Crystallisation This technique is used to crystallise a salt which is soluble in a solution (the filtrate) c. Distillation This technique is used to collect a liquid from a mixture through evaporation and condensation. 4. Fractional distillation A technique to separate miscible liquids based on the boiling points of liquids in the mixture This technique is used to separate ethanol from a fermented mixture in the alcoholic spirits industry. Ethanol and water can be separated by this technique as they have different boiling points (ethanol 78 C) 5. Paper chromatography A technique to separate mixtures dissolved in a solvent e.g. ink Separation occurs in this process due to the difference in solubilities of the different substances within the solvent.
6. History of the atom The ideas about atoms have changed overtime New evidence has been gathered from experiments of scientists who have used their model of the atom to explain their observations and calculations Key individuals who proposed ideas about the atoms were Dalton, Thompson, Rutherford and Bohr. Dalton s model Plum pudding model (Thompson) Nuclear model (Rutherford) Electron shell model (Bohr) Protons and neutrons History of the Atom Summary Atoms are tiny spheres that cannot be broken down. The atom is a ball of spread out positive charge with negative electrons studded into it An atom has a nucleus with a positive charge. Electrons orbit the nucleus. Between the nucleus and the electrons is empty space. Electrons orbit the nucleus at a fixed energy level The nucleus consists of protons which have a positive charge and neutrons which have no charge 7. Structure of the atom Atoms are made of three subatomic particles: protons, neutrons and electrons. Protons have a relative charge of +1 and electrons have a relative charge of -1. Neutrons have no electric charge, they are neutral. Relative masses of a proton and neutron are both 1. Subatomic particle Relative mass Relative charge Proton 1 +1 Neutron 1 0 Electron 0-1 On the periodic table, each element has two numbers: Atomic number: the small number This tells you the total number of protons in an atom It also tells you the number of electrons. This is because an atom must have the same number of positive charges and negative charges so it does not have an overall charge the protons and electrons cancel each other out. Mass number: the big number This tells you the total number of protons +neutrons in an atom To work out number of neutrons: mass number atomic number
8. Ions, atoms and isotopes Ions An ion is a charged particle produced by the loss or gain of electrons Atoms that gain electrons form negative ions Atoms that lost electrons form positive ions. Isotopes Atoms which have different atomic numbers are atoms of different elements. Atoms with the same atomic number but a different mass number are isotopes of the same element. Isotopes have identical chemical properties, but their physical properties, such as density, can differ. Chlorine on the periodic table has a mass number of 35.5. With a mass number of 35.5 and its atomic number is 17. How many neutrons does it have? Number of neutrons = mass number atomic number Number of neutrons = 35.5-17 = 18.5 This cannot be correct as you cannot have half a neutron. Instead, it represents the average mass of all the atoms of chlorine in the universe. Scientists have discovered that 75% of the atoms of chlorine in the universe have a mass of 35 (so 18 neutrons) 25% have a mass of 37 (so 20 neutrons) The percentage is called the abundance When we work out the mean mass we call it the relative atomic mass (abundance of isotope 1 mass of isotope 1) + (abundance of isotope 2 mass of isotope 2) 100 So for chlorine: Relative atomic mass = (75 35)+(25 37) 100 = 35.5 Worked example copper: Copper has two isotopes. 69% is Cu-63 and 31% is Cu-65. What is the relative atomic mass? We know that the equation for relative atomic mass is: (abundance of isotope 1 mass of isotope 1) + (abundance of isotope 2 mass of isotope 2) 100 Here, isotope 1 has an abundance of 69 and a mass of 63. Isotope 2 has an abundance of 31 and a mass of 65. (69 63) + (31 65) = 63.62 100
9. Electronic structure The number of electrons is the same as the atomic number of an atom Electrons orbit atoms in fixed energy levels (often called shells). Two electrons can fit on the first shell. 8 electrons can fit on the next shells. The first shell needs to be filled before the second and the second before the third. The number of electrons in the outermost shell of an element s atoms determine the way in which that element reacts. Part 3: Key questions Elements, compounds and chemical formulae a. What is the smallest part of an element that can exist? b. Define the term compound and give an example. c. Complete the table below: Name Formulae Element or compound? Oxygen Sodium sulfate CaCl 2 Number of atoms? Number of elements? Chemical equations a. Define the term conservation of mass b. What do state symbols tell you c. Balance the equations below: H 2 + O 2 H 2O CH 4 + O 2 CO 2 + H 2O Na + Cl 2 NaCl Fe + O 2 Fe 2O 3 Al + Br 2 AlBr 3 CaO + H 2O Ca(OH) 2
Separating mixtures a. When mixtures are separated is this a physical or chemical process? b. Complete the table below: Substances to Name of separating Description of how the technique works. be separated technique Sand and water Salt and water Water and ethanol Mixture of food colourings c. What is wrong with the setup of the equipment below to separate the solid yeast from the solution? d. Which property of substances in a mixture allows distillation to work? e. How many colours make up brown? How do you know? Which colour is the most soluble? The development of the Model of the Atom a. Which model describes the atom as s a ball of positive charge with negative electrons embedded in it? b. Name the experiment which led scientists to believe the mass of an atom was mostly in the centre. c. What evidence led them to believe there was a positive nucleus? d. What was the name of the model resulting from the experiment above? e. How did Niels Bohr improve the nuclear model? f. Which scientist provided evidence to show the nucleus contained neutrons as well as protons?
Structure of the atom a. Complete the table to show the names of the 3 sub-atomic particles and their relative charges and masses. Sub-Atomic Particle Relative Mass Relative Charge 1 electron +1 b. In terms of sub-atomic particles, define the following terms: atomic number mass number c. Where is the majority of mass found in an atom? d. What is the approximate radius, in standard form, of: an atom? the nucleus of an atom? Ions, atoms and isotopes a. Define the term ion b. Do metals form positive or negative ions? Why? c. Do non-metals form positive or negative ions? Why? d. Complete the table to show the ion formed from each atom? Atom Lithium Number of electrons in outer shell Ion 1 Li + Cl - Aluminium Hydrogen Bromine Calcium Oxygen Barium e. Define the term isotope and give an example. f. Define the term relative atomic mass. g. Explain why the relative atomic mass of chlorine is not a whole number. h. Explain the difference between the two isotopes of carbon below in terms of their sub atomic particles.
i. Calculate the relative atomic mass of the following elements Element Isotopes Percentage Abudance Lithium 6 7.6% 3 7 3 Li Li 92.4% Magnesium 24 79% 12 25 12 26 12 Mg Mg Mg 10% 11% Copper 63 70% 29 65 29 Cu Cu 30% Relative atomic mass Electronic structure a. How many electrons can occupy the first energy level? b. How many electrons can occupy the second energy level? c. Name the element that has its electron configuration shown below. d. On the diagram above, label the lowest and highest energy levels (shells). Which shell is filled first? e. How many electrons does an element in group 2 have in its highest occupied shell?
Chemistry Quantitative chemistry Part 1: Glossary 1. relative atomic mass Ar the average mass of the atoms of an element compared with carbon-12 (which is given a mass of exactly 12). The average mass must take into account the proportions of the naturally occurring isotopes of the element 2. relative formula mass Mr the total of the relative atomic masses, added up in the ratio shown in the chemical formula, of a substance Part 2: Key knowledge 1. Chemical equations Chemical equations show the reactants (the substances your start with) and the products (the substances made) in a reaction. Word and symbol equations can be used to represent chemical reactions. Symbol equations help you see ow much of each substance is involved in a reaction. The law of conservation of mass states: no new atoms are ever created or destroyed in a chemical reaction (the total mass of reactants = the total mass of products) State symbols can be included in chemical equations to tell you more information: (s) solids (l) liquids (aq) aqueous solutions (g) gases 2. Change in masses In a chemical reaction the amount of products might appear to increase or decrease when gases are involved. Mass of products appears to increase compared to the mass of reactants when a reactant is a gas Mass of products appears to decrease compared to the mass of reactants when a product is a gas as gas from the reaction mixture of products might escape to the surrounding.
3. Calculating Mr The Mr is the total of the relative atomic masses, added up in the ratio shown in the chemical formula, of a substance. This can be calculated using a 4-step method: Write out the elements Write the number of atoms of each element Calculate the Ar of the atoms of each element Add up the total mass of the elements (this is your Mr!) Part 3: Key questions 1. In a reaction, why does the mass of reactants always equal the mass of products? 2. In the equation: 2Li + F 2 2LiF a) What does the 2 in front of LiF mean? b) What does the 2 mean in F 2? 3. Explain why the following equation needs to be balanced: 2H 2 + O 2 2H 2O 4. Calculate the relative formula mass of the following compounds: a) H 2 b) H 2O c) CaCl 2 d) CO 2 e) CaCO 3 f) Ca(OH) 2 5. In a reaction, the mass of the products must always equal the mass of the reactant. However, if a gas is involved in can often look like the mass has gone up or down. a) Give an example of a reaction where it appears the mass of the product is greater than the reactant. b) Give an example of a reaction where it appears the mass of the reactant is greater than the product. c) A student heated 5g of calcium in an unsealed test tube so that it reacted with oxygen. At the end of the reaction, the mass of the product inside the test tube was 7g. Explain this observation.
Physics Motion Part 1: Glossary 1. acceleration change of velocity per second (in metres per second per second, m/s 2 ) 2. deceleration change of velocity per second when an object slows down 3. displacement distance in a given direction 4. gradient (of a straight line graph) change of the quantity plotted on the y-axis divided by the change of the quantity plotted on the x-axis 5. scalar a physical quantity which has magnititude only 6. tangent a straight line drawn to touch a point on a curve so it has the same gradient as the curve at that point 7. vector a physical quantity which has magnitude and direction 8. velocity speed in a given direction (in metres/second, m/s) Part 2: Key knowledge 1. Speed and distance-time graphs The speed of an object is: v = s/t The distance-time graph for any object that is: a. Stationary, is a horizontal line b. Moving at constant speed, is a straight line that slopes upwards c. The gradient of a distance-time graph for an object represents the objects speed The v=s/t equation can be rearranged to give s=vt or t=s/v
2. Velocity and acceleration Velocity is speed in a given direction A vector is a physical quantity that has a direction as well as a magnitude e.g. velocity. The acceleration of an object is: a = change in velocity / time Deceleration is the change of velocity per second when an object slows down. 3. Velocity-time graphs A motion sensor linked to a computer can be used to measure velocity changes The gradient of a line on a velocity-time graph represents acceleration If a velocity-time graph is a horizontal link, the acceleration is zero. A positive gradeient on v-t graph represents positive acceleration, a negative gradient represents deceleration. The area under a v-t grah represents distance travelled. 4. Analysing motion graphs The speed of an object moving at constant speed is given by the gradient of the line on its distance-time graph The acceleration of an object is given by the gradient of the line of its velocity-time graph The distance travelled by an object is given by the area under the line on its v-t graph The speed at any instant time, of an object moving at a changing speed is given by the gradient of the tangent to the line on its d-t graph.
Part 3: Key equations Equation Triangle/manipulation Units Speed equation Speed in Speed = distance time Distance in Acceleration equation 1 a = (v-u) t a= acceleration. v= final velocity u= initial velocity. t = time. Acceleration equation 2 v 2 = u 2 +2as v = final velocity u = initial velocity a = acceleration s = displacement Speed = Distance = Time = a= v= u= t = v = u = a = s = Time in Acceleration in Distance in Time in Final velocity in Initial velocity in Acceleration in Displacement in Part 4: Key questions 1. Speed and distance-time graphs State the equation, with units, that links speed, distance and time. Match each of the distance-time graphs with the correct description
A car travels 250m in 14 seconds. Calculate the speed of car with units. A train moves at a constant speed of 27m/s. Calculate the distance it travels in 120 seconds. A car moves at 30m/s for an hour. Calculate the distance it travels. Find the speed of the following: a. b. c. 2. Velocity and acceleration State the equation, with units, that links acceleration, change in velocity and time. A sprinter in a 100m race accelerated from rest and reached a speed of 9.2m/s in the first 3.1s. Calculate the acceleration of the sprinter. When a car joined the motorway, it accelerated from rest and reached a speed of 7.0 m/s for 10 s at an acceleration of 2.0m/s 2. Calculate its speed at the end of this time. 3. Velocity-time graphs State what each graph shows: acceleration, constant velocity, negative acceleration, or stationary: 1. 2. 3. 4. Analysing motion graphs 4.
Find the acceleration of the objects in the following graphs 1. 2. 3. 4. Define acceleration. Write out the formula v 2 = u 2 +2as and state what each letter stands for. An object begins with an initial velocity of 12m/s and ends with a velocity of 63m/s. If the distance travelled is 125m, what is the acceleration? What distance is travelled by an object travelling first at 6m/s, accelerating at 4m/s2 to a final velocity 30m/s?