Grade 10 Final Exam Study Guide PDF

Final Exam Study Guide Table of Contents Table of Contents Scientific Method Safety Symbols Unit 1: Chemistry - Atoms, Elements, and Compounds 1.01 Intro to Studying Matter Particle Theory of Matter Classifications of Matter 1.02 Physical Properties...

Final Exam Study Guide Table of Contents Table of Contents Scientific Method Safety Symbols Unit 1: Chemistry - Atoms, Elements, and Compounds 1.01 Intro to Studying Matter Particle Theory of Matter Classifications of Matter 1.02 Physical Properties Qualitative Physical Properties can be observed and described, but not measured Quantitative Physical Properties Phase Changes and Matter Calculations Phase Changes Calculation of density/volume/mass 1.03 Chemical Properties Chemical property Gas tests 1.04 Physical + Chemical Changes (Indicators) Evidence of a chemical change 1.05 Atomic Structure & Isotopes Standard Atomic Notation Mass Number (A) Atomic number (Z) Isotopes Multivalent 1.06 Periodic Table & Polyatomics Properties 1.07 Compounds Ionic Compounds Properties of ionic compounds Naming Covalent Compounds Properties of covalent compounds Naming Polyatomic Compounds  Naming Acids & Bases 1.08 pH Scales 1.09 Types of reactions Synthesis Decomposition Single Displacement Double Displacement Combustion Neutralization Corrosion 1.10 Reactivity Series Unit 2: Optics 2.01 Intro to Light 2.02 Eye anatomy 2.03 Light Sources 2.04 Reflection (Mirrors) 2.05 Refraction and Car Analogy 2.06 Refraction Index & Formulas 2.07 Calculating Refractions 2.08 Lens 2.09 Magnification Unit 3: Biology 3.01 Properties of Life 3.02 Link to content WHMIS Image Scientific Method Common sense way of observing the world and documenting findings throughout. -​ Composed of many steps -​ It is logical reasoning -​ Testing data -​ It ensures that the knowledge that is obtained is due to a strong foundation, and not some assumption that can be incorrect 1.​ Observation 2.​ Ask a question (5W and H) 3.​ Create a reason why it happened, an explanation that is testable (Hypothesis) 4.​ Experiment with your hypothesis (MUST BE REPRODUCIBLE) a.​ Design an Experiment i.​ Have a controlled environment to isolate as many variables and other factors as possible. This means having the same quantities, and exposure to light, heat, and other factors that may alter the hypothesis b.​ Predict what might happen c.​ Test the prediction 5.​ Refine/iterate the process a.​ If true, come up with another hypothesis that could also be tested that can have an impact b.​ Refine the experiment to see if it could yield better results c.​ If false, come up with an explanation as to why it was wrong i.​ Come up with another reason for the first question “The duty of the man who investigates the writing of scientists, if learning the truth is his goal, is to make himself an enemy of all that he reads, and … attack it from every side. He should also suspect himself as he performs his critical examination of it so that he may avoid falling into either prejudice or leniency.” - Hasan Ibn al-Hayatham (Alhazen) Safety Symbols -​ Hazardous Household Products Symbols Signal Words Caution: Temporary injury, possible death in high quantities Danger: May cause temporary/permanent injury or death Extreme danger: low exposure can cause death/serious injury WHMIS (Workplace Hazardous Materials Information System) Image Unit 1: Chemistry - Atoms, Elements, and Compounds 1.01 Intro to Studying Matter Particle Theory of Matter -​ All matter is made up of tiny particles (Atoms/Molecules) with empty spaces between -​ Different pure substances are made of different types of particles -​ Particles are in constant, random motion -​ As temperature increases, particles move faster -​ Particles attract each other. The force of attraction are stronger when particles are closer together Classifications of Matter Matter -​ Mass -​ Volume -​ Inertia Pure substance -​ Contains only one type of particle -​ can be an element/pure compound Element -​ contains only one type of atom -​ cannot be broken down into simpler substances Compound -​ one kind of molecule made up of different atoms Mixtures -​ An impurity where two or more other compounds are not chemically linked  Homogeneous Mixture -​ Particles are evenly distributed -​ Cannot distinguish the different types of particles Heterogeneous/Mechanical Mixture -​ Particles are unevenly distributed -​ 1.02 Physical Properties Describes the substance Qualitative Physical Properties can be observed and described, but not measured -​ Color -​ State -​ Texture -​ lustre (shininess) -​ optical clarity (transparency) -​ malleability (ability to be hammered into thin sheets), -​ Ductility (ability to turn into wires) Quantitative Physical Properties -​ Boiling point -​ Melting point -​ Height/length/width -​ Viscosity (High viscosity= thicker like honey) -​ Solubility (ability to dissolve, usually in water) -​ Hardness (Ability to be scratched) -​ Conductivity (ability to let electrons move freely) -​ Density (Mass/volume, g/cm3) Phase Changes and Matter Calculations Phase Changes -​ Sublimation is when a solid turns into a gas -​ Deposition is when a gas turns into a solid -​ Evaporation is when a liquid turns into gas -​ Condensation is when a gas turns into a liquid -​ Melting is when a solid turns into a liquid -​ Freezing is when a liquid turns into a gas Calculation of density/volume/mass -​ M = D*V -​ D = M/V -​ V = M/D -​ Remember to use the units (d,m,v = g/cm3, g, cm3) Density/Volume/Mass -​ A solid object will float in a liquid if it has a lower density than the liquid 1.03 Chemical Properties Describes how the substance reacts when mixed with other substances Chemical property -​ Ability of a substance to react to another substance and produce 1+ new substances -​ Oxidation: Reactivity with oxygen -​ Acidity of Basicity: Reactivity with acids (baking soda reacts with acids to produce CO2) -​ Combustibility (Burn in air, propane is highly combustible) -​ Stability (Ability of a substance to remain unchanged, hydrogen peroxide decomposes into H2O + oxygen at room temperature) -​ Toxicity (ability of substance to cause harmful effects in plants/animal like tetanus) -​ Flammability -​ Radioactivity Gas tests -​ Hydrogen makes a pop sound when reacting with a burning splint because hydrogen reacts rapidly with oxygen to produce water vapour -​ Oxygen reignites glowing splints -​ Carbon dioxide puts out burning splints, turns cloudy when mixed with limewater 1.04 Physical + Chemical Changes (Indicators) Physical change -​ Change in appearance/state that does not produce a new substance -​ Ex. ripping paper, freezing, dissolving -​ Usually reversible Chemical change -​ Change where one or more new substances are produced -​ Ex. burning paper, nails rusting, baking cake -​ Usually hard or impossible to reverse Evidence of a chemical change -​ Color change -​ New solid (precipitate) forms when liquids are mixed -​ Gas is produced (bubbling/new odour) -​ New odour -​ Heat/light is produced/absorbed (Change in energy) -​ Difficult to reverse 1.05 Atomic Structure & Isotopes Protons (p+), Neutrons (n0), and Electrons (e-) Particle Location Mass Charge Symbol Proton Nucleus 1u 1+ p+ Neutron Nucleus 1u 0 n0 Electron Orbitals/Shells 0 u (1/2000 u) 1- e- Shells, Energy levels, orbitals, electron clouds, etc. -​ Where electrons can be found -​ Each period indicates how many shells -​ First shell holds 2 -​ Second shell holds 8 -​ Third shell holds 8 -​ (Excludes transitional metals) -​ Standard Atomic Notation Mass Number (A) -​ Sum of protons and neutrons  -​ Round to nearest whole number Atomic number (Z) -​ Number of protons in the nucleus of an atom -​ Determines identity of an element Isotopes -​ Forms of elements that have same amount of protons but different # of neutrons -​ Specified by placing mass number after the name of the element (Carbon-12) -​ Atomic masses on the periodic table is a weighted average of naturally occurring isotopes Multivalent -​ Element with more than one different valence electron -​ Indicated by roman numerals (II) -​ Used to have old names (ous, ric) -​ This indicates how many electrons are there -​ In formulas write a superscript with e- and charge E.g. Fe2+ ​ +​ O2​ =​ FeO Bohr Rutherford Diagram Lewis Dot Diagram Rutherford Diagram 1.06 Periodic Table & Polyatomics Information about the Periodic Table 1.​ Atomic name 2.​ Atomic # 3.​ Atomic mass 4.​ Number of protons, neutrons, and electrons in an atom 5.​ Family groups 6.​ Periods 7.​ # of electrons in valence shell 8.​ # of shells 9.​ Element type: metals, nonmetals, and metalloids 10.​State of matter 11.​Physical properties Properties Group Name Properties 1 Alkali Metals 2 Alkaline Earth Metals 3 1.07 Compounds -​ All compounds are formed based on valence electron reactions -​ Must form an octet for stability (8 electrons in shell) -​ Electrons are gained, lost, or shared to form octets Ionic Compounds -​ Made of elements carrying an overall charge -​ metal + nonmetal -​ Form strong bonds Properties of ionic compounds -​ Soluble in water -​ Conduct electricity when melted or dissolved in water -​ High melting point -​ Hard -​ Brittle Ions -​ Any atom carrying a charge -​ Positive charge is cation -​ Negative charge is anion Types of Ionic Compounds -​ Binary Ionic Compounds -​ Made of metal & nonmetal -​ Multivalent Ionic Compounds -​ Type of binary ionic compound -​ Atoms have different reactivities (transitional metals) Naming Cation comes first -​ If cation is multivalent, add roman numerals (II) -​ If not skip Anion -​ Drop the ending -​ Add “ide” at the end OR -​ If polyatomic, follow polyatomic naming Covalent Compounds -​ Also called molecular compounds -​ Made of non-metals bonded together -​ Sharing electrons -​ Share a polar charge -​ Have weaker bonds when compared to ionic compounds Properties of covalent compounds -​ Insoluble in water due to no charge -​ Do not conduct electricity  Naming Use greek prefixes. 1 mono 7 hepta 2 di 8 octa 3 tri 9 nona 4 tetra 10 deca 5 penta 11 hendeca 6 hexa 12 dodeca If the begins with one of its type, drop the mono (e.g. monocarbon dioxide) Polyatomic Compounds -​ Covalent compounds with charges -​ Mostly has an oxygen, rarely ever doesn’t -​ Bonds with metals create ionic compounds Naming If it is an oxyanion, it will follow this rule below e- Naming +1 per……………………ate 0 …………………………ate -1 ………………………….ite -2 hypo………………….ite Acids & Bases 1.08 pH Scales pH stands for power of hydrogens. 1.09 Types of reactions Reactions can be written in three different ways: Word form: Iron​ ​ +​ ​ Oxygen​ →​ ​ ​ iron oxide Skeletal form: Fe​ ​ +​ ​ O2​ ​ →​ ​ ​ Fe2O Synthesis Creation of larger molecules made up of two smaller molecules A​ ​ +​ ​ B​ ​ →​ ​ ​ AB Mg​ ​ +​ ​ O2​ ​ →​ ​ ​ MgO2 2Mg​ ​ +​ ​ O2​ ​ →​ ​ ​ 2MgO2 Decomposition Breakdown of larger molecules creating smaller molecules/atoms AB​ ​ ​ ​ →​ A​ ​ +​ ​ B ​ ​ CaCO3​​ ​ ​ →​ CaO​ ​ +​ ​ CO2 Single Displacement When a metal in a compound is replaced with a more reactive metal to form a new compound (on reactivity series) AC​ ​ +​ ​ B​ ​ →​ BC​ ​ +​ ​ A NaBr2​ ​ +​ ​ K​ ​ →​ KBr​ ​ +​ ​ Na NaBr2​ ​ +​ ​ 2K​ ​ →​ 2KBr​ ​ +​ ​ Na Double Displacement When two compounds react and the cations switch places and form new compounds with the anions AC​ ​ +​ ​ BD​ ​ →​ AD​ ​ +​ ​ BC AgNO3​​ +​ ​ KCl​ ​ →​ AgCl​ ​ +​ ​ KNO3 Combustion A type of reaction where a chemical reacts with oxygen gas to produce carbon dioxide, water, and energy CH4​ ​ +​ ​ O2​ ​ →​ CO2​ ​ +​ ​ H2O CH4​ ​ +​ ​ 2O2​ ​ →​ CO2​ ​ +​ ​ 2H2O 2C8H10​​ +​ ​ 21O2​ ​ →​ 16CO2​​ +​ ​ 10H2O 4C7H7​ ​ +​ ​ 35O2​ ​ →​ 28CO2​​ +​ ​ 14H2O 2C12H22​ +​ ​ 35O2​ ​ →​ 24CO2​​ +​ ​ 22H2O Complete Combustion: When the product is only CO2, H2O, and energy Incomplete Combustion: When the product is a mix of CO2(g), CO(g), C(s), H2O(g), and energy Neutralization A chemical reaction in which an acid and a base react to form an ionic compound (salt) and water, resulting in a pH closer to 7. Not all salts have to be NaCl. HA​ ​ +​ ​ BOH​ ​ →​ AB​ ​ +​ ​ HOH HCl​ ​ +​ ​ NaOH​ ​ →​ NaCl​ ​ +​ ​ H2O HNO3​ ​ +​ ​ KOH​ ​ →​ KNO3​ ​ +​ ​ H2O Corrosion Breakdown of metal due to it reacting with its environment. Corrosion can be good. Copper can be corroded to develop patina, used to make roofs waterproof for years. Corrosion can be bad. Rust on iron makes it thinner and thinner. 1.10 Reactivity Series Unit 2: Optics Key takeaway: -​ Light has characteristics and properties -​ Can be manipulated with mirrors and lenses for a wide range of uses -​ How society benefits from optical devices -​ Telescopes, cameras, flashlights, mirrors, computers, microwaves, radios, etc. 2.01 Intro to Light -​ Light is extremely fast -​ Travels in straight lines -​ Travels through empty space -​ Form of energy (can heat stuff up) -​ Light can reflect -​ Bounce from surfaces -​ Light can refract -​ When it travels from one medium to another, and continues in a straight line Waves -​ A periodic motion -​ Repeats itself -​ The motion creates a wave, this frequency is an observable oscillate Frequencies -​ How often Word Definition incandescence chemiluminescence phosphorescence bioluminescence fluorescence LED OLED 2.02 Eye anatomy Cornea -​ The protective layer of the eye -​ Outer layer Pupil -​ Hole in the eye which allows light to pass through Iris -​ Muscles within the eye that control the size of the pupil Lens -​ Adjusts light Choroid -​ Retina -​ Receives photons and generates information to send to the optic nerve Vitreous Gel -​ Clear gel that maintains the eye shape Optic Nerve -​ 2.03 Light Sources Objects that produce light are referred to as luminous objects. They convert other forms of energy into light. Sources can be natural such as: -​ Sun -​ Forest fire -​ Fireflies Or artificial such as: -​ Glowing lightbulb -​ Computer screen Objects that do not produce light are called non-luminous objects. They may appear bright because they reflect light. Incandescent 2.04 Reflection (Mirrors) Are shiny surfaces that reflect light by bouncing photons. Types of mirrors: -​ Flat mirror -​ Concave -​ Convex Terminology Angle of Incidence ​ -​ The angle that light hits a reflective surface Angle of Reflection​ -​ The angle that light then bounces from the surface Flat mirror reflects light Parts of a mirror Center of curvature ​ ​ →​ ​ Center of the circle Focal point​ ​ ​ →​ ​ Object​​ ​ ​ →​ ​ Creating lines -​ Parallel to focal point -​ Focal point to parallel -​ Center of curvature 2.05 Refraction and Car Analogy Refraction is the phenomenon of light when it changes as it passes through When light crosses the boundary of two mediums it refracts Transparent substances are also called media (singular is medium) Refraction is used to create glasses, lenses cameras, telescopes Reason for refraction: The speed of light is 300 000 km/s https://www.youtube.com/watch?v=FDLOQSDdStk 2.06 Refraction Index & Formulas 2.07 Calculating Refractions n1 = 1.00 n2 = 1.33 2.08 Lens Rules for drawing light rays that the lens bends 1.​ Parallel Ray 2.​ Centre Ray 3.​ Focal Ray 2.09 Magnification Magnification h = height d = distance Thin lens equation f = focal length do = object distance di = image distance Unit 3: Biology 3.01 Properties of Life Properties of life: 1.​ Organization -​ Containing highly specialized coordinated parts -​ All organisms are made up of cells -​ Unicellular or multicellular organisms -​ Atoms and molecules form organelles and structures -​ Cells make up tissues -​ Tissues make up organs 2.​ Metabolism -​ Biochemical reactions in organisms are called metabolic reactions -​ Gas exchange -​ Metabolism is necessary for growing, repairing, reproducing, and maintaining body structure. -​ Two types: -​ Anabolism -​ Organisms transform simpler molecules into complex -​ Catabolism -​ Organisms transform complex molecules into simpler 3.​ Homeostasis -​ The process by which organisms regulate their body temperature for cellular activities to function properly -​ Even if the external environment is different 4.​ Growth  -​ Cells undergo regulated growth 5.​ Reproduction -​ How organisms reproduce themselves to create more organisms 6.​ Response (Reflex actions) -​ Living organisms show irritability -​ How they respond to their environment -​ Dangers -​ Moving away from fire -​ Benefits -​ Migration -​ Plants moving towards sunlight 7.​ Evolution -​ Change in organisms overtime -​ Evolving -​ Involves natural selection -​ Survival of the fittest -​ Organisms that can survive in tough environments only survive -​ Also include naturally selected genes -​ Fur colors -​ Beak or claw shape -​ Heritable traits that provide fitness advantages or advantages in general are called adaptations 8.​ 3.02 Link to content https://onedrive.live.com/redir?resid=504E7CB6A903EC71%2152070&authkey=%21APhQdWc VaYewuU4&page=View&wd=target%28Chem.one%7C644d4eb0-1e00-4471-8adb-5859587b3 1ae%2FWS%20-%20WHMIS%7C1f31f7b8-0974-494a-8920-4295bcb092eb%2F%29&wdorigin =NavigationUrl WHMIS Image