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Chem

Lexylulu Inglés 261 fichas

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  1. 1ChemistryThe study of the properties of matter and the changes it undergoes
  2. 2CausticAn agent that burns or destroys living tissues
  3. 3WHMISWorkplace hazardous materials information system
  4. 4HomogeneousA mixture in which particles are uniformly scattered; has a uniform composition
  5. 5HeterogeneousA mixture in which the particles are not uniformly scattered; does not have a uniform composition
  6. 6SolutionA homogeneous mixture that is usually clear if it is a liquid and cannot be filtered to separate particles
    -No scattering of light
  7. 7Mechanical mixtureA heterogeneous mixture where ordinarily the different parts are big enough to see, and the stay mixed
  8. 8SuspensionA heterogeneous mixture made of large particles that are uniformly mixed but will settle if left undisturbed
  9. 9ColloidHeterogeneous mixture composed if fine particles evenly distributed throughout a second substance
  10. 10EmulsionTypes of colloids in which liquids are dispersed in liquids; many emulsions quickly separate to form layers of the original liquids
  11. 11What was WHMIS designed for?-To give employers and workers information about hazardous materials in the workplace
    -Provides workers with information how to safely store and handle dangerous materials
  12. 12Where is WHMIS used?Canada-wide
  13. 13What are the three components of WHMIS-Labels
    -MSDS - Materials Safety Data Sheets
    -Worker training and education
  14. 14What does a WHMIS label contain?-Product name
    -First aid
    -WHMIS symbols
    -Precautions
    -Company and contact information
  15. 15What is matter?-Everything around you
    -Anything that has a mass
    -Anything that has a mass and takes up space
  16. 16What determines what state something is?It's temperature
  17. 17Describe the particles of solidsParticles are packed so closely together that they only vibrate in place
  18. 18Describe the particles of liquidsThe particles are touching but can flow past each other; takes the shape of the container
  19. 19Describe the particles of gasParticles are separated by large spaces and move quickly; take the shape of container
  20. 20How many things make up the particle model of matter?5
  21. 21List the statements in the particle model of matter-All matter is made up of extremely tiny particles
    -Each pur substance has it's own kind of particle, different from the one's of other pure substances
    -Particles attract each other
    -Particles are always moving
    -Particles at a higher temperature move faster than ones at a lower temperature
  22. 22List the 2 statements in the Kinetic Molecular Theory-As matter gains energy (heats up) the particles will move faster
    -When particles move faster the spread out
  23. 23All matter can be divided into ___Mixtures and pure substances
  24. 24Pure substances are made up of ___Only ONE type of particle (molecule)
  25. 25Mixtures are made up of different ___Types of particles and can be separated
  26. 26What falls under the category of pure substances?Elements and Compounds
  27. 27What 2 types of mixtures are there?Heterogeneous and Homogeneous
  28. 28What is a homogeneous mixture called?A solution
  29. 29What are the 3 types of Heterogeneous mixtures?-Ordinary mechanical mixtures
    -Suspensions
    -Colloids
  30. 30___ are a type of colloid with liquids dispersed in liquidsEmulsions
  31. 31Element cannot be _____ into any simpler substanceBroken down
  32. 32Compound is created when2 or more elements combine chemically in fixed proportions
  33. 33True or False The particles of a solution are not uniformly scatteredFalse
    They are uniform throughout
  34. 34There are __ types of Heterogeneous mixtures4
  35. 35This heterogeneous mixture has parts that are big enough to see and stay mixedA mechanical mixture
  36. 36This heterogeneous mixture is made up of large particles that will settle if left undisturbedSuspensions
  37. 37Examples of this heterogeneous mixture are hair gel and clouds; they have fine particles evenly distributed through a second substanceColloids
  38. 38Emulsifying agents are used to-Keep the particles in mixtures from separating
    -Coat liquids to prevent them from clumping together
  39. 39Whether a mixture forms a solution, colloid or suspension depends on ___The size of particles, solubility and mixing ability
  40. 40Mixing ability is also calledMiscibility
  41. 41How can you tell the difference between a colloid and a solution?By shining light through, colloids will scatter light but solutions won't
  42. 42What is the name for the scattering of light done by colloids?The Tyndall effect
  43. 43Physical changeA change in form but not in chemical composition; no new substances are formed (can be reversed)
  44. 44Chemical changeA change in which one or more new substances are formed (can't be reversed)
  45. 45Physical PropertyAny property that can be observed or measured without forming a new substance
  46. 46DensityThe amount of matter that occupies a certain space; the mass per unit volume of a substance
  47. 47CombustibilityThe ability of a substance to burn in oxygen; not a physical property because combustion creates new substances
  48. 48Chemical propertyA characteristic of matter that describes how it reacts when undergoing a chemical change
  49. 49PropertiesCharacteristic ways in which a substance behaves
  50. 50True or false Properties can changeTrue
  51. 51Properties can be ___ or ___Physical or chemical
  52. 52Changes in matter can be ___ or ___Physical or chemical
  53. 53Physical changeA substance changes in form but not in chemical composition
  54. 54In a physical change no new ____ is formedSubstance
  55. 55True or false Physical changes can not be reversedFalse
    Physical changes can be reversed
  56. 56List examples of physical changes-Ice melting
    -Taste of chlorinated water becoming less intense after sitting overnight
  57. 57Chemical changeCauses one or more new substances to be formed when two or more substances react
  58. 58Chemical change _____ to reversIs difficult or impossible
  59. 59Physical properties can be observed, examples of physical properties are-Colour
    -Texture
    -Luster
    -Smell
    -State
    -Melting point
    -Boiling point
    -Density
    -Ductility
    -Malleability
    -Viscosity
    -Solubility
    -Conductivity
    -Hardness
  60. 60A property that describes how a substance reacts with another substance is a chemical property, list some examples-Reaction with acids
    -Ability to burn in oxygen (combustibility)
    -Reaction with water
    -Behaviour in air
    -Reaction to heat
    -Toxicity
    -Stability
  61. 61Qualitative physical propertyA characteristic that can be described but not measured
  62. 62Quantitative physical propertyA characteristic that can be measured numerically
  63. 63List some qualitative physical properties-Colour
    -Texture
    -Malleability
    -Shape
  64. 64List some quantitative physical properties-Melting point
    -Boiling point
    -Density
    -Conductivity
  65. 65Melting pointThe temperature at which a substance changes from a solid to a liquid
  66. 66Boiling pointThe temperature at which a substance changes from a liquid to a gas
  67. 67How do we calculate density?Density= mass/volume (g/cm^3)
  68. 68List the 7 things that are probably evidence of a chemical change-Heat is produced or absorbed (exothermic or endothermic)
    -The starting material is used up
    -Change in colour/smell
    -Gas is produced (bubbles)
    -A precipitate is formed (new solid)
    -Material with new properties is produced
    -Change is difficult to reverse
  69. 69ElementA pure substance made up of one type of particle, or atom. Each element has it's own distinct properties and cannot be broken down into simple substances by means of chemical change
  70. 70Law of Conservation of MassIn a chemical change, the total mass of the new substances is always the same as the total mass of the original substances
  71. 71Law of Definite compositionCompounds are pure substances that contain two or more elements combined together in fixed (or definite) portions
  72. 72ElectrolysisThe process of decomposing a chemical compound by passing an electric current through it
  73. 73CompoundPure substances that are made up of two or more elements chemically combined together. Compounds can be broken down into elements again by chemical means
  74. 74LawAn action or condition that has been observed so consistently that scientists are convinced that it will always happen
  75. 75TheoryAn explanation of an event that has been supported by consisted, repeated experimental results and has therefore been accepted by a majority of scientists
  76. 76ModelA mental image, used as a building block that helps to explain an event; often for clarity, scientists diagram, make physical representations, or treat mathematically the features of a model
  77. 77ObservationThe use of the sense to gather information; in science, often aided by instruments such as telescopes, thermometers, and balances
  78. 78ElectronNegatively charged particles
  79. 79Atomic nucleusThe centre of the atom; contains protons and neutrons
  80. 80ProtonPositively charged particles found inside the atomic nucleus
  81. 81NeutronUncharged particles in the atomic nucleus
  82. 82What did ancient Greek philosophers believe all matter was made out of?Four elements: earth, air, fire and water
  83. 83AlchemistPart mystic, part pharmacist
  84. 84What 3 things did alchemists do and what thing did they believe they could do?They developed many useful procedures such as distillation, they described the properties of many different materials (boiling point, melting point) and they used special symbols to prevent others from finding out their secrets. They though they could turn copper and lead into gold.
  85. 85Who stated that all science should be based on experimental evidence rather than thoughtSir Francis Bacon
  86. 86Who recognized that element could combine to form compounds?Robert Boyle
  87. 87Bacon and Boyle ___ other to search for ___They motivated others to search for elements
  88. 88Why did scientists use heating, burning, mixing and cooling?To take matter down until it could not be broken down any further in order to determine if the substance was a pure substance or mixture
  89. 89Who defined elements as pure substances that could not be broken down any further? He also identified 23 substances as elements.Antoine Lavoisier
  90. 90Lavoisier used a balanced view of chemical change, he also had the successful technique of measuring mass. His observations are now called ___The Law of Conservation of Mass
  91. 91Mass cannot be ___ or ___Created or destroyed
  92. 92Give examples of the Law of Definite Composition- Pure water always has 11% hydrogen and 89% oxygen
    -Hydrogen peroxide always contains 6% hydrogen and 94% oxygen
  93. 93What is it called when an electric current is passed through a compound to separate the elements?Electrolysis
  94. 94Who developed a theory to explain the electrolysis of water?John Dalton
  95. 95What are the parts of Dalton's atomic theory?- All matter is made up of tiny particles called atoms
    -Atoms cannot be created, destroyed or divided into smaller particles
    -All atoms of the same element are identical in mass and size.
    -Atoms of one element are different in mass and size from the atoms of other elements
    -Compounds are created when atoms of different elements link together in definite proportions
  96. 96Give examples of elementsHydrogen
    Oxygen
    Carbon
  97. 97Give examples of compoundsWater (H2O)
    Carbon dioxide (CO2)
    Salt (NaCl)
  98. 98Scientific ideas may change over time as more ___ is gatheredEvidence
  99. 99Most of Dalton's atomic model has stood the test of time, however new things have been discovered that influence his model, what are they?Smaller particles than atoms (subatomic particles- protons, neutrons and electrons)
  100. 100Electrons are ____ and ___ the nucleusAre negative and orbit
  101. 101The nucleus of an atom is made up of what?Positive protons and neutral neutrons
  102. 102Where does most of the mass of an atom come form?The nucleus
  103. 103Who developed the plum pudding model and reasoned that if there were negatively charged particles, but atoms don't normally have a charge, there must be positive particles?J.J Thomson
  104. 104What did Ernest Rutherford predict was found in the nucleus with protons while creating his planetary model?Neutrons
  105. 105What was the model created by Neils Bohr and Rutherford in which the electrons moved around the nucleus in fixed pathways?Bohr's atomic model
  106. 106Today we use the ____ model created by French physicist Louis de Broglie, Austrian physicist Erwin Schrodinger and many othersElectron cloud model
  107. 107Element symbolsOne or more letters used to represent the name of a substance
  108. 108MalleableAble to be hammered or pressed into shape without breaking or cracking
  109. 109DuctileAble to be drawn out into a thin wire
  110. 110MetalA solid materials which is typically hard, shiny, malleable, fusible and ductile with good electrical and thermal conductivity
  111. 111Non-metalAn element or substance that is not a metal
  112. 112MetalloidElements with properties in between metals and non metals
  113. 113Chemical familyA group of related elements that have similar properties
  114. 114Alkali MetalsVery reactive metals that need special storage and have unpaired electrons; found in group 1 of the periodic table
  115. 115Alkaline earthsReactive, but not as reactive as alkali metals. Found in group 2 of the periodic table
  116. 116Noble gasesAny of the gaseous elements in group 18 of the periodic table; thought to be completely non-reactive but compound of xenon, krypton and radon are now known
  117. 117HalogensAny of the elements of group 17 of the periodic table; most reactive non-metallic elements
  118. 118The symbols of an element always have one ___, they may also be followed by a _____One capital letter, by a lower case letter
  119. 119Elements are listed in order of their ____Atomic mass
  120. 120Atomic mass is the mass of _____ of an elementOne atom
  121. 121Atomic mass is represented in what?Atomic mass units (amu)
    1.0 amu = 1.6605x10^-27 kg
  122. 122What contribute to the atomic mass?Protons and neutons
  123. 123Elements can be classified into __,___ and _Metals, non-metals and metalloids
  124. 124Stairway divides metals and non-metals, on which side of it is which?Metals are underneath and to the left , non-metals are above and to the right
  125. 125Metals are in what state (except ____) at room temp?They are solids, except for mercury which is a liquid
  126. 126What are the physical properties of metals?-Good conductors of heat and electricity
    -Shiny and have lustre
    -Malleable and ductile
  127. 127Metalloids have properties of what?Metals and non-metals
  128. 128The physical properties of metalloid are what?-Brittle
    -Non ductile
    -May conduct electricity but NOT heat
  129. 129Where are metalloids found?On or under the staircase
  130. 130What state are non-metals at room temp?Solid, gas and one liquid
  131. 131The physical properties of non-metals are what?-Can't conduct heat or electricity
    -Brittle
    -Not malleable or ductile
    -Not shiny
  132. 132Each horizontal column is called a what?A period (1-7)
  133. 133Each vertical column forms a __ or __Group of family (1-18)
  134. 134The families you need to know are:-Group 1 Alkali metals
    -Group 2 Alkaline Earth Metals
    -Group 17 Halogens
    -Group 18 Noble Gases
  135. 135True or false Alkali metals don't occur freely in nature and are softer than most metalsTrue
  136. 136Alkali metals easily _____ to form a compoundGive an electron
  137. 137List the alkali metals-Lithium (Li)
    -Sodium (Na)
    -Potassium (K)
    -Rubidium (Rb)
    -Cesium (Cs)
    -Francium (Fr)
  138. 138Alkaline Earth Metals ___ found freely in natureAren't
  139. 139Name some of the Alkaline Earth Metals-Radium (Ra)
    -Calcium (Ca)
    -Magnesium (Mg)
    -Beryllium (Be)
  140. 140How many noble gases are there?6
  141. 141Noble gases are stable becauseThey have the maximum number of electrons possible in their outer shell
  142. 142Name some of the Noble Gases-Helium (He)
    -Neon (Ne)
    -Argon (Ar)
    -Krypton (Kr)
    -Xenon (Xe)
    -Radon (Rn)
  143. 143Halogen are the ______ non-metalsmost reactive (unpaired electron)
  144. 144Name some of the Halogens-Fluorine (F)
    -Chlorine (Cl)
    -Bromine (Br)
    -Iodine (I)
    -Astatine (At)
  145. 145Who gets to name an element?The first chemist to report it
  146. 146Periodic tableTable of the chemical elements arranged in order of atomic number, usually in rows, so that elements with similar atomic structure (and hence similar chemical properties) appear in vertical columns
  147. 147Atomic massThe average mass of an atom of an element
  148. 148Atomic numberThe number of protons in the nucleus of an atom
  149. 149Mass numberA number used by chemists to give the total number of protons and neutrons in an atom
  150. 150How do we calculate mass number?Number of protons + number of neutrons=
    Mass number
  151. 151How do we calculate number of neutrons?Atomic mass - atomic number =
    number of neutrons
  152. 152What did Dimitri Mendeleev do?He organized the 63 known element into a table of rows and columns based on atomic mass
  153. 153Elements with similar physical and chemical properties were put into ____Groups or families
  154. 154Why did Mendeleev leave gaps in the table?Because there were holes in the families, in believed there was an undiscovered element that fit that gap. Hy hypothesized about the physical and chemical properties of the missing elements
  155. 155Each element on the periodic table has these 3/4 partsAtomic number
    Symbol
    Occasionally name
    Atomic weight
  156. 156If you change the number of protons what do you change?The element
  157. 157Number of protons is equal to ____The number of electrons
  158. 158Neutrons are found in ____ and have ____ chargeThe nucleus and have no electrical charge
  159. 159The number of ____ in the outer orbit will determine how this atom/element reacts with other atomsElectrons
  160. 160What do atoms do to try and achieve a complete/full outer orbital?They will either give away or steal electrons
  161. 161Metals have ____ electrons so they ____ electrons and become a ___ ionMetals have extra electrons so they donate electrons and become a positive ion
  162. 162Non-metals are ____ electrons so they ____ electrons and become a ___ ionNon-metals are missing electrons so they accept electrons and become a negative ion
  163. 163Lithium has 3 electrons, meaning it has 1 extra. Will it give away or accept electrons and what type of ion will it become?It will give away it's extra electron, making it a positive ion
  164. 164Sulfur has 16 electrons, meaning it's missing 2 Will sulfur donate or steal electrons and what type of ion will it become?It will steal 2 electrons, making it a negative ion
  165. 165True or False Argon has 18 electrons, having a complete orbital. It will donate electrons and become positiveFalse
    Because it has a complete orbital, argon will not react and therefore not donate or gain electrons. It will not become an ion
  166. 166If a magnesium looses 2 electrons, it's ion charge will be +2, what will it's symbol look like as an ion?Mg2+
  167. 167Chemical formulaA formula that shows the number and types of atoms in a molecule
  168. 168Molecular compoundFormed when atoms share electrons
  169. 169Binary compoundCompounds made of two elements
  170. 170MoleculeSmallest independent unit of a pure substance, generally a cluster of atoms joined together
  171. 171Diatomic moleculesMolecules made of two atoms of the same element
  172. 172Ionic compoundFormed when atoms transfer electrons to or from other atoms
  173. 173IonAn atom or molecule with a net charge due to the loss or gain of one or more electrons
  174. 174ConductivityThe ability of a substance to cary an electrical current
  175. 175When two or more elements bond together they form ___One compound
  176. 176Chemical compounds have a ___Chemical name and formula
  177. 177What is the International Union of Pure and Applied Chemistry (IUPAC)The universal naming system for compounds
  178. 178What uses symbols and numerals to represent the composition of a pure substance?Chemical formulas
  179. 179Each symbol in a chemical formula represents what?An atom of an element (if there is more than one atom of an element a subscript follows the element's symbol; if there is no subscript there is only one atom of that element)
  180. 180How do we know the state of a compound?It is written in subscript and parentheses after the chemical name/formula
  181. 181Give some examples of chemical formulas with their physical state-H2O (l) - liquid
    -NaCl (s) - solid
    -CH4 (g) - gas
    -NaCl (aq) if dissolved in solution (aqueous)
  182. 182What holds elements together when the form a compound?Chemical bonds
  183. 183When are chemical bonds formed?When elements gain, lose or share electrons
  184. 184What are the two types of compounds?-Ionic Compounds (formed when atoms transfer electrons to other atoms)
    -Molecular compounds (formed when atoms share electrons)
  185. 185What are the properties of ionic compounds?-Formed from metallic and non-metallic elements
    -Forms ions in solution (separate into positive and negative ions when dissolved in water)
    -Conduct electricity
    -Solid at room SATP (Standard Ambient room Temperature and Pressure)
  186. 186What are the properties of molecular compounds?-Usually formed from only non-metallic elements
    -Does not form ions in solution
    -Usually does not conduct electricity
    -Solid, liquid or gas at SATP
  187. 187When an atom gains or loses electrons, the atoms is no longer ____Neutral
  188. 188Why are atoms typically neutral?Because they contain equal numbers of positive and negative particles
  189. 189Ionic compounds stick together because of _____Electrostatic charge (opposite charges attract)
  190. 190Ionic compounds are always made up of a ___ metal ion and a ___ non-metal ion(+) and (-)
  191. 191In an ionic compound, what must balance?The charges
  192. 192Atoms donate or gain electrons in order to reach what goal?Having a full outer shell of electrons
  193. 193Ionic compounds have an overall electrical charge of ___Zero!
  194. 194Sodium chloride looks like this: Na+ and Cl- = NaCl Why is there no charge in sodium chloride?Because the positive charge cancels out the negative charge so the net electrical charge is 0 (+1 + -1= 0)
  195. 195In an ionic compound, you must always start with the name of the ____, which will not changeMetal
  196. 196In an ionic compound, the non-metal is second. The ending of it's name is changed to what?-ide
  197. 197You have ____ the charges by figuring out how many of each ion is required to do so and then subscript that numberTo balance
  198. 198Ionic compound naming: Calcium chloride Calcium ion has a charge of 2+ Chloride ion has a charge of 1- Figure out the chemical formulaCalcium has 2+ and 2 chloride 1- ions balance out
    (+2) + 2(-1) = 0
    Chemical formula is CaCl2 (s)
  199. 199What must you always remember when using the criss-cross technique?You MUST simplify the formula
  200. 200Written name to symbol example: Find formula for Calcium ChlorideCalcium 2+
    Chlorine 1-
    Ca2+ Cl1- Cl1- to balance
    CaCl2
  201. 201What are polyatomic ions?A group of atoms that together carry a negative (anion) or positive (cation) charge
  202. 202The entire group of atoms behave as _____ and will carry the net ___One ion and will carry the net charge
  203. 203Most polyatomic ions areNegative
  204. 204The most common polyatomic ion is NH4+ which is ___Ammonium
  205. 205If one of the polyatomic ions already has a subscript (i.e. NO3-) that subscript will ___Stay in place but will be put in brackets
    Example:
    Ca2+ + NO3- = Ca(NO3)2
  206. 206Multivalent ions are transitional metals with ___More than one possible valence (ion)
  207. 207Why do some metals have more than one possible valence?Because of sub-orbitals
  208. 208How do we specify the charge we are using with multivalent ions?Roman numerals that are inserted after the metallic element's name
    Example: Nickel (II) chloride
  209. 209What are diatomic molecules?Molecules made of two atoms of the SAME element
    (Written as H2, N2, O2, F2, Cl2, also P4, S8)
  210. 210How do we know what molecules are diatomic?The elements that end in -gen (hydrogen, oxygen, nitrogen) and the elements that belong to group 17
  211. 211When naming molecular compounds, you write the entire name of the ____ elementFirst
  212. 212You change the ending of the ____ element to -ide in molecular compoundsSecond
  213. 213In molecular compounds, you use a ___ to indicate the number of each type of atom in the formulaPrefix
  214. 214Right all the prefixes (remember not to right the prefix mono for the first element0Mono
    Di
    Tri
    Tetre
    Penta
    Hexa
    Hepta
    Octa
    Nona
    Deca
  215. 215Give an example of molecular compound namingCO2
    Carbon
    Change oxygen to oxide
    1 carbon atom, 2 oxygen atoms
    Carbon dioxide
  216. 216Written name to symbol - molecular compounds Try it with Pentaphosphorus DecaoxidePentaphosphorus - 5 phosphorus
    Decaoxide - 10 oxide
    P5O10
  217. 217Exceptions to molecular compound naming! What are the formulas for: Water Methane Hydrogen peroxide Ammonia Sucrose GlucoseH2O
    CH4
    H2O2
    NH3
    C12H22O11
    C6H12O6
  218. 218In molecular compounds don't usually form large structures because the ___ between atoms is ___, but the ____ between molecules is ___Bonding is strong, the attraction is weak
  219. 219During a chemical reaction ___ are broken and new substances are _______Chemical bonds are broken and new substances are always produced
  220. 220Chemical reactionA process in which a substance is changed into one or more new substances
  221. 221ReactantThe substances that go into a chemical reaction
  222. 222ProductThe substances produced by a chemical reaction
  223. 223Physical changeA change in form but not in chemical composition; no new substances are formed
  224. 224Chemical equationA representation of a chemical reaction using symbols of the elements to indicate the amount of substance, usually in molecules, of each reactant and product
  225. 225ExothermicA chemical reaction in which heat energy is released to the surroundings
  226. 226EndothermicA chemical reaction in which heat energy is taken in from the surroundings
  227. 227The properties of the reactants are different from those of the ____Products
  228. 228Give an example of a chemical equationMethane + oxygen -> carbon dioxide + water + energy
  229. 229You can convert chemical word equations into chemical formula equations. Do so with water + energy (electricity) -> oxygen + hydrogenH2O + energy -> O2 + H2
  230. 230Atoms are neither created or destroyed, what happens to them in chemical reactions?The atoms change partners as old substances are changed into new substances
  231. 231How do we break chemical bonds?We add energy
  232. 232What happens when chemical bonds are broken?Energy is released
  233. 233Give an example of an exothermic reactionAn explosion
    (think EXothermic energy EXits)
  234. 234Give an example of an endothermic reactionA cold pack or baking
    (think ENdothermic energy ENters)
  235. 235Chemical reactions involve changes in energy; energy is either ____ or ___ during a chemical reactionProduced or absorbed
  236. 236Give a chemical equation for an exothermic reactionCombustion reactions:
    C8H18 + O2 -> CO2 +H2O + energy
    or
    Octane + oxygen -> carbon oxide + water + energy (heat)
  237. 237Give a chemical equation for an endothermic reactionCooking:
    Baking soda + energy -> carbon dioxide+ water + sodium carbonate
    NaHCO3 + energy -> CO2 + H2O + Na2CO3
  238. 238Reaction rateMeasure of how fast a reaction occurs
  239. 239CatalystA substance that speeds up a chemical reaction without being used up in a reaction
  240. 240EnzymeA special protein molecule that regulates chemical reactions in living organisms
  241. 241InhibitorSubstances that slow down or prevent chemical reactions
  242. 242CorrosionA process whereby metals or stone are chemically degraded or broken down
  243. 243RustIron oxide, a product of the chemical reaction of iron, oxygen and moisture
  244. 244GalvanizationThe process of protecting metals by coating them with a thin layer of zinc
  245. 245ElectroplatingTo plate or coat with a metal by electrolysis
  246. 246CombustionThe highly exothermic combination of a substance with oxygen, requires heat, oxygen and fuel
  247. 247Chemical reactions can occur at ___different speeds
  248. 248Reaction rate can be measure by how quickly a _____ disappears or ____ appearsReactant, product
  249. 249What 4 things can you change to speed up a reaction rate?-Temperature (higher temp faster reaction)
    -Stirring (stirring increases rate of reaction)
    -Surface area (more surface area in contract faster reaction rate)
    -Concentration (higher the concentration faster the reaction)
  250. 250A catalyst does not affect what?The amount of products produced, only the speed at which they are produced
  251. 251Give examples of when catalysts are usedProduction of vegetable shortening, synthetic rubber and high-octane gas
  252. 252Enzymes helps reactions in the body that do what?Break down food
  253. 253Where is the enzyme that helps breakdown starch molecules?In the saliva
  254. 254Give examples of when inhibitors are used-In plant seeds to prevent germination until perfect conditions
    -Added to foods and medicines to slow down decomposition
  255. 255How do we prevent corrosion?-Applying a thing coat of paint
    -Galvanization (coating with zinc)
    -Electroplating (coating with metal using electrolysis)
  256. 256Give an example of corrosionRust
  257. 257When do we use combustion?Burning:
    -Gasoline in a car
    -Natural gas in a furnace
    -Food in our body
    -Propane in a bbq
  258. 258Products of combustion are not always ____Beneficial
  259. 259Burning fossil fuels produces what?-Water
    -Carbon dioxide
    -Smoke, soot, ash
    -Heat
    -Carbon
    -Sulfur and nitrogen oxides (NOX and SOX!)
  260. 260In combustion __ is used up and ___ is produceoxygen and energy
  261. 261In Rutherford's model, most of the space that is taken up by and atom is___Empty space

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Fichas sobre Chem, creado por Lexylulu el 20/01/2015.
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