- Chemistry Exam Study Sheet

8/4/2019 DOC FILE - Chemistry Exam Study Sheet

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JV SALAZAR

Chemistry Exam Study Sheet Ch. 44.1

Ionic Compound : a compound composed of oppositely charged ions andthe electrons are transferred

i.e. Binary Ionic Compound : Metal and non-metalIon : a charged particle formed from the loss or gain of one or more electrons

Cation = Positive ion // +Anion = Negative ion // -

Valence Electron : an electron in the outermost occupied energy levelMultivalent Metal : Metals that can form different ions, depending on thechemical reaction they undergo (i.e. copper can form ions with a 1+ or 2+charge)

Old naming system : -ic = highest charge/ -ous = lowest chargeNew Naming System : Roman numerals after multivalent metal // ie.Copper (II) or Copper(I)

Polyatomic Ion : an ion that is composed of more than one atom; groups of atoms that tend to stay together and carry and overall ionic charge

Ternary Compound : a compound composed of three different elements

Common Polyatomic Ions (Know the bolded ones):

1+ Charge 3- Charge 2- Charge 1- Charge

Ammonium,NH 4 +

Phosphate,PO 4 3-

Phosphite,PO 3 3-

Carbonate,CO 3 2-

Sulfate,SO 4 2-

Sulfite, SO 3 2-

Peroxide,O 2 2-

Bicarbonate(HydrogenCarbonate),HCO 3 -

Hydroxide, OH -

Nitrate, NO 3 -

Nitrite, NO 2 -

Chlorate, ClO 3 -

4.2Molecular/Covalent Compound : a compound formed when atoms of twoor more different elements share electrons

Molecule : a neutral particle composed of two or more atoms joined togetherby covalent bonds

Binary Molecular Compound : a compound that is composed of two non-metals joined by one or more covalent bonds

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Remember diatomic molecules : HONC FBI or HONC l FB rI DiphosphorusPentasulphide = P 2S 5

Note : Prefix is not needed for first atom if its only 1 // i.e. CarbonDioxide, not Monocarbon Dioxide

Molecule Prefixes

Mono- Di- Tri- Tetra- Penta-

Hexa- Hepta-

Octa- Nona- Deca-

1 2 3 4 5 6 7 8 9 10

4.3Law of Conservation of Mass : In a chemical reaction, the total mass of theproducts is always the same as the total mass of the reactants water

Skeleton Equation : Uses unbalanced chemical formulasH2 + O 2 -> H 2O

Balanced Chemical Equation : Uses balanced chemical formulas

2H 2 + O 2 -> 2H 2ORemember States : (s), ( l), (g), (aq) -> solid, liquid, gas, aqueous solution

Practical Uses of the Conservation of Mass :Sometimes a chemical spill is cleaned up by adding another chemicalwhich may also be toxic, so it is important to find out the exact amountof reactant needed so that no toxic chemical remains.

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Also, industrial chemistry utilizes this to minimize wastedchemicals/reactants, which can save them large amounts of money if they have use a lot of chemicals. Also, wasted chemicals can beharmful to the environment.

Chemistry Exam Study Sheet - Ch. 55.1

Evidence of Chemical Change: Formation of a gas Formation of a precipitate Change in colour/odour Production of light and heat Change is difficult to reverse

Precipitate : an insoluble solid formed in a chemical reaction.Classifying Chemical Reactions

Synthesis Reaction : a chemical reaction in which two or more reactantscombine to produce a new product

A + B -> AB // ie. 2H 2 + O2 -> 2H 2O (reaction used to propel spaceshuttle)

Decomposition Reaction : a chemical reaction in which a compound breaksdown (decomposes) into two or more simpler compounds or elements

AB -> A + B // ie. 2H2O -> 2H2 + O2 (reaction used as hydrogen fuel

source/electrolysis)Single Displacement Reaction : a chemical reaction in which one elementtakes the place of another element in a compound

A + BC -> AC + B (A is a metal) // ie. Zn + 2HCl -> ZnCl 2 + H 2A + BC -> BA + C (A is a non-metal) // F 2 + 2NaI -> I 2 + 2NaF

Double Displacement Reaction : a chemical reaction in which the positiveions of two different compounds exchange places, resulting in the formationof two new compounds- one of which may be a precipitate

AB + DC -> AD + CB // 2AgNO 3 + K 2CrO 4 -> Ag 2CrO + 2KNO 3

Combustion : Hydrocarbon + Oxygen (O 2) = Water (H 2O) + Carbon Dioxide(CO 2)

5.3This ch. shows examples of the use of chemical reactions in environmentalissues

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Car exhaust sometimes doesnt fully combust and creates carbon monoxideand carbon soot.

Catalyst : a substance that increases the rate of a reaction and isregenerated at the end of the reaction

Catalytic converters in cars can change unburned gasoline intoCO 2(g) and H 2O (g) .

Car exhaust also creates nitrogen oxides (NO (g) and NO 2(g) ) which cancontribute to smog and the formation of ground level ozone (O 3(g) ).

This is the only example from the book I put.

Chemistry Exam Study Sheet Ch. 66.1

Acid : a compound that produces hydrogen ions, H + (aq) , when dissolved inwater

Forming Hydrogen Ions in Water : Acid dissolves in water and reacts withwater to form hydrogen and - insert anion here - ions (ionization)

e.g. Hydrogen chloride, when dissolved in water, reacts with the waterto form ions, where the hydrogen ions and chlorine ions separate in thesolutionHCl (aq) -> H -(aq) + Cl -(aq)

Binary Acid : an acid composed of hydrogen and a non-metalNaming Binary Acids :

Classically :Hydro- + non-metal root + -ic // e.g. Hydrochloric Acid

Hydrochloric Acid is naturally found in stomach acid IUPAC Modern Naming :

Aqueous + Hydrogen + non-metal root + -ide // e.g. AqueousHydrogen Chloride

It also is used in processing plastics and metals

Oxoacid : an acid composed of hydrogen, oxygen, and another element orpolyatomic ion

Naming Oxoacids : I made it look complicated but it really isnt lol

Anions that end in -ate :Classically :

Replace -ate with -ic + acid // e.g. Sulfuric AcidH2SO 4(aq)

Sulfuric Acid is commonly used in most car batteriesIUPAC Modern Naming:

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Aqueous + Hydrogen + Anion // e.g. Aqueous HydrogenSulfate

Anions that end in -ite :

Classically:

Replace -ite with -ous + acid // e.g. Sulfurous AcidH2SO 3(aq)

Sulfurous Acid is commonly used in disinfecting and bleaching

IUPAC Modern Naming:

Aqueous + Hydrogen + Anion // e.g. Aqueous HydrogenSulfite

Base : a compound that forms hydroxide ions, OH -(aq) , when dissolved in

waterForming Hydroxide Ions in Water : Base dissolves in water to formhydroxide and -insert cation here- (dissociation)

e.g. Sodium hydroxide, when dissolved in water, reacts with the waterto form ions, where the sodium ions and hydroxide ions separate in thesolutionNaOH (aq) > Na + (aq) + OH -(aq)

Naming Bases : Use ionic compound naming rulese.g. NaOH -> sodium hydroxide

Used, sometimes in conjunction with Cl 2 and H 2 (e.g. purifying drinking water), to make paper, glass, and soap

6.2pH scale : a numeric scale ranging from 0 to 14 that is used to classifyaqueous solutions as acidic, basic, or neutral

pH : the measure of the concentration of H + ions in solutions

Acidic Solutions : pH < 7 Greater number of hydrogen ions than hydroxide ions in solution

e.g. Lemons pH 2, hydrochloric acid (gastric fluids in stomach) pH between 1 and 2, milk pH 6

Basic Solutions : pH > 7 Greater number of hydroxide ions than hydrogen ions in solution

e.g. Oven cleaner pH 13, eggs pH 8

Neutral Solutions : pH = 7

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Same number of hydrogen ions and hydroxide ions in solution

e.g. Pure water, sodium chloride, sugar

pH is a logarithmic scale, meaning that one unit on the scale is equivalent toa tenfold change in concentration -> pH 3 is 10x more acidic as pH 4 // pH 10is 1000x less basic than pH 13

pH = -log 10 [H + ]

Exponential Form : b y = x (e.g. 10 3 = 1000)Logarithmic Form : log bx = y (e.g. log 10 1000 = 3 // In other words, 10 to thepower of x is 1000, and x = 3)

To find H + concentration or pH from :H+ = 10 -pH

pH = -log 10 [H + ] e.g. -> [H + ] = 0.1 mol/L

pH = -log 10 [0.1] = 1

Indicator : a chemical that changes colour as the concentrations of H + or OH -changes

i.e. red/blue litmus paper, pH meter, phenolphthalein, cabbageindicator, universal indicator (changes from red to blue for acid tobase), etc.

Acid, Neutral, Base Comparison Chart

Acid Neutral Base

sour produces H + ions

in solution pH < 7 red litmus colourless

phenolphthalein corrosive conducts

electricity most solutions are

clear inappearance

do not produce H +

or OH-

ion insolution pH = 7 does not change

colour withcabbage indicator

will not conductelectricity

bitter slippery feel produces OH - ions

in solution pH > 7 blue litmus pink

phenolphthalein conducts

electricity most solutions are

clear inappearance

6.3

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Neutralization : the reaction of an acid and a base to produce a salt andwater

e.g. HCl (aq) + NaOH (aq) -> H2O (l) + NaCl (aq)Salt : ionic compounds that result in the neutralization of an acid and abase // any ionic compound that is neither an acid or a base

Note: Salts are usually is soluble in water and dont form precipitates

Practical Application of Neutralizations :

Antacids : to calm an over acidic stomach/heartburnTo Neutralize Acid Spills : H 2SO 4(aq) + Ca(OH) 2(aq) -> CaSo 4(aq) +

2H 2O( l)

Acid Precipitation : Fumes from a cars engine create nitrogen oxides(NO X), which react with water to form acid

e.g. NO 2(g) + H 2 O( l) -> HNO 3(aq)

Also, sulphur oxides from industrial processes can cause acid precipitation inthe form of sulphuric acid. // Scrubbers on stop of smoke stacks preventsthis; turns SO 2(g) into a solid which is then discarded

Acid precipitation can change water pH and cause aquatic life to die anddisrupt the food chain.

Liming : the application of basic materials, typically lime-based (usuallycalcium carbonate), to renew acidified lakes and regions // liming can renewacidified lakes by making them more neutral Again, in this ch. there are moreenvironmental examples but Im not gonna put them on

MISCELLANEOUS

Atomic Particles# of electrons = # of protons in nucleus // # of neutrons can varyAtoms masses are measure in atomic mass units or u . Mass number isan average of

Isotope : atoms of the same element with different # of neutrons // 2+isotopes are possible

Chemicals and Chemical ChangesPure substance : made of identical particles // compounds (can be brokendown) &

elements (cant be broken down)

Mixture : made up of different types of particles // mechanical mixtures (twovisible components) & solutions (only one visible element)

Physical Property : characteristics of a substance

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Chemical Property : characteristics of what happens when a substancechanges into a new substance

Types of Diagrams

Bohr-Rutherford Diagrams : # of protons and neutrons ina circle with lines beside it indicating the # of electrons ineach electron shell

e.g. Chlorine ->

Bohr Diagram : same as Bohr-Rutherford except the element symbol is inthe circle instead of the # of protons and # of neutrons

Lewis Structures : shows valence electrons as dots around theelements symbol Remember : [Li] + [F] - -> LiF

e.g. Chlorine ->(Remember that dots go around the negative one in brackets )

Period Table ReferencesAlkali Metals: 1 st column

Note: Hydrogen is its own group, NOT part of the Alkali Metals

Alkaline Earth Metals : 2 nd columnHalogens : 2 nd last/17 th column

Noble Gases : last/18 th columnColumns : can also be referred to as groups or families // they also show howmany valence electrons in the outer shell

Atomic Number : Number at the top left corner of the element box; showshow many electrons/protons the element has

Mass Number : Subtract atomic numbers from this to find the # of neutrons

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