Chemistry Review 2022 PDF

Chemistry Review  WHMIS Hazardous Household Product Symbols Section 1 - SDS The Theory Physical Properties vs Chemical properties Physical Change vs. Chemical Change Classification of Matter Early Ideas of Matter  h...

Chemistry Review  WHMIS Hazardous Household Product Symbols Section 1 - SDS The Theory Physical Properties vs Chemical properties Physical Change vs. Chemical Change Classification of Matter Early Ideas of Matter  http://provincialcouncils.ca/whmisgame/game.html WHMIS SYMBOLS Hazardous Household Product Symbols  A Safety Data Sheet (SDS) is a document with detailed information about a SDS chemical, including hazards, first aid measures, storage, physical and chemical properties, etc  Physical properties – describe the physical appearance and composition of a substance Physical Properties vs. What are some examples? Chemical Properties Chemical properties - describe the reactivity of a substance What are some examples?  Physical properties – describe the physical appearance and composition of a substance Physical Melting point, boiling point, density, solubility, color Properties vs. Chemical Chemical properties - describe the reactivity Properties of a substance Ability to burn, reactivity with acid, reactivity with water  A student obtains 4 unknown chemicals from her science teacher for their lab experiment. During the experiment, the student obtains the following data: Substance State of Melting Reaction to Color Conductivity matter point water litmus paper turns A liquid No evidence red Very of reaction conductive B solid dissolves Stays the Not same conductive C solid Explodes and Stays the Not ignites same conductive D solid dissolves Stays the Very same conductive From the list, determine all chemical properties of the substances 1. State of Matter 3. Reaction to water 2. Boiling point 4. Color litmus paper turns 5. Conductivity  Physical change – a substance appears different, but is still made up of the same atoms Physical Change vs. What are the 2 pieces of evidence for physical change? Chemical Chemical change – a substance has changed Change its chemical makeup into something new. It has gone through a chemical reaction What are the 5 pieces of evidence for chemical change?  Physical change - Change of state (s, l, g) - Dissolving (change of state to aq) Physical Change vs. Chemical Chemical change Change -change in color -change in odour -formation of precipitate (solid) - Formation of gas (bubbles) - Emits energy (heat/light) Physical or Chemical Change?  Use the following terms to make a flowchart that would help you classify matter: Matter Mixture Homogeneous mixture Heterogeneous mixture Element Classification Colloid of Matter Suspension Compound Mechanical mixture Solution Pure substance Classification of Matter  Scientist Model Name Model Description De Broglie and Solar System Model Atoms are like small Matching Schrodinger spheres - These are NOT in order! Bohr Quantum Mechanical The atom has a Model positively charged - Match the scientist nucleus with the model name and Dalton Raisin Bun Model Electrons exist in an description “electron cloud”, in a possible region - put them in order JJ Thompson Rutherford Model Electrons surround the from earliest to nucleus in fixed energy latest idea levels Rutherford Billiard Ball Model Electrons are embedded in a positively charged sphere  Scientist Model Name Model Description Dalton Billiard Ball Model Atoms are like small spheres Early Ideas of JJ Thompson Raisin Bun Model Electrons are embedded in a Matter positively charged sphere Matching Rutherford Rutherford Model The atom has a ANSWERS positively charged nucleus Bohr Solar System Model Electrons surround the nucleus in fixed energy levels De Broglie and Quantum Mechanical Electrons exist in an Schrodinger Model “electron cloud”, in a possible region Review Time Complete Question 1 in your Review Package Choose a study method to help you with the “theory” in this section  Periodic Table Section 2 – Using our Structure and Subatomic Particles Periodic Table Formation of Ions  On the periodic table, label the following: Periods Groups Alkaline earth metals Halogens Alkali metals Periodic Table Noble gases Transition metals Metals Nonmetals Metalloids Staircase line Periodic Table  1) Determine the period that the following elements are in: Sulfur, Lead, Calcium, Iridium Periodic Table 2) Determine the group that the following NR Questions elements are in (if it is group 11-18, just use the second digit. Example: if something is in group 18 I would just write an 8): Vanadium, barium, argon, copper  Subatomic Where is Charge Does it’s symbol How to Particle it found? mass find it “count” using your towards p. table mass of (atom) the atom? Structure and proton nucleus + yes p+ Atomic Subatomic number Particles electron outside - no e- Atomic of number nucleus neutron nucleus 0 yes n0 Mass – atomic number  Draw the Bohr Model and Energy Level diagram for: Bohr Models sodium, oxygen, phosphorous In a Bohr model, energy levels fill up before a new energy level is created. Electrons fill their own orbitals before doubling up the first energy level can hold 2 electrons, the second can hold 8 electrons The third can hold 8 electrons  Ion – an electrically charged atom or group of atoms Cation – positively charged ion, positively charged because it lost an electron (sodium ion 🡪 Na+) Anion – negatively charged ion, negatively charged because it gained an electron (oxide O2-) Formation of Ions Why would a neutral atom form an ion?  Atom Ion Isotope Are protons and electrons equal? Is there a charge? How do you calculate neutrons? How do you calculate mass? Example:  Atoms want to become stable by having a full outer shell (valence). They do so by gaining or losing elections (to form ionic compounds). Ionization Ex. sodium atom 🡪 sodium ion Atom or Ion Overall Number Number of Symbol Number of Electrons Lost Name Charge of Electrons or Gained Protons Oxygen atom O Oxide ion 10 O2- Potassium Ion 19 12 10 Practice Review Time Complete Questions 2, 3 in your review package  Ionic and Molecular Compounds Multivalent Elements Polyatomic Ions Section 3 - Properties of Ionic and Molecular Compounds Compounds Solubility Table Acids and Bases  A metal and a Non-metal Formed from ionic bonds – give or take electrons Conduct electricity when in solutions Example Sodium Chloride To Name: To Write Formulas Ionic 1) Name the cation 1) Balance charges! Compounds first 2) Name the anion 2) In nature, ionic second - change compounds are the ending to “-ide” solid  1) Write the formula for calcium nitride 2) Write the formula for magnesium chloride Practice 3) Name AlCl3(s) 4) Name CaS(s)  Multivalent elements – have more than one possible charge – use roman numerals when writing the name, Ionic when writing the formula use the charge that makes the compound balanced Compounds Example: Iron (III) bromide -Things to Polyatomic ions – ions that are made of several watch for: non-metallic atoms joined together and behave like a single ion Example: phosphate PO43-  To Name: To Write Formulas 1) Name the cation first 1) Balance charges! 2) Name the anion second 2) In nature, ionic - change the ending to compounds are solid “-ide” 3) If roman numerals are 3) Use roman numerals if given, use that as the Ionic there is more than 1 charge Compounds possible charge 4) ONLY use brackets 4) Never change the name around a polyatomic if of a polyatomic there is more than 1 poly group  1) Write the formula for strontium nitrate 2) Write the formula for iron (ii) chloride Practice 3) Name Al2(SO4) 3 (s) 4) Name CuS (s)  Two or more non-metals bond together Form covalent bonds – share electrons Molecular Do not conduct electricity in solutions Compounds Example: water To Name: To Write Formulas 1) Write the name of the 1) Follow the prefixes first element 2) Can be solid, liquid, or 2) Name the second gas element with “-ide” at 3) Recognize some the end common names (water, 3) Add prefixes indicating methane, etc) number of atoms (mono, di, tri etc.) 1) No mono at front  Write the chemical formula for carbon monoxide Write the chemical formula for sulfur dioxide Practice Write the name of the compound that has the formula PCl5(s) Write the name of the compound that has the formula N2O3(g) Molecular Compounds - Diatomic/Polyatomic elements – atoms that tend to exist grouped together Things to H2 N2 O2 F2 Cl2 Br2 I2 P4 S 8 watch for:  Property Ionic Molecular Melting Point High melting point Low Melting Point Properties of Conductivity Solutions conduct Do not conduct electricity Ionic and electricity Molecular Structure Crystal Lattice structure No crystal shape Compounds State of Matter Solid at room Can be solid, liquid or gas at room temperature temperature Solubility Some dissolve, some Some dissolve, some don’t don’t  pH less than 7 Turns blue litmus red and red litmus stays red Acids Taste sour In chemical formulas H tends to appear on the left or –COOH on the right Conducts electricity in solution  To Name: To Write Formulas 1) Write its “ionic” name 1) Use ionic rules first (balancing!) 2) State should be aqueous 2) Use the acid naming Acids chart to convert to its 3) Starts with H or ends acid name with COOH Example: Write the acid name of HNO2 (aq) Write the formula for sulfuric acid  pH greater than 7 Turns red litmus blue and blue litmus blue Taste bitter Bases When naming they - tend to have an OH in their formula Conducts electricity in solution  To Name: To Write Formulas 1) Write its “ionic” name 1) Use ionic rules (balancing!) 2) It will have the hydroxide ion (OH-) so 2) State should be aqueous Bases its ending will likely be 3) Should contain the “hydroxide) hydroxide ion (OH-) Example: Write the formula for calcium hydroxide Name the following base: KOH(aq)  A student obtains 4 unknown chemicals from her science teacher for their lab experiment. During the experiment, the student obtains the following data: Substance State of Melting Reaction to Color litmus Conductivit matter point water paper turns y A liquid No evidence red Very of reaction conductive B solid dissolves Stays the Not same conductive C solid Explodes and Stays the Not ignites same conductive D solid dissolves Stays the Very same conductive In the order A, B, C, D the substances are __, __, __, __ Review Time Complete Questions 4, 5 in your review package Section 4 – All Chemical Reactions About Writing Chemical Reactions Reactions Types of Chemical Reactions  A substance or substances react to create a different substance or substances Always involve the production of new Chemical substances with their own physical and chemical properties Reactions Remember the 5 pieces of evidence of chemical change – this indicates a chemical reaction has taken place!  Exothermic – Chemical release energy Reactions Endothermic – absorb energy Parts of a Chemical Equation  We balance chemical equations to obey the Law of Conservation of Mass – mass is neither created nor destroyed during a chemical reaction. Balancing That is, the amount of stuff reacting (reactants) must equal the Chemical amount of stuff produced (products). Equations Coefficients are used to make the number of each type of atom equal on the reactant and produce side. Example: Decomposition of Water Balance the following equations a) NH3 🡪 N2 + H2 b) C3H8 + O2 🡪 CO2 + H2O c) Ca(OH)2 + KCl 🡪 KOH + CaCl2 Solubility Table NaOH K2CO3  Write and Balance the following equations a) Aluminum metal reacts with oxygen gas to produce aluminum oxide b) Magnesium metal reacts with hydrochloric acid to produce magnesium chloride and hydrogen gas 5 Types of Chemical Reactions In order to predict the products of a chemical reaction, we must use the five reaction types: 1. Formation/Synthesis element + element 🡪 compound Ex. N2(g) + 3 H2(g) 🡪 2 NH3(g) Predicting 2. Decomposition Products compound 🡪 element + element Ex. 2 H2O(l) 🡪 2 H2(g) + O2(g) 3. Single Replacement element + compound 🡪 element + compound Ex. Cu(s) + 2 AgNO3(aq) 🡪 2 Ag(s) + Cu(NO3)2(aq) 4. Double Replacement compound + compound 🡪 compound + compound Ex. Na2S(aq) + 2 HCl(aq) 🡪 2 NaCl(aq) + H2S(aq) 5. Hydrocarbon Combustion CxHy + O2 🡪 CO2 + H2O Ex. CH4(g) + 2 O2(g) 🡪 CO2(g) + 2 H2O(g) Predict the products and balance the following reactions: a) Na(s) + Br2(l) b) solid zinc reacts with hydrochloric acid c) ethane (C2H6(g)) burns in the presence of oxygen gas Review Time Complete Questions 6, 7 in your review package  Molar mass Section 5 – Moles Some Math… Mass  Mole – quantity used to measure elements and compounds Molar Mass – the mass of one mole of a substance (found on periodic table) Mole m=nxM m is the mass in grams n is the number of moles M is the molar mass  To determine the molar mass of a compound (or polyatomic element), add up values of each element’s molar mass. Ex. Calculate the molar mass of methane (CH4). C – 1 x 12.01 g/mol = 12.01 H – 4 x 1.01 g/mol = 4.04 Molar mass 16.05 g/mol Calculate the molar mass: a) oxygen gas b) MgCl2 c) Ca(NO3)2  What is the molar mass of methanol (CH3OH)? How many moles of silicon are in a 56.18 g Practice sample? What is the mass of 10.0 mol of calcium fluoride?  Calculate the mass of each substance: a) 5.0 mol of aluminum b) 0.275 mol of sodium nitrate Practice Determine the moles of each substance: a) 25.0 g of neon b) 5.0 kg of sulfur dioxide Review Time Complete Question 8 in your review package