Honors Chemistry Finals Review

Unit 1 – Chemistry BasicsVocab: Chemistry, matter, mass Scientific method, observation, hypothesis, theory, law Mixture, heterogeneous, homogeneous Substance, element, compound Physical property vs. change Chemical property vs. change Quantitative and qualitative observations Dependent/independent/control variables Solid, liquid, gas, vapor, aqueous solution – don’t forget the symbols that show up in balanced chemical equations Solute, solvent, solution Distillation Describe the parts of the scientific method How is a theory related to a law? What is the difference between a hypothesis and a theory?

(ALL POINTS ARE UNDER TAB) What are the 5 things that all good graphs should have? What is the difference between a substance and a mixture? How do you determine if a mixture is homogeneous or heterogeneous? What is the difference between an element and a compound? What are ways you can separate a mixture? What are ways you can separate a compound? Unit 2 – Electron structure and periodicityVocab: Atom, neutron, proton, electron, nucleus Atomic number and mass Isotope, average atomic mass

CHEMISTRY DAY ONE: UNIT 1 & 2

Valence electrons Bohr model Dalton’s atomic theory Quantum mechanics, electron configuration, noble gas electron configuration Pauli Exclusion Principle, Aufbau Principal, Hund’s Rule Atomic emission spectrum, electromagnetic radiation, photon Wavelength, frequency, speed of light Ground state, excited state Period, group Alkali metals, alkaline earth metals, halogens, noble gas, transition metals, inner transition metals Representative elements Metals, metalloids, non-metals Atomic and ionic radii Ionization energy, electronegativity

Defining the atom JJ Thompson’s model Dalton’s atomic theory What are his theories? Which one do we know not to be true? Rutherford’s contribution (what did he learn from gold foil?) Bohr’s model Quantum mechanic model s-orbital What shape is this orbital? How many electrons occupy this orbital?

CHEMISTRY DAY 2: UNIT 2

p- orbital What shape is this orbital? How many sub-orbitals are there? How many electrons occupy this orbital (and sub-orbital)? d-orbital How many electrons occupy this orbital? f- orbital How many electrons occupy this orbital? What happens when an electron is excited by a photon of energy? What is the relationship between wavelength, frequency and the speed of light? Are wavelength and frequency directly or inversely proportional? Write the electron configuration for: Mg Br Rn

What are the three rules for filling electron orbitals?  What order do you apply each rule? As you work across the periodic table for energy level n, what is the rule for filling the d- and f-orbital? What is a noble gas configuration? For Calcium: Chemical symbol: Atomic number: Atomic mass: # of protons: # of electrons: # of neutrons: Why do atoms have isotopes? How do you calculate the average mass for an atom?

CHEMISTRY DAY 3: UNIT 2

Boron has two naturally occurring isotopes: boron-10 (10.013 amu and 19.8%) and boron-11 (11.009amu and 80.2%).  Calculate the average atomic mass of boron. Where are the s-, p-, d-, and f- blocks on the periodic table? What blocks make up the representative elements? Looking at the periodic table: Know where the metals are located Know where the metalloids are located Know where the non-metals are located Atomic and ionic radii What is the trend: Across the period Down the group How do ionic and atomic radii compare? How does a cation compare? How does an anion compare? Ionization energy and Electronegativity What are the trends across the group What are the trends down the group

Unit 3 – Chemical names, formulas and reactionsVocab: Valence electrons Covalent bond Polar and non-polar covalent Single, double, triple bonds Diatomic molecules

CHEMISTRY DAY 4: UNIT 2 & 3

Octet rule Lewis dot diagram Ion, cation, anion, polyatomic ions Ionic and metallic bonds Molecules, formula units Reactant, product Activity series Single displacement (replacement) Double displacement (replacement) Synthesis (combination) Decomposition Combustion Complete and net ionic equations Soluble, insoluble, precipitate What are the valence electrons for each group of the representative elements?

How do you draw a Lewis Dot diagram What ionic charge is associated with each group of the representative elements? How do ionic bonds form? What are properties of ionic bonds? How do metallic bonds form? What are properties of metallic bonds? How do you name ionic bonds? How does the naming of transition metals differ from representative elements? What seven polyatomics do you need to memorize – what is their name, formula and ionic charge? What are the seven diatomic molecules you need to memorize?

CHEMISTRY DAY 5: UNIT 3

Why do covalent bonds form? What causes a polar bond? What are properties of covalent bonds? How do you name covalent bonds?What are the 10 prefixes you need to memorize? Define the law of conservation of matter How do you know if a reaction occurs (what table to do you refer too?)? What is a balanced chemical equation? Define a subscript: Define a coefficient: Balance the following equations: a.      N2 +       O2 -->      NO2b.       Al2O3 -->     Al +     O2c.        Mg  +     HNO3 -->     Mg(NO3)2 +     H2d.     Al(OH)3 +     H2SO4 -->     Al2(SO4)3 +   H2O

Balance the following combustion equation:CH4 +    O2 -->    CO2 +    H2OBalance the following synthesis equation:Mg   +    O2  -->    MgOBalance the following decomposition equation:FeO2  -->   Fe  +   O2Balance the following single displacement reactions:Al(OH)3  +    Ca  -->     Ca(OH)2 +     AlNaCl   +   F2   -->     NaF  +   Cl2Balance the following double displacement reaction:K2O  +   MgCl2  -->   MgO  +   KCl

CHEMISTRY DAY 6 : UNIT 3

What is a precipitate? Identify the type of reaction, predict the products, and balance the following equations: nitrogen gas + hydrogen gas --> calcium oxide --> the combustion of hexane (C6H14) --> zinc + hydrochloric acid (HCl) --> bromine + potassium iodide --> silver nitrate + sodium phosphide --> How does the state of matter of the reactants and products influence ionic equations? What type of reactions form precipitates? Write the complete and net ionic equations for the following reactions.  Make sure to label spectator ions and the precipitate. 2NaOH(aq) + CuCl2(aq) --> 2NaCl(aq) + Cu(OH)2(s) 2HI(aq) + Li2S(aq) --> H2S(g) + 2LiI(aq) Sulfuric acid reacts with aqueous potassium hydroxide -->

Unit 4 – Chemical StoichiometryVocab: Accuracy, precision Error, percent error Significant figures Scientific notation Conversion factors – dimensional analysis Mole, Avogadro’s number, Molar mass Percent composition Product, Reactant

CHEMISTRY DAY 7 : UNIT 3 & 4

Limiting reactant Yield – actual and theoretical Mass stoichiometry Mole ratio stoichiometry What is the SI units for mass and length Know how to convert metric units 50mg = ______g 0.034L = _____mL 38.0km = _____ m 3.06 x 10-5km = ______ mm How many seconds are in 1 year? How many significant figures do each have: 0.0003  8000000  203.050 Express the following in scientific notation 55000000000 = 0.0022 = 65200 =

How many atoms are in a mole? Convert atoms to moles 12.2x1024 atoms to  ______ mols Convert moles to atoms 2.5 moles to _______ atoms How do you calculate molar mass? What’s the mass the Ca(OH)2

CHEMISTRY DAY 8 : UNIT 4

What’s the mass of C2H4O2 How do you calculate the mass % for each element in a compound? What is the mass % of Fe in Fe2O3? What is the mass % of O in Fe2O3? How do you find the empirical formula from mass % composition info? How do calculate the molecular formula from empirical formula and molar mass data? What is a mole? What does Avogadro’s # tell you?  Find the molar mass for: a.  CaSO4 b.  H3PO4 c.  Al2(CO3)3 What is the mass in grams of 2.50 moles of oxygen gas? How many molecules of H2O are in 36 grams? How many grams of sugar, C12H22O11, are in 2.20 x 1023 molecules

How many oxygen atoms are in 32 grams of NaHCO3? Find the percent of copper and sulfur in Cu2S. How many moles of ammonia are made when 6 moles of hydrogen gas react with nitrogen gas? When magnesium and oxygen combine to make magnesium oxide, what mass in grams of magnesium oxide is produced from 2.00 moles of magnesium? What mass of aluminum is produced by the decomposition of 5.0 g of Al2O3? If 25.0 g of chlorine is reacted with 20.5 g of sodium, which reactant is the limiting reactant?  How much of the excess reactant is ‘leftover’? If the theoretical yield of a substance is 20.0 g and the actual yield is 15.0 g, what is the percent yield? When potassium chromate is added to a solution containing 0.500 g silver (I) nitrate, solid silver chromate is formed. What is the theoretical yield of silver (I) chromate? If 0.45 g of silver chromate is obtained, what was the % yield?

CHEMISTRY DAY 9 : UNIT 4

CHEMISTRY DAY 10: QUIZ AND REVIEW