Download semester two final review key units 5 and 6 only

FUNDAMENTALS
Name: ___KEY________________ Period: ____
SEMESTER TWO FINAL REVIEW SHEET
Below are the types of questions you can expect to see on your final for Fundamentals. The topics are
arranged in the order that we learned the concepts. If there are problems you do not understand, or need
additional practice on, please revisit that unit’s review sheet from my website.
In addition to a periodic table, scientific calculator and ion chart, you may also use this HANDWRITTEN
review sheet. You may choose to answer directly on this sheet or on a separate sheet of paper and attach it.
UNIT 5: CHEMICAL REACTIONS
BALANCING AND TYPES OF REACTIONS
1. Definitions to know: chemical reaction, conservation of mass, endothermic, exothermic, subscript,
coefficient, reactants, and products.
2. Calculate the number of atoms of each element shown in each of the following:
a. Na2SO4 7
c. Cu(NO3)2
9
b. 2 MgCl2
6
d. Al2(CO3)3 14
3. Balance each of the following equations:
a. ____ Na2CO3 + _ 2___ HCl  __ 2__ NaCl + ____ H2O + ___ CO2
b. ____ Fe + __ 2__ HCl  ____ FeCl2 + ____ H2
c. ____ F2 + _ 2___ KCl  __ 2__ KF + ____ Cl2
4. What is an exothermic reaction? How could you tell if a reaction was exothermic? Reaction where
energy is released and heat is released to the surroundings; gets warmer
5. What is an endothermic reaction? How could you tell if a reaction was endothermic? Reaction where
energy is absorbed and heat is absorbed from the surroundings; gets cold
6. Name four factors that can affect the rate of a chemical reaction? Be able to explain each one. As an
example: What would happen to the rate of reaction if: a catalyst was added, a sugar cube was
crushed or 6M HCl was used instead of 2M HCl? Concentration, surface area, temperature, catalyst
7. What are the seven indicators of a chemical reaction occurred. Explosion, temperature change, color
change, new odor produced, light produced, gas forms, new precipitate formed
8. Identify the types of reactions shown in each of the following equations:
a. CaO + H2O  Ca(OH)2 synthesis
c. Mg(NO3)2 + KCl  MgCl2 + KNO double rep
b. 2 Al + NiBr2  AlBr3 + Ni single rep.
d. PbO2  Pb + O2 decomp
9. Balance the following reactions with polyatomic ions and state which type of reaction it is.
a. ___ AlCl3 + _3__ LiOH  ___ Al(OH)3 + _3__LiCl
b. ___ Ba(CN)2 + ___ H2SO4  ___ BaSO4 + _2__HCN
CARBON BASED MOLECULES (Macromolecules)
1. Definitions to know: monomer, polymer, biochemistry, hydrocarbon, carbohydrate, protein, lipids, and
nucleic acids.
Monomer: a molecule of any class of compounds, mostly organic that can react with other molecules
that can form larger molecules
Polymer: any of a class of natural or synthetic substances composed of very large molecules, called
macromolecules, that are multiples of simpler chemical units called monomers.
Biochemistry: sometimes called biological chemistry, is the study of chemical processes within and
relating to living organisms
Hydrocarbon: are the simplest organic compounds. Containing only carbon and hydrogen, they can
be straight-chain, branched chain or cyclic
Carbohydrate: is a biological molecule consisting of carbon (C), hydrogen (H) and oxygen (O) atoms,
usually with a hydrogen : oxygen atom ratio of 2:1 (as in water)
Protein: are large biological molecules, or macromolecules, consisting of one or more long chains
of amino acid residues.
Lipids: one of the four macromolecules that is made up of fatty acids
Nucleic acid: large biomolecules, essential for all known forms of life, which include DNA and RNA are
made from monomers known as nucleotides
2. What is organic chemistry? The study of carbon based molecules
3. What properties of carbon make it the building block of life? Has four valence electrons and the ability
to bond with many other atoms to form complex molecules
4. What are three examples of pure carbon? Diamond, graphite, charcoal
5. How many valence electrons does carbon have and what would the Lewis Dot Diagram look like? four
6. Be able to fill in a chart like the one shown below:
MACROMOLECULE
FOOD EXAMPLE
MONOMER
CARBOHYDRATES
Bread, pasta, starches
Monosaccharides (sugar)
Proteins
Eggs, fish, meat
Amino acids
NUCLEIC ACIDS
N/A
NUCLEOTIDES
Lipids
BUTTER, OIL
Fatty acids
FUNCTION IN BODY
Energy storage
BUILD MUSCLE
DNA/RNA
Insulation for organs,
storage
ACIDS AND BASES
1. Definitions: acid, base, neutral, amphoteric, and pH scale.
Acids: ionic compounds (a compound with a positive or negative charge) that break apart in water to
form a hydrogen ion (H+)
Bases: ionic compounds that break apart to form a negatively charged hydroxide ion (OH-) in water
Neutral: A solution that has a pH of 7. It is neither acidic nor basic
Amphoteric: a substance that can act as an acid or base under various conditions
pH scale: a measure of the strength of acidity or basicity based on the number of H+ ions in a solution
2. Know the chemical formulas for the five common acids (ex. Nitric, phosphoric, etc.)
Acetic acid CH3COOH, Hydrochloric acid HCl, Nitric acid HNO3, Sulfuric acid H2SO4
Phosphoric acid H3PO4
3. What are three characteristics of acids? What are three characteristics of bases?
Acids are sour, corrosive and typically plot in the red/orange range
Bases are chalky, bitter and typically plot in the blue/purple range
4. What is the pH for a substance that is neutral? What is an example of a neutral substance? 7, water
5. Know the definition of Bronsted-Lowry acids and know how it is different from an Arrhenius acid.
Bronsted-Lowry: Acid- proton donor, Base- proton acceptor
Arrhenius: Acids release H+ ions and bases release OH6. Identify the acid, the base, the conjugate acid and the conjugate base in the reaction:
NH3 (g) + HOH (l) ⇄ NH4+(aq) + OH-(aq)
Base
Acid
C.A.
C.B.
7. Identify the acid, the base, the conjugate acid and the conjugate base in the reaction:
HCO3 -(aq) + HOH (l) ⇄
CO3 2-(aq) + H3O+ (aq)
Acid
Base
C.B.
C.A.
8. Rank these substances from most acidic to most basic: milk of magnesia, water, vinegar, soda, blood,
hydrochloric acid and lye. HCl, vinegar, soda, water, blood, milk of magnesia, lye
UNIT 6: MOLE CONVERSIONS, MOLE RATIOS, EMPIRICAL/MOLECULAR FORMULA
1. Definitions: mole, Avogadro’s number, molar mass, molar volume, molecules (atoms/particles),
empirical formula, molecular formula, and percent composition.
Mole: The amount of elementary particles that are in exactly 12 g of Carbon. A mole is Avogadro’s
number of particles; 1Mole = 6.02 × 1023 particles = gram formula mass of an element/compound
Avogadro’s Number: 6.02 × 1023 particles of any substance
Molar Mass: The total mass (in g/M) of all substances in the compound or the element
Molar Volume: at STP, one mole of any gas is equal to 22.4L
Molecules: smallest physical unit of an element orcompound, consisting of one or more like atoms in an
element and twoor more different atoms in a compound.
Empirical formula a chemical formula showing the simplest ratio of elements in a compound rather than
the total number of atoms in the molecule
Molecular formula: a formula giving the number of atoms of each of the elements present in one
molecule of a specific compound
Percent composition: the percent of the total mass of the compound that is due to that component
FORMULA MASS, MOLAR MASSES, MOLE CONVERSIONS
1. Calculate the formula mass in a.m.u. of the following:
a. CaSO4 136.14 amu
b. RbNO3 147.47 amu
c. H2O 18.02 amu
d. NaCl 58.5 amu
2. Calculate the gram formula mass (molar mass in grams) of the following:
a. Li2CO3 73.89 amu
c. CF4 88.00 amu
b. AlPO4 121.95 amu
d. Mg(OH)2 120.37 amu
3. Make the following conversions.
a. What is the number of moles of CaS in 250 grams of the compound? 3.5 moles
b. How many moles is 18.06×1023 molecules of SO2? 3 moles
c. How many molecules of CO2 are in .75 moles? 4.515 × 1023 molecules
d. How many moles are in 800 g of HCl? 21.94 moles
e. How many moles are in 50 g Fe2O3? 0.3125 moles
f. How many moles are in 44.8 L of CO2 gas at S.T.P.? 2 moles
g. What is the volume of 5.6 moles of Cl2 gas at S.T.P.? 125.44 liters
h. How many ions of Al=3 are present in one mole of AlCl3? 6.02 × 1023
PERCENT COMPOSITION, EMPIRICAL, AND MOLECULAR FORMULAS
1. What is the percentage composition of all elements in the compound calcium carbonate, Na2CO3?
43.38% Na
11.33% C
45.29% O
2. What is the percentage composition of oxygen in strontium nitrate, Sr(NO3)2?
41.402% Sr
13.237% N
45.361% O
3. Calculate the percent composition of each element in C6H12O6.
40.001% C
6.714% H
53.285% O
4. Calculate the percent composition of oxygen in N2O. 36.352%
5. How are empirical and molecular formula related? The molecular mass is a whole number multiple of
the empirical formula mass. The empirical formula is always in lowest or simplest terms
6. Determine the empirical formulas for each of the following molecular formulas.
a. C10H20….. CH2
d. C6H12…… CH2
b. H2O2…… HO
e. Na2C2O4... NaCO2
c. Hg2Cl4….. HgCl2
7. The empirical formula for ethylene is CH. The empirical formula mass is 13 g/mole. Find the molecular
formula if the molecular mass is 78 g/mol. C6H6
8. A compound has an empirical formula of OCNCl and an empirical mass that is equal to 77.5 grams. The
molecular mass is 232.41 grams. What is the molecular formula? O3C3N3Cl3
MOLE RATIOS
1. Given this equation: N2 + 3 H2 ---> 2 NH3, write the following molar ratios:
a. N2 / H2 1 / 3
b. N2 / NH3 1 / 2
c. H2 / NH3 3 / 2
2. Answer the following questions for this UNBALANCED equation: ___ H2 + ___O2 --> ___ H2O
a. Balance the equation: _2__ H2 + ___O2 --> _2__ H2O
b. What is the H2 / H2O molar ratio? 1 / 1
c. What is the O2 / H2O molar ratio? 1 / 2