Chapters 1, 2, and 3. Chemistry is the study of matter and how it changes. Elements: Atoms: ...
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Transcript of Chapters 1, 2, and 3. Chemistry is the study of matter and how it changes. Elements: Atoms: ...
UNIT 1Chapters 1, 2, and 3
What Is Chemistry?
Chemistry is the study of matter and how it changes.
Elements:
Atoms:
Molecules and Compounds:
States of Matter
Solid:
Liquid:
Gas:
Matter
Pure Substnaces
Pure substance:
Mixture:
Heterogeneous:
Homogeneous:
Properties of Matter
Physical Properties:
Chemical Properties:
Intensive Properties:
Extensive Properties:
Atomic Theory
Subatomic Particles:
Electrostatic Forces:
Radioactivity
The Nuclear Atom
Nucleus:
Electronic Charge:
Atomic Mass:
Atomic Size:
Isotopes
Isotope:
Average Atomic Mass:
Naturally occurring chlorine is 75.78 % 35Cl, which has an atomic mass of 34.969 amu, and 24.22 % 37Cl, which has an atomicmass of 36.966 amu. Calculate the average atomic mass of chlorine.
The Periodic Table
How it’s arranged:
Law of Definite Proportions
The Law of Multiple Proportions
Ions and Ionic Compounds
Ion:
Cation:
Anion:
Group 1: H+, Li+, Na+
Group 2: Be2+, Mg2+, Ca2+
Group 15: N3-, P3-, As3-
Group 16: O2-, S2-, Se2-
Group 17: F-, Cl-, Br-
Transition elements can usually have more than one charge. Example Fe2+ and Fe3+
Common Ions and their charges
Most transition metals can have a few different charges.
Example: Fe2+, Fe3+
Fe2O3
FeO
Transition Metal Ions
Ammonium: NH4+
Nitrite: NO2-
Nitrate: NO3-
Hydroxide: OH-
Hypochlorite: ClO-
Polyatomic Ions
Chlorite: ClO2-
Chlorate: ClO3-
Perchlorate: ClO4-
Carbonate: CO32-
Sulfite: SO32-
Sulfate: SO42-
Peroxide: O22-
Phosphate: PO43-
Naming Ionic Compounds
Practice
NH4Cl
Fe(NO3)3
TiBr3
Pb(SO4)2
Chromium (VI) Phosphate
Tin (II) Nitrate
Cobalt (III) Oxide
Chromium (III) Hydroxide
Barium Carbonate
Aluminum Hydroxide
Copper (I) Sulfide
Lead (II) Phosphate
Zinc (II) Iodide
Chromium (III) Sulfite
NH4Br
NaClO3
Fe2S3
AgNO3
CuF2
Ni(ClO)3
Ru3(PO4)4
Naming Molecular Compounds
Practice
The Mole
Molar Mass
Percent Mass
Hydrates
Empirical And Molecular Formula
Chemical Reactions
Chemical Equations:
Stoichiometry
How many grams of water are produced in the combustion of 1.00 g of glucose?
C6H12O6(s) + 6 O2(g) 6 CO2(g) + 6 H2O(l)
Limiting Reactants
Consider the reaction that occurs in a fuel cell:
2 H2(g) + O2(g) 2 H2O(g)
Suppose the fuel cell is set up with 150 g of hydrogen and 1500 g of oxygen. How many grams of water can be formed?
Theoretical Yield and Percent Yield
Adipic acid (H2C6H8O4) is used to produce nylon. The acid is made commercially by a controlled reaction between cyclohexane (C6H12) and O2:
6 C6H12(l) + 5 O2(g) 2 H2C6H8O4(l) + 2 H2O(g)
a.) Assume that you carry out this reaction starting with 25.0 g of cyclohexane and that cyclohexane is the limiting reactant. What is the theoretical yeild of adipic acid?
b.) If you obtain 33.5 g of adipic acid from your reaction, what is the percent yeild?
Example AP Questions
1) Complete combustion of a sample of a hydrocarbon in excess oxygen produces equimolar quantities of carbon dioxide and water. Which of the following could be the molecular formula of the compound?
(A) C2H2
(B) C2H6
(C) C4H8
(D) C6H6
2. The mass percent of carbon in pure glucose, C6H12O6, is 40.0%. A chemist analyzes an impure sample of glucose and determines that the mass percent of carbon is 38.2 %. Which of the following impurities could account for the low mass percent of carbon in the sample?
(A) Water, H2O
(B) Ribose, C5H10O5
(C) Fructose, C6H12O6. An isomer of glucose
(D) Sucrose, C12H22O11
3. How many protons, neutrons, and electrons are in a 56
26Fe atom?Protons Neutrons Electrons
(A) 26 30 26(B) 26 56 26(C) 30 26 30(D) 56 26 26(E) 56 82 56
4) Atoms of Mg combine with atoms of F to from a compound. Atoms of which of the following elements combine with atoms of F in the same ratio?
(A) Li(B) Ba(C) Al(D) Cl(E) Ne
C3H8(g) + 5 O2(g) 3 CO3(g) + 4 H2O(l)
5) In the reaction represented above, what is the total number of moles of reactants consumed when 1.00 mole of CO2(g) is produced?
(A) 0.33 mol(B) 1.33 mol(C) 1.50 mol(D) 2.00 mol(E) 6.00 mol
LiHCO3(aq) + H2SO4(aq) Li2SO4(aq) + H2O(l) + CO2(g)
6) When the equation above is balanced and the coefficients are reduced to lowest whole-number terms, what is the coefficient of H2O
(A) 1(B) 2(C) 3(D) 4(E) 5
7) When a 3.22 g sample of an unknown hydrate of sodium sulfate, Na2SO4 * x H2O(s) is heated, H2O (molar mass 18) is driven off. The mass of the anhydrous Na2SO4(s) (molar mass 142 g) that remains is 1.42 g. The value of x in the hydrate is
(A) 0.013(B) 1.8(C) 6.0(D) 10.0(E) 20.0
8) What is the empirical formula of an oxide of chromium that is 48 percent oxygen by mass?
(A) CrO(B) CrO2
(C) CrO3
(D) Cr2O
(E) Cr2O3