Download presentation
Presentation is loading. Please wait.
1
Review of the Fundamentals
(strap on your seat belt)
2
Nomenclature Ionic MNm TmNm MXO MNm – Name the ions
Cations – no change Anions – end in –ide KCl MgBr2 CaS For fomulas make them electrically neutral by crisscrossing charges Barium oxide Sodium phosphide Aluminum fluoride
3
TmNm Roman numeral indicates charge Chromium (III) oxide Zinc iodide
Lead (II) sulfide Silver chloride Tin (II) oxide
4
Naming – have to calculate the charge of the Tm
FeCl2 FeCl3 CuO Co2O3
5
Binary Acids Hydro___________-ic acid HCl H2S H3P Hydrobromic acid
Hydroiodic acid
6
Ternary Compounds MXO or TmXO
Name metal name polyatomic ion KClO3 Na2SO4 Al(NO2)3 Crisscross charges to make electrically neutral Ammonium dichromate Calcium actetate Sodium carbonate Magnesium phosphate Potassium nitrite
7
Ternary Acids HXO (oxyacids)
-ate changes to –ic and add the word acid -ite changes to –ous and add the word acid HNO3 HNO2 H3N Perchloric acid Hypochlorous acid Bromous acid
8
Non-organic Covalent compounds NmNm
1st element sometimes gets a prefix (if subscript > 1) 2nd element always gets a prefix 2nd element always ends in –ide CO CO2 N2O NO2 Sulfur trioxide Diphosporus pentachloride
9
Notes on polyatomic ions
-ate vs ite Prefixes Bi- Hypo- Per- Elements in the same family bond the same way chlorate bromate
10
Some New Stuff Organic compounds (carbon “chains)
Organic compounds are defined by functional groups Some functional groups you will need to know for this class Acids (carboxylic acids) – C(=O)-OH Alcohols –OH Keytones – R1-C(=O)-R2 Aldehydes R-C(=O)-H Esters R1-C(=O)-O-R2
11
Hydrocarbons Alkanes CnH2n+2 Alkenes CnH2n Alkynes CnH2n-2
(saturated – all single bonds) Alkenes CnH2n (unsaturated- double bonds) Alkynes CnH2n-2 (unsaturated- triple bonds)
12
Hydrocarbon nomenclature
Prefixes Meth Eth Prop But Pent Hex Hept Oct Suffixes ane ene yne -ol -oic
13
Practice Practice C2H6 C2H5OH C2H5COOH C3H6 C3H7OH C4H6 C4H5OH butene
Butanol Propanoic Methanoic Cyclobutane cyclohexane
14
Keytones ketones are named by changing the suffix -ane of the parent alkane to -anone. The position of the carbonyl group is usually denoted by a number. C H3-CO-CH3 2-propanone (acetone)
15
Aldehydes The name is formed by changing the suffix -e of the parent alkane to -al, so that HCHO is named methanal, and CH3CH2CH2CHO is named butanal.
16
Chemical Laws Laws of Conservation Of Mass Lavoisier
Matter is not created or destroyed Application – balancing equations Atoms are conserved
17
Law of Definite Composition
Proust “Every compound always contains the mass proportions of elements” Ex : water mass proportions will always be a multiple of 2.02gH: 16.0g O Law of Multiple Proportions Dalton “When two elements form different compounds, the ratio of masses of element A combined with 1.00 g of element B is a whole number” Ex. Compound Mass of oxygen that combines with 1.0g Carbon 1 1.33g 2 2.66g
18
Historic Models Daltons model pg 46 Dalton, Thomson, Rutherford, Bohr
(chapter two)
19
Subatomic Particles A-Z format Atomic number (Z number)
Equal to the number of protons in an atom Atomic Mass Since electrons have insignificant mass, the mass atomic mass is the sum of protons and neutrons Isotopes- have the same number of protons, but different numbers of neutrons A-Z format
20
Mass spectrometer Used to determine the isotopes of an element and there fore the Average atomic mass Data is measured in percent deflection
22
Average Atomic Mass Weighted average
Takes into considerations how common the isotopes are Ex. There are 3 common isotopes of Uus. The mass spectrometer produced the data below. What is the average atomic mass of Uus Mass percent 283.4 amu 34.60 284.7 amu 21.20 287.8 amu 44.20
23
All the ways you learned to get moles Last Year
Solids Gases Moles Liquids Solutions
24
Given: 0.6331g ammonium sulfate
_______ mol _______ mol H atom _______ Formula units _______ N atoms _______ g Oxygen
25
Percentage Composition Empirical and Molecular Formula
Example 1: What is the percentage composition of potassium dichromate? Example 2: Determine the percentage composition of copper (II) sulfate pentahydrate.
26
Empirical Formula Molecular Formula CH C2H2 or C3H3 or C6H6 C6H12O6
27
Example 3. A sample of an unknown compound with a mass of g was analyzed and found to contain g of carbon and 1.469g of oxygen. What is the empirical formula of this compound?
28
Example 4. A white powder used in paints, enamels and ceramics had the following composition: % Ba, 6.090% C, and 24.32% O. Determine the empirical formula.
29
Example 5 An oxide of phosphorus is 43.7% phosphorus and has a molecular weight of 284 g/mol. Determine the molecular formula for this compound.
30
Combustion Analysis Combustion Analysis is used to determine the empirical/molecular formula for hydrocarbons. (CxHy) CxHy + O2 → CO2 + H2O CxHyOz + O2 → CO2 + H2O The formula of the hydrocarbon can be assayed when considering the amounts of carbon dioxide and water collected from the combustion.
31
Example 1: A compound contains only carbon and hydrogen. A 1.45g sample is burned and produces 2.25g of water and 4.40g of carbon dioxide. Determine the empirical formula for the hydrocarbon.
32
Example 2: 5.00g of an oxygen containing hydrocarbon is combusted to yield 9.57g carbon dioxide and 5.87g water. What is the empirical formula?
33
Composition vs. Reaction Stoichiometry
Composition deals with— Reaction deals with--
34
Reaction Stoichiometry
Balancing Equations: Ex. 1: (NH4)2Cr2O7 (s) Cr2O3 (s) + N2 (g) + H2O (l) Ex. 2: H2O (l) Ex. 3: CaCl2 (aq) + Na3PO4 (aq) Ex. 4: C3H8 (g) + O2
35
Ex. 1. What mass of potassium iodide is necessary to completely react with g of lead (II) nitrate in a double replacement reaction?
36
Ex. 2. What mass of solution that is 22
Ex. 2. What mass of solution that is 22.5% potassium iodide is needed to completely precipitate 0.28 g of lead (II) iodide?
37
Ex. 3. In an experiment performed in the classroom, a student collects 12.7 L of ammonia from the reaction of 9.0 g of nitrogen with excess hydrogen. What is the percent yield?
38
Yield Theoretical Yield: Percent Yield:
39
Make it Real Limiting Reactant: Excess Reactant:
40
Ex. 4: Consider the synthesis of Zinc and sulfur If 25
Ex. 4: Consider the synthesis of Zinc and sulfur If 25.0g of zinc and 30.0 g of sulfur are mixed, How many grams of zinc sulfide could be produced? How many grams of excess reactant should remain after the reaction is over?
41
Ex. 5: In a reaction between 38. 0g of chromium (III) oxide and 9
Ex. 5: In a reaction between 38.0g of chromium (III) oxide and 9.00 g of aluminum metal, 15.2 g of chromium metal were collected along with an unmeasured amount of aluminum oxide. What was the percent yield for this experiment?
Similar presentations
© 2025 SlidePlayer.com Inc.
All rights reserved.