Chem 103 1st EditionExam # 1 Study Guide Lectures: 1 - 7Lecture 1 (January 21)SummaryWhat is Chemistry? - The study of the physical and compositional changes of matter- Called the Central ScienceMatter: Anything that has mass, occupies space, and is made of atoms or parts of atomsMass: Measure of the amount of matter in an object - independent of locationWeight: Measure of the gravitational pull on an objectProperties of Matter- Physical Properties: Can be observed or measured without changing the composition of the matter being observed- Chemical Properties: Can be observed or measured only when the composition of matteris changedChanges of Matter- Physical Changes: Are reversible, take place without a change of composition, and no new chemicals are created as a result- Chemical Changes: Cannot be reversed, changes the composition, and new chemicals are created as a resultAccording to the Skill Book, you should:- Know what it means to study chemistry- Define matter- Define mass- Distinguish between mass and weight- Define property- Know the difference between a physical property and a chemical property and provide examples for each- Know the difference between a physical change and a chemical change and provide examples of eachLecture 1 Example Questions:1. Matter is anything that has _____ and occupies _____. a. Answer: mass, volume2. ______ is a measurement of the amount of matter in an object.a. Answer: Mass3. ______ is a measurement of gravitational force acting on matter.a. Answer: Weight4. Melting point is an example of a _______ property.a. Answer: Physical5. Reacting violently with water is an example of a _______ property.a. Answer: Chemical6. Water evaporating into water vapor is an example of a _______ change. Why?a. Answer: Physical. Phase changes do not change the chemical make-up of matter, and so this is a physical change.7. The ripening of an apple is an example of a _______ change. Why?a. Answer: Chemical. The chemical makeup of the apple is changing as a slow chemical reaction occurs, so this is a chemical change.Lecture 2 (January 23)SummaryDemocritus- First person recorded to suggest that atoms were the basis of matter- The word “atom” comes from the word “atomos,” meaning “no cut” in GreekJohn Dalton- All matter made up of atoms- Pure substances known as elements are made of atoms that are all identical- Pure substances known as compounds are combinations of two or more elements- Compounds have a fixed ratio of atoms- Chemical reactions do not destroy or create atoms- Chemical reactions can destroy or create compoundsCommonly used base units in the metric system:- Length = meter (m)- Volume = liter (L)- Mass = gram (g)- Time = second (s)- Temp = ˚Celsius (˚C)- Energy = calorie (cal), (a nutritional Calorie, or a Cal, is worth 1000 scientific calories)- Amount of substances = mole (mol)Common prefixes used in metric system- mega-; M; 1,000,000 x base unit- kilo-; k; 1000 x base unit- centi-; c; 1/100 x base unit- milli-; m; 1/1000 x base unit- miro-; µ; 1/1,000,000 x base unitAccording to the Skill Book, you should:- Know John Dalton’s Model of Matter- Know the base metric unitsExample Questions:1. The first person to define the atom was _______.a. Answer: Democritus2. According to John Dalton’s ”Particulate” Model of Matter, chemical reactions can destroy and create ______, but they cannot destroy or create _______.a. Answer: compounds/molecules, atoms3. In chemistry, the base metric unit for mass is ______.a. Answer: grams (g)4. In chemistry, the base metric unit for ______ is liters (L).a. Answer: volumeLecture 3 (January 28)SummaryScientific notation: M x 10nMultiplying scientific notation- Step 1: Multiply the M values to one another. The new M value is the M value of the product.- Step 2: Add together the n values to one another. The new n value is the n value of the product- Step 3: The final product is the new M value x 10new n valueDividing scientific notation- Step 1: Divide the M values from one another. The new M value is the M value of the quotient.- Step 2: Subtract the denominator (bottom) n value from the numerator (top) n value. The new n value is the n value of the quotient.- Step 3: The final quotient is the new M value x 10new n valueRules of Significant Figures- All non-zero numbers are significant- Zeroes between non-zero numbers are significant- The leading zeroes in tiny numbers are NOT significant; they’re there to indicate the position of the decimal point- Trailing zeroes ARE significant IF the decimal point is shown. Trailing zeroes are generally NOT significant when the number doesn’t contain a decimal point- Some numbers are considered exact, meaning that they have no uncertaintyAccording to the Skill Book, you should:- Recognize and use scientific notation- Know and follow the rules of significant figures Example Questions:1. Express the following in scientific notation while keeping the number of scientific figuresa. 123,430.0i. Answer: 1.234300 x 105b. 0.0007i. Answer: 7 x 10-4c. 350.053i. Answer: 3.50053 x 102Lecture 4 (January 30)SummaryMultiplying and Dividing Significant Figures- Answer must contain the same number of significant figures as the quantity with the fewest number of significant figures used in the calculationAdding and Subtracting Significant Figures- Answer must contain the same number of places to the right of the decimal as the quantity in the calculation with the fewest number of places to the right of the decimalConversion Factors: fractions derived from fixed relationshipsPercentage- To calculate percentage you place the # that is the part over the # that is the total and multiply it by 100 (part/total x 100 = percentage)- Percent Accuracy: how accurate a product in an experiment is - % accuracy = actual/theory x 100- Percent Error: How far the product is from the theoretical answer - % Accuracy + % Error = % 100Density- The ratio of the mass of a sample of matter divided by the volume of the same sample- Density = mass/volume- Can also be found by its displacement for solidsElements you are expected to recognize-- H – Hydrogen- He – Helium- Li – Lithium- Be – Beryllium- B – Boron- C – Carbon- N – Nitrogen- O – Oxygen- F – Flourine- Ne – Neon- Na – Sodium- Mg – Magnesium- Al – Aluminum- Si – Silicon- P – Phosphorous- S – Sulfur- Cl – Chlorine- Ar – Argon- K – Potassium- Ca – Calcium- Sc – Scandium- Ti – Titanium- V – Vanadium-