Exam # 1 Study Guide Lectures: 1 - 8Lecture 1 & 2 Matter Describe the four phases of matter.1. Solid- definite size and volume2. Liquid- definite volume, fluid shape3. Gas- undefined volume and shape4.Plasma- undefined volume and shape, interacts with magnetic fieldWhat can be classified with respect to composition?1. Pure substances- fixed composition, unique set of properties. Can be elements or compoundsa. Elements cannot be broken down into 2 or more pure substances2. Mixtures- composed of 2 or more substances. Can be homo or heterogeneousa. Homogenous mixtures are uniform and can be called a solution.i. Solutions are made through solvents (largest amount) and solutes (one ormore)ii. Ex. Brass (Cu and Zn)b. Heterogeneous mixtures are non-uniform (ex. Rocks) and can be separated by:i. Filtration- solid to liquidii. Distillation- liquid to liquidWhat are compounds?- Compounds are pure substances with 2 or more elements. Example: H2O- Properties of compounds differ from elements- Can sometimes be separated into elementsLecture 3 & 4 Measurement & TemperatureChem 1127 1st EditionI. Length measured in meter.a. Meter defined as distance light travels in 1/299792458 secondsII. Volume is expressed in 3 waysa. Liters 1L=10-3m3=103 cm3b. Cm3 1cm3= (10-2 m)3=10-6 m3cm3=mLc. mL 1 mL=10-3 L=10-6 m3III. Massa. Mass is the amount of matter, expressed in gramsb. Weight is the force of gravity acting on massIV. Temperaturea. Determines direction of heat flowb. In °C , 0°C is freezing. 100°C is boiling for pure waterc. 32°F is freezing. 212°F is boiling. d. T°F =°C x 9/5 + 32 V. Absolute Scale, Kelvina. Defined as 1/273.16 of the difference between lowest attainable temperature and the triple point (0.01°C)b. T°K =°C + 273.15 Lecture 5 & 6 Uncertainty in Numbers and Significant FiguresI. Uncertainty depends on equipment and operatora. Example. Graduated cylinder with 1 mL marking ±1mLb. Graduated cylinder with 0.1 mL marking ±0.1mLc. Graduated cylinder with 0.01 mL marking ±0.01mLd. The uncertainty is the in last digitII. What are the Significant Figures Rules?a. Non-zero numbers are significantb. Zeroes between significant numbers are significantc. Zeroes after a decimal point or at the end of a number are significantd. Zeroes before a decimal point in a number greater than 10 are significant III. What are the rounding off rules?a. Digits less than 5, leave unchangedb. Digits greater than 5, add onec. Digits equal to 5, make the number on the left of the decimal point evenIV. What are the rules for mathematical operations?a. For addition/subtraction, uncertainty in the last decimal placeb. For multiplication/division, use the least amount of sig figsV. Conversion of Units (dimensional analysis)a. Unit 1 x unit 2/unit 1VI. Pure substances have properties that are unique a. They must be intensive (can’t depend on an amount)i. Mass & volume are extensive but density=m/v is intensiveVII. Chemical properties can be observed in a reactionb. Example. 2HgO (s) 2 Hg (g) + O 2 (g)VIII. What is solubility?c. Solubility is the process of dissolving solute (thing being dissolved) in a solvent (thing doing the dissolving), expressed as g/100g at a given temperatureLecture 7 Atoms, Molecules, & IonsI. Dalton’s Modela. Elements are composed of atoms, all atoms have the same properties b. In an ordinary chemical reaction, atoms move from 1 substance to another, no atom is destroyed or created so mass is conservedc. Compounds are formed when atoms of 2 or more elements are combinedII. What are some atomic components?a. Protonsi. Have a mass equal to H atom and has a +1 chargeb. Neutronsi. Have a mass slightly larger than protons and have no chargec. Electronsi. Have a mass much lower than protons and have a -1 chargeParticle Mass Charge LocationProton 1.00728 amu +1 NucleusNeutron 1.00867 amu 0 NucleusElectron 0.00055 amu -1 Outside nucleusIII. How do you write a chemical symbol with the mass number and atomic number?a.IV. What are isotopes?a. Isotopes are atoms of the same element with the same number of protons, a different number of neutrons, and a different mass numberi. Isotopes abundance is measured by mass spectrometerii. Equation for isotope abundance is: (exact weight of isotope #1) (abundance of isotope #1) + (exact weight of isotope #2) (abundance of isotope #2) = average atomic weight of the elementV. Avogadro’s numbera. Represents the number of atoms in a sample whose mass in grams equals the atomic massb. Avogadro’s number= 6.02214129 × 10 23VI. What does Mendeleev’s original periodic table consist of?a. Periods, which are horizontal rows, going in order of electronic shellsb. Groups, which are the vertical columns and organized by similar chemical propertiesLecture 8 Evolution of the Periodic TableI. How is the periodic table currently structured?a. It is organized in groups and periods increasing by number of protons in each element, then by properties such as main group elements, metals, non-metals, and metalloids (semi-metals)II. What are compounds?a. Compounds are two or more atoms of different elements in combination to produce a neutral speciesb. An example of binary compounds:i. Na + Cl NaCl ] formula unitii. H + Cl HCl ] moleculeIII. What are the two different types of formulas used to describe molecules and compounds?a. Structural formula, which shows the connection between atomsi. Example. Glucoseb. Molecular formula, which has the whole number ratio of atoms denoted by a subscripti. Example. Glucose C6H12O6IV. What are two forms of ions?a. Cations which form by a loss of electrons and are denoted with (+) super scripti. Example. Na+b. Anions which form by gaining electrons and are denoted with a (-) super scripti. Example. Cl- V. What are the rules for writing the formulas for ionic compounds?a. Identify the action.i. Action is written first in the name of the compoundb. Write the correct formula and charge for the action.c. Identify the anioni. Anion is written last in the name of the compoundd. Write the correct formula and charge for the anion.e. Combine the action and anion to produce an electrically neutral compound.f. Make sure that the subscripts for the action and anion are the smallest whole number ratio.VI. What kind of solutions do ionic and molecular compounds tend to form?a. Ionic compounds tend to form conductive solution (electrolytes) containing metals and nonmetalsb. Molecular compounds tend to form