MATTER Fill in the following chart for TYPICAL Solids, Liquids and Gases (not water) State of Matter Particle Arrangement Regular or Irregular

Size: px
Start display at page:

Download "MATTER Fill in the following chart for TYPICAL Solids, Liquids and Gases (not water) State of Matter Particle Arrangement Regular or Irregular"

Transcription

1 Name Period Mr. Rivas Super Awesome Chemistry Final Exam STUDY GUIDE MATTER Fill in the following chart for TYPICAL Solids, Liquids and Gases (not water) State of Matter Particle Arrangement Regular or Irregular Shape Definite or Indefinite Density Rank 1 = highest 3 = lowest Gas Energy Rank 1 = highest 3 = lowest Compressibility Yes or No Liquid Solid Atoms draw a diagram of an atom of Lithium (mass number 7), labeling the following parts nucleus, electron cloud, protons, neutrons, electrons Label as: molecule, atom, compound, substance, homogeneous mixture, heterogeneous mixture H 2O A single particle of pure potassium A sample of sand scooped from a beach Sodium chloride Iced tea The smallest particle of an element that retains all of its chemical properties Chicken soup PHYSICAL AND CHEMICAL CHANGES AND PROPERTIES Classify the following as a chemical or physical property or chemical or physical change 1. Liquid collects on the side of a cold drink glass Hexane is flammable Baking soda decomposes in the cake, releasing CO 2 to make it fluffy. Copper II sulfate is blue. Ice is melting 6. Pure water has a density of 1 g/cm 3 STATES OF MATTER Mark the statements as true or false. If false, make changes to correct the statement. 1. Liquids have the greatest amount of kinetic energy among the phases of matter 2. In general, a solid is the densest phase of matter. 1

2 3. Particles in a solid demonstrate rotation, vibration and translation. 4. The particles of liquids have low amounts of translation unless they are stirred. 5. When a solid is melting, its temperature is still rising as it melts. 6. Both solids and liquids can flow. 7. Translation is the type of kinetic energy in which a particle moves from place to place. DENSITY CALCULATIONS Solve the following problems involving density calculations. Show all work. 1. What is the formula for density? 2. A cube is 17 cm 3 in volume with mass of 4.0 grams. Calculate its density. 3. If a ball has a density of 27.5 g/cm 3, determine its volume if its mass is 626 g. METRIC UNITS Perform the following determinations kilometer (km) = meters (m) 2. 1 milligram (mg)= grams (g) 3. 1 liter (L) = milliliters (ml) kilograms (kg)= grams (g) meters (m) = centimeters (cm) ATOMIC STRUCTURE Fill in the following table with the appropriate information Subatomic Particle Charge Location Nucleus or Proton Neutron Electron electron cloud Mass Order of Size 1= largest 3 = smallest PERIODIC TABLE Answer the following questions What number of valence electrons indicates the most stable arrangement? Which group on the periodic table fits this description without forming ions? Elements on the periodic table are organized in order of increasing.? Elements are identified by the number of in their nucleus. The number of and may vary. 2

3 ORGANIZATION OF THE PERIODIC TABLE Label the following on the diagram below. Then, label the number of valence electrons inside the space for each group. s-block p-block d-block f-block metals non-metals alkali metals alkali earth metals Aluminum group Carbon group Nitrogen group Oxygen Group Halogens Noble Gases transition metals inner transition metals Define each of the following trends and indicate them the periodic table above using arrows. Be sure to indicate group and periodic trends. Atomic size Electronegativity Ionization energy ELECTRON CONFIGURATION Write the full electron configuration for the following elements. Circle the valence electrons. Helium Strontium Barium Oxygen Fluorine Neon 3

4 BONDING Draw the covalent structure for the following chemical formulas. Name the shape of the molecule. 1. PBr 3 3. SO 3 2. SO 2 4. PO 4 3- Indicate the correct word(s) to complete each sentence. 1. Ionic bonds are formed between metals and (other metals / non-metals) 2. Covalent bonds are formed between non-metals and (other non-metals / metals) 3. Metals (do / do not) form bonds with other metals 4. The transition metals (lose / gain) electrons to form ions. 5. When comparing degree of polarity between two bonds, the bond with the greatest polarity has the (largest / smallest ) difference between the two atoms in the bond. ELECTRON DOT STRUCTURES Draw the electron dot structure of the valence electrons for the following elements. Indicate which, if any, fulfill the octet rule when neutral. If they do not fulfill the octet rule when neutral, indicate the number of electrons gained or lost for the atom to fulfill the rule. Sodium Silicon Chlorine Magnesium Phosphorus Argon Aluminum Sulfur ION FORMATION Fill in the following table regarding ions: Element Group Name Type cation/anion Charge # and +/- Metal / Non-Metal Sodium Selenium Boron Phosphorus Calcium Fluorine Radon Phosphorus 4

5 BONDING Fill in the following table regarding ionic bonding: Cation Charge Anion Charge Balanced Formula Calcium Sulfur Chemical Name Strontium Aluminum Cesium Magnesium Boron Sodium Chlorine Iodine Nitrogen Oxygen Phosphorus Fluorine POLYATOMIC IONS Fill in the following chart: Cation Calcium Formula and Charge Anion Hydroxide Formula and Charge Balanced Formula Chemical Name Strontium Nitrate Ammonium Acetate Cesium Chlorate Magnesium Cyanide Boron Sulfate Sodium Nitrite BALANCING EQUATIONS AND REACTION SYMBOLS Balance all equations. Label reaction type for all reactions. 1. N 2(g) + H 2(g) NH 3(g) 2. KClO 3(s) KCl (aq) + O 2(g) 3. NaCl (s) + F 2(g) NaF (aq) + Cl 2(g) 5

6 4. AgNO 3(aq) + MgCl 2(aq) AgCl + Mg(NO 3) 2(aq) 5. C 3H 8(l) + O 2(g) CO 2(g) + H 2O (l) Answer the following questions based upon the formulas above: 1. What does the subscript (g) indicate in equation 1? 2. What does the subscript (s) indicate in equation 2? 3. Does equation 3 take place in water? How do you know? 4. Write the formula for the precipitate in equation 4. Rewrite its name in word format. 5. Write the 3 criteria for identifying a combustion reaction. 6. What does indicate in equation 2? REACTIONS AND STOICHIOMETRY: Perform the following stoichiometric calculations. Make sure you have a balanced equation! CH 4 + O 2 CO 2 + H 2O How many grams of O 2 are needed to react with 9.02 g of CH 4? 2. N 2 + H 2 NH 3 How many grams of NH 3 are formed when 11.7 g of H 2 react? 3. C + O 2 CO How many grams of carbon are needed to produce 0.98 g of CO? 6

7 GASES Name and describe the three types of particle motion. Indicate the phases of matter that exhibit each. Describe the Kinetic Theory of Gases and list the three assumptions associated with it. Define phase change. Define these types of phase changes. Give an example of where you might experience each. Melting Vaporization Freezing or Crystallization Condensation Evaporation Sublimation GAS LAWS: Solve the following problems using the gas laws 1. A gas with volume of 5.3 L at 17 C decreases to -3 C. Find the new volume. 2. A 2.1 L sample of gas a standard pressure is moved to a 5.2 L container. Find the new pressure. 3. An aerosol can contains gas at 15 atm and 25 C. Find the pressure inside the can at 100. C 4. Find the number of moles of gas in a container at the following conditions 6.0 atm, 3.6 L, and 118 C. 5. A gas at 742 mmhg and -18 C occupies 1.7 L. Find the volume of the gas at STP. 6. Define absolute zero. Give the temperature for it in both C and K. 7. A mixture of four gases is stored at mmhg. H2 is 127 mmhg, O2 is 350 mmhg and CO2 is 642 mmhg. Find the partial pressure of the Helium in the mixture. 8. Under what conditions does a gas stop acting ideal and begin acting real? 9. What volume does one mole of any gas occupy at STP? 7

8 CONVERSIONS Perform the following conversions: C to K atm to mmhg C to K kpa to Torr K to C mmhg to atm K to C atm to kpa WATER AND SOLUTIONS Draw a picture of a water molecule. Indicate the poles on this polar molecule. Write a definition and example for each of the following. Soluble Supersaturated Saturated Molarity Unsaturated Molality You have a solution of NaCl dissolved in distilled water. Which is the solute and which is the solvent? How many ions will the NaCl split into? Describe three ways to increase the rate of dissolving a substance. 8

9 MOLARITY AND MOLALITY Answer the following: Write the general formula for calculating the molarity of a substance. Write the general formula for calculating the molality of a substance. A solution is made by dissolving 5.0 moles of NaCl in 2.0 Liters of dh 2O. Calculate the molarity of the solution. A solution is made by dissolving 62. g of KCl in 0.50 L of dh 2O. Determine the molarity of the solution. A solution is made by dissolving 92.0 g of BaCl 2 in 5.6 kg of dh 2O. Determine the molality of the solution. MOLAR MASS AND PERCENT COMPOSITION Find the molar mass for the following formulas: BaCl 2 CuSO 4 NaNO 3 Ba(OH) 2 Determine the percent composition of the following: S in CuSO 4 NO 3 in NaNO 3 H 2O in CuSO 4 * 5 H 2O 9

10 THERMOCHEMISTRY Perform the following conversions: 41.2 kj =? J 816 J =? cal kj =? cal 71 0 F =? 0 C C =? K 255 K =? 0 C 1. How much heat is required to raise the temperature of 23.5 g of copper from 250K to 298K? 2. What is the specific heat (in J/g 0 C) of an unknown substance if adding kj of heat to 100g of the substance causes the temperature to increase by 12 0 C? 3. How much heat is absorbed by ml of water if its temperature increased by C? 4. If 15.00g of water at an initial temperature of 19 0 C absorbs 2.03 kj of heat, what will its final temperature be? 5. If you place 50.00g of a metal at a temperature of C into 100.0mL of water at C, and stir the mixture, what is the specific heat of the metal if the final Temperature of the mixture is C? (answer in J/g 0 C) REACTION RATES AND EQUILIBRIUM Describe and give examples of three ways you can speed up the rate of a reaction. Explain Le Châtelier s Principle. How does Le Châtelier s Principle explain what happens to vapor pressure when a sealed bottle of soda is heated? Think of a reversible reaction in which heat is a product of the forward reaction. Now imagine that heat is added to the system. Which way will the system shift and why? Write the K eq equation for the following equilibrium reaction. aa + bb cc + dd What does it mean if K eq < 1. How about > 1? 10

11 What does it mean if Q > K eq? How about < K eq? Write an equilibrium constant expression for the following chemical reactions: 1. 2 HI g) H 2(g) + I 2(g) 2. 2 BrCl 2(g) Cl 2(g) + Br 2(g) 3. Fe 3O 4(s) + 4 H 2(g) 3 Fe (s) + 4 H 2O (g) Answer the questions based upon the following reaction. 2 BrCl (g) Cl 2(g) + Br 2(g) 1. Write K eq for the equation. 2. If [Cl 2] = 4.00 mol/l and [Br 2] = 4.00 mol/l, find the concentration of BrCl is K eq = ACIDS AND BASES Explain the Arrhenius model of acids and bases. Explain the Brønsted-Lowry Model of acids and bases. Explain the Lewis Model of acids and bases. Explain the difference between monoprotic acids and polyprotic acids. Explain the difference between molar mass (gram formula mass) and gram equivalent mass. Calculate the ph of solutions having the following ion concentrations. a. [H+] = 1.0 x 10-2 M b. [H+] = 3.0 x 10-6 M c. [OH - ] = 8.2 x 10-6 M d. [OH - ] = 4.0 x 10-3 M 11

12 Write balanced equations for the following acid-based neutralization reactions. a. nitric acid and cesium hydroxide b. hydrobromic acid and calcium hydroxide c. sulfuric acid and potassium hydroxide d. acetic acid and ammonium hydroxide Answer the following questions regarding titration reactions. a. Determine the molarity of a CsOH solution if 30.0 ml of the solution is neutralized by 26.4 ml of a M HBr solution. b. Find the molarity of a nitric acid solution if ml of a M KOH solution is needed to neutralize ml of a solution of unknown concentration. c. Find the concentration of a household ammonia cleaning solution if ml of M HCl is needed to neutralize ml of the cleaning solution. 12

13 BIG IDEAS Intro Unit 1. Chemists use the metric system when recording their measurements. 2. Dimensional analysis must be used to convert between measurement units. 3. Chemicals have both physical and chemical properties that can be used to tell them apart, and also to separate components of a mixture. 4. When it comes to evaluating a solute/solvent relationship, remember the phrase like dissolves like. Atoms/Periodic Table Units 1. Ionic compounds form when atoms gain or lose electrons. Metals lose electrons, nonmetals gain them. 2. The number of electrons gained or lost can be predicted with an understanding of the octet rule and the number of valence electrons an atom contains. 3. The periodic table is organized by electron configuration, and elements are classified as metals, nonmetals or metalloids based on physical and chemical properties. 4. Atoms have a central nucleus that contains the protons and neutrons, and electrons are found in orbitals located outside the nucleus. 5. Electron configurations are used to describe locations of electrons within levels, sublevels and orbitals. 6. Metal reactivity is summarized in the Metal Activity Series. Formula Writing/Moles/Chemical Reactions Units 1. Conversions between moles, particles, and mass are widely used in chemistry 2. Chemical reactions must be balanced with coefficients to obey the law of conservation of mass/atoms. 3. The quantity 6.02 x is called a mole, and the periodic table lists the mass of 1 mole of each element s atoms, called the molar mass of the element. 4. Coefficients are interpreted as either particle, mole, or (if everything is a gas) liter ratios. 5. Stoichiometry is the name given to the process of using coefficients as mole ratios to convert between chemicals in a reaction equation. How much is used? How much is made? These questions can be answered with a stoichiometric calculation. Gases Unit: 1. 4 variables describe a gas behavior: P, V, n and T. 2. Boyle, Charles and Gay-Lussac developed mathematical gas laws that are used to predict and calculate changes in gas properties. 3. At STP, one mole of any gas occupies a volume of 22.4 L. This is called the molar volume of a gas. Solutions Unit: 1. Molarity and molarity are two units used to express the concentration of a solution quantitatively. 2. Concentrated and dilute are relative terms for expressing the concentration of a solution qualitatively. 3. Solutes and solvents are the two components of a solution. Thermochemistry Unit: 1. The collision theory explains that gas-phase chemical reactions occur when molecules collide with sufficient kinetic energy and proper orientation. 2. Heat, represented by q, is energy that transfers from one object to another because of a temperature difference between the objects. 3. An endothermic process absorbs heat from the surroundings. An exothermic process releases heat to the surroundings. 4. Calorimetry is the measurement of the heat flow into or out of a system for chemical and physical processes. The insulated device used to measure the absorption or release of heat in chemical or physical processes is called a calorimeter. 5. You can calculate the heat absorbed or released by the surroundings (q surr) using q = m x C p x ΔT. Equilibrium Unit: 1. Le Châtelier s principle describes what happens when stress is applied to a system in dynamic equilibrium. 2. A catalyst lowers the activation energy of a reaction. 3. K eq is used to determine whether reactants or products are favored in a reaction. 4. Q is used to determine whether a reaction will shift forward or backward. Acids and Bases Unit: 1. The Arrhenius, Brønsted-Lowry, and Lewis definitions of acids and bases are all based on different criteria. 2. ph is based on the concentration of H+ ions in solution. 3. An imbalance of H 3O + and OH - ions causes solutions to be either acidic or basic. 4. Titrations are used to determine the concentration of a solution using a solution of known concentration. 13

2. Identify each of the following samples of matter as heterogeneous or homogeneous.

2. Identify each of the following samples of matter as heterogeneous or homogeneous. EOC REVIEW #1 1. List the following in order from smallest to largest. (A) 1 dm 3 (B) 1 ml (C) 1 cl (D) 1 L (E) 1 dl 2. Convert the following. Express your answer in standard scientific notation. (A) 36

More information

5. All isotopes of a given element must have the same (A) atomic mass (B) atomic number (C) mass number (D) number of neutrons

5. All isotopes of a given element must have the same (A) atomic mass (B) atomic number (C) mass number (D) number of neutrons 1. Which substance can be decomposed by a chemical change? (A) beryllium (B) boron (C) methanol (D) magnesium 2. The particles in a crystalline solid are arranged (A) randomly and far apart (B) randomly

More information

Spring Semester Final Exam Study Guide

Spring Semester Final Exam Study Guide Honors Chemistry Name Period AlCl3 Cu2S NaCN HI PCl3 CrBr3 Naming and Formula Writing 1. Write the name or formula for each of the following: HClO2 (NH4)2SO4 I4O10 H3N NiN H3PO4 Mercury (II) bromide Phosphorous

More information

5. What is the name of the compound PbO? 6. What is the name of HCl(aq)?

5. What is the name of the compound PbO? 6. What is the name of HCl(aq)? 1. Which idea of John Dalton is no longer considered part of the modern view of atoms? (A) Atoms are extremely small. (B) Atoms of the same element have identical masses. (C) Atoms combine in simple whole

More information

2. If a gas is released in a reaction (ex: Hydrogen gas bubbles off), is it written as a reactant or a product?

2. If a gas is released in a reaction (ex: Hydrogen gas bubbles off), is it written as a reactant or a product? PRE-AP CHEMISTRY SPRING FINAL EXAM REVIEW Name _ Period Exam Date 100% COMPLETION OF THIS REVIEW BY THE DAY OF YOUR FINAL EXAM WILL COUNT AS A 5 POINT BONUS ADDED TO YOUR FINAL EXAM SCORE. THERE WILL BE

More information

Chemistry Final Exam: Practice Problems

Chemistry Final Exam: Practice Problems Chemistry Final Exam: Practice Problems 1. Key Vocabulary/Terms: atomic number element compound kinetic theory acid base salt vaporization condensation evaporation boiling sublimation energy level valence

More information

Chemistry Final Exam Sample Items

Chemistry Final Exam Sample Items Chemistry Final Exam Sample Items 1. Which best describes the current atomic theory? a. Atoms consist of electrons circling in definite orbits around a positive nucleus. b. Atoms are composed of electrons

More information

1. Dimensional Analysis: convert the following values a. 47,340 cm to m Unit 1: Chemistry Matters b. 40.64 km to m c. 58,700 ml to L 2. Calculate the number of significant figures a. 0.0210 b. 3.6056 c.

More information

b. Na. d. So. 1 A basketball has more mass than a golf ball because:

b. Na. d. So. 1 A basketball has more mass than a golf ball because: Chem I Semester Review All of the following are general characteristics of a substance in the liquid state except a. definite volume. c. not easily compressed. b. able to flow. d. definite shape. In the

More information

CHEMISTRY CP Name: Period:

CHEMISTRY CP Name: Period: CHEMISTRY CP Name: Period: CHEMISTRY SPRING FINAL REVIEW SHEET NOTE: Below are concepts that we have covered in class throughout the second semester. Questions are organized by chapter/concept to help

More information

Gas Laws. Bonding. Solutions M= moles solute Mass %= mass solute x 100. Acids and Bases. Thermochemistry q = mc T

Gas Laws. Bonding. Solutions M= moles solute Mass %= mass solute x 100. Acids and Bases. Thermochemistry q = mc T Name Period Teacher Practice Test: OTHS Academic Chemistry Spring Semester 2017 The exam will have 100 multiple choice questions (1 point each) Formula sheet (see below) and Periodic table will be provided

More information

Chemistry Final Review 2017

Chemistry Final Review 2017 Chemistry Final Review 2017 Atomic/Molecular Structure and Periodic Trends 1. What is the atomic number trend on the periodic table? 2. On the following periodic table label metals, nonmetals, Alkali metals,

More information

Chemistry Exam Review

Chemistry Exam Review Chemistry Exam Review This exam review was compiled using the NC Essential Standards. You need to answer each question. You will receive multiple grades for your work. If you study everything on the exam

More information

Name Pd SN Date Chemistry Review Packet- Spring 2014

Name Pd SN Date Chemistry Review Packet- Spring 2014 Name Pd SN Date Chemistry Review Packet- Spring 2014 1.1.1 Draw pictures to illustrate the differing isotopes and ions of a given element. 1.1.1 Which atomic symbol represents an isotope of sulfur with

More information

Chemistry FINAL: CONTENT Review Packet

Chemistry FINAL: CONTENT Review Packet Chemistry FINAL: CONTENT Review Packet Name: Period: Date: Classification of Matter & Chemical/ Physical Changes 1. are substances that are made up of two or more elements which are chemically combined

More information

CP Physical Science Chemistry: Bell Work, Notes, Study Guides

CP Physical Science Chemistry: Bell Work, Notes, Study Guides CP Physical Science Chemistry: Bell Work, Notes, Study Guides Mr. Banker Fall 2014 ian_banker@charleston.k12.sc.us http://wandohigh.ccsdschools.com/directory/science/banker_ian/physical_science/ Remind101.com

More information

Period: Chemistry Semester 1 Final Exam Review Packet. 1. What is the difference between a hypothesis and a theory?

Period: Chemistry Semester 1 Final Exam Review Packet. 1. What is the difference between a hypothesis and a theory? Chemistry Name: Period: Chemistry Semester 1 Final Exam Review Packet 1. What is the difference between a hypothesis and a theory? 2. Distinguish between quantitative and qualitative observations. States

More information

(C) hydrogen chloride (D) perchloric acid REASON: (aq) tells us that it is a mixture of HCl with water. When HCl is mixed with water, it is an acid.

(C) hydrogen chloride (D) perchloric acid REASON: (aq) tells us that it is a mixture of HCl with water. When HCl is mixed with water, it is an acid. 1. Which idea of John Dalton is no longer considered part of the modern view of atoms? (A) Atoms are extremely small. (B) Atoms of the same element have identical masses. (C) Atoms combine in simple whole

More information

Physical Science Study Guide

Physical Science Study Guide Name: Class: Date: Physical Science Study Guide Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Mendeleev arranged the known chemical elements in a table

More information

Silver nitrate solution is added to sodium dichromate solution

Silver nitrate solution is added to sodium dichromate solution Chem. 110 50 Points Final Exam Part 1 Practice Write the chemical names or formulas for the following a H 2 SO 4 b NiNO 2 c Aluminum thiosulfate d Plumbic acetate e Ag 2 C 2 O 4 f P 2 O 5 g Cyanic acid

More information

Mr. Rivas Chemistry Final Exam Extra Credit Review Packet 2015

Mr. Rivas Chemistry Final Exam Extra Credit Review Packet 2015 Mr. Rivas Chemistry Final Exam Extra Credit Review Packet 2015 Lab Equipment, Reports and Safety: Big Ideas: 1. Laboratory equipment has specific uses, and also limitations on their uses. 2. Each piece

More information

Answer Sheet for Sample Problems for Chemistry Level 1 Final Exam 2016 Study Guide

Answer Sheet for Sample Problems for Chemistry Level 1 Final Exam 2016 Study Guide Answer Sheet for Sample Problems for Chemistry Level 1 Final Exam 2016 Study Guide Electrons in Atoms Chapter 5 1. What is the frequency of green light, which has a wavelength of 4.90 x 10-7 m? 8 c 3.00x10

More information

3. When the external pressure is kpa torr, water will boil at what temperature? a C b C c. 100 C d. 18 C

3. When the external pressure is kpa torr, water will boil at what temperature? a C b C c. 100 C d. 18 C Chemistry EOC Review 5: Physical Behavior of Matter 1. Which gas is monatomic at STP? a. chlorine b. fluorine c. neon d. nitrogen 2. What Kelvin temperature is equal to 25 C? a. 248 K b. 298 K c. 100 K

More information

CHAPTERS 4 & 25: Structure of the Atom and Nuclear Chemistry 6. Complete the table: Mass (amu) charge Proton 1 +1 Neutron 1 0 Electron 0-1

CHAPTERS 4 & 25: Structure of the Atom and Nuclear Chemistry 6. Complete the table: Mass (amu) charge Proton 1 +1 Neutron 1 0 Electron 0-1 Name: Date: Period: CP CHEMISTRY SPRING FINAL REVIEW SHEET NOTE: Below are concepts that we have covered in class throughout the year. Questions are organized by chapter/concept to help you study. You

More information

Regents Chemistry Unit 3- Bonding, Moles & Stoichiometry Study Guide & Pre-Test KEY

Regents Chemistry Unit 3- Bonding, Moles & Stoichiometry Study Guide & Pre-Test KEY Name: Regents Chemistry Unit 3- Bonding, Moles & Stoichiometry Study Guide & Pre-Test KEY Focus Questions for the Unit: How are compounds different... from elements?... from mixtures? What role do valence

More information

Part A Answer all questions in this part.

Part A Answer all questions in this part. Part A Directions (1-24): For each statement or question, record on your separate answer sheet the number of the word or expression that, of those given, best completes the statement or answers the question.

More information

NAME: Chemistry Final Exam Review *=equations not given on Reference Sheet Unit 1: Math & Measurement Main Topics: Conversions, Significant Figures,

NAME: Chemistry Final Exam Review *=equations not given on Reference Sheet Unit 1: Math & Measurement Main Topics: Conversions, Significant Figures, Chemistry Final Exam Review *=equations not given on Reference Sheet Unit 1: Math & Measurement Main Topics: Conversions, Significant Figures, Density, Percent Error Density *Percent Error 1. How many

More information

Chemistry 1-2E Semester I Study Guide

Chemistry 1-2E Semester I Study Guide Chemistry 1-2E Semester I Study Guide Name Hour Chapter 1 1. Define the following terms. Matter Mass Law of Conservation of Mass 2. Define and give 2 examples of the following: Pure substance Element Compound

More information

Chemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material

Chemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material Chemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material What is 25 mph in mm s 1? Unit conversions What is 1025 K in o F? Which is larger 1 ft 3 or 0.1 m 3? What is

More information

Final Exam Study Guide Honors Chemistry Semester Multiple Choice Questions

Final Exam Study Guide Honors Chemistry Semester Multiple Choice Questions Final Exam Study Guide Honors Chemistry Semester 1 2017 60 Multiple Choice Questions Name: Students should be able to: Convert between metric units Convert between scientific notation and expanded (decimal)

More information

Chemistry I 2nd Semester Exam Study Guide

Chemistry I 2nd Semester Exam Study Guide Chemistry I 2nd Semester Exam Study Guide Study the following topics and be able to apply these concepts to answer related questions to best prepare for the Chemistry exam. You should be able to: 1. Identify

More information

SPRING 2017 CHEMISTRY FINAL EXAM REVIEW

SPRING 2017 CHEMISTRY FINAL EXAM REVIEW SPRING 2017 CHEMISTRY FINAL EXAM REVIEW Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. BONDING What is the formula for diphosphorus pentaoxide?

More information

Solid Gas Liquid Plasma

Solid Gas Liquid Plasma Unit 1: MATTER 1. Define CHEMISTRY: 2. Define MATTER: Use one of the states of matter to complete each statement. (Words will be used more than once.) Solid Gas Liquid Plasma 3. A has definite volume and

More information

Chemistry 2 nd Semester Final Exam Review

Chemistry 2 nd Semester Final Exam Review Chemistry 2 nd Semester Final Exam Review Chemical Bonds 1. Give a physical description of how the atoms and molecules are arranged in solids, liquids, and gases. A: In a liquid, the forces between the

More information

1. Determine the mass of water that can be produced when 10.0g of hydrogen is combined with excess oxygen. 2 H 2 + O 2 2 H 2 O

1. Determine the mass of water that can be produced when 10.0g of hydrogen is combined with excess oxygen. 2 H 2 + O 2 2 H 2 O Pre-AP Chemistry Spring 2016 Final Review Objective 6.1: Students will recognize indicators of chemical change write balanced chemical equations to describe them based on common reactivity patterns. [S.12.C.1,

More information

Chemistry. Essential Standards Chemistry

Chemistry. Essential Standards Chemistry Essential Standards Chemistry Chemistry Matter: Properties & Change 1.1 Students will analyze the structure of atoms and ions. 1.2 Student will understand the bonding that occurs in simple compounds in

More information

What type of solution that contains all of the

What type of solution that contains all of the What type of solution that contains all of the solute it can hold at a given temperature? Saturated Solution What type of solution that contains less solute than it is able to hold at a given temperature?

More information

Bonding Mrs. Pugliese. Name March 02, 2011

Bonding Mrs. Pugliese. Name March 02, 2011 Bonding Mrs. Pugliese Name March 02, 2011 1. Atoms of which element have the greatest tendency to gain electrons? 1. bromine 3. fluorine 2. chlorine 4. iodine 2. Which polyatomic ion contains the greatest

More information

Chemistry Study Guide

Chemistry Study Guide Chemistry Study Guide Marking Period 3 Exam Week of 3/21/17 Study Guide due - When studying for this test, use your do nows, notes, homework, class handouts, and your textbook. Vocabulary Chapter 7 Anion

More information

Test Booklet. Subject: SC, Grade: HS MCAS 2010 High School Chemistry. Student name:

Test Booklet. Subject: SC, Grade: HS MCAS 2010 High School Chemistry. Student name: Test Booklet Subject: SC, Grade: HS MCAS 2010 High School Chemistry Student name: Author: Massachusetts District: Massachusetts Released Tests Printed: Thursday July 19, 2012 1 Which of the following statements

More information

Chemistry Midterm Review

Chemistry Midterm Review Chemistry Midterm Review Name To Do: 1) Make Note/Summary Sheet for each unit 2) Complete problems in this packet. As part of our review process, you will make a note sheet (max 1 SHEET per UNIT) that

More information

Unit Five- Chemical Quantities Chapter 9: Mole ratios, conversions between chemicals in a balanced reaction (mole, mass), limiting reactant, % yield

Unit Five- Chemical Quantities Chapter 9: Mole ratios, conversions between chemicals in a balanced reaction (mole, mass), limiting reactant, % yield Chemistry Midterm Review Exam date: Wednesday, 2/15 during class The midterm exam must be completed before February vacation if you are absent The midterm exam is worth 6% of your year grade and it contains

More information

Regents review Physical properties of matter

Regents review Physical properties of matter 2011-2012 1. Which statement describes a chemical property of oxygen? A) Oxygen has a melting point of 55 K. B) Oxygen can combine with a metal to produce a compound. C) Oxygen gas is slightly soluble

More information

Semester 1 Review Chemistry

Semester 1 Review Chemistry Name Period Date Semester 1 Review Chemistry Units & Unit Conversions Ch. 3 (p. 73-94) PART A SI UNITS What type of measurement is indicated by each of the following units? Choices are in the last column.

More information

Science 9 Midterm Study Guide

Science 9 Midterm Study Guide Science 9 Midterm Study Guide Name 1. What are the atomic mass units for protons, neutrons, and electrons? 2. What is the atomic number? 3. What is the mass number? 4. What particles are in equal numbers

More information

Name May 2, 2012 Physical Behavior of Matter and Bonding Review

Name May 2, 2012 Physical Behavior of Matter and Bonding Review Name May 2, 2012 Physical Behavior of Matter and Bonding Review Base your answers to questions 1 through 3 on the information below. Starting as a gas at 206 C, a sample of a substance is allowed to cool

More information

Name: Period: AP Take Home Practice Test for Unit 0.5 Exam

Name: Period: AP Take Home Practice Test for Unit 0.5 Exam Name: Period: AP Take Home Practice Test for Unit 0.5 Exam 1. Which of the following is a correctly balanced equation? a. Al 2(SO 4) 3 + 2 CaCl 2 2 CaSO 4 + 3 AlCl 3 b. Al 2(SO 4) 3 + 3 CaCl 2 3 CaSO 4

More information

CHEMISTRY HONORS LEOCE Study Guide

CHEMISTRY HONORS LEOCE Study Guide BENCHMARK: N.1.1-1.2, N.1.6, N.3.1, N.3.3, N.3.4 CHEMISTRY HONORS CHEMISTRY AND SCIENTIFIC MEASUREMENT TEXTBOOK: Glencoe, Chemistry: Matter and Change, Chapters 1-3 ESSENTIAL QUESTION: How is measurement

More information

Chemistry 121 Chapters 7& 8 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question.

Chemistry 121 Chapters 7& 8 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. Chemistry 121 Chapters 7& 8 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1. A sample of carbon dioxide occupies 22.4 L at STP. Which of the

More information

1. Which atomic symbol represents an isotope of sulfur with 17 neutrons?

1. Which atomic symbol represents an isotope of sulfur with 17 neutrons? Chemistry Common Exam Review Questions 1. Which atomic symbol represents an isotope of sulfur with 17 neutrons? 2. Which statement compares the amount of energy needed to break the bonds in CaCl2 (E1)

More information

This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24

This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24 Name Hour January Exam Practice A This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24 This practice exam will be graded in the exam portion of the grade book. Objectives

More information

ACP Chemistry (821) - Mid-Year Review

ACP Chemistry (821) - Mid-Year Review ACP Chemistry (821) - Mid-Year Review *Be sure you understand the concepts involved in each question. Do not simply memorize facts!* 1. What is chemistry? Chapter 1: Chemistry 2. What is the difference

More information

Chapter 4 Reactions in Aqueous Solutions. Copyright McGraw-Hill

Chapter 4 Reactions in Aqueous Solutions. Copyright McGraw-Hill Chapter 4 Reactions in Aqueous Solutions Copyright McGraw-Hill 2009 1 4.1 General Properties of Aqueous Solutions Solution - a homogeneous mixture Solute: the component that is dissolved Solvent: the component

More information

Advanced Chemistry Final Review

Advanced Chemistry Final Review Advanced Chemistry Final Review 1. What are the products of complete combustion of hydrocarbons? Hydrocarbons are compounds made of carbon and oxygen. When they burn (combine with oxygen) they form carbon

More information

2nd Semester Exam Review. C. K eq = [N 2][H 2 ]

2nd Semester Exam Review. C. K eq = [N 2][H 2 ] Name: ate: 1. Which pair of formulas represents the empirical formula and the molecular formula of a compound?. H 2 O, 4 H 6 O 4. HO, 6 H 12 O 6 8. Given the reaction at equilibrium: N 2 (g) + 3H 2 (g)

More information

Questions 1 to 58 must be answered on the Scantron sheets.

Questions 1 to 58 must be answered on the Scantron sheets. Questions 1 to 58 must be answered on the Scantron sheets. Base your answers to questions 1 to 5 on the heating curve for a pure substance that is shown below. 1. The freezing point of the substance is

More information

Final Exam Review Questions You will be given a Periodic Table, Activity Series, and a Common Ions Chart CP CHEMISTRY

Final Exam Review Questions You will be given a Periodic Table, Activity Series, and a Common Ions Chart CP CHEMISTRY Final Exam Review Questions You will be given a Periodic Table, Activity Series, and a Common Ions Chart CP CHEMISTRY Part A True-False State whether each statement is true or false. If false, correct

More information

Chapter 1 The Atomic Nature of Matter

Chapter 1 The Atomic Nature of Matter Chapter 1 The Atomic Nature of Matter 1-1 Chemistry: Science of Change 1-2 The Composition of Matter 1-3 The Atomic Theory of Matter 1-4 Chemical Formulas and Relative Atomic Masses 1-5 The Building Blocks

More information

PRACTICE COMPREHENSIVE EXAM #1 7 th GRADE CHEMISTRY

PRACTICE COMPREHENSIVE EXAM #1 7 th GRADE CHEMISTRY Name: Date: Class: PRACTICE COMPREHENSIVE EXAM #1 7 th GRADE CHEMISTRY BUBBLE SHEETS AND PERIODIC TABLES ARE ATTACHED. PLEASE DETACH. YOU MAY WRITE ON THE PERIODIC TABLE. PART ONE: Multiple choice. Choose

More information

The Periodic Table & Formation of Ions

The Periodic Table & Formation of Ions The Periodic Table & Formation of Ions Development of the Periodic Table Mendeleev: Considered to be the father of the periodic table Arranged elements by increasing atomic mass Placed elements with similar

More information

Chem 101 Review. Fall 2012

Chem 101 Review. Fall 2012 Chem 101 Review Fall 2012 Elements, Atoms, Ions Elements in nature symbols Constant composition chemical formula Dalton s atomic theory Atomic structure what makes up the atom ions isotopes Periodic table

More information

Name: Period: CHEMISTRY I HONORS SEMESTER 1 EXAM REVIEW

Name: Period: CHEMISTRY I HONORS SEMESTER 1 EXAM REVIEW Name: Period: CHEMISTRY I HONORS SEMESTER 1 EXAM REVIEW Unit 1: Nature of Science What rules must be obeyed to safely conduct an experiment? What are the components of a good scientific experiment? What

More information

Science Olympiad Regional UW-Milwaukee Chemistry test 2013

Science Olympiad Regional UW-Milwaukee Chemistry test 2013 Science Olympiad Regional UW-Milwaukee Chemistry test 2013 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. What is another name for the representative

More information

AP CHEMISTRY THINGS TO KNOW

AP CHEMISTRY THINGS TO KNOW AP CHEMISTRY THINGS TO KNOW Diatomic Molecules H2-hydrogen gas (do not write H) N2-nitrogen gas (do no write N) O2-oxygen gas (do not write O) F2-fluorine gas (do not write F) Cl2-chlorine gas (do not

More information

Symbol Atomic Number

Symbol Atomic Number Name: Date: Chemistry ~ Ms. Hart Class: Anions or Cations February Break Review Sheets - /150 Chemistry has a LOT of words. Take this break to review and strengthen your knowledge of the vocabulary you

More information

2. What is the charge of the nucleus in an atom of oxygen-17? (1) 0 (2) 2 (3) +8 (4) +17

2. What is the charge of the nucleus in an atom of oxygen-17? (1) 0 (2) 2 (3) +8 (4) +17 60 Most Missed Chemistry Regents Exams Questions 1. In the wave-mechanical model, an orbital is a region of space in an atom where there is (1) a high probability of finding an electron (2) a high probability

More information

Column B 5. periodic table a. A vertical column of elements in the

Column B 5. periodic table a. A vertical column of elements in the Unit 4 Assignment Packet Name Period: A1: The Periodic Table: Organizing the Elements A. periodic table B. metals C. nonmetals D. periods E. alkali metals F. halogens G. columns H. periodic law I. alkaline

More information

2014 Chemistry 1 st Semester Exam Review Packet

2014 Chemistry 1 st Semester Exam Review Packet Name: Date: Hour: 2014 Chemistry 1 st Semester Exam Review Packet 1. What percentage of the water on Earth is salt water? (1 point) A. 97.2% B. 0.009% C. 2.11% D. 2.8 % 2. One similarity between all mixtures

More information

Mid-Term Review (HERBERHOLZ - Honors Chemistry) Chapter 2: 1. How many significant digits are in the following numbers?

Mid-Term Review (HERBERHOLZ - Honors Chemistry) Chapter 2: 1. How many significant digits are in the following numbers? Name Hour Mid-Term Review 2017-2018 (HERBERHOLZ - Honors Chemistry) Chapter 2: 1. How many significant digits are in the following numbers? a. 417.0 b. 0.0005 c. 500 000 d. 0.30034 e. 3.970 x 10 5 f. 200.10

More information

Name Date Class PROPERTIES OF SOLUTIONS

Name Date Class PROPERTIES OF SOLUTIONS 16.1 PROPERTIES OF SOLUTIONS Section Review Objectives Identify the factors that determine the rate at which a solute dissolves Identify the units usually used to express the solubility of a solute Calculate

More information

Name Date. 9. Which substance shows the least change in solubility (grams of solute) from 0 C to 100 C?

Name Date. 9. Which substance shows the least change in solubility (grams of solute) from 0 C to 100 C? Solubility Curve Practice Problems Directions: Use the graph to answer the questions below. Assume you will be using 100g of water unless otherwise stated. 1. How many grams of potassium chloride (KCl)

More information

Chapter 6: Chemical Bonds

Chapter 6: Chemical Bonds Chapter 6: Chemical Bonds Section 6.1: Ionic Bonding I. Stable Electron Configurations Group # II. III. Ionic Bonds Group # A. Transfer of Electrons Group # B. Formation of Ions Group # C. Formation of

More information

Chapter How many grams of a 23.4% by mass NaF solution is needed if you want to have 1.33 moles of NaF?

Chapter How many grams of a 23.4% by mass NaF solution is needed if you want to have 1.33 moles of NaF? Chapter 13 1. Which of the following compounds is a strong electrolyte? a. NH 4Cl b. NaCl c. NaC 2H 3O 2 d. HCl e. All of the above 2. A solution that is 13.58% by mass of sugar contains 13.75 grams of

More information

Name: 1. Show all work on Math Problems!!! Significant Figures and Calculations (*all math problems will require the use of sig figs)

Name: 1. Show all work on Math Problems!!! Significant Figures and Calculations (*all math problems will require the use of sig figs) Name: 1 AP Chemistry Summer Assignment The goal of this assignment is to make sure that everyone has the fundamentals that they will need to be successful in Chemistry II & AP Chemistry. You should have

More information

Quantitative chemistry Atomic structure Periodicity

Quantitative chemistry Atomic structure Periodicity IB chemistry Units 1-3 review Quantitative chemistry Significant figures The mole- be able to convert to number of particles and mass Finding empirical and molecular formulas from mass percentage States

More information

Third Quarter Cumulative Review Questions. 1. Which factor distinguishes a metallic bond from an ionic bond or a covalent bond?

Third Quarter Cumulative Review Questions. 1. Which factor distinguishes a metallic bond from an ionic bond or a covalent bond? Name: Thursday, March 27, 2008 Third Quarter Cumulative Review Questions 1. Which factor distinguishes a metallic bond from an ionic bond or a covalent bond? 1. the mobility of electrons 3. the equal sharing

More information

Chemistry Final Exam Review

Chemistry Final Exam Review Chemistry Final Exam Review Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. All of the following are physical properties of matter EXCEPT.

More information

2 nd Semester Study Guide 2016

2 nd Semester Study Guide 2016 Chemistry 2 nd Semester Study Guide 2016 Name: Unit 6: Chemical Reactions and Balancing 1. Draw the remaining product 2. Write a balanced equation for the following reaction: The reaction between sodium

More information

SCI-CH Chem Test II fall 2018 Exam not valid for Paper Pencil Test Sessions

SCI-CH Chem Test II fall 2018 Exam not valid for Paper Pencil Test Sessions SCI-CH Chem Test II fall 2018 Exam not valid for Paper Pencil Test Sessions [Exam ID:25FPCV 1 When a strontium atom loses its valence electrons, it has the same electron configuration as which element?

More information

4. Draw a concept map showing the classifications of matter. Give an example of each.

4. Draw a concept map showing the classifications of matter. Give an example of each. Name Bring calculator, pencils, and this completed worksheet to the midterm exam. For problems involving an equation, carry out the following steps: 1. Write the equation. 2. Substitute numbers and units.

More information

Chm 116 (Sp 2004) - Review of Chm 115

Chm 116 (Sp 2004) - Review of Chm 115 Chm 116 (Sp 2004) Review of Chm 115 Conversions within the SI system Examples (with Answers): 1. Convert 1.29 x 10 +5 mg into the following units: kilograms, grams, micrograms, and nanograms. In order

More information

Chemistry Released Questions

Chemistry Released Questions Name: Date: 1. What was Niels Bohr s prediction about the location of the electrons in an atom? 3. An atom with which atomic diagram has chemical properties most similar to calcium? A. Electrons pair with

More information

Chemistry Spring 2018 Final Exam Review

Chemistry Spring 2018 Final Exam Review Name Date Period Chemistry Spring 2018 Final Exam Review TURN THIS COMPLETED REVIEW IN TO YOUR TEACHER BY DAY OF YOUR FINAL FOR A 5 point FINAL EXAM BONUS Unit #7 Moles 1. What is a mole? 2. What is molar

More information

Chemistry Midterm Exam Review Sheet Spring 2012

Chemistry Midterm Exam Review Sheet Spring 2012 Chemistry Midterm Exam Review Sheet Spring 2012 1. Know your safety rules 2. A shopping mall wanted to determine whether the more expensive Tough Stuff floor wax was better than the cheaper Steel Seal

More information

First Semester Final Exam Study Guide

First Semester Final Exam Study Guide First Semester Final Exam Study Guide Name: Chemistry 1 2 3 4 5 6 7 60 multiple choice questions Chapter 1 1. Define matter and list five examples. Chapter 2 2. Define pure substance. 3. Define element.

More information

Chem 127, Final Exam December 14, 2001

Chem 127, Final Exam December 14, 2001 I. (55 points) This part of the final corresponds to Exam I. It covers the material in Chapters 1, 2 and 3. A. (8 points) Fill in the empty boxes with the appropriate symbol, number, word or charge. Nuclear

More information

1. What is a dot diagram? 2. Drawing dot diagrams. Name:

1. What is a dot diagram? 2. Drawing dot diagrams. Name: Name: Skill Sheet 29.2 Dot Diagrams You have learned that atoms are composed of protons, neutrons, electrons. The electrons occupy energy levels that surround the nucleus in the form of an electron cloud.

More information

FALL SEMESTER REVIEW NAME: PERIOD: 3. (Unit 2) Is the following picture representing accuracy, precision or both? Explain the difference.

FALL SEMESTER REVIEW NAME: PERIOD: 3. (Unit 2) Is the following picture representing accuracy, precision or both? Explain the difference. FALL SEMESTER REVIEW NAME: PERIOD: 1. (Unit 7) When the equation Cu + AgNO 3 Cu(NO3) 2 + Ag is balanced the coefficient of Ag NO 3 is? 2. (Unit 7) Balance the following equation: AgNO 3 + BaCl 2 AgCl +

More information

A. ATOMS Name Period Date 1. Complete the following table. Element Symbol Number of Protons. Number of electrons Ac 227

A. ATOMS Name Period Date 1. Complete the following table. Element Symbol Number of Protons. Number of electrons Ac 227 A. ATOMS Name Period Date 1. Complete the following table. Element Symbol Number of Protons Number of electrons Number of neutrons Atomic Number 25 53 11 12 35 45 Mass Number 39 89 33 75 Ac 227 2. Fill

More information

General Chemistry First Semester Final Exam Study Guide 60 multiple choice questions

General Chemistry First Semester Final Exam Study Guide 60 multiple choice questions General Chemistry First Semester Final Exam Study Guide 60 multiple choice questions 1. Define product. 2. Define reactant. 3. Label the products and reactants in the following chemical reactions: H 2

More information

Chemistry 20 Lesson 36 The Whole Enchilada

Chemistry 20 Lesson 36 The Whole Enchilada Unit I: Science 10 Review Chemistry 20 Lesson 36 The Whole Enchilada 1. Classify the substances as ionic (i), molecular (m), or acid (a) and provide the IUPAC name and the state of matter at SATP where

More information

CP Chemistry Semester 1 Final Test Review

CP Chemistry Semester 1 Final Test Review Mass in grams 10 20 30 40 50 CP Chemistry Semester 1 Final Test Review 1. Know the symbol and the power of 10 for the following metric prefixes: A. Mega M 10 6 D. deka da 10 1 G. milli m 10 6 B. kilo k

More information

REVIEW OF BASIC CHEMISTRY ANSWER KEY

REVIEW OF BASIC CHEMISTRY ANSWER KEY REVIEW OF BASIC CHEMISTRY ANSWER KEY 1. Name the following elements. Spelling counts: 2. Write the symbols for the following elements. H hydrogen sodium Na S sulphur phosphorus P Cl chlorine fluorine F

More information

(B) K2O potassium dioxide

(B) K2O potassium dioxide PRACTICE CHEMISTRY EOC TEST 1. Which substance is a conductor of electricity? (A) NaCl(s) (B) NaCl(l) (C) C6H12O6(s) (D) C6H12O6(l) 2. Which formula is correctly paired with its name? (A) MgCl2 magnesium

More information

Test Booklet. Subject: SC, Grade: HS 2008 MCAS High School Chemistry. Student name:

Test Booklet. Subject: SC, Grade: HS 2008 MCAS High School Chemistry. Student name: Test Booklet Subject: SC, Grade: HS 2008 MCAS High School Chemistry Student name: Author: Massachusetts District: Massachusetts Released Tests Printed: Tuesday June 19, 2012 1 Which of the following statements

More information

AP Chemistry Summer Assignment

AP Chemistry Summer Assignment AP Chemistry Summer Assignment 1) Name this compound: Cr 3 (PO 4 ) 2 a) Chromium Diphosphate b) Trichromium Phosphate c) Chromium (II) Phosphate d) Chromium (II) Diphosphate 2) How many significant figures

More information

Test Booklet. Subject: SC, Grade: HS 2009 End of Course Chemistry. Student name:

Test Booklet. Subject: SC, Grade: HS 2009 End of Course Chemistry. Student name: Test Booklet Subject: SC, Grade: HS 2009 End of Course Chemistry Student name: Author: Virginia District: Virginia Released Tests Printed: Tuesday April 23, 2013 1 Which of these would be best to measure

More information

Electronic Structure and Bonding Review

Electronic Structure and Bonding Review Name: Band: Date: Electronic Structure and Bonding Review 1. For electrons: a. What is the relative charge? b. What is the relative mass? c. What is the symbol? d. Where are they located in the modern

More information

Chemistry. End of Course. Student Name and Date

Chemistry. End of Course. Student Name and Date Chemistry HS End of Course Student Name and Date Baltimore City Public Schools Assessments End of Course High School Chemistry 1 Which of the following statements is 3 Which electron dot diagram NOT TRUE?

More information

Name May 2, 2012 Physical Behavior of Matter and Bonding Review

Name May 2, 2012 Physical Behavior of Matter and Bonding Review Name May 2, 2012 Physical Behavior of Matter and Bonding Review Base your answers to questions 1 through 3 on the information below. Starting as a gas at 206 C, a sample of a substance is allowed to cool

More information