2008 SOL Test. Name: Score: 50 / 50 points (100%)

Size: px
Start display at page:

Download "2008 SOL Test. Name: Score: 50 / 50 points (100%)"

Transcription

1 Name: Score: 50 / 50 points (100%) 2008 SOL Test Multiple Choice Identify the choice that best completes the statement or answers the question. C 1. Trial Concentration M M M M M A student performed a series of titrations to find the concentration of an unknown acid. The results of the titrations are shown in the data table. What is the mean of this set of data? a M c M b M d M C Take the average of the numbers (add all numbers and divide by 5) D 2. Iodine 131 is a radioactive isotope with a half life of 8 days. How many grams of a 64 g sample of iodine 131 will remain at the end of 24 days? a. 56 g c. 32 g b. 48 g d. 8 g D 24/8 = 3 So, divide 64 by 2 three times (64/2/2/2) = 8 B 3. Which of the following is the correct name for the compound MnF 3? a. Manganese fluoride(iii) c. Manganese(I) fluoride(iii) b. Manganese(III) fluoride d. Manganese(III) fluoride(iii) B It has to be b because you don t use roman numerals for the second part of the name (name should never end with a roman numeral) file:///f:/sol%20review%20topics/2008%20sol%20exam/2008_sol_exam.htm 1/17

2 A 4. The name of the salt formed by the neutralization of hydrochloric acid and sodium hydroxide is a. sodium chloride c. sodium chlorite b. sodium chlorate d. sodium hypochlorite A HCl + NaOH > NaCl + H 2 O and NaCl is sodium chloride (no polyatomic ion in this compound) C 5. If the quantity of heat lost or gained is ( H) = mass x xhange in T x specific heat, what is the amount of heat required to raise g of water from 22.00C to 100.0C? Specific heat of water is a joules c. 65,210 joules b. 6,521 joules d. 652,100 joules C = mass Change in T = = 78 specific heat = So, 200 x 78 x = B 6. The coefficients necessary to balance the equation correctly are a. a = 2, b = 1, c = 1, d = 2 c. a = 1, b = 1, c = 1, d = 1 b. a = 1, b = 2, c = 1, d = 2 d. a = 2, b = 2, c = 1, d = 1 A B By using these coefficients, we would have 1 Mg, 2 O, 4 H, and 2 Cl on both sides 7. A balloon is filled with 3.8 L of helium gas at STP. Approximately how many moles of helium are contained in the balloon? a mol c. 72 mol b mol d. 85 mol file:///f:/sol%20review%20topics/2008%20sol%20exam/2008_sol_exam.htm 2/17

3 A 3.8 L x = 0.17mol B C 8. Which of these elements has the smallest atomic radius? a. Beryllium (Be) c. Sodium (Na) b. Oxygen (O) d. Sulfur (S) B size decreases to top right side of periodic table while they increase to bottom left 9. If ml of a 0.96 M solution of acetic acid (C 2 H 4 O 2 ) are diluted to ml, what will be the approximate molarity of the final solution? a M c M b M d M C Dilution Problem (M 1 V 1 =M 2 V 2 ) (0.96)(250)=(M)(800) M=0.30M B 10. An atom contains 70 protons, 70 electrons, and 99 neutrons. What is the mass number? a. 239 c. 140 b. 169 d. 70 B Mass = Protons + Neutrons = =169 C 11. Which set of equipment would be mostuseful to determine the density of a liquid? a. Balance and periodic table c. Balance and graduated cylinder b. Periodic table and thermometer d. Graduated cylinder and thermometer C file:///f:/sol%20review%20topics/2008%20sol%20exam/2008_sol_exam.htm 3/17

4 Density = mass/volume, so balance for mass and graduated cylinder for volume D 12. Sodium chloride conducts electricity when dissolved in water. What type of bond is present in NaCl? a. Nonpolar covalent c. Hydrogen b. Polar covalent d. Ionic D ionic compounds are good electrolytes in water D 13. The picture shows a filtration process. Which of these is least likely to pass into the test tube? a. Dissolved gases c. Liquid solvents b. Dissolved salts d. Solid particles D solid particles (that aren t dissolved) will get trapped in the filter and will not pass through. A 14. Which of the following represents the Lewis dot diagram of ammonia (NH 3 )? file:///f:/sol%20review%20topics/2008%20sol%20exam/2008_sol_exam.htm 4/17

5 a. c. b. d. A correct too many H s pair of dots H only need 1 pair of dots H only need 1 D 15. After 1911, most scientists accepted the theory that the nucleus of an atom was very dense and very small and had a positive charge. What led scientists to accept this theory? a. Dalton s theory of the atom was over 100 years old. b. Scientists before 1911 used the scientific method of inquiry improperly. c. A new model proved that the quantum theory of the atom was inaccurate. d. Rutherford did an experiment firing alpha particles at a thin piece of gold foil. D a theories are not thrown out based on age; only if new ideas are better and prove old ideas wrong b the followed a similar model of what we use today c the quantum theory is more recent than 1911 (its the most modern one that we talked about) d Rutherford used the gold foil experiment and discovered the nucleus and that the atom is mostly empty space. B 16. A sodium atom has an electron configuration of. If the sodium atom becomes ionized, its new electron configuration will be the same as which element? a. Lithium c. Magnesium b. Neon d. Potassium file:///f:/sol%20review%20topics/2008%20sol%20exam/2008_sol_exam.htm 5/17

6 B It will lose an electron and become like a noble gas, Neon. 1s 2 2s 2 2p 6 B 17. Which reaction is correctly balanced? a. c. b. d. B Fe not balanced correct SO 4 not balanced Cu not balanced D 18. Which of the following particles has a positive one (+1) charge? a. Alpha c. Neutron b. Electron d. Proton D alpha is a Helium Nucleus (+2) electron is 1 neutron is neutral C 19. What is the mass of one mole of CO 2? a. 24 g c. 44 g b. 28 g d. 56 g C this means what is the molar mass: C = 12x1=12 O = 16x2=32 44 file:///f:/sol%20review%20topics/2008%20sol%20exam/2008_sol_exam.htm 6/17

7 C 20. According to the periodic table, Mg will most likely react with elements in which of these groups? a. 1 c. 17 b. 3 d. 18 D 21. C Mg is a metal and would have to react with a nonmetal and group 18 (noble gases) don t react. A sample of a gas is in a cylinder as shown. If the temperature is kept constant and the piston moves down to decrease the volume, the pressure increases because the gas particles a. expand b. lose velocity within the container c. become smaller d. collide more frequently with the container D pressure = collisions, less space means they will hit the walls more often A 22. Which of the following shows the correct number of atoms of each element in the formula Mg(NO 3 ) 2? a. 1 magnesium atom, 2 nitrogen atoms, and 6 oxygen atoms b. 1 magnesium atom, 2 nitrogen atoms, and 5 oxygen atoms c. 1 magnesium atom, 1 nitrogen atom, and 6 oxygen atoms d. 1 magnesium atom, 1 nitrogen atom, and 5 oxygen atoms A Like in math, the 2 gets distributed and multiplied through file:///f:/sol%20review%20topics/2008%20sol%20exam/2008_sol_exam.htm 7/17

8 D 23. A student is given a container of potassium nitrate crystals. In order to determine the exact mass of the potassium nitrate using a triple beam balance, he must know the a. mass of the filled container and the chemical formula for potassium nitrate b. mass of the filled container and the density of potassium nitrate c. volume of the filled container and the volume of the potassium nitrate d. mass of the empty container and the mass of the filled container D If you know the mass of the full and empty container, you can subtract the two numbers and the result would be the mass of the potassium nitrate. C 24. C 12 and C 13 are naturally occurring isotopes of the element carbon. C 12 occurs 98.89% of the time and C 13 occurs 1.108% of the time. What calculation should be used to determine the atomic mass of this element? a. c. b. d. C To determine the atomic mass of an isotope, you need to mutliply the mass given (number after symbol) by the decimal form of the percentage B 25. The general equation shown is a reaction that is an a. exothermic decomposition c. endothermic synthesis b. endothermic decomposition d. exothermic synthesis B energy on left means energy was added endothermic AB broke down decomposition file:///f:/sol%20review%20topics/2008%20sol%20exam/2008_sol_exam.htm 8/17

9 A 26. Examine the graph of the temperature of a compound versus heat added to the compound. Which of the following most likely happens as the compound is heated from point x to point y? a. The phase of the compound changes. b. The mass of the compound is increasing. c. The molecules of the compound lose potential energy. d. The molecules of the compound are breaking apart into atoms. A When a temperature verses heat graph flat lines, it means a phase change is occuring A 27. In order to determine the identity of a substance, a student listed the following properties. Which of the following is a chemical property? a. Oxidizes in air c. Attraction to a magnet b. Conducts an electric current d. Dissolves in water A oxidation will change the chemical make up of the substance D 28. The following results of a scientific study on water were found in a chemistry handbook. file:///f:/sol%20review%20topics/2008%20sol%20exam/2008_sol_exam.htm 9/17

10 What is the independent variable in the study? a. Molar mass c. Vapor pressure b. Melting point d. Temperature D the independent variable is graphed on the x axis and the dependent is graphed on the y, so as x changes, y changes as a function of x. A 29. Which of the following is a solid/solid solution? a. An alloy of gold and copper c. A strongly electrolytic acid b. A mixture of argon and krypton d. A neutralized base A alloys are a mixture of solids, plus gold and copper are solids D 30. Which of these compounds is most likely to contain an ionic bond? a. H 2 c. CH 4 b. SO 2 d. CaCl 2 D To be ionic, you need a metal and nonmetal file:///f:/sol%20review%20topics/2008%20sol%20exam/2008_sol_exam.htm 10/17

11 B 31. The composition of dry air is approximately 78% nitrogen, 21% oxygen, and 1% other gases. What is the partial pressure of nitrogen at standard atmospheric pressure (101.3 kpa)? a kpa c kpa b kpa d kpa B What is 78% of x 0.78 = C 32. A gas has a volume of ml at a pressure of mm Hg. If the temperature is held constant, what is the volume of the gas at a pressure of mm Hg? a ml c ml b ml d ml C Either use P 1 V 1 =P 2 V 2 or the V chart P T V ? A 33. Which of the following solutions will have the greatest concentration? a. 2 moles of solute dissolved in 1 liter of solution b. 0.3 mole of solute dissolved in 0.6 liter of solution c. 2 moles of solute dissolved in 10 liters of solution d. 0.1 mole of solute dissolved in 0.5 liter of solution A concentration = mol/l a = 2 b = 0.5 c = 0.2 d = 0.2 A 34. The chemical equation shown is an example of a a. single replacement reaction c. decomposition reaction file:///f:/sol%20review%20topics/2008%20sol%20exam/2008_sol_exam.htm 11/17

12 b. synthesis reaction d. double replacement reaction A Cu replaced Ag, only one element was replaced D 35. Which element is a noble gas? a. Fluorine (F) c. Nitrogen (N) b. Hydrogen (H) d. Xenon (Xe) D noble gases are in column 18 D 36. To determine if a reaction is exothermic, a student should use a a. ph probe c. pressure sensor b. motion sensor d. temperature probe D exothermic deals with heat being released and heat can be calculated if the temperature change is known A 37. What is the name of NH 4 OH? a. Ammonium hydroxide c. Nitrogen hydroxide b. Nitrogen oxygen hydride d. Ammonium oxygen hydride A This compound is made of two polyatomic ions, NH 4 + is ammonium and OH is hydroxide (plus most names we look at only have two words) B 38. A student hypothesizes that the solubility of a particular solute in water is nearly constant as temperature varies. The student can best test the hypothesis by doing which of the following? a. Researching the chemical properties of many different solutes b. Measuring the solubility of the solute at five different temperatures c. Drawing diagrams of the molecular structures of water and of the solute d. Measuring the solubility of several different solutes at a fixed temperature file:///f:/sol%20review%20topics/2008%20sol%20exam/2008_sol_exam.htm 12/17

13 B Make the temperature your independent variable; change the temperature and measure the solublity. B 39. Which set of coefficients will balance this equation? a. 3, 1, 1 c. 3, 2, 3 b. 2, 3, 2 d. 2, 6, 2 B choice b would give 2 P and 6 Br on each side A 40. The table shows the measurements of the volume and the pressure of a portion of a gas at constant temperature. After graphing, the data reveals that the volume is a. inversely proportional to pressure b. directly proportional to pressure c. inversely proportional to pressure squared d. directly proportional to pressure squared A As volume increases, pressure decreases; this is a classic inverse file:///f:/sol%20review%20topics/2008%20sol%20exam/2008_sol_exam.htm 13/17

14 relationship (plus Boyle s Law tells us that it is inverse) D 41. What is the correct name for the compound P 4 O 6? a. Phosphoric acid c. Phosphorus(IV) oxide b. Phosphorus oxide d. Tetraphosphorus hexoxide D two nonmetals that don t start with H, use prefixes A 42. To which category does this reaction belong? a. Synthesis c. Single replacement b. Decomposition d. Double replacement A Two combined into 1 sythesis C 43. As heat is added to a substance undergoing a phase change, the temperature remains constant because the energy is being used to a. break covalent bonds c. overcome intermolecular forces b. lower the specific heat capacity d. oppose electron cloud repulsions C The energy is used to break the forces holding the molecules together. The forces between molecules are intermolecular (within are intramolecular) B 44. How many moles of hydrogen gas are produced when mole of sodium is completely reacted? a mol H 2 c mol H 2 b mol H 2 d mol H 2 B Stoichiometry mole to mole use mole ratio file:///f:/sol%20review%20topics/2008%20sol%20exam/2008_sol_exam.htm 14/17

15 0.066 mol Na x = B 45. The accepted value for the specific heat of aluminum is Which of the following sets of specific heat values for aluminum, calculated from a prior experiment, has the greatest accuracy and precision? a. b. c. d. B We are looking for the numbers that are close to each other (precise) and close to (accurate) B 46. A 1.0 M aqueous solution of which substance would have the lowest ph? a. NH 3 c. Ba(OH) 2 b. HCl d. NaF B The lowest ph would be caused by the substance that is most acidic, and HCl is the most obvious substance that is an acid (starts with H). D 47. What is the chemical formula for iron(ii) phosphide? a. Fe 2 P c. FeP 2 b. Fe 2 P 3 d. Fe 3 P 2 D file:///f:/sol%20review%20topics/2008%20sol%20exam/2008_sol_exam.htm 15/17

16 The (II) meanss that Fe has a +2 charge and from periodic table we see that P has a 3 charge, so after switchy switchy Fe +2 P 3 becomes Fe 3 P 2 B 48. In a mixture of oxygen (O 2 ) and nitrogen gas (N 2 ), 80.0 percent of the total gas pressure is exerted by the nitrogen. If the total pressure is 2.0 atm, what pressure does the oxygen exert? a atm c atm b atm d. 1.6 atm B The two gases added together should equal 2.0 atm. Since nitrogen makes up 80%, that means nitrogen would be 2 x 0.80 = 1.6 atm. Therefore, oxygen is =0.4 atm C 49. Phosphoric acid, H3 PO 4, is neutralized by magnesium hydroxide, Mg(OH) 2, according to the equation shown. How many moles of water will be produced from the neutralization of 0.24 mole of H 3 PO 4? a mol c mol b mol d mol C stoichiometry moles to moles mole ratio 0.24 mol H 3 PO 4 x = 0.72 A 50. Which of the following is a balanced equation? a. H 2 + Br 2 > 2HBr c. H 2 + 2Br 2 > 2HBr b. H 2 + Br 2 > HBr d. 2H 2 + Br 2 > HBr A This one would result in 2 H and 2 Br on each side file:///f:/sol%20review%20topics/2008%20sol%20exam/2008_sol_exam.htm 16/17

17 file:///f:/sol%20review%20topics/2008%20sol%20exam/2008_sol_exam.htm 17/17

END OF COURSE CHEMISTRY

END OF COURSE CHEMISTRY VIRINI STNRS O LERNIN Spring 2008 Released Test EN O OURSE EMISTRY orm S0118, ORE 1 This released test contains 1 fewer test item (#1 49 only) than an original SOL EO hemistry test. Property of the Virginia

More information

Chemical vs. Physical Changes: 1. How can we define a chemical change? Give example reaction equations.

Chemical vs. Physical Changes: 1. How can we define a chemical change? Give example reaction equations. Name: Teacher: Date: Period: Directions: Try to answer EVERY question on here. Some questions have multiple parts. If you are confused or want to check your answers you should attend SGI with this sheet!

More information

7. 2. KOH (you need an acid or a base, this is a base) 8. 1. 76. All gold atoms have 79 protons and electrons, this is a +3 cation.

7. 2. KOH (you need an acid or a base, this is a base) 8. 1. 76. All gold atoms have 79 protons and electrons, this is a +3 cation. IB/SL Chemistry Name ANSWERS Test; Past Chemistry Regents Exams Most Frequently Missed Questions 1. 1. A HIGH PROBABLITY OF FINDING AN ELECTRON 2. 3. +8 (every atom of oxygen in the universe) 3. 2. LOW

More information

CHEMISTRY II FINAL EXAM REVIEW

CHEMISTRY II FINAL EXAM REVIEW Name Period CHEMISTRY II FINAL EXAM REVIEW Final Exam: approximately 75 multiple choice questions Ch 12: Stoichiometry Ch 5 & 6: Electron Configurations & Periodic Properties Ch 7 & 8: Bonding Ch 14: Gas

More information

SCH3UI-02 Final Examination Review (Fall 2014)

SCH3UI-02 Final Examination Review (Fall 2014) SCH3UI-02 Final Examination Review (Fall 2014) 1. Chlorine has an atomic number of 17. Create a Bohr Rutherford diagram of a Cl-35 atom. To achieve a stable arrangement, is this atom most likely to gain

More information

1. A mixture that contains more than one type of matter and is the same throughout is a mixture.

1. A mixture that contains more than one type of matter and is the same throughout is a mixture. 2nd Semester Benchmark Review Completion Complete each statement. 1. A mixture that contains more than one type of matter and is the same throughout is a mixture. 2. A mixture in which different samples

More information

PS-4.2 Explain how the process of covalent bonding provides chemical stability through the sharing of electrons.

PS-4.2 Explain how the process of covalent bonding provides chemical stability through the sharing of electrons. PS-4.1 Explain the role of bonding in achieving chemical stability. All of the noble gases are chemically stable A noble gas electron configuration (an outside energy level with 2 or 8 electrons) is chemically

More information

Atom nucleus (protons and neutrons) electron cloud (electrons)

Atom nucleus (protons and neutrons) electron cloud (electrons) Atom nucleus (protons and neutrons) electron cloud (electrons) Atomic Number equal to the number of protons Mass Number protons + neutrons Charge when # of electrons # of protons Negatively Charged Ion

More information

Chemistry Final Exam Review

Chemistry Final Exam Review Name: Date: Block: Chemistry Final Exam Review 2012-2013 Unit 1: Measurement, Numbers, Scientific Notation, Conversions, Dimensional Analysis 1. Write 0.000008732 in scientific notation 8.732x10-6 2. Write

More information

Q1. The chart shows the processes involved in the manufacture of nitric acid from ammonia.

Q1. The chart shows the processes involved in the manufacture of nitric acid from ammonia. Chemistry C2 Foundation and Higher Questions Q1. The chart shows the processes involved in the manufacture of nitric acid from ammonia. (a) Complete the word equation for the reaction that takes place

More information

neutrons are present?

neutrons are present? AP Chem Summer Assignment Worksheet #1 Atomic Structure 1. a) For the ion 39 K +, state how many electrons, how many protons, and how many 19 neutrons are present? b) Which of these particles has the smallest

More information

12.1 How do sub-atomic particles help us to understand the structure of substances?

12.1 How do sub-atomic particles help us to understand the structure of substances? 12.1 How do sub-atomic particles help us to understand the structure of substances? Simple particle theory is developed in this unit to include atomic structure and bonding. The arrangement of electrons

More information

General Chemistry: Semester 1 Final Review

General Chemistry: Semester 1 Final Review General Chemistry: Semester 1 Final Review Name Per Unit 1: Classification of Matter Define: chemistry, matter, element, compound, pure substance, homogeneous mixture, heterogeneous mixture, chemical change,

More information

Chemistry Distributed Practice Assessment

Chemistry Distributed Practice Assessment Name Hour Chemistry Distributed Practice Assessment Practice 2011 Practice Exam A **This END OF COURSE Practice Exam is a qualifier for all Exam Takers 1 Objective 1 Answer questions relating to atomic

More information

In the box below, draw the Lewis electron-dot structure for the compound formed from magnesium and oxygen. [Include any charges or partial charges.

In the box below, draw the Lewis electron-dot structure for the compound formed from magnesium and oxygen. [Include any charges or partial charges. Name: 1) Which molecule is nonpolar and has a symmetrical shape? A) NH3 B) H2O C) HCl D) CH4 7222-1 - Page 1 2) When ammonium chloride crystals are dissolved in water, the temperature of the water decreases.

More information

Bonding Practice Problems

Bonding Practice Problems NAME 1. When compared to H 2 S, H 2 O has a higher 8. Given the Lewis electron-dot diagram: boiling point because H 2 O contains stronger metallic bonds covalent bonds ionic bonds hydrogen bonds 2. Which

More information

Introduction to Ionic Bonds

Introduction to Ionic Bonds Introduction to Ionic Bonds The forces that hold matter together are called chemical bonds. There are four major types of bonds. We need to learn in detail about these bonds and how they influence the

More information

1. Where on the graph would I put the independent variable? 2. Where on the graph would I put the dependent variable?

1. Where on the graph would I put the independent variable? 2. Where on the graph would I put the dependent variable? Physical Science: Chemistry Study Guide Final Exam Test consists of 90 multiple choice questions. Introduction Unit Graphing, measuring, and metric system 1. Where on the graph would I put the independent

More information

Chapter 5 Notes: Ions and Ionic Compounds

Chapter 5 Notes: Ions and Ionic Compounds Chapter 5 Notes: Ions and Ionic Compounds Sec. 5.1 Simple Ions 1. Relate the electron configuration of an atom to its chemical reactivity. 2. Determine an atom s number of valence electrons, and use the

More information

Bonding Web Practice. Trupia

Bonding Web Practice. Trupia 1. If the electronegativity difference between the elements in compound NaX is 2.1, what is element X? bromine fluorine chlorine oxygen 2. Which bond has the greatest degree of ionic character? H Cl Cl

More information

Name: Regents Chemistry Review Packet A

Name: Regents Chemistry Review Packet A Name: Regents Chemistry Review Packet A 1. According to the modern model of the atom, the nucleus of an atom is surrounded by one or more A) electrons B) neutrons A) an alpha particle B) a beta particle

More information

Ms. Campbell Ionic Bonding Practice Regents Chemistry

Ms. Campbell Ionic Bonding Practice Regents Chemistry Name Student # Ms. Campbell Ionic Bonding Practice Regents Chemistry 1. Which element reacts with oxygen to form ionic bonds? 1) calcium 2) hydrogen 3) chlorine 4) nitrogen 2. Element X reacts with chlorine

More information

Summer Assignment Coversheet

Summer Assignment Coversheet Summer Assignment Coversheet Course: A.P. Chemistry Teachers Names: Mary Engels Assignment Title: Summer Assignment A Review Assignment Summary/Purpose: To review the Rules for Solubility, Oxidation Numbers,

More information

Chemistry Continuing Practice Packet

Chemistry Continuing Practice Packet Chemistry Continuing Practice Packet Mrs. Andrechek Webberville High School The best way to learn and remember chemistry is to practice. Check out the following websites: http://www.chemistrylecturenotes.com

More information

Chapter 11. Chemical Bonds: The Formation of Compounds from Atoms

Chapter 11. Chemical Bonds: The Formation of Compounds from Atoms Chapter 11 Chemical Bonds: The Formation of Compounds from Atoms 1 11.1 Periodic Trends in atomic properties 11.1 Periodic Trends in atomic properties design of periodic table is based on observing properties

More information

AP Chemistry Prep - Summer Assignment 2013

AP Chemistry Prep - Summer Assignment 2013 AP Chemistry Prep - Summer Assignment 2013 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which value has only 4 significant digits? a. 6.930 c. 8450

More information

7.4. Using the Bohr Theory KNOW? Using the Bohr Theory to Describe Atoms and Ions

7.4. Using the Bohr Theory KNOW? Using the Bohr Theory to Describe Atoms and Ions 7.4 Using the Bohr Theory LEARNING TIP Models such as Figures 1 to 4, on pages 218 and 219, help you visualize scientific explanations. As you examine Figures 1 to 4, look back and forth between the diagrams

More information

STOICHIOMETRY II UNIT

STOICHIOMETRY II UNIT STOICHIOMETRY II UNIT Assignment #1 (Conversions with compounds) 1. Convert 1.806 x 10 23 molecules of Cl2 to moles. 2. Convert 1000 molecules of P4O10 to moles. 3. Convert 360 grams of NH3 (ammonia gas)

More information

CST Practice Test. Multiple Choice Questions

CST Practice Test. Multiple Choice Questions CST Practice Test Young NAME CST Practice Test Multiple Choice Questions 1) At 1 atm and 298 K, which of the K a values listed below represents the strongest acid? 5) Which electron-dot symbol represents

More information

1. Balance the following equation. What is the sum of the coefficients of the reactants and products?

1. Balance the following equation. What is the sum of the coefficients of the reactants and products? 1. Balance the following equation. What is the sum of the coefficients of the reactants and products? 1 Fe 2 O 3 (s) + _3 C(s) 2 Fe(s) + _3 CO(g) a) 5 b) 6 c) 7 d) 8 e) 9 2. Which of the following equations

More information

Chapter 5: Ions & Ionic Compounds Study Guide

Chapter 5: Ions & Ionic Compounds Study Guide Name: Date: Chapter 5: Ions & Ionic Compounds Study Guide Directions: Work to answer the following review questions. You may use your notes and textbook as a reference. Answers to the review sheet will

More information

LORNE PARK SECONDARY SCHOOL SCH 3U PRACTICE FINAL EXAM

LORNE PARK SECONDARY SCHOOL SCH 3U PRACTICE FINAL EXAM Course: SCH 3U Teacher: J.N. Frink Jr. Length of Exam: 1.5 h Student Name: Number of pages: 8 (plus data tables) Total marks: 74 marks General Instructions: read instructions carefully look at the marks

More information

Chemistry Continuing Practice Packet

Chemistry Continuing Practice Packet Chemistry Continuing Practice Packet Mrs. Andrechek Webberville High School The best way to learn and remember chemistry is to practice. Check out the following apps: - Mahjong Chem - Formulas Lite - Atoms

More information

The Structure of an Atom

The Structure of an Atom CP Biology 2016 Name KEY UNIT 2A: Basic Chemistry Chapter 2: The Chemistry of Life 2.1 The Nature of Matter The Structure of an Atom Living things share a major fundamental similarity with nonliving matter.

More information

B) atomic number C) both the solid and the liquid phase D) Au C) Sn, Si, C A) metal C) O, S, Se C) In D) tin D) methane D) bismuth B) Group 2 metal

B) atomic number C) both the solid and the liquid phase D) Au C) Sn, Si, C A) metal C) O, S, Se C) In D) tin D) methane D) bismuth B) Group 2 metal 1. The elements on the Periodic Table are arranged in order of increasing A) atomic mass B) atomic number C) molar mass D) oxidation number 2. Which list of elements consists of a metal, a metalloid, and

More information

Test 8: Review Questions

Test 8: Review Questions Name: Thursday, February 14, 2008 Test 8: Review Questions 1. Based on bond type, which compound has the highest melting point? 1. CH OH 3. CaCl 3 2 2. C H 4. CCl 6 14 4 2. Which compound contains ionic

More information

PART I: MULTIPLE CHOICE (30 multiple choice questions. Each multiple choice question is worth 2 points)

PART I: MULTIPLE CHOICE (30 multiple choice questions. Each multiple choice question is worth 2 points) CHEMISTRY 123-07 Midterm #1 Answer key October 14, 2010 Statistics: Average: 74 p (74%); Highest: 97 p (95%); Lowest: 33 p (33%) Number of students performing at or above average: 67 (57%) Number of students

More information

11. 6 C is called carbon 12. It has 6 protons (as do all carbon atoms) and an atomic mass of exactly 12, meaning that this isotope has 6 neutrons.

11. 6 C is called carbon 12. It has 6 protons (as do all carbon atoms) and an atomic mass of exactly 12, meaning that this isotope has 6 neutrons. Pierce College Putman/Biol 241 Lecture 2: General Chemistry notes Universe is made of matter (physical substance) + energy Matter is made of atoms Atomic Structure & Isotopes 1. Atom is the smallest whole

More information

4. Aluminum chloride is 20.2% aluminum by mass. Calculate the mass of aluminum in a 35.0 gram sample of aluminum chloride.

4. Aluminum chloride is 20.2% aluminum by mass. Calculate the mass of aluminum in a 35.0 gram sample of aluminum chloride. 1. Calculate the molecular mass of table sugar sucrose (C 12 H 22 O 11 ). A. 342.30 amu C. 320.05 amu B. 160.03 amu D. 171.15 amu 2. How many oxygen atoms are in 34.5 g of NaNO 3? A. 2.34 10 23 atoms C.

More information

Physical Science 1 st Semester Final Exam Review Chapters 1-7, , 10.4

Physical Science 1 st Semester Final Exam Review Chapters 1-7, , 10.4 Physical Science 1 st Semester Final Exam Review Chapters 1-7, 8.3-8.4, 10.4 1. What procedures should be followed when working with chemicals in the lab? do not touch, taste, or inhale chemicals; check

More information

midterm1, 2009 Name: Class: Date:

midterm1, 2009 Name: Class: Date: Class: Date: midterm1, 2009 Record your name on the top of this exam and on the scantron form. Record the test ID letter in the top right box of the scantron form. Record all of your answers on the scantron

More information

Stoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2.

Stoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2. Stoichiometry 1 The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 01; (4) 02 2 A 44 gram sample of a hydrate was heated until the water of hydration was driven

More information

2. In a double displacement reaction, 3. In the chemical equation, H 2 O 2 H 2 + O 2, the H 2 O 2 is a

2. In a double displacement reaction, 3. In the chemical equation, H 2 O 2 H 2 + O 2, the H 2 O 2 is a What are the missing coefficients for the skeleton equation below? Al 2 (SO 4 ) 3 + KOH Al(OH) 3 + K 2 SO 4 2. In a double displacement reaction, A. 1,6,2,3 B. 2,12,4,6 C. 1,3,2,3 D. 4,6,2,3 E. 2,3,1,1

More information

CHAPTER 12 GASES AND THEIR BEHAVIOR

CHAPTER 12 GASES AND THEIR BEHAVIOR Chapter 12 Gases and Their Behavior Page 1 CHAPTER 12 GASES AND THEIR BEHAVIOR 12-1. Which of the following represents the largest gas pressure? (a) 1.0 atm (b) 1.0 mm Hg (c) 1.0 Pa (d) 1.0 KPa 12-2. Nitrogen

More information

Chemical Reactions in Water

Chemical Reactions in Water Chemical Reactions in Water Ron Robertson r2 f:\files\courses\1110-20\2010 possible slides for web\waterchemtrans.doc Acids, Bases and Salts Acids dissolve in water to give H + ions. These ions attach

More information

Chemical Reactions in Water Ron Robertson

Chemical Reactions in Water Ron Robertson Chemical Reactions in Water Ron Robertson r2 f:\files\courses\1110-20\2010 possible slides for web\waterchemtrans.doc Properties of Compounds in Water Electrolytes and nonelectrolytes Water soluble compounds

More information

Chemistry Review. No work = No credit. Entire document must be complete for credit to be awarded.

Chemistry Review. No work = No credit. Entire document must be complete for credit to be awarded. 1 Unit 1 1. States of matter: Phase 1. Solid 2. Liquid 3. Gas Chemistry Review No work = No credit. Entire document must be complete for credit to be awarded. Definite Shape (Yes or No?) Definite Volume

More information

Name: Thermochemistry. Practice Test B. General Chemistry Honors Chemistry

Name: Thermochemistry. Practice Test B. General Chemistry Honors Chemistry Name: Thermochemistry B Practice Test B General Chemistry Honors Chemistry 1 Objective 1: Use the relationship between mass, specific heat, and temperature change to calculate the heat flow during a chemical

More information

IB Chemistry. DP Chemistry Review

IB Chemistry. DP Chemistry Review DP Chemistry Review Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant Assessment statement Apply the mole concept to substances. Determine the number of particles and the amount

More information

Chapter 2. Atoms and Elements

Chapter 2. Atoms and Elements Chapter 2. Atoms and Elements John Dalton Robert Millikan J.J. Thomson Ernest Rutherford The Components of Matter Elements, Compounds, Mixtures Dalton s Atomic Theory Modern Atomic Theory Atomic and Mass

More information

CHM1 Review for Exam 9

CHM1 Review for Exam 9 Topics 1. Reaction Types a. Combustion b. Synthesis c. Decomposition d. Single replacement i. Metal activity series ii. Nonmetal activity series e. Double replacement i. Precipitates and solubility rules

More information

CHEMICAL QUANTITIES. Chapter 10

CHEMICAL QUANTITIES. Chapter 10 CHEMICAL QUANTITIES Chapter 10 What is a mole? A unit of measurement in chemistry 1 mole of a substance = 6.02 x 10 23 (Avagadro s number) representative particles of a substance Representative particle

More information

Answer Sheet Quarterly Review Questions

Answer Sheet Quarterly Review Questions Answer Sheet Quarterly Review Questions 1. Compared to the charge and mass of a proton, an electron has a. the same charge and a smaller mass b. the same charge and the same mass c. an opposite charge

More information

MIDTERM DATES: Atoms and the Periodic Table Define and identify elements and compounds

MIDTERM DATES: Atoms and the Periodic Table Define and identify elements and compounds Chemistry 10 with Mrs. Howland MIDTERM STUDY GUIDE FORMAT: 60 multiple choice (1 pt each) 5 short answer or calculation problem OPEN RESPONSE (8 pts each) MIDTERM DATES: MY MIDTERM Lab Safety and Equipment

More information

National 4/5 Chemistry Learning Outcomes (what you need to know ) Ah! (280) The Element of Surprise! Unit 1 Chemical Changes and Structure

National 4/5 Chemistry Learning Outcomes (what you need to know ) Ah! (280) The Element of Surprise! Unit 1 Chemical Changes and Structure National 4/5 Chemistry Learning Outcomes (what you need to know ) 123 Ah! (280) The Element of Surprise! Unit 1 Chemical Changes and Structure Unit 1 Revision Planner Topic Mini-test result /10 Topic revised

More information

Formulae, stoichiometry and the mole concept

Formulae, stoichiometry and the mole concept 3 Formulae, stoichiometry and the mole concept Content 3.1 Symbols, Formulae and Chemical equations 3.2 Concept of Relative Mass 3.3 Mole Concept and Stoichiometry Learning Outcomes Candidates should be

More information

Exploring Creation With Chemistry Table of Contents

Exploring Creation With Chemistry Table of Contents Exploring Creation With Chemistry Table of Contents MODULE #1: Measurement and Units...1 Introduction... 1 Experiment 1.1: Air Has Mass... 1 Experiment 1.2: Air Takes Up Space... 2 Units of Measurement...

More information

Chapter 7: Chemical Equations. Name: Date: Period:

Chapter 7: Chemical Equations. Name: Date: Period: Chapter 7: Chemical Equations Name: Date: Period: 7-1 What is a chemical reaction? Read pages 232-237 a) Explain what a chemical reaction is. b) Distinguish between evidence that suggests a chemical reaction

More information

Notes: Formula Mass and Percent Composition

Notes: Formula Mass and Percent Composition Notes: Formula Mass and Percent Composition Formula mass - the mass of one mole of a compound, atom or ion. -also called: gram formula mass, molecular mass, gram molecular mass, formula weight, gram formula

More information

Multiple Choice Identify the letter of the choice that best completes the statement or answers the question.

Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. Introduction to Chemistry Exam 2 Practice Problems 1 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1.Atoms consist principally of what three

More information

Unit 13 Practice Test

Unit 13 Practice Test Name: Class: Date: Unit 13 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The dissolution of water in octane (C 8 H 18 ) is prevented by.

More information

Final Semester 1 Review Sheet

Final Semester 1 Review Sheet Final Semester 1 Review Sheet Chapter 1&3 What is Chemistry Matter Mass Weight Scientific method o Observation Observation vs. inference (know the difference) Qualitative data Quantitative data o Hypothesis

More information

Chemistry Objectives

Chemistry Objectives Chemistry Objectives Matter, and Measurement 1. know the definition of chemistry and be knowledgeable 3-14 about specific disciplines of chemistry. 2. understand the nature of the scientific method and

More information

14A Atomic Structure. What is inside an atom? Modeling an atom. Thinking about the atom. Atomic Structure Investigation 14A.

14A Atomic Structure. What is inside an atom? Modeling an atom. Thinking about the atom. Atomic Structure Investigation 14A. Atomic Structure Investigation 14A 14A Atomic Structure What is inside an atom? We once believed that atoms were the smallest units of matter. Then it was discovered that there are even smaller particles

More information

Chemistry Scope & Sequence Student Outcomes (Objectives Skills/Verbs)

Chemistry Scope & Sequence Student Outcomes (Objectives Skills/Verbs) s 1 Measurement and Problem Solving 2-3 Weeks Measurements are subject to errors which need to be accounted for. 1. How do you accurately measure, using significant figures, in the metric system? Understand

More information

Part B 2. Answer all questions in this part.

Part B 2. Answer all questions in this part. Part B 2 Answer all questions in this part. Directions (51 65): Record your answers in the spaces provided in your answer booklet. Some questions may require the use of the 2011 Edition Reference Tables

More information

CHEMISTRY. Stoichiometry

CHEMISTRY. Stoichiometry Stoichiometry 1gram molecular mass 6.022 x 10 23 molecules Avagadro No of particles 6.022 x 10 23 particles MOLE 1 gram atomic mass 6.022 x 10 23 atoms Molar volume 22.4dm 3 at STP Equivalent mass of an

More information

4 Know the meaning of the SI units for volume, and and temperature

4 Know the meaning of the SI units for volume, and and temperature Competencies for CHEM 1010 (Introduction to Chemistry I) Competency Number Performances or Task The student will be able to: 1 Use the steps in the scientific method in experimentation. 2 Convert between

More information

Goals Pearson Education, Inc.

Goals Pearson Education, Inc. Goals 1. What is an ion, what is an ionic bond, and what are the general characteristics of ionic compounds? Be able to describe ions and ionic bonds, and give the general properties of compounds that

More information

Chemical Reactions Packet 2 Bonding-REG.

Chemical Reactions Packet 2 Bonding-REG. Chemical Reactions Packet 2 Bonding-REG. Ms. Rabenda Name: Period: 1 Lewis Dot Diagram Notes Illustrates the number of valence electrons. Valence electrons = Placed around the symbol of the element Helps

More information

Practice Test-Chem 123

Practice Test-Chem 123 Practice Test-Chem 123 1. Calculate the number of protons in the average potassium atom if the atomic weight of potassium is 39 amu and the atomic number of this element is 19. (a) 19 (b) 20 (c) 39 (d)

More information

21 st Century Chemistry Multiple Choice Question in Topic 3 Metals Unit 11

21 st Century Chemistry Multiple Choice Question in Topic 3 Metals Unit 11 21 st Century Chemistry Multiple Choice Question in Topic 3 Metals Unit 11 1. Consider the equation: 2Ca(s) + O 2 (g) 2CaO(s) Which of the following statements are correct? (1) Calcium and oxygen are reactants.

More information

Page Which element is a noble gas? (1) krypton (3) antimony (2) chlorine (4) manganese

Page Which element is a noble gas? (1) krypton (3) antimony (2) chlorine (4) manganese 1. Which characteristics describe most nonmetals in the solid phase? (1) They are malleable and have metallic luster. (2) They are malleable and lack metallic luster. (3) They are brittle and have metallic

More information

Factors that Affect the Rate of Dissolving and Solubility

Factors that Affect the Rate of Dissolving and Solubility Dissolving Factors that Affect the Rate of Dissolving and Solubility One very important property of a solution is the rate of, or how quickly a solute dissolves in a solvent. When dissolving occurs, there

More information

5. Which temperature is equal to +20 K? 1) 253ºC 2) 293ºC 3) 253 C 4) 293 C

5. Which temperature is equal to +20 K? 1) 253ºC 2) 293ºC 3) 253 C 4) 293 C 1. The average kinetic energy of water molecules increases when 1) H 2 O(s) changes to H 2 O( ) at 0ºC 3) H 2 O( ) at 10ºC changes to H 2 O( ) at 20ºC 2) H 2 O( ) changes to H 2 O(s) at 0ºC 4) H 2 O( )

More information

Ionic/covalent/metallic bonds

Ionic/covalent/metallic bonds .1..1 Ionic/covalent/metallic bonds 07 minutes 99 marks Page 1 of 7 Q1. (a) The diagram below represents a part of the structure of sodium chloride. The ionic charge is shown on the centre of only one

More information

TEST NAME: Chemistry ES 1.3 TEST ID: GRADE:11 SUBJECT:Life and Physical Sciences TEST CATEGORY: My Classroom

TEST NAME: Chemistry ES 1.3 TEST ID: GRADE:11 SUBJECT:Life and Physical Sciences TEST CATEGORY: My Classroom TEST NAME: Chemistry ES 1.3 TEST ID: 61960 GRADE:11 SUBJECT:Life and Physical Sciences TEST CATEGORY: My Classroom Chemistry ES 1.3 Page 1 of 10 Student: Class: Date: 1. The electron configuration of an

More information

Chemistry Ex Study. A. 6 protons B. 6 neutrons C. 12 electrons D. 12 electrons

Chemistry Ex Study. A. 6 protons B. 6 neutrons C. 12 electrons D. 12 electrons hemistry Ex Study Name: Date: 1. The Periodic Table of the Elements classifies all of the known elements into categories based on their physical and chemical properties. Repeating patterns within the table

More information

Chapter 5. Name: Class: Date: Multiple Choice Identify the choice that best completes the statement or answers the question.

Chapter 5. Name: Class: Date: Multiple Choice Identify the choice that best completes the statement or answers the question. Class: Date: Chapter 5 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. What is the pressure of the sample of gas trapped in the open-tube mercury manometer

More information

W1 WORKSHOP ON STOICHIOMETRY

W1 WORKSHOP ON STOICHIOMETRY INTRODUCTION W1 WORKSHOP ON STOICHIOMETRY These notes and exercises are designed to introduce you to the basic concepts required to understand a chemical formula or equation. Relative atomic masses of

More information

Unit 2: Quantities in Chemistry

Unit 2: Quantities in Chemistry Mass, Moles, & Molar Mass Relative quantities of isotopes in a natural occurring element (%) E.g. Carbon has 2 isotopes C-12 and C-13. Of Carbon s two isotopes, there is 98.9% C-12 and 11.1% C-13. Find

More information

IB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily.

IB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily. The Mole Atomic mass units and atoms are not convenient units to work with. The concept of the mole was invented. This was the number of atoms of carbon-12 that were needed to make 12 g of carbon. 1 mole

More information

2009 Chemistry Released SOL Test

2009 Chemistry Released SOL Test Name: Score: 50 / 50 points (100%) 2009 hemistry Released SOL Test Multiple hoice Identify the choice that best completes the statement or answers the question. D D 1. Which of these would be best to measure

More information

Chemical reactions. Classifications Reactions in solution Ionic equations

Chemical reactions. Classifications Reactions in solution Ionic equations Chemical reactions Classifications Reactions in solution Ionic equations Learning objectives Distinguish between chemical and physical change Write and balance chemical equations Describe concepts of oxidation

More information

Chemistry 1 Final Exam Study Guide Spring 2009

Chemistry 1 Final Exam Study Guide Spring 2009 Chemistry 1 Final Exam Study Guide Spring 2009 1. If a substance has a mass of 36.4 g and a volume of 8.500 ml, what is its density? 2. Which involves a chemical change? a. powdering sugar b. condensing

More information

Chemistry. The student will be able to identify and apply basic safety procedures and identify basic equipment.

Chemistry. The student will be able to identify and apply basic safety procedures and identify basic equipment. Chemistry UNIT I: Introduction to Chemistry The student will be able to describe what chemistry is and its scope. a. Define chemistry. b. Explain that chemistry overlaps many other areas of science. The

More information

Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test

Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test NAME Section 7.1 The Mole: A Measurement of Matter A. What is a mole? 1. Chemistry is a quantitative science. What does this term mean?

More information

Chemistry Summer School Pre-Test 2015

Chemistry Summer School Pre-Test 2015 NAME: 1. A material consists of pure sodium. How many types of atomic structures are present in this substance? (C.1.1) A. No atomic structures are present as this is a pure substance. B. One type of atomic

More information

CHEMISTRY STANDARDS BASED RUBRIC ATOMIC STRUCTURE AND BONDING

CHEMISTRY STANDARDS BASED RUBRIC ATOMIC STRUCTURE AND BONDING CHEMISTRY STANDARDS BASED RUBRIC ATOMIC STRUCTURE AND BONDING Essential Standard: STUDENTS WILL UNDERSTAND THAT THE PROPERTIES OF MATTER AND THEIR INTERACTIONS ARE A CONSEQUENCE OF THE STRUCTURE OF MATTER,

More information

4. Which of the following elements would you expect to behave most like magnesium? a) sodium b) calcium c) aluminum d) scandium

4. Which of the following elements would you expect to behave most like magnesium? a) sodium b) calcium c) aluminum d) scandium Name Answers to Sample Exam Questions #1 Chemistry 112 Multiple Choice 1. Which of the following statements best describes what happens when chocolate melts? a) This is a physical change, and the molecules

More information

SAI. Protons Electrons Neutrons Isotope Name. Isotope Symbol 131i S3 1. Atomic Number. Mass Number

SAI. Protons Electrons Neutrons Isotope Name. Isotope Symbol 131i S3 1. Atomic Number. Mass Number ATOMIC STRUCTURE AND THE PERIODIC TABLE CHAPTER 4 WORKSHEET PART A Given the following isotopes, determine the atomic number, the mass number, the number of protons, electrons and neutrons. Isotope Symbol

More information

Periodic Table Questions

Periodic Table Questions Periodic Table Questions 1. The elements characterized as nonmetals are located in the periodic table at the (1) far left; (2) bottom; (3) center; (4) top right. 2. An element that is a liquid at STP is

More information

CHEMICAL EQUATIONS and REACTION TYPES

CHEMICAL EQUATIONS and REACTION TYPES 31 CHEMICAL EQUATIONS and REACTION TYPES The purpose of this laboratory exercise is to develop skills in writing and balancing chemical equations. The relevance of this exercise is illustrated by a series

More information

Chapter 2. Section 2.1 The Formation of Ionic and Covalent Bonds Solutions for Selected Review Questions Student Edition page 63

Chapter 2. Section 2.1 The Formation of Ionic and Covalent Bonds Solutions for Selected Review Questions Student Edition page 63 Chapter 2 Chemical Bonding Section 2.1 The Formation of Ionic and Covalent Bonds Solutions for Selected Review Questions Student Edition page 63 10. Review Question (page 63) Predict whether the bond between

More information

Atomic Structure. 1. What is the total number of electrons in the 2p sublevel of a chlorine atom in the ground state? (1) 6; (2) 2; (3) 3; (4) 5.

Atomic Structure. 1. What is the total number of electrons in the 2p sublevel of a chlorine atom in the ground state? (1) 6; (2) 2; (3) 3; (4) 5. Atomic Structure 1. What is the total number of electrons in the 2p sublevel of a chlorine atom in the ground state? (1) 6; (2) 2; (3) 3; (4) 5. 2. Which is the electron configuration of an atom in the

More information

Chemistry 151 Final Exam

Chemistry 151 Final Exam Chemistry 151 Final Exam Name: SSN: Exam Rules & Guidelines Show your work. No credit will be given for an answer unless your work is shown. Indicate your answer with a box or a circle. All paperwork must

More information

Chemistry Diagnostic Questions

Chemistry Diagnostic Questions Chemistry Diagnostic Questions Answer these 40 multiple choice questions and then check your answers, located at the end of this document. If you correctly answered less than 25 questions, you need to

More information

Packet 4: Bonding. Play song: (One of Mrs. Stampfel s favorite songs)

Packet 4: Bonding. Play song:  (One of Mrs. Stampfel s favorite songs) Most atoms are not Packet 4: Bonding Atoms will, or share electrons in order to achieve a stable. Octet means that the atom has in its level. If an atom achieves a stable octet it will have the same electron

More information

PRACTICE WITH YOUR LEARNING ASSISTANT!

PRACTICE WITH YOUR LEARNING ASSISTANT! PRACTICE WITH YOUR LEARNING ASSISTANT! An object has a mass of 20.0 g. When it is submerged in a graduated cylinder initially containing 85.0 ml of water, the water level rises to 95.0 ml. What is the

More information

Chapter 1: Moles and equations. Learning outcomes. you should be able to:

Chapter 1: Moles and equations. Learning outcomes. you should be able to: Chapter 1: Moles and equations 1 Learning outcomes you should be able to: define and use the terms: relative atomic mass, isotopic mass and formula mass based on the 12 C scale perform calculations, including

More information