CHEMISTRY HONORS LEOCE Study Guide

Size: px
Start display at page:

Download "CHEMISTRY HONORS LEOCE Study Guide"

Transcription

1 BENCHMARK: N , 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 applied to science? How do we classify matter? KEY VOCABULARY: density, significant figures, scientific notation, dimensional analysis, compound, element, mixtures, homogeneous, heterogeneous 1. Be able to classify matter. 2. Be able to interpret data. 3. Be able to use correct significant figures 4. Be able to convert units. 1. After performing a density lab in which the student places an irregularly shaped object in a cylinder, the student records the following data. Volume and Mass Data Mass of sample Volume of water Volume of water + sample g 40.0 ml 43.0 ml What is the density based on the data above? Round your answer to the correct number of significant figures. A.478 g/ml B 6.82 g/ml C.147 g/ml D 2.10 g/m 2. How many significant figures are in the measurement of the mass of the sample? A 1 C 3 B 2 D 4 BENCHMARK: SC.912.P.8.4 ATOMIC STRUCTURE TEXTBOOK: Glencoe, Chemistry: Matter and Change, Chapters 4, 5 ESSENTIAL QUESTION: How are the electrons arranged? KEY VOCABULARY: valence electrons, electron configuration, orbital, sublevels, unpaired electrons, Aufbau diagram, isotopes 1. Identify maximum number of electrons in a sublevel. 2. Identify unpaired valence electrons in an atom and shared pairs in a molecule. 3. Identify valence electrons in a family or group. 4. Write electron configuration of a neutral atom for elements Version 1401 Page 1 of 7

2 5. Be able to identify an electron configuration in an Aufbau diagram. 6. Be able to identify the number of protons, neutrons, and electrons in a given atom, isotope, or ion. 7. Distinguish between the isotopes of elements. 1. What are the maximum number of electrons that can fill the p-sublevel? A 2 C 6 B 4 D 8 2. How many neutrons would be contained in an atom of the isotope uranium 238 ( U) A 238 neutrons C 52 neutrons B 92 neutrons D 146 neutrons BENCHMARK: SC.912.P.8.5 PERIODIC TABLE TEXTBOOK: Glencoe, Chemistry: Matter and Change, Chapter 6 ESSENTIAL QUESTION: What are the fundamental trends in the periodic table? KEY VOCABULARY: electronegativity, ionization energy, atomic radius, reactivity, family/group, period, valence electrons, halogens, alkali metal, alkaline earth metals 1. Place elements in order of atomic size. 2. Describe the trend for electronegativity. 3. Place elements in order of ionization energy. 4. Compare the characteristics of elements within the same family/group. 1. Which of the following atoms has the highest electronegativity? A Na B F C P D Rb 2.Which of the following elements has the largest atomic radius? A O C Se B S D Te IONIC COMPOUNDS BENCHMARK: SC.912.P.8.7 TEXTBOOK: Glencoe, Chemistry: Chapter 7 ESSENTIAL QUESTION: What are ionic compounds? KEY VOCABULARY: ionic bonding, anion, cation, ionic bond, polyatomic ions Version 1401 Page 2 of 7

3 1. Differentiate between anion and cation. 2. Define an ionic compound. 3. Write formulas or names for ionic compounds. 1. What is the formula for Calcium acetate? A CaC2H302 B Ca(C2H302)2 C Ca2C2H302 D CaC What is the formula for copper (II) chloride? A CuCl C Cu2 Cl2 B CuCl2 D Cu2Cl BENCHMARK: SC.912.P.8.7 TEXTBOOK: Glencoe, Chemistry: Chapter 8 COVALENT MOLECULES ESSENTIAL QUESTION: How are shapes and interactions between molecules explained? What is a covalent bond? KEY VOCABULARY: linear, tetrahedral, pyramidal, bent, trigonal planar, bond angles, polar and nonpolar molecule, Octet Rule, shared pairs, unshared pairs, VSEPR Theory, covalent bond, Lewis dot diagram, Lewis structure 1. Identify covalently bonded molecules. 2. Identify the molecular shape, bond angle, and polarity. 3. Write formulas or names for covalent molecules and acids 4. Identify a correct Lewis structure for a molecule. 1. What is the molecular shape of H2O and is it polar or nonpolar? 2. In accordance with the octet rule, what is the total number of shared pairs of electrons in the BMO of an oxygen molecule? A 1 C 3 B 2 D 4 Version 1401 Page 3 of 7

4 CHEMICAL REACTIONS BENCHMARK: SC.912.P.8.8 TEXTBOOK: Glencoe, Chemistry: Chapter 9 ESSENTIAL QUESTION: How do chemical changes occur when substances interact? KEY VOCABULARY: products, reactants, coefficients, combination/synthesis, decomposition, single replacement, double replacement, combustion, Law of Conservation of Matter, precipitate 1. Identify 5 types of chemical reactions. 2. Be able to complete and balance chemical reactions. 3. Understand Law of Conservation of Matter. 4. Identify the precipitate(s) and aqueous solution (aq) in a double replacement reaction. 1. Complete and balance the following reaction. NaOH(aq) + CuCl2 NaCl + A CuOH: 1,1,1,1 B CuOH: 2,1,2,1 C Cu(OH)2: 2,1,2,1 D Cu(OH)2: 1,1,1,1 3. In the complete combustion reaction of methane, CH4, what is the coefficient in front of the oxygen, O2? A 1 C 3 B 2 D 4 BENCHMARK: SC.912.P.8.9 TEXTBOOK: Glencoe, Chemistry: Chapters 10, 11 MOLAR CALCULATIONS ESSENTIAL QUESTION: How is stoichiometry used to calculate chemical quantities from balanced chemical equations? KEY VOCABULARY: representative particles, empirical formula, molecular formula, standard temperature and pressure (STP), percent composition, limiting reagent, excess reagent, mole, stoichiometry, mole ratio, molar mass, skeleton equation 1. Perform mole conversions. 2. Calculate percent composition. 3. Perform mass to mass, mass to volume, volume to volume, moles to mass stoichiometric calculations. 4. Solve for the limiting reactant. 5. Compare and identify empirical and molecular formula. Version 1401 Page 4 of 7

5 1. When 15.0 g of Copper (II) sulfate reacts with powered aluminum according to the reaction below, how many grams of Cu could be collected from this reaction? 3CuSO4 (aq) + 2Al (s) Al2(SO4)3 (aq) + 3Cu (s) A 23.5 g Cu B 5.97 g Cu C 52.9 g Cu D 31.5 g Cu 2. What is the number of representative particles in 0.50 moles of O2? A 1.2 x atoms C 3.0 x atoms B 1.2 x molecules D 3.0 x molecules BENCHMARK: SC.912.P.8.1, P.8.6, P.10.5 STATES OF MATTER AND INTERMOLECULAR FORCES TEXTBOOK: Glencoe, Chemistry: Chapter 12 ESSENTIAL QUESTION: How do changes in the kinetic energy of particles affect the state of substances? KEY VOCABULARY: solid, liquid, gas, vaporization, condensation, melting point, boiling point, sublimation, triple point, London dispersion force, hydrogen bonding, dipole dipole, critical point 1. Identify phase changes and interpret a phase diagram as shown above (page 429). 2. Identify the strengths of the intermolecular forces. 1. What are the forces of attraction in a nonpolar molecular substance? A dipole dipo B ionic bond C London dispersion D hydrogen bonding 2 What state of matter is the substance in section A? 3. What phase change occurs as a substance transitions from A directly to C? Version 1401 Page 5 of 7

6 GASES BENCHMARK: SC.912.P TEXTBOOK: Glencoe, Chemistry: Chapter 13 ESSENTIAL QUESTION: What are the properties of an ideal gas? KEY VOCABULARY: ideal gas law, quantitative, real gas, combined gas law 1. Perform calculations using the combined gas law and ideal gas law. 2. Know the assumptions and deviations of the ideal gas law. 3. Understand the relationship between temperature, volume, and pressure of gas. 1. What is the mass of 4.0L of oxygen gas (O2) at 4.0 ATM and 25 C? A 10.0g O2 B 15.2g O2 C 20.9g O2 D 25.4g O2 2. According to the reaction below, how many liters of waters are produced from 10.0 L of O2? A 10.0 L B 20.0 L 2H2 (g) + O2 (g) 2H2O (g) C 22.4 L D 40.0 L REACTION RATES BENCHMARK: SC.912.P TEXTBOOK: Glencoe, Chemistry, Chapter 16 Section 2 ESSENTIAL QUESTION: What factors affect the rate of reaction? KEY VOCABULARY: catalyst, concentration, rate of reaction, particle size, temperature 1. Identify the factors that affect the rate of reaction. 2. Describe the role of a catalyst in the rate of reaction. 3. Understand the relationship between temperature and frequency of collision. Version 1401 Page 6 of 7

7 1. Solid magnesium is reacted with hydrochloric acid, (HCL). Which choice below would react the fastest? A Magnesium ribbon in 1M HCl B Magnesium ribbon in 2M HCl C Magnesium powder in 1M HCl D Magnesium powder in 2M HCl 2. Which of the following is a characteristic of a catalyst? A increase the pressure of the reaction C slows down the rate B is consumed in the reaction D lowers the activation energy Version 1401 Page 7 of 7

Ch. 1: Introduction to Chemistry. Ch. 2: Matter and Change

Ch. 1: Introduction to Chemistry. Ch. 2: Matter and Change Review Sheet for Chemistry First Semester Final Refer to your class notes, worksheets, and the textbook to complete this review sheet. Study early so that you will have time to ask questions about what

More information

Memorize: Understand: Know how to:

Memorize: Understand: Know how to: NAME: CLASS PERIOD: REVIEW FOR HONORS CHEMISTRY SEMESTER 1 EXAM Memorize: Understand: Know how to: 1 SI units for different measurements (length, volume, number, mass, temperature, density) Definition

More information

First Semester Review Worksheet

First Semester Review Worksheet First Semester Review Worksheet 1. Determine the number of significant figures in each of the numbers below a. 1000 b. 4.567 c. 2030 d. 0.0240 e. 0.02677 f. 200.00 g. 4.65 x 10 4 h. 100.300 2. Convert

More information

Second Semester Chemistry Study Guide

Second Semester Chemistry Study Guide Second Semester Chemistry Study Guide All of the information on this review is fair game for the final Some information will be more prevalent on the test (Think about which topics we spent more time on

More information

Topics to Expect: Periodic Table: s, p, d, f blocks Metal, Metalloid, Non metal, etc. Periodic Trends, Family names Electron Configuration: Orbitals a

Topics to Expect: Periodic Table: s, p, d, f blocks Metal, Metalloid, Non metal, etc. Periodic Trends, Family names Electron Configuration: Orbitals a Chemistry Final Exam Review and Practice Chapters Covered ESSENTIALLY CUMMULATIVE List of Chapters: Ch: 6, 7, 8, 9, 10, 13, 14, 15, 16, 19, 20 Topics to Expect: Periodic Table: s, p, d, f blocks Metal,

More information

CP Chemistry Final Exam Review

CP Chemistry Final Exam Review I. Matter and Measurement 1) Chemical or physical property? CP Chemistry Final Exam Review Diamond is a very hard substance. The density of aluminum is 2.7 g/cm 3. Zinc reacts with acid. Copper melts at

More information

NCSD HIGH SCHOOL CHEMISTRY SCOPE AND SEQUENCE

NCSD HIGH SCHOOL CHEMISTRY SCOPE AND SEQUENCE UNIT Atomic Structure & Properties Periodic Table Bonding Chemical Reactions Moles / Stoichiometry Acids and Bases 15 Days 11 Days 16 Days 16 Days 26 Days 9 Days S T A N D A R D S H.1P.1 Explain how atomic

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

CP Chemistry Final Exam Review

CP Chemistry Final Exam Review I. Matter and Measurement 1) Chemical or physical property? CP Chemistry Final Exam Review Diamond is a very hard substance. The density of aluminum is 2.7 g/cm 3. Zinc reacts with acid. Copper melts at

More information

Unit 1 Atomic Structure

Unit 1 Atomic Structure Unit 1 Atomic Structure Unit 1 Text Questions 1.1 Atoms/Ions/Isotopes Problems Ch 5 Prob: 9,23,24,38 1.2 Average Atomic Mass Problems Ch 5 Prob: 15,17 1.3 Atomic Theory Development Problems Ch 5 Prob:

More information

Chemistry B Final Exam Review Packet Winter 2017

Chemistry B Final Exam Review Packet Winter 2017 Chemistry B Final Exam Review Packet Winter 2017 The final exam will count as approximately 15% of your final grade in Chemistry B. Exam Format: Multiple choice ~35 questions Free Response/Calculations:

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

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

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 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

VOCABULARY. Set #2. Set #1

VOCABULARY. Set #2. Set #1 VOCABULARY Set #1 1. Absolute zero 2. Accepted value 3. Accuracy 4. Celsius scale 5. Conversion factor 6. Density 7. Dimensional analysis 8. Experimental value 9. Gram 10. International system of units

More information

Unit 5: Bonding. Place a checkmark next to each item that you can do. If a sample problem is given, complete it as evidence.

Unit 5: Bonding. Place a checkmark next to each item that you can do. If a sample problem is given, complete it as evidence. Unit 5: Bonding Place a checkmark next to each item that you can do. If a sample problem is given, complete it as evidence. Intramolecular Forces: 1. I can define intramolecular forces and intermolecular

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

An Incomplete Study Guide For The First Semester Exam

An Incomplete Study Guide For The First Semester Exam An Incomplete Study Guide For The First Semester Exam Dr Mandes 1. 2. Which term refers to the number of protons in an atom? a. atomic mass b. atomic number c. isotopic mass d. proton number A cation is

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

Course: CP Chemistry Year: Teacher: L. Page. Unit 2: Matter and Energy Approximate Time Frame: # of Weeks 4

Course: CP Chemistry Year: Teacher: L. Page. Unit 2: Matter and Energy Approximate Time Frame: # of Weeks 4 Course: CP Chemistry Year: 2013 14 Teacher: L. Page Unit 1: Matter and Change Approximate Time Frame: # of Weeks 4 Biological, chemical and physical properties of matter result from the ability of atoms

More information

Chemistry Mid-Term Exam Review Spring 2017

Chemistry Mid-Term Exam Review Spring 2017 Unit 1 Measurement & Math Accuracy & Precision (recognizing given lab data) Density calculations Number of SFs in a measurement, Round answers to correct number of SFs Percent Error Unit conversions in

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

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

CHM 130: Final Exam Practice Problems

CHM 130: Final Exam Practice Problems CHM 130: Final Exam Practice Problems 1. Complete the following table: Isotope Mass number # of protons # of neutrons # of electrons strontium-90 neon-19 iron-55 2. Consider Figures A-F below: A B C D

More information

Chapter 6 PRETEST: Chemical Bonding

Chapter 6 PRETEST: Chemical Bonding Chapter 6 PRETEST: Chemical In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1.The charge on an ion is a. always positive.

More information

Chem 12: Chapters 10, 11, 12, 13, 14 Unit 3 Worksheet

Chem 12: Chapters 10, 11, 12, 13, 14 Unit 3 Worksheet C h e m i s t r y 1 2 U n i t 3 R e v i e w P a g e 1 Chem 12: Chapters 10, 11, 12, 13, 14 Unit 3 Worksheet 1. What is miscible? Immiscible? 2. What is saturated? Unsaturated? Supersaturated? 3. How does

More information

molality: m = = 1.70 m

molality: m = = 1.70 m C h e m i s t r y 1 2 U n i t 3 R e v i e w P a g e 1 Chem 12: Chapters 10, 11, 12, 13, 14 Unit 3 Worksheet 1. What is miscible? Immiscible? Miscible: two or more substances blend together for form a solution

More information

Chemistry Final Exam Review Multiple Choice Practice Questions

Chemistry Final Exam Review Multiple Choice Practice Questions Chemistry Final Exam Review Multiple Choice Practice Questions Work through the following problems. Do your work in a neat orderly fashion either on this page or on another sheet. 1. Which of the following

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 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

CHM 151 Practice Final Exam

CHM 151 Practice Final Exam CM 151 Practice Final Exam 1. ow many significant figures are there in the result of 5.52 divided by 3.745? (a) 1 (b) 2 (c) 3 (d) 4 (e) 5 2. ow many significant figures are there in the answer when 9.021

More information

Name: Midterm Review Date:

Name: Midterm Review Date: Name: Midterm Review Date: 1. Which statement concerning elements is true? A) Different elements must have different numbers of isotopes. B) Different elements must have different numbers of neutrons.

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

Oxnard Union High School District Chemistry Pacing Plan SEMESTER 1

Oxnard Union High School District Chemistry Pacing Plan SEMESTER 1 Oxnard Union High School District 2013-2014 Chemistry Pacing Plan SEMESTER 1 Unit and Number of Weeks Introduction to Chemistry 1 ½ weeks CA State Standard & Sub Concepts Investigation & Experimentation

More information

Honors Chemistry Semester 2 Final Exam MC Practice

Honors Chemistry Semester 2 Final Exam MC Practice Honors Chemistry Semester 2 Final Exam MC Practice Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1. What do the alkali metals all have in common?

More information

Ionic and Covalent Bonding

Ionic and Covalent Bonding 1. Define the following terms: a) valence electrons Ionic and Covalent Bonding the electrons in the highest occupied energy level always electrons in the s and p orbitals maximum of 8 valence electrons

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

Three (3) (Qatar only) The expected learning outcome is that the student will be able to:

Three (3) (Qatar only) The expected learning outcome is that the student will be able to: Course Information for 2014-2015 COURSE NUMBER: COURSE TITLE: CH1120 Chemistry COURSE DESCRIPTION: This in an introductory course designed to give students knowledge and understanding of the fundamental

More information

Chapter 6 and 7 Practice MC

Chapter 6 and 7 Practice MC Chapter 6 and 7 Practice MC MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Ammonium fluoride is considered which of the following? 1) A) molecular

More information

Chapter 6 Chemistry Review

Chapter 6 Chemistry Review Chapter 6 Chemistry Review Multiple Choice Identify the choice that best completes the statement or answers the question. Put the LETTER of the correct answer in the blank. 1. The electrons involved in

More information

TA Wednesday, 3:20 PM Each student is responsible for following directions. Read this page carefully.

TA Wednesday, 3:20 PM Each student is responsible for following directions. Read this page carefully. Name Chemistry 111 Section FINAL EXAM Total Points = TA Wednesday, 3:20 PM 200 Directions: December 12, 2007 1. Each student is responsible for following directions. Read this page carefully. 2. Write

More information

Volume of water g g? 50.0 ml ?

Volume of water g g? 50.0 ml ? MID-TERM EXAM REVIEW! KEY! Unit 1 Convert the following: 1.) 2.02 x 10 15 mg = g 2.02 x 10 15 mg 1 g = 2.02 x 10 12 g 1000 mg 2.) 1.29 x 10-7 m = cm 1.29 x 10-7 m 100 cm = 1.29 x 10-5 cm 1 m 3.) 13.5 dm

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

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

Questions 1-2 Consider the atoms of the following elements. Assume that the atoms are in the ground state. a. S b. Ca c. Ga d. Sb e.

Questions 1-2 Consider the atoms of the following elements. Assume that the atoms are in the ground state. a. S b. Ca c. Ga d. Sb e. AP Chemistry Fall Semester Practice Exam 5 MULTIPLE CHOICE PORTION: Write the letter for the correct answer to the following questions on the provided answer sheet. Each multiple choice question is worth

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

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

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

Test Booklet. Subject: SC, Grade: HS 2008 Grade High School Chemistry. Student name: Test Booklet Subject: SC, Grade: HS 2008 Grade High School Chemistry Student name: Author: North Carolina District: North Carolina Released Tests Printed: Tuesday July 17, 2012 1 How many protons and electrons

More information

NOTES: Unit 4: Bonding

NOTES: Unit 4: Bonding Name: Regents Chemistry: Mr. Palermo Student Version NOTES: Unit 4: Bonding Name: 1. Ion 2. Positive/Negative ion 3. Stable Octet 4. Diatomic Molecules 5. Electronegativity 6. Ionic Bond 7. Covalent Bond

More information

Name: Unit 1: Nature of Science

Name: Unit 1: Nature of Science Name: Unit 1: Nature of Science 1. Using the picture above, list lab safety rules that are being ignored. 2. What are the steps to the scientific method? 3. Convert the following into scientific notation:

More information

Plum Borough School District

Plum Borough School District Course Chemistry (A) 413 Grade(s) 10 Unit/Lesson Unit 1: Measurement and Data Interpretation Overview Qualititative and quantitative observations, rules of measurement, significant figures, scientific

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

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

Greene County Schools Course Sequence Guide. Lesson#/Day SPI Topics to be Covered Supplemental Resources 1(Ch.1) N/A Syllabus/Intro to Class

Greene County Schools Course Sequence Guide. Lesson#/Day SPI Topics to be Covered Supplemental Resources 1(Ch.1) N/A Syllabus/Intro to Class School: Subject: West Greene Chemistry Greene County Schools Course Sequence Guide Lesson#/Day SPI Topics to be Covered Supplemental Resources 1(Ch.1) N/A Syllabus/Intro to Class Classroom Handouts Pretest

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

g of CO 2 gas is at a temperature of 45 o C and a pressure of 125 kpa. What is the volume of the container? 11 L

g of CO 2 gas is at a temperature of 45 o C and a pressure of 125 kpa. What is the volume of the container? 11 L Name period AP Chemistry Unit 5 answers 1. A fixed quantity of gas at 23⁰C exhibits a pressure of 748 torr and occupies a volume of 10.3 L. Calculate the volume the gas will occupy if the temperature is

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

Chapter 11 Chemical Bonds: The Formation of Compounds from Atoms Advanced Chemistry Periodic Trends in Atomic Properties Learning Objective

Chapter 11 Chemical Bonds: The Formation of Compounds from Atoms Advanced Chemistry Periodic Trends in Atomic Properties Learning Objective Chapter 11 Chemical Bonds: The Formation of Compounds from Atoms Advanced Chemistry 11.1 Periodic Trends in Atomic Properties Discuss the atomic trends Metals are located on the left side of the periodic

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

UNIT 3 IB MATERIAL BONDING, MOLES & STOICHIOMETRY

UNIT 3 IB MATERIAL BONDING, MOLES & STOICHIOMETRY UNIT 3 IB MATERIAL Name: BONDING, MOLES & STOICHIOMETRY ESSENTIALS: Know, Understand, and Be Able To Apply the mole concept to substances. Determine the number of particles and the amount of substance

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

Unit 5: Bonding. Place a checkmark next to each item that you can do. If a sample problem is given, complete it as evidence.

Unit 5: Bonding. Place a checkmark next to each item that you can do. If a sample problem is given, complete it as evidence. Unit 5: Bonding Place a checkmark next to each item that you can do. If a sample problem is given, complete it as evidence. Intramolecular Forces: forces of attraction within the same molecule. Examples:

More information

AP Chemistry Summer Assignment

AP Chemistry Summer Assignment Name AP Chemistry Summer Assignment Welcome to AP chemistry! This summer assignment is intended to help you review the basic topics you learned in pre-ap chemistry that are crucial for your success in

More information

Chemical Reactions and Equations

Chemical Reactions and Equations Chemical Reactions and Equations 1991 B The molecular formula of a hydrocarbon is to be determined by analyzing its combustion products and investigating its colligative properties. (a) The hydrocarbon

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

Houston Community College System

Houston Community College System Houston Community College System Chemistry 1305/1405 FINAL EXAM REVIEW Vitamin A Helps form and maintain healthy teeth, skeletal and soft tissue, mucous membranes, and skin. CHEM 1305/1405 Final Exam PART

More information

Chemistry Curriculum Map

Chemistry Curriculum Map Timeframe Unit/Concepts Eligible Content Assessments Suggested Resources Marking Periods 1 & 2 Chemistry Introduction and Problem Solving using the Scientific Method Approach Observations Hypothesis Experiment

More information

Science. Smyth County Schools Curriculum Map Grade:11/12 Subject:Chemistry

Science. Smyth County Schools Curriculum Map Grade:11/12 Subject:Chemistry Standards Grade:11/12 Subject:Chemistry 1st Quarter SOL Ch 1a, 1b, 1c, 1e, 1g, 1i, 1h, 1f, 1d, 2a, 2b, 2c, 2d, 2e, 2f, 2g, 2h, 2i, 5c, 5e 2nd Quarter SOL Ch 4a, 4b, 3a, 3b, 3c, 3d, 3e, 5f Content Lab safety,

More information

Practice Multiple Choice

Practice Multiple Choice Practice Multiple Choice 1. A theory differs from a hypothesis in that a theory A. cannot be disproved C. always leads to the formation of a law B. represents an educated guess D. has been subjected to

More information

Final Review Packet. When 100% correct, you will receive a

Final Review Packet. When 100% correct, you will receive a Final Review Packet When 100% correct, you will receive a 15-point bonus sticker to place on the final exam. Deadline: Wednesday, Feb. 8. NO EXCEPTIONS!!!!!! Note! The Final Exam will be worth two tests

More information

Chemistry CRT Study Guide First Quarter

Chemistry CRT Study Guide First Quarter Number AL COS # 1. #1.0 Classify sodium chloride as an element, mixture, compound, or colloid. Compound 2. #1.0 Classify air as an element, mixture, compound, or colloid. Mixture 3. #1.0 Classify a blueberry

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

Multiple Choice. Multiple Choice

Multiple Choice. Multiple Choice 1. At what temperature in degree Celcius is the value in degree Fahrenheit twice of that in degree Celcius? A) 160 o C B) -24.6 o C C) 6.4 o C D) 22.2 o C E) 32 o C 2. The correct name for NaOCl is, A)

More information

3 When chemical compounds form, valence electrons are those that may be A lost only. C shared only. B gained only. D lost, gained, or shared.

3 When chemical compounds form, valence electrons are those that may be A lost only. C shared only. B gained only. D lost, gained, or shared. CLASS SET ID: A Chapter 12 Prep-Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1 A measure of the ability of an atom in a chemical compound to attract

More information

HADDONFIELD PUBLIC SCHOOLS Curriculum Map for Accelerated Chemistry

HADDONFIELD PUBLIC SCHOOLS Curriculum Map for Accelerated Chemistry Curriculum Map for Accelerated Chemistry 1st Marking Period 5.1.12.A.1, 5.1.12.A.2,, 5.1.12.A.3,, 5.1.12.B.1, 5.1.12.B.2, 5.1.12.B.3, 5.1.12.B.4, 5.1.12.C.1, 5.1.12.C.2, 5.1.12.C.3,, 5.1.12.D.1, 5.1.12.D.2,

More information

HONORS CHEMISTRY Putting It All Together II

HONORS CHEMISTRY Putting It All Together II NAME: SECTION: HONORS CHEMISTRY Putting It All Together II Calculations in Chemistry It s time to pull out your calculators! In the first review sheet, you were able to write formulas of compounds when

More information

Final Exam Review Chem 101

Final Exam Review Chem 101 Final Exam Review Chem 101 1. Know your nomenclature. a) Know how to go from the name to the formula. b) Know how to go from the formula to the name. 1. Ionic compounds (binary and ternary) a. Example:

More information

Unit 4:Chemical Bonding Practice Packet

Unit 4:Chemical Bonding Practice Packet Name: KEY Unit 4:Chemical Bonding Practice Packet 1. I can state the three types of chemical bonds. 2. I can state the number of valence electrons that an atom attains to be most stable. 3. I can state

More information

Chemistry Chapter 6 Test Review

Chemistry Chapter 6 Test Review Chemistry Chapter 6 Test Review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. A mutual electrical attraction between the nuclei and valence electrons

More information

GENERAL CHEMISTRY I CHEM SYSTEM FINAL EXAM VERSION A Fall 2016

GENERAL CHEMISTRY I CHEM SYSTEM FINAL EXAM VERSION A Fall 2016 GENERAL CHEMISTRY I CHEM 1411 SYSTEM FINAL EXAM VERSION A Fall 2016 Departmental Final Exam General Chemistry I, CHEM 1411 Fall 2016 VERSION A Part I: 35 Multiple Choice (2 pts each). Directions: Select

More information

Student Name: Teacher: Date: District: NCGaston. Assessment: 9_12 Science Chemistry Exam 3. Description: Chemistry Mock Final Exam

Student Name: Teacher: Date: District: NCGaston. Assessment: 9_12 Science Chemistry Exam 3. Description: Chemistry Mock Final Exam Student Name: Teacher: Date: District: NCGaston Assessment: 9_12 Science Chemistry Exam 3 Description: Chemistry Mock Final Exam 2014-15 Form: 301 1. Shown below is a model of the structure of atom X.

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

Structure and IM Forces Practice Problems

Structure and IM Forces Practice Problems Structure and IM Forces Practice Problems 1) An ionic compound 1) A) hasa net positive charge. B) hasa net negative charge. C) contains only cations. D) contains covalent bonds between anions and cations.

More information

Curriculum Mapping Chemistry I 1 st Nine Weeks

Curriculum Mapping Chemistry I 1 st Nine Weeks Curriculum Mapping Chemistry I 1 st Nine Weeks Days Standard Skills Resources Vocabulary Assessments August C.1.2 INTRODUCTION TO CHEMISTRY: Students will use lab safety rules. Students will recall lab

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

Chemistry 116 Pre-test Some questions from Chem 115 Final exam; Fall 2014

Chemistry 116 Pre-test Some questions from Chem 115 Final exam; Fall 2014 1. The mass of a sample is 550 milligrams. Which of the following expresses that mass in kilograms? a. 5.5 10 8 kg b. 5.5 10 5 kg c. 5.5 10 4 kg d. 5.5 10 6 kg e. 5.5 10 1 kg 2. Select the answer that

More information

2. Which is NOT considered matter? (A) air (B) lead (C) sugar (D) sunlight. 4. Which of the following is a metalloid? (A) Se (B) Sr (C) Si (D) Sn

2. Which is NOT considered matter? (A) air (B) lead (C) sugar (D) sunlight. 4. Which of the following is a metalloid? (A) Se (B) Sr (C) Si (D) Sn Midterm Review Packet ANSWER KEY 01/26/2014 Multiple Choice Question 1. Which part of an atom is positively charged? (A) proton (B) neutron (C) electron (D) shells 2. Which is NOT considered matter? (A)

More information

Covalent Bonding. In nature, only the noble gas elements exist as uncombined atoms. All other elements need to lose or gain electrons

Covalent Bonding. In nature, only the noble gas elements exist as uncombined atoms. All other elements need to lose or gain electrons In nature, only the noble gas elements exist as uncombined atoms. They are monatomic - consist of single atoms. All other elements need to lose or gain electrons To form ionic compounds Some elements share

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

Name: Your final exam is on in room. Bring your text book, calculator, #2 pencils, and your review materials.

Name: Your final exam is on in room. Bring your text book, calculator, #2 pencils, and your review materials. Name: Final Exam Review Your final exam is on in room. Bring your text book, calculator, #2 pencils, and your review materials. Multiple Choice Section 1. Define intensive and extensive properties and

More information

Chemistry 111 Syllabus

Chemistry 111 Syllabus Chemistry 111 Syllabus Chapter 1: Chemistry: The Science of Change The Study of Chemistry Chemistry You May Already Know The Scientific Method Classification of Matter Pure Substances States of Matter

More information

Cartoon courtesy of NearingZero.net. Chemical Bonding and Molecular Structure

Cartoon courtesy of NearingZero.net. Chemical Bonding and Molecular Structure Cartoon courtesy of NearingZero.net Chemical Bonding and Molecular Structure Chemical Bonds Forces that hold groups of atoms together and make them function as a unit. 3 Major Types: Ionic bonds transfer

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

generate testable Students will be able to investigations. Biology 1 2 (can be conclusions. reveal relationships identify sources of error higher.

generate testable Students will be able to investigations. Biology 1 2 (can be conclusions. reveal relationships identify sources of error higher. Honors Chemistry Essential Questions: 1. How can one explain the structure, properties, and interactions of matter? Communication of Scientific Information Anchor Standard 1: Students will be able to design,

More information

Review for Final Exam

Review for Final Exam Review for Final Exam Chapter 1 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Types of Changes A physical change does not alter the composition or identity

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

Bonding. Honors Chemistry 412 Chapter 6

Bonding. Honors Chemistry 412 Chapter 6 Bonding Honors Chemistry 412 Chapter 6 Chemical Bond Mutual attraction between the nuclei and valence electrons of different atoms that binds them together. Types of Bonds Ionic Bonds Force of attraction

More information

MATTER AND ITS PROPERTIES

MATTER AND ITS PROPERTIES FINAL REVIEW MATTER AND ITS PROPERTIES VIDEO ATOM Smallest unit of an element that maintains the chemical identity of that element. ELEMENT A pure substance that cannot be broken down into simpler, stable

More information