chemistry 1a study guide examination for acceleration (ea)/credit … ·  · 2017-07-19chemistry...

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Chemistry 1A Study Guide Examination for Acceleration (EA)/Credit by Exam (CBE)

The exam you are interested in taking is designed to test your proficiency in the relevant subject matter. You should be thoroughly familiar with the subject matter before you attempt to take the exam. This EA/CBE Study Guide can help you prepare for the exam by giving you an idea of what you need to review. You can check your familiarity level by reviewing the Texas Essential Knowledge and Skills (TEKS) for this course (see below). To refine your skills, you can refer to any of the state-adopted textbooks.

Texas Essential Knowledge and Skills (TEKS) Every question that appears on this exam is derived from the knowledge and skills statements and student expectations within the Texas-mandated standards, the Texas Essential Knowledge and Skills (TEKS). You can view the TEKS for this exam online via the following link: http://ritter.tea.state.tx.us/rules/tac/chapter112/ch112c.html#112.35. Refer to section (c), Knowledge and skills, 1A–12C. Throughout this guide, you’ll see TEKS references. These refer to the numbers listed under (c) Knowledge and skills; for example, 1A or 3B. Note: Coverage of the TEKS is split between Chemistry 1A and 1B; so those TEKS not covered in this exam are covered in the Chemistry 1B EA/CBE. Materials Needed You will need to bring a #2 pencil to complete the exam. You are also allowed to bring and use a graphing calculator. You will receive a computer-graded answer sheet when you arrive at the testing center. You will be provided a formula sheet and periodic table with your exam. The formula sheet and periodic table are also included at the end of this Study Guide for your review. Exam Structure You will be allowed 3 hours to complete this exam. The exam consists of 50 multiple-choice questions worth 2 points each for a total of 100 points. The exam consists of the following 5 parts:

Part 1: Scientific Methods and Processes (15 questions) Part 2: Matter (10 questions) Part 3: The Periodic Table (10 questions) Part 4: Atoms (5 questions) Part 5: Chemical Bonds (10 questions)

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Scholastic Honesty When you arrive at the testing center, you will be asked to carefully read the exam rules and sign a statement agreeing to take the exam in accordance with the rules. This is called the Examinee’s Certification. The following is a copy of these rules:

Examinee’s Certification This certification must be signed before the exam is administered and then returned with the completed examination attached, or credit for the exam will not be given. Scholastic dishonesty is a serious academic violation that will not be tolerated. Scholastic dishonesty encompasses, but is not limited to: • copying from another student’s work; • using an unauthorized testing proctor or taking the exam at an unauthorized testing

location; • using materials not authorized by a testing proctor; • possessing materials that are not authorized by a testing proctor, such as lessons, books, or

notes; • knowingly using or soliciting, in whole or part, the contents of an unadministered test; • collaborating with or seeking aid from another student without authorization during the

test; • substituting for another person, or permitting another person to substitute for oneself, in

taking a course test or completing any course-related assignment; • using, buying, stealing, or transporting some or all of the contents of an unadministered

test, test rubric, homework answer, or computer program. Evidence of scholastic dishonesty will result in a grade of F on the examination and an F in the course (if applicable).

At the testing center, you will be asked to sign a statement that says you have read the above and agree to complete the examination with scholastic honesty.

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General Study Tips The bulleted lists and sample questions in this study guide can assist you in preparing for the exam. It is a fairly complete guide, but does not cover every item on the test. Ultimately, you should use the TEKS to guide your exam preparation. Additional Study Tips The following information provides direction for your studies. For each part, you will find study tips and sample questions to give you a general idea of the types of questions you can expect to see on the exam. Part 1: Scientific Methods and Processes This part relates to your knowledge of lab safety, the definition of science and its limits, scientific methods, scientific data, scientific thinking, and the historical contributions of scientists. It includes 15 questions worth 2 points each, for a total of 30 points. Study Tips for Part 1 This part relates to TEKS 1A–3F. Familiarize yourself with those TEKS, and then be prepared to demonstrate knowledge of the following topics:

• Safe lab practices, including common safety symbols and why they are important • Proper disposal of lab materials • Definition of science (including its limits) • How to formulate hypotheses • Difference between scientific hypotheses and scientific theories • How to design an experiment using the scientific method • Characteristics of a valid scientific experiment, including an understanding of the terms

control, dependent variable, and independent variable • How to select appropriate equipment for a scientific experiment • How to make proper measurements • Difference between accuracy and precision • Difference between quantitative and qualitative data • Drawing conclusions and trends from data • Thinking critically about and analyzing scientific explanations • “False balance,” as it applies to the use of scientific messages by the media • How scientific research and contributions can impact society and the environment • History of biology; particularly with regard to the contributions of Aristotle, Robert

Hooke, Leonardo da Vinci, Francis Crick, James Watson, Charles Darwin, and Carl Linnaeus

• Cell theory; particularly, the three major ideas associated with the theory

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Sample Questions for Part 1 The following are sample questions. You can find the correct answers listed after the questions, but try answering the questions without looking at the answers first to check your comprehension. DIRECTIONS: Select the BEST response to each of the following questions.

1. When disposing of leftover acids from a lab experiment, which of the following actions

is a reasonable procedure to perform? A. Mix the leftover acids with baking soda. B. Soak the leftover acids with paper towels. C. Pour the leftover acids back into their original containers. D. Flush the leftover acids down the sink with plenty of water.

2. In 1869, Russian chemist _____ published the first periodic table of chemical elements and predicted the existence of elements that had yet to be discovered. A. Niels Bohr B. John Dalton C. Ernest Rutherford D. Dmitry Mendeleev

[1: A; 2: D]

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Part 2: Matter This part relates to your knowledge of matter. It includes 10 questions worth 2 points each, for a total of 20 points. Study Tips for Part 2 This part relates to TEKS 4A–4D. Familiarize yourself with those TEKS, and then be prepared to demonstrate knowledge of the following topics: Characteristics of Matter

• Define matter. • Describe the properties of solids, liquids, and gases and be able to distinguish between

them. • Differentiate between extensive and intensive physical properties. • Understand mass as a measure of the amount of matter in an object. • Recognize characteristics of each state of matter. • Identify the properties of elements, mixtures, and compounds and be able to distinguish

between them. • Identify the characteristics and qualities of pure substances and be able to distinguish

between pure substances and mixtures. • Distinguish between heterogeneous and homogeneous mixtures. • Distinguish between physical and chemical changes. • Define and apply the law of conservation of mass.

Chemical Reactions

• Identify and determine whether a chemical reaction or a physical change has taken place. • Write and understand chemical equations, word equations, and formula equations. • Write a formula equation from a word equation. • Balance a chemical equation. • Interpret a balanced chemical equation. • Identify chemical reactions; e.g., combustion, oxidation, synthesis, decomposition,

single-replacement, double-replacement, acid–base. • Predict the reactants or products of a chemical reaction. • Understand the importance of classifying chemical reactions.

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Sample Questions for Part 2 The following are sample questions. You can find the correct answers listed after the questions, but try answering the questions without looking at the answers first to check your comprehension. DIRECTIONS: Select the BEST response to each of the following questions.

1. When an iron nail rusts or the bright, copper surface of a penny corrodes when exposed

to air, what type of chemical reaction has occurred? A. Oxidation B. Combustion C. Decomposition D. Single-replacement

2. Physical properties of matter can be categorized as either intensive or extensive. Which of the following is an extensive property?

A. How easily a substance can be scratched B. The ability of a substance to allow the flow of energy or electricity C. A measurement of the gravitational force of attraction of the Earth acting on an object D. The temperature at which the vapor pressure of a liquid is equal to the pressure on the

liquid (generally atmospheric pressure)

[1: A; 2: D]

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Part 3: The Periodic Table This part relates to your knowledge of the periodic table of the elements. It includes 10 questions worth 2 points each, for a total of 20 points. Study Tips for Part 3 This part relates to TEKS 5A–5C. Familiarize yourself with those TEKS, and then be prepared to demonstrate knowledge of the following topics:

• Know the history of the periodic table of the elements; particularly, the contributions of Mendeleev and Moseley.

• Understand how the physical and chemical properties of elements influenced the development of the periodic table.

• Know how the elements are arranged in the periodic table. • Identify groups (families) of elements within the periodic table and understand the

characteristics of each. • Identify relationships between elements in the same period, group, and block. • Describe how protons, electrons, and neutrons as represented in the periodic table. • Determine the electronegativity of elements from a (provided) periodic table of

electronegativity. • Use the periodic table to identify an element’s oxidation number. • Describe the different trends in elements that can be noted from the periodic table. • Describe the periodic trends of ionization energy, electronegativity, and atomic radii.

Sample Questions for Part 3 The following are sample questions. You can find the correct answers listed after the questions, but try answering the questions without looking at the answers first to check your comprehension. DIRECTIONS: Select the BEST response to each of the following questions.

1. In the periodic table, the _____ are the group of inert elements.

A. halogens B. noble gases C. alkali metals D. transition metals

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2. Which shaded area of the following Periodic Table of the Elements shows elements that undergo the FEWEST chemical reactions?

A. Q B. R C. S D. T

[1: B; 2: D]

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Part 4: Atoms This part relates to your knowledge of atomic theories, atomic structure, and mathematical relationships on the atomic level. It includes 5 questions worth 2 points each, for a total of 10 points. Study Tips for Part 4 This part relates to TEKS 6A–6E. Familiarize yourself with those TEKS, and then be prepared to demonstrate knowledge of the following topics:

• Understand the basic characteristics of modern atomic theory. • Know Schrödinger’s proposition that electrons behave as waves. • Understand Dalton’s postulates. • Describe Thomson’s discovery of electron properties. • Describe Rutherford’s famous experiment and what he observed. • Understand Bohr’s findings on the nuclear atom. • Be familiar with the electromagnetic spectrum and color associations with energy. • Demonstrate mathematical relationships between energy, frequency, and wavelength of

light. • Perform calculations using Planck’s constant and the speed of light. • Perform calculations to determine the average atomic mass of an element using isotopic

composition. • Know electron configurations and electron orbital notation. • Write Lewis dot structures for atoms, ionic compounds, and covalent compounds. • Apply the principles of Lewis dot structures to predict the ratio of elements in a

compound.

Sample Questions for Part 4 The following are sample questions. You can find the correct answers listed after the questions, but try answering the questions without looking at the answers first to check your comprehension. DIRECTIONS: Select the BEST response to each of the following questions.

1. In the visible spectrum of light, which color is associated with the LEAST amount of

energy? A. Red B. Blue C. White D. Yellow

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2. What would be the correct Lewis dot structure for NaAr?

A.

B.

C. D. Argon does not bond with sodium.

[1: A; 2: D]

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Part 5: Chemical Bonds This part relates to your knowledge of chemical formulas nomenclature, the nature of chemical bonding, and the geometry of molecules. It includes 10 questions worth 2 points each, for a total of 20 points. Study Tips for Part 5 This part relates to TEKS 7A–7E. Familiarize yourself with those TEKS, and then be prepared to demonstrate knowledge of the following topics: Chemical Formulas and Nomenclature

• Know the International Union of Pure and Applied Chemistry (IUPAC) nomenclature rules for naming ionic compounds.

• Understand what information chemical formulas provide and how to write chemical formulas for polyatomic ions and transition metals.

• Identify chemical names from chemical formulas. • Identify polyatomic ions that are cations.

Chemical Bonds • Use Lewis dot structures to predict the ratio of elements in a compound. • Use differences in electronegativity to identify ionic and covalent bonds. • Know and understand the reasons for the physical properties of ionic compounds. • Understand the types of atoms that are involved in covalent bonds. • Predict the behavior of electrons in polar and non-polar covalent bonds. • Explain the difference between ionic and covalent bonds. • Understand the physical properties of metals and explain the reason for these properties. • Explain the behavior of valence electrons in a metallic bond. • Explain and identify the properties of alloys. • Understand thermal electrical conductivity, malleability, and ductility.

Geometry of Molecules

• Explain and apply the Valence Shell Electron-Pair Repulsion (VSEPR) theory. • Predict the number of unshared pairs or electrons in the central atom of a molecule. • Know the angles between bonding atoms in each of the molecular shapes; specifically, be

able to identify the three-dimensional shapes of chemicals like methane and carbon dioxide.

• Predict whether a molecule will be polar or non-polar based on its shape. • Know the relationship between repulsion of pairs of electrons and the shape of a

molecule.

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Sample Questions for Part 5 The following are sample questions. You can find the correct answers listed after the questions, but try answering the questions without looking at the answers first to check your comprehension. DIRECTIONS: Select the BEST response to each of the following questions.

1. What is the correct chemical name for NH4C2H3O2?

A. Nitrogen biacetate B. Ammonium acetate C. Carbon hydrogen nitrate D. Nitrogen hydrogen carbonate

2. What three-dimensional shape will CO2 have? A. Bent B. Linear C. Pyramidal D. Tetrahedral

[1: B; 2: B]

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Chemistry Formula Chart General Formulas

Density =massvolume

         ! =  !!

Percent  yield =actual  yield

theoretical  yield  ×  100%

 Pressure  ×  Volume = moles  ×  !  ×  Temperature          !" = !"#

Heat = mass  ×  specific  heat  constant  ×  change  in  Kelvin          ! = !"∆!

Velocity = frequency  ×  wavelength          ! = !"  

Atomic Structure

ℎ = Planck!s  constant = 6.63  x  10!!"  J  ×  s amu = atomic  mass  unit  

!lpha  particle =  ! = 42!"  

Energy = Planck!s  constant frequency !!!!"!# = ℎ!

Behavior of Gases

The  Combined  Gas  Law:  Initial  pressure (Initial  volume)Initial  moles (Initial  temperature)

=(Final  pressure)(Final  volume)(Final  moles)(Final  temperature)

         !!!!!!!!

=!!!!!!!!

Charles’s  Law: Initial  volume

Initial  temperature=

Final  volumeFinal  temperature

         !!!!=!!!!

Ideal  Gas  Constant:  

 ! = 8.31!  ×  !"#!  ×  !"#

         or          0.0821!  ×  !"#!  ×  !"#

Specific Heat Values for the States of Water

Ice = 2090  J/kg  °C Water = 4186  J/kg  °C Steam = 2010 J kg °C

Thermochemistry

Heat  gained  or  lost = mass  ×   specific  heat  ×   Change  in  temperature          ! = !"∆!

Solutions

Molarity =  moles  of  soluteLiter  of  solution

     ! =!"#!

         Concentration =  amount  of  substanceVolume  of  solution

       !! =  !!!

Molality =number  of  moles  of  soluteweight  of  solvent  in  kg

         m =  molkg

pH =  −logarithm   hydrogen  ion  concentration          pH =  −log H!  

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Chemistry Formula Chart, continued Conversions

273  K = 0  ℃ 1  mL  H!O = 1  g  of  H!O 1  mol  of  gas   as  STP = 22.4  L

cc = cubic  centimeter = !"!   101.3  kPa = 1  atmosphere = 760  mm  Hg 1  kg = 1000  g

1  meter = 100  centimeters = 1000  millimeters = 1  ×  10!micrometer = 1  ×  10!  nanometers  

Electromagnetic Spectrum

speed  of  light = ! = 3.0  ×  10!  m/s  

wave  speed = wavelength  ×  frequency          ! =  !"

Gamma

rays X-rays UV

light Visible

light Microwaves Radio/TV

waves

Visible Light

Polyatomic Ions

Acetate   C!H!O!!, CH!COO!  Ammonium   NH!!  

Carbonate   CO!!!  Chlorate   CIO!!  Chlorite   CIO!!  

Chromate   CrO!!!  

Cyanide   CN!  

Dichromate   Cr!O!!!  Hydrogen  carbonate   HCO!!  Hydroxide   OH!  Hypochlorite   CIO!  Nitrate   NO!!  

Nitrite   NO!!  Perchlorate   CIO!!  Permanganate   MnO!!  

Phosphate   PO!!!  

Sulfate   SO!!!  

Sulfite   SO!!!  

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