Chemistry 100 Exam 1

Size: px
Start display at page:

Download "Chemistry 100 Exam 1"

Transcription

1 Instructor: Nicole Stevens 1 of 8 Winter Which of the following is a chemical property? a. density d. boiling point b. color e. odor c. reactivity with water f. all of these are chemical properties 2. Which measurement below is equivalent to 15.5 kilograms? a. 155 g d g b x 10 7 mg e. 1,550 g c x 10 5 g f. 15,500 mg 3. Which of the following is a chemical change? a. burning a piece of paper d. wadding up a piece of paper b. water boiling e. melting gold c. ice melting f. pouring water from a pitcher to a cup 4. Refer to the Periodic Table. Which of the following elements is a metalloid? a. calcium d. magnesium b. aluminum e. oxygen c. copper f. silicon 5. Which of the following is true of isotopes? a. they have the same number of protons, but different number of electrons b. they have different numbers of protons and neutrons, but similar physical properties c. they have the same number of neutrons, but different number of protons d. they have the same number of protons, but different number of neutrons e. they have the same number of neutrons, but different number of electrons 6. Which is the correct electron configuration of a non-metal? a. 1s 1 2s 2 3s 3 4s 4 b. 1s 2 2s 2 2p 6 3s 2 c. 1s 2 2s 2 2p 6 3s 2 3p 5 d. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 4 e. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 Part 1: Multiple Choice You may write on this test, but MARK YOUR FINAL ANSWERS on a separate bubble sheet. 7. Which can hold the fewest electrons? a. energy level 3 d. a "d" energy sublevel b. a "p" energy sublevel e. a "d" orbital c. energy level 2 f. energy level 4 8. What is the molar mass of magnesium bromate? a g/mol d g/mol b g/mol e g/mol c g/mol f g/mol 9. What is the formula mass of strontium chlorite? a g/mol d amu b amu e g/mol c g/mol f amu

2 Instructor: Nicole Stevens 2 of 8 Winter 2008 Part 1: Multiple Choice MARK YOUR FINAL ANSWERS on a separate bubble sheet. Match each of the following scientists with the scientific research they did. 10. Rutherford a. Wrote The Sceptical Chymist in 1661 b. Discovered ions, realized atoms were electrical in nature 11. Schrodinger c. Organized elements into the Periodic Table d. Coined term "electrons" based on work with cathode-ray tubes 12. Thomson e. Law of Conservation of Mass f. "Electron cloud" surrounds nucleus, region of probability g. Proposed an encompassing "atomic theory" h. Gold-foil experiment suggested atomic structure i. Oil drop experiment calculated mass of electrons 13. How many molecules of carbon dioxide are present in 1.5 moles of carbon dioxide? a. 1.5 molecule d x molecules b. 66 molecules e x molecules c molecules f. impossible to tell from given information 14. Which atom produces a cation when ionized? a. Al d. S b. O e. He c. P f. all of the above produce anions Match the following to its correct name. a. phosphorus dioxide PO 2 b. hypophosphate ion c. sodium sulfate 16. NO 3 d. disodium sulfate e. disodium sulfur trioxide 17. Na 2 SO 3 f. nitrate ion g. phosphite ion h. sodium sulfite i. hypophosphite ion j. nitrogen trioxide Match the following to its correct formula. 18. Nickel (II) chloride a. Mg 3 PO 2 f. NiCl 2 b. Ni 2 Cl g. Ni 2 ClO Magnesium phosphide c. Al 3 (NO 2 ) h. Mg 2 P 3 d. Mg 3 P 2 i. AlN Aluminum hyponitrite e. Al(NO) 3 j. AlNO What is the correct formula for ammonium carbonite? a. (NH 3 ) 2 CO 2 d. Am 2 CO 2 g. NH 4 CO 2 b. (NH 4 ) 2 CO 2 e. Al 2 CO 2 h. NH 3 CO 2 c. (NH 3 ) 2 CO 3 f. Al 2 (CO 2 ) 3 i. NH 4 CO 4

3 Instructor: Nicole Stevens 3 of 8 Winter 2008 Part 1: Multiple Choice You may write on this test, but MARK YOUR FINAL ANSWERS on a separate bubble sheet. 22. A linear VSEPR molecular shape is characteristic of which of the following? 2- SO 2 H 2 O SO 2 - NO 2 CO 2 A. B. C. D. E. a. A e. E i. C and E b. B f. A and C j. all of the above c. C g. A and D d. D h. A, B and D 23. What is the term that means an an average of all an element's isotopes? a. polarity d. molecular shape b. mass number e. electronegativity c. atomic number f. atomic mass 24. A chlorine atom has gained one electron. Which of the following is NOT true about the atom now? a. it is an anion d. it has the same electron configuration as argon b. its mass number increases e. it would be attracted to positive ions and form ionic bonds c. it carries a -1 charge f. all of the above are true 25. Sodium reacts with chlorine gas to form table salt (sodium chloride). In the balanced equation, what are the coefficients in front of sodium and chlorine gas, respectively? a. 3 and 3 d. 3 and 2 b. 2 and 3 e. 3 and 1 c. 2 and 1 f. 1 and 1 Indicate whether the following statements are true or false. a. TRUE b. FALSE 26. The subscripts in a molecular formula represent proportions or ratios of moles. 27. One mole of water contains the same number of molecules as one mole of carbon dioxide. 28. An s-orbital in energy level 1 has both the same shape and the same volume as an s-orbital in energy level Alkaline earth metals react more vigorously with water than alkali metals. 30. p-orbitals are dumbell shaped, while s-orbitals are spherical.

4 Instructor: Nicole Stevens 4 of 8 Winter 2008 Name Part 2 : Write-on Please write your answers clearly in the space provided. SHOW ALL WORK! I. Write the full electron configuration for each of the following elements in order of how the orbitals fill. a. Copper b. Krypton II. If a piece of aluminum has a density of 1.73g/mL and a volume of 8.75mL, what is its mass? (Answer to 2 decimal places) III. Convert each of the following measurements into kilometers: a x 10 9 mm b m IV. Write each of the following in scientific notation: a. 564,000 b The chemical symbol of the following elements is represented by "X". Refer to the following figures for questions V - VII. X X X X a. b. c. d. e. V. Which of the above figures are isotopes of each other? X VI. Which of the above figures have the same number of neutrons? VII. Figure (b) represents which element from the Periodic Table?

5 Instructor: Nicole Stevens 5 of 8 Winter 2008 Name Part 2 : Write-on Please write your answers clearly in the space provided. SHOW ALL WORK! VIII. Consider a molecule of nitrogen trihydride (ammonia). a. Draw the complete electron-dot configuration of nitrogen trihydride. b. What is the VSEPR molecular shape of this molecule? c. What is the intramolecular force for this molecule? d. What is the intermolecular force for this molecule? e. What state of matter is this compound most likely to be? IX. Perform the following "Roadmap" calculations: (Answers to 2 decimal places) a. How many grams of chromium are present in a sample that contains 3.25 x Cr atoms? b. How many atoms of oxygen are present in 96.4g of aluminum sulfate? c. How many grams of phosphorus are present in 49.7g of magnesium phosphite?

6 Instructor: Nicole Stevens 6 of 8 Winter 2008 Name Part 2 : Write-on Please write your answers clearly in the space provided. SHOW ALL WORK! X. Dihydrogen sulfide reacts with iron (III) perchlorate to form iron (III) sulfide and hydrogen perchlorate. a. Write the balanced equation. b. If I begin with 32.0g of iron (III) perchlorate, how many grams of hydrogen perchlorate will form? (Answer to 2 decimal places) c. If I want to form 60.0g of iron (III) sulfide, how many grams of dihydrogen sulfide to I need to react? (Answer to 2 decimal places) BONUS!! d. What state of matter is the dihydrogen sulfide most likely to be? How can you tell? e. What state of matter is the iron (III) sulfide most likely to be? How can you tell?

7 Instructor: Nicole Stevens 7 of 8 Winter 2008 Roadmap to Chemistry Mass Calculations Grams of element Grams of compound A Grams of compound B Molar mass of element (g/mol) Molar mass of compound A Molar mass of compound B Moles of element Subscripts in formula Moles of compound A Coefficients in balanced equation Moles of compound B Avogadro s number of atoms or ions Avogadro s number of molecules Atoms or Ions Molecules Atomic mass (amu / atom) Formula mass (amu / molecule) Amu of element Amu of compound

2014 Spring CHEM101 Ch1-2 Review Worksheet Modified by Dr. Cheng-Yu Lai,

2014 Spring CHEM101 Ch1-2 Review Worksheet Modified by Dr. Cheng-Yu Lai, Ch1 1) Which of the following underlined items is not an intensive property? A) A chemical reaction requires 3.00 g of oxygen. B) The density of helium at 25 C is 1.64 10-4 g/cm3. C) The melting point

More information

Electrons in Atoms & Periodic Table Chapter 13 & 14 Assignment & Problem Set

Electrons in Atoms & Periodic Table Chapter 13 & 14 Assignment & Problem Set Electrons in Atoms & Periodic Table Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Electrons in Atoms & Periodic Table 2 Study Guide: Things You

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

Exam 2 Chemistry 65 Summer 2015. Score:

Exam 2 Chemistry 65 Summer 2015. Score: Name: Exam 2 Chemistry 65 Summer 2015 Score: Instructions: Clearly circle the one best answer 1. Valence electrons are electrons located A) in the outermost energy level of an atom. B) in the nucleus of

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

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

Study Guide For Chapter 7

Study Guide For Chapter 7 Name: Class: Date: ID: A Study Guide For Chapter 7 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The number of atoms in a mole of any pure substance

More information

Moles, Molecules, and Grams Worksheet Answer Key

Moles, Molecules, and Grams Worksheet Answer Key Moles, Molecules, and Grams Worksheet Answer Key 1) How many are there in 24 grams of FeF 3? 1.28 x 10 23 2) How many are there in 450 grams of Na 2 SO 4? 1.91 x 10 24 3) How many grams are there in 2.3

More information

DAWSON COLLEGE DEPARTMENT OF CHEMISTRY & CHEMICAL TECHNOLOGY SOLUTIONS TO PRACTICE FINAL EXAMINATION INTRODUCTION TO COLLEGE CHEMISTRY

DAWSON COLLEGE DEPARTMENT OF CHEMISTRY & CHEMICAL TECHNOLOGY SOLUTIONS TO PRACTICE FINAL EXAMINATION INTRODUCTION TO COLLEGE CHEMISTRY DAWSON COLLEGE DEPARTMENT OF CHEMISTRY & CHEMICAL TECHNOLOGY SOLUTIONS TO PRACTICE FINAL EXAMINATION INTRODUCTION TO COLLEGE CHEMISTRY Solutions Print your Name: Student Number: INSTRUCTORS: Please circle

More information

Mole Notes.notebook. October 29, 2014

Mole Notes.notebook. October 29, 2014 1 2 How do chemists count atoms/formula units/molecules? How do we go from the atomic scale to the scale of everyday measurements (macroscopic scale)? The gateway is the mole! But before we get to the

More information

Sample Exercise 2.1 Illustrating the Size of an Atom

Sample Exercise 2.1 Illustrating the Size of an Atom Sample Exercise 2.1 Illustrating the Size of an Atom The diameter of a US penny is 19 mm. The diameter of a silver atom, by comparison, is only 2.88 Å. How many silver atoms could be arranged side by side

More information

Chemical Calculations: The Mole Concept and Chemical Formulas. AW Atomic weight (mass of the atom of an element) was determined by relative weights.

Chemical Calculations: The Mole Concept and Chemical Formulas. AW Atomic weight (mass of the atom of an element) was determined by relative weights. 1 Introduction to Chemistry Atomic Weights (Definitions) Chemical Calculations: The Mole Concept and Chemical Formulas AW Atomic weight (mass of the atom of an element) was determined by relative weights.

More information

The Mole Concept and Atoms

The Mole Concept and Atoms Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chapter 4 24 September 2013 Calculations and the Chemical Equation The Mole Concept and Atoms Atoms are exceedingly

More information

Iron is. Temperature is a(n) property of a substance. Select two that apply. Which of the following is a chemical change?

Iron is. Temperature is a(n) property of a substance. Select two that apply. Which of the following is a chemical change? Posting ID: 419903 Course: CHE 105 2015 SU Instructor: Sarah Edwards Question #: 1 Iron is. A. a compound B. a heterogenous mixture C. a homogenous mixture D. an element Question #: 2 Temperature is a(n)

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

MOLES AND MOLE CALCULATIONS

MOLES AND MOLE CALCULATIONS 35 MOLES ND MOLE CLCULTIONS INTRODUCTION The purpose of this section is to present some methods for calculating both how much of each reactant is used in a chemical reaction, and how much of each product

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

Chemical Quantities: The Mole Chapter 7 Assignment & Problem Set

Chemical Quantities: The Mole Chapter 7 Assignment & Problem Set Chemical Quantities: The Mole Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Chemical Quantities: The Mole 2 Study Guide: Things You Must Know

More information

Calculating Atoms, Ions, or Molecules Using Moles

Calculating Atoms, Ions, or Molecules Using Moles TEKS REVIEW 8B Calculating Atoms, Ions, or Molecules Using Moles TEKS 8B READINESS Use the mole concept to calculate the number of atoms, ions, or molecules in a sample TEKS_TXT of material. Vocabulary

More information

Chapter 3: Stoichiometry

Chapter 3: Stoichiometry Chapter 3: Stoichiometry Goal is to understand and become proficient at working with: 1. Avogadro's Number, molar mass and converting between mass and moles (REVIEW). 2. empirical formulas from analysis.

More information

More on ions (Chapters 2.1 and )

More on ions (Chapters 2.1 and ) More on ions (Chapters 2.1 and 3.5 3.7) Ion: an atom or molecule that has a net electrical charge. Examples: Na + (sodium ion), Cl - (chloride), NH 4 + (ammonium). Anion: a negative ion, formed when electrons

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

Programme in mole calculation

Programme in mole calculation Programme in mole calculation Step 1 Start at the very beginning Atoms are very small indeed! If we draw a line 1 metre long, 6,000,000,000 (6 billion) atoms could be lined end to end. So a scientist cannot

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

Unit 6 Particles with Internal Structure 3-1

Unit 6 Particles with Internal Structure 3-1 Unit 6 Particles with Internal Structure 3-1 The Elements Remember, elements are combined to form molecules the way letters are combined to form words. Presently there are about 115 known elements. Only

More information

3 large lures x 22.0 g/lure + 5 medium lures x 12.9 g/lure + 5 small lures x 8.5 g/lure g packaging = g

3 large lures x 22.0 g/lure + 5 medium lures x 12.9 g/lure + 5 small lures x 8.5 g/lure g packaging = g Answers additional questions 7.1 1. Describe how the particles of sodium bromide, an ionic compound, are different from water, a covalent compound. Give the particle name of each compound type. Ionic compounds

More information

MOLECULAR MASS AND FORMULA MASS

MOLECULAR MASS AND FORMULA MASS 1 MOLECULAR MASS AND FORMULA MASS Molecular mass = sum of the atomic weights of all atoms in the molecule. Formula mass = sum of the atomic weights of all atoms in the formula unit. 2 MOLECULAR MASS AND

More information

Chapter 7. Bellringer. Table of Contents. Chapter 7. Chapter 7. Objectives. Avogadro s Number and the Mole. Chapter 7. Chapter 7

Chapter 7. Bellringer. Table of Contents. Chapter 7. Chapter 7. Objectives. Avogadro s Number and the Mole. Chapter 7. Chapter 7 The Mole and Chemical Table of Contents Chemical Formulas Bellringer List as many common counting units as you can. Determine how many groups of each unit in your list are present in each of the following

More information

Chemical Calculations: Formula Masses, Moles, and Chemical Equations

Chemical Calculations: Formula Masses, Moles, and Chemical Equations Chemical Calculations: Formula Masses, Moles, and Chemical Equations Atomic Mass & Formula Mass Recall from Chapter Three that the average mass of an atom of a given element can be found on the periodic

More information

Chapter 2 Atoms, Ions, and the Periodic Table

Chapter 2 Atoms, Ions, and the Periodic Table Chapter 2 Atoms, Ions, and the Periodic Table 2.1 (a) neutron; (b) law of conservation of mass; (c) proton; (d) main-group element; (e) relative atomic mass; (f) mass number; (g) isotope; (h) cation; (i)

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

AP Chemistry Summer Work

AP Chemistry Summer Work AP Chemistry Summer Work 2016-2017 Welcome to AP Chemistry! This rigorous course will prepare you for the AP Chemistry test currently scheduled for May 1 st, 2017. Throughout the scope of this course we

More information

TOPIC 7. CHEMICAL CALCULATIONS I - atomic and formula weights.

TOPIC 7. CHEMICAL CALCULATIONS I - atomic and formula weights. TOPIC 7. CHEMICAL CALCULATIONS I - atomic and formula weights. Atomic structure revisited. In Topic 2, atoms were described as ranging from the simplest atom, H, containing a single proton and usually

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

The idea of arranging the elements in the periodic table according to their chemical and physical properties is attributed to. d) Ramsay.

The idea of arranging the elements in the periodic table according to their chemical and physical properties is attributed to. d) Ramsay. Chemistry I PERIODIC TABLE PRACTICE QUIZ Mr. Scott Select the best answer. 1) The idea of arranging the elements in the periodic table according to their chemical and physical properties is attributed

More information

47374_04_p25-32.qxd 2/9/07 7:50 AM Page 25. 4 Atoms and Elements

47374_04_p25-32.qxd 2/9/07 7:50 AM Page 25. 4 Atoms and Elements 47374_04_p25-32.qxd 2/9/07 7:50 AM Page 25 4 Atoms and Elements 4.1 a. Cu b. Si c. K d. N e. Fe f. Ba g. Pb h. Sr 4.2 a. O b. Li c. S d. Al e. H f. Ne g. Sn h. Au 4.3 a. carbon b. chlorine c. iodine 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

Atoms, Molecules, Formulas, and Subatomic Particles

Atoms, Molecules, Formulas, and Subatomic Particles Introduction to Chemistry Chapter 5 1 Atoms, Molecules, Formulas, and Subatomic Particles The Atom: The smallest particle of an element that can exist and still have the properties of the element building

More information

b. How is the modern periodic table arranged? In order of increasing atomic number

b. How is the modern periodic table arranged? In order of increasing atomic number Unit 3 Review Chapters 4 (Atomic Structure) & 6 (Periodic Table) Part 1: Answer the following questions. 1. a. Which scientist created the first modern atomic theory? John Dalton b. What was his theory?

More information

Chapter Two Study Guide Answers

Chapter Two Study Guide Answers Chapter Two Study Guide Answers Concepts 1. Know the law of conservation of mass 2. Know about the structure of the atom and who did what including Thomson, Rutheford, Millikan, Bohr 3. Know the three

More information

Ionic and Covalent Bonds

Ionic and Covalent Bonds Chapter 6 Inorganic and Organic Compounds: Names and Formulas 6.1 Octet Rule and Ions Octet Rule An octet is 8 valence electrons is associated with the stability of the noble gases does not occur with

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

Chemical Composition Review Mole Calculations Percent Composition. Copyright Cengage Learning. All rights reserved. 8 1

Chemical Composition Review Mole Calculations Percent Composition. Copyright Cengage Learning. All rights reserved. 8 1 Chemical Composition Review Mole Calculations Percent Composition Copyright Cengage Learning. All rights reserved. 8 1 QUESTION Suppose you work in a hardware store and a customer wants to purchase 500

More information

B. Elements: We cannot determine how many electrons are lost for the elements b/c their in their valence electrons can change.

B. Elements: We cannot determine how many electrons are lost for the elements b/c their in their valence electrons can change. Unit 6 Notepack: Chapters 9 &10 Chemical Quantities 9.1 Naming Ions NAME Period: A. ions: Ions made of single. B. Elements: There is a pattern in predicting how many electrons are lost and gained for the

More information

CHEMISTRY 101 SPRING 2010 EXAM 1 FORM D SECTION 503 DR. KEENEY-KENNICUTT PART 1

CHEMISTRY 101 SPRING 2010 EXAM 1 FORM D SECTION 503 DR. KEENEY-KENNICUTT PART 1 NAME CHEMISTRY 101 SPRING 2010 EXAM 1 FORM D SECTION 503 DR. KEENEY-KENNICUTT Directions: (1) Put your name and signature on PART 2 of the exam where indicated. (2) Sign the Aggie Code on PART 2 of this

More information

Periodic Table Trends

Periodic Table Trends Name Date Period Periodic Table Trends (Ionization Energy and Electronegativity) Ionization Energy The required to an electron from a gaseous atom or ion. Period Trend: As the atomic number increases,

More information

Name: Period: Date: Unit 3 Practice Review (the questions on the test are NOT the same as the review questions)

Name: Period: Date: Unit 3 Practice Review (the questions on the test are NOT the same as the review questions) Name: Period: Date: Unit 3 Review: things you will need to know 1. Atomic Theories: Know all the scientists in order. What did they discover? What experiment did they use? 2. Development of the periodic

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

Chapter 2 The Chemical Context of Life

Chapter 2 The Chemical Context of Life Chapter 2 The Chemical Context of Life Multiple-Choice Questions 1) About 25 of the 92 natural elements are known to be essential to life. Which four of these 25 elements make up approximately 96% of living

More information

CHM 1311: General Chemistry 1, Fall 2004 Exam #1, September 8, 2004. Name (print) SSN

CHM 1311: General Chemistry 1, Fall 2004 Exam #1, September 8, 2004. Name (print) SSN CHM 1311: General Chemistry 1, Fall 2004 Exam #1, September 8, 2004 Name (print) SSN Pledge: I have neither given nor received aid on this exam: Signature For ALL problems: SHOW ALL WORK TO GET FULL CREDIT

More information

Gen Chem I Exam 1 Review (Chapters 1 & 2)

Gen Chem I Exam 1 Review (Chapters 1 & 2) Gen Chem I Exam 1 Review (Chapters 1 & 2) 1 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. All of the following are properties of antimony. Which one

More information

AP Chemistry. Unit #3. Chapter 3 Zumdahl

AP Chemistry. Unit #3. Chapter 3 Zumdahl AP Chemistry Unit #3 Chapter 3 Zumdahl Stoichiometry C6H12O6 + 6 O2 6 CO2 + 6 H2O Students should be able to: Calculate the atomic weight (average atomic mass) of an element from the relative abundances

More information

Chemistry Assessment Unit AS 1

Chemistry Assessment Unit AS 1 Centre Number 71 Candidate Number ADVANCED SUBSIDIARY (AS) General Certificate of Education January 2012 Chemistry Assessment Unit AS 1 assessing Basic Concepts in Physical and Inorganic Chemistry AC112

More information

CHEMISTRY Quiz #1 answer key September 16, 2010

CHEMISTRY Quiz #1 answer key September 16, 2010 CHEMISTRY 123-07 Quiz #1 answer key September 16, 2010 Statistics: Average: 37 p (74%); Highest: 48 p (96%); Lowest: 20 p (40%) Number of students performing at or above average: 69 (58%) Number of students

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

GCSE to AS Chemistry

GCSE to AS Chemistry GCSE to AS Chemistry Chemistry is a rewarding yet difficult subject that is highly valued by both employers and higher education establishments. The most challenging part of AS Chemistry is bridging the

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

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

Activity 5: Ions and the Periodic Table

Activity 5: Ions and the Periodic Table Ions & the Periodic Table 1 Activity 5: Ions and the Periodic Table Why? Ions, like atoms, may also be identified by the numbers of protons, neutrons and electrons they contain. Ions are particularly important

More information

CHEMISTRY Midterm #1 answer key September 28, 2004

CHEMISTRY Midterm #1 answer key September 28, 2004 CHEMISTRY 123-02 Midterm #1 answer key September 28, 2004 Statistics: Average: 79 pts (79%); Highest: 101 pts (100%); Lowest: 32 pts (32%) Number of students performing at or above average: 61 (58%) Number

More information

Chemical Proportions in Compounds

Chemical Proportions in Compounds Chapter 6 Chemical Proportions in Compounds Solutions for Practice Problems Student Textbook page 201 1. Problem A sample of a compound is analyzed and found to contain 0.90 g of calcium and 1.60 g of

More information

Molar Mass Worksheet Answer Key

Molar Mass Worksheet Answer Key Molar Mass Worksheet Answer Key Calculate the molar masses of the following chemicals: 1) Cl 2 71 g/mol 2) KOH 56.1 g/mol 3) BeCl 2 80 g/mol 4) FeCl 3 162.3 g/mol 5) BF 3 67.8 g/mol 6) CCl 2 F 2 121 g/mol

More information

Chapter 2 Atoms Molecules and Ions

Chapter 2 Atoms Molecules and Ions Chapter 2 Atoms Molecules and Ions Student: NOTE: A periodic table is required to work many of the problems in this chapter. 1. The elements in a column of the periodic table are known as A. metalloids.

More information

Name PRE-TEST. Directions: Circle the letter indicating whether the following statements are either true ("T") or false ("F").

Name PRE-TEST. Directions: Circle the letter indicating whether the following statements are either true (T) or false (F). 1 PRETEST Directions: Circle the letter indicating whether the following statements are either true ("T") or false ("F"). T F 1. Chemical elements with similar chemical properties are referred to as a

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

Balance the following equation: KClO 3 + C 12 H 22 O 11 KCl + CO 2 + H 2 O

Balance the following equation: KClO 3 + C 12 H 22 O 11 KCl + CO 2 + H 2 O Balance the following equation: KClO 3 + C 12 H 22 O 11 KCl + CO 2 + H 2 O Ans: 8 KClO 3 + C 12 H 22 O 11 8 KCl + 12 CO 2 + 11 H 2 O 3.2 Chemical Symbols at Different levels Chemical symbols represent

More information

Chapter 6: Chemical Composition

Chapter 6: Chemical Composition C h e m i s t r y 1 2 C h 6 : C h e m i c a l C o m p o s i t i o n P a g e 1 Chapter 6: Chemical Composition Bonus: 17, 21, 31, 39, 43, 47, 55, 61, 63, 69, 71, 77, 81, 85, 91, 95, 97, 99 Check the deadlines

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

Chapter 8 Chemical Quantities

Chapter 8 Chemical Quantities Chapter 8 Chemical Quantities Introductory Info The atomic masses of the elements on the periodic table are in the units. These measurements are based on the mass of the standard isotope of the element,

More information

The Periodic Table: Chapter Problems Periodic Table Class Work Homework Special Groups Class Work Homework Periodic Families Class Work

The Periodic Table: Chapter Problems Periodic Table Class Work Homework Special Groups Class Work Homework Periodic Families Class Work The Periodic Table: Chapter Problems Periodic Table 1. As you move from left to right across the periodic table, how does atomic number change? 2. What element is located in period 3, group 13? 3. What

More information

Practice Hour Examination I. Use the Periodic Table in your book. Normally one will be provided. These are some sample problems.

Practice Hour Examination I. Use the Periodic Table in your book. Normally one will be provided. These are some sample problems. Chemistry 1111 bruary 2011 Practice Hour Examination I Use the Periodic Table in your book. Normally one will be provided. These are some sample problems. 1. What is the average mass (in grams) of one

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

Grade 9 Science Unit: Atoms and Elements Topic 4: Periodic Table & Compounds

Grade 9 Science Unit: Atoms and Elements Topic 4: Periodic Table & Compounds Grade 9 Science Unit: Atoms and Elements Topic 4: Periodic Table & Compounds Topic Using the Periodic Table Metals, Non- Metals & Metalloids I can Explain and identify the periods of the Periodic Table.

More information

Name Date Class THE PERIODIC TABLE. SECTION 6.1 ORGANIZING THE ELEMENTS (pages )

Name Date Class THE PERIODIC TABLE. SECTION 6.1 ORGANIZING THE ELEMENTS (pages ) 6 THE PERIODIC TABLE SECTION 6.1 ORGANIZING THE ELEMENTS (pages 155 160) This section describes the development of the periodic table and explains the periodic law. It also describes the classification

More information

ATOMS A T O M S, I S O T O P E S, A N D I O N S. The Academic Support Center @ Daytona State College (Science 120, Page 1 of 39)

ATOMS A T O M S, I S O T O P E S, A N D I O N S. The Academic Support Center @ Daytona State College (Science 120, Page 1 of 39) ATOMS A T O M S, I S O T O P E S, A N D I O N S The Academic Support Center @ Daytona State College (Science 120, Page 1 of 39) THE ATOM All elements listed on the periodic table are made up of atoms.

More information

BASIC IDEAS IN CHEMISTRY

BASIC IDEAS IN CHEMISTRY BASIC IDEAS IN CHEMISTRY by Michael Clark Success in studying Chemistry depends upon the familiarity of students with a few basic ideas, conventions, and methods upon which later studies are built. This

More information

Chemistry Assessment Unit AS 1

Chemistry Assessment Unit AS 1 New Specification Centre Number 71 Candidate Number ADVANCED SUBSIDIARY (AS) General Certificate of Education January 2010 Chemistry Assessment Unit AS 1 assessing Basic Concepts in Physical and Inorganic

More information

7.1 Stoichiometry and Percent Yield

7.1 Stoichiometry and Percent Yield score /10 pts. Name Class Date 7.1 Stoichiometry and Percent Yield Mole Ratios An example: The combustion of propane is used to heat many rural homes in winter. Balance the equation below for the combustion

More information

2. All of the atoms of argon have the same. 1. The atomic number of an atom is always equal to the total number of. A. mass number B.

2. All of the atoms of argon have the same. 1. The atomic number of an atom is always equal to the total number of. A. mass number B. 1. The atomic number of an atom is always equal to the total number of A. neutrons in the nucleus B. protons in the nucleus 2. All of the atoms of argon have the same A. mass number B. atomic number C.

More information

Untitled Document. 1. Which of the following best describes an atom? 4. Which statement best describes the density of an atom s nucleus?

Untitled Document. 1. Which of the following best describes an atom? 4. Which statement best describes the density of an atom s nucleus? Name: Date: 1. Which of the following best describes an atom? A. protons and electrons grouped together in a random pattern B. protons and electrons grouped together in an alternating pattern C. a core

More information

CHAPTER 13 THE PERIODIC TABLE

CHAPTER 13 THE PERIODIC TABLE CHAPTER 13 THE PERIODIC TABLE OVERVIEW The periodic table is usually the first thing that comes to mind when thinking about the subject of chemistry. We have all heard about the periodic table from as

More information

Chemistry Stoichiometry. 45 points. Do not turn page until told to do so.

Chemistry Stoichiometry. 45 points. Do not turn page until told to do so. Chemistry 2010 Stoichiometry 45 points Do not turn page until told to do so. Stoichiometry Multiple Choice (Each worth 2 points) Identify the letter of the choice that best completes the statement or

More information

CHM1 Review for Exam Which of the following elements has the highest electronegativity

CHM1 Review for Exam Which of the following elements has the highest electronegativity The following are topics and sample questions for the first exam. Topics 1. Mendeleev and the first periodic Table 2. Information in the Periodic Table a. Groups (families) i. Alkali (group 1) ii. Alkaline

More information

Chapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations

Chapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations CHE11 Chapter Chapter Stoichiometry: Calculations with Chemical Formulas and Equations 1. When the following equation is balanced, the coefficients are. NH (g) + O (g) NO (g) + H O (g) (a). 1, 1, 1, 1

More information

Name Class Date ELECTRONS AND THE STRUCTURE OF ATOMS

Name Class Date ELECTRONS AND THE STRUCTURE OF ATOMS Name Class Date The Periodic Table ELECTRONS AND THE STRUCTURE OF ATOMS 6.1 Organizing the Elements Essential Understanding Although Dmitri Mendeleev is often credited as the father of the periodic table,

More information

Useful only for measuring the mass of very small objects atoms and molecules!

Useful only for measuring the mass of very small objects atoms and molecules! Chapter 9 Chemical Composition (Moles) Which weighs more, 1 atom of He or 1 atom of O? Units of mass: Pound Kilogram Atomic mass unit (AMU) There are others! 1 amu = 1.66 x 10-24 grams = mass of a proton

More information

Molecular Formula: Example

Molecular Formula: Example Molecular Formula: Example A compound is found to contain 85.63% C and 14.37% H by mass. In another experiment its molar mass is found to be 56.1 g/mol. What is its molecular formula? 1 CHAPTER 3 Chemical

More information

Exercise 3.5 - Naming Binary Covalent Compounds:

Exercise 3.5 - Naming Binary Covalent Compounds: Chapter Exercise Key 1 Chapter Exercise Key Exercise.1 Classifying Compounds: Classify each of the following substances as either a molecular compound or an ionic compound. a. formaldehyde, CH 2 O (used

More information

CHAPTER 9. 9.1 Naming Ions. Chemical Names and Formulas. Naming Transition Metals. Ions of Transition Metals. Ions of Transition Metals

CHAPTER 9. 9.1 Naming Ions. Chemical Names and Formulas. Naming Transition Metals. Ions of Transition Metals. Ions of Transition Metals CHAPTER 9 Chemical Names and Formulas 9.1 Naming Ions Monatomic Ions: a single atom with a positive or negative charge Cation (rules): listed first Anion (rules): ide ending Transition Metals have a varying

More information

Chapter 2 Atoms, Molecules, and Ions

Chapter 2 Atoms, Molecules, and Ions Chapter 2 Atoms, Molecules, and Ions 1 Self study: The history of the development of atomic theory. 9 th Ed: pp. 36-41 or 10 th Ed: pp. 38-42. 2 The Atomic Theory of Matter John Dalton (1766-1844), began

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

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

AP BIOLOGY CHAPTER 2 WORKSHEET

AP BIOLOGY CHAPTER 2 WORKSHEET Name Date _ AP BIOLOGY CHAPTER 2 WORKSHEET MULTIPLE CHOICE. 25 pts. Place the letter of the choice that best completes the statement or answers the question in the blank.. 1. About 25 of the 92 natural

More information

Chapter 3. Stoichiometry: Ratios of Combination. Insert picture from First page of chapter. Copyright McGraw-Hill 2009 1

Chapter 3. Stoichiometry: Ratios of Combination. Insert picture from First page of chapter. Copyright McGraw-Hill 2009 1 Chapter 3 Insert picture from First page of chapter Stoichiometry: Ratios of Combination Copyright McGraw-Hill 2009 1 3.1 Molecular and Formula Masses Molecular mass - (molecular weight) The mass in amu

More information

Name Date Period. Chemistry: Unit 3 - Atoms Test Review KEY

Name Date Period. Chemistry: Unit 3 - Atoms Test Review KEY Name Date Period Concepts to know for the Unit 3 test: Chemistry: Unit 3 - Atoms Test Review KEY 1. Summarize the major experimental evidence that led to the development of various atomic models, both

More information

Unit 5 Chemical Quantities & The Mole

Unit 5 Chemical Quantities & The Mole Unit 5 Chemical Quantities & The Mole Molar mass is the mass of one mole of a substance. Molar Mass Other names for molar mass include *formula mass *gram formula mass *molecular weight Molar Mass One

More information

Practice Multiple Choice Questions:

Practice Multiple Choice Questions: Practice Multiple Choice Questions: 1) Which of the following is NOT a laboratory safety rule? a) You should never mix acids with bases b) You should tie back your long hair c) You should never add water

More information

Chemical Proportions in Compounds

Chemical Proportions in Compounds Chapter 3 Chemical Proportions in Compounds Note to teacher: You will notice that there are two different formats for the Sample Problems in the student textbook. Where appropriate, the Sample Problem

More information

Chapter 2 Atoms and the Periodic Table

Chapter 2 Atoms and the Periodic Table Chapter 2 1 Chapter 2 Atoms and the Periodic Table Solutions to In-Chapter Problems 2.1 Each element is identified by a one- or two-letter symbol. Use the periodic table to find the symbol for each element.

More information

PERIODIC TABLE OF ELEMENTS., a Russian scientist is credited with creating the periodic table.

PERIODIC TABLE OF ELEMENTS., a Russian scientist is credited with creating the periodic table. PERIODIC TABLE OF ELEMENTS, a Russian scientist is credited with creating the periodic table. Periods tell us how many are in the atoms of each element. Groups help us to know how many electrons are in

More information