EXAMPLE EXERCISE 4.1 Change of Physical State
|
|
|
- Meagan Byrd
- 8 years ago
- Views:
Transcription
1 EXAMPLE EXERCISE 4.1 Change of Physical State State the term that applies to each of the following changes of physical state: (a) Snow changes from a solid to a liquid. (b) Gasoline changes from a liquid to a gas. (c) Dry ice changes from a solid to a gas. Refer to Figure 4.1 for the changes of physical state. (a) The change from solid to liquid is called melting. (b) The change from liquid to gas is called vaporizing. (c) The change from solid to gas is called sublimation. State the term that applies to each of the following changes of physical state: (a) A refrigerant changes from a gas to a liquid. (b) Water changes from a liquid to a solid. (c) Iodine vapor changes from a gas to a solid. Answers: (a) condensing; (b) freezing; (c) deposition Figure 4.1 Changes in Physical State As temperature increases, a solid melts to a liquid and then vaporizes into a gas. As temperature decreases, a gas condenses to a liquid and then freezes to a solid.
2 EXAMPLE EXERCISE 4.1 Change of Physical State Continued Identify the physical state (solid, liquid, gas) that corresponds to each of the following pictorial representations:
3 EXAMPLE EXERCISE 4.2 Element, Compound, or Mixture Consider the following properties of the element copper: (a) Copper metal cannot be broken down by a chemical change. (b) Copper reacts with oxygen in air to give copper oxide. (c) Copper, in the form of malachite ore, is found worldwide. (d) Copper and tin compose bronze alloy. Classify each of the following copper samples as an element, a compound, a homogeneous mixture, or a heterogeneous mixture: (a) copper wire (b) copper oxide (c) malachite ore (d) bronze alloy Refer to Figure 4.2 to classify each sample. (a) Copper wire is a metallic element. (b) Copper oxide is a compound of the elements copper and oxygen. (c) Malachite ore is a heterogeneous mixture of copper and other substances. (d) Bronze alloy is a homogeneous mixture of copper and tin. Figure 4.2 Classification of Matter Matter may be either a mixture or a pure substance. The properties of a heterogeneous mixture vary within the sample (oil and water). The properties of a homogeneous mixture are constant (salt solution). A pure substance may be either a compound (water) or an element (gold). Left to right: oil and water; NaCl solution; H 2 O; and gold nugget.
4 EXAMPLE EXERCISE 4.2 Element, Compound, or Mixture Continued Consider the following properties of the element mercury: (a) Mercury liquid cannot be broken down by a chemical change. (b) Mercury oxide can be heated to give mercury and oxygen gas. (c) Mercury, in the form of cinnabar ore, is found in Spain and Italy. (d) Mercury and silver compose the alloy used for dental fillings. Classify each of the following mercury samples as an element, a compound, a homogeneous mixture, or a heterogeneous mixture: (a) mercury liquid (b) mercury oxide (c) cinnabar ore (d) dental alloy Answers: (a) element; (b) compound; (c) heterogeneous mixture; (d) homogeneous mixture
5 EXAMPLE EXERCISE 4.2 Element, Compound, or Mixture Continued Classify each of the following as an element, a compound, or a mixture as shown in the illustration:
6 EXAMPLE EXERCISE 4.3 Properties of Metals Which of the following properties is not characteristic of a metal? (a) good conductor of heat (b) malleable (c) high melting point (d) reacts with other metals Refer to Table 4.4 to classify each of the following properties: (a) Metals are good conductors of heat. (b) Metals are malleable. (c) Metals usually have high melting points. (d) Metals do not react with other metals; they mix to form alloys.
7 EXAMPLE EXERCISE 4.3 Properties of Metals Continued Which of the following properties is not characteristic of a nonmetal? (a) insulator of electricity (b) ductile (c) low density (d) reacts with nonmetals Answer: (b) Nonmetals crush to a powder and are not malleable or ductile. Which of the following is a solid metal under normal conditions: calcium, phosphorus, mercury, or silicon? (Refer to Figure 4.7.) Figure 4.7 Pictorial Periodic Table of the Elements The natural abundance is the percent by mass of an element in Earth s crust, oceans, and atmosphere. The natural abundance of an element listed as rare is less than 1 mg per metric ton (1000 kg). An element listed as synthetic is made artificially and does not occur naturally. An element listed as unstable often disintegrates in a fraction of a second.
8 EXAMPLE EXERCISE 4.4 Physical States of the Elements Indicate the physical state for each of the following elements at 25 C and normal pressure; classify each element as a metal, nonmetal, or semimetal: (a) barium (b) boron (c) bismuth (d) bromine Referring to Figures 4.5 and 4.6, we observe the following: (a) Barium (Ba) is on the left side of the periodic table; it is a solid metal under normal conditions. (b) Boron (B) is in the middle of the periodic table; it is a solid semimetal. (c) Bismuth (Bi) is to the right, but below the semimetals in the periodic table, it is a solid metal. (d) Bromine (Br) is on the right side of the periodic table; it is a liquid nonmetal at normal conditions. Figure 4.5 Metals, Nonmetals, and Semimetals The symbols of elements having metallic properties are on the left side of the periodic table, nonmetallic are on the right side, and semimetallic are midway between. Notice the special placement of hydrogen, a nonmetallic element.
9 EXAMPLE EXERCISE 4.4 Physical States of the Elements Continued Figure 4.6 Physical States of the Elements At 25 C and normal atmospheric pressure, all metals are in the solid state except Hg. Most nonmetals are gases except C, P, S, Se, and I, which are solids. The only elements in the liquid state at normal conditions are Hg and Br. Indicate the physical state for each of the following elements at 25 C and normal pressure; classify each element as a metal, nonmetal, or semimetal: (a) aluminum (b) hydrogen (c) helium (d) radium Answers: (a) solid metal; (b) gaseous nonmetal; (c) gaseous nonmetal; (d) solid metal
10 EXAMPLE EXERCISE 4.4 Physical States of the Elements Continued Which of the following is a liquid nonmetal under normal conditions: sodium, mercury, bromine, or sulfur? (Refer back to Figure 4.7.) Figure 4.7 Pictorial Periodic Table of the Elements The natural abundance is the percent by mass of an element in Earth s crust, oceans, and atmosphere. The natural abundance of an element listed as rare is less than 1 mg per metric ton (1000 kg). An element listed as synthetic is made artificially and does not occur naturally. An element listed as unstable often disintegrates in a fraction of a second.
11 EXAMPLE EXERCISE 4.5 Composition of Chemical Formulas State the total number of atoms in a molecule of vitamin B 3, C 6 H 6 N 2 O. The chemical formula for vitamin B 3 indicates 6 carbon atoms, 6 hydrogen atoms, 2 nitrogen atoms, and 1 oxygen atom. Thus C 6 H 6 N 2 O has a total of 15 atoms. Write the chemical formula for vitamin B 6, if a molecule is composed of 8 carbon atoms, 11 hydrogen atoms, 1 nitrogen atom, and 3 oxygen atoms. Answer: C 8 H 11 NO 3 (total of 23 atoms) Examine the model for vitamin C and determine the molecular formula. In the model shown, the black sphere = C atom, white = H atom, and red = O atom.
12 EXAMPLE EXERCISE 4.6 Composition of Chemical Formulas State the total number of atoms in a molecule of glycerin, C 3 H 5 (OH) 3. The chemical formula for glycerin indicates 3 carbon atoms, 5 hydrogen atoms, and 3 OH units. Thus, C 3 H 5 (OH) 3 has a total of 14 atoms. Write the chemical formula for nitroglycerin if a molecule is composed of 3 carbon atoms, 5 hydrogen atoms, 3 oxygen atoms, and 3 NO 2 units. Answer: C 3 H 5 O 3 (NO 2 ) 3 State the total number of atoms in a molecule of nitroglycerin, C 3 H 5 O 3 (NO 2 ) 3.
13 EXAMPLE EXERCISE 4.7 Physical and Chemical Properties Classify each of the following properties as physical or chemical: (a) Water appears colorless and odorless at 20 C. (b) Water dissolves sugar crystals. (c) Water produces a gas with calcium metal. (d) Water exists as ice at 10 C. If a reaction occurs, there is a change in composition and the property is chemical. Otherwise, the property is physical. (a) Color and odor are physical properties. (b) Solubility is a physical property. (c) A chemical reaction is a chemical property. (d) A physical state is a physical property. Classify each of the following properties as physical or chemical: (a) Water appears hard and crystalline at 0 C. (b) Water is insoluble in gasoline. (c) Water is a very weak conductor of electricity. (d) Water produces a gas with sodium metal. Answers: (a) physical; (b) physical; (c) physical; (d) chemical Copper melts at 1083 C, has a density of 8.92 g/ml, is a good conductor of electricity, and turns black when heated. Which of these is an example of a chemical property?
14 EXAMPLE EXERCISE 4.8 Physical and Chemical Changes Classify each of the following observations as a physical or a chemical change: (a) Touching a lit candle to hydrogen soap bubbles gives an explosion. (b) Heating water in a flask produces moisture on the glass. (c) Combining two colorless solutions gives a yellow solid. (d) Pouring vinegar on baking soda produces gas bubbles. An observation that indicates a physical change is a change of physical state. The observations that suggest a chemical change include burning, fizzing, changing color, or forming an insoluble substance in solution. (a) Hydrogen explodes; thus, it is a chemical change. (b) Water is boiled; thus, it is a physical change. (c) Two solutions give an insoluble substance; thus, it is a chemical change. (d) Baking soda fizzes; thus, it is a chemical change. Classify each of the following observations as a physical or a chemical change: (a) Freezing water in a refrigerator makes cubes of ice. (b) Adding silver nitrate to tap water gives a cloudy solution. (c) Burning sulfur gives a light blue flame. (d) Grinding aspirin tablets produces a powder. Answers: (a) physical; (b) chemical; (c) chemical; (d) physical
15 EXAMPLE EXERCISE 4.8 Physical and Chemical Changes Continued An Alka-Seltzer tablet dissolves in water and produces gas bubbles. Is this an example of a physical change or a chemical change? Alka-Seltzer An Alka-Seltzer tablet in water releases carbon dioxide gas bubbles.
16 EXAMPLE EXERCISE 4.9 Conservation of Mass Law In an experiment, g of magnesium metal was ignited and burned with oxygen in the air. If g of white magnesium oxide powder, MgO, was collected, what was the mass of oxygen gas that reacted? Applying the conservation of mass law, we find that the mass of the magnesium metal plus the mass of the oxygen gas equals the mass of the magnesium oxide powder. That is, g Mg + mass of oxygen = g MgO mass of oxygen = g MgO g Mg mass of oxygen = g If g of zinc metal reacts with g of yellow powdered sulfur, what is the mass of the zinc sulfide produced? Answer: g Heating g copper metal with yellow sulfur produces g of black copper sulfide. What is the mass of sulfur that reacted with the copper metal?
17 EXAMPLE EXERCISE 4.10 Kinetic Energy and Molecular Motion A balloon filled with helium gas is cooled from 25 C to 25 C. State the change in each of the following: (a) kinetic energy of the gas (b) motion of helium atoms Temperature, kinetic energy, and velocity are related as follows: (a) As the temperature cools from 25 C to 25 C, the kinetic energy of helium atoms decreases. (b) Since a drop in temperature produces a decrease in kinetic energy, the motion of helium atoms decreases. A steel cylinder containing air is heated from 25 C to 50 C. State the change in each of the following: (a) kinetic energy of the gas (b) motion of air molecules Answers: (a) increases; (b) increases What happens to the kinetic energy and velocity of air molecules when the temperature increases?
18 EXAMPLE EXERCISE 4.11 Forms of Energy Identify two forms of energy that are involved in each of the following conversions: (a) Radioactive emissions vaporize water to steam. (b) Steam drives a turbine. (c) A turbine spins and drives an electrical generator. We can refer to the six forms of energy listed above. It follows that (a) Nuclear energy is converted to heat energy. (b) Heat energy is converted to mechanical energy. (c) Mechanical energy is converted to electrical energy. Identify two forms of energy that are involved in each of the following devices: (a) flashlight (b) solar calculator (c) lead acid battery Answers: (a) chemical and light; (b) light and electrical; (c) chemical and electrical Which of the following is not a basic form of energy: chemical, electrical, heat, light, mechanical, nuclear, solar?
CHAPTER 3: MATTER. Active Learning Questions: 1-6, 9, 13-14; End-of-Chapter Questions: 1-18, 20, 24-32, 38-42, 44, 49-52, 55-56, 61-64
CHAPTER 3: MATTER Active Learning Questions: 1-6, 9, 13-14; End-of-Chapter Questions: 1-18, 20, 24-32, 38-42, 44, 49-52, 55-56, 61-64 3.1 MATTER Matter: Anything that has mass and occupies volume We study
Chapter Outline. 3 Elements and Compounds. Elements and Atoms. Elements. Elements. Elements 9/4/2013
3 Elements and Compounds Chapter Outline 3.1 Elements A. Distribution of Elements Foundations of College Chemistry, 14 th Ed. Morris Hein and Susan Arena Copyright This reclining Buddha in Thailand is
Chemistry Worksheet: Matter #1
Chemistry Worksheet: Matter #1 1. A mixture (is/is not) a chemical combining of substances. 2. In a compound the (atoms/molecules) are (chemically/physically) combined so that the elements that make up
Review - After School Matter Name: Review - After School Matter Tuesday, April 29, 2008
Name: Review - After School Matter Tuesday, April 29, 2008 1. Figure 1 The graph represents the relationship between temperature and time as heat was added uniformly to a substance starting at a solid
Chapter Test A. Elements, Compounds, and Mixtures MULTIPLE CHOICE. chemically combined? MIXs2 a. element b. compound c. mixture d.
Assessment Chapter Test A Elements, Compounds, and Mixtures MULTIPLE CHOICE Write the letter of the correct answer in the space provided. 1. What is a pure substance made of two or more elements that are
Chemical Formulas, Equations, and Reactions Test Pre-AP Write all answers on your answer document.
Name: Period: Chemical Formulas, Equations, and Reactions Test Pre-AP Write all answers on your answer document. 1. Which of the following is a NOT a physical property of hydrogen? A. It is gas C. It is
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
ATOMS. Multiple Choice Questions
Chapter 3 ATOMS AND MOLECULES Multiple Choice Questions 1. Which of the following correctly represents 360 g of water? (i) 2 moles of H 2 0 (ii) 20 moles of water (iii) 6.022 10 23 molecules of water (iv)
Physical and Chemical Changes Pre Test Questions
Pre Test Questions Name: Period: Date: 1. Which of the following is an example of physical change? a. Mixing baking soda and vinegar together, and this causes bubbles and foam. b. A glass cup falls from
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
Warm-Up 9/9. 1. Define the term matter. 2. Name something in this room that is not matter.
Warm-Up 9/9 1. Define the term matter. 2. Name something in this room that is not matter. Warm-Up 9/16 1. List the three most important rules of lab safety. 2. Would you classify jello as a solid or a
Name: Unit 2- Elements, Compounds and Mixtures and Physical/Chemical Properties and Changes. Elements, Compounds and Mixtures
Name: Unit 2- Elements, Compounds and Mixtures and Physical/Chemical Properties and Changes Day Page # Description IC/HW All 2 Warm-up IC 1 3 5 Matter Notes IC 1 6 Nuts & Bolts IC 1 7 Elements, Compounds
Chapter 3 Mass Relationships in Chemical Reactions
Chapter 3 Mass Relationships in Chemical Reactions Student: 1. An atom of bromine has a mass about four times greater than that of an atom of neon. Which choice makes the correct comparison of the relative
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
Chapter 1 The Atomic Nature of Matter
Chapter 1 The Atomic Nature of Matter 6. Substances that cannot be decomposed into two or more simpler substances by chemical means are called a. pure substances. b. compounds. c. molecules. d. elements.
Properties and Classifications of Matter
PS-3.1 Distinguish chemical properties of matter (including reactivity) from physical properties of matter (including boiling point, freezing/melting point, density [with density calculations], solubility,
5. Which temperature is equal to +20 K? 1) 253ºC 2) 293ºC 3) 253 C 4) 293 C
1. The average kinetic energy of water molecules increases when 1) H 2 O(s) changes to H 2 O( ) at 0ºC 3) H 2 O( ) at 10ºC changes to H 2 O( ) at 20ºC 2) H 2 O( ) changes to H 2 O(s) at 0ºC 4) H 2 O( )
Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test
Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test NAME Section 7.1 The Mole: A Measurement of Matter A. What is a mole? 1. Chemistry is a quantitative science. What does this term mean?
Metals and Non-metals. Comparison of physical properties of metals and non metals
Metals and Non-metals Comparison of physical properties of metals and non metals PHYSICAL PROPERTY METALS NON-METALS Physical State Metallic lustre (having a shining surface) Mostly solids (Liquid -mercury)
Solution. Practice Exercise. Concept Exercise
Example Exercise 9.1 Atomic Mass and Avogadro s Number Refer to the atomic masses in the periodic table inside the front cover of this textbook. State the mass of Avogadro s number of atoms for each of
SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001
SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001 1. A small pin contains 0.0178 mol of iron. How many atoms of iron are in the pin? 2. A sample
FIRST GRADE CHEMISTRY
FIRST GRADE CHEMISTRY 1 WEEK LESSON PLANS AND ACTIVITIES ROCK CYCLE OVERVIEW OF FIRST GRADE CHEMISTRY WEEK 1. PRE: Comparing solids, gases, liquids, and plasma. LAB: Exploring how states of matter can
4.4 Calculations Involving the Mole Concept
44 Section 43 Questions 1 Define Avogadro s constant, and explain its significance in quantitative analysis 2 Distinguish between the terms atomic mass and molar mass 3 Calculate the mass of a molecule
Concept 1. The meaning and usefulness of the mole. The mole (or mol) represents a certain number of objects.
Chapter 3. Stoichiometry: Mole-Mass Relationships in Chemical Reactions Concept 1. The meaning and usefulness of the mole The mole (or mol) represents a certain number of objects. SI def.: the amount of
Matter Properties and Changes
Matter Properties and Changes Section 3.1 Properties of Matter pages 70 75 b. Iron is more dense than aluminum. Problem-Solving Lab 1. Explain why the flow of a compressed gas must be controlled for practical
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
Elements, Atoms & Ions
Introductory Chemistry: A Foundation FOURTH EDITION by Steven S. Zumdahl University of Illinois Elements, Atoms & Ions Chapter 4 1 2 Elements Aims: To learn about the relative abundances of the elements,
Section 1: Arranging the Elements Pages 106-112
Study Guide Chapter 5 Periodic Table Section 1: Arranging the Elements Pages 106-112 DISCOVERING A PATTERN 1. How did Mendeleev arrange the elements? a. by increasing density b. by increasing melting point
Name Class Date. What is ionic bonding? What happens to atoms that gain or lose electrons? What kinds of solids are formed from ionic bonds?
CHAPTER 1 2 Ionic Bonds SECTION Chemical Bonding BEFORE YOU READ After you read this section, you should be able to answer these questions: What is ionic bonding? What happens to atoms that gain or lose
2 MATTER. 2.1 Physical and Chemical Properties and Changes
2 MATTER Matter is the material of which the universe is composed. It has two characteristics: It has mass; and It occupies space (i.e., it has a volume). Matter can be found in three generic states: Solid;
W1 WORKSHOP ON STOICHIOMETRY
INTRODUCTION W1 WORKSHOP ON STOICHIOMETRY These notes and exercises are designed to introduce you to the basic concepts required to understand a chemical formula or equation. Relative atomic masses of
Bonding in Elements and Compounds. Covalent
Bonding in Elements and Compounds Structure of solids, liquids and gases Types of bonding between atoms and molecules Ionic Covalent Metallic Many compounds between metals & nonmetals (salts), e.g. Na,
Experiment 5. Chemical Reactions A + X AX AX A + X A + BX AX + B AZ + BX AX + BZ
Experiment 5 Chemical Reactions OBJECTIVES 1. To observe the various criteria that are used to indicate that a chemical reaction has occurred. 2. To convert word equations into balanced inorganic chemical
Chapter 16: Tests for ions and gases
The position of hydrogen in the reactivity series Hydrogen, although not a metal, is included in the reactivity series because it, like metals, can be displaced from aqueous solution, only this time the
Chemical Change Unit Test
Chemical Change Unit Test Student Name Class Properties of Matter 1. Aluminum foam is used to create lighter, safer cars. The reason that a lighter car is a safer car is because aluminum foam is A. less
EXPERIMENT 12: Empirical Formula of a Compound
EXPERIMENT 12: Empirical Formula of a Compound INTRODUCTION Chemical formulas indicate the composition of compounds. A formula that gives only the simplest ratio of the relative number of atoms in a compound
Chemical Building Blocks: Chapter 3: Elements and Periodic Table
Name: Class: Date: Chemical Building Blocks: Chapter 3: Elements and Periodic Table Study Guide Multiple Choice Identify the letter of the choice that best completes the statement or answers the question.
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
Heterogeneous Homogenous. Mixtures; Solutions. Phases of matter: Solid. Phases of Matter: Liquid. Phases of Matter: Gas. Solid, Liquid, Gas
Phases of matter: Solid Heterogeneous Homogenous Mixtures Solutions Phases of Matter: Liquid Atoms and molecules are more spaced out and now can move. The material can be slightly compressed into a smaller
A Study of Matter. Video Notes
A Study of Matter Video Notes In this lesson you will: Define physical property, chemical property and chemical change. Describe the phases of matter. Label properties as physical or chemical. Label changes
Composition of nucleus. Priority Vocabulary: Electron, Proton, Neutron, Nucleus, Isotopes, Atomic Number, Atomic Mass, Element, Electron Shell,
Lake County, Lakeview, 9 th grade, Physical Science, Brent Starr Standard: H1P1 Explain how atomic structure is related to the properties of elements and their position in the Periodic Table. Explain how
Chemical Changes. Measuring a Chemical Reaction. Name(s)
Chemical Changes Name(s) In the particle model of matter, individual atoms can be bound tightly to other atoms to form molecules. For example, water molecules are made up of two hydrogen atoms bound to
2. John Dalton did his research work in which of the following countries? a. France b. Greece c. Russia d. England
CHAPTER 3 1. Which combination of individual and contribution is not correct? a. Antoine Lavoisier - clarified confusion over cause of burning b. John Dalton - proposed atomic theory c. Marie Curie - discovered
Balancing Chemical Equations Worksheet
Balancing Chemical Equations Worksheet Student Instructions 1. Identify the reactants and products and write a word equation. 2. Write the correct chemical formula for each of the reactants and the products.
Part B 2. Allow a total of 15 credits for this part. The student must answer all questions in this part.
Part B 2 Allow a total of 15 credits for this part. The student must answer all questions in this part. 51 [1] Allow 1 credit for 3 Mg(s) N 2 (g) Mg 3 N 2 (s). Allow credit even if the coefficient 1 is
Ionic and Metallic Bonding
Ionic and Metallic Bonding BNDING AND INTERACTINS 71 Ions For students using the Foundation edition, assign problems 1, 3 5, 7 12, 14, 15, 18 20 Essential Understanding Ions form when atoms gain or lose
Work hard. Be nice. Name: Period: Date: UNIT 1: Introduction to Matter Lesson 4: A Fine Line Between Compounds and Mixtures
Name: Period: Date: UNIT 1: Introduction to Matter Lesson 4: A Fine Line Between Compounds and Mixtures Do Now: PRE-READING OPEN-NOTES QUIZ! By the end of today, you will have an answer to: How do pure
The Mole. Chapter 2. Solutions for Practice Problems
Chapter 2 The Mole 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 contains the full set of
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
University of Pittsburgh Safety Manual Subject: COMBUSTIBLE METALS. EH&S Guideline Number: 02-005. Effective Date 09/10/13.
Page 1 of 7 These guidelines provide requirements for all University faculty, staff, and students using, handling, or storing combustible metals. These requirements are established to ensure faculty, staff
The Periodic Table: Periodic trends
Unit 1 The Periodic Table: Periodic trends There are over one hundred different chemical elements. Some of these elements are familiar to you such as hydrogen, oxygen, nitrogen and carbon. Each one has
Metalloids will also react with oxygen. Upon reaction with oxygen silicon forms silicon dioxide, the main component of sand.
The Preparation and Properties of xygen Reading assignment: Chang, Chemistry 10 th edition, pp. 135-141. Goals We will observe the thermal decomposition of several oxygen-containing compounds called oxides.
Letter to the Student... 5 Test-Taking Checklist... 6 Next Generation Sunshine State Standards Correlation Chart... 7
Table of Contents Letter to the Student..................................... 5 Test-Taking Checklist.................................... 6 Next Generation Sunshine State Standards Correlation Chart...
IB Chemistry. DP Chemistry Review
DP Chemistry Review Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant Assessment statement Apply the mole concept to substances. Determine the number of particles and the amount
7.4. Using the Bohr Theory KNOW? Using the Bohr Theory to Describe Atoms and Ions
7.4 Using the Bohr Theory LEARNING TIP Models such as Figures 1 to 4, on pages 218 and 219, help you visualize scientific explanations. As you examine Figures 1 to 4, look back and forth between the diagrams
Stoichiometry Review
Stoichiometry Review There are 20 problems in this review set. Answers, including problem set-up, can be found in the second half of this document. 1. N 2 (g) + 3H 2 (g) --------> 2NH 3 (g) a. nitrogen
Atomic mass is the mass of an atom in atomic mass units (amu)
Micro World atoms & molecules Laboratory scale measurements Atomic mass is the mass of an atom in atomic mass units (amu) By definition: 1 atom 12 C weighs 12 amu On this scale 1 H = 1.008 amu 16 O = 16.00
About the course GENERAL CHEMISTRY. Recommended literature: Chemistry: science of the matter. Responsible for the course: Dr.
About the course GENERAL CHEMISTRY University of Pécs Medical School Academic year 2009-2010. Responsible for the course: Dr. Attila AGÓCS Optional course for 2 credit points. To have grade at the and
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
Problem Solving. Percentage Composition
Skills Worksheet Problem Solving Percentage Composition Suppose you are working in an industrial laboratory. Your supervisor gives you a bottle containing a white crystalline compound and asks you to determine
CHEMICAL DETERMINATION OF EVERYDAY HOUSEHOLD CHEMICALS
CHEMICAL DETERMINATION OF EVERYDAY HOUSEHOLD CHEMICALS Purpose: It is important for chemists to be able to determine the composition of unknown chemicals. This can often be done by way of chemical tests.
Santa Monica College Chemistry 11
Types of Reactions Objectives The objectives of this laboratory are as follows: To perform and observe the results of a variety of chemical reactions. To become familiar with the observable signs of chemical
Chapter 13 - LIQUIDS AND SOLIDS
Chapter 13 - LIQUIDS AND SOLIDS Problems to try at end of chapter: Answers in Appendix I: 1,3,5,7b,9b,15,17,23,25,29,31,33,45,49,51,53,61 13.1 Properties of Liquids 1. Liquids take the shape of their container,
Chapter 7 Periodic Properties of the Elements
Chapter 7 Periodic Properties of the Elements 1. Elements in the modern version of the periodic table are arranged in order of increasing. (a). oxidation number (b). atomic mass (c). average atomic mass
Physical and Chemical Properties and Changes
Physical and Chemical Properties and Changes An understanding of material things requires an understanding of the physical and chemical characteristics of matter. A few planned experiments can help you
Mixtures and Pure Substances
Unit 2 Mixtures and Pure Substances Matter can be classified into two groups: mixtures and pure substances. Mixtures are the most common form of matter and consist of mixtures of pure substances. They
Elements, Compounds, and Mixtures
Elements, Compounds, and Mixtures Elements........... 82 Internet Connect..... 85 Compounds......... 86 QuickLab........... 87 Physics Connection... 88 Internet Connect..... 89 Mixtures........... 90 MathBreak..........
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
Moles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations
Moles Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations Micro World atoms & molecules Macro World grams Atomic mass is the mass of an
In this experiment, we will use three properties to identify a liquid substance: solubility, density and boiling point..
Identification of a Substance by Physical Properties 2009 by David A. Katz. All rights reserved. Permission for academic use provided the original copyright is included Every substance has a unique set
Experiment 12- Classification of Matter Experiment
Experiment 12- Classification of Matter Experiment Matter can be classified into two groups: mixtures and pure substances. Mixtures are the most common form of matter and consist of mixtures of pure substances.
Physical Changes and Chemical Reactions
Physical Changes and Chemical Reactions Gezahegn Chaka, Ph.D., and Sudha Madhugiri, Ph.D., Collin College Department of Chemistry Objectives Introduction To observe physical and chemical changes. To identify
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)
Chapter 6 Assessment. Name: Class: Date: ID: A. Multiple Choice Identify the choice that best completes the statement or answers the question.
Name: Class: Date: ID: A Chapter 6 Assessment Multiple Choice Identify the choice that best completes the statement or answers the question. 1. When an atom loses an electron, it forms a(n) a. anion. c.
Unit 2 Matter and Chemical Change. Unit Test
Unit Test Student Name Class Section 1 Properties of Matter 1. Aluminum foam is used to create lighter, safer cars. The reason that a lighter car is a safer car is because aluminum foam is A. less rigid
Periodic Table, Valency and Formula
Periodic Table, Valency and Formula Origins of the Periodic Table Mendelѐѐv in 1869 proposed that a relationship existed between the chemical properties of elements and their atomic masses. He noticed
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.
Chapter 5, Calculations and the Chemical Equation
1. How many iron atoms are present in one mole of iron? Ans. 6.02 1023 atoms 2. How many grams of sulfur are found in 0.150 mol of sulfur? [Use atomic weight: S, 32.06 amu] Ans. 4.81 g 3. How many moles
Review and apply Investigation 5. Let s review Pages 311-312
Review and apply Investigation 5 Let s review Pages 311-312 1. After you tested all the known powders with all the test liquids, describe what you did to identify the unknown powder. Students should have
3 CHEMICAL FOUNDATIONS: ELEMENTS, ATOMS AND IONS
3 CHEMICAL FOUNDATIONS: ELEMENTS, ATOMS AND IONS All matter is built up from chemical combinations of elements. As of 2003, there are 114 known elements, of which 88 are naturally occurring; the remaining
Question Bank Electrolysis
Question Bank Electrolysis 1. (a) What do you understand by the terms (i) electrolytes (ii) non-electrolytes? (b) Arrange electrolytes and non-electrolytes from the following substances (i) sugar solution
UNIT (2) ATOMS AND ELEMENTS
UNIT (2) ATOMS AND ELEMENTS 2.1 Elements An element is a fundamental substance that cannot be broken down by chemical means into simpler substances. Each element is represented by an abbreviation called
7. 1.00 atm = 760 torr = 760 mm Hg = 101.325 kpa = 14.70 psi. = 0.446 atm. = 0.993 atm. = 107 kpa 760 torr 1 atm 760 mm Hg = 790.
CHATER 3. The atmosphere is a homogeneous mixture (a solution) of gases.. Solids and liquids have essentially fixed volumes and are not able to be compressed easily. have volumes that depend on their conditions,
20.2 Chemical Equations
All of the chemical changes you observed in the last Investigation were the result of chemical reactions. A chemical reaction involves a rearrangement of atoms in one or more reactants to form one or more
87 16 70 20 58 24 44 32 35 40 29 48 (a) graph Y versus X (b) graph Y versus 1/X
HOMEWORK 5A Barometer; Boyle s Law 1. The pressure of the first two gases below is determined with a manometer that is filled with mercury (density = 13.6 g/ml). The pressure of the last two gases below
Unit 6 The Mole Concept
Chemistry Form 3 Page 62 Ms. R. Buttigieg Unit 6 The Mole Concept See Chemistry for You Chapter 28 pg. 352-363 See GCSE Chemistry Chapter 5 pg. 70-79 6.1 Relative atomic mass. The relative atomic mass
APPENDIX B: EXERCISES
BUILDING CHEMISTRY LABORATORY SESSIONS APPENDIX B: EXERCISES Molecular mass, the mole, and mass percent Relative atomic and molecular mass Relative atomic mass (A r ) is a constant that expresses the ratio
Cambridge International Examinations Cambridge International General Certificate of Secondary Education
Cambridge International Examinations Cambridge International General Certificate of Secondary Education *0123456789* CHEMISTRY 0620/03 Paper 3 Theory (Core) For Examination from 2016 SPECIMEN PAPER 1 hour
Periodic Table Bingo
Periodic Table Bingo Materials: Periodic Table Bingo Card Periodic Table of Elements Colored pieces of paper or plastic discs Instructions: Print the Periodic Table Bingo Cards (pages 5-44). There are
Chapter 5 TEST: The Periodic Table name
Chapter 5 TEST: The Periodic Table name HPS # date: Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The order of elements in the periodic table is based
Chapter Test B. Chapter: Measurements and Calculations
Assessment Chapter Test B Chapter: Measurements and Calculations PART I In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1.
Chapter 8: Chemical Equations and Reactions
Chapter 8: Chemical Equations and Reactions I. Describing Chemical Reactions A. A chemical reaction is the process by which one or more substances are changed into one or more different substances. A chemical
HOMEWORK 4A. Definitions. Oxidation-Reduction Reactions. Questions
HOMEWORK 4A Oxidation-Reduction Reactions 1. Indicate whether a reaction will occur or not in each of following. Wtiring a balcnced equation is not necessary. (a) Magnesium metal is added to hydrochloric
Name: Class: Date: ID: A
Name: Class: Date: ID: A Chapter 2 Assessment Multiple Choice Identify the choice that best completes the statement or answers the question. Complete short answer questions on a separate sheet of paper.
General Chemistry Lab Experiment 6 Types of Chemical Reaction
General Chemistry Lab Experiment 6 Types of Chemical Reaction Introduction Most ordinary chemical reactions can be classified as one of five basic types. The first type of reaction occurs when two or more
Name Date Class CHAPTER 1 REVIEW. Answer the following questions in the space provided.
CHAPTER 1 REVIEW Matter and Change SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. a Technological development of a chemical product often (a) lags behind basic research
PHYSICAL AND CHEMICAL PROPERTIES AND CHANGES
PHYSICAL AND CHEMICAL PROPERTIES AND CHANGES Name Key PHYSICAL PROPERTY CHEMICAL PROPERTY 1. observed with senses 1. indicates how a substance 2. determined without destroying matter reacts with something
Metals are located on the left side of the periodic table and are generally shiny, malleable, ductile, and good conductors.
Section 1: are located on the left side of the periodic table and are generally shiny, malleable, ductile, and good conductors. K What I Know W What I Want to Find Out L What I Learned Essential Questions
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
Test 5 Review questions. 1. As ice cools from 273 K to 263 K, the average kinetic energy of its molecules will
Name: Thursday, December 13, 2007 Test 5 Review questions 1. As ice cools from 273 K to 263 K, the average kinetic energy of its molecules will 1. decrease 2. increase 3. remain the same 2. The graph below