Physical Science 1 Progression
|
|
|
- Bruce Harris
- 7 years ago
- Views:
Transcription
1 Physical Science 1 Progression This progression is the about the structure and properties of matter. Matter is composed of material that is too small to be seen, but is understood in terms of the types of atoms present and how they interact. Because of these interactions, matter can be found in different states (solid, liquid, gas), have identifiable properties (hardness, conductivity, etc.) and reactions (chemical and physical), which can be predicted. In elementary grades, students learn that matter can be described and classified by its observable properties. Students investigate different kinds of materials to identify patterns such as similarities and differences in their observable properties. The properties could include color, texture, hardness and flexibility. Students plan and conduct an investigation in collaboration with others to produce data that will serve as evidence that answers a question. Also, students learn that matter can exist in various forms; solids and liquids. At middle school, students learn that the properties of substances can change when they interact. Chemical and physical reactions can occur as a result of these interactions. Students understand substances are composed of molecules. If the molecules of a substance are all of one type, the substance is considered to be pure. Students are able to determine if a chemical change has occurred by analyzing and interpreting data of the properties of a substance before and after the substances interact. Chemical changes could include oxidization, burning sugar or steel wool, and mixing zinc with hydrogen chloride. At the high school level, students learn about the periodic table. Students learn that the periodic table is designed based upon atomic structure; that is, it orders elements horizontally by the number of protons in the atom s nucleus and places those with similar chemical properties in columns. Students also learn that the repeating patterns of the periodic table reflect patterns of outer electron states and that these patterns can be used to
2 predict and support explanations for the outcome of simple chemical reactions. For example, sodium and chloride (NaCl) combine to form a stable molecule because of their electron configuration and the desire for a molecule to reach stability. Grade 4: Page 3 Grade 7: Page 4 Grade 11: Pages 5 and 6
3 Grade 4: Alternate K-PREP Aligned to KCAS for Science: Make observations (could include looking for patterns) to describe and classify different kinds of materials by their observable properties. 2-PS1-1: Plan and conduct an investigation to describe and classify different kinds of materials by their observable properties. [Clarification Statement: Observations could include color, texture, hardness, and flexibility. Patterns could include the similar properties that different materials share.] SEP (Science and Engineering Practices) Plan and conduct an investigation collaboratively to produce data to serve as the basis for evidence to answer a question. DCI (Disciplinary Core Ideas) Different kinds of matter exist and many of them can be either solid or liquid, depending on temperature. Matter can be described and classified by its observable properties. CC (Crosscutting Concepts) Patterns in the natural and human designed world can be observed.
4 Grade 7: Alternate K-PREP Aligned to KCAS for Science: Interpret data on the characteristic physical and chemical properties of substances before and after the substances interact to determine if a chemical reaction has occurred. 07-PS1-2: Analyze and interpret data on the properties of substances before and after the substances interact to determine if a chemical reaction has occurred. [Clarification Statement: Examples of reactions could include burning sugar or steel wool, fat reacting with sodium hydroxide, and mixing zinc with hydrogen chloride.] SEP (Science and Engineering Practices) Analyze and interpret data to determine similarities and differences in findings. DCI (Disciplinary Core Ideas) Each pure substance has characteristic physical and chemical properties (for any bulk quantity under given conditions) that can be used to identify it. CC (Crosscutting Concepts) Macroscopic patterns are related to the nature of microscopic and atomic-level structure.
5 Grade 11: Alternate K-PREP Aligned to KCAS for Science: Construct an explanation for the outcome of a simple chemical reaction (specific to elements in families 1, 2, and 13-18), based on the outermost electron states of atoms and trends in the periodic table. HS-PS1-2: Construct and revise an explanation for the outcome of a simple chemical reaction based on the outermost electron states of atoms, trends in the periodic table, and knowledge of the patterns of chemical properties. [Clarification Statement: Examples of chemical reactions could include the reaction of sodium and chlorine, carbon and oxygen, or carbon and hydrogen.] SEP (Science and Engineering Practices) DCI (Disciplinary Core Ideas) CC (Crosscutting Concepts) Construct and revise an explanation based on valid and reliable evidence obtained from a variety of sources (including students' own investigations, models, theories, simulations, peer review) and the assumption that theories and laws that describe the The periodic table orders elements horizontally by the number of protons in the atom's nucleus and places those with similar chemical properties in columns. The repeating patterns of this table reflect patterns of outer electron states. Different patterns may be observed at each of the scales at which a system is studied and can provide evidence for causality in explanations of phenomena.
6 natural world operate today as they did in the past and will continue to do so in the future.
7-5.5. Translate chemical symbols and the chemical formulas of common substances to show the component parts of the substances including:
7-5.5 Translate chemical symbols and the chemical formulas of common substances to show the component parts of the substances including: NaCl [salt], H 2 O [water], C 6 H 12 O 6 [simple sugar], O 2 [oxygen
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
PROTONS AND ELECTRONS
reflect Imagine that you have a bowl of oranges, bananas, pineapples, berries, pears, and watermelon. How do you identify each piece of fruit? Most likely, you are familiar with the characteristics of
Test Bank - Chapter 4 Multiple Choice
Test Bank - Chapter 4 The questions in the test bank cover the concepts from the lessons in Chapter 4. Select questions from any of the categories that match the content you covered with students. The
NaCl Lattice Science Activities
NaCl Lattice Science Activities STEM: The Science of Salt Using a Salt Lattice Model Teacher Notes Science Activities A Guided-Inquiry Approach Using the 3D Molecular Designs NaCl Lattice Model Classroom
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
NGSS Evidence Statements Executive Summary of the Front Matter
NGSS Evidence Statements Executive Summary of the Front Matter Overview The NGSS identify assessable performance expectations (PEs), or what students should know and be able to do at the end of instruction.
Lewis Dot Structures of Atoms and Ions
Why? The chemical properties of an element are based on the number of electrons in the outer shell of its atoms. We use Lewis dot structures to map these valence electrons in order to identify stable electron
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
Name Block Date Ch 17 Atomic Nature of Matter Notes Mrs. Peck. atoms- the smallest particle of an element that can be identified with that element
Name Block Date Ch 17 Atomic Nature of Matter Notes Mrs. Peck atoms- the smallest particle of an element that can be identified with that element are the building blocks of matter consists of protons and
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
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
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
Sketch the model representation of the first step in the dissociation of water. H 2. O (l) H + (aq) + OH- (aq) + H 2. OH - (aq) + H 3 O+ (aq)
Lesson Objectives Students will: Create a physical representation of the autoionization of water using the water kit. Describe and produce a physical representation of the dissociation of a strong acid
Type of Chemical Bonds
Type of Chemical Bonds Covalent bond Polar Covalent bond Ionic bond Hydrogen bond Metallic bond Van der Waals bonds. Covalent Bonds Covalent bond: bond in which one or more pairs of electrons are shared
Objectives. PAM1014 Introduction to Radiation Physics. Constituents of Atoms. Atoms. Atoms. Atoms. Basic Atomic Theory
PAM1014 Introduction to Radiation Physics Basic Atomic Theory Objectives Introduce and Molecules The periodic Table Electronic Energy Levels Atomic excitation & de-excitation Ionisation Molecules Constituents
UNIT 2 PRACTICE EXAM (Part 1: General Chemistry)
UIT 2 PRACTICE EXAM (Part 1: General Chemistry) 1. Which would be the best definition of an ionic bond? a. The attraction between the partial positive region of one molecule and the partial negative region
(1) e.g. H hydrogen that has lost 1 electron c. anion - negatively charged atoms that gain electrons 16-2. (1) e.g. HCO 3 bicarbonate anion
GS106 Chemical Bonds and Chemistry of Water c:wou:gs106:sp2002:chem.wpd I. Introduction A. Hierarchy of chemical substances 1. atoms of elements - smallest particles of matter with unique physical and
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
19.1 Bonding and Molecules
Most of the matter around you and inside of you is in the form of compounds. For example, your body is about 80 percent water. You learned in the last unit that water, H 2 O, is made up of hydrogen and
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
IB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily.
The Mole Atomic mass units and atoms are not convenient units to work with. The concept of the mole was invented. This was the number of atoms of carbon-12 that were needed to make 12 g of carbon. 1 mole
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
YIELD YIELD REACTANTS PRODUCTS
Balancing Chemical Equations A Chemical Equation: is a representation of a chemical reaction in terms of chemical formulas Example: 1. Word Description of a Chemical Reaction When methane gas (CH 4 ) burns
Which substance contains positive ions immersed in a sea of mobile electrons? A) O2(s) B) Cu(s) C) CuO(s) D) SiO2(s)
BONDING MIDTERM REVIEW 7546-1 - Page 1 1) Which substance contains positive ions immersed in a sea of mobile electrons? A) O2(s) B) Cu(s) C) CuO(s) D) SiO2(s) 2) The bond between hydrogen and oxygen in
Unit 2: Quantities in Chemistry
Mass, Moles, & Molar Mass Relative quantities of isotopes in a natural occurring element (%) E.g. Carbon has 2 isotopes C-12 and C-13. Of Carbon s two isotopes, there is 98.9% C-12 and 11.1% C-13. Find
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
Summer Holidays Questions
Summer Holidays Questions Chapter 1 1) Barium hydroxide reacts with hydrochloric acid. The initial concentration of the 1 st solution its 0.1M and the volume is 100ml. The initial concentration of the
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
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
Chemistry Diagnostic Questions
Chemistry Diagnostic Questions Answer these 40 multiple choice questions and then check your answers, located at the end of this document. If you correctly answered less than 25 questions, you need to
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
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
Chemistry 151 Final Exam
Chemistry 151 Final Exam Name: SSN: Exam Rules & Guidelines Show your work. No credit will be given for an answer unless your work is shown. Indicate your answer with a box or a circle. All paperwork must
Honors Chemistry: Unit 6 Test Stoichiometry PRACTICE TEST ANSWER KEY Page 1. A chemical equation. (C-4.4)
Honors Chemistry: Unit 6 Test Stoichiometry PRACTICE TEST ANSWER KEY Page 1 1. 2. 3. 4. 5. 6. Question What is a symbolic representation of a chemical reaction? What 3 things (values) is a mole of a chemical
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
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
List the 3 main types of subatomic particles and indicate the mass and electrical charge of each.
Basic Chemistry Why do we study chemistry in a biology course? All living organisms are composed of chemicals. To understand life, we must understand the structure, function, and properties of the chemicals
Writing and Balancing Chemical Equations
Name Writing and Balancing Chemical Equations Period When a substance undergoes a chemical reaction, chemical bonds are broken and new bonds are formed. This results in one or more new substances, often
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.
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?
Noble Gases. Outline Nobel Gas Elements Radon and Health Chemistry Homework
Radon and Other Noble Gases The elements in the last column of the periodic table are all very stable, mono-atomic gases. Until 1962, they were called inert gases because they did not react with other
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
EXAMPLE EXERCISE 4.1 Change of Physical State
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
Bonding Practice Problems
NAME 1. When compared to H 2 S, H 2 O has a higher 8. Given the Lewis electron-dot diagram: boiling point because H 2 O contains stronger metallic bonds covalent bonds ionic bonds hydrogen bonds 2. Which
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
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
PERIODIC TABLE OF GROUPS OF ELEMENTS Elements can be classified using two different schemes.
1 PERIODIC TABLE OF GROUPS OF ELEMENTS Elements can be classified using two different schemes. Metal Nonmetal Scheme (based on physical properties) Metals - most elements are metals - elements on left
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
Name Date Class CHEMICAL QUANTITIES. SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296)
Name Date Class 10 CHEMICAL QUANTITIES SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296) This section defines the mole and explains how the mole is used to measure matter. It also teaches
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
EXPERIMENT 4 The Periodic Table - Atoms and Elements
EXPERIMENT 4 The Periodic Table - Atoms and Elements INTRODUCTION Primary substances, called elements, build all the materials around you. There are more than 109 different elements known today. The elements
STUDY GUIDE AGRICULTURAL SCIENCES GRADE 11
STUDY GUIDE AGRICULTURAL SCIENCES GRADE 11 A publication of Impak Onderwysdiens (Pty) Ltd Copyright reserved. Apart from any fair dealing for the purpose of research, criticism or review as permitted under
Name Date Class CHEMICAL QUANTITIES. SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296)
10 CHEMICAL QUANTITIES SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296) This section defines the mole and explains how the mole is used to measure matter. It also teaches you how to calculate
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,
Chem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses
Chem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses B. Calculations of moles C. Calculations of number of atoms from moles/molar masses 1. Avagadro
Balancing Chemical Equations
Why? Balancing Chemical Equations Atoms are neither created nor destroyed in a chemical reaction, they are just rearranged. In other words, in a chemical reaction, what goes into the reaction must come
ATOMS AND BONDS. Bonds
ATOMS AND BONDS Atoms of elements are the simplest units of organization in the natural world. Atoms consist of protons (positive charge), neutrons (neutral charge) and electrons (negative charge). The
ANSWER KEY. Energy Levels, Electrons and IONIC Bonding It s all about the Give and Take!
ANSWER KEY Energy Levels, Electrons and IONIC Bonding It s all about the Give and Take! From American Chemical Society Middle School Chemistry Unit: Chapter 4 Content Statements: Distinguish the difference
CHEMICAL FORMULAS AND EQUATIONS
reflect Imagine that you and three other classmates had enough supplies and the recipe to make one pepperoni pizza. The recipe might include a ball of dough, a cup of pizza sauce, a cup of cheese, and
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
CHEMICAL REACTIONS AND REACTING MASSES AND VOLUMES
CHEMICAL REACTIONS AND REACTING MASSES AND VOLUMES The meaning of stoichiometric coefficients: 2 H 2 (g) + O 2 (g) 2 H 2 O(l) number of reacting particles 2 molecules of hydrogen react with 1 molecule
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,
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
Unit 3 Study Guide: Electron Configuration & The Periodic Table
Name: Teacher s Name: Class: Block: Date: Unit 3 Study Guide: Electron Configuration & The Periodic Table 1. For each of the following elements, state whether the element is radioactive, synthetic or both.
Getting the most from this book...4 About this book...5
Contents Getting the most from this book...4 About this book....5 Content Guidance Topic 1 Atomic structure and the periodic table...8 Topic 2 Bonding and structure...14 Topic 2A Bonding....14 Topic 2B
What s in a Mole? Molar Mass
LESSON 10 What s in a Mole? Molar Mass OVERVIEW Key Ideas Lesson Type Lab: Groups of 4 Chemists compare moles of substances rather than masses because moles are a way of counting atoms. When considering
THE PERIODIC TABLE O F T H E E L E M E N T S. The Academic Support Center @ Daytona State College (Science 117, Page 1 of 27)
THE PERIODIC TABLE O F T H E E L E M E N T S The Academic Support Center @ Daytona State College (Science 117, Page 1 of 27) THE PERIODIC TABLE In 1872, Dmitri Mendeleev created the periodic table arranged
Balancing Chemical Equations
Balancing Chemical Equations Academic Success Center Science Tutoring Area Science Tutoring Area Law of Conservation of Mass Matter cannot be created nor destroyed Therefore the number of each type of
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.
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
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;
Thermodynamics and Equilibrium
Chapter 19 Thermodynamics and Equilibrium Concept Check 19.1 You have a sample of 1.0 mg of solid iodine at room temperature. Later, you notice that the iodine has sublimed (passed into the vapor state).
Unit 9 Stoichiometry Notes (The Mole Continues)
Unit 9 Stoichiometry Notes (The Mole Continues) is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations
Unit 3.2: The Periodic Table and Periodic Trends Notes
Unit 3.2: The Periodic Table and Periodic Trends Notes The Organization of the Periodic Table Dmitri Mendeleev was the first to organize the elements by their periodic properties. In 1871 he arranged the
Revising the Periodic Table
Chemical misconceptions 65 Revising the eriodic Table Target level Topic Rationale This exercise is intended for students in the 14 16 year old age range, who have studied the eriodic Table. It may also
Part I: Principal Energy Levels and Sublevels
Part I: Principal Energy Levels and Sublevels As you already know, all atoms are made of subatomic particles, including protons, neutrons, and electrons. Positive protons and neutral neutrons are found
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.
In the box below, draw the Lewis electron-dot structure for the compound formed from magnesium and oxygen. [Include any charges or partial charges.
Name: 1) Which molecule is nonpolar and has a symmetrical shape? A) NH3 B) H2O C) HCl D) CH4 7222-1 - Page 1 2) When ammonium chloride crystals are dissolved in water, the temperature of the water decreases.
Name: Teacher: Pd. Date:
Name: Teacher: Pd. Date: STAAR Tutorial : Energy and Matter: Elements, Compounds, and Chemical Equations: 6.5C Differentiate between elements and compounds on the most basic level. 8.5F Recognize whether
Matter. Atomic weight, Molecular weight and Mole
Matter Atomic weight, Molecular weight and Mole Atomic Mass Unit Chemists of the nineteenth century realized that, in order to measure the mass of an atomic particle, it was useless to use the standard
hij GCSE Additional Science Chemistry 2 Higher Tier Chemistry 2H SPECIMEN MARK SCHEME Version 1.0
hij GCSE Additional Science Chemistry 2 Higher Tier Chemistry 2H SPECIMEN MARK SCHEME Version.0 Copyright 20 AQA and its licensors. All rights reserved. The Assessment and Qualifications Alliance (AQA)
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
The Mole Concept. The Mole. Masses of molecules
The Mole Concept Ron Robertson r2 c:\files\courses\1110-20\2010 final slides for web\mole concept.docx The Mole The mole is a unit of measurement equal to 6.022 x 10 23 things (to 4 sf) just like there
CHEMICAL FORMULAS AND FORMULA WEIGHT CALCULATIONS
CHEMICAL FORMULAS AND FORMULA WEIGHT CALCULATIONS 1. THE MEANING OF A CHEMICAL FORMULA A chemical formula is a shorthand method of representing the elements in a compound. The formula shows the formulas
Chemistry Post-Enrolment Worksheet
Name: Chemistry Post-Enrolment Worksheet The purpose of this worksheet is to get you to recap some of the fundamental concepts that you studied at GCSE and introduce some of the concepts that will be part
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.
The Empirical Formula of a Compound
The Empirical Formula of a Compound Lab #5 Introduction A look at the mass relationships in chemistry reveals little order or sense. The ratio of the masses of the elements in a compound, while constant,
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
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
6 Reactions in Aqueous Solutions
6 Reactions in Aqueous Solutions Water is by far the most common medium in which chemical reactions occur naturally. It is not hard to see this: 70% of our body mass is water and about 70% of the surface
NORTH DAKOTA SCIENCE CONTENT STANDARDS
NORTH DAKOTA SCIENCE CONTENT STANDARDS Draft April 2014 Draft Performance Expectations by Grade: Middle School Physical Science Released for Public Comment North Dakota Department of Public Instruction
Instructions Answer all questions in the spaces provided. Do all rough work in this book. Cross through any work you do not want to be marked.
GCSE CHEMISTRY Higher Tier Chemistry 1H H Specimen 2018 Time allowed: 1 hour 45 minutes Materials For this paper you must have: a ruler a calculator the periodic table (enclosed). Instructions Answer all
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
Instructors Guide: Atoms and Their Isotopes
Instructors Guide: Atoms and Their Isotopes Standards Connections Connections to NSTA Standards for Science Teacher Preparation C.3.a.1 Fundamental structures of atoms and molecules. C.3.b.27 Applications
Unit 9 Compounds Molecules
Unit 9 Compounds Molecules INTRODUCTION Compounds are the results of combinations of elements. These new substances have unique properties compared to the elements that make them up. Compounds are by far
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
Liquid phase. Balance equation Moles A Stoic. coefficient. Aqueous phase
STOICHIOMETRY Objective The purpose of this exercise is to give you some practice on some Stoichiometry calculations. Discussion The molecular mass of a compound is the sum of the atomic masses of all
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...
Formulas, Equations and Moles
Chapter 3 Formulas, Equations and Moles Interpreting Chemical Equations You can interpret a balanced chemical equation in many ways. On a microscopic level, two molecules of H 2 react with one molecule