Ionic Compounds - Examples
|
|
|
- Avis Townsend
- 5 years ago
- Views:
Transcription
1 Quick Review - Classification of Matter (end of Chapter 1 material) - Fundamental Laws - Dalton s Atomic Theory - Cathode-Ray Tube Experiment (J.J. Thomson) - Plum Pudding Model - Alpha-Particle Bombardment Expt. (Rutherford) - Nuclear Atom - Elemental Designation - Isotopes - Periodic Table - Simple Molecule Formation - Nomenclature
2 Ionic Compounds 1. The cation is always written first, the anion is named second. In ionic compounds, the cation is usually a metal. When a metal is in a compound, the compound is assumed ionic. 2. The cations: (a) monoatomic metals: use base name of the metal. (b) transition metals: use base name of the metal followed by a roman numeral indicating charge. (c) polyatomic cations: the only one to memorize NH 4 + = ammonium 3. The anions: (a) monoatomic nonmetals: use the base name of the nonmetal, then add the -ide suffix. (b) polyatomic anions: memorize the anions in Table 2.5.
3 Ionic Compounds - Examples Name the following compounds: (a) NaCl (b) NH 4 NO 3 (c) Li 3 N Give the molecular formula for the following compounds: (a) Aluminum oxide (b) Chromium (III) chloride (c) Sodium sulfite
4 Covalent Compounds 1. The first element in the formula is named first using the base name. 2. The second element is named like an anion (base name plus -ide suffix). 3. Use prefixes to denote numbers for cations and anions (Table 2.6) 4. The prefix mono is never used for naming the first element in a formula (it is assumed). 5. Avoid awkward pronounciations Example: CO = carbon monoxide not carbon monooxide. 6. Know common names like H 2 O = water, and C 6 H 12 O 6 = glucose; memorize the names of the acids in Table 2.7 and 2.8 (as well as HClO 4, perchloric acid).
5 Covalent Compounds - Examples Name the following compounds: (a) PCl 5 (b) SF 6 (c) SO 2 Give the molecular formula for the following compounds: (d) Tetraphosphorous decaoxide (e) Carbon dioxide (f) Sulfur trioxide
6 TO MEMORIZE (1) Names of elements 1-36 (2) Names of all alkali metals, alkaline earth metals, halogens and noble gases.
7 TO MEMORIZE
8 TO MEMORIZE (1) Identify a compound as being ionic or covalent. (2) Utilize the appropriate rules to name the compound. (3) Will also be asked to write out molecular formulas of compounds from a given name.
9 Counting by Weighing Counting individual jelly beans is a tedious process. A more efficient process would be to count by weighing. What do you need to know about each jelly bean in order to utilize this method? Need to know the average mass of a jelly bean.
10 What does this have to do w/ Chem? We count atoms in the same way! An atom is a million times smaller than the thickest human hair. We must know the average mass of atoms.
11 Atomic Mass 12 C is assigned a mass of exactly 12 atomic mass units, masses of all other atoms are relative to this standard. Mass spectrometer is used to measure accurate atomic masses.
12 Relative Atomic Masses Mass of 13 C Mass of 12 C = Mass of 13 C = ( )(12 amu) = amu The masses of all other atoms are determined in the same way.
13 Atomic Mass Question: Why is the atomic mass of carbon and not 12.00? Answer: Question: What two things do you need to know to determine average mass? Answer: Example: 98.89% (12 amu) % ( amu) = amu
14 The Mole Mole number equal to the number of carbon atoms in exactly 12 grams of pure 12 C x called Avogadro s number. A mole of anything represents x units. A mole of eggs represents x eggs. One mole of Cu, Al, Fe, S, I and Hg.
15 The Mole The mole is defined such that a sample of a natural element with a mass equal to the element s atomic mass expressed in grams contains 1 mole of atoms.
16 The Mole Since the same 12 C standard is used to define relative atomic masses and the mole, then the atomic mass of any element in units of grams will be the molar mass (mass of one mole of that substance) of that element. (6.022 x atoms) 12 amu atom = 12 g x amu = 1 g This relationship can be used to convert between atomic mass units and grams.
17 The Mole Question: A small atomic bomb requires 4.0 moles of uranium. How many grams of uranium and how many uranium atoms does 4.0 moles represent? Answer:
18 Molar Mass Molar Mass of a substance is the mass in grams of one mole of the compound. To determine molar mass of a compound we must know the molecular formula. The molecular formula tells us the actual number and kinds of atoms that make up a compound. Also tells us the mole ratios.
19 Example: H 2 SO 4 Calculation of Molar Mass
20 Review Example Chapter 3 #58: Chloral hydrate (C 2 H 3 Cl 3 O 2 ) is a drug formerly used as a sedative and hypnotic. It is the compound used to make Mickey Finns in detective stories. (a) Calculate the molar mass of chloral hydrate (b) What amount (moles) of chloral hydrate molecules are in g of chloral hydrate. (c) What is the mass in grams of 2.0 x 10-2 mol chloral hydrate? (d) What number of chlorine atoms are in 5.0 g of chloral hydrate? (e) What mass of chloral hydrate would contain 1.0 g of Cl? (f) What is the mass of exactly 500 molecules of chloral hydrate?
Using the Periodic Table
Quick Review - Dimensional Analysis - Density - Classification of Matter (end of Chapter 1 material) - Fundamental Laws - Dalton s Atomic Theory - Cathode-Ray Tube Experiment (J.J. Thomson) - Plum Pudding
Law of Definite Proportion** (Proust): A given compound always contains exactly the same proportion of elements by mass.
# 10 Notes Unit 2: Laws, Properties & Mols Ch. Atoms, Molecules, Ions 5 Chemical Laws: I. Law of Conservation of Mass** (Lavoisier): Mass cannot be created or destroyed. II. III. IV. Law of Definite Proportion**
Unit 2. Atoms, Molecules, and Ions
Unit 2. Atoms, Molecules, and Ions Upon successful completion of this unit, the students should be able to: 2.1 State and be able to apply the Law of Conservation of Mass, Law of Definite Proportions,
Atoms, Molecules, and Ions
Chapter 2 Atoms, Molecules, l and Ions Chapter 2 Table of Contents 2.1 The Early History of Chemistry 2.2 Fundamental Chemical Laws 23 2.3 Dalton s Atomic Theory 2.4 Early Experiments to Characterize the
Summary Chapter One 1. Scientific Method (know definitions). 2. Quantitative versus Qualitative measurements. 3. Accuracy versus Precision.
Summary Chapter One 1. Scientific Method (know definitions). 2. Quantitative versus Qualitative measurements. 3. Accuracy versus Precision. 4. Systematic versus Random errors. 5. Significant Figures. 6.
Chapter 2. Atoms, Molecules, and Ions
Chapter 2 Atoms, Molecules, and Ions Section 2.1 The Early History of Chemistry Early History of Chemistry Greeks were the first to attempt to explain why chemical changes occur. Alchemy dominated for
Chapter 2 Atoms, Molecules and Ions
Sec$on 2.1 The Early History of Chemistry Chapter 2 Atoms, Molecules and Ions Sec$on 2.1 The Early History of Chemistry Early History of Chemistry Greeks were the first to a?empt to explain why chemical
Summer Assignment Part 2
Summer Assignment Part 2 Name: 1. Metric Conversions. Remember 1 cm 3 = 1 ml 1 L = 1 dm 3 ITEM GIVEN METRIC UNIT DESIRED METRIC UNIT A 8.43 cm mm B 2.41 x 10 2 cm m C 294.5 nm cm D 1.445 x 10 4 m km E
Memorize For SOL. Ionization Energy = lose or remove electrons
Memorize For SOL Understanding The Periodic Table: Ionization Energy = lose or remove electrons Electronegativity = attract or steal electrons Atomic radius = Size Electron affinity = gain electrons Charge
Voltage source. Voltage source. Voltage source
Chapter 2 Atoms, Molecules, and Ions History Greeks Democritus and Leucippus atomos Aristotle elements Alchemy 1660 Robert Boyle experimental definition of element. Lavoisier Father of modern chemistry
AP* Chapter 2. Atoms, Molecules, and Ions. Monday, September 16, 13
AP* Chapter 2 Atoms, Molecules, and Ions AP Learning Objectives LO 1.1 The student can justify the observation that the ratio of the masses of the constituent elements in any pure sample of that compound
Chapter 2. Atoms, Molecules, and Ions. Copyright 2018 Cengage Learning. All Rights Reserved.
Chapter 2 Atoms, Molecules, and Ions Chapter 2 Table of Contents (2.1) (2.2) (2.3) (2.4) (2.5) (2.6) (2.7) (2.8) The early history of chemistry Fundamental chemical laws Dalton s atomic theory Early experiments
The Components of Matter
The Components of Matter Elements the basic building blocks of matter Ancient Greeks four elements: earth, air, fire and water The atomic idea Democritus there are atoms and void. Boyle (17 th century)
AP CHEMISTRY THINGS TO KNOW
AP CHEMISTRY THINGS TO KNOW Diatomic Molecules H2-hydrogen gas (do not write H) N2-nitrogen gas (do no write N) O2-oxygen gas (do not write O) F2-fluorine gas (do not write F) Cl2-chlorine gas (do not
1 st Semester Final Review Sheet (Chapters 2-7)
CP Chemistry Name: Period: 1 st Semester Final Review Sheet (Chapters 2-7) Matter (Chapter 2) 1. What is the definition of an element? 2. What is the definition of a compound? 3. What is the definition
Chapter 2 Atoms and Elements
Chapter 2 Atoms and Elements Law of Conservation of Mass in a chemical reaction, matter is neither created nor destroyed total mass of the materials you have before the reaction must equal the total mass
Naming and Counting Atoms and Molecules. Chemistry--Unit 2
Naming and Counting Atoms and Molecules Chemistry--Unit 2 Masses of 22.4 L O 2, N 2, & HCl N 2 28 g O 2 32 g HCl 36.5 g Observation: At 1 atmosphere pressure and 0 o C, 22.4 L of 3 different gases have
Chemical Bonding and Naming Compounds. Ionic. Acid. Base. Oct 4 7:40 PM
Chemical Bonding and Naming Compounds (Chapter 9) Types of Bonds Ionic Bonds Molecular Bonds Types of Compounds Ionic Molecular Acid Base Chemical Bonding Atoms will bond together using their valence electrons.
Chapter 3 - Molecules, Compounds and Chemical Equations
Chapter 3 - Molecules, Compounds and Chemical Equations Section 3.2 two general types of bonding between atoms found in compounds, ionic and covalent ionic bonds result when electrons have been transferred
Chapter 2 Reading Guide AP Chemistry Date: Per:
Chapter 2 Reading Guide Name: AP Chemistry 2016-2017 Date: Per: This chapter is foundational to concepts in AP Chemistry curriculum in Big Ideas 1 and 3. These two big ideas discuss the building materials
Chapter 2. The Components of Matter
Chapter 2. The Components of Matter 1 The Periodic Table (Section 2.6) 13 Al 26.981 Main Idea: 1. Groups: Old numbering system: New IUPAC numbering system: 2. Periods: 3. Know the names and properties
Bonding-when atoms get it on. Ionic Compounds 9/22/2013. Chemical Formulas and Bonding
Bonding-when atoms get it on Chemical Formulas and Bonding There are two types of bonds that you need to know. The first kind of bond is Ionic bond. Ionic Bond = when a positive ion is attracted to a negatively
Description Mole Activity. Late Lab Stamp (this stamp means you are not qualified to do lab and test corrections)
Unit 5 Notepack: Chapters 10 Chemical Quantities NAME Unit 5 Chemical Names, and Formulas & Moles Unit Goals- As you work through this unit, you should be able to: 1. Distinguish between ionic and molecular
7.1 Describing Reactions. Burning is a chemical change. When a substance undergoes a chemical change, a chemical reaction is said to take place.
Burning is a chemical change. When a substance undergoes a chemical change, a chemical reaction is said to take place. Chemical Equations What is the law of conservation of mass? The law of conservation
Chem 101 Review. Fall 2012
Chem 101 Review Fall 2012 Elements, Atoms, Ions Elements in nature symbols Constant composition chemical formula Dalton s atomic theory Atomic structure what makes up the atom ions isotopes Periodic table
The Mole Concept. It is easily converted to grams, no of particles or in the case of gas volume.
The Mole Concept The mole is a convenient unit A mole is the number of atoms present in exactly 12 g of the isotope carbon-12. In 12 g of carbon-12 there are 6.022 x 10 23 carbon atoms It is easily converted
Atoms, Molecules and Ions
Atoms, Molecules and Ions Chapter 2 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Dalton s Atomic Theory (1808) 1. Elements are composed of extremely small
Chemistry Chapter 2. Atoms, Molecules, and Ions Section Periodic Table Ions Chemical Bonds Nomenclature
Chemistry Chapter 2 Atoms, Molecules, and Ions Section 2 2.6-2.8 Periodic Table Ions Chemical Bonds Nomenclature Organization of the Periodic Table Columns, Groups or Families elements in the same vertical
How to Use This Presentation
How to Use This Presentation To View the presentation as a slideshow with effects select View on the menu bar and click on Slide Show. To advance through the presentation, click the right-arrow key or
CHAPTER 2: ATOMS, MOLECULES AND IONS. -matter (element) is composed of indivisible and indestructible particles termed atoms
CHAPTER 2: ATOMS, MOLECULES AND IONS DALTON's ATOMIC THEORY -matter (element) is composed of indivisible and indestructible particles termed atoms -all atoms of the same element are identical. atoms of
CHAPTER 2. ATOMS, MOLECULES, AND IONS REMEMBER correct in a different color. Questions
CHAPTER 2 ATOMS, MOLECULES, AND IONS REMEMBER correct in a different color Questions 17. A compound will always contain the same numbers (and types) of atoms. A given amount of hydrogen will react only
Books at Amazon.com on Nanotechnology
Books at Amazon.com on Nanotechnology http://www.amazon.com/s/103-9040246- 0256655?ie=UTF8&keywords=NANOTECHNOLOGY%20&tag =thenanotecinscie&index=books&search=search&link%5fcode=qs Ions Ions are charged
ب 3 18 قسم الكيمياء مصطفي عيد
memxtd@yahoo.com m.moustapha@sau.edu.sa 0115888078 ب 3 18 قسم الكيمياء مصطفي عيد The Atom Nucleus Electron Shell or Orbit The Atom. What are the 3 major parts of an atom? Proton Neutron Electron Stoichiometry
Chapter 2. Law of Definite Proportions. Law of Definite Proportions. Law of Conservation of Mass 10/7/2011 WATER H 2 O
Chapter 2 Fundamental Chemical Laws (2.2) Dalton s Atomic Theory (2.3) Defining the Atom (2.5) Atomic Structure (2.6) Molecules and Ions (2.7) The Periodic Table (2.8) Nomenclature (2.9) Law of Conservation
Chemical Formulas and Chemical Compounds
CHAPTER 7 REVIEW Chemical Formulas and Chemical Compounds SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. c In a Stock system name such as iron(iii) sulfate, the Roman numeral
9/19/07. Chemistry 6A Fall 2007 Dr. J. A. Mack. Molar Masses. Avagagro s s Number. Avogadro s Number and the Mole
Chemistry 6A Fall 007 Dr. J. A. Mack Avogadro s Number and the Mole The concept of a mole is defined so that we may equate the amount of matter (mass) to the number of particles (mole). The Standard is
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Ch. 2 Practice Test Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which formula/name pair is incorrect? 1) A) Fe2(SO4)3 iron(iii) sulfide
CHAPTER 7: CHEMICAL FORMULAS AND CHEMICAL COMPOUNDS. Chemistry 1-2 Enriched Mr. Chumbley
CHAPTER 7: CHEMICAL FORMULAS AND CHEMICAL COMPOUNDS Chemistry 1-2 Enriched Mr. Chumbley SECTION 1: CHEMICAL NAMES AND FORMULAS While the bulk of the content will come from the Naming Chemical Compounds
» Composed of more than one type of atom chemically bonded.» A pure substance, meaning its properties are the same throughout the substance.
» Composed of more than one type of atom chemically bonded.» A pure substance, meaning its properties are the same throughout the substance.» Separated chemically not physically» No overall charge; they
IGCSE Double Award Extended Coordinated Science
IGCSE Double Award Extended Coordinated Science Chemistry 4.0 - Chemical Formulae and Equations - the chemical symbols for the first 20 elements - And the charges of the ions they form - And use them to
Atoms, Molecules and Ions
Atoms, Molecules and Ions Chapter 2 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Dalton s Atomic Theory (1808) 1. Elements are composed of extremely small
Chapter 2. Atoms, Molecules, and Ions. Copyright 2017 Cengage Learning. All Rights Reserved.
Chapter 2 Atoms, Molecules, and Ions Chapter 2 Table of Contents (2.1) (2.2) (2.3) (2.4) (2.5) (2.6) (2.7) (2.8) The early history of chemistry Fundamental chemical laws Dalton s atomic theory Early experiments
Chapter 2 Atoms, Ions, and the Periodic Table. Law of Conservation of Mass. Law of Conservation of Mass
Chapter 2 Atoms, Ions, and the Periodic Table Dalton s Atomic Theory Structure of the Atom Ions Atomic Mass The Periodic Table Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction
Section 1 Chemical Names and Formulas. Lesson Starter
Preview Lesson Starter Objectives Significance of a Chemical Formula Monatomic Ions Binary Ionic Compounds Writing the Formula of an Ionic Compound Naming Binary Ionic Compounds Naming Binary Molecular
Chapter 5 Molecules and Compounds
Chapter 5 Molecules and Compounds 1 Chemical Formulas Atomic/Molecular Elements Ionic/Molecular Compounds Naming Ionic Compounds Naming Molecular Compounds Naming Acids Formula Mass Atomic / Molecular
Chapter 2 Atoms and Elements
1 Chapter 2 Atoms and Elements Sec 2.3 Modern Atomic Theory and the Laws That Led to it Law of conservation of mass states that in a chemical reaction, matter is neither created nor destroyed. Law of definite
Memorize: Understand: Know how to:
NAME: CLASS PERIOD: REVIEW FOR HONORS CHEMISTRY SEMESTER 1 EXAM Memorize: Understand: Know how to: 1 SI units for different measurements (length, volume, number, mass, temperature, density) Definition
Atoms, Molecules and Ions. Chapter 2
Atoms, Molecules and Ions Chapter 2 2.1 The Atomic Theory of Matter Democritus [460-370 BCE] Described tiny, indivisible particles Called them atomos Differed from Aristotle 17th century - idea of atoms
EIT Review S2007 Dr. J.A. Mack.
EIT Review S2007 Dr. J.A. Mack www.csus.edu/indiv/m/mackj/ Part 1 Atom: The smallest divisible unit of an element Compound: A substance made of two or more atoms Ion: A charged atom or molecule Cation:
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) A molecule of water contains hydrogen and oxygen in a 1:8 ratio by mass. This is a statement
Ch. 6 Chemical Composition - Notetaker (Key)
6.1 Counting by Weighing Name: Group: Date: Ch. 6 Chemical Composition - Notetaker (Key) Chem 6 Objective: To understand the concept of average mass and explore how counting can be done by _ weighing Average
Nomenclature (Naming Compounds) and Chemical Formulas
Nomenclature (Naming Compounds) and Chemical Formulas 1 Ions formed from a single atom Monatomic Ions Charges are determined by whether ion has lost electrons (+) or gained electrons (-) Symbols are written
Naming and Formula Writing
+ Naming and Formula Writing + Chemical Formulas Shows the kind and number of atoms in the smallest piece of a substance Use subscripts to show the number of atoms per element Molecular formula- number
Chapter 5 Molecules and Compounds (Part 2)
Introductory Chemistry, 3 rd Edition Nivaldo Tro Molecules and Compounds (Part 2) Roy Kennedy Massachusetts Bay Community College Wellesley Hills, MA 2009, Prentice Hall 5.6 Nomenclature: Naming Compounds
Compounds and their formulas
Compounds and their formulas Molecular Compounds A molecular compound is a substance made up of discreet entities called molecules. A molecule consists of a small number of non-metal atoms held together
Unit 2. Chapter 4-Atoms and Elements, continued
CHEMISTRY 110 LECTURE Unit 2 Chapter 4-Atoms and Elements, continued I Ions II ISOTOPES-Tools A. Tools 1. Atomic number, Z,, equals the number of protons 2. Mass number, A, equals the sum of protons and
Atoms, Molecules and Ions
Atoms, Molecules and Ions Atomic Theory of Matter Modern Atomic Theory Relation to Periodic Table Isotopes & Mass Number Periodic Table Ionic Compounds Molecular Compounds Acid Compounds The Atomic Theory
Chapter 4 Chemical Formulas, Reactions, Redox and Solutions
Terms to Know: Solubility Solute Solvent Solution Chapter 4 the amount of substance that dissolves in a given volume of solvent at a given temperature. a substance dissolved in a liquid to form a solution
AP Chemistry Unit 1 Review Guide: IUPAC Naming, Stoichiometry, Solution Chemistry
I. IUPAC Naming AP Chemistry Unit 1 Review Guide: IUPAC Naming, Stoichiometry, Solution Chemistry For Ionic Compounds: Formula to Name: 1. Identify the cation (positive ion) by name, then identify the
NOMENCLATURE AND WRITING FORMULAS
NOMENCLATURE AND WRITING FORMULAS PART I--FORMULAS AND NOMENCLATURE OF IONIC COMPOUND Composed of Cations and Anions. Types of Cations (positive ions): A. Metals lose electrons to form positive ions. These
Matter What is Chemistry? Chemistry is the study of matter and the changes it undergoes.
Matter What is Chemistry? Chemistry is the study of matter and the changes it undergoes. What is matter? Matter is anything that has mass and occupies space. Chemists use a scientific method to study matter.
Chapter 2. Atoms, Molecules, and Ions
Chapter 2. Atoms, Molecules, and Ions 2.1 The Atomic Theory of Matter 400-5 BC. Greek philosopher Democritus proposes the idea of matter being made up of small, indivisible particles (atomos). 18th Century.
EIT Chemistry Review S01 Dr. Mack Chemistry is really Chem is try Download available at: www.csus.edu/indiv/m/mackj/ Or look for Jeffrey Mack under CSUS faculty web pages Part 1 To do chemistry, you must:
Period: Chemistry Semester 1 Final Exam Review Packet. 1. What is the difference between a hypothesis and a theory?
Chemistry Name: Period: Chemistry Semester 1 Final Exam Review Packet 1. What is the difference between a hypothesis and a theory? 2. Distinguish between quantitative and qualitative observations. States
ACP Chemistry (821) - Mid-Year Review
ACP Chemistry (821) - Mid-Year Review *Be sure you understand the concepts involved in each question. Do not simply memorize facts!* 1. What is chemistry? Chapter 1: Chemistry 2. What is the difference
10/1/2017. General Chemistry CHEM 101 (3+1+0) Dr. Mohamed El-Newehy. Chapter 2. Chemistry: Atoms, Molecules and Ions
General Chemistry CHEM 101 (3+1+0) Dr. Mohamed El-Newehy http://fac.ksu.edu.sa/melnewehy Chapter 2 Chemistry: Atoms, Molecules and Ions 1 The Structure of the Atom Dalton s Atomic Theory (1808) o Compounds
Unit 4 Conservation of Mass and Stoichiometry
Unit 4 Conservation of Mass and Stoichiometry 7-1 Chemical Names and Formulas I. Significance of a Chemical Formula A. Molecular formulas 1. Number of atoms of each element in one molecule of a compound
Molecules and Compounds
Molecules and Compounds ed. Brad Collins Some images Copyright The McGraw-Hill Companies, Inc. A molecule is an aggregate of two or more atoms in a definite arrangement held together by chemical bonds
2007 Release Chemistry SOL Test
Name: Score: 50 / 50 points (100%) 2007 Release Chemistry SOL Test Multiple Choice Identify the choice that best completes the statement or answers the question. B 1. What is the volume of the liquid in
Atomic Theory of Matter
Chapter 2: Atoms, Molecules, and Ions Learning outcomes: Learn the basic postulates of Dalton s atomic theory. Describe the key experiments that led to the discovery of electrons and the nuclear model
10. In what way are isotopes of a given element always different? In what way(s) are they always the same?
Chem 180- Spring 2019 HW Ch 2 Name: Note: I used the problem numbers from the book, so they don t start at 1. Stay within the space provided, so keep your answers and explanations brief. (I have learned
3. Most laboratory experiments are performed at room temperature at 65 C. Express this temperature in: a. F b. Kelvin
Do all work on a separate sheet of paper so that you can show your work. Section A: Measurement and Math 1. Convert the following and show your work: a. 200 meters = miles. b. 650 in = meters c. 4 years=
Chemistry 101 Chapter 8 Chemical Composition
Chemistry 101 Chapter 8 Chemical Composition Atomic mass unit (amu): a unit of the scale relative masses of atoms (1 amu = 1.66 10-24 g). Atomic weight (Atomic mass): the atomic weight of an element given
2.1 Atomic Theory of Matter
Chapter 2 2.1 Atomic Theory of Matter The theory that atoms are the fundamental building blocks of matter re-emerged in the early nineteenth century, championed by John Dalton. Law of Conservation of Mass
Chemical Stability and Naming and Writing
Chemical Stability and Naming and Writing Section 4.2 Atoms Collide In order for substances to, particles of the substances must. Reactions between atoms involve only their. Section 4.2 Chemical Stability
Chapter 2 Atoms, Molecules, and Ions
hapter 2 Atoms, Molecules, and Ions 2.1 The Atomic Theory of Matter Is there such thing like a indivisible particle of matter (atom)? Based on the following observations: 1. Law of conservation of mass/matter
Nomenclature of inorganic compounds. = naming non carbon (mostly) compounds. Some definitions:
1 Chemistry 047 Inorganic Nomenclature Nomenclature of inorganic compounds = naming non carbon (mostly) compounds Some definitions: Nomenclature = system used by chemists to name and identify compounds
Unit Five- Chemical Quantities Chapter 9: Mole ratios, conversions between chemicals in a balanced reaction (mole, mass), limiting reactant, % yield
Chemistry Midterm Review Exam date: Wednesday, 2/15 during class The midterm exam must be completed before February vacation if you are absent The midterm exam is worth 6% of your year grade and it contains
Atoms, Molecules, and Ions
Atoms, Molecules, and Ions Atomic Theory of Matter Postulates of Dalton s Atomic Theory All matter is composed of indivisible atoms. An atom is an extremely small particle of matter that retains its identity
CHAPTER 2 ATOMS, MOLECULES, AND IONS
CHAPTER ATOMS, MOLECULES, AND IONS This chapter is a review of first year chemistry concepts and terminology used to describe atoms and molecules, atomic theory, the periodic table, and the naming of compounds.
La Salle College High School AP Chemistry Summer Homework Assignment
La Salle College High School AP Chemistry Summer Homework Assignment DUE on first day of class! Email me with questions as a last resort: stottm@lschs.org Name: 1. Metric Conversions. Remember 1 cm = 1
CHAPTER 2: ATOMS, IONS, AND MOLECULES
CHAPTER 2: ATOMS, IONS, AND MOLECULES Problems: 2.1-2.78, 2.81-2.93, 2.94-2.96, 2.111-2.119, 2.121, 2.127 2.1 THE NUCLEAR MODEL OF ATOMIC STRUCTURE Joseph John (J. J.) Thomson (1897) carried out experiments
Lecture 11 - Stoichiometry. Lecture 11 - Introduction. Lecture 11 - The Mole. Lecture 11 - The Mole. Lecture 11 - The Mole
Chem 103, Section F0F Unit IV - Stoichiometry of Formulas and Equations Lecture 11 The concept of a mole, which is a very large group of atoms or molecules Determining the formulas for a compound Stoichiometry
AP Chemistry Chapter 2
AP Chemistry Chapter 2 Atoms, Molecules & Ions The Atomic Theory of Maer > Democritus (460 370 BC) > Greek philosopher > Thought that material was made up of ny indivisible parcles called atomos > Aristotle
Ionic Compounds. And Acids
CHAPTER 7 LANGUAGE OF CHEMISTRY CLASSIFICATION OF COMPOUNDS Inorganic compounds does not contain the element carbon, but there are exception to this rule, CO 2 (carbon dioxide), CO 3 2 (carbonate), and
Chapter Two: Early History of Chemistry. Three Important Laws. Dalton s Atomic Theory (1808) Three Important Laws (continued) Greek Explanation
Greek Explanation Chapter Two: ATOMS, MOLECULES, AND IONS Notes 2.1 In the Greek model they theorized there were four elements earth, water, air, and fire. These elements were characterized by the following
Formulas and Models 1
Formulas and Models 1 A molecular formula shows the exact number of atoms of each element in the smallest unit of a substance An empirical formula shows the simplest whole-number ratio of the atoms in
Unit 2 Chapters 5 and 6 Atoms/Periodic Table/ NOMENCLATURE NAMING AND FORMING COMPOUNDS
Unit 2 Chapters 5 and 6 Atoms/Periodic Table/ NOMENCLATURE NAMING AND FORMING COMPOUNDS Review of Atomic Structure What is an atom? The smallest particle of an element that retains the properties of that
1.3 Atoms, Molecules, and Ions. Fundamental laws
1.3 Atoms, Molecules, and Ions Fundamental laws Conservation of mass Definite proportion Multiple proportions 1. You have a chemical in a sealed glass container filled with air. The setup is sitting on
Unit 7. Bonds and Naming
Unit 7 Bonds and Naming I. Ionic Bonds Positive ion is attracted to a negative ion; usually a metal & a nonmetal Ionic compound: a substance that has ionic bonds Cation: positive ion Anion: negative ion
Chemical Nomenclature
Name Period Date Chemical Nomenclature Fill-in the blanks during the PowerPoint presentation in class. Common Names A lot of chemicals have common names as well as the proper (International Union of Pure
AP CHEMISTRY READING GUIDE
Name: Due Date: AP CHEMISTRY READING GUIDE Chapters 1-3, Chemical Foundations & Stoichiometry Chapter 1 Chemical Foundations Define the following terms in your own words: Scanning Tunneling Microscope
IUPAC BOHR DIAGRAMS FOR ATOMS TYPES OF CHEMICAL BONDS MOLECULAR COMPOUNDS TYPES
IUPAC BOHR DIAGRAMS FOR ATOMS TYPES OF CHEMICAL BONDS MOLECULAR COMPOUNDS TYPES SIMPLE COVALENT COMMON NAME IONIC COMPOUNDS SIMPLE IONIC MULTIVALENT POLYATOMIC/COMPLEX HYDRATED IONIC ACIDS International
Chapter 2 Atoms, Molecules and Ions
Chapter 2 Atoms, Molecules and Ions Atomos uncuttable Dalton s Atomic Theory ~1805 (page 38) Atoms are small, indivisible balls. Mid-1800s: scientists find that atoms consist of: charge Protons +1 Neutrons
Atoms, Molecules, and Ions. Chapter 2 AP Chemistry
Atoms, Molecules, and Ions Chapter 2 AP Chemistry Building blocks of chemistry. Atom Molecule Ion Dalton s Atomic Theory 1. An element is composed of tiny particles called atoms. 2. In an ordinary chemical
Atoms, Molecules, and Ions
Atoms, Molecules, and Ions Chapter 2 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Dalton s Atomic Theory (1808) 1. Elements are composed of extremely small
CHEMISTRY - MCMURRY 7E CH.2 - ATOMS, MOLECULES AND IONS.
!! www.clutchprep.com CONCEPT: GROUP NAMES AND CLASSIFICATIONS Ever wonder where did this periodic table ever come from? At the end of the 18 th century, Lavoisier compiled a list of the 23 elements known
CHEMISTRY - TRO 4E CH.2 - ATOMS & ELEMENTS.
!! www.clutchprep.com CONCEPT: GROUP NAMES AND CLASSIFICATIONS Ever wonder where did this periodic table ever come from? At the end of the 18 th century, Lavoisier compiled a list of the 23 elements known
Chapter 2. Chapter 2
Chapter 2 Atoms, Molecules, and Ions Chapter 2 Atomic Theory Model for atom and ions that works well for chemistry Molecules Combinations of atoms Ways of representing molecules: formulas and models Names