Unit 2. Chemical Foundations: Elements, Atoms, and Ions
|
|
- Clemence Smith
- 5 years ago
- Views:
Transcription
1 Unit 2 Chemical Foundations: Elements, Atoms, and Ions
2 Memorize the list of elements You will have a quiz on this list. All of the elements will be on the quiz!
3 Elements in the Earth System (% mass in Crust, Ocean, & Atmosphere) Oxygen 49.5 % Silicon 25.7 % Aluminum 7.50 % Iron 4.71 % Calcium 3.39 % Sodium 2.63 % Potassium 2.40 % Magnesium 1.93 % Hydrogen 0.87 %
4 Your body is worth less than $1.00 Elements in the Human Body Oxygen 65.0 % Carbon 18.0 % Hydrogen 10.0 % Nitrogen 3.0 % Calcium 1.4 % Phosphorus 1.9 % Magnesium 0.50 % Potassium 0.34 % Sulfur 0.26 % Sodium 0.14%
5 An element is a pure substance containing only one kind of atom. An atom being the smallest unit of an element. A compound is a pure substance containing 2 or more kinds of atoms combined in definite proportions. A molecule is the smallest unit of a compound. Chemical symbol is one or two letters used to represent an element. The first letter is capitalized, the 2 nd (if one) is lower case. A subscript is a number telling how many of the atom before the number required. If there is no number, there is one atom.
6 Some elements take their names from Latin so their symbols don t seem to make sense.
7 Rules for Writing Formulas 1. Use element symbols 2. The number of each type of atom is indicated by a subscript (small number) written to the right of the element symbol 3. If only one of an atom type, the subscript 1 is not written
8 Chemical formulas Subscript H 2 O 1 molecule 2 hydrogen 1 oxygen Ag 2 CrO 4 1 molecule 2 silver 1 chromium 4 oxygen formula Na 2 CO 3 1 molecule 2 sodium 1 carbon 3 oxygen
9 Formulas using ( ) ( ) x means that anything inside ( ) needs to be taken x number of times. (NH 4 ) 2 CO 3 (1x2) = 2 N, (4x2) = 8 H, 1 C, 3 O Al 2 (SO 4 ) 3
10 Diatomic molecules There are 7 elements that do not exist as 1 atom alone. As an element, they are always as 2 atoms bonded together as a molecule. Location of the diatomic elements
11 Nuclear Notation Atomic mass = p + + n Atomic number = p + A X z Element symbol e - = p + when the atom is neutral (we will be working with only neutral atoms to begin with) n = Atomic mass Atomic number
12 Discovery of the Atom 1803 John Dalton discovered that elements are made of atoms. He thought that atoms were solid, like a marble Crooks discovered the electron. The electron was found to have a mass of 9.1 x g and have a negative (-) charge.
13
14 1907 J.J.Thomson finds the positive particle, the proton. Protons have a much larger mass of 1.67 x g and a positive (+) charge. His model of the atom was called the plum pudding model, the p + and e were spread throughout the mass of the atom.
15 1911 Rutherford shoots a stream of helium nuclei at gold foil. He discovers that they bounce back after hitting a positive nucleus composed of p + in the center of the atom.
16 Rutherford stated that the p + are found in the nucleus in the center of the atom. e - revolve around the nucleus.
17 1932 Chadwick discovers the neutral particle, the neutron. The neutron is found in the nucleus along with the p +. The e - revolve around the nucleus. Protons and Neutrons located in the nucleus
18 Subatomic Particles Particle Mass Charge Location in the atom Proton (p + ) 1 amu +1 Nucleus (center of atom) Neutron (n) 1 amu 0 Nucleus (center of atom) Electron (e - ) 1 / 1837 amu -1 Revolving around nucleus
19 Atomic mass is the average number of p + plus n found in the nucleus. Elements with the atomic mass in ( ) means that very little of it exists at any given time. Scientists have not been able to attain an good average atomic mass. Carbon C Chemical symbol: 1 or 2 letters used to represent an element. The 1 st letter is always capital. If there is a 2 nd letter, it is lower case. 6 Atomic number is the number of p + found in the nucleus.
20 Atomic mass is the average number of p + and n found in the nucleus. 6 Carbon C All elements have Isotopes. Atoms of the same element with a different number of neutrons found in the nucleus, therefore they have different masses. Chemical symbol: 1 or 2 letters used to represent an element. The 1 st letter is always capital. If there is a 2 nd letter, it is lower case. Atomic number is the number of p + found in the nucleus.
21 Nuclear Notation Atomic mass = p + + n Atomic number = p + A X z Element symbol e - = p + when the atom is neutral (we will be working with only neutral atoms to begin with) n = Atomic mass Atomic number
22 Light Brite Isotopes Protons Electrons Neutron Protons Electrons Neutron 1H 2H 3H
23 Dalton s Atomic Theory 1. Each element is composed of extremely small particles called atoms. 2. All atoms of a given element are identical, but the atoms of one element are different from the atoms of all other elements. 3. Atoms of one element cannot be changed into atoms of a different element by chemical reactions; atoms are neither created nor destroyed in chemical reactions. 4. Compounds are formed when atoms of more than one element combine; a given compound always has the same relative number and kind of atoms.
24 1829 Johann Dobereiner organized some elements into groups of three called triads. This was the first attempt at a periodic table. Example of triad: Cl, Br, I Other triads were: Li, Na, K Ca, Sr, Ba S, Se, Te
25 1869 Dmitri Mendeleev organized the elements according to their atomic mass. The vertical columns were families (or groups).
26 Early 1900 s Henry Mosley organized the elements according to their atomic number (number of protons). This is the modern periodic table that we use.
27 Periodicity : regular, repeating properties; the elements when arranged in the order of their atomic numbers show a periodic variation in most of their properties. Periods are the rows across the table. There are 7 periods. These also correspond to the energy levels that e - are found in. There is a variation in the properties of elements as you move from left to right, which repeats in the next period. Families (or groups) are the columns going down the table. Elements in a family show very similar properties. Go back to the last slide and check out the numbering of the periods and families.
28 Classification of elements as metals, nonmetals, and matalloids.
29 Metals : All elements to the left of the red line (metalloids) 1. conduct electricity 2. conduct heat 3. shiny silvery solids (except Au, Cu, Hg) 4. malleable and ductile Nonmetals: All elements to the right of the red line (metalloids) 1. do not conduct electricity 2. do not conduct heat 3. not shiny silvery solids 4. not malleable or ductile Metalloids: All elements with a full side bordering the red line B, Si, Ge, As, Sb, Re, Po These elements have some of the characteristics of metals and some characteristics of nonmetals.
30 Alkali metals Add all of this information to your periodic table Charge on ions +1 Family name 1 e - e - in outer energy level
31 Alkali metals Alkali Earth metals Halogens Noble gases Ionic charges atoms take on Transition metals 3 e - 4 e - 5 e - 6 e - 7 e - 8 e - 1 e - 2 e - Rare Earth elements Lanthanide series Actinide series # of e - in outer energy level
32 Alkali Metals : Li, Na, K, Rb, Cs, Fr 1. Alkali metals are all very reactive and cannot be used by themselves. 2. All Alkali metals react with water. (M = alkali metal) 2 M (s) + 2 H 2 O (L) 2 M +1 (aq) + 2 OH -1 (aq) + H 2(g) + Energy 2 Na (s) + 2 H 2 O (L) 2 Na +1 (aq) + 2 OH -1 (aq) + H 2(g) + Energy Alkali Earth Metals: Be, Mg, Ca, Sr, Ba, Ra 1. Alkali Earth Metals are quite reactive. 2. These elements have many uses. Mg combines with other metals to make light weight alloys. Ca compounds include chalk and marble. Sr and Ba are used in fireworks.
33 Halogens: F, Cl, Br, I, At 1. These elements have many uses. Cl is used to kill bacteria. F is used to prevent tooth decay. I is used in medicine (thyroid hormone thyroxine). Br is used to improve gasoline performance. 2. The halogens all react with alkali metals. 2 M (s) + X 2 2 MX (s) + energy M = alkali metal 2 K (s) + Cl 2 (g) 2 KCl (s) + energy X 2 = halogen Noble Gases: He, Ne, Ar, Kr, Xe, Rn 1. Noble gases do not chemically react. 2. Generally don t make ions.
34 Transition Metals: Element and below 1. Many useful applications 2. Most can have more than one type of ionic charge. Example: Fe +2 and Fe +3 Rare Earth Elements: Lanthanide & Actinide Series 1. Silvery white or gray solids 2. Have common properties so they are hard to separate from each other. 3. Up to element 92 are naturally occurring together with other elements in rocks. Beyond element 92 are man made. 4. Usually have +3 ions
35 Ions a. Positive and negative charges exist b. Unlike charges attract each other. c. Like charges repel each other. d. Atoms in nature are neutral even though they are made of particles which have an electrical charge. e. Positive particles are called protons (p + ) which are in the nucleus. f. Negatively charged particles are called electrons (e - ) which revolve around the nucleus. e - determine chemical reactions and bonding. g. Electrons can be added or taken away from a neutral atom to form electrically charged particles called ions. Groups of atoms can form complex ions (polyatomic ions) *Ions exist in solution. They form when solids dissolve in water (NOT all solutions have ions.).
36 Common Ions Chart Top half is positive ions Positive ions made of 1 atom keep the atom name. Bottom half is negative ions Negative ions made of 1 atom drop their ending and add ide.
37 Ionization energy is the amount of energy required to remove one electron from a neutral atom. M (g) + Ionization energy M +1 (g) + 1 e -1
38 Ionization Energy 1 Hydrogen 1,312.1 Kj / mol 2 Helium 2, Lithium Beryllium Boron Carbon 1, Nitrogen 1, Oxygen 1, Fluorine 1, Neon 2, Sodium Kj / mol 12 Magnesium Aluminum Silicon Phosphorus 1, Sulfur Chlorine 1, Argon 1, Potassium Calcium 589.9
39 Types of Bonding Covalent Bonding: between Non-metals Sharing of e - in such a way as to complete the outer energy level (valence orbitals) of both (all) atoms. All atoms end up with the e - configuration of Noble gases. Ionic Bonding between a metal & non-metal Transfer of e - resulting in a positive ion and a negative ion that are attracted to each other. Metal outer energy level (valence orbitals) are emptied Non metal outer energy level (valence orbitals) fill to have the configuration of the next Noble gas. [ ]
40 An Electrolyte is a material that dissolved in water producing ions, to make a solution that conducts an electric current. A salt is a (+) ion and a (-) ion joined to make a compound. Therefore this includes: All salts that dissolve in water Chemicals that produce ions This does not include: Organic chemicals (covalently bonded) All chemicals that do NOT dissolve in water
41 Ion Demonstration Chemical Formula 10W 60W 110W Sodium chloride.01m Sodium chloride.1 M Sodium chloride 1 M Ammonium chloride Ethyl alcohol Calcium chloride Distilled water
42 Ion Demonstration Chemical Formula 10W 60W 110W Ammonium carbonate Silver nitrate Tap water Sugar water Copper chloride Sodium bicarbonate Sodium sulfate
43 Cl + 1e - Cl -1 Na Na e - atom electron ion atom ion electron 17 e e - 18 e - 11 e - 10 e e - 17 p + 17 p + 11 p + 11 p + Anion = negative ion Cation = positive ion
44 Common Ions
45 Lite Brite Atoms Protons Protons Electrons Electrons H H e
46 Crystals 1. All solids form geometric figures in which the atoms and molecules are arranged in a regular repeating pattern. 2. Solid geometric figures are called crystals. Crystals have plane surfaces that are at definite angles to one another. 3. There are 6 crystal structures.
47 1. Cubic 4. Tetragonal 2. Monoclinic 5. Orthorhombic 3. Triclinic 6. Hexagonal
48 Crystal shape lab : The following is the true chemical formula that the wooden models represents. 1. Cr 2 K 2 (SO 4 ) 4. 24H 2 O 2. PbS 3. FeS 2 4. ZrSiO 4 5. Ca 6 Al 3 OH or F(SiO 4 ) 5 6. SiO 2 7. CaCO 3 8. S 9. BaSO CaSO 4. 2H 2 O 11. Ni(NH 4 ) 2 (SO 4 ) 2. 6 H 2 O 12. CuSO 4. 5H 2 O
49
Modern Atomic Theory
Modern Atomic Theory Review of the Discovery of the Atom 1803 John Dalton discovered that elements are made of atoms. He thought that atoms were solid, like a marble. 1875 Crooks discovered the electron.
More informationOrganizing the Periodic Table
Organizing the Periodic Table How did chemists begin to organize the known elements? Chemists used the properties of the elements to sort them into groups. The Organizers JW Dobereiner grouped the elements
More informationPeriodic Table Workbook
Key Ideas: The placement or location of elements on the Periodic Table gives an indication of physical and chemical properties of that element. The elements on the Periodic Table are arranged in order
More informationChapter 4 Atoms Practice Problems
Chapter 4 Atoms Practice Problems 1) The primary substances of which all other things are composed are A) molecules. B) compounds. C) elements. D) electrons. E) protons. 2) Which of the following is a
More information-discovered set of patterns that applied to all elements published 1st periodic table. -wrote properties of each on note cards (density, color)
Dmitri Mendeleev -discovered set of patterns that applied to all elements -1869 published 1st periodic table -total of 63 elements discovered -wrote properties of each on note cards (density, color) -noticed
More informationSearching for an Organizing Principle. Searching for an Organizing Principle. How did chemists begin to organize the known elements?
Searching for an Organizing Principle Searching for an Organizing Principle How did chemists begin to organize the known elements? Searching for an Organizing Principle A few elements, including copper,
More informationPrinciples of Chemistry: A Molecular Approach, 3e (Tro) Chapter 2 Atoms and Elements
Principles of Chemistry: A Molecular Approach, 3e (Tro) Chapter 2 Atoms and Elements 1) Which of the following is an example of the law of multiple proportions? A) A sample of chlorine is found to contain
More informationPrinciples of Chemistry: A Molecular Approach 2e (Tro) Chapter 2 Atoms and Elements
Principles of Chemistry: A Molecular Approach 2e (Tro) Chapter 2 Atoms and Elements 1) Which of the following is an example of the law of multiple proportions? A) A sample of chlorine is found to contain
More informationTest Review # 5. Chemistry: Form TR5-8A. Average Atomic Mass. Subatomic particles.
Chemistry: Form TR5-8A REVIEW Name Date Period Test Review # 5 Subatomic particles. Type of Particle Location Mass Relative Mass Charge Proton Center 1.67 10-27 kg 1 +1 Electron Outside 9.11 10-31 kg 0-1
More informationChapter 9: Elements are the Building blocks of Life
Chapter 9: Elements are the Building blocks of Life Section 9.1- Elements and the Periodic Table Keep Scale in mind Animation: http://htwins.net/scale2/ I. ELEMENTS All matter is made up of one or more
More informationCHAPTER 2. Structure of the Atom. Atoms and Elements
CHAPTER 2 Atoms and Elements 1 Atoms Dalton s Atomic Theory - 1808 1. -Element is composed of small, indivisible particles called atoms. 2. -Atoms of an element have identical properties that differ from
More information3.1 Classification of Matter. Copyright 2009 by Pearson Education, Inc.
Chapter 3 Atoms and Elements 3.1 Classification of Matter Copyright 2009 by Pearson Education, Inc. 1 Matter Matter is the stuff that makes up all things. Copyright 2009 by Pearson Education, Inc. 2 Pure
More informationUnit 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,
More informationDevelopment of the Periodic Table
Development of the Periodic Table John Newlands - Law of Octaves 1864 When arranged in order of atomic mass, every eighth element had similar properties. Dimitri Mendeleev / Lothar Meyer 1869 organized
More informationTest Review # 4. Chemistry: Form TR4-9A
Chemistry: Form TR4-9A REVIEW Name Date Period Test Review # 4 Location of electrons. Electrons are in regions of the atom known as orbitals, which are found in subdivisions of the principal energy levels
More informationChemistry: A Molecular Approach, 2e (Tro) Chapter 2 Atoms and Elements. Multiple Choice Questions
Chemistry: A Molecular Approach, 2e (Tro) Chapter 2 Atoms and Elements Multiple Choice Questions 1) In a chemical reaction, matter is neither created or destroyed. Which law does this refer to? A) Law
More informationUnit 7 Study Guide: Name: KEY Atomic Concepts & Periodic Table
Unit 7 Study Guide: Name: KEY Atomic Concepts & Periodic Table Focus Questions for the unit... How has the modern view of the atom changed over time? How does a chemist use symbols and notation to communicate
More informationPeriodic Table of Elements
Periodic Table of Elements chlorine nitrogen helium gold oxygen silver mercury hydrogen neodymium sodium niobium carbon Elements Science has come along way since Aristotle s theory of Air, Water, Fire,
More information4.1 Atomic structure and the periodic table. GCSE Chemistry
4.1 Atomic structure and the periodic table GCSE Chemistry All substances are made of atoms this is cannot be chemically broken down it is the smallest part of an element. Elements are made of only one
More informationUnit Two Test Review. Click to get a new slide. Choose your answer, then click to see if you were correct.
Unit Two Test Review Click to get a new slide. Choose your answer, then click to see if you were correct. According to the law of definite proportions, any two samples of water, H2O, A. will be made up
More informationChapter 6: The Periodic Table
Chapter 6: The Periodic Table Name: Per: Test date: In-Class Quiz: Moodle Quiz: preap Learning Objectives Trace the historical development of the periodic table Identify the major groups and key features
More informationChemistry Study Guide
Chemistry Study Guide Marking Period 3 Exam Week of 3/21/17 Study Guide due - When studying for this test, use your do nows, notes, homework, class handouts, and your textbook. Vocabulary Chapter 7 Anion
More informationCh. 3 Answer Key. O can be broken down to form two atoms of H and 1 atom of O. Hydrogen and oxygen are elements.
Ch. 3 Answer Key 1. The Greeks believed that all matter is made of elements. We currently believe the same thing. However, the Greeks believed that there were 4 elements: earth, water, air and fire. Instead,
More information1 Arranging the Elements
CHAPTER 12 1 Arranging the Elements SECTION The Periodic Table BEFORE YOU READ After you read this section, you should be able to answer these questions: How are elements arranged on the periodic table?
More informationChapter 6 The Periodic Table
Chapter 6 The Periodic Table Section 6.1 Organizing the Elements OBJECTIVES: Explain how elements are organized in a periodic table. Section 6.1 Organizing the Elements OBJECTIVES: Compare early and modern
More informationTest Review # 4. Chemistry: Form TR4-5A 6 S S S
Chemistry: Form TR4-5A REVIEW Name Date Period Test Review # 4 Development of the Periodic Table. Dmitri Mendeleev (1869) prepared a card for each of the known elements listing the symbol, the atomic mass,
More informationChemistry Notes: The Periodic Table
Warm-Up 1. What is the periodic table? 2. Who invented it? 3. How does the periodic table organize the elements? 4. Why did Mendeleev leave empty spaces when he constructed his periodic table? Chemistry
More informationHSVD Ms. Chang Page 1
Name: Chemistry, PERIODIC TABLE 1. A solid element that is malleable, a good conductor of electricity, and reacts with oxygen is classified as a (1) noble gas (2) metalloid (3) metal (4) nonmetal 2. Which
More informationCHAPTER 8 Ionic and Metallic Bonds
CHAPTER 8 Ionic and Metallic Bonds Shows the kind of atoms and number of atoms in a compound. MgCl 2 NaCl CaCO 3 Al 2 O 3 Ca 3 (PO 4 ) 2 Chemical Formulas Al: Cl: counting atoms AlCl 3 Pb: N: O: Pb(NO
More informationUNIT (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
More informationAtomic Structure and the Periodic Table. AQA Chemistry topic 1
Atomic Structure and the Periodic Table AQA Chemistry topic 1 1.1 Atoms, elements and compounds The structure of the atom Everything in the universe is basically made up of atoms. An atom is the smallest
More information1. The arrangement of the elements from left to right in Period 4 on the Periodic Table is based on
1. The arrangement of the elements from left to right in Period 4 on the Periodic Table is based on A) atomic mass B) atomic number C) the number of electron shells D) the number of oxidation states 2.
More informationPrinciples of Chemistry: A Molecular Approach (Tro) Chapter 2 Atoms and Elements
Principles of Chemistry: A Molecular Approach (Tro) Chapter 2 Atoms and Elements 1) Which of the following is an example of the law of multiple proportions? A) A sample of chlorine is found to contain
More informationEvery element has its own unique symbol.
The Periodic Table Every element has its own unique symbol. For some elements the symbol is simply the first letter of the element s name. Examples: Hydrogen = H, Sulfur = S, Carbon = C Symbols for other
More informationChemistry B11 Chapter 3 Atoms
Chapter 3 Atoms Element: is a substance that consists of identical atoms (hydrogen, oxygen, and Iron). 116 elements are known (88 occur in nature and chemist have made the others in the lab). Compound:
More informationPage 1 of 9. Website: Mobile:
Question 1: Did Dobereiner s triads also exist in the columns of Newlands Octaves? Compare and find out. Only one triad of Dobereiner s triads exists in the columns of Newlands octaves. The triad formed
More informationCHAPTER 3. Chemical Foundations
CHAPTER 3 Chemical Foundations 3.1 THE ELEMENTS 118 elements in 92 occur naturally, the rest are synthesized All matter in the universe can be chemically broken down into elements Compounds are made by
More informationChapter 4 Atoms and Elements
Atoms and Elements Experiencing Atoms Atoms are incredibly small, yet they compose everything. Atoms are the pieces of elements. Properties of the atoms determine the properties of the elements. 2 The
More informationAtoms and Ions Junior Science
2018 Version Atoms and Ions Junior Science 1 http://msutoday.msu.edu Introduction Chemistry is the study of matter and energy and the interaction between them. The elements are the building blocks of all
More informationTest Topics: Periodic Table, Atomic Theory, Physical/Chemical Properties, Atom, Isotopes, Average Atomic Mass
Elemental Properties Review Worksheet Test Topics: Periodic Table, Atomic Theory, Physical/Chemical Properties, Atom, Isotopes, Average Atomic Mass Periodic Table 1. List the element symbols for the following
More informationElectronic Structure of Atoms and the Periodic table. Electron Spin Quantum # m s
Electronic Structure of Atoms and the Periodic table Chapter 6 & 7, Part 3 October 26 th, 2004 Homework session Wednesday 3:00 5:00 Electron Spin Quantum # m s Each electron is assigned a spinning motion
More informationMendeleev s Table (1871) While it was the first periodic table, Mendeleev had very different elements, such as the very reactive potassium and the
Periodic Table Mendeleev s Table (1871) While it was the first periodic table, Mendeleev had very different elements, such as the very reactive potassium and the very stable copper, in the same family.
More informationRegents review Atomic & periodic
2011-2012 1. The diagram below represents the nucleus of an atom. What are the atomic number and mass number of this atom? A) The atomic number is 9 and the mass number is 19. B) The atomic number is 9
More informationExam Accelerated Chemistry Study Sheet Chap 04 The Atom/Periodic Table
Exam Accelerated Chemistry Study Sheet Chap 04 The Atom/Periodic Table Name /87 TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. Correct the False statements by changing
More informationChapter 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
More informationPeriods: horizontal rows (# 1-7) 2. Periodicity the of the elements in the same group is explained by the arrangement of the around the nucleus.
The Modern Periodic Table 1. An arrangement of the elements in order of their numbers so that elements with properties fall in the same column (or group). Groups: vertical columns (#1-18) Periods: horizontal
More informationElements are the building blocks of matter. Chapter 2
Elements are the building blocks of matter. Chapter 2 S In this chapter we will be covering S ELEMENTS!!! S The Periodic Table and Chemical Properties!!! S The Periodic Table and Atomic Theory! What is
More informationElectronic Structure and Bonding Review
Name: Band: Date: Electronic Structure and Bonding Review 1. For electrons: a. What is the relative charge? b. What is the relative mass? c. What is the symbol? d. Where are they located in the modern
More informationReview Package #3 Atomic Models and Subatomic Particles The Periodic Table Chemical Bonding
Chemistry 11 Review Package #3 Atomic Models and Subatomic Particles The Periodic Table Chemical Bonding 1. Atomic Models and Subatomic Particles: A. Subatomic Particles and Average Atomic Mass: - Subatomic
More informationThe Periodic Law Notes (Chapter 5)
The Periodic Law Notes (Chapter 5) I. History of the Periodic Table About 70 elements were known by 1850 (no noble gases) but there didn t appear to be a good way of arranging or relating them to study.
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
CHM 210 Chemistry Homework #2 Atoms and Elements (Ch. 3) Due: MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Helium is a(n) A) heterogeneous mixture.
More informationChapter 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
More informationDevelopment of the Modern Periodic Table
2017/2018 Development of the Modern Periodic Table Mohamed Ahmed Abdelbari Introduction Atom: the smallest, indivisible unit of an element that retains all chemical and physical properties of the element.
More informationPhysical Science Study Guide
Name: Class: Date: Physical Science Study Guide Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Mendeleev arranged the known chemical elements in a table
More informationChemistry CRT Study Guide First Quarter
Number AL COS # 1. #1.0 Classify sodium chloride as an element, mixture, compound, or colloid. Compound 2. #1.0 Classify air as an element, mixture, compound, or colloid. Mixture 3. #1.0 Classify a blueberry
More information2/15/2013. Chapter 6 6.1
Chapter 6 In a self-service store, the products are grouped according to similar characteristics. With a logical classification system, finding and comparing products is easy. You will learn how elements
More informationChemistry. The building blocks of matter Made of protons, neutrons and electrons. Pure substances that cannot be separated.
Chemistry CHEMISTRY NOTES Atom- Element- Compound- Molecule- The building blocks of matter Made of protons, neutrons and electrons. Pure substances that cannot be separated. Ex: Gold 2 or more elements
More informationChapter 2 Atoms and the Periodic Table
Chapter 2 1 Chapter 2 Atoms and the Periodic Table Solutions to In-Chapter Problems 2.1 Each element is identified by a one- or two-letter symbol. Use the periodic table to find the symbol for each element.
More informationUnit 3. Atoms and molecules
Unit 3. Atoms and molecules Index. s and compounds...2.. Dalton's Atomic theory...2 2.-The atom...2 3.-Atomic number and mass number...2 4.-Isotopes, atomic mass unit and atomic mass...3 5.- configuration...3
More informationThe Periodic Table of the Elements
The Periodic Table of the Elements All matter is composed of elements. All of the elements are composed of atoms. An atom is the smallest part of an element which still retains the properties of that element.
More informationChapter 2: Atoms and the Periodic Table
1. Which element is a nonmetal? A) K B) Co C) Br D) Al Ans: C Difficulty: Easy 2. Which element is a metal? A) Li B) Si C) Cl D) Ar E) More than one of the elements above are metals. 3. Which element is
More informationChapter 3: Atomic Theory
Chapter 3: Atomic Theory and Elements, Atoms, Compounds & Ions A. The Elements All of the materials in the universe can be chemically broken down into about 100 different elements. 1. Element can have
More informationLaw 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**
More informationChapter 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
More information2. Read pages a. Answer the five Reading Check questions on page 47
Chemistry Test #1 Review Chapters 1 & 2 1. Page 37, #4-6, 8, 9, 13, 14 2. Read pages 45 47 a. Answer the five Reading Check questions on page 47 3. Read pages 52 57 a. Copy the table on page 55 b. Define
More informationChapter 2. Atoms, Ions, and the Periodic Table. Chapter 2 Topics. 2.1 Dalton s s Atomic Theory. Evidence for Atoms. Evidence for Atoms
Chapter 2 Atoms, Ions, and the Periodic Table Chapter 2 Topics 1. Dalton s s Atomic Theory 2. Structure of the Atom 3. Ions 4. Atomic Mass 5. The Periodic Table Copyright The McGraw-Hill Companies, Inc.
More informationTest 3: Lab Safety, Measurements, Matter and Periodic Table
Name: Grade/Group: Subject: Chemistry-7 Teacher: Mrs. Raj Date: Test 3: Lab Safety, Measurements, Matter and Periodic Table Directions: Determine the best answer for each question. Circle your answer on
More information1. Demonstrate knowledge of the three subatomic particles, their properties, and their location within the atom.
1. Demonstrate knowledge of the three subatomic particles, their properties, and their location within the atom. 2. Define and give examples of ionic bonding (e.g., metal and non metal) and covalent bonding
More informationMr. Dolgos Regents Chemistry PRACTICE PACKET. Unit 3: Periodic Table
*STUDENT* *STUDENT* Mr. Dolgos Regents Chemistry PRACTICE PACKET Unit 3: Periodic Table 2 3 It s Elemental DIRECTIONS: Use the reading below to answer the questions that follow. We all know by now that
More informationUnit 2 Periodic Table
2-1 Unit 2 Periodic Table At the end of this unit, you ll be able to Describe the origin of the periodic table State the modern periodic law Key the periodic table according to metals vs. nonmetals and
More informationAtoms, Elements, and the Periodic Table Unit Assessment (2016) Page 1 of 13
TEST NAME:Atoms, Elements, and the Periodic Table Unit Assessment (2016) TEST ID:36063 GRADE:06-08 SUBJECT:Life and Physical Sciences TEST CATEGORY: Common Assessment Atoms, Elements, and the Periodic
More informationElements and the Periodic Table
Chapter 7 Elements and the Periodic Table What are metals like? Think of things that are made with metals like aluminum, copper, iron, and gold. What do they have in common? They are usually shiny, and
More informationNote Taking Guide: Episode 401. arranged elements by. predicted of missing. discovered that each has a unique. arranged elements by
Note Taking Guide: Episode 401 Dmitri Mendeleev: arranged elements by. predicted of missing. Henry Moseley: discovered that each has a unique. arranged elements by. now all elements fit into place based
More informationHonors Chemistry: Chapter 4- Problem Set (with some 6)
Honors Chemistry: Chapter 4- Problem Set (with some 6) All answers and work on a separate sheet of paper! Classify the following as always true (AT), sometimes true (ST), or never true (NT) 1. Atoms of
More informationThe Atom & Periodic Table. Unit 2 Topics 4-6
The Atom & Periodic Table Unit 2 Topics 4-6 Electrons in Atoms Topic 4 Describe Bohr s model of the atom. Sketch it! Bohr - A review electrons exist in orbits around the nucleus. Bohr - IB Information
More informationTest 5: Periodic Table, Ionic, and Molecular Compounds
Name: - Grade/Group: Subject: Chemistry-7 Teacher: Mrs. Raj Date: Test 5: Periodic Table, Ionic, and Molecular Compounds Directions: Identify the letter of the choice that best completes the statement
More informationDevelopment of the Modern Periodic Table
07/08 Development of the Modern Periodic Table Mohamed Ahmed Abdelbari Introduction Atom: the smallest, indivisible unit of an element that retains all chemical and physical properties of the element.
More informationDiscovery of Elements. Dmitri Mendeleev Stanislao Canizzaro (1860) Modern Periodic Table. Henry Moseley. PT Background Information
Discovery of Elements Development of the Periodic Table Chapter 5 Honors Chemistry 412 At the end of the 1700 s, only 30 elements had been isolated Included most currency metals and some nonmetals New
More informationUnit 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
More informationAtoms and Elements Review
Atoms and Elements Review YOU ARE EXPECTED TO KNOW THE MEANING OF ALL THE FOLLOWING TERMS: ALCHEMY ELEMENT ATOM SUBATOMIC DEMOCRITUS DALTON THOMSON RUTHERFORD BOHR ELECTRON NEUTRAL PROTON NEUTRON ORBIT
More informationUnit 3 Atomic Structure
Name: Unit 3 Atomic Structure Scientist Year Contribution and/ or Experimental Work Democritus Aristotle Alchemists Boyle Franklin Dalton Avogadro Mendeleev Moseley 1 Scientist Year Contribution and/ or
More informationNotes: Unit 6 Electron Configuration and the Periodic Table
Name KEY Block Notes: Unit 6 Electron Configuration and the Periodic Table In the 1790's Antoine Lavoisier compiled a list of the known elements at that time. There were only 23 elements. By the 1870's
More informationSCH3U- R. H. KING ACADEMY ATOMIC STRUCTURE HANDOUT NAME:
Particle Theory of Matter Matter is anything that has and takes up. All matter is made up of very small. Each pure substance has its of particle, from the particles of other pure substances. Particles
More informationNote that the protons and neutrons are each almost 2,000 times more massive than an electron; What is the approximate diameter of an atom?
Atomic Structure and the Periodic Table Evolution of Atomic Theory The ancient Greek scientist Democritus is often credited with developing the idea of the atom Democritus proposed that matter was, on
More information1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass
1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass A Br, Ga, Hg C O, S, Se B atomic number D oxidation number 2. Which list includes elements with the
More informationWP Unit 2 Practice: The Atom
WP Unit 2 Practice: The Atom Name 1. Name, and identify them clearly in your answer, one halogen, one noble gas, one alkali metal, one alkali earth metal, one metalloid, one transition metal and finally
More informationChapter 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
More informationElements, Atoms, and Ions
Elements, Atoms, and Ions Chemistry I: Chapter 2b Chemistry I Honors: Chapter 3 ICP: Chapter 17 SAVE PAPER AND INK!!! When you print out the notes on PowerPoint, print "Handouts" instead of "Slides" in
More informationCP Chemistry Semester 1 Final Test Review
Mass in grams 10 20 30 40 50 CP Chemistry Semester 1 Final Test Review 1. Know the symbol and the power of 10 for the following metric prefixes: A. Mega M 10 6 D. deka da 10 1 G. milli m 10 6 B. kilo k
More information1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass
1. The elements on the Periodic Table are arranged in order of increasing A atomic mass C molar mass A Br, Ga, Hg C O, S, Se B atomic number D oxidation number 2. Which list includes elements with the
More informationNoble gases do not join other atoms to form compounds. They seem to be most stable just as they are.
UNIT 3: TE NATURE MATTER: MLECULES There are fewer than one hundred naturally occurring elements on the earth, but there are billions of compounds made of those elements. In this unit, we will examine
More informationChemistry 1-2E Semester I Study Guide
Chemistry 1-2E Semester I Study Guide Name Hour Chapter 1 1. Define the following terms. Matter Mass Law of Conservation of Mass 2. Define and give 2 examples of the following: Pure substance Element Compound
More informationUnit 2 continued-chemical Foundations Atoms, Ions, &Elements
Unit 2 continuedchemical Foundations Atoms, Ions, &Elements The Elements Most abundant elements in/on Earth: Oxygen 49.2% Silicon25.7% Most abundant in the human body: Oxygen65.0% Carbon18.0 % Hydrogen10.0%
More informationPhysical Science Lecture Notes Chapters 16, 17 & 18
Physical Science Lecture Notes Chapters 16, 17 & 18 I. 16-1 Organizing Elements a. The periodic table is laid out by increasing atomic number as you go across and down the table b. Main body of the table
More informationScience Class 9 th ATOMS AND MOLECULES. Symbols of Atoms of Different Elements. Atomic Mass. Molecules. Ions. Mole Concept. Finish Line & Beyond
Science Class 9 th ATOMS AND MOLECULES Symbols of Atoms of Different Elements Atomic Mass Molecules Ions Mole Concept Atom An atom is a particle of matter that uniquely defines a chemical element. An atom
More informationName: Date: ChemT1. 1) Using the diagram above, answer the following question: What can be inferred from the diagram about the structure of the atom?
Name: Date: ChemT1 1) Using the diagram above, answer the following question: What can be inferred from the diagram about the structure of the atom? A. the atom is very small B. the electrons are moving
More informationMULTIPLE 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
More informationRegan & Johnston Chemistry Unit 3 Exam: The Periodic Table Class Period
Regan & Johnston Name Chemistry Unit 3 Exam: The Periodic Table Class Period 1. An atom of which element has the largest atomic radius? (1) Si (2) Fe (3) Zn (4) Mg 2. Which characteristics both generally
More informationSymbol Atomic Number
Name: Date: Chemistry ~ Ms. Hart Class: Anions or Cations February Break Review Sheets - /150 Chemistry has a LOT of words. Take this break to review and strengthen your knowledge of the vocabulary you
More informationFull file at
16 Chapter 2: Atoms and the Periodic Table Solutions to In-Chapter Problems 2.1 Each element is identified by a one- or two-letter symbol. Use the periodic table to find the symbol for each element. a.
More information