6.1 The Periodic Table
|
|
- Bernard Rodgers
- 6 years ago
- Views:
Transcription
1 6.1 The Periodic Table The elements can be divided into metals, nonmetals, and metalloids There are about 118 known elements. Based on their physical and chemical properties, they belong to one of three broad categories: metals, nonmetals, and metalloids. Metals are malleable and shiny and conduct electricity, and they are generally solid at room temperature. Examples include aluminum and copper. Nonmetals do not conduct electricity. Many nonmetals are gases or liquids at room temperature. Examples include nitrogen and oxygen. Metalloids have some properties similar to metals and some similar to nonmetals. Silicon is an important metalloid. Some elements are synthetic Technetium (number 43), promethium (number 61), and all of the elements above atomic number 92 do not have any stable isotopes. These elements are highly radioactive. They were synthesized in a laboratory by bombarding the nuclei of existing atoms with highenergy particles such as neutrons or other fast-moving atomic nuclei. 168 A NATURAL APPROACH TO CHEMISTRY
2 The periodic table and you You are made mostly of hydrogen, carbon, oxygen, and nitrogen Take approximately 44,000,000,000,000,000,000,000,000,000 atoms of the right kind, bond some of them together, mix the resulting bunch of molecules and ions together, and you could end up with a typical person weighing about 75 kg (or 165 lb). Of those atoms, over 99% of them would need to be only four different elements: hydrogen, carbon, oxygen, and nitrogen. Other elements are also essential for life, but they exist in much smaller numbers. TABLE 6.1. Elemental composition of the human body Element % by mole Hydrogen 63.0 Oxygen 26.0 Carbon 9.0 Nitrogen 1.25 Calcium 0.25 Phosphorus 0.19 Potassium 0.06 Sulfur 0.06 Sodium 0.04 Chlorine Magnesium Iron Iodine You are made from star dust There would also be trace amounts of almost every element on the table, because you are what you eat (and what you breathe), absorbing everything from your environment. Although hydrogen is the most common atom in your body, virtually all of the hydrogen in the universe was created in the Big Bang, so you have atoms in you that were present at the beginning of space and time. Even more incredible is the fact that almost all of the other atoms in your body must have been produced in the cores of exploding stars. These stars eventually provided the material from which the Earth was formed. You are literally made out of star dust! trace amount: a very small quantity. A NATURAL APPROACH TO CHEMISTRY 169
3 Essential elements Macronutrients and trace elements While traces of almost all naturally occurring elements exist in your body, there are a small number that are considered essential to life. To maintain a healthy body, there are some elements you need to have a lot of; these are called macronutrients. These are the ones that form the bulk of your body. Macronutrient elements such as Na, Mg, P, S, Cl, K, and Ca are come from mineral sources, while others such as C, H, N, and O are found in organic matter. There are also some elements that are beneficial in trace amounts but can be toxic if you have too much. The molecules of life Trace elements play special roles To make fats, carbohydrates, DNA, and proteins, you need hydrogen, carbon, nitrogen, oxygen, phosphorus, and sulfur. Calcium is needed to build your bones, and it functions in many other ways as dissolved ions. Sodium, magnesium, potassium, and chlorine all exist as dissolved ions. They help to transport other molecules into and out of cells, firing your nerves so you can see, smell, hear, and touch, and controlling the amount of water that enters and leaves your cells. These are only a few of the functions done by these other macronutrients. The trace elements tend to have more specialized functions and are only present in extremely small amounts. You might be surprised to see chromium (Cr) on the list of essential elements. Some forms of Cr are know to cause cancer. However, in small amounts, Cr +3 ions are necessary to enhance insulin function, helping to control blood sugar levels. Other trace elements work together with enzymes to help them perform necessary biological functions. You would not be able to live without functioning enzymes. macronutrients: elements needed in large quantities by your body. trace elements: elements that are needed in very small quantities to maintain optimum health. 170 A NATURAL APPROACH TO CHEMISTRY
4 Periodic properties of the elements Searching for order in the elements Back in 1869, when the science of chemistry was still young, a scientist and teacher of chemistry named Dimitri Mendeleev was trying to figure out whether there was an organization to the elements. He was searching for a pattern he could use to organize them in a logical way. At that time little was known about atoms. He knew that elements had an atomic mass and some other physical and chemical properties. Mendeleev tried arranging elements in order of atomic mass. Protons had not yet been discovered, and atomic number was not known at that time. Mendeleev When he graphed the density of the elements versus their atomic mass he saw a pattern. Density is a periodic property He observed that the density of the elements followed a periodic pattern, meaning that the pattern would repeat at regular intervals. Here he saw the density increase and then decrease in a repetitive pattern. The periodic table is named for this because the rows are organized by repeated patterns found in both the atomic structures and the properties of the elements. periodic: repeating at regular intervals. A NATURAL APPROACH TO CHEMISTRY 171
5 Atomic level periodic properties Atomic level properties match patterns of easily observable properties Mendeleev could have known nothing about the properties of individual atoms. Very little was known about atoms during his lifetime other than the belief that atoms existed. The internal structure consisting of protons, neutrons and electrons had yet to be discovered. Only the bulk properties that could be measured, such as density, melting point, boiling point, and the ratios of how one element would combine with another, were known. However, it would probably not surprise Mendeleev that atomic level properties would follow the same periodic patterns, closely matching easily observable properties already discussed. One simple example of a periodic atomic property is atomic size. The image below shows the relative size of atoms from the first 18 elements on the periodic table. Atomic level properties explain bonding As you can see, every time the pattern repeats, it coincides with the beginning of a new row in the periodic table. Density and reaction ratios with oxygen follow the exact same pattern. There are three important atomic level properties that we will consider, because they are very helpful in understanding the different kinds of bonding we will learn about in the next chapter. These properties are atomic radius, electronegativity, and ionization energy. 172 A NATURAL APPROACH TO CHEMISTRY
6 Atomic radius, electronegativity, and ionization energy Atomic radius: the size of an atom Electronegativity: how well one atom grabs electrons from another Ionization energy: how well an atom holds onto its own electrons The atomic radius describes the distance from the center of an atom to its outer edge. The words outer edge are in quotes because atoms don t have a sharply defined edge. The tiny nucleus is surrounded by a cloud of electrons. The space an electron occupies is defined by the orbitals occupied by its electrons. These orbitals describe where you are likely to find electrons. The outer edge of an atom is defined by the place where the likelihood of finding its electrons gets very low. Atoms share electrons whenever they bond together. In some cases they share the electrons equally or almost equally, causing a covalent bond to form. In other cases the sharing is so uneven that we consider one atom to have taken electrons from the other. This causes the formation of ions. An atom s electronegativity is the measure of how well it can attract electrons from another atom to which it is bonded. The ionization energy is the energy it takes to remove an electron from an atom. Electronegativity measures how well an atom can take electrons from another bonded atom, whereas ionization energy measures how well an atom holds onto its own electrons. You don t need to have an atom bonded to another atom when considering ionization energy. If you hit an individual atom with a photon of light with enough energy, you can cause an electron to get so excited that it jumps completely out of the atom, forming an ion. The minimum energy needed to make this happen is called the ionization energy. atomic radius: the distance from the center of an atom to its outer edge. electronegativity: the ability of an atom to attract another atom s electrons when bound to that other atom. ionization energy: the energy required to remove an electron from an atom. A NATURAL APPROACH TO CHEMISTRY 173
7 The first periodic table Chemical properties have a repeating pattern Density was a physical property of the elements that Mendeleev used in looking for patterns, but he also used chemical properties. For most of the elements, the ratio of how they react with either hydrogen or oxygen was already well known. Again, the elements were arranged in order of increasing atomic mass as with density, but this time the oxide or hydride formula was written instead of the value for density. Another pattern emerged. The first periodic table as suggested by Mendeleev in 1869 How the first periodic table was created If you take a look back at the density graph, you will find another reason to start a new row with Li, Na, K, Cu, and Rb. All of them, except for Cu, are at a point when the density is lowest and the pattern of densities starts to repeat. So, the repeating physical property of density seems to match up well with the repeating chemical properties of the elements. Mendeleev noticed this periodic pattern in both chemical and physical properties, so he arranged the elements into a table like the one you see above, with columns representing elements with similar chemical properties. 174 A NATURAL APPROACH TO CHEMISTRY
8 The modern periodic table The modern periodic table is organized by atomic number Nothing was known about the internal structure of atoms in Mendeleev s time. Protons hadn t been discovered yet, so the more logical ordering by atomic number was not possible. Today s periodic table includes many more elements and is ordered not by atomic mass but by atomic number. However, two things are still true of the periodic table. Each column still represents a group of elements with similar chemical properties, and each row (or period) still marks the beginning of a repeated pattern of physical or chemical properties. Elements can be broadly categorized into metals, nonmetals and metalloids, and an understanding that each column has similar chemical properties has led to names for some of these element groups. Groups of particular interest are the alkali metals (group 1), the alkaline earth metals (group 2), the halogens (group 17), and the noble gases (group 18). A NATURAL APPROACH TO CHEMISTRY 175
9 Orbitals and atomic radius The electron cloud in overlapping orbitals is what gives an atom its size One of the atomic level properties that we looked at previously was atomic radius, which is an indication of the size of an atom. The nucleus is tiny, so the size of the atom is really the space occupied by the electron cloud surrounding the nucleus. To the right is a view of a boron atom showing a unique color for each orbital containing electrons. The cloud of electrons created by the overlapping 1s, 2s, and 2p orbitals is what gives a boron atom its size. Here is another version of the table showing which orbitals are the last to be filled as the electrons fill up around an atom s nucleus. Atomic radii match orbital sizes Compare the table above with the chart to the right. Each time you start a new row, the atom gets bigger because you start filling a new primary energy level with bigger orbitals. As you go across a row, atoms get smaller because the increased number of protons pulls electrons at the same primary level closer to the nucleus. 176 A NATURAL APPROACH TO CHEMISTRY
Elements and the Periodic Table
CHAPTER 6 Elements and the Periodic Table 6.1 The Periodic Table Are you made of star dust? Are you made of star dust? The Big Bang produced hydrogen and helium and a tiny bit of lithium Are you made of
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 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 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 informationSection 6-1 Notes. Organizing the Elements
Section 6-1 Notes Organizing the Elements Organizing the Elements As new elements were discovered chemists needed to find a logical way to organize them Properties of elements were used to sort them in
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 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 informationHistory of The Periodic Table
History of The Periodic Table Organizing the Elements Chemists used the properties of elements to sort them into groups. JW. Dobreiner grouped elements into triads. A triad is a set of three elements with
More informationAssessment Chapter 5 Pre-Test Chapter: The Periodic Law Use the periodic table below to answer the questions in this Chapter Test.
Assessment Chapter 5 Pre-Test Chapter: The Periodic Law Use the periodic table below to answer the questions in this Chapter Test. In the space provided, write the letter of the term or phrase that best
More informationChapter: The Periodic Table
Table of Contents Chapter: The Periodic Table Section 1: Introduction to the Periodic Table What does periodic mean? Periodic means with a repeating pattern A periodic event is predictable Periodic Table
More informationThe Periodic Table & Formation of Ions
The Periodic Table & Formation of Ions Development of the Periodic Table Mendeleev: Considered to be the father of the periodic table Arranged elements by increasing atomic mass Placed elements with similar
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 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 informationChapter 1: Atomic Structure and the Periodic Table 1.1 Atoms are the smallest form of elements.
Chapter 1: Atomic Structure and the Periodic Table 1.1 Atoms are the smallest form of elements. All matter is made of atoms. About 100 different atoms, or elements, make up everything on Earth. Hydrogen
More informationPeriodic Table of Elements
Periodic Table of Elements The Atomic Nucleus The nucleus is a small, dense region at the center of the atom. It consists of positive protons and neutral neutrons, so it has an overall positive charge.
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 informationThe Periodic Table and Periodic Trends
The Periodic Table and Periodic Trends The properties of the elements exhibit trends and these trends can be predicted with the help of the periodic table. They can also be explained and understood by
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 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 informationHistory German J. W. Dobereiner Grouped elements into triads
The Periodic Table History 1829 German J. W. Dobereiner Grouped elements into triads One of these triads included chlorine, bromine, and iodine; another consisted of calcium, strontium, and barium. In
More informationName Class Date ELECTRONS AND THE STRUCTURE OF ATOMS
The Periodic Table ELECTRONS AND THE STRUCTURE OF ATOMS 6.1 Organizing the Elements Essential Understanding Although Dmitri Mendeleev is often credited as the father of the periodic table, the work of
More informationHOW ARE ELEMENTS ORGANIZED? (4-1) Periodic Table an arrangement of the elements in, based on a set of that repeat row after row
The Periodic Table Chemistry, Ch. 3 HOW ARE ELEMENTS ORGANIZED? (4-1) Periodic Table an arrangement of the elements in, based on a set of that repeat row after row Dmitri Mendeleev created the first useful
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 information7. What is the likeliest oxidation number of an element located in Period 3 and Group 16? a. +2 b. +3 c. -3 d The amount of energy required to
1. Which of the following is the most important factor in determining the properties of an element? a. Atomic mass b. Atomic radius c. Periodic table position d. Electron configuration 2. Similar properties
More informationModern 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 informationName Date Class THE PERIODIC TABLE
Name Date Class 6 THE PERIODIC TABLE SECTION 6.1 ORGANIZING THE ELEMENTS (pages 155 160) This section describes the development of the periodic table and explains the periodic law. It also describes the
More informationAtomic Structure and The Periodic Table. Unit 3
Atomic Structure and The Periodic Table Unit 3 Lesson 1: Atoms Unit 5: Atomic Structure & The Periodic Table Atoms How small can things get? If you break a stone wall into smaller and smaller pieces, you
More informationFor the Periodic Table above indicate each of the following TRENDS: atomic size and ionic size. Na Na + F F - Ne < < < <
Chapter 6 Organizing the Elements THE PERIODIC TABLE AND PERIODIC LAW Periodic Table Summary Sheet For the Periodic Table above indicate each of the following TRENDS: atomic size and ionic size Na Na +
More informationPERIODIC TRENDS AND THE PERIODIC TABLE
PERIODIC TRENDS AND THE PERIODIC TABLE THE PERIODIC TABLE The row tells us how many energy levels are in that atom The row is also the group The column tells us how many electrons are in the outer energy
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 informationIntroduction period group
The Periodic Table Introduction The periodic table is made up of rows of elements and columns. An element is identified by its chemical symbol. The number above the symbol is the atomic number The number
More informationPeriodic Table. Engr. Yvonne Ligaya F. Musico 1
Periodic Table Engr. Yvonne Ligaya F. Musico 1 TOPIC Definition of Periodic Table Historical Development of the Periodic Table The Periodic Law and Organization of Elements in a Periodic Table Periodic
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 informationRegents Chemistry PRACTICE PACKET
*KEY* *KEY* Regents Chemistry PRACTICE PACKET Unit 3: Periodic Table 1 Copyright 2015 Tim Dolgos 2 Copyright 2015 Tim Dolgos 3 Copyright 2015 Tim Dolgos It s Elemental DIRECTIONS: Use the reading below
More informationThe Arrangement of Atoms in the Periodic Table
1 The Arrangement of Atoms in the Periodic Table [Material is from The Free High School Science Texts: Textbooks for High School Students Studying the Sciences Chemistry Grades 10 12. www.fhsst.org unless
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 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 informationYear 8 Chemistry Knowledge Organiser Topic 1: Periodic Table
KPI 1.1: Identify, with reasons, differences between atoms, elements and compounds Key Terms Element Mixture Compound Elements Definitions A substance that contains only one type of atom A substance that
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 informationDeveloping the Periodic Table
Developing the Periodic Table Early Element Classification Mendeleev s First Periodic Table Mendeleev s First Periodic Table Mendeleev s Periodic Table Arranged by increasing atomic mass Some elements
More informationChapter 5 The Periodic Law
z Chapter 5 The Periodic Law z Section 5-1 History of the Periodic Table Mendeleev noticed that when the elements were arranged in order of increasing atomic mass, certain similarities in their chemical
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 informationPeriod Table Worksheet 1
Period Table Worksheet. While doing a research project, you noted the following information about five elements. Element A :. is a solid;. conducts electricity;. has electrons in its outermost shell;.
More informationb. Na. d. So. 1 A basketball has more mass than a golf ball because:
Chem I Semester Review All of the following are general characteristics of a substance in the liquid state except a. definite volume. c. not easily compressed. b. able to flow. d. definite shape. In the
More informationChapter 5 Review 1. The order of elements in the periodic table is based on a. the number of protons in the nucleus. b. the electric charge of the
Chapter 5 Review 1. The order of elements in the periodic table is based on a. the number of protons in the nucleus. b. the electric charge of the nucleus. c. the number of neutrons in the nucleus. d.
More informationPeriodic Trends. Name: Class: Date: ID: A. Matching
Name: Class: Date: Periodic Trends Matching Match each item with the correct statement below. a. electronegativity f. periodic law b. ionization energy g. atomic mass c. atomic radius h. period d. metal
More information8 th Grade Science. Directed Reading Packet. Chemistry. Name: Teacher: Period:
8 th Grade Science Directed Reading Packet Chemistry Name: Teacher: Period: Chapter 1, Section 1: Inside the Atom Introduction 1. Atoms are the particles of an element that still have the element s. 2.
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 informationChapter 3-1. proton positive nucleus 1 amu neutron zero nucleus 1 amu electron negative on energy levels around the nucleus very small
Chapter 3-1 Sub-atomic Charge Location Mass Particle proton positive nucleus 1 amu neutron zero nucleus 1 amu electron negative on energy levels around the nucleus very small The most mass of the atom
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 informationHomework Packet Unit 2. b. Al 3+, F, Na +, Mg 2+, O 2
Name Period Homework Packet Unit 2 1. Which of the following is the correct empirical formula for a compound that has 37.5% C, 12.6% H, and 49.9% O? (A) C 2 H 4 O (B) CH 4 O 2 (C) CH 5 O 2 (D) CH 4 O (E)
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 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 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 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 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 informationAtoms with More than One Electron
Activity 6 Atoms with More than One Electron GOALS In this activity you will: View the spectra of various materials. Graphically analyze patterns in the amounts of energy required to remove electrons from
More informationGroup Trends: the trend that the atoms follow going down any particular group
Trends of the Periodic Table Basics Trends are patterns of behaviors that atoms on the periodic table of elements follow. Trends hold true most of the time, but there are exceptions, or blips, where the
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 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 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 informationTrends in the Periodic Table
Trends in the Periodic Table OBJECTIVES FOR TODAY: Fall in love with the Periodic Table, Interpret group and period trends in atomic radii, ionization energies and electronegativity The Periodic Table
More informationCHAPTER NOTES CHAPTER 14. Chemical Periodicity
Goals : To gain an understanding of : 1. Electron configurations 2. Periodicity. CHAPTER NOTES CHAPTER 14 Chemical Periodicity The periodic law states that when the elements are arranged according to increasing
More informationUnit Five Practice Test (Part I) PT C U5 P1
Unit Five Practice Test (Part I) PT C U5 P1 Name Period LPS Standard(s): --- State Standard(s): 12.3.1 Short Answers. Answer the following questions. (5 points each) 1. Write the electron configuration
More informationIn the modern periodic table, elements are arranged by increasing atomic number
THE MODERN PERIODIC TABLE The Periodic Law Q. How is the modern periodic table organized? In the modern periodic table, elements are arranged by increasing atomic number (number of protons). Properties
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 informationMendeleev s Periodic Table Mendeleev arranged the elements in his periodic table in order of increasing atomic mass.
6.1 Searching For an Organizing Principle Chemists used the properties of elements to sort them into groups. Mendeleev s Periodic Table Mendeleev arranged the elements in his periodic table in order of
More informationUNIT 2: Matter and its changes. Mrs. Turner
UNIT 2: Matter and its changes Mrs. Turner Preassessment Take out a sheet of paper and number it from 1-25. Write down your answers to plug them into your clickers. Don t worry about not knowing an answer
More informationThe Periodic Table. Unit 4
The Periodic Table Unit 4 I. History A. Dmitir Mendeleev Russian chemist, 19th century Arranged elements by their properties Arranged by increasing atomic mass Groups: vertical groups-elements have similar
More informationUnit 3 Periodic Table and Quantum HW Packet Name Date. Periodic Table Concepts. 1. In what family are the most active metals located?
Directions: Answer the following questions. Periodic Table Concepts 1. In what family are the most active metals located? 2. In what family are the most active non-metals located? 3. What family on the
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 informationNotes: Electrons and Periodic Table (text Ch. 4 & 5)
Name Per. Notes: Electrons and Periodic Table (text Ch. 4 & 5) NOTE: This set of class notes is not complete. We will be filling in information in class. If you are absent, it is your responsibility to
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 informationPeriodic Table Practice Questions
Periodic Table Practice Questions 1. Elements in the Periodic Table are arranged according to their (1) atomic number (3) relative activity (2) atomic mass (4) relative size 2. Elements in a given period
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 informationPeriodic Table Practice 11/29
Periodic Table Practice 11/29 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
More informationClassify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
ELECTRONS IN ATOMS Chapter Quiz Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 1. The orbitals of a principal energy level are lower in energy than the orbitals
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 informationChapter 6 - The Periodic Table and Periodic Law
Chapter 6 - The Periodic Table and Periodic Law Objectives: Identify different key features of the periodic table. Explain why elements in a group have similar properties. Relate the group and period trends
More informationTextbook: Section B, Chapter 1
Atoms and the Periodic Table Review Sheet Textbook: Section B, Chapter 1 1. What is the Atomic number of nitrogen? 2. How many protons does nitrogen have? 3. How many electrons does nitrogen have? 4. How
More informationUnit 2. Chemical Foundations: Elements, Atoms, and Ions
Unit 2 Chemical Foundations: Elements, Atoms, and Ions Memorize the list of elements You will have a quiz on this list. All of the elements will be on the quiz! Elements in the Earth System (% mass in
More informationChapter 5. Preview. Lesson Starter Objectives Mendeleev and Chemical Periodicity Moseley and the Periodic Law The Modern Periodic Table
Preview Lesson Starter Objectives Mendeleev and Chemical Periodicity Moseley and the Periodic Law The Modern Periodic Table Section 1 History of the Periodic Table Lesson Starter Share what you have learned
More informationFundamentals of General, Organic & Biological Chemistry 4 th Edition. Matter and Life
Fundamentals of General, Organic & Biological Chemistry 4 th Edition Chapter One Matter and Life Mohammed Hashmat Ali Southeast Missouri State University 2003 Prentice Hall, Inc. 1.1 Chemistry: The Central
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 informationPeriodic Table & Families
Periodic Table & Families 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
More informationPart I Assignment: Electron Configurations and the Periodic Table
Chapter 11 The Periodic Table Part I Assignment: Electron Configurations and the Periodic Table Use your periodic table and your new knowledge of how it works with electron configurations to write complete
More informationCHAPTER 6 The Periodic Table
CHAPTER 6 The Periodic Table 6.1 Organizing the Elements Mendeleev: listed the elements in order of increasing atomic mass and in vertical columns according to their properties. Left blank spaces for undiscovered
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 informationSection Objectives: Section Objectives: Distinguish mixtures and solutions. Define acids and bases and relate their importance to biological systems.
Section Objectives: Relate the structure of an atom to the identity of elements. Relate the formation of covalent and ionic chemical bonds to the stability of atoms. Section Objectives: Distinguish mixtures
More informationChapter 6 The Periodic Table The how and why History. Mendeleev s Table
Chapter 6 The Periodic Table The how and why History 1829 German J. W. Dobereiner grouped elements into triads Three elements with similar properties Properties followed a pattern The same element was
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 informationTHE PERIODIC TABLE & PERIODIC LAW! Development of the Modern Periodic Table!
THE PERIODIC TABLE & PERIODIC LAW! Development of the Modern Periodic Table! Development of the Periodic Table! Main Idea: The periodic table evolved over time as scientists discovered more useful ways
More informationSolid Gas Liquid Plasma
Unit 1: MATTER 1. Define CHEMISTRY: 2. Define MATTER: Use one of the states of matter to complete each statement. (Words will be used more than once.) Solid Gas Liquid Plasma 3. A has definite volume and
More informationValence electron- Energy sublevel- Transition element- Period 10. Electronegativity- Alkaline earth metal- 11. Ion- Halogen- 12.
Mrs. Hilliard 1. Valence electron 2. Period 3. Alkaline earth metal 4. Halogen 5. Metalloid 6. Hund s Rule 7. Representative element 8. Energy sublevel 9. Transition element 10. Electronegativity 11. Ion
More informationSAMPLE PROBLEMS! 1. From which of the following is it easiest to remove an electron? a. Mg b. Na c. K d. Ca
SAMPLE PROBLEMS! 1. From which of the following is it easiest to remove an electron? a. Mg b. Na c. K d. Ca 2. Which of the following influenced your answer to number one the most? a. effective nuclear
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 informationQuantitative chemistry Atomic structure Periodicity
IB chemistry Units 1-3 review Quantitative chemistry Significant figures The mole- be able to convert to number of particles and mass Finding empirical and molecular formulas from mass percentage States
More informationThe Periodic Table. LESSON 10 Breaking the Code. Think About It. Exploring the Topic. The Modern Periodic Table
Printed Page 43 [Notes/Highlighting] LESSON 10 Breaking the Code Think About It The elements copper, Cu, and gold, Au, share many similarities. Both are relatively unreactive elements. They are soft so
More informationChapter 5 Trends of the Periodic Table Diary
Chapter 5 Trends of the Periodic Table Diary A Brief History of the Periodic Table I began to look about and write down the elements with their atomic weights and typical properties, analogous elements
More informationChemical Periodicity. Periodic Table
Chemical Periodicity Periodic Table Classification of the Elements OBJECTIVES: Explain why you can infer the properties of an element based on those of other elements in the periodic table. Classification
More information