Elements, Atoms and Ions (Ch. 3). 3.1 The Elements The alchemists tried to create gold from other metals, but failed. They discovered new elements (mercury,

Slides:



Advertisements
Similar presentations
Atoms, Elements & The Periodic Table
Advertisements

Chapter 2 Atoms, Molecules, and Ions History of Atomic Theory Started with the Greeks and four elements (earth, air, water and fire) Democritus termed.
Copyright©2004 by Houghton Mifflin Company. All rights reserved. 1 Introductory Chemistry: A Foundation FIFTH EDITION by Steven S. Zumdahl University of.
Copyright©2004 by Houghton Mifflin Company. All rights reserved. 1 Introductory Chemistry: A Foundation FIFTH EDITION by Steven S. Zumdahl University of.
Copyright©2004 by Houghton Mifflin Company. All rights reserved. 1 Elements, Atoms & Ions Chapter 4.
Copyright © Houghton Mifflin Company. All rights reserved. 4 | 1 Dalton’s Atomic Theory Elements are composed of tiny particles called atoms. All atoms.
Chapter 5 Atomic Structure
Ch. 5: Atomic Structure Standards: Matter consists of atoms that have internal structures that dictate their chemical and physical behavior. Targets:
Chemical Foundations: Elements, Atoms, and Ions
Atomic Structure and the Periodic Table
Unit 3 Particles with Internal Structure
Elements, Atoms & Ions Chapter 4
Chapter 5 Atoms and Periodic Table
Unit 3 - Elements, Atoms and Ions
Chapter Three Chemical Foundations: Elements, Atoms, and Ions
Atomic Structure and the Periodic Table. Early Models of the Atom Dalton’s Atomic Theory - All elements are composed of atoms - All elements are composed.
Introduction to Chemistry: Matter and its Interactions Mr. Pierson Fall 2013.
Periodic Patterns.
Courtesy: Tiny nucleus: diameter of about cm. Electrons: move about the nucleus at an average distance of about from.
Chapter 4: Elements, Atoms, and Ions Chemistry 1020: Interpretive chemistry Andy Aspaas, Instructor.
Unit 2 - Chapter 3 Elements, Atoms, Ions. The elements Can we name some? How many are there? Where would you find that information?
AP Chemistry – Chapter 2 Atoms, Molecules and Ions.
1 Elements, Atoms & Ions Chapter 4 (except 4.3, 4.5)
Chemical Foundations: Elements, Atoms, and Ions
Classifying Elements Each element has a name and a symbol. The symbol is an abbreviated, or shortened version, of the element’s name. It is used to represent.
The Periodic Table (Your new best friend!!)
Chapter 3Atoms and Elements 3.1 Elements and Symbols Elements are pure substances that cannot be separated into simpler substances by ordinary laboratory.
Words Compounds The Elements
Unit 2.  There are about 118 different known elements with 88 of them occurring naturally.  The names and symbols of each element are listed on the.
CHEMISTRY World of Zumdahl Zumdahl DeCoste. Chapter 3 Chemical Foundations: Elements, Atoms, and Ions.
Chemistry Chapter 3 Chemical Foundations: Elements, Atoms, and Ions
Chapter 3Atoms and Elements Elements and Symbols Elements are pure substances that cannot be separated into simpler substances by ordinary laboratory.
Introduction to Chemistry. Chemistry Is the Science that deals with the composition, structure, and properties of matter and the transformations which.
Introduction to Atomic Structure Chemistry Chemistry is the study of matter and the changes it undergoes. The type of matter that is changing and what.
Chapter 3Atoms and Elements Classification of Matter Copyright © 2009 by Pearson Education, Inc.
Chemistry Review. ATOMS Smallest unit of matter. –Atoms make up everything (that has mass and takes up space).
Elements, Atoms, and Ions. Elements 88 occur naturally Table most abundant elements in Earth’s crust, oceans, and atmosphere Table Abundance.
Section 3.1 The Elements Objectives 1.To learn about the relative abundances of the elements 2.To learn the names of some elements 3.To learn the symbols.
Elements and Their Properties
IPC 7.D Relate the chemical behavior of an element, including bonding, to its placement on the periodic table.
Atomic Theory John Dalton Four Part Theory adopted as basis for the Modern Atomic Theory Four Part Theory adopted as basis for the Modern Atomic Theory.
Chapter 3 Classification of Matter Objectives: Define and give examples of 3 states of matter (3.1 & 3.2) Distinguish between substances and mixtures (3.3.
Some Notes on Charge Two Kinds of Charge called + and – Opposite Charges Attract + attracted to – Like Charges Repel + repels + – repels – To be Neutral,
Atomic Structure and the Periodic Table. Early Models of the Atom Democritus (4 th century BC) –atomos – “unable to be divided.” Democritus (4 th century.
Chapter 4 Chemical Foundations: Elements, Atoms, and Ions Chemistry B2A.
CHAP 2 Atoms, Molecules, and ions. History Greeks everything made up of 4 fundamental substances (earth,air,fire,water) “atomos” – later became atom –
Atomic Structure and the Periodic Table
Elements and the Periodic Table Chapter 4. What will we learn today? Today we will describe the atomic theory using Cornell Notes and a timeline.
Chapter 4 The Greeks thought that matter was composed of fire, earth, water, and air.
Ch. 5: Atomic Structure Standards: Matter consists of atoms that have internal structures that dictate their chemical and physical behavior. Targets: State.
Pages  What are the parts of an atom?  Nucleus – The center of the atom. It contains…  Protons – Positively charged particles.  Neutrons.
Chapter 4 Chemical Foundations: Atoms & Elements Chemistry 100.
Atoms, Elements, and the Periodic Table Everything in the universe is made up of matter.
Chemistry Review. ATOMS Smallest unit of matter. –Atoms make up everything (that has mass and takes up space).
Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed. by Steven S. Zumdahl & Donald J. DeCoste University.
Write the correct vocabulary term for the given definition. 1. ability of a substance to be pulled into thin wires 2. ability of a substance to be hammered.
CHAPTER THREE Atoms and Elements. Section 1: Structure of Matter  Matter is anything that has mass and takes up space.  Early Philosophers:  Earth.
Unit #2 Atoms, Molecules and Ions. Introduction Atoms Composed of electrons, protons and neutrons Molecules Combinations of atoms Ions Charged particles.
Chemical Foundations: Elements, Atoms, and Ions Chapter 4.
Copyright©2004 by Houghton Mifflin Company. All rights reserved. 1 Introductory Chemistry: A Foundation FIFTH EDITION by Steven S. Zumdahl University of.
Atomic Structure. Matter Anything that has mass and takes up space Matter can take many forms and is not always visible to the eye Matter can change form.
Atomic Structure.
Chapter 4 Elements, Atoms & Ions
Atomic Theory Chapter 4.
Chapter 4 Study Sheet Atomic Theory for 6th Graders.
Chapter 5: Atomic structure & the Periodic Table
Matter, Atoms and The Periodic Table.
WoC Ch 3.8 Intro to the Periodic Table
Inside the Atom Chapter 1.
Presentation transcript:

Elements, Atoms and Ions (Ch. 3)

3.1 The Elements The alchemists tried to create gold from other metals, but failed. They discovered new elements (mercury, sulfur) and purified acids.

The Elements The most abundant element in the earth’s crust and atmosphere is oxygen. Oxygen is also the most abundant element in the human body. Oxygen is found as… –An element (O 2 ) in the air –A compound in water and in rocks.

The elements The names of elements came from… –Latin and Greek –places –famous scientists. Chlorine = color in Greek Californium – discovered in California. Element symbols are abbreviations for the elements. C = carbon, F = fluorine Practice questions p55

3.2 John Dalton (1808) First true scientist to study atoms The law of constant composition – a compound always has the same proportion of elements. –In water, there is always 8g Oxygen : 1g Hydrogen

Dalton’s Atomic Theory 1.All elements are made of atoms… atoms are indestructible 2.All atoms of an element are the same 3.Compounds are made by combining 2 or more different kinds of atoms 4.In chemical reactions, atoms just rearrange to make new chemicals.

Formulas Formulas – show how many atoms are in a compound Example: 4H 2 SO 4 Subscript – Tells us how many of the atom there are. Only for Atom directly to its left

3.3 Joseph John (J.J.) Thomson (1897) Thomson’s experiment J.J. Thomson pumped electricity through a glass tube. “Cathode rays” shoot out from the metal cathode.

Observation 1: The glowing ray was repelled by a negatively charged plate –Conclusion: Rays are negatively charged particles. Observation 2: Any metal could be used as as electrode with the same result. –Conclusion: all elements must have these particles. Electrons are small, negatively charged particles.

Plum Pudding Model JJ Thomson and William Thomson thought that electrons were stuck in a positively charged ball.

Ernest Rutherford (1911) Gold foil experiment Setup

Gold foil experiment α-particles (α = alpha) are relatively massive (heavy) and positively (+) charged Hypothesis: If an atom had a spread out positive charge, then α-particles could go straight through the atom.

Planetary model Observation Most alpha rays passed straight through Some pushed away Some bounced straight back Conclusion Most of the atom is empty space Small area of positive charge Small area of huge mass (high density) Discovered the Nucleus

Gold foil experiment on the atomic level

Nucleus is really small If we built a scale model of an atom, with a baseball as the nucleus, how far away would the outer edge of the atom be located?

The Nuclear Atom The dense, positive center is called the nucleus. The nucleus contains protons and neutrons. In atoms, # protons = # electrons (“#” is my symbol for “number”) Nucleus

The Nuclear Atom ProtonsNeutronsElectrons MassHigh Very small (1/1836 th of a proton) Charge+10

Isotopes Isotopes are atoms with the same number of protons but different numbers of neutrons. –Example: Carbon can have 6 neutrons or 7 neutrons. The atomic number = # protons The mass number = # protons + neutrons

Isotopes A = mass number Z = atomic number Mass number = # protons + # neutrons –Electrons have very little mass, so we ignore them.

Isotope Notation Mass number Atomic number Charge Element Symbol Practice problems p67 #3, 4, 7

3.4 Using the Periodic Table The periodic table shows the atomic number above the symbol of each element. What is the atomic number of carbon? Yes, 6 The columns (up and down) are called groups. They have similar chemical properties. “1A” is called “group 1.”

Group 1 23 Periodic Table Etc…

Groups “1A” is called “group 1.” Group 1: alkali metals Group 2: alkaline earth metals Group 7: halogens Group 8: Noble gases

metals, metalloids and non-metals Stair-step line Metals to left Non-metals to Right Metalloids Touch Stair-Step

Groups Metals are: –Good conduction of electricity –Malleable (can be hammered flat) –Ductile (can be pulled into wires) –Lustrous (shiny)

Nonmetals are: –Usually poor conductors. –Brittle (break easily). –Dull (not shiny) appearance. Metalloids have properties of both metals and nonmetals.

Groups Some elements exist in the pure form. Ex: gold (Au). Most elements exist in a combined form, not the pure form. Ex.: Iron is found as Iron Oxide Fe 2 O Atoms in group 8 (“the noble gases”) usually do not combine with other elements.

Groups Some gases are diatomic molecules, which have two atoms. Ex: O 2 –Remember: HOFBrINCl (H, O, F, Br, I, N and Cl form diatomic molecules). Gas, liquid or solid? –H, N, O, F, Cl and group 8A are gases at room temperature (25°C). –Bromine (Br 2 ) and mercury (Hg) are liquids at 25 °C. –All other elements are solid at 25°C.

3.5 Ions Atoms are neutral. Example: sodium NameSymbol# protons# electrons SodiumNa11

3.5 Ions If sodium loses an electron, it will have a positive charge (+1) because there is one more proton than electrons. If chlorine gains an electron, it will have a negative charge (-1). NameSymbol# protons# electrons SodiumNa ChlorineCl

3.5 Ions Cations have a (+) positive charge. Anions have a (-) negative charge. If the charge is only 1+ or 1-, don’t write “1.” –Ex: Na +

3.5 Ions Group1A2A3A6A7A Charge ExampleNa + Mg 2+ Al 3+ O 2- F-F- Some groups form one type of ion:

Ionic compounds Ionic compounds contain a cation and an anion. The attraction between the positive and negative charges holds them together Ionic compounds… –have high boiling points. –cannot conduct electricity as a solid. –can conduct electricity when melted because the electrons are free to move around.

3.5 Ions Ionic compounds form when a cation (+) combines with an anion (-). Ex. Na + + Cl -  NaCl Compounds will ONLY form if the overall charge is zero.

3.5 Ions What is the charge of a Mg ion? +2 What is the charge of a Cl ion? If we mixed a beaker Mg with a beaker of Cl, what would the formula of the compound? Mg 2+ + Cl - + Cl -  MgCl 2 Charge: 2+ 2(1-) 0