Preview Multiple Choice Short Answer Extended Response Standardized Test Preparation Chapter 3.

Slides:



Advertisements
Similar presentations
Chapter 3 Preview Multiple Choice Short Answer Extended Response
Advertisements

Atoms and Atomic Structure
P. 122 – Q # 35 What were the limitations of Democritus’s ideas?
The structure of the atom
Ch Dalton’s Atomic Theory 1.All elements are composed of indivisible atoms (atoms are divisible) 2.Atoms of the same element are identical 3.Atoms.
Subatomic Particles What are three kinds of subatomic particles? 4.2
Chemistry 4.2.
© Copyright Pearson Prentice Hall Slide 1 of 25 Structure of the Nuclear Atom Cathode-ray tubes are found in TVs, computer monitors, and many other devices.
Slide 1 of 18 © Copyright Pearson Prentice Hall Defining the Atom > Early Models of the Atom II. The Atom : smallest particle of an element that retains.
 You cannot see them, yet they make up everything…
» What is the name of this device? » Which scientist used this device?
Chapter Two: Atoms, Molecules and Ions
Chapter 2 Atoms, molecules, and ions
History of Atomic Theory. Scientists B.C. DemocritusAristotle BC Believed matter is continuous 400 BC Coined the term “atom”
Chemistry Chapter 3 Review Game. ChemistryChemistry Chemistry 1 point 1 point 1 point 1 point 1 point 1 point 1 point 1 point 2 points 2 points 2 points.
Slide 1 of 18 Chemistry 4.1. Slide 2 of 18 © Copyright Pearson Prentice Hall Defining the Atom > Early Models of the Atom An atom is the smallest particle.
Chapter 3 Table of Contents
Chapter 3 Atoms and Atomic Structure Write the bullets that are in black font.
AP Chemistry – Chapter 2 Atoms, Molecules and Ions.
Chapter 1 Atomic Structure 1.1 The Atomic Nature of Matter
CHAPTER 4 – THE ATOM John Dalton’s Atomic Theory (19 th Century) 1) All matter is composed of small particles called atoms 2) All atoms of an element.
Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu How to Use This Presentation To View the presentation as a slideshow.
STRUCTURE OF THE ATOM.
FAMOUS SCIENTISTS ATOMIC MASS ATOMIC NUMBER ATOMIC.
Atoms and Atomic Structure
Unit 2: Atomic Theory and Structure. (c. 400 B.C.) Democritus proposed that “atomos” are indivisible. Atom: smallest particle of matter that retains its.
Atoms and Moles.  All matter is made of atoms  Law of definite proportions  Water is 88.8 % oxygen and 11.2 % hydrogen  Law of conservation of mass.
, who was from was the first person to use the term atom during B.C.  Democritus defined the atom as being.  opposed Democritus because believed that.
Review. What was wrong with Dalton’s atomic theory?
The History of the Atom…. went against, Aristotle, who believed that matter was composed of four qualities: earth, fire, air and water all matter is composed.
Atomic Theories. Atomic timeline Your poster should contain: –The date the theory was developed –A picture of the ‘model’ –The name of the main contributor.
Chapter 3 Atoms: The Building Blocks of Matter. The Atomic Theory  Law of conservation of mass  Mass is neither destroyed nor created  Law of definite.
Chapter 4: Atomic Structure Democritus believed that matter was made up of particles. he called nature’s basic particle an “atom”. The …… Aristotle’s idea.
Review Scientist who discovered the electron using the cathode ray tube –Thomson Scientist who used the oil drop experiment to discover the charge on the.
Atoms, Molecules, and Ions Chapter 2 Atoms, Molecules, and Ions John D. Bookstaver St. Charles Community College St. Peters, MO  2006, Prentice Hall,
Slide 1 of 18 © Copyright Pearson Prentice Hall Defining the Atom > Atomic Structure Chapter 4 Video 3.
Chapter 3 pages Modern Chemistry Chapter 3 Atoms: the building block of matter.
Atomic Timeline WARM-UP: Take out your Ch. 3 VOCABULARY and timeline materials and begin completing timeline. With your table, you are to create an Atomic.
The Atom Chapter 3. From Idea to Theory Democritus, Greek philosopher, 400 B.C., introduced the concept of an atom, an ‘indivisible’ particle. Democritus,
Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Table of Contents Chapter 3 Atoms: The Building Blocks of Matter.
Atoms Isotopes Average Atomic Mass Development of Atom
Atoms and Molecules By Doba Jackson, Ph.D.. Outline of Concepts in this chapter Law of Constant Composition (sec. 2-4) –Mass Percentages Dalton’s Atomic.
Chapter 3 – Atoms: The Building Blocks of Matter 3.1: Atomic Theory History A. 1700s: quantitative studies of chemical reactions led to several laws: 1.
Atomic Structure Chapter 4. Dalton’s Atomic Theory 4.1 John Dalton – 18 th century All matter is composed of atoms All atoms of a given element are identical.
Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu How to Use This Presentation To View the presentation as a slideshow.
Chemistry – King William High School.  Foundations…  Law of conservation of mass – mass is neither created nor destroyed  Law of definite proportions.
1 Modern Chemistry Chapter 3 Atoms: The Building Block of Matter.
Modified by M. Sparks Atomic Structure Atomic Mass/Number Ions/Charges of Molecules Isotopes/Perc ent Abundance
Chapter 4 Review 1. Which of the following was the conclusion reached by Ernest Rutherford and his Gold Foil Experiment? a. the atom has a dense positive.
Understanding the Atom 4-1: Basic Units of Matter.
Chapter 3. Section 1 Objectives Explain the law of conservation of mass Summarize the five essential points of Dalton’s atomic theory. Explain the relationship.
Chemistry Chapter Three – Atoms: The Building Blocks of Matter South Lake High School Science Department Ms. Sanders.
Chapter 3: Atoms and Moles Sections 1 and 2
{ Atom and Isotope Review Physical Science. An atom has 6 protons, 8 neutrons, and 6 electrons. What is the atomic mass?
Atomic Theory & Periodic Table Unit 3 Part 1 (Ch. 4 & 5) Atomic Theory Introduction, Isotopes.
Atomic Structure.  Smallest particle of an element w/ properties of that element  About 90 natural elements  Combine to form compounds ◦ Atoms  elements.
End Show © Copyright Pearson Prentice Hall Slide 1 of 25 Structure of the Nuclear Atom Cathode-ray tubes are found in TVs, computer monitors, and many.
Atomic Theory In 1808, the English Chemist John Dalton proposed the first theory of the nature of matter in stating that all matter was composed of atoms.
Atoms: The Building Blocks of Matter Chapter 3 Pages
How to Use This Presentation
REVIEW GAME.
Atoms: The Building Blocks of Matter
Chapter 3 – Atoms: The Building Blocks of Matter
Atoms – The Building Blocks of EVERYTHING
Chapter 3 Objectives Explain what isotopes are.
Chapter 3 Table of Contents
Image Bank Chapter 3 Preview Law of Conservation of Mass
Chapter 3 Preview Multiple Choice Short Answer Extended Response
How to Use This Presentation
Presentation transcript:

Preview Multiple Choice Short Answer Extended Response Standardized Test Preparation Chapter 3

Standardized Test Preparation Multiple Choice 1.A chemical compound always has the same elements in the same proportions by mass regardless of the source of the compound. This is a statement of A.the law of multiple proportions. B.the law of isotopes. C.the law of definite proportions. D.the law of conservation of mass. Chapter 3

Standardized Test Preparation Multiple Choice 1.A chemical compound always has the same elements in the same proportions by mass regardless of the source of the compound. This is a statement of A.the law of multiple proportions. B.the law of isotopes. C.the law of definite proportions. D.the law of conservation of mass. Chapter 3

Standardized Test Preparation Multiple Choice Chapter 3 2.An important result of Rutherford’s experiments with gold foil was to establish that A.atoms have mass. B.electrons have a negative charge. C.neutrons are uncharged particles. D.the atom is mostly empty space.

Standardized Test Preparation Multiple Choice 2.An important result of Rutherford’s experiments with gold foil was to establish that A.atoms have mass. B.electrons have a negative charge. C.neutrons are uncharged particles. D.the atom is mostly empty space. Chapter 3

Standardized Test Preparation Multiple Choice 3.Which subatomic particle has a charge of +1? A.electron B.neutron C.proton D.meson Chapter 3

Standardized Test Preparation Multiple Choice 3.Which subatomic particle has a charge of +1? A.electron B.neutron C.proton D.meson Chapter 3

Standardized Test Preparation Multiple Choice 4.Which particle has the least mass? A.electron B.neutron C.proton D.All have the same mass. Chapter 3

Standardized Test Preparation Multiple Choice 4.Which particle has the least mass? A.electron B.neutron C.proton D.All have the same mass. Chapter 3

Standardized Test Preparation Multiple Choice Chapter 3 5. Cathode rays are composed of A.alpha particles. B.electrons. C.protons. D.neutrons.

Standardized Test Preparation Multiple Choice 5. Cathode rays are composed of A.alpha particles. B.electrons. C.protons. D.neutrons. Chapter 3

Standardized Test Preparation Multiple Choice 6.The atomic number of an element is the same as the number of A.protons. B.neutrons. C.protons + electrons. D.protons + neutrons. Chapter 3

Standardized Test Preparation Multiple Choice 6.The atomic number of an element is the same as the number of A.protons. B.neutrons. C.protons + electrons. D.protons + neutrons. Chapter 3

Standardized Test Preparation Multiple Choice 7.How many neutrons are present in an atom of tin that has an atomic number of 50 and a mass number of 119? A.50 B.69 C.119 D.169 Chapter 3

Standardized Test Preparation Multiple Choice 7.How many neutrons are present in an atom of tin that has an atomic number of 50 and a mass number of 119? A.50 B.69 C.119 D.169 Chapter 3

Standardized Test Preparation Short Answer 10. Which atom has more neutrons, potassium-40 or argon-40? Chapter 3

Standardized Test Preparation Short Answer 10. Which atom has more neutrons, potassium-40 or argon-40? Answer: Argon-40 has 22 neutrons (40 − 18 = 22), and potassium-40 has 21 neutrons (40 − 19 = 21). Chapter 3

Standardized Test Preparation Extended Response 12. Cathode rays emitted by a piece of silver and a piece of copper illustrate identical properties. What is the significance of this observation? Chapter 3

Standardized Test Preparation Extended Response 12. Cathode rays emitted by a piece of silver and a piece of copper illustrate identical properties. What is the significance of this observation? Answer: All cathode rays are the same, regardless of their source. Therefore, the particles responsible for the cathode rays must be present in all atoms. The particles are electrons. Chapter 3

Standardized Test Preparation Extended Response 13.A student believed that she had discovered a new element and named it mythium. Analysis found it contained two isotopes. The composition of the isotopes was 19.9% of atomic mass and 80.1% of atomic mass What is the average atomic mass, and do you think mythium was a new element? Chapter 3

Standardized Test Preparation Extended Response 13.A student believed that she had discovered a new element and named it mythium. Analysis found it contained two isotopes. The composition of the isotopes was 19.9% of atomic mass and 80.1% of atomic mass What is the average atomic mass, and do you think mythium was a new element? Answer: When the average atomic mass is calculated, it is Because the atomic mass is the same as the atomic mass of boron, mythium was not a new element. Chapter 3

Feedback: Privacy Policy Feedback
Do Not Sell My Personal Information
About project: SlidePlayer Terms of Service

© 2025 SlidePlayer.com. Inc. All rights reserved.