Chemistry Daily 10’s Week 3.

Slides:

Advertisements

Similar presentations

Atomic Theory Timeline

Advertisements

Have 1 Periodic Table per group!.  The mass number.

Atomic Theory History of Atom Early Greeks believed that matter consisted of tiny particles – they called the “atoms”

CHEMISTRY 161 Chapter The Early Atomic Theory pure substances compounds elements combine different elements H 2, O 2 H 2 O [O 3 ] John Dalton.

» What is the name of this device? » Which scientist used this device?

Atoms, Ions and the Periodic Table Chemistry 131 Chapter 2.

The Law of Conservation of Mass

Atomic Mass and the Mole. Relative Atomic Mass Units of grams are TOO LARGE for atoms! Relative atomic mass – compare to small particles – amu – “atomic.

Basic concepts for general chemistry Lec.2. Important definitions Element  Any substance that contains only one kind of an atom.  Each element is represented.

AIM: Models of the Atom DO NOW:

Chapter 3 Atoms. People have been thinking about the nature of matter for a long time. The ancient Greeks thought about matter and it wasn’t until the.

Unit 3 Language of Chemistry Part 1 Zumdahl: Chapter 4 Holt: Chapter 3.

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.

Atoms The Basics… or Part I CHM 1010 PGCC Barbara A. Gage.

Atomic Theory History of Atom Early Greeks believed that matter consisted of tiny particles – they called the “atoms”

Chapter 3 Atoms and Atomic Structure Write the bullets that are in black font.

AP Chemistry – Chapter 2 Atoms, Molecules and Ions.

Early Theories & Subatomic Particles ( )

History of the Atomic Theory. Law of Definite Proportions A given compound contains the same elements in exactly the same proportions by mass, regardless.

Atoms: The Building Blocks Of Matter

Midterm Review Chapter 3 Pg Atomic Theory pg  Atomic Theory – the idea that atoms are the building blocks of all matter  Everything is.

Video 3-1 Foundations of Atomic Theory Development of Atomic Models Forces in the Nucleus.

Atomic Theory and Structure Unit 2. Atomic Theory Based on experimental data Elements are made of only one kind of particle. This basic particle is called.

Weighing and Counting Atoms

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.

By: Andres Sanchez. Law Of Definite Proportions  Law of definite proportions states that two samples of a give compound are made of the same elements.

DALTON’S ATOMIC THEORY 1803 Read each of the following postulates and determine whether each is True or False.

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.

1.3 Atomic Theory 1. John Dalton’s atomic theory - Matter is made up of small particles called atoms - Atoms cannot be created, destroyed or divided.

Chapter 3 pages Modern Chemistry Chapter 3 Atoms: the building block of matter.

History of Atom Flip Book

Atoms and Moles – Chapter 3 Substances are made of atoms 3.1.

The Atom Chapter 3. From Idea to Theory Democritus, Greek philosopher, 400 B.C., introduced the concept of an atom, an ‘indivisible’ particle. Democritus,

Atom : The smallest particle of an element that keeps all the properties of that element. Lesson: Old Dead Guys.

Development of the atomic theory. Important laws Law of conservation of mass – Mass is neither created or destroyed during ordinary chemical reactions.

Ch. 3: Atoms 3.1 Foundations. History  Democritus named the most basic particle named the most basic particle atom- means “indivisible atom- means “indivisible.

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.

ATOMS: The Building Blocks of Matter Objectives 1.Law of conservation of mass 2.Law of definite proportions 3.Law of multiple proportions 4.Dalton’s Atomic.

MODERN CHEMISTRY CH 3 Atoms: The Building Blocks of Matter.

Chapter 3 Atoms: The Building Blocks of Matter. Sect. 3-1: The Atom: From Philosophical Idea to Scientific Theory  Democritus vs. Aristotle  Atom vs.

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.

Atoms, Molecules and Ions Chapter 2 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

Unit 3.  smallest particle of an element that can exist alone or in combinations with other atoms.

Chapter 3 Atoms and matter. laws The transformation of a substance or substances into one or more new substances is known as a chemical reaction. Law.

Atoms, Molecules and Ions Chapter 3. Dalton’s Atomic Theory (1808) 1. Elements are composed of extremely small particles called atoms. All atoms of a.

Dalton’s Atomic Theory. Law of Conservation of Mass The total mass of materials after a chemical reaction is the same as the total mass before the reaction.

Chemistry What is chemistry? –Chemistry is the study of matter, what it is made of, and how it changes. What is matter? –Matter is anything that… Has.

The Atom, Periodic Table, and Chemical Reactions Mrs. Hooks Unit 3.

Chapter 4. Atom Smallest particle of an element that retains its chemical identity Atoms of the same element cannot be separated chemically because they.

The Atom CHAPTER 3.1 MS. COX’S CHEMISTRY CLASS. Lesson Objectives Explain the law of conservation of mass, the law of multiple proportions and the law.

Chapter 3 Atoms : The Building Blocks of Matter. Foundations of Atomic Theory  Several basic laws were after the 1790’s (emphasis on quantitative analysis):

Atomic Theory ScientistExperimentContributionAtomic Model Democritus (ca 400 BCE ) (thought)atomos = indivisible particle ‘grains of sand’

Ch. 3 – Atoms: The Building Blocks of Matter

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

Atomic Theory & Periodic Table Unit 3 Part 1 (Ch. 4 & 5) Atomic Theory Introduction, Isotopes.

Chapter 3 Atoms: The Building Blocks of Matter. Lesson 1.1: Early Atomic Theory Learning Target: I will understand the history and structure of the atom.

Atomic Structure.  Smallest particle of an element w/ properties of that element  About 90 natural elements  Combine to form compounds ◦ Atoms  elements.

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.

Chapter 3: Discovering the Atom and Subatomic Particles

Atomic Theory and the Atomic Model. Objectives Describe evidence that Greek philosophers used to develop the idea of atoms. Distinguish between a scientific.

Atoms: The building blocks of matter

Chapter 3 – Atoms: The Building Blocks of Matter

Atoms – The Building Blocks of EVERYTHING

Atoms, Molecules and Ions

Atoms, Molecules and Ions

Ch. 3 – Atoms: The Building Blocks of Matter

CH 3 Atoms: The Building Blocks of Matter 3

Presentation transcript:

Chemistry Daily 10’s Week 3

1 1. If each atom of element D has 3 mass units and each atom of element E has 5 mass units, a molecule composed of one atom each of D and E has A. 2 mass units. B. 8 mass units. C. 15 mass units. D. 35 mass units.

2. If 6.0 g of element K combine with 17 g of element L, how many grams of element K combine with 85 g of element L? a. 17 g b. 23 g c. 30. g d. 91 g

2 1. According to the law of definite proportions, any two samples of KCl have a. the same mass. b. slightly different molecular structures. c. The same melting point. d. the same ratio of elements.

2. According to the law of conservation of mass, when sodium, hydrogen, and oxygen react to form a compound, the mass of the compound is ____ the sum of the masses of the individual elements. a. equal to b. greater than c. less than d. either greater than or less than

3 1. The principles of atomic theory recognized today were conceived by a. Avogadro. b. Bohr. c. Dalton. d. Rutherford.

2. Which of the following is not part of Dalton's atomic theory? a. Atoms cannot be divided, created, or destroyed. b. The number of protons in an atom is its atomic number. c. In chemical reactions, atoms are combined, separated, or rearranged. d. All matter is composed of extremely small particles called atoms.

4. 1. Experiments with cathode rays led to the discovery of the a. proton. b. nucleus. c. neutron. d. electron.

2. In Rutherford's experiments, most of the particles a. bounced back. b. passed through the foil. c. were absorbed by the foil. d. combined with the foil.

5. 1. Protons within a nucleus are attracted to each other by a. the nuclear force. b. opposite charges. c. their energy levels. d. electron repulsion.

2. The smallest unit of an element that can exist either alone or in combination with other such particles of the same or different elements is the a. electron. b. proton. c. neutron. d. atom.

Answers & Standards 1.1 – b – sc2 sc3 1.2 - c – sc2 sc3 2.1 - d – sc2 sc3 2.2 - a – sc2 sc3 3.1 – c – sc3 3.2 - b – sc3 4.1 - d – sc3 4.2 - b – sc3 5.1 - a – sc3 5.2 - d – sc3