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Chapter 4 Atomic Structure 4.1 Defining the Atom

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1 Chapter 4 Atomic Structure 4.1 Defining the Atom
4.2 Structure of the Nuclear Atom 4.3 Distinguishing Among Atoms Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

2 Early Models of the Atom
Do Now: Draw a picture of what you think an atom looks like. Write down what you know about atoms. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

3 Early Models of the Atom
Atom: smallest particle of an element that retains its identity in a chemical reaction. Atomos – Greek word for indivisible Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

4 Sizing up the Atom Atoms are very small. A copper coin the size of a penny contains about 2.4  1022 atoms. 24,000,000,000,000,000,000,000 atoms! Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

5 Key Concepts If an atom were the size of a football stadium, the nucleus would be the size of a marble Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

6 Atoms contain 3 types of subatomic particle
Key Concepts Atoms contain 3 types of subatomic particle Subatomic Particle Symbol Charge Location Proton p+ +1 nucleus Neutron n0 Electron e- -1 surrounding nucleus Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

7 Mass of Subatomic Particles Relative mass (mass of proton = 1)
Interpret Data Mass of Subatomic Particles Particle Relative mass (mass of proton = 1) Actual mass (g) Proton 1 amu 1.67  10–24 Neutron Electron 1/1840 amu 9.11  10–28 Atomic Mass Unit: 1/12 of the mass of a Carbon-12 atom Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

8 It’s like an ID number for an element
Atomic Number Atomic Number: number of protons in the nucleus of an atom of that element It’s like an ID number for an element

9 Mass Number Mass Number: total number of protons and neutrons in an atom Hyphenated notation: Helium-4

10 Atoms If you know the atomic number and mass number, you can determine the atom’s composition. # Protons = Atomic Number # Electrons = # Protons # Neutrons = Mass Number – Atomic Number

11 Determining the Composition of an Atom
Sample Problem 4.2 Determining the Composition of an Atom How many protons, electrons, and neutrons are in each atom? a. Be b. Ne c. Na 9 4 20 10 23 11 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

12 Determining the Composition of an Atom
Sample Problem 4.2 Determining the Composition of an Atom How many protons, electrons, and neutrons are in each atom? Protons: Neutrons: Electrons: a. Be b. Ne c. Na 9 4 20 10 23 11 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

13 Isotopes Isotopes: atoms that have the same number of protons but different numbers of neutrons. Neon-20, neon-21, and neon-22 are three isotopes of neon. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

14 Hydrogen has 3 isotopes The correct way to represent an isotope is to write the chemical name followed by the mass number (protons + neutrons)

15 Hydrogen has 3 isotopes 1 1 1 1 1 1 2 1

16 Most elements occur as a mixture of two or more isotopes.
Atomic Mass Most elements occur as a mixture of two or more isotopes. Each isotope of an element has a fixed mass and a natural percent abundance. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

17 How many protons, electrons, and neutrons are in each atom?
Do Now: How many protons, electrons, and neutrons are in each atom? Protons: Neutrons: Electrons: a. F b. Ti c. Ca 19 9 48 22 40 20 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

18 How many protons, electrons, and neutrons are in each atom?
Do Now: How many protons, electrons, and neutrons are in each atom? Protons: Neutrons: Electrons: a. F b. Ti c. Ca 19 9 48 22 40 20 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

19 If a student’s grade is weighted per the table below, what would their grade be?
Average Tests 50% 79 Classwork 30% 95 Homework 20% 85

20 Atomic Mass Atomic mass - weighted average mass of atoms in a naturally occurring sample of the element. reflects both mass and relative abundance of the isotopes Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

21 Interpret Data Natural Percent Abundance of
Stable Isotopes of Some Elements Name Symbol Natural percent abundance Mass (amu) Atomic mass Hydrogen H 99.985 0.015 negligible 1.0078 2.0141 3.0160 1.0079 Helium He 0.0001 4.0026 Carbon C 98.89 1.11 12.000 13.003 12.011 Oxygen O 99.759 0.037 0.204 15.995 16.995 17.999 15.999 Chlorine Cl 75.77 24.23 34.969 36.966 35.453 35 17 37 1 2 3 12 6 13 4 18 8 16 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

22 Atomic Mass To calculate atomic mass, multiply the mass of each isotope by its natural abundance, expressed as a decimal, and then add the products. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

23 Calculating Average Atomic Mass
Chlorine-35 has an amu of with an abundance of % while Chlorine-37 has an amu of and an abundance of %. What is the average atomic mass of chlorine? Carbon-12 (12.00 amu) makes up 98.93% of all of the carbon atoms, while carbon-13 ( amu) is about 1.07% abundant. What is the average atomic mass of carbon?

24 Calculating Average Atomic Mass
Chlorine-35 has an amu of with an abundance of % while Chlorine-37 has an amu of and an abundance of %. What is the average atomic mass of chlorine? Carbon-12 (12.00 amu) makes up 98.93% of all of the carbon atoms, while carbon-13 ( amu) is about 1.07% abundant. What is the average atomic mass of carbon?

25 Radioactivity: release of energy & matter that results from changes in the nucleus of an atom
All elements with an atomic number greater than 83 are radioisotopes (unstable nucleii) Elements with atomic numbers less than or equal to 83 have isotopes with stable nucleii and may have a radioactive isotope

26 END OF CHAPTER 4 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

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