1. Chapter 2 Atoms, Molecules, and Ions

2. Section 2.2 Fundamental Chemical Laws Return to TOC Copyright © Cengage Learning. All rights reserved 2 Law of conservation of mass (Lavoisier):  Mass is neither created nor destroyed. Law of definite proportion (Proust):  A given compound always contains exactly the same proportion of elements by mass. Three Important Laws

3. Section 2.2 Fundamental Chemical Laws Return to TOC Copyright © Cengage Learning. All rights reserved 3 Law of multiple proportions (Dalton):  When two elements form a series of compounds, the ratios of the masses of the second element that combine with 1 gram of the first element can always be reduced to small whole numbers. Three Important Laws (continued)

4. Section 2.3 Dalton’s Atomic Theory Return to TOC Copyright © Cengage Learning. All rights reserved 4 Each element is made up of tiny particles called atoms. Dalton’s Atomic Theory (1808) The atoms of a given element are identical; the atoms of different elements are different in some fundamental way or ways.

5. Section 2.3 Dalton’s Atomic Theory Return to TOC Copyright © Cengage Learning. All rights reserved 5 Chemical compounds are formed when atoms of different elements combine with each other. A given compound always has the same relative numbers and types of atoms. Dalton’s Atomic Theory (continued)

6. Section 2.3 Dalton’s Atomic Theory Return to TOC Copyright © Cengage Learning. All rights reserved 6 Chemical reactions involve reorganization of the atoms—changes in the way they are bound together. The atoms themselves are not changed in a chemical reaction. Dalton’s Atomic Theory (continued)

7. Section 2.3 Dalton’s Atomic Theory Return to TOC Copyright © Cengage Learning. All rights reserved 7 Concept Check Which of the following statements regarding Dalton’s atomic theory are still believed to be true? I. Elements are made of tiny particles called atoms. II. All atoms of a given element are identical. III. A given compound always has the same relative numbers and types of atoms. IV. Atoms are indestructible.

8. Section 2.3 Dalton’s Atomic Theory Return to TOC Copyright © Cengage Learning. All rights reserved 8 Avogadro’s Hypothesis  At the same T and P, equal volumes of different gases contain the same number of particles.

9. Section 2.3 Dalton’s Atomic Theory Return to TOC Copyright © Cengage Learning. All rights reserved 9 Gay—Lussac  Measured (under same conditions of T and P) the volumes of gases that reacted with each other.

10. Section 2.3 Dalton’s Atomic Theory Return to TOC Copyright © Cengage Learning. All rights reserved 10 Representing Gay—Lussac’s Results

11. Section 2.5 The Modern View of Atomic Structure: An Introduction Return to TOC Copyright © Cengage Learning. All rights reserved 11 The atom contains:  Electrons – found outside the nucleus; negatively charged.  Protons – found in the nucleus; positive charge equal in magnitude to the electron’s negative charge.  Neutrons – found in the nucleus; no charge; virtually same mass as a proton.

12. Section 2.5 The Modern View of Atomic Structure: An Introduction Return to TOC Copyright © Cengage Learning. All rights reserved 12 The nucleus is:  Small compared with the overall size of the atom.  Extremely dense; accounts for almost all of the atom’s mass.

13. Section 2.5 The Modern View of Atomic Structure: An Introduction Return to TOC Copyright © Cengage Learning. All rights reserved 13 Nuclear Atom Viewed in Cross Section

14. Section 2.5 The Modern View of Atomic Structure: An Introduction Return to TOC Copyright © Cengage Learning. All rights reserved 14 Atoms with the same number of protons but different numbers of neutrons. Show almost identical chemical properties; chemistry of atom is due to its electrons. In nature most elements contain mixtures of isotopes. Isotopes

15. Section 2.5 The Modern View of Atomic Structure: An Introduction Return to TOC Copyright © Cengage Learning. All rights reserved 15 Two Isotopes of Sodium

16. Section 2.5 The Modern View of Atomic Structure: An Introduction Return to TOC Element Symbol Atomic Number = number of protons Mass Number = number of protons + neutrons (mass numbers are always whole numbers, different from average atomic mass!) Copyright © Cengage Learning. All rights reserved 16

17. Section 2.5 The Modern View of Atomic Structure: An Introduction Return to TOC Copyright © Cengage Learning. All rights reserved 17 Exercise A certain isotope X contains 23 protons and 28 neutrons. What is the mass number of this isotope? Identify the element. Mass Number = 51 Vanadium

18. Section 2.6 Molecules and Ions Return to TOC Copyright © Cengage Learning. All rights reserved 18 Exercise A certain isotope X + contains 54 electrons and 78 neutrons. What is the mass number of this isotope? 133

19. Section 2.6 Molecules and Ions Return to TOC Copyright © Cengage Learning. All rights reserved 19

20. Section 2.6 Molecules and Ions Return to TOC Copyright © Cengage Learning. All rights reserved 20

21. Section 2.7 An Introduction to the Periodic Table Return to TOC Copyright © Cengage Learning. All rights reserved 21 Metals vs. Nonmetals Groups or Families – elements in the same vertical columns; have similar chemical properties Periods – horizontal rows of elements The Periodic Table

22. Section 2.7 An Introduction to the Periodic Table Return to TOC Copyright © Cengage Learning. All rights reserved 22 The Periodic Table

23. Section 2.7 An Introduction to the Periodic Table Return to TOC Copyright © Cengage Learning. All rights reserved 23 Table of common charges formed when creating ionic compounds. Groups or Families Group or FamilyCharge Alkali Metals (1A)1+ Alkaline Earth Metals (2A) 2+ Halogens (7A)1– Noble Gases (8A)0

24. Section 2.7 An Introduction to the Periodic Table Return to TOC Chapter 2 Homework P 70 # 33, 34, 47a, 49, 51, 53, 55, 59, 61 –Due: Copyright © Cengage Learning. All rights reserved 24