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AP* Chapter 2 Atoms, Molecules, and Ions AP Learning Objectives LO 1.1 The student can justify the observation that the ratio of the masses of the constituent elements in any pure sample of that compound is always identical on the basis of the atomic molecular theory. (Sec 2.2) LO 1.17 The student is able to express the law of conservation of mass quantitatively and qualitatively using symbolic representations and particulate drawings. (Sec 2.2, 2.3) LO 2.17 The student can predict the type of bonding present between two atoms in a binary compound based on position in the periodic table and the electronegativity of the elements. (Sec 2.6, 2.7) LO 3.5 The student is able to design a plan in order to collect data on the synthesis or decomposition of a compound to confirm the conservation of matter and the law of definite proportions. (Sec 2.2) LO 3.6 The student is able to use data from synthesis or decomposition of a compound to confirm the conservation of matter and the law of definite proportions. (Sec 2.2) Section 2.2 Fundamental Chemical Laws AP Learning Objectives, Margin Notes and References Learning Objectives LO 1.1 The student can justify the observation that the ratio of the masses of the constituent elements in any pure sample of that compound is always identical on the basis of the atomic molecular theory. LO 1.17 The student is able to express the law of conservation of mass quantitatively and qualitatively using symbolic representations and particulate drawings. Additional AP References LO 3.5 (see APEC Lab 7, " Hydrates and Thermal Decomposition") LO 3.6 (see APEC Lab 7, " Hydrates and Thermal Decomposition") Section 2.2 Fundamental Chemical Laws Three Important Laws Law of conservation of mass (Lavoisier): Mass is neither created nor destroyed in a chemical reaction. Law of definite proportion (Proust): A given compound always contains exactly the same proportion of elements by mass. 4 Section 2.2 Fundamental Chemical Laws Three Important Laws (continued) 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. 5 Section 2.3 Dalton’s Atomic Theory AP Learning Objectives, Margin Notes and References Learning Objectives LO 1.17 The student is able to express the law of conservation of mass quantitatively and qualitatively using symbolic representations and particulate drawings. Section 2.3 Dalton’s Atomic Theory Dalton’s Atomic Theory (1808) Each element is made up of tiny particles called atoms. 7 Section 2.3 Dalton’s Atomic Theory Dalton’s Atomic Theory (continued) The atoms of a given element are identical; the atoms of different elements are different in some fundamental way or ways. 8 Section 2.3 Dalton’s Atomic Theory Dalton’s Atomic Theory (continued) 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. 9 Section 2.3 Dalton’s Atomic Theory Dalton’s Atomic Theory (continued) 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. 10 Section 2.3 Dalton’s Atomic Theory Gay-Lussac and Avogadro (1809—1811) Gay—Lussac Measured (under same conditions of T and P) the volumes of gases that reacted with each other. Avogadro’s Hypothesis At the same T and P, equal volumes of different gases contain the same number of particles. Volume of a gas is determined by the number, not the size, of molecules. 11 Section 2.3 Dalton’s Atomic Theory Representing Gay—Lussac’s Results 12 Section 2.3 Dalton’s Atomic Theory Representing Gay—Lussac’s Results 13 Section 2.3 Dalton’s Atomic Theory Representing Gay—Lussac’s Results 14 Section 2.3 Dalton’s Atomic Theory Representing Gay—Lussac’s Results 15 Section 2.6 Molecules and Ions AP Learning Objectives, Margin Notes and References Learning Objectives LO 2.17 The student can predict the type of bonding present between two atoms in a binary compound based on position in the periodic table and the electronegativity of the elements. Section 2.6 Molecules and Ions Chemical Bonds Covalent Bonds Bonds form between atoms by sharing electrons. Resulting collection of atoms is called a molecule. 17 Section 2.6 Molecules and Ions Covalent Bonding To play movie you must be in Slide Show Mode PC Users: Please wait for content to load, then click to play Mac Users: CLICK HERE 18 Section 2.6 Molecules and Ions Chemical Bonds Ionic Bonds Bonds form due to force of attraction between oppositely charged ions. Ion – atom or group of atoms that has a net positive or negative charge. Cation – positive ion; lost electron(s). Anion – negative ion; gained electron(s). 19 Section 2.6 Molecules and Ions Molecular vs Ionic Compounds To play movie you must be in Slide Show Mode PC Users: Please wait for content to load, then click to play Mac Users: CLICK HERE 20 Section 2.6 Molecules and Ions EXERCISE! A certain isotope X+ contains 54 electrons and 78 neutrons. What is the mass number of this isotope? 133 21 Section 2.6 Molecules and Ions 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. 22 Section 2.7 An Introduction to the Periodic Table AP Learning Objectives, Margin Notes and References Learning Objectives LO 2.17 The student can predict the type of bonding present between two atoms in a binary compound based on position in the periodic table and the electronegativity of the elements. Section 2.7 An Introduction to the Periodic Table The Periodic Table Metals vs. Nonmetals Groups or Families – elements in the same vertical columns; have similar chemical properties Periods – horizontal rows of elements 24 Section 2.7 An Introduction to the Periodic Table The Periodic Table Section 2.7 An Introduction to the Periodic Table Groups or Families Table of common charges formed when creating ionic compounds. Group or Family Charge Alkali Metals (1A) 1+ Alkaline Earth Metals (2A) 2+ Halogens (7A) 1– Noble Gases (8A) 0 26