02 - Atoms and Ions in the Periodic Table ADA Lecture
Page 1: Introduction
Atoms and Ions in the Periodic Table: Topic overview
Page 2: Daily Learning Goal
Objectives:
Understand Dalton’s Atomic Theory and its connection to the Law of Proportions and the Law of Conservation of Mass.
Learn about subatomic particles.
Explain average atomic mass based on relative abundance.
Identify and label features of the periodic table.
Classify elements as metals, non-metals, or metalloids related to their position on the periodic table.
Identify diatomic elements.
Page 3: Review Vocabulary
Key Terms:
Subatomic particle, Proton, Neutron, Electron, Atomic mass unit (amu or u), Ion, Cation, Anion, Atomic number (Z), Mass number (A), Atomic symbol, Isotopes, Atomic weight, Periodic Table, Alkali metals, Alkaline earth metals, Halogens, Noble gases.
Equation:
Atomic weight = Σ(mass)(% abundance)
Page 4: Dalton’s Atomic Theory
Core Principles:
Matter consists of indivisible and indestructible atoms.
All atoms of a specific element are identical.
Atoms of different elements have varying weights and chemical properties.
Atoms from different elements combine in simple whole-number ratios to form compounds.
Page 5: Law of Conservation of Mass
Definition: The total mass of reactants is equal to the mass of products in a chemical reaction.
Example: Reaction between silver nitrate (AgNO3) and sodium chloride (NaCl) produces a white precipitate with unchanged mass (300.23g).
Page 6: Law of Proportions (Proust's Law)
Principle: A chemical compound always contains fixed mass ratios of its constituent elements.
Ratios:
Example: C + O = 1:1 for 12 amu of C and 16 amu of O leading to a ratio of 12 amu to 32 amu for a 1:2 ratio for C:O.
Page 7: Situation Analysis
Questions:
Will the total mass of nitrogen (N) and oxygen (O) change during a reaction with no leaks?
Will the ratio of N to O atoms in N2O and N2O2 increase if the number of N atoms increases?
Conclusion: Conservation of matter holds, and the law of definite proportions dictates fixed atom ratios.
Page 8: Atomic Composition
Subatomic Particles:
Proton
Charge: +,
Atomic mass: 1 amu,
Location: In the nucleus.
Neutron
Charge: 0,
Atomic mass: 1 amu,
Location: In the nucleus.
Electron
Charge: -,
Atomic mass: approximately 0 amu,
Location: Outside the nucleus.
Page 9: Atoms and Ions
Ions:
Cations: Protons > electrons.
Anions: Electrons > protons.
Examples:
Lithium ion (Li+), Fluoride ion (F-), Fluorine (F), Lithium (Li).
Page 10: Atomic Symbols
Definitions of atomic symbol, atomic number (Z), and mass number (A).
Examples:
Fluorine, Lithium.
Page 11: Isotopes
Definition: Elements with differing neutrons affecting their stability.
Example: Carbon isotopes (12C and 14C) used in radiocarbon dating.
Page 12: Atomic Weight Calculation
Formula: Atomic weight = Σ(mass)(% abundance).
Example: For Chlorine:
75.78% as 35Cl and 24.22% as 37Cl, averaging to 35.48 amu.
Page 13: Situation Analysis
Problem: An unknown element has two isotopes with known masses and abundances.
Task: Calculate the average atomic weight and identify the element (Copper - Cu).
Page 14: Periodic Table Overview
Identification of groups and classifications within the Periodic Table, including metals, nonmetals, metalloids.
Page 15: Periodic Table Groups Identified
Groups:
Halogens, Noble Gases, Alkali Metals, Alkaline Earth Metals.
Transition Metals listed with corresponding symbols and atomic weights.
Page 16: Diatomic Elements
Elements:
H2, O2, Br2, N2, Cl2, F2, I2.
Characteristics: These elements do not exist as single atoms in nature.
Page 17: Studying Strontium
Characteristics of strontium:
Atomic Symbol: 38Sr or 87Sr.
Properties: Solid, metallic, conducts electricity.
Group: 2A, Alkaline Earth Metal.
Page 18: Daily Learning Goal
Objectives:
Determine charges of various ions and naming conventions for inorganic compounds, acids, bases, and salts.
Write covalent compound chemical formulas and names.
Page 19: Review Vocabulary
Key terms include:
Covalent compounds, Structural formula, Condensed structural formula, Inorganic acids, Monoatomic and Polyatomic ions.
Page 20: Predicting Ionic Charges
Cations: List of charges for monoatomic ions across groups.
Anions: Corresponding ionic charges for ions, exemplifying systematic trends.
Page 21: Naming Ions
Monoatomic Ions (Cations):
Group A metals named typically as "element name + ion".
Group B metals include the charge in roman numerals.
Anions: Named by changing the suffix to “ide” plus “ion”.
Page 22: Polyatomic Ions Naming
Cations: Suffix “ium” added.
Anions: Use “ide” for diatomic ions and “ate/ite” for those with oxygen.
Page 23: Nomenclature for Ionic Compounds
Naming: Combine cation and anion names.
Fomulas: Determine chemical names from formulas without prefixes.
Page 24: Conductivity of Ionic Compounds
Task: Determine formulas for lithium chloride, potassium nitrate, rubidium sulfate, and potassium phosphate.
Higher Conductivity: Potassium phosphate (K3PO4) expected to have the highest meter reading.
Page 25: Naming Inorganic Acids
Monoatomic Acids: Naming involves changing hydrogen to hydro, dropping "ine", adding