Unit 3: Ioinic bonding and Lewis Structures
Big Idea: Lower energy state = stronger interactions.
Chemistry: Atoms First (OpenStax)
Sequence - Part 1:
Sequence - Part 2:
Learning Targets - Part 1:
Learning Targets - Part 2:
Vocabulary - Part 1:
Vocabulary Part 2:
Chemistry: Atoms First (OpenStax)
- Chapter 3 sections 1-7
- Chapter 4 sections 4-6
Sequence - Part 1:
- Homework - here
- Valence electrons - slides
- Ionic state - activity
- Ionic compounds - Slides - activity
- Periodic trends: Size, Ionization energy and Electronegativity - here
- Lewis structures of Ions - slides
- Metals
Sequence - Part 2:
- Homework - here
- Covalent compounds intro - simulation
- Lewis structures for covalent compounds - practice and steps
- Molecular Geometry - simulation
- Exceptions to the rules for Lewis structures and resonance
- Polarity
- Intra molecular forces
Learning Targets - Part 1:
- Be able to name columns in the periodic table
- Be able to identify valence electrons from the periodic table
- Be able to predict relative atomic radius of atoms
- Be able to predict relative ionization energy of atoms
- Be able to predict relative electronegativity of atoms
- Be able to predict ionic state of an atom
- Be able to draw electron dot structures of atoms and ions
- Be able to predict the chemical formula of ionic compounds
- Be able to describe metallic bonding
Learning Targets - Part 2:
- Be able to define covalent compounds and interpret information from a molecular formula
- Be able to explain the result of electron sharing in covalent bonds
- Be able to draw lewis structures for covalent compounds and polyatomic ions
- Be able to identify some exceptions to the octet rule
- Be able to explain how the strength of a covalent bond is related to its bond dissociation energy
- Be able to draw resonance structures and describe how they are used
- Be able to describe relationship between atomic and molecular orbitals
- Be able to use the VSEPR theory to predict the shape of a molecule (Linear, Bent, Trigonal planar, trigonal pyramidal, tetrahedral)
- Be able to predict polarity of a bond and polarity of a molecule
- Be able to describe how electronegativity values determine the charge distribution in a polar molecule
- Be able to evaluate the strengths of inter-molecular interactions compared with the strengths of ionic and covalent interactions
Vocabulary - Part 1:
- Metals, Non-metals, Metalloid
- Alkali metals, Alkaline earth metals, Halogens, Noble gases, Transition metals
- Atomic radius
- Cation
- Anion
- Ionization energy
- Electronegativity
- Valence electron
- Electron dot structures
- Octet rule
- Halide ion
- Ionic compound, Ionic bond
- Chemical formula
- Formula unit
- Coordination number
- Metallic bonds
- Alloy
Vocabulary Part 2:
- Covalent bond
- Covalent molecule
- Molecular compound
- Molecular formula
- Single covalent bond
- Structural formula
- Unshared pair
- Double covalent bond
- Triple covalent bond
- Coordinate covalent bond
- Polyatomic ion
- Bond dissociation energy
- Resonance structure
- Molecular orbital
- Bonding orbital
- Sigma bond
- Pi bond
- Tetrahedral angle
- VSEPR theory
- Hybridization
- Nonpolar covalent bond
- Polar covalent bond
- Polar molecule
- Dipole
- Van Der Walls forces
- Dipole interaction
- Dispersion force
- Hydrogen bond
- Network solid
Key Objectives:
Part I - Trends and Ions
Part II - Covalent compounds
Chemistry - Wilbraham et al (Pearson 2012)
Chapters:
6,7,8
Good Problems to Master:
6:26,29,37,39,40,41,44,45,52,54,59,62,64,67,99
7:29,32,36,39,44,45,48,50,60,64,65,77,82,103
8:39,40,43,44,45,46,47,49,51,52,53,56,57,58,60,61,64,65,67,68,70,72,73,74,75,77,79,85,89,103,114
Part I - Trends and Ions
Part II - Covalent compounds
Chemistry - Wilbraham et al (Pearson 2012)
Chapters:
6,7,8
Good Problems to Master:
6:26,29,37,39,40,41,44,45,52,54,59,62,64,67,99
7:29,32,36,39,44,45,48,50,60,64,65,77,82,103
8:39,40,43,44,45,46,47,49,51,52,53,56,57,58,60,61,64,65,67,68,70,72,73,74,75,77,79,85,89,103,114