Module 2, Topic 4 - Bonding & Structure Flashcards
Define “ionic bonding”
The electrostatic attraction between positive and negative ions
Define “covalent bonding”
The strong electrostatic attraction between a shared pair of electrons and nuclei of the bonded atoms
What is meant by a “dative” covalent bond?
Where 1 atom contributes both electrons needed for the bond to form
Define “electronegativity”
The ability of an atom to attract a pair of electrons in a covalent bond
Define “London forces”
The weakest intermolecular forces. They form between non-polar (molecules with different types of atoms) molecules as electrons become attracted to each other.
What is meant by “permanent dipole - dipole attraction”?
Forms between 2 polar covalent molecules. Forces of attraction between opposite charges on neighboring molecules.
What is meant by “hydrogen bonding”?
Strong forces of attraction formed between Hydrogen and Fluorine/Oxygen/Nitrogen
They are 100x stronger than London forces
What is the bond angle in a tetrahedral molecule?
The bond angle in a tetrahedral molecule is approximately 109.5 degrees.
Fill in the blank: Molecules with two bonding pairs and no lone pairs have a _____ shape.
linear
Which shape corresponds to a bond angle of about 120 degrees?
Trigonal planar
What is the molecular shape of a molecule with four bonding pairs and one lone pair?
Trigonal bipyramidal
Multiple Choice: What is the bond angle in a pyramidal molecule with two bonding pairs and one lone pair? A) 120 degrees B) 109.5 degrees C) 104.5 degrees
C) 104.5 degrees
What is the shape and bond angle of a molecule with 2 bonded pairs and 0 lone pairs?
Linear and 180°
True or False: Lone pairs of electrons occupy more space than bonding pairs.
True
What is the bond angle in an octahedral molecule?
The bond angle in an octahedral molecule is 90 degrees.
