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.
As lone pairs are added, what happens to the bond angle?
It shrinks by 2.5°
