Bonding Flashcards
Monoatomic Molecules
Elements that show no tendency to combine with either atoms or other elements
Noble Gases
Stable Octet
The arrangement of 2 s electrons & 6 p electrons in valence energy level
Noble Gases
Ionic Bond
When ions are stuck together by electrostatic attraction
Electronegativity differ by 1.7 or more
Conduct electric currents
Covalent bond
Sharing of electrons so that atoms can fill their outer shells
Nonpolar Covalent Bond
When Electronegativity difference between 2/more atoms is between 0 & 0.4
Tend to share valence electrons in their outer energy levels
Polar covalent bond
Unequal sharing of electrons between atoms
Electronegativity differences between 0.4 & 1.6
Metallic Bond
Positive ions in a “sea” of electrons
The strong attraction between these differently charged particles
Intermolecular Forces
Attractions between molecules
Johannes van dee Waals
VSEPR
Valence shell electron pair repulsion
Assumes that each atom in a molecule will achieve a geometry that minimise the repulsion between electrons in valence shell of atom
Hybridisation
The combinations of more than 2 orbitals to form new orbitals
Number of new hybrid orbitals must be = to number of atoms & non-bonded electron pairs surrounding the central atom
Linear Arrangement
Mutual repulsion of 2 electron clouds
Forces them to opposite sides of a sphere
Trigonal-Planar arrangement
Minimum repulsion between 3 electron pairs occurs when pairs are at vertices if an equilateral triangle inscribed in a sphere
Tetrahedral Arrangement
4 electron pairs are farthest apart at the vertices if a tetrahedron inscribed in a sphere
Octahedral Arrangement
Mutual repulsion of 6 identical electron clouds directs them to the corners of an inscribed octahedron
Sigma Bond
A bond between s orbitals or between a s orbital & another kind of orbital
Pi Bond
A bond between p orbitals;
When 2 p orbitals share electrons in a covalent bond & the interaction is not symmetrical about a line between the 2 nuclei
Molecule
The smallest particle of an element/compound that retains the characteristics of the original substance
Dipole Molecule
Unequal sharing of electrons, molecule has 2 distinct ends from a charge perspective
van der Waals forces
All intermolecular forces = attractions BETWEEN molecules
London Dispersion Force
Attractions between molecules by temporary dipoles
Dipole-dipole Attraction
Weak electrostatic forces of attraction between polar molecules due to partial charges on these molecules
Hydrogen Bonding
Hydrogen atoms form weak bonds with lone pair of electrons of other molecule, F, N, O
Double Bond
Produced by sharing two pairs of electrons
Triple Bond
Produced by sharing 3 pairs of electrons
Molecular Geometry
3D arrangement of the molecule’s atoms in space
VSEPR Unshared
Lone pairs occupy space around central atom but actual shape of molecule is determined by the positions of the atoms
