Topic 4 - Bonding & Structure Flashcards
You gotta pass this test, no other option really
Hybridization
The process of mixing atomic orbitals to form new hybrid orbitals that can be used for bonding in molecules
Sigma Bonds
The overlapping of hybrid orbitals across the axis.
sp Hybridization
1 s orbital and 1 p orbital mix to form 2 equivalent sp hybrid orbitals, typically seen in linear molecules (2 bonding sites).
sp2 Hybridization
1 s orbital and 2 p orbitals resulting in 3 sp2 hybrid orbitals, commonly found in trigonal planar structures (3 bonding sites).
sp3 Hybridization
1 s orbital and 3 p orbitals combine to form 4 equivalent sp3 hybrid orbitals, characteristic of tetrahedral geometry (4 bonding sites).
dsp3 Hybridization
1 s orbital and 3 p orbital and 1 d orbital resulting in 5 dsp3 orbitals, found in trigonal bipyramidal structures (5 bonding sites).
d2sp3 Hybridization
1 s orbital and 3 p orbitals and 2 d orbitals combine to form 6 equivalent d2sp3 hybrid orbitals, found in octahedral structures (6 bonding sites).
Orbital Mixing
atomic orbitals combine to create new orbitals with different shapes and energies.
Tetrahedral Geometry
The central atom is bonded to 4 other atoms, bond angles of approximately 109.5 degrees, typical of sp3 hybridization.
Trigonal Planar Geometry
The central atom is bonded to 3 other atoms, with bond angles of 120 degrees, associated with sp2 hybridization.
Elements happy with an incomplete octet
Boron and Beryllium because they are electron deficient they react with molecules that have lone pairs of electrons like H2O + NH3, they are also Lewis Acids = electron seeking.
Resonance Structures
different ways of drawing the same molecule, showing the delocalization of electrons across multiple positions, which contributes to the overall stability of the molecule.
Lewis Structures
Diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist, helping to visualize the arrangement of electrons
Delocalized Electrons
electrons that are not associated with a single atom or bond but are spread over several atoms, contributing to the stability and reactivity of molecules.
Double Bond
Formed from the overlapping of a hybridized and overlapping of an unhybridized orbital. 4 electrons, 2 pairs
Bond length
distance between the nuclei of two bonded atoms, which can vary depending on the type of bond
Single > Double > Triple
Bond Strength
Refers to the energy required to break a bond between two atoms; stronger bonds have shorter lengths and higher bond orders
Metallic bonding
A type of chemical bonding that occurs between metal atoms, characterized by the sharing of free electrons among a lattice of cations
Delocalized Electrons contribute to characteristics such as..
Malleability, Ductility, Conductivity of heat and energy, shine/luster
Cation Size/# of delocalized Electrons contribute to….
The smaller the cation and as the number of delocalized Electrons increases, the stronger the metallic bond.
Mg+2 is stronger than Na+ because it is smaller and has more delocalized electrons
Transition metals
Found in the d-block of the periods. Greater delocalization of electrons and stronger metallic bonding.
Strength of Metallic bonds
Increases with the number of delocalized electrons and size of cations; smaller cations and more delocalized electrons increase bond strength.
Pi orbitals
The overlapping of unhybrid orbitals above and below the axis.
Triple bonds
formed from the overlapping of hybridized and two unhybridized orbitals
Stronger IMFs result in…
Higher Boiling and Melting Points
Dipole-Dipole
Polar molecules only
LDFs
All molecules. Weakest IMF
Electrostatic
forces of attraction between charge particles
Hydrogen Bonding
H bonded to F, O, N. Strongest IMF
Cation
Positively Charged ion
Anion
Negatively Charged ion
Alloy
A homogenous mixture of metals. Solid Solution. Two types; Substitutional and Interstitial.
Substitutional Alloy
The added atoms are similar in size to the original metals atoms and replace some of the original metal atoms.
Brass is a Substitutional Alloy of copper and zinc
Interstitial Alloy
The added atoms are smaller than the original metal atoms and fits into the spaces between metal atoms.
Steel is an electrical alloy of Iron and Carbon.
Allotrope
A different form of an element in the same physical state with different bonding within the structure.
Solubility
Like dissolves Like.
Polar dissolves Polar.
Non polar dissolves Non polar.
Non Polar and Polar do not mix.
Conductivity of covalent compounds
Covalent bonds do not conduct due to no mobile ions and electrons are fixed.