Intro to bonds
Type of bond where electrons are shared
Covalent Bond
Ability of an atom to attract e- in a bond
Electronegativity
another name for a covalent compound
a molecule
what gives the metallic appearance
Strong absorbers and reflectors of light
non-polar
Type of bond where electrons are transferred
Ionic Bond
Positively charged due to losing an electron
Cation
Type of bond when 4e- are shared
a double bond
Property that allows it to be made into thin sheets
malleable
A fluid’s resistance to movement
viscosity
A “bond”/chemical attraction formed from a shared pool of valence e-
Metallic bond
Negatively charged due to gaining an electron
anion
When there is a ΔEN then this type of covalent bond is formed because the electrons are shared unequally
Polar covalent bond
Typically a solution to two metals mixed together
Alloys
When a hydrogen atom bonded to a highly electronegative atom ( like N, O, or F ) is attracted to an unshared pair of e- of an electronegative atom in a nearby molecule
Hydrogen bonding
Forces between different substances
Intermolecular forces
This rule states that the charges of metal cations and nonmetal anions should result in the overall compound being neutral with no charge
The rule of zero
When 2 atoms of the same element exist naturally as a molecule
Diatomic elements
Name of electrons not associated with a single atom or bond
Delocalized electrons
An intermolecular attraction resulting from an instantaneous and temporary dipole created from the constant motion of e-
London dispersion forces
Forces within a substance
Intramolecular forces
Properties of Ionic compounds
Crystalline solids, High melting and boiling points, Can conduct electricity when dissolved in water
The theory that states the tendency for electron pairs to be as far apart from one another as possible
Valence Shell Electron Pair Repulsion (VSEPR) Theory
Combination of copper and tin
Bronze
The short-range attractive force between polar molecules
dipole-dipole forces