Periodic Trends and Bonding Flashcards
– solid is held together by the electrostatic attraction between cations and anions in a lattice structure
ionic
The bonds that hold all the ions together in the crystal lattice are the same as the bonds that hold – together
each pair of ions
Ionic bonds are strong and most ionic substances (like NaCl and other salts) are – at room temperature
solid
strength of bonds is primarily dependent on the – of ionic charges and to a lesser extent to the size of the ions according to Coulomb’s Law
magnitudes
The – the charge, the stronger the force of attraction between the ions
greater
The smaller the ions, the – they are attracted to each other
more
In a – solid, atoms are connected in a lattice of covalent bonds, meaning that all interactions between atoms are covalent bonds
network
Like in an ionic solid, in a network solid the intermolecular forces are identical to the – forces
intramolecular
Network solids are very strong and tend to be very – at room temperature (diamonds and quartz)
very hard
A sample of – can be thought of as a covalently bound lattice of nuclei and their inner shell electrons, surrounded by a “sea” or “cloud” of electrons
metal
In metallic solids, at least one valence electron per atom is not bound to any one particular atom and is free to move throughout the lattice. These free roaming valence electrons are called –
conduction electrons
Metals are excellent conductors of electricity and heat and are – and ductile
malleable
Metallic bonds vary widely in strength, but almost all metals are – at room temperature
solid
The particles at the lattice points of a crystal of a molecular solids are molecules held together by one of three types of intermolecular forces: hydrogen bonds, – forces or London dispersion forces
dipole-dipole
The forces of molecular compounds are significantly – than ionic, network or metallic bonds
weaker
molecular compounds typically have much – melting and boiling points than ionic, network, and metallic solids
lower
molecular solids are often – at room temperature and are more likely to be solids as the strength of their intermolecular forces increase
liquids or gases
relatively weak interactions that take place between neutral molecules
intermolecular forces
polar molecules are attracted to ions, producing – forces
ion-dipole
attractions between the positive end of one polar molecule and the negative end of another polar molecule
dipole-dipole forces
strongest dipole-dipole force
hydrogen bonds
a permanent dipoles in one molecule may induce a dipole in a neighboring nonpolar molecule, producing a momentary – force
dipole-induced dipole force
an instantaneous dipole in a nonpolar molecule may induce a dipole in a neighboring nonpolar molecule, resulting in a – force
London dispersion force
London dispersion forces are very weak and – interactions between instantaneous dipoles in non polar molecules
transient
All a molecule needs to experience the default London forces is – and the more – it has the greater the force
electrons
For nonpolar molecules, – is the only intermolecular force present
London dispersion forces
many substances whose molecules experience only dispersion forces are – at room temperature
gases
dipole forces, hydrogen bonding, and London forces area ll collectively known as –
van de Waals forces
substances with stronger intermolecular forces will exhibit greater melting points, boiling points, viscosities, and – vapor pressure than similar compounds with weaker intermolecular forces
lower
hydrogen bonds only occur between the H attached to an N, O, or F and a – on another N, O, or F atom
one pair
