Bonding Flashcards
what is ionic bonding
strong electrostatic forces of attraction between oppositely charged ions
what are the properties of ionic bonds
conduct electricity when melted or in solution
high melting points
second strongest structure and bond
what is a covalent bond
shared pair of electrons
what is a covalent lattice
many strong covalent bonds (shared pair of electrons)
what is a dative covalent bond
shared pair of electrons with both electrons supplied by one atom
properties of covalent bonds
strongest structure and bond
don’t conduct electricity apart from graphite (has delocalised electrons and van der waals forces)
what are metallic bonds
strong electrostatic forces of attraction between delocalised electrons and positively charged ions.
properties of metallic bonds
conduct electricity
have high melting points
ductile and malleable
third strongest structure and bond
what do lone and bonding pairs do to each other
repel each other
lone pairs repel 2-2.5 degrees more than bp
name, drawing and bond angle with 2bp 0lp
name, drawing and bond angle with3bp 0lp
name, drawing and bond angle with4bp 0lp
name, drawing and bond angle with3bp 1lp
name, drawing and bond angle with2bp 2lp
name, drawing and bond angle with5bp 0lp
name, drawing and bond angle with6bp 0lp
name, drawing and bond angle with4bp 2lp
name, drawing and bond angle with 4bp 0lp (nickel, platinum and pallidium)
what is electronegativity
ability of an atom to attract a bonding pair of electrons in a covalent bond
what affects electronegativity
atomic radius and number of protons
what element is most electronegative
fluorine
what are polar bonds
bonds that have a permanent uneven distribution of electron density caused by a large difference in electronegativity
what causes symmetrical molecules
the electronegative elements pull in equal and opposite directions so cancel out
what does d- mean
negative charge
more electron density
more electronegative
what does d+ mean
positive charge
less electron density
less electronegative
what is hydrogen bonding
the electrostatic attraction in a hydrogen bond is between the lone pair on the N/O/F and the d+ hydrogen
is between molecules
* strongest intermolecular foce
what causes permanent dipole-dipole forces
large differnce in electronegativity between two elements in a covalent bond
* second strongest intermolecular force
what bond does permanent dipole-dipole forces create
polar bonds where one of the elements usually N/O/F/Cl id d- as they are more electronegative and the less electronegative element is d+
what are van der waal forces and how are the caused
caused by a random movement of electrons causing a temporary dipole in that molecule (with a d- and d+)
the partial charge causes electron density to be attracted/repelled in other nearby molecules which induces a dipole
properties of vdw forces
weakest intermolecular forces
larger the surface area the stronger the intermolecular force
large molecules vdw’s forces are stronger between molecules
order melting point from highest to lowest
- diamond graphite as they are giant covalent lattices bonds to break
- metal and non metal is a giant ionic lattice forces of attraction to overcome
- metals are giant metallic lattices forces of attraction to overcome
*2 or more non metals bonded together are simple molecular forces of attraction between molecules to overcome - hydrogen bonding
- permanent dipole dipole
- van der waals
