chem bonding Flashcards
what is electronegativity?
the measure of an atom’s ability to attract electrons in a covalent bonds to itself
what is the trend of electronegativity down a group? explain.
down a group, electronegativity decreases - effective charge increase, shielding effect increase, no. of quantum shells increase, hence outermost electrons are further away from nucleus so nucleus of the atom has a weaker attraction for electrons of another nucleus
what is the trend of electronegativity across the period?explain.
across a period, electronegativity increases - effective nuclear charge increase, shielding effect remains unchanged, hence nucleus of atom has higher attraction for electrons of another nucleus
what is a covalent bond?
the electrostatic force of attraction between the positively charged nucleus of both atoms and their shared electrons
what are the factors affecting the strength of a covalent bond?
- bond length - bond length increase, covalent bond strength decrease
- bond order - no. of covalent bonds between a pair of atoms - bond order increase, bond strength increase
what is a sigma bond and a pi bond?
head on overlap and side on overlap. a sigma bond must exist first for a pi bond to exist
what is a metallic bond?
the electrostatic force of attraction between a lattice of metal cations and sea of delocalised valence electrons
what are the factors affecting the strength of a metallic bond?
- charge and radius of cation - charge increase, radius decrease, charge density increase, hence strength increase
- no. of valence electrons contributed per atom - ~ increase, no. of delocalised electrons increase, hence strength increase
what are alloys? what are the properties of alloys?
they are mixtures of metals (with small quantities of other elements). they make metals harder as the atoms of different sizes disrupt the orderly arrangement of the main metal atoms so they cannot slide over each other easily when force is applied.
what is an ionic bond?
it is the electrostatic force of attraction between oppositely charged ions in a giant ionic lattice
what are the factors affecting the strength of ionic bonding?
- ionic charge (greater impact)
2. ionic radius
what is lattice energy?
the heat evolved when 1 mole of pure ionic solid is formed from its constituent gaseous ions
what are the types of intermolecular forces of attraction?
- dispersion forces/ instantaneous dipole-induced dipole attraction
- permanent dipole-permanent dipole attraction
- hydrogen bonding
when do dispersion forces occur?
non polar molecules/atoms
what are the factors affecting the strength of dispersion forces?
- no. of electrons - ~increase, size of electron cloud increase, polarisability increase, dispersion forces form more easily, hence strength increase
- surface area of of contact - ~increase, s.a for electron cloud to be distorted increase (for molecules with a similar no. of electrons)