bonding Flashcards
what is ionic bonding?
- strong electrostatic forces of attraction between oppositely charged ions held in a lattice .
- electrons transferred from metal to non metal to achieve full other shells
give an example of an ionic ally bonded substance .
- NaCl (sodium chloride - salt)
- sodium loses an electron and chlorine gains electron to produce ions will full other electron shell
how high are ionically bonded substances bp and mp? why?
- high —> takes lots of energy to break strong electrostatic forces of attraction between oppositely charged ions.
- thus, makes ionic compounds solid at room temp
do ionic compounds conduct electricity ? why?
- yes, when molten/ in (aq) solution as ions are free to move and carry charge (don’t when solid)
what is simple molecular covalent bonding?
- string covalent bonds between atoms, weak van der waals forces of attraction between molecules .
- H2O, CO2 and NH3
what is covalent bonding?
- a bond in which high two atoms share one or more pairs of electrons .
- multiple electron pairs can be shared to produce multiple covalent bonds . + represented using dot and cross diagram
are there any lone electrons in simple covalent bonding ?
- no- all involved in bonding
can simple molecular covalent molecules conduct electricity ? why?
- no - all electrons used in bonding and aren’t free to move
do. simple molecular substances have low/high mpt and bpt? why?
- low = weak van der waals forces of attraction between molecules that don’t take much energy to overcome (these are overcome rather than covalent bonds)
describe macromolecular covalent bonding.
- lattice of many atoms held together by strong covalent bonds .
do substances with macromolecular covalent bonds have high/low mpt and bpts? why?
- high, as it takes lots of energy to overcome many strong covalent bonds .
do substances with macromolecular covalent bonds conduct electricity ?
- most don’t as all electrons are used in bonding .
what’s meant by metallic bonding ?
- consisted of a lattice of positively charged bed ions surrounded by a “sea” of delocalised electrons.
- produces very strong electrostatic force of attraction between these oppositely charged ions.
- layers slide over each other = malleable
do metallic compounds have high/low bpt and mpts? why?
- high = strong forces of attraction between positive metal ions + negatively charged sea of delocalised electrons
do metallic compounds conduct electricity? why?
- yes as delocalised electrons can move throughout the metal to carry charge
how does the strength of metallic bonds change across the periodic table ? why ?
- increases —> higher melting and boiling points , stronger
- higher charge on metal ions
- more delocalised electrons per ion
- stronger force of attraction between them
define electronegativity.
- the ability of an atom to attract the pair of electrons (electron density) in a covalent bond
what affects electronegativity ?
- nuclear charge
- atomic radius
- electron shielding
—> increases along period as atomic r decreases and decreases down group as shielding increases