Bonding Flashcards
(52 cards)
*Orbital
A region around the nucleus that can hold up to two electrons, with opposite spins
*ionic bonding
The electrostatic attraction between oppositely charged ions.
- covalent bonding
Strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms
*polar molecule
has polar bonds with dipoles that do not cancel due to their direction
*electronegativity
the ability of an atom to attract the bonding electrons in a covalent bond
Dipole
: partial charged atoms in a covalent bond due to different electronegativity
allotropes
different forms of the same element in the same state, e.g graphite and diamond
dative covalent bond
When both electrons come from one atom in a covalent bond.
when and why can ionic compounds conduct electricity
Ionic compounds don’t conduct as solid due to no mobile ions, they can conduct when molten/ in solution as ions are mobile.
can covalent compounds conduct electricity? why?
Covalent compounds can’t conduct as solids or liquids/solutions as they have no ions or mobile electrons.
can metals conduct electricity
Metals can conduct when solid or molten as they have delocalised electrons.
When explaining shapes of molecules or bond angles state:
o Number of bond pairs and lone pairs of electrons
o Electron pairs repel so spread out
o Lone pairs repel more than bonded pairs
what is an induced dipole- dipole
caused by movement of electrons causing a temporary dipole which induces a dipole in a neighbouring molecule. The more electrons a molecule has the larger the force, e.g. I2 has lots of electrons so induced dipole forces are strong enough that it’s a solid.
what is a permanent dipole
a difference in electronegativity causes a permanent dipole so molecules are attracted to each other.
what is hydrogen bonding
occurs between molecules that have N, O or F with a lone pair and H attached. Strong compared to other IM bonds
what are the rules of orbitals
the two electrons have opposite spins
the orbitals in he same sub shell fill up singly before pairing up
shape of s orbital
spherical
shape of p orbital
3d - dumbell shape
how many orbitals and electrons are in the s sub-shell
1 orbital
2 electrons
how many orbitals and electrons are in the p sub-shell
3 orbitals
6 electrons
how many orbitals and electrons are in the d sub-shell
5 orbitals
10 electrons
how many orbitals and electrons are in the f sub-shell
7 orbitals
14 electrons
what sub-shells are in the first shell (and electrons)
1s - 2 electrons
what sub-shells are in the second shell (and electrons)
2s 2p - 8 electrons
