Chapter 5 Electrons And Bonding Flashcards
Principle quantum n
The number of shells or energy level
number of electrons= 2n^2
Atomic orbitals
A region around the nucleus that can hold up to two electrons, with opposite spins.
s p d and f orbitals which each have a different shape
S- orbital
- shape of a sphere
- each she’ll From n=1 contains one s orbital
- the greater the shell number, the greater the radius of its s orbital
P- orbital
- shape of a dumb-bell
- 3 separate p- orbitals at right angles to one another
- each shell from n=2 contains 3 p- orbitals
- the greater the shell number the further the p- orbital is from the nucleus
D-orbital and f-orbital
- Each shell from n=3 contains 5 d-orbitals
- each shell from n=4 contains 7 f orbitals
Sub shells
A group of orbitals of the same type within a shell.
Shell
A group of atomic orbitals with the same principal quantum number, n. Also known as a main energy level.
electron configuration
A shorthand representation that shows how electrons occupy sub-shells in an atom.
cation
A positively charged ion with fewer electrons than protons. formed when atoms lose electrons
anion
A negatively charged ion with more electrons than protons. formed when atoms gain electrons
ionic bonding
The electrostatic attraction between positive and negative ions.
giant ionic lattice
A three-dimensional structure of oppositely charged ions, bonded together by strong ionic bonds.
covalent bond
The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.
molecule
The smallest part of a covalent compound that can exist while retaining its chemical
identity, consisting of two or more atoms covalently bonded together.
Lone pair
An outer shell pair of electrons that is not involved in chemical bonding.
displayed formula
A formula showing the relative positioning of all the atoms in a molecule and the bonds between them.
dative covalent/coordinate bond
A shared pair of electrons in which the bonded pair has been provided by one of the bonding atoms only; also called a coordinate bond.
Common cations
Na^+, Ca^2+, Al^3+, NH4^+
Common anions
Cl^-, O^2-, NO3^- , SO4^2-
polar (molecule)
With δ+ and δ– charges at different ends of the molecule.
A molecule with an overall dipole, having taken into account any dipoles across
bonds and the shape of the molecule.
Expansion of the octet
When more than 8 electrons in the outer shell in covalent bonding.
This is possible from the n=3 shell (18 electrons can fit in this shell), when a d sub- shell becomes available for the expansion
Double bond
The strong electrostatic attraction between two shared pair of electrons and the nuclei of the bonded atoms.
