an atom has a dense, positively charged nucleus surrounded by a cloud of electrons
Explain electronic structure of the atom in terms of its electron density.
the electron density is highest at the nucleus and drops off exponentially with increasing distance from the nucleus in any direction
What are orbitals?
probabilities
What does every orbital after the 1s orbital contain? Define. Locate.
nodes
a surface of zero electron density within an orbital
at periphery of spheres (least likely place to find an electron)
Explain probability of finding an electron in relation to the nucleus.
closer: increase probability
further: decrease probability
Explain the shapes of the s orbitals?
spheres... as you get higher in number, they become spheres within spheres
There are __ 2p orbitals,, oriented at __ to eah other.
Each p orbital consists of __.
Each is labeled according to what?
3
right angles
two lobes
orientation along the x, y, or z axis (2px, 2py, 2pz)
Explain the 2px, 2py, and 2pz orbitals.
they are dumbbell shaped
What is organic chemistry?
the study of carbon compounds
What makes carbon so special?
it has four valence electrons and can form four strong covalent bonds
it can also bind with other carbon compounds
Explain the d orbitals.
four out of five of them are cloverleaf shaped
the fifth is an elongated dumbbell with a doughnut around its middle
What does the graph of a moving electron look like?
a wave function (Greek letter psi)
Explain the charges of the p orbitals.
they are arranged perpendicular to one another with each orbital region separated by the node having different signs, which will affect reactivity
What is the aufbau principle?
fill the lowest energy orbitals first
What is Hund's Rule?
when there are two or more orbitals of the same energy (degenerate), electrons will go into different orbitals rather than pairing up in the same orbital
What are valence electrons?
electrons on the outermost shell of the atom
Explain covalent bonding.
electrons are shared between the atoms to complete the octet
when shared equally: Nonpolar (pure) covalent
when not: polar
Bonding Patterns
Tell the following of each element:
For carbon:
- valence electrons (Group #)
- # bonds
- # lone pair electrons
- 4
- 4
- 0
Bonding Patterns
Tell the following of each element:
For Nitrogen:
- valence electrons (Group #)
- # bonds
- # lone pair electrons
- 5
- 3
- 1
Bonding Patterns
Tell the following of each element:
For Oxygen:
- valence electrons (Group #)
- # bonds
- # lone pair electrons
- 6
- 2
- 2
Bonding Patterns
Tell the following of each element:
For Halides:
- valence electrons (Group #)
- # bonds
- # lone pair electrons
