GENCHEM

Gas laws

• Describe the behavior of gases in relation to pressure, volume, temperature, and the number of gas particles. 

• Explains natural and industrial processes like weather patterns, chemical reactions, and respiratory functions.

Boyle’s Law

Constant temperature

Charle’s Law

Constant pressure

 atomic orbital

An electron in an atom is described in terms of 4 quantum numbers. 3 are n, l, and ml, which describe ______

region of space around the nucleus

An atomic orbital is the ____________ where the chance of finding an electron with a given energy is greatest 

Principal Quantum Number (n)

Describes the energy of the electron

2(n²) where n = the energy level

Maximum # of electrons in each energy level is calculated by _____ where _____

Azimuthal or angular momentum quantum number (l)

Describes the shape of the orbital

s(harp) sublevel 

p(rincipal) sublevel 

d(iffused) sublevel 

f(undamental) sublevel

What are the 4 sublevels?

Magentic quantum number (ml)

• Describes the orientation of the orbital in space 

Spin quantum number (ms)

Refer to the spin of the electron in a given orbital

Electron Configuration 

• This tells us which orbitals the electrons for an element are located 

• electrons fill orbitals starting with the lowest n and moving upwards (aufbau)

• No 2 electrons can fill one orbital with the same spin (pauli)

• For degenerate orbitals, electrons fill each orbital singly before any orbital gets a second electron (hund’s rule)

What are the 3 rules? for electron config

• lowest to the highest

• orbitals

• 1s

• In a given atom, electrons are distributed from the _______ energy level 

• The ______ are arranged in order of increasing energy based on the principal energy levels and the sublevels where they are in

• The lowest energy orbital is ___ orbital that makes up the only sublevel in the first principal energy level

n+1
lowest

The _____ rule-the orbital with the ______ energy is usually the one for which the sum of n and l is lowest

Hund’s rule of maximum multiplicity

• Electrons occupy orbitals of equal energy singly so that all the orbitals contain one electron each before pairing up 

Pauli’s exclusion principle 

• Two electrons may occupy an atomic orbital only if they have opposite spins. This also means that the maximum number of electrons that can occupy an orbital is two. In a given atom, no 2 electrons have the same set of quantum numbers. In other words, each electron is unique. 

singly

• Electrons occupy orbitals of equal energy _____ so that all the orbitals contain one electron each before pairing up 

opposite spins

two

• Two electrons may occupy an atomic orbital only if they have ______. This also means that the maximum number of electrons that can occupy an orbital is ___. In a given atom, no 2 electrons have the same set of quantum numbers. In other words, each electron is unique. 

Thomson’s Plum-Pudding Model

Electrons were supposed to be embedded in a positive cloud 

(spherical cloud of positive charge and negatively charged electrons)

Rutherford’s Nuclear Model of the Atom

The nucleus is very small, dense, and positively charged. 

Electrons surround the nucleus 

Most of the atom is empty space

The Bohr Model

Another concept of atomic structure was proposed in 1913, also known as the planetary model. 

The electrons were supposed to move in orbits around the nucleus, but they could orbit only in certain specified energy levels; they cannot exist between energy levels 

• Electrons occupy orbits that are at fixed energies and radii. Each orbit was given a number, a quantum number (n)

• The bigger the orbit the further the electron is from the nucleus and the higher is its energy with a higher quantum number 

• A specific amount of energy is required to move an electron from one level to another. 

• The lowest allowable energy state of an atom is called the ground state 

• When an atom gains energy, it’s in an excited state

Schrodinger’s Model

He treated electrons as waves in a model called the quantum mechanical model of the atom, aka the Electron Cloud Model. 

• Small, dense, positively charged nucleus surrounded by electron clouds of probability 

• Doesn’t define an exact path an electron takes around the nucleus 

• In other words, the position of an electron within an atom can’t be pinpointed. Using his wave mechanics, we can only specify regions around the nucleus of an atom in which there is a large chance of finding the electrons.

Electron cloud

the volume in which the electron is found 90% of the time