Quantum mechanics of atoms - Q2

He integrated the contributions of various researchers

into the Quantum Mechanical Model of the atom.

Erwin Schrödinger

He developed complex mathematical equations known as “wave

functions” to estimate where electrons in an atom are likely to be

found, 95% of the time.

Erwin Schrödinger

He referred to these regions as “______”. It is a

three-dimensional space where there is a greater than 95%

chance of locating an electron, and it can hold a maximum of two

electrons.

orbitals

Unlike orbits, which precisely define an object's path, these do not specify an exact location for an electron but rather a probable area where it can be found 95% of the time.

Orbitals

He further divided Bohr’s principal

quantum levels (n) into sub-levels, each

containing a specific type of orbital (s, p, d, f,

etc.).

Erwin Schrödinger

The principal quantum level and sub-level (type

of orbital) together indicated what?

The distance of the electron from the nucleus and its energy.

The energy levels are numbered 1, 2, 3, etc. the ________ the number, the closer the energy level is to the nucleus. The Letter ‘‘n’’ is used to represent the energy level.

Smaller

Each energy level can only hold a certain number of?

Electrons

The first energy level can only hold 2 electrons, the second can only hold 8, and the third can only hold how much?

18

2n2 is the what?

Equation for the max # of electrons per energy level.

Number of electrons in the first shell

2

Number of electrons in the second shell

8

Number of electrons in the third shell

18

Within each energy level are what?

Energy sublevels

These are labeled as s, p, d, and f.

Energy sublevels

Notice that the number of sublevels in an energy level is?

equal to the number of the energy level.

Within each sublevel, there are?

Orbitals.

This is the final location where the electrons reside.

Orbitals

Each of these may contain 1 or 2 electrons that spin on their axis.

Orbitals

If two electrons occupy an orbital, they must spin in?

The opposite directions.

Electron configurations,

orbital diagrams and quantum numbers to

describe which of the following statement?

The energy and motion of electrons

What does this represent in an electron configuration.

Principal quantum level (n)

What does this represent in an electron configuration.

Orbital shape (sub-level)

What does this represent in an electron configuration.

Number of electrons in sub-level

These are visual representations of electron configurations.

Orbital diagrams

They also show individual orbitals and the spin of electrons within those

orbitals.

Orbital Diagrams

The lowest energy orbitals are filled before the

higher energy orbitals. this is the?

(Aufbau Principle)

Each orbital gets one electron first, before adding

the second electron to the orbital, this is the?

(Hund’s Rule)

Only 2 electrons, of opposite spins, can occupy

each orbital, this is the?

(Pauli Exclusion Principle)

describe the properties of atomic orbitals and the electrons in

them. There are four quantum numbers.

Quantum Numbers

The symbol of this quantum number is n (symbol n)

Principal Quantum Number 

The values of this quantum number are: Positive integers (1, 2, 3, 4)

Principal Quantum Number

The significance of this quantum number indicates the energy level and size

of the orbital. Higher n values correspond to

higher energy levels and larger orbitals.

Principal Quantum Number

Higher n values (Principal Quantum Number) correspond to

_______ energy levels and _______ orbitals.

higher and larger

The symbol for this quantum number is 1 (Symbol: 1).

Angular Momentum Quantum Number 

The significance of this quantum number indicates the shape of the orbital.

Angular Momentum Quantum Number

l=0: s orbital (spherical)

l=1: p orbital (dumbbell-shaped)

l=2: d orbital (cloverleaf-shaped)

l=3: f orbital (complex shapes)

These are all examples of what quantum number?

Angular Momentum Quantum Number

l=0 shows which orbital?

s orbital (spherical)

l=1: shows which orbital?

p orbital (dumbbell-shaped)

l=2: shows which orbital?

d orbital (cloverleaf-shaped)

l=3: shows which orbital?

f orbital (complex shapes)

f orbital consists of?

(complex shapes)

d orbital consists of?

(cloverleaf-shaped)

p orbital consists of?

(dumbbell-shaped)

s orbital consists of?

(spherical)

The symbol for this quantum number is ml (Symbol: ml)

Magnetic Quantum Number

The values for this quantum number ranges: Integers from - l to +l

Magnetic Quantum Number

The significance of this quantum number Indicates the orientation of the orbital in space.

Magnetic Quantum Number

The symbol for this quantum number is ms (Symbol: ms)

Spin Quantum Number

The values for this quantum number are either: +1/2 or −1/2

Spin Quantum Number

The significance of this quantum number indicates the spin of the

electron.

Spin Quantum Number

Each energy level can only hold a certain number of electrons. The first energy level can only hold how many electrons? The second can only hold 8, and the third can only hold 18.

2

Each energy level can only hold a certain number of electrons. The first energy level can only hold 2 electrons, the second can only hold how many? And the third can only hold 18.

8