Scientists
Quantum Model
Quantum Numbers
Orbitals
Electron Configuration
100

This scientist is who provided evidence for the existence of the electron.

J.J Thomson were the first to provide evidence for the existence of the electron, a negatively charged subatomic particle.

100
What mechanical model describes an electron as standing wave?

Quantum (wave) mechanical model

100

How many Quantum Numbers are there? Name them.

There are 4 Quantum Numbers:

1. Principal Quantum Number

2. Angular Momentum (secondary) Quantum Number

3. Magnetic Quantum Number 

4. Spin Quantum Number

100

What is an orbital?

An orbital is the region around the nucleus where an electron has a high probability of being found.

100

What are 3 ways that electron configuration can be shown?

1. Energy Level Diagrams

2. Complete Electron Configuration

3. Condensed Electron Configuration

200

This scientist introduced the concept of the Wave Particle Duality.

Louis De Broglie - what is matter (electrons) had wave-like properties

200

What replaced Bohr Theory?

Bohr Theory was replaced by Quantum Mechanics.

200

The principal quantum number (n) in the quantum model represents this.

The principal quantum number (n) describes the size & energy of an orbital (e.g. n = 1,2,3,... to ∞)

200

This type of orbital is described as having a dumbell shape.

P orbitals have a dumbell shape & exist in sets of three (px, py & pz).

200

What is the complete & condensed configuration for chlorine?

complete - 1s22s22p63s23p5

condensed - [Ne] 3s23p5

300

He formulated the famous equation E=nhf, which relates the energy of a photon to frequency.

Max Planck

300

In quantum mechanics, this term is the mathematical probability of finding an electron in a certain region of space.

Wave function is the mathematical probability of finding an electron in a certain region of space.

300

What are the letters used to describe the secondary quantum number (l)?

The secondary quantum number (l), describes the shape of an atomic orbital.

l = 0: s (sharp)

l = 1: p (principal)

l = 2: d (diffuse)

l = 3: f (fundamental)

l = 4: g

300

What are the 4 types of orbitals? How many electrons can each hold?

There are 4 main types of orbitals:

s - 2 electrons

p - 6 electrons

d - 10 electrons

f - 14 electrons

300

What is [Kr] 5s24d105p3.

Antimony.

400

This scientists developed the first successful atomic model to incorporate quantum theory.

Niels Bohr, he introduced a model of the atom with electrons orbiting the nucleus in quantized energy levels, this is called the Bohr model.

400

What is Heisenberg's Uncertainy Principle?

Heisenberg's Uncertainy Principle is the idea that it is impossible to know the exact position and speed of an electron at a given time.

400

Explain the Pauli Exclusion Principle.

The Pauli Exclusion Principle states that in a given atom, no two electrons in the same atom can be in the same set of four quantum numbers (n, l, ml, ms).

400

These orbitals have no nodes & are spherically symmetric around the nucleus.

s orbitals have no nodes (except the spherical node present in higher energy s orbitals) & are spherically symmetric.

400

Write the electron configuration for bromine.

bromine - 1s22s22p63s23p64s23d104p5

500

What are the differences between the old and new theories?

Old:

1. Electrons can move between different orbitals by absorbing/emitting quanta of energy

2. Orbitals

New:

1. Electrons act like particles & waves

2. The location of an electron is given by a probability distribution

3. Orbitals

500

What are the two main ideas of the quantum mechanical model?

The two main ideas of the quantum mechanical model are that electrons can move between orbitals by absorbing or emitting quanta of energy, and that the location of electrons is given by a probability distribution.

500

List all the possible quantum numbers for an 2s orbital.

n = 2

l = 0

ml = 0

ms = +1/2 -1/2

500

Explain the differences between Orbitals & Orbits.

Orbitals:

- 2 electrons

- three dimensions

- distance from nucleus varies

- no set path

Orbits

- 2n2 electrons

- two dimensions

- path is elliptical or circular

500

Describe the Aufbau Principle.

The Aufbau Principle states that electrons occupy the lowest energy orbitals available before filling higher energy orbitals.

- The # of electrons in an atom is equal to the atomic number

- When adding electrons to orbitals, start by filling the orbital with the lowest energy & work your way up

- Remember each orbital can have a maximum of 2 electrons

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