Atomic Theory

Atoms

• Matter is made of atoms

•Atoms are the basic building block of matter

History of the Atom400 BC DemocritusTHE ATOM IS AN INDIVISIBLE PARTICLE• the atom is the smallest particle of matter1808 DaltonTHE SOLID SPHERE MODEL• atoms are solid , indestructible spheres (like billiard balls)

1897 J.J. ThompsonTHE RAISIN BUN MODEL• atoms are solid spheres made up of solid positive mass with tiny negative particles embedded in the positive

History of the Atom1911 RutherfordTHE PLANETARY MODEL• the atom is composed of a positive nucleus and negative electrons which surround the nucleus• atom is mostly empty space• Gold foil experiment

The Gold Foil Experimentby Rutherford

PredictionIn accordance to the J.J. Thomson model of an atom, the alpha particles should have passed directly through the gold foil for all instances. Observation

most of the alpha particles passed straight through the foil, a small percentage of them were deflected at an angles and some were even backscattered. Conclusion two conclusions: one, an atom is mostly

empty space and scattered electrons and two, an atom must have a positively charged centre that contains most of its mass

History of the Atom

1932 Sir James Chadwick• the nucleus contains particles called neutrons and positively charge protons

1913 Niels Bohr • electrons orbit the nucleus in different energy levels• electrons can move from one level to another by gaining or losing packets of energy• electrons are more stable when they are closer to the nucleus

History of the Atom

Structure of the Atom

Consists of sub-atomic particles. •protons•neutrons•electrons

•Protons and neutrons are located in the nucleus•Electrons orbit the nucleus

Determining the number of subatomic particles

Each element has an atomic number and a mass number

Atomic number = no. of protons = no. of electrons

Mass number = no. of protons + no. of neutrons

Therefore, no. of neutrons = mass number – atomic number

Example: How many protons, neutrons and electrons does carbon have?

Atomic number = 6Mass number = 12

Number of protons: 6Number of neutrons: 12-6 = 6Number of electrons: 6

A

ZE

mass number

chemical symbol

atomic number

An international recognized system that allows anyone to commuicate information about the atom

Atomic Symbol

Isotopes and ions

Isotope is an atom of an element with a different number of neutrons and hence a different mass number.

An Ion is an atom that has lost or gained electron/s.

The Bohr Model• Electrons move around the nucleus in fixed energy levels called shells.•Shells close to the nucleus are lower in energy while shells farther away are high in energy. • Shells are number outwards from the nucleus (1,2,3..) and are also lettered (K,L,M,N...)

Number of electrons in shells

Different shells hold different numbers of electrons. The maximum number of electrons that can fit into a shell is 2n2 (n = shell number)

Shell number (n) Representative letter Maximum

number of electrons in this shell (2n2)

1 K 2 X 1 2 = 22 L 2 X 2 2 = 83 M 2 X 3 2 =

184 N 2 X 4 2 =

32

Drawing Atoms

Bohr diagram number of protons and neutrons written in the center•electrons drawn in circular orbits around the nucleus

10 P10 N

17 P18 N

Example: Chlorine

Atomic number is 17.17 protons and electrons

Mass number is 35.35 - 17 = 18 neutrons

Subshells

subshell Number of electrons

s 2

p 6

d 10

f 14

Subshells are energy levels found within shells.

There are four different types of subshells

Named- s, p, d, f .

Subshell energy: s<p<d<f

Shells and subshells

Electron configuration

The way in which electrons are arranged around the nucleus of an atom is called the electron configuration of the atom.

Aufbau Principle

Electrons occupy orbitals of lower energy first.

Order of electron filling

Electrons fill shells and subshells of lowest energy first.

Write the full electronic configuration of:

Aluminum – 13 electrons

Calcium – 20 electrons

Iron – 26 electrons

Bromine – 35 electrons

Answers

Aluminum – 13 electrons 1s22s22p63s23p1

Calcium – 20 electrons 1s22s22p63s23p64s2

Iron – 26 electrons 1s22s22p63s23p64s23d6

Bromine – 35 electrons 1s22s22p63s23p64s23d104p5

Timberlake LecturePLUS 2000

Orbital is the 3 dimensional space

around a nucleus in which electrons

are most likely to be found

Each orbital can hold up to 2

electrons.

ShellSubshell Orbital

Orbitals

s subshell: spherical1 orbital-2 electrons

p subshell: pair of lobes3 orbital- 6electronsx

y

z

d subshell: double dumpbells5 orbital-10 electrons

xy

z2

xz

x

y

yz

x2-y2

Ground state and excited state

At ground state the electron is at its lowest possible energy level (electrons are as close to the nucleus as possible).

Example: Sodium (Z=11)

Ground state electron configuration: 2, 8, 1

Evidence for the Bohr Model

If atoms are given large amounts of energy (heat, light or electricity), the electrons can jump to an orbit further away from the nucleus. The atom is then in an excited state. Fluorine

Ground state F: 1s2 2s2 2p5

Exited stateF*: 1s2 2s1 2p5 3s1

Evidence for the Bohr Model

When the electrons return to the ground state, they release this energy in the form of light. The light released has a specific wavelength corresponding to the difference between the energy levels.

Electromagnetic Energy

Evidence for the Bohr Model

Emission Spectra are emissions of light from atoms that have been heated or provided with energy.

Evidence for the Bohr Model

Emission Spectra are different for each material.

Fe

They can be used to determine the identity of an unknown sample of an element.

Practise

1) Draw 2 Bohr-Rutherford diagrams for lithium; one in the ground state and one in the excited state. Make sure to include the energy put into the system, and energy released.

Hydrogen

Helium

2) Explain why different elements have different emission line spectrums.

Practise

A

B

C

D

Identify each of the unknown gases based on the emission line spectrums provided. The 4 possibilities are oxygen, hydrogen, helium and neon.