UNIT 4: Energy and Motion

& Electron Configuration

Wavelength: (l) ______.

Frequency: (n), usually second.

SPEED OF LIGHT EQUATION

C = ln

C = ______(______m/s)

l = is the ______of the electromagnetic wave

n = ______of the electromagnetic wave

EX: If the wavelength of a wave is 350 nm, what is the frequency of the wave?

C = ln

1) If the frequency of a wave is 8.32 x 105 Hz, what would be the wavelength in meters? (l = ?)

Quantum: ______that can be ______or ______by an atom.

– Plank suggested that ______in
______, specific amount called ______

– Proposed a relationship between ______
and ______

ENERGY EQUATION

E = hn

E = ______in joules of a quantum of radiation

n = ______of radiation emitted (in Hertz) (Hz = 1/s)

h = plank’s constant = 6.626 x 10-34 J*s

1) How much energy is emitted from a wave with a frequency of 3.65 x 1017 s?

E= h n

= (6.626 x 10-34 ) x ( 3.65 x 1017)

2) How much energy is emitted from a wave with a frequency of 7.48 x 1012 s?

E= h n

= ( ) x ( )

HOW LIGHT WORKS

Ø Photon: a particle of ______that has ______and ______mass. (tiny packets of energy)

Ø ______wavelengths of ______carry ______amounts of ______.

Ø The ______in a photon ______on the ______released when an atom goes from an ______to a ______.

Photoelectric Effect:

Ø When______, with sufficient energy, was shined on a metal, that metal ______.

Ø Dual Wave-Particle Nature of light:

–Max Plank suggested that ______emit energy in small specific amounts called ______rather than a continuous stream of energy.

–Einstein suggested that radiation/light exists as ______of ______, where each particle carries a specific amount of energy. In order for an ______to be ejected from a metal, the ______must be struck by a single ______possessing a ______amount of energy.

Electromagnetic Radiation:

Ø that exhibits as it travels through__.

Ø moves at the ______.

Ø Electromagnetic radiation is usually called______. It is divided into various classes

Ø , and light, , and __waves form the electromagnetic spectrum

Types of Electromagnetic Radiation

X-rays: ______
______

Microwaves: ______

Ultraviolet:______.

– The ______absorbs most of the sun’s UV rays

Visible light: ______.

– our eyes and brain interpret different frequencies as ______

– ______

Infrared:______. (fire, heaters)

Radio: ______

• Ground State: the ______state of an atom

• Excited State: the ______of an atom

– when atoms to their state, they. ( ex: Neon signs)

• Line-emission spectrum: resulting from a shined through a __.

• The ______of each element is

______.

HYDROGEN

Ø Hydrogen studied because it is the simplest with only _____e-

Ø In the normal H atom; the e- is in the ______state when n = 1.

Ø When the e- absorbs energy it moves to a ______excited state.

Ø When an excited e- gives off energy in the form of______, it drops back to a ______energy state.

o if e- returns to ground state (n = 1): Lyman series (ultraviolet)

o if e- returns to n = 2: Balmer series (visible)

o if e- returns back to n = 3: Paschen series (infrared)

Ø Whenever an excited hydrogen atom falls to its ______state or to a ______energy state, it emits a ______of radiation. (Emission) The energy of the photon is equal to the difference between the initial and final state.

Ø Energy states are______.

Ø In order for an electron to go to a ______energy level, it must ______energy (absorption)

Ø Bohr proposed a model to explain this.

Bohr Model of Hydrogen Atom

Ø The electron orbits or ______can be compared to the______.

Ø According to the model:______.

Ø The electron is therefore is its ______state when its orbit is ______to the______.

Ø This ______is ______from the ______by a ______where the______.

Ø The ______from the nucleus, the ______the ______of the electron.

Bohr was WRONG!

• Bohr’s model of the atom only worked for the first _____ elements.

Chlorine:

• Electrons do NOT travel in a fixed orbit, but in______.

Molecular Orbitals are what we have instead:

Ø Electrons ______atoms are concentrated into regions of space called ______or ______orbitals.

ARRANGEMENT OF ELECTRONS

Heisenberg Uncertainty Principle: ______
______.

o We just have a______!

Orbital: a ______region around the ______that indicates the ______
______of an electron

o only ______electrons exist in any ______
(Pauli-exclusion principle)

4 Blocks or Subshells of the Periodic Table:

__ block - ___ orbital - max ___ electrons- ______shape

__ block- ___ orbitals- max ___ electrons- ______shape

The s Orbital

The 2py Orbital

The 2px orbital

The 2pz orbital

Various d Orbitals

Various f Orbitals

S-ORBITALS:

______-to-______overlap ______compatible______creates a ______(σ) bond

P-ORBITALS:

______-to-______overlap generates a ______(s) bond.

______-to- ______overlap (usually between ____ orbitals) generates a ______(π) bond.

· Each type of ______holds a ______number of______, and therefore, a ______number of______.

The Periodic Table

QUANTUM THEORY:

Ø Classical theory predicted that the ______atoms would be excited by whatever amount of energy that was added to them.

Ø Thus they expected to observe the emission of a ______range of frequencies of electromagnetic radiation, but hydrogen only gave off ______visible bands of color.

Ø Attempts to explain why Hydrogen atoms gave only specific frequencies of ______is explained by the Quantum Theory!

Ø Schrodinger used De Broglie’s hypothesis that electrons also have a ______-______nature to develop an equation that treated electrons as waves. He came up with Quantum theory to describe mathematically, the wave properties of electrons.

Ø These are only probable locations because of Heisenberg uncertainty principle. Hence the orbital: a general space indicating the ______location of electrons.

Quantum Numbers

Principle Quantum Number: (n) indicates the ______level occupied by the ______(also called shells)

Ø n = ______(1,2,3…)

Ø The ______/ ______of the periodic table represent the ______

Ø There are ____ periods, so there are ____ energy levels.

Angular Momentum:(l) indicates the______.

Ø • l = 0 to (n-1)

Ø except at the first energy level, ______have ______known as______.

Ø Orbital shapes are: s (______), p (______/______), d (______), f (______).

Magnetic Quantum Number: (m) indicates the ______of an ______around the______.

Ø • m = - l to + l

Ø Orbitals can have the______, but ______:

– s subshell: only _____orientation or ___ orbital

– p subshell: ___orbital -___, ___, & ___ axis

– d subshell: ___ orbitals

– f subshell: ___ orbitals

Spin Quantum Number: indicates the ______of the ______or which of the ______in the ______you have.

– A ______can hold a ______of______, which must have ______. (+1/2, -1/2)

– An ______is a ______spin and a ______is a ______spin.

– All ______fill with an ______then ______and fill with a______.

QUANTUM NUMBER EXAMPLE:

Ø •n =1 , then l = 0, then m = 0, with +1/2 and –1/2. This represent the Hydrogen (+1/2) and Helium (-1/2) atoms.

Ø •n = 2, then l = 0 or 1,

Ø If l = 0, then m = 0, with +1/2 and –1/2 spins.
Lithium would have the +1/2 and Beryllium would be the –1/2.

Ø If l = 1, then m = -1, 0, +1. Each m has a +1/2 and –1/2 spin.

So….

Ø •The s block is always l =0, m = 0

o 1 orbital

Ø •The p block is always l =1, m = -1, 0, +1

o 3 orbitals

Ø •The d block is always l =2, m = -2, -1, 0, +1, +2

o 5 orbitals

Ø •The f block is always l =3, m = -3, -2, -1, 0, +1, +2, +3

o 7 orbitals

Electron Configuration

• Describes the ______in an atom

RULES:

1) Aufbau Principle:______.

-1s orbital______, then______,then______.

2) Pauli Exclusion Principle:______.

3) Hund’s Rule: ______are occupied by ______before any ______is occupied by a______, and all electrons in singly occupies orbitals must have the______.

– (they fill with, then go back and fill the )

– Place as many as possible in in the __sublevel.

– Ex: p subshell fills ______

______

Three ways to indicate electron configuration: Orbital Notation, Electron-Configuration Notation, Noble Gas Notation.

1. Orbital Notation: H ___ or He ___

1s 1s

Na ______

Br ______
______

2. Electron Configuration Notation: ______of orbital notation. Instead represented by ______and ______. (like a code)

Hydrogen is 1s1 Helium is 1s2

Si:

Ca:

3. Noble Gas Notation: (group _____elements are Noble Gases) When the ______main energy level is filled, usually with______, this is used.

Ø The ______in configuration to be filled is in______. Then continue with electron configuration notation.

o Ex: Ne: 1s22s22p6
Na: [1s22s22p6 ] 3s1 or [Ne] 3s1

Ø The electrons in the stable (Noble gas) configuration are termed ______.

Ø The electrons in the outer shell (beyond the stable core) are called ______.

Br:

HUND'S RULE

Electrons ______simply ______of one shell and then move onto the next. The fill order is called ______. The diagram below is a convenient reminder of how subshells fill.

1s2

• The large number “1” refers to the ______“n” which stands for the______.

• The letter “s” stands for ______“l” which tells us the ______or ______that the electrons occupy.

• The exponent “2” refers to the ______in that subshell.

EXAMPLES:

Magnesium has an atomic number of ______.

This means what….

EC: 1s2 2s2 2p6 3s2 (2+2+6+2 = 12)

ON: ______1s 2s 2p 3s

NG:

Titanium has an atomic number of _____ .

This means what….

EC:

ON: ______

1s 2s 2p 3s 3p 4s

______

NG:

Chlorine has an atomic number of _____.

This means what….

EC:

ON: ______

1s 2s 2p 3s 3p

NG:

Lithium:

EC:

ON:

NG:

Nitrogen:

EC:

ON:

NG:

UNIT 4: Energy and Motion