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CHEM 1201 > Chapter 6 > Flashcards

Chapter 6 Flashcards

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1
Q

What is a wave?

A

A vibrating disturbance by which energy is transferred

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2
Q

Examples of waves

A

Microwaves, Ocean Waves

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3
Q

Properties of Waves

A

Wavelength
Amplitude
Frequency

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4
Q

Wavelength

A

Waves consist of alternating peaks and troughs separated by a constant amount

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5
Q

Amplitude

A

The heights of the peaks (or lows of the troughs)

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6
Q

Frequency

A

The number of peaks (or troughs) that pass by a certain fixed point in a certain amount of time

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7
Q

In a wave, what is mathematically related?

A

wavelength and frequency

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8
Q

Electromagnetic radiation

A

the transmission of energy in the form of electromagnetic waves

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9
Q

What is special about electromagnetic radiation?

A

Can travel through a vaccum

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10
Q

What is the smallest piece of light called?

A

Photon

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11
Q

Emission Spectrum

A

When large amounts of energy are provided to a substance, the substance releases that energy as electromagnetic radiation of certain frequencies
The specific frequencies given off are characteristic of the substance

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12
Q

What is the wavefunction?

A

Square is the probability of finding an electron in a certain region of space

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13
Q

Principal Quantum Numner

A

Corresponds to the one for the Bohr atom

It can take positive integer values (1, 2, 3, etc)

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14
Q

Angular Momentum Quantum Number

A

Gives the 3-D shape of the orbital
It can take on integer values from 0 to n-1
Designated by a letter

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15
Q

What are the letters for the Angular Momentum Quantum Number?

A

s, p, d, f, g, h

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16
Q

Magnetic Quantum Number

A

This quantum number describes the orientation of the orbital in space
The values of ml are integer values from -ℓ to +ℓ

17
Q

Level

A

Collection of orbitals with the same value of n

18
Q

Sublevel

A

One or more orbitals with the same value of n and ℓ

19
Q

Subshell

A

Contain a single orbital or several orbitals

20
Q

s Orbitals

A

s orbitals (ℓ = 0) are spherical in shape
The size of the orbital increases as n increases
The value (phase) of the wavefunction in all s orbitals is always positive
Larger values of n correspond to orbitals that have larger numbers of nodes (areas of zero electron density)
One node

21
Q

p orbitals

A

p orbitals have ℓ = 1, therefore there cannot be any p orbitals with n = 1 (remeber n must be larger than ℓ), they start at the n = 2 level
Each p sublevel consists of three orbitals (mℓ = -1, 0, +1), they are generally called px, py and pz - there is no simple relation between the subscript and the value of mℓ
All three orbitals are identical in size, shape, and energy
p orbitals have a “dumb-bell” shape, with one lobe on either side of the nucleus
The value (phase) of the wave-function (positive or negative) is opposite on the two sides of the nodal plane
2 Nodes

22
Q

d Orbitals

A

d orbitals have ℓ = 2, therefore there cannot be any d orbitals with n = 1 or n = 2, they start at the n = 3 level
Each d sublevel consists of five orbitals (mℓ = -2, -1, 0, +1, +2)
All five orbitals can expressed in a form so that they are identical in size, shape and energy … but they usually aren’t
2 Nodes

23
Q

Maxwell

A

Visible light consisted of electromagnetic waves

24
Q

Einstein

A

Used work on Photoelectric effect to show that under certain circumstances, light behaved more like particles

25
Q

Balmer

A

Derived a formula to explain the position of the lines in the visible region of the hydrogen spectrum

26
Q

Rydberg

A

Generalized Balmer’s equation to all regions (infrared and ultraviolet)

27
Q

De Broglie

A

Linked Einstein’s idea about light having particle like properties with electrons

28
Q

Davisson and Thomson

A

Showed that a beam of electrons could be diffracted by a sample in the same way as x-rays

29
Q

Shrodinger

A

Derived equation tat describes the energies and movement of subatomic particles

30
Q

Heisenberg’s Uncertainty Principle

A

It is impossible to know both the momentum and the position of a particle with certainty

CHEM 1201 (6 decks)

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