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CHEM 1201 > Final Study > Flashcards

Final Study Flashcards

(73 cards)

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1
Q

What does accuracy mean?

A

How close a measurement is to the true and accepted value

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2
Q

What does precision mean?

A

How close measurements are to one another

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3
Q

What is the first wave nature of light?

A

Reflection

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4
Q

What is the second wave nature of light?

A

Refraction

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5
Q

What is the third wave nature of light?

A

Inference

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6
Q

What is the fourth wave nature of light?

A

Interference and Diffraction

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7
Q

Constructive vs. Destructive

A

involves inference

Constructive - waves in phase that produce a bright region

Destructive - waves out of phase that produce a dark region

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8
Q

What produces the electromagnetic spectrum?

A

Wavelength and frequency varying

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9
Q

Name the order of the electromagnetic spectrum

A
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10
Q

Whats the frequency equation?

A

Speed of light over wave length

OR

Velocity over wavelength

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11
Q

What is black body radiation?

A

its electromagnetic radiation depends upon temperature for its wave lengths and colors to be emitted

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12
Q

What is photoelectric effect?

A

Occurs when a light is shone on a metal and electrons get ejected if threshold frequency is passed

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13
Q

Name each colors wavelength

A
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14
Q

When temp increases what happens?

A

Frequency increases parallely

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15
Q

What is proportional to energy of a photon?

A

Frequency

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16
Q

Because photons are massless, what is their velocity?

A

Speed of light

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17
Q

What is the speed of a particle related to?

A

Wavelength

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18
Q

How are wavelength and energy related

A

They are inversely related to each other

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19
Q

What is conservation of energy?

A

Energy cannot be created nor destroyed, only transferred from one source to another.

Applies to both atom and photon

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20
Q

What causes chemical reactions?

A

Changes in electron structure

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21
Q

What causes change in electron structure?

A

Interactions with light and/or electromagnetic radiation

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22
Q

How can light be used to investigate electron structure?

A

1) You can add electrical energy to a vaporized sample (Investigate lights) (Emission spectra)

2) Shine full spectrum of light at a vaporized sample (Look for absorption of light) (Absorbtion Spectra)

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23
Q

What is emission spectra?

A

Adding energy to atoms resulting in an emission of light

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24
Q

What is absorption spectra?

A

Shining light through a vaporised element, resulting in absorption of some wavelengths of light

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25
Electron excitation
When an electron is transferred to a more energetic energy state
26
Electron relaxation
When an electron in an excited state drops to a lower energy state
27
Photon absorbtion
When a photon loses it's energy to an atomic electron which is then emitted from an atom
28
Photon emission
When an electron drops to a lower energy state the atom emits a photon
29
Whats a ground sate for an atom?
Its the lowest energy state for an atom, electrons can't move to a lower orbital
30
What is lyman series
Transitions from higher energy orbits to the lowest energy orbit available (visible series; Ultra-violet)
31
What is paschen series?
Transitions from higher energy orbits to the orbit n=3 (Infra-red)
32
What is balmer series
Transitions from higher energy orbits to the orbit n=2 (visible series)
33
What is pfund series?
Transitions from higher energy orbits to the orbits n=5
34
What is brackett series?
Transitions from higher energy orbits to the orbit n=4
35
Rydbergs formula
Calculates the wavelength of a spectral line in many chemical elements
36
Bohr's model
- atoms have certain energy levels - Atom doesn't radiate energy while its in a stationary phase - Atom changes to another stationary state only by absorbing or emitting a photon - Energy of a photon equals the difference in the energies of the two states
37
What are the limitations of Bohr's model?
- Fails for multi electron systems; only works for single electron systems - No explanation for why there are allowed orbits
38
What is Z?
Charge of the nucleus, +1 for Hydrogen
39
What was DeBroglies hypothesis?
- Proposed if energy is particle like, matter is wave like - Electrons only have certain allowable frequencies if they have wave like motion in orbits at fixed distances from nucleus - His equation can find the wavelength of any particle mass
40
What is P?
P= momentum which is inversely proportional to wavelength
41
Whats the wave concept for electrons?
- Constructive & destructive inference - Allowed orbits = constructive inference - Forbidden orbits will self destruct - Allowed orbits correspond to complete wavelengths
42
What are the consequences of electron wave?
- Location of wave like particle is imprecise - Heisenberg uncertainty principle; cannot know both precision and momentum with certainty (If one is known accurately the other is imprecisely)
43
Uncertainty principle
Single plane wave - will have precise energy and momentum; position of electron is infinite Wave packett - position of electron is localized from adding different waves; energy and momentum now imprecise
44
Schrodingers equation
Allows us to determine allowed energies
45
Wave function Significance
- wave function squared is related to the probability of finding a particle in a certain region of space - Electron density also describes the probability of finding an electron and is directly related to the wave function squared - High wave function value = high electron density
46
Wave Function
Wave function is used to describe motion of electrons in an atom
47
Outcomes of Schrodinger equation
- Electron location is described by a standing wave - Gives allowed energies of electron - Exact position of electron is unknown - Orbital is not equivalent of an orbit - 90% chance of finding electron in its orbital
48
Bohr vs. Schrodinger describing orbitals
- Bohr describes circular orbits for electrons - Schrodinger describes different solutions possible with orbitals of different shapes
49
Quantum numbers
n = principle quantum number l = angular momentum quantum number m1 = magnetic quantum number ms = spin quantum number
50
What is a subshell?
Division of atoms energy levels that are given by l values l0 = s subshell l1= p subshell l2= d subshell l3= f subshell
51
What is a shell?
Atoms energy levels given by n values; smaller the n value the greater the probability the electron is closer to the nucleus
52
What is an orbital?
A combo of n,l,m which specifies the size (E), shape and spacial orientation of one atoms orbital
53
Shielding effect
core electrons screen valence electrons from the attractive force of the nucleus
54
Orbital penetration
- Orbitals and sub shells define how close an electron can get to the nucleus - The ability of an electron to get close to the nucleus is called penetration
55
What are paramagnetic atoms
Atoms that have more electrons spinning in one direction than the other
56
What are diamagnetic atoms?
Atoms with the same number of spin up and spin down electrons
57
What are periodic trends in atomic radii
ANSWER
58
How atomic radii changes with the addition or loss of electron
With an addition - Creates an anion, more e-e repulsion, larger radius With a removal - Creates anion, less e-e repulsion, smaller radius
59
What is an isoelectronic species
Two elements or ions that have the sme total number electrons (same configuration)
60
1st ionization energy trends
Increases from the bottom to top and from left to right; as distance increases its easier to remove an electron
61
What is ionization energy
Minimum energy required to break a bond; its always endothermic as this process requires energy
62
2nd ionization energy
The energy it takes to remove an electron from a 1+ ion (meaning the atom has already lost one electron and now removing the second).
63
What is electron affinity
The energy change that occurs when an electron is accepted to form an anion
64
What are trends in electron affinity
increases from bottom to top and left to right; the more negative EA the more likely it will gain an electron Trends are not regular as Zeff and atomic size affect EA
65
Electronegativity trends
property related to the ability of an electron to attract towards an atom
66
Metallic characteristics
A good heat and electricity conductor, malleability, shiny and tend to lose e in a reaction - Metallic characteristics decrease as you move up and to the right ; increase in IE and more negative EA
67
What are lattice energies
Formed by ionic bonding
68
Trends in lattice energies
- Ions with a greater charge create higher energy lattices - Smaller ions can get closer together, increasing the interaction between them (thus the lattice energy)
69
What are bond strengths
Its a measure of how much energy is required to break a bond - Bond length decreases as bond strength increases
70
Whats a non-polar covalent bond
- Bonding electrons shared equally - No charges on atoms
71
Whats a polar covalent bond
- Bonding electrons shared unequally - Partial charges on atoms
72
Whats an ionic bond
- Complete transfer of one or more valence electrons - full charges on resulting ions
73
1st ionization energy
the energy that is required to remove the first electron from a neutral atom

CHEM 1201 (6 decks)

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