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CHEM 1201 > Final Study > Flashcards

Final Study Flashcards

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
Q

Electron excitation

A

When an electron is transferred to a more energetic energy state

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26
Q

Electron relaxation

A

When an electron in an excited state drops to a lower energy state

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27
Q

Photon absorbtion

A

When a photon loses it’s energy to an atomic electron which is then emitted from an atom

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28
Q

Photon emission

A

When an electron drops to a lower energy state the atom emits a photon

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29
Q

Whats a ground sate for an atom?

A

Its the lowest energy state for an atom, electrons can’t move to a lower orbital

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30
Q

What is lyman series

A

Transitions from higher energy orbits to the lowest energy orbit available (visible series; Ultra-violet)

31
Q

What is paschen series?

A

Transitions from higher energy orbits to the orbit n=3 (Infra-red)

32
Q

What is balmer series

A

Transitions from higher energy orbits to the orbit n=2 (visible series)

33
Q

What is pfund series?

A

Transitions from higher energy orbits to the orbits n=5

34
Q

What is brackett series?

A

Transitions from higher energy orbits to the orbit n=4

35
Q

Rydbergs formula

A

Calculates the wavelength of a spectral line in many chemical elements

36
Q

Bohr’s model

A
  • 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
Q

What are the limitations of Bohr’s model?

A
  • Fails for multi electron systems; only works for single electron systems
  • No explanation for why there are allowed orbits
38
Q

What is Z?

A

Charge of the nucleus, +1 for Hydrogen

39
Q

What was DeBroglies hypothesis?

A
  • 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
Q

What is P?

A

P= momentum which is inversely proportional to wavelength

41
Q

Whats the wave concept for electrons?

A
  • Constructive & destructive inference
  • Allowed orbits = constructive inference
  • Forbidden orbits will self destruct
  • Allowed orbits correspond to complete wavelengths
42
Q

What are the consequences of electron wave?

A
  • 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
Q

Uncertainty principle

A

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
Q

Schrodingers equation

A

Allows us to determine allowed energies

45
Q

Wave function Significance

A
  • 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
Q

Wave Function

A

Wave function is used to describe motion of electrons in an atom

47
Q

Outcomes of Schrodinger equation

A
  • 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
Q

Bohr vs. Schrodinger describing orbitals

A
  • Bohr describes circular orbits for electrons
  • Schrodinger describes different solutions possible with orbitals of different shapes
49
Q

Quantum numbers

A

n = principle quantum number
l = angular momentum quantum number
m1 = magnetic quantum number
ms = spin quantum number

50
Q

What is a subshell?

A

Division of atoms energy levels that are given by l values
l0 = s subshell
l1= p subshell
l2= d subshell
l3= f subshell

51
Q

What is a shell?

A

Atoms energy levels given by n values; smaller the n value the greater the probability the electron is closer to the nucleus

52
Q

What is an orbital?

A

A combo of n,l,m which specifies the size (E), shape and spacial orientation of one atoms orbital

53
Q

Shielding effect

A

core electrons screen valence electrons from the attractive force of the nucleus

54
Q

Orbital penetration

A
  • 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
Q

What are paramagnetic atoms

A

Atoms that have more electrons spinning in one direction than the other

56
Q

What are diamagnetic atoms?

A

Atoms with the same number of spin up and spin down electrons

57
Q

What are periodic trends in atomic radii

A

ANSWER

58
Q

How atomic radii changes with the addition or loss of electron

A

With an addition
- Creates an anion, more e-e repulsion, larger radius
With a removal
- Creates anion, less e-e repulsion, smaller radius

59
Q

What is an isoelectronic species

A

Two elements or ions that have the sme total number electrons (same configuration)

60
Q

1st ionization energy trends

A

Increases from the bottom to top and from left to right; as distance increases its easier to remove an electron

61
Q

What is ionization energy

A

Minimum energy required to break a bond; its always endothermic as this process requires energy

62
Q

2nd ionization energy

A

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
Q

What is electron affinity

A

The energy change that occurs when an electron is accepted to form an anion

64
Q

What are trends in electron affinity

A

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
Q

Electronegativity trends

A

property related to the ability of an electron to attract towards an atom

66
Q

Metallic characteristics

A

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
Q

What are lattice energies

A

Formed by ionic bonding

68
Q

Trends in lattice energies

A
  • 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
Q

What are bond strengths

A

Its a measure of how much energy is required to break a bond
- Bond length decreases as bond strength increases

70
Q

Whats a non-polar covalent bond

A
  • Bonding electrons shared equally
  • No charges on atoms
71
Q

Whats a polar covalent bond

A
  • Bonding electrons shared unequally
  • Partial charges on atoms
72
Q

Whats an ionic bond

A
  • Complete transfer of one or more valence electrons
  • full charges on resulting ions
73
Q

1st ionization energy

A

the energy that is required to remove the first electron from a neutral atom

CHEM 1201 (6 decks)

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