Chapter 5 and 6 Test Flashcards

0
Q

The Bohr Model

A
  • Created by Neils Bohr
  • Showed how energy of an atom changes when absorbing or emitting light
  • Proposed that an electron is found only in specific circular paths, or orbits, around the nucleus.
  • Each orbit= different energy level
  • Absorbs energy–> higher orbit
  • Emits energy–> lower orbit
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1
Q

Limitations of Rutherford’s Atomic Model

A
  • RAM: Explained only a few simple properties of an element

- RAM: Could not explain the chemical properties of an element

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2
Q

Ground State

A
  • When an electron is at the lowest energy orbit (stable)

- When at a high energy level, an electron is unstable)

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3
Q

What is the formula for energy emitted by an electron?

A

E=h x v

  • V is the frequency
  • H is a constant #
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4
Q

What are the two things that effect the color being emitted by an electron when releasing energy?

A
  • The electrons in their outer energy levels are unique for each element
  • The quantum of energy released. The quantum released is represented by the distance of energy levels .
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5
Q

Energy levels

A
  • The fixed energies an electron can have

- Unequally spread upart

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6
Q

Quantum

A

-The amount of energy required to move an electron from one energy level to another energy level

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7
Q

The Bohr model vs. Rutherford’s Atomic Model

A
  • RAM: could not explain why elements that have been heated to higher temps give off different colors of light
  • Bohr model explains that when an atom emits light it is moving from one energy level to another
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8
Q

The Quantum Mechanical Model

A
  • Created by Edward Schrodinger
  • Devised a mathematical equation to describe the behavior of the electron in a hydrogen atom
  • Came from mathematical solutions to the Schrodinger equation
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9
Q

The Quantum Mechanical Model vs. The Bohr Model

A
  • The quantum mechanical model describes the energy of electrons like the Bohr Model
  • Unlike the Bohr Model, QMM does not specify the exact path the electron takes around the nucleus
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10
Q

Orbitals

A
  • A region of space an electron will be in at any given time

- Types: S,D, F, P

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11
Q

Sublevel

A

-The shape of an orbital

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12
Q

Aufbau principle

A

-Electrons occupy the orbitals of the lowest energy level first

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13
Q

Hund’s rule

A
  • Every orbital in a subshell gets one electron before any orbital gets 2 electrons
  • Single electrons have parallel spin
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14
Q

Pauli Exclusion Principle

A

-To occupy the same orbital, two electrons must have opposite spins.

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15
Q

Three ways to show electron configurations

A
  • Aufbau Diagram
  • Standard Electron Configuration
  • Orbital filling Diagram
16
Q

Amplitude

A

-The wave’s height from zero to the crest

17
Q

Wave length

A
  • The distance between the crests

- Represented by the greek letter lamba (upside down y)

18
Q

Frequency

A
  • The number of wave cycles to pass a given point per unit of time
  • Represented by the greek letter nu (v)
19
Q

The Frequency and Wave Length of Light

A
  • Inversely proportional ( As one decreases, the other increases)
  • As wave length increases, frequency decreases
20
Q

Electron Magnetic Radiation

A
  • Massless yet has energy
  • Light
  • Examples: radio waves, visible light, X-rays, gamma rays
  • Higher the frequency, the more dangerous it is
21
Q

Atomic Emission Spectra

A

AES: The pattern formed when light passes through a prism or diffraction grating to separate it into the different frequencies of light it contains

  • Ex: White light separates to the colors of the rainbow
  • Unique finger print of an element (each 1 is different)
22
Q

Spectra Line

A

-the line that forms when white light is separated using the Atomic Emission Spectra

23
Q

How energy travels from one place to another

A
  • By traveling on a particle (particle is charged then moved)
  • By traveling as a wave
24
Energy traveling by particle
- Follow classical mechanics (laws of motion, projectile motion) - Have energy and mass
25
Energy in wave motions
- Electromagnetic radiation travels as waves - Are massless and have energy - Travels in chunks (photons) - Wave Particle Duality: the characteristics of light, it travels like a wave behaves like a particle
26
Photons
- Chunks or quanta of energy that behave as though they were particles - 1 quanta= 1 photon - Energy of photon= h x v
27
Planck's constant
- (h in E=h x v) | - 6.626 x 10^-32 j x s
28
Why the Atomic Emission Spectra is Unique
- Every element has a unique number of electrons which occupy unique orbitals and energy levels - Because the electrons and the orbitals/energy levels they occupy is unique, the amount of energy released is unique. - Energy released (photons) effects frequency and wavelength directly
29
Dmitri Mendeleev
- Constructed the periodic table of elements | - Arranged the elements in his periodic table in order of increasing atomic mass
30
What are the 3 classes of elements?
- Metals - Nonmetals - Metalloids (characteristics of metals and nonmetals)
31
Metals
- 80% of periodic table - Good conductors of heat and electricity (best= silver, second best= copper) - Freshly cleaned metal will have a sheen (can reflect light) - All metals are a solid @ room temp. (except mercury) - Metals= ductile (can be turned into wire) - Most metals= malleable ( able to be made into sheets without breaking)
32
Nonmetals
- Most nonmetals are gases @ room temp - few= solids (phosphorus, sulfur) - Nonmetal that is liquid= bromine - Because of many different types of nonmetals, no set characteristics - Hard non-metals (diamond), brittle (break if hit)nonmetals (phosphorus) - Poor conductors of heat & electricity
33
Metalloids
- Has properties similar to metals and nonmetals - Under some conditions, act like metals, in other conditions act like nonmetals - Poor conductor of electricity
34
How the Atomic Emission Spectra works with the Bohr Model
- When an electron goes from a higher energy level to a lower energy level, or vice verse, it emits or absorbs energy - Depending on the amount of quantums/ energy levels moved down or up, an amount of energy will be absorbed or given off - Higher the energy, higher the frequency - Frequencies of light give off a color depending on the frequency (red to purple, lower to higher frequency) - Spectra lines on the AES depend on how much electrons and element has and how much energy the electrons are giving off - E=hv means higher energy of the light has a higher frequency