Chapter 5 and 6 Test

Question 0

The Bohr Model

Answer 0

• 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

Question 1

Limitations of Rutherford’s Atomic Model

Answer 1

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

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

Question 2

Ground State

Answer 2

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

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

Question 3

What is the formula for energy emitted by an electron?

Answer 3

E=h x v

• V is the frequency
• H is a constant #

Question 4

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

Answer 4

• 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 .

Question 5

Energy levels

Answer 5

• The fixed energies an electron can have

- Unequally spread upart

Question 6

Quantum

Answer 6

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

Question 7

The Bohr model vs. Rutherford’s Atomic Model

Answer 7

• 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

Question 8

The Quantum Mechanical Model

Answer 8

• 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

Question 9

The Quantum Mechanical Model vs. The Bohr Model

Answer 9

• 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

Question 10

Orbitals

Answer 10

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

- Types: S,D, F, P

Question 11

Sublevel

Answer 11

-The shape of an orbital

Question 12

Aufbau principle

Answer 12

-Electrons occupy the orbitals of the lowest energy level first

Question 13

Hund’s rule

Answer 13

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

Question 14

Pauli Exclusion Principle

Answer 14

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

Question 15

Three ways to show electron configurations

Answer 15

• Aufbau Diagram
• Standard Electron Configuration
• Orbital filling Diagram

Question 16

Amplitude

Answer 16

-The wave’s height from zero to the crest

Question 17

Wave length

Answer 17

• The distance between the crests

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

Question 18

Frequency

Answer 18

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

Question 19

The Frequency and Wave Length of Light

Answer 19

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

Question 20

Electron Magnetic Radiation

Answer 20

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

Question 21

Atomic Emission Spectra

Answer 21

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)

Question 22

Spectra Line

Answer 22

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

Question 23

How energy travels from one place to another

Answer 23

• By traveling on a particle (particle is charged then moved)
• By traveling as a wave

Question 24

Energy traveling by particle

Answer 24

• Follow classical mechanics (laws of motion, projectile motion)
• Have energy and mass

Question 25

Energy in wave motions

Answer 25

• 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

Question 26

Photons

Answer 26

• Chunks or quanta of energy that behave as though they were particles
• 1 quanta= 1 photon
• Energy of photon= h x v

Question 27

Planck’s constant

Answer 27

• (h in E=h x v)

- 6.626 x 10^-32 j x s

Question 28

Why the Atomic Emission Spectra is Unique

Answer 28

• 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

Question 29

Dmitri Mendeleev

Answer 29

• Constructed the periodic table of elements

- Arranged the elements in his periodic table in order of increasing atomic mass

Question 30

What are the 3 classes of elements?

Answer 30

• Metals
• Nonmetals
• Metalloids (characteristics of metals and nonmetals)

Question 31

Metals

Answer 31

• 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)

Question 32

Nonmetals

Answer 32

• 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

Question 33

Metalloids

Answer 33

• Has properties similar to metals and nonmetals
• Under some conditions, act like metals, in other conditions act like nonmetals
• Poor conductor of electricity

Question 34

How the Atomic Emission Spectra works with the Bohr Model

Answer 34

• 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