Chemistry Matter and Change Chap 5 – Flashcards
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Unlock answers 48| The distance from the origin of one wave to its crest |
| Amplitude |
| Which wave lengths bend more? |
Shorter wave lengths (higher frequencies) bend more
[image]
Red has a longer wavelength (shorter frequency) and therefore bends the least. |
| What are the wavelengths of visible light? |
400 nanometers to 700 nanometers
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| What are the names of the visible light spectrum in order from small wavelength to longer wavelength |
Roy G Biv
Red Orange Yellow Green Blue Indigo violet
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| quantum |
| Minimum amount of energy that can be gained or lost by an atom |
| Formula for energy as a function of wave frequency |
Plank's Constant h=6.626 x10-34
Equantum=h?
As frequency increases energy increases |
| Photon |
| A particle of electromagnetic radiation with no mass that carries a quantum of energy |
| Photoelectric effect |
| electrons from a metal are emitted when a certain frequency shines on the surface |
| Ground State |
| Lowest allowable energy state of an atom |
| ?E=Ehigher orbit - Elower orbit |
Formula for Orbital energy released when an electron drops from one orbital to another.
Lyman Series - Ultraviolet light (low frequency) emitted when electron drops to 1st orbital
Balmer Series: Visible light emitted when electron drops to 2nd orbital
Paschen Series - Infrared light (high frequency) emitted when electron drops to 3rd orbital |
| De Broglie theory |
| All moving particles have wave characteristics (emit light) but wavelength is inversely proportional to mass so large objects wavelength is too low to see. |
| Heisenberg Uncertainity Principle |
| It is fundamentally impossible to know precisely both the velocity and position of a particle at the same time. |
| boundary of an atom |
| Volume that encloses 90% probability of containing its electrons |
| Quantum Mechanical Model of the Atom |
| Atomic model in which electrons are treated as waves |
| Principal Quantum Numbers (n) |
| Indicate the relative sizes and energy of atomic orbitals |
| Aufbau Principle ; Diagram |
Aufbau (from the German Aufbau meaning "building up, construction")
Each electron occupies the lowest energy orbital available.
[image] [image] |
| Pauli Exclusion |
| Each electron has an associated spin. A single atomic orbital may contain 2 electrons but they must spin in opposite directions |
| Hunds Rule |
Single Electrons with the same spin must occupy each equal energy orbital before additional electrons with opposite spin can occupy the same orbitals.
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| electron Configuration Notation |
| The electron configuration of an atom is the particular distribution of electrons among available shells. It is described by a notation that lists the subshell symbols, one after another. Each symbol has a subscript on the right giving the number of electrons in that subshell. For example, a configuration of the lithium atom (atomic number 3) with two electrons in the 1s subshell and one electron in the 2s subshell is written 1s22s1. |
What element is represented by the electron configuratoin notation
1s22s22p2 |
| Carbon -- 6 electrons |
What element is represented by the electron configuratoin notation
[Ne]3s1 |
Sodium
To use this shortcut it is necessary to know the noble gas number of electrons. Since only the outside electrons are reactive and all the inside electrons represented by the noble gas that is before the element are non-reactive - it is more important to know about the valence electrons.
In this case there is 1 valence electron |
Use the chart to write the Electron Configuration notation for Chlorine
[image] |
[Ne]3s23p5
[Ne] - Neon is the noble gas before chlorine 3s2 first two columns on the left 3p5 5th element from the left in the 3P Group |
Use the chart to write the Electron Configuration notation for Phosphorus
[image] |
[Ne]3s23p3
[Ne] - Neon is the noble gas before chlorine 3s2 first two columns on the left 3p3 3rd element from the left in the 3P Group |
| What two elements are exceptions to the Aufbau method of electron configuration? |
Chromium: Z:24 [Ar] 3d54s1 and Copper: Z:27 [Ar] 3d104s1 |
Name this element
1s1 |
| Hydrogen |
Name this element
1s2 |
Name this element
1s22s1 |
Name this element
1s2 2s2 |
Name this element
1s22s2 2p1 |
Name this element
1s22s2 2p2 |
| Carbon |
Name this element
1s22s2 2p3 |
| Nitrogen |
Name this element
1s22s2 2p4 |
| Oxygen |
Name this element
1s22s2 2p5 |
| Fluorine |
Name this element
1s22s2 2p6 |
| Neon |
name this element
[Ne] 3s1 |
| Sodium |
Name this element
[Ne] 3s2 |
| Magnesium |
Name this element
[Ne] 3s2 3p1 |
| Aluminum |
Name this element
[Ne] 3s2 3p2 |
| Silicon |
Name this element
[Ne] 3s2 3p3 |
| Phosphorus |
Name this element
[Ne] 3s2 3p4 |
| Sulfur |
Name this element
[Ne] 3s2 3p5 |
| chlorine |
Name this element
[Ne] 3s2 3p6 |
| Argon |
Name this element
[Ar] 4s1 |
| Potassium |
Name this element
[Ar] 4s2 |
| Calcium |
