Chemistry Test #1 – Flashcards
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All Of The Following Statements Are True Except... |
a) laws are statements of relationships that seem to always be the same b) theories are proven explanations of experiemental observations c) hypothesis are tentative explanations of experimental observations d) Laws summarize facts of nature and rarely change e) theories are unified principles that explain a body of facts |
Approximately How Many Elements Are Found In Nature? |
90 |
A Chemical Compound Is... |
A pure substance that is composed of two or more different elements |
Examples of a Physical Property |
odor, taste, color, appearance, melting point, boiling point, and density |
Examples of Chemical Properties... |
Corrosiveness, flammability, acidity, toxicity, and other characteristics. |
Mixture is.... |
Is a substance comppsed of two or more components in proportions that can vary from one sample to another ex. sugar water. |
Compound: |
A substance composed of two or more elements |
When Converting Kelvin to Celcuis |
K - 273 = C |
When converting Celcius to Kelvin... |
C + 273 = K |
Distillation |
A process in which the mixture is heated to boil off the easily vaporized liquids
|
Filtration |
The mixtured is poured through a funnel |
Intensive Property |
One that is independent of the amount of the substance. Ex. Density |
Extensive Property |
One that depends on the amount of the substance ex. Mass |
According to Kinetic Molecular Theory... |
Particles in a liquid are close together, but they are not confined to specific positions. |
Solution |
A Homogenous Mixture of two substances |
Accuracy of Measurements |
Accurancy is an indicator of how close a measurement is to the correct value |
Precision of Measurements |
Precision is an indicator of how close two or more measurements are to each other. |
Daltons Atomic Theory |
1) Matter is composed of Atoms 2) Atoms are Indivisible and Indestructible 3) All atoms of a given element are identical
Both 2 and 3 Were proven wrong
|
Milikan Oil Experiement |
Determined the charge of an electron |
Rank Particles from Highest to Lowest Mass |
Neutron, Proton, Electron |
J. J Thompson |
Determined the charge to mass ratio of an electron by deflecting cathode rays with magnetic and electric fields with cathode ray tube. He also created the plum pudding model. Suggested positive charge was inside and electrons were outside |
Gamma Rays are.. |
high energy radiation |
Photographic Plates |
First evidence for the disintegration of nuclei was obtained |
Beta Particles |
Are identical to electrons |
Alpha Particles |
are 7000 times more massive than electrons |
After Rutherfords Gold Foil Experiment he concluded that.. |
Atoms are composed of a small, dense nucleus surrounded by a cloud of electrons |
Amu is defined as... |
1/12 the mass of one carbon- 12 atoms |
Mass Spectrometry |
The method used to determine the exact masses of Isotopes and their relative abundance |
Isotope |
Atoms of the same element with the same number of protons but a different number of neutrons |
What Element comprises over Three quarters of the Earths atomosphere? |
Nitrogen |
What are the two most abundant elements in the Earth's Crust? |
; ; ; Oxygen and silicon |
; ; ; ; Marie Curie |
; ; ; Was the first person to isolate the element polonium, which she named after he native country |
; ; Allotropes |
; ; ; Same state of matter. Pure carbon can exisit as a diamond, graphite, and buckerministerfullerene |
; ; ; Mendeleev's |
first arranged the periodic table by placing the elements in increasing mass. |
Brimestone or Burning Stone are ancient names for what element? |
Sulfur |
What are the fiour elements comprise approximately 99% of the atoms of the human body? |
Hydrogen, Oxygen, Carbon, and Nitrogen |
What are the names of the Electromatic Spectrum from Greatest wavelength to Smallest? |
Radio, Microwaves, Infrared, Visible Light, Ultraviolet Light, X-Ray, Gamma Rays |
Name the Electromatic Spectrum from Great Potential Energy to Smallest. |
Gamma Rays, X rays, Ultraviolet, Visible Light, Infrared, Microwaves, Radiowaves. |
According to the Photoelectric effect, what is the effect of the increasing wavelength of the light that strikes the metal surface? |
The energy of the ejected electrons decreases |
Electron Diffration |
Was the first experiment to show that electrons can have wave properties |
Schrodinger Equation |
Can be solved to find the probability of finding an electron in a region of space |
The "n" Orbital is the |
Oribital Size |
The "l" Quantum number is associated with |
Orbital Shape |
"Ml" quantum number is associated with.. |
Orbital Orientation |
Heinsburg Uncertainty Principle
|
It is impossible to simultaneously measure the exact position and momentum of an electron |
A node is... |
A region of an electron probability density graph where the probability of finding an electron is zero |
The lowest energy state of an atom is called |
ground state |
The orientation of an orbital space is known as |
magnetic quantum number
ml |
What is a photon? |
A massless particle of radiation |
The maximum height for a wave is... |
amplitude |
What evidence does the photoelectric effect provide that photons are not only waves? |
The photon electric effect provides evidence that an electron is ejected when a single particle of light interacts with a metal surface. When photons of sufficent energy strike a metal surface, electrons are ejected. The number of ejected electrons is proprtion to the number of protons striking the surface. If light was only a wave, then increasing the intensity of light should increase the energy striking the surface and thus increase the energy of the ejected electrons |
Phase of Orbitals is |
The sign of the amplitude of the wave, can be positive or negative |
Paramagnetic |
A substance that contains unpaired electrons is attracted to a magnetic field |
Ferromagnetic |
Substances that retain their magnetism after they are withdrawn from a magnetic field |
The Pauli Exclusion Principle States that |
no two electrons in an atom can have the same 4 quantum numbers |
|
The state of an atom or ion that contains only paired electrons and is therefore slightly repelled by an external magnetic field. Ex. Ba |
Hunds Rule States |
The most stable arrangement of electrons (for ground state configuration) is when there are the maximum number of unpaired electrons, all with the same spin. |
Ionization Energy |
How much energy it takes to remove an electron |
Electron Afffinity |
How much this element is attracted to an electron. How much does it really want to gain an electron.
IT IS MEASURING ELECTRONEGATIVITY |
Excited state is when |
n is greater than 1 |
Bohr's model |
; ; ; Only works for hydrogen |
; ; ; Interference |
; ; ; Interaction between waves |
; ; ; Diamagnetic: Paramagnetic: |
; ; unpaired electrons ; paired electrons |
; ; ; Conversion: Kilo- Gram |
; ; 1g=1*10^3kg |
; ; ; Conversion: Centi-Gram |
; ; 1g= 1*10^2 cg |
; ; ; Conversion: Mili |
; ; ; 1g= 1*10^3mg |
; ; ; Conversion: Micro |
; ; ; 1g= 1*10^6 |
; ; ; Conversion: Nano |
; ; ; 1g=1*10^9 |
; ; ; Conversion: Pico |
; ; ; 1g=1*10^12 |
; ; ; ionization energies |
; ; ; the amount of energy that is required to gain an electron |
; ; ; An Atomic radius is.. |
; ; ; Half the distance between two metal atoms in a pure crystal of the metal |