Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
60 Cards in this Set
- Front
- Back
|
Scanning Tunneling Mircroscope |
A device that uses tunneling currents which rely on distance to rearrange atoms; often used to form atomic resolution pictures. |
|
|
Law of Definite Proportions |
A law introduced by Joseph Proust in 1797 which stated that all samples of a compound, no matter how small or large, will have the same proportions of elements |
|
|
Law of Multiple proportions |
A law introduced in 1804 by John Dalton which stated that when two elements form different compounds the ratio of mass between elements will be a small whole number (ex. CO(2) has twice as many oxygen as CO) |
|
|
Dalton's Atomic Theory |
A theory stated in 1808 by John Dalton which stated the following: 1) Each element is composed of tiny, indestructible atoms/particles 2) All atoms of a given element have the same mass and properties 3)Atoms combine in simple, whole number ratios to form compounds 4) Atoms cannot change from one element to another element, only in the way they bind to other atoms |
|
|
Law of conservation of mass |
States that the mass of the all the products is the same as the mass of all the reactants |
|
|
Cathode Ray tube (CRT) |
A device created by J.J Thompson in the late 1800's that applied high voltage to electrodes.
|
|
|
Oil Drop Experiment |
An experiment performed by Robert Millikan in 1909 that helped to deduce the charge of an electron. Small drops of oil were radiated and suspended in an EM field. The volume of the drop and the strength of the field helped to determine the charge of the electron |
|
|
Charge Of electron |
-1.60x10^-14C |
|
|
Mass of an electron |
9x10^-28 |
|
|
Parts of the Atom |
1) Nucleus -Neutron -Proton 2)Electron Cloud -Electron |
|
|
Gold Foil Experiment
|
An experiment performed by Ernest Rutherford in 1909 to further facilitate Thompson's Plum Pudding model of the yet unseen atom. The experiment bombarded gold foil with alpha particles. Was originally suppose to go straight through but instead was reflected, led to the discovery of the nucleus. |
|
|
Define Chemistry |
Study of matter through the study of atoms and molecules and their interactions |
|
|
Define Atom |
The fundamental building block of matter |
|
|
Define molecule |
Two ore more atoms joined together in a specific shape |
|
|
Define Element |
Only one type of atom |
|
|
Define Compound |
Two or more elements joined together in a fixed shape |
|
|
Break down matter into 2 categories and then into two more |
-Matter 1)Pure Substance a)Elements b) Compounds 2)Mixture a)Homogeneous b)Heterogenous |
|
|
Define a solid |
Atoms and molecules being close together and in fixed positions |
|
|
Define a liquid |
Atoms and molecules being close together but not in fixed positions |
|
|
Define a gas |
Atoms and molecules that are not close together or in fixed postitions |
|
|
Define a plasma |
A gas with a charge |
|
|
Name the two types of solids and explain them |
Crystalline: Regular repeating patterns Amorphous- No regular pattern |
|
|
What is a physical change |
No change in physical composition ex phase changes |
|
|
What is a chemical change |
A change in composition ex. reactions with other elements |
|
|
Extensive property |
A physical property that depends on amount Mass volume length |
|
|
Intensive property |
A property that is independent of amount Ex density temperature boiling point |
|
|
Name three ways to separate mixture with physical changes |
Melting Alloy, Evaporate H(2)O from salt water, Distillation, Filtration |
|
|
Define Energy |
Ability to do work; force through a distance |
|
|
Kinetic energy |
Energy associated with movement |
|
|
Potential energy |
energy associated with position or composotion |
|
|
Thermal energy |
Energy associated with temperature |
|
|
Law of conservation of energy |
Energy cannot be created or destroyed, only transformed |
|
|
Minimum energy principle |
High energy systems tend to go to lower potential energy systems |
|
|
Precision |
When points are close together but not necessarily close to the target |
|
|
Accuraccy |
How close to the actual value the points are |
|
|
Dimensional analysis |
A method of solving unit conversions using cross cancelling of units |
|
|
Multidimensional Unit Conversions |
Each dimension must be accounted for in a unit conversions (watch for units squared and units cubed) |
|
|
Atomic mass unit |
1/12 of carbon-12 |
|
|
Mass of protons and electrons in respect to AMUs |
1 AMU |
|
|
Charge of a proton |
1.60218x10^-19 |
|
|
Mass of a proton in KG |
1.67262x10^-27 |
|
|
Who devised the periodic table |
Dimitri Mendelev |
|
|
How is the periodic table organized |
Ascending number of electrons from left to right similar properties in columns |
|
|
What equation is used to find the atomic masses of elements |
The sum of all isotopes multiplied by their abundance in the world |
|
|
Mass spectrometer |
A device used to calculate the mass of a certain sample of an element. |
|
|
Mole |
The mass of 6.022x10^23 atoms of any element, is also it's atomic mass listed on the periodic table |
|
|
What are two ways electrons bond |
Electron sharing and electron exchange |
|
|
Electron sharing |
Sharing electrons to form molecules |
|
|
Electron Exchange |
Giving or taking an electron to from ions |
|
|
Molecular compounds |
Only contain covalent bonds |
|
|
Ionic compounds |
Formed between a metal or nonmetal; a metal or polyatomic ion; or two polyatomic ions. Bond through electrostatic force (attraction) ions of two elements form a total of zero |
|
|
Covalent molecular compounds |
Two nonmetals bonded together; bonded together through attraction forces between protons and electrons |
|
|
Emperical Formulas |
Formulas that contain simplified versions of all molecules |
|
|
Molecular Formula |
Formulas that contain the number of molecules that a formula has (not necessarily simplified) |
|
|
Atomic mass |
mass of the atom |
|
|
Formula mass |
mass of one formula unit |
|
|
molecular mass |
mass of one molecule |
|
|
Molar mass |
mass of one mole of an element or a compound |
|
|
Empirical mass |
mass based on the empirical formula |
|
|
How does combustion analysis work |
substance is weighed and burned completely and then the mass of the CO(2) and H(2)O is analyzed to find how much carbon and hydrogen they had |
