Fin Flashcards
Chemistry
The study of matter and the changes it undergoes
Matter
anything that has mass and volume
Mass
the amount of matter in an object
Weight
the force of gravity acting on an object’s mass
Kinetic Energy
-energy of motion
-measured by temperature
Potential Energy
inversely related to kinetic energy
Kinetic Theory of Matter/Kinetic Molecular Theory
matter is made up of particles which are in continual random motion
States of Matter
-based on particle arrangement
-based on energy of particles and
-the distance between solid particles
sublimation
solid to gas
deposition
gas to solid
plasma
-ionized gas
-excellent conductor of electricity
-affected by magnetic fields
-indefinite shape and volume
-most common state of matter
point where something is a solid, liquid, and gas
triple point
Pure Substances
-have a uniform and definite composition
-Elements
-Compounds (elements are bonded)
Mixtures
-two or more substances mixed together
-blended
-no definite composition, cannot assign a fixed ratio
Types of Mixtures
Heterogeneous
Homogeneous
Heterogeneous
do not have a uniform composition
-parts of the mixture can be seen and removed
Homogeneous
uniform composition
Physical Properties
Properties that can be measured or observed without changing the identity or composition of a substance
-Ex. color, odor, texture etc
Physical Changes
Changes in appearance without changing the composition of a substance
-Ex. cutting, breaking, pulverizing
Changes in state
-melting, freezing, boiling, subliming
Chemical Properties
-Properties that indicate HOW a substance reacts with other substances
-only observed when the substance undergoes a chemical change
-Ex. combustible, flammable
Chemical Changes (reactions)
-One or more substances react to form a completely new substance(s) with DIFFERENT chemical and physical properties
-Ex. rusting, corrosion, digestion, respiration
Law of Conservation of Mass
matter cannot be created or destroyed
Measurement
a type of observation
-two types, qualitative and quantitative
Qualitative
descriptive
Quantitative
observation made with a measuring instrument and includes both a number and a unit
Accuracy
how close a measurement is to the true or accepted value
Precision
how close multiple measurements are to each other
% Yeild
expected/experimental x 100
% Error
abs(expected-experimental) all over expected then x 100
Significant Figure rules
-All non-zero digits are significant
-Leading zeros are never significant (zeros to the left)
-Captive zeros are always significant
-Trailing zeros are sometimes significant
Sig Figs- Addition and Subtraction
Answer is rounded to the same number of decimal places as the number used in the calculations with the least decimal places
-can only be as accurate as the least accurate value
Sig Figs- Multiplication and Division
Look at the total number of sig figs
Answer is rounded to the same number of decimal places as the number used in the calculations with the least s. figs
-Round at the END of calculations
Density?
D=M/V
Volume?
V=M/D
Mass?
M=VD
Dmitri Mendeleev
Organized elements by increasing atomic mass so that the elements in the same row had similar properties
-First periodic table
Henry Mosely
Rearranged the elements by increasing atomic number
-Current table
Periodic Law
When elements are arranged in order of increasing atomic number, there is a periodic pattern in their physical and chemical properties
Elements in the same group have _______ properties.
similar
Elements in the same period have _______ properties
different
Metals
-left of the staircase
-lustrous
-malleable and ductile
-good conductors
*Includes aluminum
Nonmetals
-right of the staircase
-non-lustrous
-brittle
-poor conductors
*Includes hydrogen
Metalloids
touch staircase and have properties of both metals and nonmetals
Semiconductors
normally do not conduct electricity, but will at high temps or when certain substances are added
Democritus
First person to think about atoms
-“atomos”
-believed matter was composed of indivisible particles
John Dalton
- All elements are composed of indivisible particles called atoms
- Atoms of the same element are identical. Atoms of any one element are different from those of another
- Atoms of different elements mix or combine in whole number ratios
- Chemical reactions occur when atoms separate, join, or rearrange. In a chemical reaction, atoms of one element NEVER change into another
Cathode Ray Tube Experiment
JJ Thompson
-In a tube was an inert gas and two plates, one positive and one negative
-therefore particles must have a positive and a negative charge
JJ Thompson
-Discovered the electron
-Cathode Ray Tube Experiment
-Plum Pudding Model
Ernest Rutherford
-Gold foil experiment
-discovered the nucleus
Gold foil expriment
Rutherford
-Shot high-energy beam of alpha particles into gold foil
Observations:
-Most went through, a few particles were deflected at small anges
-Very rarely particles were deflected at large angles
Conclusions:
-atom is mostly empty space
-alpha particles came close to small and positively charged particles (deflected at small angles)
- hit very small, very dense, positively charged nucleus (deflected at large angles)
Eugene Goldstein
discovered the proton
James Chadwick
discovered the neutron