Studied by 8 people
Life Science
Observing, studying, and experimenting to find the nature of things
Geology
Physical nature & history of earth
Precision
indicates the exactness of a measurement; how close measurements are to each other
Sl units
Standard unit of measure; allows consistency; includes all units+prefix
Meter
Length; m
Gram
Mass; g
Line Graph
used to show data over time
Bar Graph
compare values of items
Significant Figures
used by scientists to show the precision of a measurement
Natural Science
tries to understand “nature”, or the whole universe behaves
Physics
Science of force & energy
Earth Science
Geology, meteorology, 7 other areas
Physical Science
Chemistry, Physics
Density
Measurement of how much matter is contained in a certain volume of a substance
Element
A substance that cant be broken down into a simpler substance by simple chemical means
Compound
Substance that are made up of atoms of different elements
Molecule
The smallest unit of a substance that behaves like that substance
Mixture
Combination of substances that are not chemically combined
Chemical Property
Describes how a substance changes into a new substance either by combining with other elements or by breaking apart into a new substance
Boiling point
Temperature where liquid boils
Non Flammability
Inability to burn
Matter
anything that has mass and takes up space
Chemical Change
happens when 1 or more substances are changed into entirely new substances that have different properties/characteristics
Scientific Method
Make Observations, State the problem, Gather information, Form hypothesis, Test hypothesis, Draw conclusions, Report results
Accuracy
indicates how close a measurement is to the true value
Liter
Volume, L
Pie Graph
Shows all the parts of a whole
Scientific Notation
Method of reducing the number of zeros in a very big or very small number & expressing them as a power of 10
Chemistry
Study of Matter and its changes
Hypothesis
Possible explanation of an event or solution to a problem
Atom
Smallest part of an element that still has all properties of an element; Made up of various subatomic particles
Pure Substance
Matter that has a fixed composition and definite properties
Physical Property
Characteristics that can be observed without changing identity of the substance
Melting point
the temperature where a substance changes from a solid to a liquid
Volume
Length x Width x Height
Physical Change
Effects one or more physical properties of a substance without changing the identify of the substance
Miscible
Able to be mixed
Flammability
Ability to burn
Coefficients
In front of a chemical formula indicates how many molecules are present
Water Displacement
An object is largely immersed in a fluid, pushing it out of the way and taking its place
Homogeneous
parts are evenly distributed, the mixture is the same throughout
Math
Language of science
Metric System
the decimal measuring system based on the meter, liter, and gram
Kelvin
Measured in Kelvins (K), used by scientists
Meteorology
Study of atmosphere & weather
Sound
No matter
Periodic Table
A table of the chemical elements arranged in order of atomic number, usually in rows, so that elements with similar atomic structure
Subscripts
Used to indicate when there is more than one atom of an element present
Classification
The action or process of classifying something according to shared qualities or characteristics.
Heterogeneous
Meaning the parts of the mixtures are not evenly distributed
Conclusion
An opinion about the hypothesis, based on the data you have collected and analyzed
Data
facts and statistics collected together for reference or analysis
Control
Observation/Record data variable
Celsius
Measured in degrees (°c), designed for the metric system; Freezing point > 100°c, Boil Point > 100°c
Fahrenheit
Measured in degrees (°F), Freezing pt (H20) > 32°F, Boiling pt (H2O) > 212°F
Immiscible
Won’t remain mixed, you will be able to see 2 layers
Experiment
Experimental variable and control variable
Energy
Ability to change or move matter
Temperature
Measurement of how fast the particles in a substance are moving
Kinetic energy
Energy in motion
Pressure
The amount of force exert on a given area
Archimedes principle
The buoyant force on an object in a fluid is an upward force equal to the weight of the fluid that the object displaces
Buoyant force
Pushes things up from underwater
Solid
Particles vibrate in place
Liquid
Particles are closely packed but can slide past each other
Kinetic Theory of Matter
All matter is made up of atoms and molecules. These atoms and molecules act like tiny particles that are always in motion.
Sublimation
Changing of a solid directly to a gas without it ever being a liquid
Condensation
Changes from a gas to a liquid
Freezing
Changing from a liquid to a solid
Melting point
Temperature where a substance changes from a solid to a liquid
Boiling point
Temperature where a liquid boils
Condensation point
Temperature where gas becomes a liquid
Fluid
Possess unique characteristics that allow things like jets to fly and ships to float; liquids and gasses are classified
Law of conservation of energy
Energy can not be created or destroyed
Viscosity
A liquid’s resistance to flow; Depends on the particle attraction
Gas
particles in constant motion and far apart (don't usually stick together)
Evaporation
Changing a liquid to a gas
Thermal energy
The total kinetic energy of a substance
Law of conservation of mass
Mass is neither created nor destroyed
Plasma
Most common phase of matter in the universe; Similar to gasses, but gasses CANNOT conduct a current like plasma can
Melting
changing a solid to a liquid
Freezing point
Temperature where a liquid becomes a solid
Atomic Theory
Atoms are everywhere and they determine all the properties of the matter they compose
Experimental evidence
Dalton based his theory on ______ by using Law of Definite Proportions
Dalton
Revised the Atomic Theory in 1808; All atoms of a given element were exactly alike, the atoms of different elements could join to form compounds; Foundation for the modern atomic theory
Electrons
Negatively charged, outside of the nucleus orbiting
Spread throughout
Thomson’s Model of electrons in an atom (blueberries in a muffin)
Protons
Positively charged, inside nucleus
Neutrons
No charge, inside nucleus, neutral
Atomic number
Tells you how many protons are in an atom of an element
Mass number
Equals the total number of subatomic particles in the nucleus
Isotopes
Elements that vary in mass numbers because their number of neutrons differ
6.02 x 10^23
1 mole
Avogadro's number
6.02 x 10^23
Behave like waves
Electrons in the new model of an atom
Orbitals
Electron levels
Photon
Particle of light
Atom diagram
An illustration pf what the inside of an atom looks like
Positive charge at center
Atoms nucleus
Gain or lose energy
How electrons move to a higher/lower energy level
Note
Flashcard