Chapter 1 vocabulary Flashcards
understand all matter by understanding how atoms work
Chemistry
sub-microscopic particles that make up everything
Atoms
atoms bound together
Molecules
has to be falsifiable
Hypothesis
has to do with numbers
Quantitative
has to do with observations
Qualitative
summary of past observations to predict future ones
Law
a model that explains why nature works
Theory
volume: fixed
shape: fixed
movement: small vibrations
Solid
volume: fixed
shape: changes based on container
movement: 3D movement in liquid
Liquid
volume: changes based on container
shape: changes based on container
movement: 3D in the container
Gas
–> Pure Substance
–> Mixture
Matter
–> Element
–> Compound
Pure Substance
–> Heterogeneous
–> Homogeneous
Mixture
a physical combination of two or more substances that are not chemically bonded together
Mixture
a form of matter composed of only one type of particle
Pure Substance
a mixture in which the composition is not uniform throughout the mixture
Heterogeneous mixture
a mixture where the components are evenly distributed throughout
Homogeneous mixture
carefully pouring off
Decanting
separating a homogeneous mixture of liquids. (separate by boiling points)
Distillation
separate a liquid from a solid using paper
Filtration
property that is displayed without changing its composition (bonded)
Physical Property
displayed when you change composition via reaction
Chemical Property
associated with the temperature (actually it is kinetic energy)
Thermal energy
he energy an object has because of its motion
Kinetic Energy
a type of energy that is stored in an object due to its position relative to other objects
Potential Energy
Kinetic + Potential
Total Energy
0 = water freezing
100 = water boiling
Fahrenheit
no negative numbers
273 = water freezing
373 = water boiling
Kelvin
how much something weighs per its volume
a derived unit
independent on amount of stuff
Intensive Property
dependent on amount of stuff
Extensive Property
no limit to significant figures
exact numbers
how close a measured value is to the actual value
Accuracy
how close measurements are to each other
Precision
inevitable mistakes during trails (can average out with enough trials)
Random Error
repeated error that is too high or too low.
Systematic Error
atoms of the same element that have the same number of protons (i.e., atomic number, “Z”) but a different number of neutrons, meaning that their mass number, “A”, varies
Isotopes
an atom or group of atoms that has an electric charge
Ion
