Chapter 1 Flashcards
Matter
anything that has mass and takes up space
diatomics
molecule made up of 2 atoms of the same element
Atoms
smallest identifiable part of an element
element
made up of unique kind of atoms
compound
2 or more different types of elements
solid matter characteristics
molecules and atoms very ordered, crystalline, close together
liquid matter characteristics
molecules can move around (still close together though)
variable composition
can put more or less of a component in the mixture
classifying a heterogeneous mixture
not uniform throughout
classifying a homogeneous mixture
uniform throughout and has variable composition
classifying an element
uniform throughout, pure substance, and one kind of atom
classifying a compound
uniform throughout, not variable throughout, and contains more than one type of atom
type of substances
elements and compounds
substance
any material with a definite chemical composition
difference between compound and element
compound can be decomposed to simpler substances
law of constant composition
the relative number of atoms of each element that makes up the compound is the same in any sample
other name for law of constant composition
law of definite proportions
Mixture
when two or more substances are combined such that each substance retains its own chemical identity
a mixture that can vary in composition throughout a sample
heterogeneous
physical properties
can be observed without changing the substance
chemical properties
can only be observed when the substance is changed into another substance
intensive properties
same regardless of the amount of substance present
extensive properties
depend on how much of the substance is present
examples of physical properties
boiling point, density, mass, volume
examples of chemical properties
flammability, corrosiveness, reactivity with acid
examples of intensive properties
density, boiling point, color
examples of extensive properties
mass, volume, energy
physical changes
do not change composition of substance
chemical changes
result in a new substance
examples of physical changes
change in state, temperature, volume
examples of chemical changes
combustion, oxidation, decomposition
how are mixtures separated
based on the physical properties of the components of the mixture
filtration
solid substances are separated from liquid solutions
solution
homogeneous mixture
chromatography
the separation, especially of closely related compounds, by allowing a solution or mixture to seep through an adsorbent (such as clay, gel, or paper) so each compound becomes adsorbed into a separate, often colored, layer
Distillation
uses differences in boiling points to separate a homogenous mixture into its components (separates two liquids)
SI unit for mass
kilogram
SI unit for length
meter
SI unit for time
seconds
SI unit for temperature
Kelvin
SI unit for amount of substance
mole
SI unit for electric current
Ampere
SI unit for luminous intensity
candela
what about units for things like volume
those are derived units and come about from the standards
where do metric system units differ from SI
mass is in grams;
temp is in K or Celsius;
volume is in cubic centimeters or liters
centi
10^-2
deci
10^-1
Kilo
10^3
Micro
10^-6
Tera
10^12
Mega
10^6
Pico
10^-12
Femto
10^-15
Giga
10^9
Milli
10^-3
nano
10^-9
mass
amount of material in an object
what is a liter made up of
a cube 1 decimeter long on each side
what is a mL made up of
a cube 1 centimeter long on each side (hence cubic centimeter)
conversion of K to Celsius
K=C+273
conversion of F to C
F = 9/5 (C) + 32
Kelvin and Celsius intervals
same; have 100 degree intervals
Density units and equation
D=m/v
g/mL or g/cm3
exact numbers
counted or given by definition
inexact numbers
measure numbers;
depend on how they were determined
accuracy
proximity of a measurement to the true value of a quantity
precision
proximity of several measurements to each other
