Matter Flashcards
the study of matter (composition &
properties), the changes that it
undergoes, and the energy associated
with those changes
Chemistry
Chemistry is the study of * (composition &
properties), the * that it
undergoes, and the * associated
with those *
matter, changes, energy, changes
Chemistry at three levels:
M -
P -
S -
Macroscopic * - observe
Particulate * - imagine
Symbolic * - represent
a hot ionized gas consisting of approximately equal
numbers of positively charged ions and negatively
charged electrons; it is strongly influenced by …
plasma, electric and magnetic fields
According to democritus (400 BC), matter is made up of
atoms
5 main elements of Earth’s crust
Oxygen, Silicon, Aluminum, Iron, Calcium… other
3 main elements of human body
Carbon, Oxygen, Hydrogen
Uuo 118
113, 115, 117,
Ununoctium
Ununtrium, Ununpentium, Ununseptium
Formed when two or more atoms join together chemically
molecule
a molecule that contains at least two different elements
compounds
Properties of matter:
physical/chemical: consider the *
intensive/extensive: consider the *
change in composition
in the amount of substance
can be observed without changing a
substance into another substance
physical properties
color, odor, density, length, melting point,
boiling point, hardness, etc.
physical properties
Examples of physical properties
color, odor, density, length, melting point,
boiling point, hardness, etc.
individual components of a *
may be separated by *
mixture, physical properties
Physical Property vs Means of Separation density boiling point state of matter intermolecular forces vapor pressure magnetism solubility
decantation, centrifugation distillation filtration chromatography evaporation magnets filtration
Means of Separation vs Physical Property decantation, centrifugation distillation filtration chromatography evaporation magnets filtration
density boiling point state of matter intermolecular forces vapor pressure magnetism solubility
only observed when a substance is changed into
another substance
Chemical Properties
flammability,
coordination number,
radioactivity, oxidation
Chemical Properties
Example of Chemical Properties
flammability,
coordination number,
radioactivity, oxidation
independent of the amount of the substance that is present; important for * a substance
Intensive properties; identifying
depend upon the amount of the substance present
extensive properties
Example of extensive properties
Volume, mass, size, weight, length, energy?
Example of intensive properties
Boiling point, color, temperature, luster, hardness
changes in matter that do not change
the composition of a substance
examples include changes of state, temperature, and volume
Physical change
result in new substances
examples include combustion, oxidation, and decomposition
CHEMICAL CHANGES
Example of physical change
changes of state, temperature, and volume
Example of chemical change
combustion, oxidation, and decomposition
the energy of motion; magnitude depends
on an object’s mass (m) and its velocity (v)
Kinetic Energy
depends on an object’s relative position
with respect to other objects
POTENTIAL ENERGY
in science, a * is collection of
quantitative or numerical data that describes a
property of an object or event
measurement
in science, a measurement is collection of
- that describes a
- of an object or event. Measurement is made by comparing a quantity with a …
quantitative or numerical data, property
standard unit.
in chemistry, we use the *
in measuring different quantities/properties
measurement =
SI units
number + unit
STANDARD UNITS =
Système International
d’Unités (SI)
(The International System of
Units)
- a measure of the amount of material in an object
SI base unit = kilogram; metric base unit = gram - a measure of distance
base unit = meter
MASS
LENGTH
- in general usage, it is the “hotness and coldness” of
an object that determines the direction of heat flow*
base unit = kelvin
Temperature
K —–> °C CONVERSION | K =
°C + 273.15
Celsius scale is based on the *
—-> 0 °C is the freezing point of water, while 100 °C is its boiling point
properties of water
- is the SI unit of temperature
–based on the properties of *
–there are no * Kelvin temperatures
–the lowest possible temperature is called *
Kelvin, gases, negative, absolute zero (0 K)
quantities that are calculated from base units
derived units
quantity that indicates the amount of matter per
unit volume of a sample
density
percentage of a component in
relation to the total mass of the compound
percent composition
how closely individual measurements agree
with the correct, or “true,” value
ACCURACY
measure of how closely individual
measurements agree with one another
PRECISION
Differentiate accuracy and precision
Accuracy refers to how closely individual measurements agree with the correct, or “true,” value while Precision is a measure of how closely individual
measurements agree with one another
smallest particle that is
characteristic of a given element
Atom
Development of the atomic model 5th Century BC: 1773: 1799: 1800s:
DEMOCRITUS AND THE Atomos
Lavoisier’s Law of Conservation of Mass
Proust’s Law of DEFINITE PROPORTIONS
DALTON’S ATOMIC THEORY OF MATTER
Development of the atomic model DEMOCRITUS AND THE Atomos Lavoisier’s Law of Conservation of Mass Proust’s Law of DEFINITE PROPORTIONS DALTON’S ATOMIC THEORY OF MATTER
5th Century BC:
1773:
1799:
1800s:
ideological and philosophical reasoning on the existence of atoms § tiny, indivisible particles of matter called atomos § atoms differ in size, shape, and arrangement in space § first theory of atoms
Democritus
father of modern chemistry
§ observed that matter is
conserved in his experiments
ANTOINE LAURENT
LAVOISIER (1743 – 1794)
LAW OF CONSERVATION OF
MASS
matter is neither created nor
destroyed in a chemical reaction
Dans la nature rien ne se crée,
rien ne se perd, tout change.
In nature, nothing is created,
nothing is lost, everything changes.
each compound always contains the
same elements in a certain definite
proportion and in no other combination
LAW OF DEFINITE PROPORTIONS
JOSEPH LOUIS PROUST
If two elements A and B combine to form more than one
compound, the masses of B that can combine with a given mass of A are in the *
{Law of Multiple Proportions}
ratio of small whole numbers
“each element is composed of
unique type of atom which can
combine in different ratios to form
different compounds”
John Dalton (1766 – 1844) ATOMIC THEORY OF MATTER
DALTON’S ATOMIC THEORY
1. Elements are made of extremely small particles called atoms.
2. Atoms of a given element are identical in size, mass, and other properties; atoms of different elements differ in size, mass, and other properties.
3. Atoms cannot be subdivided, created, or destroyed.
In chemical reactions, atoms are combined, separated, or rearranged.
4. Atoms of different elements combine in simple whole-number ratios to form chemical compounds.
read
1869:
1886:
1897:
1909:
Mendeleev’s PERIODIC TABLE of elements Goldstein and THE PROTON JJ Thomson, THE ELECTRON, AND THE PLUM PUDDING MODEL Millikan and THE CHARGE OF AN ELECTRON
Mendeleev’s PERIODIC TABLE of elements Goldstein and THE PROTON JJ Thomson, THE ELECTRON, AND THE PLUM PUDDING MODEL Millikan and THE CHARGE OF AN ELECTRON
1869:
1886:
1897:
1909:
1911:
1913:
1926:
1932:
Rutherford’s NUCLEAR MODEL
Bohr’s PLANETARY model
Schrödinger’s QUANTUM MECHANICAL MODEL
Chadwick and the NEUTRON
Rutherford’s NUCLEAR MODEL
Bohr’s PLANETARY model
Schrödinger’s QUANTUM MECHANICAL MODEL
Chadwick and the NEUTRON
1911:
1913:
1926:
1932:
mass of electron, proton, neutron
- 11 * 10^-31 kg
- 67 * 10^-27 kg
- 67 * 10^-27 kg
A,z (x)c
A = atomic mass Z = atomic number x = element c = electric charge
H-1, H-2, H-3
Protium, Deuterium, Tritium
are atoms that have the same atomic number (Z)
but different mass numbers (A)
ISOTOPES
The * of an element is the average of the isotopic masses, weighted according to the naturally occurring abundances of the isotopes of the element
atomic mass (weight)
