GEN CHEM MT1 Flashcards
study of matter its properties structure composition
CHEMISTRY
whats about matter being studied in chemistry
PROPERTIES
STRUCTURE
COMPOSITION
matter have? (2)
MASS
VOLUME
amount of matter
MASS
amount of occupied space
VOLUME
properties that can be measured / observed without change of composition
PHYSICAL
composition stay the same
PHYSICAL CHANGE
freezing of water
PHYSCIAL CHANGE
molding of clay
PHYSICAL CHANGE
ability of substance to react with another substance
CHEMICAL properties
formation of new substance by reaction
CHEMICAL CHANGE
rusting, digestion
CHEMICAL CHANGE
two types pf physical properties
EXTENSIVE
INTENSIVE
observed by SI units ( mass, length, volume…)
EXTENSIVE
observed by not the amount but the characteristic
INTENSIVE
chemical properties give example (5)
COLOR CHANGE
EVOLUTION OF GAS
TEMP CHANGE
PRECIPITATE
EMISSION OF LIGHT
made up of only one kind of particle
PURE SUBSTANCE
has a fixed or constant structure
PURE SUBSTANCE
simplest form of matter composed of only one kind of atom
ELEMENT
two or more kind of atom combined CHEMICALLY IN DEFINITE PROPORTION
COMPOUND
combination of two or more substances retain their distinct identities
MIXTURE
two types of mixtures
HOMOGENEOUS
HETEROGENEOUS
solution with uniform in composition
HOMOGENEOUS
different in composition and can be seperated physically
HETEROGENEOUS
seperating using filter paper
FILTRATION
seperating by allowing the solid particles to settle at the bottom and liquid poor in another
DECANTATION
seperating using magnet to removeb magnetic solid from non magnetic components
MAGNETIC SEPERATION
seperating homogeneous mixtures of different boiling point
DISTILLATION
seperation complex mixture using chromatography paper
CHROMATOGRAPHY
mixture is heated and water vaporized leaving the particles in the dish or pan
EVAPORATION
extensive prroperties are
MASS LENGTH VOLUME
what does john dalton discovered?
ATOMIC THEORY OF MATTER
three laws that led with dalton’s atomic theory
LAW OF CONSERVATION OF MASS
LAW OF DEFINITE PROPORTIONS
LAW OF MULTIPLE PROPORTIONS
can neither be created or destroyed
MASS
the total mass of the reactions and the products involved is conserved
LAW OF CONSERVATION OF MASS
if a compound is broken down into its constituent elements the proportions will remain the same
LAW OF DEFINITE PROPERTIES
if two elements form more than 1 compound between them the ratios of the masses of the second elemnt which combined with the fixed mass of the first elemtn will always be the ratio of small whole numbers
LAW OF MULTIPLE PROPERTIES
mass is always the same
LAW OF DEFINITE PROPERTIES
mass is not always the same
LAW OF MULTIPLE PROPOTIONS
no matter how you
make a chemical
compound, it have the
same ratio of elements
LAW OF DEFINITE PROPERTIES
number of protons
ATOMIC NUMBER
atomic number is equal to the number of?
ELECTRONS
sum of protons and neutrons
ATOMIC MASS
atoms that lose and gain electrons in order to become stable
IONS
formed between metals and non metals
IONIC BONDS
found in the middle and on the left hand side of the periodic table
METALS
found on the right hand side of periodic table
NONMETALS
oppositely charged ions are very strongly attracted to each other
ELECTROSTATIC ATTRACTION
metal atoms lose electrons to form positively charged ions
POSITIVE IONS
non meta atoms gains electorns to form negatively charged ions with a full outer shell of electrons
NEGATIVE IONS
refers to the combination of atleast two atoms with definite proportion
MOLECULES
involved in metallic bonding
METALS
not involved in molecular compunds
NON METALS
made up of nonmetal and metal elements
MOLECULAR COMPOUND
very simplified representation of the valence shell electronbs in a molecule
LEWIS STRUCTURE
if may ite or ate
MAY OXYGEN
identifies the amount of atom in a compound
MOLECULAR FORMULA
identifies the elements present in simplest forms amount of atoms/ shortened
EMPIRICAL
electrons as particles that are moving around the nucleus with fixed energy called as energy level
BOHR’S MODEL OF ATOM
when the electrons of an atom are in their lowest possible energy levels
GROUND STATE
when the electrons of an atom absorbs energy like heat or electricity
EXCITED STATE
after the excited state, electrons eventually jump back to a lower energy level which releases an energy through light
RELEASING ENERGY
made up of sublevels of energy in which the energy level is made up of one or more sublevels
MAIN ENERGY LEVEL
position and momentum of an electron cannot be determined simultaneously with absolute accuracy
HEISENBERG’S UNCERTAINTY PRINCIPLE
represents the area around an atom’s nucleus where electrons are most likely to be found
ELECTRON CLOUD
who introduced quantum mechanical model
SCHRODINGER
describes the probability of finding three electrons within given orbitals, or 3d regions of space within an atom
QUANTUM MECHANICAL MODEL
fuzzy region of space around the nuclei where electrons are found
ATOMIC ORBITALS
describes the energy level of an electron in an atom
PRINCIPAL QUANTUM NUMBER (n)
describes the way on how the electrons move around the nucleus and determines the shape of an orbital
AZIMUTHAL QUANTUM NUMBER
describes the energy level in a subshell and refers to the possible behavior of the electrons in a magNEtic field
MAGNETIC QUANTUM NUMBER
describes the rotation or the spins on how the electrons move on their own axis as they move around the nucleus
SPIN QUANTUM NUMBER
the electrons that have -1/2 values
SPINNING CLOCKWISE
the electrons that have + 1/2 values
SPINNING COUNTERCLOCKWISE
arrangements of electrons within the orbitals of an tom to know more about an atoms electronic property
ELECTRON CONFIGURATION
the outermost electrons of an atom
VALENCE ELECTRONS
the highest energy electrons in an atom and the most reactive
VALENCE ELECTRONS
valence electrons can be gained, lost or stored to form?
CHEMICAL BONDS
meaning of Aufbau in German
BUILDING UP
electrons must occupy the lowest possible energy level before filling up the next
AUFBAU PRINCIPLE
maximum electron per subshell S
2
maximum electron per subshell P
6
maximum electron per subshell D
10
maximum electron per subshell F
14
requires that the electrons fill the orbitals in a sublevel, one by one , before pairing the electrons in an orbitals
HUND’S RULE
no two electrons can have the same four electronic quantum numbers, as an orbital can contain a maximum of only two electrons and the two electrons must have opposing spins
PAULI EXCLUSION PRINCIPLE
repelled by magnetic field
DIAMAGNETISM
atom with electrons that will be very slightly affected by magnetic field
DIAMAGNETISM
attracted to magnetic field
PARAMAGNETISM
atoms that do not have all their electrons spin-paired and are affected by magnetic fields
PARAMAGNETISM
si susan
PUMASOK SA PINTUAN
si daddy
PUMASOK SA DILIM
when orbitals are incomplete
PARAMAGNETISM
when orbitals are complete
DIAMAGNETISM
