Chemistry Flashcards
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atomic model; the atom is hard and indestructible
Billiard Ball Model (John Dalton)
atomic model; electrons are embedded in a positively-charged sphere
Plum Pudding Model (JJ Thompson)
atomic model; the mass and all of the positive charge of an atom are concentrated on the nucleus
Nucleus Model (Ernest Rutherford)
atomic model; electrons travel around the nucleus in a circular orbit; their energy is proportional to their distance from the nucleus
Planetary Model (Niels Bohr)
atomic model; the electron is a wave (found in orbitals)
Quantum Model
5 atomic models
- Billiard Ball
- Plum Pudding
- Nuclear
- Planetary/Bohr
- Quantum
number of protons in the nucleus; also equal to the number of electrons
atomic number
protons + neutrons
mass number
True or False: in an atom, the number of protons is constant
True
The Atomic Theory
- all matter are made up of atoms
- all atoms of an element have identical chemical and physical properties
- atoms of different elements have different sets of chemical and physical properties
atoms of the same element that differ in the number of neutrons
isotopes
highly reactive metals
alkali metals
highly reactive non-metals
halogens
inert gases, highly stable elements
noble gases
charged atom
ion
negatively charged ion; gain in electrons
anion
positively charged ion; loss in electrons
cation
energy required to remove an electron from an atom
ionization energy
energy released when an electron is added to an atom
electron affinity
ability to attract electrons
electronegativity
4 Quantum numbers
- principal
- azimuthal
- magnetic
- spin
the number of excess electrons of an atom
valence electrons
every element has the same electronic configuration as the element before it in the periodic table, plus one extra
Aufbau Principle
electrons tend to stay unpaired in orbitals with equal energies
Hund’s Rule
Phases of Matter
- Solid
- Liquid
- Gas
3 types of Mixture
- solution
- colloid
- suspension
type of solution that can still dissolve more solute
unsaturated
type of solution that already contains the maximum amount of sollute
saturated
type of solution that used pressure or heat to dissolve more than the usual amount of sollute
supersaturated
6 Gas Laws
- Boyle’s
- Charles’
- Gay-Lussac’s
- Combined
- Avogadro’s
- Ideal
P1V1= P2V2
Boyle’s
V1/T1 = V2/T2
Charles’
P1VI/T1= P2V2/T2
Combined
VI/n1 = V2/n2
Avogadro’s
pV = nRT
Ideal
Kinetic Molecular Theory of Gases
- particles are infinitely small
- in constant random motion
- elastic collisions
- do not experience intermolecular force
- kinetic energy are directly proportional to their temperatures
mass of reactants = mass of products
law of conservation of mass
ratio of elements are always the same
law of definite proportion/composition
weight of one mole of a material
molar mass
avogadro’s number
1 mole = 6.02x10^23
the chemical formula in lowest
emirical formula
Laws of Thermodynamics
- Law of Conservation of Energy - energy can neither be reated nor destroyed. it can only change forms.
- Entropy - degree of disorder
- entropy at absolute zero is zero
amount of energy needed to raise the temperature of a substance by one degree
specific heat
hotness or coldness
temperature
total kinetic energy of molecules
heat
heat lost or gained during a change in temperature
sensible heat
heat lost or gained during a phase change
latent heat
factors that increase rates of reaction
- higher temperature
- higher concentration of reactants
- large surface area
catlyst
transfer electrons
ionic compound
sharing of electrons
covalent compund
comparative strengths of chemical bonding
ionic > covalent > hydrogen > dipole-dipole forces > London dispersion
