Random terms Flashcards
(33 cards)
law of conservation of mass
the law stating that matter can be neither created nor destroyed; in any chemical reaction, the mass of the products is always equal to the mass of the rectants
kilopascal = ___ Pa
1000 Pa
State all 5 points of the Kinetic molecular theory
- Gases are made of tiny particles in constant, random motion. 2. The volume of individual gas particles is negligible compared to the total volume the gas occupies. 3. There are no intermolecular forces negligible. 4. Collisions between gas particles and container walls are elastic, meaning no kinetic energy is lost. 5. The average kinetic energy is directly proportional to the temperature (in Kelvin).
law of definite proportions
the law stating that the elements in a chemical compound are always present in the same proportions by mass
bonding capacity & how to calculate
the number of covalent bonds that an atom can form. take 8 - charge/group # = bonding capcity
Boyle’s law
𝑃1𝑉1 = 𝑃2𝑉2
where n and T are constant
the statement that as the volume of a gas is decreased, the pressure of the gas increases proportionally, provided that the temperature and amount of gas remain constant; the volume and pressure of a gas are inversely proportional
Charles law
V1/T1 = V2/T2
n and P are constant
the statement that as the temperature of a gas is increased, the volume of the gas increases proportionally, provided that the pressure and amount of gas remain constant; the volume and temperature of a gas are directly proportional
Dalton’s law of partial pressures
the statement that the total pressure of a mixture of non-reacting gases is equal to the sum of the partial pressures of the individual gases
Octet rule
a generalization stating that when atoms combine, they tend to achieve 8 valence electrons like of Noble gases.
Any element of full octet is…
stable
spectator ions
ions that are not involved in a chemical reaction
London dispersion force
a weak attractive force acting between all entities, including non-polar molecules and unbonded atoms, caused by the temporary imbalance of electrons within entities
immiscible
unable to mix to form a solution; usually describing liquids that do not readily mix
hydronium ion
a proton that I sbonded to a water molec. chemical formula is H3O+
ionization energy
The energy required to remove and electron from atom or ion in gaseous state
Reactivity
the ability to lose or gain electrons
Electron affinity
the energy change that occurs when an electron is added to a neutral atom in the gaseous state. Higher the electron affinity the more reactive, easily to gain/lose electrons
Arrhenius theory of acide and bases
the theory stating that an acid is a substance that produces hydroium ions in water and a base is a substance that produces hydroxide ions in water
advogadro’s constant
6.022 x 10^23
dipole-dipole force
an intermolecular force of attraction that forms between the slightly positive end of one polar molecule and the slightly negative end of an adjacent polar molecule
dissociation
the separation of individual ions from an ionic compound as it dissolves in water
effective nuclear charge
the net force experienced by an electron in an atom due to the positively charged nucleus
Equivalence point
the point in a titration when the number of moles of added solution is stoichiometrically equal to the number of moles os standard solution
Gay lussac law
P1/T1 + P2/T2
for n and V constant
the statement that as the temperature of a gas increases, the pressure of the gas increases proportionally, provided that the volume and amount of gas remain constant; the temperature and pressure of a gas are directly proportional
